SOLUBILITIES 

OF 

INORGANIC   AND   ORGANIC 
SUBSTANCES 


A  COMPILATION  OF  QUANTITATIVE  SOLUBILITY 

DATA    FROM   THE   PERIODICAL 

LITERATURE 


BY 

ATHERTON   SEIDELL,   PH.D. 

Hygienic  Laboratory,   U.  S.  Public  Health 
Service,  Washington,  D.  C. 


SECOND  EDITION 

ENLARGED  AND  THOROUGHLY  REVISED 


NEW  YORK 

D.  VAN  NOSTRAND  COMPANY 

25   PARK  PLACE 
1919 


COPYRIGHT,  1907,  1911,  1919, 

BY 
D.  VAN   NOSTRAND   COMPANY 


Stanbope  jpress 

F.    H.GILSON   COMPANY 
BOSTON,  U.S.A. 


PREFACE 

The  principal  object  in  preparing  a  compilation  of  solubility 
data,  from  the  point  of  view  of  the  advancement  of  chemistry,  is 
to  furnish  material  for  the  origination  and  verification  of  theories 
of  solution.  The  majority  of  investigators  who  have  been  en- 
gaged on  such  problems,  have  been  compelled  to  determine  ex- 
perimentally the  values  required  for  developing  the  generalizations 
they  hoped  to  establish.  In  fact,  a  large  part  of  the  most  accurate 
data  which  are  here  brought  together,  are  the  outgrowth  of  such 
studies.  It  is  hoped,  therefore,  that  the  present  effort  to  make 
these  and  all  other  quantitative  results  more  accessible  for  theo- 
retical studies  of  solubility,  will  lead  to  noteworthy  advances  in 
this  field  of  chemistry. 

Of  the  various  properties  which  determine  the  uses  of  com- 
pounds in  a  chemical  way,  solubility  is  of  first  importance.  There- 
fore, solubility  data  are  perhaps  of  even  greater  interest  from  a 
practical  than  from  a  theoretical  point  of  view.  For  this  reason  it 
has  been  necessary  to  consider  the  needs  of  those  who  require  such 
information  only  incidentally  and  may,  therefore,  be  less  familiar 
with  some  of  the  forms  used  for  its  expression.  With  this  in 
mind,  and  at  the  suggestion  of  users  of  the  preceding  edition, 
chapters  have  been  prepared  in  which  are  described,  among  other 
things,  the  sources  of  solubility  data,  the  methods  of  calculating 
them  to  desired  terms,  the  interpretation  of  their  tabular  arrange- 
ment, as  well  as  some  of  the  methods  used  for  the  accurate  deter- 
mination of  solubilities. 

Soon  after  the  previous  edition  was  issued,  the  collection  of  the 
new  data,  to  be  used  in  keeping  the  subject  matter  up  to  date, 
was  systematically  begun.  In  doing  this,  the  experiment  was 
made  of  examining  each  journal  page  by  page,  instead  of  scan- 
ning the  titles  of  original  papers  contained  in  it.  This  resulted  in 
the  discovery  of  many  data  that  would  otherwise  have  been  over- 
looked, and  it  soon  became  apparent  that  a  more  careful  search  of 
the  literature  than  that  previously  made  was  necessary.  It  was, 
therefore,  decided  not  only  to  examine  the  current  periodicals 
minutely,  but  to  go  through  the  back  volumes  in  a  manner  equally 
as  thorough.  The  data  collected  in  this  way  soon  amounted  to  more 
than  could  be  advantageously  added  as  a  supplement  to  the  tables 
in  the  first  edition,  and  it  was  decided  to  wait  until  the  whole 
book  could  be  completely  rearranged,  before  making  any  additions 

iii 


PREFACE 

to  the  subject  matter.  It  also  appeared  advisable  to  extend  the 
scope  to  include  freezing-point  and  certain  other  data,  which  had 
been  omitted  entirely  from  the  first  edition.  The  undertaking, 
therefore,  developed  far  beyond  the  original  expectation  of  regu- 
larly adding,  from  year  to  year,  the  new  data  which  would  keep 
the  compilation  up  to  date.  Since  the  amount  of  time  at  my  dis- 
posal for  this  work  was  limited,  progress  necessarily  has  been 
slow.  Finally,  the  advent  of  the  war  extended  the  period  far  be- 
yond the  limit  caused  by  other  conditions. 

Although  the  compilation  has  now  been  completed,  I  realize 
that  in  a  work  of  this  kind,  more  satisfactory  results  would  have 
been  achieved  if  several  individuals  had  cooperated  in  its  prepara- 
tion. The  recent  decision  of  the  American  Chemical  Society  to 
extend  its  activities  to  the  publication  of  reference  books,  will,  I 
hope,  insure  that  hereafter,  compilations  of  the  present  character 
will  be  made  in  the  exceptionally  thorough  manner  which  only  an 
organization  with  elaborate  facilities  can  provide. 

In  this  connection  I  wish  to  express  the  opinion  that  the  new 
venture  of  publishing  compendia  of  chemical  literature,  which  the 
chemical  societies  of  England  and  America  are  just  now  about  to 
undertake,  will  prove  of  service  to  the  progress  of  chemistry  in 
English  speaking  countries,  second  only  to  that  rendered  by  the 
journals  of  original  and  of  abstract  literature,  which  these  societies 
have  so  successfully  developed. 

I  realize,  more  than  ever,  that  opportunities  for  the  occurrence 
of  errors  are  innumerable  and  although  I  have  endeavored  to 
maintain  unremitting  vigilance  to  avoid  them,  my  efforts  toward 
this  end  have  not  always  been  successful.  I  desire  to  express  my 
appreciation  to  all  who  have  called  attention  to  errors  in  the 
former  edition  and  I  will  be  equally  grateful  to  those  who  point 
out  to  me  needed  corrections  in  the  present  book.  In  this  con- 
nection, I  am  greatly  indebted  to  Professor  B.  N.  Menschutkin  of  the 
Polytechnic  Institute  (Sosnovka),  Petrograd,  Russia,  who,  in  calling 
my  attention  to  an  error  in  the  tabulation  of  some  of  his  work 
given  in  the  first  edition,  sent  me  a  complete  set  of  reprints  of  his 
many  papers  on  solubility  and  personally  corrected  the  tables 
which  I  prepared  from  them,  for  use  in  the  present  volume. 

In  conclusion  I  wish  gratefully  to  acknowledge  the  assistance 
rendered  me  by  Dr.  W.  S.  Putnam  of  the  Cooper  Union  of  New 
York  during  the  compilation  of  the  first  150  pages  of  the  tables. 

A.  S. 

WASHINGTON,  D.  C., 
Feb.  22,  1919. 

iv 


GENERAL  INFORMATION 

The  following  detailed  account  of  the  collection  and  arrangement 
of  the  solubility  data  contained  in  the  present  volume,  has  been 
prepared  particularly  for  those  who  need  quantitative  solubilities 
rarely,  and  are  more  or  less  unfamiliar  with  the  usual  tabular 
methods  of  expressing  such  data.  To  those  who  are  better  ac- 
quainted with  the  subject,  the  descriptions  in  some  cases  at  least, 
will  probably  be  considered  more  elementary  than  necessary.  It  is 
hoped,  however,  that  with  the  aid  of  the  explanations  here  given, 
no  one  need  remain  uncertain  as  to  the  true  meaning  of  any  result 
or  form  of  expression  found  in  the  book. 

Sources  of  the  Data.  —  In  addition  to  those  determinations  made 
for  the  specific  purpose  of  ascertaining  particular  solubilities,  many 
results  are  reported  in  connection  with  the  study  of  theories  of 
solution  and  are,  therefore,  easily  located.  On  the  other  hand,  since 
solubilities  often  form  only  an  incidental  part  of  an  investigation, 
many  valuable  data  can  be  found  only  by  a  very  careful  search  of 
the  literature.  Consequently,  in  collecting  material  for  the  present 
compilation,  the  procedure  was  adopted  of  perusing,  page  by  page, 
every  volume  of  a  selected  number  of  chemical  journals,  for  the 
years  1900  to  1918.  In  doing  this,  attention  was  paid  particularly, 
to  collecting  all  tabulated  data,  but  a  vigilant  watch  for  solubility 
statements  in  the  text  was  also  maintained.  The  twenty-three 
journals  which  were  examined  in  this  manner  are  designated  with 
asterisks  (*)  in  the  volume-year  table  of  journals  given  at  the  end 
of  the  book.  There  is  also  listed  in  this  table  a  somewhat  larger 
number  of  other  journals,  containing  relatively  few  papers  in  which 
solubility  data  may  be  expected.  In  these  cases,  a  page  by  page 
examination  would  have  required  more  effort  than  the  results  to  be 
gained  appeared  to  justify.  Consequently,  only  the  tables  of  con- 
tents of  these  journals  were  searched  for  references  to  solubility 
data.  The  last  volume  number  given  for  each  journal  in  this  table 
shows  the  final  volume  examined  as  above  mentioned. 

Of  the  abstract  journals,  only  "Chemical  Abstracts"  was  syste- 
matically searched  for  references  to  data  published  in  other  than 
the  twenty-three  journals  which  were  minutely  examined.  The 
original  of  practically  all  references  obtained  in  this  way  was 
consulted. 


GENERAL   INFORMATION 

The  larger  handbooks  of  inorganic  and  organic  chemistry,  such 
as  those  of  Dammer,  Moissan,  Gmelin-Kraut,  Abegg,  Beilstein  and 
others,  were  not  examined,  since  it  was  believed  that  the  major  part 
of  the  data  so  obtained  would  undoubtedly  have  been  already  col- 
lected from  the  journals. 

Of  the  available  compendia  of  physical  constants,  only  the  fourth 
edition  of  Landolt  and  Bornstein's  "Tabellen"  and  the  three  issues 
of  the  international  "Tables  annuelles  de  Constantes  et  Donnees 
Numerique"  were  systematically  examined,  and  in  these  cases  the 
volumes  were  used  principally  to  check  the  completeness  of  the 
compilation  made  directly  from  the  journals. 

Of  the  various  pharmacopoeias  and  pharmaceutical  reference 
books,  only  the  eighth  edition  of  the  U.  S  Pharmacopoeia  (1905) 
was  used  to  any  extent  as  a  source  of  solubility  data.  Most  of  the 
results  contained  in  the  subsequent  ninth  edition  (1916),  are  taken 
from  the  previous  edition  and  calculated  to  the  basis  of  volume,  in- 
stead of  weight,  of  solvent  required  to  dissolve  unit  weight  of  solid. 
It  is  believed  that,  for  the  present  compilation,  the  weight  basis  for 
expressing  the  results  is  to  be  preferred,  and  moreover,  by  taking 
the  data  directly  from  the  eighth  edition,  the  errors  incidental  to 
the  recalculation  and  rounding  off  to  whole  numbers,  are  elimi- 
nated. 

In  this  connection,  it  should  be  mentioned  that  the  results  ob- 
tained from  pharmaceutical  reference  books  for  the  more  complex 
compounds  such  as  the  alkaloids,  are  for  the  most  part  of  only 
qualitative  interest,  and  although  probably  of  sufficient  exactness 
for  use  in  pharmaceutical  compounding,  do  not  come  within  the 
scope  of  quantitative  accuracy  adopted  for  the  present  volume. 

Collection  and  Compilation  of  the  Data.  —  In  all  cases  where  solu- 
bility results  were  found  recorded  in  an  original  communication, 
the  data  and  accompanying  descriptions  of  the  experiments  were 
copied  and  the  record  thus  made  filed  for  future  use.  In  preparing 
these  abstracts  the  actual  experimental  results  were  always  recorded 
when  available,  rather  than  the  values  as  recalculated  by  the  author 
to  terms  which  best  suited  the  solution  of  the  problem  in  hand.  In 
many  cases  the  original  analytical  data  were  not  given  and  uncer- 
tainties arose  as  to  the  factors  used  and  as  to  just  how  the  calcula- 
tions had  been  made.  This  was  particularly  true  in  the  many  cases 
where  the  results  were  expressed  in  gram  molecular  quantities  per 
given  volume  of  solution  or  on  the  basis  of  molecular  percentage. 

The  supplementary  information  sought  in  each  paper  included 
such  points  as  the  method  which  had  been  employed  for  securing 

vi 


GENERAL   INFORMATION 

equilibrium,  the  care  exercised  in  purifying  the  material,  the  exact 
composition  of  the  solid  phase,  the  procedure  followed  in  separating 
the  saturated  solution  and  analyzing  it,  as  well  as  any  other  details 
which  might  be  of  value  in  forming  a  correct  estimate  of  the  ac- 
curacy of  the  work.  The  time  consumed  in  this  part  of  the  exami- 
nation of  the  original  papers  was  usually  found  to  have  been  well 
spent  when  the  compilation  of  the  solubility  tables  from  these  data 
sheets  was  undertaken.  This  was  especially  the  case  when  it  be- 
came necessary  to  compare  the  results  for  the  same  compounds 
obtained  by  two  or  more  investigators.  When  practically  all 
abstracting  of  the  solubility  data  in  the  journals  already  referred  to 
had  been  completed,  the  data  sheets,  which  were  at  first  grouped 
according  to  the  journals  examined,  were  arranged  alphabetically 
in  accordance  with  the  names  of  the  compounds  for  which  data  had 
been  determined.  In  this  way  all  results  for  a  particular  compound 
were  brought  together  and  the  actual  preparation  of  the  systemati- 
cally arranged  tables  could  be  begun. 

It  will  be  noted  that  by  this  plan  the  original  papers  were  practi- 
cally all  consulted  before  the  actual  compilation  of  any  of  the  data 
was  started.  In  only  a  small  percentage  of  cases  was  the  author's 
paper  again  consulted,  at  the  time  the  manuscript  of  the  compiled 
tables  was  prepared  or  later.  Although  this  plan  introduces 
numerous  opportunities  for  errors  resulting  from  the  recopying  of 
the  original  data,  it  appeared  to  be  the  only  practical  procedure. 
A  more  direct  transference  of  the  original  results  to  the  finished  page 
would  have  required  that  the  work  be  done  in  the  library  or  that  a 
much  larger  number  of  books  be  withdrawn  than  is  ordinarily 
permitted. 

Although  it  was  originally  intended  to  have  the  manuscript 
pages  typewritten  before  transmitting  them  to  the  printer,  this 
plan  had  to  be  abandoned  on  account  of  the  difficulty  in  obtaining 
the  services  of  a  competent  person  and  also  on  account  of  the 
considerable  added  expense.  This  necessity  may  possibly  have 
resulted  advantageously,  since  one  of  the  several  opportunities  for 
the  introduction  of  mistakes  through  copying  the  figures,  was 
eliminated. 

The  copy  as  forwarded  to  the  printer  was,  for  the  most  part, 
clear  and  legible  but  it  was  far  from  the  orderly  character  of  type- 
written pages,  consequently,  it  would  be  surprising  if  none  of  the 
many  errors  made  by  the  compositors  as  a  result  of  imperfect 
copy,  were  overlooked  during  the  proof-reading,  which  from  be- 
ginning to  end  was  done  without  assistance.  In  order  to  reduce 

vii 


GENERAL  INFORMATION 

typographical  and  all  other  errors  to  the  least  possible  number,  it 
would  be  necessary  to  compare  every  original  paper  with  the  final 
printer's  proof  and  to  repeat  every  calculation  of  a  result  one  or 
more  times.  That  this  was  not  possible  in  the  present  case  will 
be  easily  realized  when  the  very  large  amount  of  the  data  is 
considered. 

These  details  are  mentioned  at  this  time  because  it  is  believed 
that  the  user  of  the  book  is  entitled  to  exact  information  in  regard 
to  the  conditions  under  which  the  compilation  was  made.  It  is 
only  with  a  clear  understanding  of  its  limitations  that  the  book 
can  be  used  to  greatest  advantage. 

In  this  connection  it  should  be  pointed  out  that  although  oppor- 
tunities for  errors  in  recording  the  purely  numerical  data  here 
brought  together  are  abundant,  in  the  majority  of  cases  the  mis- 
takes are  not  necessarily  misleading  if  proper  regard  is  paid  to  the 
general  import  of  the  results  as  a  whole.  Thus  on  the  basis  of  the 
well-established  principle  that  changes  in  solubility,  such  as  are 
due  to  temperature  or  concentration  of  solvent,  always  proceed 
regularly,  errors  in  the  case  of  one  or  more  figures  in  a  table  will 
become  apparent  on  careful  comparison  with  the  remaining  results, 
or  by  plotting  them  on  cross  section  paper  and  drawing  the  curve. 
Consequently,  the  table  as  a  whole  provides  a  check  on  the  indi- 
vidual results  of  which  it  is  composed. 

Scope.  —  In  brief,  it  may  be  stated  that  it  has  been  the  inten- 
tion to  include  in  this  compilation,  the  actual  results,  or  a  reference 
to  all  quantitative  solubility  data,  recorded  in  the  journals  referred 
to  in  a  preceding  section  and  listed  in  the  table  at  the  end  of  the 
book. 

Freezing-  or  melting-points  of  binary  or  more  complex  systems, 
as  explained  in  the  footnote  on  page  I ,  are  considered  to  be  quanti- 
tative solubility  data.  The  experimental  results  are  quoted  for 
only  those  systems  in  which  one  component  is  water  or  alcohol, 
or  which  are  mixtures  of  fairly  well-known  compounds,  and  ref- 
erences are  given  to  all  others  for  which  data  were  found 

Owing  to  the  uncertainty  of  the  boundary  between  solubility 
and  other  equilibria,  it  has  been  necessary  arbitrarily  to  draw  the 
line  in  regard  to  certain  data  which  it  has  appeared  wise  to  exclude. 
In  accordance  with  this,  no  attempt  has  been  made  to  gather 
either  figures  or  references,  for  the  following: 

(a)  Melting-point  data  for  mixtures  of  metals  (alloys). 
(6)   Melting-point  data  for  mixtures  of  minerals,  except  a  few 
of  relatively  simple  composition, 
viii 


GENERAL   INFORMATION 

(c)  Freezing-points  of  very  dilute  solutions  made  for  the  de- 

termination of  molecular  weights  or  electrolytic  disso- 
ciation. 

(d)  Data  for  the  solubility  of  gases  in  molten  metals. 

(e)  The  so-called  solubility  of  metals  in  various  solvents,  due 

to  a  chemical  reaction  which  occurs. 
(/)    Data  for  solid  solutions. 
(g)  Data  for  compounds  of  unknown  or  variable  composition. 

Order  of  Arrangement.  —  The  alphabetical  arrangement  is  be- 
lieved to  have  the  advantage  that  data  for  particular  compounds 
can  be  more  easily  located  than  would  be  the  case  if  various  com- 
pounds- or  systems  had  been  grouped  according  to  selected  rela- 
tionships. There  is  one  difficulty  which  applies  equally  to  any  ar- 
rangement designed  to  avoid  duplications,  and  that  is  the  placing 
of  those  systems  for  which  solubility  results  are  given  for  two  or 
more  of  the  constituents  involved.  This  applies  especially  to 
freezing-point  lowering  data  for  binary  mixtures.  In  these  cases 
the  results  show  in  turn  the  solubility  of  each  component  in  the 
other  and  it  is  necessary  to  choose  one,  or  to  record  the  results  under 
the  name  of  each  member  in  two  separate  places.  There  are  many 
similar  cases,  in  aqueous  systems  of  two  or  more  salts  and  of  mix- 
tures of  liquids,  where  results  are  given  in  succession  for  the  solu- 
bility of  each  component  in  solutions  of  varying  concentrations 
of  the  other.  In  order  to  prevent  duplication  in  these  cases  it  was 
necessary  arbitrarily  to  select  that  component  under  which  the 
results  for  the  entire  system  are  to  be  recorded.  In  harmony  with 
the  general  alphabetical  plan  of  the  book,  it  appeared  most  logical 
to  make  the  selection  on  the  basis  of  the  alphabetical  order  of  the 
names  of  the  compounds  involved.  In  the  majority  of  cases, 
therefore,  every  system  in  which  solubility  data  for  two  or  more 
compounds  are  given,  is  placed  under  the  name  of  that  component, 
the  initial  of  which  comes  earliest  in  the  alphabet. 

The  advantage  of  this  plan  is  that  every  system  is  assigned  to  a 
single  position  by  rule  and  opportunities  for  unknowingly  record- 
ing independent  investigations  of  the  same  system,  under  different 
headings  at  widely  separated  portions  of  the  book,  are  avoided. 

An  exception  to  this  rule,  which  it  was  considered  wise  to  observe, 
is  in  connection  with  mixed  systems  containing  a  compound  of  one 
of  the  rarer  elements.  In  these  cases,  on  account  of  the  greater 
interest  in  the  rare  earth  compound,  the  data  have  been  located 
under  its  name. 

In  the  case  of  those  mixtures  of  salts  and  liquids  which  yield 

ix 


GENERAL  INFORMATION 

liquid  layers  over  certain  concentrations  and,  therefore,  to  all  in- 
tents and  purposes  become  reciprocally  soluble  liquid  mixtures,  they 
are  placed  under  the  name  of  the  salt  or  of  that  component  which 
exists  as  a  solid  under  ordinary  conditions.  It  has  only  rarely  been 
possible  to  give  cross  references  in  the  body  of  the  book,  but  in 
all  cases  those  components  of  the  mixtures,  other  than  the  one 
under  which  the  data  are  alphabetically  recorded,  are  included 
in  the  subject  index  of  the  book  and  the  reader,  therefore,  should 
not  fail  to  consult  the  index  when  results  or  a  cross  reference  to 
the  desired  compound  are  not  found  in  the  proper  place  in  the 
body  of  the  book. 

Nomenclature.  —  In  regard  to  questions  of  the  proper  naming  of 
compounds  for  the  purpose  of  their  correct  alphabetical  arrange- 
ment, particularly  in  respect  to  organic  compounds,  the  usage 
followed  in  the  index  of  "Chemical  Abstracts"  Has  been  adopted. 
Thus  the  name  under  which  a  given  compound  is  indexed  in 
"Chemical  Abstracts"  is,  in  practically  all  cases,  the  one  used  for 
deciding  its  position  in  the  present  compilation. 

The  most  notable  deviation  from  this  rule  is  in  the  case  of  com- 
pounds of  those  metals  to  which  specific  names,  differing  from  the 
name  of  the  metal  itself,  have  been  given;  thus,  for  example  in 
the  present  compilation,  iron  salts  are  not  classed  under  ferrous 
and  ferric  and  tin  salts  under  stannous  and  stannic  but  under  iron 
and  tin,  respectively.  Another  exception  is  the  grouping  of  di 
and  tri  substituted  amines  under  the  mono  substituted  compound, 
instead  of  placing  them  under  the  widely  separated  headings  Di 
and  Tri.  Thus  results  for  diethylamine  and  triethylamine  are 
given  in  connection  with  ethyl  amine  instead  of  being  grouped, 
on  the  one  hand  with  dimethyl,  dipropyl,  diphenyl,  etc.,  amines, 
and  on  the  other  with  trimethyl,  tripropyl,  triphenyl,  etc.,  amines. 

In  harmony  with  the  adoption  of  "Chemical  Abstracts"  as 
authority  for  the  correct  naming  of  compounds,  the  rules  adopted 
for  that  publication  (see,  in  connection  with  index  to  Vol.  n, 
1917)  have  been  followed  as  closely  as  possible  in  all  other  matters 
connected  with  systematic  nomenclature.  The  exceptions  which 
may  be  found  are  either  mistakes,  or  occur  in  those  tables  reused 
from  the  first  edition,  in  which  corrections  of  the  original  plates 
would  have  cost  more  than  the  advantage  to  be  gained  appeared 
to  justify.  (For  example,  see  first  table,  page  144,  and  many 
others  in  which  the  old  forms  of  spelling  names  such  as  aniline, 
sulfate,  glycerol,  etc.,  have  not  been  corrected.) 

Abbreviations.  —  Although,  in  practically  every  case  the  abbre- 


GENERAL   INFORMATION 

viations  which  have  been  used  are  identical  with  those  adopted 
for  "Chemical  Abstracts"  and  will,  in  general,  be  readily  under- 
stood, for  the  sake  of  accuracy  and  as  a  matter  of  convenience  a 
list  of  those  made  use  of  in  the  present  volume  is  given  at  the 
close  of  this  chapter.  (Page  xxi.) 

Literature  References.  —  In  order  to  save  space,  when  several 
references  must  be  given  in  connection  with  one  result  or  table, 
and  to  avoid  the  repetition  of  the  complete  journal  reference 
when  data  for  different  compounds  are  given  in  the  same  paper, 
an  abbreviated  form  of  reference,  consisting  of  the  name  of  the 
author  and  year  of  the  work,  has  been  adopted.  These  are  to  be 
used  in  connection  with  the  author's  index,  in  which  the  complete 
references  are  arranged  chronologically  under  each  name. 

Deviations  from  this  system  occur  in  connection  with  the  tables 
reused  from  the  first  edition.  In  these  cases  it  was  decided  not 
to  incur  the  expense  of  altering  the  plates  simply  for  the  sake  of 
uniformity.  The  complete  references  given  with  the  old  tables 
are  sometimes,  but  not  always,  repeated  in  the  author's  index. 

Forms  of  Stating  and  Methods  of  Calculating  Solubilities  to  Desired 
Terms.  —  When  a  solid  compound  is  brought  in  contact  with  a 
liquid,  more  or  less  of  it  dissolves  with  the  production  of  a  homoge- 
neous liquid  mixture.  The  disappearance  of  the  solid  in  the 
liquid  continues,  however,  only  up  to  a  certain  point,  beyond 
which  at  a  given  temperature,  no  more  of  the  solid  can  be  made 
to  dissolve.  This  quantity  is  designated  as  the  solubility  of  the 
compound  in  the  particular  liquid.  Solubility,  therefore,  always 
refers  to  a  saturated  solution  and  is  expressed  numerically  in 
terms  of  the  composition  of  the  homogeneous  liquid  in  equilib- 
rium with  an  excess  of  undissolved  solid.  It  is  obvious  that  the 
composition  of  a  saturated  solution  may  be  expressed  in  a  great 
variety  of  terms  and  it  is,  therefore,  to  be  expected  that  investi- 
gators will  choose  those  terms  which  best  suit  the  elucidation  of 
the  particular  problems  in  hand. 

As  might  be  expected,  the  terms  in  most  general  use  and  those 
which  permit  of  the  widest  applicability  of  the  results,  are  based 
on  the  weights  of  the  ingredients  of  the  saturated  solution.  These 
may  be  either  the  weight  of  the  dissolved  compound  contained  in  a 
unit  weight  (usually  100  grams)  of  the  homogeneous  liquid  mixture, 
which  corresponds  to  percentage  of  the  dissolved  compound  in 
the  saturated  solution,  or  else  the  weight  of  the  dissolved  sub- 
stance in  a  unit  weight  of  the  solvent.  In  either  case  the  one 
form  may  be  easily  calculated  to  the  other.  Thus,  for  instance, 

xi 


GENERAL  INFORMATION 

if  it  is  found  that  100  grams  of  the  saturated  solution  contain 
20  grams  of  the  dissolved  compound,  there  can  be  present  only 
loo  —  20  =  80  grams  of  solvent,  and  since  this  80  grams  of  solvent 
holds  20  grams  of  the  dissolved  compound,  20  -r-  80  X  100  =  25 
grams  of  it  are  present  per  100  grams  of  solvent.  The  calculation 
in  the  opposite  direction  is,  of  course,  just  as  simple.  If  100  grams 
of  solvent  contain  25  grams  of  dissolved  compound,  then  100  +  25 
grams  of  solution  must  contain  25  grams  or  100  grams  of  saturated 
solution  contain  ^  X  100  =  20  grams  of  the  dissolved  compound. 

In  the  case  of  most  solubility  statements  contained  in  the  phar- 
maceutical literature,  the  results  are  given  in  terms  of  weight  or 
volume  of  solvent  required  to  dissolve  unit  weight  of  solid.  Since 
all  such  results  are  simply  the  reciprocal  of  the  terms,  grams  solid 
contained  in  unit  number  of  grams  of  solvent,  the  procedure  for 
transforming  them  to  the  more  usual  form  simply  involves  dividing 
I  gram  by  the  stated  number  of  grams  of  solvent.  In  <  those 
cases,  however,  where  the  amount  of  solvent  is  expressed  in  vol- 
ume instead  of  weight,  it  is  first  necessary  to  multiply  by  the 
specific  gravity  of  the  solvent  in  order  to  find  the  weight  corre- 
sponding to  the  given  volume. 

A  more  serious  complication  is,  however,  introduced  in  those 
cases  where  the  results  have  been  reported  only  in  terms  of  vol- 
ume of  the  saturated  solution  (100  cc.  or  I  liter).  On  account  of 
the  change  in  volume  which  always  results  when  a  solid  dissolves 
in  a  liquid,  a  calculation  of  the  weight  of  the  solvent  present, 
when  only  the  weight  of  the  dissolved  compound  and  total  volume 
of  the  solution  is  given,  cannot  be  made.  .  In  these  cases  it  is 
also  necessary  to  know  the  weight  of  a  unit  volume  of  the  satu- 
rated solution,  that  is,  its  specific  gravity,  in  order  to  convert 
the  results  from  the  volume  to  the  weight  basis.  Consequently, 
for  solubility  results  to  be  most  generally  useful,  the  specific  gravity 
of  the  saturated  solution  should  always  be  determined. 

The  calculation  of  a  given  result  from  the  volume  to  the  weight 
basis  or  vice  versa,  with  the  aid  of  the  specific  gravity  (density), 
is  readily  understood  when  it  is  remembered  that  this  factor  is 
simply  the  weight  in  grams  of  I  cc.  of  the  solution.  If,  for  example, 
it  is  stated  that  100  cc.  of  saturated  solution  contain  25  grams  of 
salt  and  the  specific  gravity  is  1.15,  it  is  apparent  that  115  grams 
of  the  solution  contain  25  grams  of  the  salt,  or  100  grams  contain 

— £-  =21.7    grams.     Conversely,    when    the    calculation    of    the 

amount  of  salt  in  100  cc.  from  that  in  100  grams  of  solution,  is  to 

xii 


GENERAL   INFORMATION 

be  made,  the  weight  of  dissolved  compound  must  be  multiplied 
by  the  specific  gravity. 

One  of  the  forms  of  presenting  solubility  data  for  which  especial 
care  is  needed  in  converting  the  values  to  a  different  basis  is  in 
the  case  of  results  for  salts  with  water  of  crystallization.  In  some 
instances  these  results  are  expressed  in  weight  of  the  hydrated 
compound  in  a  given  volume  or  weight  of  the  saturated  solution. 
If  it  is  desired  to  ascertain  the  weight  of  anhydrous  salt  present, 
it  will  be  necessary  first  to  calculate  the  grams  of  anhydrous  salt 
equivalent  to  the  stated  number  of  grams  of  the  hydrated  com- 
pound and,  if  the  results  have  been  expressed  in  terms  of  volume 
of  saturated  solution,  this  will  be  all  that  is  necessary,  but  if,  for 
instance,  the  grams  of  hydrated  salt  per  100  grams  of  saturated 
solution  or  of  water  have  been  given,  then  it  will  be  necessary  to 
add  the  weight  of  water  present  as  water  of  crystallization  in  the 
salt,  to  the  weight  of  water  present  as  solvent.  The  total  weight 
of  solvent  is,  therefore,  made  up  of  the  weight  of  water  used  for 
preparing  the  solution  and  that  carried  by  the  salt  as  t^O  of 
crystallization. 

In  the  case  of  solvents  composed  of  mixtures  of  water  and  alcohol, 
or  other  liquids,  authors  sometimes  fail  to  specify  whether  the 
figures  for  such  mixtures  refer  to  the  weight  or  volume  basis, 
consequently,  without  a  specific  gravity  determination,  the  exact 
composition  of  the  mixture  is  uncertain.  The  above  remarks  con- 
cerning the  calculation  of  solubility  results  from  one  form  to  another 
apply  equally  to  determinations  made  in  mixed  solvents,  provided 
all  supplementary  data  for  accurately  establishing  the  composition 
of  the  mixed  solvent  are  given. 

Although  in  most  cases  the  actual  experimental  results  of  solu- 
bility determinations  are  obtained  in  terms  of  weight,  many  investi- 
gators find  that  certain  advantages  are  to  be  gained,  in  particular 
problems,  by  converting  their  analytical  results  to  the  basis  of 
normality  or  gram  molecules,  and  in  practically  all  such  cases  it  is 
not  thought  necessary  to  present  also  the  gram  quantities  from 
which  the  molecular  values  were  calculated.  Although  this  may 
be  justified  from  the  narrow  point  of  view  of  the  particular  problem 
in  hand,  it  is  greatly  to  be  deplored  when  the  broader  aspects  of  the 
value  of  solubility  data  as  a  whole  are  considered.  As  already 
mentioned,  solubility  results  which  have  been  determined  for  some 
one  purpose  may  frequently  be  applied  to  the  solution  of  other 
problems,  or  serve  in  the  development  or  testing  of  generalizations 
or  of  laws  of  solution.  It  is,  therefore,  important  that  in  the  case  of 

xiii 


GENERAL   INFORMATION 

all  solubility  data  the  results  should  either  be  expressed  in  the 
gravimetric  terms  derived  most  directly  from  the  experimental  de- 
terminations, together  with  the  specific  gravities  of,  and  solid  phases 
in  contact  with  the  solutions,  or  else,  when  presented  in  terms  more 
or  less  remote  from  those  of  the  directly  determined  values,  the 
method  of  making  the  calculations  should  be  plainly  indicated  and 
all  factors  or  supplementary  data  which  have  been  used,  presented 
in  detail. 

In  preparing  the  present  compilation  occasion  was  several  times 
taken  to  write  to  authors  for  data  supplementary  to  those  published, 
which  although  not  essential  to  the  solution  of  the  particular  prob- 
lem in  hand,  and  therefore  omitted  from  the  paper,  were,  neverthe- 
less, needed  for  calculating  the  results  to  a  form  which  would  permit 
comparison  with  similar  data  by  others  or  their  use  in  the  solution 
of  other  problems. 

The  calculation  of  results  from  the  molecular  basis  to  the  gram 
basis  or  vice  versa,  introduces,  in  addition  to  the  errors  incidental 
to  the  calculation  itself,  those  resulting  from  the  selection  of  the 
atomic  or  molecular  weights  which  are  used  as  the  factors.  It  is 
indeed  rare  for  an  author  to  state  the  actual  molecular  weights  used 
for  a  calculation,  and  although  the  revisions  of  atomic  weights 
which  are  occasionally  made  are  usually  not  of  great  magnitude, 
opportunities  for  slight  differences  in  recalculating  results  to  a 
desired  basis,  due  to  differences  in  molecular  weights,  are  worthy  of 
consideration.  A  source  of  greater  inaccuracies,  however,  is  that 
resulting  from  the  failure  of  authors  to  differentiate  clearly  between 
the  significance  of  normality  (gram  equivalents)  and  gram  molecules 
(formula  weights)  in  calculating  or  in  expressing  their  results. 

It  also  occasionally  happens  that  the  compounds  involved  are  de- 
scribed only  by  names  which  are  not  specific  and  a  doubt  may  arise 
as  to  the  exact  formula  expressing  the  composition  of  the  compound 
in  question.  This  applies  particularly  to  work  described  in  lan- 
guages other  than  English.  In  cases  of  complex  mixtures  of  several 
salts  the  results  are  sometimes  given  in  terms  of  the  ions  present 
and  the  calculation  of  such  results  to  the  gram  basis  calls  for  especial 
care. 

The  general  procedure  for  calculating  gram  quantities  to  the 
molecular  basis  consists  simply  in  dividing  by  the  molecular  weight, 
or  molecular  equivalent  weight  in  the  case  of  results  to  be  expressed 
in  normality,  and  pointing  off  according  to  the  unit  quantity  of 
solution  selected.  The  reverse  calculation  is,  of  course,  made  by 
multiplying  the  molecular  or  normality  values  as  given,  by  the 

xiv 


GENERAL   INFORMATION 

molecular,  or  molecular  equivalent  weights.  An  example  which 
will  illustrate  the  principal  points  involved,  is  the  case  of  the  calcu- 
lation of  the  grams  of  dissolved  compound  per  100  grams  of  solvent, 
from  a  result  expressed  in  terms  of  molecular  per  cent,  that  is,  in 
terms  of  molecules  of  dissolved  compound  present  in  a  total  of  100 
molecules  of  dissolved  compound  plus  solvent.  Thus,  in  the  case 
of  the  solubility  of  mercuric  iodide  in  pyridine,  it  has  been  found 
that  the  saturated  solution  at  100°  contains  25  mol.  per  cent  HgI2, 
which  designates  a  mixture  of  25  gram  mols.  of  HgI2  and  100  —  25 
=  75  gram  mols.  of  pyridine.  To  convert  to  gram  quantities,  each 
figure  is  multiplied  by  the  respective  molecular  weight  and  the 
product  for  the  HgI2  divided  by  the  product  for  the  C5H5N.  Thus, 
(25  X  45445)  •*•  (75  X  79.08)  =  1.915,  which,  X  100,  =  191.5 
grams  HgI2  per  100  grams  of  C6H5N. 

Although,  in  the  present  compilation  an  attempt  has  been  made 
to  calculate  as  many  as  possible  of  the  data  to  terms  of  weight  of 
the  compounds  involved,  especially  for  the  commoner  substances, 
this  has  not  appeared  advisable  in  some  cases,  either  on  account  of 
uncertainties  as  to  the  factors  to  be  used,  or  on  account  of  the  rela- 
tive unimportance  of  the  data  and  the  considerable  labor  which 
would  have  been  involved  in  making  the  calculations. 

The  principal  terms  used  in  expressing  the  solubility  of  gases  in 
liquids  are  defined  in  connection  with  the  tables  of  data  in  the  body 
of  the  book.  See,  for  instance,  p.  227. 

Explanation  of  Tables.  —  Although  the  tables  of  results  contained 
in  the  present  volume  will,  it  is  hoped,  be  easily  understood  by  all 
who  are  familiar  with  the  subject,  for  the  benefit  of  those  who  need 
solubility  data  only  rarely,  it  has  appeared  desirable  to  mention 
some  of  the  principles  followed  in  constructing  the  tables  and  ex- 
plain in  detail  the  exact  meaning  of  the  results  contained  in  a  num- 
ber of  typical  tables. 

The  main  consideration  in  connection  with  a  compilation  such 
as  the  present  one,  is  to  arrange  the  very  large  amount  of  material 
in  the  most  concise  manner  compatible  with  perfect  clearness.  It 
has,  therefore,  been  necessary  to  adopt  forms  and  abbreviations 
which  eliminate  the  repetition  of  readily  understandable  details. 

In  general,  it  may  be  stated  that  the  record  of  a  solubility  de- 
termination consists  of  the  analytical  results  showing  the  composi- 
tion of  a  homogeneous  liquid  mixture  in  equilibrium  at  a  given 
temperature,  with  one  or  more  solid  compounds  or  with  another 
homogeneous  liquid  mixture.  In  the  case  of  aqueous  solutions  of 
salts,  for  instance,  the  analysis  will  show  the  weight  of  salt  and  of 

xv 


GENERAL  INFORMATION 

water  contained  in  a  given  amount  of  the  saturated  solution.  In 
recording  this  analysis,  however,  as  solubility  data,  it  is  not  cus- 
tomary to  state  the  weight  of  water  directly,  since  its  quantity  is 
derivable  from  the  given  weight  of  salt  and  of  solution  (salt  plus 
water).  Thus,  in  all  cases  the  amount  of  the  dissolved  compound 
is  numerically  reported  in  terms  of  unit  quantity  (100  grams,  one 
liter,  etc.)  of  the  saturated  solution  or  of  the  solvent.  The  tables, 
therefore,  all  show  in  the  heading  above  the  columns  of  figures,  the 
terms  in  which  the  results  are  expressed  (grams,  cubic  centimeters, 
gram  molecules,  etc.)  and  the  unit  quantity  of  solution  or  solvent 
in  which  the  numerically  recorded  amounts  of  dissolved  compound 
are  contained.  When  more  than  one  column  of  figures  are  inclosed 
under  a  bracket  below  the  heading,  the  arrangement  is  an  abbrevia- 
tion designed  to  eliminate  the  repetition  of  the  heading  over  each 
column  separately,  and,  therefore,  indicates  that  the  heading  applies 
independently  to  each  separate  column  of  figures.  Thus,  in  the 
case  of  the  table  showing  the  solubility  of  sodium  nitrate  in  water 
(see  p.  656)  the  heading  which  is  as  follows: 

Cms.  NaN03^per  100  Gms.  j^ols 

Solution.  Water.     '  per  Liter. 

o  42.2  72.9-73*  6.71* 

10  44.7  80.8-80.5  7.16 

when  translated  into  its  detailed  meaning  shows,  (i)  that  at  o°,  100 
grams  of  the  saturated  solution  of  sodium  nitrate  in  water  contain 
42.2  grams  NaNO3,  (2)  that  at  o°,  100  grams  of  water  dissolve  from 
72.9  to  73  grams  NaNOs  according  to  the  authorities  quoted 
(Mulder  or  Berkeley),  and  (3)  that  one  liter  of  a  saturated  solution 
of  sodium  nitrate  in  water  at  o°  contains  6.71  gram  molecules  of 
NaNO3. 

This  general  form  of  heading  is  typical  and  will  be  found  in  prac- 
tically all  cases  where  results  for  the  solubility  of  a  single  salt  in  a 
single  solvent  at  various  temperatures  are  given.  As  will  be  noted, 
tables  of  this  form  show  the  results  for  a  single  series  of  determina- 
tions at  increasing  temperatures  expressed  in  more  than  one  set  of 
terms.  As  a  general  rule,  and  especially  when  determinations  of 
the  specific  gravities  of  the  solutions  are  also  given,  any  one  of  the 
figures  for  a  given  temperature  may  be  calculated,  as  described  in 
the  previous  section,  from  either  of  the  others  at  the  same  tempera- 
ture. The  advantages  of  tables  giving  the  results  in  several  sets  of 
terms  are  that  the  reader  is  relieved  of  making  the  calculations 
individually. 

xvi 


GENERAL   INFORMATION 

In  a  number  of  cases  where,  either  the  importance  of  the  com- 
pound does  not  warrant  very  detailed  results,  or  where  similar  data 
for  several  near  related  compounds  have  been  determined,  com- 
posite tables  showing  the  results  for  two  or  more  compounds  in  one 
or  more  solvents  have  been  constructed.  Although  by  this  pro- 
cedure considerable  space  has  been  saved  and  frequent  repetitions 
avoided,  it  is  possible  that  clearness  has  sometimes  been  sacrificed. 

An  example  of  such  a  composite  table  is  that  for  the  three  com- 
pounds, CdI2.KI.H2O,  CdI2.2KI.2H2O  and  CdI2.2NaI.6H2O  given 
in  the  first  table  on  p.  178.  The  three  solvents  in  which  the 
solubilities  were  separately  determined  are  placed  in  the  first 
column  of  the  table.  Next  follow  the  results  for  CdI2.KI.H2O, 
given  in  terms  both  of  grams  of  anhydrous  salt,  CdI2.KI,  per  100 
grams  of  solution  and  per  100  grams  of  solvent.  The  next  group  of 
figures  shows  successively  the  solubility  of  CdI2.2KI.2H2O  in  water, 
in  absolute  alcohol  and  in  absolute  ether,  reported  in  each  case,  in 
terms  of  grams  of  anhydrous  salt  per  100  grams  of  saturated  solution 
and  also  in  grams  per  100  grams  of  each  solvent.  The  last  group  of 
figures,  columns  6  and  7,  gives  similar  results  for  CdI2.2NaI.6H2O. 

Other  examples  of  this  type  of  table  are  given  on  p.  188.  In 
these  cases  results  for  three  compounds,  each  in  the  same  solvent 
but  at  different  temperatures,  are  given.  The  abbreviation  here 
adopted  consists  in  providing  only  one  column  of  temperatures  to 
serve  for  each  of  the  three  sets  of  results  given  in  the  succeeding 
columns.  This  general  plan  is  followed  in  a  very  large  number  of 
cases  throughout  the  book. 

One  other  example  is  that  of  the  results  for  platinic  double 
chlorides,  given  in  the  first  table  on  p.  498.  In  this  case,  although 
each  column  of  results  represents  an  independent  series  of  solubili- 
ties in  water,  they  have  all  been  grouped  under  the  same  bracket, 
instead  of  each  being  given  under  a  separate,  complete  heading. 
By  this  plan  a  very  compact  arrangement  has  been  provided  but  the 
results  are  apt  to  be  misunderstood  unless  the  reader  bears  in  mind 
that  here  as  elsewhere  it  has  been  necessary  to  condense  the  data 
as  much  as  possible. 

Before  leaving  the  general  subject  of  composite  tables,  attention 
should  be  called  to  one  point  which  will  be  found  illustrated  in  a 
large  number  of  them.  This  is  in  reference  to  results  at  other  tem- 
peratures than  those  which  apply  to  the  table  as  a  whole,  as  recorded 
in  the  first  column  under  the  designation  t°.  In  these  cases  the 
figure  for  the  temperature  is  given  in  a  parenthesis  immediately 
following  the  result  for  grams  of  compound  dissolved  and,  of  course, 

xvii 


GENERAL  INFORMATION 

means  that  the  particular  determination  was  made  at  the  tem- 
perature stated  in  the  parenthesis,  instead  of  at  the  temperature 
shown  in  the  column  t°,  which  applies  to  all  the  results  not  so 
modified. 

This  principle  of  indicating  in  parentheses  any  variations  from 
the  general  order  of  the  table,  and  also  in  respect  to  the  introduction 
of  additional  matter,  such  as  results  for  densities,  points  on  the 
character  of  the  solutions,  etc.,  is  one  which  has  been  followed  in 
many  instances. 

As  already  stated,  a  solubility  is  an  expression  of  the  con- 
centration of  a  solution  in  equilibrium  with  a  particular  solid  com- 
pound. Therefore,  if  a  compound  can  exist  in  more  than  one  form 
at  a  given  temperature,  such  as  in  different  states  of  hydration,  its 
solubility  will  show  variations  in  accordance  with  which  one  of  its 
forms  is  in  contact  with  the  saturated  solution  at  the  particular 
temperature.  Information  in  regard  to  the  solid  phase  is,  conse- 
quently, essential  to  the  accurate  expression  of  a  solubility.  When- 
ever such  facts  are  available  they  are  shown  in  the  tables  by  means 
of  formulas  recorded  under  the  heading  "Solid  Phase."  These 
formulas  are  usually  placed  on  a  line  with  the  numerical  results  for 
the  solution  in  contact  with  the  solid  represented  by  the  formula 
given. 

A  case  which  illustrates  strikingly  the  multiplicity  of  variations 
in  solubility  with  change  in  degree  of  hydration  is  that  of  the  solu- 
bility of  the  hydrates  of  ferric  chloride  in  water  (see  p.  337).  In 
this  case,  to  economize  space,  the  formula  for  the  hydrate  has  been 
placed  immediately  above  that  group  of  data  to  which  each  refers, 
instead  of  on  the  same  line  with  the  results  for  each  solution  in 
contact  with  that  particular  hydrate.  An  examination  of  this  table 
will  show  the  apparent  anomaly  that  the  same  hydrate  possesses 
two  different  solubilities  at  certain  temperatures.  Thus,  in  the 
section  of  the  table  giving  results  for  solutions  in  contact  with  the 
solid  phase  Fe2Cl6.i2H2O,  it  will  be  noted  that  100  grams  of  H2O 
dissolve  106.8  grams  FeCla  at  30°  and  two  lines  below,  the  same 
amount  of  water  is  stated  to  dissolve  201.7  grams  FeCl3  at  30°. 
This  is  due  to  the  fact  that  each  of  the  hydrates  gives  a  more  or  less 
well  developed  reverse  solubility  curve.  The  character  of  these 
curves  is  plainly  indicated  by  plotting  them  on  cross-section  paper 
from  the  results  given  in  the  table.  If  this  is  done  it  will  be  seen 
that  in  case  of  the  results  for  Fe2Cl6.i2H2O,  the  grams  of  FeCl3  con- 
tained in  100  grams  of  water  increase  regularly  with  rise  of  tem- 
perature up  to  37°,  which  is  the  melting-point  of  this  hydrate.  If 

xviii 


GENERAL   INFORMATION 

more  crystals  are  added  and  the  temperature  raised  above  37°,  they 
melt  and  form  a  homogeneous  solution  of  increased  concentration. 
K,  however,  this  more  concentrated  solution  is  cooled  again  below 
37°,  and  crystals  then  added,  they  remain  as  solid  phase  and,  when 
equilibrium  is  established,  the  composition  of  the  solution  corre- 
sponds to  a  point  on  the  upper,  reverse  arm,  of  the  solubility  curve. 
With  this  salt,  therefore,  it  is  seen  that  for  certain  ranges  of  tem- 
perature the  concentration  of  the  saturated  solution  depends  upon 
the  procedure  by  which  the  point  of  equilibrium  has  been  ap- 
proached. 

In  cases  where  results  are  given  for  the  solubility  of  a  particular 
compound  in  aqueous  solutions  of  another,  the  heading  above  the 
columns  of  figures  shows,  as  usual,  the  terms  in  which  the  results 
are  expressed  (gms.,  cc.,  mols.,  etc.)  and  the  unit  amount  of  solution 
or  solvent  in  which  the  recorded  amounts  of  each  compound  is  con- 
tained; while  below  the  bracket  are  given,  at  the  heads  of  the 
columns,  the  formulas  of  the  respective  compounds  simultaneously 
present  in  the  solution.  Thus,  there  will  usually  be  found  in  one 
column,  the  increasing  concentrations  of  the  salt  present  in  the 
aqueous  solution  constituting  the  solvent,  and  in  the  other  the 
amounts  of  the  other  compound  of  which  the  solubility  is  being  de- 
termined and  which  is  present  as  solid  phase  in  contact  with  the 
solution.  Examples  of  this  form  of  table  are  those  for  the  solubility 
of  calcium  sulfate  in  aqueous  salt  solutions  (pp.  215  to  219)  and 
numerous  others  throughout  the  book.  In  all  cases  where  the  solid 
phase  exists  in  more  than  one  form,  this  information,  when  available, 
is  recorded  in  the  usual  manner  in  the  column  under  the  heading 
"Solid  Phase."  (See  pp.  174,  185,  203,  404,  and  many  others.) 
The  results  for  the  specific  gravities  of  the  saturated  solutions  are 
also  given,  when  available.  It  is  needless  to  say  that,  according  to 
the  arrangement  of  these  tables,  the  figures  in  the  horizontal  lines 
refer  to  the  same  solution  and  those  in  the  vertical  columns  to  dif- 
ferent solutions  of  the  series. 

In  the  case  of  tables  showing  the  distribution  of  a  compound 
between  two  immiscible  solvents  (see  for  example,  results  for  mer- 
curic chloride,  pp.  420  and  421),  the  amounts  of  the  dissolved  com- 
pound in  the  conjugate  layers  are  given  under  the  same  bracket 
with  column  headings  designating  the  respective  layers.  In  the 
case  of  equilibria  in  ternary  systems,  which  form  two  liquid  layers 
(see  for  example,  last  table,  p.  511),  the  compositions  of  the  upper 
and  lower  layers  are  given  under  separate  brackets,  the  results  on 
each  horizontal  line  being  for  layers  in  contact  with  each  other. 

xix 


GENERAL  INFORMATION 

Data  of  this  character  are  described  more  fully  in  the  chapter  on 
Methods  for  the  Determination  of  Solubility. 

The  types  of  cases  which  have  just  been  described  were  pointed 
out  by  users  of  the  first  edition  of  the  book  who  did  not  understand 
the  arrangement  in  these  cases  and  suggested  that  an  explicit  de- 
scription of  them  would  make  the  book  more  generally  useful.  It 
is  realized  that  the  explanations  which  have  been  given  here  apply 
only  to  a  certain  proportion  of  the  tables  in  the  book.  There  are, 
no  doubt,  many  tables  and  forms  of  expression,  especially  for  the 
more  complex  systems,  which  will  not  be  understood  by  the  casual 
reader.  In  some  of  these  cases  brief  remarks  in  connection  with 
the  tables  have  been  given,  but  to  just  what  extent  these  explanatory 
remarks  are  warranted,  it  has  been  difficult  to  decide.  In  conclu- 
sion, it  should  be  mentioned  that  the  title  of  the  table  is  intended 
to  describe  the  nature  of  the  results  and  should  always  be  used  as  a 
guide  in  the  interpretation  of  the  tabular  arrangement. 


xx 


ABBREVIATIONS 


Most  of  the  following  abbreviations  will  be  found  written  both  with  capitals 


and  without. 

WD-  —  Specific  Rotation. 

abs.  —  Absolute. 

abs.  coef .  —  Absorption  Coefficient. 

alcohol.  —  Ethyl  Alcohol. 

amt(s).  —  Amount  (s). 

anhy.  —  Anhydrous. 

aq.  —  Aqueous. 

atm(s).  —  Atmosphere(s). 

at.  wt.  —  Atomic  Weight. 

b.-pt.  —  Boiling-point. 

C.  —  Centigrade. 

calc.  —  Calculate  (ed). 

cc.  —  Cubic  Centimeter  (s). 

cm.  —  Centimeter  (s). 

coef.  —  Coefficient. 

com.  —  Commercial. 

compd.  —  Compound. 

cone.  —  Concentration,  Concentrated. 

cond.  —  Conductivity. 

const.  —  Constant. 

cor.  —  Corrected. 

crit.  —  Critical. 

cryo.  —  Cryohydric. 

cryst.  —  Crystalline. 

d.  —  Dextro  (in  connection  with  the 
name  of  an  optically  active  com- 
pound). 

d.  —  Density  (dis  —  Specific  Gravity 
at  1 8°,  referred  to  water  at  4°;  d^ 
at  20°  referred  to  water  at  20°), 

decomp.  —  Decomposition. 

dif.  —  Different. 

dil.  —  Dilute. 

dist.   coef.  —  Distribution   Coefficient. 

ed.  —  Edition. 

elec.  —  Electric  (al). 

equil.  —  Equilibrium. 

equiv.  —  Equivalent  (s). 

eutec.  —  Eutectic. 

F.  —  Fahrenheit. 

f.-pt.  —  Freezing-point. 


g.,  gm.,  gms.  —  Gram(s). 

gm.  mol.  —  Gram  Molecule  (s). 

G.  M.  —  Gram  Molecule  (s). 

hr(s).  —  Hour(s). 

i.  —  (d  +  /)    Inactive    (in    connection 

with  the  name  of  an  optically  active 

compound.) 
inorg.  —  Inorganic, 
insol.  —  Insoluble. 
/.  —  Laevo    (in    connection    with    the 

name  of  an  optically  active  com- 

poun4). 

kg.  kgm.  —  Kilogram  (s). 
1.  —  Liter(s). 
mm.  —  Millimeter  (s) 
m.  —  Meta. 
max.  —  Maximum, 
mg.,  mgm.  —  Milligram(s). 
mol(s).  —  Molecule(s),  Molecular, 
mol.  wt.  —  Molecular  Weight, 
millimol.  —  Milligram  Molecule, 
m.-pt.  —  Melting-point. 
n.  —  Normal  (gm.  equiv.  per  1.). 
N.  —  Normal  (used  rarely). 
o.  —  Ortho. 
ord.  —  Ordinary, 
org.  —  Organic, 
p.  —  Page. 
p.  —  Para, 
pet.  —  Petroleum, 
ppt.  —  Precipitate, 
pt.  —  Point. 

quad.  pt.  —  Quadruple  Point, 
qual.  —  Qualitative, 
sapon.  —  Saponification. 
sat.  —  Saturated, 
sol(s).  —  Solution  (s). 
sp.  gr.  —  Specific  Gravity  (Density), 
sq.  cm.  —  Square  Centimeter. 
s.  —  Symmetrical, 
sym.  —  Symmetrical. 


xxi 


ABBREVIATIONS 

fc°.  —  Temperature,  Centigrade-  Scale.  wt.  —  Weight. 

temp(s).  —  Temperature  (s).  oo  —  Infinity. 

tr.pt.  —  Transition  Point.  .lo"2,    .io~5,   etc.,   following  a  result 

vol(s).  —  Volume  (s).  means  that  the  decimal  point  is  to  be 

undissoc.  —  Undissociated.  moved  as  many  places  to  the  left  as 

U.  S.  P.  —  U.  S.  Pharmacopoeia,  indicated  by  the  minus  exponent. 


XXll 


ACENAPHTHENE  C12Hi0. 

SOLUBILITY  IN  SEVERAL  ORGANIC  SOLVENTS. 

(Speyers  —  Am.  J.  Sci.  [4]  14,  294,  1902.) 

NOTE.  —  In  the  original  paper  the  results  are  given  in  terms  of  gram  mole- 
cules of  acenaphthene,  acetamide,  acetanilide,  etc.,  per  100  gram  molecules  of 
solvent,  at  temperatures  which  varied  with  each  solvent  and  with  each  weigh- 
ing of  the  solutions.  The  tabulated  results  here  given  were  obtained  by  re- 
calculating and  reading  the  figures  from  curves  plotted  on  cross-section  paper. 

In  Methyl  Alcohol.  In  Ethyl  Alcohol.  In  Propyl  Alcohol. 


t  °.        (a) 

(ft) 

(c) 

(a) 

(ft) 

(c)   • 

"(a) 

(ft) 

(0    " 

0 

81 

•33 

I 

.80    o 

•39 

81.1 

1.9 

0.57 

82.3 

2.26 

0.88 

10 

80 

.40 

I 

.70    o 

•38 

80.3 

2.8 

0.84 

8l.8 

2.40 

i  .00 

2O 

79.60 

2 

.25     o 

.48 

79.6 

4.0 

1.20 

81.4 

3-40 

!-35 

30 

79 

.00 

3 

.50     o 

.72 

79.1 

5-6 

1.70 

80.9 

4-75 

i  .90 

40 

78 

•45 

6 

.00       I 

.20 

78.7 

8.4 

2.6o 

80.6 

7.10 

2.90 

50 

78 

•15 

9 

.00       I 

•77 

78.8 

13.2 

3-90 

80.7 

II.  10 

4.40 

60 

78 

•30 

ii 

.70      2 

•35 

79-4 

23.2 

7.00 

81  .5 

19.60 

8.20 

70 

78 

.60 

14 

.30       2 

.90 

80.75 

40-5 

12.50 

83-9 

37.00 

16.20 

In  Chloroform. 

In  Toluene. 

t  °. 

(a) 

(ft) 

(c) 

<«) 

(ft) 

(c) 

0 

143-8 

16. 

4     12-7 

90.7 

I3.I8 

7-9 

10 

I40.I 

20. 

6     16.0 

90.8 

18.0 

10.7 

20 

I36-3 

27. 

o     19.5 

91.0 

24-5 

14-5 

30 

132.4 

34- 

o     25  .0 

91.8 

33-5 

20.5 

40 

128.0 

42. 

5     32-0 

92-7 

47.0 

28.0 

50 

123.4 

Si- 

5    40.0 

94.0 

60.5 

35-7 

60 

119.3 

62. 

5    5°-° 

95-5 

74.0 

43-5 

70 

. 

97.2 

89.0 

52-5 

(a)  Weight  of  100  cc.  solution  in  grams.  (b)  Grams  dissolved  substance  per  100  grams  solvent. 

(c)  Gram  molecules  of  dissolved  substance  per  100  gram  molecules  of  solvent. 

looo  gms.  Aq.  25%  NH3  dissolve  0.07  gm.  acenaphthene  at  25°.     (Hilpert,  1916). 


RECIPROCAL  SOLUBILITIES  DETERMINED  BY  THE  METHOD  OF  LOWERING  OF  THE 
FREEZING-POINT  *  ARE  GIVEN  BY  GIUA  (1915),  FOR  THE  FOLLOWING  PAIRS 
OF  COMPOUNDS: 

Acenaphthene  +  m  Dinitrobenzene. 
+  2.4  Dinitrotoluene. 
"  +  a.  Trinitrotoluene. 


•  Freezing  or  Melting-point  Curves  as  Solubility  Data.  —  When  a  mixture  of  two  compounds,  rendered 
liquid  by  elevation  of  temperature,  is  gradually  cooled,  a  point  will  be  reached  at  which  one  or  the  other 
of  the  constituents  will  separate  as  a  solid.  This  point  represents  the  solubility  of  the  one  compound  in 
the  other.  The  method  involved,  differs  principally  from  that  ordinarily  employed  for  solubility  de- 
terminations, in  that  the  composition  of  the  mixture  remains  constant  while  the  saturation  tempera- 
ture is  being  approached,  instead  of  the  reverse  procedure. 

A  considerable  amount  of  data  of  this  character  is  available,  but,  after  careful  consideration,  it  has 
been  decided  that  references  only  will  be  given  to  it  in  the  present  volume,  except  in  cases  of  mixtures 
of  well-known  compounds  or  of  those  in  which  water  is  one  of  the  constituents. 


RECIPROCAL  SOLUBILITIES  (Freezing-point  Lowering  Data,  see  footnote,  page  i ) 
ARE  GIVEN  FOR  THE  FOLLOWING  PAIRS  OF  COMPOUNDS: 


Acenaphthene  +  Chloroacenaphthene 
-j-  Bromoacenaphthene 
"  -|-  lodoacenaphthene 

+  Benzil 

-j-  p  Nitrobenzoic  Aldehyde 
"  +  Piperonilic  Aldehyde 

+  Vanillic  Aldehyde 
Chloroacenaphthene  +  Bromoacenaphthene 

+  lodoacenaphthene 
Bromoacenaphthene  -j-     " 


(Crompton  and  Walker,  1912.) 


(Pawlewski,  1893.) 
(Fazi,  1916.) 


(Crompton  and  Walker,  1912.) 


ACETALDEHYDE  CH3COH. 

SOLUBILITY  IN  ETHYL  ALCOHOL  DETERMINED  BY  THE  METHOD  OF  LOWERING 
•OF  FREEZING-POINT  (de  Leeuw,  1911).  Liquid  air  was  used  as  the  cooling 
medium  and  temperatures  were  measured  with  the  aid  of  a  specially  con- 
structed resistance  thermometer. 


-123-3 

-125.4 

—  127.6 

-132 

-126 

-126 

-124.3 

-123.5 


Wt. 
Per  Cent 
CH3COH 
in 
Mixture. 

Mol. 
Per  Cent 
CH3COH 
in 
Mixture. 

100 

ICO 

90.7 

84.5 
80.9 
78.1 

90.3 
83-9 
80.2 

77-3  ' 

75-2 
67.0 
60.8 

74-4 
66.0 

59-7 

Solid  Phase. 


r. 


CH3COH         —122.3 

-I25-3 
-128 

(Eutectic)         —123.2- 
77.3  CH3COH.C2H5OH  —126.8 
-130.6 
—  120.6 
-II4.9 


Wt.  Mol. 

Per  Cent  Per  Cent 

CH3COH  CH3COH      Solid  Phase. 

in  in 

Mixture.  Mixture. 

51.8  50.7  CH3COH.C2H5OH 

45-6  44-5 

40.6-  39.5  CH3COH.2C2H5OH 

35-3  34-3 

30.2  29.3 

17.9  17.3  C2H6OH 
10.2            Q.8 

o.o        o.o 


Freezing-point  data  for  mixtures  of  acetaldehyde  and  paraldehyde  as  well 
as  the  complete  x  —  T  diagrams  are  given  by  Holleman  (1903).  Results  for 
mixtures  of  paraldehyde  and  p  xylene  are  given  by  Paterno  and  Ampola  (1897). 

Results  for  mixtures  of  the  a  and  /3  forms  of  Acetaldehyde  phenyl  hydrazone 
are  given  by  Laws  and  Sidgwick  (1911). 

AOETAMIDE     CH3CO.NH2. 

SOLUBILITY  IN  WATER  AND  IN  ALCOHOL. 

(Speyers.) 


In  Water. 


In  Ethyl  Alcohol. 


t°. 

(«0 

(ft) 

(c) 

'  (a) 

(ft)    («)" 

0 

105 

•5 

70 

.8 

29 

.6 

85 

.62 

J7 

•3 

18.5 

10 

104 

•9 

81 

.0 

34 

•  o 

86 

.2 

24 

.0 

26.0 

20 

104 

•3 

97 

•5 

40 

.8 

87 

3 

31 

.5 

33-8 

30 

103 

•7 

114 

.0 

47 

•7 

88 

.8 

40 

•5 

43-0 

40 

103 

.0 

133 

.0 

55 

•5 

90 

•7 

5o 

.0 

S3  -5 

50 

102 

•3 

154 

.0 

64 

.0 

93 

.0 

61 

.0 

60 

101 

.6 

177 

•5 

74 

•  0 

95 

5 

72 

•  o 

76S 

1  (a)  Wt.  of  100  cc.  sat.  solution  in  gms. 
Acetamide  per  100  gm.  mols.  solvent. 

100  gms.  pyridine  dissolve  17.75  gms.  acetamide  at  20-25°;  Io°  gms.  aq.  50  per 
cent  pyridine  dissolve  84.7  gms.  acetamide  at  20-25°.  (Dehn,  1917.) 

Freezing-point  curves  are  given  for:  Acetamide  +  Benzene  (Moles  and 
Jimeno,  1913);  Acetamide  +  Phthalide  (Lautz,  1913);  Acetamide  +  Triphenyl 
guanidine  (Lautz,  1913);  Tribromoacetamide  +  Trichloroacetamide  (Kiister, 
1891). 


ACETANILIDE 


ACETANILIDE  C6H6NH.COCH3. 

SOLUBILITY  IN  SEVERAL  SOLVENTS. 


Solvent. 


Water 


Ether 

Formic  Acid  (95%) 

Acetic  Acid  (99.5%) 

Acetone 

Amyl  Acetate 

Amyl  Alcohol 

Aniline 

Benzene 

Benzaldehyde 

Toluene 

Xylene 

Pyridine 

50%  Aq.  Pyridine 

Petroleum  Ether 


i6 

25 
30 
25 

21-5 
30^31 

25 
30-31 


25 

32.5 

20-25 

u 

about  20 


0-997 
i  .000 

1. 121 


O.9O2 
0.882 


1.034 

0-875 
1.068 
0.862 
0.847 


0-47 
0-54 
0.69 
2.8 

56.74 

33-21 

10.46 
14.00 
19.38 

2.46 
18.83 

0.50 

1.65 
32.7 
35-7 

0.03 


Authority. 

(Greenish  and  Smith,  1903.) 
(Holleman  and  Antush,  1894.) 

(Seidell,  1907.) 
(Marden  and  Dover,  1916.) 

(Aschan,  1913.) 

(Seidell,  1907.) 


(Dehn,  1917.) 


(Salkower,  19x6.) 


SOLUBILITY  IN  METHYL  ALCOHOL,  ETHYL  ALCOHOL  AND  IN  CHLOROFORM. 

(Speyers,  1902.)     See  Note,  page  i. 


In  CH3OH. 


O 

10 

20 

30 
40 

50 
60 


Sp.  Gr.  of 
Sat.  Solu- 
tion. 

0.860 
0.864 

0.875 
0.892 
O.9II 
0.932 
0.957 


Gms. 

C8H5NH.COCH, 
per  zoo  Gms. 
Sat.  Solution. 

18-5 
23.1 
29.1 

35-i 
42.9 

5!-7 
59-2 


In 

C2H5OH. 

Sp.  Gr.  of 

Sat.  Solu- 

Cms. 
C6H5NHCOCH3 
per  too  Gms. 

tion. 

Sat.  Solution. 

0.842 

12.8 

0.844 

16.7 

0.850 

21.3 

0.860 

26.5 

0.874 

32.9 

0.895 

39-4 

0.920 

46.4 

In  CHCV 

Sp.  Gr.  of 
Sat.  Solu- 
tion. 

Gms. 
CeHjNHCOCHa 
per  100  Gms. 
Sat.  Solution. 

I-503 

3-53 

1-475 

7.24 

1.440 

10.7 

1.398 

14-5 

1-354 

18.7 

1.3*4 

23-7 

1.272 

29.1 

SOLUBILITY  OF  ACETANILIDE  IN  MIXTURES  OF  ETHYL  ALCOHOL  AND  WATER. 


wt. 

nesuiis  at  25  .    \r\ 

Loiieman  ana  /wuusn,  1094.; 

K.CSUILS  at  j 

50  .     v^e'ueu,  1907.; 

lerCent 
:2H5OH  in 
Solvent. 

Sp.  Gr.  of  Sat. 
Solution. 

Gms.  C6H6NH.COCH3 
per  too  Gms.  Sat. 
Solution. 

Sp.  Gr.  of  Sat. 
Solution. 

Gms.  C6HSNH.GOCH, 
per  loo  Gms.  Sat. 
Solution. 

0 

0.997 

o-54 

I  .OOO 

0.69 

10 

0.985 

0-93 

0.984 

I.QD 

2O 

0-973 

1.28 

0.970 

2.20 

30 

0.962 

2.30 

0.956 

4.80 

40 

0.950 

4-85 

0-945 

9.40 

50 

0-939 

8.87 

Q-934 

15.40 

60 

0.928 

14.17 

0.926 

22.00 

70 

0.918 

19.84 

0.917 

27.60 

80 

0.907 

25-I7 

0.907 

31.20 

85 

0.899 

26.93 

0.900 

31.70 

00 

0.890 

27.65 

0-893 

51.60 

95 

0.874 

26.82 

0.885 

30.80 

IOO 

0.851 

24-77 

0.876 

29.OO 

(See  remarks  under  a  Acetnaphthalide,  page  13.) 


ACETANILIDE  4 

SOLUBILITY  OF  ACETANILIDE"  IN  MIXTURES  OF  ETHER  AND  CHLOROFORM  AND  OF 

ACETONE  AND   BENZENE  AT  25°.      (Marden  and  Dover,  1916.) 
Results  for  Ether-Chloroform  Mixtures.  •  Results  for  Acetone-Benzene  Mixture. 

Wt   Per  Cent  C  H           Gms'  C6H5NH.COCH3 
Wt.  .rer  l^ent  ^srls  __  /-• n/r:»«j 


Wt.  Per  Cent  CHC13 
in  Mixed  Solvent. 

Gms.  C6H5NH.COCH3 
per  100  Gms.  Mixed 
Solvent. 

100 

17.7 

90 

80 

II.7 
8.2 

70 
00 

6.2 

4-95 

50 
40 

4-25 
3-8 

30 

3-5 

20 

3-25 

10 

3-05 

0 

2.9 

100          1.36 

90        6.78 
•80         13.0 

70  20.0 

60  29.2 

50  30.0 

40  3°-5 

30         33-o 

20  36.0 

10  45-7 

o  '  39-4 

DISTRIBUTION  OF  ACETANILIDE  BETWEEN  IMMISCIBLE  SOLVENTS  AT  25°. 
Cone.  C6H5NH.COCH3  in  Benzene       layer  -f-  Cone,  in  H2O  layer  =  1.65. 

(Farmer  and  Warth,  1904.) 
"  Chloroform      "      -r-  Cone,  in  H2O  layer  =  7.75. 

(Marden,  1914.) 

"  Ether  "     -f-  Cone,  in  H2O  layer  =  2.98. 

(Marden,  1914.) 

SOLUBILITY  OF  HALOGEN  SUBSTITUTED  ACETANILIDES  IN  ETHYL  ALCOHOL  AT 
DIFFERENT  TEMPERATURES.    (Chattaway  and  Lambert,  1915.) 

Gms.  of  Each  Anilide  per  100  Gms.  of  Each  Sat.  Solution. 


t°. 

p  Chloro- 
acetanilide. 

2.4  Dichloro- 
acetanilide. 

p  Bromo- 
acetanilide. 

2.4  Dibromo- 
acetanilide. 

4  Chloro- 
2  Bromo- 
acetanilide. 

2  Chloro- 
4  Bromo- 
acetanilide. 

5 



4.244 

2.480 

.  .  . 

.  .  . 

10 

3.278 

3.008 

4.847 

2.876 

4-334 

2-575 

15 

3-777 

3-564 

5-56I 

3-382 

5.088 

2.961 

20 

4.366 

4.192 

6.390 

4.002 

5.986 

3.466 

25 

5.040 

4.962 

7.300 

4.714 

7-043 

4-095 

30 

5.828 

5.864 

8.440 

5-6I5 

8.328 

4.891 

35 

6.700 

6-937 

9-7I5 

6.686 

9.844 

5.820 

40 

7.728 

8.276 

11.156 

7.914 

11.586 

6.887 

45 

8.918 

9-750 

12.767 

9-357 

13.718 

8.186 

(Results  for  unstable  needle  forms  of  p  bromoacetanilide  and  2.4  dibromo- 
acetanilide  are  also  given.) 

SOLUBILITY  OF   p  NITROACETANILIDE  AND   OF  2.4  DICHLOROACETANILIDE  IN 

ACETIC  ACID  AT   l6°.      (Orton  and  King,  1911.) 
Compound.  Solvent.  <5SS£&SR 

p  Nitroacetanilide  Glacial  Acetic  Acid  o .  83 

50% Aq.    "  0.38 

2.4  Dichloroacetanilide         Glacial  Acetic  Acid  6.37 

50% Aq.    "  0.83 

Freezing-point  curves  (see  footnote,  page  i)  are  given  for  mixtures  of: 
Acetanilide  and  Antipyrine  (Comanducci,  1912.) 

'     m  Nitraniline '  (Crompton  and  Whiteley,  1895.) 

"    m  Dinitrobenzene  " 

'    a  Dinitrophenol 

"    p  Nitroacetanilide  (Kiister,  1891.) 

p  Nitroacetanilide  and  Dinitroacetanilide  (Holleman  and  Sluiter,  1906.) 

p  Bromoacetanilide  and  2.4  Dibromoacetanilide    (Sidgwick,  1915.) 


ACETIC  ACID 


ACETIC  ACID   CH3COOH. 

RECIPROCAL  SOLUBILITY  OF  ACETIC  ACID  AND  WATER  DETERMINED  BY  THE 

METHOD  OF  LOWERING 

OF   THE 

FREEZING-POINT 

. 

Gms.  CH3COOH 

Gms.  CH3COOH 

t°. 

per  100  Gms.         Solid  Phase. 
Sat.  Solution. 

t°. 

per  100  Gms. 
Sat.  Solution. 

Solid  Phase. 

o 

o                   Ice 

—  2O 

67.0 

CH3COOH 

-  5 

15-2 

—  15 

72.3 

" 

—  10 

28.5 

—  10 

77-5 

" 

"~I5 

40.0 

-  5 

82.2 

it 

—  20 

49.2 

0 

87.0 

it 

—  25 

K 

+  5 

91.8 

tt 

-26. 

7     60  .  o         (Eutectic) 

10 

95-8 

it 

-25 

62.5        CH3COOH 

16.6 

100.  0 

ft 

The  data  in  the  above  table  were  obtained  by  plotting  the  results  of  Pickering 
(1893),  Roloff  (1895),  Dahms  (1896)  (1899),  deCoppet  (1899),  Kremann  (1907), 
Faucon  (1910),  Ballo  (1910),  Groschuff  (1911),  Paterno  and  Salimei  (1913),  and 
Tsakalotos  (1914),  on  cross-section  paper  and  drawing  a  curve  through  the  points 
in  best  agreement.  In  addition  to  making  determinations  of  the  freezing-points 
of  the  mixtures,  Ballo  also  analyzed  the  solid  phases  which  separated,  and  snowed 
that  these  contained,  in  all  cases,  increasing  percentages  of  acid  and,  therefore, 
must  have  consisted  of  mixed  crystals.  This  formation  of  mixed  crystals  is 
offered  as  an  explanation  of  the  abnormality  of  the  freezing-point  lowering  of 
the  system. 

SOLUBILITY  OF  ACETIC  ACID   IN   ETHYL    ALCOHOL   (98.9%)   DETERMINED  BY 
THE  METHOD  OF  LOWERING  OF  FREEZING-POINT.    (Pickering,  1893.) 

Gms.  CH3COOH 


Gms.  CH3COOH 

t°. 

per  zoo  Gms. 
Sat.  Solution. 

Solid  Phase. 

-75 

26.O 

CH3COOH 

-70 

27.7 

tt 

-60 

33-o 

it 

-So 

38.2 

ft 

-40 

43-7 

tt 

-30 

50.2 

tt 

—  20 

58.0 

ft 

t°. 

per  too  Gms. 
Sat.  Solution. 

Solid  Phase. 

—  10 

67.7 

CH3COOH 

-  5 

73-2 

n 

0 

79.1 

tt 

+  s 

85.2 

tt 

10 

Qi-5 

ft 

15 

98.0 

tt 

16.6 

IOO.O 

tt 

(The  original  results  were  plotted  on  cross-section  paper  and  the  above  figures 
read  from  the  curve.) 

SOLUBILITY  DATA  DETERMINED  BY  THE  METHOD  OF  LOWERING  OF  THE  FREEZ- 
ING-POINT (see  footnote,  page  i)  ARE  GIVEN  FOR  MIXTURES  OF  Acetic  Acid 

AND   EACH   OF  THE   FOLLOWING   COMPOUNDS: 
Chloroacetic  Acid  (Mameli  and  Mannessier,     Dimethyl  pyrone  (Kendall,  1914  (a).) 


.  J9I3:  Kendall,  1914.) 
DlchloroacetlC  Add  (Kendall,  1914.) 

Tnchloroacetic  Acid  (Kendall,  1914.) 
Acetic  Anhydride  (Pickering,  1893.) 


Booge,  1916.) 

Benzene  +  Vaseline  (Roloff,  1895-) 
Benzene  +  Naphthalene  (Roloff,  1895.) 
Benzene  +  Water  (Roloff,  1895.) 
Benzoic  Acid  (Kendall,  1914.) 
Chlorobenzene  (Baud,  1913  (c).) 
Nitrobenzene  (Dahms,  1895;  Baud,  1913  (c).) 
Carbon  Disulfide  (Pickering,  1893.) 
Cyclohexane  (Baud,  1913  (a)  (6).) 


Dimethyl  Oxalate  (Kendall  and  Booge,  1916.) 
Dimethyl  Succinate  (Kendall  and  Booge,  19x6.) 

Eth  j  Ether  (Pickermg>  l893.} 

Ethylene  Bromide  (Dahms.tSgs;  Baud,  I9i2(a).) 
Ethylene  Dibromide  (Baud,  *'„  (>,) 
tormamide  (English  and  Turner,  1915.) 

Formic  Acid  (Baud,  1913  (c).) 
Methyl  Alcohol  (Pickering,  1893.) 
Picric  Acid  (Kendall,  1916.) 
Propyl  Alcohol  (Pickering,  1893.) 
Sulfuric  Acid  (Pickering,  1893.) 
Thymol  (Paterno  and  Ampola,  1897.) 
p  Xylene  (Paterno  and  Ampola,  1897.) 


ACETIC  ACID  6 

DISTRIBUTION  OF  ACETIC  ACID  BETWEEN: 

Water  and  Amyl  Alcohol  at  20°.  Water  and  Benzene  at  25°. 

(Herz  and  Fischer,  1904.)  (Herz  and  Fischer,  1905.) 

Cms.  CHaCOOH  G.  M.  CHaCOOH  Cms.  CH8COOH  G.  M.  CHaCOOH 

per  IPO  cc.  per  100  cc.  per  100  cc.  per  100  cc. 

H20    Alcoholic'  HsO '  Alcoholic"  H^O C6H6  '  TlzO C6H6     " 

Layer.      Layer.  Layer.  Layer.  Layer.       Layer.  Layer.        Layer. 

1  0.923  o-oi  0.0095  5  0.130  0.05  0.0014 

2  1.847  °-°3  0-0280  io  0.417  o.io  0.0005 

3  2.741  0.05  0-0460  20  i-55  0.20  0.0030 

4  3-694  0.07  0.0645  30  3-03  0.30  0.0290 

5  4-587  0.09  0.0830  40  4.95  0-50  0.051 

6  5-475  o-11  o.ioio  0.70  0.090 

7  6.434  0.13  0.1190 

8  7.328 

NOTE.  —  The  distribution  results  of  Herz  and  co-workers  are  reported  in 
millimolecules  per  io  cc.  portions  of  each  layer  in  the  several  cases.  To  obtain 
the  figures  given  in  the  tables  here  shown,  the  original  results,  before  and  after 
calculating  to  gram  quantities,  were  plotted  on  cross-section  paper,  and  from 
the  curves  thus  obtained,  readings  for  regular  intervals  of  concentration  of 
acetic  acid  in  the  aqueous  layer  were  selected. 

DISTRIBUTION  OF  ACETIC  ACID  BETWEEN  WATER  AND  BENZENE. 

(Waddell,  1898;  see  also  Lincoln,  1904.) 

The  measurements  were  made  by  adding  varying  amounts  of  benzene  or  water 
to  5  cc.  of  acetic  acid  and  then  running  in  water  or  benzene  till  saturation  was 
reached.  The  observed  readings  were  calculated  to  grams  per  100  grams  of  the 
liquid  mixture. 

Upper  Layer.  Lower  Layer. 

t°.        CHaCOOH.      C6H6.          5^6.  CHaCOOH.    CeH6.        H&T 

25          0.46      99-52     0.02  9.4      0.18    90.42 

25  3-10         96.75      0.15  28.2         0.53       71.27 

25  5.20  94-55  °-25  37-7  °-84  61.46 

25  8.7  90.88  0.42  48.3  1.82  49.88 

25  16.3  82.91  0.79  61.4  6.1  32.5 

25  30-5  67.37  2.13  66.0  13.8  20.2 

25  52-5  39-6o  7-60  52.8  39.6  7.6 

35  1.2  98.68  0.08  16.4  0.62  82.98 

35  5-7  93-97  °-33  36-8  1.42  62.78 

35  9-°  90.42  0.58  49 -o  2.10  48.90 

35  45.0  49-0°  6.0  61.3  25.5  13.2 

35  52-2  39.4  8.4  52.2  39.4  8.4 

Additional  data  in  connection  with  the  distribution  of  acetic  acid  between 
water  and  benzene  are  given  by  King  and  Narracutt  (1909),  Kuriloff  (1898), 
Farmer  (1903),  Bubanovic  (1913),  and  Lincoln  (1904).  This  latter  investigator 
points  out  that  the  same  degree  of  clouding  does  not  represent  the  end  point  in 
all  cases  as  was  assumed  by  Waddell  (1900). 

Data  for  the  distribution  of  acetic  acid  between  benzene  and  aqueous  solu- 
tions of  sodium  acetate  at  25°  are  given  by  Farmer  (1903). 


ACETIC  ACID 


DISTRIBUTION  OF  ACETIC  ACID  BETWEEN  WATER  AND  CHLOROFORM: 

At  Room  Temperature.  At  25°. 

(Wright,  Thomson  and  Leon  —  Proc.  Roy.  (Herz  and  Lewy;  Rothmund  and  Wilsmore.) 

Soc.  49»  185, 1891.) 


Results  in  parts  per  100  parts  of  solution. 
Upper  Layer.                           Lower  Layer. 

Cms.  CHaCOOH 
per  TOO  cc. 

G.  M.  CHgCOOH 

per  100  cc. 

CHaCOOH.  CHCla- 

H2O.    CHsCOOH 

.  CHC13. 

H20. 

H20 

Layer. 

CHC13 
Layer. 

H20 
Layer. 

CHCI; 

Layer. 

O 

0.84 

99 

.16 

o 

99.01 

0.99 

2 

o. 

089 

0.05 

0.0032 

6.46 

0.92 

92 

.62 

1.04 

98.24 

0.72 

4 

O. 

3i3 

0.075 

0.0062 

17.69 

0.79 

81 

•52 

3.83 

94.98 

I.I9 

6 

o. 

596 

0.100 

O.OIOO 

25.10 

I.  21 

73 

.69 

6.77 

91.85 

1.38 

8 

o. 

974 

0.150 

0.0198 

33  7i 

2-97 

63 

•32 

11.05 

87.82 

I-I3 

10 

I. 

43° 

0-175 

0.0260 

44.12 

7-30 

48 

•58 

17.72 

80.00 

2.28 

12 

I. 

982 

0.200 

0.0325 

50.18 

15.11 

34 

•7i 

25-75 

70.13 

4.12 

20 

5- 

10 

0.30 

0.070 

30 

10.2 

0.50 

O.I7O 

40 

15- 

3 

O.70 

0.275 

50 

21. 

9 

0.80 

o-335 

52-3 

39- 

54 

0.87 

0.659 

See  Note,  page  6. 

In  addition  to  the  above  results,  data  for  somewhat  lower  concentrations  of 
acetic  acid  determined  at  20°  are  given  by  Dawson  and  Grant  (1901). 

Results  showing  the  influence  of  electrolytes  upon  the  distribution  of  acetic 
acid  between  water  and  chloroform  are  given  by  Rothmund  and  Wilsmore  and 
by  Dawson  and  Grant. 

DISTRIBUTION  OF  ACETIC  ACID  AT  25°  BETWEEN: 


Water  and  Carbon  Disulphide. 

(Herz  and  Lewy.) 


Cms.  CHsCOOH 

G.  M.  CHsCOOH 

per  ipo  cc. 

per  100  cc. 

H20            CS2' 

H2O            CS2" 

Layer.        Layer. 

Layer.        Layer. 

65           2.64 

I.I         0-45 

7O           3-O 

1.2         0.55 

75        3-3 

1.2          0.80 

80        5.4 

i-35    0.97 

85        6.4 

1.4      1.3 

Water  and  Carbon  Tetrachloride. 

(Herz  and  Lewy.) 
Cms.  CH3COOH        G.  M.  CH3COOH 


per  IPO  cc. 


per  100  cc. 


H20 
Layer. 


30  1.8  0.5  0.03 

40  3.0  0.7  0.055 

50  4.8  0.9  0.095 

60  5.8  i.i  0.155 

7O  12. 0  1.2          0.235 

76.2       25.2  1.27       0.420 

Results  for  the  distribution  of  acetic  acid  between  water  and  mixtures  of 
equal  volumes  of  carbon  disulfide  and  carbon  tetrachloride  at  25°  are  given 
by  Herz  and  Kurzer  (1910)* 

DISTRIBUTION  OF  ACETIC  ACID  AT  25°  BETWEEN: 


ecu 

Layer. 


Water  and  Bromoform. 

(H.  and  L.  — Z.  electro.  Ch.  ix,  818,  '05.) 
Cms.  CHaCOOH        G.  M.  CHaCOOH 


Water  and  Toluene. 

(H.  and  F.  —  Ber.  38,  1140,  '05.) 
Cms.  CH3COOH        -G.  M.  CH3COOH 


per  100  cc. 


per  ipo  cc. 


H20 

Layer. 

CHBr3 
Layer. 

'H20 
Layer. 

CHBr3 
Layer. 

20 

I  .5 

0-4 

0-035 

30 

3-o 

0.6 

0.070 

40 

4-8 

0.8 

0.120 

50 

7.8 

i  -o 

O-2O 

60 

12.0 

i  .1 

0.28 

65 

I5.6 

1.15 

o-395 

70 

27.0 

per  ipo  cc. 


per  100  cc. 


H2O     C6H5CH3 
Layer.    Layer. 

H2O 
Layer. 

C6H5CH3 
Layer. 

5    Q-II9 

O.I 

0.0025 

10    0.328 

0.2 

0.0075 

20       I-I32 

0-4 

O.O26O 

30       2.265 

0.6 

0.0530 

40     3-725 

0.8 

0.090 

50     5.841 

i.o 

0.140 

60     8.344 

See  Note,  page  6. 


ACETIC  ACID  8 

DISTRIBUTION  OF  ACETIC  ACID  BETWEEN  WATER  AND  ETHYL  ETHER. 

(de  Kolossovsky,  1911.) 


Results  at  Several  Temperatures. 

Gms.  CH3COOH  per  100  cc.  of: 


H2O 

Ether 

P 

Layer  (p). 

Layer  (p'). 

P'' 

13 

0.365 

0.207 

I.76 

18 

0.367 

O.2OI 

1.82 

27 

0-379 

0.195 

1.94 

7-5 

0-799 

0.551 

I  .45 

12 

0.803 

0.529 

1.52 

18 

0.802 

0.501 

1.  60 

25 

0.789 

0.474 

1.66 

Results  at  18°. 

Gms.  CHgCOOH  per  100  cc.  of: 


H20 

Ether 

p 

Layer  (p). 

Layer  (p'). 

p'' 

1.0 

0.5               i 

l.O 

2.0 

1.0              J 

2.0 

4.0 

2.1                ] 

•9 

6.0 

3-5          3 

•7 

8.0 

4-9          J 

.6 

10.  0 

6.6 

•5 

15-0 

EX.4 

•3 

20.  o 

17.0 

.2 

25.0 

23-3         : 

[.07 

According  to  results  obtained  at  25°  by  Morgan  and  Benson  (1907),  the  ratio 
of  distribution  for  concentrations  of  acetic  acid  up  to  12  grams  per  100  cc.  of 
the  H2O  layer  is  more  nearly  constant  (1.92)  than  shown  above  for  18°.  A 
similar  constancy  of  distribution  (approx.  2.08  at  15°)  was  also  found  by  Pinnow 

(1915)- 

Results  showing  the  influence  of  varying  concentrations  of  a  large  number  of 
electrolytes  upon  the  distribution  of  acetic  acid  between  water  and  ether  are 
given  by  de  Kolossovsky,  Dubrisay  (1912),  and  by  Hantzsch  and  Vagt  (1901). 

Data  for  the  distribution  of  acetic  acid  between  ether  and  molten  CaCl2.6H2O 
and  ether  and  molten  LiNO33H2O  are  given  by  Morgan  and  Benson  (1907). 

One  determination  of  the  distribution  of  acetic  acid  between  sat.  aq.  CaCl2 
solution  (20  gms.  per  1.)  and  kerosene  gave  97.7  gms.  acid  per  100  gms.  aq.  layer 
and  27  gms.  per  100  gms.  kerosene  layer  at  ordinary  temperature.  (Crowell, 
1918.) 


DISTRIBUTION  OF  ACETIC 
Water  and  o  or  p  Xylene. 

(Herz  and  Fischer.) 


ACID  AT  25°  BETWEEN: 

Water  and  m  Xylene. 

(Herz  and  Fischer.) 


Gms.  CH3COOH 
per  100  cc. 

G, 

,  M.  CH3COOH 
per  100  cc. 

Gms.  CH3COOH 
per  100  cc. 

G 

.  M.  CH3COOH 

per  100  cc. 

IT  r»           o  or  p 

l52.       X*lene 
Layer. 

H20 
Layer. 

o  or  p                       TT  Q            m 
Xylene                     L  vr  X^ene 
Layer.                          y    '  Layer. 

H2O 
Layer 

m 
Xylene 
Layer. 

C                  O 

.24 

O 

.1 

O 

.004 

5 

0 

.06 

0 

.1 

0.0015 

IO              O 

.48  , 

0 

.2 

0 

.010 

IO 

0 

•30 

0 

.2 

O.OO7 

20               I 

.13 

O 

•4 

0 

.025 

20 

0 

•95 

O 

•4 

O-O22 

30               2 

mI5 

o 

.6 

0 

.047 

30 

I 

.91 

o 

.6 

0.042 

40          3 

.40 

o 

.8 

0 

.079 

40 

3 

.04 

o 

.8 

0.072 

50          5 

.10 

I 

.0 

0 

.122 

50 

4 

•65 

I 

.0 

O.III 

60          7 

.27 

I 

.2 

0 

.230 

60 

6 

•65 

I 

.2 

... 

70            12 

•52 

»• 

See  Note,  page  6. 

Data  showing  effect  of  camphor  on  the  reciprocal  solubility  of  acetic  acid  and 
olive  oil  are  given  by  Wingard,  1917. 


ChloroACETIC  ACIDS 


ChloroACETIC  ACIDS   CH2C1COOH,  CHC12COOH,  and  CCUCOOH. 

SOLUBILITY  OF  THE  a,  ft,  AND  7  MODIFICATION  OF  MONOCHLORO  ACETIC  Aero 
IN  WATER  AT  DIFFERENT  TEMPERATURES. 

(Miers  and  Isaac,  1908;  Pickering,  1895.) 

The  determinations  were  made  by  the  sealed  tube  method.     The  following 
figures  were  obtained  by  plotting  the  original  results  on  cross-section  paper: 


Cms.  per  100  Gms.  of  Each  Sat. 
Solution. 


Gms.  per  100  Gms.  of  Each  Sat. 
Solution. 


a  'Modifi- 

/3 Modifi- 

7 Modifi- 

t . 

cation. 

cation. 

cation. 

20 

... 

.  .  . 

88.0 

25 

.  .  . 

85.8 

90.0 

30 

86.0 

88.2 

92.2 

35 

88.4 

90.6 

94.1 

40 

90.8 

93-9 

95-8 

45 

93-o 

95-o 

97.8 

*o                                 a  Modifi- 

0 Modifi- 

•y Modifi- 

cation. 

cation. 

cation. 

50 

95 

.0 

97 

.0 

99 

.6 

51 

(m.  pt.) 

. 

.; 

100 

.0 

55 

97 

.2 

99 

•  3 

.•  t 

. 

56 

.5  (m.pt.) 

, 

too 

.0 

. 

60 

99 

.0 

t 

. 

62 

.4  (m.  pt.) 

0:00 

.0 

.  . 

.  . 

,  . 

,  • 

Reciprocal  solubilities  of  mono-,  di-,  and  trichloroacetic  acids  and  water  de- 
termined by  the  freezing-point  method  are  given  by  Pickering  (1895). 


SOLUBILITY  OF  TRICHLQROACETIC  ACID  IN  WATER  AT  25°. 

(Seidell,  1910.) 

100  gms.  saturated  solution  of  d&  =  1.615  contain  92.32  gms.  GC13.COOH. 


SOLUBILITY  DATA  DETERMINED  BY  THE  METHOD  OF  LOWERING  OF  THE  FREEZ- 
ING-POINT (see  footnote,  page  i)  ARE  GIVEN  FOR  MIXTURES  OF  Chloro- 
acetic  Acid  AND  EACH  OF  THE  FOLLOWING  COMPOUNDS: 


Dichloroacetic  Acid  (Kendall,  1914.) 
Trichloroacetic  Acid  (Kendall,  1914.) 

Acetophenone  (Kendall  and  Gibbons, 
Dibenzyl  Acetone  (Kendall  and  Gibbons,  1915.) 
Benzil  (Kendall  and  Gibbons,  1915.) 
Benzene  (Kendall  and  Booge,  1916.) 
Benzoic  Acid  (Kendall,  1914.) 

Camphor  (Pawlewski,  1893.) 

Cinnamic  Acid  (Kendall,  1914.) 

Crotonic  Acid 

Cetyl  Alcohol  (Mameli  and  Mannessier,  1913.) 

0  Cresol  (Kendall,  1914.) 

Methyl  Cinnamate  (Kendall and  Booge,  1916). 


Dimethyl  Oxalate  (Kendall  and  Booge,  1916.) 

Dimethyl  Succinate  (Kendalland  Booge,  1916.) 

Dimethylpyrone  (Kendall,  1914  (a).) 

Naphthalene  (Miers  &  Isaac,  1908;  M.  &  M.,i9i3.) 

Phenol  (Kendall,  1916.) 

Piperonal  (Kendall &Gibbons,  I9IS;M.&M.,I9I3.) 

Salol  (Mameli  and  Mannessier,  1913.) 

Sulfuric  Acid  (Kendall  and  Carpenter,  1914.) 

0   Toluic  Acid  (Kendall,  1914.) 

m      " 

p       "         " 

a       " 

Vanillin  (Kendall  and  Gibbons,  1915.) 


SOLUBILITY  DATA  DETERMINED  BY  THE  METHOD  OF  LOWERING  OF  THE  FREEZ- 
ING-POINT (see  footnote,  page  i)  ARE  GIVEN  BY  KENDALL  (1914)  FOR  MIX- 
TURES OF  Dichloroacetic  Acid  AND  EACH  OF  THE  FOLLOWING  COMPOUNDS: 


Trichloroacetic  Acid 
Benzoic  Acid 
Cinnamic  Acid 
Crotonic  Acid 
Dimethylpyrone 


o  Toluic  Acid 
m      " 
p      "         " 
a      " 


(Phenylacetic  Acid) 


ChloroACETIC  ACID 


10 


SOLUBILITY  DATA  DETERMINED  BY  THE  METHOD  OF  LOWERING  OF  THE  FREEZ- 
ING-POINT (see  footnote,  page  i)  ARE  GIVEN  FOR  MIXTURES  OF  Trichloro- 
acetic  Acid  AND  EACH  OF  THE  FOLLOWING  COMPOUNDS: 


(Kendall  and 

Gibbons, 

I9IS-) 


AcetOphenone  (Kendall  and  Gibbons,  1915.) 
Anisaldehyde 

Benzene  (Kendall  and  Booge,  1916.) 

Benzaldehyde  (Kendall  and  Gibbons,  1915.) 

m  Hydroxy  Benzaldehyde 

p         " 

o  Nitro  Benzaldehyde 

m     " 

p      " 

Benzophenone 

Benzil ' 

Benzoquinone 

Benzoic  Acid  (Kendall,  1914.) 

Camphene  (Timofeiew  &  Kravtzov,  1915, 1917.) 
Cinnamic  Acid  (Kendall,  1914.) 
Crotonic  Acid 
0    Cresol  (Kendall,  1914.) 


Diethyl  Oxalate      (Kendall  and  Booge,  1916.) 

Diethyl  Succinate 

Dimethyl  Oxalate 

Dimethyl  Malonate 

Dimethyl  Succinate 

Dimethyl  Terephthalate       (Kendall  and 

Booge,  1916.) 

Dimethylpyrone   (Plotnikov,  1911;  Kendall, 
1914  (o)-) 


Ethyl  Ether  (Tsakalotos  and  Guye,  1910.) 
Ethyl  Acetate       (Kendall  and  Booge,  1916.) 
Ethyl  Benzoate  "  " 

Methyl  Benzoate 
Anisate 

"       Cinnamate     "  " 

"       />Toluate 
a  Naphthol  (Kendall,  1916.) 
0         " 
a  Naphthyl  Acetate  (Kendall  and  Booge,  1916.) 

a  «  «  (( 

P 

Phenol  (Kendall,  1916.) 

o  Nitro  Phenol  (Kendall,  1916.) 

m     " 

p      "          " 

Piperonal  (Kendall  and  Gibbons,  1915.) 

Nitro  Piperonal 

Phenyl  Anisylketone  " 

"        Benzoate  (Kendall  and  Booge,  1916.) 
"       Salicylate          "  " 

Salicylic  Aldehyde  (Kendall  and  Gibbons.igis.) 

Sulfuric  Acid  (Kendall  and  Carpenter,  1914.) 

0  Toluic  Acid  (Kendall,  1914.) 

m     " 

p      "        " 

a        "          "  " 

Thymol  (Kendall,  1916.) 
Vanillin  (Kendall  and  Gibbons,  1915.) 


DISTRIBUTION  OF  CHLORACETIC  ACID  BETWEEN: 

(Herz  and  Fischer.) 


Water  and  Benzene  at  25°. 


Water  and  Toluene  at  25°. 


Cms.  CH2C1COOH 

G.  M.  CH2C1COOH 

Cms.  CH2C1COOH 

G.  M.  CH2C1COOH 

per  zoo  cc. 

per  i  po  cc. 

per  100  cc. 

per  100  cc. 

HaO           C*He' 
Layer.        Layer. 

Layer.          Layer. 

H20        QHsCfta 
Layer.        Layer. 

620        CeHsCHs 
Layer.          Layer. 

0.25*     8.69 

O.OO25      0.090 

o.i*      5.22 

o.ooi     0.055 

o-S      15-59 

O.OO5         0.155 

0-5         20.31 

O.OO5      O.2O 

1.0      27.87 

o.oio      0.28 

i.o       34.87 

o.oio    0.36 

1.5      41.10 

0.015        0.415 

1-5         49.14 

O.OI5      0.50 

2.0         52.90 

O.O2           0-54 

2.O         60.46 

O.O2         O.62 

3.0      68.01 

O.O3           0.70 

3-0         72.28 

0.03         0-77 

40      76.52 

O.O4           O-79 

4-0         81.72 

O.O4         0.85 

5.0         86.94 

0.05         0.90 

*  See  Note,  page  6. 

Additional  data  for  the  distribution  of  monochloroacetic  acid  between  water 
and  benzene  as  well  as  similar  results  for  dichloroacetic  acid  are  given  by 
Georgievics,  1915. 


II 


ChloroACETIC  ACIDS 


DISTRIBUTION  or  CHLORACETIC  ACID  BETWEEN: 

(Herz  and  Lewy.) 

Water  and  Chloroform  at  25°.  Water  and  Bromoform  at  25°. 


Cms.  CH2C1COOH 

G.  M.  CH2C1COOH 

Cms.  CH2C1COOH 

G.  M.  CHaClCOOH 

.       per 

100  CC, 

per  100  cc. 

per  100  cc. 

per  100  cc. 

H20 
Layer. 

CHC13 
Layer. 

1H20 
Layer. 

CHC13 

Layer. 

H2O 
Layer. 

CHBr3 
Layer. 

H2o 

Layer. 

CHBrs 
Layer. 

5* 

0.283 

0.05 

0.0025 

40* 

0.850 

0-45 

O-OII 

10 

0.6l4 

o.io 

O.OO6O 

So 

1.889 

0.50 

0.0165 

20 

1.  088 

O.2O 

O.OI3S 

60 

2.994 

O.6o 

O.O28 

40 

2.948 

O.4O 

O.O29 

70 

4.241 

0.70 

0.040 

50 

3.684 

0-6o 

0.045 

80 

5.620 

0.8o 

0-053 

60 

4.440 

0.70 

0.061 

90 

7.560 

0.90 

0-067 

70 

7.086 

o-75 

0.077 

91  .6 

11.340 

0-97 

0.120 

DISTRIBUTION  OF  CHLORACETIC  ACID  BETWEEN: 

(Herz  and  Lewy.) 


Water  and  Carbon  Disulphide 


at   25°. 


Water  and  Carbon  Tetra- 
chloride  at  25°. 


Cms.  CHzClCOOH 
per  100  cc. 

G 

.  M.  CH2C1COOH 

per  100  cc. 

Cms.  CH2C1COOH 
per  100  cc. 

G 

.  M.  CH2C1COOH 

per  100  cc. 

'H20 
Layer. 

CS2 

Layer. 

H20 
Layer. 

CS2 
Layer. 

H2O 
Layer. 

ecu 

Layer. 

"l^O 
Layer. 

ecu 

Layer. 

60* 

0 

.426 

O 

.6 

0 

.0042 

90* 

I.4I7 

0 

•95 

0.0150 

80 

0 

.691 

O 

.8 

O 

.007 

95 

2.031 

I 

.00 

0-0195 

90 

O 

.803 

I 

.0 

0 

.009 

100 

2.645 

I 

•05 

0-0270 

100 

I 

.040 

I 

•05 

O 

.0105 

«>5 

4.26 

I 

.10 

0.0415 

105 

I 

.464 

I 

.10 

0 

.015 

106.7 

5-19 

I 

•13 

0.0550 

106.7 

I 

.890 

I 

•13 

O 

.020 

*  See  Note,  page  6. 


Results  showing  the  influence  of  sulfuric  acid  upon  the  distribution  of  mono- 
chloroacetic  acid  between  water  and  ethyl  ether  at  26°  are  given  by  Hantzsch 
and  Vagt  (1901). 


CyanoACETIC  ACID  CH2(CN)COOH. 

DISTRIBUTION  OF  CYANOACETIC  ACID  BETWEEN: 

(Hantzsch  and  Sebalt,  1899.) 


Water  and  Ethyl  Ether. 

Cms.  CH2(CN)COOH  per 
Liter. 


•  • 

H20 

(G>H  )  O 

Layer. 

Layer. 

O 

0.070 

0.042 

10 

0.076 

0.044 

21 

0.083 

0.030 

30 

0.089 

0.027 

Water  and  Benzene. 

Cms.  CH2(CN)COOH  per 
Liter. 


6 
25 


H20 

C,H9 

Layer. 

Layer. 

0.067 

0.02O 

0.130 

O.OIQ 

PhenylACETIC  ACID  12 

PhenylACETIC  ACID  («  Toluic  Acid)  CH2(C«H5)COOH. 

SOLUBILITY  IN  WATER  AND  IN  ALCOHOLS.    (Timofeiew,  1894.) 


Gms.CH2(C6H5)COOH                                                 Cms. 
Solvent.                 t°.           per  100  Gms.                Solvent.                      t°. 

CH2(C«H5)COOH 
per  100  Gms. 

Sat.  Sol. 

Sat.  Sol. 

Water                     20 

1.64 

Ethyl  Alcohol          o.o 

50-7 

Methyl  Alcohol  —17 

50.6 

+  19-4 

64.4 

-13 

S3-2 

20.0 

65.1 

"                   o 

59-2 

Propyl  Alcohol  —17.0 

29.4 

+  19-4 

70.8 

-13-0 

32.3 

"                          20 

71.8 

0.0 

40.9 

Ethyl  Alcohol     -17 

39-7 

+19.4 

56.8 

-13 

4i.5 

20.0 

57-2 

SOLUBILITY  OF  PHENYLACETIC  ACID  IN  SEVERAL  SOLVENTS  AT  25°. 

(Herz  and  Rathmann,  1913.) 

Gms.  Gms. 

Solvent.                      CH2(C6H5)COOH                         Solvent.  CH2(C6H5)COOH 

per  100  cc.  Sat.  Sol.  per  100  cc.  Sat.  Sol. 

Chloroform  60.17  Tetrachlorethylene          21.19 

Carbon  Tetrachloride       25.07  Tetrachlorethane  61.45 

Trichlorethylene  44-89  Pentachlorethane  44.26 

The  freezing-point  curve  (Solubility,  see  footnote,  page  i)  is  given  by  Sal- 
kowski  (1885)  for  mixtures  of  phenylacetic  acid  and  hydrocinnamic  acid. 

ACETIC  ACID  ESTERS. 

SOLUBILITIES  OF  SEVERAL  ACETIC  ACID  ESTERS  IN  AQUEOUS  ALCOHOL  AT  ROOM 
TEMPERATURE.     (Pfeiffer,  1892.) 

~.  TTfV,  i          cc-  HjjO  added  to  cause  separation  of  a  second  phase  in  mixtures  of  the  given 
Alcohol  m  amounts  of  Alcohol  and  3  cc.  of: 

Mixtures. 

3 
6 

9 

12 
IS 

18 

21 

24 
27 

30 

33 
ChloroACETIC  ACID  ESTERS. 

SOLUBILITY  OF  MONOCHLOR,  DICHLOR,  AND  OF  TRICHLORACETIC  ESTER 
IN  AQUEOUS  ALCOHOL  AT  ROOM  TEMPERATURE." 

(Bancroft  —  Phys.  Rev.  3,  193,  1895-06,  from  results  of  Pfdffcr,  Z.  physik.  chem.  9,  469,  *9a.) 


CH3COOCH3.    CH3COOC2HS. 

CH3COOC3H7. 

CH3COOC4H0. 

CHsCOOCgHu. 

00                     6.0 

4-50 

2.08 

I.76 

...                 °o 

10.48 

6.08 

4.24 

...                     ... 

17.80 

10.46 

9-°3 

...                  ... 

26.00 

15.37 

13.24 

...                  ... 

35.63 

20.42 

I7-52 

...                          ... 

47-5° 

26.60 

22.22 

...                     ... 

58.71 

3J-49 

26.99 

...                ... 

00 

37.48 

32.14 

...                     ... 

.  .  . 

43-75 

37.23 

...                     ... 

.  .  . 

50-74 

42.06 

...                     ... 

59-99 

48.41 

cc.  Ethyl 
Alcohol  in 

cc.  H2O  added  to  cause  separation  of  a  second  phase 
in  mixtures  of  the  given  amts.  of  Alcohol  and  3  cc.  of: 

Mixtures. 

CHaClCOOCzHs. 

CHC12COOC2H5 

CC13COOC2H4. 

3 

1-32 

0.90 

0.65 

6 

4.01 

2-45 

1.  80 

9 

7-30 

4-33 

3.02 

12 

10.78 

6.60 

4.50 

IS 

16.16 

9.20 

6.50 

18 

22.16 

•  •  • 

21 

28.74 

•  •  • 

•  •  • 

13  ACETIN 

Mono-,  Di-f  and  Tri  ACETIN  C3H6(OH)2(OC2H8O),  C3H5(OH)(OC2H3O)2,  and 


Trie  partition  coefficients  of  these  three  compounds  between  olive  oil  and 
water  are  given  by  Baum  (1899)  and  Meyer  (1901,  1909),  as  0.06,  0.23,  and  0.3 

respectively. 

MethACETIN     (p    Acetanisidine,    or    p    oxymethylacetanilide)     C6H4.OCH8. 

NHCHaCO. 

100  gms.  H2O  dissolve  0.19  gms.  of  the  compound  at  15°  and  8.3  gms.  at  100°. 

(German  Pharmacopoeia.) 

a  ACETNAPHTHALIDE  C2H3ONH(CioH7). 

SOLUBILITY  IN  MIXTURES  OF  ALCOHOL  AND  WATER  AT  25°. 

(Holleman  and  Antusch  —  Rec.  trav.  chim.  13,  289,  1894.) 


Vol.% 
Alcohol. 

Gms.  per 
100  Gms. 
Solvent. 

Sp.  Gr.  of 

Solutions. 

Vol.% 
Alcohol. 

Gms.  per 
100  Gms. 
Solvent. 

Sp.  Gr.  of 

Solutions. 

100 

4-02 

0.7916 

65 

I.78 

0.8977 

95 

4-31 

0.8150 

60 

1-44 

0.9091 

90 

4.II 

0.8344 

55 

I  -O2 

0.9201 

85 

3-69 

0.8485 

5o 

0-71 

0.9290 

80 

3.l8 

0.8624 

35 

0.25 

Q-9537 

75 

2-73 

0.8761 

20 

O.O9 

0.9717 

70 

2.31 

0.8798 

10 

O.O4 

0.9841 

Constant  agitation  was  not  employed.  The  mixtures  were  allowed  to  stand 
in  bath  and  the  solutions  analyzed  after  different  lengths  of  time.  Formulas 
are  not  given.  This  applies  to  all  determinations  by  Holleman  and  Antush. 

ACETONE   (CH3)2CO. 

SOLUBILITY  OF  ACETONE  AT  25°  IN  AQUEOUS  SOLUTIONS  OF: 
Electrolytes.  Non-Electrolytes. 

(Bell  —  J.  Phys.  Ch.  9,  544,  1905;  Linebarger  —  Am.  Ch.  J.  14,  380,  1802.) 


Gms.  Electro- 
lyte per 
100  Gnis*  AQ< 

Gms.  (CH3)2CO  per  100  Gms.              Gms.  Non-    Gms.  (CH3)2CO  per  100  Gms. 
Solvent  in  Solutions  of:                    Electrolyte           Solvent  in  Solutions  of: 

Solution. 

K2C03 

Na2CO3 

(NH4)2CO3  MgCO3"     Xq.  Solution.  CioHat 

Anethol*  (C6H6)2CO 

I 

•25 

. 

83-5 

5 

92 

•5 

103.0 

90.0 

2 

•50 

51.0 

IIO.O 

65.0 

10 

117 

.0 

123.0 

108.5 

5 

-CO 

65' 

o 

38.0 

73-5 

47-o 

20 

137 

.0 

144-5 

126.0 

7 

•5 

46, 

5 

27-5 

57-o 

38.0 

30 

148 

•5 

155-0 

i33-o 

10 

.0 

34 

5 

19-5 

44-5 

29.0 

40 

155 

•5 

162  -O 

136.0 

12 

•5 

25 

5 

14.0 

35-o 

50 

159 

•5 

166.0 

135-5 

15 

.0 

18 

o 

9-0 

28.0 

60 

160 

.2 

165.0 

I3I-5 

20 

•  O 

8 

0 

2-7 

70 

155 

•  O 

158.0 

123.0 

25 

.0 

3 

7 

80 

.      i 

108.5 

30 

.0 

i 

6 

... 

90 

. 

82.0 

*  Anethof  =  p  Propenylanisol,  CH3.CH:CH.C6H4OCH3.          f  Naphthalene  results  at  35°. 

NOTE.  —  In  the  case  of  the  results  for  the  aqueous  solutions  of  electrolytes, 
the  determinations  were  made  by  adding  successive  small  quantities  of  acetone 
to  the  mixtures  of  given  amounts  of  water  and  electrolyte,  and  noting  the  point 
at  which  a  clouding,  due  to  the  separation  of  a  second  phase,  occurred.  In  the 
case  of  the  aqueous  non-electrolyte  solutions,  successive  small  amounts  of  water 
were  added  to  mixtures  of  known  amounts  of  acetone  and  the  non-electrolyte. 
In  all  cases  the  results,  as  given  in  the  original  papers,  have  been  recalculated 
and  plotted  on  cross-section  paper.  From  the  curves  so  obtained,  the  above 
table  was  constructed. 

Additional  data  for  systems  containing  acetone  are  given  under  the  salt  involved, 
as,  for  instance,  Potassium  Carbonate,  p.  51 1,  Potassium  Fluoride,  p.  534.  etc. 


ACETONE  14 

MlSCIBELITY  OF  ACETONE  AT  O°   WITH    MIXTURES   OF: 


Chloroform  and  Water  (Bonner,  1910). 


Bromobenzene  and  Water  (Bonner,  1910). 


Gms. 

Gms.              Gms. 

Sp.  Gr.  of 

Gms. 

Gms. 

Gms. 

Sp.  Gr.  of 

CHClj. 

H20.          (CHa)2CO. 

Mixture. 

C«H5Br. 

H20. 

(CH3)2CO. 

Mixture. 

0.988 

O.OI2         O.5OI 

z.i8 

0.977 

0.023 

0.685 

1.  12 

0.900 

O.IOO 

.300 

1.  01 

0.90 

O.IO 

I  .13 

1.  01 

0.792 

0.208 

.633 

0.98 

0.80 

O.2O 

I.4I 

0.98 

0.696 

0.304 

•  750 

0.96 

0.70 

0.30 

1.52 

0.97 

0.600 

O.4OO 

.770 

0.95 

0.60 

0.40 

i-S7 

0.96 

0.500 

0.500 

.720 

0.94 

0.50 

0.50 

i  .60 

°-95 

*O.42O 

0.580 

.650 

*°-49 

0.51 

i.  60 

0.400 

O.6OO 

.630 

o-93 

0.40 

0.60 

i-59 

0.94 

0.300 

0.700 

-530 

0.94 

0.30 

0.70 

i-55 

o-93 

O.2OO 

0.800 

.321 

°-95 

0.20 

0.80 

1.46 

o-93 

O.IOO 

o  .  900      i  .  144 

0.97 

0.10 

0.90 

1.30 

o-93 

O.OlS 

0.982       0.464 

0.98 

,    O.O2 

0.98 

0.849 

o-95 

NOTE.  —  The  determinations  were  made  by  gradually  adding  acetone  to  the 
mixtures  of  the  given  amounts  of  water  and  the  other  constituent  until  a  homo- 
geneous solution  was  obtained.  The  results  give  the  binodal  curve  for  the  sys- 
tem. The  author  also  determined  "tie  lines"  showing  the  compositions  of  the 
various  pairs  of  liquids  which  may  exist  in  equilibrium.  When  the  two  layers 
are  practically  of  the  same  composition  the  tie  line  is  reduced  to  a  point  desig- 
nated as  the  "plait  point"  of  the  binodal  curve.  This  point  is  indicated  by  a  * 
in  the  above  tables. 

SOLUBILITY  OP  ACETONE  IN  AQUEOUS  SOLUTIONS  OF  CARBOHYDRATES. 

(Krug  and  McElroy  —  J.  Anal.    Ch.  6,  184,  '92;  Bell  —  J.  Phys.  Ch.  9,  547.  '05.) 


In  Aqueous  Solutions  of  Cane  Sugar. 

Gms.  (CH3)2CO  per  100  Gms.  Sugar  Solution  at: 


Percent 

Sugar. 

10 
20 
30 
35 

40 
45 
50 
55 
60 

65 
70 


In  Aqueous  Dextrose  Solutions. 


15°. 

20°. 

25°. 

30°. 

35°. 

40°. 

597-2 

581.8 

574-8 

272.5 

250.0 

251.8 

172.4 

150.0 

150.6 

no 

96.4 

92.8 

89.8 

85 

.  .  . 

71.9 

68.8 

65-7 

.  .  . 

62 

50.8 

48.1 

45-9 

42 

... 

35-8 

33-8 

32-5 

.... 

29 

25.2 

24.2 

23-4 

.  .  . 

18-3 

17.7 

17.0 

•  •  • 

13-2 

12.8 

12-5 

... 

In  Aqueous  Maltose  Solutions. 


Per 

cent 

Gms.  (CH3)2CO  per  100  Gms. 
Solvent  at: 

Per 

cent 

Gms. 

(CH3)2CO  per 
Solvent  at: 

too  Gms. 

Dextrose. 

15°. 

25°. 

35°.    ' 

Maltose. 

15° 

25°. 

35°." 

10 

736 

•7 

747-9 

761-5 

10 

353 

.6 

348 

.1 

342 

•  0 

20 

255 

•3 

247-7 

240.8 

20 

185 

•4 

181 

.2 

I76 

•9 

30 

157 

•5 

149.8 

142.5 

30 

119 

•9 

116 

•  O 

112 

•4 

40 

86 

•9 

79.6 

74-o 

40 

78 

•4 

74 

•7 

70 

•5 

50 

36 

.2 

33-o 

31.2 

50 

46 

.2 

42 

9 

39 

.8 

*/  IS  \J%J  \J  \J  S  \J  S 

The  determinations  were  made  as  in  the  case  of  the  solubility  of  acetone  in 
aqueous  solutions  of  electrolytes.     See  preceding  page. 


ACETONE 


DISTRIBUTION  OF  ACETONE  BETWEEN: 


Benzene  and  Water. 
Results  at  20°.  Results  at  25°. 


(Philip  and  Bramby,  1915-) 
Gm.  (CH3)2CO  per  1000  cc. 

'       H^O  C6Hg 

Layer. 

0.08 


Layer. 
O.IO 
0.20 
0-30 
O.40 


0.12 
0.25 
0-34 


(Herz  and  Fischer,  1905.) 
Cms.  (CH3)2CO  per  1000  cc. 

C6H6 
Layer. 

12.0 

41-7 
IOI.5 


Toluene  and  Water. 

At  Different  Temps. 
(Hantzsch  and  Vagt,  1901.) 
Cms.  (CH;j)2CO  per  1000  cc. 


H20 
Layer. 


50 

100 

150 

200 


155-9 
225.0 

See  Note,  page  6. 


*° 

H20 
Layer. 

C6H5CH3 
Layer. 

0 

2.105 

0-993 

10 
20 
30 

2.000 
1.960 
1.867 

0-957 
0-957 
0-957 

Philip  and  Bramby  also  give  data  for  the  effect  of  NaCl,  KC1  and  LiCl  upon 
the  distribution  of  acetone  between  benzene  and  water. 

In  the  determinations  by  Hantzsch  and  Vagt  the  equilibrium  was  approached 
from  above.  The  amount  of  acetone  in  the  lower  layer  was  determined  by 
analysis,  and  that  in  the  upper  layer  calculated  by  difference. 


Water  and 
Carbon  Tetrachloride. 

Mols.  (CHs)2CO  per  Liter. 
CC14 


DISTRIBUTION  OF  ACETONE  BETWEEN: 

(Herz  and  Rathmann,  1913.) 

Water  and 

Chloroform. 

Mols.  (CH,)2CO  per  Liter. 


H20 
Layer. 

0.186 

0.322 
1. 01 

1.66 
2.87 


Layer. 
0.0833 
0.146 
0.514 
0.997 
2.10 


'    H20 

CHC13 

Layer. 

Layer. 

0.032 

0.168 

0.0781 

0-399 

0.145 

0.676 

0.263 

1.17 

0-493 

1.98 

1.  01 

3-o6 

Water  and 

Pentachlorethane. 

Mols.  (CH3)2CO  per  Liter. 


H20 
Layer. 

O 


144 
271 

541 
806 
149 


QHC16 
Layer. 

0.251 
0.469 
0.859 
1-275 
I-763 


Water  and 

Tetrachlorethane. 

Mols.  (CH3)2CO  per  Liter. 


Water  and 
Tetrachlorethylene. 

Mols.  (CH3)2CO  per  Liter. 


H20 
Layer. 


0.249 

0.317 
0.363 
0.569 


C2H2CU 
Layer. 

0.341 
0.994 
I.  210 

I-323 
1.936 


H20 

Layer. 


CC)2:CCI2 
Layer. 

0.081 


0.274 

0.562        0.174 

1.020  0.343 

1.545  0.629 

2.007  0.891 

The  distribution  coefficient  of  acetone  between  olive  oil  and  water  is  given  by 
Meyer  (1901),  as  0.146  at  3°  and  0.235  at  30°. 


^  Water  and 
Trichlorethylene. 

Mols.  (CH3)2CO  per  Liter. 

Layer. 

0.160 

0.350 
0.654 
0.946 

CHCl:CCla 
Layer. 

0.193 

0-359 
0.719 
1.029 
1.562 

SOLUBILITY   DATA   DETERMINED  BY  THE    METHOD    OF    LOWERING    OF    THE 
FREEZING-POINT  (see  footnote,  p.  i)  ARE  GIVEN  FOR  MIXTURES  OF  Acetone 

AND   EACH   OF  THE   FOLLOWING   COMPOUNDS: 


(Maass  and  Mclntosh,  1912.) 


Phenol 

Resorcinol 

Pyrogallol 


(Schmidlin  and  Lang,  1910.) 


Bromine 

Chlorine 

Hydrobromic  Acid 

Chloroform  (Tskalotos  and  Guye,  1910.)    Pyrocatechol 

0  Chlorophenol        (Bramby,  1916.) 

Depression  of  the  freezing-point  of  mixtures  of  acetone  and  water  and  each  of 
the  following  compounds  are  given  by  Waddell  (1899):  Ether,  hydroquinone, 
phenol,  p  nitrophenol,  salicylic  acid. 


ACETOPHENONE  16 

ACETOPHENONE   CH3COC6H6. 

The  freezing-point  curve  for  mixtures  of  acetophenone  and  sulfuric  acid  is 
given  by  Kendall  and  Carpenter  (1914). 

Freezing-point  curves  (solubility,  see  footnote,  page  i)  for  mixtures  of  Cinna- 
mylidene  Acetophenone  and  each  of  the  following  compounds  are  given  by 
Giua  (1916):  Acenaphthene,  azobenzene,  ethyl  ether  and  a  trinitrotoluene. 

ACETYLACETONE    CH3COCH2COCEL 

SOLUBILITY  IN  "WATER. 

(Rothmund  — Z.  phys.  Ch.  26,  475,  '98.) 

Cms.  CH3COCH,COCHS  per  100  Cms. 


to  H2O  Acetyl  Acetone 

Layer.  Layer. 

30  15-46          95-02 

40  17.58  93.68 

50  20.22  91.90 

60  23.23  89.41 

70  27.10  85.77 

80  33-92  78.82 

87.7  (crit.  temp.)  56.8 

NOTE.  —  Weighed  amounts  of  water  and  acetyl  acetone  were  placed  in  small 
glass  tubes,  which  were  then  sealed  and  slowly  heated  until  the  contained  mix- 
tures became  homogeneous.  The  temperature  was  then  allowed  to  fall  very 
gradually  and  the  point  noted  at  which  cloudiness  appeared.  This  point  was 
accurately  established  for  each  tube  by  repeated  trials.  The  curve  plotted  from 
these  determinations  shows  two  percentage  amounts  of  acetyl  acetone  which 
cause  cloudiness  at  each  temperature  below  the  critical  point.  Of  these  two 
points,  for  each  temperature,  one  represents  the  aqueous  layer,  i.e.,  the  solu- 
bility of  acetyl  acetone  in  water;  and  the  other  represents  the  acetyl  acetone 
layer,  i.e.,  the  solubility  of  water  in  acetyl  acetone.  This  method  is  known  as  the 
'Synthetic  Method,"  and  yields  results  in  harmony  with  those  obtained  by  the 
analytical  method,  i.e.,  by  analyzing  each  layer  after  complete  separation  occurs. 
See  also,  chapter  on  Methods  of  Solubility  Determinations. 

ACETYLENE  C2H2. 

SOLUBILITY  IN  WATER. 

(Winkler;  see  Landolt  and  Bernstein's  Tabellen,  3d  ed.  p.  604,  '05.) 
t°.  a.  q. 

O  1-73  0.20 

5  x-49  o-1; 

10  1.31  0.15 

15  i-iS  °-I3 

20  1.03  O°I2 

25  0.93  o.n 

30  0-84  0.09 

a,  "Absorption  Coefficient,"  =  the  volume  of  gas  (reduced  to  o°  and  760 
mm.  pressure)  taken  up  by  one  volume  of  the  liquid  at  the  given  temperature 
when  the  partial  pressure  of  the  gas  equals  760  mm.  mercury. 

q,  "Solubility,"  =  the  amount  of  gas  in  grams  which  is  taken  up  by  100  grams 
of  the  pure  solvent  at  the  given  temperature  if  the  total  pressure,  i.e.,  the  partial 
pressure  of  the  gas  plus  the  vapor  pressure  of  the  liquid  at  the  absorption  tem- 
perature, is  760  mm. 


17  ACETYLENE 

SOLUBILITY  OF  ACETYLENE  IN  WATER,  AQUEOUS  SOLUTIONS  OF  ALKALIES  AND 

SULFURIC  ACID   AT   15°. 

(Billitzer,  1902.) 


Aq.  Solution 
of: 

Ba(OH)2 
Ca(OH)2 
NH4OH 
NaOH 
KOH 
Na2S04 
H2S04 

SOLUBIL 

/150f 

Acetylen 

e  in  Aq.  Sol 

utions 

ot 

Norma 

lity: 

O.OI 

1.230 

1.216 

1.  210 
1.  212 

ITY  IN 

0.025 

1.218 

0.05 

O.IO 

1.230 

0.15 
1.240 

0.25 

0.50 

1.  00 

2.OO 

3-oo 

WATER 

I.2OO 
,   /15  = 

1.218 

I.lSo 
1.185 
I.I70 
I.I90 

I.25L 

I.22O 
...        I.I28 
I.I30 

.  .  .      1.068 

1.225 
1.040 
1.056 
0.940 
I.I2O 

1.230 

0.885 

0.912 
0.720 
1.040 

1-235 
0.6OO 
0.660 
0.340 
0.900 

1.240 
0.370 
0.460 

0.780 

.The  above  results  were  determined  by  the  method  of  Ostwald  (Handbuch 
physiko-chemischen  Messungen  207  ff.).  A  thermostat  was  used  and  great 
care  taken  to  reduce  experimental  errors  and  purify  the  acetylene.  The  results 
are  in  terms  of  the  Ostwald  Solubility  Expression,  for  which  see  page  227,  following. 

SOLUBILITY  OF  ACETYLENE  IN  AQUEOUS  ACETONE  SOLUTIONS. 

(Kremann  and  Honel,  1913.) 

Vol.  Per  Cent  H2O  Cms.  CzH.2  dissolved  per  Liter  Sat.  Solution  at: 

in  Solvent 
(HjO  +  Acetone). 

O 

5 
10 

20 

35 

5o 

75 

100 

The  freezing-point  curve  for  mixture*  of  acetylene  and  methyl  ether  are 
given  by  Baume  and  German  (1911,  1914). 

ACETYLENE   Biiodide,  cis  and  trans. 

Data  for  the  lowering  of  the  freezing-points  of  mixtures  of  these  two  isomers 
are  given  by  Chavanne  and  Vos  (1914). 

ACONITIC  ACID  C3H3(COOH)3. 

100  grams  of  formic  acid  (95%  HCOOH)  dissolve  2.01  grams  C3H3(COOH)S 

at  2O.6°  C.  (Aschan,  1913.) 


0° 

18° 

25° 

37 

21 

15-2 

3i 

18.2 

13-5 

26 

15-0 

io-5 

i5 

9-5 

8.0 

8.4 

5-5 

4-45 

5-7 

1.23 

2.22 

1.23 

0.98 

AOONITINE  (Amorphous)  C34H47NOU. 

SOLUBILITY  IN  SEVERAL  SOLVENTS. 

(At  25°  U.S.P.;  at  i8°-22°,  Miiller  —  Apoth.-Ztg.  18.  a,  '03.) 


Solvent. 

Water  .  . 
Alcohol  . 
Ether  .  . 

100  gms. 


Cms.  CaJItfNOi  per 
loo  Gms.  Solvent  at: 


Solvent 


l8°-32°. 

0.054 
1.44 


25°. 

0.031 

4-54 
2.27 


Gms.  CsilL^NOii  pet 

100  Gms.  Solvent  at: 

~~^ 


l8°-22°. 

Benzene      *7 -%$ 

Carbon  Tetrachloride   i .  99 
Petroleum  Ether  .    .     0.023       0.028 


dissolve  0.0226  gm.  aconitine  at  22°    (Dunstan  and  Umney,  1892.) 
abs.  alcohol     "         2.7  "  "  "      "       (Jiirgens,  1885.) 

"     ether       "-      1.56       " 


TrichloroACRYLIC  ACID  18 

TrichloroACRYLIC  ACID  CC12:CC1COOH. 

SOLUBILITY  OF  TRICHLOROACRYLIC  ACID  IN  WATER 

(Boeseken  and  Carriere,  1915.) 


Gms.  CC12: 

44 

,                CC1COOH 

t 

•              per  100  Gms. 
Sat.  Solution. 

O.O 

0.0 

—0.36 

2.0 

-  0.6 

Eutec.      4.5     : 

+13.7 

64.1 

68.5 

17.0 

74-5 

19.2 

m.  pt.      80.0 

17.0 

Eutec.     8  1  .  i 

20.3 

82.8 

25.0 

84-5 

30.0 

86.0 

40.0 

89.5 

50.0 

92.5 

60.0 

94-5 

70.0 

98.5 

72.9 

IOO.O 

Solid  Phase. 


Ice 


Ice+CCl2: 

CCl2.CClCOOH.2iH2Q 


CC12:CC1COOH+ 

CC12:CC1COOH.2JH2O 
CC12:CC1COOH 


Between  the  concentration  4.5 
and  64.1  two  liquid  layers  are 
formed.  The  percentage  of 
CC12:CC1COOH  in  each  is  as 
follows: 

Gms.  CC12:CC1COOH  per 
t°  loo  Gms.  Sat.  Solution. 


Lower  Layer. 

Upper  Layer. 

10 

5-0 

20 

5-2 

64.1 

30 

6.0 

63.8 

40 

7-5 

62.2 

50 

13-0 

59-5 

55 

18.0 

56.0 

60 

27.0 

49.0 

62  crit. 

t.             38 

.0 

The  original  results  were  plot- 
ted on  cross-section  paper  and 
the  above  figures  read  from  the 
curves. 


ACTINIUM  EMANATIONS. 

SOLUBILITY  IN  SEVERAL  SOLVENTS. 

(Hevesy,  1912.) 

A  method  was  elaborated  for  determining  the  partition  coefficient  between  a 
gas  and  a  liquid  phase.  The  solubility  of  actinium  emanations  was  then  de- 
termined in  KC1,  H2O,  H2SO4,  CjHsOH,  C5HnOH,  (CH3)2CO,  C6H5CHO,  C6H6, 
CyHs,  petroleum  ether  and  CS2.  The  solubility  increases  in  the  order  named. 
Close  relations  are  indicated  between  actinium,  thorium  and  radium. 


ADIPIC  ACID    (Normal)  (CH2)4(COOH)2. 

100  grams  H2O  dissolve  1.44  grams  adipic  acid  at  15°. 


(Henry  —  Compt.  rend.,  99,  1157,  '84;  Lamouroux  —  Ibid.,  128,  998,  '99.) 


ADIPINIC  ACID   (CH2)4(COOH)2. 

loo  grams  of  formic  acid  (95%  HCOOH)  dissolve  4.04  grams  of  (CH2)4 
(COOH)2  at  18.5°;  100  cc.  of  the  saturated  solution  contain  4.684  grams  of 
the  acid.  (Aschan,  1913.) 


AGARIC  ACID   CioH3oO6.H2O. 

IOO  grams  trichloroethylene  dissolve  0.014  gram  agaric  acid  at  15°. 

(Wester  and  Bruins,  1914.) 


I9  AIR 

AIR 

SOLUBILITY  IN  WATER. 

(Winkler  —  Bcr.  34.  1409.  'ox;  see  also  Peterson  and  Sondern  —  Ber.  22,  1439,  '89.) 

cc.*  of  atmospheric  O  and  N  per  liter  of: 
Dist.  HjjO  (at  760  mm.).        Sea  Water  (at  760  mm.). 
f.  B. 

o   0.02881 

5  -02543 

10  .02264 

15  .02045 

20  .01869 

25  .01724 

30  .01606 

40  .01418 

50  .01297 

60  .01216 

80  .01126 

100  .01105 

B  =  "  Coefficient  of  Absorption,"  i.e. 

by  the  liquid  when  the  pressure  of  the  gas  itself  without  the  tension 
of  the  liquid  amounts  to  760  mm. 

Bf  =  "  Solubility,"  i.e.,  the  amount  of  gas,  reduced  to  o°  and  760 
mm.,  which  is  absorbed  by  one  volume  of  the  liquid  when  the  barometer 
indicates  760  mm.  pressure. 

*  Reduced  to  o°  and  760  mm. 

SOLUBILITY  OP  AIR  IN  AQUEOUS  SULPHURIC  ACID  AT  18°  AND  760  MM. 

(Tower  —  Z.  anorg.  Ch.  50,  382,  '06.) 


B'. 

Oxygen. 

Nitrogen. 

Oxygen. 

Nitrogen. 

0.02864 

10.19 

18.45 

7-77 

14.85 

.02521 

8.91 

16.30 

6-93 

I3-32 

.02237 

7.87 

14.50 

6.29 

12.  06 

.O2OI  I 

7-04 

13.07 

5-70 

11.05 

.Ol826 

6-35 

II.QI 

10.25 

.01671 

5-75 

10.96 

... 

9.62 

•01539 

5-24 

10.15 

•OI3I5 

4.48 

8.67 

.OII4O 

3-85 

7-55 

.00978 

3.28 

6.50 

.OO6OO 

1.97 

4-03 

.00000 

o.oo 

o.oo 

the  amount  of  gas  dissolved 


Wt.  %  H2SO4  98  90  80  70 

Solubility  Coef.       0.0173    0.0069    0.0069    °-°°5S 

SOLUBILITY  OF  AIR  IN  ALCOHOL,  ETC. 

(Robinet,  1864.) 


60  50 

0.0059      0.0076 


Vols.  Air  per  100 
Vols.  Solvent. 


Solvent. 

Alcohol  (95  . i%)    .    .  14.1 

Petroleum 6.8 

Benzene 14.0 


Solvent. 

Oil  of  Lavender .    . 
Oil  of  Turpentine  . 


Vols.  Air  per  too 
Vols.  Solvent. 

.  .   6.9 

.     .    24.2 


ALANINE    («  Aminopropionic  Acid)   CH3CH(NH2)COOH. 

SOLUBILITY  IN  MIXTURES  OP  ALCOHOL  AND  WATER  AT  25°. 

(Holleman  and  Antusch,  1894.) 


!•% 
:ohol. 

Gms.  per 
100  Gms. 
Solvent. 

Sp.  Gr.  of 

Solutions. 

0 

16.47 

I  .0421 

5 

14-37 

I.03II 

10 

12-43 

I  .0280 

15 

10-49 

I.OIOI 

20 

8.48 

o  9984 

25 

7-  II 

0.9886 

31 

5-53 

o  9761 

Vol.  % 
Alcohol. 

Gms.  per 
100  Gms. 
Solvent. 

Sp.  Gr.  of 

Solutions. 

35 

4.91 

0.9670 

40 

3-89 

0-9577 

5o 

2.38 

0-9355 

60 

i-57 

0.9102 

70 

0.85 

0.8836 

80 

o-37 

o  8556 

See  remarks  under  a  Acetnaphthalide,  page  13. 

100  gms.  pyridine  dissolve  0.16  gm.  a  alanine  at  20-25°. 


.(Dehn,  1917.) 


ALANINE  20 

SOLUBILITY  OF  d  ALANINE  AND  OF  dl  ALANINE  IN  WATER  AT  DIFFERENT 

TEMPERATURES. 

(Pellini  and  Coppola,  1913.) 

Results  for: 

d  Alanine.  d  —  I  Alanine.          Mixtures  d  +  1  Alanine. 


o 

17 
3<> 

45 

ALBUMIN,  (Egg). 

100  gms.  H2O  dissolve  100  gms.  egg  albumin  at  20-25°.  (Dehn,  1917.) 

loo  gms.  pyridine  dissolve  o.i  gm.  egg  albumin  at  2O°-25°.  " 

loo  gms.  aq.  50%  pyridine  dissolve  6.29  gms.  egg  albumin  at  2O°-25°. 

(Dehn,  1917.) 


Gms.  d  Alanine  per 
100  Gms.  IfcO. 

12.99 

Gms.  d  —  I  Alanine  pe 
100  Gms.  H2O. 

12.89 

r               Gms.  per  100  Gms.  H2O. 

d  Alanine. 

J3-27 

/  Alanine". 
4-OI 

15-17 

J4-95 

14-5 

4.1 

17.39 
20.55 

17.72 
21.58 

J7.o5 

4.99 

ALLANTOIN 

SOLUBILITY  IN  WATER. 

(Titherly,  1912.) 

The  author  obtained  results  varying  from  0.7  to  0.77  gms.  allantoin  per  100 
gms.  H2O  at  25°.  The  variations  were  considered  to  be  due  to  slow  decompo- 
sition of  the  compound. 

ALIZARIN  Ci4H602(OH)2. 

SOLUBILITY  IN  WATER  AT  VARYING  TEMPERATURES. 

(Hiittig,  1914;  Beilstein.) 
t°.  2S°.V  100°.  250°. 

Grams  Alizarin  per  liter  0.00x3595  0.340  3-OI7 

According  to  Dehn  (1917),  100  gms.  H2O  dissolve  0.04  gm.  alizarin  at  2o°-25°. 

SOLUBILITY  OF  ALIZARIN  IN  AQUEOUS  SOLUTIONS  OF: 
Ammonia  at  25°.  Sodium  Hydroxide  at  25°  (Huttig,  1914.) 


Gms.  NHs  per 
Liter. 

Gms.  Alizarin 
per  Liter. 

Gms.  NaOH 
per  Liter. 

Gms.  Alizarin 
per  Liter. 

Solid  Phase. 

0.160 
4-025 

0.132 
0.228 

0.427 
I  .050 

I-I59 
3.820 

C]4H804 
Ci4H804  +  CnHANa 

loo  gms.  95%  formic  acid  dissolve  o.io  gm.  alizarin  at  20.8°.          (Aschan,  1913.) 

Alizarin  is  soluble  in  all  proportions  in  pyridine  and  in  aqL.  50%  pyridine  at 

20°-25°.  (Dehn,  1917.) 

ALOIN. 

Squires  and  Caines  (1905)  found  the  solubility  of  aloin  in  water  at  room  tem- 
perature to  be  0.83  gm.  per  100  cc.  and  in  90%  alcohol,  5.55  gms.  per  100  cc. 

According  to  Wester  and  Bruins  (1914)  100  gms.  trichloroethylene  dissolve 
0.013  gm-  aloin  at  15°. 


21  ALUMINIUM  BROMIDE 

ALUMINIUM  BROMIDE  AlBr,. 

SOLUBILITY  IN  SEVERAL  ORGANIC  SOLVENTS. 

(Mcnschutkin,  1909-10.) 


(Determinations  by  Synthetic  Method.) 


In  Benzene. 


In  Para  Xylene. 


5-7m.pt. 

0 

4-5 

10 

3 

20 

1.8  Eutec. 

27.4 

10 

35-3 

20 

46.5 

30 

59 

40 

70 

60 

83 

80 

91.2 

90 

95-3 

96 

IOO 

Gms.  AlBra  per 
loo  Gms.  Sat.     Solid  Phase. 
Sol. 


QH, 


AlBra 


Gms.  AlBra  per 

t°.              100  Gms.  Sat.          Solid  Phase. 

Sol. 

14  m.  pt. 

0 

p  QlfcCCHa), 

12.5 

11.4 

r 

10.2  Eutec. 

25 

AlBra+£  QH4(CHi)i 

20 

35-7 

AlBr, 

30 

47.2 

" 

40 

61.2 

M 

5° 

72.2 

M 

60 

79.6 

M 

80 

90.9 

a 

90 

95-4 

M 

96 

IOO 

M 

In  Toluene. 


Gms.  AlBrs 

per  loo  Gms.  Solid  Phase. 
Sat.  Sol. 


•15 

O 

10 

20 

30 
40 

50 
70 
90 
96 


16.1 

23-7 
32.1 

42.5 
56 

68.8 

76.5 
87.2 

95-7 

IOO 


AlBrs  — 


In  Benzoyl  Chloride. 

Gms.  AlBrs 

~ 

t°. 

per  loo  Gms. 

Solid  Phase. 

Sat.  Sol. 

—  0.5 

m.  pt.       o 

CgHsCOCl 

-   2.5 

.    n-7 

1 

-  5 

Eutec.     22.2 

QHsCOCl+AlBra.CgHiCOCl 

20 

33-7 

AlBra-QHsCOCl 

40 

42.6 

" 

00 

51-6 

" 

80 

60.5 

M 

90 

m.  pt.     65.5 

M 

80 

68.9 

M 

60 

71.8 

« 

30 

75-8 

" 

7 

Eutec.     78.8 

AlBrl.C6H5COCl+AlBr, 

20 

80.6 

AlBra 

50 

85.6 

« 

80 

93-2 

" 

96 

IOO 

" 

Reciprocal  solubilities  determined  by  the  method  of  lowering  of  the  freezing- 
point  (see  footnote,  page  i)  are  given  by  Kahlukow  and  Sachanow  (1909)  for 
mixtures  of  Aluminium  Bromide  and  each  of  the  following  compounds:  ani- 
line, benzene,  benzonitrile,  methylbenzoate,  p  bromaniline,  bromobenzene, 
methylene  bromide,  p  dibromobenzene,  dimethylaniline,  diphenylamine,  methyl- 
aniline,  naphthaline,  nitrobenzene, p  yridine,  toluene  and  p  xylene.  Similar  data 
for  mixtures  of  Aluminium  Bromide  and  dimethylpyrone  are  given  by  Plot- 
nikow  (1911). 


ALUMINIUM  BROMIDE  22 

SOLUBILITY  OF  ALUMINIUM  BROMIDE  IN  SEVERAL  ORGANIC  SOLVENTS  (Con.') 
(Determinations  by  Synthetic  Method.) 


In  Benzophenone. 


In  Ethylene  Bromide^ 


Gms.  AlBrs  per 
t°.          ioo  Gm.  Sat.             Solid  Phase. 

Gms.  AlBrs  per 
t°.             ioo  Gm.  Sat.     Solid  Phase.? 

Sol. 

Sol. 

48  m.  pt.        O            (QHfi^CO 

10  m.  pt.         0                   C2H4Br2 

45                I2 

6               11.5 

42            19 

2                      21.3 

38EutCC.     24.7           "  +AlBr3.(C6H5)2CO 

—    2  EutCC.     29.7        C2H4Br2+AlBn 

60                     3°  •  9               AlBrs.  (C«H5)2CO 

10                     36  .  1                AlBr3 

80           36.4 

20                     42  .  I 

IOO                     42  .  2                        " 

30                     48.7 

120                49 

40                      56 

130               53 

50                      63.7 

I42m.pt.     59.5 

60                      71.5 

130               64 

70                      79.1 

ioo                69 

80                86.8 

70                72.2 

90                94.5 

50                74 

96              ioo 

38  EutCC.     75                             "      +AlBn 

50                    78                        AlBn 

••   ".- 

80               88 

90               93-5 

96              ioo 

In  Nitrobenzene. 

In  o  Chloronitrobenzene. 

Gms.  AlBrs  per 
t°.        ioo  Gm.  Sat.        Solid  Phase. 

Gms.  AlBrs  per 
t°.           ioo  Gm.  Sat.            Solid  Phase. 

Sol. 

Sol. 

5.  5m.pt.     o      CoHsNOj 

32 

,  5  m.  pt.        O         o  CeHUClNOa 

o               18 

25 

21.8       " 

-5               28.8     " 

13 

.  8  EutCC.    37.5       "  +AlBr3.o  C6H4ClNOa 

-l5EutCC.      42             "  +AlBr3.C«HsNO2 

30 

43  .  1        AlBrs.0  QH^ClNOj 

O                      44-3        AlBn.QHsNOs 

50 

50-3 

30                      49.4 

70 

57-6 

60                      56.7 

83 

,5  m.  pt.    62.9 

80                      63.6 

70 

67 

87m.pt.      68.4 

40 

73-7 

80          71.3 

21 

EutCC.    77.5                     "  +AlBrt 

60          73.9 

40 

80  .  6                     AlBn 

40             76.4 

60 

84 

2oEutCC.       78.9                  "  +AlBn 

80 

88.6 

40                      82  .4              AlBrj 

90 

93-4 

60                      85.8 

96 

IOO 

80                      89.8 

93                96.6 

96              ioo 

23  ALUMINIUM  BROMIDE 

SOLUBILITY  OF  ALUMINIUM  BROMIDE  IN  SEVERAL  ORGANIC  SOLVENTS  (Con.). 
(Determinations  by  Synthetic  Method.) 


In  m  Chloronitrobenzene. 


In  p  Chloronitrobenzene. 


' 

Gms.  AlBrs  per 
t°.          100  Gms.  Sat.        Solid  Phase. 

Gms.  AlBrs  per 
t°..        100  Gms.  Sat.       Solid  Phase. 

Sol. 

'Sol. 

44 

.5m.pt.    o      wC«H4CiN02 

83 

m.  pt.    o 

£C«H4ClNOi 

40 

18.9    " 

80 

9 

" 

35 

.  5  EuteC.  27.8      "  +AlBr3.»M  C6H4C1NO» 

70 

24.8 

" 

50 

34.8       AlBrs.»t  C6HiClNOj 

60 

Eutec.  36.6 

"+AlBrs.£C6H4ClNOj 

70 

44-5 

80 

45-6 

AlBrs.£  C6H4C1NO« 

90 

54-5 

100 

54-9 

" 

io3 

.5  m.  pt.  62.9 

MS 

m.  pt.  62.9 

" 

90 

68.6 

100 

66.8 

" 

70 

73-4 

60 

72.4 

M 

5o 

77-3 

20 

Eutec.  78 

"  4-AlBri 

40 

Eutec.       79.1                     "  +AlBrj 

60 

85-3 

AlBrs 

6o 

82.2                   AlBrs 

80 

89.3 

H 

80 

87.t 

93 

95-4 

H 

90 

92.2 

96 

100 

M 

95 

95-1 

96 

100 

In  o  Bromonitrobenzene. 


In  m  Bromonitrobenzene. 


Gms.  AlBrs  per 
t°.           100  Gms.  Sat.        Solid  Phase. 

Gms.  AlBrs  per 
t°.            100  Gms.  Sat.       Solid  Phase. 

Sol. 

.Sol. 

38 

m.  pt.       o     o. 

.C,EUBrNOi                           54 

m.  pt.        o     t 

»QH4BrNOj 

30 

19.7 

50 

ii.  6 

" 

21 

Eutec.     30 

"  +AlBrs.o  CglMBrNOz       45 

.5  Eutec.  19.5 

40 

37-6 

AlBr*>  CeH4BrNOa            60 

25-5 

AlBr3.w  QHiBrNOj 

60 

45-3 

80 

34-5 

" 

80 

53 

no 

49-5 

• 

88 

.5m.pt.  56.9 

"                         122 

m.  pt.      56.9 

it 

80 

59-7 

no 

61.6 

" 

60 

64.1 

80 

69.2 

H 

40 

68.6 

60 

74.1 

" 

24 

Eutec.     72 

"  +AlBn            42 

Eutec.      78.7 

"  +AlBn 

40 

75-5 

AlBrs                       60 

80.3 

AlBn 

60 

79.8 

80 

84.9 

i< 

80 

86.3 

93 

93-6 

" 

93 

94-5 

;;           96 

100 

a 

96 

IOO 

ALUMINIUM  BROMIDE  24 

SOLUBILITY  OF  ALUMINIUM  BROMIDE  IN  SEVERAL  ORGANIC  SOLVENTS  (Con.}. 
(Determinations  by  Synthetic  Method.) 


In  p  Bromonitrobenzene. 


In  p  Nitrotoluene. 


Gms.  AlBr3  per                                                               Gms-  AlBrs  per 
t°.        loo  Gms.  Sat.         Solid  Phase.                        t°.        100  Gms.  Sat.       Solid  Phase. 
Sol.                                                                               Sol. 

I24.5m.pt.     0      ^.CBHiBrNOa                      53.5m.pt.    0      *C«H4CH3NOj 

119                 10        "                            50                 10 

no 

25.2 

40 

31  .3 

" 

98  Eutec. 

,35-3    "• 

{-AlBrs.0  C6H4BrNO2     29  EutCC. 

46.1 

"+AlBr3.£C4H4CHsNOi 

no 

39-7     A 

[Era.p  C6H4BrNOa         50 

52.9 

AlEr3.p  C«H4CHsNOi 

130 

48.7 

80 

63 

ii 

144  m.  pt. 

56-9 

88  m.  pt. 

66 

" 

120 

65.5 

80 

68.5 

" 

90 

7o-5 

50 

74-3 

* 

60 

74.1 

27  Eutec. 

78.9 

"  +AlBn 

45  Eutec. 

76 

"  +AlBr3          50 

83-3 

AlBrs 

60 

79.6 

AlBrs                    70 

87.7 

• 

80 

86.6 

8S 

92.2 

" 

93 

95-4 

93 

96.7 

ii 

96 

IOO 

96 

IOO 

" 

In  m  Nitrotoluene. 


In  o  Nitrotoluene. 


i  — 

16 

12 

Gms.  AlBrs 
t°.       per  loo  Gms.       Solid  Phase. 
Sat.  Sol. 

m.  pt.     0       m  CjHiCHsNOa 
14-5     " 

Gms.  AlBr3 
t°.             per  loo  Gms.       Solid  Phase. 
Sat.  Sol. 

—    8  .  5  m.  pt.      0       o  C6H4CH3N02 
—  II  EuteC.          8.7     !'-J-  AlBrs.  2oC«H4CHsNO2 

8 

21.8     " 

10 

12.8- 

MBr3.20C«H4CaNOa 

•  I 

EuteC.  32           "+AlBrs.»»  QEUCHsNOz 

30 

24.8 

" 

20 

38.5      AlBrs-m  CeHiCHsNOj 

40 

38 

" 

40 

46.6 

42 

.5  Eutec.  47.7 

"+  AlBrs.aoCjHjCHsNO! 

80 

59-7 

60 

54-3 

AlBrs.o  C6H4CHsNOj 

90 

63.3 

75 

59-5 

" 

96 

m.  pt.  66 

90 

m.  pt.      66 

" 

90 

68.8 

70 

72 

" 

60 

73-8 

40 

76.1 

" 

27 

EuteC.  78.9                       "  +AlBr3 

19 

Eutec.      79.1 

"  +AlBa 

40 

82                        AlBr, 

40 

82.5 

AlBrs 

70 

89 

70 

87.5 

" 

90 

95-3 

90 

93-8 

" 

96 

IOO 

96 

IOO 

" 

ALUMINIUM  CHLORIDE 


ALUMINIUM  CHLORIDE  A1C13.6H2O. 

SOLUBILITY  IN  WATER. 

(Gerlach  —  Z.  anal.  Ch.  8,  250,  '69.) 

ioo  gms.  saturated  solution  contain  41.13  gms.  A1C13  at  15°,  Sp.  Gr.  of  solu 
tion  =  1.354. 

SOLUBILITY  OF  ALUMINIUM  CHLORIDE  IN  SEVERAL  ORGANIC  SOLVENTS. 

(Menschutkin,  1909.) 

(Determinations  by  Synthetic  Method.) 
In  Nitrobenzene.  In  o  Chloronitrobenzene. 


Gms.  A1CL, 
t°.        per  ioo  Gms.      Solid  Phase. 

Gms.  A1CU 
t°.        per  ioo  Gms.       Solid  Phase. 

Sat. 

Sol 

Sat   ~ 

.Sol. 

5 

•5 

m.  pt. 

0 

CgHsNOj 

32 

.5  m.  pt.  o 

o  C,H4C1N02 

2 

Eutec. 

10 

•3 

"  +A1CU.2C6H5N02 

27 

10 

.2 

" 

15 

18 

A1C13.2C.H5NO2 

21 

16 

.1 

" 

25 

-5 

Eutec.  30  .  5 

"  +A1C13.C6H5NO2 

15 

Eutec.    20 

•3 

"  +A1C13.0C.H4C1N02 

45 

34 

.2 

AlCls.CelfcNOi 

35 

25 

•5 

AlCls.o  C6H4ClNOj 

65 

39 

•5 

" 

55 

31 

•5 

" 

85 

48 

" 

75 

38 

•7 

tt 

90 

m 

.pt. 

52 

" 

89 

m.  pt.     45 

•9 

" 

82 

55 

.6 

" 

80 

51 

tt 

72 

58 

" 

69 

Eutec.    54 

•4 

"  +A1C1. 

52 

Eutec. 

61 

.6 

"+A1C1, 

no 

.    57 

•5 

A1CU 

90 

64 

A1C1* 

150 

65 

•4 

" 

130 

67 

•7 

" 

175 

74 

.6 

" 

160 

72 

•4 

" 

194 

IOO 

" 

180 

80 

.1 

" 

194 


IOO 


In  m  Chloronitrobenzene. 


In  p  Chloronitrobenzene. 


t°. 


Gms.  A1CU 

per  ioo  Gms. 

Sat.  Sol. 


Solid  Phase. 


44 . 5  m.  pt.  O       m  C8H4ClNOa 

44  10.7    " 

36  Eutec.  16.6    "+Aici3.w c6H4CiN02 

50  21 

70  28.3 

90          36.8 


104  m.  pt. 
90 
81  Eutec. 

120 

140 
160 


45-9 

52-4 

55-6 

60 

64.1 

70.2 


"  +A1CU 
A1CU 


Gms.  A1CU 
t°.         per  ioo  Gms.      Solid  Phase. 

Sat.  Sol. 

83 

.5  m.  pt.  o 

p  C6H4ClNOa 

78 

7.1 

" 

73 

12.8 

" 

68 

Eutec.    17.1 

"  +MC\3.p  C8H4C1NO, 

80 

22.2 

MOa.p  C4H4C1NO» 

IOO 

31-4 

" 

120 

41.8 

" 

126 

m.  pt.    45.9 

• 

no 

53-2 

" 

94 

Eutec.    58.1 

"+  AlCli 

125 

60.5 

AlCli 

155 

66.9 

s.  -              " 

180 

77-7 

M 

190 

88.2 

" 

104 

IOO 

" 

The  solubility  of  aluminium  chloride  in  anhydrous  hydrazine  is  stated  by 
Welsh  and  Broderson  (1915)  to  be  i.o  gm.  in  ioo  cc.  at  room  temperature. 


ALUMINIUM  CHLORIDE  26 

SOLUBILITY  IN  SEVERAL  ORGANIC  SOLVENTS  (Con.). 
(Determinations  by  Synthetic  Method.) 


In  o  Bromonitrobenzene. 


In  m  Bromonitrobenzene. 


Gms.  AlCb 
t°.       per  100  Gms.        Solid  Phase. 

Gms.  AlCb 
t°.         per  100  Gms.       Solid  Phase. 

Sat.  Sol. 

Sat.  Sol. 

38.5 

0        o  QlfcBrNO, 

54 

•7            o 

m  C6H4BrNOa 

32 

7-5      "f 

51 

6.5 

" 

26 

47 

Eutec.  11.9 

"+  AlCU.ro  C6H4BrNOi 

20  Eutec. 

17.5       "  +A1C13.0  C6H4BrNOa 

60 

16 

AlCb.ro  C6H4BrNO» 

40 

21.7        AlCb.o  C»H4BrNO» 

80 

22.9 

" 

60 

26.4 

100 

30.7 

" 

80 

31.7                      " 

no 

35-9 

« 

97  m.  pt. 

38 

116 

m.  pt.  39.8 

M 

100 

39.8 

H3 

42.3 

«« 

90 

44.6 

107 

44-5 

• 

80  Eutec. 

46.5                    "  +A1CU 

97 

Eutec.  47.4 

"+A1CU 

no 

50.1                  Aid, 

120 

5i-5 

A1CU 

130 

54-1 

140 

56.5 

" 

150 

60.2 

160 

64-5 

" 

170 

70 

180 

77-4 

« 

180 

77-4 

190 

88.8 

M 

197 

100 

U 

In  p  Bromonitrobenzene. 


In  o  Nitrotoluene. 


^ 

Gms.  AlCb 

Gms.  AlCb 

t°.       per  zoo  Gms.        Solid  Phase. 

t°.        per  100  Gms.        Solid  Phase. 

Sat.  Sol. 

Sat.  Sol. 

124 

,  5  m.  pt.  0      P  QI&BrNOa 

—  8.5  HI.  pt.   O       o  C6H4CH3N02 

117 

7-4     " 

—  9.3  EuteC.  I           "+AlCb.2o  C,H4CTfcNOi 

III 

12.8     " 

0                         1-5  AlCb.20  CeHiCHsNOi 

105 

17.7  " 

20                        4 

99 

EuteC.     22.2      "+AlCb.£  CVEfcBrNOa 

40                      II 

120 

28  .  4       MC\a.p  CjHiBrNOj 

<<  EuteC.      31           "  +AlCb.o  C«H4CHjNOj 

\s  \s                                      \s 

I4O 

36.4 

85                      41.8       AlCb.o  C6H4CH3NOj 

145 

m.  pt.    39.8 

95.  5m.  pt.49.3 

140 

44-5 

70               56.8 

120 

51-2 

45  Eutec.    61.5                "+AICI, 

"3 

Eutec.   52.8               "+AICU 

95               64.5             Aicb 

130 

55.9                  AlCb 

145                73-7 

150. 

61.3 

180               86.2 

180 

77-4 

185               89.5 

190 

88.8 

194              100 

194 

100.  0 

One  liter  sat.  solution  of  A1C13  in  CC14  contains  0.74  gm.  at  4°,  0.22  gm.  at  14°, 
0.15  gm.  at  20°  and  0.06  gm.  at  34°. 

One  liter  sat.  solution  of  A1C13  in  CHC13  contains  0.65  gm.  at  — 15°,  i.o  gm  at 
o°  and  0.72  gm.  at  25°.  (Lloyd,  1918.) 


ALUMINIUM  CHLORIDE 


SOLUBILITY  IN  SEVERAL  ORGANIC  SOLVENTS  (Con.). 
(Determinations  by  Synthetic  Method.) 


In  m  Nitrotoluene. 


In  p  Nitrotoluene. 


' 

Gms.  AlCla 

Gms.  A1CU 

t°.         per  100  Gms.        Solid  Phase. 

t°.      per  100  Gms.       Solid  Phase. 

Sat.  Sol. 

Sat.  Sol. 

i6 

m.  pt.        0       m  CeHiCHsNCb 

52 

.  5  m.  pt.  0       P  CaHUCHaNOj 

13 

EuteC.       7.8     "+AlCl3.2wC6H4CH3NOa 

47 

9.2  « 

27 

13  .4  A1C13.2W  CfrfoCHsNOz 

42 

15     " 

35 

EuteC.     24.5     "+AlCl3.«tC6H4CH3NOa 

37 

EuteC.  19          "+AlCU.0CeH4CHsNO, 

65 

34            AlCls.w  CeEUCHsNOa 

55 

29  .  1      AlCla.*  C«H4CH,NOi 

90 

44.2 

80 

34-8 

95 

46.7 

95 

41.3 

99 

.Sm.pt.  49.  3 

109 

m.  pt.  49.3 

70 

56.8 

100 

53-4 

45 

Eutec.  61.5                "+Aici3 

60 

61.7 

95 

64  .  S                   AlCla 

45 

Eutec.  64                   "  +Aicii 

120 

68.2 

105 

69  .  5                    AlCli 

130 

70.2 

165 

80 

190 

94-3 

194 

IOO.O 

In  Benzophenone. 

In  Benzoyl  Chloride. 

f 

Gms.  AlCls 

\ 

Gms.  AlCls 

t°.           per  loo  Gms.      Solid  Phase. 

t°.         per  100  Gms.     Solid  Phase. 

Sat.  Sol. 

Sat.  Sol. 

48 

m.  pt.           0        (C8H5)2CO 

—  o. 

5  m.  pt.      0        CeHsCOCl 

44 

8-5      - 

4 

7.9  " 

39 

.  5  Eutec.  15.4    "  +Aici3(c,H5)2CO 

-7- 

S  Eutec.  12.7    "  +Aici3.c,H6coci 

60 

19.3        AlCl3.(C6H5)*CO 

o 

14  .  1       AlCU-QHsCOCl 

90 

26  .  s 

20 

18.8 

120 

37 

40 

25 

130 

m.  pt.     42.3 

60 

33 

110 

48.8 

80 

42.2 

80 

53-5 

93m.pt.      48.7 

60 

Eutec.     56  .  i              "  +AICU 

80 

52.9 

100 

58                     AlCli 

60 

57.2 

140 

63 

40 

61 

160 

68.6 

180 

78.5 

190 

89.1 

• 

192 

93 

104 

100 

ALUMINIUM  FLUORIDE  A1F3. 

Fusion-point  data  (Solubility,  see  footnote,  page  i)  are  given  by  Pushin  and 
Baskov  (1913)  for  the  following  mixtures: 

A1F3  +  NaF,  A1F3  +  KF,  A1F3  +  LiF,  A1F3  +  CsF,  A1F3  +  RbF. 

Similar  data  for  mixtures  of  A1F3  +  NaF  are  given  by  Fedotieff  and  Illjinsky 
(1913). 


ALUMINIUM  HYDROXIDE 


28 


ALUMINIUM  HYDROXIDE  A1(OH)3. 

SOLUBILITY  OF  MOIST  FRESHLY  PRECIPITATED  ALUMINIUM  HYDROXIDE  IN 
AQUEOUS  SOLUTIONS  OF  ALUMINIUM  SULPHATE. 

(Kremann  and  Hiittinger,  1908.) 

Results  at  40°. 


Results  at  20°. 

Gms.  per  zoo  Gms.  H2O. 

'A12(SO4)3. 

Al(OH)a. 

2-37 

0.15 

A12O3.SO3.9H2O 

5 

0.30 

tt 

7 

0.65 

tt 

9.1 

1.30 

Transition  Point 

10 

1.23 

Al2O32SO3.i2H2O 

15 

1.04 

" 

20 

1.40 

tt 

25 

2.40 

11 

3° 

3-70 

tt 

31.6 

4.20 

Transition  Point 

33 

2-75 

Al2O3.3S03.i6H2O 

34-73 

0.92 

tt 

Gms.  per  100  Gms.  HbO. 
Al(OH)r 


Solid  Phase. 


5.22 


.  .  .* 

Transition  Point 

8.85 

1.82 

Al2O3.2SO3i2H20 

10 

1.65 

tt 

15 

1.40 

ft 

20 

2-15 

" 

25 

3.80 

" 

28.5 

5.80 

Transition  Point 

30 

4-35 

Al203.3SO3.i6H2O 

35 

i.  60 

tt 

49 

0.60 

ft 

Results  at  60°.  f 


Gms.  per  100  Gms.  HzO. 


*  The  figures  given  are  not  sufficient  to  deter- 
mine this  transition  point  accurately. 

t  The  author's  figures  for  60°  are  reproduced 
without  change  as  they  are  not  sufficient  to  deter- 
mine transition  points. 


A12(SO4)3. 

3-24 

8.83 

12.67 

24.07 

31-55 
42.38 

49 -85 


A1(OH)3 

2-53 
I.8S 

4.89 
6.02 

1.42 


Solid  Phase. 


A12O3.SO3.9H2O 
Al203.2S03.i2H2O 


Al2O3.3S03.i6H2O 


SOLUBILITY  OF  ALUMINIUM  HYDROXIDE  IN  AQUEOUS  SODIUM  HYDROXIDE 

SOLUTIONS.      (Haber  and  van  Oordt,  1904.) 

The  mixtures  were  agitated  for  24  hours-  So-called  acetic  acid  soluble  tonerde 
(E.  Merck)  was  used  for  the  experiments.  Temp.  2O°-23°. 

Normality  of  Aq.  NaOH.  Gms.  AUOa  per  Liter. 

0.49  9.27 

0.99  13.90 

2.OO  14.40 

SOLUBILITY  OF  ALUMINIUM  HYDROXIDE  IN  AQUEOUS  SOLUTIONS  OF  SODIUM 

HYDROXIDE.       (Herz,  1911;  Slade,  1911  and  1912.) 

The  experiments  show  that  the  ratio  of  Na  to  Al  in  the  solution  varies  con- 
siderably depending  upon  whether  the  used  Al  hydroxide  was  precipitated  hot 
or  cold,  also  upon  the  length  of  time  it  was  dried  and  upon  the  nature  of  the 
drying  agent.  Herz  found  a  nearly  constant  ratio  of  3  Na  to  I  Al  in  solution. 
Slade  gives  ratios  of  approximately  2.5  : 1  in  normal  NaOH  at  25°  for  cold  pre- 
cipitated hydroxide  dried  over  HgSCX  and  9.0  :  I  for  hot  precipitated  Al  hydroxide 
dried  over  PzO^  Drying  in  thin  layers  also  increased  this  ratio  but  to  a  some- 
what less  extent.  Slade  reports  the  solubility  of  A1(OH)3  in  a  0.6414  normal 
NaOH  solution  to  be  1.34  gm.  per  100  cc.  at  room  temperature. 

ALUMINIUM   OXIDE   A12O3. 

m  Fusion-point  lowering  data  for  mixtures  of  aluminium  oxide  and  cryolite  are 
given  by  Lorenz,  Jabs  and  Eitei  (1913).  The  results  show  one  eutectic  at  ap- 
proximately 940°.  The  eutectic  mixture  contains  19.8%  A12O3. 

Results  for  aluminium  oxide  and  magnesium  oxide  are  given  by  'Rankin  and 
Merwin  (1916). 


29  ALUMINIUM  SULFATE 

ALUMINIUM  SULFATE  Al2(SO4)3.i8H2O. 

SOLUBILITY  IN  WATER. 

(Poggiale,  1843;  Kremann  and  HUttinger,  1908.) 

Mid  Phase.  t°.     ^G^^tToL  SoM  Phase. 

AU(SO4),.i8HiO 


— 

I 

.02 

8 

.09                      Ice 

20 

26 

•7 

— 

I 

•43 

10 

•7 

30 

28 

.8 

— 

2 

.04 

14 

•3 

40 

31 

•4 

— 

2 

-65 

17 

•5 

50 

34 

•3 

— 

2 

•85 

19 

.2 

60 

37 

.2 

— 

4 

Eutec. 

23 

.  I          Ice  +  Al2(SO4)3.i8H2O 

70 

39 

.8 

o 

23 

.  8                     Al2(SO4)3.l8H2O 

80 

42 

.2 

-f- 

7 

•73 

24 

.8 

90 

44 

•7 

10 

25 

.1 

IOO 

47 

.1 

SOLUBILITY  OF  ALUMINIUM  SULFATE  IN  AQUEOUS  SOLUTIONS  OF  FERRIC 
SULFATE  AT  25°  AND  VICE  VERSA.    (Wirth  and  Bakke,  1914.) 

Gms.  per  100  Gms.  Sat.  Sol.  .  Gms.  per  100  Gms.  Sat.  Sol. 

•AWSO.)..      '     Fe,(SO.),.             SohdPhaSe-  'AMSO.),.     '     Fe^SO.)..'      S<"'d "— 

27.82              O             .  Ak(SO4)3.i8H2O  10.03              32-42       Fe2(SO4)3-9H2O 

26.01               6.064        "  8.819           34-02 

24.21  9.819        "  6.626           35.82 

21.64         13-02        "  5-200        38.83 

15.22  23.28  2.342  42.44 
10.46            31.90           "  +Fe2(SO4)3.9H2O                  ...  44-97 

EQUILIBRIUM  BETWEEN  ALUMINIUM  SULFATE,  LITHIUM  SULFATE,  AND  WATER 

AT  30°.      (Schreinemaker  and  De  Waal,  1906.) 

Composition  in  Weight  per  cent: 

Solid 
Phase. 


Of  Solution. 

Of  Residue. 

%  Li2S04. 

%  A12(S04)3. 

%  Li2SO4. 

%  A12(SO4)3. 

25.1 

0 

21-93 

5-34 

16.10 

14-89 

63.70 

4-02 

13.63 

20.76 

14.72 

3I-I7 

13.24 

21  .71 

61  .24 

7.22 

"•73 

22.08 

6.92 

33-54 

6-75 

24-34 

3-77 

37.06 

3-44 

26.12 

o.o 

28.0 

.  .  . 

{      Al2(So!)3.i8H20 

Li2S04.4H20 

Al2(S04)3.i8H20 


SOLUBILITY  OF  ALUMINIUM  SULFATE  IN  AQUEOUS  SOLUTIONS  OF  SULFURIC 

ACID  AT  25°.  (Wirth,  1912.) 

Gms.  per  IOo  Gms.  Sat.  Sol  -  Gms.  per  100  Gms.  Sat  Sol. 

'Al2(S04)s.  H2S04.  "  '     Al2(S04)3.          H2S04. 

27.82  O  AU(SO4)s.i8H2O  4.8  40  Ali(SO4)3.i8HzO 

29.21  5.13  1.5  5° 

26.2  10  i  60 

19.5  20  2.3  70 

11. 6  30  4  75 

A  curve  was  plotted  from  the  published  results  and  the  above  figures  read 
from  the  curve. 

loo  gms.  glycol  dissolve  16.82  gms.  A12(SO4)3.  We  Coninck,  1905-) 

ALUMINIUM  SULFIDE  A12S3. 

Fusion-point  data  for  mixtures  of  Al2Sa  +  Ag2S  are  given  by  Cambi  (1912). 


ALUMS 
ALUMS. 


SOLUBILITY  OP  AMMONIUM  ALUM  AND  OP  POTASSIUM  ALUM 
IN  WATER. 

(Mulder;   Poggiale  —  Ann.  chim.  phys.  [3]  8,  467,  '43;  Locke  —  Am.Ch.  J.26,  174,  '01;  Marino  — 
Gazz.  chim.  ital.  35,  II,  351,  '05;  Berkeley  —  Trans.  Roy.  Soc.  203  A,  214,  '04.) 


O 

5 
10 

15 

20 
25 
30 
40 

50 
60 
70 
80 
90 
92. 

95 


Ammonium  Alum. 


Potassium  Alum. 


Gms.  (NH4)2    Gms. 

Al2(S04)4      A12(S04J424H20 

per  100  g. 
H20. 


G.M.(NH4)2 
A12(S04)4 
per  100  g. 
H20. 


Gms.  K2 

A12(S04)4 

per  100  g. 

H20. 


Gms.  K2          G.  M.  K2 
A12(S04)424H20    A12(S04)4 
per 


2.10 

3-90 

O.OO44 

3-o 

5-65 

0.0058 

3-5° 

6.91 

O.OO74 

3-5 

6.62 

0.0068 

4-99 

9-52 

O.OIO5 

4-0 

7.60 

0.0077 

6.25 

12.66 

0.0132 

5-o 

9-59 

0.0097 

7-74 

15.13 

0.0163 

5-9 

ii  .40 

O.OII4 

9.19 

19.19 

O.OI94 

7-23 

14.14 

0.0140 

10.94 

22  .OI 

0.0231 

8-39 

16.58 

0.0162 

14.88 

30.92 

0.0314 

11.70 

23-83 

0.0227 

20.10 

44-10 

O.O424 

17.00 

36.40 

0.0329 

26  .  70 

66.65 

0.0569 

24-75 

57-35 

0.0479 

40.0 

110.5 

0-0774 

71.0 

321-3 

0-1374 

... 

... 

109.0 

2275.0 

0.2IIO 

119.0 

GO. 

0-2313 

109.7 


CO 


0.2312 


NOTE.  —  The  potassium  alum  figures  in  the  preceding  table  were 
taken  from  a  curve  plotted  from  the  closely  agreeing  determinations  of 
Mulder,  Locke,  Berkeley,  and  Marino.  For  the  higher  temperatures 
(above  60°),  however,  the  results  of  Marino  are  lower  than  those  of 
the  other  investigators,  and  are  omitted  from  the  average  curve. 

Locke  called  attention  in  his  paper  to  the  fact  that  Poggiale's  results 
upon  ammonium  and  potassium  alum  had  evidently  become  inter- 
changed through  some  mistake.  This  explanation  is  entirely  sub- 
stantiated, not  only  by  Locke's  determinations,  but  also  by  those  of 
Mulder  and  Berkeley.  The  ammonium  alum  figures  given  above  were 
therefore  read  from  Poggiale's  potassium  alum  curve,  with  which 
Locke's  determination  of  the  solubility  of  ammonium  alum  at  25°  is  in 
entire  harmony. 


SOLUBILITY  OF  AMMONIUM  ALUM  IN  PRESENCE  OF  AMMONIUM  SULFATE  AND  IN 
PRESENCE  OF  ALUMINIUM  SULFATE  IN 


Mixture  Used. 


(Rudorff  — Ber.  18,  1160,  '85.) 

100  Gms.  Saturated  Solution  Contain: 


Saturated  Ammonium  Alum  at  18.5°  .  .  .  . 
20  cc.  above  sol.  +  6  gms.  cryst.  A12(SO4)3  . 
20  cc.  above  sol.  +  4  gms.  cryst.  (NH4)2SO4. 


Grams  (NILJjjSCU  +  Grams  Al^SO*)* 
.     .       1.42  3.69 


0-45 
20. 8l 


16.09 
0.29 


ALUMS 


SOLUBILITY  OF  MIXTURES  OF  POTASSIUM  ALUM  AND  ALUMINIUM  SULFATE 
AND  OF  POTASSIUM  ALUM  AND  POTASSIUM  SULFATE  IN  WATER. 


t°. 

o 

20 

35 

65 

77 

o 

5- 
10 

*5 
30 
40 

60 
3o 


(Marino  —  Gazz.  chim.  ital.  35,  II,  351,  '05.) 


Gms.  per  1000  Gms. 


Al2(S04)3.i8H20. 

K2S04. 

243-73 

23-45 

824-25 

30.85 

911  .02 

35-29 

1243.21 

59-55 

1598.00 

ii9-43 

l872.II 

183.80 

5-06 

75  -83 

8.66 

75  •I8 

16.07 

85.78 

18.52 

96.50 

20.56 

109.30 

39.60 

147-8 

73-88 

163.1 

126.0 

195-4 

249.7 

238.8 

529.0 

323-7 

1044.0 

5*7-27 

Gm.  Mols.  per ti OOP  Mols.  H2O. 
Al2(S04)3.i8H20.     K2S04." 

6.1 


Solid 

Phase. 


24.1 
33-5 


o.i 

O.2 
0-4 

o-5 
o-55 
i  .o 
1.9 

3-4 
6.7 

14.2 
28.1 


2-3 

3-6 
6.1 

12.6 

18.9 

7.8 

7-7 
8.8 

9-9 

II  .2 

15.2 

16.8 
20.  i 
24.6 
32.6 
53-4 


K2A12(SO4)2.24H2O 
+  A12(S04), 


K2A12(S04)2.24H20 
+  K2S04 


SOLUBILITY  OF  MIXTURES  OF  POTASSIUM  ALUM  AND  OF  THALLIUM 
ALUM  IN  WATER  AT  25°. 

(Fock  —  Z.  Kryst.  Min.  28,  397,  '97.) 

K,A12(S04)4.24H,0 ;  T12A13(SO4)4.24H2O. 


Composition  of  Solution. 
A                 .  ._ 

Solid  Phase 
Mol.  %  of 
Potassium 
Alum. 

KAl(S04)2j>er  Liter. 

T1A1(SO4)2  per  Liter. 
Grams.       Mg.  Mols. 

Mol.  %           Sp.  Gr.  of 
KA1(S04)2.         Solutions. 

Grams. 

Mg.  Mols. 

69.90 

270.5 

o.oo 

o-oo 

ioo               i  -0591 

IOO-O 

74-56 

288.2 

0.48 

1-13 

99.61             I.  0601 

99-32 

67.90 

262.8 

1.72 

4-07 

98.48             1.0598 

96.84 

65-30 

252.7 

4-52 

10.67 

95-95 

.0603 

90.84 

64  95 

25I-4 

9.60 

22.67 

91  .73 

.0605 

82.94 

53-23 

205-9 

18.44 

43.56 

82.54 

.0609 

68.24 

45-32 

175-4 

24.60 

58.10 

75-12 

.0609 

58.23 

38.02 

147.2 

32-48 

76.75 

65-73 

.0611 

46.72 

34-54 

133-6 

35-59 

84.10 

61.36 

.0611 

44.23 

28-35 

109-7 

42.99 

101.60 

5*-93 

.0623 

32.07 

10.94 

42.4 

66.12 

156.2 

21.34        1-0654 

7-94 

o.oo 

O-O 

75-46 

178-3 

o.oo        1.0674 

o.oo 

Data  for  the  influence  of  pressure  on  the  solubility  of  potassium  alum  in 
water  at  o°  are  given  by  Stackelberg,  1896. 
Data  for  the  solubility  of  Rubidium  Alums  are  given  on  p.  582. 


ALUMS 


SOLUBILITY  OF  SODIUM  ALUM  IN  WATER. 

(Smith,  1909.) 


Gms.  Na2Al2(SO4)4  per  100  Cms. 


Cms.  Na2Al2(S04)4.24H20  per  100  Gms 


Sat.  Sol. 
26.9 
27.9 

Water. 
36.7 
38.7 

29 

40.9 

3O.I 
31-4 

43-i 
45-8 

' 

Sat.  Sol. 

Water. 

IO 

50.8 

I03.I 

15 

52.7 

III.3 

20 

54-8 

121  .4 

25 

56-9 

I3I.8 

30 

59-4 

146.3 

10 

15 

20 

25 
30 

Above  30°,  sodium  alum  is  decomposed  in  contact  with  its  saturated  solution. 
The  exact  temperature  of  transition  has  not  been  determined. 

Single  determinations  differing  from  the  above  are  given  by  Tilden  (1884) 
and  by  Auge  (1890). 

SOLUBILITY  OF  CAESIUM  ALUM,  RUBIDIUM  ALUM,  AND  OP  THALLIUM 

ALUM  IN  WATER. 

(Setterburg~Liebig's  Annalen,  211,   104,  '82;  Locke  —  Am.  Ch.  J.  26,  183,  '01;  Berkeley  —  Trans. 

Roy.  Soc.  203  A,  215,  '04.) 

Thallium  Alum. 
Gms.  per  100  Gms.  H2O. 


t°. 

Caesium  Alum. 
Gms.  per  100  Gms.  H2O. 

Al2Cs2(S04)4. 

Al2Cs2(S04)4 
.24H2O. 

o 

0.21 

o-34 

5 

0.25 

0.40 

10 

0.30 

0.49 

20 

0.40 

0.65 

25 

0.50 

0.81 

30 

O.6o 

0.97 

40 

0.85 

1.38 

50 

1.30 

2.  II 

60 

2.0O 

3-27 

70 

3-20 

5-27 

80 

5-40 

9-01 

90 

10.50 

i8.ii 

100 

22.70 

42-54 

Rubidium  Alum. 
Gms.  per  100  Gms.  H2O. 

Al2Rb2(S04)4.  Al2^f(2o°*)4 

0-72 

I.  21 

0.86 

1.48 

1.05 

1.81 

1.50 

2-59 

i.  80 

3.12 

2.20 

3-82 

3-25 

5-69 

8.50 

7.40 

13-36 

12.40 

23-25 

21.  60 

43-25 

A12T12(S04)4. 

A12T12(SO< 

3-15 

'4.84 

3.8o 

5-86 

4.60 

7.12 

6.40 

10.00 

7.60 

11  -95 

9-38 

14.89 

14.40 

23-57 

22.50 

38-41 

35.36 

65.19 

NOTE.  —  Curves  were  plotted  from  the  closely  agreeing  determina- 
tions recorded  by  the  above  named  investigators  and  the  table  con- 
structed from  the  curves. 

Recent  determinations  of  the  solubility  of  caesium  alum  in  water,  by  Hart 
and  Huselton  (1914),  agree  well  with  the  data  in  the  above  table.  For  addi- 
tional caesium  alums  see  page  180. 

SOLUBILITY  OF  Ammonium  Chromium  Alum  IN  WATER. 

(Koppel,  1906.) 

It  was  shown  that,  due  to  the  transition  between  the  violet  and  green  forms 
of  the  compound,  the  saturation  point  is  reached  very  slowly,  especially  at  the 
higher  temperatures.  From  the  determinations  at  o°  it  was  found  that  equi- 
librium is  reached  in  2\  hours.  If  this  saturation  time  is  taken  for  the  other 
temperatures,  the  results  are  considered  to  show  the  solubility  of  the  violet 
form  alone.  The  final  saturation  represents  the  attainment  of  an  equilibrium 
between  the  violet  and  green  forms. 


Results  for  the  Violet  Form. 


Results  for  Final  Equilibrium. 


~- 

Time  of 

Gms. 

r 

Time  of 

Gms. 

t°. 

Saturation, 

(NH4)  Cr  (S04)2 

t°. 

Saturation, 

(NH4)Cr(S04)2 

Hrs. 

per  100  Gms.  Sol. 

Hrs. 

per  100  Gms.  Sol. 

0 

2-5 

3-8 

0 

2-5 

3-8 

30 

2-5 

10.6 

30 

300 

I5.7-I6 

40 

2-5 

15-5 

40 

250 

24.5-24.8 

33 


AMMONIA 


AMMONIA    NH3. 

SOLUBILITY  OP  AMMONIA  IN  WATER. 

(Roscoe  and  Dittmar  —  Liebig's  Annalen,  112,  334,  '59;  Raoult  —  Ann.  chim.  [5]  i,  a6a,  '74;  Mallet  — 

Am.  Ch.  J.  19,  807,  '97.) 


-40 
-30 

—  20 

—  10 

O 

5 

10 

15 


At  760  mm. 

Pressure. 

G.NH3 

Vol.  NH3 

per  100  g. 
H2O. 

per  i  g. 
1l20. 

294.6 

278.1 

... 

176.8 

III-5 

87-5 

1299 

77-5 

1019 

67.9 

910 

60.0 

802 

20 
25 
30 

35 
40 

45 
5o 
56 


At  760  mm. 

Pressure. 

G.NH3 
per  100  g. 
H20. 

Vol.  Nils 
per  i  g. 

52.6 
46.0 
40-3 

710 
635 

595  (28°) 

35-5 

30-7 

27.0 

... 

22.9 

... 

SOLUBILITY  OF  AMMONIA  IN  WATER  DETERMINED  BY  METHOD  OF  LOWERING  OF 

FREEZING-POINT. 

(Rupert,  1910.) 


j.o                vjins, 

INX13  PC 

f  Solid  Phase. 

0 

0 

Ice 

—       2 

2 

" 

-    4.6 

4 

" 

-    7.6 

6 

" 

—   10.6 

8 

* 

-  13-9 

10 

it 

-   17.6 

12 

.  tt 

-   21.4 

14 

tt 

-   25.8 

16 

ft 

18 

ft 

-  37 

20 

tt 

-  43-6 

22 

« 

-   50-7 

24 

ft 

-  60.3 

26 

it 

-   72.2 

28 

" 

-87.2 

30 

tt 

-102.3 

32 

tt 

—  116.7 

34 

" 

—  120     Eutec. 

34-5 

Ice  +  NHjH2O 

-103.8 

36 

NHjHjO 

-  92-9 

38 

" 

-  86.7 

40 

" 

-  83.5 

42 

ft 

-  81.4 

44 

tt 

-  80 

46 

" 

-  79-3 

48.7 

it 

-   79-4 

50 

" 

t° 

Cms.  NHa  per 
100  Gms.  Sol. 

Solid  Phase. 

-80.6 

52 

NHsHjO 

-82.8 

54 

M 

-85.8 

56 

" 

-87 

Eutec.  56  .  5  N 

Hs.H2O+2NH3.Hj 

-84.8 

58 

aNHaHzO 

-82.2 

60 

" 

-80.4 

62 

« 

-79.2 

64 

a 

-79.8 

m.  pt.  66 

tt 

-79.2 

68 

" 

-80.3 

70 

" 

-82.1 

72 

it 

-84.5 

74 

it 

-87.4 

76 

it 

-90.4 

78 

it 

-93-6 

80 

it 

-94 

Eutec.  80.3 

2NH3.HjO-f-NHi 

-91.7 

82 

NHi 

-89.4 

84 

" 

-87.4 

86 

" 

-85.6 

88 

it 

—  84.1 

90 

" 

-82.7 

92 

M 

-81.5 

94 

M 

-80.3 

96 

" 

-79.1 

98 

It 

-78 

100 

* 

More  recent  data  on  the  above  system,  by  Smits  and  Postma  (1914)  agree 
quite  closely  with  the  above  except  in  the  region  of  the  eutectic  Ice  +  NH3H2O. 
These  authors  report  a  temperature  of  —100.3  instead  of  —120  for  this  point. 
Additional  determinations  are  also  given  by  Baume  and  Tykociner  (1914).  Older 
data  for  the  ice  curve  are  given  by  Guthrie  (1884)  and  Pickering  (1893). 


'  o1 

10°. 

20 

30°. 

40°. 

50°. 

60°. 

* 

4 

•5 

9 

17 

•5 

31 

5 

55 

125 

149. 

5 

13 

18 

32 

•5 

56. 

•5 

91 

146 

234 

20 

27 

47 

•5 

83 

134. 

5 

210 

327 

* 

27 

•5 

40 

70 

IX5 

183- 

5 

28l 

425 

35 

54 

93 

153 

•5 

241.5   363.5 

539- 

5 

45 

69 

118 

193, 

•5 

303- 

5 

455 

666 

57 

•5 

89 

151 

245 

377. 

5 

564 

816. 

5 

75 

"5 

191 

305 

5 

465- 

5 

688.5 

985 

93 

144 

237 

393 

569. 

5 

834.5 

1191 

117 

180.5 

291 

455 

5 

690 

1005 

1432 

144 

•5 

226.5 

360 

561. 

5 

830. 

5 

1195 

... 

181 

280 

440 

680 

1007 

... 

•  •  • 

222 

346 

537 

8i7 

1189. 

5 

AMMONIA  34 

VAPOR  PRESSURE  OF  AQUEOUS  AMMONIA  SOLUTIONS. 

(Perman,  1903.) 

G    s  NHs  oer  Vapor  Pressure  in  mm.  of  Mercury  at: 

100  Cms.  Sol. 

O 
2.5 

5 

7-5 
10 

12.5 

15 

I7-S 

20 

22.5 

25 

27-5 

30 

The  apparatus  (Perman,  1901)  used  for  the  above  determinations,  consisted 
of  a  pipet  provided  with  a  stop-cock  at  its  upper  end  and  connected  with  a 
Hg  leveling  tube  at  its  lower  end.  For  maintaining  constant  temperatures  the 
vessel  was  surrounded  by  a  glass  jacket  into  which  water  or  vapors  of  liquids 
boiling  at  various  temperatures  could  be  introduced.  The  aqueous  ammonia 
solution  was  drawn  in  above  the  Hg  and  boiled  to  expel  air.  A  portion  of  it 
was  withdrawn  for  analysis  through  the  stop-cock  at  the  top,  by  elevating  the 
level  of  Hg.  The  vapor  pressures  of  the  analyzed  mixture  at  various  constant 
temperatures  were  then  read  with  the  aid  of  an  adjacent  millimeter  scale.  Curves 
were  plotted  from  the  results  and  readings  for  regular  intervals  of  concentration 
and  temperature  made. 

By  means  of  a  modification  of  the  above  apparatus  the  author  was  also  able 
to  estimate  the  partial  pressure  of  the  ammonia  and  of  the  water  of  each  mix- 
ture. Tables  for  these  values  are  given.  Data  have  also  been  calculated  for 
the  latent  heat  of  evaporation  of  aqueous  ammonia  solutions. 

INFLUENCE  OF  SALTS  AND  OTHER  COMPOUNDS  ON  THE  VAPOR  PRESSURE  OF 
AQUEOUS  AMMONIA  SOLUTIONS. 

(E.  G.  Perman,  J.  Chem.  Soc.  (Lond.),  81,  480,  1902.) 

Vapor  pressure  determinations  were  made  as  above  described  on  aqueous 
solutions  of  the  following  compositions  —  (a)  10.43%  Urea  -+-  16.36%  NHs, 
(b)  5-29%  Urea  +  17.22%  NH3,  (c)  4.56%  Mannitol  +  12.27%  NH3,  (d)  3.05% 
K2S04  +  749%  NH3,  («)  5.27%  NH4Cl  +  16.85%  NH3,  (/)  10.26%  NH4C1 
+  12.9%  NH3f  (g)  2.68%  CuS04  +  14-65%  NH3,  (h)  3.94%  CuSO4  +  6.54% 
NH3. 

The  author's  data  were  plotted  on  cross  section  paper  and  the  following  values 
read  from  the  curves. 

t°.  Vapor  Presure  of  Each  Solution  in  mm.  of  Mercury. 


(a) 

(b) 

to 

(d) 

(e) 

(/) 

tt 

(*) 

20 

204 

200 

120 

.  .  . 

193 

130 

155 

.  .  . 

30 

325 

325 

198 

.  .  . 

302 

220 

235 

87 

40 

485 

500 

3H 

200 

471 

345 

365 

145 

50 

715 

727 

465 

304 

695 

522 

545 

223 

60 

1050 

1060 

705 

453 

975 

770 

344 

In  an  earlier  paper  Perman  (1901)  gives  data  similar  to  the  above  for  the 
vapor  pressure  of  ammonia  in  aqueous  solutions  of  sodium  sulfate. 


35  AMMONIA 

MUTUAL  SOLUBILITY  OP  AQUEOUS  AMMONIA  AND  POTASSIUM  CARBON- 

ATE  SOLUTIONS. 

(Newth  —  J.  Chem.  Soc.  77.  776,  1900.) 

The  solutions  used  were:  Potassium  Carbonate  saturated  at  15° 
(contained  57.2  grams  K2CO3  per  100  cc.).  Aqueous  Ammonia  of 
0.885  Sp.  Gr.  (contained  about  33  per  cent  ammonia).  The  determina- 
tions were  made  by  adding  successive  small  quantities  of  one  of  the 
solutions  to  a  measured  volume  of  the  other,  and  observing  the  point 
at  which  opalescence  appeared. 

Saturated  K2CO3  in  Aq.  Ammonia.  Aq.  Ammonia  in  Saturated 


t*.        cc.  KaCOa  per         %K2COa  Solution  cc.  Ammonia       %K2COa  Solution 

100  cc.  Ammonia,  in  Mixture.  in  100  cc.  K2COa.      in  Mixture. 

i  2.0  2.0  37.5  72.7 

6  3.0  3.0  47-5  67-6 

ii  5-0  4-7  52-5  65-o 

16  6.5  6.1              %  60.0  63.0 

21  8.5  8.0  77-5  56-3 

26  10.5  9.5  105.0  49-0 

31  12.5  ii. i  152.5  39.0 

38  20.0  16.6  i9S-o  33 -° 

39  21  .o  17.0  220- o  31-0 

42  25.0  20.0  250.0  28.5 

43  35.0  26.0  285.0  26.5 

Above  43°  the  solutions  are  completely  miscible.  If  10  per  cent  of 
water  is  added  to  each  solution  the  temperature  of  complete  miscibility 
is  lowered  to  25°.  The  mutual  solubilities  are: 

Per  cent  K2CO3  Solution  in; 

t°.  Ammonia  K2CO3  Sol. 

Layer.  Layer. 

o  8  62 

10  ii  52 

20  15  38 

25  (crit.  pt.)  25 

With  the  addition  of  12.9  per  cent  of  water  to  each  solution  the 
temperature  of  complete  miscibility  (crit.  pt.)  is  lowered  to  10°.  With 
the  addition  of  18.1  per  cent  water  this  temperature  becomes  o°. 

SOLUBILITY  OF  AMMONIA  IN  AQUEOUS  SALT  SOLUTIONS. 

(Raoult.) 

In  Calcium  Nitrate  Solutions          In  Potassium  Hydroxide  Solutions 
Gms.  NHa  per  too  Gms.  NHa  per  100 

Cms.  Solvent  in:  Gms.  Solvent  in: 


t*.                  28.38%           In  59.03%  n-25% 

Ca(N03)2.        CMJ88S  KOH 

o            96.25        104.5  72-o            49-5 

8            78.50         84.75  57-o           37-5 

16           65.00          70.5  46-0            28.5 

24  373           21.8 

The  freezing-point  curve  for  mixtures  of  ammonia  and  ammonium  thiocyanate 
is  given  by  Bradley  and  Alexander  (1912). 


AMMONIA  36 

SOLUBILITY  OF  AMMONIA  IN  AQUEOUS  SALT  SOLUTIONS  AT  25°. 

(Abegg  and  Riesenfeld,  1902.) 

The  determinations  were  made  by  the  dynamic  method  of  vapor  pressure 
measurement  previously  used  by  Doyer  (1890),  Konowalow  (1898),  Gahl  (1900), 
and  Gaus  (1900).  It  consists  in  passing  an  indifferent  gas  through  an  aqueous 
ammonia  solution  of  known  concentration  and  calculating  the  vapor  pressure 
from  the  volume  of  indifferent  gas  required  to  remove  a  definite  amount  of 
ammonia  from  solution.  The  indifferent  gas  (H  +  O)  was  generated  by  an 
electric  current  and  its  volume  measured  by  means  of  a  voltmeter.  The  accom- 
panying ammonia  was  removed  by  passing  through  o.oi  n.  HC1  and  estimated 
by  means  of  electrolytic  conductivity.  The  molecular  vapor  pressure  was 
obtained  by  dividing  the  absolute  vapor  pressure,  calculated  from  above  meas- 
urements, by  the  concentration  (normality)  of  the  ammonia.  For  i  n.  am- 
monia in  water  at  25°  the  molecular  vapor  pressure  was  13.45  mm-  Hg;  for 
0.5  n.  solution  it  was  13.27  mm.  Hg. 

Since  it  has  been  shown  by  much  experimental  evidence,  that  Henry's  Law  of 
the  proportionality  of  the  concentration  in  the  liquid  and  vapor  phase  applies 
very  closely  in  the  present  case,  see  also  Gaus  (1900),  it  follows  that  the  am- 
monia pressure  relation  of  two  solutions  of  equal  ammonia  content  is  recipro- 
cally proportional  to  the  solubility  relation  of  the  ammonia  in  them.  Hence, 
to  calculate  the  solubility  from  the  vapor  pressures,  it  is  only  necessary  to  divide 
the  value  for  the  molecular  vapor  pressure  in  H2O  by  that  for  the  salt  solution. 
Thus  the  solubility  of  NH3  in  HzO  becomes  unity.  All  determinations  were 
made  with  i  n.  aqueous  ammonia  in  salt  solution  of  0.5,  i  and  1.5  normality. 
The  figures  therefore  show  mols.  NH3  per  liter  of  the  particular  salt  solution  at 
25°.  In  a  later  paper  by  Riesenfeld  (1903),  additional  determinations  are  given 
for  35°. 


Salt 

Mols.  NH3 

per 

Liter  S 

altS 

iol.  of: 

Salt 

Mols.  NH3  per  Liter  Salt  Sol.  of: 

Solution. 

0.5  n. 

i  n. 

i 

•5n. 

Solution. 

0.5  n. 

i  n. 

i-S  n. 

KC1 

0.930 

0 

.866 

O 

.809 

KCN 

O 

.926 

o 

.858 

O.8O2 

KBr 

0.950 

O 

.904 

O 

•857 

KCNS 

0 

•932 

o 

.868 

0.8l4 

KI 

0.970 

0 

•942 

0 

.900 

K2SO4 

0 

.875 

o 

.772 

0.678 

KOH 

0.852 

o 

.716 

o 

.607 

K2SO3 

o 

.865 

o 

.768 

0.675 

NaCl 

0.938 

o 

.889 

o 

843 

K2CO3 

o 

.788 

o 

.650 

0-554 

NaBr 

0.965 

0 

.916 

0. 

890 

K2C2O4 

0 

.866 

o. 

.771 

0.675 

Nal 

0-995 

o 

.992 

0. 

985 

K2CrO4 

o 

.866 

o 

.771 

0.675 

NaOH 

0.876 

0 

.789 

o. 

7l6 

CH3COOK 

0 

.866 

o. 

765 

0.685 

LiCl 

0.980 

I 

.008 

I. 

045 

HCOOK 

0 

.868 

o. 

760 

0.678 

LiBr 

I  .OOI 

I 

.040 

I. 

090 

KBO2 

o 

,814 

0. 

677 

0.560 

Lil 

1.030 

I 

.094 

I  . 

190 

K2HPO4 

0. 

860 

o. 

749 

0.664 

LiOH 

0.863 

0 

.808 

0. 

768 

Na2S 

0. 

887 

0. 

795 

0.726 

KF 

0.839 

0.722 

p. 

626 

*KC1O3 

0.927     

KNO3 

0.923 

o 

.862 

o. 

804 

*KBrO3 

o. 

940 

. 

.  . 

.  .  . 

KN02 

0.920 

0 

.855 

0. 

798 

*KIO3 

0. 

951 

•  . 

*  These  salt  solutions  are  0.25  normal. 

Konowalow  (1898)  expressed  the  results  of  determinations  of  the  solubility 
of  ammonia  in  aqueous  silver  nitrate  by  the  equation  H  =  56.58  (m  —  2  n)  in 
which  H  =  partial  pressure  of  NH3  in  mm.  of  Hg.,  m  =  molecular  concentra- 
tions of  NH3  and  n  =  molecular  concentration  of  AgNO3.  Similar  results  are 
given  in  later  papers  (Konowalow,  1899,  a,  b)  for  a  large  number  of  other  salt 
solutions. 

Gaus  (1900)  gives  data  for  the  vapor  pressure  of  ammonia  in  aqueous  0.4  n 
solutions  of  about  20  salts,  only  a  few  of  which  occur  in  the  above  table. 


37  AMMONIA 

SOLUBILITY  OF  AMMONIA  IN  ABSOLUTE  ETHYL  ALCOHOL. 

(Delepine —  J.  pharm.  chim.  [5]  25,  496,  1892;  de  Bruyn  —  Rec.  trav.  chim.  n,  112,  '92.) 

Gms.  NHa        Gms.  NH3  per  100  Gms.  Solution.     Gms.  NH3  per  100  Gms.  Alcohol 


t  . 

Density. 

per  100  cc. 
Solution. 

(Delepine.) 

(de  Bruyn.) 

(Delepine.) 

(de  Bruyn.) 

o 

0.782 

13 

•05 

20 

•95 

19 

•7 

26 

•5 

24 

•5 

5 

0.784 

12 

.00 

19 

.00 

17 

•5' 

23 

•o 

21 

.2 

10 

0.787 

10 

•8S 

16 

•43 

15 

.0 

19 

.6 

17 

.8 

15 

0.789 

9 

.20 

13 

.00 

13 

.2 

15 

•  0 

15 

.2 

20 

0.791 

7 

•5° 

10 

.66 

II 

•5 

II 

•9 

13 

.2 

25 

0-794 

6 

.00 

10 

.0 

10 

.0 

II 

.0 

II 

.2 

30 

0.798 

5 

•J5 

9 

•  7^ 

8 

.8 

10 

•7 

9 

•5 

According  to  Miiller  (1891),  one  volume  of  alcohol  absorbs  340  volumes  of 
ammonia  at  20°  and  760  mm.  pressure. 

SOLUBILITY  OF  AMMONIA  IN  AQUEOUS  ETHYL  ALCOHOL. 

(Delepine.) 
In  06%  Alcohol.  In  90%  ^Alcohol.  In  8o%AAlcohol. 


t°.                 Sp.  Gr.       G.  NH3  per 

Solution,     zoo  Gms.  Sol. 

Sp.  Gr. 
Solution. 

G.  NH3  per    * 
100  Gms.  Sol. 

fc'Sp.  Gr.        G.  NHS  per 
Solution.     100  Gms.  Sol. 

0 

O 

•783 

24 

•5 

O 

.800 

30.25 

0.8o8 

39-o 

10 

0 

.803 

18 

.6 

0 

•794 

28.8 

O.Soo 

28.8 

20 

o 

.788 

14 

.8 

0 

•795 

15-8 

0.821 

19.1 

30 

o 

.791 

10 

•7 

O 

.796 

II-4 

0.826 

12.2 

In  60% 

Alcohol. 

In  so%_  Alcohol. 

t  . 

Sp.  Gr. 
Solution. 

G.  NH3  p 
100  Gms.  S 

. 

Sp.  Gr. 
Solution. 

G.  NH3  per" 
100  Gms.  Sol. 

0 

0-830 

50-45 

0.835 

69.77 

10 

0.831 

37-3 

0.850 

43.86 

20 

0.842 

26.1 

0.869 

33-8 

30 

0.846 

21  .2 

0.883 

25.2 

SOLUBILITY  OF  AMMONIA  IN  ABSOLUTE  METHYL  ALCOHOL. 

(de  Bruyn  —  Rec.  trav.  chim.  n,  112,  '92.) 

0       G.  NH3  per  100  Grams.  0       G.  NH3  per^ioo  Grams. 

Solution.        Alcohol.  Solution.        Alcohol. 

O  29.3  41.5  20  19.2  23.8 

5        26.5        36.4  25        16.5        20.0 

10        24.2        31.8  30        14.0        16.0 

15        21.6        27.8 

SOLUBILITY  OF  AMMONIA  IN  ETHYL  ETHER. 

(Christoff,  1912.) 

Results  in  terms  of  the  Ostwald  Solubility  Expression  (see  page  227),  at 
o°  =  17.13,  at  10°  =  12.35,  at  15°  =  10.27. 

Freezing-point  lowering  curves  (Solubility,  see  footnote,  page  i)  are  given 
by  Baume  and  Perrot  (1910),  (1914)  for  mixtures  of  ammonia  and  methyl 
alcohol  and  for  mixtures  of  ammonia  and  methyl  ether;  results  for  ammo- 
nium and  potassium,  ammonium  and  sodium,  and  ammonium  and  lithium  are 
given  by  Ruff  and  Geisel  (1906);  results  for  ammonium  and  hydrogen  sulfide 
are  given  by  Scheffer  (1912). 

SOLUBILITY  OF  AMMONIA  IN  HYDROXYLAMINE. 

(de  Bruyn,  1892.) 

100  gms.  of  the  sat.  solution  contain  26  gms.  NH3  at  ±0°  and  19-20  gms.  at 
I50-i6°. 


AMMONIA  38 

DISTRIBUTION  OF  AMMONIA  BETWEEN: 
Water  and  Amyl  Alcohol  at  20°.          Water  and  Chloroform  at  20°. 

(Herz  and  Fischer  —  Ber.  37,  (Dawson  and  McCrae  —  J   Ch.  Soc.  79,  496,  '01;  see 

4747.  '04)  also  Hantsch  and  Sebaldt  —  Z.phys.Ch.ao,  258,  '99.) 


Cms  .  NHg  per  100  cc. 

G 

.  M.  NHa  per  too  cc. 

Cms 

.  NHaper  100  cc. 

G.  M.  NH3  per  100  cc. 

'    Aq. 

Alcoholic 

Aq. 

Alcoholic 

Aq. 

CHC13 

Aq. 

CHCla 

Layer 

Layer. 

Layer. 

Layer. 

Layer. 

Layer. 

Layer. 

Layer. 

o-5 

0. 

.072 

O 

•25 

O 

•0035 

O 

.2 

O.OO7 

O.OI 

0.00038 

I    0 

0 

.147 

O 

•50 

0 

.0073 

0 

•4 

0-015 

0-02 

0.00073 

2  -O 

O 

.272 

I 

.00 

0 

.0148 

0 

.6 

0.023 

C.03 

O.OOII4 

30 

0 

438 

2 

•  oo 

0 

-02Q5 

O 

.8 

0.031 

O.O4 

O.OOI52 

40 

0 

595 

3 

.00 

O 

•  0460 

I 

•  o 

0.039 

O.O5 

0.00193 

5-° 

0 

•756 

I 

.2 

0-046 

0.06 

0.00232 

I 

•4 

0-055 

0.08 

O.OO3II 

I 

.6 

0-063 

o.io 

0-00396 

For  calculations  of  above  distribution  results  see  Note,  page  6. 

Additional  data  for  the  distribution  of  ammonia  between  water  and  chloroform 
are  given  by  Dawson  and  McCrae  (1900),  (19010),  (19016);  Dawson  (1906), 
(1909);  Abbott  and  Bray  (1907);  Sherrill  and  Russ  (1907);  Bell  (1911),  and 
by  Moore  and  Winmill  (1912).  The  results  show  that  with  increase  of  concen- 
tration of  ammonia,  the  relative  amount  in  the  aqueous  layer  diminishes.  Thus 
Bell  found  that  at  25°  the  distribution  ratio  is  22.7  when  the  aqueous  layer  con- 
tains 1. 02  gm.  mols.  NH3  per  liter  and  only  10  when  12.23  Sm-  mols.  NH3  are 
present  in  the  aqueous  layer.  The  influence  of  increase  of  temperature  was 
also  found  to  be  in  the  direction  of  diminution  of  the  relative  amount  in  the 
aqueous  layer. 

The  influence  of  the  presence  of  a  large  number  of  salts  in  the  aqueous  layer 
has  been  studied  by  several  of  the  above-mentioned  investigators.  In  the  case 
of  copper,  zinc  and  cadmium  salts  (Dawson  and  McCrae,  1900),  {Dawson,  1909), 
the  distribution  ratio  varied  with  salt  concentration  in  a  manner  indicating  that 
metal  ammonia  compounds  were  formed. 

Results  for  the  effect  of  KOH,  NaOH  and  Ba(OH)2  on  the  distribution  at  18° 
are  given  by  Dawson  (1909). 

Results  for  the  effect  of  ammonium  chromate  upon  the  distribution  at  25° 
are  given  by  Sherrill  and  Russ  (1907). 

Results  for  the  distribution  of  ammonia  between  water  and  mixtures  of  chloro- 
form and  amyl  alcohol  at  25°  are  given  by  Herz  and  Kurzer  (1910). 


DISTRIBUTION  OF  AMMONIA  BETWEEN  TOLUENE  AND  AIR. 

(Hantzsch  and  Vagt,  1901.) 

Gms.  NHajrer  1000  cc.  Mols.  NHs  per  1000  cc. 

Air.  C6H8CH3  Layer.  Air. 


o  0.366  0.0396  0.0215  0.00233 

10  °-357  °-°435  0.0210  0.00256 

20  0.326  0.0451  0.0192  0.00265 

30  0.286  0.0462  0.0168  0.00272 


39 


AMMONIUM  ACETATE 


AMMONIUM  ACETATE  CH,COONH4. 

100  cc.  of  sat.  solution  in  acetone  contain  0.27  gm.  CH3COONH4  at  19°. 

(Roshdestwensky  and  Lewis,  1912.) 

AMMONIUM  ARSENATES. 

THE  SYSTEM  AMMONIA,;  ARSENIC  TRIOXIDE  AND  WATER  AT  30°. 

(Schreinemakers  and  de  Baat,  1915.) 


Gms.  per  100  Gms.  Sat.  Sol. 

NHj. 
0 
I.4I 

2.78 

2.86 
2.88 

2.26 
10.98 
20.49 

21  .17 
18-43 

Solid  Phase. 

AsA 


Gms.  per  100  Gms.  Sat.  Sol. 


NH3. 

3-13 
3-91 
6-95 

9-93 
4.28 


Data  are  also  given  for  the  system  NH4C1 
100  gms.  H2O  dissolve  0.02    gm.  NH4CaAsO4.£H2O. 
"      "       "          "       0.014    "    NH4MgAsO4.*H8O. 


AS203. 

12.30 

7-63 
4.72 
3.20 
2.16 

+  H20  at  30°. 


Solid  Phase. 


(Field,  1873.) 


SOLUBILITY  OF  AMMONIUM  MAGNESIUM  ARSENATE  IN  WATER  AND  IN 
AQUEOUS  SOLUTIONS  OF  AMMONIUM  SALTS. 

(Wenger,  1911.) 
Gms.  NH4MgAsO4  per  100  Gms.  of  Each  Solvent. 

Solid  Phase. 
NH4MgAs04.6HzO 


Water. 

Aq.  5% 
NH4N03. 

Aq.  5% 
NH4C1. 

Aq.* 
NH4OH. 

NH4OH  t 

Aq. 
NH4OH  f 

+10% 

-vfrr  pi 

O 

O 

•0339 

0.092 

0 

.084 

0 

.0087 

... 

JN±14C1. 

20 

0 

.0207 

0. 

114 

0 

.113 

0 

.0096 

0.013 

0.032 

30 

0. 

118 

O 

•113 

40 

0 

.0275 

0. 

139 

0 

.190 

0 

.0117 

50 

o 

.0226 

0. 

189 

O 

.189 

0 

.0100 

•  .  . 

... 

60 

O.O2IO 

o. 

211 

0 

.219. 

0 

.0090 

0.047 

0.054 

70 

0 

.0156 

0. 

I89 

0 

.221 

o 

.0095 

... 

... 

80 

O 

.0236 

o. 

189 

O 

.231 

0 

.0091 

*  Composed  of  i  part  NHt(4  =  0.96)  +  4  parts  KfeO. 

t  Contained  4  parts  NHi(d  =  0.96)  per  100  parts  NH4C1  solution. 

AMMONIUM  BENZOATE  C.H,COONH4. 

SOLUBILITY  IN  WATER  AND  IN  AQUEOUS  ALCOHOL  AT  25°. 

(Seidell,  1910.) 


Gms.  CzHsOH 
per  100  Gms. 
Solvent. 

d&  of  Sat.  Sol. 

Gms. 
C6H6COONH4 
per  100  Gms. 
Sat.  Sol. 

Gms.  C2HsOH 
per  100  Gms. 
Solvent 

0 

1.043 

18.6 

60 

10 

I  .027 

18 

70 

20 

1.  012 

18 

80 

30 

0.997 

18.1 

90 

40 

0.979 

18 

95 

50 

0.956 

17 

100 

<fe  of  Sat.  Sol. 


Gnis. 

C6H5COONH4 

per  100  Gms. 

Sat.  Sol. 


0.930  15 

0.901  12.2 

0.864  8.3 

0.828  4.2 

O.SlO  2.7 

0.796  1.6 

100  gms.  water  dissolve  19,6  gms.  C6H5COONH4  at  14°  5,  du  of  sat.  sol.  = 

1.042.  (Greenish  and  Smith,  1901.) 

ioo  gms.  water  dissolve  83.33  gms.  C6H6COONH4  at  b.-pt.  (U.  S.  P.) 

100  gms.  glycerol  dissolve  10  gms.  C6HBCOONH4  at  room  temp.  (Hager.) 


AMMONIUM  BORATES 


40 


THE  SYSTEM  AMMONIA,  BORIC  ACID  AND  WATER  AT  30°  AND  AT  60°. 

(Sborgi,  1913-15;  Sborgi  and  Meccacci,  1916.) 

Results  at  30°.  Results  at  60°. 


(NI 
O 
0 

•23 
.70 

B 

4 
7 

.81 

.20 

oana  irnase. 
Jtis-ljOs 

n 

(NH4)2O. 
0 
0.78 

B203. 

7-39 

12.12 

ouiiu  .rua.se. 

H3BO3 

0 

.78 

7 

.62 

HJBOH-  1.5.8 

I 

.42 

15- 

60 

H3B03+  1.5.8 

0 

•99 

7 

•53 

1.5-8 

I 

.70 

15- 

29 

1.5-8  " 

I 

.08 

7 

.66 

tt 

3 

•23 

18. 

60 

a 

I 

.71 

9 

•13 

" 

4 

.02 

20. 

38 

1.5-8+1. 

4.6 

2 

•25 

10 

tt 

4 

.88 

21  . 

76 

1.4.6 

2 

.89 

12 

-32 

It 

6 

.41 

24. 

32 

" 

3 

•13 

12 

•59 

tt 

7 

.90 

27. 

3i 

1.4.6+1. 

2.4 

3 

•43 

6 

•35 

24.5 

7 

-83 

26. 

76 

1.2.4 

6 

.51 

4 

48 

tt 

7 

.91 

17- 

57 

u 

10 

•45 

3 

•37 

" 

9 

•57 

13- 

56 

(i 

18 

•05 

2 

.02 

11 

15 

•45 

8. 

33 

(i 

24.80 

I 

•51 

" 

19 

•47 

5- 

92 

" 

30 

-56 

I 

.22 

(t 

22 

•57 

4- 

47 

" 

45 

•34 

0 

.84 

U 

1.5-8 

=  (NH4)20, 

,5B203.8H20 

1.4.6  = 

(NH4)20.4B203.6H20 

2-4-5 

=  2(NH4)20.4B203.5H02 

1.2.4  = 

(NH< 

)20.2B203.4H20 

AMMONIUM  BROMIDE   NH4Br. 

SOLUBILITY  IN  WATER. 

(Smith  and  Eastlack,  1916.) 

(Determinations  by  sealed  tube  method.) 

Gms.  NH4Br 
per  too  Gms.  t°. 

HzO. 

107.8  130 

116.8  137.3 

126  140 

135-6  150 

145.6  160 

156.5  170 
167.8 

SOLUBILITY  OF  AMMONIUM  BROMIDE  IN  ABSOLUTE  ETHYL  ALCOHOL, 
METHYL  ALCOHOL,  AND  IN  ETHER. 

(Eder;  de  Bruyn  —  Z.  phys.  Ch.  10,  783,  '92.) 


Cms  NH4Br 

t°. 

per  100  Gms. 

t°. 

H20. 

—  17  Eutec. 

47-3 

60 

0 

60.6 

70 

10 

68 

80 

20 

75-5 

90 

30 

83-2 

£00 

40 

91.1 

no 

5° 

99.2 

120 

Gms.  NH4Br 

per  100  Gms. 

HzO. 

1 80 

Transition  pt. 
192.3 
202.5 
213.4 
225-5 


In  Ethyl  Alcohol. 
Gms.  NHiBr 
per  100  Grams. 

15 
19 

78 

Solution. 
2.97 
3.12 

9-50 

Alcohol. 
3.06 
3-22 
10.50 

In  Methyl  Alcohol. 
Gms 


per  100  Grams. 


Solution 


II. I 


Alcohol. 


I2-5 


In  Ether  (o  729  Sp.  Gr.). 
Gms.  NHjBr 
per  100  Grams. 

Ether. 
0.123 


loo  cc.  ethyl  alcohol  of  di6  =  0.8352  dissolve  7.8  grams  NH4Br  at  15°,  di&  of 

sat.  sol.  =  0.8848.  (Greenish,  1900.) 

100  cc.  anhydrous  hydrazine  dissolve  no  gms.  NH4Br  at  room  temp,  with 

evolution  of  ammonia.  (Welsh  and  Broderson,  1915.) 


4i  AMMONIUM  BROMIDE 

SOLUBILITY.  OF  AMMONIUM  BROMIDE  AT  25°  IN  MIXTURES  OF: 

(Herz  and  Kuhn,  1908.) 


Methyl  and  Ethyl 
Alcohols. 

Propyl  and  Methyl 

Alcohols. 

-A 

Propyl  and  Ethyl 
Alcohols. 

t 

Gms. 

/"•* 

Gms. 

Gms. 

Gms. 

<    Gms. 
CHsOH  per 
zoo  Gms. 
Solvent. 

Sat.  Sol. 

NH4Br 
per  100 
cc.  Sat. 
Sol. 

CsHyOHper      d  ^  of 
100  Gms.       Sat.  Sol. 
Solvent. 

NH4Br 
per  100 
cc.  Sat. 
Sol. 

C3H7OH 
per  100 
Gms.  Sol- 
vent. 

Sat.  Sol. 

NftBr 
perioo 
cc.  Sat. 
Sol. 

0 

0 

.8065 

2-55 

0 

0.8605 

9.83 

0 

0.8065 

2-55 

4-37 

0 

.8083 

2.99 

II 

.11 

0.8524 

8.51 

8. 

5i 

0.8o62 

2.51 

10.40 

o 

.8117 

3.2I 

23 

.8 

0.8426 

6.90 

17- 

85 

0.8052 

2-37 

41.02 

0 

.8252 

5.06 

65 

.2 

0.8184 

3.08 

56. 

6 

0.8048 

1.63 

80.69 

o 

.8501 

8.13 

91 

.8 

o  .  8097 

1.28 

88. 

6 

o  .  8042 

I.  II 

84.77 

o 

.8508 

8.47 

93 

•75 

0.8089 

1-25 

91. 

2 

o  .  8049 

I  .05 

91.25 

0 

.8551 

9-34 

100 

0.8059 

95- 

2 

o  .  8059 

1.04 

100 

o 

.8605 

9.83 

100 

0.8059 

0.95 

AMMONIUM  Cadmium  BROMIDE   (NH4)CdBr3.|H2O. 

100  parts  water  dissolve  137  parts  of  the  salt;    100  parts  of  alcohol  dissolve 
18.8  parts  and  100  parts  of  ether  dissolve  0.36  part.  (Eder,  1876.) 

AMMONIUM   Platinum  BROMIDE  (NH4)2PtBr6. 

100  gms.  sat.  aqueous  solution  contain  0.59  gm.  salt  at  20°.      (Halberstadt,  1884.) 

SOLUBILITY  OF  TETRA  ETHYL  AMMONIUM  BROMIDE  N(C2H6)4Br,  AND  OF 
TETRA  METHYL  AMMONIUM  BROMIDE  N(CH3)4Br  IN  ACETONITRILE. 

(Walden  — Z.  phys.  Ch.,  55,  712,  '06.) 

100  cc.  sat.  solution  in  CH3CN  contain  9.59  gms.  N(C2H6)4Br  at  25°. 
100  cc.  sat.  solution  in  CH3CN  contain  0.17  gm.  N(CH3)4Br  at  25°. 

SOLUBILITY  OF  TETRA  ETHYL  AMMONIUM  BROMIDE  IN  WATER  AND 
IN  CHLOROFORM  AT  25°. 


(Peddle  and  Turner,  1913.) 

loo  gms.  H2O  dissolve  279.5  gms-  N(C2H6)4Br. 
100  gms.  CHC13  dissolve  25.01  gms.  N(C2Hs)4Br. 


Data  for  the  distribution  of  propyl  benzyl  methyl  phenyl  AMMONIUM 
BROMIDE  between  water  and  chloroform  at  25°  are  given  by  Wedekind  and 
Paschke  (1910). 

AMMONIUM   CARBONATE   (NH4)2CO3. 

100  gms.  H2O  dissolve  25.4  gms.  ammonium  carbonate,  calculated  as 
C2HnN3O5  at  16.7°  d  of  sat.  sol.  =  1.095.  (Greenish  and  Smith,  1901.) 

100  gms.  of  carefully  purified  glycerol  dissolve  20  gms.  (NH4)2CO3  at  15°. 

(Ossendowski,  1907.) 

AMMONIUM  BICARBONATE   NH4HCO3. 

SOLUBILITY  IN  WATER. 

(Dibbits  — J.  pr.  Ch.  [2]  10.  417,  '74.) 

to          Gms.  NH4HCO3  per  100  Grams.  Grams  NlfrNCOa  per  100  Grams. 

Solution.          Water.  Solution.          Water. 

O  10.6  II-9  20  17.4  21.0 

5  I2-i        13-7  25  J9  3        23.9 

10  13.7        15.8  30  21.3        27.0 

*5  iS-5        18.3 


AMMONIUM  BICARBONATE 


42 


SOLUBILITY  OP  AMMONIUM  BICARBONATE  IN  AQUEOUS  SOLUTIONS  OP 
AMMONIUM  CHLORIDE  SATURATED  WITH  CO2. 

(Fedotieff  —  Z.  phys.  Ch.  49,  168,  '04.) 


Per  1000  cc.  Solution. 


Per  1000  Grams  H2O. 


o 

Wt.OI 

zee.  Sol. 

G. 

NE 

M. 

uci. 

G.  M.        Gms. 
NEUHCOa-  NEUCl. 

Gms 
NH4H 

COa. 

G.M. 
NEUCl. 

0.0 

G.M. 
NEUHCO 

1.22 

Gms. 
3.  NH4C1. 

O*O 

Gms. 
NH4HCOj 

II9.0 

o 

1.077 

4 

.41 

0-37 

235-9 

29 

.2 

5-42 

0.46 

290.8 

36.0 

15 

1.064 

0 

.0 

2.12 

0-0 

I67 

.2 

o.o 

2.36 

o.o 

186.4 

15 

1.063 

0 

•5 

1.84 

26.8 

145 

.2 

0.56 

2.06 

29.9 

162.9 

15 

I  .062 

I 

.0 

I  .59 

53-5 

I25 

•5 

1.13 

1.  80 

60.6 

142.2 

15 

I  .062 

I 

.41 

1.42 

75-4 

112 

.2 

i-59 

1.  60 

85.1 

126.9 

IS 

1.065 

I 

.89 

4.28 

100.8 

101 

.1 

2.18 

1.48 

II6.8 

116.8 

IS 

1.069 

2 

-87 

0-99 

153-3 

78 

.2 

3-42 

1.18 

183.0 

93-3 

IS 

1.076 

3 

.84 

0-79 

205.2 

62 

•5 

J-03 

0.98 

269.3 

77-3 

IS 

1.085 

4 

.82 

0.65 

257-9 

51 

•4 

6.21 

0.84 

332.5 

66.4 

IS 

1.085 

4 

•95 

O.62 

264.8 

48 

•9 

6.40 

0.81 

343-5 

64.2 

30 

... 

o.o 

3-42 

o.o 

270.0 

*o 

... 

7.4 

1.1* 

307.  0 

oi.o 

SOLUBILITY  OF  AMMONIUM  BICARBONATE  IN  AQUEOUS  SOLUTIONS  OP 
SODIUM  BICARBONATE  SATURATED  WITH  CO2. 

(Fedotieff.) 
Per  1000  cc.  Solution.  Per  1000  Grams  H2O. 


t° 

Wt. 

of 

G.M. 

G.M. 

Gms. 

Gms. 

G.M. 

G. 

M. 

Gms. 

Gms. 

I  CC. 

Sol. 

NaHCO3.  NH4HCO3. 

NaHCOa.  NHiHCOa- 

NaHCOa. 

NHiHCOs.  NaHCO3. 

NHiHCOg 

O  -O 

I 

.  <\I' 

o  .0 

110  -O 

0 

I. 

072 

o-53 

1.28 

44.6 

IOI-4 

0-58 

I 

0  A 

•39 

48.2 

J.J.V/  -w 
109.4 

IS 

I. 

064 

0.0 

2.12 

o.o 

167.2 

o.o 

2 

-36 

o.o 

186.4 

15 

I. 

090 

0.63 

1.92 

S2'5 

I5I-3 

0.71 

2 

.16 

59-2 

170.6 

2n 

o«o 

.42 

O-O 

27O.O 

3° 

30 

% 

0.83 

2 

.01 

7o.o 

230.0 

SOLUBILITY  OF  AMMONIUM  BICARBONATE  IN  AQUEOUS  SOLUTIONS  OF 


AMMONIUM  NITRATE. 

(Fedotieff  and  Koltuno'ff,  1914.) 


d  of  Sat. 

Gms.  per  100  Gms.  H2O. 

t° 

d  of  Sat. 

Gms.  per  100  Gms.  HzO. 

. 

Sol. 

NH4NO3. 

NH*HCO3. 

w  • 

Sol. 

NH4NOs. 

NH4HCOs. 

0 

O 

11.90 

IS 

1.242 

103.4 

8.25 

o 

1.265 

1x8 

4-52 

IS 

1.269 

128.9 

7-79 

15 

1.064 

o 

18.64 

15 

1.302 

166.9 

7.46 

15 

I.H3 

23.26 

12.91 

30 

0 

26.96 

15 

1.164 

49-82 

10-33 

30 

... 

231.9 

12-57 

43 


AMMONIUM  BICARBONATE 


SOLUBILITY    OF    MIXTURES    OF    AMMONIUM    BICARBONATE, 
BICARBONATE,  AND  AMMONIUM  CHLORIDE  IN  WATER 
SATURATED  WITH  CO2. 

(Fedotieff.) 


SODIUM 


*«,       *Wt.  of 

*    *           »  *•*•    C*-J 

Gram  Mols.  per 
Gms.  H2O 

IOOO 

Gms.  per  1000  Gms.  HgO. 

Solid 

pu___ 

I  CC.  oOJ 

o     1.114 

'    NaHC03. 
0-59 

NaCl. 
0.96 

4.92 

NaHCOa. 
49.61 

NaCl. 
56.16 

NHiC 

263. 

4 

rnase. 

a+b-h 

o     1.187 

0-12 

4-83 

2.74 

10. 

09 

282 

.6 

146. 

7 

" 

15     1.116 

o-93 

0.51 

6.28 

78. 

18 

29 

.84 

'336. 

2 

" 

15     1.178 

0.18 

4.44 

3-73 

15 

*3 

259 

.8 

199. 

6 

M 

15     1.151 

0.30 

3-09 

4-56 

25- 

22 

180 

.8 

244. 

i 

a  +  c 

r5 

.128 

0.51 

1.68 

5-45 

42. 

87 

98 

.28 

291  . 

7 

" 

15 

.112 

0.99 

o-35 

5-65 

83- 

22 

20 

•47 

302. 

4 

a  +  b 

J5 

.108 

1.07 

0.20 

5.21 

89. 

95 

ii 

.70 

278. 

9 

" 

.106 

I  .12 

o.n 

4.92. 

94- 

14 

6 

•44 

263. 

4 

'* 

15 

.101 

1.16 

0.14 

4.00 

97- 

52 

8 

.19 

214. 

i 

M 

15     i  .090 

o-93 

0-95' 

2.03 

78. 

18 

55 

•58 

108. 

6 

M 

a  = 

NaHC03 

b  = 

NH 

'V-/3j 

c 

- 

NH4C1. 

AMMONIUM  Uranyl  CARBONATE  2(NH4)2CO8UO2CO3. 

(Ebelmen.) 

100  grams  H2O  dissolve  5  grams  of  the  salt  at  15°... 


AMMONIUM   Lead   COBALTICYANIDE   NH4PbCo(CN)6.3H2O. 

(Schuler  —  Sitz.  Ber.  K.  Akad.  W.  (Berlin)  79,  302.) 

100  grams  H2O  dissolve  12  grams  of  the  salt  at  18°. 


AMMONIUM  PerCHLORATE  NH4C1O4. 

SOLUBILITY  IN  WATER. 

(Carlton,  1910.) 


Sp  Gr 

Gms.  NH4C1O4 

t°. 

Sat.  Sol. 

per  100  cc. 
Sat.  Sol. 

o 

1.059 

11.56 

20 

1.098 

20.85 

40 

I.I28 

30.58 

60 

I.I58 

39-05 

t° 

Sp.  Gr. 
Sat.  Sol. 

Gms.  NH4CKX 
per  TOO  cc. 

Sat.  Sol. 

80 

I-I93 

48.19 

100 

1.216 

'  57-01 

107  b.  pt. 

I.  221 

59.12 

.In  a  paper  by  Thin  and  Gumming  (1915),  it  is  stated  that  ammonium  per- 
chlorate  is  "sparingly  soluble"  in  water  and  according  to  one  determination 
at  14.2°,  100  gms.  of  the  sat.  solution  was  found  to  contain  1.735  gms.  NH4C1O4. 
It  is  probable  that  these  authors  have  misplaced  the  decimal  point.  This  ap- 
pears more  probable  since  a  determination  of  the  solubility  in  98.8  per  cent 
ethyl  alcohol  at  25.2°  gave  1.96  gms.  NH4C1O4  per  100  gms.  sat.  solution,  and 
in  98.8  per  cent  alcohol  containing  0.2  per  cent  HC1O4  gave  1.97  gms.  per  100 
gms.  sat.  solution. 


AMMONIUM   PerCHLORATE 


44 


SOLUBILITY  OF  AMMONIUM  PERCHLORATE  AND  SEVERAL  OF  ITS  DERIVATIVES  IN 

WATER  AT   15°.      (Hofmann,  Hobald  and  Quoos  (1911-12).) 

Gms.  Salt  per  Gms.  Salt  per 

100  Gms.  H2O.  100  Gms.  H2O. 

18.5  CH3(C2H5)3NC1O4  23.6 

109 . 6  C3H7(C2H5)3NC1O4  7 . 9 

208.7  (CH3)2(C2H5)2NC104  134.3 
208.7  C2H3(CH3)3NC104  5 
150.9  BrCx2H4(CH3)3NClO4                              3-5 

1 9 . 9  BrC2H2(CHs)2NC104  2 . 5 

'0.5  (OH)C2H4(CH3)3NC1O4  290.7 

3.7  (OH)CH2CH(OH)CH2(CH3)3NC104 155 . 7 

17.9  NO3C2H4(CH3)3NC104  o .  6 

3.1  C3H5(CH3)3NC104  199.5 
10.9  C2H4(NH3C1O4)2  144.5 
15.4  C2H4[(CH3)3NC104]2  ,1.2 

3.7      C3H6[(CH3)3NC104]2  1.5 

2.2  Br2C2H3(CH3)3NClO4  2.2 
BrC3H3(CH3)3NClO4  2.6 

Milbauer  (1912-13)  found  that  100  gms.  of  cold  H2O  dissolve  1.126  gm.  tetra- 
methyl  ammonium  perchlorate  (CH3)4NC1O4  and  100  gms.  alcohol  dissolve 
0.04  gm.  of  the  salt. 

AMMONIUM  CHLORIDE  NH4CL. 

SOLUBILITY  IN  WATER. 

(Mulder;  below  o°,  Meerburg  —  Z.  anorg.  Ch.  37,  203,  1903.) 


CH3NH3C104 

(CH3)2NH2C1O4 

C2H5NH3C1O4 

(C2H5)2NH2C1O4 

(CH3)3NHC1O4 

(CH3)4NC104 

(C2H5)4NC104 

C6H5(CH3)3NC1O4 

ICH2(CH3)3NC1O4 

C2H5(CH3)3NC1O4 

C3H7(CH3)3NC104 


C5H11(CH3)3NC1O4 


Gms.  NHjCl  per  100  Gms. 


Gms.  NH4C1  per  too  Gms. 


»  . 

Solution. 

Water. 

-IS 

19.7 

24-5 

—  10  9 

20-3 

25-5 

~5-7 

21-7 

27.7 

0 

22-7 

29.4 

+  5 

23-8 

31.2 

10 

24.9 

33-3 

15 

26.0 

35-2 

20 

27.1 

37-2 

25 

28.2 

39-3 

30 

29-3 

41.4 

m  .• 

Solution. 

Water. 

40 

31-4 

45-8 

50 

33-5 

5°  4 

60 

35-6 

55-2 

70 

37-6 

60.2 

80 

39-6 

65.6 

90 

41  .6 

7i-3 

100 

43-6 

77-3 

no 

45  -6 

83.8 

115.6 

46.6 

87-3 

Density  of  saturated  solution  at  o°  =  1.088,  at  15°  =  1.077,  at  19°  =  I-°75- 
Eutectic,  Ice  +  NH4C1  =  —  16°  and  19.5  gms.  NH4C1  per  100  gms.  sat.  sol. 
100  gms..  H2O  dissolve  31.25  gms.  NH4C1  at  3.5°,  38.5  gms.  at  25°  and  49.6 

gms.  at  50°.  (Biltz  and  Marcus,  1911.) 

Data  for  the  solubility  of  ammonium  chloride  in  water  at  o°  under  pressures 
up  to  500  atmospheres  are  given  by  Stackelberg,  1896. 

SOLUBILITY  OF  AMMONIUM  CHLORIDE  IN  AQUEOUS  AMMONIUM  BICARBONATE  SO- 
LUTIONS SATURATED  WITH  CO2.    (Fedotieff— z.  Phys.  Ch.  49, 169, 1904.) 


Per  1000  cc.  Solution. 


Per  1000  Gms. 


t<>. 

Wl.  01 

i  cc.  Sol. 

G.M. 
NHJICOa. 

G.  M. 
NH4C1. 

Gms. 
NH4HCO 

Gms.  '' 

O 

1.069 

0-0 

4.60 

o.o 

246.1 

O 
15 

IS 
2O 

1.077 
1.077 
1.085 

o-37 
o.o 
0.62 

4.41 
5-29 

4-95 

29.2 
O-O 
48.9 

235-9 
283.1 
264.8 

J° 
•?r» 

G.  M.        G.  M.  Gms.        Gms. 

NH4HC03.  NH4C1.  NH4HC1.  NEUCl. 

o.o      5.57  o.o     298.0 

0.46      5.42  36.0      290-8 


O.O 

0.8l 

0-0 


6.64      o.o 
6.40    64.2 

7.78 


355-Q 
343-5 
416.4 

7.40    91.0    397.  o, 


o.o 


45  AMMONIUM  CHLORIDE 

SOLUBILITY  IN  AQUEOUS  AMMONIA  SOLUTIONS  AT  o°. 

(Engel  —  Bull.  soc.  chim.  [3]  6,  17,  1891.) 

Milligram  Molecules  Grams"  per  100  cc. 

Sp.  Gr.  of  per  10  cc.  Solution.  Solution. 

SolUtionS.  TT— ' f  VrTrp.tr       ' MTT  ri 

JNiia.  JNrUd.  XMJtliUxl.  JNli^Ll. 

1.067  5.37        45-8  0-92        24.52 

1.054  12-02  45.5  2.05  24.35 

1.031                  38.0  44-5  6-48  23.82 

1.025                  47.0  44-o  8.02  23.56 

1-017                  54-5  43-63  9-30  23.35 

0.993                  80.0  43-12  13-66  23.09 

0.992                  90.0  44.0  15-36  23.56 

o-983                 95-5  44-37  l6-29  23.75 

o-953  J3Q  o  49-75  22-i8  26.63 

0.931  169.75  60.0  28.97  32.14 

SOLUBILITY  OF  NH4C1  IN  AQUEOUS  AMMONIA  SOLUTIONS  AT  17.5°. 

(Stromholm,  1908.) 

Normality  Equiv.  per  Liter.  Gms.  per  1000  cc.  Solution. 

'  NH3.  NH4C1.  '  '    NH3.  NH4C1." 

o  5.435  o  290.8 

0.15  5.420  2.55  290 

4.76  5.082  81  271.9 

SOLUBILITIES  OF  MIXTURES  OF  AMMONIUM  CHLORIDE  AND  OTHER  SALTS 

IN  WATER. 

(Riidorff,  Karsten,  Mulder.) 

Both  salts  present  in  solid  phase; 

te  Grams  per  100  Grams  HgO.  to  Grams  per  100  Grams  H2O. 

19.5  29 . 2  NH4C1+  1 74 . o  NH4N03 *  R  b.  pt.  67.7  NH4C1+ 21.9  KC1    M 

21.5  26.8      "     +  46.5(NH4)2SO4R  14-8  38.8      "     +34-2KNO3K 

20.0  33.8      "     +    ii.6BaC!2          R  18.5  39.8      "      +38.6KNO3K 

18.5  39.2      "     +    i7.oBa(NO3)2   K  14.0  36.8      "      +i4-iK2SO4R 

15.0  28.9      "     +   16.9  KQ  R  18.7  37.9      "     +i3.3K2S04K 

22.0  30.4      "     +   i9.iKCl  R  iS.f  22.9  -f-23.9NaCl   R 

SOLUBILITY  OF  AMMONIUM  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  AMMONIUM 

SULFATE  AT  30°. 
(Wibaut,  1909;  Schreinemakers,  1910.) 

Gms.  per  100  Gms.  Sat.  Sol.  Gms.  per  100  Gms.  Sat.  Sol. 

tNHO.504.     '      NH4C1.    -     SolldPhase-  '(NH4),S04.    '  NH.C1.       '  Sohd  Phase. 

o  29.5  NH4C1              25  18.3     NH4C1+(NH4)2S04 

5  28.5  30  13.2            (NH4)2SOi 

10  25.7  35  8.5 

15  23.2  40  2.8 

20  20.2  "  42  O 

SOLUBILITY  OF  MIXTURES  OF  AMMONIUM  CHLORIDE  AND  COBALT  CHLORIDE 

IN  WATER  AT  25°.    * 

(Foote,  1912.) 
Gms.  per  100  Gms.  Sat.  Sol.  Gms.  per  100  Gms.  Solid  Residue. 

Solid  Phase. 

Mixed  crystals  of 
NH4Cl+CoCl2. 
2H2O 

Mixed  crystals  + 
CoCl2.6H2O 


NH4C1.  CoCl2.  NH4C1.  CoC!2.  H2O. 

17.90  15.63  ...  3.2 

13-59  25.19  83.01  13.52  3^7 

8.75  34.28  35.12  50.66  14.22 

7-45  35-24  34-02  49.64  16.31 

7.62  34.61  7.07  55.27  37.66 


AMMONIUM  CHLORIDE 


46 


SOLUBILITY  OF  AMMONIUM  CHLORIDE  IN  AQUEOUS  HYDROCHLORIC  ACID. 


Results  at  O°.      (Engel,  1888.) 
So  Gr.  of  Sat.         Gms-  P**  I0    cc-  &&•  so1- 


Sol. 
.076 
.069 
.070 

•073 
.078 
.106 
.114 


HCl. 


i.99 

3-93 

7-74 

19. i8 

22.07 


NH4C1. 

24.6l 

23.16 

21.78 

19.36 

14-54 

5-78 

4.67 


Results  at  25°.   (Armstrong  and  Eyre,  1910-11.) 
Gms.  HC1  pe 
too  Gms.  H2( 

O 

O.QI 

1.82 

3.65 
18.25 


d  $f           Gms.  NIL.C1  per 
Sat.  Sol.     100  Gms.  Sat.  Sol. 

.080 

28.3 

.079 
.082 
•083 

27.4 
26.4 
24.6 

.099 

n-3 

SOLUBILITY  OF  MIXTURE  OF  AMMONIUM  CHLORIDE  AND  LEAD  CHLORIDE  IN 
WATER  AT  SEVERAL  TEMPERATURES. 

(At  17°,  50°  and  100°  Demassieux  (1913)  at  25°  Foote  and  Levy,  1907.) 

At  23°.  At  50°.  At  100° 


At  17°. 


Solid  Phase 


Gms.'per  100  Gms.  Sol. 

Gms.  per  100  Gms.  Sol. 

Gms.  per  100  Gms.  Sol. 

Gms.  per  100  Gms.Sol. 

in  Each 

fPbCl,. 

NH4C1. 

PbCl2. 

NH.C1.  * 

'  PbCl2. 

NH4C1.  ' 

PbCJ2. 

NH4C1.  " 

Case. 

0.30 

27 

•03 

... 

... 

0.32 

34 

.14 

1.61 

43 

.42 

NH4C1 

0.52 

26 

.68 

.  .  . 

.  .  . 

2.65 

33 

.62 

4.21 

42 

.91 

" 

0.64 

26 

•49 

I.  2O 

28.15 

3.96 

33 

•56 

.  .  . 

. 

.  . 

"        +1.2 

0.26 

41 

.00 

"        +2.1 

7 
9.88 

T^ 

v/v 

.22 

2.1 

II  .60 

38 

.^2 

12.67 

o 
37 

o 
.62 

"  +1.2 

0-34 

22 

•32 

0-93 

27-45 

3-31 

31 

.90 

/ 
11.40 

O  1 

36 

.29 

1.2 

0.098 

12 

•36 

o-35 

21-59 

1.76 

27 

.16 

8.32 

32 

.64 

" 

0.078 

4 

•93 

0.29 

17.97 

0.71 

19 

.42 

4-54 

26 

.08 

• 

0.078 

4 

•23 

O.II 

10.25 

0.49 

12 

•45 

1.98 

13 

.12 

" 

0.076 

3-48 

0.03 

2-77 

0.48 

4 

.86 

1.76 

8 

•59 

"  +PbCl, 

0.16 

I 

•43 

... 

0.67 

I 

•45 

1.85 

5 

•33 

PbCl2 

0.21 

0 

.96 

.  .  . 

.  .  . 

1.  08 

o 

2.02 

i 

•32 

" 

0.89 

0 

1.69 

0 

3.10 

0 

" 

Gm.  Equiv.    Gm.  Equiv.  PbCla 


NH4C1  per 
iooGms.H2O. 

per  TOO  Gms. 
Sat.  Sol. 

°       i 

^.49  Xio-3 

o.i        '; 

5.10  Xio-3 

O.2 

.9i6Xio-3 

0.4          ' 

.  348XIQ-3 

0-5       ' 

.  263  X  lo"8 

o-55 

.  189X10-3 

[0.6 

.092X10-3 

0.7        < 

).  956X10-3 

Solid  Phase. 


PbCl2 


Solid  Phase. 


2PbCl2.NH4Cl 


1.2  =  NH4C1.2(PbCl2X  2.1  =  2NH4Cl.PbCl2. 

The  following  additional  data  for  the  above  system  at  22°  are  given  by  Bron- 
sted  (1909). 

Gm.  Equiv.  PbCl2 

per  100  Gms. 

Sat.  Sol. 

0.837XIO-3 
0.758XIO-3 
0.695XIO-3 
0.968X10-3 
I . 502  X I0~3 
2.338X10-3 
3.580XIO-3 


Gm.  Equiv. 

NH4C1  per 

100  Gms.  H2O. 

0.8 
i 

2 

3 

4 

6 


7. 29 sat.   6.46  Xio" 


+NH4C1 


YThe  two  curves  intersect  at  0.52  normal  NH4C1. 
SOLUBILITY  OF  MIXTURES  OF  AMMONIUM  CHLORIDE  AND  MAGNESIUM  CHLORIDE 

IN  WATER.      (Biltz  and  Marcus,  1911.) 

„    Gms.  per  loo  Gms.  Sat,  Sol.       „....,.  *<>    Gms.  per  100  Gms.  Sat.  Sol. 

*'      '    MgCl2.    "    NH4C1.  '  ^     -    MgCl,       NH4C1, 

3-5     21.41         5.93   NH4Cl+MgCl2.6H20  3.5   34.43      0.09 

25          20.95        8.78  "  25        35.41      0.09 

50   20.84  12.46     "       50   36-92  0.15 


47 


AMMONIUM  CHLORIDE 


SOLUBILITY  OF  MIXTURES  OF  AMMONIUM  AND  MANGANESE  CHLORIDES'  IN 


WATER  AT  25°. 

(Foote  and  Saxton,  1914.) 


Cms,  per  100  Gms.  Sat.  Sol. 


NH4C1. 

23-97 
22.94 

MnCl2. 

7.97 
9.65 

21.44 
21.  18 

12.31 
13.38 

20.  10 

I5-I9J 

19.70 

\ 

19.75 
19.67 

15-47] 

Solid  Phase. 


a  mixed  crystals 


Cms.  per  100  Cms.  Sat.  Sol. 


NH4C1. 

MnCl2.     ' 

17.09 

18.76 

15.05 

22.44 

13.17 
9.15 

24.52 
29.24 

ft  mixed  crystals  or 
double  salt  2NH4C1. 
MnCl2.2H2O 

5.90 

34.78 

3-77 

39.48 

2.98 

43.71 

2NH4Cl.MnCl2.2H,O 

2.94 

43-44 

+MnCl2.2H20 

a  mixed  crystals  consist  of  NH4C1  with  varying  amounts  of  MnCl2.2H2O; 
/3  mixed  crystals  consist  of  the  double  salt  2NH4Cl.MnCl2.2H2O  with  excess  of 
NH4C1. 

This  case  represents  a  very  rare  type  of  solid  solution  "in  which  a  single  salt 
and  a  double  salt  are  each  capable  of  taking  up  very  considerable  quantities  of 
the  other  to  form  homogeneous  mixed  crystals." 

EQUILIBRIUM  IN  THE  SYSTEM  AMMONIUM  CHLORIDE,   MERCURIC  CHLORIDE, 

WATER  AT  30°. 

(Meerburg,  1908.) 


Gms.  per  100  Gms.  Sat.  Sol. 


'  HgCl2. 

NH4C1. 

0 

29.50 

22.80 

26.91 

42.45 

25-05 

50.05 

24-79 

53-08 

22.77 

58.90 

20.02 

56.38 

18.50 

55.58 

16.82 

57-01 

14.12 

56.26 

13.04 

Solid 
Phase. 


Gms.  per  100  Gms.  Sat.  Sol. 


NH4C1 


+1.1.1 


1    +3-2.1 

3-2.1 

1.2.1  =  HgCl2.2NH4Cl.H2O;  i.i.i  =  HgCl2.NH4Cl.H2O; 
3.2.1  =  3HgCl2.2NH4Cl.H2O;    9.2  =  9HgCl2.2NH4Cl. 

*  In  these  solutions  2  to  3  weeks  were  required  for  attainment  of  equilibrium. 


'    HgCl2. 

NHjCl.' 

57.05 

9.92 

58.65 

9.20 

*5i-83 

8.76 

*46 

7.52 

*35-6o 

5.26 

*32.90 

5-06 

29.65 

3.62 

40.12 

5.13 

21 

2.29 

7.67 

0 

Solid 
Phase. 


3-2.1 


+9-2 


+HgCl2 
HgCl2 


SOLUBILITY  OF  MIXTURES  OF  AMMONIUM  AND  NICKEL  CHLORIDES  IN  WATER 

AT  25°. 

(Foote,  1912.) 


Gms.  per  100  Gms.  Sat.  Sol. 


NH4C1. 

NiCl2.    ' 

26.07 

3.10 

22.27 

8.04 

20.68 

10.32 

Mixed  crystals  of 

17-43 

11.22 

I5.OI 
26.93 

NH4C1  and 
NiCl2.2H20 

IO.2I 

30.56 

Q.l6 

35.70 

Gms.  per  100  Gms.  Sat.  Sol. 


Solid  Phase. 


NH4C1. 

NiCl2. 

7.98 

37-41 

8.07 

37.73 

Mixed  crystals  and 

8.23 

37-45 

NiCl2.6H2O 

8.17 

37.64 

7.51 

37.191 

3-06 

37.98|         NiCl,.6H20 

O 

37.53U 

AMMONIUM  CHLORIDE  48 

SOLUBILITY  OF  MIXTURES  OF  POTASSIUM  CHLORIDE  AND  AMMONIUM 
CHLORIDE  IN  WATER  AT  25°. 

(Fock  — Z.  Kryst.  Min.  28,  353,  '97-) 


Grams  per  Liter 
Solution. 

Mol.  per  cent 
in  Solution. 

Sp.  Gr.  of 

Mol.  per  cent  in 
Solid  Phase. 

'  NH4C1. 

KCl. 

NHiCl. 

KCl." 

•Solutions* 

NHtCi. 

KCl. 

o.oo 

311-3 

o.oo 

IOO-O 

1.1807 

o.o 

100 

22.  Si 

293.3 

9.41 

90.59 

1.1716 

1.  21 

98.79 

35-39 

278.7 

15.04 

84.96 

1.1678 

2.  II 

97.89 

89.17 

273.2 

34.26 

65-74 

1.1591 

6.18 

93-82 

127.8 

234.6 

46.59 

53-44 

1-1493 

8.90 

91.10 

147.2 

204.2 

5I-63 

48.37 

1.1461 

Jo-  53 

89.47 

197-3 

157.7 

63.56 

36-44 

1.1391 

17.86 

82.14 

232.5 

116.8 

73-49 

26.51 

1.1326 

60.20 

39-80 

244.5 

123.0 

73-48 

26.52 

1.1329 

76.88 

23.12 

261.9 

III.O 

79.10 

20.90 

1.1245 

97-51 

2.49 

259.0 

102.2 

82.14 

17.86 

I.I2I2 

97-79 

2.21 

278.6 

53  -16 

87.96 

12.04 

I.I009 

98.85 

^S 

320.7 

31-24 

93-45 

6-55 

I.09I2 

99-33 

0.67 

273-5 

o.oo 

100.00 

o.oo 

1.0768 

100  .0 

o.oo 

The  following  additional  data  for  the  above  system  are  given  by  Biltz  and 
Marcus  (1911).  The  results  show  that  NH4C1  +  KCl  form  a  series  of  mix- 
crystals  broken  by  a  gap  which  extends  between  about  20  and  98  mol.  per  cent 
NH4C1  in  the  crystals. 

Composition  of  Sat.  Solution.  Composition  of  Solid  Phase. 


Gms.  per  icx)  Gms. 

Mols.  per  1000  Mols. 

Gms.  per  100  Gms.             Mnl   <£, 

Sat. 

Sol. 

H,0. 

Crystals. 

NH4C1  in 

NH4C1. 

KCl. 

NHiCl. 

KCl/ 

NHtCl. 

KCl. 

Crystals. 

5-13 

22  .29 

23.8 

74.2 

I.  21 

98.79 

1.7 

7 

20.40 

32.5 

67.9 

2.22 

97.78 

3.1 

ii 

18.04 

52.2 

61  .4 

4 

96 

5-5 

13-73 

16.11 

65.9 

55-5 

5.89 

94.11 

8 

15.46 

14-53 

74.4 

50.2 

7-24 

92.76 

9.8 

19.54 

12.  l6 

96.3 

43 

II  .20 

88.80 

14.9 

22.04 

10.49 

109 

37-4 

16.90 

83.10 

22.1 

21.68 

10.40 

109 

37-4 

26.04 

73.96 

32.9 

21.95 

10.48 

109 

37-4 

97.60 

2.40 

98.3 

24.30 

6.48 

1x8.2 

22.6 

98.28 

1.72 

98.8 

These  authors  also  give  data  for  the  ammonium  chloride  carnellite  and 
potassium  chloride  carnellite  diagram  at  25°. 

SOLUBILITY  OF  MIXTIJRES  OF  AMMONIUM  AND  POTASSIUM  CHLORIDES  IN  WATER 

AT  25°,  65°  AND  90°. 

(Uyeda,  1912.) 

The  results  as  presented  by  Uyeda  show  the  percentage  composition  of  the 
dissolved  mixture  and  of  the  undissolved  residue  in  the  several  cases,  but  not 
the  quantity  of  salts  dissolved.  Mixed  crystals  were  formed  over  certain  ranges 
of  concentration  at  each  temperature. 

Data  for  the  cryohydric  temperatures  and  composition  of  the  saturated  solu- 
tions of  mixtures  of  the  chlorides,  nitrates  and  sulfates  of  ammonium,  potas- 
sium and  sodium  are  given  by  Mazatto  (1891). 


49 


AMMONIUM  CHLORIDE 


SOLUBILITY   OF   AMMONIUM    CHLORIDE    IN   AQUEOUS    {SOLUTIONS   or 
SODIUM  CHLORIDE  SATURATED  WITH  CO2. 

(Fedotieff.) 


Per  1000  cc.  Solution. 


Per  1000  Cms.  H2O. 


t°.     Wt.of 

G.  M. 

G.  M. 

Cms. 

Gms. 

G.  M. 

G.  M. 

Gms. 

Gms. 

i  cc.  Sol. 

NaCl. 

NH4C1. 

NaCl. 

NH4C1. 

NaCl. 

NHiCl. 

NaCl. 

NH4C1. 

0 

.069 

0-0 

4.60 

0 

.0 

246 

.1 

o.o 

5-57 

o.o 

298.0 

O 

.185 

4.04 

2.26 

236 

•5 

121 

.0 

4.89 

2-73 

286.4 

146.1 

15 

.077 

0-0 

S-29 

O 

•o 

283 

.1 

o.o 

6.64 

o.o 

355-Q 

15 

.097 

0.81 

4.71 

47 

•5 

252 

.1 

1.02 

5-91 

59-8 

316.4 

15 

.120 

1.68 

4-13 

98 

.0 

221 

•7 

2.09 

5-i8 

122.4 

277.0 

15 

•*S3 

2.87 

3-38 

168 

•  o 

180 

•7 

3-57 

4.20 

208.9 

224.7 

15 

•175 

3-65 

2.98 

213 

•5 

159 

•4 

4-55 

3-72 

266.8 

198.8 

30 

o.o 

7.78 

0-0 

416.4 

30     1.166 

3-30 

3-70 

J93 

•  o 

I98 

.0 

4.26 

4-77 

249.0 

255-4 

45       ••• 

o.o 

9-03 

o-o 

483.7 

AC 

4-0 

6.02 

233.9 

322.1 

SOLUBILITY  OF  AMMONIUM  CHLORIDE  IN  AQUEOUS  ETHYL  ALCOHOL  AT  15°  AND 

AT  30°. 


Gms.  C2HfiOH  per 
joo  Gms.  Solvent.         ' 

ms.  NELjCl  per  100  C 

ims.  Solvent  at: 

15°. 

30°. 

0 

35-2 

40.4 

20 
40 
60 

80 

25 
16.8 

9-5 

4 

29.7 
19 

5-3 

92.3 
100 

0^6 

.  .  . 

Results  at  15°  by  interpolation  from  Gerardin 
;Bruyn  (1892).     Those  at  30°  from  Bathrick  (185 

(1865),  Greenish 
,6). 

(1900)  and 

100  gms.  absolute  methyl  alcohol  dissolve  3.35  gms.  NH4C1  at  19°. 

100  gms.  98%  methyl  alcohol  dissolve  3.52  gms.  NH4C1  at  19.5°. 

(deBruyn,  1892.) 

SOLUBILITY  OF  AMMONIUM  CHLORIDE  IN  MIXTURES  OF  SEVERAL  ALCOHOLS 

WITH  WATER. 

(Armstrong,  Eyre,  Hussey  and  Paddington  (1907);  and  Armstrong  and  Eyre  (1910-11.) 
Gm.  Mols.  Al-  Gms.  NH4C1  per  100  Gms.  Sat.  Solution  in: 


Gms.  H2O. 

Aq.  CH3OH. 

Aq.  CjHsOH. 

Aq.  C3H7OH. 

O 

0 

23 

23 

23 

0 

o 

•25 

22 

.8 

22 

.6 

22. 

7 

0 

0 

•50 

22 

.6 

22 

.2 

22. 

3 

O 

I 

22 

.1 

21 

•5 

21. 

i 

0 

3 

20 

•5 

19 

.  . 

25 

0 

28 

•3 

28 

•13 

(1.0805) 

28. 

3 

25 

0 

•25 

28.1 

28 

(i 

.0780) 

28.1 

25 

0 

•50 

27 

•9 

27 

.6 

d 

•0753) 

27. 

5 

25 

I 

27 

.6 

27 

d 

.0704) 

26. 

6 

25 

3 

26 

.1 

26 

•5 

d 

.0528) 

.  . 

25 

5 

...        22.6 

d 

.0376) 

(Figures  in  parentheses  show  Sp.  Gr.  of  sat.  sols.) 


AMMONIUM  CHLORIDE 


SOLUBILITY  OF  AMMONIUM 

CHLORIDE  IN  SEVERAL  ALCOHOL  MIXTURES  AT  25°. 

(Herz  and  Kuhn,  1908.) 

In  Methyl  and  Ethyl 
Alcohol. 

In  Methyl  and  Propyl 
Alcohol. 

In  Propyl  and  Ethyl 
Alcohol. 

Cms.  CH3OH 
per  100  Gins. 
Solvent. 

Cms.  NH4C1  per 
loo  Gms.  Sat. 
Solution. 

Gms.  C3H7OH 
per  100  Gms. 
Solvent. 

Gms.  NH4C1  per 
100  Gms.  Sat. 
Solution. 

Gms.  C3H,OH 
per  loo  Gms. 
Solvent. 

Gms.  NH4C1" 
per  100  Gms. 
Sat.  Solution. 

0 

o-53 

0 

2.76 

0 

o-53 

10 

0.67 

IO 

2-33 

10 

0.50 

20 

0.80 

20 

1.90 

20 

0.47 

30 

0.98 

30 

1.58 

30 

0.42 

40 

1.18 

40 

1.26 

40 

o-39 

50 

1.40 

50 

1.03 

5° 

0.36 

60 

1.65 

60 

0.82 

60 

0.32 

70 

1.92 

70 

0.60 

70 

0.30 

80 

2.18 

80 

0.41 

80 

0.26 

00 

2.48 

90 

0.30 

90 

O.22 

100 

2.76 

100 

0.18 

100 

0.18 

SOLUBILITY  OF  AMMONIUM  CHLORIDE  IN  AQUEOUS  GLYCEROL  SOLUTIONS  AND 
IN  AQUEOUS  ACETONE  SOLUTIONS  AT  25°. 

(Herz  and  Knoch  —  Z.  anorg.  Chem.  45,  263,  267,  '05.) 

In  Aqueous  GlyceroL 

(Sp.  Gr.  of  Glycerine  1.255,  Impurity  about  1.5%.) 


Wt.% 
Glycerine. 

O. 

13.28 
25.98 
45-36 
54-23 
83.84 
IOO-OO 


NHiCl  per 
Soluti 

'Millimols" 
585-I 
544-6 
502.9 

434-4 

403-5 
291.4 
228.4 


tion. 
Grams. 

29.16 
26.93 
23  .26 
21. 60 
15.60 
12.23 


Sp.  Gr, 
at  £ 

I .0793 

1.0947 
I.II27 
I.I452 
I .1606 
1.2225 
1.2617 


Vol.% 


O 
10 
20 
30 

40 

*S 
90 


In  Aqueous 

NH4C1  per  too  cc. 
S  1  tion. 

Acetone. 

Sp.  Gr. 
at-^-- 

1.0793 

r.o6i8 
1.0451 
1.0263 
0.9998 
o  .  9800 
0.8390 
0.8274 

L  indicates 

L 

U 

jepa 

MHlimols»     Grams. 
585-1      3I-32 
534-1      28.59 
464.6      24.87 
396.7      21.23 
328.5      17-59 
283.7      15.19 

18.9      i.  oi 
9-4      0.50 

rates  into  two  kyers. 

lower  layer,  U  indicates  upper  layer. 
ioo  cc.  anhydrous  hydrazine  dissolve  75  gms.  NH4C1  at  room  temp,  with 

evolution  of  ammonia.  (Welsh  and  Broderson,  1915.) 

SOLUBILITY  OF    TETRA  ETHYL  AMMONIUM  CHLORIDE  N(C2H5)4C1,  AND 
ALSO  OF  TETRA  METHYL  AMMONIUM  CHLORIDE  N(CH3)4C1  IN  ACETONITRILE. 

ioo  cc.  sat.  solution  in  CH3CN  contain  29.31  gms.  N(C2H5)4C1  at  25°. 
ioo  cc.  sat.  solution  in  CH3CN  contain  0.265  gms.  N(CH3)4C1  at  25°. 

(Walden  —  Z.  physik.  Chem.  55,  712,  '06.) 

SOLUBILITY  OF  TETRA  ETHYL  AMMONIUM  CHLORIDE  IN  WATER  AND  IN 

CHLOROFORM. 

(Peddle  and  Turner,  1913.)  '  «     • 

ioo  gms.  H2O  dissolve  141.0  gms.  N(C2H5)4C1  at  25°. 
ioo  gms.  CHC13  dissolve  8.24  gms.  N(C2H5)4C1  at  25°. 

SOLUBILITY    OF    DIMETHYL  AMMONIUM    CHLORIDE  IN   WATER   AND   IN 

CHLOROFORM. 

(Hantzsch,  1902.) 

ioo  gms.  H2O  dissolve  208  gms.  of  the  salt. 

ioo  gms.  CHC13  dissolve  26.9  gms.  of  the  salt  (temp,  not  stated  in  abstract). 


51  AMMONIUM   CHROMATE 

AMMONIUM    CHROMATES. 

SOLUBILITY  IN  WATER  AT  30°. 

(Schreinemaker  —  Z.  physic.  Chem.  55,  80,  '06.) 
Composition  in  Wt.  per  cent  of: 

'   The  Solution.  The  Residue/  Solid  Phase- 

%  CrO3.      %  NH3.    %  CrO3.    %  NH3. 

6.933  22.35       (NH4)2Cr04 

9.966  16.53  47-59    20.44 

16.973  8.20       

22.53  6.37  38.03     12.15 

27.09  6.87  48.02     12.01        (NH4)2CrO4+(NH4)2Cr2O, 

26.19  5-7o  47-38      8.81                    (NH4)2CraO? 

25-99  5-10  4i -56  7-58 

30.16  3.50  

38.89  3.10  61.08  8.80 

42.44  3-i5  59-72  6.75        (NHOAsO^CNHOaCrAu 

44.08  2.27  54.90  4-14                   (NH4)2Cr3O10 

52.91  i. i i  60.88  3-09 

54.56  1.03  63.07  3.09        (NH4)2Cr3O10+(NH4)2Cr4Olt 

56.57  0.97  65.70  2.95                   (NH4)2Cr4O3 
58.87  0.65  69.74  3.24 

62.48        0.46    71.93      3-10 

63.60        0.40     73-68      1.18 

63.66       0.41    71.47      2*.o; 

62.94        0.21       CrOa 

62.28        o.o         CrO» 

too  gms.  of  the  sat.  aq.  solution  contain  28.80  gms.(NH4)2CrO4  at  30°. 
100  gms.  of  thesat.  aq.  solution  contain 32. 05  gms.  (NH4)2Cr2O7at  30°. 

AMMONIUM  CITRATES. 

SOLUBILITY  IN  AQUEOUS  SOLUTIONS  OF  CITRIC  ACID  AT  30°. 

(van  Itallie,  1908.) 

(Data  read  from  curve  plotted  from  original  results.) 

Gms.  per  too  Gms.  Sat.  Sol. 
•     C.HA.   '        NH3.     '          SohdPhase- 
65  O  C,HA.H20 

68          0.5 

72       1.3 

75  2.3  C6HA.H20+C6H7Q, 

70  2.4  C6H7O7.NH4 

65  2.5 

60  2.7 

55  2.8 

52  2.8 

50  3-6 
49-2  5.1 
50  6.2 

Composition  of  the  solid  phases  determined  by  "  Rest  Method." 

(Schreinemakers,  Z.  anorg.  Ch.  37,  207.) 

AMMONIUM  CALCIUM  FERROCYANIDE. 

100  gms.  sat.  aqueous  solution  contain  0.258  gm.  (NH4)2CaFe(CN)6  at  16°. 

(Brown.) 

AMMONIUM  FLUOBORIDE   NH43BF3. 

100  parts  of  water  dissolve  25  parts  salt  at  16°,  and  about  97  parts  at  b.  pt.1 

(Stolba  —  Chem.  Techn.  Cent.  Anz.  7,  459  ) 


,53 

56 

54 

NH3. 

7-5 

8.2 

8.5 
8.5 

—  ^                     OU11U  JTUO3C. 

C.HA.NH4 
C6H707NH4+C(1H»07(NH<), 

50 
45-8 

7-9 
8.4 

" 

47 

ii.  i 

" 

50 

12.9 

c  HA(NH!),+C«HA 

54-5 

14.5 

6  (NHJj.p'HjO' 

52 

50 
48.4 

15 
16 
17.9 

It 

AMMONIUM  FORMATE 


AMMONIUM  FORMATE  HCOONH4|  and  also  Ammonium  Acid  Formate. 
SOLUBILITY  IN  WATER. 

(Groschuff  —  Ber.  36,  4351,  '03.) 


to 

Gms.  HCOONH 

4  per  ioo  Gms.     Solid                +0 

Gms.  per  ioo  Gms.  Solution.          Solid 

. 

Solution. 

Water. 

Phase. 

HCOONH2.  HCOOH 

.    '           Phase. 

—  20 

4I 

•9 

72 

HCOONH4     —    6 

•5 

46 

•7 

34 

.1 

HCOONH4.HCOOH 

0 

50 

•5 

102 

+    I 

•5 

49 

.6 

36 

.2 

" 

20 

58 

•9 

143 

6 

51 

•3 

37 

•4 

* 

40 

67 

.1 

204 

8 

•5 

52 

.1 

38 

* 

60 

75 

-7 

311 

~~  7 

49 

.6 

36 

.2 

HCOONH4  labil. 

80 

84 

.2 

531 

"         +13 

53 

38 

.6 

" 

stabil. 

116 

m.pt. 

29 

55 

.8 

40 

•7 

" 

" 

39 

57 

.8 

42 

.2 

H2O  free  solution 

SOLUBILITY  OF  AMMONIUM  FORMATE  IN  FORMIC  ACID  SOLUTIONS. 

(Groschuff.) 

30  grams  of  HCOONHU  dissolved  in  weighed  amounts  of  anhydrous  formic 
acid  and  cooled  to  the  point  at  which  a  solid  phase  separated. 


Gms. 
to          HCOONH, 

per  ioo  Gms. 
Solution. 

G.  M. 
HCOONH4        Solid 
penooG.M.     Phase. 
HCOOH. 

Gms.             G.  M. 
to           HCOONH4.    HCOONH, 
per  ioo  Gms.  per  ioo  G.M 
Solution.       HCOOH. 

Solid 
Phase. 

-  3 

35-3 

~n   n      HCOONH, 

39-9      HCOOH 

II 

50 

73      HCOONHi  labil. 

+  8 

•5 

40.6 

49.9 

39 

57-8 

IOO 

stabil. 

21 

•5 

50 

73 

78 

73-1 

199 

"              " 

Il6  m.pt. 

IOO 

00 

•i              « 

ioo  gms.  95%  Formic  Acid  dissolve  6.2  gms.  HCOONH4  at  21°.     (Aschan,  1913.) 

AMMONIUM  IODATE  NHJO3. 

SOLUBILITY  IN  AQUEOUS  IODIC  ACID  AT  30°. 

(Meerburg,  1905.) 

Gms.  per  ioo  Gms.  Sat.  Sol. 

—HIO; NHJOT       SolidPhase- 

24  0.62       NH4TO:.2HIO3 

44 • 43  o • 39 

76.35          0.31          «  +mo3 

76 . 70  O  HI03 

AMMONIUM   Per  IODATE   NH4IO4. 

ioo  gms.  H2O  dissolve  2.7  gms.  salt  at  16°,  du  =  1.078.  (Barker,  1908.) 

AMMONIUM  IODIDE   NH4I. 

SOLUBILITY  IN  WATER.  SOLUBILITY  IN  AQUEOUS  ALCOHOL  AT  25°. 

(Smith  and  Eastlack,  1916.) 
Gms.  NHJ 


Gms.  per  ioo  Gms.  Sat.  So 

-         Solid  Phase. 
NH,IO3 

HIO3. 
O 

NH4I03. 
4-2O 

2-54 
4-52 
6-57 

3  '83 
1.94 

"+NH4IO3.2HIO3 
NH4I03.2HI03 

Gms.C2H5OH      ,      f 
- 


(Seidell,  unpublished.) 

Gms.  NH4I  per  ioo  Gms. 


—  20 

—  10 

o 

10 

15 

20 
25 
30 


L  iuu  \jrui3. 

H20. 

*  . 

JC1    IUU    VTIIlb. 

H20. 

PCI   iuu  vjiiia.     < 

Solvent. 

>at.  Sol. 

Sat.  Sol. 

Solvent. 

125.2 

40 

190.5 

O           3 

[  .646 

64.5 

l8l.9 

136 

50 

199.6 

10        : 

C.590 

6l.7 

161  .1 

145 

60 

208.9 

20 

•525 

58.7 

142.1 

154.2 

70 

218.7 

30 

.462 

55-5 

124.8 

163.2 

80 

228.8 

4° 

•395 

52 

108.3 

167.8 

IOO 

250-3 

5°    ii 

.320 

48 

92.3 

172.3 

120 

273.6 

60 

.250 

43-8 

77-9 

176.8 

140 

299.2 

70 

.168 

39 

64 

l8l.4 

80 

.094 

33-3 

49.9 

9° 

.013 

27-5 

37-9 

IOO           < 

5.929 

20.8 

26.3 

53 


AMMONIUM  IODIDE 


Tetra  Ethyl  AMMONIUM   IODIDE  N(C2H6)J, 


SOLUBILITY  IN  SEVERAL  SOLVENTS. 

(Walden  —  Z.  physik.  Chem.  55,  698,  '06.) 


Solvent. 


Water 

Water 

Methyl  Alcohol 

Methyl  Alcohol 

Ethyl  Alcohol 

Ethyl  Alcohol 

Glycol 

Glycol 

Acetonitrile 

Acetonitrile 

Propionitrile 

Propionitrile 

Benzonitrile 

Methyl  Sulphocyanide 

Ethyl  Sulphocyanide 

Nitro  Methane 

Nitro  Methane 

Nitroso  Dimethyline 

Acetyl  Acetone 

Furfurol 

Furfurol 

Benzaldehyde 

Salicylaldehyde 

Anisaldehyde 
Acetone 
Acetone 
Ethyl  Acetate 
Ethyl  Nitrate 


'     Formula. 

H20 

H2O 

CHaOH 

CHaOH 

C2H5OH 

C2H5OH 

(CH2OH)2 

(CH2OH)2 

CHaCN 

CH3CN 

CH3CH2CN 

CH3CH2CN 


o 
25 
o 

25 

o 

25 

o 

25 

o 

25 

o 

25 
25 
25 
25 

o 

25, 
25 

CH3COCH2COCH3  25 

C4H3O.COH  o 

C4H3O.COH  25 

CeH5COH  25 

CeH4.OH.COH  25 


CH3SCN 

C2H5SCN 

CH3NO2 

CH3N02 

(CH3)2N.NO 


C6H4.OCH3.COH 

(CH3)2CO 

(CH3)2CO 


C2H5ONO2 


25 
o 

25 
25 
25 


Benzoyl  Ethyl  Acetate  C6H5COCH2COOC2H5  25 

Dimethyl  Malonate     CH2(COOCH3)2 

Methyl  Cyan  Acetate  CH2CNCOOCH3 

Methyl  Cyan  Acetate  CH2CNCOOCH3 

Ethyl  Cyan  Acetate     CH2CNCOOC2H5 

Ethyl  Cyan  Acetate 

Nitrobenzene 

Acetophenone 

Amyl  Alcohol 

Paraldehyde 

Methyl  Formate 


CH2CNCOOC2H5 
C6H5NO2 


25 
o 

25 
o 

25 
25 


Bromobenzene 


C5HnOH 
(C2H40)3 
HCOOCH3 
CeHaBr 


(Walden 


Sp.  Gr.      Gms.  N(C2Ha)4l  per  IPO. 

Solution.       cc.  Solution.  g^ 

1.0470   16.31  15.58 

I.I02I    36.33(35.5)  32.9 

0.8326      3-7-4-3  4-44 

0.8463    10.5     (10.7)  12.29 

0.7928      0.348  0.439 

0.7844      0.98(0.88)  I.II3 

I.I039      3-27  2.97 

1.0904  7-63(7.55)  7 

0.8163  2.24  2.74; 

0.7929  2.97(3.54)  3.74 

0.8059  0.618  0.767 

0.7830  0.81-1.01  0.99 

0.467  0.451 

1.0828  4.40  4.06 

I. 0012   0.475  0.47 

1.1658  '3.59  3-004 

1.1476  5.38-6.27  4.72 

^.0059  2.67  2.66 

0.268 

I.I738  3-91  3-33 

1.1692  5.33  4.55 

0.43 

change- 

able-i7.7 

0.59 

0.7991  0.174  0.218 

0.249  0.316 

.0.00039 

1.0984    0.062  0.056 

1.1303    0.321  0.284 

1.1335    0.040  0.035 

1.1341     1.82  1.605 

2.83 

1.0760  1.057  0.981 

1.0607  I-7I  1.41 

0.504  0.422 

0.13  0.127 

0.071  0.089 

0.036  0.037 

"...         0.031  0.032 

'. . .         0.009  0.006 

—  Z.  physik.  Chem.  61,  635,  igo7-'o8.) 


AMMONIUM  IODIDE 


54 


Tetra  Methyl  AMMONIUM  IODIDE  N(CH3)4I. 

SOLUBILITY  IN  SEVERAL  SOLVENTS. 

(Walden  —  Z.  physik.  Chem.  55,  708,  '06.) 


Sp.  Gr.  of 

Cms.  N(CH3)4  1 

'.  per  roo. 

Solvent. 

Formula. 

t  °. 

Solution. 

cc 

.  Solution. 

Gms. 
Solution. 

Water 

H20 

0 

\ 

.0188 

2 

.01 

I 

•97 

Water 

H20 

25 

I 

•0155 

5 

•31-5 

.89 

5 

.22 

Methyl  Alcohol 

CH3OH 

o 

0 

.8025 

o 

.18-0 

.22 

0 

.22 

Methyl  Alcohol 

CH3OH 

25 

0 

.7920 

0 

.38-0 

.42 

o 

.48 

Ethyl  Alcohol 

C2H5OH 

25 

0 

.7894 

o 

.09 

Glycol 

(CH2OH), 

0 

x 

.014 

Glycol 

(CH2OH)8 

25 

I 

.0678 

o 

.240 

0 

.224 

Acetonitrfl 

CH3CN 

25 

o 

.650 

.  .  . 

Nitro  Methane 

CH3NO, 

0 

I 

•1387 

0 

.25-0 

•32 

o 

.22 

Nitro  Methane 

CH3NOa 

25 

I 

.1285 

o 

•34-0 

•38 

o 

.21 

Acetone 

(CH3)2CO 

o 

.  .  . 

o 

.118 

Acetone 

(CH3)2CO 

25 

o 

.187 

Salicyl  Aldehyde 

C6H4.OH.COH 

0 

I 

.1492 

0 

.302 

0 

.263 

Salicyl  Aldehyde 

CJl4.OH.COH 

25 

I 

•1379 

0 

.510 

o 

.484 

Very  exact  determinations  of  the  solubility  of  tetra  methyl  ammonium  iodide 
in  aqueous  solutions  of  KOH  and  of  NH4OH  at  25°  are  given  by  Hill  (1917). 

Tetra  Propyl  AMMONIUM  IODIDE   N(C3H7)4l. 

SOLUBILITY  IN  SEVERAL  SOLVENTS, 

(Walden  —  Z.  physik.  Chem.  55,  709,  '06.) 
Formula. 


CH3OH 
CH3OH 
C2H5OH 
C2H5OH 
CHsCN 
CHaCN 
C2H5CN 


Solvent, 

Methyl  Alcohol 

Methyl  Alcohol 

Ethyl  Alcohol 

Ethyl  Alcohol 

Acetonitrile. 

Acetonitrile 

Propionitrile 

Propionitrile 

Benzonitrile 

Nitro  Methane 

Nitro  Methane 

Nitro  Benzene 

Benzaldehyde 

Benzaldehyde 

Anisaldehyde 

Anisaldehyde 

Salicylaldehyde 

Ethylnitrite  C2H5NO2 

Ethylnitrite  C2H5NO2 

DimethylMalonate  CH2(COOCH3)2 

DimethylMalonate  CH^COOCH^ 

Acetone  (CHs)2CO 

Acetone  (CH3)2CO       ' 

Ethyl  Acetate          CH3COOC2H5 

Ethyl  Bromide         C2H5Br 


CeH6CN 
CH3NO2 
CH3NO2 
C6H5NO2 
C6H5COH 


Sp.  Gr.  of 

Gms.  N(C3H7)J  per  100. 

t°. 

Solution. 

cc.  Solution 

Gms. 
Solution. 

0 

0.9756 

40.92 

41.94 

25 

I.OI87 

56.42 

55-37 

0 

0.8349 

6.5-6.8 

8.14 

25 

0.8716 

19.88-20.29 

23-28 

0 

0.8553 

I3-03 

15.24 

25 

0.8584 

18.69 

21.77 

0 

0.8280 

6.37 

7.66 

25 

0.8191 

9-65 

10.29 

25 

I.OI99 

8.44 

8-35 

o 

I.lSl 

14.79 

12.52 

25 

I.I58 

22.24 

19.21 

25 

I-IQ3 

5-71 

4  79 

0 

I.058l 

7.06 

6.67 

25 

1.0549 

9.87 

9-35 

0 

I.III4 

5-60 

5-04 

25 

I.I004 

6-75 

6.14 

25 

.  .  . 

39.28 

o 

I.I207 

0.522 

0.466 

25 

I.I025 

0.653 

0.592 

o 

I-I532 

0.298 

0.259 

25 

I-I345 

0.320 

0.282 

0 

0.8259 

2.692 

4-65 

25 

o  .  8049 

3-944 

4.90 

25 

0.8975 

0.0063 

0.007 

25 

0.187 

(Walden  —  2.  physik.  Chem.  61,  639, 


55 


AMMONIUM  IODIDE 


SOLUBILITY  OF  TETRA  AMYL,  TETRA  ETHYL  AND  TETRA  a  PROPYL  AMMONIUM 
IODIDES  IN  WATER  AND  IN  CHLOROFORM  AT  25°.    (Peddle  and  Turner,  1913.) 

Gms.  Each  Salt  (Determined  Separately),  per  100  Gms.  Solvent. 

Solvent.  t * > 

N(CsHn)4I.  NCCtH^J.         aN(C3H7)4I. 

Water  0.74  45  18.64 

CHC13  210.8  1.55          54.56 

Freezing-point  data  for  mixtures  of  tetra  methyl  ammonium  iodide  and  iodine, 
and  for  phenyltrimethyl  ammonium  iodide  and  iodine  are  given  by  Olivari  (1908). 

AMMONIUM  Iridium  CHLORIDES. 

SOLUBILITY  IN  WATER  AT  19°.    (Delepine,  1908.) 

Name  of  Salt.  Formula. 


^ 

Ammonium  iridium  chloride  (NH4)2IrCl6  0.77 

Diammonium  aquo  penta  chloro  indite  IrCl5(H2O)(NH4)2     15.4 
Triammonium  hexa  chloro  iridite  IrCl6(NH4)3+H2O     10.5 

AMMONIUM  lodo  MERCURATE  2NH4I.HgI2.H2O. 

100  gms.  of  the  saturated  aqueous  solution  contain  4.5  gms.  NH4,  22.6  gms. 
Hg  and  62.3  gms.  I  at  26°,  sp.  gr.  =  2.98.  (Duboin,  1905.) 

AMMONIUM  Tetra  MOLYBDATE  (NH4)2O.4MoO3.2H2O. 

100  gms.  H2O  dissolve  3.52  gms.  salt  at  15°  (d  =  1.03),  3.67  gms.  at  18°  (d  = 
1.04)  and  4.60  gms.  at  32°  (d  =  1.05).  (Wempe,  1912.) 


AMMONIUM  Phospho  MOLYBDATE 

SOLUBILITY  IN  WATER  AND  AQUEOUS  SOLUTIONS  AT  15°.    (de  Lucchi,  1910.) 

Solvent.  Gms.  Salt  per  1000  Gms.  Solvent. 

Water  0.238 

5  per  cent  aqueous  NHiNOs  solution  o.  137 

i  per  cent  aqueous  HNOs  solution  o  .  203 

AMMONIUM     NITRATE    NH4NO3. 

SOLUBILITY  IN  WATER. 

(Schwarz  —  Ostwald's  Lehrbuch,  ad  ed.  p.  425;  Muller  and  Kaufmann  —  Z.  physik.  Chem,- 
42,  497.  oi-'oa.) 


... 

Sp.  Gr. 

Solution. 

G.  Mols. 
NI^NOa  per 
loo  Mols.  HaC 

Gms.  NH4NO8  per 
)ioo  Gms. 

Solid 
Phase. 

•   Solution. 

Water: 

0 

26 

63 

54 

.19 

118 

•3 

NH4NOa  rhomb. 

ft 

12 

2 

•2945 

34 

50 

60 

•53 

153 

•4 

" 

20 

2 

.3116 

43 

30 

65 

.80 

192 

•4 

" 

25 

O 

•3!97 

48 

19 

68 

.17 

214 

.2 

M 

30 

O 

•3299 

54 

40 

70 

•73 

241 

.8 

ft 

32 

I 

•3344 

57 

.60 

•97 

256 

•9 

NH4NOa  rhomb. 

ft  +  rhomb,  a 

35 

.0 

•3394 

59 

.80 

72 

.64 

265 

.8 

NH4NO8  rhomb. 

a 

40 

o 

•3464 

66 

80 

74 

.82 

297 

-0 

ii 

So 

o 

77 

.41 

77 

•49 

344 

•  O 

M 

60 

0 

94 

•73 

80 

.81 

421 

.0 

M 

70 

.0 

112 

•30 

83 

•32 

499 

•  0 

" 

80 

.0 

130 

•5° 

85 

•25 

580 

.0 

M 

90 

.0 

166 

88 

.08 

740 

.0 

NH^Oa  rhombohedral  ? 

100 

.0 

196 

oo 

89 

7i 

871 

.0 

" 

SOLUBILITIES  OF  MIXTURES  OF  AMMONIUM  NITRATE  AND  OTHER  SALTS. 

(RUdorf— Mulder.) 

loo  gms.  H2O  dissolve  162.9  gms.  NH4NO3  +  77.1  gms.  NaNO3  at  16°  R. 
100  gms.  H2O  dissolve    88.8  gms.  NH4NO3  +  40.6  gms.  KNO3  at  9°  M. 
100  gms.  H2O  dissolve  101.3  gms.  NH4NO3  +  6.2  gms.  Ba(NO3)2  at  9°  M. 


AMMONIUM  NITRATE 


SOLUBILITY  OF  AMMONIUM  NITRATE  IN  AMMONIA. 

(Kuriloff— Z.  physic.  Chem.  25, 109,  '98.) 


Gms. 

Mols.  NEUN03 
Gms.          per  100  Mols. 

Gms. 

Mols.  NEUNO, 
Gms.      per  100  Mols, 

f. 

NEUNOa- 

NHa. 

+  NHa. 

t 

o 

NH4NO3. 

NHa.           NH4NO« 
+  NHT 

80 

O 

100 

0 

.0 

33 

•3 

O 

•9358 

0 

2352 

45-9 

60 

1.3918 

4-4327 

6 

•25 

35 

•9 

O 

•7746 

0 

•1857 

47  o 

44-5 

0.9526 

1-2457 

13 

•9 

68 

.8 

4 

.2615 

o 

•7747 

53-8 

30 

0-8308 

0.3700 

32 

•3 

94 

.0 

0 

•6439 

o 

.0665 

67-3 

10.5 

0.9675 

o-4&5 

36 

•9 

190 

.8 

0 

•7578 

0 

.0588 

74-2 

0 

o  .  7600 

o  .  2607 

38 

•3 

168 

.0 

IOO-O 

t°  «=  temperature  of  equilibrium  between  solution  and  solid  phase 


SOLUBILITY  OF  AMMONIUM  NITRATE  IN  AQUEOUS  SOLUTIONS  OF  AMMONIUM 
SULFATE  AND  VlCE  VERSA. 

(Massinik,  1916,  1917.) 


Results 

(de  Waal 

Gms.  per 
loo  Gms.  Sat.  Sol. 

ato°. 

,  1910.) 

Solid  Phase 

Results  at  30°.                      Results  at  70°. 

(Schreinemakers  and  Haenen,  1910.)                (de  Waal,  1910.) 

Gms.  per                                              Gms.  per 

100  Gms.  Sat.  Sol.                               100  Gms.  Sat.  Sol. 
e~i:j  T>I  .                 ••        c_i:j  T>I  —  .*_ 

54-19 

(Nl 
1     S( 

o 

[U>2 

NH4NO3 

70.1 

(NH*), 
S04. 

0 

NEUN03 

NH4NO3. 
84-03 

o 

J?" 

NH4N03 

49.12 

6 

" 

67.63 

2.38 

" 

81 

-38 

2. 

4i 

" 

45-99 

9 

53 

NEUN03+i.3 

66.93 

3-46 

NEUN03+i.3 

81 

.01 

2. 

45 

NHiNOs+i.s 

31.61 

19 

5 

1.3 

63-84 

4.96 

1.3 

80 

•  25 

2. 

68 

i-3 

30.87 

20 

43 

1.3+1.2 

58.06 

8.22 

1.3+1-2 

76 

.01 

3- 

96 

" 

31.04 

20, 

4 

1.2 

52.75 

11.42 

1.2 

73 

.48 

1.3+1.2 

29.81 

21, 

33 

" 

49.80 

13.27 

"  +(NEU)2S04 

.58 

5- 

82 

1.2 

29.58 

41, 

64 

i.2+(NEU)2SO4 

37.20 

19.48 

(NH4)2S04 

70 

•  15 

6. 

71  3 

t.a+(NEWaS04 

S.6l 

37 

89 

(NEU)3S04 

19.91 

28.83 

" 

ii 

.10 

40. 

81 

(NILJzSO, 

o 

4i 

4 

" 

I2.O5 

34-7 

" 

0 

47- 

81 

" 

O 

44.1 

" 

1.2  = 


1.3  =  (NH4)aS04.3NH,NO.. 

Freezing-point  lowering  data  for  mixtures  of  ammonium  nitrate  and  lead 
nitrate  are  given  by  Bogitch  (1915). 


SOLUBILITY  OF  AMMONIUM  NITRATE  IN  NITRIC  ACID. 

(Groschuff  —  Ber.  37,  1488,  '04.) 

Determinations  by  the  "  Synthetic  Method,"  see  Note,  page  16. 


Gms. 

Mols. 

Gms. 

Mols. 

to            NH4NOJ 

NEUNOa 

Solid 

t° 

NEUNO3 

NH4NO3 

Solid 

Gms. 

100 

Sol. 

per  100 
Mols.  HNO3. 

Phase. 

per  100 
Gms.  Sol. 

per  100 
Mols.  HNO3. 

Phase, 

8 

21 

.  I 

21.  1        ] 

tfEUNOa.2HNOa 

II. 

0 

51.7         84  .  3        NH.NO3.HNOs 

23 

28 

•7 

31-6 

a 

12. 

0 

54.7 

95-1 

« 

labil. 

29.5m 

Pt.  38 

.8 

50.O 

" 

II. 

5 

57-6 

IOS.0 

" 

b 

27 

•5 

44 

.6 

63-4 

b 

II. 

5 

54-0 

92.4        NH4NO3 

labil 

23 

•5 

49 

•  4 

76.8 

•' 

17. 

0 

54-7 

95-1 

stabil 

17 

•  5 

54 

.0 

92.4 

•i 

27. 

o 

56.2 

IOI.O 

•' 

16 
4 

•5 

.0 

54 
45 

:I 

93-5 
66.7 

NEUNO3.HNO3 

49- 
79- 

o 

0 

60.4 
68.1 

I2O.O 

168.0 

•• 

a  = 

solution 

in  HNO8!  l 

6  = 

solution 

in  NH,NO,. 

57 


AMMONIUM  NITRATE 


SOLUBILITY  OF  AMMONIUM  TRI-NITRATE  IN  WATER. 

(Grcschuff.) 

Cms.  NI^NOs   Cms.  HNO3    Mols.  NH4NO3*  Mols.  NIL.NO, 
per  100  Cms.   per  100  Gms.     per  100  Mols.    per  100  total  Solid  Phase. 


Solution. 

Solution. 

H20. 

Mols.  Solution. 

O 

34-2 

53-9 

64.3 

22 

-  2.5 

34-8 

54-8 

75.1 

23.1 

+  3 

35  4 

55-8 

90 

24-3 

8-5 

36.6 

56-9 

"3 

25-7 

19-5 

37-4 

58.9 

225 

29 

25 

38.1 

60 

45° 

31 

29-5 

m.  pt.  38  8 

61.2 

00 

33 

SOLUBILITY  OF  MIXTURES  OF  AMMONIUM  NITRATE  AND  SILVER  NITRATE  IN 
WATER  AT  VARIOUS  TEMPERATURES. 

(Schreinemakers  and  deBaat,  1910.) 


Gms.  per  100  Gms. 
to               Sat.  Sol.                  Solid  Phase.               t°. 

Gms 

.  per  100  Gms. 
Sat.  Sol.                Solid  Phase. 

AgNO3.  NI^NOj. 

'AgN03. 

NH4NO3: 

-    7-3 

47. 

,i 

o 

Ice+rb 

AgNO3 

109  6 

67 

•9 

32 

.1 

D+rb.AgNO3 

—  10.7 

44- 

52 

8.43 

{ 

*    • 

0 

22 

•13 

44 

•87 

D+rb-NHiNOj 

—  14.9 

42 

16.8 

Ice+D+rb 

.  AgN03 

18 

27 

.07 

49 

.22 

" 

-14.8 

39 

Si 

18.79 

"  +D 

30 

29 

.76 

52 

•50 

" 

-18.7 

15 

99 

37-3 

"  +D+0rb.NH4NO3 

±32 

{D-frb.  NH4NO8+ 
a+rb.  NH4NO3 

—  17.4 
0 

18 
30 

l/t  Cn  c/v 
OOVx  O  C 

36 

:3896 

41.2 

19-59 
22.06 
23.42 

D+rb. 

AgNO3 

40 
55 
85.4 

32 
36 

.68 
.6 

52 
52 

.22 
.38 

D+«rb.NH4NO3 

(D+rb.NH4NO3+ 
\     rbd.NH3NO3 

55 

63 

32 

26.12 

1 

* 

101.5 

47 

•  5 

52 

•  5 

D+rbd.  NH3NO3 

D  =  NH4NO3.AgNO3.        rb.  =  rhombic.        rbd.  =  rhombohedric. 


SOLUBILITY  OF  AMMONIUM  NITRATE  IN  AQUEOUS  SOLUTIONS  OF  SILVER 
NITRATE  AND  VICE  VERSA  AT  30°. 

(Schreinemakers  and  deBaat,  1910.) 


Solid  Phase. 

D 

u 


D+AgN03 
AgN03 


Results  are  also  given  by  Schreinemakers  (1908-09)  for  the  reciprocal  solubility 
of  ammonium  nitrate  and  silver  nitrate  in  aqueous  alcohol  solutions  at  30°. 

100  cc.  anhydrous  hydrazine  dissolve  78  gms.  NH4NO3  at  room  temp,  with 

decomp.  (Welsh  and  Broderson,  1915.) 

Freezing-point  data  for  mixtures  of  ammonium  nitrate  and  silver  nitrate  are 
given  by  Flavitzkii  (1909)  and  by  Zawidzki  (1904).  The  eutectic  is  at  102.4° 
and  30.9  Mol.  %  AgNO3.  Results  for  NH4NO3  +  T1NO3  are  given  by  Boks  (1902). 


Gms.  per  100  Gms. 
Sat.  Sol. 

AgN03. 
0 

NH4N03- 
70.1 

12.51 
21.31 

58.64 

27-75 
29.76 
35-62 
41.09 

54.12 
52.5 

45-44 
39.60 

Solid  Phase. 

Gms.  per  100  Gms. 
Sat.  Sol. 

AgNO3. 

NH4NO3." 

NH4NO3 

45-85 

34-47 

" 

52.45 

28.86 

" 

57-93 

24-33 

" 

58.88 

23-42 

[H4N03+D 

63-27 

15.62 

D 

69.08 

6-59 

Cl 

73 

o 

D  =  NH4NO3, 

,AgN03. 

AMMONIUM  NITRATE  58 

RECIPROCAL  SOLUBILITY  OF  AMMONIUM  NITRATE  AND  SODIUM  NITRATE  IN 
WATER  AT  o°,  15°  AND  30°. 

(Fedotieff  and  Koltunoff,  1914.) 


I  . 

o 

0 
0 

Sol. 

•354 
.407 
.264 

'  NH4N03. 
0 

105.5 
II8.4 

NaN03. 

73-33 
66 
o 

i>  . 

15 
15 
15 

Sol. 
1.429 
1.405 
1.364 

'  NH4NO3. 

155-3 
I56.I 

159 

NaNO3. 

75.38 
60.76 

36.50 

15    » 

•375 

0 

83 

•9 

15 

1-350 

1  60 

27.79 

15 

.386 

24 

•03 

81 

.21 

15 

I. 

330 

l62. 

3 

17.63 

•392 

42 

.81 

79 

•34 

15 

I. 

298 

167. 

4 

O 

15 

.401 

64.6 

78 

.06 

30 

I  . 

401 

0 

96.12 

15 

.417 

110 

•9 

75 

.81 

30 

I. 

450 

220. 

8 

88.31 

15         1.428 

152 

75 

•35 

30 

I. 

329 

232. 

6 

O 

SOLUBILITY 

OF  AMMONIUM 

NITRATE 

IN 

AQUEOUS  ETHYL  ALCOHOL. 

(Fleckenstein  -  Physik 

.  Z., 

6,  419,  '05.) 

t° 

Grams  of  NH«N03  Dissolved  per  100  Grams  Aq.  Alcohol  of  (Wt.  %): 

100%. 

86.77%. 

76.12%. 

51.65%. 

25.81%. 

0%. 

20               2.5 

II 

23 

70 

I4O 

195 

30           4 

14 

32 

90 

165 

230 

40           5 

18 

43 

196 

277 

50           6 

24 

55 

144 

244 

365 

60.          7.5 

30 

70 

183 

320 

70           9 

41 

93 

230 

80         10.5 

56 

NOTE.  —  The  figures  in  the  preceding  table  were  read  from  curves  shown  in 
the  abridged  report  of  the  work,  and  are,  therefore,  only  approximately  correct. 
Determinations  of  the  solubility  in  methyl  alcohol  solutions  were  also  made  but 
not  quoted  in  the  abstract.  The  "Synthetic  Method"  (see  Note,  page  16)  was 
used. 

100  grams  absolute  ethyl  alcohol  dissolve  4.6  grams  NKUNOs  at  14°  and  3.8 


100  grams  absolute  methyl  alcohol  dissolve  14.6  grams  NP^NOs  at  14°,  16.3 
grams  at  18.5°  and  17.1  grams  at  20.5°. 

(Schiff  and  Monsacchi  —  Z.  physik.  Chem.,  21,  277,  '96;  at  20.5°  de  Bruyn  —  Ibid.,  10,  783,  '92.) 

SOLUBILITY  OF  AMMONIUM  NITRATE  IN  AQUEOUS  ETHYL  AND  METHYL 
ALCOHOLS  AND  IN  A  MIXTURE  OF  THE  Two  AT  30°. 

(Schreinemakers,  1908-09.) 
Gms.  per  100  Gms.  Sat.  Sol.  Gms.  per  100  Gms.  Sat.  Sol.  Gms.  per  100  Gms.  Sat.  Sol. 


H20. 

QHsOH. 

NILJSTOa. 

H20. 

CH3OH. 

NIL.NO3. 

H20. 

*CH3OH 
+Q.H.O. 

NH<NO. 

0 

96 

•4 

3-6 

0 

83.3 

16 

•7 

3-4 

•9 

II.7 

5 

89 

.6 

6.5 

5 

74-8 

21 

•3 

5 

82 

•9 

12.3 

10 

80 

•4 

10.7 

10 

63-8 

27 

.1 

10 

74 

.6 

16.4 

15 

68 

.6 

17 

15 

50.7 

35 

15 

63 

•5 

24 

20 

53 

•5 

26.8 

20 

35-2 

46 

•3 

20 

48 

.2 

35.1 

25 

32 

•5 

44-8. 

25 

19.8 

59 

25 

22 

•4 

54 

29.9 

0 

70.1 

29.9 

0 

70 

.1 

29.9 

0 

70.1 

•  Weight  per  cent  CH3OH  =  si-7,  C2H5OH  =  48.3. 

Additional  determinations  of  the  solubility  of  ammonium  nitrate  in  aqueous 
ethyl  alcohol  solutions  at  o°,  30°  and  70°  are  given  by  deWaal  (1910).  At  cer- 
tain concentrations  at  67.5°  the  solutions  separate  into  two  layers. 


59 


AMMONIUM  NITRATE 


AMMONIUM   Magnesium  NITRATE  2NH4NO3.Mg(NO3)2. 

100  parts  water  dissolve  10  parts  salt  at  12.5°. 


(Foucroy.) 


AMMONIUM  Manganic  MOLYBDATE  5(NH4)2MoO4.Mn2(Mo2O7)s.i2H2O. 
100  parts  water  dissolve  0.98  part  salt  at  17°.        (Struve  — J.  pr.  Chem.,  6i,'46o,  '54.) 

AMMONIUM  OLEATE   Ci7H33COONH4. 

SOLUBILITY  IN  SEVERAL  SOLVENTS. 

(Falciola,  1910.) 
Solvent  Cms.  QiHssCOONIL,  dissolved  per  100  cc.  solvent: 

Absolute  Alcohol  31  at  o°  59      at  10°  100       at  50° 

75  per  cent  Alcohol  ...  8.2    at.  20°  10 . 86  at  30° 

i  part  Alcohol  +  2  parts  Ether  ...  9.45  at  15°  16.9   at  20° 

Acetone  ...  4.7    at  15° 

AMMONIUM  OXALATE   (COONH4)2.H2O. 

SOLUBILITY  IN  WATER. 

(Av.  curve  from  results  ot  Engel,  1888;  Foote  and  Andrew,  1905;  Woudstra,  1912;  Colani,  1916.) 


O 
IO 

15 

20 


Cms.  (COONH4)2  per 
100  Gms.  Sat.  Solution. 

2.1 
3 

3-5 
4.2 


25 
30 
40 


Gms.  (COONH4)2  per 
100  Gms.  Sat.  Solution. 

4.8 
5-6 
7-4 
9-3 


SOLUBILITY  IN  AQUEOUS  SOLUTIONS  OF  OXALIC  ACID. 

(Woudstra,  1912.) 

Results  at  30°.     (Interpolated 
from  Original.) 


(COONHi)2. 

(COOH),. 

ooiiu  .rua.se. 

(COONH4)2. 

(COOH)2. 

DOIIQ  rnase. 

0.14 

12.36 

A 

O.22 

21  .22 

A 

0.28 

12.78 

A+T 

0.31 

21.31 

(i 

0.30 

12 

T 

o-53 

20.54 

A+T 

0-39 

10 

a 

0.56 

21.23 

T 

0.47 

8 

(( 

0.61 

20-55 

u 

0.52 

7 

it 

0-54 

20.92 

tt 

0.68 

6 

tt 

0.79 

16.44 

tt 

i 

5 

(C 

1.23 

12.88 

tt 

2 

3-96 

(I 

7.16 

7.98 

tt 

3 

3-6i 

(( 

3-54 

5-83 

tt 

4 

3-6o 

u 

5-65 

5-67 

it 

5 

3.81 

(( 

6.72 

5-95 

tt 

5-98 

4.21 

T+A.  O. 

8.74 

6-53 

T+A.  O. 

7 

3-63 

A.  O. 

8-93 

6.27 

A.  O. 

8.19 

3-36 

A.  O.+N.  O. 

9.04 

6.14 

u 

7 

2.32 

N.  O. 

12.38 

5 

A.  O.+N.  O. 

6 

1.02 

a 

8.31 

3-°4 

N.  O. 

5-53 

O.22 

u 

9-59 

i-45 

tt 

A.  =  Oxalic  Acid  (COOH)2.H2O. 
A.  O.  =  Acid  Ammonium  Oxalate  (COO)2HNH4.H2O. 
T  =  Ammonium  tetroxalate  (COOH)2(COO)2HNH4.2H2O. 
N.  O.  =  Neutral  Ammonium  Oxalate  (COONH4)2.H2O. 

Additional  data  for  this  system  at  25°  are  given  by  Walden  (1905),  and  at  o°, 
by  Engel  (1888). 


AMMONIUM   OXALATE 


60 


SOLUBILITY  IN  WATER  OF  MIXTURES  OF  AMMONIUM  OXALATE  AND: 


Other  Oxalates  at  25°. 

(Foote  and  Andrew,  1905.) 
Cms.  per  100  Cms.  Sat.  Solution. 


2.79  (COONH4)2.H20  +  2 5  . 96  (COOK)2H2O  1 5 

4.8  "  +5-75     (COOLi)2  50 

5.45  "  +0.59  (COO)2Mg.2H20  18 

6.19  "  +1.45  (COO)2Zn.2H2O  50 

5 . 06          "          +o .  28  (coo)2  Cd.3H2o    19 

50 


Other  Ammonium  Salts. 
(Colani,  1916.) 

Gms.  per  100  Gms.  Sat.  Solution. 
0.14   (COONH4)2  +  26.35     NH4C1 


0.67 
O.II 
0.65 
0.085 

o-35 


+32-55 

+42.43  (NH4)2S04 

+45-92         " 
+  62.26    NH4N03 
+  72.11 


Both  salts  in  excess  in  every  case.     No  double  salts  formed. 

SOLUBILITY  OF  AMMONIUM  OXALATE  AND  OF  AMMONIUM  THORIUM  OXALATE 

IN  WATER  AT  25°. 

(James,  Whittemore  and  Holden,  1914.) 

The  mixtures  were  constantly  agitated  for  periods  varying  from  many  weeks 
to  several  months. 


Solid  Phase. 

2.I.7+2.I.2 

2.1.2 
(t 


2.1.2  =  2Th(C2O4)2.(NH4)2C2O4.2H2O. 
gms.  (NH4)2C2O4  at  21°.       (Aschan,  1913.) 
44  gms.    (NH4)2C2O4  at  room   temp. 
(Welsh  and  Broderson,  1915.) 


Gms.  per  100  Gms.  H2O. 

Solid  Phase. 

(NHdtCA. 

Th(C2O4)2. 

5-25 

0              (1 

srH4)2c2< 

L/4 

6.04 

i-54 

tt 

7-78 

4-51 

a 

10.37 

8.87 

(f 

15.46 

16.89 

(( 

21.47 

26.37 

tt 

28.18 

36.54 

"+2, 

•i-7 

Gms.  per  100  Gms.  H2O. 

(NH4)2C204. 
29.47 
23.04 
16.84 

Th(C204)2. 

39-iQ 
29-87 

21.  l8 

13.27 

8.13 
5.36 

15.96 
9-13 

5-63 

1.70 

1.42 

2.1.7  =  2Th(C204)2.(NH4)2C204.7H20; 
100  gms.  95%  formic  acid  dissolve  6.2 
100  cc.  anhydrous  hydrazine  dissolve 
with  evolution  of  ammonia. 


AMMONIUM  PALMITATE  Ci6H3iO2NH4. 

SOLUBILITY  IN  SEVERAL  SOLVENTS. 

(Falciola,  1910.) 
Gms.  Ci6H31O2NH4  per  100  c.c.  of: 


«•• 

Absolute 
Alcohol. 

75%  Alcohol. 

50%  Alcohol. 

Mixture  of  i  Pt. 
Alcohol  +  2  Parts 
Ether. 

Acetone. 

0 
10 

o-5 

0.7 

I.  '78 

0.37(13°) 

0.2  '(13°) 

20 

1.4 

4-33 

5-33 

O.29 

30 
40 

4-5 

EI.02 
14.84 

6.69 

50 

ii 

.  .  • 

AMMONIUM  PHOSPHATES   (NH4)3PO4,  (NH4)2HPO4,  and  NH4H2PO<. 
loo  gms.  H2O  dissolve  131  gms.  (NH4)2HPO4  at  15°,  du  sat.  sol.  =  1.343. 

(Greenish  and  Smith,  1901.) 

Data  for  the  solubility  of  mono  ammonium  phosphate  in  anhydrous  and  in 
aqueous  ortho  phosphoric  acid,  determined  by  the  synthetic  method,  are  given 
by  Parravano  and  Mieli,  1908. 


6i  AMMONIUM  PHOSPHATES 


SOLUBILITY  OF 

Cms.  per  100  Gms. 
Sat.  Solution. 

AMMONIUM  PHOSPHATES  IN  AQUEOUS  SOLUTIONS  OF  £)RTHO 
PHOSPHORIC  ACID  AT  25°. 

(Parker,  1914.) 
Gms.  per  100  Gms. 
Solid  Phase.                                  Sat-  S9lution.       Solid  Phase. 

H3PO4.          NH3. 
4.1          22.6 
4-4         18.4 

10          13.1 

20            7 

30           7-7 
34.4      10 

40              10.2 

48  .  2       ii  .6 

(NH4)3P04.3H20 

It 
tt 

11 

(NH4)3P04.3H20+  (NH4)2HP04 
(NH4)2HPO4 
(NH4)2HP04+NH4H2PO4 

H3P04.      NH3. 

40        9 

30        5-4 
20.6     4 

30        3-8 
40        4 
50        4.2 
60.6     4.4 

tfH4H2P( 

n 

n 
ti 
tt 
tt 
tt 

The  original  figures  have  been  calculated  to  grams,  plotted  on  cross-section 
paper  and  the  above  table  read  from  the  curve. 

Data  for  this  system  are  also  given  by  D'Ans  and  Schreiner  (1910).  The 
agreement  is  satisfactory  except  for  the  (NH^aPO^HaO  end  of  the  curve,  for  which 
much  lower  values  for  the  NHs  component  are  given  by  D'Ans  and  Schreiner. 

AMMONIUM   Magnesium  PHOSPHATE   NH4MgPO4.6H2O  and  iH,O. 
SOLUBILITY  IN  WATER  AND  SALT  SOLUTIONS, 

(Bube,  1910.) 

The  solutions  were  saturated  in  7-16  liter  flasks.  The  stirrer  was  introduced 
through  a  mercury  sealed  connection,  in  order  to  prevent  loss  of  moisture  or 
ammonia  during  the  long  periods  required  for  saturation,  ^reat  care  was  ex- 
ercised to  eliminate  errors  of  manipulation.  Large  volumes  of  the  saturated 
solutions  were  used  for  analysis.  In  the  cases  where  equilibrium  was  approached 
from  above  (designated  by  *,  in  table  below)  the  mixtures  were  heated  to  about 
90°  for  \  hour,  and  then  cooled  while  being  continually  stirred  for  4-5  hours  at 
50°,  and  then  in  a  thermostat  at  25°  for  the  remaining  period  shown. 

Solver                              t°  Time  for      Cms,  per  100  Cms.  Sat.  Sol. 

*  '  Saturation.  ^7           p^  NH^ 

Water                                                25°  69  hrs.      0.0808  0.0965  ...        Mixed  Hydrates 

"  25  9  days   0.0867  0.0992 

25  14     "       0.1352  0.1333  0.1301 

"                                                  22.7  17  hrs.*  0.1076  0.1084.  0.1040     Monohydrate 

anNI^Cl                                        25  20  days    0.3129  0.3057  ...       Mixed  Hydrates 

—  »NH4Cl+i»NHs  25.2     16  hrs.*   0.0249     0.02025       ...         Monohydrate 

0.2  Mol.  MgCl2  per  liter  H2O  25         27  days        ...         0.0206         ...       Mixed  Hydrates 

0.2    "         "  "        "  25.2    16  hrs.*       ...         0.0512         ...         Monohydrate 

-i-  Mol.  (NH4)2HPO4  per  liter  H2O  24  .  25      ...     *   0  .  1  229          ...  ...  " 

3*2 

SOLUBILITY  OF  AMMONIUM  MAGNESIUM  PHOSPHATE  IN  SEVERAL  SOLVENTS. 

(Wenger,  1911.) 
Cms.  NH4MgPO<  per  100  Cms.  Solvent  in: 


t°. 

Water. 

Aq.  5% 

AqwSn° 

Mixture  of  i  Pt. 
NH3(<f=o.96) 

NH.ci+4 

Aq.  10% 
NH4Cl+4 

NH4NO3. 

NH4C1. 

+4  Pts.  H2O. 

NH3  per  100. 

NH3  per  100. 

0 

0.023 

O.IIO 

0.060 

0.0087 

.  .  . 

.  .  . 

20 

O.O52 

0.046 

0.105 

0.0098 

0.0l65 

0.0541 

30 

.  .  . 

0.054 

O.II3 

. 

40 

0.036 

0.064 

0.071 

O.OI36 

50 

O.O3O 

O.O72 

0.093 

0.0153 

60 

0.040 

0.085 

0.173 

0.0174 

0.0274 

0.0731 

70 

0.016 

0.083 

O.I24 

0.0178 

... 

80. 

0.019 

O.IOI 

O.I9I 

0.0145 

... 

... 

AMMONIUM  PHOSPHATES 


62 


AMMONIUM 


Manganese  PHOSPHATE   NH4MnPO4.7H,O. 
SOLUBILITY  IN  SEVERAL  SOLVENTS. 

(Wenger,  1911.) 
Gms.  NH^MnPC^  per  100  Gms.  Solvent  in: 


Water. 

KH^NO". 
0.021 

Aq.  5% 
NH4C1. 

O.OO2 

Mixture  of  i  Pt.  NH3 
(d  =0.96)  +4  parts  H2O. 

0.0116 

0 

0.020 

0.025 

0.0122 

0 

0.023 
O.O2I 

0.034 
0.039 

o.onS 

O 
0.005 

0.023 
0.027 
O.O28 

0-035 
0.038 
O.O4I 

0.0132 
0.0194 
0.0191 

0.007 

0.033 

0.045 

0.0197 

O 
20 

30 
40 

50 
60 
70 
80 


AMMONIUM  Sodium  PHOSPHATES 

Data  for  the  distribution  of  each  of  5  ammonium  sodium  ortho-  and  pyro- 
phosphates  between  water  and  chloroform  at  18°,  are  given  by  Abbott  and  Bray 
(1909). 

AMMONIUM   Hydrogen  PHOSPHITE   (NH4H)HPO3. 

100  grams  water  dissolve  171  grams  (NH4H)HPO3  at  o°,  190  grams  at  14.5° 
and  260  grams  at  31°.  (Amat.,  1887.) 


AMMONIUM   Hypo  PHOSPHITE   NH4H2PO2. 

100  cc.  H2O  dissolve  83  gms.  NH4H2PO2  at  room  temp. 


(Squire  and  Caines,  1905.) 


AMMONIUM  PERMANGANATE  NH4MnO4. 

100  parts  water  dissolve  approximately  8  parts  of  NH4MnO4  at  15°.     (Aschoff.) 

AMMONIUM  PICRATE  C6H2(NO2)3ONH4. 

100  cc.  H2O  dissolve  i.i  gm.  Am.  picrate  at  room  temp.     (Squire  and  Caines,  1905.) 
100  cc.  90%  alcohol  dissolve  1.2  gm.  Am.  picrate  at  room  temp. 

(Squire  and  Caines,  1905.) 

AMMONIUM  Fluo  SILICATE   (NH4)2SiF6. 

100  parts  water  dissolve  18.5  parts  (NH4)2SiF6  at  17.5,°  Sp.  Gr.  1.096. 

(Stolba,  1877.) 

AMMONIUM  SALICYLATE  C6H4.OH.COONH4. 

SOLUBILITY  IN  AQUEOUS  ALCOHOL  SOLUTIONS  AT  25°. 

(Seidell,  1909,  1910.) 


Gms.  C2H6OH         s 
per  too  Gms. 
Solvent. 

3.  Gr.  of 
at.  Sol.       x 

Gms.  C6H4. 
OHCOONH4  per 
oo  Gms.  Sat.  Sol. 

Gms.  C2H5OH 
per  100  Gms. 
Sat.  Sol. 

Sp.  Gr.  of     c 
Sat.  Sol. 

Gms.  C6H4.OH. 
:OONH4  per  too 
Gms.  Sat.  Sol. 

0 

.148 

50.8 

70 

I.OI5 

42 

20 

.122 

50.3 

80 

0.979 

38 

40 

.088 

48.3 

90 

0.936 

31.6 

50 

.067 

46.7 

95 

0.907 

27.8 

60 

.042 

44-7 

•100 

0.875 

22.3 

AMMONIUM  SELENATE  (NH4)2  SeO4 

loo  gms.  H2O  dissolve  1.22  gms.  (NH4)2  SeO4  at  12°. 


(Tutton,  1907) 


63 


AMMONIUM   STEARATE 


Absolute  Alcohol.      75%  Alcohol.      50%  Alcohol. 


AMMONIUM   STEARATE   Ci8H36O2NH4. 

SOLUBILITY  IN  SEVERAL  SOLVENTS. 

(Falciola,  1910.) 
Cms.  CigHjaANIL,  per  100  cc.  of: 


O 

10 

20 

30 
40 

50 


O.I 


0.9 

1.8 
5-5 


0.56 

1.83 
5 


0.25 

1.16 
3-21 


Ether. 


O.I 


Acetone. 
0.08  fo 


AMMONIUM  SULFATE   (NH4)2SO4. 

SOLUBILITY  IN  WATER. 

(Mulder.) 


Grams  (NBU)2SC>4  per  100  Grams. 


O 

5 

10 

15 

20 
25 


Water. 
70.6 
71.8 

73-o 
74-2 

75-4 
76.7 


Solution. 
41.4 
41.8 
42  .2 
42.6 

43-o 
43-4 


t°. 

Grams  (NIL^S 

D4  per  TOO  G 

'  Water. 

Solution  o 

30 

78.0 

43-8 

40 

81.0 

44.8 

60 

88.0 

46.8 

80 

95-3 

48.8 

100 

103  .3 

50  8 

108.9 

I07-5 

5i-8 

Sp.  Gr.  of  saturated  solution  at  15°  —  i  248;  at  19°  =  1.241 

Eutectic  point,  Ice  +  (NH4)2SO4  =  —  19.05°  and  38.4  gms.  (NH4)2SO4  per  100 
gms.  sat.  solution. 

SOLUBILITY  IN  AQUEOUS  AMMONIA  SOLUTIONS  AT  25°. 

(D'Ans  and  Schreiner,  1910.) 


Mols.  per  1000  Gms.  Sat.  Sol. 


Gms.  per  looo^Gms.  Sat.  Sol. 


(NHa). 

(NH4)2S04. 

0 

3-28 

I  .02 

2.60, 

i-95 

2.13 

3-44 

i-S9 

5-35 

i  .16 

7-i3 

0.78 

9-47 

0 

'(NH3). 

(NH4)2S04. 

O 

433-4 

17.4 

343-6 

33-2 

281.5 

58.6 

210.  1 

91.1 

153-3 

121.4 

103 

161.2 

0 

SOLUBILITY  OF  AMMONIUM  SULFATE  IN  AQUEOUS  SOLUTIONS  OF  COPPER 
SULFATE  AT  30°  AND  VICE  VERSA. 

(Schreinemakers,  1910.) 


Gms.  per  100  Gms.  Sat. 
Solution. 


CuS04. 

o 


Solid  Phase. 


Gms.  per  100  Gms.  Sat. 
Solution. 


Solid  Phase. 


44 

38.32 

29.27 

17.53 

9.33 


(NH4)2SO4 


8.19 


1.  1.  6 


1.  1.6 


CuSO4. 

13.65 
16.77 

20.53  i.i.6-fCuSO4.5H2O 
20.19        CuSO4.5H2O 
°  20.32 

*  =  Solubility  of  1.1.6  in  water. 

1.  1.6  =  CuSO4(NH4)2SO4.6H2O. 

Several  additional  determinations  for  the  above  system  at  19°,  are  given  by 
Riidorff  (1873),  and  by  Schiff  (1859). 


0.77 
1.57 

4-°S 
11.03 


(NH4)2S04+i.i.6  6.98 
5.79 
2.45 


AMMONIUM   SULFATE 


64 


SOLUBILITY  OF  AMMONIUM  SULFATE  IN  AQUEOUS  SOLUTIONS  OF  FERROUS 
SULFATE  AT  30°  AND  VICE  VERSA. 

(Schreinemakers,  1910  a.) 


Gms. 

per  100  Gi 

Solution. 

T1S. 

Sat. 

Solid  Phase. 

(NH4)2S04 
(NH)SO+i.i.6 

1.  1.6 
it 

u 

Gms.  per  100  Gms 
Solution. 

.Sat. 

Solid  Phase. 

1.  1.6 

it 

i.i.6+FeSO4.7H2O 
FeSO4.7H20 

(NH4)2S04. 
'44.27 
43-88 
34.24 
19.64 
16.29 

n-45 

FeS04. 
O 

o-79 

1.72 

5-70 

7-95 

(NH4)2S04. 
8.90 
6.44 
5-91 
5-24 
O 

FeS04.    ' 
17.64 

23-59 
25.24 
25.24 
24.90' 

1.1.6  =  (NH4)2SO4.FeSO4.6H2O. 
Data  for  the  quaternary  system  (NH4)2SO4o  +  FeSO4  +  Li2SO4  +  H2O  at  30° 
are.  also  given. 

SOLUBILITY  OF  AMMONIUM  SULFATE  IN  AQUEOUS  SOLUTIONS  OF  LITHIUM 
SULFATE  AND  VICE  VERSA. 

(Schreinemakers,  Cocheret,  Filippo  and  deWaal,  igos^igo;.) 


Results  at  30°. 


Results  at  50°. 


Gms.  per  100  Gms.  Sat. 
Solution. 

Solid  Phase. 

Gms.  per  100  Gms.  Sat. 
Solution. 

Solid  Phase. 

(NH4)2S04. 

Li2S04- 

(NH4)2S04. 

Li2S04. 

44 

.1 

0 

(NHJjSO* 

45 

•7 

0 

(NIL^SO, 

40 

.8 

3 

43 

•05 

5.86 

(NH4)2SO4+NH4LiSO4 

39 

•5 

6.6 

(NH4)2SO4+NH4LiSO4 

19 

•65 

16.35 

NH4LiSO4 

30 

10 

NH4LiSO4 

13 

.90 

21.20 

" 

21 

.6 

15 

« 

13 

•97 

21.23 

NH4LiS04+Li2S04.H2O 

15 

20 

« 

ii 

•45 

21-75 

Li2SO4.H2O 

12 

-5 

21.9 

NH4LiSO4+Li2SO4.H2O 

9 

•63 

22.79 

" 

8 

•9 

23 

Li2SO4.H2O 

8 

•58 

23.09 

« 

0 

25.1 

" 

7 

•56 

22.86 

« 

o 

24-3 

" 

Additional  data  for  the  triple  points  of  the  above  system  at  20°,  57°  and  97° 
are  given  by  Spielrein  (1913),  but  the  terms  in  which  the  results  are  presented 
are  not  clearly  shown. 

Data  for  the  quaternary  system,  ammonium  sulfate,  lithium  sulfate,  alco'hol 
and  water  at  6.5°,  30°  and  50°  are  given  by  Schreinemakers  and  van  Dorp  (1907). 

A  mixture  of  an  excess  of  ammonium  and  of  potassium  sulfates  in  water  at 
19°  was  found  by  Rudorff  (1873)  to  contain  37.97  gms.^  (NH4)2SO4  +  39-3  gms. 
K2SO4  per  100  gms.  sat.  solution. 

SOLUBILITY  OF  AMMONIUM  SULFATE  IN  AQUEOUS  SOLUTIONS  OF  SULFURIC 

ACID  AT  30°. 

(Van  Dorp,  1910  and  1911.) 


Gms.  per  100  Gms.  Sat. 
Solution. 

(NH4)2S04.  * 

H2S04. 

44-3 
43-6 

O 
10 

44.1 

13.2 

42.9 

15 

41 
40.8 

20 
25 

43 
45-5 

30 
33-8 

42.3 

35 

Solid  Phase. 

(NH4)2S04 
(NH4)2S04+3.i 


3.i+(NH4)HS04 
(NH4)HSO4 
3.i=3[(NH4)2S04].H2SO. 


Gms.  per  100  Gms.  Sat. 
Solution. 

(NH4)2S04. 

H2S04. 

32-8 

40 

26.1 

45 

20.9 

50 

I7.6 

55 

I7.8 

60 

20 

61.7 

30 

62.9 

37 

62.2 

Solid  Phase. 

(NHOHSO 


6s  AMMONIUM   SULFATE 

Data  for  the  solubility  of  ammonium  sulfate  in  aqueous  solutions  of  sulfuric 
acid  of  concentration  extending  to  10  gm.  mols.  per  liter,  are  given  by  D'Ans 
(1909  and  1913). 

Data  for  the  solubility  of  ammonium  and  lithium  sulfates  in  concentrated 
sun  uric  acid  containing  traces  of  water,  at  30°,  are  given  by  Van  Dorp  (1913-14). 


SOLUBILITY  OF  AMMONIUM  SULFATE  IN  AQUEOUS  SOLUTION  OF  ETHYL 
ALCOHOL  AT  30°  AND  AT  50°. 

(Results  at  30°,  Wibaut,  1909;  at  50°,  Schreinemakers  and.de  Baat,  1907.) 

Results  at  30°.     Two  liquid  layers  are  formed  at  concentrations  of  alcohol 
between  5.8  and  62%.     These  have  the  compositions: 

Upper  Layer.  Lower  Layer. 

Gms.  per  100  Gms.  Sat  Solution.  Gms.  per  100  Gms.  Sat.  Solution. 


(NH4)2SO4.  C2H8OH.  H2O.  (NH»)jSO4.  QHBOH.  H2O. 

2.2  56.6  41.2  37.1  5.8  57.1 

2.6  54.5  42.9  35.7  6.3  58 

3-4  52-3  44-3  33-8  7-4  $8-8 

13.2  31.8  55.  21.7  18.4  59.9 

17  25  58  17  25  58 

At  a  concentration  of  62%  alcohol  the  liquid  is  homogeneous  and  contains 
1.3  gms.  (NH4)2SO4  per  100  gms.  sat.  solution,  At  90.4%  alcohol  no  (NH4)2SO4 
is  dissolved. 

Results  at  50°. 

Gms.  per  too  Gms.  Saturated  Solution. 


43.02  2.32    '  54.66 

41.1  4-1  54-8 

1-2  64.5  34.3 

0-2  75.5  24.3 

Between  the  concentrations  4.1  and  64.5%  C2H5OH  the  mixtures  separate 

into  two  layers.     The  percentage  composition  of  each  member  of  several  such 
conjoined  layers,  is  as  follows: 

Upper  Layer.  Lower  Layer. 

Gms.  per  100  Gms.  Sat.  Solution.  Gms.  per  roo  Gms.  Sat.  Solution. 


(NH4)2SO4.  QHSOH.  H2O.  (NHt)iSO4.  QHsOH.  H2O. 

1.2  64.5  34.3  4I.I  4.1  54.8 

1.6  60  38.4  36.8  6  57.2 

3.8  50  46.2  30.8  9  60.2 

7.4  40  52.6  26.6  12  61.4 

10  34.4  55.6  23.6  15  61.4 

Two  determinations  at  o°  Jby  deWaal  (1910)  gave  30  gms.  (NH4)2SO4  per  100 
gms.  sat.  solution  in  9.41%  alcohol  and  0.14  gm.  (NH4)2SO4  in  73.03%  alcohol. 
Between  these  concentrations  of  alcohol  two  liquid  layers  are  formed. 

loo  gms.  95%  formic  acid  dissolve  25.4  gms.  (NH4)2SO4  at  16.5°. 

(Aschan,  1913.) 


AMMONIUM   SULFATE  66 

SOLUBILITY  OF  AMMONIUM  SULFATE  IN  AQUEOUS  ETHYL  ALCOHOL  SOLUTIONS. 

(Continued.) 

(Traube  and  Neuberg  —  Z  physik.  Chem.  i,  510,  '87;  Bodlander  —  Ibid.  7,  318,  '91;  Schreinemaker  — 
Ibid.  23,  657,  '97  ;  de  Bruyn —  Ibid.  32,  68,  'oo;  Linebarger  —  Am.  Ch.  J.  14,  380,  '"92.) 


Upper  Layer  Results. 
Grams  per  100  Gms.  Solu- 
tion at  io°-4o°. 

Lower  Layer  Results. 
Gms.  C8H5OH      Gms.  (NH<)2SO4  per  100  g. 
per  100  Gms.                     Solution  at: 

CaHeOH. 

(NH4)2S04. 

Solution. 

6.5°. 

IS0- 

33°. 

100 

O-O 

O 

42  .O 

42.6 

44 

80 

o.-i 

2-5 

39-o 

40.2 

? 

70 

o-3 

36.2 

37-2 

? 

60 

1.4 

7-5 

33-2 

34-5 

42 

50 

3-2 

IO-O 

30.0 

31.0 

35 

45 

4.8 

12.5 

27.2 

28.0 

40 

6.6 

15-0 

24.6 

25.2 

? 

35 

9.2 

'75 

22  .O 

22.4 

? 

30 

12.2 

20-0 

20.0 

20.  o 

? 

25 

14.6 

NOTE.  —  When  ammonium  sulfate  is  added  to  aqueous  solutions  of  alcohol, 
it  is  found  that  for  certain  concentrations  and  temperatures  the  solutions  sep- 
arate into  two  liquid  layers,  the  upper  of  which  contains  the  larger  percentage 
of  alcohol. 

Most  of  the  determinations  which  have  been  made  upon  this  system,  as  con- 
tained in  the  papers  referred  to  above,  are  given  in  terms  of  grams  of  ammo- 
nium sulfate,  of  alcohol  and  of  water  per  100  grams  of  these  three  components 
taken  together.  Those  results  which  are  given  in  other  terms  can  be  readily 
calculated  to  this  basis,  and  it  is,  therefore,  possible  to  make  a  comparison  of  the 
several  sets  of  determinations  by  plotting  on  cross-section  paper  and  drawing 
curves  through  the  points.  In  the  present  case  the  grams  of  alcohol  per  100 
grams  of  solution  were  taken  as  ordinates,  and  the  grams  of  ammonium  sulfate 
in  the  same  quantity  of  each  solution  taken  as  abscissae.  It  was  found  that  a 
single  curve  could  be  drawn  through  practically  all  the  points  representing  the 
upper  layer  solutions  at  the  several  temperatures,  but  the  points  for  the  solutions 
containing  the  larger  amounts  of  water  gave  curves  which  diverged  with  increase 
of  temperature.  The  results  given  for  33°  in  the  above  table  are  not  to 
be  accepted  as  correct  until  further  work  has  been  done. 

SOLUBILITY  OF  AMMONIUM  SULFATE  IN  AQUEOUS  PROPYL  ALCOHOL  SOLUTIONS 

AT  20°. 
(Linebarger — Am.  Ch.  J.  14, 380,  '92.) 


Gms  per  100  Gms, 

Gms.  per 

100  Gms. 

Solution. 

Solution  . 

CaH7OH. 

(NH4)2SO4. 

C3H7OH. 

(NH4)2SO4c 

70 

0-4 

40 

3-2 

60 

1.0 

30 

4.8 

50 

2.0 

20 

6.7 

67     AMMONIUM  Cadmium  SULFATE 

AMMONIUM  Cadmium  SULFATE     (NH4)2Cd(SO4)26H2O. 

100  cc.  H2O  dissolve  72.3  gms.  (NH4)2Cd(SO4)2  at  25°.  (Locke,  1901.) 

AMMONIUM  Chromium  SULFATE  (Alum)  (NH4)2Cr2(SO4)4.24H2O. 

100  cc.  H2O  dissolve  10.78  gms.  anhydrous  or  21.21  gms.  hydrated  salt  at  25°. 

(Locke,  1901.) 

AMMONIUM  Cobalt  SULFATE  (NH4)2Co(SO4)2.6H2O. 
SOLUBILITY  IN  WATER. 


(Tobler  —  Liebig's  AnnalenQS,  193,  '55;  v.  Hauer—  J.  pr.  Chem.  74,  433.  '58;  at  25°,  Locke—  Am 
Ch.  J.  27,  459.  V>i.) 

Gms.  (> 

rH4)2Co(S04)2                                 Gms.  (NH4)2Co(SO4)2 

t°.                  Per 

ioo  Gms. 

t°. 

per 

ioo  Gms. 

Water. 

Solution. 

'Water. 

Solution.' 

0             .6.0 

5-7 

40 

22  -O 

18.0 

10          9.5 

8.7 

50 

27.0 

21-3 

2O            I3-O 

"•5 

60 

33-5 

25.1 

25            14.72 

12.8 

70 

40.0 

28.6 

30            17.0 

14-5 

80 

49-o 

32-9 

NOTE.  —  The  determinations  reported  by  the  above  named  inves- 
tigators were  plotted  on  cross-section  paper  and  although  considerable 
variations  were  noted,  an  average  curve  which  probably  represents 
very  nearly  the  true  conditions  was  drawn  through  them,  and  the  above 
table  made  from  this  curve. 

AMMONIUM  Indium  SULFATE  (NH4)2In2(SO4)4.24H2O. 

ioo  gms.  H2O  dissolve  200  gms.  salt  at  16°  and  400  gms.  at  30°.     (Rossler,  1873-) 


AMMONIUM  Iron  SULFATE  (Alum)  (NH4)2Fe2(SO4)4.24H2O. 

ioo  cc.  H2O  dissolve  44 
25°.     Sp.  gr.  of  saturated  j 


ioo  cc.  H2O  dissolve  44.15  gms.  anhydrous  or  124.40  gms.  hydrated  salt  at 
solution  at  15°  =  1.203.  (Locke,  1901.) 


AMMONIUM   Iron   SULFATE  (ferrous)    (NH4)2Fe(SO4)2.6H2O. 

SOLUBILITY  IN  WATER. 
(Tobler;  at  25°,  Locke  —  Am.  Ch.  J.  2KK,  459,  '01.) 


0 

G.  (NH4)2Fe(S04)2 

0 

G.  (NH4)2Fe(SO4)2 

0 

G,  (NH4)2Fe(S04)2 

* 

per  ioo  g.  H2O. 

per  ioo  g.  H2O. 

per  ioo  g.  H2O. 

o 

12  5 

25 

25.o(T) 

50 

40 

15 

20-0 

25 

35-i(L) 

70 

52 

40 

33  o 

AMMONIUM  Lead  SULFATE  (NH4)2SO4.PbSO4. 
SOLUBILITY  IN  WATER. 

(Barre,  1909.) 
Gms.  (NH4)2SO4  per  ioo  Gms. 


Sat.  Solution. 

Water. 

20 

12.17 

13.86 

50 

16.15 

19.25 

75 

19.52 

24.31 

IOO 

22.74 

29.42 

(NH4)2SO4.PbSO4 


AMMONIUM  Lithium  SULFATE      68 

AMMONIUM  Lithium  SULFATE   NH4LiSO4. 

SOLUBILITY  IN  WATER. 

(Schreinemakers,  Cocheret,  Filippo  and  deWaal,  1905,  1907.; 

Cms.  NH4LiSO4  Cms.  NH4LiSO4 

t°.  per  100  Cms.  Solid  Phase.  t°.         per  100  Gms.         Solid  Phase. 

Sat.  Sol.  Sat.  Sol. 

o  o  Ice               -10  35.25      NKjLiSC^ 

-  5  14  +10  35-58 

-io  23.5  30  ^.87 

-15  29.7  50  36 

-2o.6Eutec.  35.15  Ice+NH4LiSO4        70  36.18 

AMMONIUM  Magnesium  SULFATE    (NH4)2Mg(SO4)2. 

SOLUBILITY  OF  AMMONIUM  MAGNESIUM  SULFATE  IN  WATER. 

(Porlezza,  1914.) 

to.             Gms  per  xoo  Gms.  ^  ^                ^  Cms.  per  .zoo  Gms. 

Sat.  Sol.      Water.  Sat.  Sol.  Water. 

—0.34                  1. 01         1.02  Ice                      20  15.23  17.96  (NH4)2Mg(SO4)a 

—0.8o                  2.98        3.07  25  16.45  19-69 

-1.23                  4.92        5.17  30  17.84  21.71 

—  1. 60                  6.56        7-02  40  20.51  25.86 

—  2.02                  8.34        9.10  "                       50  23.18  30.17 

-2.34Eutec lce+(NH4)2Mg(S04)2     60    26.02    35.17 

O  10.58      11.83         (NILJMgSO,  80     32.58     48.32 

io       12.75  14.61      "       loo  39.66  65.72     " 

AMMONIUM  Manganese  SULFATE   (NH4)2Mn(S04)2.6H2O. 

100  cc.  water  dissolve  37.2  gms.  (NH4)2Mn(SO4)2  at  25°.  (Locke,  1901.) 

AMMONIUM  Nickel  SULFATE  (NH4)2Ni(SO4)2.6H2O. 
SOLUBILITY  IN  WATER. 

(Average  curve  from  Tobler,  Locke,  at  25°.) 


G.  (NH4)2Ni(S04)2 

G.  (NH4)2Ni(S04)2 

t°. 

per 

ioo  Gms. 

t°. 

per 

ioo  Gms. 

Water. 

Solution. 

Water. 

Solution. 

0 

1.0 

0-99 

40 

12  .O 

IO.72 

10 

4.0 

3-85 

50 

14-5 

12.96 

20 

6-5 

6.10 

60 

17-0 

14-53 

25 

7-57 

7.04 

70 

20.  o 

16.66 

30 

9.0 

8-45 

AMMONIUM  Sodium  SULFATE  NH4NaSO4.2H2O. 

ioo  gms.  water  dissolve  46.6  gms.  NH4.NaSO4.2H2O  at  15°  Sp.  Gr.,  of  Sol. 
1.1749. 

AMMONIUM  Strontium  SULFATE  (NH4)2SO4.SrSO4. 
SOLUBILITY  IN  WATER. 

(Barre,  1909.) 

t°.  Gms.^Hj.SO.perxooGms.  Solid  Phase. 

Sat.  Solution.  Water. 

50     <43-99     78.54 
75      45-40     83.15 
ioo      46.27     66.2 


69    AMMONIUM  Vanadium  SULFATE 

AMMONIUM  Vanadium  SULFATE  (Alum)    (NH4)2V2(SO4)424H2O. 

100  cc.  H2O  dissolve  31.69  gms.  anhydrous  or  78.50  gms.  hydrated  salt  at  25°. 

AMMONIUM  Zinc  SULFATE   (NH4)2Zn(SO4)2.6H2O. 
SOLUBILITY  IN  WATER. 

(Average  curve,  see  NOTE,  p.  67,  Tobler,  Locke,  at  25°.) 

G.  (NHJzZntSO^a  G.  (NIL^ZnCSOJj 

^•f  per  100  Gms.  $o^  per  100  Gms. 

Solution.          Water.  Solution.       Water. 

o          6.54          7.0  40        16.66        20 

10  8.67  9.5  50  20.0  25 

20  II. II  12-5  6b  23.1  30 

25    12.36    14.1        70   25.9    35 
30   13-79   16.0        80   29.6    42 

AMMONIUM  PERSULFATE   (NH^S-A. 

100  parts  H2O  dissolve  58.2  parts  (NHOsSgOg  at  o°.  (Marshall,  1891.7 

AMMONIUM  Sodium  Hydrogen  SULFITE  (NH4)Na2H(SO3)24H2O. 
100  gms.  H2O  dissolve  42.3  gms.  salt  at  12.4°  and  48.5°  gms.  at  15°. 

(Schwincker,  1889.) 

AMMONIUM  Antimony  SULFIDE  (Sulfoantimonate)  (NH4)3SbS4.4H2O. 
SOLUBILITY  IN  WATER  AND  IN  AQUEOUS  ALCOHOL. 

(Donk,  1908.) 
In  Water.  In  Aqueous  Alcohol  at  10°. 

,„  Gms.  (NH4)3SbS4  c:  IM  Pll!10,  Gms.  per  100  Gms.  Sat.  Solution. 

per  100  Gms.  Sat.  Sol.  '     C2H6OH.  (NH^SbS..  " 

—  1.9  9.9  Ice  o  43.2 

-  5  20  5-i  35-9 

-  8  30.2  19.1  23.1 

-13.5          41-6          Ice+(NH4)3SbS4.4H2O  43.1  8.7 

o              41.6               (NH4)3SbS4.4H2O  53.1  4.1 

+  20               47-7  93-3  o 

30  54-5 

AMMONIUM  0-Naphthalene  Mono  SULFONATE  Ci0Hi7SO3NH4. 

100  cc.  of  the  saturated  aqueous  solution  contain  13.05  gms.  of  the  salt  at 

25°,  and  dz$  =  1.034.  (witt»  I9I5-> 

AMMONIUM  Phenanthrene  Mono  SULFONATES  Ci4H9SO3NH4  (2),  (3)  and 
SOLUBILITY  IN  WATER  AT  20°. 

(Sandquist,  1912.) 

ioo  gms.  H2O  dissolve  0.37  gms.  Ci4H9SO3NH4  (2). 
100  gms.  H2O  dissolve  0.26  gms.  d4H9SO3NH4  (3). 
ioo  gms.  H2O  dissolve  4.41  gms.  Ci4H9SO3NH4  (10). 

AMMONIUM  2.5  di-iodobenzene  SULFONATE  C6H3I2SO3(NH4). 

ioo  gms.  H2O  dissolve  4.35  gms.  salt  at  20°.  (Boyle,  1909.) 

AMMONiUM  TARTRATES   (NH4)2C4H4O6. 

ioo  cc.  H2O  dissolve  2.83  gms.  (NH4)2C4H4O6.2H2O  at  o°.  (Fenton,  1898.) 

ioo  cc.  H2O  dissolve  5.9  gms.  (NH4)2C4H4O6  at  15°  (d  =  1.04). 

(Greenish  and  Smith,  1903.) 

AMMONIUM  Lithium  TARTRATES  dextro  and  racemic. 

ioo  gms.  sat.  sol.  inH2O  contain  13. 104  gms.  racemate(NH4)Li(C4H4O6).H2Oat2O°. 

ioo  gms.  sat.  solution  in  H2O  contain  14.186  gms.  dextro  (NH4)Li(C4H4O6). 
£  H2O  at  20°.  (Schlossberg,  1900.) 

Freezing-point  data  for  mixtures  of  water  and  ammonium  tartrate  and  of 
water  and  ammonium  racemate  are  given  by  Bruni  and  Finzi  (1905). 


AMMONIUM  THIOCYANATE         70 

AMMONIUM  THIOCYANATE  NH4SCN 

SOLUBILITY  IN  WATER. 

(Average  curve  from  results  of  Riidorff,  1868  and  1872;  Wassilijew,  1910;   Smits  and  Kettner,  1912.) 

to  Gms.  NH4SCN  -,.,  p,  «          Cms.  NH4SCN  Solid 

*  '       per  100  Gms.  Sat.  Sol.  Phase'  *  '    per  too  Gms.  Sat.  Sol.      Phase. 

-io  20  Ice                     o  54.5        NH4SCN 

-15  28.5  +10  59 

-20  35.5  20  63 

-25.2  42Eutec.  Ice+NH4SCN          25  65.5 

-io  50  NKtSCN              30  67.5 

Data  for  the  system  ammonium  thiocyanate,  thiourea  and  water  at  25°  are 
given  by  Smits  and  Kettner  (1912)  in  the  form  of  a  triangular  diagram,  but  the 
numerical  results  are  omitted.  The  diagram  confirms  the  freezing-point  lowering 
results  in  showing  that  the  molecular  compound  NhUSCN^NH^CS  is  formed. 

IOO  gms.  acetonitrile  dissolve  7.52  gms.  NH4SCN  at  l8°.     (Naumann  and  Schier,  1914.) 

Freezing-point  curves  have  been  determined  for  the  following  mixtures: 

Ammonium  Thiocyanate  +  Ammonia.  (Bradley  and  Alexander,  1912.) 

+  Potassium  Thiocyanate.  (Wrzesnewsky,  1912.) 

+  Thiocarbamide  (Thiourea).       (Renolds  and  Werner,  1903; 

Findlay,  1904;  Atkins  and  Werner,  1912;  Smits  and  Kettner,  1912;  Wrzesnewsky,  1912.) 

AMMONIUM   URATE  (Primary)  CgHsN^NH*. 

SOLUBILITY  OF  THE  LACTAM  AND  LACTIM  FORMS  IN  WATER. 

(Gudzeit,  1908-09.) 
Gms.  of  Each  per  1000  cc.  Sat.  Solution. 

Lactam.  Lactim.  Mixture  of  the  Two. 

1  8  0-456  0.304  0.414 

37  0.817  0.540  0.741 

AMMONIUM  Meta  VANADATE  NH4VO3. 

SOLUBILITY  IN  WATER  AND  IN  AQUEOUS  AMMONIUM  SALT  AND  AMMONIUM 
HYDROXIDE  SOLUTIONS. 

(Meyer,  1909.) 
Gms.  per  1000  cc.  in  Each  Solvent. 


18 
25 
35 
45 

55 
70 

loo  cc.  anhydrous  hydrazine  dissolve  2  gms.  ammonium  metavanadate  at 
room  temp.  (Welsh  and  Broderson,  1915.) 

AMYGDALIN   C20H27NO.3H2O. 

IOO  gms.  trichlorethylene  dissolve  0.029  gm-  amygdalin  at  15°. 

(Wester  and  Bruins,  1914.) 

AMYL  ACETATE  BUTYRATE,   FORMATE,  etc. 

SOLUBILITY  IN  WATER  AND  IN  AQUEOUS  ALCOHOL  AT  20°. 

[(Bancroft—  Phys.  Rev.  3,  131,  106,  205,  'Q5-'o6;  Traube.  —  Ber.  17,  2304,  '84.) 

p.  t._  cc.  Ester  per        Sp.  Gr.  v  .  cc.  Ester  per  Sp.  Gr. 

loocc.  H20.        of  Ester.  100  cc.  H2O.  of  Ester. 

Amy  1  acetate        0.2  0.88     Amyl  propionate     o.i  0.88 

Iso  amyl  acetate  0.2(1.2?)       ...      Iso  amyl  formate    0.3  (gms.  at  22°) 
Amyl  butyrate    0-06  0.85 


Water. 

0.05  n. 
NH4C1. 

o.i  n. 
NH4C1. 

0.05  n. 
NH4NO3. 

o.i  n. 
NH4N03. 

0.0668  n. 
NH3. 

0.245  n. 
NH3. 

0.588  n. 
NH3. 

4-35 

1.66 

0.41 

.1.67 

0.58 

5-58 

7-97 

1  2.  06 

6.08 

2.63 

I.I7 

2.77 

1.23 

7.06 

8.58 

12.66 

IO.  77 

r    21 

2  .60 

I  cj    71 

8  88 

5  40 

IQ    O7 

ii  18 

7  40 

3O.A7 

AMYL  ACETATE 


SOLUBILITY  IN  AQUEOUS  ALCOHOL  AT  ROOM  TEMPERATURE. 

(Pfeiffer,  1892.) 

Solubility  of  I  so  Amyl  Acetate  Solubility  of  Amyl  Acetate  and  Amyl 
in  Aq.  Alcohol  Mixtures.  Formate  in  Aq.  Alcohol  Mixtures. 


Per  5  cc.  C2H5OH. 


cc.  H2O. 

cc.IsoAmyl 
acetate. 

7 
6 

0.41 
0-7 

3-6i 

I-3I 

3-o 

3.01 
2.60 

4-0 
S-o 

cc. 

in  Mixture. 


cc.  H2O  added  to  cause  separation 
of  second  phase  in  mixtures  of  the 
given  amounts  of  alcohol  and  3  cc 
portions  of : 


Amyl 
Formate. 


Amyl 
Acetate. 


3  i. 80  1.76 

9  8.77  9.03 

15  17.01  17.52 

21         27.06       26.99 
27         38-3I       37-23 

33  So-71     48-41 

39  65.21 

45  85.10 

48  94 . 20 

AMYL  ALCOHOL  C6HUOH. 

SOLUBILITY  OF  AMYL  ALCOHOL  IN  WATER  AT  22°. 

(Herz  —  Ber.  31,  2671,  '98.) 

ioo  cc.  water  dissolve  3.284  cc.  amyl  alcohol.  Sp.  Gr.  of  solu- 
tion =  0.9949,  Volume  =  102.99  cc. 

ioo  cc.  amyl  alcohol  dissolve  2.214  cc.  water.  Sp.  Gr.  of  solu- 
tion =  0.8248,  Volume  =  101.28  cc. 

Sp.  Gr.  of  H2O  at  22°  =  0.9980;  Sp.  Gr.  of  amyl  alcohol  at  22°=  0.8133. 

SOLUBILITY  IN  AQUEOUS  SOLUTIONS  OF  ETHYL  ALCOHOL. 

(Pfeiffer,  1892;  Bancroft,  1895-96.) 

Mixture  of 


Mixture  of 

c.c.  H2O  added  to  * 

n«r*    A 

C6HUOH+C2HSOH 

Mixture  at 

C.C.                        C.C. 

9.1°. 

19.2°. 

3              3 

3-21 

3-5 

3               6 

IO-35 

10.80 

3               9 

18.34 

19.10 

3             12 

27.47 

29.15 

3             15 

41.25 

43-15 

c.c.  H2O  Added  to  * 
Mixture  at 


c.c. 

3 
6 

9 

12 
15 


c.c. 

3 
3 
3 
3 
3 


13.3  • 

3.36 

2.  2O 
2.10 
2.10 
2.10 


17.4°- 
3-47 
2.25 
2.15 
2.10 
2.IO 


.*  Just  enough  water  was  added  to  produce  cloudiness. 

NOTE.  —  The  effect  of  various  amounts  of  a  large  number  of  salts 
upon  the  temperature  (39.8°)  at  which  a  mixture  of  20  cc.  of  amyl 
alcohol  +  20  cc.  of  ethyl  alcohol  -f  32.9  cc.  of  water  becomes  homo- 
geneous has  been  investigated  by  Pfeiffer  (Z.  phys.  Ch.  9,  444,  '92). 
The  results  are  no  doubt  of  interest  from  a  solubility  standpoint,  but 
their  recalculation  to  terms  suitable  for  presentation  in  the  present 
compilation  has  not  been  attempted. 

DISTRIBUTION  OF  ISOAMYL  ALCOHOL  BETWEEN  WATER  AND  COTTON  SEED 

OIL  AT  25°. 

(Wroth  and  Reid,  1916.) 
Cms.  CjHuQH  per  ioo  c.c. 
Oil  Layer.  H2O  Layer. 

1.947  0.9153  0.470 

2.195  I.II56  0.508 

2.273  I.I050  0.486 

2.372  0.9995  0-421 


AMYL  ALCOHOL  72 

SOLUBILITY  OF  AMYL  ALCOHOL  IN  WATER  AND  IN  AQUEOUS  SOLUTIONS  OF 
ETHYL  AND  METHYL  ALCOHOLS. 

(Fontein,  1910.) 


t°. 


15 

20 

40 

60 

80 

IOO 

120 

140 

1 00 

170 

180 

187, 


In  Water. 

Gms.  CjHnOH  per 
ioo  Gms. 


H20 
Layer. 

C6HUOH 
Layer. 

4 

2.6 

90.7 

2.6 

90.6 

2.1 

89.5 

2 

88 

2-5 

86 

3 

83.8 

3-8 

80.8 

5 

76.4 

7-3 

70 

9-3 

65.1 

13-5 

57-3 

In  Aq.  Ethyl  Alcohol." 

In  Aq.  Methyl  Alcohol.f 

Gms.  CcHuOH  per 

Gms.  CsHnOH  per 

to 

ioo  Gms. 

t°. 

ioo  Gms. 

2H5OH+] 

320  CjHuQH 

CH3OH+H2O  CsHuOH* 

Layer. 

Layer. 

Layer. 

Layer. 

4-5 

16.2 

.  .  . 

3-6 

II 

.  .  . 

20 

20.8 

.  .  . 

20 

19-3 

.  .  . 

40 

26.7 

.  .  . 

38.4 

.  .  . 

78.4 

60 

33 

.  .  . 

40 

31.2 

78 

67.8 

24.4 

50 

37-i 

74.8 

70 

36,'s 

73-7 

60 

43-3 

71.6 

80 

40.8 

70.1 

70 

52.7 

65 

90 

47 

64 

72 

(crit. 

temp.) 

94.2 

(crit. 

temp.) 

(crit.  temp.) 

Of  33-55  per  cent  QHjOH. 


f  Of  33  Per  cent  CH3OH. 


The  "synthetic  method"  was  used  for  the  preceding  determinations.  Fer- 
mentation amyl  alcohol  of  b.  pt.  I3i°-I3i.4°  and  ^15.5  =  0.814  was  employed. 
It  contained  16%  of  optically  active  amyl  alcohol.  Many  other  series  of  deter- 
minations were  made  with  solvents  containing  other  percentages  of  ethyl  and 
methyl  alcohol.  Also,  other  series  were  made  for  the  above-named  ternary 
systems  at  constant  temperatures  from  which  binodal  curves  were  obtained. 
The  author  uses  a  very  ingenious  indirect  method  for  determining  the  composi- 
tion of  the  conjugated  solutions.  Data  are  also  given  for  the  distribution  of 
ethyl  alcohol  between  water  and  amyl  alcohol. 

"The  results  of  Alexejew  (1886)  for  the  solubility  of  amyl  alcohol  in  water 
agree  fairly  well  with  the  above  data. 

AMYL  AMINE  C6HU.NH2. 

The  freezing-point  curve  for  mixtures  of  amyl  amine  and  water  is  given  by 
Pickering  (1893). 

Iso  AMYLAMINE  HYDROCHLORIDE  C6Hn.NH2.HCl  (iso). 

IOO  gms.  H2O  dissolve  192.2  gms.  of  the  salt  at  25°.  (Peddle  and  Turner,  1913.) 

ioo  gms.  CHC13  dissolve  5.1  gms.  of  the  salt  at  25°. 

Data  for  the  distribution  of  e-chloramyl  amine  between  water  and  tetra- 
chlorethane  at  o°,  water  and  nitrobenzene  at  25°  and  water  and  benzene  at  25° 
are  given  by  Freundlich  and  Richards  (1912). 


AMYLENE   (Trimethylethylene)   (CH3)2C:  CHCH3. 

RECIPROCAL  'SOLUBILITY  IN  ANILINE;  DETERMINATIONS  BY  SYNTHETIC  METHOD. 

(Konowalow,  1903.) 

Gms.  Aniline  per  ioo  Gms. 
Amylene  Layer.  Aniline  Layer. 

28 


Gms.  Aniline  per  ioo  Gms. 
Amylene  Layer.  Aniline  Layer. 


19-5 
19.7 
20.5 
21-7 
24.2 


81.5 
80.5 

79-5 

78 

75-8 


10 

12 
13 
14 


34 

38.5 

45 


14.5  (crit.  temp.)     51.6 


73 
68 

64.7 
59 


•73  AMYLENE 

SOLUBILITY  OF  AMYLENE  IN  LIQUID  CARBON  DIOXIDE. 

(Buchner,  1905-06.) 

(Determinations  made  by  the  synthetic  method.) 

t°.     (crit.)  31  103  201 

Cms.  CsHio  per  100  gms.  sat.  sol.  o  38  100 

AMYLENE  HYDRATE   (CH3)2C(OH)CH2.CH8. 

•  The  distribution  coefficient  of  amylene  hydrate  between  olive  oil  and  water 
at  ord.  temp,  is  I.  (Baum,  1899.) 

ANDROMEDOTOXINE  C3iH6iOi0. 

SOLUBILITY  IN  SEVERAL  SOLVENTS  AT  12°  AND  AT  THE  BOILING-POINTS  OF 

THE  SOLVENTS. 

(Zaayer,  1886.) 

Gms.  CsiHjiOxo  per  100  Gms.  Sat.  Sol.  at  : 
Solvent.  t  --  -  >  -  -, 

12°.  B.  Pt. 

Water  2.81                0.87 

Ethyl  alcohol  (&&  =  0.821)  n  .70 

Amyl  alcohol  i  .  14 

Chloroform  o  .  26                o  .  26 

Commercial  ether  o  .  07               o  .  07 

Benzine  o  .  004 


ANETHOLE  (p  Propylanisole)  C 

SOLUBILITY  IN  AQUEOUS  ALCOHOL  AT  20° 

(Schimmel  and  Co.,  Reports,  Oct.  1895,  p.  6.) 

Vol.  per  cent  alcohol  =  -20        25        30        40        50 

Gm.  anethole  per  liter  aq.  alcohol  =  0.12     0.20    0.32    0.86     2.30 
333-3  gms-  anethole  dissolve  in  one  liter  of  90%  alcohol  at  room  temperature. 

(Squire  and  Caines,  1905.) 

Freezing-point  data  for  mixtures  of  anethole  and  menthol  are  given  by  Scheuer 
(1910). 

ANILINE  C6H6(NH2). 

SOLUBILITY  IN  WATER  AT  22°. 

(Herz,  1898;  see  also  Vaubel,  1895;  Aignan  and  Dugas,  1899.) 

loo  cc.  H2O  dissolve  3.481  cc.  C6H5(NH2)  —  Vol.  of  Sol.  =  103.48,  Sp.  Gr.  = 
0.9986. 

100  cc.  C6H6(NH2)  dissolve  5.22  cc.  H2O  —  Vol.  of  Sol.  =  104.96,  Sp.  Gr.  = 
1.0175. 

100  cc.  sat.  aq.  sol.  contain  3.607  gms.  C6H5NH2  at  25°.  (Reidel,  1906.) 

SOLUBILITY  OF  ANILINE  IN  WATER.     (Determination  by  synthetic  method.) 

(Sidgwick,  Pickford  and  Wilsden,  1911.) 
to  Gms.  QHSNH2  per  100  Gms.  Gms.  QHiNHz  per^ioo  Gms. 

Aq.  Layer.         Aniline  Layer.  Aq.  Layer.  Aniline  Layer. 

13.8  3-6lI  5.12  (200)  120  Q.I  14.6 

3°  3-7  5-4  130          ii-2  16.9 

50  4.2  6.4  140          13.5  19.5 

70  5  7.7  150          17.1  24 

9O  6.4  9.9  l6o  22  32 

no  8  13  165          26.1 

The  critical  solution  temperature  for  aniline  and  water  is  168°. 
Alexejew  (1886)  and  Rothmund   (1898)  obtained  results  for  the  preceding 

system  which  differ  in  part  quite  widely  from  the  above  table. 

More  recent  determinations,  in  terms  of  cc.  aniline  per  IOO  cc.  of  mixture,  are 

given  by  Kolthoff  (1917). 


ANILINE 


74 


SOLUBILITY  OF  ANILINE  IN  AQUEOUS  SOLUTIONS  OF  ANILINE  HYDROCHLORIDE. 

(Sidgwick,  Pickford  and  Wilsden,  1911.) 

The  temperatures  at  which  a  second  liquid  phase  separated  from  homogeneous 
mixtures  of  known  amounts  of  aniline  +  HC1  +  H2O  were  determined  for  a  very 
extensive  series  of  mixtures.  The  procedure  consisted  in  first  heating  a  given 
mixture  until  it  became  homogeneous  and  then  cooling  it  slowly,  with  constant 
shaking.  A  critical  turbidity  preceding  the  actual  separation  by  a  few  de- 
grees was  always  noticed.  The  point  of  separation  was  taken  as  that  at  which 
a  small  gas  flame  seen  through  the  liquid  disappeared.  At  higher  temper- 
atures, the  observations  were  made  on  mixtures  contained  in  sealed  bulbs.  In 
the  actual  experiments,  binodal  curves  for  mixtures  of  Aq.  HC1  (of  different 
strengths)  and  aniline  were  determined.  By  interpolation  from  these,  the  fol- 
lowing isothermal  curves  were  obtained. 


Isotherm  for  15°. 


Isotherm  for  25°. 


H2O  Rich  Mixtures. 
Gms.  per  100  Cms. 
Sat.  Solution. 

Aniline  Rich  Mixtures.  ' 
Gms.  per  100  Gms. 
Sat.  Solution. 

H2O  Rich  Mixtures. 
Gms.  per  100  Gms. 
Sat.  Solution. 

Aniline  Rich  Mixtures. 
Gms.  per  100  Gms. 
Sat.  Solution. 

C6H5NH2.  C6H5NH2.HC1. 

H2O.    C6HBNH2.HCi. 

C«H6NH2.  C,H6NH2.HC1.  '    H2O.   C6H5NH2.HC1. 

3-6IS 

0 

7 

.276 

3 

.025 

3 

.681 

0 

14 

8.884 

3-7QI 

1-529 

7 

.231 

i 

.989 

4 

.020 

3.02 

10. 

84 

6.062 

4.144 

5.829 

5 

.816 

i 

•  195 

5 

.380 

ii  .40 

6. 

949 

1.912 

4.940 

11.44 

5 

.230 

o 

•340 

7 

.023 

15-83 

6. 

043 

0.828 

5-995 

16.03 

5 

.006 

0 

.163 

ii 

.86 

19.02 

5- 

568 

0-363 

10.44 

19-35 

4 

.960 

0 

.080 

3i 

•35 

20.15 

5- 

3H 

0.089 

26.80 

21.49 

4 

.942 

o 

59 

•95 

15-55 

5- 

299 

0 

9-30 
21.21 


Isotherm  for  40°. 


Isotherm  for  60°. 


3-941 

0 

15-65   8 

•752 

4.58 

0 

14 

.27 

5-93 

4-i87- 

i 

523 

10 

.21 

4 

.243 

4.87 

1.512 

9 

.569 

2.632 

4-371 

3 

009 

7 

.874 

2 

.166 

5.13 

2.984 

8 

.109 

1.  112 

4.823 

e 

815 

7 

.069 

I 

.452 

5.67 

5.762 

7 

•492 

0.4876 

6.2IO 

II  . 

30 

7 

.058 

0 

.9669 

7.69 

II  .14 

7 

.051 

0.2284 

8.779 

15 

55 

6 

.225 

0 

-4052 

n-53 

15-25 

7 

.047 

O.II38 

38.69 

18 

5 

.940 

0 

.0960 

22.80 

16.66 

7 

.030 

0 

64.20 

12 

.84 

5 

•930 

0 

51.10 

14.36 

Isotherm  for  8e°. 


Isotherm  for  100°. 


5-66 

o 

12 

•31 

3-387 

7 

.10 

0 

41-57 

n-45 

5-95 

i 

•495 

9 

.848 

1-35° 

7 

.68 

I 

.467 

18.16 

4-995 

6.26 

2 

•950 

8 

.998 

0-5857 

8 

.10 

2 

.891 

12.76 

1.784 

7.11 

5 

.678 

8 

-524 

0.2769 

9 

.60 

5 

.522 

n-37 

0.1836 

9-95 

10 

•85 

8 

.512 

0.1387 

13 

.60 

10 

.41 

11.90 

0 

31.18 

14 

•85 

8 

.500 

0 

Isotherm  for  120°. 

o  17-94 

9.497      14.45 


2-459 
o 


T3-75 
38.75 


Isotherm  for  140°. 
o  29-52       4.043 

7-384     21.09       o 


The  authors  also  calculated  the  position  of  tie  lines  for  the  binodal  curves 
with  the  aid  of  distribution  coefficients,  which  they  determined  at  25  and  which 
are  quoted  in  a  subsequent  table  (page  78  following). 

Additional  data  for  the  system  aniline  +  HC1  +  H2O  at  o°,  25°  and  at  35 
are  given  by  Thonus  (1913),  and  for  aniline  -f  HC1  by  Leopold  (1910). 


75  ANILINE 

SOLUBILITY  OF  ANILINE  IN  AQUEOUS  SALT  SOLUTIONS  AT  18°. 

(Euler  —  Z.  physik.  Chem.  40,  307,  '04.) 

Aq.  Solution.        Cms.  Salt    Cms,  C6H5(NH2)  Aq.  Cms.  Salt   Cms.  C«H6(NH2) 

per  liter,     per  100  g.  solvent.  Solution.          per  liter,    per  looitsolvent! 

H2O  alone  o  3.61  i  wNaOH  40.06  1.90 

o.5wKCl  37.3  3.15  i  wLiCl  42.48  2.80 

iwKCl  74.6  2.68  iwCaCl2  67.25  3.00 

iwNaCl  58.5  2.55 

SOLUBILITY  OF  ANILINE  IN  AQUEOUS  ANILINE  HYDROCHLORIDE 
SOLUTIONS  AT  18°. 

(Lidow  — J.  russ.  phys.  chem.  Ges.  15,  420,  '83;  Ber.  16,  2297,  '83.) 
Per  cent  C6H6NH2HC1    Cms.  CeNsNHz  Per  cent  C6H5NH2JIC1      Cms.  CeHsNHj 

insolvent,  per  100  g.  Solvent  in  Solvent.  per  loog?  Solvent. 

5  3-8  30  39.2 

5-3  35  So-4 

SOLUBILITY  OF  ANILINE  IN  AQUEOUS  SOLUTIONS  OF  GLYCEROL  AND 
VICE  VERSA. 

(Kolthoff,  1917.) 

(The  liquids  were  measured  from  burets.     The  determinations  at  100°  were 
made  in  sealed  tubes.     The  others  were  made  in  open  tubes.) 

Results  for  the  Solubility  of  Aniline  in  Aqueous  Glycerol. 


Per  cent  Glycerol  in 
Aq.  Mixture  used. 

cc.  Am 

line  dissc 

lived  by 

ioo  cc.  of  Aq.  G 

Uycerol  of  Com 

:.  shown  at: 

18°.                        25°. 

36°. 

r  00°. 

o  (=  water) 

3 

•25 

3 

•4 

5-6 

9.9 

39 

5 

•15 

5 

•3 

.  .  . 

56 

7 

•5 

7 

.6 

28  (58* 

7o  Glycerol) 

65 

10 

. 

38  (66< 

7o        "     ) 

74-3 

ii 

•75 

12 

.1 

.  .  • 

.  .  . 

78 

20 

2O 

16 

... 

87 

70 

. 

.  .  . 

Results  for  the  Solubility  of  Aqueous  Glycerol  in  Aniline. 

Per  cent  Glycerol  in  CC-  °*  Aq>  Glycerol  Mixture  dissolved  by  too  cc.  Aniline  at: 

Aq.  Mixture  used. 

o  (=  water) 
39 
47 
56 
74-3 


DISTRIBUTION  OF  ANILINE  BETWEEN  WATER  AND  BENZENE  AT  25°. 

(Farmer  and  Warth,  1904.) 

Cms.  C6H5NH2  per  100  cc. 

Ratio. 


18°. 

25°- 

36°. 

IOO  . 

4.6 

5 

4 

5-3 

6.4 

5-2 

.  .  . 

•  •  • 

... 

7-9 

7-7 

.  .  . 

15  (58%  Glycerol) 

I3-I 

11.7 

... 

17(66%       "     ) 

I7.I 

14.8 

Water  Layer.  C6H6  Layer. 

0.0135  O.I3I2  9.7 

0.0122  0.1282  10.5 

0.0065  0.0656  10.  i 

.Data  for  the  distribution  between  water  and  benzene  at  25°  of  each  of  the  fol- 
lowing substituted  anilines;  o,  m  and  p  nitraniline,  chloraniline,  bromaniline, 
P  nitrosmethylaniline,  and  p  nitrosodimethylaniline  are  given  by  Farmer  and 
Warth  (1904). 


ANILINE  76 

SOLUBILITY  OF  ANILINE,  PHENOL  MIXTURES  IN  WATER. 

(Schreinemaker  —  Z.  physik.  Chem.  29,  584;  30,  460,  '09.) 


Mitture  used  =  2^.4  Mols.  Aniline 
+  74  6  Mols.  Phenol                „ 

Mixture  used  =  50  Mols.  Aniline 
+  50  Mols.  Phenol 

•  «                        Gms.  of  Mixture  per  ioo  Gms.      *   • 

Gms.  of  Mixture  per  ioo  Gms. 

*^Aq.  Layer.    A. 

+  P  .  Layer. 

Aq.  Layer.    A, 

,  +  P.  Layer. 

40 

5-o 

86-0 

40 

4-0 

91-5 

60 

55 

82.0 

80 

5-5 

85  5 

80 

8.0 

77  o 

IOO 

8.0 

82  o 

IOO 

12  5 

67  o 

120 

13  5 

73  5 

no 

19.0 

56.5 

130 

19.0 

66  o 

104 

(crit.  temp.)         33 

23  5 

58.0 

140 

(crit.  temp.)       35 

Determinations  in  above  table  by  "Synthetic  Method,"  see  NOTE,  p.  16. 
Schreinemakers  gives  results  for  several  other  mixtures  of  aniline  and  phenol 
which  yield  curves  entirely  similar  to  those  for  the  two  mixtures  here  shown. 

DISTRIBUTION  OF  ANILINE  BETWEEN: 

(Vaubel  —  J.  pr.  Chem  [2]  67,  477,  '03.) 

Water  and  Ether.  Water  and  Carbon  Tetrachloride. 

Composition  of  Solutions.         Gms.  CeHsNHain:         Com  position  jof  Solutions.     Gms.C6H6NH2  in: 

G.CeHfiNHa          ^  Aq.  EtLer     G.  CeHgNHa    "    gl  '    Aq.    '    CCU  ' 

Used.  Layer.         Layer.          Used.  Layer.     Layer. 

1.2478  50  cc.  H2O  50  cc.  H2O 

+  2occ.  Ether  0.1671  1.0807  °«3478  +2occ.CCl4  0.33580.012 

1.2478  50  cc.  H2O  50  cc.  H2O 

+  50  cc.  Ether  0.0835  1.1643  1.2478  +5occ.  CC14  0.2767  1.971 

1.2478  50  cc.  H2O  50  cc.  H2O 

4-  1  oo  cc.  Ether  0.0594  1.1884  1.2478  +ioocc.  CC14  0.1845  1.063 

SOLUBILITY  OF  ANILINE  IN  SULPHUR. 

(Alexejew  —  Ann.  Physik.  Chem.  28,  305,  '86.) 


.  loog.  Gms.  C6HsNH2  per  loog. 

S.  Layer.  Anilin  Layer.  S.  Layer.      Anilin  Layer. 

ioo  4  75  *3Q  I5  58 

no  6  70  135  17.5  47 

120  10  64  138  (crit.  temp.)         23     .  . 


DISTRIBUTION  OF  ANILINE  BETWEEN  WATER  AND  TOLUENE  AT  25°. 

(Riedel,  1906.) 

NOTE.  —  Mixtures  of  aniline  and  toluene  were  shaken  with  water  and  after 
separation  of  the  two  layers  the  Sp.  Gr.  of  the  A  :  T  mixture  (layer)  was  de- 
termined and  also  the  amount  of  aniline  in  each  layer. 


Solution  Shaken  with 
A  :  T  Mixture. 

Vol.  per  cent     Sp.  Gr.  of  A  :  T 
Aniline  :  Toluene  Mixture  after 
in  Mixtures  Used  .      Separation  . 

Gms.  C6H5N 

H2  in  ioo  cc.  c 

A  :  T  Layer. 

Aq.  Layer. 

HaO 

50:50                0.9257 

41-5 

2.14 

u 

25:75           0.8928 

20-7 

I  .5 

tt 

12.5:87.5       0.8737 

8.62 

0.86 

ti 

5.5:94.5       0.8661 

3-87 

o  45 

" 

2.5:97.5       0.8627 

1.68 

0.21 

The  author  also  gives  data  for  the  distribution  of  aniline  between  toluene 
and  aqueous  solutions  of  K2SO4,  KBO3,  Ba(OH)2,  Sr(OH)2  and  Ca(OH)2. 


77 


ANILINE 


SOLUBILITY  DATA  DETERMINED  BY  THE  FREEZING-POINT  METHOD  (see  foot- 
note, page  i)  ARE  GIVEN  FOR  MIXTURES  OF  ANILINE  (m.  pt.  —5.5°  to  —6.8°) 
AND  OTHER  COMPOUNDS. 


Name  and  M.  Pt.  of  the  Other  Com- 
pound of  Each  Mixture.. 

Nitrosodimethyl  aniline  (85.5°) 
Benzene  (5.42°) 
Nitrosobenzene  (63.5°) 
Nitrobenzene  (2.8°) 
o  Dinitrobenzene  (116.5°) 
m  (91°) 

P 

s  Trinitrobenzene  (122.2°) 
o  Chloronitrobenzene  (32°) 
»  (43°) 

P  "  (82.5°' 

Benzoic  acid  (121.25°) 
Chloroform  (-63°) 
o  Cresol  (30.4°) 
m      "      (4.2°) 
P       "      (33-2°) 
Ethylacetate  (-83.8°) 
Hydroquinone 
Allyl  mustard  oil 

o  Chlorophenol 
o  Nitrophenol  (46°) 
m  (96°) 

P  "  (H3°) 

m  Dinitrophenol  (110.5°) 
Pyrocatechol  (105°) 
Resorcinol  (110°) 
Nitrotoluene  (51.3°) 
Dmitrotoluene  (71°),  1.3.4;    1.3. 

and  1.2.6 

Trinitrotoluene  (82°) 
Isopentane  (less  than  —  24°) 


Data  for  First  Eutectic. 


M.  Pt. 

-  9.2 

-12.5 

—  30.6 

—  10 

-  8 


Wt.  Per  Cent. 
QH5NH2. 

94-  2  ' 

77.2 

53-4 
92.2 
92.7 


no  eutectic 
not  determined 3 
—  19.5        66.1 
-12.6        79.7 
-16.3        72.7 


-71 
-17 
-30 
-IS- 

'89 


21.7 
78. 84 
74- 3s 
85- S6 

62" 


7 

-13.5  80.2 

-18.7  74. 28 

-17.5        86. 8» 

-  7-3        94- S10 
-13  86. 5  u 

not  determined 
-17  89 

5  |  -13.,         80.8 

-  8  96. 412 


Authority. 

(Kremann,  1904.) 

(Kremann  and  Borjanovics,  1916.) 

(Kremann,  1904.) 

(Kremann  and  Rodinis,  1906.) 
(Kremann.  1904.) 
(Kremann  and  Rodinis,  1906.) 
(Kremann,  1904.) 
(Kremann,  1907.) 
(Kremann  and  Rodinis,  1906.) 

(Baskov,  1913.) 

(Tsakalatos  and  Guye,  1910.) 

(Kremann,  1906.) 

(Kremann,  1906;  Philip,  1903.) 
(Wroczynski  and  Guye,  1910.) 
(Kremann  and  Rodinis,  1906.) 
(Kurnakov  and  Kriat,  1913.) 
(Kurnakov  and  Solover,  1916.) 
(Bramley,  1916.) 
(Kremann  and  Rodinis,  1906.) 


(Kremann.  1906.) 

((Kremann  and  Rodinis.  1906.) 
(Kremann,  1904.) 

(Kremann.  1906.) 


(Campetti  and  del  Grosso,  1913.) 


1  A  second  eutectic  melts  at  76°  and  contains  7  per  cent  C6H6NH2,  a  molecular  compound  of  m.  pt.  92° 
and  containing  24  per  cent  C6H5NH2  exists  between  these  eutectics.  The  author  also  gives  data  for  the 
effect  of  nitrobenzene,  o  nitrophenol  and  of  m  xylene  upon  the  lowering  of  the  m.  pt.  of  the  above  com- 
pound. 2  A  break  in  the  curve  at  41.5°  and  39.2  per  cent  QHsNHj  indicates  that  a  molecular  compound 
exists  between  the  first  eutectic  and  this  point.  •  The  first  eutectic  apparently  lies  too  near  pure  aniline 
to  be  determined.  An  equi-molecular  compound  of  aniline  and  s  trinitrobenzene  (m.  pt.  30°)  exists  over 
the  range  pure  aniline  to  the"  second  eutectic  which  melts  at  101°  and  contains  8.7  per  cent  QHsNHj. 
4  A  second  eutectic  melts  at  o  and  contains  28.7  per  cent  C6H5NH2,  the  molecular  compound  between 
these  points  melts  at  8.3°  and  contains  46.2  per  cent  C8HSNH2.  5  A  second  eutectic  melts  at  —31°  and 
contains  17  per  cent  C6H8NH2,  the  molecular  compound  between  these  points  melts  at  —14.6°  and  con- 
tains 49  per  cent  C6H6NH2.  •  The  second  eutectic  melts  at  6°  and  contains  23  per  cent  QH6NH2,  the 
molecular  compound  melts  at  19.2°  and  contains  47.5  per  cent  C6H5NH2.  7  There  are  two  eutectics 
between  which  an  equi-molecular  combination  exists.  8  There  is  a  break  in  the  curve  at  26°  and  421. 
per  cent  C6HBNH2  indicating  the  existence  of  a  molecular  compound  from  the  eutectic  up  to  this  point. 
9  There  is  a  break  in  the  curve  at  42°  and  39.8  per  cent  CtHsNH*  indicating  formation  of  a  molecular 
compound.  »  There  is  a  break  in  the  curve  at  74°  and  32.9  per  cent  C6H5NH2  indicating  the  existence  of 
a  molecular  compound  from  the  eutectic  up  to  this  point.  "  There  is  a  break  in  the  curve  at  39°  and 
48.9  per  cent  CeHBNH2.  «  A  second  eutectic  melts  at  60°  and  contains  7  per  cent  CsHjNHz,  the  molec- 
ular compounds  melts  at  85°  and  contains  30  per  cent  QHsNHg. 


ANILINE  78 

RECIPROCAL  SOLUBILITY  OF  ANILINE  AND  HEXANE. 

(Keyes  and  Hildebrand,  1917.) 

t°  of  Complete          Gms.  Hexane  per  100  t°  of  Complete         Gms.  Hexane  per  100 

Miscibility.  Gms.  Mixture.  Miscibility.  Gms.  Mixture. 

26.1  9-6  59-2  35-9 
43.9  14.8  59.4  41-6 
45.9  16.3  59.6  48 
49-9  20  57.9  62.9 
Si-4  21  53.9  73.1 
56  27.2  47.2  80.6 

58.2  31  35-6  88.1 
58.2                    34-6                         16.5  93.8 

RECIPROCAL  SOLUBILITY  OF  ANILINE  AND  PHENOL,  DETERMINED  BY  THE 
FREEZING-POINT  METHOD. 

(Schreinemakers,  1899.) 

Mols.  C6H5NH2  Mols.  C6H5NH2 

t°  of  Melting.       per  100  Mols.     Solid  Phase.           t°  of  Melting.  per  100  Mols.    Solid  Phase. 

Mixture.  Mixture. 

—  6.1  loo         C6H5NH2  3o.4m.pt.        50  1.1 

-  8.9  96  "  28.6  40 

—  n.7Eutec.        92.3  c6H6NH2+i.i        22.3  30 

—  6.5  90  i.i  14.8  EuteC.  21.2      i.i+C«H6OH 
+  10. 1                            80                   "                      18.4  20  QH5OH 

22  70  "  31.4  10 

28.5  60  "  37.3  4 

i.i  =  C6H5NH2.C6H6OH. 

Data  for*  the  solubility  of  aniline  in  cyclohexane  at  pressures  up  to  300  at- 
mospheres are  given  by  Kohnstamm  and  Timmermans  (1913). 

ANILINE  HYDROCHLORIDE   C6H6NH2.HC1. 

IOOCC.  H2O  dissolve  17.8  gms.  of  the  salt  at  15°.        (NiementowskiandRoszkowski,  1897.) 
IOO  gms.  H2O  dissolve  IO7.I  gms.  of  the  salt  at  25°.  (Peddle  and  Turner,  1913.) 

ioo  gms.  sat.  solution  in  water  contain  52.1  gms.  C6H6NH2.HC1  at  25°. 
loo  gms.  sat.  solution  in  aniline  contain  8.89  gms.  CeHsNHg.HCl  at  25°. 

(Sidgwick,  Pickford  and  Wilsden,  1911.) 

DISTRIBUTION  OF  ANILINE  HYDROCHLORIDE  BETWEEN  WATER  AND  ANILINE  AT  25°. 

(Sidgwick,  Pickford  and  Wilsden,  1911.) 

O.II 
O.2 

0-3 

0.4 
0.5 

C»q.  =  gms.  salt  per  ioo  gms.  aq.  layer.     C»n.  =  gms.  salt  per  ioo  gms.  ani- 
line layer. 

NitrANILINES      C6H4NH2NO2.     o,  m,  and  p. 
SOLUBILITY  IN  WATER. 

(Carnelly  and  Thomson  —  J.  Chem.  Soc.  S3.  768,  '88;  Vaubel  —  J.  pr.  Chem.  [2]  52,  73.  '95',  above  ao°, 
Lowenherz  —  Z.  physik.  Chem.  25,  407,  '98.) 

"  Grams  Nitraniline  per  Liter  of  Solution. 

Ortho  Nitraniline.    Meta  Nitraniline.    Para  Nitraniline. 
20  ...  1.14-1.67  0.77-0.80 

24-2  1.25  (25°)          1.205 

27.3  ...  1.422 

IOO  CC.  H2O  dissolve  2.2  gms.  p  nitraniline  at  IOO°.  (Jaeger  and  Kregten,  1912.) 


C»n. 

c^ 

'CM. 

c.q. 

C»n. 

c* 

./c... 

C»q. 

< 

-M. 

Caq./Can. 

0.006 

19 

•30 

0.6 

0 

.219 

2 

•74 

I 

o 

.804 

1.24 

O.O2O 

10 

0.7 

0 

•327 

2 

.14 

I.I 

I 

.005 

I 

0.043 

6 

.98 

0.8 

o 

.471 

I 

.70 

1.2 

I 

.228 

0.98 

0.086" 

4 

•65 

0.9 

o 

.631 

I 

•43 

i-3 

I 

.412 

0.92 

0.146 

3 

.42 

79  NitrANILINES 

SOLUBILITY  OF  ORTHO  AND  OF  META  NITRANILINE  IN  HYDROCHLORIC 

ACID. 

(Lowenherz.) 

Ortho  Nitraniline  at  25°.  Meta  Nitraniline. 


G.  Mols.  per  Liter. 

Grams 

_ger_ 

Liter. 

G.  Mols.  per  Liter. 

Grams 

per  Liter. 

'HCl 

o.o 

0.63 
1.26 

C6H6NH2. 
N02(o) 
O.OO9I 
0.0143 
0.0174 
0.021^ 

HCl 

o.o 

22.97 
34-63 

45-94 

N02(<7)2' 

1-25 
1.97 

2.40 
2.97 

(25°) 
(26-5°) 
(23-3°) 

O 
O 
O 

HCl 

•  O 
.OI25 
.0247 

NO2(w) 
0-0091 
0.0183 
0.0274 

HCl 

o.o 

0.46 
0.90 

1.  2O 

2-S3 
3-85 

SOLUBILITY  DATA  DETERMINED  BY  THE  FREEZING-POINT  METHOD  ARE  GIVEN 
FOR  THE  FOLLOWING  MIXTURES. 

o  Nitraniline  +  m  Nitraniline          \ 

««  ,  «<  f     (Kremann,  1910;   Valeton,  1910;   Holleman,  Hartogs 

•   *  I  and  van  der  Linden,  1911,  Nichols,  1918.) 

m  +  p  ' 

o  "          4-  o  Nitracentanilide       (Jaeger,  1906.) 

p  +  p  Nitrosoaniline  (Jaeger  and  van  Kregten,  1912.) 

0  +  Benzene  (Bogojawlensky,  Winogradow  and  Bogalubow,  1906.) 

m'          "  + 

p  ."_[_"  «  «  U 

o  "          +  Nitrobenzene  "  "  «• 

m          »          + 

p  "  _1_  "  «  «  €i 

o  "  +  Ethylenebromide 

m  "  + 

p  '«  _i_  »  "  «  «« 

m  +  m  Dinitrobenzene       (Crompton  and  Whitely,  1895.) 

m  -\-  s  Trinitrobenzene          (Smith  and  Walts,  1910;  Sudborough  and  Beard,  1910.) 

p  «  +  5 

m  +  Naphthalene  (Pushin  and  Grebenschikov,  1913.) 

O  "  +  Phenol  (Kremann  and  Rodinis,  1906.) 

m  "  +        " 

P  »  +        » 

s  Tribromaniline  +  2  Chlor,  4.6  Dibromaniline      (Sudborough  and  Lakhamalani,  1917.) 

p  Nitroethylaniline  +  p  Nitrosoethylaniline  (Jaeger  and  van  Kregten,  1912.) 

p      "      propylaniline  +  p  Nitrosopropylaniline 

Nitrodiethylaniline  +  Nitrosodiethlyaniline  (Jaeger,  1905, 1907.) 

Methylaniline  +  Benzylchloride  (Wroczynski  and  Guye,  1910.) 

Dimethylaniline  +  Benzene  (Schmidlin  and  Lang,  1912.) 

+  Tetramethyldiaminobenzophenone 
"  +  Phenol  (Bramley,  1916;  Kremann,  1906.) 

+  o  Chlorophenol  (Bramley,  1916.) 

Tetranitromethylaniline  +  a  Trinitrotoluene  (Giua.  1915.) 

+  P  Nitrotoluene 
Nitrosodimethylaniline    +  0  Naphthylamine  (Kremann,  1904.) 

4-  Phenol 

+  o  Toluidine 

+  p         « 
"  +  m  Xylidine 


NitrANILINE  80 

SOLUBILITY  OF  META  AND  or  PARA  NITRANILINE  IN  ORGANIC 
SOLVENTS  AT  20°. 

(Carnelly  and  Thomson.) 

Gms.  per  Liter.  Solvent  Cms,  per  Liter. 

Meta.        Para.  Meta.        Para. 

Methyl  Alcohol  no. 6  95.9  Benzene  24.5  19.8 

Ethyl  Alcohol  70 . 5  58.4  Toluene  17.1  13.1 

Propyl  Alcohol  56.5  43.5  Cumene  "-5  9-o 

Iso  Butyl  Alcohol  26 . 4  19.1  Chloroform  30 .  i  23 .  i 

Iso  Amyl  Alcohol  85 .  i  62 .9  Carbon  Tetra  Chloride  2.1  1.7 

Ethyl  Ether  78.9  61.0  Carbon  Disulfide  3.3  2.6 

ANILINE  SULFATE  C6H6NH2.H2SO4, 

loo  cc.  H2O  dissolve  6.6  gms.  C6H5NH2.H2SO4  at  15°. 

(Niementowski  and  Roszkowski,  1897.) 

ANISIC  ACID   (£-Methoxybenzoic  Acid)  CH3O.C6H4COOH. 

1000  cc.  sat.  aqueous  solution  contain  0.2263  gm.  acid  at  25°.  (Paul,  1894.) 

SOLUBILITY  OF  ANISIC  ACID  IN  SEVERAL  ALCOHOLS. 

(Timofeiew,  1894.) 
In  Methyl  Alcohol.  In  Ethyl  Alcohol.  In  Propyl  Alcohol. 

Gms.  per  100  Gms.  Gms.  per  100  Gms.  Gms.  per  100  Gms. 

Sat.  Sol.     "      Solvent.  Sat.  Sol.     "     Solvent.  Sat.  Sol.         Solvent! 

o     51.1    104.5      46.7    87.6      35    53.8 
16.5    64.9    183.5      53.6    115.5      43    75.5 

Data  for  the  distribution  of  anisic  acid  between  water  and  olive  oil  at  25° 
are  given  by  Boeseken  and  Waterman  (1911,  1912). 

pANISIDINE  C6H4(OCH3).NH2. 

DISTRIBUTION  BETWEEN  BENZENE  AND  WATER  AT  25°. 

(Farmer  and  Warth,  1904.) 
Gms.  C6H4(OCH3).NH3  per  100  cc. 

QHfi  Layer.  H2O  Layer. 

0.4356  0.0747 

0.6662  O.III2 

O.9OIO  O.I472 

ANISOLE  C6H6OCH3. 

RECIPROCAL  SOLUBILITY  OF  ANISOLE  AND  BENZYL  CHLORIDE  DETERMINED 
BY  THE  FREEZING-POINT  METHOD. 

(Wroczynski  and  Guye,  1910.) 
« nf        Gms.  C6H5OCH3    ~  llV1  « nf  Gms.  C 


—37.2  ioo  QHsOCH,  —  72.8Eutec.  46.1 

—  40  93.3  "  —60  28  C6H5CH2C1 

-50  75-3  -50  13 

—  60  62.1          "  —41.1  o 


p  NitrANISOLE 

FREEZING-POINT  CURVES  (Solubilities,  see  footnote,  page  i)  ARE  GIVEN  FOR 
THE  FOLLOWING  MIXTURES. 

p  Nitranisole  +  Mercuric  Chloride  (Mascarelli,  1908,  1909;  Mascarelli  and  Ascoli,  1907.) 

"  _j_  Urethan  (Mascarelli,  1908, 1909;  Pushin  and  Grebeuschukov,  1913.) 

"  +       "  +  HgCl2  (Mascarelli,  1908,  1909.) 

-f  Diphenylamine         (Pushin  and  Grebenschukov,  1913.) 

Dinitranisole  -f-  Dinitrophenetol      (Blanksma,  1914-) 


8i 


ANTHRACENE 


ANTHRACENE  Ci4H10 

SOLUBILITY  OF  ANTHRACENE  IN  SEVERAL  SOLVENTS. 


Solvent.                                 t°        «^f|j£.                     Authority. 

Ethyl  Alcohol  (abs.)             16            0.076    (v.  Becchi.) 

"               "               "                        19-5            I-9           (de  Bruyn,  1892.) 
".             "              "                      25                0.328     (Hildebrand,  Ellefson  and  Beebe,  1917.) 
"              "              "                    b.  pt.           0.83        (v.  Becchi.) 
Methyl  Alcohol  (abs.)               19.5            1.8           (de  Bruyn  1892) 
Benzene                                            25                1.86        (Hildebrand,  Ellefson  and  Beebe,  1917.) 

Carbon  Bisulphide               25            2.58 
Carbon  Tetrachloride           25            0.732 
Ether                                    25            1.42 
Hexane                                  25            0.37 
95%  Formic  Acid                 18.3        0.03      (Aschan,  1313.) 
Toluene                                 16.5        0.92      (v.  Becchi.) 
"                                    loo          12.94 

Trichlorethylene                           15                 I.OI         (Wester  and  Bruins,  1914.) 

SOLUBILITY  OF  ANTHRACENE  IN  BENZENE  AND  IN  MIXTURES  OF  BENZENE 
AND  PENTANE  AND  OF  BENZENE  AND  HEPTANE. 

(Tyrer,  1910,  and  private  communication.     See  Note,  p.  447.) 

Tn  „                       In  Benzene  -f-  Pen-           In  Benzene  +  Heptane 
In  Benzene.                 tane  at  I5<>                         at  ^o  and  ^ 

t°. 

d.  of  Sat.  Sol. 

Gms.  C^HIQ 
per  100  Gms. 

insol- 

Gms. C14H,0 
per  loo  Gms. 

Solvent. 

Gms.  QHio  per  100  Gms. 
Solyent              \ 

Solvent. 

vent. 

Solvent. 

at  14°. 

at  70°. 

0 

0.9008 

0.605 

O 

0.184 

0 

0.2IO 

1.67 

10 

o  .  8909 

o-975 

10 

0.225 

12-5 

0.284 

2.10 

,20 

0.8812 

i-43 

20 

0.279 

25 

0.372 

2.64 

30 

0.8717 

2.03 

30 

o-357 

37-5 

0.474 

3.23 

40 

0.8627 

2.78 

40 

0.447 

50 

0.592 

3-87 

50 

0.8541 

3-75 

50 

0-549 

62.5 

0.718 

4-59 

60 

o  .  8460 

5-i4 

60 

0.600 

75 

0.850 

5-37 

70 

0.8374 

7 

70 

0.780 

87.5 

0.976 

6.15 

75 

0-8347 

8-35 

80 

0.915 

IOO 

I.lSo 

6-93 

90 

1.059 

IOO 

i.  221; 

Results  for  the  solubility  in  benzene,  differing  from  the  above  in  some  cases  by 
15%.  are  given  by  Findlay  (1902). 

SOLUBILITY  OF  ANTHRACENE  IN  ALCOHOLIC  PICRIC  ACID  SOLUTIONS 

AT  25°. 

(Behrend  —  Z.  physik.  Chem.  15,  187,  '94.) 


Solid  Phase 

Anthracene  Picrate 
« 

a 

N 

Anthracene  Picrate 

-f  Picric  Acid 
Picric  Acid 


Grams  per  100  Grams 
Solution. 

Grams  per  100  Gms. 
Solution. 

^Acicf     Anthracene 

Add.    Anthracene. 

O 

o 

.176 

Anthracene 

3 

•999 

o 

.202 

I 

.017 

o 

.190 

it 

5 

.087 

0 

.180 

2 

.071 

0 

.206 

14 

5 

•843 

0 

.162 

2 

•673 

0 

.215 

(I 

6 

.727 

0 

•151 

3 

•233 

o 

.228 

ftf 

7 

•511 

o 

.149 

3 

.469 

0 

.236 

Anthracene  and 

7 

•452 

0 

Anthracene  Picrate 


ANTHRACENE 


82 


SOLUBILITY  IN  LIQUID  SULFUR  DIOXIDE  IN  THE  CRITICAL  REGION. 

(Centnerswer  and  Teletow,  1903.) 

Weighed  amounts  of  anthracene  and  liquid  SO2  were  placed  in  glass  tubes 
which  were  sealed  and  rotated  at  a  gradually  increasing  temperature,  and  the 
point  observed  at  which  the  solid  disappeared. 


Gms  CnHi. 
100  Gms.  ! 


40.1 
45.8 

47-9 


2. II 
2.48 
2.65 


65 
78.2 

88 


Gms.  CMHio  per 
loo1  Gms.  SO,. 


9-9 
12.7 


too  Gms. 

4  98 

5-66  99.1 

7.14  106.5 

Freezing-point  curves  are  given  for  mixtures  of  anthracene  and  each  of  the  fol- 
lowing compounds:  Diphenyl,  diphenylamine,  a  and  /3  naphthylamines,  a  and  /3 
naphthols,  resorcinol,  p  toluidine  and  triphenyl  methane  (Vignon,  1891);  Naph- 
thalene (Vignon  and  Miolati,  1892);  Phenanthene  (Vignon,  1891,  Garelli,  1894); 
Picric  acid  (Kremann,  1905). 

ANTHRAQUINONE   (C6H4)2(CO)2. 

SOLUBILITY  IN  LIQUID  SULFUR  DIOXIDE  IN  THE  CRITICAL  REGION. 

(Centnerswer  and  Teletow,  1908.)     (See  Anthracene,  above.) 

Gms.  CuHgOi!  per 
100  Gms.  SO2. 

5.60 

7-53 
9.60 
12.70 
18.30 

100  parts  of  absolute  ethyl  alcohol  dissolve  0.05  part  anthraquinone  at  18° 
and  2.249  parts  at  b.  pt.  (v.  Becchi.) 

loo  gms.  alcohol  dissolve  0.437  gni.  anthraquinone  at  25°. 

(Hildebrand,  Ellefson  and  Beebe,  1917.) 

SOLUBILITY  OF  ANTHRAQUINONE  IN  BENZENE  AND  IN  CHLOROFORM. 

(Tyrer,  1910.) 

In  Benzene.  In  Chloroform. 


jo        Gms.  CMH8O2  per           f  e        Gms.  CUH8O2  per               f  0 
100  Gms.  SO2.                            100  Gms.  SO2. 

3.96 

0.64 

92.1 

2.81 

118.5 

51-5 

0.88 

101.4 

3-67 

141.6 

67.9 

1.73 

106.3 

4.23 

160 

82.4 

2.24 

108.7 

4.40 

179 

183-7 

t°. 

Sp.  Gr.  Solution. 

Gms.  Ci4H8O2  per 
100  Gms.  C6He. 

t°.         Sp.  Gr.  Solution. 

Gms.  C14H8O2  per 
loo  Gms.  CHC13. 

o 

0.8900 

O.IIO 

0 

-5244 

0.340 

20 

0.8794 

0.256 

10 

.5046 

0-457 

30 

0.8692 

0-350 

20 

.4850 

0.605 

40 

0.8591 

0.495 

30 

.4656 

0.780 

50 

0.8439 

0.700 

40 

.4461 

0.994 

00 

0.8389 

0.974 

50 

.4261 

1.256 

70 

0.8288 

1-355 

55 

.4164 

1-415 

80 

O.8I90 

1-775 

00 

.4070 

1-577 

SOLUBILITY  OF  ANTHRAQUINONE  IN  A  MIXTURE  OF  CHLOROFORM  AND 
HEXANE  AT  12.6°  AND  49°. 

(Tyrer,  1910,  also  private  communication.    See  Note,  p.  447.) 


O 
IO 
20 
30 
SO 


Gms.  CuH^  per  too  Gms. 
Solvent  at: 

%CHCl,in 
Solvent. 

60 

90 
100 

Gms.  CuHjOj  per  100  Gms. 
Solvent  at: 

12.6°. 

O.OO6 

0.016 
0.024 
0.034 
0.068 

49.0°. 
0.056 
0.074 
0.096 
0.124 

0.212 

12.6°. 

O.IOI 
0.148 
O.222 

0-334 
0.482 

49  .0°. 
0.292 
0.417 
0.6o8 
0.852 
I.2O9 

83  ANTHRAQUINONE 

SOLUBILITY  OF  ANTHRAQUINONE  IN  ETHER. 

(Smits  — Z.  Electrochem.  pi  663,  '03.) 

Weighed  amounts  of  ether  and  anthraquinone  were  placed  in  glass 
tubes  which  were  then  sealed.  The  temperature  noted  at  which  the 
anthraquinone  disappeared  and  also  at  which  the  liquid  phase  disap- 
peared (critical  temp.).  The  two  curves  cross  at  195°  and  again  at 
241°.  Between  these  two  temperatures  the  critical  curve  lies  below 
the  solubility  curve,  hence  for  this  range  of  temperature  no  solubility 
curve  is  shown.  The  following  figures  were  read  from  the  curves,  and 
are  therefore  only  approximately  correct. 


Cms.  CuHgOa  Cms.  C 

t*.  per  too  g.  t°.  per  100  g.  t    .          per  100  g. 

Solution.  Solution.  Solution. 

130  3  241  30  260  80 

150  4  245  40  270  90 

170  4-5  247  So  275  100 

195  5.0  250  60 

100  parts  of  toluene  dissolve  0.19  part  anthraquinone  at  15°  and  5.56  parts  at 
100°  (v.  Becchi). 
loo  gms.  ether  dissolve  o  104  gm.  anthraquinone  at  25°. 

(Hildebrand,  Ellefson  and  Beebe,  19170 

Data  for  the  solubility  of  anthraquinone  in  mixtures  of  phenol  and  water 
are  given  by  Timmermanns  (1907). 

Hydroxy  ANTHRAQUINONES  C6H4  <  (CO)*  >  C6H3OH. 

1000  cc.  H2O  dissolve  0.0035  gm.  a  oxyanthraquinone  at  25°.  (Huttig,  1914.) 

1000  cc.  H2O  dissolve  o.oon  gm.  £  oxyanthraquinone  at  25°. 
1000  cc.  H2O  dissolve  0.000012-0.000062  gm.  1.4  dioxyanthraquinone  (=  chin- 
izarin)  at  25°. 

1000  cc.  H2O  dissolve  0.00158  gm.  1.6  dioxyanthraquinone  ( =  chrysazin)  at  25°. 

(Huttig,  1914.) 

ANTHRAFLAVINE  (2.6  Dioxyanthraquinone)  Ci2H6(CO)2(OH)2. 

1000  cc.  H2O  dissolve  0.0003  Sm-  anthraflavine  at  25°.  (Huttig,  1914.) 

ANTHRARUFINE    (1.5  Dioxyanthraquinone)  Ci2H6(CO)2(OH)2. 

looo  cc.  H2O  dissolve  0.000285  gm.  anthrarufine  at  25°.  (Huttig,  1914.) 

ANTIMONY  Sb. 

Fusion-point  data  for  mixtures  of  antimony  and  iodine  are  given  by  Jaeger 
and  Dornbosch  (1912);  for  mixtures  of  antimony  and  sulphur  by  Jaeger  and 
Van  Klooster  (1912),  and  for  mixtures  of  antimony,  iodine  and  arsenic  by 
Quercigh  (1912). 

ANTIMONY  TriBROMIDE      SbBr,. 

SOLUBILITY  IN  BENZENE  DETERMINED  BY  "SYNTHETIC  METHOD." 

(Menschutkin,  1910.) 

Gms.  SbBr3  Gms.  SbBr3 

t°.            per  loo  Gms.  Solid  Phase.                        t°.  per  100  Gms.     Solid  Phase. 

Sat.  Sol.  Sat.  Sol. 

5 . 6  m.  pt.          O                  QH,                    90  83               2SbBr,.CA 

4 . 5  Eutec.       8 . 3  c8H6+2sbBr3.c(lH(1       92.5111.  pt.       90 . 2 

15  12.5       aSbBrs-QH,  91.5  Q2.8  " 

35  23  "  90  93.8 

55  39  85  EuteC.  96.3    2SbBr,.C6H6+SbBr, 

75  60.5  "  QO  98  SbBr, 

85  74.3  "94  ioo 


ANTIMONY  TriBROMIDE 


84 


RECIPROCAL    SOLUBILITIES    OF    ANTIMONY    TRIBROMIDE    AND    VARIOUS 
ORGANIC  COMPOUNDS,  DETERMINED  BY  THE  "SYNTHETIC  METHOD." 

(Menschutkin,  1911.) 


SbBr3  +  Acetic      SbBr3  4-  Benzoic 

SbBr3  4-  Benzoyl 

SbBr3 

+  Benzene 

Acid. 

Acid. 

Chloride. 

Sulphonic  Acid. 

r. 

Gms.  SbBr3 
per  loo  Gms. 
Sat.  Sol. 

r. 

Gms.  SbBr8 
per  loo  Gms. 
Sat.  Sol. 

t'. 

Gms.  SbBr3 
per  100  Gms. 
Sat.  Sol. 

t°. 

|  Gms.  SbBr3 
per  100  Gm. 
1    Sat.  Sol. 

16.5* 

0 

120* 

o 

-  0-5 

*        0 

52.5 

*          0 

is 

12.2 

"5 

20.  1 

—  3 

19-5 

So 

15.8 

10 

41.8 

no 

36.8 

—  6  f 

32 

47-5 

26.2 

4t 

S8.2 

105 

50 

+10 

41.2 

44  t 

36.9 

20 

64.3 

IOO 

61.5 

20 

47-5 

So 

39-1 

40 

72-5 

95 

71 

30 

54 

60 

45-7 

60 

81.9 

85 

83.1 

40 

60.8 

70 

55-2 

70 

97.1 

79  t 

87.6 

5° 

67.8 

80 

68.1 

80 

92.4 

85 

92 

60 

74-9 

85 

77.6 

90 

97-8 

90 

96.4 

80 

89.4 

90 

90-3 

94 

IOO 

94 

IOO 

94 

IOO 

94 

IOO 

Molecular  compounds  are  not  formed  in  the  above  systems.    The  diagram  in 
each  case  consists  of  two  arms  meeting  at  the  eutectic. 


SbBr3 

+  Acetophenone. 

Gms.  SbBr3     ^VA 

SbBr3  +  Amylbenzene. 

Gms.  SbBr3         ^^A 

SbBr3  +  Anisole. 

Gms.  SbBrs       c^i:j 

t°.     i 

»er  100  Gr 

ns'  Phase. 

t°.   pei 

"-  r?°s  I™3'       Phase. 

t°.        pei 

:  loo  Gr 

081    Phase. 

19-5* 

O 

C6H6COCH3 

—  70 

4.5  SbBrjj.CgHfj.CjjHu 

-34* 

o 

C6H5OCH3 

15 

22.7 

" 

-50 

8-3 

-35 

2.5 

"-fi.i 

i.S* 

48.6 

"  +1.1 

-30 

16.6 

—  20 

11.7 

i.i 

20 

56.8 

i.i 

-25 

21                     " 

0 

26.5 

" 

30 

63.3 

" 

-17  t 

32.5            "+SbBr3 

10 

37-i 

" 

37-5* 

75 

" 

—  10 

33  .  5            SbBr3 

20 

50-5 

" 

31  t 

83-2 

i.i+SbBr3 

o 

35-6 

25 

59 

" 

40 

84.6 

SbBr3 

20 

41.6 

30-5* 

77 

" 

60 

88.4 

" 

40 

S1^              " 

30  t 

77-9 

"+SbBr, 

[80 

94.1 

• 

60 

65 

40 

80.6 

SbBr3 

194 

IOO 

H 

80 

84 

60 

86.4 

" 

80 

93-6 

" 

SbBr3  -f  Benzaldehyde.        SbBr3  -f-  Benzonitrile. 


SbBr3  +  Benzophenone. 

Gms.  SbBr3       q  ,. , 


•20 

38. 

4 

i.i 

-13.2' 

*       0 

.0  C«HBCN 

48 

* 

0 

C6HfiCO.C6H6 

0 

45- 

5 

" 

-16 

19 

.2         " 

40 

24 

" 

20 

54- 

3 

" 

—  18  t 

28 

.7      "+i.i 

29 

t 

41. 

2 

"+i.i 

35 

64. 

i 

" 

0 

43 

i.i 

40 

50 

i.i 

40 

70. 

3 

" 

20 

59 

" 

45 

56, 

3 

" 

41. 

5*       77- 

" 

30 

67 

" 

48 

•  5 

*66, 

A 

K 

37. 

8f       84. 

4    i 

,i+SbBr3 

38* 

77 

.8 

45 

76 

" 

55 

88 

SbBr8 

35  t 

'82 

.5      i.i+SbBr, 

40 

80 

i.i+SbBr3 

75 

93. 

i 

" 

55 

87 

.  5          SbBr3 

.  So 

82, 

6 

SbBr3 

85 

96. 

i 

" 

75 

93 

•3 

70 

88. 

7 

" 

90 

98. 

2 

« 

85 

96 

•5 

80 

92, 

A 

" 

94 

IOO 

• 

90 

98 

•3 

90 

97. 

3 

.    " 

94 

IOO 

94 

IOO 

" 

*  m 

.pt. 

t  Eutec. 

t 

tr.  pt. 

I.I 

=  compound 

of  equimolecular 

amounts  of  the  two  constituents  in  each  case. 

ANTIMONY  TriBROMIDE 


RECIPROCAL  SOLUBILITIES  OF  ANTIMONY  TRIBROMIDE  AND  VARIOUS  ORGANIC 
COMPOUNDS,  DETERMINED  BY  THE  "SYNTHETIC  METHOD." 

(Menschutkin,  1910.) 

SbBr3  + 
Brombenzene. 

Gms.  SbBr3 
t°.        per  100  Gms. 
Sat.  Sol. 


-31* 

o 

-32 

5-7 

-25  1 

9-5 

-15 

15 

—  5 

20.8 

+  5 

26.8 

i5 

33 

25 

39-6 

45 

54-6 

65 

71.9 

85 

90.7 

94 

roo 

SbBr; 

5   + 

SbBr3  + 

SbBr3  + 

Chlorbenzene. 

lodobenzene. 

Fluorbenzene. 

Gms.  SbBr3 

Gms.  SbBr3 

Gms.  SbBr! 

t°. 

per  100  Gms. 
Sat.  Sol. 

t°. 

per  100  Gms. 
Sat.  Sol. 

t°. 

per  100  Gms. 
Sat.  Sol. 

-45-2* 

0 

-28.6* 

0 

-39- 

2*        0 

-47  t 
-40 

5-2 
6.8 

-30.3 

-32  t 

7.0 
14-3 

-39- 
-25 

5t        1-3 
4-3 

-30 

Q.6 

—  20 

21.6 

-15 

6-7 

-20 

12.6 

—  10 

27.5 

+  5 

12.6 

-10 

16 

o 

33-4 

25 

21.8 

0 

20 

+10 

39-3 

45 

35-3 

20 

30 

20 

45-2 

55 

45-5 

40 

45-4 

40 

57-6 

65 

60.8 

60 

65.8 

60 

71.1 

75 

81.8 

80 

86.3 

80 

86.3 

85 

93-5 

94 

100 

94 

IOO 

94 

IOO 

SbBr3  + 

SbBr,  + 

SbBr3  + 

SbBr3  + 

p  Dibrombenzene. 

p  Dichlorbenzene. 

Nitrobenzene. 

m  Dinitrobenzene. 

Gms.  SbBr3 
t°.         per  i  oo  'Gms. 
Sat.  Sol. 

Gms.  SbBr3 
t°.           per  100  Gms. 
Sat/  Sol. 

Gms.  SbBr3 
t°.             per  loo  Gms. 
Sat.  Sol. 

Gms.  SbBr3 
t°.         per  loo  Gms. 
Sat.  Sol. 

88*           o 

54-5*           o 

6*            o 

90*           o 

85            10 

51-5               14 

I                    22 

80           29  .  I 

80            25.2 

48.  5  t         26.5 

-  4              37-4 

70        50 

75             39-2 

55                35-9 

-  9              48.4 

60        63 

70             52 

60                43-1 

-14-  5t       55-3 

50            70  .  8 

65  f          62.2 

65                50.7 

-  5              58.3 

47-5  t      72 

70             68.7 

70                58.8 

+  5              61.5 

50            73-4 

75             75-3 

75                67.2 

25              68.6 

60            78.2 

80             8r.8 

80                75.8 

45              76.6 

70            84 

85             88.3 

85                84.5 

65              85.3 

80            90.4 

90             94-3 

90                93-4 

85              94-7 

90           96  .  8 

94           100 

94              100 

94            loo 

94          loo 

Molecular  compounds  are  not  formed  in  the  above  systems.    The  diagram 
in  each  case  consists  of  two  arms  meeting  at  the  eutectic. 


SbBr3  +  Ethylbenzene.      SbBr3  +  Propylbenzene. 


SbBr3  +  p  Cymene. 


Gms.  SbBr3     <,,.  . 
t°.        per  loo  Gms.  pS,olld 
Sat.  Sol.      Phase- 

Gms.  SbBr3     A  ..  . 

*••  Tssr«    *••  F 

Gms.  SbBr3      g^ 

-93* 

0 

C8H6.C2H5 

-80 

i. 

3           I-1 

-75* 

0 

-93-2  t 

0.4 

"+i.i 

-60 

3- 

7 

-77  t 

2 

—  70 

I 

i.i 

—40 

9- 

4 

-So 

6. 

I 

i.i 

-50 

2.2 

" 

—  20 

22. 

5 

-30 

12. 

3 

" 

-30 

4.8 

" 

—  10 

38. 

4 

—  10 

27 

" 

—  10 

12 

'« 

-  si 

49 

i.i+SbBr, 

0 

42. 

3 

" 

+10 

29.2 

" 

+10 

53- 

3         SbBr3 

+5  t 

51- 

5 

x.x+SbBit 

20 

46.3 

M 

20 

57- 

I 

20 

56 

SbBr, 

29  1 

69.7 

i.i+SbBrs 

40 

66. 

2                " 

40 

64. 

i 

M 

50 

78.2 

SbBr3 

60 

77 

2 

60 

75 

" 

70 

87.3 

" 

so 

89. 

8                it 

80 

88. 

5 

M 

90 

97-7 

" 

94 

IOO 

" 

94 

IOO 

M 

*  m.  pt. 


t  Eutec. 


tr.  pt. 


i.i  =  compound  of  equimolecular  amounts  of  the  two  constituents  in  each  case. 


ANTIMONY  TriBROMIDE 


86 


RECIPROCAL  SOLUBILITIES  OF  ANTIMONY  TRIBROMIDE  AND  VARIOUS  ORGANIC 
COMPOUNDS,  DETERMINED  BY  THE  "SYNTHETIC  METHOD." 

(Menschutkin,  1911.) 

SbBr3  +  Cyclohexane.     SbBr3  +  Pseudo  Cymene.         SbBr3  +  Mesitylene. 


Gms.  SbBr3     s  ,-,                          Gms.  SbBr3       «,,..                          Gms.  SbBr3        <,  ... 
t°.  per  loo  Gms.  p>._..                 t°.      per  100  Gms.     ^u                     t°.     per  100  Gms.      i2~ 
Sat.  Sol.                                          Sat.  Sol.                                            Sat.  Sol.         Phase' 

6.4*     o             CsHu         —57-^*      o      C6H3(CH3)  !,  2,  4  —  54.4*    o       QH^CHj),  i,  3,  5 
6f         0.3  CeHu+SbBr,   -58.8  f       9-7      "  +i-i              ~55-2f     2.1      "     +1.1 
•20            1.4         SbBr3         —50            II                  i.i              —30            3.6              i.i 
40            3.7                         —30           16.2                             —io           9 
60           7.1                         —io           31                                +10         25.4               " 
80         12.5                              o           47.6             "                  20         35.  $ 

liquid  layers  formed 

7§        63.5         1.1+2.1 

29  t      46.5         i.i  +2.1 

92.5     17.4        97.6 

IS           67.4            2.1 

40         54  .  2              2.1 

no         25.8        96.5 

25           73 

50         61.7 

130        36.4        95 

33  §        79.1      2.i+SbBrs 

60            70  .  2                   " 

150        47.8        92.7 

50           82.8          SbBr3 

69.5*85.8 

170        62.3        86.3 

70           88.4 

69!      87.7        2.i+SbBr3 

175  1               74.0 

90           97.4 

80         92.7            SbBr3 

SbBr3  +  Diphenylmethane 

.    SbBr3  +  Naphthalene. 

SbBr3  +a  Nitronaphthalene. 

Gms.  SbBr3      g0ji(j 

Gms.  SbBr3      ~  ,.. 
t°.      per  loo  Gms.    £?™ 

Gms.  SbBr3     Sojjd 

Sat.  Sol.            ase' 

Sat.  Sol.        •Fhase' 

Sat.  Sol.        Phase. 

26  *           o          CH2(C6H5)2 

79.4*        0           '  C10H8 

57*           o.o    aC10H7N02 

22.  5  f     12.8         "+2.1 

75            23.7 

50               23.2 

40               22.8                2.1 

70            37-4 

40              42.6 

50               29.5 

65            48.6 

33-5  1      50.5           "+« 

60           37-5 

57               6l.2              "  +2.: 

t      37.5        62.6          i.ilf 

70           47-8 

60            68              2.1 

38.2*     67.6 

80           60.2 

65            81.3 

38  f          68          i.i+SbBr, 

90  *        81  .  i 

66*         84.9 

50              73.4          SbBr3 

85           89.6 

65  f           86.7      2.i+SbBr3 

70              83.8 

82f         92.2       2.i+SbBr3 

75              90.1          SbBr3 

90              96.4 

90            96  .  2           SbBr3 

85             94-9 

94          IOO                  " 

90             97.7 

SbBr3  +  Diphenyl. 

SbBr3  +  Phenol. 

SbBr3  +  Phenetol. 

Gms.  SbBr3      s  ,.  , 
t°.        per  loo  Gms.    ^,?lld 
Sat.  Sol.        Phase- 

Gms.  SbBr3       c  rj 

*••  •isssr  $£• 

Gms.  SbBr3        goli(j 

,'70.5*         o           C6H6C6H5 

41  *             0             C6H5OH 

-28.6*        o           C6H6OC2H5 

60               35.7 

35            22.5 

—  29  1           1.6        "  +1.1 

50               54-3 

30         40 

—  io              4.8            i.i 

47  1          57-4            "+2.1 

28.5!      44-6           "+2.1 

+10            12.9 

55             68.5           2.1 

40             53                2.1 

20            19.2             " 

60.5*      82.7 

50             62.5 

30            29.7 

70              86  .  S          SbBr2 

60             75.8 

4O                 46  .  2 

80              91.5 

65             84.7 

48.8*        74-7 

90             97-3 

66.5*      88.5 

47  1          77-8       i.i+SbBr8 

94           loo 

75             91  •  7          SbBr3 

60             83               SbBr3 

85             95-8 

70             87.3 

90             98.1 

90             97.4 

*  m.  pt. 

t  Eutec.                      t  crit.  t. 

§  tr.  pt. 

H  Not  obtained  regularly, 

in  such  cases,  single  eutectic  at 

23°  and  61.5  per  cent  SbBr3. 

i.i  =  compound  of  equimolecular  amounts  of  the  two  constituents  in  each  case. 
2.1  =  compound  of  2  molecules  of  SbBr3  with  one  molecule  of  the  other  con- 
stituent. 


ANTIMONY  TriBROMIDE 


RECIPROCAL  SOLUBILITIES  OF  ANTIMONY  TRIBROMIDE  IN  VARIOUS  ORGANIC 
COMPOUNDS,  DETERMINED  BY  THE  "SYNTHETIC  METHOD." 

(Menschutkin,  1910-12.) 


naphthalene. 

Gms.  SbBr3 

per  loo  Gms. 

Sat.  Sol. 

O 

,3.8 

22.6 
27.3 
35-5 
46.7 
61.6 
69.9 
78.6 

87.5 
96.6 
IOO 


SbBr3  +  a  Brom- 

SbBr; 

naphthalene. 

nap 

Gms.  SbBr3 

t°.       per  100  Gms. 

t°. 

Sat.  Sol. 

3* 

-17s 

o              15-8 

—  21 

-  3-St      3i-4 

—  24. 

15             38.7 

—  IO 

35             49-9 

+10 

45             56.9 

30 

55             64.7 
65             72.9 

g 

75             81.8 

70 

80             86.3 

80 

85             90.8 

90 

90            95.4 

94 

SbBr3+/3Chlor- 
naphthalene. 

SbBr3  +  Tetra- 
hydrobenzene. 

Gms.  SbBr3 

Gms.  SbBr3 

t°. 

per  100  Gms. 
Sat.  Sol. 

t°. 

per  100  Gms. 
Sat.  Sol. 

56* 

O 

... 

50 

26.1 

-5 

ii.  7 

45 

38.5 

IS 

40 

49 

35 

24.1 

37-  St 

53-6 

55 

41 

45 

58.8 

65 

55-1 

55 

66.8 

70 

64-5 

65 

75-2 

75 

76.2 

75 

83-8 

80 

84-4 

80 

88.1 

85 

90.7 

85 

92.4 

90 

95-8 

90 

96.7 

94 

IOO 

SbBr3  + 

SbBr3  + 

SbBr3  + 

SbBr3  + 

o  Chlortoluene. 

m  Chlortoluene. 

p  Chlortoluene. 

m  Nitroluene. 

Gms.  SbBr3 

Gms.  SbBr3 

Gms.  SbBr3 

Gms.  SbBr3 

t°. 

per  loo  Gms. 
Sat.  Sol. 

t°. 

per  100  Gms. 
Sat.  Sol. 

t° 

per  loo  Gms. 
Sat.  Sol. 

tv, 

i 

per  100  Gms. 
Sat.  Sol. 

-36, 

2*          0 

-47-8* 

0 

6 

.2*                0 

16* 

0 

-38. 

St      i°-7 

-50  t 

8.1 

2 

•St         23.3 

10 

24.2 

—  20 

15-4 

-30 

IX  .7 

2O 

33 

5 

39 

0 

22.S 

—  io 

17.5 

30 

39-3 

o 

46.6 

+  20 

32.5 

+  10 

25.8 

40 

47-2 

-  9t 

56.8 

30 

38.8 

30 

37-5 

50 

56.3 

+10 

62.7 

40 

46.8 

40 

45-1 

60 

66.7 

30 

69.7 

50 
60 

56 
66.5 

£ 

54-4 
65 

70 
80 

77-8 
88.2 

f 
60 

77-5 
8i-S 

g 

77-8 
88.2 

70 
80 

77 
88.2 

90 

94 

97 

IOO 

70 
80 

86.3 
91.4 

90 

97 

90 

97 

90 

97-2 

Molecular  compounds  are  not  formed  in  the  above  systems.     The  diagram  in 
each  case  consists  of  two  arms  meeting  at  the  eutectic. 


SbBr3  +  Toluene.         SbBr3  +  o  Nitrotoluene. 

Gms  SbBr3        Solid 


SbBr3  +  p  Nitrotoluene. 

Gms.  SbBrj        «,  ... 


Sat.  Sol. 

5at.  Sol 

rnase.j 

Sat.  So 

-93* 

0 

C6H5.CH3 

-   8.5* 

O 

o  N02.C6H4.CH3 

52-5* 

0 

-93-5t 

I.O 

"+i.i 

-13-5 

19-5 

"  +1.1 

45 

29.8 

-80 

2.4 

i.i 

O 

27.6 

i.i 

40 

42.2 

-60 

6.2 

" 

IO 

35-6 

" 

35 

50 

—40 

12.4 

" 

20 

47-5 

" 

25 

61 

—  20 

25-7 

" 

25 

55-7 

H 

i6f 

67 

-  It 

53.1 

1.  1+2.  1 

31  t 

70 

"  +SbBr3 

30 

71.6 

+  20 
30  t 

69.4 

78 

2.1 

2.i+SbBr3 

40 

5° 

73-5 

77-5 

SbBr3 

g 

78.9 
82.9 

40 

80.6 

SbBr3 

60 

81.7 

• 

70 

87.2 

60 

86.6 

•« 

80 

91.4 

" 

80 

92 

80 

93-8 

" 

90 

97-2 

" 

90 

97-5 

94 

IOO 

" 

P  N02.C6H4.CH3 


+SbBr, 
SbBr3 


*  m.  pt. 


t  Eutec. 


tr.  pt. 


i.i  =  compound  of  equimolecular  amounts  of  the  two  constituents  in  each  case. 
2.1  =  compound  of  2  molecules  of  SbBr3  with  i  molecule  of  the  other  con- 
stituent. 


ANTIMONY  TriBROMIDE  88 

RECIPROCAL  SOLUBILITIES  OF  ANTIMONY  TRIBROMIDE  AND  VARIOUS  ORGANIC 
COMPOUNDS,  DETERMINED  BY  THE  "SYNTHETIC  METHOD." 

(Menschutkin,  1910-11.) 

phe^y?mtt£iie.      SbBr3  +  o  Xylene.      SbBr3  +  m  Xylene.     SbBr3  +  p  Xylene. 


Gms.  SbBrs 
t°.      per  100  Gms. 
Sat.  Sol. 

Gms.  SbBr3 
t°.          per  100  Gms. 
.     '      Sat.  Sol. 

Gms.  SbBr3 
t°.           per  loo  Gms. 
Sat.  Sol. 

Gms.  SbBr3 
t°.         per  100  Gms. 
Sat.  Sol. 

92* 

0 

-29* 

O 

-57* 

o 

14* 

o 

85 

18 

-33  t 

10-5 

-59-  2  t 

5-5 

12 

16.6 

80 

30.1 

—  20 

17 

-45 

10 

lot 

28 

70 

47 

—  10 

24.6 

-35 

14.2 

2O 

36 

00 

48  1 

58.2 
67.1 

0 
2O 

34-5 
65.8 

-25 
-  5 

20 
38.8 

30 
40 

44-6 
53-8 

60 
70 

73-3 
79-5 

24* 

22.  St 

77.2 
78.6 

+  5 
12.5  $ 

56.6 

75-4 

t 

63-5 
74 

80 

86.4 

30 

80 

25 

77-6 

67-5* 

87.3 

90 

95-2 

50 

84.7 

45 

82.3 

66.  st 

88.3 

94 

100 

70 

90.1 

65 

87.9 

75 

91.4 

90 

97-7 

87 

95-3 

85 

95-7 

*  m.  pt.  f  Eutec.  J  tr.  pt. 

In  the  case  of  each  of  the  above  xylenes  the  compound  existing  between  the 
first  and  second  eutectic  consists  of  equimolecular  amounts  of  SbBr3  and  xylene. 

Solubility  data  determined  by  the  freezing-point  method  (see  footnote,  page  i) 
are  given  for  mixtures  of  antimony  tribromide  and  each  of  the  following  compounds : 
azobenzene,  benzil,  s  diphenylethane  and  stilbene  (Van  Stone,  1914),  aniline,  ben- 
zophenone,  triphenylmethane  and  toluene.  (Kurakov,  Krotkov  and  Oksman,  1915.) 

ANTIMONY  TriCHLORIDE  SbCl3. 

SOLUBILITY  IN  WATER.     SOLID  PHASE  SbCl8. 

(Meerburg  —  Z.  anorg.  Chem.  33,  299,  1003.) 

Mols.  SbCU  Gms.  SbCla  Mols.  SbCla  Gms.  SbCl3 

t°.          per  loo  per  100  t°.  per  100  per  100 

Mols.  H2O.  g.  H2O.  Mols.  H2O.  g.  H2O. 

o   47.9       601.6        35      91.6      1152.0 
15    64.9       815.8        40     108.8       1368.0 

(72.4  9IO-I  50  152.5  1917.0 

(74-1  931.5  60  360.4  4531-0 

25          78.6  988.1  72  oo  oo 

30        84.9  1068. o 

SOLUBILITY  OP  ANTIMONY  TRICHLORIDE  IN  AQUEOUS  HYDROCHLORIC 
ACID.    SOLID  PHASE  SbCl3.     TEMP.  20°. 

(Meerburg.) 


Mols.  per 
100  Mob.  H2O. 

Gms 

100  g 

:Sb. 

Mols.  per 
100  Mols.  H2O. 

Gms.  per 
100  g.  H2O. 

HC1. 
0 
2.4 

6.1 

8-3 

SbCla. 
72.4 
71.2 
69.9 

68.2 

HC1. 

o.o 

4-86 
12-34 

16.80 

SbCla. 

910.1 

895-4 
879.0 

857.6 

HC1. 
9.1 
II-7 
28.7 

SbCl3'. 
68.9 

68.1 
62.8 

HC1. 
18.41 
23.68 
58.08 

SbCla. 
866.4 

856.3 
789.8 

loo  gms.  absolute  acetone  dissolve  537.6  gms.  SbCla  at  18°.    d*p  sat.  sol.  =  2.216. 

(Naumann,  1904.) 

loo  gms.  ethyl  acetate  dissolve  5.9  gms.  SbCl3  at  18°  d  sat.  sol.  =  1.7968. 

(Naumann,  1910.) 


89  ANTIMONY  TriCHLORIDE 

RECIPROCAL  SOLUBILITIES  OF  ANTIMONY  TRICHLORIDE  AND  VARIOUS  ORGANIC 
COMPOUNDS,  DETERMINED  BY  THE  "SYNTHETIC  METHOD." 

(Menschutkin,  1911.) 

SbCl3  +  Acetic  Acid.         SbCl3  +  Acetophenone.  SbCl3  +  Anisol. 

Gms.  SbCl3     o-,,  Gms.  SbCl3       S,;H  Gms.  SbCl, 


16.5*      o 
10          22.7 
o          42.5 
-  5          48.5 
-  9t       52.7 
o          59 

CH3COOH      19  .  5 
IS 

ft 

"  +1.1        IS 
i.i          35 

* 

o          C6H6COCH3    -34* 

14-3                           -36.5 
28.5                           -30 
31.8              '•   +1.1  —io 
35-4.           LI          +10 

41.6                                        20 

t 

0 

n.  8 
16 
28.3 

43 
52.8 

C«H6OCH3 
"  +1.1 
i.i 

IO 

67.3 

55 

55 

.2 

" 

251 

63.6 

"  +2.1 

19* 

"79.1 

60.5 

* 

65 

4 

" 

35 

70 

2.1 

25 

81.5 

SbCl,        45 

79 

3 

" 

41-5 

* 

80.9 

" 

45 

87.4 

32  t 

84 

i.i+SbCl, 

40  t 

84-5 

"+SbCl3 

65 

95-3 

So 

89 

3 

SbCl3 

60 

.92 

SbCl3 

73 

IOO 

70 

98 

,2 

70 

98 

SbCl3  +  Aniline. 

SbCl3  +  Benzaldehyde. 

SbCl3 

+-  Benzophenone. 

Gms.  SbCl3          g  ,5.                          Gms.  SbCl3     Solid 

Gms.  SbCl3      o  ,.  , 

t°.       per  too  Gms.         T>I     '                 t°.       per  ioo  Gms.  pv,00             t°.      per  ioo  Gms.     pu^ 
c«4-   c.r.1              jrnase.                              GO+-   c^i        iiio.sc.                         Qot   Q/^I          x  ua,»c. 

t        x 

C6H5NH2+i.4 

IO 

43 

.  5          x.i 

48 

* 

o 

C8H5COC,H5 

+  20  '2 

7 

1.4 

20 

47 

•  5 

40 

16.3 

" 

60 

18. 

7 

" 

30 

52 

•  4 

35 

t 

21.6 

"  +1.1 

77  t 

29. 

6 

I-4+I-3 

40 

60 

.2 

45 

26.2 

i.i 

88* 

44- 

8 

1-3 

43 

•  5* 

68 

.  I                " 

55 

31-4 

" 

87  t 

46. 

3 

1.3+1-2 

40 

74 

.2                " 

65 

37-5 

" 

94-5*      54- 

9 

1.2 

30 

80 

.6 

76 

* 

55-4 

" 

89-5 

61. 

7 

1.  2+1.  1 

25 

t 

83 

i.i+SbCl3 

65 

71.6 

" 

100.5 

*      71 

I.I 

35 

85 

SbCl3 

45 

80.6 

it 

70 

82. 

2 

" 

45 

87 

•5 

39 

t 

82.7 

"+SbCl3 

3i  t 

88 

i.i+SbCl3 

65 

95 

.2 

50 

87 

SbCl3 

60 

94- 

9 

SbCl3 

73 

IOO 

" 

70 

97-7 

" 

i.i  =  compound  of  equimolecular  amounts  of  the  two  constituents  in  each  case. 

2.1  =  compound  of  2  molecules  of  SbCl3  with  i  molecule  of  the  other  constit- 
uent. 

1.2,  1.3  and  1.4  =  compounds  of  i  molecule  of  SbCl3  with  2,  3  and  4  molecules 
of  aniline. 


SbCl3  +  Benzoic 
Acid. 

SbCl3  +  Benzoyl 
Chloride. 

SbCl3  +-  Benzene 
Sulphonic  Acid. 

SbCl3  +  Tetra- 
hydrobenzene. 

Gms.  SbCl3 

'Gms.  SbCl3 

Gms.  SbCl3 

Gms.  SbCl3 

t°. 

per  ioo  Gms. 
Sat.  Sol. 

t° 

per  ioo  Gms. 
Sat.  Sol. 

t°. 

per  ioo  Gms. 
Sat.  Sol. 

t°. 

per  ioo  Gms. 
Sat.  Sol. 

1  20 

O 

-  5 

I7.8 

52-5* 

O 

-25 

19.1 

no 

23 

-IS 

36.8 

45 

18 

-15 

24 

IOO 

38.8 

-23  t 

45 

25 

43-7 

-  5 

30 

90 

50 

—  5 

5°-  7 

5 

56.i 

+  5 

37-  * 

80 

59 

+15 

58.2 

-5t 

60.8 

IS 

45-1 

70 

66 

25 

62.9 

+5 

49-8 

25 

54-3 

60 

71.6 

35 

68.4 

25 

56.7- 

35 

64.5 

46  1 

78 

45 

74-9 

45 

69.2 

45 

74 

60 

89.2 

55 

82.4 

65 

90.2 

55 

83.6 

70 

97-5 

70 

96.5 

73 

65 

92.8 

Molecular  compounds  are  not  formed  in  the  above  systems.     The  diagram  in 
each  case  consists  of  two  arms  meeting  at  the  eutectic. 


*  m.  pt. 


t  Eutec. 


I  tr.  pt. 


ANTIMONY  TriCHLORIDE 


90 


RECIPROCAL  SOLUBILITIES  OF  ANTIMONY  TRICHLORIDE  AND  VARIOUS  ORGANIC 
COMPOUNDS,  DETERMINED  BY  THE  "SYNTHETIC  METHOD." 

(Menschutkin,  igio-'n.) 

SbCl3  +  Benzene.  SbCl3  +  Brombenzene.        SbCl3  +  Chlorbenzene. 

Gms.  SbCl,     <^,.,1  Gms.  SbCl,     <,,..  Gms.  SbCl,     -... 


4* 

7-3 

QH,      . 

-3i  t 

0 

C«H6Br 

-45 

.2f          0 

QH5C1 

i 

19.4 

"   +2.1 

-32-5* 

4.8 

"  +1.1 

-47 

4-3 

"  +1.1 

10 

24.6 

2.1 

-30 

6.8 

i.i 

-40 

7 

i.i 

20 

30.5 

" 

—  20 

14.8 

" 

-30 

ii.  i 

40 

44.1 

" 

—  io 

23-9 

" 

-IS 

20.5 

60 

60.6 

H 

o 

34-3 

H 

-  5 

32.5 

79  t 

£5 

« 
« 

+  3t 

20 

40-3 
52 

i.i+SbCl, 
SbCl, 

o 

20 

t         44-2 
56 

70 

93-5 

" 

40 

68 

" 

40 

72.1 

62* 

96 

2.1+SbCl, 

60 

85.8 

II 

60 

88.2 

67.5 

97-9 

SbCl, 

73 

IQO 

II 

73 

100 

SbCl3  +  Fluorbenzene. 

SbCl3 

+  lodobenzene. 

SbCl3  +  Nitrobenzene. 

Gms.  SbCl,     g^                           Gms.  SbCl,      Solid                           Gms.  SbCl,     Solid 

-39.2 

t     o 

QHjF 

-28.  6f 

Sat.  Sol. 

0 

C«H5I 

6f        o 

CANO, 

-40-5 

*      2.4 

"+  i.i 

-35  ^ 

12.8 

" 

—    2 

20.4 

1 

-25 

II 

i.i 

-45* 

29.8 

"+i.i 

—  10 

*    32 

M 

-IS 

17.3 

" 

-34-5 

11.7 

i.i,  unstable 

-16 

•5*   38 

"   +I.I 

—  10 

21.4 

" 

-IS 

26.4 

(i         « 

—  io 

5      44 

I.I 

-  5 

26.4 

" 

-  3 

.  49  •  i 

"         " 

-  7 

5       So 

ii 

0 

34.1 

" 

-35 

32.5 

i.i+SbCl, 

-  6 

t       64.8 

1C 

+  5-5 

t  45.8 

i.i+SbCl, 

-IS 

38.9 

SbCl, 

-  6 

5*    67.5 

i.i+SbCls 

15 

53.6 

SbCl, 

+  5 

46.4 

" 

+  5 

69.6 

SbCl, 

25 

61.6 

" 

25 

56 

<i 

35 

78.7 

" 

45 

77.7 

« 

45 

69.6 

« 

55 

87.4 

" 

93.8 

« 

65 

88.8 

<< 

70 

96.6 

" 

SbCl3 

+  Ethylbenzene. 

SbCl3 

+  Benzonitrile. 

SbCl 

3  +  Isoamylbenzene. 

Gms.  SbCl,     C^I.M                              Gms.  SbCl,     ^.j 

Gms.  SbCl, 

t°. 

per  100  Grr 

MMBU 

t  . 

Der  zoo  G 

ms.    p]ko 

t  . 

per  100  Gms 

Ph 

Sat.  Sol. 

Sat.  So 

L 

Sat.  Sol. 

-93  t 

0 

QHs-QHs 

—  13.2  f 

0 

QHsCN 

-80 

4 

I.I 

-93-5 

*      0.3 

"  +1.1 

-16 

IO.2 

" 

-60 

11.7 

" 

-70 

0.6 

i.i 

-19* 

17.2 

"  +1.1 

—40 

25-4 

« 

-50 

i.i 

—  10 

21.9 

i.i 

-33 

t     32.7 

1.  1+2.  1 

-30 

2.5 

0 

28.5 

-25 

38.7 

2.1 

—  10 

7 

10 

38.7 

-15 

47-2 

" 

+  10 

18.8 

15 

47.4 

-  5 

t      56.8 

2.i+SbCl, 

30 

44-4 

20 

62.6 

o 

57-4 

SbCl, 

39  t 

68.1 

21.  5t 

68.7 

20 

63.3 

" 

35* 

77-4 

I.I+2.I 

20 

72.4 

40 

72.6 

«< 

37  t 

81.1 

2.1 

IS* 

78.9 

60 

.87.1 

«< 

36.8 

*  81.8 

2.1+SbCl, 

25 

81.6 

70 

97.3 

ii 

So 

87.2 

SbCl, 

45 

87.6 

70 

98 

" 

65 

95-6 

-25 

44.4  unstable  i.i 

73 

—  21 

t      54-9 

"i.i+SbCl, 

33 

8o.*4 

i.i+SbCl, 
(unstable) 

—  IO 

56 

"SbCl, 

Eutec. 


t  m.  pt. 


t  tr.  pt. 


i.i  =  compound  of  equimolecular  amounts  of  the  two  constituents  in  each  case. 
2.1  =  compound  of  2  molecules  of  SbCl3  with  i  molecule  of  the  other  con- 
stituent. 


ANTIMONY  TriCHLORIDE 


RECIPROCAL  SOLUBILITIES  OF  ANTIMONY  TRICHLORIDE  AND  VARIOUS  ORGANIC 
COMPOUNDS,  DETERMINED  BY  THE  "SYNTHETIC  METHOD." 

(Menschutkin,  1910-11.) 

SbCl3  +  m  Dinitrobenzene.  SbCl3  +  Propylbenzene. 

Gms.  SbCl3         <.,..,,  Gms.  SbCl3    «^HH  Gms.  SbCl, 


90* 

O              m  CeH4(NO 

2)3      20 

72.  8  unstable    i.i     —70              O.6              2.1 

80 

18.6 

IS 

76.2       "           "     —30           10.  1 

70 

31-3 

10 

78.6       "           "     —  10           26.6               " 

60 

40.7 

5 

80.8       "          "           o           40.4              " 

5° 

48 

o 

82.7       "          «           7           57.5 

40 

53-6 

—  IO 

64.9       '•       SbCl3        8.  si   68.2              "+SbCl, 

30 

58 

+  IO 

69           "          "         20           71.4          SbCls 

20 

61.6  unstable      " 

20 

71.6       "          "        40           78.5 

IO 

64.5        " 

30 

74.8                  "         65           92.5 

it 

66  .  8       "          "  +SbCl3  40 

78.7                  "       

—  ii 

68.8      " 

50 

83.5                    "     —  70              1.  5  i.i          unstable 

+27-S 

52-5       "       1.1 

60 

89                       "     —30           16 

28.5* 

58.2 

70 

96.4                    "     -   5           48.2    " 

27-5 

63 

73 

ioo                     "     +  1.5*    65.3    " 

25 

67.5 

it        66.3    "+SbCl3  " 

10           68.6          SbCU  " 

^3b< 

ben 

p  Dichlor-                SbCl3  +  Cyclohexane. 
zcric* 

t°. 

Gms.  SbCl3 
per  ioo  Gms. 
Sat.  Sol. 

t°. 

Gms.  SbCls                                Gms  Sbcj3  pg,.  I00  Gmg 
Sat^Sol                        '                        Sat>  S°l 

88* 

0 

54-5*. 

0                           6.4*                      0.0 

85 

5-7 

So 

14                      6f                      0.2 

80 

15-4 

45 

30                             20                                  1.2 

70 

35 

40 

48                      40                          4-2 

60 

52.8 

39-5  t 

50.5                        60                                  9.7 

55 

59 

45 

59  .  5                    Two  liquid  layers  formed 

49-  5  t 

64 

So 

67.8                 70              13.7            97 

65 

71.8 

55 

75-7                 80              19.5            96.1 

60 

79-3 

60 

83                   ioo             32.3            92.7 

70 

95 

70 

96.2                120             57.1            83.2 

124             58.9            76.7 

125.  5  §                68 

SbCl 

3  +  P  Cymene, 

SbCl3  +  Pseudocymene.          SbCl3  +  Diphenyl. 

Gms.  SbCl3       ^r.A 

Gms.  SbCl3       Solid                           Gms.  SbCl3     Solid 

.*.'•       P* 

*  too  Gms.    phase 

t°. 

Per  ioo  Gms.     phase                *°.       ^c^Sol118'  Phase- 

-75* 

0       P  C6H4CH3C3H7 

—57.4 

*      o       C6H3(CH3)3l,2,4     70.5*      0        QH5.QH, 

-76.  st 

2                       "  -{-I.I 

-6ot 

18.6               "     +1.1      65            14 

-So 

7              i-i 

-45 

23.6             i.i               55          33-4 

-30 

IS 

-25 

33-3                              sot       40             "+2.1 

—  IO 

30 

—  IO 

45                                  55          45-2        2.1 

-.3.  si 

41                   I.I+2.I 

-  si 

50.7              "  +2.1       60          51.4 

10 

46.1                   2.1 

+15 

55.8                     2.!                        70                 70.7 

30 

60 

35 

62.2              "                71*        74-6 

40  i 

76.4      2.I-fSbCl» 

So 

69.7              "                65          85.5 

So 

81.2 

56* 

79.2              "                57  1       88.9  2.1+SbCl, 

60 

87 

Sit 

87.5        2.i+SbCl3          65           93.1       SbCl, 

70 

95-6 

65 

93.9           SbCl,             70          97 

*  m.  pt. 


t  Eutec. 


tr.  pt. 


§  crit.  t. 


i.i  =  compound  of  equimolecular  amounts  of  the  two  constituents  in  each  case. 
2.1  =  compound  of  2  molecules  of  SbCl3  with  I  molecule  of  the  other  constituent. 


ANTIMONY  TriCHLORIDE 


92 


RECIPROCAL  SOLUBILITIES  OF  ANTIMONY  TRICHLORIDE  AND  VARIOUS  ORGANIC 
COMPOUNDS,  DETERMINED  BY  THE  "SYNTHETIC  METHOD." 

(Menschutkin,  1910-11.) 


SbCl3  +  Mesitylene. 

Cms.  SbCl3 


Cms.  SbCl3      oni;j 


SbCl3  +  Triphenyl 

Methane. 
Cms.  SbClj      o  1; , 


—  54-4        o         CgHs(CH^3i, 

3,5     26* 

o 

CHZ(C6H5)2 

92* 

o 

CH(C6H6)3 

-55-6 

i. 

5 

"   +1 

i        22.5' 

t     7-9 

"  +2.! 

85 

ii.  8 

" 

-40 

3 

I.I 

40 

15.1 

2.1 

80 

19-3 

" 

—  20 

7 

« 

60 

26 

« 

70 

32 

" 

0 

14.2 

(i 

70 

33 

60 

42.4 

" 

10 

20. 

3 

« 

80 

41.6 

So 

49-6 

«« 

3° 

39- 

3 

" 

9° 

52-7 

49  t 

5° 

"  +1.1 

f* 

65 

£: 

4 
4 

2.1 

1        9S* 

100* 

59-8 
72.9 

45 
40 

62.8 
68.3 

i.i 

75-5*   79- 

2 

" 

95 

82.2 

35$ 

72 

i.i+SbCl3 

70 

87 

" 

90 

86.7 

45 

76.6 

SbCl3 

58.5 

92. 

4 

"  +SbCl3    80 

91-5 

55 

82.4 

«« 

63 

94 

SbCl3 

67  I 

95-7 

*. 

i+SbC!3 

65 

90.6 

« 

70 

98 

" 

70 

97 

SbCl? 

70 

96.1 

" 

SbCU 

+  Naphthalene.             ^naphthalene?1'" 

SbCl8  +  18  Chlor- 
naphthalene. 

Cms.  SbCl3      c  vj                           Gms.  SbCl3      Solid                         Gms.  SbCl3      g  i-  j 
t°.       per  i  oo  Gms.    pv,oca             t°.         pe^ioo  Gms.    pv..^,,             t°.       per  100  Gms.    pv,oco 

I79-4* 

Sat. 
o 

sol. 

C10H8 

i 

-17* 

0 

a  CioH7Cl 

56 

£ 

at.  Sol 

0 

0  C10H7C1 

75    . 

IS 

.2 

M 

—  21  t 

8.1 

"  +2.1 

5° 

16.6 

" 

.65 

35 

" 

O 

14.4 

2.1 

45 

27.2 

" 

59  t 

42 

.8 

"  +2.1 

IO 

18.7 

" 

40 

35-4 

" 

65 

48 

•4 

2.1 

20 

24.6 

ii 

30  A 

47-3 

* 

75 

58 

.8 

" 

30 

33-5 

" 

25  t 

52-3 

"  +1.1 

80 

65 

" 

40 

47-7 

" 

29-5* 

58.2 

i.i 

86* 

78 

" 

45 

61.5 

" 

28  1 

64 

i.i+SbCl, 

80 

88 

•7 

«' 

46* 

73-6 

" 

35 

68.3 

SbCl3 

70 

93 

* 

45-5  J 

75 

2.1+SbCla 

45 

75-3 

» 

65  J 

94 

2.1+SbCl, 

55 

82.2 

SbCl3 

60 

87.5 

" 

70 

97 

.2 

SbCl3 

70 

90-5 

73 

I 

00 

" 

SbCl3  +  a 

Bromnaphthalene. 

SbCl3  + 

a  Nitronaphthalene. 

t°. 

Gms.  SbCl3  per  100 
Gms.  Sat.  Sol. 

Solid 
Phase. 

t° 

Gms.  SbCl3  per  100 
Gms.  Sat.  Sol. 

Solid 
Phase. 

3* 

o 

a  CwH7Br 

57 

* 

0 

a  C10H7N02 

-  it 

8-3 

"  +1.1 

50 

13 

.6 

• 

" 

10 

12.8 

i.i 

40 

27 

•3 

" 

25 

•  24 

" 

30 

t 

35 

.8 

"  +1.1 

33 

38.5 

" 

35 

43 

.2 

i.i 

34-5 

* 

52.4 

" 

37 

•5 

49 

•3 

" 

33 

62.1 

«< 

39 

* 

56 

•7 

" 

31.5 

t 

64.7 

i.i+SbCl3 

37 

•5 

64 

" 

40 

69.7 

SbClj 

34 

i.St 

72 

.8 

i.i+SbCla 

£ 

76.2 
84.5 

«. 

45 
60 

78 
87 

•4 

SbCl3 

70 

94-8 

" 

70 

96 

.6 

" 

"  m  pt.  t  tr.  pt.  t  Eutec. 

i.i  =  compound  of  equimolecular  amounts  of  the  two  constituents  in  each 


case. 


2.1  =  compound  of  2  molecules  of  SbCl8  with  I  molecule  of  the  other  con- 
stituent. 


93' 


ANTIMONY  TriCHLORIDE 


RECIPROCAL  SOLUBILITIES  OF  ANTIMONY  TRICHLORIDE  AND  VARIOUS  ORGANIC 
COMPOUNDS,  DETERMINED  BY  THE  "SYNTHETIC  METHOD." 

(Menschutkin,  1910-12.) 


SbCl3  +  Phenol. 

Gms.  SbCl,     o-ijj 

SbCl3  +  Phenetol. 
Gms.  SbCl3    o,.. 

SbCl3  +  Toluene. 

Gms.  SbCl3     o^i:-i 

t°.        per  zoo  Gms.  £?**                t°.         per  !oo  Gms.  fT"™              t°.         per  100  Gms.  pT"t 
Sat.  Sol.      ££se'  ,                           Sat.  Sol.                                             Sat.  Sol. 

41* 

0 

C6HBOH 

-28 

.6* 

O 

1"*  TT  r\(~*  T3 

[5     -93 

* 

0 

C,H6.CH3 

35 

16.2 

" 

-29 

t 

I 

•  4                  "+!• 

i      -94 

t 

i 

.1 

"  +i.l 

30 

25.6 

" 

—  20 

4 

.5      I.I 

—  70 

3 

.  i 

i.i 

20 

38.7 

" 

—  10 

8 

.1 

-30 

IS 

.8 

" 

10 

48 

Cl 

+  10 

18 

.2 

O 

•5 

" 

St 

52 

"  +3.1 

2O 

27 

4 

II 

I 

57 

.8 

"  +2.1 

IS 

58.6 

2.1 

30 

39 

.4 

20 

62 

.8 

2.1 

30 

70.6 

" 

40 

58 

" 

40 

78 

" 

37* 

83    - 

" 

42 

.2* 

65 

" 

42 

•5* 

83 

.  i 

" 

36.  5  t 

83.7 

2.I+SbCl3 

35 

t 

77 

.8 

40  t 

85 

.8 

2.i+SbCl3 

55 

90.6 

SbCls 

So 

86 

8 

50 

89 

SbCl3 

70 

98.2 

H 

70 

97 

i 

70 

97 

.8 

" 

SbCl3  +  o  Chlortoluene.      SbCl8  +\m  Chlortoluene. 


I 

to 

ims.  SDI 

nS       Solid 

Li 

rmS.  3D 

pe 

r  100  Gi 

ns-   Phase. 

t°.'      pe 

r  100  G 

-36.2* 

O 

o  C1C6H4CH3 

-47-8* 

0 

-37-  St 

6.9 

"  +1.1 

-49  t 

6.9 

—  20 

I8.3 

i.i 

—40 

12.3 

—  10 

29.2 

" 

-30. 

20.1 

-  5 

37-i 

" 

—  20 

31 

-  o.st 

47-9 

i.i+SbCl3 

—  14  1 

40 

+  10 

SbCl3 

o 

46.! 

20 

5^2 

M 

10 

51.6 

3° 

64.6 

M 

20 

57-4 

40 

71.8 

II 

40 

72.8 

60 

88.4 

" 

60 

89.1 

+1.1 


SbCl3 


-  7-St 


73 


73 


IOO 


o 

10 

30 
40 
50 
60 
70 


o 

12.7 

23-5 
32.2 

43-8 
47-2 
52.2 
64.8 

72-3 
80.2 
88.8 
97-4 


SbCl3  +  p  Chlortoluene. 

Gms.  SbCl3     c  ... 


6.2 

3 

o 

3 

7 


'+SbCl3 


SbCl3  +  o  Nitrotoluene.       SbClg  +  m  Nitrotoluene.      SbCl3  +  p  Nitrotoluene. 


Gms.  SbCl3  '  Sol. 

,                 .     [Gms.  SbCl3          g. 

Gms.  SbCl3      q  ... 

t°.    per  loo  Gms.  ^ 

J.             t°.      per  toe  Gms.        ,$£ 

se               t°. 

>er  100  Gms.    pi? 

Sat.  Sol.    ,Fha 

>e-                           Sat.  Sol. 

Sat.  Sol.       *flase' 

-8.5*     0       oNOsQ 

H4CH3        16*        0          wNOjC 

^CHs    52.5 

*      o      p  NOzQ^CH 

-13-5      II-  3 

io         15 

45 

18.5 

-iS.st  18.5 

+n          o         30.7 

35 

33-6 

—  io          21.3           i. 

i           —io        39.2 

30    ' 

38.8             " 

+  10         31.1 

—  20           42.8 

1                  20 

46 

20         39 

crystallization  not 

7-5 

t    52                "  +i.x 

30         So 

obtained  here 

7-5 

*    62.3 

34-5  *  62.3 

o        67  .  2            Sb 

Cl,            5 

66.1 

33         68 

20        72.5 

3t 

68.5     i.i+SbClj 

27-  St  74-6 

+SbCl3     30        76.3 

10 

70             SbCU 

40         79  .  i         Sbl 

:i,             40        80.8 

30 

^75-5 

50         84-5            * 

50        86 

So 

85 

70         97-5 

1                60        91.6 

70 

97-5 

73      loo 

t  Eutec. 


t  tr.  pt. 


•  m.  pt. 

i.i  =  compound  of  equimolecular  amounts  of  the  two  constituents  in  each 
case. 

2.1  =  compound  of  2  molecules  of  SbCl8  with  i  molecule  ot  the  other  con- 
stituent. 


ANTIMONY  TriCHLORIDE 


94 


RECIPROCAL  SOLUBILITIES  OF  ANTIMONY  TRICHLORIDE  AND  VARIOUS  ORGANIC 
COMPOUNDS,  DETERMINED  BY  THE  "SYNTHETIC  METHOD." 

(Menschutkin,  1910.) 


SbCl3  +  o  Xylene. 


SbCl3  +  m  Xylene. 


SbCI3  +  p  Xylene. 


Cms.  SbCls      Solid 
t°.   per  100  Gms.    -pi                    t°.     p 
Sat.  Sol.        Phase' 

Gms. 

SbCls       Solid                               GmS'  SbC13                 Snlirl 

'  Gms'  Phase               *°-  Per  I0°  Gms-           PI? 
Sol.      Phase'                      Sat.  Sol.             Phase.  _ 

•29. 

0 

0C6H4(CH3)2    -57* 

O 

7W  L-c-H-4  (0.11.3)2      14 

* 

0 

P  C6H4(CH3)2 

•35 

t     14 

"  +1.1  —60.5 

t    7 

•5 

"    +I.I     II 

•71 

1"  Ir 

•  7 

" 

+I.I 

30 

17- 

5 

™          —45 

15 

.8 

I.I                 2O 

i7 

•5 

i.i 

•20 

24. 

8 

-25 

29 

40 

37 

•3 

" 

10 

33- 

4 

—  5 

46 

.  2 

So 

52 

•3 

«« 

o 

43- 

4 

-  aj 

49 

.8 

"  +2.1    55 

t 

62 

•  7 

«• 

+2.1 

IO 

55 

5 

53 

.1 

2.1                  60 

66 

.1 

2.1 

19. 

5*68. 

i 

IS 

58 

•7 

70 

* 

81 

25 

71- 

3 

2.1                     25 

65 

•7 

6S 

88 

.1 

" 

30 

75. 

7 

33 

73 

.8 

58 

t 

92 

11 

+SbCl3 

33. 

5  *  81 

38* 

81 

69 

97 

.  2 

SbCl3 

5t82. 

5 

2.i+SbCl3         36.5 

t  83 

,  7 

2.I+SbCl3 

m 

5° 

88 

SbCl3             50 

87 

•7 

SbCl3           10 

20 

•  7 

P  C6H4(CH3)2  unstable 

60 

92. 

4 

60 

91 

5 

"               7 

t 

32 

.8 

"k+2. 

1 

71 

98. 

5 

70 

97 

,2 

35 

50 

•3 

2.1 

•« 

55 

62 

•7 

" 

* 

*  m.  pt. 


t  Eutec. 


t  tr.  pt. 


i.i  =  compound  of  equimolecular  amounts  of  the  two  constituents  in  each  case. 
2.1  =  compound  of  2  molecules  of  SbCl3  with  i  molecule  of  the  other  con- 
stituent. 

DISTRIBUTION  OF  ANTIMONY  TRI  AND  PENTACHLORIDES  BETWEEN  AQUEOUS 
HC1  AND  ETHER  AT  ROOM  TEMPERATURE 

(Mylius,  1911 ) 

When  i  gm.  of  antimony  as  SbCl3  or  as  SbCl5  is  dissolved  in  100  cc.  of  aq. 
HC1  of  the  following  strengths  and  the  solution  shaken  with  100  cc.  of  ether, 
an  amount  of  metal,  depending  upon  the  concentration  of  the  aq.  acid  solution, 
enters  the  ethereal  layer. 


With  i%  SbCl3  Solution. 

Per  cent  Cone.      Per  cent  of  Total 
of  HC1.  Sb  in  Ether  Layer. 


With  i  %SbCl6  Solution. 


20 

15 
10 

S 

i 


6 
13 

22 
8 
0-3 


Per  cent  Cone, 
of  HC1. 

Per  cent  of  Total 
Sb  in  Ether  Layer. 

20 

81 

15 
10 

22 
6 

5 

i 

2-5 

trace 

Solubility  data  determined  by  the  freezing-point  method  (see  footnote,  p.  i) 
are  given  for  mixtures  of  antimony  trichloride  and  each  of  the  following  com- 
pounds: azobenzene,  benzil,  s  diphenylethane,  and  stilbene  (Van  Stone,  1914); 
benzene,  naphthalene,  diphenylmethane  and  triphenylmethane  (Kurnakov, 
Krotkov  and  Oksman,  1915);  SbBr3,  SbI3,  and  SbBr3  +  SbI3  (Bernadis,  1912); 
SbCU  (Aten,  1909). 


ANTIMONY  PentaCHLORIDE  SbCl6. 

Data  for  the  freezing-points  of  mixtures  of  antimony  pentachloride  and  anti- 
mony pentafluoride  are  given  by  Ruff  (1909). 


95  ANTIMONY  TriFLUORIDE 

ANTIMONY  TriFLUORIDE  SbF3. 

SOLUBILITY  IN  WATER. 

(Rosenheim  and  Grunbaum,  1909.) 

Gms.  SbF3  per  100  Gms. 

O 
2O 
22.5 

25 

30 

SOLUBILITY  IN  AQUEOUS  SOLUTIONS  OF  SALTS  AND  OF  HYDROFLUORIC  ACID  AT  o°. 

Normality  Gms.  SbF3  per  100  Gms.  H2O  present  in  Aq.  Solutions  of: 


Water. 

Sat.  Solution. 

384.7 

79-4 

444-7 

8l.6 

452.8 

81.9 

492.4 

83.1 

563.6 

84.9 

Solution.          KC1.  KBr.          KNO3.        K2SO4.        K2C2O4.  (NH^CA-  K2C4H4O6.         HF. 

4  I  461.8      448.7      458.2      419.9      465.7          ...         461.4         432.5 

0.5    448-3  45°   45J-9  408.5  481.2  431.9  430.5   404 

0.25       431.9    455-6    418.3    406.6    451.3    442.3    430.8 

o  125     407.3    417-2    401.4       ...       405-2    433-3    435-2     *479-4 

*  (2  n  HF.) 

Celluloid  flasks  were  used  and  all  measuring  apparatus  provided  with  HF  re- 
sistant coating.  The  SbF3  was  prepared  in  the  form  of  rhombic  transparent 
crystals  from  Sb2O3  and  HF. 

ANTIMONY  TrilODIDE  SbI3. 

SOLUBILITY  IN  METHYLENE  IODIDE  AT  12°. 

(Retgers,  1893.) 

loo  parts  CH2l2  dissolve  11.3  parts  SbI3.     Sp.  Gr.  of  solution  =  3.453. 

SOLUBILITY  DATA  DETERMINED  BY  THE  FREEZING-POINT  METHOD  ARE  GIVEN 

FOR  MIXTURES  OF: 

Antimony  triiodide  and  arsenic  triiodide. 

(Quercigh,  1912;  Jaeger  and  Dornbosch,  1912;  Vasilev,  1912.) 
phosphorus  triiodide.  Qaeger  and  Dornbosch,  1912.) 

iodine.  (Quercigh,  1912.) 

ANTIMONY  TriOXIDE  Sb2O3. 

Freezing-point  data  are  given  for  mixtures  of  antimony  trioxide  and  antimony 
trisulfide.  (Quercigh,  1912.) 

ANTIMONY  TriPHENYL  Sb(C6H6)3. 

Freezing-point  data  are  given  for  mixtures  of  antimony  triphenyl  and  mercury 
diphenyl  and  for  antimony  triphenyl  and  tin  tetraphenyl.  (Cambi,  1912.) 

ANTIMONY  SELENIDES  SbSe,  Sb2Se. 
Freezing-point  data  for  SbSe  +  Ag2Se  and  Sb2Se  +  AgSe.  (Pglabon,  1908.) 

ANTIMONY  TriSULPHIDE   Sb2S3. 

looo  cc.  water  dissolve  0.00175  gm.  Sb2S3  at  18°.  (Weigel,  1907.) 

SOLUBILITY  DATA  DETERMINED  BY  THE  FREEZING-POINT  METHOD  ARE  GIVEN 

FOR  MIXTURES  OF: 

Antimony  trisulphide  and  cuprous  sulfide.  (Parravano  and  Cesaris,  1912.) 

stannous  sulfide.  "  " 

lead  sulfide.     (Jaeger  and  Van  Klooster,  1912;  Pe*labon,  1913.) 
"  "  "      silver  sulfide.  (Jaeger  and  Van  Klooster,  1912,) 


ANTIMONY  TARTRATE 


96 


ANTIMONY  Potassium  TARTRATE   C2H2(OH)2(COOK)(COOSbOUH2O. 

loo  gms.  water  dissolve    5.9  gms.  salt  at  room  temp.          (Squire  and  Caines,  1905.) 

6.9     "        "     "  25°.  (S  and  S.  1903.) 

"  "  "  8          "         "      "  21°.  (Aschan,  1913.) 

"        95%  HCOOH  dissolve  82.7  gms.  salt  at  20.8°.  (Aschan,  1913.) 

"        glycerol  dissolve  5.5  gms.  salt  at  15.5°. 

SOLUBILITY  OF  ANTIMONY  POTASSIUM  TARTRATE  IN  AQ.  ALCOHOL 
SOLUTIONS  AT  25°. 

(Seidell,  1910.) 


Wt.  Per  cent 
QH6OH  in 

.      t             Gms.  C4H4O«. 

Sat  Sol           KSbO.|H2Oper 
Sat.  bol.        IOQ  Qms  gat  Sol 

Wt.  Per  cent 
C2H5OH  in 
Solvent. 

<*25  Of 

Sat.  Sol.      l 

Gms.  C4H4O6. 
KSbO.*H2O  per 

0 

I.O52 

7^5 

40 

o-935 

0.38 

5 

1.025 

5-50 

50 

0.913 

0.23 

10 

1.007 

3-92 

60 

0.890 

0.12 

20 

0.980 

I.  Q2 

70 

0.866 

0.06 

30 

0.958 

0.84 

IOO 

0.788 

trace 

ANTIPYRINE  CUH12N2O. 

IOO  gms.  water  dissolve    80    gms.  CnHi2N2O  at  15°.  (Greenish  and  Smith, '03.) 


" 

IOO 

* 

alcohol 

"        IOO 

90%  alcohol 

'       75-2 

chloroform 

1       IOO 

; 

ether 

1.3 

pyridine 
50%  aq.  pyridine 

1     38.0 
1    79.61 

« 

25 


at  20-25' 


(U.  S.  P.) 


(Enell,  1899.) 
(Dehn,  1917.) 


THE  SOLIDIFICATION  POINTS  OF  MIXTURES  OF  ANTIPYRINE  AND  CHLORAL 

HYDRATE. 

(Tsakalatos,  1913.) 


toof 
Solidification. 


Gms. 


108.9 

90 
70 

50 . 5  Eutec. 

60 

62.3  m.  pt. 

60 

56  Eutec. 


IOO 

86.1 

73 

64.2 
56.8 
53-2 

50-3 

47.2 


Solid 
Phase. 

CUH12N20 


"+i.a 


to  of          Gms.  CUH12N20              SnllM 

Solidification.      f 

>er  zoo  urns 
Mixture. 

Phase. 

60 

61.8  m.  pt. 

40.9 
36.7 

1.2 
it 

57 
So 

30.1 
26.1 

it 

40 
33.  8  Eutec. 
40 
5i.6 

20.2 
I6.5 

6 

0 

i.2+CCl3.COH.H20 
CC13.COH.H,0 

I.I 
1.2 


CUH12N2O.CC13COH.H2O  (Hypnal). 
CnHi2N2O.2(CCl3.COH.H2O)'(Bihypnal). 


THE  SOLIDIFICATION  POINTS  (Solubility,  see  footnote,  p. 
'    ANTIPYRINE  AND  SALOL. 

(Bellucci,  1912,  1913.) 


i),  OF  MIXTURES  OF 


Initial  t°  of       Gms'  C"H,2N2O 

Initial  t°  of     Gm?'  C" 

Solidification. 

per  zoo  L»ms. 
Mixture. 

Solidification. 

112.  6 

IOO 

65 

40 

104.5 

90 

53 

30 

98 

80 

30  Eutec. 

i7 

91 

70 

34 

20 

83 

60 

35 

10 

75 

50 

42 

0 

97    APOMORPHINE  HTDROCHLORIDE 
APOMORPHINE  HYDROCHLORIDE  Ci7H17NO2.HCl. 

100  gms.  water  dissolve  1.7  gms.  salt  at  15°  and  2  gms.  at  25°. 
100  gms.  90%  alcohol  dissolve  2  gms.  salt  at  25°. 

(Dott,  1906;  Squires  and  Caines,  1905.) 

ARACHIDIC  ACID  C20H4oO2. 

SOLUBILITY  DATA  DETERMINED  BY  THE  FREEZING-POINT  METHOD  ARE 
GIVEN  BY  MEYER,  BROD  AND  SOYKA  (1913),  FOR  MIXTURES  OF: 

Arachidic  and  Stearic  Acids. 

Palmitic  Acids. 
'    Lignoceric  Acids. 

ARBUTIN  Ci2Hi607.£H2O. 

100  gms.  trichlorethylene  dissolve  o.on  gm.  arbutin  at  15°. 

(Wester  and  Bruins,  1914.) 

ARGON,  A. 

SOLUBILITY  IN  WATER. 

(Estreicher  — Z.  physik.  Chem.  31,  184,  '99.) 


to         Cor.  Bar. 

Vol.           Vol.  Absorbed 

Absorption  Coefficients.* 

Solubility. 

Pressure. 

HaO. 

Argon. 

a. 

/. 

0. 

0 

. 

. 

0-0578 

0 

.0102 

I 

764 

•9 

77 

.40 

4 

•34 

0 

.0561 

0-0561 

O 

.0099 

5 

765 

•o 

77 

•39 

3 

.92 

O 

.0507 

0-0508 

O 

.0090 

10 

765 

•3 

77 

.41 

3 

•49 

o 

.0450 

0-0453 

0 

.0079 

15 

762 

•4 

77 

.46 

3 

•13 

0 

.O4O4 

O.O4IO 

0 

.0072 

20 

757 

.6 

77 

•53 

2 

.86 

o 

.0369 

0.0379 

O 

.0066 

25 

766 

•7 

77 

.62 

2 

.64 

o 

•0339 

0.0347 

O 

.0060 

30 

760 

.6 

77 

•73 

2 

•43 

0 

.0312 

0.0326 

0.0056 

35 

757 

.1 

77 

.86 

2 

.24 

o 

.0288 

0.0305 

O 

.O052 

40 

758 

•3 

77 

•99 

2 

.07 

o 

.0265 

0.0286 

O 

.0048 

45 

756 

•4 

78 

•15 

I 

.92 

0 

.0246 

0.0273 

0 

.0045 

5° 

747 

.6 

78 

•31 

I 

•73 

o 

.0221 

0.0257 

o 

.0041 

a  = under  barometric  pressure  minus  tension  of  H2O  vapor. 

/  = under  760  mm.  pressure. 

q  =  grams  argon  per  100  g.H2O  when  total  pressure  is  equal  to  760  mm. 

*  See  Acetylene,  page  16. 

SOLUBILITY  OF  ARGON  AND  WATER. 
(von  Antropoff,  1909-10.) 


O 
10 
20 

30 
40 

50 


Coef .  of  Absorption. 
0.0561 
0.0438 
0.0379 
0.0348 
0.0338 
0-0343 


The  coef .  of  absorption  adopted  for  these  results  is  that  of  Bunsen  as  modified 
by  Kuenen.  The  modification  consists  in  substituting  unit  of  mass  in  place  of 
unit  of  volume  of  water  in  the  formula. 

Data  for  the  solubility  of  argon  in  water  and  in  sea  water,  together  with  a 
critical  discussion  of  the  literature,  are  given  by  Coste  (1917). 

Data  for  the  solubility  and  diffusion  of  argon  in  solid  and  liquid  metals  are 
given  by  Sieverts  and  Bergner  (1912). 


ARSENIC  98 

ARSENIC  As. 

Data  for  the  fusion-points  of  mixtures  of  arsenic  and  iodine  are  given  by 
Jaeger  and  Doornbosch  (1912). 

MetaARSENIC  ACID  AsO2H. 

DISTRIBUTION  AT  25°  BETWEEN: 

(Auerbach,  1903.) 
H2O  and  Amyl  Alcohol.         Sat.  Aq.  H3BO3  Solution  and  Amyl  Alcohol. 

Cms.  AsO2H  per  1000  cc.  Gms.  AsQ2H  per  1000  cc. 

Aq.  Layer.  Alcoholic  Layer.  Aq.  Layer.  Alcoholic  Layer. 

4.82  O.gO  9.28  1.75 

9-63  i-75  18.74  3.47 

18.44  3-5o 

ARSENIC  TriBROMIDE  and  TrilODIDE  AsBr3  and  AsI3. 

100  gms.  H2O  dissolve  about  6  gms.  AsI2  at  25°.  (U.  S.  P.) 

100  gms.  carbon  disulfide  dissolved  about  5.2  gms.  AsI3.  (Squires.) 

100  gms.  methylene  iodide,  CH2I2,  dissolve  17.4  gms.  AsI3  at  12°,  d  of  sat 

Solution  =  3.449.  (Retgers,  1893.) 

SOLUBILITY  DATA  DETERMINED  BY  THE  FREEZING-POINT  METHOD  ARE  GIVEN 

FOR  MIXTURES  OF: 
Arsenic  tribromide  and  naphthalene.  (Pushin  and  Kriger,  1914-) 

"      phosphorus  triiodide.  (Jaeger  and  Doornbosch,  1912.) 

"       triiodide  and  iodine.  (Quercigh,  1912.) 

ARSENIC  TriCHLORIDE  AsCl3. 

When  i.o  gm.  of  arsenic  as  the  trichloride  is  dissolved  in  100  cc.  of  aq.  HC1 
and  the  solution  shaken  with  100  cc.  of  ether  the  following  percentages  of  the 
metal  enter  the  ethereal  layer;  with  20%  HC1,  68%;  15%  HC1,  37%;  10% 
HC1,  7%;  5%  HC1,  0.7%  and  with  i%  HC1,  0.2%  of  the  arsenic.  (Mylius,  1911.) 

ARSENIC    TRIOXIDE     As2O3. 

SOLUBILITY  OF  THE: 

Crystallized  Modification.  Amorphous  Modification, 

In  Water.  In  Water. 


.  Gms.As203per 

Sat.  Solution.  ioocc.H2O. 

2  1  .  201  ord.  temp.          3  .  7 

15  1-657  b.  pt.  11.86 

25  ft  2  '°38  In  Alcohol,  Ether  and  CS2. 

39'8  2.930  G.As203  per  xoog.  Solvent. 

b-Pt-  Alcohol  0.446 

(Bfuner  and  St.  Tolloczko  —  Z.  anorg.  Chem.  37,  456,    Ether  O  .  454 

'03;  Chodounsky  —  Listy.  Chem.  13,  114,  '88.)         £§  O.OOI 

(Winkler  —  J.  pr.  Chem.  [2]  31,  347,  '85.) 

SOLUBILITY  OF  ARSENIC  TRIOXIDE  IN  AQUEOUS  SOLUTIONS  OF  AMMONIA  AT 
30°  (INTERPOLATED  FROM  ORIGINAL  RESULTS). 

(Schiememakers  and  deBaat,  1915.) 

Gms.  per  100  Gms.  Sat  Sol.  Gms.  per  100  Gms.  Sat.  Sol. 

"  Solid  Phase.  .  -  ••  -  "  -  .      Solid  Phase. 


.  . 

NH3.  AsjOg.  NH3. 

0  2.3  As2O3                       4  7.6        NH4AsO4 

1  8.3  "                          5  6.2 

2  14.9  "                          7  4.6 
2.8  20.5  As2O3+NH4AsO2  10  3.1 

3  13  NH4As04  13  2.4 
3-5            9-i  14-3  2.2 


99 


ARSENIC  OXIDES 


SOLUBILITY   OF  ARSENIC  TRIOXIDE  IN  WATER  AND  IN  '  AQUEOUS   SOLUTION 

OF  HYDROCHLORIC  ACID  AT  15°  (Interpolated  from  the  original). 

(Wood,  1908.) 


Mols.  HC1  per 
Liter. 

Gms.  AsA  per 
100  cc.  Solution. 

0 
0.46 

1-495 

2 

1.2 

4 

1-3 

Mols.  HC1  per 
Liter. 

Cms.  AsA  per 
100  cc.  Solution. 

6 

3-8 

7 

7-5 

8 

12.5 

9 

17.7 

SOLUBILITY  OF  ARSENIC  TRIOXIDE  IN  AQUEOUS  SALT  SOLUTIONS. 

(Schreinemakers  and  deBaat,  1917.) 
In  Aq.  Ammonium  Bromide  at  30°. 
Gms.  per  too  Gms.  Sat.  Sol.        ^  ^^ 

AsA 


AsA- 

NH4Br. 

2.26 

0 

2.25 

0-339 

0.679 

4-37 

0.518 

7.l8 

0.386 

I3-3I 

0.303 

2O.I4 

0.237 

31.69 

0.154 

41-34 

0.190 

45.66 

0 

44-8 

As203.NH4Br 


"+NH,Br 
NI^Br 


In  Aq.  Sodium  Bromide  at  30°. 

Gms.  per  too  Gms.  Sat.  Sol. 

NH^Br. 

2.19 

5-57 

AsA 

2.09 

10.89 

" 

1.88 

20.79 

« 

1.63 

30.39 

" 

1.50 

35-75 

" 

1.20 

39-24 

(AsA)3NaBr 

0-953 

43.64 

" 

0.852 

45-99 

<( 

0.719 

50.25 

"  -f-NaBr.2: 

0 

±49-5 

NaBr.2H2O 

In  Aq.  Barium  Bromide  at  30°. 

Cms.  per  too  Gms.  Sat.  Sol. 


In  Aq.  Barium  Chloride  at  30°. 


AsA 
2.09 
2.03 

BaBr2. 
9.41 
16.88 

1.97 
1.87 
1.58 

24.03 
24.41 
23.49 

0-757 
0.678 
0.464 

29.09 
33-08 
38.19 

0.322 

43-02 

0.277 
O 

50.03 
50.62 

Cms.  per  100  Cms.  Sat.  Sol. 


'  +BaBr2.2H2O 
BaBr2.2H2O 


AsA 

BaCl2. 

2.24 

3-84 

2.  2O 

8.72 

2.19 

8.86 

2-15 

10.34 

1.69 

9-55 

1.  12 

13.62 

0.905 

16.93 

0-737 

20.06 

0.608 

23.87 

0.506 

26.54 

0 

27.6 

Solid  Phase. 
AsA 


(AsA)2.BaCl, 


'  +BaCl2.2H2O 
BaCl2.2H2O, 


In  Aq.  Calcium  Bromide  at  20°.  In  Aq.  Calcium  Chloride  at  I9.5°-2O°. 


Gms.  per  100  Gms.  Sat.  Sol. 

Solid  Phase. 

As2  O3 

CaBr2.  ' 

1-58' 

9.65 

AsA 

1.28 

20.13 

" 

O.9I2 

34-90 

« 

0.789 

41 

« 

0.698 

47.67 

« 

0-5I3 

52.06 

« 

0.687 

58.22 

"  +CaBr2.6H2O 

0 

58.20 

CaBr2.6H2O 

Gms.  per  100  Gms.  Sat.  Sol. 


AsA. 
I.78 

i-39 

1. 01 

0.865 

0-757 
0.697 
0.675 

O 


CaClz. 
O 

12.66 

23.09 
27.68 
31.85 

36.01 
41.92 
42.7 


Solid  Phase. 
AsA 


100  gins.  95%  formic  acid  dissolve  0.02  gm.  AszO3  at  19.8°. 


"  +CaCl2.6H20 
CaCl,.6H,O 

(Aschan,  1913.) 


ARSENIC  OXIDES 


100 


SOLUBILITY  OF  ARSENIC  TRIOXIDE  IN  AQUEOUS  SALT  SOLUTIONS.     (Continued.) 


In  Aq.  Lithium  Bromide  at  30°. 
Gms.  per  100  Gms.  Sat.  Sol.  ^  ^^ 


AsA 


In  Aq.  Lithium  Chloride  at  30°. 

Cms.  per  too  Cms.  Sat.  Sol. 


AsA. 

LiBr. 

2.26 

O 

1.69 

11.68 

1.20 

23-23 

0-734 

35-54 

0-534 

37 

0.332 

42.62 

0.28l 

43-87 

0.198 

46.75 

0 

59.62 

+(As203)2.LiBr 
(As2O3)2.LiBr 


LiBr.H2O 


AsA. 

LiCl.    ' 

LOOUU  1  IK1SC. 

1.69 

7-57 

AsA 

I-I5 

15-30 

« 

0.77 

22.67 

« 

0-54 

29.04 

it 

0.43 

35-37 

" 

0-39 

41.13 

" 

0.385 

43-oi 

<« 

0.41 

45.12 

"  +LiCl.H2O 

0 

46.1 

LiCl.H2O 

In  Aq.  Potassium  Bromide  at  30°. 

Gms.  per  100  Gms.  Sat.  Sol. 


In  Aq.  Potassium  Iodide  at  30**. 


Solid 


Gms.  per  100  Gms.  Sat.  Sol. 


Solid 


'AsA- 
2.25 
0.8l8 
0.460 

0.327 

0.290 
0.275 

0.207 
0.166 

0 


KBr. 
0.336 
2.51 
12.78 

22.59 

27.40 
36-98 

39  -°4 
42.07 


AsA+0 


'AsA- 
2.26 
0.772 
0.296 


AsA 
(AsA)2-KI 


150 
II9 


"+KBr 

KBr 


0.081 
0.115 

0.134 


D  variesfrom  (As2O3)2KBrto  (As203)7(KBr)4.  ° 
1  In  Aq.  Strontium  Bromide  at  30°. 

Gms.  per  100  Gms.  Sat.  Sol. 


AsA- 
.69 
.74 
.48 
.25 
.07 

0.991 

0 


SrBr2. 
1  1  .  69 
22.09 

31.98 
41.91 
46.87 
48.91 
49-H 


AsA 


As2O3. 
2.14 
1.92 
1.67 
1.46 
I  .  28 

"+SrBr2.6H20  x  .  23 

SrBr2.6H2O  O 

ARSENIC  PENTOXIDE  As2O6. 

SOLUBILITY  IN  WATER. 

(Menzies  and  Potter,  1912.) 
Solid  Phase.  t°. 

Ice 


KI. 
O 

I.I9 
9-56 
22.89 

34-31 
40.79 
47.07 

53-51 
60.54 
61.5 
In  Aq.  Strontium  Chloride  at  30°. 

Gms.  per  100  Gms.  Sat.  Sol. 

SrCl2. 

6.27 
13.67 
21.29 
27.46 
34-03 
36.16 

37-5 


"+KI 
KI 


Solid  Phase. 
AsA 


+SrCl2.6H20 
SrCl2.6H,0 


-  5  10.6 

—  io  15.6 

—  20  21.3  " 
-30                   25.1 

—  40  27.8 
-50  29.9 

—  59  EutCC.  31.7  Ice+AsA4H20 

—  50  32.6  AsA4H20 

-40  33-5 

-30  34-4 

-20  35.4 

100  gms.  95%  HCOOH  dissolve  7.6  gms. 


—  io 
o 
+  10 

20 

29 

40 

60 

80 

100 

120 

140 


36.2 

37-3 
38.3 
39-7 
41.4 
41.6 
42.2 
42.9 
43-4 
43-7 
44-5 


Tol    Solid  Phase. 
AsA4H20 


"+3AsA.5H20 
3As206.5H2O 


19 


(Aschan,  1913.) 


ioi  A&5FNIOCS  r&lELFIDE 

ARSENIOUS  SULFIDE  As^Ss. 

looo  cc.  water  dissolve  0.000517  gm.  As2S3  at  1 8°.  (Weigel,  1907.) 

Data  for  the  fusion-points  of  mixtures  of  arsenious  sulfide  and  silver  sulfide 

are  given  by  Jaeger  and  Van  Klooster  (1912). 

ASPARAGINE  C4H8N2O3.H2O. 

SOLUBILITY  /S-/-ASPARAGINE,  C4H8N2O3.H2O,  AND  OF  ^-/-ASPARAGINIC  ACID, 
C4H7NO4,  IN  WATER. 

(Bresler  —  Z.  physik.  Chem.  47,  613,  '04.) 
/3-/- Asparagine.  /3-/-Asparaginic  Acid. 


Gms. 
t°.   C4H8N203.H20    t°. 
per  100  g. 

Gms. 
C4H8N203.H20          t 
per  loo  g. 

0 

Gms. 
C4H7NO4 
per  100  g. 

t 

Gms. 
'.         C4H7NO4 
per  100  g. 

H2O. 

H20. 

H2O. 

H2O. 

0-7 

0.9546 

55-5 

10. 

650 

0 

.2 

0-2674 

51 

•  O 

i 

.2746 

7-9 

I  .  4260 

71.7 

19. 

838 

9 

•5 

0.4042 

63 

•5 

i 

.8147 

17-5 

2.1400 

87.0 

36. 

564 

16 

•4 

0.5176 

70 

.0 

2 

•3500 

28.0 

3.1710 

98.0 

52- 

475 

31 

•5 

0-75*4 

80 

•5 

3 

.2106 

41-4 

5.6500 

40 

•  o 

0.9258 

97 

•4 

5 

•3746 

)  gms.  H2O  dissolve  2.4 

gms. 

asparagine  at  2o°-25°. 

(Dehn,  1917.) 

100  gms.  pyridine  dissolve  0.03  gm.  asparagine  at  2o°-25°. 
;ioo  gms.  50%  aq.  pyridine  dissolve  0.15  gm.  asparagine  at  2O°-25°. 
loo  gms.  trichlorethylene  dissolve  o.oi  8  gm.  asparagine  at  1  5°.  (Wester  &  Bruins,  1914-) 
Data  for  the  solubility  of  asparaginic  acid  in  aqueous  salt  solutions  are  given 
by  Wiirgler  (1914). 

ASPIRIN   (Acetyl  salicylic  acid)   C6H4(OCH3CO)COOH. 

loogms.  water  dissolve  0.25  gm.  aspirin  at  room  temperature.  (Squire  and  Caines,  1905.) 
loo  cc.  90%  alcohol  dissolve  20  gm.  aspirin  at  room  temperature.   " 


ATROPINE 

SOLUBILITY  OF  ATROPINE,  Ci7H23NO3,  AND  OF  ATROPINE  SULFATE, 
$      (CnH23NO3)2.SO2(OH)2,  IN  WATER  AND  OTHER  SOLVENTS. 

(U.  S.  P.;  Muller,  1903.) 

Grams  Atropine  per  xoo  Grams. 


Solution.  Solvent.  (U.  S.  P.)      Gf^|$Jlt 

Water  25  1.782  (20°)  0.222  (0.13*)    263.1 

Water  80  ...  1.15                   454-5 

Alcohol  25  ...  68.44                     27 

Alcohol  60  ...  in.  ii                     52.6 

Ether  25  2.21  (20°)  6.02                       0.047 

Chloroform  25  68.03  (20°)  64.10                       0.161 

Benzene  20  3.99 

Carbon  Tetrachloride  20  0.661 

Ethyl  Acetate  20  3 .88 

Petroleum  Ether  20  o .  83 

Glycerol  15  ...  3                          33 

Aniline  20  ...  34§ 

Diethylamine  20  ...  67  § 

Pyridine  20  ...  73§ 

Piperidine  20  ...  H4§ 

50%  Aq.  Glycerol )  -r 

+  3%H3B03      j 

Oil  of  Sesame  20  ...  0.25* 

*Zalai,  1910.  tAti7°,Schnidelmeiser,i9oi.  JGori,i9i3.  §  Scholtz,  1912.   IFBaroni and  Borlinetto,  1911. 


102 


DISTRIBUTION  OF  ATROPINE  BETWEEN  WATER  AND  CHLOROFORM  AT  25°. 

(Seidell,  19100.) 
Gms.  Atropine  Recovered  per  15  cc. 


per  15  cc.  HssO+is  cc. 
CHCla. 

Aqueous 
Layer  (a). 

Chloroform 
Layer  (b). 

b  < 
a 

O.OO5 

O.OOIO 

0.0057 

5-7 

0.025 

0.0021 

0.0256 

12.2 

0.125 

0.0049 

o  .  i  246 

25.4 

0.625 

0.0160 

0.6267 

39-i 

ATROPINE  METHYLBROMIDE 

IOO  gms.  water  dissolve  IOO  gms.  of  the  salt  at  room  temp.    (Squires  and  Caines,  1905.) 
100  cc.  90%  alcohol  dissolve  10  gms.  of  the  salt  at  room  temp.       " 

AZELAIC  ACID  C7H14(COOH)2. 

SOLUBILITY  IN  WATER. 

(Lamouroux,  1899.) 

t°.  =  o          15          20         35         50         65 

Gms.  C7Hi4(CqOH)2 

per  100  cc.  solution  =     o.io      0.15      0.24      0.45      0.82      2  20 
loo  gms.  95%  HCOOH  dissolve  3.79  gms.  azelaic  acid  at  19.4°.      (Aschan,  1913.) 
DISTRIBUTION  OF  AZELAIC  ACID  BETWEEN  WATER  AND  ETHER  AT  25°. 

(Chandler,  1908.) 


Gms.  C7Hi4(COOH)j  per  1000  cc. 


Aq.  Layer. 
O.O6 


Ether  Layer* 
0.47 
1. 10 
2.71 
4.26 


Gms.  C7Hi4(COOH)2  per  1000  cc. 

Aq.  Layer.  Ether  Layer. 

0.40  5.83 

0.50  7.40 

0.58  8.65 


O.IO 
0.20 
0.30 

AZOBENZENE   C6H5.N2.C6H6. 

SOLUBILITY  OF  AZOBENZENE  IN  SEVERAL  BINARY  MIXTURES. 

(Timmermans,  1907.) 


Solvent,  Binary  Mixture  of:                                           t°. 

Gms.  (CeHsN)?  per 
loo  Gms.  Sat.;Sol. 

6.4 

0.46 

34.9%  Butyric  Acid  +  65.1%  H2O  (=  sat.  sol. 

10 

IT  *J 

at  2.3°) 

20 

•I3 

O    / 

30 

i  .92 

40.6 

2-95 

80 
.0 

3.22 

36%  Triethylamine  +  64%  H2O  (=  sat.  sol.  at 

II 

2.57 

19.1°) 

14 

1.66 

17.4 

°-54 

69-3 

0-43 

36.5%  Phenol  +  63.5%  H2O  (=  sat.  sol.  at 
6-^°) 

72.7 
80 

0.47 
1.47 

o  o  / 

90 

2-43 

IOO 

3-45 

23-9 

0.52 

71.4%   Phenol  +  28.6%  H2O  (=  sat.  sol.  at 

20.6°) 

25.2 
40 

0.87 
4.45 

60 

10.35 

72.6 

I33-40 

46%  Succinic  Nitrile-j-  54%  H2O  (  =  sat.  sol.  at  54°)    56  .  9 

0.54 

103 


AZOBENZENE 


SOLUBILITY  OF  AZOBENZENE  IN  SEVERAL  ALCOHOLS. 

(Timofeiew,  1894.) 


Solvent. 


Methyl  Alcohol          9 . 5 


Ethyl  Alcohol 


9-5 


Gms.  (C6H3N)2 
per  loo  Gms. 

Solvent. 

Gms.  (C«HsN)2 
t°.         per  100  Gms. 

Sat.  Sol. 

Sat.  Sol. 

3-8 

Ethyl  Alcohol 

10.5            5.88 

3-95 

Propyl  Alcohol 

9-5            5-42 

5-29 

"            " 

10.5        6.02 

SOLUBILITY  OF  AZOBENZENES  IN  WATER  AND  IN  PYRIDINE. 

(Dehn,  1917.) 

Gms.  Each  Compound  (Determined  Separately)  per 
100  Gms.  Solvent: 


Solvent. 


Water 

Pyridine 

Aq.  50%  Pyridine 


20-25 
20-25 
20-25 


Azobenzene. 

Diazoamino- 

Dimethylamino- 

benzene. 

azobenzene. 

0.03 

O.O5 

0.016 

76.44 

I36.7 

27.90 

16.78 

67.7 

4-Si 

HydroxyAZOBENZENE   C6H6.N:  N.C6H4OH. 

1000  cc.  sat.  solution  in  H2O  contain  0.0225  gm.  C6HsN:  N.C6H4OH  at  25°. 

1000  cc.  sat.  solution  in  H2O  sat.  with  C6H6  contain  0.0284  gm.  C6H6N:N. 
C6H4OH  at  25°. 

looo  cc.  sat.  solution  in  C6H6  sat.  with  H2O  contain  15.20  gms.  C6H6N:N. 
C6H4OH  at  25°.  (Fanner,  1901.) 

Distribution  results  for  hydroxyazobenzene  between  benzene  and  water  gave: 
cone,  in  C6H6  -*•  cone,  in  H2O  =  539  at  25°.  (Farmer,  1901.) 

AminoAZOBENZENE   C6H6N:  N.C6H4.NH2. 

Distribution  results  for  amino  azobenzene  between  benzene  and  water  gave: 

COnc.  in  C6H6  -f-  COnc.  in  H2O  =3,173  at  25°.  (Farmer  and  Warth,  1904.) 

AZOANISOL,   AZOBENZENE,   AZOPHENETOL,  etc. 

SOLUBILITY  DATA,  DETERMINED  BY  THE  FREEZING-POINT  METHOD  (see  footnote, 

p.  l),   ARE   GIVEN  FOR  THE   FOLLOWING   MIXTURES: 

p  Azoanisol  Azobenzene 


+  p  Azoxyanisol  (i) 

-j-  p  Azoanisolphenetol  (i) 

+  Methylpropylazophenol  (i) 
"     +  p  Azophenetol  (i) 
p  Azoxyanisol 

+  p  Azoanisolphenetol  (i) 

+  p  Azoxyphenetol  (3),  (4) 

+  Benzene  (2) 

-j-  Ethylene  bromide  (2) 

+  Hydroquinone  (5) 

+  Benzophenone  (5) 

+  p  Methoxycinnamic  Acid  (5) 

-f  Nitrobenzene  (2) 
p  Azoanisolphenetol 
to     +  Azophenetol  (i) 

+  p  Dipropylazophenetol  (i) 
Azobenzene 

+  Azoxybenzene  (6) 

+  p  Azotoluene  (7) 

+  p  Azonaphthalene  (7) 

-+-  Benzalaniline  (7) 
p  Azobenzoic  Acid  Ethyl  Ester 

+  p   Azoxybenzoic    Acid    Ethyl 
Ester  (5) 

(i)  Bogojawlausky  and  Winogrodow,  1907;    (2) 
(3)  Ratinjanz  and  Rotaiski,  1906;    (4)  Prins,  1909;    (5) 
(7)  T 
1907 


Pascal  and  Normand,  1913;  (8)  Vanstone,  1913;  (9)  Beck,  1904;  (10)  Isaac  (1910-11); 
';   (12)  Hasselblatt,  1913;   (13)  Garelli  and  Calzolari,  1899;   (14)  Bruni  and  Gorni,  1899. 


+  Benzeneazonapthalene  (9) 

+  Benzil  (8) 

+  Benzoin  (8) 

+  Benzylaniline    (7),    (9),    (10), 
(n),  (12) 

+  Dibenzyl  (7),  (13),  (14),  (12) 

+  Diphenyl  (9) 

-j-  p  Dimethoxystilbene  (7) 

+  Hydrobenzene  (7) 

+  Stilbene  (7),  (9) 

+  Tolane  (7) 
Hydrazobenzene 

+  Benzoin  (8) 
p  Azophenetol 

+  p  Azoxyphenetol  (i)  ' 

-j-  p  Dipropylazophenetol  (i) 
p  Azoxyphenetol 

+  Cholesterylisobutyrate  (A) 
"     +  Cholesterylpropionate  (4) 

+  Cholesterylbenzoate  (4) 
"     4-  P  Methoxycinnamate  (4) 
p  Azotoluene 

+  Stilbene  (7) 


fawlauski,  Winogrodow  and  Bogolubow,  1906; 
Kock,  1904;   (6)  Hartley  and  Stewart,  1914; 
(n)  Jaeger, 


AZOLITMINE 


104 


AZOLITMINE  C7H7NO4. 

100  gms.  H2O  dissolve  39.5  gms.  azolitmine  at  2O°-25°. 

100  gms.  pyridine  dissolve  0.05  gm.  azolitmine  at  20-25°. 

loo  gms.  aq.  50%  pyridine  dissolve  0.12  gm.  azolitmine  at  2O°-25°. 


(Dehn,  1917.) 


AZOPHENETOL  (p)  C^ 

SOLUBILITY  IN  100  PER  CENT  ACETIC  ACID. 

(Dreyer  and  Rotarski  —  Chem.  Centr.  76,  II,  1016,  '05.) 

t°=  89.2          91  93  95«6  97-2  99-6 

Mols.  per  liter.        0.153     0.176         0.185         0.209         0.232         0.252 

A  break  in  the  curve  at  94.7°  corresponds  to  the  transition  temperature  of  the 
a  modification  into  the  ft  modification. 

BARIUM  ACETATE  Ba(CH3COO)2.     . 

SOLUBILITY  IN  WATER. 

(Walker  and  Fyffe,  1903;  Krasnicki,  1887,  gives  incorrect*  'results.) 


Gms.  Ba(CH3COO)2 
per  100  Gms. 


Solid  Phase. 


Gms.  Ba(CH3COO)2 

per  100  Gms.         Solid  Phase. 


Water. 

Solution. 

Water. 

Solution 

o-3 

58 

.8 

37 

.0 

Ba(C2H302)2.3H20 

40 

•5 

79 

.0 

44.1 

Ba(C2H302)3 

7-9 

61 

.6 

38 

.1 

ft 

41 

•5 

78 

•7 

44.0 

u 

17-5 

69 

.2 

40 

•9 

1C 

44 

•5 

77 

•9 

43-8 

11 

21  .6 

72 

.8 

42 

.1 

(I 

51 

.8 

76 

•5 

43-4 

(I 

24.1 

78 

.1 

43 

•9 

11 

63 

.0 

74 

.6 

42.7 

1C 

26.2 

76 

•4 

43 

•3 

Ba(C2H302)2.H20 

73 

•  o 

73 

•5 

42.4 

(C 

30.6 

75 

.1 

42 

•9 

« 

84 

.0 

74 

.0 

42.5 

cc 

35-o 

75 

.8 

43 

.1 

u 

99 

.2 

74 

.8 

42.8 

(( 

39-6 

77 

•9 

43 

.8 

a 

Transition  temperatures  24.7°  and  41°. 
loo  cc.  97%  ethyl  alcohol  dissolve  0.0723  gm.  barium  acetate  at  room  temp. 

(Crowell,  1918.) 

AQUEOUS  SOLUTIONS  OF  ACETIC  ACID 
° 


SOLUBILITY   OF    BARIUM  ACETATE  IN 

AT  25 

(Iwaki,  1914.) 


5-18 


Mols.  per  too  Mols.  Sat.  Sol. 
CHaCOOH. 

Lo 

0.41 

1.40 

1.46 

3.30 
10.23 
20.60 


(CH3COO)2Ba.3H2O 
"  +3.3.11 


4.52 


5.34 
5.32 
3.48 
3.14 
3.62 
3(CH3COO)2Ba.3CH3COOH.iiH20, 


3.3.11 


Mols.  per  100  Mols.  Sat.  Sol. 
CHaCOQH. 

28.72 

36.54 
42.08 
46.51 
51.98 
65.77 


85.27 


7.85 
8.87 
8.62 
8.40 
7.36 


;<  +1.3 


1.3 


=  (CH3COO)2Ba.3CH,COOH. 


3.3.11 

BARIUM  ARSENATE   Ba3(AsO4)2. 

loo  gms.  H2O  dissolve  0.055  gm.  Ba3(AsO4)2;  100  gms.  5%  NH4C1 
dissolve  0.195  gm.,  and  100  gms.  10%  NH4OH  dissolve  0.003  Sm- 
Ba3(AsO4)2 

(Field  —  J.  Ch,  Soc.  n   6,  i8sp.) 

BARIUM  BENZOATE   (C6H6COO)2Ba.6H2O. 

100  gms.  sat.  aqueous  solution  contain'  4.3  gms.  salt  (anhydrous  P)1  at  15° 

and  IO.I  gms.  at  IOO°.  (Tarugiand  Checchi,  1901.) 


105  BARIUM  BORATE 

BARIUM  BORATES. 

SOLUBILITY  IN  AQUEOUS  BORIC  ACID  SOLUTIONS  AT  30°. 

(Sborgi,  1913.) 

Cms.  per  ioo  Gms.Sat.  Sol.  Cms.  per  100  Cms.  Sat.  Sol. 

•    Ba2Q3.      '      BaQ.  Sohd  Phase.  .  -  t  Sohd  Phase. 


3.6         0.04      H3B03+i.3.7  0.3          0.23  1.3.7 

3.4  0.04  1.3.7  0.3          0.31         1.37+1.1.4 

2.5  0.04  0.2          0.8  1.1.4 

2.0  0.04  0.2  1.2 

i.o         0.05  0.24        4.8  " 

0.5         0.09  0.26        5.8        i.i4+Ba(OH)2 

0.4         0.12  0.08        5.3  Ba(OH)2 

1.3.7  =  BaO.3B2O3.7H2O  (Triborate);    1.1.4  =  BaO.B2O3.4H2O  (Metaborate). 
The  original  results  were  plotted  and  above  figures  read  from  curve. 

BARIUM  BROMATE  Ba(BrO3)2H2O. 

SOLUBILITY  IN  WATER. 

(Trautz>nd  Anschiitz,  1906;  Rammelsberg,  1841.) 

Cms.  Ba(BrO3)2  Cms.  Ba(BrO3)2  Cms.  Ba(BrO3)i 

t.  per  ioo  Gms,  t°.  per  ioo  Cms.  t°.  per  ioo  Cms. 

Solution.  Solution.  Solution. 

—    0.034  0.28  30  0-95  70  2.922 

o  0.286  40  1.31  80  3-521 

+  10  0.439  5°  J-72  90  4-26 

20  0.652  60  2.271  98.7  5-  .256 

25  0.788  99.65         5.39 

SOLUBILITY  OF  BARIUM  BROMATE  IN  AQUEOUS  SOLUTIONS  OF  SALTS  AT  25°. 

(Harkins,  1911.) 


Cone,  of  Salt 
in  Gms.  Equiv- 
alents per  Liter. 
0 
0.025 
0.050 
O.  IOO 
O.2OO 

Gms. 

Ba(BrOs)2  Dissolved  per  Liter  in  Aqueous  Sol. 

of 

y 

8 

9 

10 

KI 

93 
62 
91 
25 

JOa. 
1.0038) 
1.0059) 
1.0080) 
I.  OI2O) 

Ba(I 

7-93 
7.22 
6.83 
6.415 
6  .  230 

ro3)2. 

1.0059) 
1.0083) 
1.0132) 
1.0233) 

7 
5 
3 

i 

KBrOs. 
93 
216  (1.0046) 
415  (1.0062) 
72     (1.0109) 

7 
8 

Mg(NOs)2. 
•93 

.196(1.0114) 

25° 

Figures  in  parentheses  show  densities  of  the  sat.  sols,  at  — 5-* 

4 

BARIUM    BROMIDE     BaBr2.2H2O. 

SOLUBILITY  IN  WATER. 

(Kremers  —  Pogg,  Ann.  99,  47,  '56;  Etard  —  Ann.  chim.  phys.frja,  540,  '94.) 

Gms.  BaBr2  per  TOO  Grams.  Gms.  BaBr2  j>er  ioo  Grams. 

t°.  'Water.  Solution.  t°.  '  Water.  Solution. 

(Kremers.)  (Kremers.)  (Etard.)  (Kremers.)  (Kremers.)   (Etard.) 

—20 45-6    40     114   S3-2   S^S 

o    98    49.5    47-5    50     II8    S4-i    52-5 
10    101    50.2    48.5    60     123    55.1    53.5 

20     104     51.0     49-5      70       128     56.1     54.5 

25    106   51.4   50.0    80     135   57-4   55-5 
30    109    52.1    50.6    ioo     149    60.0    57.8 

140         ...   59.4 

Sp.  Gr.  of  saturated  solution  at  19.5°  =  1.710. 


BARIUM   BROMIDE  106 

Data  for  the  system  Barium  Bromide  +  Barium  Oxide  +  H2O  at  25°  are 
given  by  Milikau  (1916). 

SOLUBILITY  OF  MIXTURES  OF  BARIUM  BROMIDE  AND  BARIUM  IODIDE  IN  WATER 
AT  DIFFERENT  TEMPERATURES. 

(Etard.) 

Grams  per  ioo  Gms.  Solution.  0  Grams  per  too^Gms.  Solution. 

' 


'  BaBr2.  BaI2.  BaBr2. 

—  16  4.8        58.4  170  ii.  o        67.4 

|-6o  5.5        66.0  210  14.9        67.7 

135  9.2        67  .  2  Both  salts  present  in  solid  phase. 

SOLUBILITY  OF  BARIUM  BROMIDE  IN  METHYL  AND  ETHYL  ALCOHOLS. 

(de  Bruyn  —  Z.  physik.  Chem.  10,  783,  .92  ;  Richards  —  Z.  anorg.  Chem.  3,  455,  '93  ;  Rohland  —  Ibid. 

15  412,  '97.) 

Parts  BaBr2  per  ioo  Parts  BaBr2.aH2O  per  ioo 

o  parts  Aq.  QjHfiOH  of;  parts  of  Aq.  CH3OH  of: 


97%.  »7%.  i°o%.  93-5%.  50%. 

15.0       ..  0.48   (BaBr2.2H20)  ..  45.9  27.3  4.0 

22.5      3  6  56.1 

ioo  gms.  sat.  solution  in  methyl  alcohol  at  the  crit.  temp,  contain  0.4  gm. 

BaBr2.  (Centnerszwer,  1910.) 

Data  for  the  lowering  of  the  melting  point  of  BaBr2  by  BaF2  and  by  BaCl3 
are  given  by  Ruff  and  Plato  (1903). 

BARIUM   PerBROMIDE   BaBr4. 

Data  for  the  formation  of  barium  perbromide  in  aqueous  solutions  at  25°  are 
given  by  Herz  and  Bulla  (1911).     See  reference  calcium  perbromide,  p.  189. 

BARIUM  BUTYRATE  Ba(C4H7O2)22H2O. 

SOLUBILITY  IN  WATER. 

(Deszathy  —  Monatsh.  Chem.  14,  249,  '93.) 

Gms.  Ba(C4H7O2)2  per  ioo  Gms.  Gms.  Ba(C4H7O2)2  per  ioo  Gms. 

**"  Water.  Solution".  Water.  Solution. 

o     37-42    27.24         50      36.44   26.77 
10     36.65    26.82         60      37.68    27.36 

20       36.12     26.55  70         39-58     28.36 

30       35.85     26.38  80         42.13     29.64 

40  35-82         26.37 

ioo  gms.  97%  ethyl  alcohol  dissolve  0.17  gm.  barium  butyrate  at  ord.  temp. 

(Crowell,  1918.) 

BARIUM  CAMPHORATE  BaCioHi4O44H2O. 

SOLUBILITY  OF  BARIUM  CAMPHORATE  IN  AQUEOUS  SOLUTIONS  OF  CAMPHORIC 

ACID  AT  i6°-i7°. 

(Jungflisch  and  Landrieu,  1914-) 

Gms.  per  ioo  Gms.  Sat.  Sol.  Gms.  per  ioo  Gms.  Sat.  Sol. 

Camphoric         Barium  "            SoUd  Phase.  Camphoric  Barium               Solid  Phase. 

Acid.         Camphorate.  Acid.  Camphorate. 

O.68           0.134      d  Camphoric  ac.  +  1.3         0.48  22.71  1.3 

0.84           0.150                      "  0.45  32.19 

0.693         0.20                        1.3  0.50  37-22 

0  .  38           2  .  59                        "  0.51  40  .  99       1.3  +  Ba  Camphorate 

O.44         II.  IO                        "  O  42.59           Ba  Camphorate 
1.3  =  Barium  tetracamphorate, 


ID; 


BARIUM   CAPROATE 


BARIUM  CAPROATE  AND  BARIUM  ISO  CAPROATE. 

SOLUBILITY  IN  WATER. 


(Kulisch,  1893.) 

Barium  Caproate  (Methyl  3  Pentan.) 
Ba(CH3.CH2CH(CH3)CH2COO)2. 

^    Gms.Ba(C6HuO2)2 
40^           per  100  Gms.                  Solid  Phase. 

Water. 

Solution. 

0 

11.71 

10. 

49      Ba(C6Hu02)2.3iH20 

10 

8.38 

7- 

73 

20 

6.89 

6. 

45 

30 

5-87 

5- 

55 

40 

5-79 

5- 

47 

5° 

6.63 

6. 

21 

60 

8-39 

7- 

74 

70 

11.09 

9- 

98 

80 

14.71 

12  . 

82 

90 

19.28 

16. 

16 

(Konig,  1893.) 

Barium  Iso  Caproate  (Methyl  2  Pentan.) 
Ba(CH3CH(CH3)CH2.CH2COO)2. 


Gms.  B3.(C(5rJiiO2/2 
per  loo  Gms.                  gelid  Phase. 

Water. 

Solution. 

14-34 

12 

.  54       Ba(C6HuO2)2.4H2O 

13-33 

II 

•77 

12.67 

II 

.26 

12.37 

II 

.01 

12  .42 

II 

.05 

12.83 

II 

.38 

13  .63 

II 

•99 

14.68 

12 

.80 

16.24 

13 

•97 

17-95 

15 

•23 

BARIUM  CARBONATE   BaCOg. 

SOLUBILITY  IN  WATER. 

(Holleman,  Kohlrausch  and  Rose,  1893.) 

Electrolytic  conductivity  method  used. 

i  liter  H2O  dissolves  0.016  gin.  BaCO3  at  8.8°,  0.022  gm.  at  18°,  and  0.024  g™-  at 
24.2°. 

SOLUBILITY  OF  BARIUM  CARBONATE  IN  WATER  CONTAINING  CO2. 

The  average  of  several  determinations  at  about  10°,  by  Bineau,  Lassaigne, 
Foucroy  and  Bergmann  is  i.io  gms.  BaCO3  per  liter  water.  Wagner  (Z.  anal. 
Ch.  6,  167,  '67)  gives  7.25  gms.  BaCO3  per  liter  of  water  saturated  with  CO2  at 
4-6  atmospheres  pressure. 

Eleven  determinations  by  McCoy  and  Smith  (1911),  of  the  solubility  of 
barium  carbonate  at  25°  in  water  in  contact  with  pressures  of  CO2  varying  from 
0.2  to  30  atmospheres,  showed  that  a  maximum  solubility  is  reached  at  22  atmos- 
pheres (see  also  calcium  carbonate,  p.  192),  at  which  point  the  saturated  solution 
contains  0.727  mols.  =  45.1  gms.  H2CO3  per  liter  and  0.028  mols.  =  7.3  gms. 
Ca(HCO3)2  per  liter.  The  equilibrium  constant  is  k  =  2.24  X  IO"2  and  the 
solubility  product  Ba  X  CO3  =  k*  =  8.1  X  lo"9. 

SOLUBILITY  OF  BARIUM  CARBONATE  IN  AQUEOUS  SOLUTIONS  OF  AMMONIUM 

CHLORIDE  AT  30°. 

(Kernot,  d'Agostino  and  Pellegrino,  1908.) 


Gms.  per  1000  cc. 


NH4C1. 
O 

8.0Q9 

64-536 

92-593 

160.265 

186.775 

268.920 


Solid 
Phase. 


BaCOs. 

0.035  °  BaCOs 

0.521 

1-333 
1.596 

2 

2.093 

2.256 

Data  are  also  given  for  25°.  Some  uncertainty  exists  as  to  the  terms  in  which 
the  results  are  expressed.  In  some  cases  the  column  headings  read  "Gms.  per 
liter  of  H2O"  and  in  others  "Gms.  per  liter  of  solution."  The  saturation  was 
effected  by  adding  just  the  necessary  amount  of  one  constituent  to  cause  the 
disappearance  of  the  last  particle  of  the  other.  The  amounts  so  added  were 
determined  by  weighing  the  flasks.  At  high  concentrations  of  the  two  salts,  the 
sudden  increase  in  solubility  appears  to  indicate  a  molecular  combination. 


Gms.  per  1000  cc.  HzO. 

Solid 
Phase. 

BaCOs. 

NH4C1. 

2.245 

335-70 

BaCOa 

2.706 

358.66 

" 

2.630 

418.33 

NHiCl 

2.I5I 

414.71 

1.558 

4I3-77 

" 

0.730 

4IO.I6 

u 

0 

397-58 

" 

BARIUM  CARBONATE 


108 


SOLUBILITY  OF  BARIUM  .  CARBONATE  IN  AQUEOUS  SOLUTIONS  OF  POTASSIUM 
CHLORIDE  AND  OF  SODIUM  CHLORIDE. 

(Cantoni  and  Goguelia,  1905.) 

In  KClatB.pt.  of  Sol.    In  NaCl  at  B.pt.  of  Sol.    In  10%  KC1  Sol.    In  io%NaC!Sol. 


Cms.  KC1 
per  100 
Cms.  Sol. 

0.15 
1. 00 

3 

IO 

30 


Cms.  BaCOs 

per  1000  cc. 

Sat.  Sol. 


Gms.  NaCl  Gms.  BaCOs 

Gms.  BaCOa 

Gms.  BaCOs 

per  100 
Gms.  Sol. 

per  1000  cc. 
Sat.  Sol. 

t. 

per  1000  cc. 
Sat.  Sol. 

t°. 

per  1000  cc. 
Sat.  Sol. 

0.15 

0.0587 

10 

0.2175 

10 

0.1085 

I 

0.0787 

2O 

o  .  2408 

20 

O.II26 

3 

0.1056 

40 

0.2972 

40 

0.1231 

10 

0-1575 

60 

0-3491 

40 

0.1303 

30 

0.2784 

80 

o  .  4049 

40 

0.1418 

o . 0847 
o. 1781 
0.2667 

0.4274 
0-5550 

Barium  carbonate  boiled  with  aqueous  NH4C1  is  slowly  but  completely  decom- 
posed. The  time  required  varies  inversely  as  the  concentration  of  the  NH^Cl 
solution. 

Data  are  also  given  for  solubility  in  10%  aqueous  KC1  and  NaCl  at  the  boiling 
point,  the  time  factor  being  varied  from  I  to  198  hours. 

Data  for  lowering  of  the  melting  point  of  BaCO3  by  Na2CO3  are  given  by  Sackur 
(1911-12). 


BARIUM  CHLORATE  Ba(ClO3)2.H2O. 
SOLUBILITY  IN  WATER. 

(Carlson,  1910;  Trautz  and  Anschiitz,  1906.) 

fo           Sp.  Gr.  of       Cms.  Ba(ClO»)j  per  100                                 Sp.  Gr.  of 
*•            Sat.  Sol.                Gms.  Sat.  Sol.                       t.                 Sat.  Sol. 

Gms.  Ba(C103)2  per  too 
Gms.  Sat.  Sol. 

O 
IO 
20 
25 
30 

1  .  195              2O 

24 
1.274              28 
30 
32 

3* 

3 

2 

16.90!' 
21.23 
25.26 
27-53 
29-43 
*  C. 

40 
60 
80 

100 

105  .  6  b.  pt. 
t  (rand  4.) 

•355 
•433 
-508 
-580 
.660 

35 
42 
48 
53 
54 

8* 
6 

i 
6 

33 

40 

45 
Si 
52 

i6f 

05 
90 

2 
62 

The  determinations  of  Trautz  and  Anschiitz  appear  to  have  been  made  with 
very  great  care.  The  original  paper  of  Carlson  was  not  available  and  it  has 
been  impossible  to  explain  the  discrepancy  between  the  two  sets  of  results. 


BARIUM   PerCHLORATE   Ba(C104)2.3H2O. 

SOLUBILITY  IN  WATER. 

(Carlson,  1910.) 


O 

20 

40 
60 


Sp.  Gr. 
Sat.  Sol. 

1.782 
1.912 
2.009 
2.070 


Gms.  Ba(C104)2 

per  100  Gms. 

Sat.  Sol. 

67-3 
74-3 
78.2 
81 


80 
100 
1 20 
140 


Sp.  Gr. 
Sat.  Sol. 

2.114 

2.155 
2.195 
2.230 


Gms.  Ba(C104)2 

per  too  Gms. 

Sat.  Sol. 

83-2 

84.9 
86.6 
88.3 


BARIUM  CHLORIDE   BaCl2.2H2O. 

SOLUBILITY  IN  WATER. 

(Mulder,  Engel,  1888;  Etard,  1894.) 
,„  Gms.  BaCla  per  100  Gms. 


O 
10 
20 
25 
30 
40 
50 


Water. 
31-6 
33-3 
35-7 

3£ 
38.2 

40.7 
43-6 


Solution. 
24 
25 

26.3 
27 

27-7 
28.9 

3°-4 


60 

70 

80 

IOO 

130 

1 60 

215 


Gms.  Bad?  per  TOO  Gms. 


Sp.  Gr.  of  solution  saturated  at  o°  =  1.25;  at  20° 


Water. 

Solution. 

46.4 

31-3 

49-4 

33-i 

52.4 

34-4 

58.8 

37 

59-5 

"37-3 

63-6 

38.9 

75-9 

43-1 

1.27. 

109 


BARIUM  CHLORIDE 


SOLUBILITY  OF  MIXTURES  OF  BARIUM  CHLORIDE  AND  AMMONIUM  CHLORIDE 

IN  WATER. 


At  30°.      (Schreinemakers,  1908.) 
Cms,  per'ioo  Cms.  Sat.  Sol 
'   BaCb.  NH4C1. 

22.16  5.71 

18.36         10.06 
15.42         13.84 

10.89  20.01 

8.33       24.69 

7-97         25.92 
3-S6         27.47 


Solid  Phase. 
BaCl2.2HjO 


BaCh.2H20+NH4Cl 
NH4C1 


At  Varying  Temps.      (Schreinemakers,  igiob.) 

Cms.  per  too  Cms.  Sat.  Sol. 

Solid  Phase. 

BaCU.2HjO+NH4Cl 


t 

16.2 
o 

30 
40 

So 


BaCl2. 
8.07 
8.22 
8.19 
8.40 

8-55 


NH<C1. 
16.10 
19.26 
24.89 
26.93 
29-53 


SOLUBILITY  OF  BARIUM  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  BARIUM 
HYDROXIDE  AND  VICE  VERSA  AT  30°. 

(Schreinemakers,  1909-1910,  igiob.) 

Gms.  per  roo'Gms.  Sat.  Sol. 


BaClz. 

BaO. 

27.6 

O 

BaCI2.2H20 

27.42 

1.78 

" 

,57.36 

1.77 

"  +BaCl(OH).2H2O 

'24.98 

2-33 

BaCl(OH).2H2O 

21.46 

3-27 

« 

19.18 

4.67 

it 

BaCl2. 

BaO. 

ia  rnase 

18.67 

4.61 

BaCl(OH).2 

HjO+B 

18.04 

4.62 

BaO.gHjO 

17.08 

4.60 

" 

12.  8l 

4.58 

M 

10.77 

4-45 

« 

O 

4-99 

U 

SOLUBILITY  OF  MIXTURES  OF  BARIUM  CHLORIDE  AND  BARIUM  NITRATE 

IN  WATER: 

At  30°.     (Coppadoro,  1912,  1913.) 
Gms.  per  100  Gms.  Sat.  Sol. 


BaCl2. 
6.06 

13-75 
16.14 
22.70 
26.  II 
26.64 
26.91 
27.38 


Ba(NO3)2. 
9-55 
8.20 
7.92 
7-94 
7.88 

5-37 
4-13 
1.58 


Solid 
Ba(NO»)i 


Ba(NO3)j+BaCl2.2H2O 
BaCl2.2HzO 


At  Varying  Temps.     (Etard,  1894.) 

Gms.  per  100  Gms.  Sat.  S 

S'      Solid  Phase. 

BaCl2. 

Ba(NOs)2. 

O 

22.5 

4-3 

BaCU.2H2O+Ba(NO»)» 

20 

24-5 

6 

" 

40 

26.5 

7-5 

" 

60 

28.5 

9-5 

«< 

IOO 

31 

14 

" 

140 

32 

20 

" 

180 

33 

26 

• 

210 

32 

32 

" 

SOLUBILITY  OF  BARIUM  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  COPPER 
CHLORIDE  AT  30°  AND  VICE  VERSA. 

(Schreinemakers  and  de  Baat,  1908-09.) 


Gms.  per  100  Gms.  Sat.  Sol. 


BaCU. 
O 

1-25 

3.08 

2.72 

2.84 
3.98 


CuCl2. 
43-95 
42.45 
42.07 
42.36 
41.18 
37-42 


Solid  Phase. 
CuCli.2H2O 

(unstable) 

CuCk.  2H2O  +BaCl2. 2H«0 
BaCli.2HiO 


jiiis.  per  it>o 

\jins.  oat.  oui- 

.    Solid  Phase. 

BaCk. 

CuCl2. 

5-49 

30.76 

BaCk^HsO 

10.13 

21.76 

• 

17.08 

11.49 

" 

22.78 

•5-13 

« 

27.6 

O 

it 

Solubility  data  have  been  determined  for  the  following  systems: 

BaCl2.2H2O  4-  CuCl2.2H2O  +  NH4C1  +  H2O  at  30°.  (Schreinemakers,  1909.) 

+  "  4-  KC1  +  H2O  at  40°  and  60°.  (    "   and  de  Baat,  1914.) 

4-  "  +  NaCl  +  H2O  at  30°.  (    "    and  de  Baat,  1908^9.) 

+  BaO  +  Na2O  +  H2O  at  30°.  (Schreinemakers,  igiob.) 

4-  Ba(NO3)2      4-  NaNO3  +  NaCl  +  H2O  at  30°.        (Coppadoro,  1913.) 
4-  HCl  4-  NaCl  4-  H2O  at  30°.  CSchreinemakers,  1909-10.  igiob.) 


BARIUM  CHLORIDE 


no 


SOLUBILITY  OF  BARIUM  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  HYDRO- 
CHLORIC ACID: 


Ato°. 

(Engel,  1888.) 


At  30°. 

(Masson,  1911, 1912-13;  Schreinemakers,  1909-10.) 


>p.  Gr 

Gms.  per  100 

jms.  Sat.  Sol.                  « 

at.  Sol. 

'   HC1. 

BaCli.    '                  S 

.250 

'o 

24.07                      I 

.242 

0.32 

23-3I 

.228 

0.83 

22.11 

.2IO 

I-5I 

2O.I4 

•143 

4.58 

12.76 

.118 

6.13 

9-37 

.099 

7-55 

6-33 

.079 

10.81 

2.64 

.088 

16.92 

0.28 

Sp.  Gr. 

Sat.  Sol. 


Gms.  per  100  Gms.  Sat.  Sol. 


1.3056 
.2651 

.2147 
-1789 
.1419 
.io68 
.o88o 
.0895 
1024 
.!6o9 

The  results  of  Schreinemakers  show  that  at  37.34%  HC1  the  barium  chloride 
dihydrate  is  converted  into  monohydrate. 

Less  than  i  part  of  BaCl2  is  soluble  in  20,000  parts  of  concentrated  HC1  and  in 
120,000  parts  of  cone.  HCl  containing  |  volume  of  ether.  (Mar,  1892.) 

SOLUBILITY  OF  BARIUM  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  MERCURIC 

CHLORIDE: 


HC1. 

BaCb. 

0 

97.84 

1.36 

24.02 

3-32 

19.20 

5-oi 

IS-2 

7-13 

II.  I 

10 

5-8 

13-43 

2.4 

16.92 

0.38 

20.62 

o 

32.18 

o 

At  O°.      (Schreinemakers,  1910.) 
Gms.  per  100  Gms.  Sat.  Sol. 


At  30°.      (Schreinemakers,  1910.) 


'    HgCl*. 

BaCh. 

0 

23.70 

14.25 

24 

36.20 

24.89 

46.08 

24.05 

46.59 

23.28 

47-78 

21.05 

48.46 

20.67 

44-33 

18.50 

29 

"•59 

16.36 

6.  ii 

3-95 

o 

Solid  Phase. 
BaClt.2HjO 


BaClt.3HgClj.6HjO 

"  +HgCl« 
HgClj 


SOLUBILITY  OF  MIXTURES  OF  BARIUM  CHLORIDE  AND  MERCURIC 
CHLORIDE  IN  WATER. 

(Foote  and  Bristol  — Am.  Ch.  J.  32,  248,  '04.) 


HgCh. 

BaCk. 

oouu  jriiase. 

O 

27.77 

BaClj.2HjO 

2.90 

27.56 

" 

12.98 

26.99 

« 

34-57 

26.69 

« 

46.50 

25.22 

" 

55-22 

23.17 

"  +HgCl« 

48.97 

17.87 

HgClj 

41-30 

14.26 

" 

27.62 

8.4I 

«i 

14.19 

2.65 

« 

7-67 

O 

" 

Gms.  per  100  Gms. 
t°.                  Solution. 

Solid 
Phase. 

BaCl2. 

Hgci2: 

10.4 

23-58 

50.54 

(  BaCl,2H,O+ 
I      HgCl,. 

10.4 
10-4 
10.4 

23-44 
22.58 
22.48 

50-74 
51-23 
51.41 

(  Double  Salt 

Gms.  per  100  Gms. 
t°.                 Solution. 

Solid 
Phase. 

BaCl2. 

HgCl2. 

10.4 

22.10 

51.66] 

[  Double  Salt 

IO-4 
25 

21.64 
23.02 

51-74. 
54.83 

(  BaCl,.2H,O+HgCl8. 

SOLUBILITY  OF  MIXTURES  OF  BARIUM  CHLORIDE  AND  SODIUM  CHLORIDE 

IN  WATER: 
At  30°. 

(Schreinemakers  and  de  Baat,  1908-09.) 


Gms.  per  100  Gms, 

Sat.  Sol. 

BaCh.  NaCl.  ' 

O  26.47 

2.28  25.28 

3.80  23.77 

5.76  20.25 

8.19  17.89 


Solid  Phase. 


Gms.  per  100  Gms. 
Sat.  Sol. 


NaCl 


'  +BaCU.2HiO 
BaCb.2HiO 


BaCk. 
12.25 
15-83 
20.93 
24.24 
27.60 


NaCl. 
13-39 
10.06 

5-39 
2.76 
o 


Solid  Phase. 


BaClZ.2H20 


At  Varying  Temps. 

(Precht  and  Wittgen,  1881 ; 
Rudorff,  1885.) 

Gms.  per  100  Gms' 
*o  Sat.  Sol. 


20 
40 
60 
80 
100 


BaCk. 
2-9 

4.5 

6.8 
9-4 
ii. 8 


NaCl. 

25 

23 

23-4 

22.8 

22.2 


in  BARIUM  CHLORIDE 

SOLUBILITY  OF  MIXTURES  OF  BARIUM  CHLORIDE  AND  POTASSIUM  CHLORIDE 
IN  WATER.     (Foote,  1904.) 

100  gms.  saturated  solution  contain  13.83  gms.  BaCl2  +  18.97  gms.  KC1  at  25°. 

Fusion-point  curves  (solubility,  see  footnote,  p.  i)  are  given  for  the  following 
mixtures: 


BaCl2 


+  BaCOs  (Sackur,  1911-12.) 

+  BaCrO4 

-j-  BaO  (Sackur,  1911-12,  Arndt,  1907.) 

-j-  BaSO4  (Sackur,  1911-12,  Ruff  and  Plato,  1903.) 

-j-  BaF2  (Botta,  1911;  Ruff  and  Plato,  1903;  Plato,  1907.) 

+  BaI2  (Ruff  and  Plato,  1903.) 

+  CdCl2  (Sandonini,  1911,  1914;  Ruff  and  Plato,  1903.) 

-j-  CaCl2  (Sandonini,  1911,  1914;  Ruff  and  Plato,  1903;  Schaefer,  1914.) 

-j-  CuCl2  (Sandonini,  1914-) 

-j-  PbCl2  (Sandonini,  1911,  1914;  Ruff  and  Plato,  1903.) 

-f-  LiCl  (Sandonini,  1913,  1914-) 

-|~  MgCl2  (Sandonini,  1912,  1914.) 

-j-  MnCl2  (Sandonini,  1912,  1914;  Ruff  and  Plato,  1903.) 

-f-  KC1  (Sandonini,  1911;  Ruff  and  Plato,  1903;  Vortisch,  1914.) 

+  NaCl  (Sackur,  1911-12;  Ruff andPlato,  1903;  LeChatelier,  1894;  Vortisch,  1914.) 

+  NaCl-f-KCl    (Vortisch,  1914 («);   Gemsky.) 

4*  SrCl2  (Sandonini,  1911,  1914;  Ruff  and  Plato,  1903;  Vortisch,  1914.) 

-j-  ZnCl2  (Sandonini,  1912  a,  1914.) 

-f  T1C1  (Korreng,  1914.) 


SOLUBILITY  OF 
At  15°. 

(Schiff,  1861; 
'Rohland,  1897.) 

Wt   £«    Gms.BaCk 
r  Tilr\u  Per  100  Gms. 
C2H{OH-     Solvent. 

10         31  -i 
20         21.9 
3°         H-7 

4O            IO.2 

60          3-5 
80          0.5 
97           0.014 

BARIUM 

Gms.  per 

Sat. 

CHLORIDE  IN  AQUEOUS  ETHYL  ALCOHOL  SOLUTIONS. 
At  30°.                                       At  60°. 

(Schreinemakers  and  Messink,  1910.) 

loo  Gms.                                    Gms.  per  100  Gms. 
Sol.                Solid  Phase.                  Sat.  Sol.                  Solid  Phase. 

C^OH. 
o 
32.67 
50.16 
60.72 
92-53 
94-73 
97-14 
98.17 
99.41 

BaCk. 

27  95 
10.63 
5-68 
2.23 
0.05 
0.06 

0.08 

BaCk.2H20 

"  +BaCk.H2O 
BaCk-HbO 
"  -f-BaCk 
BaCla 

C^OH. 
0 

16.68 
34.10 
66.02 

88.55 
90.25 

93-95 

BaCk.' 

31-57 
20.16 
13.21 
2.82 
0.25 
0.09 

BaCk.2HzO 

"  +BaCk.H20 
BaCk-HzO 

100  gms.  methyl  alcohol  dissolve  2.18  gms.  BaCl2  at  15.5°  and  7.3  gms.  BaCl2. 

2  H2O  at  6°.  (de  Bruyn,  1892.) 

loo  gms.  glycerol  dissolve  9.73  gms.  BaCl2  at  i5°-i6°.  (Ossendowski,  1907.) 

loo  cc.  anhydrous  hydrazine  dissolve  31  gms.  BaCl2  at  room  temp. 

(Welsh  and  Broderson,  1915.) 

100  gms.  95%  formic  acid  dissolve  7.3  gms.  BaCl2  at  19°.  (Aschan,  1913.) 

One  liter  sat.  sol.  in  nitrobenzene  contains  0.167  gm«  BaCl2  at  20°,  0.33  gm.  at 

50°  and  0.40  gm.  at  100°.  (Lloyd,  1918.) 

Data  for  the  system  BaCl2  +  Triethylamine  +  H2O  are  given  by  Timmermans 
(1907). 

SOLUBILITY  OF  MIXTURES  OF  BARIUM   CHLORIDE  AND  GLYCINE.  IN  WATER 

AT  2O°.      (Pfeiffer  and  Modelski,  1912.) 


Gms.  per  100  cc.  Sat.  Sol. 


Nft2CH2COOH. 

5-5 
26 


BaCk 
37 

16 


Solid  Phase. 

BaCU.  2H2O+BaCk.  2NH2CH2COOH.HjO 
NH4CHjCOOH+BaClj.2NH2CHjCOOH.HaO 


BARIUM  CHROMATE 


112 


BARIUM  CHROMATE   BaCrO4. 

SOLUBILITY  OF  BARIUM  CHROMATE  IN  WATER. 

One  liter  of  sat.  solution  contains  0.002  gm.  of  the  salt  at  o°;  0.0028  gm.  at 
10°;  0.0037  gm.  at  20°  and  0.0046  gm.  at  30°.  (Kohkausch,  1908.) 

Results  higher  than  the  above  are  given  by  Schweitzer,  1890,  as  follows: 
One  liter  of  aqueous  solution  saturated  at  room  temp,  contains  o.oi  gm.  BaCrO4; 
if  ignited  barium  chromate  is  used,  only  0.0062  gm.  dissolves. 

One  liter  sat.  sol.  contains  0.043  Sm-  °f  the  salt  at  boiling  point.      (Mescherzski,  1882.) 

Fresenius  (1890)  gives  the  following:  i  liter  of  sat.  sol.  at  room  temp,  con- 
tains 0.02  gm.  of  the  salt,  the  solvent  being  1.5%  sol.  of  CH3CO2NH4  and  0.022 
gms.  when  the  solvent  is  0.5%  sol.  of  NH4NO3. 

One  liter  of  45%  aq.  ethyl  alcohol  solution  dissolves  0.000022  gm.  at  room  temp. 
BARIUM  CINNAMATES.  (Guenm,  I9i2.) 

SOLUBILITY  OF  BARIUM  CINNAMATES  IN  WATER,  METHYL" ALCOHOL  AND  ACETONE. 

Gms.  Anhy- 

Authority. 

o.  726  (Tarugi  and  Checchi,  1901.) 

(Liebermann,i903.) 
(Michael  and  Garner,  1903.) 
(Michael,  1901.) 


(Michael  and  Garner,  1503.) 
(Michael,  1901.) 


Compound. 

Formula.           t°. 

Solvent. 

arous  o 
Der  ioo  G 

Sat.  Sc 

Barium  Cinnamate 

Ba(C9H702)2.2H20     15 

HjO 

0.72* 

u 

" 

"                    IOO 

" 

2.27 

" 

Allocinnamate 

Ba(C9H7O2)2.H2O      19 

CHsOH 

15.8 

" 

u 

12 

" 

I5-4 

" 

" 

Ba(C»H7O2)j3HjO     20 

" 

2.56 

II 

" 

"                   2O 

(CH3)zCO 

0.80 

" 

" 

"                   2O 

HzO 

6 

" 

Hydrocinnamate 

Ba(C9H70J)2.2HiO     27 

" 

2.9 

" 

« 

25 

CHsOH 

O.I 

" 

" 

16 

" 

9-7 

" 

Isocinnamate 

20 

* 

70 

" 

" 

20 

(CHs)2CO 

20 

u 

" 

20 

HjO 

17 

BARIUM 


CITRATE     Ba3(C6H6O7)2.7H2O. 

SOLUBILITY  IN  WATER  AND  IN  ALCOHOL. 

ioo  grams  water  dissolve  0.0406  gram  Ba3(C6H6O7)2.7H2O  at  18°, 
and  0.0572  gm.  at  25°. 

ioo  grams  95%  alcohol  dissolve  0.0044  gram  Ba3(C6H6O7)2.7H2O  at 
18°,  and  0.0058  gm.  at  25°. 

(Partheil  and  Hiibner  —  Archiv.  Pharm.  241,  413,  '03.) 

BARIUM    CYANIDE     Ba(CN)2. 

SOLUBILITY  IN  WATER  AND  IN  ALCOHOL  AT  14°. 

(Joannis  —  Ann.  chim.  phys.  [5]  26,  489,  '82.) 

ioo  parts  water  dissolve  80  parts  Ba(CN)2. 

ioo  parts  70%  alcohol  dissolve  18  parts  Ba(CN)2. 

BARIUM  FERROOYANIDE  AND  BARIUM  POTASSIUM  FERRO- 

CYANIDE. 

(Wyrouboff  —  Ann.  chim.  phys.  [4]  16,  292,  '69.) 

ioo  parts  water  dissolve  o.i  part  Ba3Fe(CN)6.6H2O  at  15°,  and  i.o 
part  at  75°. 

ioo  parts  water  dissolve  0.33  part  BaK2Fe(CN)0.5H2O  at  ord.  temp. 

BARIUM  FLUORIDE   BaF2. 

SOLUBILITY  IN  WATER. 

»  (Kohkausch,  1908.) 

One  liter  sat.  sol.  contains  1.586  gms.  of  the  salt  at  10°;  1.597  gms.  at  15°; 
1.607  g1115-  at  2°°j  1-614  gms«  at  25°  and  1.620  gms.  at  30°. 

Freezing-point  curves  are  given  for  mixtures  of  BaFz+KF  by  Puschin  and 
Baskow  (1913),  and  for  BaF2-J-BaIj  by  Ruff  and  Plato  (1903). 


BARIUM  FORMATE 


BARIUM  FORMATE   Ba(HCOO)2. 

SOLUBILITY  IN  WATER.      (Stanley,  1904.    See  also  Krasnicki,  1887.) 

Gms.  Ba(HCOO)j  to 

2r  too  Gms.  Sat.  Sol. 


per 


Gms.  Ba(HCOO)« 
per  zoo  Gms.  Sat.  SoL 


23.24 
23.22 


O 
10 

20  23.0< 

25  23.9 

30  24.2 

BARIUM  HYDROXIDE  Ba(OH)2.8H2O. 

SOLUBILITY  IN  WATER.     SOLID  PHASE  Ba(OH)2.8H2O. 


40 
So 
60 
80 
100 


25 

25-9 

26.9 

29-3 
32.8 


(Rosenthiel  and  Riihlmanu '—  Jahresber.  Chem.  314,  '70.) 


Gms.  Ba(OH)z  per  100  Gms. 


Gms.  Ba(OH)2  per  100  Gms. 


Water. 

Solution 

0 

1.67 

I  .  6C 

5 

I  .95 

I  •  02 

10 

2.48 

,  2  .42 

15 

3-23 

3-13 

20 

3-89 

3-74 

25 

4-68 

4-47 

Water. 

Solution. 

30 

5-59 

5  -29 

40 

8.22 

7.60 

50 

13.12 

ii  .61 

00 

20-94 

17.32 

75 

63-51 

38.85 

80 

101  .40 

50-35 

Data  are  given  by  Sill  (1916),  for  the  influence  of  pressures  up  to  490  kgs.  per 
sq.  cm.  on  the  solubility  of  Ba(OH)2.8H2O  in  H2O  at  25°. 


Sat.  Sol. 
.0512 
.0651 
.0790 

•0975 
.1220 


SOLUBILITY  OF  BARIUM  HYDROXIDE  IN  AQUEOUS  SOLUTIONS  OF  BARIUM 
NITRATE  AT  25°  AND  VICE  VERSA.    (Parsons  and  Carson,  1910.) 

Sp.  Gr.  Gms.  per  100  Gms.  H2O.       Solid  Sp.  Gr. 

Ba(OH)2.  Ba(NO3)2.        Phase-  Sat-  So1- 

4.29      O  Ba(OH)j.8H2O     I.I37I 

4.35     1.88          "  1.1448 

4.48      3.47  "  I.I2IO 

4.40      5-66  "  I.IOO2 

4-72    7-55          "  1-0797 


Ba(OH)2.Ba(NO3)2. 
4.93  10.21 
5.02  11.48 

Phase. 
Ba(OH)2.8H2O 
"  +Ba(N03)a 

3-22  11.04 

1.55  10.66 

Ba(N03)8 

o  10.30 

« 

SOLUBILITY  OF  BARIUM  HYDROXIDE  IN  AQUEOUS  SOLUTIONS  OF  ALKALI 
CHLORIDES  AT  25°.    (Herz,  1910.) 


In  Lithium 
Chloride. 
Gms.  per  100  cc.  Sat.  Sol. 

In  Potassium 
Chloride. 

Gms.  per  100  cc.  Sat.  Sol. 

In  Rubidium 
Chloride. 

Gms.  per  loqcc.  Sat.  Sol. 

In  Sodium 
Chloride. 

Gms.  per  loocc.  Sat.  Sol. 

Lid. 

9-75 
6.  02 

3-i8 
o 

Ba(OH)2.  " 

n-45 

8.03 

6-39 
4.76 

KC1. 
25-95 
I3-05 
8.60 
0 

Ba(OH)2. 

5-93 
5-66 

5-53 
4.76 

'  RbCl. 
15.11 
0 

Ba(OH)2. 

5-55 

4.76 

NaCl. 
16.51 

8-37 
4-27 
0 

Ba(OH)i". 
6.91 

5-99 
5-40 
4.76 

SOLUBILITY  OF  BARIUM  HYDROXIDE  IN  AQUEOUS  SOLUTIONS  OF  SODIUM 

>      HYDROXIDE  AT  30°.      (Schreinemakers,  1909-10.) 


Gms.  per  100  Gms.  Sat.  Sol. 


BaO. 

NacO. 

4-99 

O 

1.29 

4.78 

0.89 

6-43 

0-57 

9.63 

0-53 

11.62 

0.47 

17.87 

1.  06 

23.28 

1.87 

24.63 

Solid  Phase. 


Gms.  per  100  Gms.  Sat.  Sol. 


Ba0.9H20+Ba0.4HjO 


BaO. 

NazO.  ' 

ouuu  riiitsc. 

1.84 

26.14 

BaO.4H2O 

i-75 

27.72 

" 

1.58 

28.43 

" 

i-34 

29.24 

"  +Ba0.2H20 

0.82 

32.12 

BaO.2H2O 

0-59 

34.72 

" 

o-57 

41.09 

"  +NaOH.H«O 

0 

+42 

NaOH.HiO 

BARIUM  HYDROXIDE  114 

SOLUBILITY  OF  BARIUM  HYDROXIDE  IN  AQUEOUS  ACETONE  AT  25°. 

(Herz  and  Knoch  —  Z.  anorg.  Chem.  41,  321,  '04.) 

r       t  v  i  of      Ba(OH)2  per  100  cc.  Sat.  Gms.  Ba(OH)2 

Sp.  Gr.  of  Vol.%  Solution.  per 

Solutions.  Acetone.    , — — • .  xoo  Gms. 

Millimols.  Grams.  Solution. 

1.0479  o  55.08  4.722  4.506 

i. 0168  10  31-84  2.730  2.686 

0.9927  20  17.79  i-S2S  I-536 

0.9763  30  9.10  0.779  0.798 

0.9561  40  4.75  0.407  0.426 

0.9398  50  1.54  0.132  0.141 

0.9179  60  0.48  0.041  0.045 

0.8956  70  0.08  0.007  0.018 

Data  for  the  systems  Ba(OH)2  +  Phenol  +  H2O  at  25°  and  Ba(OH)2  + 
Resorcinol  +  H2O  at  30°  are  given  by  van  Meurs  (1916). 

BARIUM  IODATE   Ba(IO3)2.H2O. 

SOLUBILITY  IN  WATER. 

(Trautz  and  Anschutz,  1906.) 

to          Gms.  Ba(IO3)2  per  „        Gms.  Ba(IO3)  per  ±0       Gms.  Ba(I03)2  per 

100  Gms.  Solution.  100  Gms.  Solution.  100  Gms.  Solution, 

-  0.046     O.OOS         30       0.031          70       0-093 

+  io      0.014      40     0.041       80     0.115 

2O         O-O22          5O       0.056  9O       O.I4I 

25  0-028  60  0.074  100  o>197 

One  liter  sat.  aqueous  solution  contains  0.3845  gm.  Ba(IO3)2  at  25°. 

(Harkins  and  Winninghoff,  1911.) 

At  room  temperature  Hill  and  Zink  (1909),  found  0.284  gm.  Ba(IOs)2  per  liter 
sat.  aqueous  solution. 

SOLUBILITY  OF  BARIUM  IODATE  IN  AQUEOUS  SALT  SOLUTIONS  AT  25°. 

(Harkins  and  Winninghoff,  1911.) 

Added    Mols.  Salt 
Salt.       per  Liter. 

Ba(NOs)2  o .  ooi 
0.002 

"     0.005 

"      O.O2O 

"          o . 050 
loo  cc.  cone,  ammonia  (Sp.  Gr.  0.90)  dissolve  0.0199  gm.  Ba(IOs)2  at  room 

temp.  (Hill  and  Zink,  1909.) 

100  cc.  95%  ethyl  alcohol  dissolve  o.oon  gm.  Ba(IO3)2  at  room  temp. 

(Hill  and  Zink,  1909.) 

BARIUM    IODIDE     BaI2. 

SOLUBILITY  IN  WATER. 

(Kremers  —  Pogg.  Ann.  103,  66,  1858;  Etard  —  Ann.  chim.  phys.  [7]  2,  544,  '94.) 
Gms-BaI2RerzooGms.  ^  Gms ,.BaI2  per  xooGms. 

Water.     Solution.  Water.      Solution. 

-20  143-9  59-0  BaI2.6H.5O          40  231.9  69.8    BaI2.2  H2O 

o  170.2  63.0  60  247.3  71-2 

+  10  185.7  65.0  80  261.0  72.3 

20  203.1  67.0  100  271.7  73.1 

25  212.5  68.0  "                120  281.7  73.8             " 

30  219.6  68.7  160  294.8  74.6             " 

Sp.  Gr.  of  sat.  solution  at  I9°.5  =  2.24. 

100  gms.  95%  HCOOH  dissolve  75  gms.  BaI2  at  20.2°.  (Aschan,  1913.) 

100  gms.  97%  ethyl  alcohol  dissolve  1.07  gms.  BaI2.2H2O  at  15°.  (Rohland,  1897.) 
Data  for  the  system  BaI2+BaO+H2O  at  25°  are  given  by  Milikau  (1916). 


Gms. 
Ba(IO3)2 
per  Liter. 

Added 
'   Salt. 

Mols.  Salt 
per  Liter. 

Gms. 
Ba(I03)2 
per  Liter. 

Added 
Salt. 

Mols.  Salt 
per  Liter. 

Gms.' 
Ba(I03)j 
per  Liter.  , 

0-331 

Ba(NO3)2 

O.IOO 

o.  148 

KNO3 

O.2OO 

0.777 

0.294 

" 

0.200 

0.136 

KIO3 

O.OOOIO6 

0.368 

0.237 

KNO3 

O.OO2 

0.396 

" 

0.000530 

0.303 

o.  164 

" 

O.OIO 

0-445 

" 

o.  001061 

0.229 

0.149 

" 

0.050 

0.643 

115  BARIUM  PerlODIDE 

BARIUM  PerlODIDE   BaI4. 

Data  for  the  formation  of  barium  periodide  in  aqueous  solutions  at  25°  are 
given  by  Herz  and  Bulla  (1911).  (See  reference  calcium  perbromide,  p.  186.) 

BARIUM  IODOMERCURATE. 

A  saturated  solution  of  BaI2  and  HgI2  in  water  at  23.5°  was  found  by  Duboin 
(1906)  to  have  the  composition  BaI2.i.33HgI2.7.76H2O,  d  =  2.76. 

BARIUM    MALATE     BaC4H4Os. 

SOLUBILITY  IN  WATER. 

(Cantoni  and  Basadonna  —  Bull.  soc.  chim.  [3]  35,  731,  '06.) 

to      Gms.BaC4H4O5  to       Gms.  BaC4H4O5  to      Cms.  BaC4H4O8 

per  100  cc.  Sol.  per  100  cc.  Sol.  per  100  cc.  Sol. 

20          0.883  35        0.895  60         i.  on 

25      0.90!          40     0.896          70      I.04I 
30      0.903          50     0.942          80      1.044 

SOLUBILITY  IN  WATER  AND  IN  ALCOHOL. 

(Rartheil  and  Hiibner  —  Archiv.  Pharm.  241,  413,. '03.) 

ioo  grams  water  dissolve  1.24  gms.  BaC4H4O6  at  18°,  and  1.3631 
gms.  at  25°. 

too  grams  95%  alcohol  dissolve  0.0038  gms.  BaC4H4O6  at  18°,  and 
0.0039  gm.  at  25°. 

BARIUM  MALONATE  BaC3H2O4.2H2O. 

SOLUBILITY  IN  WATER. 

(Miczynski  —  Monatsh.  Chem.  7,  263,  '86.) 

Gms .  BaC3H2O4  per  ioo  Gms.  A  „        Gms.  BaC3H2O4  per  too  Gms. 

t   . 

O 
10 
2O 
30 

40 

Results  slightly  higher  than  the  above,  from  o°-5O°  are  given  by  Cantoni  and 
Diotalevi  (1905). 

BARIUM  MOLYBDATE   BaMoO4. 

ioo  parts  water  dissolve  0.0058  part  BaMoC>4  at  23°.      (Smith  and  Bradbury,  1891.) 


Water. 

Solution. 

»       * 

Water. 

Solution. 

0-143 

0.143 

50 

0.287 

0.285 

0.179 

0.179 

60 

0.304 

0.303 

0-212 

0-2II 

70 

0.317 

0.316 

0.241 

0.240 

80 

0.326 

0-325 

0.266 

0.265 

IARIUM    NITRATE     Ba(NO3)2. 
SOLUBILITY 

IN  WATER. 

(Mulder;  Gay  Lussac;  Etard  —  Ann.  chim.  phys.ty]  2,  528,  94;  Euler  —  Z.  physik.  Chem.  49,  3i5.'o4-> 

Gms.  Ba(NO3)2 
t°.                   per  ioo  Gms. 

80 

IOO 
120 

Gms.  Ba(NO3)2 
per  ioo  Gms. 

Water.           Solution. 

o          5.0          4.8 
10          7.0          6.5 

20              9-2              8.4 

Water.          Solution. 
27.0            21-3 

•    34-2         25.5 
42.0        29.6 

25        10.4          9-4 
30        ii.  6        10.6 
40        14.2        12.4 
50        17.1         14.6 
60        20.3        16.9 

140 

160 
180 

200 
215 

5o-o        33-3 
58.0        36.7 
67.0        40.1 
76.0        43.2 
84.5        45.8 

Results  from  o°-35°  differing  from  the  above  are  given  by  Vogel  (1903). 

ioo  gms.  sat.  aqueous  solution  contains 4.74  gms.  Ba(NO3)2ato°.     (Coppadoro.ign.) 


BARIUM  NITRATE 


116 


SOLUBILITY  OF  MIXTURES  OF  BARIUM  NITRATE  AND  LEAD  NITRATE  IN  WATER 

AT  25°.     (Fock,  1897;  Euler,  1904.) 
In  Solution. 


>p.  W.  01 

Solution. 

Cms. 

per  Liter. 

Mg.  Mols. 

per  Liter. 

Mol.  % 

Mol.% 

T>  _/"VTr\  A 

Ba(N03)2. 

Pb(N03)2." 

Ba(NO3)2. 

Pb(N03)2" 

Ba(NO3)2. 

*>a^iN  Usja 

1.079 

102.2 

O 

391.0 

0 

100 

100 

I  .088 

54-9 

17.63 

2IO.I 

53-3 

79.78 

98.30 

I.loS 

86.5 

49-80 

330-7 

J50-7 

68.70 

96.74 

I  .Up 

79-7 

68.10 

304-9 

205-7 

59-69 

94-So 

I.I40 

77.0 

97.20 

294.4 

293.6 

50-09 

93.62 

1.163 

69.8 

130.7 

266.8 

395-o 

40.31 

92-49 

1.198 

66.0 

177-3 

252-5 

535  -6 

32.03 

90.07 

1.252 

57-5 

247-7 

222  .6 

748.5 

22.91 

83-47 

1.294 

25-9 

334-3 

99-2 

1010.3 

8.  ii 

75-44 

1.376 

28.8 

429.7 

110.3 

1298.0 

.  7-77 

35-n 

1.  4*9 

553-* 

o.o 

1673.0 

o.o 

o.o 

Tables  of  results  are  also  given  for  15°,  30°,  and  47°. 
SOLUBILITY  OF  MIXTURES  OF  BARIUM  NITRATE  AND  POTASSIUM  NITRATE  IN  WATER. 

(Findlay,  Morgan  and  Morris,  1914;  Foote,  1904.) 


Gms.  per  100  Gms.  Sat.  Sol.  '      Solid 


Ba(NO3)2. 
6.62 

5-49 
3-04 
2.04 

n-39 
8.18 
8.08 
8.42 

5-85 
5.02 

3-02 

1.77 

O 
24.77  b  *  Results  by  Foote. 

a  =  Ba(NO3)2,        2b.a  =  2KN03.Ba(NO3)2,        b  =  KNO3. 
SOLUBILITY  OF  MIXTURES  OF  BARIUM  NITRATE  AND  SODIUM  NITRATE  IN  WATER. 

(Coppadoro,  at  o°,  1912;  at  30°,  1913.) 

Results  at  o°.  Results  at  30°. 


Ba(NOs)2. 

KNOs.     Phase. 

9.1    6 

•25 

0 

a 

9.1    4 

.20 

8 

•15 

0+26.0 

9- 

I 

.98 

12 

.02 

26.0 

9- 

0 

.98 

16 

.80 

6+26.0 

9- 

0 

16 

.76 

6 

21. 

8 

.46 

o 

a 

21. 

7 

•47 

2 

.12 

" 

21.  1     6 

•35 

5 

.98 

« 

21.  1     6 

.06 

8 

•47 

" 

2i.  i   5 

.98 

13 

.24 

0+26.0 

21.  i    3 

.35 

18 

.24 

26.0 

21.  1     2 

-30 

21 

•47 

" 

21.  1     I 

.76 

24 

.86 

6+26.0 

t°. 

25* 

25 

25 

25 

35 

35 

35 

35 

35 

35 

35 

35 

35 


Gms.  per  100  Gms.  Sat.  Sol. 


KN03. 
14-89 
16.30 
21.99 
27.76 

O 

12.99 
17.48 
19-75 
24 
26.05 

34.87 
34.98 

35-01 


Solid 
Phase. 


0+26.0 

zb.a 
« 

6+26.0 


0+26.0 

26.0 
6+26.0 

6 


21. I 


Gms.  per  loo^Gms.  Sat.  Sol. 
Ba(NO3)2.         NaNCb. 

33 


Solid  Phase. 
Ba(NO3)2 


4.33  0.41 

3.34  1.68 
2-50          3-54 

I. 60  8.02  " 

1.56  12.71  « 

1.53  20.24 

1.56  27.74 

i-55  30.81 

1.49  35.83 

1.55  40.85    98    %Ba(NOs)2+    2    %NaNO3 

1.55  41.3°    26    %        "       +  73-8%      " 

1.54  42.06      2.6%        "       +97-4%      " 

0.51,  41.68      o    %        "       +ioo    %      " 


Gms.  per  100  Gms.  Sat.  Sol 

Solid  Phase. 

Ba(NOs)2. 

NaNOs. 

10-33 

0 

Ba(NOs). 

8.58 

2-33 

" 

5-28 

7.09 

• 

3.89 

12.07 

• 

3-54 

14.41 

" 

3.20 

17.87 

H 

3-07 

19.06 

ii 

2.81 

23-55 

" 

2.27 

41  .22 

" 

2.  II 

48.22 

Ba(N03)2+  NaNOs 

I 

48.50 

NaNOs 

9 

49.16 

" 

117  BARIUM  NITRATE 

SOLUBILITY  OF  BARIUM  NITRATE  IN  AQUEOUS  SOLUTIONS  OF  NITRIC  ACID  AT  30°. 

(Masson,  1911.) 

Cms,  per  100  cc.  Sat.  Sol.  Gms.  per  100  cc.  Sat.  Sol. 

P          '  HNOa.     Ba(NOs)2.  HNO3.      Ba(NO»)"t. 


1.0891     o  54-31 

1.0811     8.303  30.50 

15.72  27.73 

1.0663      31.49  22-76 

1.0619     47 .18  19 .71 

1.0609      63  17-84 


•0633          78.54  16.66 

.0668         98.40  15.88 

.0783  125.9  14.99 

.1050  188.6  14.11 

.1341  251.6  13.75 

•1645  315.7  13.52 


Fusion-point  curves  (solubility,  see  footnote,  p.  i)  are  given  by  Harkins  and 
Clarke,  1915,  for  the  following  mixtures: 

Ba(N03)2  +  NaN03  +  KNO3,     Ba(NO3)2  +  NaNO3,     Ba(NO3)2'+  KNO3, 
Ba(N03)2  +  LiN03,  Ba(NO3)2  +  LiNO3  +  KNO3. 

SOLUBILITY  OF  BARIUM  NITRATE  IN  AQUEOUS  SOLUTIONS  OF  ETHYL  ALCOHOL  AT  25°. 

(D'Ans  and  Siegler,  1913.) 

Gms.  C2H6OH        Gms.  per  100  Gms.  Sat.  Sol.  Gms.  CtHsOH         Gms.  per  100  Gms.  Sat.  Sol. 

^SS^ST  'OaOH.      "    BatNOa),:  ^sS^T  ckoH.       *    Ba(NO3)Z. 

o  o  9.55  58  57  1.85 

10.25  9.5  7.63  78.7  78.2  0.62 

18.6  17.5  6.02  90.1  89.9  0.18 

25-05  23.7  5.25  99.4  99.39  0.005 

40.2  38.3  3.53 

Data  are  also  given  by  Vogel  (1903),  but'as  the  results  are  given  in  gms.  per  100 
cc.  and  densities  are  omitted,  no  exact  comparison  can  be  made  with  the  above. 

SOLUBILITY  OF   BARIUM  NITRATE  IN  AQUEOUS  PHENOL  SOLUTIONS 

AT  25°. 

(Rothmund  and  Wilsmore  —  Z.  phyisk.  Chem.  40,  620,  'oa.) 


G.  Mols.  per  Liter. 

Gms.  per  Liter. 

G.  Mols.  per  Liter. 

Gms.  j>er  Liter. 

CflHfiOH    Ba(N03)2. 

o.ooo    0.3835 
0.045    °-3785 

0-082      0.3746 
0.146      0.3664 

QHsOH.  Ba(NO3)2. 
0.0         100.2 
4.23         98.97 

7-7i      97-95 
13-73      95  -81 

C6H6OH.  Ba(N08)2. 
0.310  0.3492 
O-4OI  0.3400 
0.501  0.3299 

0.728  (sat.)  0.3098 

CoHcOH.  Ba(NO3)a. 
29.12      91.31 

37-73    88.90 
47.11    86.26 
68.45    81.00 

Data  for  the  above  system  are  also  given  by  Timmermans  (1907). 

100  gms.  hydroxylamine  dissolve  1  1.4  gms.  Ba(NO3)2  at  i7°-i8°.    (de  Bruyn,  1892.) 

100  cc.  anhydrous  hydrazine  dissolve  3  gms.  Ba(NO3)2  at  room  temp. 

(Welsh  and  Brodersen,  1915.) 

100  gms.  methyl  alcohol  dissolve  0.5  gm.  Ba  (NO3)2  at  25°.      (D'Ans  and^Siegler.  1913.) 
100  gms.  acetone  dissolve  0.005  Sm-  Ba(NO3)2  at  25°. 

BARIUM  NITRITE  Ba(NO2)2.H2O. 

SOLUBILITY  IN  WATER. 

(Oswald,  1914;  see  also,  Vogel,  1903-) 
t°.  Gms.  Ba(N02)2  ^  ...  Gms. 


—  1-7                    9-2  Ice  20  40.3         Ba(NOi)j.HiO 

-  3-2  19-5  "  43  50-3 

-  5.8  33.1  ••  61  58-6 

—  6.5  34.5  "  +Ba(NOl)i.H20  80  67.3 

—  4.3  34.9            Ba(NOJ)».HlO  92  71.7 

+  17  40*                 •*  no  82 

*  d  of  the  sat.  solution  =  1.4897. 


BARIUM  NITRITE 


118 


SOLUBILITY  OF  MIXTURES  OF  BARIUM  NITRITE  AND  SILVER  NITRITE  IN 
WATER  AT  13.5°.    (Oswald,  1914.) 

Cms.  per  100  Gms.  HjO. 
Ba(NO,),.        ' AiNO?.  S°Ud  Phase" 

64  10.2  AgN02+BaAg2(N02)4.H2O 

75-6  9-5  Ba(N02)2+BaAg2(N02)4.H20 

SOLUBILITY  OF  BARIUM  NITRITE  IN  AQUEOUS  ALCOHOL  SOLUTIONS  AT 

I9.5°-20.5°.      (Vogel,  1903.) 

%  alcohol  in  solvent:  10   20   30   40   50  60   70   80 

184    13.3    9.1    4.8     2.7    0.98 


Gms.  Ba(N02)2.H20  j 
per  100  cc.  sat.  soli49'3    29*3 
BaC2O4. 


90 
o 


BARIUM  OXALATE 

SOLUBILITY  OP  THE  THREE  HYDRATES  IN  WATER. 

(Groschuff —  Ber.  34,  3318,  '01.) 


BaC2043*H20. 


BaC2O4.2H2O. 


BaC2O4.}H2O. 


t°.   Gms.BaC2O4  G.M.BaC2O4 
per             per  100  Mol. 

Gms.  BaC2O4 
per 

G.  M.  BaC2O4 
per  100  G.  M. 

Gms.BaC2O4 
per 

G.  M.  BaC204" 
per  loo  Mol. 

1000  g.  Sol. 

H20. 

looo  g.  SoL 

H2O. 

looo  g.  Sol. 

H20. 

O 

0.058 

O.OOO46 

0-053 

O.OOO42 

0.089 

O.OOO7O 

9-5 

0.082 

O.OOO66 

.  .  . 

18 

O.II2 

0.00090 

0-089 

O.OOO7I 

O.I24 

0.00099 

3° 

0.170 

O.OCI36 

O-I2I 

0.00097 

0.140 

0-OOII2 

40 

O.I52 

O.OOI22 

O.I5I 

O.OOI2I 

45 

0-169 

0.00135 

50 

... 

... 

0.164 

O.OOI3I 

55 

... 

O.2I2 

0.00170 

00 

0-175 

0.00140 

65 

... 

o  250 

O.OO2OO 

73 

... 

0.285 

0.00228 

75 

... 

... 

0.188 

O.OOI5I 

90 

... 

... 

... 

... 

0.200 

0.00100 

100 

... 

•  *. 

•  .. 

*  ... 

O.2II 

o  00169 

The  following  additional  data  for  the  solubility  of  the  above  three  hydrates  in 
water  are  given  by  (Kohlrausch,  1908).  i 


BaC2O4.2H20. 


BaCi-CMHzO. 


'   t» 

Gms.  per  Liter. 

*  t°. 

Gms.  per  Liter. 

'     t°. 

Gms.  per  Liter. 

2.07 

0.0553 

3 

0.0519 

0.08 

0.0499 

4.2 

0.059 

5-47 

0.0575 

2.46 

0-053 

16.1 

0.0962 

11.28 

0.0693 

9.62 

0.0619 

17.8 

0.1047 

17.9 

0.085 

15.04 

0.0699 

23-3 

0.0987 

17-54 

0.0751 

28.4 

O.II24 

27.02 

0.091 

33-73 

O.IOlS 

Cantoni  and  Diotalevi  (1905)  obtained  higher  results  than  either  of  the  above. 
SOLUBILITIES  OF  BARIUM  OXALATE  (BaCzO4.iH2O)  IN  AQUEOUS  ACETIC  ACID  AT 

26°-27°.      (Herz  and  Muhs,  1903.) 


Normality    G.  Residue*  Gms.  per  IOQCC.  Solution.    Normality 


of  Acetic 
Acid. 

per  50.  05  cc. 

CH3COOH 

Ba 
*  Oxalate. 

of  Acetic 
Acid. 

0 

0.0077 

O 

.00 

0 

.0154 

3-85 

O 

•565 

0.0423 

3 

•39 

0 

.0845 

5-79 

I 

.425 

o  0520 

8 

•55 

0 

.1039 

I7-30 

2 

•8S 

0.0556 

17 

.11 

0 

.1111 

,            •  Dried  at  70°. 

G.  Residue*  Gms.  per  100  cc.  Solution 

^Sof."'  CH3COOH.    BaOxalate 

0.0564  23.12    O.II27 

0.05II  34-76 

0.0048  103.90 


O    1021 

o  0096 


119  BARIUM   OXALATE 


BARIUM    AOID    OXALATE     BaC2O4.H2C2O4.2H2O. 
SOLUBILITY  IN  WATER. 

(Groschuff.) 


f.    ' 

jms.per  K 

x>  Gms.  Solution.         Mols.  per  too  Mols.  H2O. 

Mols.  HaCtO* 
per  i  Mol.BaC2O4. 

HjC2O4 

iC_O4. 

H2C204. 

BaC204. 

o 

0.27 

O 

.030 

0.054 

0.0024 

22 

18 

0.66 

O 

.070 

0.130 

0.0056 

24 

20.5 

0.76 

0 

.076 

0.15 

0.0061 

25 

38 

1.61 

0.16 

o-33 

0.013 

25 

4i 

1.82 

o 

.18 

o-37 

0.015 

25 

53 

2.92 

0 

•31 

0.60 

0.026 

24 

60 

3.60 

o 

.40 

0-75 

0-033 

22. 

5 

80 

6.21 

o 

.81 

i-34 

0.070 

J9 

90 

7.96 

I 

.11 

0.098 

18 

99 

10.50 

1 

•55 

2-39 

0.141 

17 

BARIUM   OXIDES. 

Data  for  the  lowering 
mixtures  of  BaO  and  B2( 

r  of  the  fusion 
33  are  given  by 

points  (solubility,  see  footnote,  p.  i),  of 
Guertler  (1904).     Results  for  mixtures  of 

BaO  and 

CaCl2 

and  for 

BaO  and  SrCl2 

are  given 

by  Sackur  (1911-12). 

BARIUM  Glycerol  PHOSPHATES. 

SOLUBILITY  IN  WATER. 

Gms.  Anhy- 
t°.  Compound.  Formula.       drous  Salt  per  Authority. 

loo  Gms.  Sat.  Sol. 

21     Barium  Glycerolphosphate       BaCsHrOsP.HzO         4.5        (Rogier  and  Fiore,  1913.) 
13  "       a  Glycerolphosphate         BaCsHrOsP  1.4        (King  and  Pyman,  1914.) 

12  ft  BaCaHvOsP.IHzO        5.8  "  "     "      . 

21  Glycerolphosphate       BaCaHeOeP.^HzO        8.4        (Langheld  and  Oppmann,  1912.) 

22  "      di  Glycerolphosphate  ____  3.76 

BARIUM  PICRATE.     Solubility  in  H2O  +  C2H6OH  at  25°.  (Fischer,  1914.) 

BARIUM    PROPIONATE     Ba(C3H5O2)2.H2O,  also  6H2O. 
SOLUBILITY  IN  WATER. 

(Krasnicki  —  Monatsh.  Chem.  8,  597,  '87.) 


Gms.  Ba(C3H5O2)2  Gms.  Ba(C3HfiO2)2 

t».  per  IPO  Gms.  $°.  per  100  Gms. 

Water.  Solution.  Water.  Solution. 

o        47  -98        32-4i  5°          62  -74          38-57 

10        51-56        34-02  60          64.76          39  .31 

20        54-82        35.42  70          66.46          39.93 

3o        57-77        36-65  80          67.85          40.42 

40        60.41        37-66  ..  ...  ••• 

100  cc.  95%  ethyl  alcohol  dissolve  0.1631  gm.  barium  propionate  at  room  temp. 

(Crowell,  1918  ) 

BARIUM  SALICYLATE   Ba(C6H4OHCOO)2.H2O. 

100  gms.  sat.  aqueous  solution  contain  28.65  g1115-  anhydrous  salt  at  15°  and 
54.08  gms.  at  I  OO°.  (Tarugi  and  Checchi,  1901.) 

BARIUM  DinitroSALICYLATE.     Solubility  in  H2O  +  C2H6OH  at  25°. 

(Fischer,  1914.) 
BARIUM  SILICATE   BaSiO3. 

Fusion-point  curves  (solubility,  see  footnote,  p.  i)  for  mixtures  of: 
BaSiO3+CaSiO3  and  BaSiO3-fMnSiO3  are  given  by  (Lebedeu,  1911). 
BaSiO3+Li2SiO3  and  BaSiO3+Na2SiO3  are  given  by  Wallace,  1909. 
BaSiO3-j-BaTiOj  are  given  by  Smolensky  (1911-12). 


BARIUM   STEARATE  120 

BARIUM   STEARATE  and  Salts  of  Other  Fatty  Acids. 

SOLUBILITY  OF  BARIUM  STEARATE,  PALMITATE,  MYRISTATE  AND  LAURATE 

IN  SEVERAL  SOLVENTS.      (Jacobson  and  Holmes,  1916.) 
Solvent.  t°.       Cms.  Each  Salt  (Determined  Separately)  per  100  Cms.  Solvent. 

Ba  Stearate.     Ba  Palmitate.  Ba  Myristate.    Ba  Laurate. 

Water  15.3  0.004  0.004  0.007  0.008 

"  50  0.006  0.007  o.oio  o.on 

Abs.  Ethyl  Alcohol  16.5  0.006  0.009  0.009  o.oio 

50  0.003  0.004  0.004  0.007 

Methyl  Alcohol  15  o .  042  o .  045  o .  05  7  o .  084 

"            "  50.5  0.077  0.088  0.108  0.163 

Ether  25  o.ooi  o.ooi  0.003  0.007 

Amyl  Alcohol  25  0.007  0.008  0.009  0.009 

BARIUM    SUCCINATE  AND  BARIUM  ISO  SUCCINATE 

Ba.CH2CH2(COO)2.  Ba.CH3CH2(COO)3. 

SOLUBILITY  OF  EACH  IN  WATER. 

(Miczynski  —  Monatsh.  Chem.  7.  263,  1886.) 

Cms.  Ba.  Succinate  Cms.  Ba.  Iso  Succinate 

IjO^  per  IPO  Gms.  per  iqo  Gms. 

Water.          Solution.  Water.          Solution. 

o  0.421  0.420  1.884        1.849 

10  0.432  0.430  2.852        2.774 

20  0.418  0.417  3-618        3-493 

30  0.393  0.392  4.181        4.014 

40  0.366  0.365  4.542        4.346 

50  0.337  °-336  4-7oo        4-594 

60  0.306  0.305  4-656        4-45° 

70  0.273  0.272  4.410        4.224 

80  0.237  0.237  3-962        3-8l° 

100  gms.  H2O  dissolve  0.396  gms.  Ba  Succinate  at  18°  and  0.410 
gms.  at  25°. 

100  gms.  95%  alcohol  dissolve  0.0015  gms-  Ba  Succinate  at  18°  and 

0.0016  gms.  at  25°.     '  (Partheil  and  Hiibner  —  Archiv.  Pharm.  241,  413.  '03-) 

Cantoni  and  Diotalevi  (1905),  and  Tarugi  and  Checchi  (1901),  obtained  data 
in  close  agreement  with  the  above. 

BARIUM   SULFATE   BaSO4. 

SOLUBILITY  IN  WATER.    (Kohlrausch,  1908.) 

One  liter  of  sat.  solution  contains  0.00115  gm.  BaSO4  at  o°;  0.0020  gm.  at  10°; 
0.0024  gm.  at  20°  and  0.00285  gm-  at  30°. 

Melcher  (1910)  obtained  results  a  little  lower  than  the  above.  His  data  for 
higher  temperatures  are  0.00336  gm.  at  50°  and  0.0039  gm.  at  100°. 

Kohlrausch  obtained  the  following  results  for  the  solubility  of  heavy  spar 
(BaSO4);  0.0019  gm-  at  o°,  0.0023  gm.  at  10°;  0.0027  gm.  at  20°;  0,00315  gm 
at  30°  and  0.0033  gm.  at  33.5°. 

100  gms.  sat.  solution  of  BaSO4  in  21.37%  aqueous  ammonium  acetate  solu- 
tion contain  O.OI6  gm.  at  25°.  (Harden,  igzG.) 

SOLUBILITY  OF  BARIUM  SULFATE"  IN  AQUEOUS  SOLUTIONS  OF  IRON,  ALUMINIUM 
AND  MAGNESIUM  CHLORIDES  AT  2o°-25°.    (Fraps,  1901.) 

Gms.            Milligrams  BaSO4  per  Liter  in:  Gms.  Mgs.  BaSO4  per  Liter  in: 

Chloride       , ^— ,  Chloride 


Vxiuuiiue  /-     •  •      -^  v-mui  me  s 

per  Liter.  Aq.  FeCl8.  Aq.  AlCla.  Aq.  MgCl2-  per  Liter.  Aq.  FeCl3.    Aq.  A1C13.    Aq.MgCl2- 

i    58     33     30      25       150    116    50 
2i   72     43     30      5°      l6°    *7o    5° 

5  115     °o     33  ioo      170    175    So 

10  123     94     33  ...       


121  BARIUM  SULFATE 

SOLUBILITY  OF  BARIUM  SULFATE  IN  AQUEOUS  SOLUTIONS  OF  HYDROCHLORIC 
AND  OF  NITRIC  ACIDS. 

(Banthisch,  1884.) 
In  Hydrochloric  Acid.  In  Nitric  Acid. 

cc.  containing  Mgs.  BaSO4       Gms.  per  100  cc.    cc.  containing    Mgs.  BaSO4          Cms.  per  100  cc. 
i  MK  Equiv.  per  i  Mg.  Equiv.          Solution.  i  Mg.Equiv.  per  i  Mg.Equiv.  Solution. 

ofHCl.  ofHCl.  HC1.         BaSO/.       of  HNO3.       of  HNO3.  tiNO3.    '   BaSOl. 

2.       0.133     1.82   0.0067     2.      0.140      3.15   0.0070 
I.       0.089     3.65   0.0089     I.      0.107      6.31   0.0107 

0.5    0-056    7-29  o.oioi    0.5    0.085    12. 61  0.0170 

0.2      0.017    18.23   0.0086     O.2     0.048     3I-52   0.0241 

TOO  cc.  HBr  dissolve  0.04  gm.  BaSO4;  100  cc.  HI  dissolve  0.0016  gm.  BaSO4 

at  the  boiling  point.  (Haslam,  1886.) 

SOLUBILITY  OF  BARIUM  SULFATE  IN  CONCENTRATED  AQUEOUS  SOLUTIONS  OF 
SULFURIC  ACID  AT  2O°. 

*   (Von  Weimarn,  1911.) 


Gms.  HtSOi  per 

Gms.  BaS04  per 

Gms.  HzSO4  per 

Gms.  BaS04  per 

ico  Gms.  Solvent. 

100  cc.  Sat.  Sol. 

ico  Gms.  Solvent. 

100  cc.  Sat.  Sol. 

73.83 

0.0030 

85.78 

0.3215 

78.04 

0.0135 

88.08 

1.2200 

80.54 

0.0285 

93 

.  .  .* 

83.10 

O.OSOO 

96.17 

4.9665 

84.15 

...t 

96.46 

18.6900 

*  Solid  Phase  =  BaSCMIfcSO^.H^  +  BaSCU.EkSO*.    f  Solid  Phase  =  BaSO4  +  BaS04.H2S04.H2O. 

Data  for  the  above  system  are  also  given  by  Volkhouskii  (1910). 

100  cc.  sat.  solution  of  BaSO4  in  abs.  H2SO4  contain  28.51  gms.  BaSO4,  solid 
phase  =  BaSO4.3oH2SO4.  (Bergius,  1910.) 

100  cc.  of  sat.  solution  of  BaSO4  in  95%  formic  acid  contain  o.oi  gm.  BaSO4 
at  18.5°.  (Aschan,  1913.) 

Fusion-point  curves  (solubility,  see  footnote,  p.  i)  are  given  the  following 
mixtures  of  barium  sulfate  and  other  salts: 

BaSO4  +  NaCl  (Sackur,  1911-12.) 
+  KC1 
+  CaCl2 

-f-  K2SO4  (Grahmann,  1913;  Calcagni,  1912.) 

+  Li2SO4  (Calcagni  and  Marotta,  1912.) 

+  Na2SO4  (Calcagni,  1912.) 

BARIUM  Amyl  SULFATE   Ba(C5HnSO4)2.2H2O. 

SOLUBILITY  OF  MIXED  CRYSTALS  OF  THE  ACTIVE  AND  INACTIVE  SALT  IN 
WATER  AT  20.5°. 

(Marckwald,  1904.) 

Gms.  Salt  per    Per  cent  Active  Salt  Gms.  Salt  per     Per  cent  Active  Salt 

ico  Gms.  H2O.     in  Dissolved  Salt.  100  Gms.  HjO.       in  Dissolved  Salt. 

28.2  ico  18.3  49.6 

26.3  91.6  16.6  36.3 

24.8  84.5  15  25.8 

21.7  71.2  13.6  10.6 

19.5  59.5  12.8  o 

Mixed  crystals  of  the  active  and  inactive  barium  amyl  sulfate  were  dissolved 
in  water  by  warming,  then  cooled  to  the  beginning  of  crystallization  and  shaken 
two  hours  at  20.5°.  The  percentage  of  the  active  salt  was  determined  by  the 
polariscope.  Its  specific  rotation  was  [a]D=  +2.52°. 


BARIUM  SULFATE  122 

BARIUM  Isoamyl  SULFATE   Ba(C5HiiSO4)2.2H2O. 

100  gms.  H2O  dissolve  9.71  gms.  of  the  anhydrous  salt  at  10°,  11.85  Sms.  at 
19.3°  and  12.15  8mS.  at  20.5°.  (Marckwald,  1902.) 

BARIUM    PerSULFATE    BaS2O8.4H2O. 

100  parts  water  dissolve  39.1  parts  BaS2O8  or  52.2  parts  BaS2O8. 
4H2O  at  o°. 

(Marshall  —  J.  Ch.  Soc.  59,  771,  '91** 

BARIUM    SULFITE    BaSO3. 

SOLUBILITY  IN  WATER  AND  IN  AQUEOUS  SUGAR  SOLUTIONS. 

(Rogowicz  — Z.  Ver  Zuckerind.  938,  1905.) 

Cone,  of  Gm.  BaSO4  per  100  cc.  Sol.  ^^  Q{  Gm.  BaSO4  per  100  cc.  Sol. 

S^Sfll.  'at  20°.  "TTsoX  Sugar  Sol.  'at  2o°.  "!Ts>. 

o°  Bx        0.0197        0.00177        40°  Bx  0.0048        0.00158 

10°  0.0104        0.00335        5°°  "  0.0030        0.00149 

20°  "      0.0097     0-00289     60°  "  (Sat.)   0-0022     0-OOII2 

30°  "         0.0078        0.00223 

BARIUM  SULFONATES. 

SOLUBILITY  OF  SEVERAL  BARIUM  SULFONATES  IN  WATER. 

Gms.  Anhy- 

Salt.  Formula.  f.      pj^g..       Authority. 

Barium:  HzO. 

3.4  Diiodobenzene  Sulfonate  CuHeOek&Ba.H^          21.5        0.27      (Boyle,  1909.) 

2.5  "  "  CuHeOehSiBa.^H^         2O  0.522  " 

2  Phenanthrene  Sulfonate       (Ci4H9SO3)2Ba.|H2O         20  0.016     (Sandquist,  1912.) 

3  "  "  (CuH9SO3)2Ba.3H2O  2O  0.03  " 
10                                                        (C,4H9S03)2Ba.3H20          2O              0.13 

Bromobenzene  Sulfonate     (CelfcBrSOshBa  17.5        3.31      (Meyer,  1875.) 


BARIUM    TARTRATE     Ba(C2H2O3)2. 

SOLUBILITY  IN  WATER. 

(Cantoni  and  Zachoder  —  Bull.  soc.  chim.  [3]  33,  751,  '05;  see  also  Partheil  and  Hiibner.) 


Gms.  Ba(C2H2O3)2 
t°.              DCT  loo  cc.                 t°. 

Gms.  Ba(C2H2O3)2 
per  100  cc. 

t". 

Gms.  Ba(C2H2 
per  loo  cc. 

Solution. 

Solution. 

Solution. 

0 

O.O2O5 

30 

0.0315 

70 

0.0480 

10 

O.O242 

40 

0.0352 

00 

0.0527 

20 

0.0279 

50 

0.0389 

85 

0.0541 

25 

0.0297 

60 

0.0440 

•• 

SOLUBILITY  OF  BARIUM  TARTRATE  IN  AQUEOUS  SOLUTIONS  OF  POTASSIUM 
CHLORIDE,  SODIUM  CHLORIDE  AND  AMMONIUM  CHLORIDE. 

(Cantoni  and  Jolkowski,  1907.) 

At  Different  Temperatures.  Varying  Concentrations  at  16°. 

Gms.  Ba(C2H2Os)2  per  100  cc.  Sat.  Sol.  in:    Gms.  Chlo-   Gms.  Ba(C2H2Oa)2  per  100  cc.  Sat.  Sol  in: 


7%  KC1. 

7%NaCl. 

7%  NEUC1.  Gms.  Solvent. 

KC1. 

NaCl. 

NH4C1. 

16 

O 

.0823 

0, 

,0887 

0.1050 

o-5 

0.0398 

0, 

,0410 

0 

.0441 

30 

0 

.1017 

0 

,1151 

0.1370 

i 

o  .  0466 

0 

0514 

o 

.0589 

55 

0 

.1230 

O 

1348 

0.1590 

3 

0.0723 

o. 

,0826 

o 

.0892 

70 

0 

.I5OO 

O 

.1781 

o  .  2030 

10 

O.II99 

o, 

1260. 

0 

.1342 

85 

O 

.1828 

0 

.2168 

o  .  2360 

15 

0.1435 

o, 

1440 

0 

.1585 

20 

o  .  1466 

0, 

1573 

0 

•1663 

(See  Note  p.  222.) 

123  BARIUM   TARTRATE 

SOLUBILITY  OF  BARIUM  TARTRATE  IN  AQUEOUS  ACETIC  ACID  SOLUTIONS  AT 

26°-27°. 
(Herz  and  Muhs,  1903.) 

Normality  Cms.  residue*  Gms.  per  100  cc.  Solution.  Normality.  Cms,  residue*  Gms.per  IOQCC.  Solution. 


01  /vceuc 
Acid. 

per  50  cc. 
Sol. 

CH3COOH.  Batartratc!    ^Atid 

L    50   tA.. 

Sol. 

CH3COOH. 

Ba  tartrate. 

O 

0.0328 

o. 

o 

•0655 

3 

•77 

o 

.1866 

22 

.62 

0.3728 

o-565 

O.II5I 

3-39 

0 

.2300 

5 

•65 

0 

.1865 

33 

.90 

0.3726 

1-425 

0-1559 

8-55 

o 

•3"5 

16 

•85 

0 

.02l8 

101 

.10 

0.0436 

2.85 

o  1739 

17.11 

0 

•3475 

*  Dried  at  7-° 

TOO  grams  95%  alcohol  dissolve  0.032  gm.  Ba  tartrate  at  18°  and  0.0356  gm. 

at  25°.  (Partheil  and  Hubner.) 


BARIUM   P  TRUXILATE. 

100  cc.  sat.  solution  in  water  contain  0.028  gm.  of  the  salt  at  26°.  (de'Jong,  1912.) 

BEHENIC  ACID   C2iH43GOOH. 

Freezing-point  data  (solubility,  see  footnote,  p.  i)  are  given  for  the  following 
mixtures  of  behenic  icid  and  other  compounds. 
Behenic  Acid  +  Erusic  Acid  (Mascarelli  and  Sanna,  1915.) 

+  Isoerusic  Acid 

+  Brassidinic  Acid 

+  Isobehenic  Acid  (Meyer,  Brod  and  Soyka,  1913.) 

Methylester+Isobehenic  Acid  Methyl  Ester.   " 

BENZALANILINE   CeHsCHiN.CeHs. 

Solubility  data  determined  by  the  freezing-point  method  are  given  by  Pascal 
and  Normand  (1913),  for  mixtures  of  benzalaniline  and  each  of  the  following 
compounds:  Azobenzene,  benzylaniline,  dibenzyl,  hydrazobenzene,  stilbene  and 
tolane. 

BENZALAZINE   C6H5CH  :  N.N  :  CHC6H5. 

Solubility  data  determined  by  the  freezing-point  method  are  given  by  Pascal 
(1914),  for  mixtures  of  benzalazine  and  each  of  the  following  compounds:  Di- 
phenylhydrazine,  diphenyldiacetylene,  naphthalene,  furfuralazine,  diphenylbuta- 
diene  and  cinnamylidene.  Data  are  also  given  for  mixtures  of  thiophenylalazine 
and  cinnamylidene. 

BENZALDEHYDE   C6H5CHO. 

100  gms.  H2O  dissolve  0.3  gm.  C6H5.CHO  at  room  temp.    (Fluckinger,  1875;  U.  S.  P.) 
Freezing-point  data  for  mixtures  of  C6H5.CHO  and  HNO3  are  given  by  Zukow 
and  Kasatkin  (1909). 

Para  HydroxyBENZALDEHYDE  p  C6H4OH.CHO. 

Freezing-point  data  are  given  for  mixtures  of  p  hydroxybenzaldehyde  +  di- 
methylaniline  and  p  hydroxybenzaldehyde  +  phenol.  (Schmidlin  and  Lang,  1912.) 

Ortho  NitroBENZALDEHYDE   o  C6H4NO2.CHO. 

SOLUBILITY  IN  WATER  AND  IN  AQUEOUS  SOLUTIONS  AT  25°. 

(Goldschmidt  and  Sunde,  1906.) 

Gms.  CelfcNOz.  Gms.  CelfcNOj.  Gms.  C«H«NO« 

Solvent.          CHO  per  100  cc.         Solvent.          CHO  per  100  cc.  Solvent.  CHO  per  100 

Sat.  Sol.  Sat.  Sol.  cc.  Sat.  Sol. 

H2O  0.2316  i     raNaCl  0.1899  I      wKNO3  0.3199 

o.5wHCl  0.2391  2      n     "  0.1390  2      n     "  0.3419 

1  n    "  0.2466  o.5nHNOa  0.3207  o.swNaNOa  0.3013 

2  n  "  0.2658  i  n   "  0.3758  i   n  0.3132 

1  nKCl       0.2046    o.5wKNO3     0.3123     2     n  0.3201 

2  n    "         0.1912 


BENZALDEHYDE  124 

Meta  NitroBENZALDEHYDE  m  C6H4NO2.CHO. 

100  CC.  H2O  dissolve 0. 1625  gm.  m  C6H4NO2.CHO  at  25°  (Goldschmidt  and  Sunde,  1906.) 
"      I  n  HC1   "   0.1813    " 
"      inKCl   "   0.1542    ." 
11      2wKCl   "   0.1417    " 

Para  NitroBENZALDEHYDE  p  C6H4NO2.CHO. 

Data  for  the  system  p  nitrobenzaldehyde  +  nitrobenzene  +  hexane  are  given 
by  Timmermans  (1907). 

Solubility  data  determined  by  the  freezing-point  method  are  given  for: 
p  Nitrobenzaldehyde  +  Sulfuric  Acid         (Kendall,  1914.) 
m  +  Benzene  (Schmidlin  and  Lang,  1912.) 

m  -j-  Phenol 

BENZALDOXIME   C6H6CH:NOH. 

Solubility  data  determined  by  the  freezing-point  method  are  given  for  mix- 
tures of: 

a  Benzaldoxime  +  ft  Benzaldoxime  (Cameron,  1898.) 

a  Nitrobenzaldoxime  +  ft  Nitrobenzaldoxime.      (Beck,  1904.) 

BENZAMIDE     C6H6CONH2. 

SOLUBILITY  IN  ETHYL  ALCOHOL. 

(Speyers  —  Am.  J.  Sci.  [4]  14,  295,  '02.) 

G.M.                  Cms.                                                        G.  M.  Cms. 

to    Sp.  Gr.  of    C6H8CONH2  C6H6CONH2  to          Sp.  Gr.  of      C6H6CONH2  C6H6CONHa 

*     Solutions,    per  100  G.M.  per  100  Gms.                    Solutions,      per  100  G.M.  per  100  Gms. 

CaHfiOH.          C-sHcOH.                                                C2H6OH.  C^OK. 

0  °-^33  3-1  8.15  40  0.848  ii  .o  28.92 

10  0.832  4.2  11.04  50  0.862  14.2  37-34 

20  0.833  5.9  15-52  60  0.881  17.2  45-22 

25  0.835  6.8  17.87  70  0.913  20.4  53-63 

30  0.838  8.2  21.56 

SOLUBILITY  OF  BENZAMIDE  IN  MIXTURES  OF  ALCOHOL  AND  WATER 


AT  25". 

(Holleman  and  Antusch  —  Rec.  trav.  chim.  13,  294,  '94.) 

Alcohol. 
100 

95 
90 

85 
83 
80 

75 

See  rematks  under  a  Acetnaphthalide,  p.  13. 

loo  gms.  pyridine  dissolve  31.23  gms.  benzamide  at  2p°-25°.  (Dehn,  1917.) 

100  gms.  aq.  50%  pyridine  dissolve  39.15  gms.  benzamide  at  2O°-25°. 
The  coefficient  of  distribution  of  benzamide  between  oil  and  water  is  0.66  at 
3°  and  0.43  at  36°.  (Meyer,  1900, 1909.) 

BENZANILIDE. 

Solubilities  determined  by  the  freezing-point  method  are  given  by  Vanstone 
(1913)-  for  mixtures  of  benzanilide  and  each  of  the  following  compounds:  ben- 
zil,  benzylideneaniline,  and  benzoin. 

Results  for  mixtures  of  o  chlorobenzanilide  and  p  chlorobenzanilide  are  given 
by  King  and  Orton  (1911). 


Gms. 

Gms. 

per  100  Gms. 

Sp.  Gr.  of 

Solutions. 

Vol.  % 
Alcohol. 

QsHsCONHjj 
per  100  Gms. 

Sp.  Gr.  of 
Solutions. 

Solvent. 

Solvent. 

17.03 

0.830 

70 

23.87 

0.925 

21  .12 

0.856 

60 

18.98 

0-939 

24.50 

0.878 

50 

13-74 

0.949 

26.15 

0.895 

40 

8.62 

0.958 

26.63 

O.9OO 

31 

5-33 

0.967 

26.43 

0.907 

15 

2.28 

0.982 

25  41 

O.Qiy 

0 

i-35 

0.999 

125  BENZENE 

BENZENE     C6He. 

SOLUBILITY  IN  WATER  AT  22°. 

(Herz  —  Ber.  31,  2671,  '98.) 

ioo  cc.  water  dissolve  0.082  cc.  C6Hfr,  Vol.  of  Sol.  —  100.082, 
Sp.  Gr.  =  0.9979. 

ioo  cc.  C6H6  dissolve  0.211  cc.  H2O,  Vol.  of  sol.  =  100.135, 
Sp.  Gr.  -  0.8768. 

SOLUBILITY  OF  WATER  IN  BENZENE. 

(Groschuff,  1911.) 

j.o  Gm.  HkO  per  ioo  j.°  Gms.  HsO  per  ioo 

1  '  Gms.  Sat.  Sol.  Gms.  Sat.  Sol. 

3  0-030  55  0.184 

23  0.061  66  °-255 

40  0.114  77  0.337 

BENZENE,  AQ.  ALCOHOL  MIXTURES;  BENZENE,  AQ.   ACETONE  MIX- 

TURES AT  20°. 

H2O  added  to  mixtures  of  known  amounts  of  the  other  two  and 
appearance  of  clouding  noted. 

(Bancroft  —  Phys.  Rev.  3,  31,  1895.96.) 

C6H6,C2HSOH  and  H2O  C6H6,CH3OH  and  H2O  C6H5,  (CH3)2CO  and  H2O 

Per  5  cc.C2H5OH.  Per  5  cc.  CH3OH.  Per  5  cc.  (CH3)2CO. 

* 


cc.  H20.       cc.  C6H6.  'cc.  H2O.    cc.  C6H8.'  cc.  H2O. 

20  0.03  5.0      0.15  8.0        o.io 

8  0.13  3.0      0.215  3.0        0.395 

4  0-39  2.0         0-59  2.0  0.69 

2  1.17  1-4         I.O  1.3  1.0 

1.5  1.87  I.o         1-9  O.5I         2.0 

i.o          3.57  0.8      3.0  0.295    3.0 

0.605      8.0  0.69    4.0  0.2        4.0 

0.34      20.0  0.49    8.0  0.15      5.0 

C2H5OH  added  to  mixtures  of  known  amounts  of  CeH6  and  H2O  until  the 
solutions  became  homogeneous  at  20°.  (Lincoln,  1900.) 

Per  5  cc.  CsHe.  Per  5  cc.  CeH6.  Per  5  cc.  C6H6. 

cc.  HzO.       '  cc.  CzHiOH.  cc.  HzO.         cc.  CzHsOH.  cc.  H2O.         cc.  CzHsOH.'  . 

I  4-6  20  31.6  50  58 

5  12.8  30  41.4  60  65.6 

10  19.8  40  39.5  70  73.1 

Lincoln  also  gives  results  at  10°.  Data  of  a  similar  character  for  mixtures  of 
benzene,  ethyl  alcohol  and  water  at  20,  25  and  35°  are  given  by  Taylor  (1897). 

For  results  at  15°,  see  page  287. 

Data  for  mixtures  of  benzene,  ethyl  alcohol  and  glycerol  and  for  mixtures  of 
benzene,  ethyl  alcohol  and  lactic  acid  are  given  by  Rozsa  (1911). 

MUTUAL  SOLUBILITY  OF  BENZENE  AND  CARBON  TETRACHLORIDE. 
(Determined  by  the  synthetic  method.) 

(Baud,  1913.) 

to  Gms.  CeHg  per  ioo  f0  Gms.  CsHe  per  100        to       Gms.  C«H«  per  ioo 

Gms.  Mixture.  Gms.  Mixture.  Gms.  Mixture. 

—  24.2  O  —40  19.3  —20  48 

.   —30  2.8        —34  24.2        —io  64.1 

-40  8.5        -35tr.pt.          31  o  85.3 

—  46.3Eutec.     12.9        —30  36  +5-5       ioo 


BENZENE  126 

MUTUAL  SOLUBILITY  OF  BENZENE  AND  CHLOROFORM.    FREEZING-POINT 

METHOD.     (Wroczynski  and  Guye,  1910.) 

Cms.  CeH6           «  ,. .                            Cms.  C6H6      ~  ,. ,  Gnfs.  CeH6          . 

t°.        periooGms.         **»£               t°.       per  100  Gms.  pSh°^             t°.  per  100  Cms. 

Solution.           rhase>                            Solution.      Phase-  Solution. 

—  63.5           O                 CHCb            —60         26.8        C6H«           —20  58.3       C6H6 

—  70         1 1. 8  "  —50      32  "          —io        70.8 

-75          H-7  "  -40      39  "  o        88 

—  81.7      18.4    CHCU+c6H6    —30      47.8        "  5       100 

—  70  22.6  CsH« 

The  eutectic  point  was  found  by  extending  the  curves  to  their  intersection. 
The  temperature  of  the  eutectic  could  not  be  reached  by  use  of  liquid  CO2. 

MUTUAL  SOLUBILITY  OF  BENZENE  AND  FORMIC  ACID.    SYNTHETIC  METHOD. 

(Ennis,  1914.) 

t°  of  Cms.  HCOOH  t°  of         Cms.  HCOOH  per  t°  of          Cms.  HCOOH 

Miscibility     per  100  Gms.  Sol.         Miscibility.        100  Cms.  Sol.  Miscibility.  per  100  Gms.  Sol. 

21  9.2  70  31.5  60  74 

30  10.3  72  35  40  82 

40  12.2  73.2  43-51  20  87 

50  16.5  72  60  5  89.6 

60  22  70  65 

SOLUBILITY  OF  BENZENE  IN  AQUEOUS  SOLUTIONS  OF  FORMIC  ACID.    SYNTHETIC 
METHOD.    (Ennis,  1914.) 


iirr 
riCL 

iVt.  % 
(OH. 

Gms.  CeHj 

In  85  Wt.  % 
HCOOH. 

jo  Q£           Gms.  CeHj 

'«H% 

yo  Q£           Gms.  CeHe 

In  60  Wt.  % 
HCOOH. 

i        t»  of           Gms.  CeHs 

Miscibility. 

per  ioo 
Gms.  Sol. 

Miscibility. 

per  ioo 
Gms.  Sol. 

Misdbility.      G^r  gj 

Miscibility. 

per  ioo 
Gms.  Sol. 

57-5 

96.3 

71 

97-5 

122 

12 

105 

6 

77 

94-4 

87 

96.6 

97-5 

8-5 

82 

3-8 

95 

89.8 

101 

96 

74 

6 

76 

3 

112 

85-2 

100.5 

14.3 

94-5 

24.7 

81 

IO 

80.5 

20 

46 

7 

51        12.5 

MUTUAL  SOLUBILITY  OF  BENZENE  AND  ETHYL  ALCOHOL.    FREEZING-POINT. 

METHOD.         (Viala,  1914;  see  also  Rozsa,  1911  and  Pickering,  1893.) 
t o  Gms.  CeHe  per  f 0  Gms.  CeHe  per  fo  Gms.  CeHe  per 

ioo  Gms.  Sol.  ioo  Gms.  Sol.  ioo  Gms.  Sol. 

-113.9  o  -60  19.3  -io  57.6 

—  ioo  8  —50  24.1  o  85 

—  90  io  —40  29.8  i  93 

-  80  12  -30  37  5.5          ioo 

-  70  15  -20  45.7 

MUTUAL  SOLUBILITY  OF  BENZENE  AND  /3  NAPHTHALENE  PICRATE, 

C6H2(Np2)3OH.CioH7OH.    (Kuriioff,  1897.) 

Synthetic  method  used  —  see  Note,  p.  16 

|.o  Gms.  Gma.  fo  Gms.  Gms. 

Picrate          Benzene  Picrate.         Benzene. 

157    ioo.      ...   100.0    in. 6   1.173    I-°37  J9-2 

148.4  2.128         O.II5          79.3  IO2.O          I.oS/  1.780       II. 2 

137.4        1-274      0.170      61.1  29.5      0.390        8.430      0.95 

134.2     1-384    0.297    49.3         4.6    1.329    21. 80     0.48 

126.8         1.019      0.343       38.3  5.02       ...       loo.o 

a  =  Mols.  ft  Naphthalene   Picrate  per  ioo    Mols.  of  ft  Napthalene 
Picrate  plus  Benzene. 
Determinations  for  a  large  number  of  isothermes  are  also  given. 


127 


BENZENE 


THE  SYSTEM  BENZENE,  PHENOL  AND  WATER  AT  25°. 

(Horiba,  1914.) 

In  the  case  of  phenol,  the  bromine  method  was  used  for  its  determination.  In 
the  case  of  the  other  two  compounds,  the  amounts  required  to  produce  constant 
turbidity  were  measured  directly  from  burettes. 


Solubility  of  Benzene  in  Aqueous  Solu- 
tions Containing  Phenol  and  Vice  Versa. 


Solubility  of  Phenol  in  Benzene  Solu- 
tions Containing  Water  and  Vice  Versa. 

Saturating 


<*«• 

Gms.  per  ioo  Gms. 
CsHsOH+CeHe+HzO.       ^jgj™* 

^36- 

Gms.  per  ioo  Gms. 

IS 

CeHiOH. 

QHe.     * 

3s             ' 

UHsOH. 

C«H«. 

I 

.0002 

O 

0 

.198             CeH, 

29 

,29 

0 

I 

.0008 

I 

•059 

O 

.  204 

71 

63 

I 

.62 

I 

.OO2I 

2 

.602 

0 

.205 

74 

5 

3 

I 

.00305 

3 

.526 

o 

•  199 

I 

.0256 

69. 

,18 

16.33 

5 

•65 

0 

.17     CoHs+CsHsOH 

O 

.9891 

55< 

80 

36 

•13 

5 

•953 

0 

.132         QHsOH 

0 

.9629 

44 

39 

5o 

•56 

I 

.0059 

6 

.516 

o 

•075 

0 

.9142 

21. 

15 

77 

.22 

I 

.0069 

7 

•  683 

0 

.025 

o 

.8818 

4 

78 

94 

.98 

I 

.0073 

8 

•195 

o 

" 

0 

.8764 

0 

99 

•95 

CsHsOH 

CeHfiOH+CeH, 
CeH. 


Data  are  also  given  for  the  solubility  of  phenol  as  solid  phase,  in  C6H6  and  in 
water  and  in  their  mixtures.  A  complete  table  for  the  conjugate  points,  showing 
the  distribution  of  phenol  between  the  aqueous  and  the  benzene  layers,  is  given. 
The  results  agree  with  those  of  Rothmund  and  Wilsmore.  See  page  482. 


RECIPROCAL  SOLUBILITY,  DETERMINED  BY  FREEZING-POINT  METHOD,  OF 

MIXTURES  OFC 
Benzene  and  Phenol. 

(Hatcher  and  Skirrow,  1917.) 


Benzene  and  Pyridine. 

(Hatcher  and  Skirrow,  1917.) 


t°  of  Melting.       Ifl*g^*y 

«r       Solid 
;ure.  Phase. 

t°  of  Meltine        Gms>  C<sH?  ***         Solid 
*'   ioo  Gms.  Mixture.     Phase. 

39-4 

O 

CeHsOH 

-39-4 

0 

OHsN 

30 

II.  8 

" 

-45 

IO 

" 

20 

25 

" 

-50 

17 

" 

10 

38.2 

" 

-55 

23-3 

" 

0 

51.5 

" 

-58Eutec. 

26 

"  +C.H, 

—  5.4Eut 

ec.        58.4 

"  +GH8 

-5o 

31 

OH« 

-  2.5 

67-5 

GHa 

-40 

37-7 

" 

0 

78.3 

" 

-30 

46 

<« 

+  2.5 

89 

" 

—  20 

57 

" 

5-i 

IOO 

" 

—  10 

7i-5 

" 

o 

90-5 

M 

Additional 
Paterno  and 

data  on  the  system  Benzene  +  Phenol  are  given  by  Dahms,  1895; 
Ampola,  1897;  Tsakalotos  and  Guye,  1910,  and  Rosza,  1911.     Add:- 

,1               ,T-»                      IT-»      •  !•                     •  i  T»;_  i  :  -  o~_ 

SOLUBILITY  OF  BENZENE  IN  SULPHUR. 

By  "Synthetic  Method"  see  Note,  p.  16. 

(Alexejew,  1886.) 

^o     Gms.  C6Ha  per  ioo  Gms.  ^.0 

S  Layer.  C6He  Layer i 

ioo  6  75  140 
no  8  72.5  150 
120  10  70  160 


Gms.  CBHB^per  ioo  Gms. 
S  Layer.  QHe  Layer." 

16  6l 


I30 


12 


66 


25 

164  (crit  temp.)        35 


55 
45 


BENZENE  128 

SOLUBILITY  DATA,  DETERMINED  BY  THE  FREEZING-POINT  METHOD  (see 
footnote,  p.  i),  ARE  GIVEN  FOR  THE  FOLLOWING  MIXTURES: 

Benzene  +  Benzoic  acid  (Roloff,  1895.    See  Benzoic  Acid,  p.  135.) 

"         +  o  Nitrobenzylchloride  (Schmidlin  and  Lang,  1912.) 
"        -f-  Bromoform  "  " 

"        -j-  Tetramethyldiamino    benz- 
hydrol 

+  Benzhydrol 

"        +  Nitrobenzene  (Dahms,  1895.) 

+  0,wand£Chloronitrobenzene)(Bogojawlensky,  Winogradow  and  Bogolubow, 

"        -f-  m  Bromonitrobenzene  )        (1906.) 
"        +  o,  m  and  p  Dinitrobenzene       (Kremann,  1908.) 

+  Carbon  disulfide  (Pickering  1893.) 

"         +  Camphene  (Kurnakoff  and  Efremoff,  1912.) 

-f-  m  Cresol  (Kremann  and  Borjanovics,  1916.) 

"          +  Cyclohexane  (Mascarelli  and  Pestalozza,  1907,  1908.) 

"         +  Diphenyl  (Washburn  and  Read,  1915.) 

"        +  Diethylamine  (Pickering,  1893.) 

"        +  Diphenylamine  (Bruni,  1898;  Dahms,  1895.) 

"        +  Ethyl  ether  (Pickering,  1893.) 

"        +  Ethylene  bromide  (Dahms,  1895.) 

-f-  Ethylene  dibromide  (Baud  and  Gay,  1911.) 

"        +  Ethylene  chloride  (Baud  and  Gay,  1910.) 

"        -f-  Ethylene  dichloride  (Baud  and  Gay,  1911.) 

"         +  Menthol  (Dahms,  1895.) 

"          +  Methyl  alcohol  (Pickering,  1893.) 

"        +  Naphthalene  r^ad^xlf^5' ****''  ^^^  "^ 

"         +  "  +j8Naphthol         (Bruni,  1898.) 

"        +  +  Diphenylamine          " 

"        +  Phenanthrene 

+  +  Carbazol 

"        +  Paraldehyde  (Patemo  and  Ampola,  1891, 1897.) 

"          +  0,  m  and  p  Nitrophenol  jCBogojawlensky,  Winogradow  and  Bogolubow, 

"        +  Propyl  alcohol  (Pickering,  1893.) 

+  Quinine  (Van  Iterson-Rotgans,  1913.) 

+  Thiophene  (Tsakalotos  and  Guye,  1910.) 

"         +  Bromotoluene  (Paterno  and  Ampola,  1897.) 

"        +  1.2.4,  1.2.6  and  1.3.4  Dinitro-L., 

toluene  }  (Kremann,  1908.) 

+  Urethan  (Pushin  and  Glagoleva  and  Mazarovich,  1914.) 

"         +  p  Xylene  (Paterno  and  Ampola,  1897.) 

Bromobenzene  +  Chlorobenzene  (Pascal,  1913.) 
T  lodobenzene  " 

+  Fluorobenzene  " 

p  Dibromobenzene  +  0  Dibromobenzene  (Holleman  and  van  der  Linden,  1911.) 

+  p  Dichlorobenzene 

-|-  p  Diiodobenzene      (Nagornow,  1911.) 
+  p  Bromoiodoben-    ?  „ 

zene  J 

|  (Bruni  and  Gorni,  l899.) 
Chloronitroben-  |(pawlewsk.  l89g>) 

+  m 

+  p  Bromotoluene        (Borodowski  and  Bogojawlenski,  1904.) 


129  BromoBENZENES 

SOLUBILITY  OF  p  DIBROMOBENZENE  IN  SEVERAL  SOLVENTS  AT  25°. 

(Hildebrand,  Ellefson  and  Beebe,  1917.) 

Cms.  CeH4Br2  (p)  Gms.  CeffcBn  (p) 

Solvent.  per  100  Gms.  Solvent.  per  100  Cms. 

Solvent.  Solvent. 

Methyl  Alcohol        10.35  Carbon  Tetrachloride       36.6 

Benzene  83.8  Ethyl  Ether  71.3 

Carbon  Bisulfide     90  Hexane  25.9 

DiBromoBENZENE  (p}   C6H4Br2. 

SOLUBILITY  IN  ETHYL,  PROPYL,  Iso  BUTYL  ALCOHOLS,  ETC. 

(Schroder  —  Z.  physik.  Chem.  n,  456,  '93.) 

Determinations  by  "  Synthetic  Method"  see  Note,  p.  16. 

Grams  C6H4Br2  (P)  per  too  Grams  Sat.  Solution  in: 

CzHcOH. Crf 
O 
10 
20 

30 
40 
50 
60 

70 

75 
80 

SOLUBILITY  OF  MIXTURES  OF  p  DIBROMOBENZENE  AND  p  DICHLOROBENZENE 
IN  AQUEOUS  SOLUTIONS  OF  ETHYL  ALCOHOL 

Solvent,  50  Vol.  %  C2H5OH,  t  =  ^.i°.        Solvent,  90.9  Vol.  %  C2H6OH,  t  =  25° 

(Kiister  and  Dahmer,  1905.)  (Kiister  and  Wiirfel,  1904-05.) 


f"LS  /~\1X 

CsHyOH. 

(CHa)CH.CH2OH. 

(C2H6)20. 

CS2. 

C6H6. 

\ 

27 

30 

34 

34 

22 

38 

43 

43 

29 

14 

15 

47 

53 

53 

36 

19 

2O 

57 

62 

62 

45 

26 

2? 

30 

67 

72 

71 

54 

38 

40 

44 

77 

8! 

80 

67 

576 

67 

65 

87 

90 

88 

79 

80-5 

85 

77 

84 

94.4 

95 

94-6 

•  » 

90 

Gms.  per  100  cc. 

Sat.  Sol. 

Mol.  %  CeHiBra 
in  Solute. 

Gms.  per 

loo  cc.  Sat.  Sol. 

Mol.  %  CeHtBra 
in  Solute. 

CeH4Br2. 

CeHiCk. 

CgHxBrj. 

CsHiCh. 

0.484 

0 

100 

2.909 

0 

100 

0.505 

O.O44 

89.8 

2.674 

0.696 

94-3 

0.496 

0.084 

80.7 

2.220 

2.808 

70.7 

0.477 

0.503 

59-3 

1.769 

4.249 

49.1 

0.470 

0.721 

54-4 

I.27I 

6.237 

24-5 

0.196 

I.3II 

ii.  6 

0.675 

6.877 

9.9 

O 

I  .614 

0 

0 

8.271 

0 

Additional  data  for  the  above  system  are  given  by  Thiel  (1903). 
Tribrpmo  BENZENE,    C6H3Br3.     Solubility,  gms.  per   100  gms.  at  20-25°: 
In  H2(X 0.004;  in  pyridine,  24.3;  in  Aq.  50%  pyridine  ,  2.01.  (Dehn,  1917.) 

SOLUBILITY  DATA,  DETERMINED  BY  THE  FREEZING-POINT  METHOD  (see  foot- 
note, p.  i),  ARE  GIVEN  FOR  THE  FOLLOWING  MIXTURES. 

p  Bromochlorobenzene  +  p  Dichlorobenzene        (Bruni  and  Garni.  1899.) 

+  0   Bromochlorobenzene     (Holleman  and  Van  der  Linden,  1911.) 
p  Bromoiodobenzene      -j-  p  Diiodobenzene          (Nagomow,  1911.) 

O    Bromonitrobenzene     -j-  0   Chloronitrobenzene  (Kremann;  Kremann  and  Ehrlich.  1908.) 
+  P  Bromonitrobenzene  (Holleman &deBruyn,  1900; Narbutt,  '05.) 

m  -j-  o  "  (Narbutt,  1905.) 

+  p 

+  m  Chloronitrobenzene  (Hasselblatt,  1913;  Kuster,  1891.) 
-j-  m  lodonitrobenzene      (Hasselblatt,  1913.) 
-j-  m  Fluoronitrobenzene 
-j-  m  Chloronitrobenzene  (Kremann,  1908.) 

p  "  -j-  p  "    (Kremann,  1908;  Isaac,  1913;  Kremann  &  Ehrlich,  1308.) 


ChloroBENZENES 


130 


ChloroBENZENE   C6H5C1. 

SOLUBILITY  OF  CHLOROBENZENE  IN  SULPHUR. 

"  Synthetic  Method,"  see  page  16. 
(Alexejew.) 

Grams  C6H5Cl^per  TOO  Grams. 


*"•  Sulphur 

Layer. 

QO  13 

ioo  18.5 

no  27 

116   crit.  temp. 


38 


Chlor  Ben- 
zene  Layer. 

70 

63 
53 


^DichloroBENZENE,  C6H4C12.     o  and  m  ChloronitroBENZENE,  C6H4C1NO2. 
SOLUBILITY  OF  EACH  IN  LIQUID  CARBON  DIOXIDE. 

(Biichner,  1905-06.) 
o  Chloronitrobenzene.      m  Chloronitrobenzene. 


£  'Dichlorobenzene. 

Gms.  p  C6H4Cl2 

t°. 

per  ioo  Gms. 

t°. 

Sat.  Solution. 

-33 

1.2 

-32 

—  10 

4.2 

+  5 

+  10 

II.4 

7 

20 

22.7 

8 

22 

34-4 

ii 

Gms.  o  CeH4ClNO2  per  ioo 
Gms.  Sat.  Solution. 

I 

7.8 

16 . 5-36  quad.  pt. 

58.8 
65.8 


Gms.  m  C6H4C1NO2 
t°.         per  ioo  Gms.  Sat. 
Solution. 

-   i  1.8 

+  16.5  II. 2 

7.5    38.2quad.pt. 
20  53.2 


SOLUBILITY  OF  o,  m  AND  p  CHLORONITROBENZENES  IN  ANILINE,  DETER- 
MINED BY  THE  FREEZING-POINT  METHOD  (see  also  p.  77). 

(Kremann,  1907.) 
Gms.  Each  Compound  (Determined  Separately)  per  too  Gms.  Sat.  Sol. 


C6H4C1N02. 


51.30  (  =  39 
69-  IS  (  =  57 


m  CeftClNO*. 
21.60  (=i4Mol. 
31.67  (  =  21.5 
49.29  (  =  36.5 


P  C6H4ClNOz. 
27.75(=i8.SMol.%) 

31.67  (  =  21.5 
38. 50  (  =  27 


SOLUBILITY  DATA,  DETERMINED  BY  THE  FREEZING-POINT  METHOD  (see 
footnote,  p.  i),  ARE  GIVEN  FOR  THE  FOLLOWING  MIXTURES: 

(Pascal,  1913.) 


(Holleman  and  Van  der  Linden,  1911.) 
(Nagornow,  1911.) 


(Van  der  Linden,  1912.) 


Chlorobenzene  +  lodobenzene 

-f-  Cyanbenzene 

-j-  Fluorobenzene 

o  Dichlorobenzene  +  p  Dichlorobenzene 
P  "j  +  p  Diiodobenzene 

+  p  Chloroiodobenzene 
1.2.4  Trichlorobenzene  +  1.2.3  Trichlorobenzene 

+  1.3-5 

+  +  i.  2. 3  Trichlorobenzene       " 

a  Hexachlorobenzene  +  0  Hexachlorobenzene 
p  Chloroiodobenzene  +  p  Diiodobenzene          (Nagornow.  1911.) 
o  Chloronitrobenzene  -j-  p  Chloronitrobenzene  (Holleman  and  de  Bruyn,  1900.) 

-f-  (Bogaiawlewsky,  Winogradow  and  Bogolubow,  1906.) 

-j-  Formic  acid  (Bruni  and  Berti,  1900.) 

+  m  lodoijitrobenzene     (Hasselblatt,  1913.) 

+  m  Fluoronitrobenzene  " 

-(-  Naphthalene  (Kremann  and  Rodenis,  1906.) 

-j-  Diphenylamine  (Tinkler.  1913.) 

-j-  Naphthalene  (Kremann  and  Rodenis,  1906.) 

o  lodonitrobenzene  +  p  lodonitrobenzene          (Holleman,  1913.) 

m  Benzene  disulf  one  chloride  -{-p  Benzene  disulfone  chloride.  (Holleman  and  Pollak,  1910.) 


m 


131 


NitroBENZENES 


MUTUAL  SOLUBILITY  OF  NITROBENZENE  AND  WATER 

(Campetti  and  Del  Grosso,  1913;  Davis,  1916.) 
Oms  r«HiN( 

t°. 

20 
40 
00 

80 

100 
120 
140 

160 

Data  for  the  solubility  of  nitrobenzene  in  hexane,  diisoamyldecane  and  Ameri- 
can petroleum  at  pressures  up  to  3000  atmospheres,  are  given  by  Kohnstamm  and 
Timmermans  (1913). 

SOLUBILITY  OF  o,  m  AND  p  NITROBENZENE  IN  WATER  AND  IN  PYRIDINE. 

(Dehn,  1917.) 

Gms.  Each  Compound  Separately  per  100  Gms.  Solvent. 
Solvent. 


Gms.  CoHsNOi  per  100  Gms. 

H,O  Layer.     < 

HjHiNOz  Layer. 

0.19 

99.76 

0-3 

99.6 

0.4 

99-3 

0.8 

99 

i 

98.7 

1.3 

98.2 

1.9 

97.2 

2.8 

95-8 

* 

H2O  Layer. 

C«HSN02  Layer. 

180 

4-2 

93-7 

200 

7.2 

91 

220 

II.  8 

87 

230 

15.8 

83 

240 

23 

72 

241 

26 

67 

242 

32 

58 

244-5 

crit.  t.      50. 

I 

Water  20-25 

50%  Aq.  Pyridine       20-25 
Pyridine  20-25 


o  Nitrobenzene,      m  Nitrobenzene.  p  Nitrobenzene. 

0.21+                  2.14+  1.32  + 

1 73              two  layers  formed  85.3 

260            .      394  53.2 


SOLUBILITY  DATA,  DETERMINED  BY  THE  FREEZING-POINT  METHOD  (see  foot- 
note, p.  i),  ARE  GIVEN  FOR  MIXTURES  OF  NITROBENZENE  AND  EACH  OF  THE 
FOLLOWING  COMPOUNDS: 

Ethyl  Ether  (Tsakalotos  and  Guye,  igro.)  Mercuric  Bromide  (Mascarell  and  Ascoli,  1907.) 

Hexane  (Timmermans,  1907, 1911.)    Mercuric  Chloride 


Hexane  -f-  Resorcine  (Timmermans,  1907.) 
Isopentane  (Timmermans,  1910, 1911.) 

Diethyldiacetyltartrate  (Scheuer,  1910.) 
Menthol 


Nitrosobenzene  (Jaeger  and  van  Kregten,  1912.) 
Phenol  (Dahms,  1895.) 

Ethylene  Bromide          " 
Naphthalene  (Kremann,  '04;  Kurnakov,  etal,  '15.) 


DiNitroBENZENE  (m)   C6H4(NO2)2. 

SOLUBILITY  IN  BENZENE,  BROM  BENZENE  AND  IN  CHLOROFORM. 
"  Synthetic  Method." 

(Schroder.) 

Gms  CaH4(NO2)2  per  100 
t°  Gms.  Sol.  in: 


15 
20 

25 
30 


C6H6 
*7  5 

26  .o 
33  o 
40.0 


I8.S 

23  7 
28.7 


CHCI3 
22  .2 

25  o 

29.0 

33-o 


Gms.  CflH4(N08)2  per 
t°.               100  Gms.  Sol.  in: 

C6Ha 

C8H5Br 

CHC13. 

40 

52 

.0 

38 

.0 

42 

.0 

50 

62 

•5 

47 

5 

52 

•5 

60 

71 

.0 

57 

.0 

65 

.0 

SOLUBILITY  OF  m  DINITROBENZENE  IN  SEVERAL  ALCOHOLS  AND  ACIDS 

(Timofeiew.  1894.) 


Solvent. 

Gms.  m  C6H4(NO»)j 
t°.                per  100  Gms. 

Solvent. 

Gms.wtCeEUCNCtoj 
t°.                  per  100  Gms. 

Sat.  Sol. 

Solvent. 

Sat. 

Sol. 

Solvent. 

CH3OH 

13 

.8 

5.38 

5 

•65 

CHaCOOH 

15 

•5 

15 

•7 

18.6 

C2H5OH 

13 

.8 

2.83 

2 

.92 

t4 

23 

17 

.8 

21.6 

C3H7OH 

13 

.8 

2 

2 

C2H5COOH 

•  5 

12 

13.6 

C3H7OH 

73 

43-6 

77 

•3 

" 

15 

•5 

12 

•9 

14  8 

HCOOH 

13 

•5 

9 

9 

•9 

" 

23 

*3 

•45 

15-5 

HCOOH 

•5 

9.6 

10 

•  5 

C3H7COOH 

13 

•  5 

7 

3 

8-3 

CH3COOH 

13 

•5 

15-2 

X7 

•9 

" 

15 

•5 

8. 

2 

8.9 

i oo  gms.  95%  formic  acid  dissolve  1 1.89  gms.  m  dinitrobenzene  at  20.8°.  (Aschan.'is). 
100  gms.  pyridine  dissolve  106.3  Sms.  m  dinitrobenzene  at  2O°-25°.  (Dehn,  1917.) 
100  gms.  50%  aq.  pyridine  dissolve  45.5  gms.  m  dinitrobenzene  at  2O°-25°.  " 


NitroBENZENES 


132 


Solubilities  of  Di-Nitro  BENZENES  and  of  Tri-Nitro  BENZENES  in 
Several  Solvents. 

(de  Bruyn  —  Rec.  trav.  chim.  13,  116,  150,  '94.) 

Grams  per  100  Grams  Solvent. 


Solvent. 

(No62)2; 

(wz) 
(N 

o5)a.' 

(N 

$&§/     <«X*WQ*, 

Methyl  Alcohol 
Ethyl  Alcohol 

20.5 
20.5 

3-3° 

6.75 

3-5 

o 
o 

.69 
•4 

4-9  (16°)   i6.a     (15.5°) 
1-9(16°)     5.45d5.S0) 

Propyl  Alcohol 

20.5 

i 

.09 

•2 

.4 

o 

298 

Carbon  Bi-Sulphide 

i7.6 

0 

.236 

•  i 

•35 

o 

I48 

0.25 

Chloroform 

i7.6 

27 

.  I 

32 

•4 

I, 

82 

6.1 

Benzene 

18.2 

5 

.66 

39 

-45 

a, 

56 

6.2  (16°) 

Ether 

17-5 

.  . 

. 

1-5 

Ethyl  Acetate 

18.2 

12 

.96 

36 

.27 

3- 

56 

Toluene 

16.2 

3 

.62 

3° 

.66 

2. 

36 

.  «  • 

Carbon  Tetra  Chloride 

16.2 

0 

•  143 

I 

.18 

0. 

12 

.  •  • 

Water 

(ord.) 

0 

.014 

'  o 

•0525 

0. 

008 

Symmetrical  Tri-Nitro  BENZENE. 

SOLUBILITY  IN  AQUEOUS  ALCOHOL  AT  25°. 

(Holleman  and  Antusch  —  Rec.  trav.  chim.    13,  296,  '94.) 


Vol.% 
Alcohol. 

G.  C6H3(N03)3(*) 
per  100  g. 
Solvent. 

Sp.  Gr.  of 
Solutions. 

Vol.  % 
Alcohol. 

G.  C6H3(N03)3(5) 
per  100  g. 
Solvent. 

Sp.  Gr.  of 

Solutions. 

100 

2-34 

0-7957 

80 

o-57 

0.8582 

95 

*-S7 

0.8131 

75 

0-47 

0-8708 

90 

1.  12 

0.8288 

70 

0-37 

0.8808 

85 

0-79 

0.8436 

60 

0.23 

0-9064 

See  remarks  under  a  Acetnaphthalide,  p.  13. 

100  gms.  93  vol.  %  ethyl  alcohol  dissolve  2.1  gms.  of  o  CeH^NC^,  3.1  gms. 
m  C6H4(NO2)2  and  0.33  gm.  p  C6H4(NO2)2  at  25°.  (Holleman  and  de  Bruyn,  1900.) 

loo  gms.  of  each'of  the  following  solvents  dissolve  the  indicated  gms.  of  1.2.4 
trinitrobenzene  at  15.5°:  C6H6,  140.8  gms.;  CHC13,  12.87  gms.;  CH3OH,  12.08 
gms.;  (C2H5)2O,  7.13  gms.;  C2H5OH,  5.42  gms;  €82,  0.4  gm.  (de  Bruyn,  1890.) 

Data  for  the  solubility  of  m  dinitrobenzene  in  a  solution  of  nitrobenzene  in 
hexane  are  given  by  Timmermans  (1907). 

Solubility  data,  determined  by  the  freezing-point  method,  are  given  for  mix- 
tures of  o,  m  and  p  dinitrobenzene  with  fluorene,  Kremann  (1911);  with  phen- 
anthrene,  Kremann,  et  al  (1908).  Results  for  mixtures  of  o  and  p  dinitrobenzene 
with  naphthalene,  by  Kremann  and  Rodinis  (1906).  Data  for  m  dinitrobenzene 
with  nitrotoluenes  are  given  by  Giua  (1915)  and  for  m  dinitrobenzene  and  diphenyl- 
amine  by  Giua  (191 5a).  Similar  data  for  mixtures  of  s  trinitrobenzene  with 
xanthone,  quinol,  dimethylpyrone,  5  tribromophenol,  fluorenone,  coumarine, 
and  phenyl  ether  are  given  by  Sudborough  and  Beard  (1911).  Results  for  s 
trinitrobenzene  and  77  dipyridyl  are  given  by  Smith  and  Watts  (1910)  and  for  s 
trinitrobenzene  and  fluorene  by  Kremann  (1911).  Results  for  mixtures  of  m 
dinitrobenzene  and  naphthalene  and  for  1.3.5  trinitrobenzene  and  naphthalene 
are  given  by  Kremann,  (1904)  and  Kurnakov,  Krotkov  and  Oksman  (1915). 

BENZYHYDROL   (C6H6)2CHOR 

Solubility  data,  determined  by  the  freezing-point  method  (see  footnote,  p.  i), 
are  given  for  mixtures  of  benzhydrol  and  phenol  and  for  benzhydrol  and  di- 
methylaniline  by  Schmidlin  and  Lang  (1912). 


133  BENZIL 

BENZIL  CgHsCO.COCeHs. 

Data  for  the  solubility  of  benzil  in  aqueous  ethyl  alcohol  are  given  by  Tim- 
mermans  (1907)  and  by  Kendall  and  Gibbons  (1915).  Data  for  aqueous  solu- 
tions of  benzil  and  phenol,  for  benzil  and  succinic  acid  nitrile  and  for  benzil  and 
triethyl  amine  are  given  by  Timmermans  (1907). 

SOLUBILITY  DATA,  DETERMINED  BY  THE  FREEZING-POINT  METHOD  (see 
footnote,  p.  i),  ARE  GIVEN  FOR  THE  FOLLOWING  MIXTURES: 

Benzil  +  Dibenzyl  (Vanstone,  1913.) 
+  Azobenzene 
-|-  Stilbene  " 

4-  Hydrobenzoin  " 

-j-  Benzoin  (Beurath,  1912-13;  Vanstone,  1909.) 

-j-  Benzoic  acid  (Kendall  and  Gibbons,  1915.) 

BENZINE     (Petroleum)  C5H12C6H14. 

100  parts  of  alcohol  dissolve  about  16  parts  benzine  of  0.638  — • 
0.660  Sp.  Gr.,  at  25°. 

BENZOIO    ACID     C6H5COOH. 

SOLUBILITY  IN  WATER. 

(Bourgoin  —  Ann.  chim.  phys.  [5]  15,  171,  '78.) 

Grams.  C6HsCOOH  Grams.  C«HsCOOH 

t<^  per  100  Gms.  t°.  per  100  Gms. 

Water.         "  Solution."  'Water.  Solution. 

o  0.170  0.170  40  °-555  0-551 

10  0.210  0.209  50  o-775  0.768 

20  0.290  0.289  60  I-I55  1-142 

25  0.345  0.343  80  2.715  2.643 

30  0.410  0.408  100  5-875  5-549 

100  grams  saturated  aqueous  solution  contain  0.25  gm.  C6H5COOH  at  15°; 
0.3426  gram  at  25°;  0.353  gram  at  26.4°;  0.667  gram  at  45°;  5.875  gms.  at 
100°. 

(Paul,  1894;  Noyes  and  Chapin,  1898;  Greenish  and  Smith,  1903;  Hoffman  and  Langbeck,  1905;  Lums- 
den,  1905;  Philip,  1905;  see  also  Alexejew,  1886;  Ost,  1878;  Vaubel,  1895;  Freundlich  and  Seal,  1912.) 

SOLUBILITY  OF  MIXTURES  OF  LIQUID  BENZOIC  ACID  AND  WATER. 

(Alexejew.) 

Determinations  by  "Synthetic  Method,"  see^Note,  p.  16.  Figures  read  from 
curve. 

Gms.  C6H5COOH  per  100  Gms.  Gms.  C6HsCOOH  per  too  Gms. 

Aq.  Layer.    Benzoic  Ac.  Layer.  Aq.  Layer.  Benzoic  Ac.  Layer. 

70        6  83  ioo  12.0  69.0 

80        7.5  79.5  no  18.0  59.0 

90        8.5  76  116  (crit.  temp.)    35 

SOLUBILITY  OF  BENZOIC  ACID  IN  AQUEOUS  SOLUTIONS  OF: 

(Hoffman  and  Langbeck.) 

Potassium  Chloride  at  25°.  Potassium  Nitrate  at  25°. 


Nor- 
mality 

Gms. 
KC1. 

Dissolved  C6H5COOH. 

Nor- 
mality 

Gms. 
KN03 

Dissolved  C6H5COOH. 

of  Aq. 
KC1. 

per 
Liter. 

Mol  .  Cone  .       Wt  .  per  cent  . 

of  Aq. 
KN03 

per 
Liter. 

Mol.  Cone 

Wt.  per  cent. 

0.02 

I. 

49 

5.0254-IO"4 

0. 

339 

0.02 

2.02 

5 

.0326-10—* 

0.340 

0.05 

-3- 

73 

4.9801       " 

o. 

333 

0.05 

5.06 

5 

.0421 

tt 

0.341 

O.2O 

14. 

92 

4-7639 

o. 

322 

O.2O 

2O  .24 

5 

.0297 

K 

0.340 

0.50 

37- 

3° 

4.3632 

O- 

295 

0.50 

5°  -59 

4 

.9400 

ft 

°-334 

I-  00 

101.19 

4 

.7646 

" 

0.322 

BENZOIC  ACID 


134 


SOLUBILITY  OF  BENZOIC  ACID  IN  AQUEOUS  SOLUTIONS  OP: 

(Hoffmann  and  Langbeck.) 


Nor- 
mality 

of  Aq. 

NaCl. 

o.oo 


Gms. 

NaCl 

per 

Liter. 


0.02 
0.05 
O-2O 
0.50 
1. 00 


Sodium  Chloride. 

Gms.  C6H5COOH 
per  100  Gms.  Sol. 

at  25°. 
0.340 

o-339 
0-335 
o-336 
0.282 


Sodium  Nitrate. 


at  45°. 
0-667 
0.663 
0.654 
0.617 
0.546 
0-449 


o.oo 

1.17 

2-93 
11.70 
29.25 
58-50 

SOLUBILITY   OF   BENZOIC  ACID   IN  AQUEOUS   SOLUTIONS   OF  SODIUM 
ACETATE,  FORMATE,  BUTYRATE,  AND  SALICYLATE. 

(Noyes  and  Chapin  —  Z.  physik.  Chem.  27,  443,  '98;  Philip  —  J.  Ch.  Soc.  87,  992,  '05.) 


Nor- 
mality 
of  Aa 

Gms. 
NaN03 
T)PT 

Gms.QHgCOOH 
per  zoo  Gms.  Sol. 

NaN03. 

pel 
Liter. 

at  25°. 

at  45°. 

O.O2 

1.70 

0-340 

0.666 

O.O5 

8-51 

0-339 

0.663 

O.20 

17  .02 

o-333 

0.647 

0.50 

42-54 

0.319 

0.613 

1.  00 

85.09 

0.294 

Grams 

Gram 

s  C6H5COOH 

per  Liter  of  S< 

A 

Dlution  in: 

Sodium 
Salt  per 
Liter. 

CH3COONa. 

HCOONa. 

CaH7COONa.  C^OH.COONa. 
At  26.4°.            At  26.4°. 

At  25°. 

At  26.  46. 

At  25°. 

At  26.4°.' 

0 

3-4i 

3-53 

3-41 

3-53 

3-53 

3-53 

I 

4-65 

4-75 

4-25 

4-35 

4-5o 

3-62 

2 

5-7o 

5-85 

4-75 

4-85 

5-40 

3-7o 

3 

6.70 

6.90 

5.20 

5-3o 

6-15 

3.80 

4 

7.60 

7-85 

5-6o 

5-70 

6.90 

3-87 

6 

8.40 

4.00 

8 

... 

4.10 

SOLUBILITY  OF  BENZOIC  ACID  IN  AQUEOUS  SOLUTIONS  OF  SODIUM  MONO- 
CHLORACETATE,  SODIUM  SUCCINATE  AND  POTASSIUM  FORMATE  AT  25°. 

(Philip  and  Garner,  1909.) 
In  Aq.  (CH2COONa)2. 

Gms.  per  Liter  Solution. 
(CH2COONa)?.    CeHsCOOH". 
3-38 
4.087 


In  Aq.  CH2ClCOONa. 

Gms.  per  Liter  Solution. 
CHzClCOONa.'    CeHsCOOH.' 
3-38 
3.684 


O 

1-375 

3.426 

6.839 

13.710 


4.026 
4.417 
4.929 


o 

1.182 

2.932 

5-848 

11.730 


In  Aq.  HCOOK. 

Gms.  per  Liter  Solution. 

HCOOK.      'CeHoCOOH. 
3-38 
4.087 


O 

1.025 


5.II2 
6.564 
9.005 


5.124 


4-734 
5-503 


The  authors  also  obtained  data  for  the  solubility  of  benzoic  acid  in  aqueous 
solutions  of  sodium  acetate  and  sodium  formate  which  agree  closely  with  those 
quoted  in  the  second  table  above. 

ioocc.90%ethylalcoholdissolve36.i  gms.  C6H5COOHat  i5.5°.(Greenish&Smith,'o3.) 

100  cc.  of  a  i.o  n  aqueous  solution  of  aniline  hydrochloride  dissolve  0.537  Sm- 

C6H6COOH  at  25°.  (Sidgwkk,  1910.) 

SOLUBILITY  OF  BENZOIC  ACID  IN  AQUEOUS  SOLUTIONS  OF  ETHYL  ALCOHOL 

AT  25°. 

(Seidell,  1908,  1910.) 


wt.  % 

C2H8OH 
in  Solvent. 

Sp.  Gr.  of 

Sat.  Sol. 

Gms.  per  too  Gms  Sat. 
Sol. 

Wt.  % 
C2H5OH 

n  Solvent. 

Sp.  Gr.  of 
Sat.  Sol. 

Gms.  per  100  Gms.  Sat. 
Sol. 

C2HsOH. 

CeHsCOOH.    ' 

C2H6OH.     CaHsCOOH. 

0 

I 

O 

0.367 

60 

0-943 

45-72 

23.80 

IO 

0.985 

9-94 

O.OO 

70 

0.940 

49.21 

29.70 

20 

0.970 

19.66 

1.70 

80 

0-934 

52-8 

34 

30 

0-959 

28.83 

3-90 

90 

0.922 

57-6 

36 

40 

0.951 

36.36 

9-IO 

IOO 

0.908 

63-1 

36-9 

50 

0.946 

41.50 

17 

135  BENZOIC  ACID 

SOLUBILITY  OF  BENZOIC  ACID  IN  90%  ALCOHOL,  IN  ETHER  AND  IN  CHLOROFORM. 

ABourgoin.) 

0  Cms.  C6HsCOOH  per  TOO  Grams. 

'Solvent.  Solution/ 

90%  Alcohol  15  41.62  29.39 

Ether  15  31.35  23.86 

Chloroform  25  14-30  12.50 

SOLUBILITY  OF  BENZOIC  ACID  IN  SEVERAL  ALCOHOLS.    (Timofeiew,  1894.) 


Alcohol. 

Cms.  CeHsCOOH  per  100  Gm: 

-'         Alcohol.              t°.GmS 

CeHsCOOH  per  100  Gms. 
Sat.  Sol.      Solvent. 

• 

Sat.  Sol. 

Solvent. 

Methyl 

-18 

23.1 

3° 

Propyl              —  18 

14-5 

16.9 

(4 

-13 

24-3 

32.1 

-13 

15-7 

18.5 

<( 

+  3 

33-5 

50-4 

+  3 

23.1 

30 

it 

19.2 

40.1 

67.1 

19.2 

28.2 

39-3 

ll 

23 

4i-7 

71-5 

23 

29.8 

42.3 

Ethyl 

—  18 

20.3 

25-4 

Isopropyl            21.2 

32-7 

48.5 

« 

-13 

21.2 

26.9 

Allyl                   21.2 

25.1 

33-4 

« 

+  3 

28.8 

40.4 

Isobutyl               o 

15-3 

18 

M 

19.2 

34-4 

52.4 

Isoamyl              18 

2O.  2 

25-4 

« 

23 

35-9 

55-9 

Capryllic            21.2 
Ethyleneglycol  18 

22.7 

8 

28.7 
8.69 

Additional  data,  agreeing  closely  with  the  above,  are  given  by  Timofeiew 
(1891)  and  Bourgoin  (1878),  .,-,'. 

SOLUBILITY  OF  BENZOIC  ACID  IN  AQUEOUS  SOLUTIONS  OF  DEXTROSE. 

(Hoffman  and  Langbeck.) 

Normality  of      Gms.  C6Hl2Oa  ^solved  C^COOH  at  25°,         Dissolved  CeH.COOH  at  45*. 

Aq.  Dextrose,          per  Liter.  Mol.  Cone.  p^Cent.  Mol.  Cone.  p^St 

0.02  3.67  5.0322.10"*        0.34        9-9o88.io~4    0.674 

0.05  9-00  5-0403    "  0-34  9-9328    "  0.669 

0.204         36-73  5-0303  l(  0.34        9-9323  "          0.669 

o-533          96-J5  5-0321  "  0.34      10.0101  '  0-674 

i. 068        192.30  5-0443  "  0-341     10-0369  "          0.676 

SOLUBILITY  OF  BENZOIC  ACID  IN  AQUEOUS  SOLUTIONS  OF  UREA  AND  OF  THIO  UREA. 

(Hoffman  and  Langbeck.) 

Normality  Gms.  CpHsCOOH  Dissolved  at  25°. 

of  Solution.  per  Liter.  Mol.  Cone.     Wt.  per  cent! 

In  Aqueous  Urea  o.io       6.01  CO(NH2)2      5.i876.io~4     0.350 

In  Aqueous  Thio  Urea    0.20      15 .23  CS(NH2)2       5-4994    "         0.372 

Data  for  the  system  benzoic  acid,  succinic  acid  nitrile  and  water  are  given  by 
Schreinemakers,  1898,  and  for  the  system  benzoic  acid,  phenol  and  water  by 
Timmermanns,  1907. 

SOLUBILITY  OF  BENZOIC  ACID  IN  BENZENE  AND  VICE  VERSA.    (Roioff,  1895.) 

,o       Gms.  CeHsCOOH  per         „  ,.,  p.  xo    Gms.  C«HsCOOHper  c  ,. .  p. 

t  •         ioo  Gms.  Sat.  Sol.  Solld  Phase'  *  '     100  Gms.  Sat.  Sol.    Solld  Phase' 

5.37  o  C6H6                  20           8.8      C6H5COOH 

5  1-75  30  13 

4-50  3-95  50  25 

4.20  5  C6H6+C6H5COOH        70  43.5 

5  5.05  C6H5COOH             90  64 

7  5-50  no  91.5 

9  5.70  121  ioo 

ii  6 

Von  Euler  and  Lowenhamn  (1916)  found  7.76  gms.  C6H5COOH  per  ioo  cc.  of  sat. 
solution  in  benzene  at  25°,  and  7.76  gms.  C6H5COOH  +  2.50  gms.  C6H4OHCOOH 
o  per  ioo  cc.  of  benzene  solution  saturated  with  both  acids. 


BENZOIC   ACID 


136 


SOLUBILITY  OF  BENZOIC  ACID  IN  ORGANIC  SOLVENTS. 


Gms. 

Gms 

Solvent. 

to          CeHsCOOH 
per  100  cc.  Sat 
Sol. 

Solvent. 

t°. 

Sat 

Solution. 

CsHsCOOH 
per  loo  Gms. 
Sat.  Sol. 

Aq.  75%  Acetic  Acid 

14-16 

10.92  (i) 

Amyl  Alcohol 

25 

0.875 

32.37 

(6) 

Benzene 

14-16 

7.04   (i) 

Amyl  Acetate 

25 

0.912 

22 

(6) 

Carbon  Disulfide 

14-16 

4-24  d) 

Alcohol  (Abs.) 

25 

0.908 

58.40 

(6) 

Carbon  Tetrachloride  14-16 

4-50  ( 

i) 

Benzene 

25 

0.897 

12.23 

(6) 

H 

25 

6.70  (2) 

Chloroform 

25 

1.456 

I5-I4 

(6 

" 

26 

6.58  (3) 

Carbon  Tetrachloride  25 

1.564 

4.l8 

(6 

Chloroform 

25 

18.03  (2) 

Carbon  Disulfide 

25 

1.282 

4.82 

(6 

Ethyl  Ether 

14-16 

39.80  (i) 

Cumene 

25 

0.906 

8-59 

(6 

Glycerol 

15-16 

9-07*(4) 

Ethyl  Ether  (Abs.) 

25 

.  .  . 

46.74 

(6) 

Ligroin 

14-16 

0.72  (i) 

Ligroin 

25 

0.720 

i-75 

(6 

Petroleum  Ether  f 

26 

0.98  (3) 

Naphtha  • 

25 

0.730 

2.65 

(6 

Pentachlor  Ethane 

25 

10.92  (2) 

Nitrobenzene 

25 

1.225 

10.05 

(6 

Tetrachlor  Ethane 

25 

I5-I7 

2) 

Toluene 

25 

0.884 

10.69 

(6 

Tetrachlor  Ethylene 

25 

8.06 

2) 

Spts.  Turpentine 

25 

0.859 

5-09 

(6) 

Trichlor  Ethylene 

25 

13.62 

2) 

Water 

25 

I 

0.368(6) 

it 

IS 

6-44*(5) 

Xylene 

25 

0.877 

9.71 

(6) 

Dichlor  Ethylene 

15 

9-67*(5) 

Gms.  CeHsCOOH  per  100  gms.  sat.  sol. 


t  (B.  pt.  30-70.) 


(i)  Bomwater  and  Holleman  (1912);   (2)  Herz  and  Rathmann  (1913);   (3)  de  Jong  (1909);  (4)  Ossen- 
dowski  (1907);  (5)  Wester  and  Bruins  (1914);  (6)  Seidell  (1910). 

One  liter  sat.  sol.  of  benzoic  acid  in  ethyl  acetate  contains  8  gms.  at  —6.5°, 
37.7  gms.  at  21.5°  and  95.7  gms.  at  75°.  (Lloyd,  1918.) 

SOLUBILITY  OF  BENZOIC  ACID  IN  MIXTURES  OF  ORGANIC  SOLVENTS  AT  25°. 

(Harden  and  Dover,  1916.) 

Mixtures  of  Ethyl  Ace- 
tate +  Benzene. 

Gms.  CeHsCOOH 

per  zoo  Gms. 

Solvent. 

ii. 6 

14 
16.5 

20 

2O.4 
22 
23-9 


Mixtures  of  Ether 

Mixtures  of  Acetone 

+  Chloroform. 

+  Benzene. 

%  CHClj*  in 
Solvent. 

Gms.  CsHsCOOH 
Solvent. 

%  CeHo  in 
Solvent. 

Gms.  CeHsCOOH 
per  loo  Gms. 
Solvent. 

100 

38.4 

100 

ii.  6 

90 

34 

QO 

18.3 

80 

30.1 

80 

24.1 

70 

26.6 

70 

31 

60 

23.2 

60 

33-5 

50 

20.8 

50 

37 

40 

18.6 

40 

42.2 

30 

16.8 

30 

47 

20 

15-6 

20 

49 

10 

i5-2 

IO 

Si-3 

0 

15.0 

0 

55-6 

Solvent. 

IOO 
QO 
80 
70 
60 
50 
40 

30  26.5 

20  29 

10  28.2 

o  41.2 

*  This  is  probably  a  mistake  in  the  original  and  should  be  %(CzHs)£>  in  Solvent. 

SOLUBILITY  DATA,  DETERMINED  BY  THE  FREEZING-POINT  METHOD  (see  footnote, 
p.  i),  ARE  GIVEN  FOR  MIXTURES  OF  BENZOIC  ACID  AND  EACH  OF  THE  FOL- 
LOWING COMPOUNDS: 

°n  CUor0^icA<!d Un^ter  and  Holler,  «£"£»          ™^ta*  ^ 

p  "  "I      I9I2>)  Salicylic  Acid  Qaeger,  1907.) 

m  Nitrobenzoic  Acid  (Bakunin  and  Angrisani,  1915.)  Succinic  Acid  Nitrile  (Schreinemakers,  1898.) 

Benzil  (Kendall  and  Gibbons,  1915.)     Sulfuric  Acid  (Kendall  and  Carpenter,  1914.) 

Camphor  (Joumiaux,  1912.)  o  Toluic  Acid  (Kendall,  1914.) 

Cinnamic  Acid         (Kachler,  1870;  Kendall,  1914.)  o  Toluidine  (Baskov,  1913.) 

Dimethylpyrone       (Kendall,  1914.)  p  (Baskov,  1913;  Vignon,  1891.) 

Fluorobenzoic  Acid  (Koopal, 


137 


BENZOIC  ACID 


DISTRIBUTION  OF  BENZOIC  ACID  BETWEEN  WATER  AND  BENZENE: 


At  10°. 

(Hendrixon,  1897.) 

At  20°. 
(Nernst,  1891.) 

At  25°. 

(Farmer,  1903.) 

At  40°. 
(Hendrixon,  1897.) 

Cms.  CeHsCOOH 
per  100  cc. 

Cms.  CeHsCOOH 
per  zoo  cc. 

Cms.  CsHsCOOH  per  100  cc. 

Cms.  CeHsCOOH  per 

100  CC. 

H20. 

C«H« 

'H2O. 

C6H6. 

H2O  Laver. 

C«H6 

H2O 

CeH«     " 

Lciycr. 

Layer. 

Layer. 

Layer. 

Layer. 

Layer. 

Lciycr. 

0.0215 

0.0725 

0.0163 

0-0535 

0.2002 

(0.1885*) 

3-33S 

0.0238 

0.0714 

0.0412 

0.2363 

0.0244 

0.099 

O.2OI2 

(0.1891*) 

3-329 

o  .  0404 

0.1637 

0.0562 

0.4422 

0.0452 

0.273 

0.2020 

(0.1902*) 

3.319 

0.0837 

0.5740 

o  .  0890 

1.0889 

0.0788 

0-737 

O.H5S 

1.0269 

0.1215 

2.0272 

0.1500 

2.42 

0.1715 

2.1420 

o  .  1409 

2.7426 

0.2890 

9.70 

k     •  • 

i 

0.2313 

3-9167 

unionized. 

DISTRIBUTION  OF  BENZOIC  ACID  BETWEEN  BENZENE  AND  AQUEOUS 
POTASSIUM  BENZOATE  SOLUTIONS  AT  25°. 

(Farmer,  1903.) 

Cms.  CeHsCOOK  Qms.  CeHsCOOH  per  liter. 

per  Liter  Aq.         

Sol.  Aq.  Layer.         C6H6  Layer. 

33-88 
33-79 
33-71 


Gms.  Mols. 
CeHsCOOK  per 
Liter  Aq.  Sol. 

O.OOQ3 
0.028 
0.047 

Gm.  Mols.  CeHsCOOH  per  Litei 

Aq.  Layer. 
0.01587 
O.OIS97 
0.01603 

CsHe  Layer. 
0.2776 
0.2768 
0.2762 

1.341  1.937 
4.035  1.950 
6.774  1.956 

DISTRIBUTION  OF  BENZOIC  ACID  BETWEEN: 
Water  and  Chloroform.  (Hendrixon,  1897.)         Water  and  CC14. 

At  40°. 

Gms.  CeHsCOOH  per  too  cc. 


At  10' 
Gms.  CsHsCOOH  per  too  cc. 


H2O  Layer. 
O.O2O8 


CeHe  Layer. 
0.0880 


(Seidell,  igioa.1) 
At  25°. 

Gms.  CeHsCOQH  per  100  cc. 

HzO  Layer.        CCU  Layer." 
0.134  0.830 

0.291  4.41 


CeHe  Layer.  H:zO  Layer. 

O.O9I5  0.0258 

0.0269     0.1518  0.0432     0.2059 

0.0327     0.2170  0.0885     0.6961 

0.1057      2.0930  0.1553     2.0435 

The  coefficient  of  distribution  of  benzoic  acid  between  olive  oil  and  water  at 
25°  is  given  by  Boeseken  and  Waterman  (1911)  as  12.6. 


AminoBENZOIC  ACID   (o)  C6H4.NH2.COOH. 

SOLUBILITY  OF  o  AMINOBENZOIC  ACID  IN  WATER. 


(Lunden,  1905-06.) 


Sp.  Gr.     Gms.  C6N4NH2COOH(o) 
Sat.  Sol.       per  100  cc.  Sat.  Sol. 


25 

26.1 

28.1 


0.999 


0.519 
0-540 
0.570 


t°. 

Sp.  Gr. 
Sat.  Sol. 

Gms. 
CeH4NH2COOH(0) 

per  100  cc.  Sat.  Sol. 

34-9 

0.998 

0.731 

35 

0.997 

0.744 

39-8 

0.997 

0.889 

SOLUBILITY  OF  AMINOBENZOIC  ACID  IN  AQUEOUS  SALT  SOLUTIONS  AT  25°. 

(Lunden,  1905-06.) 

Gms. 

Normality  of  Salt 
Solution. 


SPo<*r-    CeH4NlScOOH(0)  Normality  of 
Solution. 


0.768  iBa(N03)2 

0.507 

0.3427 

0.1780 

0-IS4S 


1.080 
1.052 
1.037 
1.018 
1.015 


Sat.  Solution. 
0.634         2.633 

0.603      i-372 

0.598 
1.853 

0.946 
0.560 


0-585 
0.555 
0.549 


lity  of 
It 
ion. 

Sp.  Gr. 

Sat. 
Solution. 

CeH4NH2- 
COOH(o) 
per  100  cc. 
Sat.  Sol. 

KNOj 

1         I  -155 
1.083 

0.501 
0-544 

I-°33 

0-549 

KI 
tt 

(C 

I.  221 
I  .114 
1.  068 

0.541 
0-559 
0-550 

The  author  also  gives  additional  data  for  aqueous  salt  solutions  at  28.1°. 
Additional  data  for  the  solubility  of  aminobenzoic  acid  in  aqueous  salt  solu- 
tions are  given  by  Euler  (1916). 


AminoBENZOIC   ACIDS 


138 


AminoBENZOIC  ACID   C6H4.NH2.COOH  (w). 

SOLUBILITY  IN  WATER  AND  IN  OTHER  SOLVENTS. 

(de  Coninck  —  Compt.  rend.  116,  758,  '93.) 


In  Water. 


Gms. 
t°.    C6H4.NH3.COOH(m) 
per  100  cc.  HjO. 

0 

o-43 

10 
20 
30 

0.52 
0.67 
0.87 

40 

i-i5 

SO 
60 

1.50 
2.15 

70 

3-15 

In  Organic  Solvents. 

Gms. 

Solvent.  t°.       C«H4.NH2.COOH(m) 

per  100  cc.  Solvent. 

Ethyl  Alcohol  (95  °/0 )  12.5  2.92 

Methyl  Alcohol  (pure)  10.5  4.05 

Acetone  11.3  6.22 

Methyl  Iodide  10-0  0.04 

Ethyl  Iodide  o-o  0.02 

Chloroform  12.0  0.07 

Bromoform  8.0  trace 


MUTUAL  SOLUBILITY  OF  AMINOBENZOIC  ACIDS  AND  WATER  AT  HIGH  TEMPERA- 
TURES, DETERMINED  BY  THE  SYNTHETIC  METHOD. 

(Flaschner  and  Rankin,  1910.) 

Mixtures  of  m  Acid 
and  H2O. 

t°  of  Gms.  m  Acid  p 

Melting.       100  Gms.  Mixt 

66  crit.  sol.  temp. 


4.8 
9.9 

18.5 
30.6 

38 
49.4 

59-4 
69.7 
80 

87.2 

95 
100 


Mixtures  of  p  acid  and 
H2O. 

t°  of          Gms.  p  Acid  per 
Melting.      100  Gms.  Mixture 

47  crit.  sol.  temp. 


MIXTURES  OF  o  ACID 
and  H2O. 

t°  of  Gms.  o  Acid  per 

Melting.      100  Gms.  Mixture. 

83.6 

95-8 
101.4 
103.4 
104.4 

105 

105.6 

107.8 

112 

Il6.2 

128.4 

144.6 

/°  reading,  for  critical  saturation  and  for  separating,  also  given  in  the  case  of  the 
o  acid. 

Data  for  the  distribution  of  o  aminobenzoic  acid  between  water  and  benzene 
at  25°  are  given  by  Farmer  and  Warth  (1904). 


77.8 

4-6 

82.2 

5 

90 

5-8 

90 

7-1 

100 

9-7 

100 

iS-8 

no 

20.2 

105 

22 

120 

51-2 

no 

32.3 

130 

73-7 

116 

SI.8 

140 

83.7 

120 

62 

ISO 

90.7 

130 

77 

160 

95-8 

150 

91.1 

170 

99-2 

170 

98 

174-4 

100 

186 

100 

AminonitroBENZOIC  ACIDS  C6H3.NO2.NH2.COOH  o,  m  and  p. 

SOLUBILITY  OF  THE  THREE  ISOMERIC  AMINONITROBENZOIC  ACIDS: 
In  Ether. 


Gms.  C6H3.N02.NHj.COOH  per 
100  cc.  Ether. 


In  Ethyl  Alcohol  (90%). 
Gms.  CeH3N02.NH2.COOH  per 
100  cc.  Alcohol. 


2.7 
5-8 


Ortho. 
10.84 
16.05(6.8°) 


Meta. 
1.70 


Para. 
6.41 
8.21 


3 
9.6 


Ortho. 

8.13 

10.70 


Meta.  Para. 

1.79  8.4 

2.20         II.3 


SOLUBILITY  IN  WATER  OF  THE  THREE  ISOMERIC: 

(Vaubel,  1895.) 
Aminobenzo  Sulphonic  Acids.  Amino  Phenols. 

G.  qifr.NHt.SOiH^per  100  G.  Aq.  Sol.  o       G.  CrfMOH)  .NH2  per  too  G.  Aq.  Sol. 


Ortho. 
1. 06 


Meta.  Para. 

1.276        0.592(6°) 


Ortho. 


Meta. 
2.6(20°) 


Para. 
I.I 


139  BENZOIC  ACIDS 

Brom,  Chlor  and  lodoBENZOIC  ACIDS. 

SOLUBILITY  IN  WATER  AT  25°.       (Paul,  1894;  Lowenherz,  1898;  Vaubel,  1895.) 

_          ,  Per  1000  cc.  Aqueous  Solution. 

Compound.  Formula.  /— -*- » 

Grams.  Gram  Mol. 

Brombenzoic  Acid     Cel^Br.COOH  (ortho)  1.856  0.00924 

Brombenzoic  Acid     CeH4Br.COOH  (meta)  0.402  0.00200 

Brombenzoic  Acid     CeHiBr.COOH  (para)  0.056  0.00028 

Chlorbenzoic  Acid     CettiCl.COOH  (ortho)  2 . 087  o . 01333 

lodobenzoic  Acid       CeKJ .  COOH     (ortho)  0.952  o .  003  84 

lodobenzoic  Acid       CeKJ.COOH     (meta)  0.116  0.00047 

lodobenzoic  Acid       CeELJ.COOH     (para)  0.027  (Koopoi,  1912.) 

The  following  results  at  28°.    (Sieger,  1912.) 

Chlorobenzoic  acid    C^CICOOH   (ortho)  2.25 

(meta)  0.45 

(para)  0.093 

MUTUAL  SOLUBILITY  OF  BROMO  AND  CHLOROBENZOIC  ACIDS  AND  WATER  AT  HIGH 

TEMPERATURES,  DETERMINED  BY  SYNTHETIC  METHOD.^FiasdmerandRankin,  1910.) 

p  Bromobenzoic        o  Chlorobenzoic          m  Chlorobenzoic       p  Chlorobenzoic 

Acid  +  Water.  Acid  +  Water.  Acid  +  Water,  j         Acid  +  Water. 

j.o  Qf        Gms.  Acid          f.0  Qf  Gms.  Acid  ^.0  Qf  Gms.  Acid       *0  nt       Gms.  Acid 


170  (Crit.  sol.  temp.)  IOO  . 

169     3    102  , 

8     5.5 
,7    10 

123 
123.8 

4.2 

18.9 

167  (crit.  t) 

162    3 

180 

6.2 

104 

20 

I42.8(crit.t.)34.3 

170 

5-4 

190 

10-5 

126 

.2(crit.  1034.9 

123.8 

75-8 

180 

10 

196 

27 

104 

76 

125 

81.5 

183 

14-5 

2OO 

61 

no 

85.3 

130 

87.5 

184 

21.5 

210 

80 

120 

92 

140 

93-2 

187. 

47 

22O 

88.3 

130 

96.5 

150 

97-5 

200 

79-5 

240 

96.9 

139 

5    loo 

156 

IOO 

220 

92 

254 

IOO 

240 

IOO 

SOLUBILITY  OF  ORTHOCHLOROBENZOIC  ACID  IN  AQ.  SOLUTIONS  OF  SODIUM  ACE- 


TATE, SODIUM  FORMATE  AND  POTASSIUM  FORMATE  AT  25°.  (Philip  and  Garner,  1909.) 
In  Aq.  CH3COONav                In  Aq.  HCOONa.                   In  Aq.  HCOOK. 

Grams  per  Liter.                                   Grams  per  Liter.                                 Grams  per  Liter. 

CHaCOONa. 
1.009 
2.484 
5.027 
10.07 

CeH4ClCOOH. 
3-599 

6.181 

15.60 
18.27 

HCOONa. 
0.843 
2.IO2 
4.196 
8.410 

C6H4C1COOH." 
3.381 
5.258 

7.637 
11.02 

HCOOK. 
0 
1.025 

2.563 
5.124 

C6H4C1COOH. 
2.128 

3.396 
5.226 

7-543 

SOLUBILITY  OF  CHLOROBENZOIC  ACIDS  IN  SEVERAL  SOLVENTS  AT  14-16°. 

(Bornwater  and  Holleman,  1912.) 

Gms.  per  100  cc.  Sat.  Solution. 
Solvent.  i -*- — — ^ 


0C«H4C1COOH.  m  CoHiClCOOH.  p  CeH4ClCOOH. 

Ligroin                                  0.07  0.084  trace 

Carbon  Tetrachloride           0.58  o .  48  o .  04 

Benzene                                0.92  0.66  0.017 

Carbon  Disulfide                  0.52  0.62  0.016 

75%  Aq.  Acetic  Acid           6 . 22  ...  0.32 

Ethyl  Ether                         16 . 96  14  1.72 

Acetone                               28.42  ...  2 . 58 

Ethyl  Acetate                     13 . 20  ...  i .  64 

Freezing-point  data  are  given  by  Bornwater  and  Holleman  (1912)  for  mix- 
tures of  o,  m  and  p  Chlorobenzoic  acids. 


BENZOIC  ACIDS 


140 


FluoroBENZOIC  ACIDS   C6H4FCOOH. 

100  cc.  aqueous  solution  saturated  at  32°  contain  0.882  gm.  o 

"       0.308    "     m 
"       0.107    "     p 

(Slothouwer,  1914.) 

lodoBENZOIC  ACID   p  CeHJCOOH. 

MUTUAL  SOLUBILITY  OF  PARA  IODOBENZOIC  ACID  AND  WATER  AT  HIGH  TEM- 
PERATURES DETERMINED  BY  THE  SYNTHETIC  METHOD. 

(Flaschner  and  Rankin,  1910.) 


t°of 
Melting. 

175  crit.  sol.  t. 

178 

190 
200 


Gms.  Acid  per 
100  Gms.  Mixture. 


3 

5-8 
10 


t°  of  Gms.  Acid  per 

Melting,  zoo  Gms.  Mixture. 

207  22 

210  41 

215  63.5 

220  77 


t°  pf         Gms.  Acid  per 
Melting.  100  Gms.  Mixture 

230  87.4 

240  92.7 

269  98 . I 

270  ioo 


p  lodo  Bromo  and  ChloroBENZOIC  ACID   Methyl  Esters. 

FREEZING-POINT  DATA  (Solubility,  see  footnote,  p.  i)  ARE  GIVEN  FOR  THE 
FOLLOWING  MIXTURES. 

Qaeger,  1906.) 

p  Chlorobenzoic  methyl  ester  +  p  Bromobenzoic  methyl  ester. 

-j-  p  lodobenzoic 
p  lodobenzoic  "     +  P  Bromobenzoic 

HexahydroBENZOIC  ACID   CH2(CH2.CH2)2.CH.COOH. 

ioo  gms.  H2O  dissolve  0.201  gm.  of  the  acid  at  15°,  d.  saturated  solution  =  1.048. 

(Lumsden,  1905.) 

HydroxyBENZOIC  ACIDS   m  and  p  (o  =  Salicylic  Acid,  see  p.  588). 

SOLUBILITY  OF  META  AND  PARA  HYDROXYBENZOIC  ACIDS  IN  WATER, 

BENZENE,  ETC. 
(Walker  and  Wood,  1898.) 


In  Water. 


In  Benzene. 


Gms.  CeHvOH.COOH 
t°.                   per  ioo  Gms.  H2O. 

Meta. 

Para. 

10 

o-55 

0-25 

20 

0.90 

0.50 

25 

1.  08 

0.65 

30 

i-34 

0-81 

35 

1.64 

I  .01 

40 

2.10 

1.24 

5° 

3.10 

2.12 

00 

80 

.  .  . 

Gms.  CoH4.OH.COOH 

Meta. 

Para. 
O.OOlS 

0.008 

0.0027 

o.oio 

0.0035 

O.OI2 
0.015 
0.017 
0.028 

0.0045 
O.OO6O 
0.0082 
0.0162 

0.047 

0.028 
0.066 

In  Acetone. 

G.  CeH4.OH.COOH 
per  ioo  cc.  Sol. 

Meta.  Para. 

26.0  22-7 


te. 


In  Ether. 

G.  C8H4.OH.COOH 
per  loo^  cc.  Sol. 


Meta. 

9-73 


Para. 

9-43 


ioo  gms.  sat.  sol.  in  H2O  contain  0.7    gm.  m  acid  at  15°  and  4  gms.  at  50°. 
"          "      "     "     "          "       044  "     p    "      "    "      "2.98"      "    " 
4i      „     „  CH3OH  «     53  5g   «    m    «      «    « 

'    236.22    "      p     '  (Savorro,  1914-) 

"        95%  formic  acid  dissolve  2.37  gms.  m  acid  at  20.8°.  (Aschan,  1913.) 


141 


BENZOIC  ACIDS 


MUTUAL  SOLUBILITY  OF  META  AND  PARA  OXYBENZOIC  ACIDS  AND  WATER  AND 
OF  PARAMETHOXYBENZOIC  ACID  AND  WATER  AT  HIGH  TEMPERATURES,  DE- 
TERMINED BY  THE  SYNTHETIC  METHOD. 

(Flaschner  and  Rankin,  1910.) 


Meta  Oxybenzoic  Acid 

Para  Oxybenzoic  A 

+H20. 

+H20. 

t°of 
Melting. 

Cms.  Acid  per 
100  Gms. 
Mixture. 

t°of 
Melting. 

Gms.  Acid  p 
loo  Gms. 
Mixture. 

78.2 

9-9 

77 

10 

Q0.8 

20 

90 

19.8 

98 

30 

97-4 

29-5 

103.2 

39-8 

104.4 

40.1 

108.8 

49 

in.  8 

50 

119.2 

60 

1  20 

59-6 

I3I-4 

70 

134 

69.2 

143-4 

77-9 

154-4 

80 

175-6 

90.8 

180.6 

90.4 

199.8 

IOO 

213 

IOO 

Para  Methoxy  benzole 

Acid  + 

H20. 

t°of 
Melting. 

Gms.  Acid  per' 
zoo  Gms. 
Mixture. 

138.2 

crit.  sol.  t. 

140 

9 

142 

12 

144 

18 

145 

30 

146 

59-4 

150 

73-3 

160 

89.8 

170 

95-6 

184 

IOO 

Readings  for  t°  of  critical  saturation  obtained  by  cooling  from  t°  of  melting, 
are  also  given  by  the  authors. 

Coefficients  of  distribution  of  oxybenzoic  acids  between  water  and  olive  oil 
are  given  by  Boeseken  and  Waterman  (1911)  as  follows:]  p  oxybenzoic  acid, 
0.6;  m  oxybenzoic  acid,  0.4;  2.4  dioxybenzoic  acid,  i.o;  2.5  dioxybenzoic  acid, 
0.3;  3.4  dioxybenzoic  acid,  0.05;  3.4.5  trioxybenzoic  acid  0.025. 

MethylBENZOIC  ACIDS   C6H4COOH.CH3.     o,  m,  and  p. 
SOLUBILITY  IN  WATER. 

(Vaubel,  1895.) 
Gms.  C6H4COOH.CH3  per  1000  Gms.  Sat.  Solution. 


25 


Ortho 

1.18 


Meta. 
0.98 


Para. 

o-35 


NitroBENZOIC  ACIDS   C6H4.NO2.COOH.     o~m,  and  p. 
SOLUBILITY  IN  SEVERAL  SOLVENTS. 

(de  Connick,  1894;  for  solubility  inHzO,  see  also  Paul;  Vaubel;  Lowenherz;  Goldschmidt,  1898;  Holle- 
man,  1898;  Noyes  and  Sammet,  1903;  Sidgwick,  1910.) 

Gms.  CeH4.NO2.COOH  per  100  cc.  Solvent. 


Ortho. 

Meta. 

Para. 

""* 

Water 

15 

0 

-625 

0. 

238 

0 

.0213 

tt 

20 

o 

.682 

(o. 

645G.) 

o. 

315 

o 

•039 

" 

25 

0 

.738 

(o. 

779G.) 

o. 

341 

0 

.028(0. 

045) 

tt 

30 

0 

.922 

(o. 

922G.) 

it 

35 

I 

.141 

(i 

054) 

0. 

477 

o 

.0419 

Methyl  Alcohol 

10 

42 

.72 

47- 

34 

9 

.6 

Ethyl  Alcohol 

IO 

28 

.2 

33- 

1(11.7°) 

o 

•9 

"       (abs.) 

15 

37 

.58* 

47- 

26* 

XQ 

.71* 

"  (33Vol.%) 

15 

o 

.64  (ll. 

8°) 

o. 

52 

O 

•055 

Acetone 

10 

41 

•  5 

41 

5 

4 

•54 

Benzene 

IO 

0 

.294 

0. 

795 

0 

.017(12..?°) 

Carbon  Bisulfide 

10 

0 

.OI2 

o. 

10(8.5°) 

o 

.007 

Chloroform 

10 

15 

0 

i 

•455 
.o6f 

(n 

°) 

5- 
3- 

678 
4St 

o 
o 

.066 
.o88f 

" 

25 

i 

-i3t 

4- 

o 

•H4t 

M 

35 

i 

•59t 

3Jt 

0 

Ether 

10 

21 

•58 

25- 

175 

2 

.26 

Ligroin 

IO 

trace 

0. 

013 

0 

Gms.  acid  per  100  cc.  saturated  solution.  f  =  Gms.  acid  per  100  gms.  solvent. 


NitroBENZOIC  ACIDS 


142 


SOLUBILITY  OF  ORTHO  NITROBENZOIC  ACID  IN  WATER.  (Noyes  and  Sammet,  1903.) 

C6H4N02COOH  o  per  Liter  Sol.  ^  CelfrNChCOOH  o  per  Liter  Sol. 

Millimols.  Grams.  Millimols.  Grams. 

10  26.62  4.645  25  43.3  7.231 

15  31-06  5-187  30  51.6  8.616 

20  36.57  6.106 

Additional  determinations  by  other  investigators,  in  millimols  C6H4NO2COOH 

o  per  liter  at  25°,  are:  46.5  (van  Maarseveen,  1898);   44.19  (Paul,  1894);   42.3 

(Holleman,  1898);  43.6  (Kendall,  1911). 

SOLUBILITY  OF  ORTHO,  META  AND  PARA  NITROBENZOIC  ACIDS  IN  WATER 
AT  HIGH  TEMPERATURES,  DETERMINED  BY  THE  SYNTHETIC  METHOD. 

(Flaschner  and  Rankin.  1910.) 

o  C6H4NO2COOH+H*O.     m  C6H4NO2COOH+H2O.      p  C6H4NO2COOH+H2O. 


to      t 

Gms.  Acid 

t°  of: 

Gms.  Acid 

to  -f 

Gms.  Acid 

Of 

per  zoo  Gms. 

per  100  Gms. 
Sat.  Sol. 

OI 

Melting. 

per  100  Gms. 
Sat.  Sol. 

Melting. 

Solution' 

52  crit.  t. 

.  .  . 

63.2 

2 

118  crit. 

t. 

69 

5 

77-4 

6 

143 

5 

75 

9.9 

77-4 

90 

7 

150 

9 

78 

13-5 

77-4 

100 

10.5 

155 

14-5 

79 

49-5 

77-4 

105 

17 

1  60 

30 

80 

62 

77-4 

107  .  5  crit. 

t.    30 

165 

53-5 

85 

73-5 

77-4 

106 

So 

170 

65-5 

90 

78.6 

77-4 

100 

58.6 

180 

76.7 

100 

83.5 

77-4 

90 

65-4 

190 

83-2 

120 

94 

80 

74 

200 

88 

I48 

100 

100 

.  .  . 

88.5 

220 

J  95-2 

120 

96.8 

237 

100 

140.4 

100 

Data  for  the  solubility  of  mixtures  of  o,  m  and  p  nitrobenzoic  acids  in  water  at 
24.4°  are  given  by  Holleman  (1898). 

SOLUBILITY  OF  ORTHO  NITROBENZOIC  ACID  IN  AQUEOUS  SOLUTIONS  OF  HYDRO- 
CHLORIC, FORMIC,  MALONIC  AND  SALICYLIC  ACIDS  AT  25°.    (Kendall,  191  ij 

Gms.  o 

Normality  CeHUNCfe.COOH 
of  Solvent.      per  Liter  Sat. 

Solution . 

7.28l 
7.144 
6-934 


Solvent. 


Normality 
of  Solvent. 


HC1 


Gms. 
C6H4Np2COOH 
per  Liter  Sat. 
Solution. 


Solvent. 


HCOOH 


0.0179 

0-0357 

0.125 

0.250 

0.500 

0.0517 

o . 0998 


6.146 
5-66i 
4.976 
4-997 
4.752 
7.188 
7.124 


CH2(COOH)2 


C6H4(OH)COOH 


o 
0.0313 

O.IOOI 

0.2004 

0.0094 
0.0136 
0.0162 


6.656 
7.276 
7-352 
7-369 


SOLUBILITY  OF  ORTHO  NITROBENZOIC  ACID  IN  AQUEOUS  SOLUTIONS  OF 

DEXTROSE,  SODIUM  CHLORIDE,  AND  OF  SODIUM  NITRATE. 
Original  results  in  molecular  quantities.    (Hoffman  and  Langbeck,  1905). 

In  Dextrose.  In  NaCl.  In  NaNO3. 


G.QH1208  G.(0)C«H4N02.COOHG.NaCl.  G.^C^NOa-COOH  G.NaNO8  G.^CeEUNOz-COOH 
i*r  TOO  cc.      per  100  g.  Solvent,    per  I00  cc.  per  100  g.  Solvent.    pgr  IOO  cc.      per  100  g.  Solvent. 


Solution. 

At  25°.      j 

M  35b. 

Solution. 

At  25°. 

At  35°- 

Solution. 

At  25°.    i 

Vt  35*. 

0-0 

0.736 

-063 

O.II7 

o-743 

I  .072 

O.I7O 

0.746 

.074 

0.36 

0-736 

.064 

0.195 

0.746 

I  .075 

0.284 

o-754 

.080 

1.  80 

0.732 

.061 

0.585 

0.749 

I  .070 

0.851 

0.767 

.096 

9-50 

0.722 

.051 

2.425 

0.688 

0.967 

4-255 

o-774 

.097 

20-00 

0-703 

•030 

S.8o 

0-597 

0.831 

8.510 

0.748 

•047 

143 


NitroBENZOIC  ACIDS 


SOLUBILITY  OF  ORTHO  NITROBENZOIC  ACID  IN  AQUEOUS  SOLUTIONS  OF 
SODIUM  BUTYRATE,  ACETATE,  FORMATE,  AND  SALICYLATE  AT  26.4°. 

(Philip,  1905.) 

Original  results  in  terms  of '-  per  liter. 

100 


Gms.  Na  Salt 

o-ms.  \jn 

.iiu  v^n^v^^JLi. 

i.>*  v/2  l-'C1    Jt-*itci    UJ 

per  Liter. 

C3H7COONa. 

CH3COONa. 

HCOONa. 

C6H4.OH.COONa. 

0 

7-85 

7-85 

7-85 

7-85 

0-5 

8-35 

8.50 

8.60 

8-35 

1.0 

8.90 

9.15 

9-50 

8.70 

2 

10.  0 

IO.8o 

n-5 

9-4 

3 

II.  2 

12-55 

13  .5 

II.  0 

4 

12-4 

14-5 

15.6 

11.5 

6 

15.2 

Solvent. 

CH3OH 

<( 

C2H5OH 


SOLUBILITY  OF  ORTHO  NITROBENZOIC  ACID  IN  SEVERAL  ALCOHOLS. 

(Timofeiew,  1894.) 

Gms.  Acid  per  100  Gms.  Gms.  Acid  per  100  Gms 

Sat.  Sol.      Solvent.  i  Sat.  Sol.        Solvent. 

56.6    C3H7OH  o      17.7 

I09.I                "  22         31.2 

(CH3)2CH.CH2OH      o 


o 

22 

O 

22 


36.2 

52.2 

23-3 
42.7 


30-4 

74-5 


9-65 


21.5 

45-5 
10.7 


Freezing-point  data  for  mixtures  of  o  nitrobenzoic  acid  and  dimethylpyrone  are 
given  by  Kendall  (i9i4a). 


SOLUBILITY  OF  META  NITROBENZOIC  ACID  IN  SEVERAL  ALCOHOLS. 


Solvent. 

CH3OH 


C2H5OH 


(Timofeiew,  1894.) 


^0          Gms.  Acid  per  100  Gms. 

Solvent. 

C2H5OH 
C3H7OH 

^0         Gms.  Acid  per  100  Gms 

0 
19 

Sat.  Sol. 
41-9 

53-7 

Solvent. 
72.2 

116 

21-5 
0 

Sat.  Sol. 

43-9 
24.1 

Solvent. 
89.8 
31-8 

21.5 
0 

57-i 
33-6 

I33-I 
50.6 

tt 

19 
21.5 

32.5 

45 
48 

19 

42-3 

73-2 

SOLUBILITY  OF  META  NITROBENZOIC  ACID  IN  AQUEOUS  SOLUTIONS  OF  SODIUM 
ACETATE,  SODIUM  FORMATE,  SODIUM  MONOCHLORACETATE  AND  POTASSIUM 
FORMATE  AT  25°. 

(Philip  and  Garner,  1909.) 


In  CHsCOONa. 

Gms.  per  Liter. 

In  HCOONa. 

Gms.  per  Liter. 

In  CH2ClCOONa. 

Gms.  per  Liter. 

In  HCOOK. 

Gms.  per  Liter. 

CHs- 
COONa. 

m  CeH4N02- 
COOH. 

HCOONa. 

m  C6H4NOr 
COOH. 

CH2C1- 
COONa. 

m  CeH4NO2- 
COOH. 

HCOOK. 

m\.  COOH. 

O 
I.OO9 
2.484 
5.027 
10.07 

5-144 
7.932 
12.  6l 

20.77 

0 
0 
2 
4 

8 

.843 

.102 
.196 
.410 

3.424 
4.776 
6.380 

8.616 
11.90 

0 

1-375 
3.426 
6.839 
13.710 

3 
4 
4 

5 

7 

.424 

•075 
.876 
.861 
.264 

0 
I  . 
2. 
5. 

025 

563 
124 

3 
4 
6 
8 

.424 
.742 
.446 
•5Si 

NitroBENZOIC  ACIDS  144 

SOLUBILITY  OF  PARA  NITRO  BENZOIC  ACID  IN  AQUEOUS  SOLUTIONS 
OF  ANILIN  AND  OF  PARA  TOLUIDIN  AT  25°. 

(Lowenherz —  Z.  physik.  Chem.  25,  395,  '98.) 

In  Anilin.  In  ^-Toluidin. 

G.  Mols.  per  Liter.  Gms.  per  Liter.  G.  Mols.^per  Liter.  Gms.  per  Liter. 


HoNH"     %oS"        ^^H'-(aX)H2'           CCH3NH*~   SoH02' 

CH3. 

CfiHtNO,.' 
COOH. 

D.O 

O 

.00164 

o.o 

0 

.274 

0 

.0 

0.00164 

O 

.0 

0.274 

D.OI 

O 

.00841 

0.91 

I 

.406 

0 

.01 

O-OIOO 

I 

.071 

I  .671 

D.02 

0 

.01379 

1.82 

2 

•3°4 

o 

.02 

0.0174 

2 

.142 

2  .OX>2 

3.04 

0 

.02172 

3-64 

3 

.629 

o 

•03 

0.0245 

3 

.213 

4-097 

3.08 

o 

•0347 

7.29 

5 

.798 

1000  cc.  of  sat.  solution  of  pira  nitrabenzoic  acid  in  aqueous  I  normal  sodium 
para  nitrobenzoate  contain  0.0046  gm.  mols.  =  0.768  gm.  ^Cgl^NC^COOH  at 
25°.  (Sidgwick,  igzo.) 

SOLUBILITY  OF  PARA  NITROBENZOIC  ACID  IN  SEVERAL  ALCOHOLS. 

(Timofeiew,  1894.) 

Gms.  Acid  per  100  Gms.  Gms.  Acid  per  100  Gms. 

S°1VCnt-  *  '        'Sat.  Sol.'   Solvent.'  ^^  *  '  Sat.  Sol.    '  Solvent.  ' 

18.5  3-45  3-57  C2H5OH   21  3.22  3.32 

21  3-75  3-90  C3H7OH   18.5  2.12  2.17 

C2H5OH   18.5  3.25  3.36            19.5  1.85  1.90 

19-5  3-16  3-26            21  2.29  2.34 


DinitroBENZOIC  ACIDS  C6H3(NO2)2COOH.    1.3.5  and  1.2.4. 

SOLUBILITY  OF  3.5  AND  OF  2.4  DINITROBENZOIC  ACIDS  IN  AQUEOUS 
SOLUTIONS  OF  SODIUM  ACETATE  AT  25°. 

(Philip  and  Garner,  1909.) 
Gms.  per  100  cc.  Sat.  Sol.  Gms.  per  100  cc.  Sat.  Sol. 


CHaCOONa. 

3.5C«H,(NOi)jCOOH. 

CHsCOONa. 

2.4C6H3(N02)2COOH. 

0 

0.1314 

0 

0.0572 

O.0976 

0.3392 

0.0976 

0.2056 

0.2428 

0.6720 

0.2428 

0-3434 

0.4846 

I.2OI 

0.4846 

0.5023 

0.9718 

2.H5 

0.9718 

0.7440 

Data  for  the  solubility  of  1.3.5  dinitrobenzoic  acid  in  water  and  aqueous 
solutions  of  KC1,  NaCl,  KNOs  and  NaNOs,  and  for  its  distribution  between 
water  and  benzene  at  25°,  are  given  by  B.  de  Szyszkowski  (1915). 

SOLUBILITY  OF  1.3.5  DINITROBENZOIC  ACID  IN  WATER  AT  HIGH  TEMPERATURES, 
DETERMINED  BY  THE  SYNTHETIC  METHOD. 

(Flaschnw  and  Rankin,  1910.) 

+„               Gms.  Acid  per                  *°           Gms.  Acid  per                  to  Gms.  Acid  per 

100  Gms.  Sol.                                 100  Gms.  Sol.  100  Gms.  Sol. 

i23.8crit.  t.     ...                  123          66.5                160  90.9 

113                      4-4               125          72.7                180  95 

120  9.3                130          79-3                200  99 

121  14.5                140          85.7                206  100 

122  40  150  89 


145 


NitroBENZOIC  ACIDS 


SOLUBILITY  OF  NITROBROMOBENZOIC  ACIDS  AND  OF  NITROCHLOROBENZOIC 
ACIDS  IN  WATER  AT  25°. 

(Holleman,  1910.) 


Acid. 


C6H3COOH.NO2.Br  1.2.3 
C6H3COOH.NO2.Br  1.2.5 


Cms.  Acid  per 
100  cc.  Sol. 

0.033 
0.741 


Acid. 


Cms.  Acid  per 
100  cc.  Sol. 


C6H3COOH.NO2C1 1.2.3      0.047 
C6H3COOH.NO2.C1 1.2.5    0.967 


Holleman  also  gives  data  for  the  solubility  of  various  mixtures  of  the  above 
two  bromo  compounds  and  of  the  two  chloro  compounds  and'  uses  the  results  for 
estimating  the  quantity  of  each  in  an  unknown  mixture. 

Dinitro  p  oxyBENZOIC  ACID   C6H2OH(NOj)2COOH. 

SOLUBILITY  OF  MIXTURES  OF  DINITRO  PARA  OXYBENZOIC  ACID  AND  OTHER 
COMPOUNDS  IN  ABSOLUTE  ETHYL  ALCOHOL  AT  29.6°. 

(Morgenstern.  1911 ) 


Dinitro  p  Oxybenzoic 
Acid  -f  Phenanthrene. 


Dinitro  p  Oxybenzoic 
Acid  +  Fluorene. 


Dinitro  p  Oxybenzoic 
Acid  +  Retene. 


Gms.  per 

IOC 

ems.                                    Gms.  per  ioo  Gms. 

Gms.  per 

ioo  Gms. 

Sat..  Sol.'           C,,.M  T>U_                    Sat,  Sol.                   Solid 

Sat. 

Sol. 

Solid 

Acid. 

p] 
tl 

Sre^e1."                                    AdcL 

_„                   Phase. 
Fluorene. 

Acid. 

Retene. 

Phase 

2.0483 

O 

.1333        Acid                 2.0440 

0.1232         Acid 

2.0232 

0 

Acid 

2.0776 

O 

.2796                                2.0823 

0.3484 

M 

2  .  0484 

0.1236 

1 

2.1249 

0 

.5267                                 2.1045 

0.4824 

w 

2-0933 

0.3446 

' 

2.2195 

i 

•  0311 

2.1744 

o  .  8960 

M 

2.  1276 

0.5162 

1 

2.2883 

i 

•4310 

2.2618 

I  .  4308 

M 

2  .  2346 

1.0489 

' 

1.2171 

6 

.0092  Phena 

threne        1  .  0490 

3.8618     Flu< 

jrene 

2  •  3034 

1.3634 

1 

0.8681 

5 

.8300 

0.8004 

3.7566 

M 

1.9664 

3-3698 

Retene 

0.6017 

5 

.6890 

0.5620 

3-6532 

w 

0.7830 

3-0032 

" 

0.3487 

5 

.5619 

0.3900 

• 

0-5597 

2.9331 

" 

0.2157 

5 

.4890 

0.2113 

3-5024 

• 

o.  2740 

2.8466 

" 

0 

5 

.3781 

O 

3.4II5 

O 

2.2795 

" 

BENZOIC  ANHYDRIDE   (C6H5CO)2O. 

Freezing-point  data  are  given  for  mixtures  of  benzoic  anhydride  and  sulfuric 
acid  by  Kendall  and  Carpenter  (1914). 


BENZOIN   (Benzoyl  phenyl  carbinol)  C6H6CH(OH)COC6H5. 

SOLUBILITY  OF  BENZOIN  IN  WATER,  PYRIDINE  AND  AQUEOUS  50%  PYRIDINE 

AT  20-25°. 

(Dehn,  1917.) 


Solvent.' 


Water 

Aq.  5°  %  Pyridine 

Pyridine 


Cms.  Benzoin  per  ioo 
gms.  Solvent. 

o  03 

6.63 
20.20 


ioo  gms.  95%  formic  acid  dissolve  3.06  gms.  benzoin  at  18.5°.        (Aschan,  1913.) 
Freezing-point  data   (solubilities,  see  footnote,  p.  i)  are  given  by  Vanstone 

.  for  mixture  of  benzoin  and  each  of  the  following  compounds: 
Dibenzyl,  benzylaniline,  benzylideneaniline  and  hydrazobenzene. 


BENZOPKENONE 


146 


BENZOPHENONE     (C6H6)2CO. 

SOLUBILITY  IN  AQUEOUS  ALCOHOL  AND  IN  OTHER  SOLVENTS. 

(Derrien  —  Compt.  rend.  130,  722,  'oo;  Bell  —  J.  Physic.  Chem.  9,  550,  '05.) 

In  Aqueous  Alcohol  at  40°. 


Wt.  %     Cms.  (C6H6)2CO 
Alcohol        per  100  Gms. 


(BeU.) 


Jolveni 

'•  Solvent. 

Solution. 

40 

2 

1.0 

45 

5 

4-8 

50 

8 

8-3 

55 

II 

9-9 

60 

16 

13-8 

65 

28 

22.6 

Wt.% 

Gms.  (CftH6)2CO 

Alcohol 

per  100  Gms. 

in  Solvent. 

Solvent.      Solution. 

67-5 

39        28.1 

70 

56        35-9 

71 

67        39.2 

72 

90        47.4 

72-5 

105        51.2 

73 

156        61.0 

In  Aqueous  Alcohol  and  other  Solvents. 

(Derrien.) 


Solvent. 


Gms.  Gms. 

£"££  «o,ven,  f.  £*«» 

Solvent.  Solvent. 


17 

13-5 

Ethyl  Ether  (rectifiec 

I)  12.7 

*7-S 

17 

3-8 

Benzene 

17 

76.9 

17 
17 

2.2 
J-3 

Xylene 
Nitro  Benzene 

17.6 
iS-8 

38-4 
58.8 

9.8 

II 

Chloroform  (com.) 

16.5 

55-5 

15 

14-3 

Bromoform 

17-3 

33-3 

9.6 

19.2 

Toluene 

17.2 

55-5 

16.1 

66.6 

Ligroine 

14.6 

6-7 

97%  Ethyl  Alcohol 
85  cc.  97%  Alcohol  +  15  cc.  H2O  17 
80  "  "       +20 

75  "  "       +  26 

Methyl  Alcohol  (pure) 
«  it  « 

Acetic  Ether  (pure) 
Carbon  Disulfide 

Determinations  made  by  means  of  the  Pulfrich  refractometer  (Osaka,  1903-8), 
gave  39  gms.  benzophenone  per  100  gms.  absolute  ethyl  alcohol  at  20°,  and 
78.6  gms.  benzophenone  per  100  gms.  benzene  at  25°. 

SOLUBILITY  OF  BENZOPHENONE  IN  AQUEOUS  SOLUTIONS  OF  PHENOL  AND  OF 
n  BUTYRIC  ACID,  DETERMINED  BY  THE  SYNTHETIC  METHOD,  ARE  GIVEN 

BY  TlMMERMANS    (1907). 

In  Aq.  71.4%  C6H6OH 


36.51%  C6H5OH 


(Sat. 

t  =  65.3). 

(Sat. 

t   =  20.6). 

t°of 
Sat. 

Gms.  (C«Hi)«CO 
per  loo  Gms.  Sat. 
Sol. 

t°of 
Sat. 

Gms.  (C6H5)2CO 
per  100  Gms. 
Sat.  Sol. 

75-4 

0.685 

26.1 

0.96 

81.1 

1.  06 

29-3 

1.77 

85.3 

I.4I 

39-5 

4.06 

88.1 

1.67 

55-5 

7.82 

82.6 

16.82 

In  Aq.  39.4%  C3H7COOH 

(Sat.  t  =  -2.3). 


t°.  of 
Sat. 

Gms.  (C6ft)2C( 
per  100  Gms. 
Sat.  Sol. 

6.1 

0-439 

18.5 

1.  12 

28.9 

I.7I 

44 

2.66 

61.6 

3-92 

75-2 

5-09 

Solubility  data  for  mixtures  of  benzophenone  and  resorcinol  and  for  benzo- 
phenone" and  pyrocatechinol,  determined  by  the  freezing-point  method,  are  given 
by  Freundlich  and  Posnjak  (1912).  Similar  data  for  mixtures  of  benzophenone 
and  thymol  are  given  by  Pawlewski  (1893).  Results  for  mixtures  of  benzophenone 
and  sulfuric  acid  are  given  by  Kendall  and  Carpenter  (1914). 


BENZOYL  CHLORIDE,   BENZOYL  tetra  hydro  quinaldine,  d  and  /. 

Fusion-point  data  are  given  for  mixtures  of  benzoyl  chloride  and  phenol  by 
Tsakalotos  and  Guye  (1910),  and  for  mixtures  of  the  d  and  /  forms  of  benzoyl 
tetrahydroquinaldine,  by  Adriani  (1900). 


147 


BENZYLAMINES 


BENZYLAMINE  HYDROCHLORIDE  C6H5CH2.NH2.HC1. 

IOO  gms.  H2O  dissolve  50.6  gms.  of  the  compound  at  25°.      (Peddle  and  Turner,  1913.) 

DiBENZYLAMINE  HYDROCHLORIDE   (C6H5CH2)2NH.HC1. 

IOO  gms.  H2O  dissolve  2.17  gms.  of  the  compound  at  25°.    (Peddle  and  Turner,  1913.) 
loo  gms.  chloroform  dissolve  0.37  gm.  of  the  compound  at  25°.    ' 

TriBENZYLAMINE  HYDROCHLORIDE   (CeHsCH-OsN.HCl. 

IOO  gms.  H2O  dissolve  o.6l  gm.  of  the  compound  at  25°.       (Peddle  and  Turner,  1913.) 
ioo  gms.  chloroform  dissolve  1 1 .41  gms.  of  the  compound  at  25°.    ' 

DiBENZYL  C6H5CH2.C6H6CH2,  BENZYLANILINE   C6H5CH2.NHC6H6. 
SOLUBILITY  DATA,  DETERMINED  BY  THE  FREEZING-POINT  METHOD  (see 
footnote,  p.  i),  ARE  GIVEN  FOR  THE  FOLLOWING  MIXTURES: 

Dibenzyl+  Stilbene 

"        +  Benzylphenol 

"        -j-  Hydrobenzene  " 

+  Tolane 

Benzylaniline  +  Dibenzyl  " 

+  Stilbene 
+  Benzylphenol 
+  Hydrazobenzene 
+  Tolane 

NitroBENZYL  CHLORIDE  p  C6H5CHNO2.C1. 

SOLUBILITY  IN  SEVERAL  SOLVENTS  AT  25°. 

Gms.  p  GiHsCH.NCkCl 
Solvent. 


(Bruni,  1898:  Pascal  and  Normand,  1903.) 
(Pascal  and  Normand,  1913-) 


per  ioo  Gms. 


Solvent. 


(v.  Halban,  1913.) 

Gms.  p  CsHsCHNOz-Cl 
per  ioo  Gms. 


Solvent. 

Sat 

.Sol. 

Methyl  Alcohol 

8 

.87 

8 

•15 

Ethyl  Alcohol 

7 

.10 

6 

.63 

Propyl  Alcohol 

5 

.70 

5 

•39 

Amyl  Alcohol 

4 

.88 

4 

•65 

Butyl  Alcohol 

21 

•5 

17 

•  7 

Acetic  Acid 

18 

.1 

15 

•3 

Acetone 

107 

5i 

•7 

Acetophenone 

63 

.1 

38 

•7 

Paraldehyde 

24 

•9 

19 

•9 

Ether 

23 

.1 

18 

.8 

Acetonitrile 

96 

.6 

49 

.1 

Nitromethane 

68 

.8 

40 

.8 

o  Nitrotoluene 

5i 

.1 

33 

.8 

Solvent. 

Sat.  Sol. 

57-8 

36-4 

57-8 

36-4 

43-3 

30.2 

51.2 

33-9 

12.5 

10.4 

32 

24.2 

47.6 

32-3 

6.05 

5-69 

45-3 

31.2 

31-7 

.  23.4 

1.30 

1.28 

0.49 

0.49 

69.7 

37-4 

Nitrobenzene 
Ethylacetate 
Ethylbenzoate 
Ethylnitrite 
Isoamylbromide 
Brombenzene 
Chloroform 
Carbon  Tetrachloride 
Benzylchloride 
a  Bromnaphthaline 
n  Hexane 
Isopentane 
Benzene 

Data  for  the  lowering  of  freezing-point  are  given  by  Holleman  (1914)  for  mixtures 
of  o  and  p  nitro  benzylchloride. 

DiBENZYL  HYDRAZINE  C6H6CH2.NH.C6H5CH2NH. 

Reciprocal  solubilities  of  dibenzylhydrazine  and  cinnamylidene,  determined  by 
the  method  of  lowering  of  the  fr.-pt.  (see  footnote,  p.  i),  are  given  by  Pascal  ('14). 

ChloronitroBENZYLIDENES  C6H6C:  N02.C1.    BENZYLIDENE  NAPHTHAL- 

AMINES   C6H5CH:NCi0H7. 

DATA  FOR  THE  LOWERING  OF  THE  FREEZING-POINTS  (solubilities,  see  foot- 
note, p.  i)  ARE  GIVEN  FOR  THE  FOLLOWING  MIXTURES. 
o  Chloronitrobenzylidene  -f  m  Chloronitrobenzylidene      (Holleman,  1914.) 
p  +m 

P  "  +o 

a  Benzylidene  naphthalamine  +/3  Benzylidene  naphthalamine  (Pascal  and  Normand,  '13.) 

BERYLLIUM  ACETATE   (basic)  Be4O(CH3COO)6. 

ioo  gms.  chloroform  dissolve  33.3  gms.  Be4O(CH8COO)6  at  18°.      (Wirth,  1914.) 


BERYLLIUM  FLUORIDE  148 

BERYLLIUM   Potassium  FLUORIDE,   etc. 

SOLUBILITY  IN  WATER  AND  IN  ACETIC  ACID  SOLUTIONS. 

(Marignac;  Sestini,  1890.) 

Gms.  Anhydrous  Salt 

Salt.  Formula.  Solvent.  per  100  Gms.  Solvent. 

At  20°.  At  100°. 

Beryllium  potassium  fluoride  BeF2.KF  Water  2.0  5.2 

sodium  "       BeF2.NaF  "  1.4  2.8 

hydroxide  Be(OH)2  Water  +  CO2  sat.  0.0185  (BeO). .. 

phosphate  Be3(PO4)2.6H20     2%  CHaCOOH  0.055 

10%          «  0.1725 

BERYLLIUM  HYDROXIDE  Be(OH)2. 

SOLUBILITY  IN  AQUEOUS  SOLUTIONS  OF  SODIUM  HYDROXIDE. 

(Rubenbauer  —  Z.  anorg.  Chem.  30  334,  '02.) 

Moist  Be(OH)2  used,  solutions  shaken  5  hours,  temperature  prob- 
ably about  20°. 

Per  20  absolution.  Dilution  Gms.  per  100  cc.  Solution. 

Gms.  Na.  Gms.  Be.  jd^jg  NaOH.  Be(OH)2." 

0-3358     0.0358     1.37        2.917     0.850 

0.6716        0.0882        0.68  5-840        2.094 

0.8725        0.1175        0.53  7.585        2.789 

1.7346        0.2847        0.27  18.310        6.760 

SOLUBILITY  IN  AQUEOUS  SODIUM  HYDROXIDE  AT  DIFFERENT  TEMPERATURES. 

(Haber  and  Oordt,  1904.) 

Normality  of  Gm.  BeO  per  Liter  Sat.  Sol,  at: 

Aq.  NaOH. 

0-5 

I 
2 

BERYLLIUM   OXALATE   BeC2O4.3H2O. 

100  gms.  water  dissolve  63.2  gms.  BeC2O4.3H2O  at  25°  (Wirth,  1914.) 

o.i  n  oxalic  acid  "  75-92  " 
o.insulfuric  "  "  72.65  " 
i.on  "  "  52.8  " 

BERYLLIUM  PALMITATE  and  Salts  of  Other  Fatty  Acids. 
SOLUBILITIES  IN  ETHYL  AND  METHYL  ALCOHOLS  AT  25°.    (jacobson  and  Holmes,  1916.) 

Gms.  of  Each  Salt  (Determined  Separately)  per  100  Gms.  Solvent. 

Solvent.  / * • N 

Be  Palmitate.         Be  Stearate.  Be  Laurate.          Be  Myristate. 

Ethyl  Alcohol  o .  004  ...  o .  004  o .  004 

Methyl  Alcohol  o .  042  o .  040  o .  050  o .  047 


20-23°. 

0.060 

50-53°. 
0.080 

100°. 

0.080 

0.170 

0.570 

0.230 
0.900 

0.290 
1.020 

Mols.  H2O 
«.  o      per  i  Mol. 
*   '       BeS04. 

SOLUBILITY  IN 

Gms.  BeSO4  per 
100  Gms.                  S< 

WATER.     (Levi,  Malv 

m                   Mols.  H20 
base.         t<».    P^e's^01 

ano,  1906.) 

Gms.  BeSO4  per 
too  Gms. 

Solid 
Phase. 

Water. 

Solution. 

Water. 

Solution. 

31 

ii.  18 

52-23 

34- 

32     BeS04.6H,0      95.4 

6.44 

90. 

63 

47- 

55  BeS04.4HO 

5° 

9.62 

60.67 

37 

77 

107.2 

5-o6 

3 

53- 

58 

" 

72.2 

7-79 

74-94 

42 

8$ 

'             ill 

4-55 

14* 

•3 

56 

I9 

11 

77-4 

81.87 

45- 

01 

'    80 

6.89 

84 

76 

45 

87  B 

eSO4  .aH,0 

30 

13.33 

43.78 

3°' 

45     BeSO 

•4lIjO       91.4 

5-97 

97- 

77 

49 

.42 

" 

40 

12.49 

46.74 

31- 

85 

'               IO5 

4-93 

118 

4 

54 

21 

" 

68 

9.42 

61.95 

38. 

27                          119 

3,91 

149. 

3 

59-88 

<4 

85 

7-65 

76,30 

43. 

28            « 

149  BERYLLIUM   SULFATE 

SOLUBILITY  OF  BERYLLIUM  SULFATE  IN  AQUEOUS  SULFURIC  ACID  AT  25°. 

(Wirth,  1912-13.) 

Cms.  H2SO<       Cms.  BeSO«                                         Cms.  H2SO4  Cms.  BeSCh 

per  100  Cms.     per  100  Cms.        Solid  Phase.              per  100  Cms.  per  100  Cms.        Solid  Phase. 

Solvent.             Sat.  Sol.                                                  Solvent.  Sat.  Sol. 

o  8.212      BeSO4.6H2Q  45.51  6.628      BeSO4.6H2O 

5.23         8.429  50-63  5-438     BeSO4.4H2O 

9-61         7-944  56.59  3-640 

18.70         6.603  63.24  2.244 

34  5-63i  65.24  2.128 

40.35         5-773  73-64  2.185 
Freezing-point  data  for  mixtures  of  beryllium  sulfate  and  potassium  sulfate  are 
given  by  Grahmann  (i9I3)« 

BERYLLIUM  MetaVANADATE   Be(VO3)24H2O. 

100  gms.  H2O  dissolve  o.i  gm.  of  the  salt  at  25°.  (Brinton,  1916.) 

BETAINE    (Trimethyl  glycocoll)  C5HUO2N.H2O. 

SOLUBILITY  OF  ANHYDROUS  BETAINE  IN  WATER  AND  ALCOHOLS. 

(Stoltzenberg,  1914-) 
(Figures  read  from  the  author's  curves.) 
'•  Gms.  CsHuCfeN  per  100  Gms.  Gms.  CsHnQiN  per  100  Gms. 


c2H5OH.  HO  CKOH.  c2H5OH; 

-10  134  38  5  5o  197  70  16 

o  140  43  6  60  215  75  18.5 

+  io  147  49  7  70  236  80  22 

20  157  54  8.5  80  259  25 

30  168  60  ii  90  286  .. 

40  182  65  13  100  328 


BETAINE  SALTS. 


SOLUBILITY  OF  EACH,  SEPARATELY,  IN  WATER. 

(Stoltzenberg,  1914.) 

Grams  per  100  Grams  H2O. 


—  10 

o 
+  10 

20 
30 
40 
50 
60 
70 
80 
90 

100       169         206 

Data  are  also  given  by  Stoltzenberg  for  the  following  basic  salts  of  betaine 
(C6HUO2N)2HC1.H2O,  (C5HuO2N)2.HBr,  (C6HnO2N)2HI,  (C6HUO2N)2H2SO4  and 
(C6H11O2N)2HAuCl4.H2O. 


CsHiiOjjN.   CsHnCfeN.        CsHnCfeN.     CsHnCfcN.  CsHnQzN. 

CsHnOaN. 

CsHnCfcN^ 

HC1. 

HBr. 

HI. 

H2SO4.H2O. 

HsPO4. 

HMnO4. 

HAuCl4. 

38 

28 

35 

67 

35 

1.5 

1.3 

44 

39 

66 

86 

45 

i-75 

1-5 

52 

S2 

98 

107 

58 

2-5 

2 

60 

65 

130 

132 

73 

5 

3 

70 

79 

162 

164 

91 

9 

4.5 

8l 

94 

198 

203 

112 

16 

6 

93 

no 

231 

250 

135 

30 

8 

106 

127 

269 

306 

160 

(55°)  48 

n-5 

120 

144 

304 

.  .  . 

190 

15 

135 

162 

(75°)  321 

.  .  . 

223 

18 

!5X 

183 

23 

BETOL    03-Naphthylsalicylate) 

Freezing-point  data'including  super  solubility  curves,  are  given  for  mixtures  of 
betol  a-nd  salol  by  Miers  and  Isaac,  1907. 


BISMUTH  150 

BISMUTH   Bi. 

RECIPROCAL  SOLUBILITIES,   DETERMINED  BY  THE  METHOD  OF  LOWERING  OF 
TUSION-POINT  (see  footnote,  p.  i),  ARE  GIVEN  FOR  THE  FOLLOWING  MIXTURES: 
Bismuth  +  Bromine       (Eggink,  1908.) 
"        4"  Chlorine  " 

+  Iodine  (Amadori  and  Becarelli,  1912.) 

"          +  Sulfur  (Aten,  1905;  Palabon,  1904.) 

MUTUAL  SOLUBILITY  OF  BISMUTH  AND  ZINC.    (Spring  and  Romanoff,  1906.) 


t  °. 

266 
419 

475 

Upper  Layer. 

Lower^  Layer. 

t  °. 

584 
650 

75o 

Upper  Layei  . 

Lower  Layer. 

°86 
84 

%Zn. 
14 

16 

3 

5 

%Zn. 

97 
95 

80 

77 
70 

%Zn. 
20 

23 
30 

10 

15 
27 

90 
85 

73 

810-820  (crit.  temp.) 

BISMUTH  CHLORIDE.   BiCl3.    BSMUTH  OxyCHLORIDE   BJOC1.H2O. 
SOLUBILITY  IN  AQUEOUS  SOLUTIONS  OF  HYDROCHLORIC  ACID. 

Results  at  25°.     (Noyes  and  Hall,  1917.)  Results  at  30°.     (Jacobs,  1917.) 


Cl. 

Bi.            H(  =  Cl-3Bi). 

Bi2O3.            HC1. 

1.002          0.3477 

0.00130        0.3438 

0.60           2.40        BiOCl.HaO 

1.007          0.4350 

0.00376         0.4237 

5-35        5-69 

i.  oio       0.5221 

o  .  00869      o  .  4960 

8.17           8.47 

I.OI3          0.6244 

0.01767         0.5714 

8.70           8.93 

.018          0.7375 

0.03138         0.6434 

14.52         13.02 

.025       0.8824 

0.05338         0.7223 

18.60      15.80 

.036       1.0760 

0.08937         0.8079 

30.10      21.7 

.044      1.2277 

O.II77            0.8746 

36.95     25.4 

.061      1.5321 

O.lSlO           0.9891 

54.70    31-5 

.083       1.9021 

0.2657            I.I05 

56                32.8              BiOCl 

.157     3-1865 

0.5685            1.481 

58.5           33                BiCl^H^ 

.237     4.5056 

0.9022        1-799 

56.6           33.8                   +BiCU 

.288    5.325 

i.  100          2.025 

56.25        34.9                BiCU 

.329       6.066 

1.317          2.115 

55-9        35-9        BICU.HCI 

SOLUBILITY 

OF  BISMUTH  CHLORIDE 

IN  SEVERAL  SOLVENTS. 

Cms.  I 

5iCb  per  100. 

to 

.   .      A            .,                           - 

solvent. 

cc.  Solvent. 

Cms.  Solvent.                       Authority. 

Acetone 

18°       ...  17. 

9     (^is=O.9I94)(Naumann,  1904/05.) 

Ethyl  Acetate 

18°       ...     i  . 

66  (Ji8  =  O.9Io6)(Naumann,  1910). 

Anhydrous  Hydrazine  ord.  temp.  32         ...  (Welsh  and  Broderson,  1915.) 

loo  gms.  95%  formic  acid  dissolve  0.05  gm.  bismuth  oxychloride  (BiOCl)  at 
19.8°.  (Aschan,  1913.) 

Freezing-point  data  are  given  for  BiCl3+CuCl,  BiCl3+FeCl3,  BiCl3-f  PbG2, 
BiCl3-f-PbBr2  and  BiCl3+ZnCl2  by  Herrmann  (1911)  and  for  BiCl3+TlCl  by 
Scarpa  (1912). 

BISMUTH     CITRATE    (CH2)2C(OH)(COO)3Bi.          BISMUTH    Ammonium 
CITRATE. 

SOLUBILITY  OF  EACH  IN  WATER  AND  IN  AQUEOUS  ETHYL  ALCOHOL  AT  25°.  (Seidell.  '10.) 

-«*4 

o  o.on  o  22.25  1.25 

51  0.041  51  1.34  0.92 

91.4  0.065  91.4  None  0.81 


151  BISMUTH  HYDROXIDE 

BISMUTH  HYDROXIDE   Bi(OH),. 

SOLUBILITY  OF  BISMUTH  HYDROXIDE  IN  AQUEOUS  SOLUTIONS  OF  SODIUM 
AND  POTASSIUM  HYDROXIDES  AT  20°  AND  AT  100°. 

(Moser,  1909.) 

Cms  KOH  Gms>  Dissolved  Bi(QH)3  per  Liter  at:   Qmg  j^aOH    ^ms.  Dissolved  Bi(OH)j  per  Liter  at: 
per  Liter.    '  ^~  —  ^T         *      perLiter.       '       20^  I0o».    * 

28  o  0.188  20  o  0.188 

50  trace  0.249  4°  trace  (0.0014)*  0.249 

112  0.037  °-373  80  0.050  (0.0029)*  0.436 

168  0.074      ...  120  0.087(0.0054)*  0.622 

224  o.ioo  0.622  160  o.ioo  ... 

280  0.124  0.622  200  0.124   ,  0.622 

336  0.137  ...  240  0.137 

448  0.137  1.494  320  0.137  1.494 

560       0.174       2.054       400      0.199  2.120 

*  Results  at  25°  by  Knox  (1909). 
At  100°  some  Bi(OH)3  was  converted  into  BiO(OH). 

SOLUBILITY  OF  BISMUTH  HYDROXIDE  IN  AQUEOUS  SOLUTIONS  OF  POTASSIUM 
CHLORIDE  AND  OF  POTASSIUM  BROMIDE  AT  30°. 

(Herz  and  Bulla,  1909.) 

(An  excess  of  bismuth  hydroxide,  prepared  according  to  Moses  and  having  the 
composition  corresponding  to  BiO.OH,  was  shaken  2-3  weeks  at  30°  with  aqueous 
KC1  and  KBr.  The  analyses  of  the  sat.  solutions  are  expressed  in  terms  of  milli- 
mols  KOH  and  KC1  or  KBr.  They  have  been  calculated  for  the  following 
table  to  gms.  BiO.OH  and  KC1  or  KBr.) 

Gms.  per  100  cc.  Sat.  Sol.  Gms.  per  100  cc.  Sat.  Sol. 

'  -  ' 


SolVCnt-  BiO.OH.  KCl  '  BiO.OH.  r 

2nKC\         3.759        13.75  iwKBr          8.555          7.67 

3^KC1         5-745        20.71  2wKBr        17.785        15.02 

BISMUTH  IODIDE   BiI3. 

100  gms.  absolute  alcohol  dissolve  3.5  gms.  BiI3  at  20°.  (Gott  and  Muir,  1888.) 

•     100  gms.  methylene  iodide,  CH2l2,  dissolve  0.15  gm.  BiI3  at  12°.       (Retgers,  1893.) 

BISMUTH  NITRATE  Bi(NO3)3.5H2O. 

100  gms.  acetone  dissolve  48.66  gms.  Bi(NO3)3.5H2O  at  o°,  and  41.7  gms.  at 

IQ  «  (von  Laszczynski,  1894.) 

SOLUBILITY  OF  BISMUTH  NITRATE  IN  AQUEOUS  NITRIC  ACID  AND  IN  AQUEOUS 
NITRIC  ACID  CONTAINING  ACETONE,  AT  ORDINARY  TEMPERATURE. 

(Dubrissay,  1911.) 


SolidPhaSC- 

0.922  n  HNO3  86.86          Bi(N03)3.5H2O 

0.922"      "  +  6.66%  Acetone  85.51 

0.922"     "  +13.33%        "  81.96 

2.3      "      "  80.37 

2.3      "      "  +16.66%  74.47 

SOLUBILITY  OF  DOUBLE  NITRATES  OF  BISMUTH  AND  MAGNESIUM,  NICKEL, 
COBALT,  ZINC  AND  MANGANESE  IN  CONC.  HNO3  AT  16°. 

(Jantsch,  1912.) 

(di6  of  HNO3  =  1.325,  ioo  cc.  of  this  acid  contained  51.59  gms.  HNOa.) 

Gms.  Hydrated  Gms.  Hydrated 

Double  Salt.  Salt  per  ioo  cc.  Double  Salt.  Salt  per  ioo  cc. 

Sat.  Solution.  Sat.  Solution. 

Bi2Mg3(NO3)i2.24H2O        41  -69  Bi2Zn3(NO3)i2.24H2O      57  .51 

Bi2Ni3(NO3)12.24H2O         46.20  Bi2Mn3(N03)i2.24H2O     65.77 

Bi2Co3(NO3)i2.24H2O         54  .  67 


BISMUTH  OXIDE 


152 


BISMUTH  OXIDE   Bi2O3. 

SOLUBILITY  OF  BISMUTH  OXIDE  IN  AQUEOUS  NITRIC  ACID  AT  20°. 

(Rutten  and  van  Bemmelen,  1902.) 


Present  in  Shaker 
Flask. 

Gms.  per  TOO  Gms. 
Solution. 

Mols.  per  100  Mols.  H2O. 

Solid 

Per  i  part  Bi2Os. 
3N2O5.ioH2O. 

Bi203 

N20S 

Bi203 

N206  R 

fSfof3 

Phase. 

24.4  parts  H-P 
3.2  parts  H2O 

0.321 
6.37 

0.963 
7.17 

o  126 
2.844 

1.61 
13.82 

i 

12.8) 

4.8  ( 

B52O3.N2O6.2H2O 

Dilute  HNO3 
Dilute  HNO3 

18.74 
31.48 

15-9 
23-7 

10.50 
27.2 

38.65 
83.8 

i 
i 

3-6} 
3.Q  J 

Bi2OsN205.H20 

Dilute  HNO3  = 
6.13%  N2OS 

32-93 

24.83 

3°-I5 

97-97 

» 

Bi2O,.N2O5.HjO  and 
Bi203.3N205.ioH20 

6.816%  N205 

32.67 

24.70 

29.70 

96.57 

i 

3-21 

24.0%  N2O6 
51.0%  N206 

24.16 
11.66 

28.25  ...» 
46.62 

19.65 
10.81 

98.76 
186.23 

i 
i- 

5-0 
17.2  J 

Bi2O3.3N2Os.ioH2O 

70.0%  N206 

20.76 

53-75 

33-51 

355.87 

i 

io.6j 

27.85 

51.02 

51.0 

403.0 

i 

7-9  { 

Bi2O3.3N2O5.ioH2O  and 
Bi203.3N205.3H20 

Anyhdrous  HNO 
Bi203+      " 

38.56 
4-05 

68.28 
74.90 

14-35 
7-45 

492.0 
592.9 

j 

34-31 
79-5* 

Bi208.3N,06.3HaO 

Results  are  also  given  for  9°,  30°,  and  65°. 

BISMUTH  TriPHENYL   Bi(C6H6)3. 

Fusion-point   data   (see  footnote,  p.   i)  are  given    for  mixtures  of   bismuth 
triphenyl  and  mercury  diphenyl  by  Cambi  (1912). 

BISMUTH  SALICYLATE   (basic,  64%  Bi2O3). 

SOLUBILITY  IN  AQUEOUS  SOLUTIONS  OF  ETHYL  ALCOHOL  AT  25°. 

(Seidell,  1910.) 


Gms.  C2HsOH  per 
100  Gms.  Solvent. 

Gms.  Salt  per 
100  Gms.  Sat.  Sol. 

Gms  C2H6OHper 
zoo  Gms.  Solvent. 

Gms.  Salt  per 
100  Gms.  Sat.  Sol. 

O 

O.OIO 

80 

0.065 

20 

0.015 

00 

0.095 

40 
60 

0.022 
0.036 

92.3 
100 

O.IO5 

0.160 

BISMUTH  SELENIDE   Bi2Se3. 

Fusion-point  data  (see  footnote,  p.  i)  are  given  for  mixtures  of  bismuth  sele- 
nide  and  silver  selenide  by  Pelabon  (1908). 

BISMUTH  SULFIDE   Bi2S3. 

i  liter  H2O  dissolves  0.00018  gm.  Bi2S3  at  18°. 

(Weigel,  1906;  see  also  Bruner  and  Zawadski,  1912.) 

SOLUBILITY  OF  BISMUTH  SULFIDE  IN  AQUEOUS  ALKALI  SULFIDE  SOLUTIONS  AT  25°. 

(Knox,  1909  ) 
Gms.  Bi2Ss  per 

Solvent.  100  cc.  Sat.  Solvent. 

Solution. 

0.5  n  Na2S 

wNaOH 


0.0040  0.5 

i.on     "          0.0238  i 

1.5  n     "          0.1023  0.5 

o.5«K2S        0.0043  I 

i     n    '  0.0337  1.25  n  K2S  +i.25wKOH 

1.5  w    "  0.0639 

Freezing-point  data  (see  footnote,  p.  i)  are  given  for  mixtures  of  bismuth 
sulfide  and  bismuth  telluride  by  Amadori  (1915). 


Gms.  BizSs  per 

loo  cc.  Sat. 

Solution. 

0.0185 
0.0838 

o . 0240 

0.1230 
0.2354 


BORAX,  see  sodium  tetraborate,  p.  629. 


I53  BORIC  ACID 


BORIC    ACID    H3B03. 

SOLUBILITY  OF  BORIC  ACID  IN  WATER. 

(Nasini  and  Ageno,  1909.) 


.  0                  Gms.  HsBOa  per 
1  •                 loo  Gms.  Sat.  Sol. 

,0       Gms.  HsBOs  per 
100  Gms.  Sat.  Sol. 

to         Gms.  HaBO3  per 
100  Gms.  Sat.  Sol. 

—  o.76Eutec 

2.27 

30 

6.30 

80 

19.11 

0 

2-59 

40 

8.02 

90 

23.30 

+  10 

3-45 

50 

10.35 

100 

28.7 

20 

4.8 

60 

12.90 

1  10 

38-7 

25 

5-5 

70 

15.70 

120 

52.4 

The  results  of  Herz  and  Knoch  (1904),  and  one  determination  by  Auerbach 
(1903),  given  in  terms  of  gms.  per  100  cc.  sat.  solution,  appear  to  be  in  good 
agreement  with  the  above.  The  earlier  data  of  Ditte  (1877)  are  low. 


SOLUBILITY  OF  BORIC  ACID  IN  AQUEOUS  SOLUTIONS  OF  HYDROCHLORIC, 
SULPHURIC,  AND  NITRIC  ACIDS  AT  26°. 

(Herz  —  Z.  anorg.  Chem.  33,  355.  34.  205,  '03.) 

Normality  of     Normality  of  Gms.  Strong  Acid        Gms.  B(OH)3  per  100  cc.  Solution, 

the  H2SO4,  HC1      Dissolved  per  100  cc 


or  HNO3.  B(OH)3.  Solution.          In  HC1.  In  H2SO4.          In  HNO3. 

o  0.91  o  5.64  5.64  5.64 

0.5  0.78  5  4.0  4.25  4.50 

i.o  0.71  10  3-2  3.6  3.9 

2.0  0.58  15  2.45  3-o  3-35 

3.0  0.49  20  1.8  2.5  2.9 

4.0  0.41  25  2.0  2-55 

5-o  0-35  30  •••  i-55  2.1 

6.0  0.26  35  ...  ...  1.75 

The  determinations  given  in  the  original  tables  in  terms  of  normal 
solutions  when  plotted  together  lay  close  to  an  average  curve  drawn 
through  them.  The  figures  in  the  tables  here  shown  were  read  (and 
calculated)  from  the  average  curve. 


SOLUBILITY  OF  BORIC  ACID  IN  AQUEOUS  SOLUTIONS  OF  ELECTROLYTES 

AT  25°. 

(Bogdan  —  Ann.  Scient.  Univ.  Jassy,  2,  47,  'oz-'o3.) 


Gms.  Electro- 

Grams  H3BO3 

per 

too  Gms. 

H2Oin 

Aq.  Solutions  of: 

Gms.  H2O. 

NaCl. 

KC1. 

NaNO3. 

KN03. 

Na2S04. 

K2SO-4. 

O 

5 

•75 

5 

•75 

5 

•75 

5-75 

c 

•75 

5-75 

IO 

5 

•75 

r 

.80 

5 

.78 

5.8l 

5 

.88 

5-92 

20 

5 

•74 

5 

.86 

5 

.81 

5.88 

6 

•  oo 

6.10 

40 

5 

.72 

3 

.98 

5 

.87 

6.04 

6 

•33 

6.50 

60 

5 

.72 

6 

.12 

5 

•95 

6.  20 

6 

.70 

6.92 

80 

5 

•7i 

6 

.29 

6 

.02 

6.37 

7 

.10 

7-40 

Interpolated  from  the  original. 


BORIC  ACID  154 

SOLUBILITY  OF  BORIC  ACID  IN  AQUEOUS  SOLUTIONS  OF  HYDROCHLORIC  ACID 

AND  OF  ALKALI  CHLORIDES  AT  25°.    (Herz,  1910.) 

(The  original  results  are  given  in  millimols  per  10  cc.  They  have  been  calcu- 
lated to  gram  quantities,  plotted  on  cross-section  paper  and  the  following  values 
read  from  the  curves.) 

Cms.  HC1  or  Alkali  Cms.  HsBOs  Dissolved  per  100  cc.  Sat  Sol.  in  Aq.: 

Chloride  per  100  cc. 
Sat.  Sol. 

O 
2 
4 

6 

8 
10 
15 

20 

30  ...  6.55 

THE  SYSTEM  BORIC  ACID,  ACETIC  ACID  AND  WATER  AT  30°.    (Dukelski,  1909.) 
(The  sat.  solutions _and  residues  were  analyzed  by  titrating  total  acidity  with 
o.i  n  NaOH  and  the  acetic  acid  alone  by  an  iodometric  method.) 


HCl. 

Lid. 

NaCl. 

RbCl. 

KCl. 

5-59 

5-59 

5-59 

5-59 

5-59 

4.92 

5-20 

5-4o 

5.60 

5-67 

4-36 

4.85 

5-30 

5-62 

5-75 

3.88 

4-45 

5.20 

5-67 

5.85 

3-50 

4.07 

5-i5 

5-72 

5-9° 

3-i5 

3-75 

5.10 

5-77 

6 

3 

5-07 

5-90 

6.25 

6.10 

6.50 

Cms.  per  100  Gms. 

Sat.  Sol. 

Solid 
Phase. 

B(OH)3 

Gms.  per  100  Gms. 
Sat.  Sol.                Solid 

Gms.  per  100  Gms. 
Sat.  Sol.                 Soiid  phase. 

BiOs.       (CH3CO)20. 

3-55 
3-i8       7.78 
2.98      16.44 
2.34      28.96 
1.98      41.06 
i-47      52-63 

1.  12         67.76 

B203.     (CH3CO)2O. 
I.OI       73.96     B(OH)3 
0-54      80.67 
0.45       84.55           "+(?) 
0.39      84.65 
O.4I       84.48 

o  .  46     84  .  44 
0.50     84.51 

B203.     (CH3CO)20. 
4.98      82.13    B203.2(CH3CO)20 
5.13      84.60 
5.41      85.68 
4.82      88.74   BzOs.sCCHsCO)^ 
4.71      89.98 
4.06      92.68 
3.10      95.76 

SOLUBILITY  OF  BORIC  ACID  IN  AQUEOUS  SOLUTIONS  OF: 

Acetic  Acid  at  26°.  (Herz,  19030.)                      Acetone  at  2O°.      (Herz  and  Knoch,  1904.) 

Normality  of  Solutions.  Gms.  per  100  cc.  Solution.            cc>  Acetone     B(OH)3  per  100  cc.  Solution. 

CHaCQOH.    B(OH)'3.  CHaCOOH.    B(OH)3.              ^SoiwnU*         Millimols.              Grams! 

0  0-91  o         5-64 

1  0.82  5        4.7 

2  0.65  1C            4-2 

4            0.42  20        3.0 

6            p.  25  30        2.0 


o 

79  -J5 

4.91 

20 

81.71 

5-o7 

30 

83-35 

5-*7 

40 

82.72 

5-*3 

50 

81.62 

5-06 

60 

76.40 

4-74 

70 

67.62 

4.19 

80 

55-05 

3-4i 

100 

8.06 

0.50 

SOLUBILITY  OF  BORIC  ACID  IN  AQUEOUS  SOLUTIONS  OF  UREA,  ACETONE, 
AND  OF  PROPYL  ALCOHOL  AT  25°    (Bogdan.) 

Grams  of  Gms.  HaBOs  per  100  g.  H2O  in  Aq. 

CO(NH2)2,(CH3)2CO  Solutions  of: 

or  of  CsHyOH  per 
100  Gms.  H2O. 

O 
10 
20 

40 

60 


CO(NH2)2 

(CH3)2CO. 

CaHyOH. 

5-75 

5-75 

5-75 

5-84 

5-84 

5.80 

5-93 

5-93 

5-85 

6.13 

6.12 

5-94 

6.31 

6.29 

6.03 

155 


BORIC  ACID 


SOLUBILITY  OF  BORIC  ACID  IN  AQUEOUS  SOLUTIONS  OF  SEVERAL  ALCOHOLS  AT  25°. 

(Mueller  and  Abegg,  1906.) 


In  Aq.  Methyl  Alcohol.   In  Aq.  Ethyl  Alcohol. 


In  Aq.  Propyl  Alcohol. 


Solvent. 

Gms.  HaBOa          Solyent.         Gms.  HaBOa          Solvent. 

</     of    Gms.HaBOj 

dv 

Wt. 
CHaO 

%    per  100  cc. 
H.    Sat.  Sol.        4y 

Wt.  % 
C2HsOH. 

per  loo  cc. 
Sat.  Sol.        <**f  • 

cM. 

_  T          per  too  cc. 
Sat.  Sol.     sat  gol. 

0.9691 

19 

5 

•55 

0.9714 

20.2 

5-14 

0.9043 

50.83 

O 

9193 

3  99 

0.9340 

41- 

5      6 

•27 

0.9350 

42.3 

4.96 

0.8231 

79-41 

o 

.8570 

2.83 

0.9185 

50 

6 

.81 

0.8789 

67'-  3 

4.52 

0.8133 

95-5 

o 

.8466 

3.58 

0.9019 

58 

7 

.20 

0.8576 

76.2 

4-34 

0.8010 

IOO 

o 

.8297 

5-96 

0.8842 

66 

8 

.  10 

0.8198 

91.1 

5-54 

0.7960 

IOO 

17 

-99* 

0.8089 

95 

6.85 

* 

J 

0.7947 

IOO 

9-47t 

+   A        —  «  flf  ft 

d*t  = 

0.8904. 

j    "-25  —  W«UDO»J» 

In  Aq.  i  Butyl  Alcohol. 

Solvent.  j     _f       Gms.  HaBOa 


In  Aq.  i  Amyl  Alcohol. 


v 

Mol.  % 
CJfcOH. 

Sat.  Sol. 

per  loo  cc. 
Sat.  Sol. 

0.9923 

0.70 

1.0124 

5.48 

0.9853 

2.15 

1.0038 

5-32 

0.9855 

2.18 

1.0046 

5-32 

0.8173 

71-4 

0-8351 

2 

0.8133 

77.1 

0.8220 

2-15 

0.8081 

85-6 

0.8195 

2.6l 

0.7984 

IOO 

0.8172 

4-30 

Solvent. 

Mol.  % 

•y* 

CsHuOH. 

0.9943 

0.448 

0.9936 

0.520 

0.9931 

0.525* 

0.8232 

67.26f 

0.8183 

75-54 

0.8142 

83.40 

0.8068 

IOO 

d     of    Gms.HaBOs 
Sat.  Sol.  ^tVsa? 

1.0132 
1.0125 
1.0123 
0.8290 
0.8253 
0.8223 
0.8220 


=  HzO  sat.  with  amyl  alcohol. 


t  =  Amyl  alcohol  sat.  with  H2O. 


5.48 
5.46 
5.46 
I.  60 
1.69 
1.98 
3.54 


One  liter  H2O  saturated  with  amyl  alcohol  dissolves  55.5  gms.  H3BO3  at  15°. 

(Auerbach,  1903.) 

SOLUBILITY  OF  BORIC  ACID  IN  AQUEOUS  SOLUTIONS  OF  ETHYL 
ALCOHOL  AT  15°  AND  AT  25°. 

(Seidell,  1908.) 

Results  at  15°.  Results  at  25°. 


disof 
Sat.  Sol. 

Gms.  C2H6OH   Gms.HaBOs 
per  loo  Gms.  per  100  Gms. 
Solvent.           Sat.  Sol. 

1.014 

O                    4.  II 

0.9986 

8.9                3.90 

0.9658 

32                     3.58 

0.9268 

51                     3-48 

0.8820 

70.2                3.22 

0.8389 

91.3                5.06 

0.8370 

93-6              5-70 

0.8356 

99.8              9.18 

(*250f 

Sat.  Sol. 

Gms.  C2H»OH 
per  loo  Gms. 
Solvent. 

Gms.  per  100  Gms.  Sat.  Sol. 

'  HaBOa. 

CzHsOH. 

1.018 

O 

5-42 

O 

0-987 

20 

5-20 

18.96 

0.952 

40 

5-io 

37-96 

0.908 

60 

5 

57 

0.862 

80 

5-05 

75.96 

0.853 

85 

5-30 

80.50 

0.842 

90    , 

6.20 

84.4 

0.838 

95 

8 

87.4 

0.838 

IOO 

ii.  20 

88.8 

SOLUBILITY  OF  BORIC  ACID  IN  AQUEOUS  SOLUTIONS  OF  LACTIC  ACID, 
OXALIC  ACID,  d  and  i  TARTARIC  ACIDS  AT  25°. 


In  Aq.  Lactic  Acid. 
(Mueller  and  Abegg,  1906.) 


In  Aq.  Oxalic  Acid. 

(Herz,  1910.) 


In  Aq.  d  and  i  Tartaric  Acid. 

(Herz,  1911.) 


Solvent. 
d              Mol.  % 
V           CaHeOa. 

d     of     Gms.  HaBO 

c   To    i        Per  I0°  cc- 

Sat.  Sol.       sat.  Sol. 

a  Gms.  per  100  cc. 
Sat.  Sol. 

Solid  Phase. 

Gms.  per  100  cc. 

Sat.  Sol. 

H2C204. 

HaBOa 

C4H606. 

HaBOa. 

1.0252 

2 

.321 

1.0444 

6 

•64 

2.26 

6.17 

HaBOa 

O 

5-59 

1.0722 

6 

.819 

1.0986 

9 

.98 

5.36 

6.70 

" 

11.25 

JAcid 

6.20 

1.1405 

18 

-77 

1-1635 

II 

•53 

12.39 

7-44 

"  +H2C20« 

22.5 

" 

6.63 

I  .  2023 

36 

•33 

1.2254 

12 

.90 

11.27 

3-45 

H2C204 

45 

M 

7.48 

10.84 

0.97 

" 

9-45 

i  Acid 

6.  ii 

10.77 

0-55 

" 

18.90 

M 

6.48 

10.63 

0 

" 

37 

" 

7-23 

BORIC  ACID 


156 


SOLUBILITY  OP  BORIC  ACID  IN: 

Pure  Glycerol    (Sp.Gr.  =1.260 
at  15.5°)- 


iHooper  —  Pharm.  J.  Trans.  [3]  13,  258,  '82.) 


Aq.    Solutions  of  Glycerol 
at  25°. 

(Herz  and  Knoch  —  Z.  anorg.  Chem.  45,  268,  '05.) 


Cms.  B2O3 
t  o     3H2O  per 

100  CC. 

Glycerine 

•"'  Cms.  B(OH)3  per  100 
Gms. 

Wt.  %          Millimols 
Glycerine   B(OH)3  per 
in  Solvent.    100  cc.  Sol. 

Sp.  Gr. 

t  25° 

Gms.  B(OH)3 
per  TOO 

Glycerine.  Solution. 

av 

cc.  Solution 

Gms  .So- 
lution. 

0 

20 

15 

.87 

I3-1? 

O 

90.1 

.017 

5 

•59 

5-50 

10 

24 

J9 

.04 

16.00 

7 

•J5 

90.1 

.038 

5 

•59 

5-38 

20 

28 

22 

.22 

.18.21 

20 

•44 

90.6 

.063 

5 

.62 

5.28 

30 

33 

26 

.19 

20.75 

3i 

•55 

92.9 

.090 

5 

.76 

5'29 

40 

38 

30 

.16 

23-I7 

40 

•95 

97-0 

•"3 

6.  02 

5-41 

50 

44 

34 

.92 

25-95 

48 

•7 

103.0 

•J33 

6 

•39 

5-64 

60 

So 

39 

.68 

28.41 

69 

.2 

140.2 

.187 

8 

.69 

7-32 

70 

56 

44 

•65 

30.72 

100 

•  O 

300.3       1.272 

24 

.20 

19.02 

80 

61 

48 

.41 

32.61 

90 

67 

53 

.18 

34-70 

100 

72 

57 

.14 

36-36 

IN  AQUEOUS  SOLUTIONS  OF  GLYCEROL 
AT  25°. 

(Mueller  and  Abegg,  1906.) 


Solvent. 


I.IS74 


Mol.  %      Wt.  % 
3sH( 

60 


j     of     Gms.  HsBOs 
TC-  per  ioo  cc. 

Sat.  Sol.       Sat.  Sol. 


AQUEOUS  SOLUTIONS  OF  DULCITE 
AT  25°. 

(Mueller  and  Abegg,  1906.) 
Solvent. 


24.64 

46.75 

1.2370    67.71 
1.2531    90.58 

ioo  gms.  glycerol 


,  Mol.  % 

dV       C6H8(OH)6. 
0.9995        0.065 
I.OOlS        0.130 
I. 0060       0.260 


Of     Gms.  HsBOa 
'     ,      per  ioo  cc. 
Sol.      Sat.  Sol. 


I. 0686  5.50 
I. 0212  5.63 
1.0260  5.81 


1.1707  7.49 

1.2260  13.22 

90  1.2526  18.35 

96.6  1.2710  23.44 

1.256)  dissolve  n  gms.  H3BO3  at  i5°-i6°. 

(Ossendowski,  1907.) 

ioo  gms.  dichlorethylene  dissolve  0.006  gm.  H3BO3  at  15°.     (Wester  and  Brunis,  1914.) 
ioo  gms.  trichlorethylene  dissolve  0.016  gm.  H3BO3  at  15°.  "  " 

ioo  cc.  anhydrous  hydrazine  dissolve  55  gms.  H3BO3  at  room  temp. 

(Welsh  and  Broderson,  1915.) 

SOLUBILITY  OF  BORIC  ACID  IN  AQUEOUS  SOLUTIONS  OF  MANNITE  AT  25° 
AND  VICE  VERSA. 

(Ageno  and  Valla,  1912,  1913.) 


Grams  per  ioo  cc.  Sat.  Sol. 

Solid  Phase. 

HsBOj. 

CsHwOe. 

5-50 

0 

H3BO3 

5-90 

1.82 

" 

6.29 

5.46 

" 

6.44 

7-28 

tt 

6.64 

9.II 

" 

6.83. 

10.93 

" 

7.08 

12-75 

tt 

7.27 

14.57 

tt 

7.71 

18.99 

tt 

HsBOs. 

C6Hl406. 

OUIIU   K  lldoC. 

8.70 

25.65 

H3B03 

9-43 

32.43 

"  +C6H1406 

7.71 

27-97 

C6H1406 

5-75 

25.65 

,  -  ' 

4.92 

24.65 

u 

3-46 

23-03 

tt 

2.87 

22.98 

tt 

1.64 

20.80 

" 

0 

19.58 

tt 

Additional  determinations  at  30°  also  given. 

Determinations  at  25°,  differing  somewhat  from  the  above,  are  given  by  Mueller 
and  Abegg  (1906).  *  - 

Data  for  the  system  boric  acid,  phenol  and  water  are  given  by  Timmermans 
(1907). 


157 


BORIC  ACID 


DISTRIBUTION  OF  BORIC  ACID  BETWEEN  WATER  AND  AMYL  ALCOHOL 

AT  25°. 

(Fox  —  Z.  anorg.  Chem.  35*  130,  '03.) 
Millimols  B(OH)3  in       Cms.  B(OH)3  in  100  cc. 


Aq 

Alcoholic 

Aq. 

Alcoholic 

Layer. 

Layer. 

Layer. 

Layer. 

26S 

.8 

76 

.6 

I 

.648 

0 

•475 

196 

•5 

59 

•5 

I 

.219 

0 

•369 

159 

.6 

47 

•5 

O 

.990 

O 

.294 

126 

.0 

37 

,i 

O 

.781 

O 

.230 

Millimols  B(OH)3  in 

Cms.  B(OH)3  in  100  cc 

TAq. 
Layer. 

87.9 

75-2 
64.6 

Alcoholic 
Layer. 

33-2 

22  .7 
19.76 

Aq. 
Layer. 

0-545 
0.466 

0.400 

Alcoholic 
Layer. 

O.2O6 
O.I4I 
0.123 

RESULTS  AT   15°.      (Mueller  and  Abegg,  1906.) 
Millimols  B(OH)3  per  Liter.  Gms.  B(OH)3  per  100  cc.     Mifflmok.BCOH),  per      Gms.  B(OH)3  per  100 


Aq.  Layer. 

Alcohol 
Layer. 

Aq. 

Layer. 

Alcohol 
Layer 

Aq.  Layer. 

Alcohol 
Layer. 

Aq. 

Layer. 

Alcohol 
Layer. 

894 

264 

5 

-44 

I  .64 

427.4 

127.6 

2 

•65 

0.79 

607.2 

176.4 

3 

.76 

1.09 

372 

1  10 

2 

.31 

0.68 

589-3 

177-4 

3 

-65 

I  .IO 

289.1 

84.9 

I 

'79 

0-53 

Data  agreeing  with  those  of  Fox  at  25°  are  afso  given  by  Mueller  and  Abegg, 
1906.  One  determination  at  35°  gave  0.907  gm.  B(OH)3  per  100  cc.  aq.  layer  and 
0.274  gm.  per  100  cc.  alcohol  layer. 

DISTRIBUTION  OF  BORIC  ACID  BETWEEN  AQUEOUS  SODIUM  CHLORIDE 
SOLUTIONS  AND  AMYL  ALCOHOL  AT  25°. 

(Mueller  and  Abegg,  1906  ) 


Gms.  per  100  cc.: 

Aq.  Layer.  Alcohol  Layer. 


NaCl. 
O 

5-53 

8.72 

10.91 

13-84 


HsBOs.        H20. 

5-46        7   39 
6.40 

5-90 
5-46 
5-15 


5-37 
5-27 
5-23 
5-i6 


•65 
•65 
.67 
.69 

•77 


Alcohol 
Layer. 
0.8296 
0.8277 
0.8268 
0.8259 
0.8254 


Gms.  per 

Aq.  Layer. 

100  cc.: 

Alcohol  Layer. 

NaCl. 

H3B03. 

H20.       HsBOs. 

16.64 

5-13 

4.71 

•79 

17.90 

5.02 

4-31 

•79 

20.36 

5-02 

4.19 

.87 

23-52 

4-97 

3-59 

.96 

25-03 

4-95 

3-20 

•99 

d^  of 

Alcohol 
Layer. 
0.8247 
O . 8241 
0.8240 
0.8233 
0.8229 


DISTRIBUTION  OF  BORIC  ACID  BETWEEN  WATER  AND  MIXTURES  OF  AMYL 
ALCOHOL  AND  CARBON  DISULFIDE  AT  25°. 

(Herz  and  Kurzer,  1910.) 

50  Vol.  %C6HUOH+50 
Vol.  %  CSa. 

Gms.  HaBOs  per  100  cc. 

Aqueous 
Layer. 

0.469 
0.839 
I  .207 


75  Vol.  %C.HnOH+25 
Vol.  %  CS,. 

Gms.  HsBOs  per  100  ec. 


25  Vol.  %C5HnOH+95 
Vol.  %  CSa. 

Gms.  HsBOs  per  100  cc. 


Aqueous 
Layer. 

0.387 

0-743 
I.I43 
1.590 


CoHuOH+CSa. 
Layer. 

0.095 
O.I7I 
0.266 
0-365 


C5HiiOH+CS2. 
Layer. 


Aqueous 


1.791 


0.095 
0.161 
0.226 
0-344 


'Yqut 
Layer. 

0-433 
0.910 

1-343 
1.940 


CsHuOH+CSz.' 
Layer. 

0.053 

0.108 
0.164 
0.238 


BORIC  ANHYDRIDE   B2O3. 

Fusion-point  data  (solubilities,  see  footnote,  p.  i)  are  given   for  mixtures  of 
B2O3+CaO  and  B2O3+SrO  by  Guertler  (1904). 

BORIC  ACID   (Tetra)  H2B4O7. 

TOO  grams  water  dissolve  2.69  grams  H2B4O/  at  15°,  Sp.  Gr.  =  1.015. 

(Gerlach,  1889.) 

BORON  TRI-FLUORIDE  BF3. 

i  cc.  H2O  absorbs  1.057  cc>  BF3  at  o°  and  762  mm.;  i  cc.  cone.  H2SO4  (Sp.  Gr. 
1.85)  absorbs  50  cc.  BF3. 


BRASSIDIC  ACID  158 

BRASSIDIC  ACID 

Solubility  data  determined  by  the  freezing-point  method  are  given  by  Mas- 
carelli  and  Sanna  (1915),  for  mixtures  of  brassidic  and  erucic  acids  and  brassidic 
and  isoerucic  acids. 

BROMAL  HYDRATE  CBr3.CH(OH)2 

The  distribution  coefficient  of  bromal  hydrate  between  olive  oil  and  water  is 
0.665  at  ord.  temp.  (Baum,  1899);  0.7  at  ord.  temp.  (Meyer,  1909). 

BROMINE   Br. 

SOLUBILITY  IN  WATER. 

fWinkler  —  Chem.  Ztg.  23,  687,  '99;  Roozeboom  —  Rec.  trav.  chim.  3,  29,  59,  73,  84,  '84;  Dancer  — 
J.  Chem.  Soc.  15,  477,  '62;  at  15°,  Dietze  —  Pharm.  Ztg.  43,  290,  '08  J 

Grams  Bromine  per  100  Grams.  __^ 

Solubility."* 


*   *  Water.  Solution. 

(W.)      (R.  D.  &  D.)     (W.)       (R.  D.  &  D.)  ff- 

o  4-^7  4.22  3-98  4-05  60.5  43.1 

5  3-92  3-7  3-77  3-57  45-8  32-4 

10  3.74  3-4  3-61  3-29  35-1  24.8 

15  3-65  3-25  3-S2  3-J5  27.0  19.0 

20  3.58  3.20  3.46  3.10  21.3  14.8 

25  3-48  3-J7  3-36  3-o7  17  o  11.7 

30  3.44  3-!3  3-32  .3-03  13-8  9-4 

40  3.45  •••  3-33  •••  9-4  6.2 

50  3.52  ...  3.40  ...  6.5  4.0 

60  ...  4-9  2.8 

80  ...  ...  3-o  LI 

*  For  definition  of  "Absorption  Coefficient  "  a  and  "Solubility  ''  q,  see  Acetylene,  p.  16. 

One  liter  sat.  solution  of  bromine  in  water  contains  0.21  mol.  Br2  =  33.56 
gms.  Br  at  25°.  (Bray  and  Connolly,  1910.) 

The  coefficient  of  solubility  of  bromine  in  water  at  15°,  determined  by  an 
aspiration  method,  is  given  as  33  by  Jones  (1911).  This  investigator  also  gives 
the  figure  56  for  the  solubility  coefficient  in  25  vol.  %  acetic  acid  and  551  for 
90  vol.  %  acetic  acid  at  15°. 

Data  for  the  distribution  of  bromine  between  water  and  air  at  25°,  are  given 
by  Hantzsch  and  Vagt  (1901). 

SOLUBILITY  OF  BROMINE  IN  AQUEOUS  SOLUTIONS  OF  MERCURIC  BROMIDE 
AT  25°  AND  VICE  VERSA. 

(Herz  and  Paul,  1914.) 

Gms.  per  100  cc.  Sat.  Sol.        Soiy  Gms.  per  100  cc.  Sat.  Sol.  Solid 

HgBrz.  Br.  Phase.  HgBr2.  fiT Phase. 

o  3.40  Br2               0.763  3.57        Br2+HgBr2 

0.202  3.53  0.701  2.88             HgBr2 

0-285  3-55  0.664  1-20 

0.462  3.56  " 


159 


BROMINE 


SOLUBILITY  OF  BROMINE  IN  AQUEOUS  SOLUTIONS  OF  POTASSIUM  BROMIDE. 

(Results  at  o°  and  25°,  Boericke,  1905;  at  o°,  Jones  and  Hartmann,  1916; 

at  18.5°  and  26.5°,  Worley,  1905.) 

Cms.  Bromine  Dissolved  per  Liter  of  Sat.  Solution  at: 


Br  per  Liter. 

Liter. 

o°. 

18.5°. 

25°. 

26.5°. 

0 

0 

41.6  (24.2) 

35-56 

34 

34-23 

O.OO5 

o-59 

41-7  (25-5) 

36.1 

34.3 

35-i 

0.010 

1.19 

42.6  (26.2) 

37 

35 

36 

0.020 

2.38 

44.4  127.5) 

38.56 

36.5 

37-35 

o  .  050 

5-95 

50.2  (31.5) 

43-8 

4i 

42.5 

0.100 

11.90 

59-7  (4o) 

52-23 

49-3 

51.87 

O.2O 

23.80 

79-i  (57-i) 

69.69 

67-3 

68.69 

0.50 

59-5i 

138.6  (111.9) 

123 

119 

116 

0.80 

92.22 

200         (174) 

178.70 

176 

168  .  10 

I 

119.02 

243.1    (217.5) 

216 

216.5 

204 

I-725 

205.2 

402.3    (395-9) 

.  .  . 

.  .  . 

... 

1.82 

216.6 

423.8    (423) 

... 

... 

• 

2.17 

258.2 

5II.7    (5H.7) 

.  .  . 

... 

... 

3-033 

360.8 

736.7         ... 

632.4 

Very  accurate  determinations  at  o°,  at  concentrations  of  KBr  below  o.oi 
normal,  are  given  by  Jones  and  Hartmann.  Liquid  bromine  in  contact  with 
aqueous  solutions  at  o°  is  slowly  converted  to  the  hydrate,  Br2.ioH2O,  with  a 
reduction  in  amount  of  dissolved  bromine.  At  this  temperature  there  are,  con- 
sequently, two  saturation  concentrations.  The  unstable  one  being  for  solutions 
in  contact  with  liquid  bromine  and  the  stable  one  being  for  solutions  in  contact 
with  Br2.ioH2O.  The  results  for  the  latter  are  shown  in  parentheses  in  the 
above  table. 

SOLUBILITY  OF  BROMINE  IN  AQUEOUS  SOLUTIONS  OF  POTASSIUM  SUL- 
PHATE, SODIUM  SULPHATE,  AND  OF  SODIUM  NITRATE  AT  25°. 

(Jakowkin  —  Z.  physik.  Chem.  20,  38,  '96.) 


Normality  o: 
Salt  Solution 

i 
1 

In  K2S04 
Gms.  per  Liter. 

In  Na2SO4 
Gms.  per  Liter. 

In  NaNOs 
Gms.  per  Liter. 

9I.I8 

45-59 
22.79 

5-69 

Br. 
25.14 
29.44 
31.46 
32.70 

33  ^o 

Na2SO4. 
15.88 

7-94 
3-97 

Br.  " 
25.07 
29.20 

32-94 
33-26 

NaN03. 
85.09 

42-54 
21.27 
10.63 
5-31 

Br. 
28.80 

31-35 
32.62 

33-33 
33-74 

SOLUBILITY  OF  BROMINE  IN  AQUEOUS  SALT  SOLUTIONS  AT  25°. 


(McLauchlan,  1903.) 


Gms. 

Normality 

Gms. 

Gms. 

Normality       Gms. 

Salt. 

Salt  per 

of  Dis- 

Br. per 

Salt.                   Salt  per 

of  Dis-        Br.  per 

Liter. 

solved  Br. 

Liter. 

Liter. 

solved  Br.        Liter. 

Water 

0.0 

0.424 

33-95 

NH4NO3          80.  1  1 

0.688      55.15 

Na2S04 

63-55 

0.286 

23-9 

I^aCl                58.50 

0.701        55.90 

K2S04 

9I.I8 

0.310 

24.8 

KC1                  74.60 

0.718        57.40 

(NH,)2SO4 

70.04 

0.971 

77-7 

NH4C1              53.52 

1.028        82.2 

NaNO3 

VKTr\ 

85.09 

0-3495 

28.0 

CH3COONH477.o9 

4.26        340.5 

KNO3 

101.19 

0.362 

28.95 

H2SO4*            49-03 

0.366        29.26 

*  Wildeman. 


BROMINE 


160 


SOLUBILITY  OF  BROMINE  IN  AQUEOUS  SOLUTIONS  OF  SODIUM  BROMIDE  AT  25°. 

(Bell  and  Buckley,  1912.) 
Grams  per  Liter  Sat.  Sol.  j^  of 

NaBr. Ei.  Sat.  Sol. 

92.6  99.2  I.2I3 

160.5  176.7  1.372 

205.8          247.8          1-515 
255-8  343  1-678 

RECIPROCAL  SOLUBILITY  OF  BROMINE  AND  CHLORINE,  BROMINE  AND  HYDRO- 
BROMIC  ACID  AND  BROMINE  AND  SULFUR  DlOXIDE,  DETERMINED  BY  METHOD 
OF  LOWERING  OF  THE  FREEZING-POINT  (see  footnote,  p.  i). 


Gms.  per  Litei 

•  Sat.  Sol. 

d>*  of 
Sat.  Sol. 

1.997 
2.137 
2.327 
2.420 

NaBr. 
319-7 

359 
408  '.3 

Br. 
546 

641  .6 
769.2 
834 

Results  for  Bromine 
+  Chlorine. 

(Lebeau,  1906;  see  also 
Karsten,  1907.) 


Bromine  +  Hydro- 
bromic  Acid. 

(Buchner  and  Karsten,  1908-09.) 


Bromine  -f-  Sulfur 
Dioxide. 

(van  der  Goot,  1913.) 


t°of 
Melting. 

Gms.  Br  per 
loo  Gms. 
Mixture. 

"     t°of 
Melting. 

Gms.  Br  per 
loo  Gms. 
Mixture 

Mol.  % 
Br.  in 
Mixture. 

t°of 
Melting. 

Gms.  Br  per 
loo  Gms. 
Mixture. 

— 

102.5 

O 

-87-3 

0 

O 

-75-i 

0 

.— 

IOO 

6 

•5 

-90 

6 

2. 

5 

-75-3* 

I 

•73 

— 

90 

31 

-95* 

II 

.2 

4- 

8 

-60 

4 

— 

80 

48 

.6 

-90 

II 

.8 

5 

-40 

12 

-5 

— 

70 

60 

-4 

-80 

15 

.2 

.6. 

8 

-30 

21 

— 

60 

70 

-70 

22 

n. 

5 

—  20 

35 

•5 

— 

50 

79 

-60 

31 

-7 

19 

-18 

40 

•5 

—  • 

40 

86 

•3 

—  50 

43 

30 

-16 

48 

— 

30 

91 

.1 

-40 

54 

•5 

43- 

5 

-14 

72 

— 

20 

95 

.2 

-30 

66 

.2 

60 

-13 

90 

— 

IO 

89 

—  20 

79 

•5 

76. 

5 

—  10 

96 

•5 

— 

7-3 

IOO 

-12.5 

90 

90 

—   7.1 

IOO 

*  Eutec.. 

SOLUBILITY  DATA,  DETERMINED  BY  THE  FREEZING-POINT  METHOD  (see  footnote, 

p.  i),  ARE  GIVEN  FOR  THE  FOLLOWING  MIXTURES: 
Bromine  +  Methyl  alcohol    (Maass  and  Mclntosh,  1912.) 

+  Ethyl  alcohol 
"        +  Ethyl  acetate 

"          +  Ethyl  bromide     (Wroczynski  and  Guye,  1910.) 

"          +  Iodine  (Meerum-Terwogt,  1905;  Kruyt  and  Heldermann,  1916.) 

41          +  Sulfur  (Ruff  and  Winterfeld,  1903.) 

TOO  grams  saturated  solution  of  bromine  in  carbon  disulfide  contain  45.4 

grams'Br  at  —95°,  39  grams  at  - 1 10.5°,  and  36.9  grams  at  - 1 16°. 

(Arctowski,  1895  —  1896.) 

DISTRIBUTION  OF  BROMINE  BETWEEN  WATER  AND  CARBON  TETRACHLORIDE 


AT  0°. 
(Jones  and  Hartmann,  1916.) 

Gm.  Br»  per 
Gm.  CCU 

Solution. 

Density  , 
CCU-Br2. 

jms.  Bromine  per  Litei 

'•  Gm.  Brcper 
'  Gm.  CCU. 
Solution. 

Density    / 
CCl4-Br2. 

Gms.  Bromine  per  Liter. 

HzO 
Layer. 

ecu 

Layer. 

H20 
Layer. 

ecu 

Layer. 

0.01640 

1.6454 

1.28 

26.99 

0.07261 

1.6896 

5-35 

122.82 

0.01847 

1.6470 

1.44 

30-45 

O.o8l62 

1.6972 

6.03 

138.66 

0.05433 

I-6755 

4.12 

91.12 

0.08661 

I.70I2 

6.30 

184.41 

0.06126 

1.6809 

4-59 

103.07 

0.1646 

1.7667 

II  .22 

29I.IO 

161  BROMINE 

DISTRIBUTION  OF  BROMINE  AT  25°  BETWEEN  WATER  AND: 

(Calculated  from  results  of  Jakowkin,  1895.    Those  in  parentheses  from  Herz  and  Kurzer,  1910.) 

Carbon  Disulfide.  Bromoform.  Carbon  Tetrachloride. 

Gms.  Br.  per  Liter  of;  Gms.  Br.  per  Liter  of:  Gms.  Br.  per  Liter  of; 

Aq. 'Layer.  CS2  Layer.  Aq.  Layer.   CHBr3  Layer.        Aq.  Layer.        CC14  Layer. 

0.5          36  (35)  o-5  33  0.5          15  (13) 

1  80  (75)  i  66  i  28  (23) 

2  163    (155)  2  136  2  60    (45) 

3  240  (230)  3  206  3  90  (70) 

4  330  (31°)  4  276  4  123  (95) 

5  420  (395)  5  346  5  156  (122) 

6  515  (480)  6  415  6  190  (150) 

7  620  (565)  ...  ...  8  260  (220) 

10  340  (300) 

12  430  (400) 

Lewis  and  Storch  (1917)  point  out  that  Jakowkin  (1896)  failed  to  take  into 
consideration,  the  hydrolysis  of  the  bromine  in  the  aqueous  phase  in  the  very 
dilute  solutions.  They  used  o.ooi  n  HC1  which  prevents  the  hydrolysis  but  is 
presumably  too  dilute  to  affect  the  true  solubility.  The  distribution  coefficient 
found  in  this  way,  given  in  terms  of  mols.  Br  per  1000  gms.  H2O,  divided  by  the 
mol.  fraction  of  Br  in  the  CC14,  is  0.3705  at  25°.  These  authors  also  give  a  series 
of  determinations  of  the  distribution  of  bromine  between  o.i  n  HBr  and  CCU 
at  25°. 

DISTRIBUTION  OF  BROMINE  BETWEEN  WATER  AND  MIXTURES  OF  CARBON 
DISULFIDE  AND  CARBON  TETRACHLORIDE  AT  25°. 

(Herz  and  Kurzer,  1910.) 

75  Vol.  %  CS2+25  Vol. 
%  CC14. 

Gms.  Bromine  per  Liter. 

Aq.  Layer.  CS2+CCU  Layer. 

0.71  46 

1.34  87.2 

3.98  213.8 

5.06  330.5 

6.82  444-2 


DISTRIBUTION  OF  BROMINE  AT  25°  (Herz  and  Rathmann,  1913)  BETWEEN: 

Water  and  Tetrachlorethane.  Water  and  Pentachlorethane. 

Grams  Bromine  per  Liter.  Gms.  Bromine  per  Liter. 

Aq.  Layer.               CzIfeCU  Layer.  Aq.  Layer.               C2H.CU  Layer. 

0.216                 6.47  0.402                10.70 

0.592                18.20  0.670                18.29 

0.944               29.46  0.864               23.49 

1.348           41.65  1.300           35.46 

2.444               74-57  2.408               67.44 


25  Vol.  %  CSa  +  75  Vol. 
%  CC14. 

Gms.  Bromine  per  Liter. 

,  50  Vol.  %CSi+5oVol. 
%  CC14. 

Gms.  Bromine  per  Liter. 

Aq.  Layer. 
0.79 

i-53 
2.32 
2.98 
3.66 
5-26 

7-95 
9.66 

CS2+CCU  Layer. 
28.4 
58.4 

86.6 

111.3 
137.8 

205.1 

324.9 
432.2 

Aq.  Layer. 
0.63 
I.I9 
I.76 
2-45 
2-95 
6.47 

7-97 

CS2+CCU  Layer. 
28.7 

54-5 
8l.I 
II0.9 
132.9 

343-8 
447-7 

BROMINE 


162 


DATA  FOR  THE  DISTRIBUTION  OF  BROMINE  BETWEEN  AQUEOUS  SALT  SOLUTIONS 
AND  ORGANIC  SOLVENTS  ARE  GIVEN  BY  THE  FOLLOWING  INVESTIGATORS: 


Immiscible  Solvents.  t°. 

Aqueous  CdBrz+CCU  25 

Aqueous  CdBr2.2KBr+CCl4  25 

Aqueous  HBr-j-CCL;  25 

Aqueous  HgBr2+CCLi  25 

Aqueous  HgBra^KBr-fCCU  25 

Aqueous  KBr+CCU  o 

Aqueous  KBr-j- €82  32.6 


Authority. 
(Van  Name  and  Brown,  1917.) 

(Lewis  and  Storch,  1917.) 

(Herz  and  Paul,  1914;  Van  Name  and  Brown,  1917.) 

(Van  Name  and  Brown,  1917.) 

(Jones  and  Hartmann,  1916.) 

(Roloff,  1894.) 


BROMOFORM   CHBr3. 

100  cc.  H2O  dissolve  0.125  gin.  CHBr3  at  I5°-2O°. 


(Squire  and  Caines,  1905.) 


SOLUBILITY  (Freezing-point  lowering  data,  see  footnote,  p.  i)  FOR 
MIXTURES  OF:. 


Bromoform  and  Liquid  Carbon  Dioxide. 

(Biichner,  1905-06.) 


Bromoform  and  Toluene. 
(Baud,  1912.) 

'  Cms.  CHBra  per 

t°  of  Freezing.  !        100  Cms.  Solid  Phase. 

CHBrs+CeHs.CHs. 


+  7.7 

IOO 

CHI 

-11.4 

86.6 

(i 

—  22.2 

75-6 

tt 

-30.9 

69.8 

14 

-48.5 

60.3 

11 

Gms.  CHBrs  per 
t°.  100  Gms. 

CHsBr+C02. 

—31  o 

-32  3-7 

-30  4-9 

-16  13-5 

-  8  24 

-  5  35-2-67.7  quad.pt. 

-  3-5  92-1 

BRUCINE  C2iH20(OCH3)2N202.4H20. 

SOLUBILITY  OF  BRUCINE  IN  SEVERAL  SOLVENTS. 

Qnl«»nf  t o     Gms-  Brucine  per  A.ithnritv 

Solvent.  t.   I00  cms.  Sat.  Sol. 

18-2  2  o .  056-0 . 1 25  (Muller,'i903 ;  Squire  and  Caines,  1905;  Zalai,  1910.) 

20  12  (Scholtz,  1912.) 

1 8-2 2     I .  Il-l .  86     (Muller,  1903;  Schaefer,  1913.) 
0.08  "  "    . 

1.96 


Water 

Aniline 
Benzene 

Carbon  Tetrachloride  18-22 
"  "  20 

Chloroform  25 

Trichlor  Ethylene  15 

Ether  18-22 

Ethyl  Acetate  18-22 

Ethyl  Alcohol  25 

Diethylamine  20 

Methyl  Alcohol  25 

Petroleum  Ether 
Glycerol 
Pyridine 


ii. 6 
2-5 
o-75 
4.26 

45-2 
1.6 

55-6 


(Schindelmeiser,  1901;  Gori,  1913.) 
(Schaefer,  1913.) 
(Wester  and  Bruins,  1914.) 
(Muller,  1903.) 


Aq.  50%  Pyridine 
Piperidene 


(Schaefer,  1913.) 
(Scholtz,  1912.) 
(Schaefer,  1913.) 

18-22  0.055-0.088  (Muller,  1903;  Zaki,  1910.) 
1 8-2  2  2  .  2  (Muller,  1903.) 

2O  28  (Scholtz,  1912.) 

20-25          21.9  (Dehn,  1917.) 

20-25          3T-6  " 

20  I  (Scholtz,  1912.) 


Results  for  the  solubility  of  brucine  and  brucine  sulfate  in  mixtures  of  alcohol, 
chloroform  and  benzene  are  given  by  Schaefer  (1913). 

BRUCINE  Per  CHLORATE  C21H20(OCH3)2N2O2.HC1O4. 

loo  gms.  H2O(+  2%HC1O4)  dissolve  0.15  gm.  of  the  salt  at  18°. 

(Hofmann,  Roth,  Hobold  and  Metzler,  1910.) 


163  BEUCINE 

BRUCINE   SULFATE. 

100  cc.  methyl  alcohol  dissolve  0.28  gm.  brucine  sulfate  at  25°.      (Schaefer,  1913.)^ 

"        ethyl  "  "         1.66     "  "  (Schaefer,  1913.) 

"       chloroform  O.6  (Schaefer.  1913.) 

BRUCINE  d,  /,  and  i  TARTRATE. 

SOLUBILITY  OF  EACH  OPTICAL  ISOMER  IN  WATER    (Dutiih,  1912.) 

Gms.  per  100  Cms.  Water. 

t°.  t * \ 

d  Tartrate.  I  Tartrate.          Racemic  Tartrate. 

20  ...  ...  1.38 

25  1.008  1.84 

35  1-272  3-24 

44  1.590  4-64 

50  1.854  6.56 

BUTANE  C4H10. 

SOLUBILITY  IN  WATER  AT  t°  AND  760  MM. 

t°.  o°.  4°.  10°.  15°.  20°. 

Vol.  C4Hio  per 
icovols.  H2O         3.147          2.77        2.355  2.147        2.065 

DiphenylBUTADIENE. 

Freezing-point  curves  (solubility,  see  footnote,  p.  i),  are  given  by  Pascal 
(1914)  for  mixtures  of  diphenylbutadiene  and  each  of  the  following  compounds: 
diphenyldiacetylene,  diphenylhydrazine  and  cinnamylidene. 

BUTYL  ACETATE  CHj.C02.CiH9. 

SOLUBILITY  OF  BUTYL  ACETATE  AND  OF  BUTYL  FORMATE  IN  MIXTURES 
OF  ALCOHOL  AND  WATER. 

(Bancroft  —  Calc.  from  Pfeiffer  —  Phys.  Rev.  3.  205,  '? 


cc.  H2O  added  to  cause  separation  of  a 
Air  h  1  second  phase  in  mixtures  of  the  given 

in  Mixture  quantity  of  alcohol  and  3  cc.  portions  of: 

Butyl  Formate.  Butyl  Acetate. 

3          3-45        2-°8 
6          8.83        6.08 

9  14-75  IO-46 

12  21.45  J5-37 

15  29.65  20.42 

18  39.0  25".  60 

21  51.8  31.49 

24  <*>  37-48 

27  43-75 

30  50-74 

33  59-97 

100  cc.  H2O  dissolve  0.7  cc.  isobutyl  acetate  at  25°.  (Bancroft.) 

IsoBUTYL  ACETATE,  etc. 

SOLUBILITY  IN  WATER.    (Traube,  1884;  at  20°,  Vaubel,  1899.) 

Grams  Com- 

*  o  Compound.  pound  per  zoo 

Grams  HaO. 

22  Iso  Butyl  Acetate  0.5 

22  Iso  Butyl  Formate  x.o 

20  Normal  Butyric  Aldehyde  3 .6 

20  Iso  Butyric  Aldehyde  10.0 


BUTYL  ALCOHOLS  164 

Secondary  BUTYL  ALCOHOL  CH3.CHOH.CH2CH,. 
Iso  BUTYL  ALCOHOL  (CH3)2CH.CH2OH. 


SOLUBILITY  OF  BUTYL  ALCOHOLS  IN  WATER,  "SYNTHETIC  METHOD." 
(see  Note,  p.  16). 
(Alexejew,  1886.) 

Secondary  Butyl  Alcohol  Iso  Butyl  Alcohol 

and  Water.  and  Water. 

Cms.  Secondary  Butyl  Alcohol  per  too  Gms.        Cms.  Iso  Butyl  Alcohol  per  100  Cms. 

Aqueous  Alcoholic 

Layer.  Layer. 


13  85 

9  84 

7-5  83 

7  82 

7  77 

8  72 

16  62 

28  50 

49 


Additional  determinations  of]  the  reciprocal  solubility  of  secondary  butyl 
alcohol  and  water  are  given  by  Dolgolenko  (1908).  This  investigator  prepared 
three  fractions  of  980-o.8.60,  98.6°-99°  and  99°-99.5°  boiling  point  respectively, 
and  determined  the  curve  for  each  fraction  and  water  by  the  "synthetic  method." 
The  first  fraction  gave  a  closed  curve  having  both  a  lower  and  an  upper  critical 
solution  temperature,  while  the  other  fractions  gave  curves  with  only  an  upper 
critical  solution  temperature,  and  in  other  respects  in  fair  agreement  with  the 
results  of  Alexejew  as  shown  in  the  above  table.  The  explanation  of  this  differ- 
ence in  the  case  of  the  first  fraction,  is  supposed  to  be  that  this  fraction  contained 
a  larger  proportion  of  tertiary  butyl  alcohol  than  the  others,  due  to  the  lower 
boiling  point  of  this  isomer.  Since  the  tertiary  alcohol  is  entirely  miscible 
with  secondary  alcohol  and  water  its  presence  would  restrict  the  boundaries  of 
inhomogeneity  and,  therefore,  tend  to  favor  a  closed  curve  for  the  system. 

SOLUBILITIES,  DETERMINED  BY  THE  FREEZING-POINT  METHOD  (see  footnote,  p.  i), 
ARE  GIVEN  FOR  THE  FOLLOWING  MIXTURES  CONTAINING  BUTYL  ALCOHOLS. 

Isobutyl  alcohol  +  Water  (Dreyer,  1913.) 

"        +  Liquid  CO2  (Buchner,  1905-06.) 

Normal  butyl  alcohol  +  Water  (Dreyer,  1913.) 

"  "  "        +  Liquid  CO2  (Buchner,  1905-06.) 

Secondary  butyl  alcohol  +  Water  (Dreyer,  1913;  Timmermans,  1907,  1910,  X9«.) 

}"  "         +        "        +  Hydroquinine  (Timmermans,  1907.) 

Tertiary  butyl  alcohol  -f  Water.  (Dreyer,  1913.) 


Aqueous 

Alcoholic 

* 

Layer. 

Layer- 

—  20 

27 

66 

—  10 

28 

60 

0 

27-5 

56 

10 

26.0 

57 

20 

22-5 

60 

30 

18 

63-5 

40 

16 

65-5 

6o 

13 

67 

80 

IS 

63 

100 

20 

52 

io7crit. 

temp.         33 

120 

130 

133  crit.  ternp. 

1  65  IsoBUTYL  ALCOHOL 

DISTRIBUTION  OF  ISOBUTYL  ALCOHOL  BETWEEN  WATER  AND  COTTON  SEED 

OIL  AT  25°.      (Wroth  and  Reid,  1916.) 

Cms.  C4H9OH  per  TOO  cc.  Cms.  C«H»OH  per  too  cc. 

OU  Layer.          HZO  Layer.  Ratio.  [Oil  Layer.         H2O  Layer.          -  Ratio 

1.168          2.043  i-74  1-375          2-3oi          1.67 

1.276          2.250  1.76  1-405          2.429          1.72 

1.288          2.135  X-6S  x-495          2-45o          1-64 

The  partition  coefficient  of  tertiary  butyl  alcohol  (CH3)2C(OH)CH3,  between 

olive  oil  and  water  is  given  as  0.176  at  ord.  temp.  (Baum,  1899.) 

IsoBUTYLAMINE  HYDROCHLORIDE   (CH3)2CHCH2NH2.HC1. 

IOO  gms.  H2O  dissolve  238.9  gms.  of  the  salt  at  25°.  (Peddle  and  Turner,  1913.) 

IOO  gms.  CHC18  dissolve  11.56  gms.  of  the  salt  at  25°.       (Peddle  and  Turner,  1913.) 

BUTYLCHLORAL  CH3CHC1.CC12CHO. 

The  distribution  coefficient  of  butylchloral  between  oil  and  water  is  given  as  1.6. 

(Meyer,  1907.) 

BUTYLCHLORALHYDRATE  CH3CHC1.CC12.CH(OH)2. 

100  gms.  H2O        dissolve      2.7  gms.  butylchloralhydrate  at  15.5° 

(Greenish  and  Smith,  1903.) 

2.3    "  "  at  I5°-20°. 

(Squire  and  Caines,  1905.) 

glycerol       "        100       "  "  at  I5°-2O°. 

(Greenish  and  Smith,  1903.) 

The  partition  coefficient  of  butylchloralhydrate  between  olive  oil  and  water  is 
given  as  1.589  at  ord.  temp.  (Baum,  1899.) 

BUTYRIC  ACIDS   (normal)  CH3(CH2)2COOrJ;  (iso)  (CH3)2CH.C6OH. 

SOLUBILITY  OF  NORMAL  BUTYRIC  ACID  IN  WATER,  DETERMINED  BY  THE 
FREEZING-POINT  METHOD.    (Faucon,  1909,  1910.) 

t-of  Gms.  Acid  per  f.  of          Gms.  Acid  per  t<>  of  Gms.  Acid  per  100 

Congealing.  Congealing.  '  Congealing.  Gms.  Mixture 


oo—  3.57      67.38        —13-40        87.62Eutec. 

—  i.  08          5.12        —  5.20      75  —12.40        90.08 

—  2.70         12.75        —  6.80      80  —10  95  .92 

—  2.96         25.32        —  8.61      84  —  8  98.60 
-3.07         50.60        -10.25      85.41        -  5.40        99.15 
-3.14         59.72        -12.54      86.54        -  3.12       loo 

Higher  values  for  the  temperature  of  congealing  of  the  above  mixtures  are 
given  by  Ballo  (1910).  For  additional  data  see  also  Timmermans  (1907)  and 
Tsakalotos  (1914).  Data  for  the  miscibility  of  normal  butyric  acid  and  water 
are  also  given  by  Faucon.  The  curve  is  entirely  in  the  metastable  region.  The 
mixtures  are  either  opalescent  or  completely  homogeneous  and  never  form  two 
distinct  layers,  even  with  the  application  of  centrifugal  force.  The  results  are 
as  follows: 

t°  of  opalescence    —5.2     —4.2     —4        —  3.8crit.  t.    —4-5     —  7 

Gms.  acid  per  100 

v  gms.  mixture        25         30         35          40  50          58  .  2 

SOLUBILITY  OF  ISOBUTYRIC  ACID  IN  WATER,  DETERMINED  BY  THE  FREEZING- 
POINT  METHOD.     (Faucon,  1910.) 

The  congealing  temperatures  for  mixtures  containing  up  to  60  grams  iso- 
butyric  acid  per  ipo  gms.  coincide  with  the  results  given  in  the  above  table  for 
normal  butyric  acid  and  water.  For  higher  concentrations  the  following  results 
were  obtained. 

t°  of  congealing  -3.09      —3-35       ~3-6i        -12.5      -80 

Gms.  acid  per  100 

gms.  mixture  70.10        82.08        86.44  97-21      IO° 


BUTYRIC  ACID 


166 


MlSCIBILITY   OF    ISOBUTYRIC   ACID  AND   WATER,    DETERMINED   BY  THE 

"SYNTHETIC  METHOD." 

(Smirnoff,  1907.) 

Gms.  "Acid  per  100  Gms.: 


10.05 

12 
14 

16 
18 

20 
22 

22.5 
23 


Upper  Layer. 

Lower  Layer. 

69.08 

17.82 

67.I 

18.3 

64.9 

I9.I 

62.3 

20 

59-2 

21.  1 

55-4 

22.8 

49 

25.8 

46 

27 

4i 

29 

34-7 


Determinations  varying  more  or  less  from  the  above  are  given  by  Rothmund 
(1898),  Friedlander  (1901)  and  Faucon  (1910).  The  discrepancies  are  shown  by 
Smirnoff  to  be  due  to  the  effect  of  variations  in  purity  of  the  isobutyric  acid  upon 
the  position  of  the  curve.  Smirnoff  fractionated  the  purest  obtainable  acid  and 
determined  the  miscibility  curve  for  each  fraction.  The  above  results  were 
obtained  with  fraction  4  of  boiling  point  154°-!  55°,  twice  refractionated. 

An  extensive  series  of  determinations  are*  given  by  Smirnoff  of  the  effect  of 
various  percentages  o£  different  salts  upon  the  temperature  of  immiscibility  of 
aqueous  16.46%  isobutyric  acid  solution. 

DISTRIBUTION  OF  BUTYRIC  ACID  BETWEEN  WATER  AND  BENZENE  AT  I3°-I5° 

(Georgievics,  1913.) 

Gms.  Acid  Found  per- 


Gms.  Butyric  Acid 
Used. 


2.0044 
2.9968 
3.5028 
4.0088 
4-5342 


150  cc. 
Benzene  Layer. 

1.7643 
2.6965 

3-I740 


25  cc. 
HzO  Layer. 

o . 2401 

0.3003 
0.3288 

0-3544 
0.3821 


4-I52I 

The  distribution  ratio  of  normal  butyric  acid  between  water  and  benzene  at 
room  temperature  was  found  by  King  and  Narracott  (1909),  to  be  I  to  0.7585, 
and  for  isobutyric  acid,  the  ratio  was  I  to  0.810. 

One  determination  of  the  distribution  of  butyric  acid  between  sat.  aqueous 
CaCl2  solution  and  kerosene  gave  7.2  gms.  acid  per  100  gms.  aqueous  layer  and 
92.8  gms.  per  100  gms.  kerosene  layer  at  ord.  temp.  (Crowell,  1918.) 

DATA  FOR  THE  FOLLOWING  TERNARY  SYSTEMS  CONTAINING  NORMAL 
BUTYRIC  ACID  ARE  GIVEN  BY  TIMMERMANS,  1907. 
Normal  Butyric  acid  +  Water  +  Azobenzene. 

+  Barium  nitrate. 
+  Benzophenone. 
-j-  Camphor. 
+  Cane  sugar. 
-j-  Mannite. 
-j-  Naphthalene. 
+  Potassium  sulfate. 
+  Sodium  chloride. 

Freezing-point  data  are  given  for  mixtures  of  n  butyric  acid  and  formamide  by 
English  and  Turner  (1915),  and  for  mixtures  of  trichlorobutyric  acid  and  dimethyl 
pyrone  by  Kendall  (1914). 


167  CADMIUM  BROMIDE 

CADMIUM    BROMIDE    CdBr,. 

SOLUBILITY  IN  WATER. 

(Dietz  —  Ber.  32,  95,  '99;  Z.  anorg.  Chem.  20,  260,  '09;  Wiss.  Abh.  p.t.  Reichanstalt,  3,  433,  'oo;  see  also 
Eder  —  Dingier  polyt.  J.  221,  189,  '76;  Etard  —  Ann.  chim.  phys.  [7]  2,  536,  '94.) 

Gms.CdBr2   Mols.  CdBr2  Gms.  CdBr2  Mols.  CdBr2 

t°.  per  ioo  Gms.      per  ioo  Solid  Phase.  t°.  per  ioo  Gms.      per  ioo      Solid  Phase. 

Solution.      Mols.  H2O.  Solution.      Mols.  H2O. 

o  37.92  4.04  CdBr2.4H2O       40  60.65  10.20  CdBr2.H2O 

18  48.90  6.21  45  60.75  10.24 

30  56.90  8.73  60  61.10  10.39 

38  61.84  10.73  80  62.29  10.48 

35  60.29  10.05  CdBr2.H2O       ioo  61.63  .10.63 

Density  of  saturated  solution  at  18°=  1.683. 

SOLUBILITY  OF  CADMIUM  BROMIDE  IN  ALCOHOL,  ETHER,  ETC. 

ioo  gms.  sat.  solution  of  CdBr2.4H2O  in  abs.  alcohol  contain  20.93  gms-  CdBr2 

at  15°.  (Eder.) 

ioo  gms.  sat.  solution  of  CdBr2.4H2O  in  abs.  ether  contain  0.4  gm.  CdBr2  at  15°. 

(Eder.) 

ioo  gms.  absolute  acetone  dissolve  1.559  gms.  CdBr2  at  18°.     dj^  sat.  sol.  = 

0.8073.  (Naumann,  1904.) 

ioo  gms.  benzonitrile  dissolve  0.857  gm.  CdBr2  at  18°.  (Naumann,  1914.) 

ioo  gms.  anhydrous  hydrazine  dissolve  40  gm.  CdBr2  at  room  temp. 

(Welsh  and  Broderson,  1915.) 

RECIPROCAL  SOLUBILITIES,  DETERMINED  BY  THE  METHOD  OF  LOWERING  OF  THE 
FREEZING-POINT  (see  footnote,  p.  i),  ARE  GIVEN  FOR  THE  FOLLOWING  MIXTURES: 

Cadmium  Bromide  +  Cadmium  Chloride  (Nacken,  1907;  Ruff  and  Plato,  1903.) 

-j-  Cadmium  Iodide  (Nacken,  1907.) 

+  Calcium  Fluoride  (Ruff  and  Plato,  1903.) 

+  Cuprous  Bromide  (Herrmann,  1911.) 
-j-  Potassium  Bromide  (Brand,  1913.) 

+  Sodium  Bromide 
+  "     +  Potassium  Bromide     " 

CADMIUM   (Mono)AMMONIUM  BROMIDE  CdBr2.NH4Br 
SOLUBILITY  IN  WATER. 

(Rimbach,  1905;  Eder.) 
ioo  Grams  Solution  contain  Gms.  Atomic  Relation.       G.  CdBr2.NH4Br 


(1   . 

Cd. 

Br. 

NH4. 

'Cd    : 

Br    : 

NH*. 

per  ioo  Lri 
Solution. 

i.o 

16.33 

34.87 

2.63 

I 

3 

I 

53-82 

14.8 

17.40 

37-15 

2.80 

I 

3 

I 

58.01 

52.2 

19.79 

42.38 

3-21 

I 

3 

I 

65.3I 

no.  i 

22.99 

49.17 

3-72 

I 

3 

I 

75.98 

ioo  gms.  sat.  solution  of  CdBr2.NH4Br  in  abs.  alcohol  contain  15.8 
gms.  double  salt  at  15°  (Eder). 

ioo  gms.  sat.  solution  of  CdBr2.NH4Br  in  abs.  ether  contain  0.36 
gm.  double  salt  at  15°  (Eder). 

CACODYLXC  ACID  (CH3)2AsO.OH. 

ioo  cc.  H2O  dissolve  about  200  gms.  cacodylic  acid  at  15°.  (Squire  and  Caines,  1905.) 
ioo  cc.  90%  alcohol  dissolve  about  28.5  gms.  cacodylic  acid  at  15°.  "  " 


CADMIUM  BROMIDE 


168 


CADMIUM    (Tetra)    AMMONIUM    BROMIDE   CdBr2.4NH4Br. 
SOLUBILITY  IN  WATER. 

(Rimbach.) 

The  double  salt  is  decomposed  by  water  at  temperatures  below  1 


ioo  Gms.  Solution  contain  Gms 


t> 

* 

Cd. 

Br. 

NH4.           Cd 

:     Br     :    NH4.  * 

Cd    : 

Br      ; 

;      NH4.  " 

0 

.8 

14.72 

50.46 

6.67            I 

4 

.82       2 

.82 

I      10.02 

8.02 

13 

•o 

14-95 

51  .48 

6.85            I 

4 

-85       2 

•85 

I       II 

•57 

9-57 

44.0 

15  -OI 

53-85 

7-35        i 

5 

•04    3 

.04 

I 

6 

.84 

4.84 

76 

•4 

14.6 

55-28 

7.80      I 

5 

•32     3 

•32 

I 

6 

•63 

4-63 

123 

•5 

15  .5 

59-50 

8.45      I 

5 

•38    3 

•38 

I 

7 

.40 

5-40 

1  60 

.0 

14-7 

62.67 

9-43        i 

5 

•99    3 

•99 

I 

6 

•03 

4-03 

CADMIUM  (Mono)  POTASSIUM 

BROMIDE 

CdBr2. 

KBr.H2O. 

SOLUBILITY 

IN 

WATER. 

(Rimbach;  see  also  Eder.) 

*o 

ioo  Gms.  Solution 

contain  Gms. 

Atomic  Relation  in  Sol. 

Gms.CdBr2.KBr 

* 

Cd.                Br.            K. 

Cd     : 

Br 

:      K. 

Solution. 

0 

•4 

IS- 

4i     33- 

o       5.42 

I 

3 

I 

53-63 

JL5 

.8 

16. 

85    35- 

96      5.86 

I 

3 

I 

58.61 

5° 

•  O 

19. 

58    41. 

86    6.85 

I 

3 

I 

67-87 

112 

•5 

22  . 

24    48. 

28    8.14 

0.98 

3 

1.03 

78.11 

CADMIUM    TetraPOTASSIUM    BROMIDE  is    decomposed    by    water    at 
ordinary  temperatures. 


CADMIUM   (Mono)RUBIDIUM  BROMIDE  CdBr2.RbBr. 
SOLUBILITY  IN  WATER. 

(Rimbach.) 


to 

ioo  Gms. 

Solution  contain  Gms.                        Atomic  Relation  in  Sol.      Gms.  CdBrz.RbBr 

. 

Cd. 

Br. 

Rb. 

'  Cd       : 

Br 

:     Rb.' 

Solution. 

o 

4 

8-37 

17-93 

6-43 

I 

3 

1.  01 

32. 

65 

14 

•5 

10, 

,72 

23.02 

8.30 

O. 

99 

3 

I  .OI 

41. 

87 

49 

.2 

15.01    32.13 

11.51 

I 

3 

I 

58. 

54 

107 

•5 

19.65 

41.12 

14.06 

I. 

02 

3 

0.96 

75- 

77 

CADMIUM 

(Tetra)RUBIDIUM 

BROMIDE 

CdBr2.4RbBr. 

SOLUBILITY  IN  WATER. 

(Rimbach.) 

^0              ioo  Gms.  Solution  contain  Gms.                       Atomic 

Relation  in  Sol.     ^ 

per  ioo  Gms. 
Solution. 

'   Cd 

Br 

Rb. 

'Cd 

:      Br 

:      Rb. 

0 

-5 

5 

.70 

24.94 

17.97 

0. 

98 

6 

4-05 

47- 

95 

13 

•5 

6 

•55 

28.74 

20.74 

0. 

97 

6 

4-05 

55- 

17 

•5 

8 

•25 

35-51 

25-39 

0. 

99 

6 

4.O2 

68. 

82 

114 

•5 

9 

•50 

40.67 

29.0O 

I  . 

00 

6 

4.0 

79- 

04 

169 


CADMIUM  BROMIDE 


CADMIUM    (Mono)    SODIUM    BROMIDE    CdBra.NaBr2jH,O. 
SOLUBILITY  IN  WATER,  ETC.,  AT  15°. 

(Eder  — Ding,  polyt.  J.  221,  189,' '76.) 


Solvent. 


Gms.  CdBr2.NaBr  per  100  Cms. 
Solution.  Solvent.' 

Water  49 -o  96.1 

Absolute  Alcohol          21.2  27.0 

Absolute  Ether  0.52  0.53 


Solid 

Phase. 


CdBr2.NaBr.2iH2O 


CADMIUM  CHLORATE  Cd(ClO3)2.2H2O. 

SOLUBILITY  IN  WATER. 

(Meusser,  1902  ) 


Gms. 


-  6.5 
-I3.0 
—  2O.O 
-15.0 


Solution. 
26.18 

52.36 
72.10 

72.53 


Mols. 

Gms. 
to      Cd(ClO»)z 
"  '  per  100  Gms 

Mols. 
Cd(C103)2     solid  Phase. 
.     per  100 

er  i£b.  °  j 

Solution. 

Mols.  H2O. 

3 

.07 

Ice 

db 

O 

74 

•95 

25 

.92 

Cd(ClO3)2.2HzO 

9 

•52 

" 

18 

76 

.36 

27 

.98 

'* 

22 

.47    Cd(ClO3)2.2HiO 

49 

80 

.08 

34 

.82 

M 

22 

.87 

65 

82 

-95 

42 

.14 

" 

;.  solution 

at  18°  =  2 

.284. 

CADMIUM  CHLORIDE  CdCl2.2|H2O. 

SOLUBILITY  IN  WATER. 

(Dietz  —  W.  Abh.  p.  t.  Reichanstalt  3,  433,  'oo;  above  100°,  Etard  —  Ann.  chim.phys.fr]  2,  536,  '94.) 


G.  CdCl2  per  Mols.CdCl2        ~  ,.  . 
t  °.        100  Gms.        per  100            ^T 
Solution.    Mols.H2O.        Phase' 

G.CdCljper 
t  °.         loo  Gms. 
Solution. 

-  9 

43 

•S8 

7 

•5" 

+  10 

57 

•47 

0 
+  10 

49 
55 

•39 
•58 

9 

12 

.6 
•3 

•CdCI2.4H20 

20 

40 

57 
57 

•35 
5i 

15 

59 

.12 

14 

.2. 

60 

57 

•7i 

—  10 

44 

•35 

7 

.8" 

80 

58 

.41 

o 

47 

•37 

9 

•  O 

100 

59 

•S2 

+  18 

52 

•53 

10 

•9 

•CdCI2.2iH2O 

150 

64 

.8 

30 

56 

.91 

12 

.8 

(monoclinic) 

200 

72 

•  0 

36 

57 

.91 

13 

•5. 

270 

77 

•7 

Mols.CdCl, 

per  TOO 
Mob.H,0. 


13.2 

13-3 
13-4 

13.8 

14. 4J 


Density  of  saturated  solution  at  18°  =  1.741. 


Solid 

PV,~<M 
Phase' 


100  gms.  abs.  ethyl  alcohol  dissolve  1.52  gms.  CdCl2  at  I5°.5. 

100  gms.  abs.  methyl  alcohol  dissolve  1.71  gms.  CdCl2  at  i5°-5.    (de  Bruyn,  1891.) 

loo  gms.  abs.  methyl  alcohol  dissolve  1.5  gms.  CdCl2  at  the  crit.  temp. 

(Centnerszwer,  1910.) 

ioo  gms.  benzonitrile  dissolve  0.063  gm.  CdCl2  at  18°.  (Naumaan,  1914.) 


CADMIUM  CHLORIDE 


170 


RECIPROCAL  SOLUBILITIES,  DETERMINED  BY  THE  METHOD  OF  LOWERING  OF 
THE  FREEZING-POINT  (see  footnote,  p.  i),  ARE  GIVEN  FOR  THE  FOLLOWING 
MIXTURES: 


Cadmium  Chloride  +  Cadmium  Iodide 
"  "         +  Cadmium  Fluoride 

+  Cadmium  Sulfate 
+  Calcium  Chloride 
"  "        +  Cuprous  Chloride 

"        +  Lead  Chloride 


(Nacken,  1907  (c);  Ruff  and  Plato,  1903.) 
(Ruff  and  Plato,  1903) 


(Sandonnini,  1911,  1914;  Menge,  1911.) 

(Herrmann,  1911.) 

(Sandonnini,  1912,  1914;  Herrmann,  1911.) 

+  Magnesium  Chloride  (Menge,  1911.) 

-f-  Manganese  Chloride  (Sandonnini,  1914;  Sandonnini  and  Scarpa,  1911.) 

-j-  Mercuric  Iodide  (Sandonnini,  1912.) 

•f-  Potassium  Chloride    (Brand,  1911.) 

-j-  Sodium  Chloride 

+        "  .  "        +  Potassium  Chloride    (Brand,  1911.) 

+  Strontium  Chloride  (Sandonnini,  1911;  1914.) 

+  Thallium  Chloride  (Korreng,  1914;  Sandonnini,  1913.) 

-j-  Tin  (ous)  Chloride  (Herrmann,  1911;  Sandonnini,  1914.) 

4"  Zinc  Chloride  (Herrmann,  1911.) 


CADMIUM    AMMONIUM    CHLORIDE   CdCl2.NH4Cl. 
SOLUBILITY  IN  WATER. 

(Rimbach  —  Ber.  30,  3075,  1897.) 
IPO  Gms.  Solution  contain  Cms.          Gms.  CdCl2.NH*Cl  per  100  Cms. 


*    . 

'Cd. 

Cl. 

NH. 

'Solution. 

Water. 

2.4 

14.26 

13-44 

2.24 

29.94 

42.74 

16.0 

15.82 

I5-07 

2.56 

33-45 

50.26 

41.2 

18.61 

17.46 

2.89 

38.96 

63-83 

63.8 

20.92 

J9-73 

3-34 

43-99 

78-54 

105.9 

24.70 

23-52 

4.01 

52-23 

109-33 

OADMIUM    (Tetra)    AMMONIUM    CHLORIDE   CdCl2.4NH4Cl. 
IN  CONTACT  WITH  WATER. 


The  salt  is  decomposed  in  aqueous  solution. 

(Rimbach.) 


100  Gms.  Solution  contain  Gms. 


Atomic  Relation  in  Solution. 


V        • 

'   Cd. 

Cl. 

NH*. 

Cd 

:      Cl      : 

NH*: 

3-9 

5-75 

18.17 

7-37 

i 

9.96 

7.96 

16.1 

6.96 

20.26 

7-97 

i 

9-20 

7-13 

40.2 

9.91 

23.84 

8.92 

i 

7.6l 

5-61 

58.5 

12.50 

26-53 

9-35 

i 

6.7I 

4.66 

112.9 

16.66 

3r-79 

10.78 

i 

6.02 

4-02 

H3-9 

16.51 

32.71 

11.30 

i 

6.26 

4.26 

SOLUBILITY  OF  MIXTURES  OF  CADMIUM  TETRA  AMMONIUM  CHLORIDB 
AND  CADMIUM  AMMONIUM  CHLORIDE  IN  WATER. 

(Rimbach  —  Ber.  35»  1300,  '02.) 


4.0 

100  Gms.  Solution  contain  Gms. 

Atomic  Relation. 

Solid  Phase, 
Mol.  per  cent  of: 

•     . 

Cd. 

Cl. 

NH*. 

Cd 

:    Cl       : 

NH*. 

CdCl,. 
NH*C1. 

CdClj. 
4NH4C 

I.I 

5-34 

17.62 

7.27 

I 

10-47 

8.50 

49.6 

50-4 

14.0 

7.12 

19.86 

7.84 

I 

8.84 

6.87 

47-o 

53-o 

40-7 

10.24 

23.82 

8.85 

I 

7-37 

5-37 

77-0 

23-0 

58.5 

12.50 

26.53 

9-35 

I 

6.71 

4.66 

... 

... 

171  CADMIUM  CHLORIDE 

SOLUBILITY  OP  MIXTURES  OF  CADMIUM  TETRA  AMMONIUM  CHLORIDE 
AND  AMMONIUM  CHLORIDE  IN  WATER. 

(Rimbach.) 

100  Cms.  Solution  Atomic  Solid  Phase, 

$0^  contain  Gms.  Relation.  Mol.  per  cent  of: 

Cd. Cl.  NH".  Cd     :    Cl' :      NIL,.      '  Nt^Cl.    CdCl2.4NH«Cl. 

i.o  2.82  17.11  7.82  i  19.21  17.28  59.0  41.0 

13.2  2.76  18.84  8.71  i  21.62  19.62  74-o  26.0 

40.1  3.16  22.56  10.49  l  22.65  20.74  71.0  29.0 

58.2  3.51  25.21  11.72  i  22.79  20.89  69.0  31.0 

CADMIUM    BARIUM    CHLORIDE    2(CdCl2).BaCl2.sH2O. 
SOLUBILITY  IN  WATER. 

(Rimbach  —  Ber.  30,  3083,  '97.) 


t°. 

100  Gms.  Solution 
contain  Gms. 

Gms.  2(CdCl2).BaCl2 
per  100  Gms. 

Cd. 

Cl.                   Ba. 

Solution.              Water. 

22.6 

17.71 

16.89         ii.  o 

45-60              83.82 

41-3 

19.22 

18.15            11.77 

49.14              96.62 

53-9 

I9-85 

18.75            12.41 

51.04            104.25 

62  .2 

20-59 

19.66            12.83 

53.08            II3-I3 

69-5 

21  .20 

20.  18         13-09 

54.47            119.64 

IO7  -2 

24.25 

23.23         14.90 

62.38            165.85 

CADMIUM 

BARIUM    CHLORIDE   CdCl 

2.BaCl2.4H20. 

SOLUBILITY  IN  WATER. 

(Rimbach.) 

100  Gms.  Solution 

Gms.  CdCl2.BaCla 

t». 

contain  Gms. 

per  loo  Gms. 

Cd. 

Cl.                  Ba. 

Solution.             Water. 

22.5 

11.98 

15.19            14.71 

41.88              72.06 

32-9 

12.40 

16.18        16.09 

44.67              80.73 

41.4 

I3-05 

16.95         16.81 

46.81          88.01 

53-4 

13.96 

18.21         18.13 

50.30        101.21 

62.0 

14-73 

18.81         18.74 

52.28        109.56 

97-8 

17-57 

22.48        22.00 

62.05         163.50 

108.3 

18-53 

23.51         22.79 

64.83         184.33 

109.2 

18.67 

23.69        29.95 

65.31         188.27 

CADMIUM   MAGNESIUM  CHLORIDE    2(CdCl2)MgCl2.i2HA 
SOLUBILITY  IN  WATER. 

(Rimbach.) 


100  Gms.  Solution 
t».                                   contain  Gms. 

Gms.  2(CdCl2).MgClj 
per  100  Gms. 

2.4 

20-8 

45-5 

67.2 
121.  8 

Cd. 
22  .14 
24.30 
26.24 

28.45 
31.84 

Cl. 
21  .06 
22.80 

24-55 
26.71 
30.20 

Mg. 
2.41 

2-55 

2  .72 
2-98 

3-44 

Solution. 
45.6l 
49.69 

53-51 
58.14 
65.48 

Water. 
83.86 
98.77 
115.10 
138.90 
189.69 

CADMIUM  CHLORIDE 


172 


CADMIUM   (Mono)RUBIDIUM   CHLORIDE  CdCl2.RbCl. 

SOLUBILITY  OF  CADMIUM  MONORUBIDIUM  CHLORIDE  IN  WATER. 

(Rim  bach,  1902.) 


1.2 

14-5 
41.4 

57-6 
103.9 


ioo  Gms.  Solution  contain  Gms. 


Cms.  CdCl2.RbCl  per  ioo  Gms. 


Cd. 

Cl. 

Rb.  ^ 

Solution. 

Water. 

4.80 

4-53 

3^3 

I2.Q7 

14.90 

6.20 

5.88 

4-75 

16.80 

2O.I9 

9-34 

8.86 

7-14 

25-31 

33.89 

11.40 

10.78 

8.63 

30-83 

44.58 

17.14 

16.37 

J3-39 

46.62 

87.36 

CADMIUM   (Tetra)RUBIDIUM  CHLORIDE   CdCl2.4RbCL 

IN  CONTACT  WITH  WATER. 
(Rimbach.) 

•     The  double  salt  decomposes  to  CdCl2.RbCl  and  RbCl. 


t  °  . 

100  Gms. 

Solution  contain 

Gms. 

Atomic  Relation. 

Solid  Phase, 
Mol.  per  cent  of: 

Cd. 

Cl. 

Rb. 

Cd 

: 

Cl 

:     Rb. 

CdClo. 
RbCl. 

CdCl2. 
4RbCl. 

0.7 

0.65 

6.52 

14 

•73 

I 

31 

.88 

29 

.88 

30 

70 

8.8 

1.07 

7-37 

16 

•!3 

I 

21 

.89 

!9 

.89 

24 

76 

13.8 

1.32 

7.86 

16 

•93 

I 

18 

.88 

16 

•83 

16 

84 

42.4 

3-21 

"•35 

22 

•45 

I 

II 

.21 

9 

.21 

14 

86 

59-o 

4.61 

i3-4i 

25 

•31 

I 

9 

•23 

7 

•23 

33 

67 

108.4 

8.94 

18.57 

31 

•*5 

I 

6 

•57 

4 

•59 

SOLUBILITY  OF  MIXTURES  OF  CdCl2.4RbCl  AND  RbCl  IN  WATER. 

(Rimbach.) 


0-4 
14.8 
17.9 


ioo  Gms.  Solution  contain  Gms. 


Cd. 


Cl. 

12.86 
13.62 
I4-O 


Rb. 

30-97 
32-8I 

33-71 


Atomic  Relation. 


Cd 


Cl  :  Rb. 

I  I 

I  I 

I  I 


Solid  Phase, 
Mol.  per  cent  of: 

CdCl2.4RbCi      RbCl. 

55          45 
67          33 

80  20 


THE  EFFECT  OF  THE  PRESENCE  OF  HC1,  CaCl2  AND  OF  LiCl  UPON  THE  DECOMPO- 
SITION OF  CADMIUM  TETRARUBIDIUM  CHLORIDE  BY  WATER  AT  16°. 

(Rimbach,  1905.) 


ioo  Gms.  Solution  contain  Gms. 


Mols.  per  ioo  Mols.  H2O.      Molecular  Ratio. 


Total  Cl. 

Cl. 

HCl. 

Cd. 

Rb. 

CdCl2. 

RbCl. 

HCl.      CdCl2  :    K 

bCl. 

36.44 

0.84 

36.61 

0.41 

i-39 

O 

.109 

O 

483 

29.76 

4 

•43 

28.45 

0.80 

28.44 

o-35 

1-38 

O 

.082 

0 

422 

20.35 

5 

•JS 

12.09 

3-24 

p.II. 

0.69 

6.74 

O 

•139 

I 

772 

5.60 

12 

•75 

Ca. 

CaCl2. 

CaCl2. 

14.98 

7-56 

20.91 

o-73 

2.80 

O 

.159 

0 

•799 

4-59 

5 

.04 

12.70 

5-77 

15.96 

0.77 

4.87 

O 

.163 

I 

•353 

3-41 

8 

.31 

10.85 

3-78 

14.47 

1.  00 

8.51 

O 

.211 

2 

•365 

2.24 

ii 

.22 

9.08 

1.84 

5-10 

1.24 

12  .14 

O 

.262 

3 

•385 

1.09 

12 

.92 

Li. 

LiCl. 

LiCl. 

26.49 

4.87 

29.40 

0.56 

3-871 

O 

•139 

I 

.271 

19.40 

9 

.13 

20-37 

3-33 

2O  -II 

0.52 

7.84 

0 

.122 

2 

•433 

12.54 

19 

.88 

See  Note  on  next  page. 


173 


CADMIUM  CHLORIDE 


CADMIUM    (Mono)    POTASSIUM    CHLORIDE    CdCl2.KCl.H2O. 
SOLUBILITY  IN  WATER. 

(Rimbach—  Ber.  30,  3079,  '97;  see  also  Croft  —  Phil.  Mag.  [3]  21,  356,  '42.) 


ioo  Gms.  Solution 
$o_                                 contain  Gms. 

2.6 

Cd. 

9-53 
11.63 

Cl. 

9-03 
10.98 

K. 
3-31 

3-99 

41-5 
60.6 

I05.I 

15-47 
17.68 
22.46 

14-73 
16.80 
21.34 

5-45 
6.  20 

7.87 

Cms.  CdCb.KCl 
per  100  Gms. 

Solution. 
21.87 
26.60 

35-66 
40.67 
5J-67 

Water. 
27.99 
36.24 

55-34 

68-55 
106.91 

CADMIUM    (Tetra)    POTASSIUM    CHLORIDE    CdCU^KCL 

IN  CONTACT  WITH  WATER. 

(Rimbach.) 

The  double  salt  is  decomposed  when  dissolved  in  water  at  ordinary 
temperature. 

ioo  Grams  Solution  contain  Gms. 
C 

4 

23 .6 
50.2 
108.9 


t°. 


Cd. 

Cl. 

K. 

3.64 

9.84 

8.31 

5-66 

14.02 

11.52 

9.10 

18.09 

13.60 

11.94 

23.11 

17.16 

NOTE.  —  The  effect  of  the  presence  of  certain  chlorides  upon  the 
decomposition  of  cadmium  tetra  potassium  chloride  by  water  at  16° 
was  investigated  by  Rimbach  in  a  manner  similar  to  that  used  in  the 
case  of  cadmium  tetra  rhubidium  chloride  (see  preceding  page).  The 
results,  which  show  the  extent  to  which  increasing  amounts  of  the 
several  chlorides  force  back  the  decomposition  of  the  double  salt,  were 
plotted  on  cross-section  paper,  and  the  points  at  which  the  decom- 
position was  prevented,  were  determined  by  interpolation.  These 
values  which  show  the  minimum  amount  of  the  added  chlorides  which 
must  be  present  to  insure  the  crystallization  of  the  pure  double  salt  are 
shown  in  the  following  table. 


Added 
Chloride. 

Mols. 

per 

ioo  Moli 

5.  H2< 

L). 

Density  of 
Solutions. 

Mols. 

per 

Liter  of  ! 

Solution. 

CdCl2. 

KC1. 

Added] 
Chloride. 

CdCl2. 

KC1. 

Added" 
Chloride. 

HC1 

0.074 

0 

.296 

19 

.80 

I 

.1403 

0-033 

O 

.132 

8.828 

LiCl 

0-344 

X 

•376 

9 

•30 

I 

.1380 

0.166 

o 

.663 

4-483 

CaCl, 

0-544 

a 

.I76 

3 

.80 

I 

•2333 

0.270 

X 

.080 

1.887 

KC1 

1.034 

6 

•5*4* 

2 

•378 

I 

.214 

0.507 

3 

.195* 

1.167 

*  Total. 


CADMIUM  CHLORIDE 


174 


SOLUBILITY  OF  CADMIUM  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  POTASSIUM 
CHLORIDE  AT  SEVERAL  TEMPERATURES  AND  VICE  VERSA.    (Sudhaus,  1914.) 


Gms.  per  100  gms.  H2O. 

Solid  Phase. 

Gms.  per  100  gms.  HzO. 

Solid  Phase. 

'CdCh. 

KCL' 

CdCh. 

KCL  ' 

Results  at 

i9-3°. 

Results  at 

40.1°. 

in-  3 

o.o 

CdCl2.2|H2O 

133.85 

O.O 

CdCl2.H2O 

59-59 

6.7 

"  -j-  DM-I 

92.15 

2.70 

"  +  DI.M 

*26.98 

11.09 

DI.I.I 

51.90 

11.50 

DI.I.I 

n.  61 

30.04 

"    +  DL4 

*37-9i 

15.21 

" 

1.44 

34.76 

DL4+KC1 

24-45 

21.73 

tt 

o.o 

33-94 

KC1 

18.97 

35-51 

" 

Results  at 

29.7°. 

19.92 

37-63 

"  +D,.4 

129.65 

o.o 

CdCl2.2jH20 

2.98 

40.45 

Di.4+KCl 

97.62 

0.70 

a 

o.o 

40.36 

KC1 

68.23 

7.08 

"~\~  DI.I.I 

Results  at 

54-5. 

47.12 

9.89 

DI.I.I 

133.9 

0.0 

CdCl2.H2O 

*32.67 

13.06 

(t 

102.15 

2.32 

"  +DM.I 

24.26 

16.10 

" 

*44.oi 

18.39 

DI.I.I 

15-99 

25-97 

" 

26.13 

43.78 

"    +Di.4 

15-47 

33.58 

"      +  DL4 

4.20 

45-52 

Di.4+KCl 

2.42 

37-66 

DL4+KC1 

o.o 

43.00 

KC1 

o.o          37.21 
DI.I.I  =  CdCl2.KCl.H2O, 

KC1 
Di.4  =  CdCl2.4KCl. 

)ws;  the  solubility  of  the  double  salt  in  water. 

SOLUBILITY  OF  THE  DOUBLE  SALT.    CdCl2.4KCl  IN  WATER. 


(Sudhaus,  1914.) 


19-3 
23-6 

29.7 
40.1 
50.2 
54-5 


Gms.  CdCl2.4KCl  per 
100  gms.  HzO. 

41.65 

45-35 
49-05 
57-55 
68.89 
69.91 


Mol.  Ratio  in  Solution. 


iCdC!2 


6.37KC1 

5-85  " 
5-34  " 
4.60  " 

4.30  " 
4.12  " 


SOLUBILITY  OF  CADMIUM  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  SODIUM  CHLORIDE 
AT  SEVERAL  TEMPERATURES  AND  VICE  VERSA.     (Sudhaus,  1914.) 


Gms.  per  100  gms.  HjO. 

Solid  Phase. 

CdCl2.2|H2O 

"  +DL,., 

Di.2.3 

u 

"  +NaCl 
NaCl 

CdCU.           NaCl. 
Results  at  19.3°. 
111.30      o.o 
116.64      7-52 
85.15    12.19 

*40.oi     25.67 
5.96     36.76 
o.o      35.84 

Gms.  per  too  gms. 


Solid  Phase. 


Results  at  29.7°. 


CdCl2.         NaCl. 
Results  at  29.7°  (con.). 
*43-74     27.46       Di.2.3 

9.43     37-54         "     +NaCl 
Results  at  40.1°. 

137.03     15.14  CdCl2.H2Of-D1.2.3 
*48.i7     29.50      Di.2.3 

13.31     38.16  +NaCl 

Results  at  54.5°. 


9.63  CdCl2.2jH20+Di.2.3i4o.42     19.10  CdCl2.H2O+Di.2.3 


Di.2.3 


*52-76 

22.53 
o.o 


32.97 

39-07 
36.82 


132.67 

123.54       10.10 

106.16    12.92 
91.10    15.41        " 
Di.w  =  CdCl2.2NaCl.3H20. 

*  Shows  the  solubility  of  the  double  salt  in  water. 

CADMIUM  CINNAMATES  (C6H5CH:CH.COO)2Cd. 
100  gms.  water  dissolve  0.070  gm.  cadmium  cinnamate  at  26°. 
loo  0.56       '    cadmium  isocinnamate  at  20°. 

100     "         "  "       o.io      "    cadmium  allocinnamate  at  20° 


Di.2-3 

"    +NaCl 
NaCl 


(de  Jong,  1909.) 
(Michael,  1903.) 


175 


CADMIUM  CYANIDE 


CADMIUM   CYANIDE   Cd(CN)2. 

100  gms.  H2O  dissolve  1.7  gms.  Cd(CN)2  at  15°. 


Qoannis,  1882.) 


CADMIUM  FLUORIDE  CdF2. 

loo  cc.  of  sat.  solution  in  water  contain  4.33  gms.  CaF2  at  25°. 

100  cc.  of  sat.  solution  in  1.08  n.  HF  contain  5.62  gms.  CaF2  at  25°.  Qaeger,  1901.) 
jFreezing-point  lowering  data  (solubility,  see  footnote,  p.  i)  are  given  for  mix- 
tures of  cadmium  fluoride  and  cadmium  iodide  by  Ruff  and  Plato  (1903),  and 
for  mixtures  of  cadmium  fluoride  and  sodium  fluoride  by  Puschin  and  Baskov, 
(1913). 

CADMIUM  HYDROXIDE  Cd(OH)2. 

SOLUBILITY  IN  WATER. 

I  liter  of  aqueous  solution  contains  0.0026  gm.  Cd(OH)2  at  25°. 

(Bodlander,  1898.) 

SOLUBILITY  IN  AQUEOUS  AMMONIUM  HYDROXIDE  SOLUTIONS. 
Results  at  25°.  Results  at  16-21°. 

(Bonsdorff,  1904.)  (Euler,  1903.) 


Normality  of 
NHs. 


i.o 
1.8 
4.6 


Gms.  Cd(OH)z 
per  liter. 

0.274 
0.707 
I.5l6 
5.609 


16-17 


21 

u 


Normality  of 
NHs. 

Gms.  Cd(OH)2 
per  liter. 

0.47 
0.87 
0.26 

0.44 
I.I7 

0-51 

0.32 

CADMIUM  IODIDE  CdI2. 


SOLUBILITY  IN  WATER. 

(Dietz,  1900;  see  also  Kremers,  1858;  Eder,  1876;  Etard,  1894.) 


Gms.  CdI2  per  too  Gms.      M°k-  CdI2 

^0           Gms.  Cdl2  per  100  Gms. 

Mols.  Cdli 

Solution.           Water.       Mols.  HjO. 

Solution.            Water. 

per  100 
Mols.  H2O. 

o      44.4          79.8        3.9 

30         47.3                  89.7 

4-43 

10      45.4          83.2        4.1 

40         48.4                 93.8 

4.6 

15         45.8              84.5           4.17 

5°      49-35          97-4 

4.8 

18      46.02        85.2        4.2 

75      52.65        in.  2 

5-4 

20      46.3          86.2        4.26 

100      56.08         127.6 

6-3 

*2S         46.8              87.9            4.34 

Density  of  saturated  solution  at  18 

0  =  1.590. 

SOLUBILITY  OF  CADMIUM 

IODIDE  IN  ORGANIC  SOLVENTS. 

"Solvent                              t°          G^- 

Cdlj  per  loo  Gms. 

Solution.       Solvent/ 

Absolute  Alcohol         15        50 

.5       I  O2                   (Eder.) 

Ethyl  Alcohol               20        42 

.6         74  .  27           (Timofeiew,  1891.) 

Methyl  Alcohol            20        59 

.O      143.7             (Timofeiew,  1891.) 

Propyl  Alcohol             20        28 

.9         40  .  67           (Timofeiew,  1891.) 

Absolute  Acetone        18        20 

25  *                (Naumann,  1904.) 

Benzonitrile                  18 

I  .  63           (Naumann,  1914.) 

Ethyl  Acetate              18 

I  .  84  |       (Naumann,  1910.) 

Ethyl  Ether                 12° 

0.143        (Tyrer,  1911.) 

Anhy.  Hydrazine     15-20 

84  J               (Welsh  and  Broderson,  1915.) 

Benzene                     16.0 

0  .  047        (Linebarger,  1895.) 

35.0 

0.094 

?(fca=.994.                           \d 

is  =.9145-                        tperioocc. 

CADMIUM  IODIDE  176 

SOLUBILITY  OF  CADMIUM  IODIDE  IN  METHYL  ALCOHOL,  ETHYL  ALCOHOL,  PROPYL 
ALCOHOL  AND  IN  ISOPROPYL  ALCOHOL  AT  DIFFERENT  TEMPERATURES. 

(Muchin,  1913,  see  also  Timofeiew,  1894.) 

Grams  Cdl2  per  100  Grams  Sat.  Solution  in: 


.•  • 

CHaOH. 

CtHsOH. 

CsHvOH. 

C3H7OH(iso). 

0 

67 

33-5 

16 

36.9 

5 

.  .  . 

4i 

22 

36-9 

10 

68 

54  (at  1  2  .6°  =  tr.  temp.) 

28.5 

37-2 

20 

69 

53 

41  .  5    (tr.  temp.) 

37-3 

25 

69-5 

52.2 

37-8 

37-3 

30 

70 

51  .5 

35-5 

37-3 

40 

7i 

50.8 

34-5 

37-3 

So 

72-5 

50 

34-o 

37-3 

SOLUBILITY  OF  CADMIUM  IODIDE  IN  ETHYL  ETHER.    (Linebarger,  1895.) 

f  o  Mols  Cdlz  per  Gms.  CdI2 

100  Mols.  CdIi+(C2Hs)2O.    100  gms. 

o  0.03  0.148 

15.5  0.04  0.198 

20-3  0.05  0.247 

SOLUBILITY  OF  CADMIUM  IODIDE  IN  METHYL  FORMATE,  ETHYL  FORMATE,  PROPYL 
FORMATE  AND  INJETHYL  ACETATE  AT  DIFFERENT  TEMPERATURES.  (Muchin,  1913.) 

Gms.  CdI2  per  100  Gms.  Sat.  Solution  in: 


l>  . 

HCOOCHs. 

HCOOCzHs. 

HCOOC3H7. 

CH3COOC2H5. 

0 

0.84 

1.16 

2-37 

4-73(?) 

13.0 

o-75 

1.05 

2.07 

1.67 

26.0 

0.66 

0.77 

i-53 

2.02 

CeHsNHz. 

CsHsN. 

C9H7N. 

1-7 

2-3 

O.I 

3-i 

o-S 

2 

4 

i-7 

3-5 

5-i 

4.8 

5 

6.4 

13-4 

6.7 

8.4 

30 

8-3 

SOLUBILITY  OF  CADMIUM  IODIDE  IN  ANILINE,  PYRIDINE  AND  IN  QUINOLINE  AT 
DIFFERENT  TEMPERATURES.     (Muchin,  1913.) 

Gms.  CdI2  per  100  Gms.  Sat.  Solution  in: 
t". 

40 

50 
60 
70 
80 
90 
100 

SOLUBILITY  OF  CADMIUM  IODIDE  IN  MIXTURES  OF  SOLVENTS  AT  DIFFERENT 
TEMPERATURES.     (Muchin,  1913.) 

Composition  of  Solvent          *£*££%?  Gms.  CdI2  per  100  Gms.  Sat.  Solution  at: 

to  Mols.  Solvent.  'V.  16.8°.  36.8°. 

iCH3OH+2CHCl3  ii. 8  ii  .o  10.4  9.3 

iCHsOH+iCHCla  21.1  22.4  22.3  20.6 

iC2H5OH+2CHCl3  16.2  7.5  7.1  6.6 

iCjjHsOH+iCHCls  27.8  13.9  14.3  13.6 

43.5  25.2  24.1 

60.3  34.4 

91-5  45-4 

i<^H50H+2C6H6          22.8  17.6        16.3(16.3°)     15.2(31.2°) 

iC2H50H+iC6H6          37.1  26.1        26.0(15.7°)     26.0    " 

aC^OH+iQft          54.1  33.5        35-3(i50) 
9.8  6.5 


177  CADMIUM  IODIDE 

SOLUBILITY  OF  CADMIUM  IODIDE  IN  MIXTURES  OF  SOLVENTS. 

(Muchin,  1913.) 

Results  for  a  mixed  solvent  composed  of: 

One  Mol.  Pyridine+One  Mol.  Chloroform.  One  Mol.  Pyridine-hOne  Mol.  Benzene. 

Cms.  CdLz  per  Gmsi  Cdh  per         .   ••      Cms.  Cdlj  per  Cms.  CHfcper 

t°.  100  Gms.  t°.  100  Cms.  t°.  100  Gms.  t°.  100  Gms. 

Sat.  Sol.  Sat.  Sol.  Sat.  Sol.  Sat.  Sol. 

50.1          1.27  63  6.3  57.9  1.77  72.5  32.6 

54     1-72    64      8.3    60      2.2    74.0    35.9 

56       2.3      64.5     12.35    65        4.2     76       36.3 

58     3.0    64     14.8    70      8.1    80     40.8 

60      4.0      62       22.0     71       II.5     85       41.6 
62       5.6      6I.I5    24.67    71.5     15.0     90.4     42.67 

SOLUBILITY  OF  CADMIUM  IODIDE  IN  ETHYL  ETHER  CONTAINING  WATER  AT  12°. 

(Tyrer,  19  n.) 

Gms.  H2O  per 
100  gms.  ether -{-H^O— >  o.o       o.io    0.30    0.50    0.70    0.90  i.oo     i.io  1.14 sat. 

Gms.  Cdl2  per 
100  gms.  solvent— >      0.1430.78     2.07     3.36     4.77    6.46  7.30    8.278.68 

DISTRIBUTION  OF  CADMIUM  IODIDE  AT  30°  BETWEEN: 

(Dahr  and  Batter,  1913.) 

Water  and  Amyl  Alcohol.  Water  and  Ethyl  Ether. 

Gms.  per  100  cc.  c  Gms.  per  100  cc.  c 


HaO  Layer  (c).  Alcohol  Layer  (c1).           c/                        HzO  Layer  (c).     Ether  Layer  (c7).  c/ 

47-75     43       I- ii       37 -18      8.38  4.43 

29.08     25.86    1.13       30.03      6.61  4.54 

14.46     12.55    1.15        15.38      3.09  4.97 

10.69         ^.94      1.20           12. 60         2.38  5.29 

6-23      4-94     i-33        9-89      1-83  5.40 

2.42      i-54    1-55        7-68      i. 06  5.52 

i-93      i.io    1.76        4-03      0.73  5.60 

1.76      0.94    1.87        3.10      0.51  6.03 

Freezing-point  data  (solubility,  see  footnote,  p.  i)  are  given  for  the  following 
mixtures: 

Cadmium  Iodide  +  Cuprous  Iodide       (Herrmann,  1911.) 
+  Mercuric  Iodide      (Sandonnini,  1914.) 
-j-  Potassium  Iodide    (Brand,  1912.) 
"       +  Sodium  Iodide 


CADMIUM  AMMONIUM  IODIDES  (Mono  and  Di). 

SOLUBILITY  OF  EACH  SEPARATELY  IN  WATER,  ETC. 

(Rimbach,  1905;  Eder,  1876.) 
Cd.  Mono  Ammonium  Iodide.  Cd.  Diammonium  Iodide. 

Gms.  Cdfc.NHJ  per  Gms.  CdI2.2NHJ  per 

Solvent.  t°.  IPO  Gms.  t«_  too  Gms. 

Solution.         Solvent.  Solution.       Solvent* 

Water  15        52.6      in  14.5        85.97    611.6 

Abs.  Alcohol       15        53          113  15  59          143 

Abs.  Ether          15        29.4        41.7  15  10  n 


CADMIUM  IODIDES  178 

CADMIUM    POTASSIUM    IODIDES,    Mono  =  CdI2.KI.H2O, 

Di  =  CdI2.2KI.2H2O. 

CADMIUM  DiSODIUM  IODIDE  CdI2.2NaI.6H2O. 

^SOLUBILITY  OF  EACH  SEPARATELY  IN  WATER,  ETC.,  AT  15°. 

(Eder.) 

Gms.  Gdljj.KI 
Solvent. 

Water 

Abs.  Alcohol 
Abs.  Ether 

CADMIUM    NITRATE    Cd(NO3)2. 

SOLUBILITY  IN  WATER. 

(Funk  —  Wiss.  Abh.  p.  t.  Reichanstalt  3   440,  'oo.) 


Gms.  CdI2.KI 
per  100  Gms. 

Gms.  CdI2.2KI 
per  100  Gms. 

Gms.  CdI2.2NaI 
per  100  Gms. 

Solution.       Solvent. 

Solution. 

Solvent. 

Solution. 

Solvent. 

51.5        106 

57-8 
41.7 

137 
71 

53-7 

158.8 

116.2 

... 

3-9 

4-1 

9.0 

9-9 

Gms.  Cd(N03)2 
%  o.                    per  i  oo^  Gms. 

Mols.  Cd(N03)2                          Solid 

Solution. 

Water.' 

per  100  Mols.  H2O.                     Phase. 

—  13 

37-37 

59  -67 

4-55 

Cd(N03)2.9H20 

~     I 

47-33 

89.86 

6.85 

Tt 

+     I 

52-73 

in.  5 

8.50 

11 

0 

52-37 

109.7 

8-37 

Cd(N03)2.4H20 

+  18 

55-9 

126.8 

9.61 

" 

30 

58-4 

140.4 

10.7 

u 

40 

61.42 

159.2 

12.  1 

" 

59-5 

76-54 

326.3 

25.0 

tt 

Density  of  saturated  solution  at  18°  =  1.776. 

The  eutectic  of  the  system  Cd(NO3)2.4H2O  +  Cd(NO3)2  is  at*44.8°and  has  the 
composition  Cd(NO3)2.2.65H2O.  (Vasilev,  1910.) 

CADMIUM  OXALATE  CdC2O4.3H2O. 

i  liter  of  sat.  aqueous  solution  contains  0.033  gm.  CdC2O4  at  18°.  (Kohlrausch,  1908.) 

CADMIUM  SILICATE  CdSiO3. 

Fusion-point  data  are  given  for  CdSi03  +  ZnSiOj.  (van  Klooster,  1910-11.) 

CADMIUM    SULPHATE    CdSO4. 

SOLUBILITY  IN  WATER. 

(Mylius  and  Funk  —  W.  Abh.  p.  t.  Reichanstalt  3,  444,  'oo;  see  also  Kohnstamm  and  Cohn  —  Wied 
Ann.  65,  344,  '98;  Steinwehr  —  Ann.  der  Phys.  (Drude)  [4]  9,  1050,  '02;  Etard  —  Ann.  chim.  phys 
[?J  2  536,  '94-) 

Gms.  CdSO4  Gms.  CdSO4 

t°.  per  IPO  Gms.  Ph  *  °-  per  100  Gms.  Solid 

Solution.     Water.  Solution.     Water. 

-17  44.5  80.2  CdSO4>7H2O         40  43.99  78.54    CdSO4.fH2O. 

—  10  46.1  85.5  60  44.99  83.68             " 

-  5  48.5  94-2  "                   73.5  46.6  87.28 

-18  43.35  76.52  CdS04.|H20         74.5  46.7  87.62    CdS04.H2O 

-10  43.27  76.28  77  42.2  73.02 

o  43.01  76.48  85  39.6  65.57 

•J-io  43.18  76.00  90  38.7  63.13 

20  43-37  76-6o  100  37.8  60.77 

For  results  at  high  pressures,  see  Cohen  (1909). 


179 


CADMIUM  SULFATE 


SOLUBILITY  OF  CADMIUM  SULPHATE  IN  AQUEOUS  SOLUTIONS  OP  SUL- 
PHURIC ACID  AT  o°. 

(Engel  — Compt.  rend.  104,  507,  '87.) 


Equivalents  per  10  Gms.  H2O. 


H2S04. 
O. 

3-87 
12.6 

28.1 

43-3 
47.6 

53-8 


CdS04. 
71.6 
70.9 
62  .4 
50.6 
40.8 

37-o 

32-7 
23.0 


Density 
of  Solutions. 

.609 

•591 
•545 
.476 

•435 
.421 

1.407 
1-379 


Grams  per  log  Grams  H2O. 


H2S04. 

CdSO4. 

O-OO 

74.61 

1.90 

73-87 

6.18 

65-03 

13-78 

52-73 

21.23 

42.52 

23-34 

38.56 

26.38 

34-07 

35-06 

23.96 

ioo  gms.  95%  formic  acid  dissolve  0.06  gm.  CdSO4  at  18.5°.          '  (Aschan,  1913.) 
Freezing-point  data  (solubility,  see  footnote,  p.  i)  are  given  for  mixtures  of 

CdSO4  +  Li2SO4,  CdS04  +  K2SO4  and  CdSO4  +  Na2SO4  by  Calcagni  and  Marotta 

(1913)- 


SOLUBILITY  OF  MIXED  CRYSTALS  OF  CADMIUM  SULPHATE  AND  FERROUS 
SULPHATE  IN  WATER  AT  25°. 

(Stortenbecker  —  Z.  physik.  Chem.  34,  109,  'oo.) 


VxUIIlp 

usuion  01  ooiu 

Gms.  per 

ioo  Gms.  H2O. 

Mols.  per  ioo  Mols.  H2O. 

Mol.  %  Cd. 
in  Sol. 

Crystals  of 
Solid  Phase. 

CdSO4. 

FeSO4. 

Cd. 

Fe. 

Crystals  with  a\ 

}  Mols.  H2O. 

76.02 

O-O 

6-57 

0-0 

IOO 

IOO 

57-6i 

10.63 

4.98 

1.26 

79-8 

99-o 

Crystals  with  7 

Mols.  H2O. 

57'6l 

10.63 

4.98 

1.26 

79.8 

36-6 

78.5 

34-6 

44.6 

n.  i 

.  .  . 

.  .  . 

24.4 

4-8 

0.0 

26.69 

o.o 

3-I65 

o.o 

o.o 

CADMIUM  POTASSIUM  SULFATE  CdK2(SO4)2 
SOLUBILITY  IN  WATER. 

(Wyrouboff,  1901.) 


t»    G.  CdK2(SO4)2  per 
ioo  Gms.  HzO. 

16        42.89 

31  46.82 

40  47-40 


Solid  Phase. 

CdK2(SO4)2.2H20 


f  o     G.  CdK2(SO4)2  per 
ioo  Gms.  H2O. 

26 

31 

40 

64 


Solid  Phase. 

42.50    CdK2(SO4)2.ijH20 

42.80 

43-45        ;; 

44.90 


CADMIUM   SODIUM  SULFATE     180 
CADMIUM  SODIUM  SULFATE  CdNa2(SO4)2.2H2O. 

SOLUBILITY  IN  WATER,  ALSO  WITH  THE  ADDITION  OF  CADMIUM  SUL- 
PHATE  AND  OF  SODIUM  SULPHATE. 

(Koppel,  Gumpery  —  Z.  physik.  Chem.  52,  413,  '05.) 


Gms.  per  100  Gms. 
t».              Solution. 

Gms.  per  100  Gms.  Mols.  per  100  Mols. 
H2p-                              H?O.                             Solid  Phase. 

24 

30 
40 
0 
10 

CdS04. 
22.25 

22-55 

22  .89 
40.32 
39-91 

Na2SO4. 

I5-29 
I5-65 
4-85 
5-24 

CdSO4. 

35-49 

36.28 
37-24 

73-54 
72.77 

Na2S04. 
24.04 
24.60 

25-45 
8.85 

9-55 

CdSO4.    * 
3-07      , 

3-!4    , 

3-22      , 
6.36 
6.30 

5-05] 
5.12  [•  CdNa2(SO4)2.2H2O 
5.28] 

•I2} 
.21     CdNa2(S04)2.2H20 

2O 

40 

.26 

73 

.81 

9-45 

6 

•39 

.20  I     +CdSO4-.|H2O 

40 

39 

.89 

7^8 

75 

•38 

13 

•56 

6 

•52 

.72 

1 

•  14. 

840 

.18 

4.60 

72 

.68 

8 

•32 

6 

.29 

•05 

0 
IO 
20 

37 
32 

22 

•30 
•53 
.69 

6-53 
8.69 
14.71 

66 

55 
36 

•32 
•34 
•25 

ii 
14 
23 

.62 

.78 
•52 

5 
4 
3 

•74 

•79 

.14     ; 

•47 
.84 
;.98 

CdNa2(SO4)2.2H2O 
+  Na2SO4.ioH2O 

25 

16 

•33 

19.82 

25 

.60 

31 

.06 

2 

.21     3.94^ 

30 

35 
40 

9 
8 

9 

.21 
.26 
.98 

27.80 

29-35 
28.27 

14 

13 
16 

.62 
.26 
.24 

44 

47 
46 

.14 
.06 

I 
I 

I 

.26     4.59" 
.41     5.86. 

CdNa2(SO4)2.2H2O 

+  Na2S04 

CADMIUM  SULFIDE  CdS. 

1000  cc:  H2O  dissolves  9  X  lo"6  gms.  CdS  at  18°. 


(Weigel,  1906.) 


CAESIUM    ALUMS 

SOLUBILITY  OF  CAESIUM  CHROMIUM  ALUM,  CAESIUM  IRON  ALUM, 
CAESIUM  INDIUM  ALUM,  AND  OF  CAESIUM  VANADIUM  ALUM  IN 
WATER. 

(Locke  —  Am.  Ch.  J.  27,  174,  '01.) 


Formula  of  Alum. 

Cs2Cr2(S04)4.24H20 
tt 

tt 
ii 

Cs2Fe2(S04)4.24H20 


Cs2In2(S04)4.24H20 
Cs2V2(S04)2.24H20 

See  also  Alums,  p.  32. 


25 
30 
35 
40 

25 
30 

35 
40 

25 
25 


Gms.  per  100  cc.  H2O. 


Anhydrous 
Salt. 


0.96 
I  .206 


I.7I 

2.52 

3-75 
6.04 

7-57 
0.771 


Hydrated 
Salt. 


1.52 
1.91 

2-43 
2.72 
4.01 
6.01 
9.80 


Gram  Mols.  Salt  per 
100  cc.  H2O. 


0.0025 

0.0032 

O.OO4O5 

0.0045 

O.OO66 

0.0099 

0-0156 

O.OI72 

O-O0204 


I8i  CAESIUM  CHLORAURATE 

CAESIUM  CHLORAURATE  CsAuCl*. 

SOLUBILITY  IN  WATER. 

(Rosenbladt,  1886.) 


Cms.  CsAuCU 

Gms.  CsAuCU 

Gms.  CsAuO< 

t°. 

per  100  Gms. 

t°. 

per  100  Gms. 

t°. 

per  100  Gms. 

Solution. 

Solution. 

Solution. 

IO 

o-5 

40 

3-2 

80 

I6.3 

20 

0.8 

50 

5-4 

90 

21.7 

30 

i-7 

60 

8.2 

IOO 

27-5 

70 

12.  0 

CAESIUM  FLUOBORIDE  CsBFl4. 

loo  grams  water  dissolve  0.92  gram  CsBFl4  at  20°,  and  0.04  gram  at  100°. 

(Godeffroy,  1876.) 

CAESIUM  BROMIDE  CsBr. 

SOLUBILITY  OF  CAESIUM  AND  LEAD  BROMIDES  AND  THEIR  DOUBLE  SALTS 
IN  WATER  AT  25°. 

(Foote,  1907.) 

Gms.  per  100  Gms.  Sat.  Sol.  Gms.  per  100  Gms.  Sat.  Sol. 

1 CsBr^      PbBr2.  7~Cs&-  PbBrT^ 

0.24      0.33    PbBr2+CsPb2Br5      33.65      trace    CsPbBr3 

0.33      0.36        "  "  36-7  "  +Cs4PbBr8 

1 2. 8s      trace    CsPb2Br5  46.4  "       Cs4PbBr6 

a          u  ti          it 

17*68         "          "  +CsPbBr3        54.4  "'         "  +CsBr 

18.58  CsPbBr3  55.23          o  CsBr 

CAESIUM  Mercuric  BROMIDE  CsBr.2HgBr2. 

100  grams  saturated  aqueous  solution  contain  0.807  gram  CsBr.2HgBr2  at  16°. 

(Wells,  1892.) 

CAESIUM  CARBONATE  Cs2CO3. 

100  grams  absolute  alcohol  dissolve  n.i  grams  Cs-jCOs  at  19°,  and  20.1  grams 
at  b.  pt.  (Bunsen.) 

CAESIUM  BiCARBONATE  CsHCO3. 

100  grams  sat.  solution  in  H2O  contain  67.8  grams  CsHCO3  at  about  20°. 

(de  Forcraud,  1909.) 

CAESIUM  CHLORATE  CsClO3  CAESIUM  PerCHLORATE  CsClO4. 
SOLUBILITY  OF  EACH  IN  WATER. 

(Calzolari,  1912;  see  also  Carlson,  1910.) 

Results  for  CsClOj.  Results  for  CsClO4. 

Gms.  CsClOa     Gms.  CsClOs       Gms.  CsClOi  Gms.  CsClO4 

t°.   per  loo  Gms.  t°.  per  100  Gms.    t°.  per  100  Gms.        t°.  per  100  Gms. 
HzO.          H20.  HzO.  ^  HjO. 

o   2.46  50   19.4     o   0.8       50   5.4 
10   3.8   60   26.2    10    i.o       60    7.3 

20     6.2    70    34.7      20     1.6          7O     9.8 

25     7.6    80    45.0      25     2.o(d=I.Ol)8o    14.4(^=1.084) 

30   9.5   90   58.0    30    2.6       90   20.5 
40   13.8  loo   79.0    40   4.0      zoo   30.0 


CAESIUM  CHLORIDE  182 

CAESIUM    CHLORIDE    CsCl. 

SOLUBILITY  IN  WATER. 

(Berkeley  — Trans.  Roy.  Soc.  (Lond.)  203  A,  208,  '04;  see  also  Hinrichsen  and  Sachsel  — Z.  physik. 
Chem.  50,  99,  '04- '05;  at  25°,  Foote.) 


t  °. 

G.  CsCl  per  100  Gms. 

G.Mol.CsCl 

0          G.  CsCl  per  ioo  Gms. 

G.  Mol  rsri 

Solution. 

,     Water. 

per  Liter. 

v     * 

Solution 

.     Water. 

per 

Liter. 

0 

6l.7 

161 

•4 

6 

•74 

60 

69.7 

229 

•7 

8 

.28 

10 

63.6 

174 

•7 

7 

.11 

70 

70.6 

239 

•5 

8 

.46 

20 

6S.I 

186 

•5 

7 

•38 

80 

71.4 

250 

.0 

8 

.64 

30 

66.4 

197 

•3 

7 

•63 

90 

72.2 

260 

.1 

8.80 

40 

67-5 

208 

.0 

7 

.86 

IOO 

73-o 

270 

.5 

8 

.96 

So 

68.6 

218 

•5 

8 

.07 

119.4 

74-4 

290 

.0 

9 

y 
.22 

SOLUBILITY  OF  MIXTURES  OF  CAESIUM  CHLORIDE  AND'  MERCURIC  CHLORIDE 
IN  WATER  AT  25°.    (Foote,  1903.) 


Gms.  per  ioo  Gms. 
Solution. 

Solid  Phase. 

Gms.  per  ioo  Gms 
Solution. 

Solid  Phase. 

CsCl.             HgCl2. 
65.61         o.o 

65.78       0.215 
62.36       0.32 

CsCl 

CsCl  +  Cs3HgCl6 
)     Double  Salt 

CsCl. 
17.03 

HgCl2. 
o.H  \ 

0.42  , 

Double  Salt 
CsHgCl3=  38.3%  CsCl 

57.01       0.64 
52-35        -23 

>     CssHgClB 
j           =  65.1%  CsCl 

0.61 
0.49 

2.64 
2.91  1 

CsHg       +  CsHg,Cl5 
Double  Salt 

51-08 

•44 

Cs3HgCl5  +  Cs,HgCl4 

0.40 

3-78  ! 

CsHg2Cl6  =  23.7%  CsCl 

49-30 

45-95 

•49 
.69 

)     Double  Salt 
\    CsjHgCU  =  55.4%CsCl 

0.44 
0.41 

t'el  j 

CsHgzCl6  +  CsHg5Clu 
Double  Salt 

45-23 

•73 

CsjHgCU  +  CsHgCl, 

0.25 

5-65  i 

CsHg5Clu=  n.i%C6Cl 

0.18 

7.09 

CsH&Clu  +  HgCl, 

o.o 

6.90 

HgCl2 

SOLUBILITY  OF  MIXTURES  OF  CAESIUM  CHLORIDE  AND  MERCURIC  CHLORIDE  IN 
ACETONE  AT  25°.    (Foote,  1911.) 

Gms.  per  ioo  Gms.  Solution. 

. pfpi -7T-F1 '          Solid  Phase- 

CsCl.         HgCh. 

0.48    28.48  CsC1.2HgCl2 

0.48  39.65    " 

0.47    44.40      "  +CsCl.5HgCl2 
0.32    49.83  CsC1.5HgCl2 


Gms.  per  ioo  Gms.  Solution 
CsCl.      '  HgClz. 
O 

O.O2 
O.l6 


0.032 
O.II 

0.19 

0.25 
0.45 

0.46 

0.56 


Solid  Phase. 

CsCl 
Mixed  salts 


0.17 
13.08  CsCl.HgCl2 

21  .50 


0.20       57.74 

0-13     57-76      "  +HgCl2 
57.74HgCl2 


27.2  "  +  CsCl.2HgCl2  o.o 

CAESIUM  Iridium  CHLORIDES  Cs2IrCl6,  etc. 

loogms.  HzO  dissolve  o.oi  I  gm.  caesium  chloroiridate,  Cs2lrCleat  19°.  (Delepine,  1908.) 
ioo     '  0.05  gm.  caesium  hexachloroiridite,  Cs3IrCl6.3H2O  at  19°. 

ioo     "  0.83    "    caesiumaquopentachloroiridite,|Cs2H2OIrCl6ati90. 

CAESIUM  Platinic  CHLORIDE  CsPtCle. 

IOO  gms.  H2O  dissolve  0.135  Sm-  CsPtCle  at  2O°.       (Rosenheimand  Weinheber,  1910-11.) 

CAESIUM  Tellurium  CHLORIDE  CsTeCl6. 

SOLUBILITY  IN  AQUEOUS  HYDROCHLORIC  ACID.    (Wheeler,  1893.) 

ioo  parts  HC1  (Sp.  Gr.  1.2)  dissolve  0.05  part  CsTeCU  at  22°. 
ioo  parts  HC1  (Sp.  Gr.  1.05)  dissolve  0.78  part  CsTeCle  at  22°. 

CAESIUM  Thallium  CHLORIDE  3CsCl.TlCl3.2H2O. 

ioo  parts  H2O  dissolve  2.76  parts  3CsCl.TlCl3.2H2O  at  17°,  and  33.3  parts  at 
I  OO°.  (Godeffroy,  1886.) 


183 


CAESIUM  CHLORIDE 


Freezing-point  lowering  data  (solubilities,  see  footnote,  p.  i)  are  given  for  the 
following  mixtures  of  caesium  chloride  and  other  salts. 

Mixture.  Authority. 

Caesium  Chloride  +  Cuprous  Chloride    (Sandonnini  and  Scarpa,  1912;  Sandonnini,  1914.) 
-j-  Silver  Chloride 

+  Thallium  Chloride  "  " 

+  Lithium  Chloride        (Korreng,  1915;  Richards  and  Meldrum,  1917.) 

+  NaCl    (Richards  and  Meldrum,  1917.) 
-|-v  Potassium  Chloride    (Zemcznzny  and  Rambach,  1910.) 
+  Rubidium  "  " 

+  Sodium 

CAESIUM  CHROMATES,   Cs2CrO4,  Cs2Cr2O7,  etc. 


SOLUBILITY  IN  WATER  AT  30°. 

(Schreinemakers  and  Meijeringh,  1908.) 


Gms.  per  100  Gms. 
Sat.  Sol. 


Solid  Phase. 


Gms.  per  100  Gms.  Sat. 
Sol. 


Solid  Phase. 


CsaO. 
70.63 
69.22 
36.06 
31.00 
31.68 
35-80 

3I-05 
24.05 

3-°4 
1.61 
1.18 

0.586 


CrOs. 
0.0 
O.II9 
1.883 

7-523 
9.652 
13.08 
10.79 
8.98 
2.16 

4-57 

7-95 

15-05 


'       CS20. 

CrOs. 

0.169 

21  .21 

t    0.096 

25-59 

1.89 

36.19 

2.79 

41.68 

3.29 

44-23 

±3.13 

±44-45 

2.96 

44.66 

3-40 

46.03 

3-94 

56.77 

>10  4.35 

62.70 

2.33 

62.50 

0 

62.28 

"   +082014013 


"  +Cr03 
CrO3 


CAESIUM  FLUORIDE  CsF.i|H2O. 

100  gms.  H2O  dissolve  366.5  gins.  CsF  at  18°,  solid  phase  CsF.i£H2O. 

(de  Forcrand,  191  x.) 

CAESIUM  HYDROXIDE  CsOH. 

100  gms.  sat.  solution  in  H2O  contain  79.41  gms.  CsOH  at  15°  (de  Forcrand, 
i9Oo,a);  for  30°,  see  above. 

CAESIUM  IODATE  CsIO4. 

loo  parts  H2O  dissolve  2.6  parts  CsIO3  at  24°,  and  2.5  parts  2CsIO3.I2O6  at 
21°.  (Wheeler,  1892;  Barker,  1908.) 


CAESIUM   Per  IODATE  CsIO4. 

loogms.  H2O  dissolve  2.  15  gms.  CsIO4at  15°, 

CAESIUM  IODIDES  Csl,  CsI3,  etc. 


sat.  solution  =  1  .0166.  (Barker,  1908.) 


SOLUBILITY  IN  WATER  AT  25°. 

(Foote  and  Chalker,  1908.) 
Gms.  per  100  Gms.  Sat.  Solution.  Empirical  Comp. 


Csl. 
7.72 
7.69 

i. 
1.19 

2.40 

1.23 

2-35 

1.23 

2-39 

1-25 

of  Residue 
CsI3.29 
CsI3.98 

Csi5:75 

CsI7.43 
CsIiQ.3 


Present  in  Residue. 

CsI3  and 

it  « 

CsI5  and  I 

u  u 


CAESIUM  IODIDE 


184 


CAESIUM    IODIDE    Csl. 
SOLUBILITY  OF  MIXTURES  OF  CAESIUM  IODIDE  AND  IODINE  IN  WATER. 

(Foote  —  Am.  Ch.  J.  29,  210,  '03.) 


Gms.  per  ioo  Gms. 
t  °.                     Solution.                             40 

Gms.  per  ioo  Gms. 
Solution. 

Solid  Phase  at 

Csl. 

i. 

Csl. 

i. 

both  Temps. 

-4 

27.68 

o.o 

35-6 

51.48 

o.o 

Csl 

-4 

27.52 

0.09 

35-6 

51.66 

0.71 

Csl  and  CsI3 

-4 

3.18 

0.31 

35-6 

10.72 

1.78 

CsI3  and  CsI5 

—  0.2 

0.85 

o.34 

35-6 

3-74 

i.  60 

CsI5  and  I 

Gms.  per  ioo  Gms. 
t  <\                    Solution. 

Csl. 

i. 

52.2 

16.75 

4-52 

52.2 

6.69 

3-36 

52.2 

6.72 

3-32 

52.2 

6.65 

3-45 

73 

26.98 

15-07 

73 

16.66 

10.50 

73 

6.27 

4-08 

In  Separated  Heavy  Solution 
Gms.  per  ioo  Gms.  Solution. 


Csl. 

I. 

.rnase. 

CsI3  and  CsI5 

CsI5  and  I 

22.94 

73-72 

CsI5 

22.8o 

I 

CsI3  and  CsI6 

27.56 

68.40 

CsI5 

17.68 

80.02 

I 

CAESIUM    (Tri)  IODIDE    CsI3. 

100  cc.  saturated  aqueous  caesium  iodide  (about  17  per  cent  Csl) 
solution  contain  0.97  gram  CsI3  at  20°,  density  of  solution  =1.154. 

(Wells  — Am.  J.  Sci.  [3]  44,  221,  'pa.) 

CAESIUM    NITRATE     CsNO3. 

SOLUBILITY  IN  WATER. 

(Berkeley  —  Trans.  Roy.  Soc.  (Lond  )  203   A,  213,  '04.) 


Gms.  CsNO3  per 
t  °.                ioo  Gms. 

G.  Mols. 
CsNO3               t  °. 

Gms.  CsNO3  per 
ioo  Gms. 

G.  Mols  CsN03 

Solution. 

Water. 

per 

Liter. 

Solution. 

Water'. 

per  Liter. 

0* 

8-54 

9 

•33 

o. 

476 

60 

45-6 

83 

.8 

3 

.41 

10 

12-97 

14 

•9 

o. 

725 

70 

51  .7 

107 

.0 

4 

.10 

2O 

I8.7 

23 

.0 

I. 

II 

80 

57-3 

134 

.0 

4 

.81 

30 

25-3 

33 

•9 

I  . 

58 

90 

62  .0 

I63 

.0 

5 

-50 

40 

32.1 

47 

.2 

2. 

12 

IOO 

66.3 

197 

.0 

6 

.19 

50 

39-2 

64 

•4 

2. 

73 

106 

.2  68.8 

2  2O 

•3 

6 

•58 

THE  ICE  CURVES  FOR  MIXTURES  OF  CAESIUM  NITRATE  AND  WATER, 
DETERMINED  BY  THE  SYNTHETIC  METHOD. 

(Jones,  1908.) 


Solubility  curve. 

t°  of  Crystalli-  Gms.  CsNOs  per 

zation.  ioo  Gms.  HjO. 

-0.3  0.21 

—  0.4  1.28 

—  1.2  6.01 

— i.l  8.0 


Solid 
Phase. 

Ice 

M 

u 


Supersolubility  curve. 

t8  of  Crystalli-  Gms.  CsNOs  per       Solid 
e'zation.          ioo  Gms.  HjsO.        Phase. 

Ice 


—  1.2 
-2-5 

-3-2 

-3.2 


O.2I 
1.28 

3-99 
6.01 
8 


-i.4(Eutec.) 

The  eutectic  is  given  as  —1.254°  and  8.51  gms.  CsNOs  per  ioo  gms.  H2O,  by 
Washburn  and  Maclnnes  (1911). 


185 


CAESIUM  "OXALATE 


CAESIUM  OXALATE  Cs2C2O4.H2O. 

SOLUBILITY  OF  MIXTURES  OF  CAESIUM  OXALATE  AND  OXALIC  ACID  IN  WATER 

AT  25°. 

(Foote  and  Andrew,  1905.) 

Varying  amounts  of  the  two  substances  were,  dissolved  in  hot  water  and  the 
solutions  allowed  to  cool  in  a  thermostat  held  at  25°. 


Gms.  per  100 
Gms.  Solution. 

G.  Mols.  per  100 
G.  Mols.  H20. 

Solid 

Phao» 

HjC^.    CsjjCjA.          H2C2O4.      Cs2C2O4. 

i  na.se. 

10 

.20 

2.274 

H2C2O4.2H2O 

10 

.29 

o 

.61        2.314 

0 

•035 

H2C204.2H20+H3Cs(C2O4)2.2H20 

7 

.90 

9 

.92        1.924 

o 

.614  ^ 

Double  Salt. 

4 

.11 

25 

.12             I.l62 

I 

.81 

J 

H3Cs(C2O4)2.2H2O 

4 

•32 

27 

•55 

•279 

2 

.06 

H3Cs(C204)22H20+H4Cs2(C204)3 

4 

.27 

28 

.30        ] 

.267 

2 

.14 

I 

Double  Salt. 

4 

•  40 

35 

.90        3 

.476 

3 

.07 

\ 

H4Cs2(C204)3 

4 

.82 

40 

.10 

•752 

3 

.71 

H4Cs2(C204)3+HCsC204 

4 

3 
i 

•45 
•05 
.04 

42 
48 
68 

.32      ] 
.80 

.69         c 

.672 
.268 

5.688 

4 

5 
ii 

•05 
.16 

•56 

\ 

Double  Salt. 
HCsC204 

0 

.91 

71 

.24        0.648 

13 

.06 

HCsC2O4+  HgCsg^OJ- 

o 

•77 

73 

•45        < 

3.598 

14 

•51 

I 

Double  Salt. 

0 

•75 

74 

.04        0.596 

14 

.96 

\ 

H6Cs8(C204)7 

o 

•74 

75 

.20        0.625 

15 

•93 

H6Cs8(C204)7+  Cs2C204.H20 

o 

.0 

75 

.82        o.o        15 

•97 

Cs2C204.H20 

CAESIUM  Telluracid  OXALATE  Cs2[H6TeO6.C2O4]. 

100  gms.  H2O  dissolve  6.42  gms.  Cs2[H6TeO6.C2O4]  at  o°,  12.39  S1118-  at  20°, 
15.08  gms.  at  30°,  19.78  gms.  at  40°  and  27.66  gms.  at  50°. 

(Rosenheim  and  Weinheber,  1910-11.) 

CAESIUM  PERMANGANATE  CsMnO4. 

100  cc.  sat.  aqueous  solution  contain  0.097  gm.  CsMnO4  at  i°,  0.23 
gm.  at  19°,  and  1.25  gms.  at  59°.  (Patterson  —  J.  Am.  Chem.  Soc.  28,  1735,  '06.) 

CAESIUM   SELENATE  Cs2SeO4. 
100  grams  H2O  dissolve  245  grams  Cs2SeO4  at  12°. 

(Tutton  —  J.  Chem.  Soc.  7ii  850,  *97<) 

CAESIUM    SULPHATE   Cs2SO4. 

SOLUBILITY  IN  WATER. 

(Berkeley  —  Trans.  Roy.  Soc.  (Lond.)  203  A,  210,  '04.) 


Gms.  Cs2SO4  per 
tc.                 ioo  Gms. 

G.  Mols. 
Cs2S04                    t°. 

Gms.  Cs2SO4  per 
ioo  Gms. 

G.Mols. 
Cs2S04 

Solution. 

Water. 

per 

Liter. 

Solution. 

Water. 

per  Liter. 

O 

62 

.6 

I67 

.1 

3 

•  42 

60 

66.7 

199 

•9 

3-78 

10 

63 

•4 

173 

.1 

3 

.49 

70 

67.2 

205 

•  O 

20 

64 

.1 

I78 

•7 

3 

•56 

80 

67.8 

210 

•3 

3-88 

30 

64 

.8 

184 

.i 

3 

.62 

90 

68.3 

214 

•9 

3-92 

40 

65 

•5 

I89 

9 

3 

.68 

IOO 

68.8 

220 

•3 

3-97 

50 

66 

.1 

194 

9 

3 

•73 

108.6 

69.2 

224 

•5 

4-00 

CAESIUM  DOUBLE  SULFATES     186 

SOLUBILITY  OF  CAESIUM  DOUBLE  SULPHATES  IN  WATER  AT  25°. 

(Locke  — Am.  Ch.  J.  27,  459,  'ox.) 

Cms.  Anhydrous  Salt    Gm.  Mols. 

Name.  Formula.  per  100  Cms.          Salt  per  100 

Solution.      Water.       Gms.H2O. 

Caesium  Cadmium  Sulphate  -  Cs2Cd(so4)2.6H2o  58.16  139.9  0.2455 

Caesium  Cobalt  Sulphate          Cs2Co(so4)2.6H2o  29.52  41.9  0.081 

Caesium  Copper  Sulphate         c^Cu(so4)2.6H2o  31-49  46.0  0.0882 

Caesium  Iron  Sulphate             Cs2Fe(so4)2.6H2o  50.29  101.1  0.1967 

Caesium  Magnesium  Sulphate  Cs2Mg(so4)2.6H2o  34-77  53-3  o . i 106 

Caesium  Manganese  Sulphate  Cs2Mn(SO4)2.6H2o  44 .58  80. 4  0.157 

Caesium  Nickel  Sulphate          Cs2Ni(so4)2.6H2o  20.37  25-6  0.0495 

Caesium  Zinc  Sulphate              Cs2Zn(so4)2.6H2o  27.87  38.6  0.0738 

SOLUBILITY  OF  CAESIUM  SODIUM  SULFATES  IN  WATER  AT  25°. 

(Foote,  1911.) 

Cms,  per  100  Cms.  Sat.  Solution.  Per  cent  CsSC>4         Empirical  C9mposition  of 

Cs2SO4.  NazSO4.  in  Residue.  **,    *  Residue. 

54.65  11.44  89.98        iNa2SO4.3.53Cs2SO4 

54.58  11.63  78.22        iNa2S04.i.4iCs2SO4 

54.81  11.25  34.67        4.8Na2SO4.iCs2SO4 

The  author's  solubility  method  for  determination  of  the  formation  and  com- 
position of  double  salts  is  described  in  the  paper  containing  the  above  results. 

CAESIUM  DihydroxyTARTRATE  Cs2C4H4O8.2H2O. 

100  gms.  H2O  dissolve  22.5  gms.  Cs2C4H4O8.2H2O  at  o°.  (Fenton,  1898.) 

CAFFEINE    C6H(CH3)3N4O2.H2O. 

SOLUBILITY  IN  WATER. 

(Average  curve  from  results  of  Zalai,  1910;  Pellini,  1910,  and  U.S.P.,  8th  Ed.) 
t»  Gms.  C6H(CH3)3N4O»  t»  Gms.  C6H(CH3)3N4O» 

per  100  Gms.  HiO.  per  100  Gms.  HjO. 

o  0.6  40          .     4.64 

15  i.o  50  6.75 

20  1.46  60  9.7 

2$  2.13  70  13.5 

30  2.8  80  19-23 

SOLUBILITY  OF  CAFFEINE  IN  ORGANIC  SOLVENTS. 

Solvent  t°        Gms-   C5H(CH3)3N402  Solve_t  t»       Gms.  CsH(CHs)iN4O, 

bolvent.  t  .       pe,.  I00  Gms-  Solvent.  bolvent.  t  .      per  IQQ  Gmg  Solvent. 

Ethyl  Alcohol       25  1.32(2)  Carbon  Tetra-    (    18      0.09(4) 

"          "  25  1.88(1)  chloride  ]    20      0.26(6) 

60  5.85(1)  'b.pt.    0.70(4)      . 

Methyl    '  25  1.14(2)  Chloroform  17     12.9   (5) 

Amyl       "  25  o.5o(3)(<*»=o.8io)  25     12.3    (i) 

Amyl  Acetate       30.5  0.72(3)0*30=0.862)  25     11.92(2) 

Acetic  Acid  (99.5%)  2 1. 5  2.6    (3)  b.pt.  15.63  (4) 

Acetone  30.5  2 . 3  2  (3)  (dm =0.83  2)  Ether  1 8      o .  1 2  (4) 

Aniline  30.5  29.4(3)0*30=1.080)  25      0.27(1) 

Benzaldehyde       30.5  13.1(3)0*30=1.087)      "  b.pt.    0.30(4) 

Benzene  18.0  0.91(4)  Trichlorethylene     15      0.76(7) 

25.0  1.16(2)  Dichlorethylene       15       1.82(7) 

30. 5  i .  23  (3)0*30=0.875)  Pyriclme    "          20-25  34.39  (8) 

b.pt.  5.29(4)  50%  Aq.  Pyridine   "      11.12(8) 

Carbon  Bisulfide  17  0.06(5)  Toluene  25      0.58(3)^=0.861) 

Xylene  32.5  1.13(3)0*32=0.847) 

(i)  =  U.  S.  P.;  (2)  =  Schaefer,  1913;  (3)  =  Seidell,  1907;  (4)  =  Gockel,  1898;  (5)  =  Commaille,  1875; 
(6)  =  Gori,  1913;  (7)  =  Wester  and  Bruins  (1914);  (8)  =  Dehn,  1917. 

Data  for  the  solubility  of  caffeine  in  mixtures  of  alcohol  and  chloroform  and 
alcohol  and  benzene  are  given  by  Schaefer  (1913). 


187 


CAFFEINE 


SOLUBILITY  OF  CAFFEINE  IN  AQUEOUS  SOLUTIONS  OF  SODIUM  BENZOATE  AND 

VICE  VERSA.    (Peilmi,  1910.) 
Results  at  25°. 

Gms.  per  too  Gms.  HzO. 


C8H10N402. 

CrHiOiNa. 

2.13 

O 

8.32 

6.67 

38.10 

45 

5*-74 

76.75 

46.27 

76.68 

24.79 

69.56 

9-47 

62.97 

o 

61.17 

Solid  Phase. 


Results  at  40°. 

Gms.  per  too  Gms.  H2O. 


+C7Hfi02Na.H20 


4°-  64 

o 

3J-43 

25-3I 

56.82 

69.68 

57-99 

74.64 

55.98 

74.02 

18.31 

67.97 

0 

59.82 

Solid  Phase. 


SOLUBILITY  OF  CAFFEINE  IN  AQUEOUS  SOLUTIONS  OF  SODIUM  SALICYLATE  AND 

VICE  VERSA.      (P^llini  and  Amadori,  1912.) 
Results  at  25°  .  Results  at  40°. 

Gms.  per  100  Gms.  H2O. 


C8H10N402. 
2.13 
38.36 

CrtUOsNa. 
0 
30.76 

55-23 
74-32 
16.78 

47-31 
68.81 
124.96 

13.22 

121  .27 

9-03 

120.54 

0 

115-43 

Solid  Phase. 
CsH10N402.H20 


Gms.  per  100  Gms.  H2O. 


:8H10N402. 

CvHsOsNa. 

4.64 

O 

59-49 

37-47 

86.49 

62.47 

95-94 

69.15 

26.93 

131-52 

iQ-75 

124-35 

0 

119.66 

Solid  Phase.  • 


Data  for  the  depression  of  the  freezing-point  of  sodium  salicylate  solutions  by 
caffeine  and  theobromine  are  also  given. 

DISTRIBUTION  OF  CAFFEINE  BETWEEN  WATER  AND  CHLOROFORM.  (Marden,  1914.) 

Grams  Caffeine  in: 


105  cc.  EbO  Layer. 

o . 0090 

O.OlSo 
0.0291 


50  cc.  CHCla  Layer. 
0.0563 

o . 1048 

0.1770 


Ratio  of  Caffeine  in 
Equal  Vols.  H2O  and  CHC1«. 

0.0456 

o . 0492 

O.0470 


Gms.  Ca(CH3COO)2 
.        per  100  Gms. 


CALCIUM  ACETATE   Ca(CH3COO)2.2H3O. 

SOLUBILITY   IN    WATER.     (Lumsden,  1902;  Krasnicki,  1887.) 

Gms.  CaCCHaCOCOa 

jo^       per  IPO  Gms.  Solid  Phase. 

Water. 

37.4  Ca(CH3COO)2.2H2O 
Ca(CH3COO)2.2H2O 
Ca(CH3COO)2.2H2O 
Ca(CH3COO)2.2H2O 
Ca(CH3COO)2.2H2O 
Ca(CH3COO)2.2H2O 


Solid  Phase. 


30 

40 


32-9 

31-1 


Solution. 

o    27.2 
10    26.5     36.0 

20      25.8 
25       25.5 

25-3 

24-9 

SOLUBILITY  OF  CALCIUM  ACETATE  IN  AN  AQUEOUS  SATURATED  SOLUTION  OF 

SUGAR  AT  31.25°.    (Kohier,  1897.) 

100  gms.  solution  contain  8.29  gms.  Ca(CH3COO)2  +  60.12  gms.  sugar. 
100  gms.  water  dissolve  26.3  gms.  Ca(CH3COO)2  +  190.3  gms.  sugar. 

loo  cc.  anhydrous  hydrazine  dissolve  i  gm.  calcium  acetate  at  room  temp. 

(Welsh  and  Broderson,  1915.) 


34-7 
34-2 
33-8 
33-2 


60 
80 
84 

85 
90 

IOO 


Solution. 
24.6 
25-1 
25-3 
24-7 

23-7 
22-9 


Water. 

32.7  Ca(CH3COO)2.2H20 
33.5     Ca(CH3COO)2.2H20 

33.8  Ca(CH3COO)2.2H20 
Ca(CH3COO)3.H2O 
Ca(CH3COO)2.H2O 


29  . 7     Ca(CH3COO)2.H,O 


CALCIUM  ACETATES 


188 


CALCIUM    (Tri)    Methyl    ACETATE    Ca[(CH3)3CCOO]2. 
CALCIUM    (Di)    Ethyl    ACETATE   Ca[(C2H6)2CHCOO]2. 
CALCIUM   Methyl   Ethyl   ACETATE   Ca[CH3(C2H6).CHCOO]2. 
SOLUBILITY  OF  EACH  IN  WATER. 

(Landau  —  Monatsh.  Chem.  14,  717,  '93;  Keppish  —  Ibid,  g,  600,  '88;  Sedlitzki  —  Hid.  8,  573,  '87.) 

Ca.  Tri  Methyl  Acetate.     Ca.  Di  Ethyl  Acetate.      Ca.  Methyl  Ethyl. 

Acetate. 


Gms.  Ca(CsH9O2)2 
t  o.             per  100  Gms. 

Water.    Solution". 

0 

7  .30 

6.81 

10 

6.84 

6.40 

20 

6-54 

6.14 

30 

6.40 

6.01 

40 

6.44 

6.05 

50 

6.64 

6.22 

60 

6.86 

6.42 

70 

7.11 

6.64 

80 

7-38 

6.87 

Gms.  ' 

Ca(CeHiiO2)2 

Gms.  Ca(C5H902)2 

per 

100  Gms. 

per   ipo   Gms. 

'Water 

.     Solution. 

Water.       Solution. 

30-3 

23.22 

28.78       22-35 

27.8 

2i-75 

31.71       24.07 

25.6 

20.38 

33  -76    25.23 

23-7 

19.16 

34.92     25.89 

22  .1 

18.10 

35.20    26.04 

20.8 

17.22 

34.60    25.71 

19.9 

16.60 

33.11     24.89 

19.2 

i6.n 

30.74    23.41 

27.49    21.56 

CALCIUM    Methyl   Propyl    ACETATE     Ca[CH3(C3H7).CHCOO]L. 
CALCIUM    (Di)    Propyl    ACETATE    Ca[(C3H7)2CHCOO]2. 
CALCIUM    (Iso)    Butyl    ACETATE    Ca[(CHE)2CH(CH2)2COO]2. 

SOLUBILITY  OF  EACH  IN  WATER. 

(Stiassny  —  Monatsh.  Chem.  12,  596,  '91;  Furth  —  Ibid.  9,  313,  '88;  Konig  —  Ibid.  15,  22,  '94.) 

Ca.  Methyl  Propyl  Acetate.     Ca.  Di  Propyl  Acetate.     Ca.  Iso  Butyl 

Acetate. 


Gms.  Ca(C6HnO2)2 
t  o.                per  100  Gms. 

Water. 

Solution. 

O 

16.58 

14.22 

10 

15.80 

I3-65 

2O 

15.14 

13.15 

30 

I4.6l 

"•75 

40 

14.21 

12.45 

50 

13-94 

12.24 

60 

13-79 

12.13 

70 

I3-78 

12.12 

80 

13.89 

12.  2O 

90 

Gms.  Ca(C8H15O2)2 
per  100  Gms. 

Gms.  Ca(C6H11O2)2 
per  TOO  Gms. 

Water. 

Solution. 

Water. 

Solution. 

9 

•57 

8 

•73 

7 

.48 

6 

.96 

8 

•35 

7 

•7i 

6 

•38 

5 

•99 

7 

.19 

6 

•7i 

5 

.66 

5 

•36 

6 

.11 

5 

•77 

5 

•3i 

5 

.04 

5 

.09 

4 

.84 

5 

•3i 

5 

.04 

4 

.14 

3 

98 

•5 

.68 

5 

•37 

3 

•25 

3 

15 

6 

.41 

6 

.02 

2 

•44 

2 

38 

7 

•51 

6 

.98 

I 

•65 

I. 

62 

8 

•97 

8 

•23 

. 

10 

•79 

9 

•74 

CALCIUM  BENZOATE  Ca(C6H5COO)2. 

loocc.  sat.  solution  in  water  contain  3.02  gms.  Ca[C6H6COO]2at  26°.  (de  Jong,  1912.) 
100  gms.  sat.  solution  in  water  contain  8.6  gms.  Ca[C6H5COO]2  at  15°  and  10.2 

gms.  at  I  OO°.  (Tarugi  and  Checchi,  1901.) 

CALCIUM  BORATES  CaB2O4.4H2O,   CaB2O4.6H2O. 

SOLUBILITY  OF  EACH  SEPARATELY  IN  WATER. 

(Mandelbaum,  1909.) 


3O 

50 
70 
90 


0.0365 
0.036 
0.048 
0.0315 


0.310 
0.307 
0.392 
0.310 


(amorphous) 


B203. 
30      0.0205 
50      0.032 
70      0.068 
90      0.0675 

0.254 

0-353 
0-457 
0-359 

CaB204.6H2O 
"  (cryst.) 

I89 


CALCIUM  BORATE 


SOLUBILITY  OF  CALCIUM  BORAXES  IN  AQUEOUS  SOLUTIONS  OF  BORIC,  Aero 

AT  30°. 

(Sborgi,  1913-) 


Gms.  per  100  Gms.  Sat 

.Sol. 

Solid 

Gms.  per  10 

o  Gms.  Sal 

:.  Sol. 

Solid 

'BzOs. 

CaO. 

Phase. 

BijOa.                      CaO. 

Phase. 

0 

.014 

O. 

126 

Ca(OH)j 

0. 

869 

0. 

067 

2.3.9 

0 

.032 

0. 

140 

" 

I. 

116 

0. 

076 

• 

0 

.098 

0. 

194 

" 

I. 

339 

0.093 

"  +1.3.12 

O 

.127 

O. 

217 

"  +1.1.6 

2. 

058 

0. 

093 

1.3.12 

0 

•134 

0. 

220 

1.  1.  6 

2. 

509 

o. 

099 

" 

0 

.138 

O. 

118 

H 

2. 

730 

0. 

III 

" 

O 

.162 

O. 

106 

" 

3- 

732 

0. 

325 

(C 

O 

.166 

0. 

107 

"    +2.3-9 

2. 

798 

0. 

109 

M 

0 

.171 

O. 

109 

"           " 

3- 

313 

0. 

143 

" 

O 

.290 

0. 

052 

2-3-9 

3- 

841 

o. 

152 

It 

0 

.610 

0. 

054 

" 

4- 

250 

0. 

155 

"  +HiBO, 

0 

.767 

o. 

059 

" 

4- 

179 

o. 

137 

HaBOj 

1.  1.6  = 

CaO, 

,B2O3.6H2O, 

2.3-9 

=  2Ca0.3B2O8.9H2O, 

I-3- 

12  =  CaO.3B203.i2H2O. 

Many  determinations,  in  addition  to 

the  above,  are 

given  in  the  original  paper. 

CALCIUM  BROMIDE 


CaBr2.6H2O. 
SOLUBILITY  IN  WATER. 


(Kremers,  1858; '  Etard,ri894,  gives  results  which  yield  an  irregular  curve  and  are  evidently  less 

than  those  of  Kremers.) 


Solid  Phase. 

CaBn.6HjO +CaBr».4HjO 
CaBr,.4H,0 


*  Eutec.  t  tr.  pt. 

Density  of  saturated  solution  at  20°  =  1.82. 

Data  for  the  system  calcium  bromide,  calcium  oxide  and  water  at  25°  are  given 
by  Milikau  (1916). 

Freezing-point  data  are  given  for  mixtures  of  calcium  bromide  and  calcium 
chloride,  calcium  bromide  and  calcium  fluoride  by  Ruff  and  Plato,  1903. 


t°.  - 

-22* 
0 
10 
20 
25 

Gms.  CaBrz  per 
100  Gms. 

Solid  Phase. 

CaBtt.SHzO+Ice 
CaBr2.6H2O 

<( 

it 

t°. 

34- 
40 
60 
80 
105 

Gms.  CaBra  per 
100  Gms. 

Water.    Solution. 

ioi     50.5 
125     55-5 
132     57 
143    58.8 
153    60.5 

Water.  Solution. 
2f     185      65.1 

213    68.1 
278     73-5 
295     74-7 
312     75.7 

CALCIUM   PerBROMIDE   CaBr4. 

Data  for  the  formation  of  calcium  perbromide  in  aqueous  solutions  at  25° 
are  given  by  Herz  and  Bulla  (1911).  The  experiments  were  made  by  adding 
bromine  to  aqueous  solutions  of  CaBr2  and  agitating  with  carbon  tetrachloride. 
From  the  bromine  content  of  the  CC14  layer,  the  amount  of  free  bromine  in  the 
aqueous  layer  can  be  calculated  on  the  basis  of  the  distribution  ratio  of  bromine 
between  water  and  CC14.  This  furnishes  the  necessary  data  for  calculating  the 
amount  of  ^calcium  perbromide  existing  in  the  aqueous  layer. 


CALCIUM  BUTYRATB  190 

CALCIUM    (Normal)    BUTYBATE    Ca[CH3(CH2)2COO]2.H2O. 

CALCIUM    (Iso)    BUTYRATE   Ca[(CH3)2CH.COO]2.5H2O. 
SOLUBILITY  OF  EACH  IN  WATER. 

(Lumsden  —  J.  Chem.  Soc.  81,  355,  '02;  see  also  Chancel  and  Parmentier  —  Compt.  rend.  104,  474, 
'87;  Deszathy  —  Monatsh.  Chem.  14,  251,  '93,  and  also  Hecht  —  Liebig's  Annalen  213,  72,  '82,  give 
results  for  the  normal  salt  which  are  somewhat  below  those  of  Lumsden  for  the  lower  temperatures. 
SedJitzki  —  Monatsh.  Chem.  8,  566,  '87,  gives  slightly  different  results  for  the  iso  salt.) 

Calcium  Normal  Butyrate.  Calcium  Iso  Butyrate. 


Gms.  Ca(C4H7O2)2  Cms.  Ca 

t  o^  per  iqo  Gms.  t  °.  per  100  Gms. 

Water.    Solution.  Water.     Solution. 

o        20.31     16.89  o        20.10     16.78  Ca(C4H7O2)2.5H2O 

10        19-15     16.08  20        22.40    18.30- 

20     18.20   15.39          30     23.80   19.23 

25  I7-72  I5-°5  4°  25.28  20.65 

30  I7-25  14-71  60  28.40  22.12 

40  16.40  14.09  62  28.70  22.30 

60  15.15  13.16  65  28.25  22.03  Ca(C4H703)2.H2O 

80  14-95  I3-°I  80  27.00  21.26 

100  I5-^5  I3-^9  Io°  26.10  20.69 

CALCIUM  d  CAMPHORATE  Ci0H14O4Ca.7H2O. 

SOLUBILITY  OF  CALCIUM  CAMPHORATE  IN  AQUEOUS  SOLUTIONS  OF  CAMPHORIC 
ACID  AT  15°  AND  VICE  VERSA. 

(Jungfleisch  and  Landrieu,  1914.) 
Gms.  per  100  Gms.  Sat.  Sol.  Gms.  per  100  Gms.  Sat.  Sol. 

Sohd  Phase'  '  '  Sohd  Phase. 


C^^Ca. 

1.35  1.23        C8HH(COOH)8  2.90  7.75        C8H14(COOH)2 

1-57  1.97  "  3  8.66          "  +C10Hi4O4.Ca.7H2O 

I.7I  2.55  "  3.07  8.57 

2.18  4.34  «  1.50  7.94 

2-33  4-73  "  o  7.37 


gms.  CioHuC^Ca  per  100  gms.  sat.  solution. 

CALCIUM  CAPROATE   (Hexoate)   Ca[CH3(CH2)4COO]2.H2O. 

CALCIUM  3  Methyl  PENTANATE  Ca[CH,.CH2.CH(CH,)CH2.COO]2.3H2O. 

CALCIUM  CAPRYLATE  Ca[CH3(CH2)6COO]2.H2O. 
SOLUBILITY  OF  EACH  IN  WATER. 

(Lumsden;  the  Pentanate,  Kulish,  1893;   see  also  Keppish,  1888,  and  Altschul,  1896, 
for  results  on  the  Caproate.) 

Ca.  Caproate.  Ca.  3  Methyl  Pentanate.     Ca.  Caprylate. 


Gms.  CaCCeHnO^j  per 

Gms.Ca(C6HnO2)2l 

>er  100  Gms 

•  Gms.  Ca(C8Hi5O2)2  ] 

' 

loo  Gms.  H20. 

"    Water. 

Solution. 

loo  Gms.  HzO. 

0 

2.23 

12-33 

10.98 

o-33 

20 

2.18 

I7.I8 

14.66 

0.31 

40 

2.15 

18.99 

15-97 

0.28 

50 

2.IO 

18.73 

I5-78 

0.26 

60 

2-15 

17.71 

15.04 

0.24 

80 

2.30 

13-37 

II.80 

0.32 

100 

2-57 

9-94 

9.04 

0.50 

CALCIUM  CARBONATE 


CALCIUM  CARBONATE  CaCO3. 


EQUILIBRIUM  IN  THE  SYSTEM  CaO-H2O-CO2  AT  16°. 

The  following  data  for  the  solubility  of  calcite  (CaCO3)  in  water  at  16°  in  con- 
tact with  air  containing  the  partial  pressure  P  of  CO2  were  calculated  from  the 
results  of  Schloesing  (1872),  Engel  (1888),  and  others  by  Johnston  (1915)  and 
Johnston  and  Williamson  (1916).  These  authors  describe  the  changes  in  the 
system  resulting  from  a  gradual  increase  in  partial  pressure  of  COa,  as  follows: 

"We  begin  by  considering  the  equilibrium  between  the  hydroxide  M(OH)2  and  the  aqueous 
solution  saturated  with  it  as  affected  by  a  progressive  increase  from  zero  of  the  partial  pressure 
P  of  CO2  in  the  atmosphere  in  contact  with  the  solution.  Addition  of  CCk  is  followed  by  a  dis- 
tribution between  the  vapor  and  liquid  phases  until  there  is  equilibrium  between  the  residual 
partial  pressure  of  CQj  and  the  HzCOs  in  solution,  and  in  ^urn  between  the  latter  and  the 
several  ions;  the  net  effect  of  this  is  a  definite  decrease  in  [OH  ],  the  concentration  of  hydroxide 
ion,  which  necessitates  that  more  of  the  hydroxide  dissolve  in  order  to  keep  the  solubility- 
product  [M++][OH  ]2  constant.  Consequently  the  total  concentration  of  M++  increases, 
part  of  it  being  now  associated  with  carbonate  and  bicarbonate;  in  other  words,  the  apparent 
solubility  of  the  base  increases  if  the  method  of  analysis  of  the  solution  is  a  determination  of 
M,  whereas  it  would  decrease  if  one  should  determine  [OH  ]2.  This  process  continues  until 
the  product  [M++][CO3=]  reaches  the  value  requisite  for  the  precipitation  of  MCOs  (on  the 
assumption  that  supersaturation  does  not  occur)  which,  for  a  given  base,  takes  place  at  a 
definite  value  of  P  which  depends  only  upon  the  temperature;  this  transition  pressure  Pi  is, 
at  a  given  temperature,  the  highest  under  which  solid  hydroxide  is  stable  and  the  lowest  at 
which  solid  carbonate  is  stable. 

At  Pi  the  solubility  (as  measured  by  the  total  [M])  begins  to  diminish,  because  increase  of 
P  increases  [CO3=]  while  the  product  [M-H-][CO3=]  must  remain  constant  so  long  as  MCO3  is 
the  stable  solid  phase;  this  increase  of  [CO3=]  continues  until  a  definite  pressure  Po  is  reached, 
when  the  formation  of  bicarbonate  in  the  solution  becomes  the  predominant  reaction  and 
[CO3=]  begins  to  decrease  again.  JP0  is  thus  a  minimum  in  the  solubility  curve.  With 
further  increase  beyond  Po  the  concentration  of  both  M-H-  and  HCOs  increases  steadily 
until  the  precipitation  value  of  the  product  [M-H-][HCOs~]2  is  reached  at  Pz,  which  is  a  transi- 
tion pressure  at  which  both  carbonate  and  bicarbonate  are  present  as  stable  solid  phases. 
Beyond  P2  bicarbonate  alone  is  stable,  and  its  total  solubility  falls  off  very  slowly  with 
further  increase  of  partial  pressure  of  CCh." 


THE  CALCULATED  ION-CONCENTRATIONS  AND  SOLUBILITY  OF  CALCITE  IN 
WATER  AT  16°  IN  CONTACT  WITH  AIR  CONTAINING  THE  PARTIAL  PRESSURE 
P  OF  CO2. 


Partial  Pressure  P 
of  CO2  Measured 
in  Atmospheres. 

Ion-concentrations  per  Liter  X  10-*. 

Total  Ca, 
Mols.  per 
*         Liter 
Xio-*. 

Grams 
CaCOa  per 
Liter. 

Ca-H-. 

OH-. 

C0s=. 

HCOr. 

3 

.16X10-" 

138 

•5 

277 

O.OO7I 

o 

.0000235 

2 

2 

.80  Xio-10 

6 

.81 

13 

-3 

0.144 

0 

.01 

. 

.  . 

0.074 

9 

.78Xio-9 

2 

•377 

3 

.82 

0.414 

0 

.10 

0.026 

6 

.i4Xio~8 

I 

•654 

i 

.82 

0-593 

o 

•30 

. 

O.OlS 

2 

.19X10-7 

I 

.476 

i 

.02 

0.665 

0 

.60 

. 

0.016 

3 

.73X10-7 

I 

•459 

o 

.787 

0.672 

o 

.787 

. 

0.0159 

3 

.85X10-7 

I 

•459 

o 

•774 

0.672 

o 

.80 

. 

.  . 

0.0159 

6 

.07X10-7 

I 

•473 

0 

.614 

0.666 

i 

. 

.  . 

0.016 

7 

.62  Xio"6 

2 

•051 

0 

.147 

0.478 

3 

. 

0.022 

7 

.63X  io~5 

3 

•777 

0 

•034 

0.260 

7 

. 

0.040 

2 

.I5X  lo"4 

5 

.197 

0 

•0174 

0.188 

10 

. 

.  . 

0.056 

2 

Xio"4 

5 

.09 

o 

.0182 

0.19 

9 

.96 

5 

•52 

0.055 

2 

•5  Xio-4 

5 

.46 

o 

•oi57 

0.18 

10 

•54 

5 

•93 

0.059 

3 

Xio-4 

5 

•79 

0 

.0140 

0.17 

ii 

.22 

6 

.31 

0.063 

3 

•5  Xio-4 

6 

.08 

0 

.0126 

0.16 

ii 

.82 

6 

•64 

0.066 

4 

XlO"4 

6 

•35 

o 

.0115 

0.16 

12 

.36 

6 

•94 

0.069 

4 

.5  Xio"4 

6 

•59 

o 

.0107 

0.15 

12 

.86 

7 

.21 

0.072 

5 

Xio-4 

6 

.82 

o 

.0100 

0.14 

13 

•32 

7 

.46 

0.075 

CALCIUM   CARBONATE 


192 


THE  SOLUBILITY  OF  CALCIUM  CARBONATE  (CALCITE)  IN  WATER  AT  16°  IN 
CONTACT  WITH  AIR  CONTAINING  PARTIAL  PRESSURE  P  OF  CO2. 

(Calc.  from  Schloesing,  1872,  and  Engel,  1888,  by  Johnston,  1915.) 

Total  Ca,  Mols.  Total  Ca(HCp3)j 
per  Liter.         Mols.  per  Liter 

0.007825   0.007874 

0.008855   0.008854 

O.OO972 

O.OIO86 

0.01085 

O.OI4II 

0.01834 


P  of  CO2  in 
Atmospheres. 

Total  (Ja,  Mols. 
per  Liter. 

Total  ua(.nuj3)2 
Mols.  per  Liter. 

P  of  CCh  in 

Atmospheres. 

o  .  000504 

o  .  000746 

0.000731 

0.4167 

0.000808 

O.OOO85O 

0.000837 

0-5533 

0.00333 

0.001372 

0.001364 

0.7297 

0.01387 

0.002<23I 

O.OO2226 

0.9841 

O.O282O 

0.002965 

O.O0296I 

i 

o  .  05008 

0.003600 

0.003597 

2 

0.1422 

0.005330 

0.005328 

4 

0.2538 

o  .  006634 

0.006632 

6 

0.02139 


O.OO972 
O.OIO86 
0.01085 
O.OI4II 

0.01834 
0.02139 


THE  SOLUBILITY  OF   CALCIUM  CARBONATE]  (CALCITE)   IN  WATER  AT  25°  IN 
CONTACT  WITH  CO2  UNDER  INCREASING  PRESSURES.    (McCoy  and  Smith,  1911.) 

B*     Cot        C^vl 

Solid  Phase. 

CaC03 
tt 


Appro*.  Pres- 
sure of  CO2  in 

Mols.  per  Liter  Sat.  Solution. 

Gms.  per  Liter  Sat.  Sol. 

Atmospheres.* 

H2COs. 

Ca(HCO3)2. 

H2COs. 

Ca(HCOs)2. 

O.I 

0.003522 

0.004Il6 

0.22 

0.67 

I.I 

0.03728 

0.009734 

2-3 

I.58 

9.9 

0.3329 

0.02236 

20.  6 

3.62 

13.2 

0.444 

0.02495 

27-5 

4.04 

16.3 

0.550 

0.02600 

34-1 

4.21 

25-4 

0.858 

11-                e                 *-+f* 

o  .  02603 

53-2 

4.22 

Ca(HCO3)2 

u 

Calc.  by  Henry's  Law  from  CO2  concentrations.     See  also  remarks  under  Ferrous  Bicarbonate,  p.  336. 

These  results  show  that  the  solution  becomes  saturated  with  Ca(HCO3)2  at 
about  15  atmospheres  pressure  of  CO2,  and  it  would  be  theoretically  possible  to 
convert  all  the  CaCO3  to  Ca(HCO3)2  by  introducing  sufficient  CO2  at  pressures 
greater  than  15  atmospheres.  Under  the  conditions  of  the  present  experiment, 
it  was  calculated  that  more  than  3  months  time  would  have  been  required  for 
the  complete  conversion. 

The  solubility  of  calcium  carbonate  in  water  saturated  with  CO2  at  one  at- 
mosphere pressure  was  found  by  Cavazzi  (1916)  to  be  1.56  gms.  CaCO3  at  o° 
and  1.1752  gms.  at  15°.  A  supersaturated  solution  prepared  by  passing  a  rapid 
stream  of  CO2  through  sat.  Ca(OH)2  solution  at  15°  contained  2.29  gms.  CaCO3. 

SOLUBILITY  OF  CALCIUM  CARBONATE  IN  WATER  AT  15°.  (Tread well  and  Reuter,  1896.) 

(Among  the  investigators  who  have  reported  results  upon  the  solubility  of  calcium  carbonate  may 
be  mentioned,  Cossa,  1869;  Schloesing,  1872;  Caro,  1874;  Reid,  1887-88;  Irving  and  Young,  1888;  Ander- 
son, 1888-89;  Engel,  1888;  Lubavin,  1892;  Pollacci,  1896.) 

Gms.  per  100  cc.  Saturated  Solution. 


cc.  CO2  per  100  cc. 
Gaseous  Phase 
(o°  and  760  mm.). 

8.94 
6.04 

Partial  Pres 
of  CO2  in  n 
Hg. 

67.9 

45-9 

5-45 
2.18 

41.4 
16.6 

1.89 

14.4 

1.72 

0.79 

i3-i 
6 

0.41 

3-i 

0.25 
0.08 

1.9 
0.6 

Free  CO*. 

Ca(HCO3)2. 

Ca. 

0.1574 

0.1872 

0.0462 

0.0863 

0.1755 

0.0433 

0.0528 

0.1597 

0.0394 

0.0485 

O.I54O 

0.0380 

0.0347 

O.I492 

0.0368 

0.0243 

O.I33I 

0.0329 

O.OI45 

0.1249 

o  .  0308 

O.OO47 

0.0821 

o  .  0203 

O.OO29 

0.0595 

0.0147 

O.O4O2 

o  .  0099 

0-0385 

0.0095 

Therefore  i  liter  sat.  solution  at  15°  and  o  partial  pressure  of  CO2  contains 
0.385  gram  Ca(HCO3)2.  Determinations  similar  to  the  above,  made  in  o.i  n 
NaCl  solutions  at  15°,  are  also  given.  It  is  pointed  out  by  Johnston  (1915),  that 
although  Treadwell  and  Reuter  made  very  painstaking  analyses,  their  mode  of 
working  did  not  secure  equilibrium  conditions,  a  fact  which  is  borne  out  by  the 
lack  of  constancy  of  the  calculated  solubility-product  constant. 


193  CALCIUM  CARBONATE 

SOLUBILITY  OF  CALCIUM  CARBONATE  (CALCITE)  IN  WATER  IN  CONTACT 
WITH  AIR  AT  DIFFERENT  TEMPERATURES.  " 

(Wells,  1915.) 

(Joplin,  Mo.,  calcite  was  used.  The  solutions  were  kept  in  a  thermostat  and 
agitated  by  a  current  of  out-door  air  filtered  through  cotton  and  washed  by 
water.  The  CO2  content  of  the  air  varied  from  3.02  to  3.27  parts  per  10,000. 
The  calcium  content  of  the  solutions  was  determined  by  titrating  with  0.02  n 
NaHSO4,  using  methyl  orange  as  indicator.  The  solutions  were  slightly  acid 
to  phenolphthaleine,  showing.that  the  calcium  was  present  chiefly  as  bicarbonate.) 

t°.  Cms.  CaCOs  per  Liter. 

o      0.081 
10      0.070 

20        0.065 

25        0.056  (0.046) 

30        0.052 

40      o . 044 

50        0.038  (0.029) 

Results  in  parentheses  by  Kendall  (1912).  In  connection  with  these  it  is 
stated  by  Johnston  (1915),  that  assurance  is  wanting  that  the  partial  pressure  of 
CO2  was  the  same  at  both  temperatures  and  the  results  are,  therefore,  not  neces- 
sarily comparable. 

SOLUBILITY  OF  CALCIUM  CARBONATE  IN  WATER  AT  DIFFERENT  TEMPERATURES 
AND  IN  CONTACT  WITH  AIR  CONTAINING  DIFFERENT  PARTIAL  PRESSURES  OF 
C02. 

(Leather  and  Sen,  1909.) 


Results  at  15". 

Partial 
Pressure       Gms-  per  Liter  Sol. 

Results  at  25°. 

Pressure         Gms.  per  Liter  Sol. 

Results  at  40°. 

Partial 
Pressure      Gms.  per  Liter  Sol. 

CO2  in  Gas   '  CaCOs. 

C02. 

C02inGas      CaCOs. 

C02.      ' 

COz  in  Gas"  CaCOs. 

C02.       ' 

Phase. 

Phase. 

Phase. 

0.8 

0 

•  193 

0.117 

0.7 

0 

•159 

0 

.091 

0.6 

0.136 

0.078 

i  .5 

0 

•  193 

0.152 

1.6 

0 

.177 

o 

.III 

i  .7 

0.143 

0.085 

1.7 

o 

.238 

0.135 

4-6 

o 

•341 

o 

.208 

2.9 

0.175 

0.106 

6.8 

0 

•445 

0.327 

7.8 

0 

.446 

0 

.301 

3-5 

0.232 

0.169 

9.9 

0 

.627 

0.456 

16.5 

o 

•539 

o 

.522 

7 

0.284 

0.234 

13-6 

o 

.723 

0.560 

30.1 

o 

•743 

o 

•715 

14.9 

0.384 

0.293 

14.6 

0 

.686 

0.623 

35-5 

0 

•755 

o 

.803 

22.2 

0.427 

o  333 

31.6 

I 

.050 

1.117 

31-7 

0.480 

0.476 

Similar  results  also  given  for  20°,  30°  and  35°. 

The  mixtures  were  constantly  agitated  at  constant  temperature.  The  solid 
phase  in  each  case  was  found  to  be  CaCO3  and  it  is  concluded  that  Ca(HCO3)2 
cannot  exist  in  this  solid  state  above  15°. 

In  discussing  the  experiments  of  Leather  and  Sen,  Johnston  (1915)  points 
out  that  their  method  of  analysis  gives  low  results  for  CO2.  A  calculation  of 
the  data  yields  very  irregular  results  and  the  most  that  can  be  deduced  from 
them  is  that  the  solubility-product  constant  of  calcite  probably  decreases  some- 
what with  temperature,  becoming  apparently  about  0.5  X  io~8  at  40°. 

Data  for  the  solubility  of  CaCOs  in  boiling  water  are  given  by  Cavazzi  (1917). 

Data  for  the  solubility  of  calcium  carbonate  in  water  containing  excess  of 
carbon  dioxide  are  also  given  by  Seyler  and  Lloyd  (1909).  The  experiments 
were  made -at  room  temperature.  Additional  experiments  showed  that  small 
amounts  of  CaCl2,  CaSO4  or  NaHCO3  did  not  affect  the  solubility-product  con- 
stant. Small  amounts  of  Nad,  Na2SO4  and  MgSO4,  containing  no  ion  in  common 
with  CaCOs,  resulted  in  an  increase  of  the  total  calcium  in  the  solution. 

Data  for  the  solubility  of  calcium  carbonate  in  water,  determined  by  the  con- 
ductivity method,  are  given  by  Holleman  and  by  Kohlrausch  and  Rose  (1893). 


CALCIUM   CARBONATE 


194 


SOLUBILITY  OF  CALCIUM  CARBONATE  IN  AQUEOUS  SOLUTIONS  OF  AMMONIUM 

CHLORIDE. 
Results  at  I20-i8°. 

(Cantoniand  Goguelia,  1905.) 
(Flasks>llowed  to  stand 

98  days.) 
Cms.  per  Liter  Sat.  Sol. 


NH4C1. 

53-5 
100 
2OO 


CaCOs. 
0.423 
0.609 
0.645 


Results  at  25°. 

(Rindell,  1910.) 
(Constant  agitation 
^  24  hrs.),.-. 
Cms.  per  Liter  Sat.  Sol. 

Results  at  60°  for  Calcite  and  Aragonite. 

(Warynski  and  Kouropatwinska, 
1916.) 

G*ms.  per  Liter.                  Cms.  per  Liter. 

NH4C1. 
6.7 

13-4 
26.8 

53-5 

CaCOs. 
0.285 

0-373 
0.502 
0.678 

1    NH4C1. 
O 

1.07 

5-35 
10.70 
26.76 
53-52 
160.56 

Calcite. 
0.028 
0.164 
0-333 
0-453 
0.664 

0-934 
I.  21 

NH4C1. 
O 
1.07 

5-35 
10.70 
26.76 
53-52 
160.56 

Aragonite. 
0.041 
0.184 
0.371 

0-505 
0.728 
I.OI5 
1.36 

SOLUBILITY  OF  CALCIUM  CARBONATE  IN  AQUEOUS  SOLUTIONS  OF  AMMONIUM 

NITRATE  AND  OF  TRIAMMONIUM  CITRATE. 
laAq.  NH4NO3  at  18°.  InAq.NH4NO3at25°.  In  Aq.  Triammonium  Citrate  at  25°. 


(Berju  andiKosminiko,  1904.) 
Gms.  per  Liter  Sat.  Sol. 


(Rindell,  1910.) 
Gms.  per  Liter  Sat.  Sol. 


(Rindell,  1910.) 

Mols.  Citrate         Gms.  CaCOs 
per  Liter. 

0.0625 
0.125 
0.250 
0.500 


per  Liter. 
1.492 
2.264 
3.980 
6.687 


NH*NOs.  CaCOs.  NH4NOs.  CaCOs. 

o  0.131  5  0.200 

5  0.211  10  0.278 

10  0.258          20        0.383 

20  0.340          40        0.526 

4O  0.462 

80  0.584 

SOLUBILITY  OF  CALCIUM  CARBONATE  IN  AQUEOUS  SOLUTIONS  OF  MAGNESIUM 
CHLORIDE,  MAGNESIUM  SULFATE,  SODIUM  CHLORIDE  AND  SODIUM  SULFATE 
UNDER  CO2  PRESSURE  OF  Two  ATMOSPHERES.  (Ehlert  and  Hempei,  1912.) 

Gms.  Hv-        ^.          ^   r,^ 
Aq.  Salt 
Solution. 


MgCl2.6H2O 


«•• 

Gms.  Hy- 
drated  Salt 
per  1000  Gms. 
HaO. 

Gms.  CaCOs          .      Salt 

"SSL*     &S        ''• 

Gms.  Hy- 
drated  Salt 
per  looo 
Gms.  H20 

Gms.  CaCOs 
per  looo  cc. 
Solvent. 

5 

O 

2-337 

NaCl 

5 

8 

3-740 

5 

6.1 

2.352 

" 

5 

86 

3-  783 

5 

50 

3-404 

u 

5 

106.9 

3.690 

5 

86.9 

4.083 

tc 

5 

175-6 

3-350 

5 

350 

3-301 

" 

263.4 

2.8x1 

5 

700 

2.736 

cc 

8 

35i-2 

2.163 

5 

1150 

2.205 

MgSO4.7H2O 

14 

105-3 

2.177 

5 

1725 

i  .706 

u 

14 

(sat.) 

0.914 

5 

2300  sat. 

i  .406 

Na2S04.ioH20 

14 

137-7 

1  .406 

5 

28 

3.280 

" 

14 

(sat.) 

1  .920 

NaCl 

SOLUBILITY  OF  CALCIUM  CARBONATE  IN  AQUEOUS  SOLUTIONS  OF  POTASSIUM 

CHLORIDE  AND  OF  POTASSIUM  SULFATE  AT  25°.    (Cameron  and  Robinson,  1907.) 
Results  for  Aqueous  KCI:  "  Results  for  Aqueous  K2SO4: 


iii  coiiuici  wnn  air. 

Gms.  per  100  Gms. 
Sat.  Sol. 

atmosphere  of  CO2. 
Gms.  per  100  Gms. 
Sat.  Sol. 

:'  atmosphere  of  C02. 

Gms.  per  100  Gms.             Gms.  per  100  Gms. 
Sat.  Sol.                                 Sat.  Sol. 

KCI. 
0 
3-9 
7-23 
13-82 
18.21 
26 

CaCOa. 
0.0013 
0.0078 
0.0078 
0.0072 
0.0070 
0.0060 

KCI. 
O 

3-9 
7-23 
13.82 
18.21 
26 

CaCOs. 
0.062 
0.145 
0.150 
0.165 

0.154 
0.126 

K2S04. 
1.  60 

3.15 

4-73 
6.06 
8.88 
10.48 

CaCOs. 
0.0104 
0.0116 
0.0132 
0.0148 
0.0192 
0.0188 

K2S04 
0.69 

i-37 
1.67 
2.18 
2.99 

CaO.     ' 
0.69 
0.69 
0.47* 
0.30* 
0.24* 

*  J5olid  phase  syngenite. 

One  liter  aqueous  solution  containing  223.8  gms.  KCI  dissolves  0.075  gm. 
calcite  at  60°. 

One  liter  aqueous  solution  containing  223.8  KCI  dissolves  0.093  gm-  aragonite 
at  60°.  (Warynski  and  Kouropatwinska,  1916.) 


195  CALCIUM  CARBONATE 

SOLUBILITY  "OF  CALCIUM  CARBONATE  IN  AQUEOUS  SOLUTIONS  OF  SODIUM 

CHLORIDE  AT  25°. 
Solutions  in  contact  with. 

CO2  Free  Air.  Ordinary  Air.         CO2atOne  Atmos.  Pressure. 

(Cameron,  Bell  and  Robinson,  1907.)        (Cameron  and  Seidell,  1902.)   (Cameron,  Bell  and  Robinson,  1907.) 
Cms.  per  100  Gms.  HzO.  Gms.  per  100  cc.  Sat.  Sol.  Gms.  per  100  Cms.  H2O. 


NaCl. 

CaCOa. 

'  NaCl. 

CaCOs. 

NaCl. 

CaCOa. 

1.  60 

o  .  0079 

I 

O.OII2 

1.49 

0.150 

5.18 

0.0086 

4 

O.OI4O 

5-69 

0.160 

9-25 

o  .  0094 

8 

0.0137 

II.  06 

0.174 

11.48 

O.OIO4 

10 

0.0134 

15.83 

0.172 

16.66 

0.0106 

15 

O.OII9 

19.62 

0-159 

22.04 

O.OII5 

20 

0.0106 

29.89 

0.123 

30-50 

O.OII9 

25 

0.0085 

35-85 

0.103 

Data  for  the  solubility  of  calcium  carbonate  in  aqueous  solutions  of  mixtures 
of  sodium  chloride  and  sodium  sulfate  in  contact  with  air  and  with  CO2  are 
given  by  Cameron,  Bell  and  Robinson  (1907). 

Data  for  solubility  of  CaCO3  in  aqueous  NaCl  and  other  salt  solutions,  de- 
termined by  boiling  and  cooling  the  solution,  are  given  by  Gothe  (1915). 

Data  for  the  solubility  of  mixtures  of  calcium  carbonate  and  calcium  sulfate  in 
aqueous  solutions  of  sodium  chloride  at  25°tare  given  by  Cameron  and  Seidell  (1901  ). 

Data  for  the  solubility  of  mixtures  of  calcium  carbonate  and  calcium  sulfate 
in  aqueous  solutions  of  mixtures  of  sodium  chloride  and  sodium  sulfate  at  25°, 
in  contact  with  air  and  with  CO2,  are  given  by  Cameron,  Bell  and  Robinson  (1907). 

One  liter  aqueous  solution  containing  175.5  gms.  NaCl  dissolves  0.062  gm. 
calcite  at  60°. 

One  liter  aqueous  solution  containing  175.5  gms-  NaCl  dissolves  0.071  gm. 

aragonite  at  60°,  (Warynski  and  Kouropatwinska,  1916.) 

SOLUBILITY  OF  CALCIUM  CARBONATE  IN  AQUEOUS  SOLUTIONS  OF  SODIUM 
HYDROXIDE  IN  CONTACT  WITH  CO2  FREE  AIR. 

(LeBlanc  and  Novotny,  1906.) 

Gms.  CaCOs  per  Liter  Sat.  Sol. 


Water  0.0128  0.0207 

About  o  .  oooi  n  NaOH  0.0087  0.0096 

"      o.ooiow      "  0.0042  0.0069 

"      o.oioow      "  0.0042  0.0057 

Data  on  the  equilibrium  in  aqueous  solutions  of  CaCO3,  Na2CO3  and  NaOH 
are  given  by  Wegscheider  and  Walter  (1907). 

SOLUBILITY  OF  CALCIUM  CARBONATE  iNAQUEOUs.SoLUTiONs  OF  SODIUM  SULFATE. 
Solutions  in  contact  with: 

CO2  Free  Air  at  25°.  Ordinary  Air  at  24°. 

(Cameron,  Bell  and  Robinson,  1907.)  (Cameron  and  Seidell,  1902.) 

Gms.  per  IPO  Gms.  HsO.  Gms.  Na.SCu       S^E'SL? 

Na2SO<.  CaCOs.  ^  per  Liter.          ECa(HCO8),.' 

0.97     0.0151        5     0.175 
1.65     0.0180        10      0.232 

4.90  O.O262  2O  0.277 

12.69  0.0313  40  0.332 

14.55  0.0322  80  0.400 

19.38  0.0346  I5O  0.510 

23.90  0.0360  250  0-725 

Freezing-point  data  for  mixtures  of  calcium  carbonate  and  calcium  chloride 
are  given  by  Sackur  (1911-12). 


CALCIUM  CHLORATE 


196 


CALCIUM  CHLORATE  Ca(ClO3)2.2H2O. 

loo  grams  saturated  aqueous  solution  contain  64  grams  Ca(ClO3)2  at  18°. 

Density  of  solution  is  1.729.  (Mylius  and  Funk,  1897.) 

CALCIUM    CHLORIDE   CaCl2. 

SOLUBILITY   IN   WATER 

(Roozeboom  —  Z.  physik.  Chem.  4,  42,  '89;  see  also  Mulder;  Ditte  —  Compt.  rend.  92,  242,  '81;  Engel 
—  Ann.  chim.  physic.  [6Ji3,  381,  '88;  Etard  —  Ibid,  [7]  2,  532,  '94.) 


Cms.  CaClj  per 

100  Gms. 


Solid 
Phase. 


-55 

-2$ 

O 

10 

20 


Water.  Solution. 

42.5       29.8  Ice  +  CaCl2^H2O 

50.0      33.3  CaCl2.6H20 

59-5    37-3  CaC1*-6H*° 

65.0      39.4  CaCl2.6H2O 

42.7  CaCl2.6H20 

50.7  CaCl2.6H2O 

47.6  CaCl2.4H2Oa 

50.1  •4H2Oa+.6H20 

53.4  -4H2Oa. 

5I.I  CaCl2.4H200 

0  wiH2O  /3  +  .6H2O 


74-5 


3O.2  IO2-7 
20     91.0 

29.8  100.6 

40    II5-3 
20    104.5 

29.2  112. 8 

35   I22-5 
38.4  127.5 

45-3  130-2 

Density  of  saturated  solution  at  o°  =  1.367,  at  15°  =  1.399,  'at  18°  =  1.417; 
at  25°  =  1.47. 

SOLUBILITY  OF  CALCIUM  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  HYDROCHLORIC 

ACID  AT  o°. 

(Engel,  1887.)  _ 


53 

55.0 

56.0    wtH2Q/3+CaCl2.2H20 

56.6    ^H2O  a  +  CaCl2.2H2O 


Gms.  CaCl2  per 

t°. 

100 

Gms. 

Solid 

Water. 

Solution. 

ase. 

60 

136.8 

57-8 

CaCl2.2H2O 

70 

I4I.7 

58.6 

CaCl2.2H2O 

80 

147.0 

59-5 

CaCl2.2H2O 

90 

152  .7 

60.6 

CaCl2.2H2O 

100 

159.0 

61  .4 

CaCl2.2H2O 

120 

173.0 

63-4 

CaCl2.2H2O 

I4O 

I9I.O 

65.6 

CaCl2.2H2O 

160 

222-5 

69.0 

CaCl2.2H2O 

170 

255-0 

71.8 

CaCk-aHaO 

175-5 

297.0 

74-8; 

(  CaClz.2H20 
t  -t  CaCla-iizC 

180 

300.0 

75-o 

CaCl2.H3O 

200 

3II.O 

75-7 

CaCl2.H20 

235 

332-0 

76.8 

CaCl2.H2O 

260 

347-0 

77.6 

CaCl2.H20 

CaCb. 

HC1. 

U0  01    JH.L.    OU1. 

'    CaCh. 

HC1. 

51-45 

0 

1.367 

29.84 

I5-84 

1.283 

46.45 

3-32 

1-344 

20.  1  2 

23-I5 

I.25O 

42.80 

5-83 

1.326 

11.29 

34.62 

1.238 

36.77 

10.66 

1.310 

SOLUBILITY  OF  MIXTURES  OF  CALCIUM  CHLORIDE,  MAGNESIUM  CHLORIDE  AND 
CALCIUM  MAGNESIUM  DOUBLE  CHLORIDE  (TACHHYDRITE). 

(Van't  Hoff  and  Kenrick,  1912.) 
Gms.  per  100  Gms. 


CaCl2. 

MgCk 

41.2 

31-6 

57-i 

26 

54-5 

28.4 

o 

85.63 

32-3 

17.9 

80.  i 

16.1 

88.7 

7.24 

16.7 

21-95 
28.2 
116.7 

25 

28.2 

28.2 

Tachhydrate  =  2MgCl2.CaCl2.i2H2O. 

100  grams  H2O  dissolve  63.5  grams  CaCl2  +  4.9  grams  KC1  at  7°  (M). 
100  grams  H2O  dissolve  57.6  grams  CaCl2  +  2.4  grams  NaCl  at  4°  (M). 
loo  grams  H2O  dissolve  59.5  grams  CaCl2  +  4.6  grams  NaCl  at    7°  (M). 
100  grams  H2O  dissolve  72.6  grams  CaCl2  +  16  grams  NaCl  at  15°  (R). 
(M)  =  Mulder.     (R)  =  Rudorff. 


Solid  Phase. 

MgCU.6H20-r-CaCl2.6H20 

"  "        +Tachhydrite 

Tachhydrite+MgCl2.6H2O 

+  "  +MgCl2.4HsO 
+CaCl2.6H2O  +CaCl2.4H2O 
+CaCl2.4H20 

CaCl2.6H204-CaCl2.4H20 


197  CALCIUM  CHLORIDE 

SOLUBILITY  OF  CALCIUM  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  SODIUM 
CHLORIDE  AT  25°  AND  VICE  VERSA. 

(Cameron,  Bell  and  Robinson,  1907.) 


1M 

Sat.fol. 

I.444I 
I-365I 
1.3463 
1.2831 

Gms.  per  100  Cms.  HzO 

'•          Solid 
Phase. 

CaCl2.6H2O 
"  +NaCl 
NaCl 

dtt        ( 
Sat.  Sol. 

1-2653 
1.2367 
I  .  2080 
I  .  2030 

Gms.  per  100  Gms.  HzO 

•     Solid 

*     CaCl2. 
84 
78.49 
58.48 
53-47 
36.80 

NaCl. 
o 

1.846 
1.637 
1.799 

7-77 

CaCl2. 
30.08 
19-53 
3-92 
O 

NaCl. 
10.70 
18.85 
32.48 
35-80 

'  Phase. 
NaCl 

SOLUBILITY  OF  CALCIUM  CHLORIDE  IN  AQUEOUS  ALCOHOL  AT  ROOM  TEMPERATURE. 

(Bodtker,  1897.) 

Vol.  Gms.  Vol.  Gms. 

Solution  Used.  Per  Cent  CaCk  per  Solution  Used.  Per  Cent    CaClsper 

Alcohol.    5  cc.  Sol.  Alcohol.    5  cc.  Sol. 

15  Gms.  CaCl2.6H2O  15  Gms.  CaCl2.6H2O+2o  cc.: 

+  20  cc.  alcohol        92.3       1.430          alcohol  +  2  Gms.  CaCl2        99.3       1.561 

15  Gms.  CaCl2.6H2O  +  3  99-3       i  •  59° 

+  20  cc.  alcohol         97.3       1.409  "       +4     "  99.3       1.641 

15  Gms.  CaCl2.6H2O  "       +5     "  99-3       1.709 

+  20  cc.  alcohol        99.3       1.429 
15  Gms.  CaCl2.6H2O 
+  20  cc.  alcohol 
+  i  Gm.  CaCl2         99.3       1.529 

SOLUBILITY  OF  CALCIUM  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  ACETONE 

AT  20°. 

(Frankforter  and  Cohen,  1914.) 

Measured  amounts  of  acetone  were  added  to  known  solutions  of  CaCl2  in  water, 
until  opalescence,  indicative  of  the  separation  of  a  second  liquid  layer,  was  ob- 
served. The  composition  of  a  large  number  of  such  mixtures  gives  the  limiting 
values  for  the  binodal  curve  of  the  system.  Tie  lines  were  also  determined  in 
several  instances  by  using  such  quantities  of  the  three  components  that  an  ade- 
quate amount  of  each  layer  would  be  formed  to  permit  the  determination  of  the 
CaCl2  in  it.  The  points  thus  located  on  the  curve  fix  the  tie  lines,  and  from  them 
the  approximate  position  of  the  plait  point  can  be  estimated. 

Points  on  the  Binodal  Curve  Composition  of  Points  Representing 

at  20°.  Tie  Lines  at  20°. 

Gms.  per  100  Gms.  Sat.  Sol.        Gms.  per  100  Gms.  Upper  Layer.  Gms.  per  100  Gms.  Lower  Layer. 


Acetone. 

Cadi. 

Acetone. 

CaCl2.                     Acetone.          CaCl2. 

9 

40.5*    /(solid  phase 

90.2 

0.186                  28.5           16.61 

22.7 

38.l6tf     CaCl2) 

83-3 

0.628                      34.6             12.97 

20.8 

31.2 

8l 

o  .  948                  40              10  .  6 

2O.  2 

28 

78.5 

1.321                  43-5            9-36 

21 

24.4 

60 

5        (plait  point)    60                   5 

23 

21.1 

Points  on 

the  Binodal  Curve  at  Different 

25 

19.2 

is  6 

Temperatures. 

35 

•*•  0  •  w 

12.8 

Gms.  per  loo^Gms.  Sat.  Sol. 

40 

' 

Acetone.                           CaCl2. 

45 

8.8 

5 

3I.09                            I5-52 

50 

7-4 

10 

22.77                            23.64 

55 

6.1 

15 

31.09                      I5-52 

60 

5 

18 

30-58                      15-27 

65 
70 

3-9 

2.8 

25 
25 

21.44                      22.25 
29.83                      14.89 

75 

1.8 

30 

20.99                      21.79 

80 

i 

30 

29.27                      14.62 

85 

35 

21.14                      20.91 

9° 

O.2 

35 

28.59                      14-29 

95 

O.I 

40 

19.83                      20.58 

Point  on  solubility  curve,     t  Quadruple  point.   4° 

27.90                      13.93 

CALCIUM  CHLORIDE  198 

SOLUBILITY  OF  CALCIUM  CHLORIDE  IN  A  SATURATED  SOLUTION  OF  SUGAR  AT 

31-25°. 

.  (Kohler,  1897.) 

100  grams  saturated  solution  contain  42.84  grams  sugar  +  25.25  grams  CaCl2, 
or  100  grams  water  dissolve  135.1  grams  sugar  +  79.9  grams  CaCl2. 

100  gms.  95%  formic  acid  dissolve  43.1  gms.  CaCl2  at  19°.  (Aschan,  1913.) 

loo  cc.  anhydrous  hydrazine  dissolve  16  gms.  CaCl2  at  room  temp. 

(Welsh  and  Broderson,  1915.) 

ioo  gms.  propyl  alcohol  dissolve  10.75  S1118-  CaCl2  (temp.?).  (Schlamp,  1894.) 


FREEZING-POINT  DATA  (Solubility,  see  footnote,  p.  i)  ARE  GIVEN  FOR  THE 
FOLLOWING  MIXTURES  OF  CALCIUM  CHLORIDE  AND  OTHER  SALTS. 


CaCl2+CaF2  (i)  (2) 
CaCl2+CaI2  (i) 
CaCl2+CaO(3) 
CaCl2+CaSi03  (4) 


CaCl2+CuCl  (5 


(3) 
5) 


(i)  =  Ruff  and  Plato,  1903;  (2)  =  Pla 
=  Menge,  1911;  (6)=  Sandonnini,  1911; 
reng,  1914;  (10)  =  Schaefer,  1914. 


CaCl2+PbCl2  (5)  (6)  (7) 
CaCl2+LiCl  (7)  (8) 
CaCl2+MgCl2  (5)  (6) 
CaCl2+MnCl2  (6)  (7) 
CaCl2+KCl  (5)  (3) 
CaCl2+NaCl  (5)  (3) 


CaCl2+AgCl  (5) 
CaCl2+SrCl2  (6)  (7)  (3)  (10) 
CaCl2+SrO  (3) 
CaCl2-fTlCl  (9)  * 
CaCl2+SnCl2  (5) 
CaCl2+ZnCl2  (5) 


Plato,  1907;  (3)  =  Sacfcur,  1911-12;  (4)  =  Karandeeff,  1910;  (5) 
(7)  =  Sandonnini,  1913;   (8)  =  Sandonnini,  1913;   (9)=  Kor- 


CALCIUM  CHLORIDE  ACETAMIDATE  CaCl2.3CH3CONH2. 

SOLUBILITY  IN  ACETAMIDE  AT  VARIOUS  TEMPERATURES,  DETERMINED  BY  THE 

SYNTHETIC  METHOD. 

(Menschutkin,  1908.) 


t°           /- 

Gms.  per 

Sat. 

too  Gms. 
So1-                   Solid 

Gms.  per  ioo  Gms. 
^0                         Sat.  Sol. 

Solid 

CaCl2.3CH3-l_rarl  '        Phase. 
CONH2    /-CaCl2- 

CaCl2-3CH3-\      r  r, 
CONH2    j=CaC!2. 

Phase. 

82  m.  pt. 

0 

0         CHaCONIfc 

IOO 

65.6 

25-3 

1-3 

78 

8 

3.1        " 

150 

70-5 

27.1 

" 

74 

15-4 

5-9     " 

165 

74.8 

28.8 

" 

66 

27 

10.4       " 

175 

80.6 

31 

" 

54 

39-2 

I5.I        '« 

180 

85-5 

32.9 

it 

46  Eutec. 

45 

17.3       "  +1.6 

184 

90-5 

34-8 

" 

58 

48-5 

18.7           1.6 

186  tr. 

pt.  94.5 

3^-4 

"  +CaCl2(?) 

62 

54-5 

21 

200 

97-5 

37-5 

CaCla(?) 

64  tr.  pt. 

62.1 

23.9       1.6+1.3 

2IO 

IOO 

38.5 

« 

1.6  =  CaCl2.6CH3CONH2.  1.3  =  CaCl2.3CH3CONH2 


CALCIUM  CHLORIDE  ACETIC  ACIDATE  CaCl2.4CH3COOH. 

SOLUBILITY  IN  ACETIC  ACID  AT  VARIOUS  TEMPERATURES,  DETERMINED  BY  THE 

SYNTHETIC  METHOD. 

(Menschutkin,  1906.) 
Gms.  per  ioo  Gms. 

Sat.  Sol.  SoUd 

Phase. 


CaCl2.4CH3-l     ran 

COOH     /-CaCl2. 

16.2 

m.  pt.        o          o 

15 

18          5-7 

14 

27          8.5 

13 

34        10.7 

II.  I 

Eutec.     42        13-3 

30 

47.6     15 

35 

5o        15-8 

1.4 

t°. 


CHsCOOH 


40 

45 


60 

"   +1-4  65 

1.4  70 

73  m.  pt. 
CaCl2.4CH3COOH. 


Gms.  per  ioo  Gms. 
Sat.  Sol. 

Solid 
Phase. 

CaCWCHs-l 

COOH     / 

=  CaCl2. 

54-7 

17-3 

1*4 

63 

19.9 

" 

69.5 

21-9 

" 

79-5 

25.1 

" 

84-5 

26.7 

" 

91  .2 

28.8 

H 

IOO 

31-6 

• 

199 


CALCIUM  CHLORIDE 


CALCIUM  CHLORIDE  ALCOHOLATES   CaCl2.3CH3OH,    CaCl2.3C2H5OH. 

(The  compounds  were  prepared  by  mixing  anhydrous  CaCl2  with  the  alcohbf. 
In  the  case  of  the  methyl  alcohol  compound,  the  tri  CH3OH  salt  crystallizes 
above  55°,  the  tetra  salt  below  this  temperature.) 

SOLUBILITY  OF  EACH  IN  THE  RESPECTIVE  ALCOHOL  AT  VARIOUS  TEMPERATURES, 
DETERMINED  BY  THE  SYNTHETIC  METHOD. 

(Menschutkin,  1906.) 

Results  for  CaCl2.3CH3OH.  Results  for  CaCl2.3C2H5OH. 


Gms.  per  100  Gms.                                  Gms.  per  100  Gms. 
•  o                Sat.  Sol.                   Solid         *<,                Sat.  Sol.                 Solid 

Gms.  per  100  Gms. 
to               Sat.  Sol. 

CaCl2.3CH3OH  -  CaCl2.'                            CaCU-sCHaO] 

H  =  CaClz.                     CaCl2.3C2HsOH  =  CaCl2 

0 

33 

O 

17-85       1-4              95 

66 

3 

35- 

5       1.3 

O 

34-8 

iS-5 

10 

37 

6 

20.15 

"5 

70 

3 

37- 

6 

2O 

46 

20.5 

2O 

42 

2 

22.6 

135 

75 

2 

40. 

3 

40 

58.7 

26.1 

30 

47 

25.2 

155 

81 

8 

43- 

8 

60 

73 

32.5 

40 

S2 

27.8 

165 

86 

2 

46. 

2           " 

70 

80.8 

36 

5° 

57 

3 

30-7 

'             170 

89 

5 

47- 

9 

80 

86.8 

38.7 

55 

60 

32.1                                  174 

93 

5 

50. 

i        " 

85 

89.2 

39-7 

56 

61 

3 

32.8              «                  177* 

IOO 

53- 

6 

90 

91.9 

40.8 

55 

60 

5 

32.4             "+1.3      190 

55- 

7     i.i(?) 

95 

96.2 

42.8 

75 

63 

i 

33-8            1.3         215 

57- 

7        " 

97* 

IOO 

44-5 

14  =  CaCl2.4CH3OH.    1.3 


*  M.  pt. 

CaCl2.3CH3OH,  i.i  =  CaCl2.CH3OH. 


CALCIUM    CHROMATE   CaCrO4. 

SOLUBILITY  OP  THE  SEVERAL  HYDRATES  IN  WATER. 

(Mylius  and  Wrochem  —  Wiss.  Abh.  p.  t.  Reichanstalt  3,  462,  'oo.) 

-. o       Gms.  CaCrO4  per  100  Gms.  Mols.  CaCrO4 

*  •         i — ; • — — — ; >  per  100  Mols. 

Water.  Solution.  H2O. 

SoHd  Phase,  o  CaCrO4.2H2O.  (Monoclinic.) 


0 

17-3 

14-75 

2.O 

18 

16.68 

14-3 

i-93 

20 

16.6 

14.22 

i-93 

30 

16-5 

I3-89 

1-85 

45 

14-3 

I2-53 

1-65 

Solid  Phase,  ft  CaCr04.2H20  (Rhombic.) 


o         10.9            9.8  i 

18        11.5          10.3  i 

40         1 1 . 6          10 . 4  i 

Solid  Phase,  CaCrO4.H2O. 


•25 
•33 

•34 


0 

13.0 

"•5 

1.50 

18 

10.6 

9.6 

I  .22 

25 

10.0 

9.1 

*•*$ 

40 

8-5 

.     7-8 

0.98 

60 

6.1 

5-7 

0.70 

75 

4-8 

4.6' 

0.56 

IOO 

3-2 

3-i 

o-37 

f.c 

Jms.  CaCrO4  per  TOO  Gms.   ^ 

[ols.CaCr04 
er  TOO  Mols. 
H20. 

Water. 

Solution.'  * 

Solid  Phase, 

CaCr04.iH20 

o 

7-3 

6.8 

0.84 

18 

4-8 

4.4 

0.51 

3i 

3-84 

3-7 

0.44 

38 

•5    2.67 

2,6 

0.31 

5o 

1.63 

1.6 

0.19 

60 

1-13 

i.i 

0.13 

ICO 

0.81 

0.8 

O.O9 

Solid  Phase,  CaCrO4. 

O 

4-5 

4-3 

0.52 

18 

2.32 

2.27 

0.27 

31 

2  .92 

1.89 

O-22 

5o 

1.  12 

i.  ii 

0.13 

60 

0.83 

0.82 

O.II 

70 

0.80 

0.79 

O.OQ 

IOO 

0.42 

0.42 

0.05 

Densities  of  the  saturated  solutions  of  the  above  several  hydrates 
at  18°  are:  a  CaCrO4.2H2O,  1.149;  £  CaCrO4.2H2O,  1.105;  CaCrO4.H2O, 
1.096;  CaCrO4.iH2O,  1.044;  CaCrO4,  1.023. 

loo  cc.  29%  alcohol  dissolve  1.206  grams  CaCrO4. 
loo  cc.  53%  alcohol  dissolve  0.88  gram  CaCrO4. 

(Fresenius  —  Z.  anal.  Chem.  30,  672,  '91.) 


CALCIUM  CINNAMATES  200 

CALCIUM   CINNAMATE   Ca(C6H6.CH:CHCOO)2.3H2O. 

SOLUBILITY  OF  CALCIUM  CINNAMATE  AND  ITS  ISOMERS  IN  SEVERAL 

SOLVENTS. 


Name  of  Salt. 
Calcium  Cinnamate 


Formula. 


Ca(C6H6CH:CHCOO)1.3HiO 


Ca(C9H702)2.3H20 


Isocinnamate 

M 

Allocinnamate 
« 

tt 

Hydrocinnamate 


(i)   =  De  Jong,  1909;   (2)   =  Tarugi  and  CheccnC  1901; 


1903;  (s) 


.  and  Garner,  1903. 


(3) 


Gms.  Anhy- 

Solvent. 

t°. 

drous  Salt  per 
100  Gms. 

Solvent. 

Water 

2 

0.19(1) 

" 

15 

0.2l(2) 

" 

26 
100 

0.24(1) 
1.15(2)1 

" 

20 

23-8   (3) 

Acetone 

2O 

19-6   (3) 

M 

2O 

2        (3 

Water 

2O 

10.2    (4 

Acetone 

18 

2-7  (5 

u 

14 

0.19(5) 

" 

19 

0.21(5) 

Water 

27 

4.25(3) 

Acetone 

25 

3-3  (3) 

=  Michael, 

1901;    (4 

)_=  Liebermann, 

CALCIUM  CITRATE  Ca3(C6H6O7)2.4H2O. 

SOLUBILITY  IN  WATER  AND  IN  ALCOHOL  AT  18°  AND  AT  25°. 

(Partheil  and  Hubner,  1903.) 
Solvent. 


100  Gms.  Solvent  at: 


Water 

Alcohol  (Sp.  Gr.  0.8092  =  95%) 


18°. 

0.08496 
0.0065 


25  • 

0.0959 
0.0089 


EQUILIBRIUM  IN  THE  SYSTEM  CALCIUM  OXIDE-CITRIC  ACID-WATER  AT  30°. 

(van  Itallie,  1908.) 

The  compositions  of  the  solid  phases  were  determined  by  the  "  Rest  Method  ' 
of  Schreinemakers  (1903).  The  results  are  presented  in  the  triangular  diagram 
and  it  was  necessary  to  select  the  fictitious  compound  CeHsOj.i^HsO  instead  of 
CeHgO?  in  order  to  keep  the  citrate  component  within  the  limits  of  the  diagram. 
This  is  in  harmony  with  the  choice  of  anhydrides  as  components  in  the  inorganic 
oxy  acid  systems. 


Gms.  per  100  Gms. 
'    Sat.  Sol. 

QHsCh. 

CaO. 

5*5.86 

0 

54-8 

OK  24 

55-4 

0-35 

53-7 

0.40 

48.3 

0.52 

42.6 

O.6O 

38.5 

0.77 

36.5 

0.70 

34-8. 

0.77 

27-5 

0-45 

Solid  Phase. 


+C«H«O7Ca.4H2O 


Gms.  per  100  Gms.  Sat. 
Sol. 

^StjO 

CaO. 

20.3 

0.35 

I6.3 

0-33 

12-5 

0-39 

8-3 

0.28 

5-2 

0.25 

4.1 

O.2O 

3-2 

0.20 

2.4-0 

0.2I-O.I3 

0.18 

0.24 

0 

O.II3 

Solid  Phase. 


Quadruple  pt. 


Quadruple  pt. 
Ca(OH), 


CALCIUM  Potassium  FERROCYANIDE  CaK2Fe(CN)6.3H2O. 

100  parts  H2O  dissolve  0.125  part  salt  at  15°,  and  0.69  part  at  boiling-point. 

(Kunheim  and  Zimmerman,  1884.) 


ioo  gms.  H2O  dissolve  0.41  gm.  CaK2Fe(CN)6  at  15-17°. 


(Brown,  1907.) 


201  CALCIUM  FLUORIDE 

CALCIUM  FLUORIDE  CaF2. 

One  liter  sat.  aqueous  solution  contains  0.016  gm.  CaF2  at  18°  and  0.017 
gm.  at  26°. 

One  liter  sat.  aqueous  solution  contains  0.0131  gm.  fluorspar  at  o°,  0.0149 
gm.  at  15°,  0.0159  gm.  at  25°  and  0.0167  gm.  at  40°.  (Kohlrauscb,  1904-05, 1908.) 

Freezing-point  data  for  mixtures  of  calcium  fluoride  and  calcium  iodide  are 
given  by  Ruff  and  Plato  (1903)  and  for  mixtures  of  calcium  fluoride  and  calcium 
silicate  by  Karandeeff  (1910). 

CALCIUM  FORMATE  Ca(HCOO)2. 

SOLUBILITY  IN  WATER. 

(Lumsden,  1902;  see  also  Krasnicki,  1887.) 

Cms.  Ca(HCOO)2  per  100  Gms.  Cms.  Ca(HCOO)»  per  100  Gms. 

Water.  Solution.  Water.  Solution.  " 

o          16.15  I3-9°  60          17-50  14.89 

20          16.60  14.22  80          17-95  15-22 

40          17.05  14.56  100          18.40  15.53 

Results  in  good  agreement  with  the  above  are  given  by  Stanley  (1904). 

CALCIUM    GLYCEROPHOSPHATES    a  =  OH.CH2.CH(OH)CH2.OPO3Caf 
0  =  OH.CH2.CH.OPO3Ca.CH2OH. 

SOLUBILITY  OF  CALCIUM  a.  GLYCEROPHOSPHATE  IN  WATER. 

(Power  and  Tutin,  1905;  Couch,  1917.) 

to          Gms.  CaCaHrOeP  ^o  Gms.  CaCsHrOeP 

per  loo  Gms.  Sat.  Sol.!  per  100  Gms.  Sat.  Sol. 

05  40  3-5 

10             4.6  60  2.7 

20              5.2  80  1.8 

25             5  100  0.9 

Results  varying  from  1.7  to  5.4  gms.  per  100  gms.  sat.  solution  at  or  near 
1 8°  are  given  by  Rogier  and  Fiore  (1913),  Willstaetter  (1904)  and  King  and 
Pyman  (1914).  It  is  pointed  out  by  Couch,  however,  that  since  the  solubilities 
of  the  a  and  ft  isomer  differ,  and  also  that  the  commercial  product  contains 
both  isomers,  variable  results  will  be  obtained,  depending  on  the  composition  of 
the  product  and  the  method  used  for  determining  the  solubility.  These  authors 
also  show  that  increasing  amounts  of  alcohol  in  the  solvent  decrease  the  solu- 
bility of  calcium  glycerophosphate. 

i  oo  grams  H2O  dissolve  i  .66  grams  calcium  /3  glycerophosphate  at  20°.  (Couch,  1917.) 
The  results  of  King  and  Pyman  (1914)  are:   1.4  gms.  at  13°  and  I  gm.  at  15°. 

CALCIUM  HEPTOATE   (Oenanthate)   Ca[CH3(CH2)5COO]2.HaO. 
SOLUBILITY  IN  WATER. 

(Lumsden,  1902;  see  also  Landau,  1893;  Altschul,  1896.) 
t .  o°.  20°.  40°.  60°.  80°.  '100* 

Gm.  Ca(C7Hi3O2)2  per 

100  gms.  solution  0.94      0.85      0.81      0.81      0.97      1.24 

CALCIUM  HYDROXIDE  Ca(OH)«. 

Recent  determinations  of  the  solubility  of  calcium  hydroxide  in  water,  agree- 
ing fairly  well  with  the  average  results  given  in  the  table  on  next  page,  are  given 
by  Bassett,  Jr.  (1908),  Moody  and  Leyson  (1908),  Chugaev  and  Khlopin  (1914) 
and  Seliwanow  (1914). 

One  liter  sat.  aqueous  solution  contains  0.305  gm.  CaO  at  120°,  0.169  Sm-  at 
150°  and  0.084  gm.  at  190°.  (Herold,  1905.) 

One  liter  of  aqueous  5.2%  NH3  solution  dissolves  0.81  gm.  Ca(OH)2  at  about 
20°.  (Konowalow,  *899&.,> 


CALCIUM  HYDROXIDE  202 

CALCIUM  HYDROXIDE   Ca(OH)2. 

SOLUBILITY  IN  WATER. 

(Average  curve  from  the  results  of  Lamy,  1878;  Maben,  1883-84;  Herzfeld,  1897,  and  Guthrie  ,^19.01.) 

Grams  per  100  Grams  EhO.          -  ,  0  "Grams  per  too  Grams  H2O. 

*'  '  Ca(OH)2.  CaO.  '  Ca(OH2).  CaO. 

o  0.185  0.140  50  0.128  0.097 

10  0.176  0.133  60  0.116  0.088 

20  0.165  °-I25  7°  0.106  0.080 

25  °-I59  0.120  80  0.094  0.071 

30  o^SS  0.116  90  0.085  0.064 

40  0.141  0.107  I0°  0.077  0.058 

SOLUBILITY    QF    CALCIUM    HYDROXIDE    IN    AQUEOUS    SOLUTIONS    OP 
AMMONIUM  CHLORIDE  AT  25°. 

(Noyes  and  Chapin  —  Z.  physik.  Chem.  28,  520,  '09.) 

Millimols  per  Liter.  Grams  per  Liter  of  Saturated  Solution. 

NH^Cl.          Ca(OH)2.  NI^Cl.          ClT(OH)2  =     CaO. 

o.oo        20.22  o.oo          1-50        1.13 

21.76  29.08  1-165  2.l6  1.63 

43.52  39-23  2.330  2.91  2.20 

83-07        59  -68  4-447        4-42        3-45 

SOLUBILITY    OF    CALCIUM    HYDROXIDE    IN    AQUEOUS    SOLUTIONS    OF 

CALCIUM  CHLORIDE. 

(Zahorsky  —  Z.  anorg.  Chem.  3,  41,  '93;  Lunge  —  J.  Soc.  Chem.  Ind.  u,  882,  '92.) 

Concentration  Grams  CaO  Dissolved  per  100  cc.  Solvent  at: 

—      —~        ~ 


itions,Wt.%.    f 

20°. 

40°. 

60°. 

80°. 

100°.  ' 

0 

o. 

1374 

0 

.Il62 

0 

.1026 

0 

.0845 

0 

.0664 

5 

o. 

1370 

0 

.Il6o 

0 

.1020 

0 

.0936 

0 

.0906 

10 

o. 

1661 

0 

.1419 

0 

•1313 

o 

.1328 

0 

.1389 

IS 

o. 

*993 

o 

.I78l 

0 

.1706 

o 

.1736 

0 

.1842 

20 

o. 

1857* 

0 

.2249 

0 

.22O4 

0 

.2295 

o 

•2325 

25 

o. 

1661* 

o 

.3020* 

0 

.2989 

0 

.3261 

o 

.3710 

30 

o. 

1630* 

o 

.3680* 

o 

.3664 

0 

.4122 

0.4922 

*  Indicates  cases  in  which  a  precipitate  of  calcium  oxychloride  separated  and  thus  removed  some  of 
the  CaCh  from  solution. 

The  results  in  o%  CaCh  solutions,  i.e.,  in  pure  water,  are  high  wken  compared  with  the  average 
results  given  above. 

SOLUBILITY  OF  CALCIUM  HYDROXIDE  IN  AQUEOUS  SOLUTIONS  OF  CALCIUM 

CHLORIDE  AT  25°. 

(Schreinemakers  and  Figee,  1911.) 


JC&Clt. 

5.02 

CaO. 
O  .  IOI    Ca(OH)2 

CaCl2. 

33-21 

CaO. 
0.245 

>               ooiiu  imase. 
CaCl2.4CaO.i4H2O 

10 

O.II5 

" 

33-72 

0.254 

"  +CaCl2.Ca0.2H2O 

15.14 

0.140 

" 

34.36 

0.173 

CaCl2.CaO.2H2O 

18.15 

0.148 

"  +CaCl2.4CaO.i4H2O 

38.61 

O.O6O 

" 

18.01 

0.152 

CaCl2.4CaO.i4H2O 

41  .32 

0.048 

M 

21.02 

0.147 

" 

44.30 

O.O3O 

" 

28.37 

0.170 

« 

44.61 

0.029 

"  +CaCl2.6H20 

32.67 

O.225 

Ca(OH)2? 

44-77 

CaCl2.6H20 

Data  for  the  above  system  at  10°,  25°,  40°,  45°,  48°,  and  50°  are  given  by 
Milikau  (1916). 

Data  for  the  solubility  of  calcium  hydroxide  in  aqueous  calcium  iodide  solu- 
tions at  25°  are  also  given  by  Milikau. 


203 


CALCIUM  HYDROXIDE 


SOLUBILITY  OF  CALCIUM  HYDROXIDE  IN  AQUEOUS  SOLUTIONS  OF  CALCIUM 
NITRATE  AT  25°  AND  AT  100°. 

(Bassett  and  Taylor,  1914;  see  also  Cameron  and  Robinson, 


Results  at  25°. 

Gms.  per  100  Gms. 
Sat.  Sol. 


Results  at  100°. 

Gms.  per  100  Gms. 


Solid  Phase. 


,  per  i 
Sat.  S 


Sol. 


Solid  Phase. 


Results  at  100°  (Con.). 

Gms.  per  100  Gms. 

Sat.  Sol.          solid  Phase. 


'CaO. 

Ca(NO,)2. 

CaO. 

Ca(NO3)2.                             CaO. 

Ca(N03)2.' 

O.II50 

o 

Ca(OH)2       0.0561 

O 

Ca(OH)»                 .  576 

58 

.67 

( 

'a2N2Ct7.2H2O 

0.0978 

4- 

836 

0.0550 

2 

.42     "                          .348 

60 

•44 

" 

0.1074 

9- 

36 

"             0.0624 

4 

.91     "                          .167 

62 

.82 

H 

O.H93 

77 

"               O.IIIO 

15 

•39     "                        -077 

66 

•44 

" 

0.1444 

22. 

46 

"                O.I2OO 

16 

.  10    "                      .  141 

69 

.12 

" 

0.1650 

27. 

83 

0.155 

21 

.86    " 

I 

"  +  a  very 

0.1931 

32- 

94 

0.269 

33 

.03    "                    1.252 

70 

.60 

.    little  Caj- 

0.2579 

.40. 

66 

"                0.480 

42 

.26 

I 

NiOr.ilbO 

o  .  3060 

44- 

44 

0.973         50 

•94 

*                       I  .  203 

70 

.40 

( 

o.  2802 

45- 

28  Ca2NjOr.3H20  1.261 

53 

•75 

1.103 

71 

•44 

" 

0.2314 

47- 

79 

1-477 

55 

.40 

0-937 

73 

•85 

M 

0.1894 

51- 

07 

.476 

55 

•43 

0.849 

75 

•74 

" 

0.1659 

53- 

20 

"              3 

.491 

55 

•65 

•                      0.815 

76 

•94 

" 

o  .  1486 

55- 

25 

" 

•635 

56 

•89  I 

+Ca2N2O;.-  o  .  804 

77 

.62 

Ca(NO,), 

0.0836 

57- 

72  Ca(NOs)2.4H2O 

.686 

57 

.03  S         aHzO         0.412 

77 

•74 

" 

0 

57- 

98 

M 

.596 

57 

.91    Ca2N2O7.2H2O   0 

78 

•43 

" 

Cerasine  wax  bottles  were  used  and  more  than  6  months  constant  agitation 
allowed  for  attainment  of  equilibrium  at  25°  and  4-14  days  at  100°. 


SOLUBILITY  OF  CALCIUM  HYDROXIDE  IN  AQUEOUS  SOLUTIONS  OF  CALCIUM 

SULFATE   AT   25°. 
(Cameron  and  Bell,  1906.) 


Gms.  per  100  cc.  Sat.  Sol. 


CaO. 

0.1166 
0.1141 
0.1150 
0.1215 
0.1242 

0.1222 


Solid 
Phase. 


Ca(OH)2 


Gms.  per  100  cc.  Sat.  Sol. 


CaSO4. 
O 

0.0391 
0.0666 
0-0955 
O.I2I4 
0.1588 

The  mixtures  were  constantly  agitated  at  25°  for  two  weeks. 


CaSO4. 

CaO. 

0.1634 

0.0939 

0.1722 

0.0611 

0.1853 

0.0349 

O.IQiS 

0.0176 

o  .  2030 

0.0062 

0.2126 

0 

Solid 
Phase. 

CaS04.2H«0 


SOLUBILITY  OF  CALCIUM  HYDROXIDE  IN  AQUEOUS  SOLUTIONS  OF  POTASSIUM 

CHLORIDE  AND  OF  SODIUM  CHLORIDE. 

(Cabot,  1897.) 


-  In  KC1  Solutions. 


Gms.  of  the 
Chloride 

Gms.  CaO  per  Liter  at: 

per  Liter.    . 

'      o°.                    15°. 

99°. 

O 

1.36               I.3I 

0.635 

30 

I.70I            1.658 

0.788 

60 

1.725            1.674 

0.876 

120 

I.7l8            I.  606 

0.894 

240 

I  .  248            I  .  199 

0.6l7 

320 

...                   ... 

In  NaCl  Solutions. 

Gms.  CaO  per  Liter  at: 


0°. 

15°. 

99°. 

1.36 

1.31 

0-635 

1.813 

1-703 

0.969 

1.824 

I  .004 

1.86 

1.722 

I.OI5 

i  .37 

1.274 

0.771 

1.054 

0.929 

0.583 

Results  in  harmony  with  the  above  for  the  solubility  of  calcium  hydroxide 
in  aqueous  solutions  of  potassium  chloride  at  50°,  are  given  by  Kernot,  d'Agostino 
and  Pellegrino  (1908). 


CALCIUM  HYDROXIDE 


204 


SOLUBILITY  OF  LIME  IN  AQUEOUS  SOLUTIONS  OF  SODIUM  CHLORIDE  ALONE  AND 

CONTAINING   SODIUM   HYDROXIDE. 
(Maigret,  1905.) 


Gms.  CaO  per  Liter  of  Solution. 

tier  liter    Without    o-89.NsOH    4 .09  .NaOH 
'    NaOH.      per  Liter.        per  Liter. 

0.22 


o-SS 


0 

•3 

0.8 

5 

•4 

0.9 

10 

.6 

I.O 

25 

•7 

i.i 

5° 

.8 

1-25 

75      , 

•9 

1.4 

100 

.85 

1.4 

c   Naa  Gms.  CaO  per  Liter  of  Solution. 

per  Liter  Without     o.8g.NaOH    4-oo.NaOH 

'  NaOH.  per  Liter.        per  Liter. 

150  1.65  1.25     0-44 

175  1.6  1.2 

182  1.6  1.2 

225  1.4  i.o 

250  1.3  0.9 

300  I.I  0-7      0.22 


SOLUBILITY    OF    CALCIUM    HYDROXIDE    IN    AQUEOUS    SOLUTIONS  OF 
SODIUM   HYDROXIDE. 


(d'Anselme  —  Bull.  soc.  chim.  [3]  29,  938,  '03.) 


Concentration  of  NaOH: 


Normality. 

Gms.  per  Liter 

0 

O 

N/ioo 

0-4 

N/25 

1.6 

N/i5 

2.66 

N/8 

S-oo 

N/5 

8.00 

N/2 

20-00 

Grams  CaO  per  Liter  Sat.  Solution  at: 


20°. 

50°. 

70°. 

100°. 

I.I70 
0-94 

0.880 
0.65 

0-75 

o-53 

0-54 

o-3S 

o-57 

o-3S 

0.225 

0.14 

o-39 
0.18 

0.20 
O-o6 

o.n 

0.04 

0.05 
o.oi 

o.n 

0-02 

O-OI 

trace 

0.02 

trace 

o.oo 

o.oo 

For  results  upon  mixtures  of  calcium  hydroxide  and  alkali  carbonates 
and  hydroxides,  see  Bodlander  —  Z.  angew.  Chem.  18,  1138,  '05. 


SOLUBILITY  OF, CALCIUM  HYDROXIDE  IN  AQUEOUS  SOLUTIONS  OF 
GLYCEROL  AT  25°. 


(Herz  andKnoch  —  Z.  anorg.  Chem.  46,  193,  '05;  for  older  determinations,  see  Berthelot  —  Ann.  chim 
phys.  [3]  46,  176;  and  Carles  —  Arch.  Pnarm.  [3]  4,  558,  '74.) 

Density  of 
Solutions 

Wt.  per  cent 
Glycerine 
in  Solution. 

Millimols 
*Ca(OH)2per 
i  oocc.  Solution. 

Gms.  per  100  cc.  Solution. 

Ca(OH)2 

-       CaO.  " 

.0003 

o.o 

4-3 

0.1593 

0.1206 

.0244 

7-15 

8-13 

0.3013 

0.2281 

•0537 

20-44 

14.9 

0.5522 

0.4180 

.0842 

31-55 

22.5 

0.8339 

0.6313 

•H37 

40.95 

40.1 

1.486 

1.125 

•J356 

48.7 

44.0 

1.631 

1.234 

.2072 

69.2 

95-8 

3-550 

2.687 

Data  tor  the  solubility  of  calcium  hydroxide  in  aqueous  solutions  of  phenol 
at  25°  are  given  by  van  Meurs  (1916). 


205 


CALCIUM  HYDROXIDE 


SOLUBILITY  OF  CALCIUM  HYDROXIDE  IN  AQUEOUS  SOLUTIONS  OF  GLYCEROL 
AND  OF  CANE  SUGAR  AT  25°. 

(Cameron  and  Patten,  1911.) 

In  order  to  obviate  the  uncertainties  due  to  the  presence  of  a  large  excess  of 
the  solid  phase  in  contact  with  the  solutions,  the  clear  liquids,  saturated  at  o°, 
were  decanted  from  the  solid  and  slowly  brought  to  25°  and  constantly  agitated 
at  this  temperature,  until  equilibrium  with  the  finely  divided  solid  phase,  which 
separates  at  the  higher  temperature,  was  reached. 


Results  for  Glycerol  Solutions.                      Results  for  Sugar  Solutions. 

da  of    Gms.  per  TOO  Gms.  Sat.  Sol.     Solid              d*  of      Gms.  per  100  Gms.  Sat.  Sol.         Solid 

Sat.  Sol.  "~ 

Ca(OH)2. 

CsH5(OH)3.        Pnase-           bat.bol. 

Ca(OH)2.      CwHaOu 

Phase. 

0 

-983 

0 

.117 

0 

Ca(OH)« 

0 

.188 

0 

.62 

Ca(OH)j  +  Sugar 

I 

.008 

O 

.178 

3 

.50 

.021 

0 

•730 

4 

.82 

" 

0 

•413 

15-59 

•037 

I 

•355 

7 

•50 

" 

I 

.042 

O 

.48 

17 

.84 

.067 

3 

.21 

ii 

.90 

« 

I 

.088 

0 

.88 

34 

.32 

.109 

5 

-38 

17 

.42 

" 

I 

.149 

I 

•34 

55 

.04 

.123 

6 

.07 

19 

.86 

" 

SOLUBILITY  OF  CALCIUM  HYDROXIDE  IN  AQUEOUS  SOLUTIONS  OF  CANE  SUGAR 

AT  80°. 

(von  Ginneken,  1911.) 


Gms.  per  100  Gms.  Sat.  Sol. 


CaO. 
O.II7 
0.189 
0.230 


Sugar. 
4.90 
9.90 

14-75 


Solid 
Phase. 

Ca(OH)5 


Gms.  per  100  Gms.  Sat.  Sol. 

CaO.  Sugar. 

0.358  19.50 

0.548  24.60 

I.OI7  29.70 


Solid 
Phase. 

Ca(OH), 


SOLUBILITY  OF  LIME  IN  AQUEOUS  SOLUTIONS  OF  SUGAR. 

(Weisberg  —  Bull.  soc.  chim.  [3]  21,  775,  '99.) 

The  original  results  were  plotted  on  cross-section  paper  and  the 
following  table  constructed  from  the  curves. 

ist  series,  t°  =  i6'-i7°. 


Jms. 

per  100  Gms. 
Solution. 

G.  CaO  per  100 
Gms.  Sugar  in  Sol. 

Sugar.       CaO. 

I 

0.30 

35-o 

2 

0.56 

28.7 

3 

0.85 

28.0 

4 

1.  12 

27.7 

5 

1.40 

27-5 

6 

1.65 

27-5 

8 

2  .22 

27-5 

10 

2.77 

27-5 

12 

3-27 

27-5 

14 

3-85 

27-5 

2d,  series  t°  = 

15°. 

rms.  per  100  Gms. 
Solution. 

G.  CaO  per  100 

Gms.  Sugar  in  Sol. 

Sugar. 

CaO: 

I 

0.50 

62.5 

2 

0-75 

36.0 

3 

I  .02 

32-5 

4 

I  .22 

30.2 

5 

i-45 

28.5 

6 

1.67 

27.7 

8 

2  .22 

27-5 

10 

2.77 

27-5 

12 

3-27 

27-5 

14 

3-85 

27-5 

In  the  second  series  a  very  much  larger  excess  of  lime  was  used  than 
in  the  first  series.  The  author  gives  results  in  a  subsequent  paper,  — 
Bull.  soc.  chim.  [3]  23,  740,  'oo,  — which  show  that  the  solubility  is  also 
affected  by  the  condition  of  the  calcium  compound  used,  i.e.,  whether 
the  oxide,  hydrate,  or  milk  of  lime  is  added  to  the  sugar  solutions. 

A  very  exhaustive  investigation  of  the  factors  which  influence  the  solubility 
of  lime  in  sugar  solutions  is  described  by  Claasen  (1911). 


CALCIUM  IODATE  206 

CALCIUM    IODATE   Ca(IO3)2.6H2O. 

SOLUBILITY  IN  WATER. 

(Myiius  and  Funk  — Ber.  30,  1724.  '97;  W.  Abh.  p.  t.  Reichanstalt  3,  448,  'oo.) 


t  * 

Gms. 

Ca(I03)2 

Mols. 
Ca(I03)2                    Solid 

t  °. 

Gms. 
Ca(I03)2 

Mols. 
Ca(I03)2 

Solid 

I      . 

per  100 
Gms.  Sol. 

per  100                     Phase. 
Mols.H2O. 

per  100 
Gms.  Sol. 

per  100                   Phase. 
Mols.  HaO. 

0 

0 

.10 

0 

.0044    Ca(IO3)  .6Hj 

jO         21 

0 

•37 

0 

.016 

Ca(I03)2.H20 

10 

0 

•17 

0 

.0075 

35 

0 

.48 

O 

•  O2I 

it 

18 

O 

•25 

0 

.Oil 

40 

o 

•52 

O 

023 

u 

30 

0 

.42 

O 

.019 

45 

o 

•54 

0 

.024 

it 

40 

0 

.61 

0 

.027 

5° 

0 

•59 

0 

.026 

" 

50 

0 

.89 

0 

.040 

60 

0 

•65 

O 

.029 

" 

54 

I 

.04 

0 

.046 

80 

0 

•79 

O 

•034 

tt 

60 

I 

•36 

O 

.063 

100 

o 

•94 

0 

.042 

tt 

Density  of  solution  saturated  at  18°  =  i.oo. 

CALCIUM    IODIDE   CaI2. 

SOLUBILITY  IN  WATER. 

(Average  curve  from  the  results  of  Kremers  —  Pogg.  Ann.  103,  65,  '58;  Etard —  Ann.  chim.  phys.  [7] 

2,  532,  '94-) 

«.  o       Cms.  CaI2  per  100  f  0      Cms.  CaI2  per  100  .  0      Cms.  CaI2  per  100 

Cms.  Solution.  Cms.  Solution.  Cms.  Solution. 

o  64.6  30  69  80  78 

10  66. o  40  70.8  100  81 

20  67.6  60  74 

Density  of  solution  saturated  at  20°  =  2.125. 

The  fusion-point  curve  (solubility,  see  footnote,  p.  i)  is  given  for  mixtures  of 
calcium  iodide  and  iodine  by  Olivari  (1908). 

CALCIUM  IODO  MERCURATE. 

A  saturated  solution  of  CaI2  and  HgI2  in  water  at  15.9°  was  found  by  Duboin 
(1906)  to  have  the  composition  CaI2.i.3HgI2.i2.3H2O;  d  =  2.89  and  the  solid 
phase  in  contact  with  the  solution  was  CaI2.HgI2.8H2O. 

CALCIUM  PerlODIDE  CaI4 

f  Data  for  the  formation  of  calcium  periodide  in  aqueous  solution  at  25°  are 
given  by  Herz  and  Bulla  (1911).  (See  reference  note  under  calcium  perbromide, 
p.  189.) 

CALCIUM  LACTATE  Ca(C6H10O6).5H2O. 

100  gms.  H2O  dissolve  3.1  gms.  of  the  salt  at  o°,  5.4  gms.  at  15°  and  7.9  gms. 
at  30°.  (Hill  and  Cocking,  1912.) 

CALCIUM  MALATE  CaC4H4O6.H2O. 

SOLUBILITY  OF  CALCIUM  MALATE  IN  WATER  AND  IN  ALCOHOL. 

(Partheil  and  Hubner,  1903.) 

ioo  gms.  H2O  dissolve  0.9214  gm,  CaC4H4O6.H2O  at  18°,  and  0.8552  gm.  at 

100  gms.  95%  alcohol  dissolve  0.0049  gm.  CaC4H4O6.H2O  at  18°,  and  0.00586 
gm.  at  25°. 


207 


CALCIUM  MALATE 


CALCIUM   (Neutral)  MALATE  Ca(C4H4O6).3H2O. 
CALCIUM   (Acid)  MALATE  Ca(C4HBO6)2.6H2O. 
CALCIUM  MALONATEtCa(C3H2O4)4H2O. 

SOLUBILITY  OF  EACH  IN  WATER. 

(I wig  and'Hecht,  1886;  Cantoni  and  Basadonna,  1906;  the  malonate,  Mic^ynski,  1886.) 


Ca.  Neutral  Malate. 

Cms.  CaCCJfcOs)  per  100 


t°. 

6ms. 

Gms. 

cc.  Sol. 

HzO. 

Sol. 

(C  and  B). 

0 

10 

0.85 

0.84 

20 

0.82 

0.81 

0.907 

30 

0.78 

0.77 

0.835 

40 

0.74 

0-73 

0.816 

50 

0.66 

0.65 

0.809 

57 

0-57 

0.56 

60 

0.58 

0.58  . 

0.804 

70 

0.63 

0.63 

0-795 

80 

0.71 

0.70 

0-754 

90 

0.740 

Ca.  Acid  Malate. 

Cms.  Ca(C4H5O5)2  per 
100  Cms. 


Ca.  Malonate. 


Water. 


2 
5-2 

15  ' 
32.24 
26 

II 
6.8 


Solution. 

1.77 
I.48 
1.96 

4-94 

13.09 

24.29 

20.64 

9.91 

6-37 


per  100  Gms.  HjO. 

0.290  (0.374) 
0.330  (0.419 
0.365  (0.460 
0.396  (0.495 
0.422  (0.524 
0.443  (0.544) 

0.460 
0.472 
0.479 


The  results  for  calcium  malonate  given  above  in  parentheses  are  by  Cantoni 
and  Diotalevi  (1905),  but  these  authors  fail  to  state  the  terms  in  which  their 
data  are  reported.  By  comparison  with  other  papers  of  the  series,  it  is  prob- 
able that  in  this  case  the  figures  refer  to  grams  per  100  cc.  saturated  solution. 

CALCIUM  NITRATE  Ca(NO3)2.4H2O. 

SOLUBILITY  IN  WATER. 

(Bassett  and  Taylor,  1912.) 

(Silica  vessels  used.  Constant  agitation  at  constant  temperature  for  two  to  three 
days.  Calcium  determined  by  precipitation  as  oxalate  and  weighing  as  oxide.) 

Gms. 

Ca(NOs)2       Solid 
per  100  Gms.    Phase. 
Sat.  Sol. 

53.55  Ca(N03)2.4HJ0 
54-94 
56.39 
57.98 
60.41 
62.88 
66.21 
68.68 
68.74 

71.7 
70.37 


Gms. 

to         Ca(N03>2 
per  100  Gms. 
.          Sat.  Sol. 

Solid 
Phase. 

—   0.4 

1.4 

Ice 

—    1-4 

4.78 

" 

-    1-9 

6-53 

" 

-   3-05 

IO 

" 

—   4-15 

12.98 

" 

-15-7 

33-13 

" 

-21.7 

38.7 

" 

-28.7 

* 

-26.7 

43-37  C* 

t(NOs)j.4 

—  IO 

47-31 

" 

o 

50.50 

M 

5 

Si-97 

1C 

10 

IS 

20 
25 
30 

35 
40 

42.4 
42.4 
42.7 

42-45 
40 
t  m.  pt. 


Gms. 

to 

Ca(NO3)2          Solid 

. 

per  100  Gms.      Phase. 

Sat.  Sol. 

45 

7L45 

Ca(N03)i.3H,0 

50 

73-79 

" 

Si 

74-73 

« 

49 

77  -4£ 

Ca(NOj)«.2H.O 

5i 

78.05 

" 

£ 

78.16 
78.2 

Ca(NOi)i 

100 

78.43 

" 

125 

78.57 

• 

147. 

5     78.8 

" 

151 

79 

" 

Eutectic. 


SOLUBILITY  OF  THE  UNSTABLE  CALCIUM  NITRATE  TETRAHYDRATE  /3  IN  WATER. 
(Results  supplementary  to  the  above.) 

(Taylor  and  Henderson,  1915.) 
Gms.  Ca(NO3)2 


t°. 

per  100  Gms. 

Sat.  Sol. 

o 

50.17 

22.2 

56.88 

25 

57-9° 

30 

60.  16 

30 

6i.57 

34 

63.66 

35 

62.88 

38 

64.34 

Solid  Phase. 
aCa(N03)j.4H20 


/3Ca(NOa)2.4H2O 


Gms.  Ca(NO..)a 

t8. 

per  zoo  Gms. 

Sat.  Sol. 

38 

66.65        , 

39 

67-93 

39.6  (m.  pt.) 

69.50 

39  (reflex  pt.) 

75-34 

40 

66.22          < 

42  .  7  (m.  pt.) 

69.50 

42.4  (reflex  pt.) 

71.70 

25 

77.30 

Solid  Phase. 
0Ca(NOs)«.4H»O 


Ca(NOi)« 


CALCIUM  NITRATE 


208 


SOLUBILITY  OF  CALCIUM  NITRATE  IN  AQUEOUS  SOLUTIONS  OF  CALCIUM 
THIOSULFATE  AT  9°  AND  AT  25°  AND  VICE  VERSA. 

(Kremann  and  Rodemund,  1914.) 


Results  at  9°. 

Results 

at  25°. 

Gms.  per  ioo  Gms.  Sat.  Sol. 

Gms.  per  ioo  Gms.  Sat.  Sol. 

Solid  Phase. 

'Ca(NOa)«. 

CaS203.  ' 

'Ca(NO3)2. 

CaS2O3. 

46.02 

5.46         Ca(NOs)2.4H:O 

54-03 

4.27 

Ca(N03)2.4HiO 

45-68 

6.  8  1            "  •fCaSiOs.GHzC 

>          50.25 

9-IO 

" 

27.92 

10.46            CaS^.GHzO 

45-92 

13 

"  +CaS2Oa.6HK) 

10.49 

22.  8l 

42-93 

I3-83 

CaSzOs-GHW) 

29-33 

32.01 

17.09 

" 

I9-5I 

23.78 

" 

8.15 

SOLUBILITY  OF  CALCIUM  NITRATE  IN  AQUEOUS  SOLUTIONS  OF  SODIUM 
NITRATE  AT  9°  AND  AT  25°  AND  VICE  VERSA. 

(Kremann  and  Rodemund,  1914.) 


Results  at  9°. 

Gms.  per  100  Gms.  Sat.  Sol. 
Ca(NO3)2. NaNOa. ' 

47.51  9.51 

46.08  12.56 

26.67  23.32 

11.76  34.26 


Solid  Phase. 

Ca(N03)2.4H20 
"  +NaN03 
NaNO« 


Results  at  25' 
Gms.  per  100  Gms.  Sat,  Sol. 


Ca(NO3)2. 

NaNO3." 

54.58 

7-25 

53-22 

10.70 

52-73 

12.08 

52.40 

11.88 

37-31 

19.48 

26.91 

24.98 

I4.6l 

36.12 

Solid  Phase. 
Ca(NOi)2.4H20 

"  +NaNO, 
NaNOi 


These  authors  also  give  the  complete  solubility  relations  of  the  reciprocal 
salt  pairs,  Ca(NO3)2  +  Na^Oj  ±=>  2NaNO3  +  CaS2O3  at  9°  and  25°. 

SOLUBILITY  OF  CALCIUM  NITRATE  IN  AQUEOUS  SOLUTIONS  OF  NITRIC  ACID  AT  25°. 

(Bassett  and  Taylor,  1912.) 

(The  mixtures  were  shaken  intermittently,  by  hand,  during  quite  long  periods; 
one  week  was  allowed  between  duplicate  determinations.) 

Gms.  per  100  Gms.  Gms.  per  100  Gms.  Gms.  per  100  Gms. 

Sat.  Sol.  Solid  Phase.  Sat.  Sol.  Solid  Phase.   _      Sat.  Sol.  Solid  Phase. 

Ca(NOi)i.    HN03.  Ca(NO3)2.  HNO3.  Ca(NO3)2.  HNO3. 

57 . 98   O    Ca(N03)j.4H20  3 2  . 84  32 . 63  Ca(NO3)2.4H2O  9 . 34  65 . 69  Ca(NO3)2.2HjO 

54.82   3.33 

52.96   5.87 

51.58   7.21 

47.82   11.27 

45-59  I3-7I 

40.70  19.65 

38.17  22.80 

34.46  28.81 

Freezing-point  data  for  the  Ternary  System  Ca(NO3)2-r-KNO3  +  NaNOs  are 
given  by  Menzies  and  Dutt,  1911. 

SOLUBILITY  OF  CALCIUM  NITRATE  IN  SEVERAL  ORGANIC  SOLVENTS. 


32.50 

33-52 

" 

8.52 

67.20 

33-44 

35.63 

Ca(NO3)2.3HjO 

5-o6 

71.12        Ca(NOi)2 

29.05 

41.66 

" 

2-53 

74-77 

27-79 

45-70 

" 

1.05 

78.56 

31.09 

40.56 

Ca(NOa)«.2H,0 

0-54 

80.83 

26.07 

45-70 

ft 

0.36 

85-83 

17.41 

55-48 

" 

O.OI 

90.90 

12.25 

62.05 

" 

o 

96.86 

Solvent. 


Gms.  Ca(NO3)j  per  100  Gms. 
N  Sat.  Solution. 


Methyl  Alcohol 
Propyl        " 
i  Butyl       " 
Amyl 
Acetone 
Methyl  Acetate 

25 
25 
25 
25 
25 
18 

65.$ 
36.5 
25 
13-3 
58.5 
4i 

Authority. 
(D'Ans  and  Siegler,  1913.) 


(d  sat .  sol. =1.313)    (Naumann,  1 909.)  j 


209 


CALCIUM  NITRATE 


SOLUBILITY  OF  CALCIUM  NITRATE  IN  AQUEOUS  SOLUTIONS  OF  ETHYL  ALCOHOL 

AT  25°.      (D'Ans  and  Siegler,  1913.) 


Gms.  per  too  Gms.  Sat.  Sol. 


C2HsOH. 

Ca(N03)2. 

O 

57-5 

8.1 

55-2 

14.1 

52-9 

22.3 

50.2 

29.4 

49 

31.2 

52 

29-5 

56.2 

27.8 

60 

26.5 

62.3 

0 

82.5 

5-8 

77 

Solid  Phase. 


Gms.  per  100  Gms.  Sat.  Sol. 


Ca(N03)2.4H20 


"  +Ca(NOi), 
Ca(NOa)j  unstable 


CALCIUM  NITRITE  Ca(NO2)2.4H2O. 

SOLUBILITY  IN  WATER. 


CzHaOH. 

Ca(NO.-)2. 

15-2 

69.52 

20-4 

66.08 

35-9 

57-7 

41.8 

51-4 

27-39 

61.96 

28.5 

61.15 

29.6 

60.3 

60.2 

38.6 

54-6 

41.9 

42.5 

50-97 

35-8 

55-3 

Solid  Phase. 
Ca(NOs)2  unstable 


CaCNOs)*  stable 


Ca(NOs)2.2C2H60H 


(Oswald,  1914.) 


Solid  Phase. 


-    4 

~    9-3 
-12. 5 

-14-5 
-17-5 

^  9-5 

o 

16 


16.7 
25-5 
29-5 
32 

35 
36.2 

38-3 


Ice 


[r       Solid  Phase. 
CaCNO^^HzO 


+Ca(N02)2.4H20 


42 
44 

54 
64 
70 

73 


+Ca(NOJ)J.2H10 


43 

51.8 

53-5 

55-2 

58 

60 

61 

71 
An  aqueous  solution  simultaneously  saturated  with  calcium  nitrite  and  silver 

nitrite,  contains  92.4  gms.  Ca(NO2)2  +  11.2  gms.  AgNO2  per  100  gms.  H2O  at  14°. 

(Oswald,  1914.) 

100  cc.  sat.  solution  of  calcium  nitrite  in  90  %  alcohorcontain  39  gms.  Ca(NO2)2. 
H2O  at  20°. 

100  cc.  sat.  solution  of  calcium  nitrite  in  absolute  alcohol  contain  i.i  gms. 
Ca(NO2)2.H2O  at  20°.  (Vogel,  1903.) 

CALCIUM  OLEATE  (C^O-OCa. 

One  liter  water  dissolves  about  o.  i  gm.  calcium  oleate  at  t°not  stated.  (Fahrion,  1916.) 
100  gms.  glycerol  (of  d  =  1.114)  dissolve  1.18  gms.  calciumoleate  at  t°  not  stated. 

(Asselin,  1873.) 

CALCIUM  OXALATE  Ca(COO)2.H2O. 

SOLUBILITY  IN  WATER,  BY  ELECTROLYTIC  CONDUCTIVITY  METHOD. 

(Holleman,  Kohlrausch,  and  Rose,  1893;    Richards,  McCaffrey,  and  Bisbee,  1901.) 


*o  Gms.  CaC2O4  per 

Liter  of  Solution. 

13        0.0067  (H) 

08.       0.0056  (K  and  R) 

24        0.0080  (H) 


«.<>  Gms.  CaC2O4  per 

Liter  of  Solution. 

25        0.0068  (R,  McC  and  B) 
50        0.0095 
95        0.0140 


SOLUBILITY  OF  CALCIUM  OXALATE  IN  AQUEOUS  SOLUTIONS  OF  ACETIC  ACID  AT 

26°-27°.      (Herz  and  Muhs,  1903.) 


Normality  of 
Acetic  Acid. 

O 

0.58 

2.89 

5-79 


G.  CH3COOH 
per  100  cc.  Sol. 

0-00 


17-34 

34-74 


Residue  from  50.053 
cc.  Solution. 


0.0017 
0.0048 
0-0058 
0.0064 


The  residues  were  dried  at  70°  C. 


CALCIUM  OXALATE  210 

SOLUBILITY  OF  CALCIUM  OXALATE  IN  AQUEOUS  SOLUTIONS  OF  HYDROCHLORIC 

ACID  AT  25°. 

(Henderson  and  Taylor,  1916.) 
NonnaUtyofHCl.       ^S^  Normality  of  HC1. 

o  0.009  0.500  2.638 

0.125  0.717  0.625  3.319 

0.250  1.359  0.750  3.922 

0.375  2.019  I  5.210 

These  authors  also  give  data  showing  the  effect  of  increasing  amounts  of  KC1 
and  KNO3  upon  the  solubility  of  calcium  oxalate  in  0.5  normal  HC1  at  25°,  and 
also  of  the  effect  of  increasing  amounts  of  potassium  trichloracetic  acid  upon  the 
solubility  in  0.5  normal  trichloracetic  acid,  and  of  increasing  amounts  of  potas- 
sium monochloracetic  acid  upon  the  solubility  of  calcium  oxalate  in  0.5  normal 
monochloracetic  acid. 

SOLUBILITY  OF  CALCIUM  OXALATE  IN  AQUEOUS  SOLUTIONS  OF  SODIUM  CHLORIDE 
AND  OF  SODIUM  PHOSPHATE. 

(Gerard,  1901.) 

Salt  in  Aq.       Cms.  Salt         to    Cms.  CaCzOt  Salt  in  Aq.  Cms.  Salt          to      Cms.  CaCzCU 

Solution.         per  Liter..  per  Liter.  Solution.  per  Liter.  per  Liter. 

NaCl           i  25  0.0075  NaCl                25  37  0.0414 

5  25  0.0188  Na2H(P04)2       4.8  15  0.016 

10  25  0.0255                                  4.8  37  0.033 

25  ,25  0.0291 

One  liter  45%  ethyl  alcohol  dissolves  0.000525  gm.  calcium  oxalate,  temp,  not 

Stated.  (Gueiin,  1912.) 


CALCIUM  OXIDE  CaO. 

100  gms.  molten  CaCl2  dissolve  16.2  gm.  CaO  at  about  910°. 

(Arndt  and  Loewenstein,  1909.) 

Data  for  the  systems,  CaO  -f-  MgO  and  for  CaO  +  A12O3  +  MgO  are  given  by 

Rankin  and  Merwin  (1916);    for  CaO  +  A12O3  +  SiO2  by  Rankin  and  Wright 

(1915);   for  CaO  +  Fe2O3  by  Sosman  and  Merwin  (1916);   and  for  CaO  +  MgO 

+  SiO2  by  Bowen  (1914). 

Data  for  the  system  CaO  +  C  +  CaC2  +  CO  are  given  by  Thompson  (1910). 


CALCIUM  PHOSPHATE  (Tribasic)  Ca3(PO4)2. 

SOLUBILITY  IN  WATER. 

The  determinations  of  the  solubility  of  this  salt  in  water,  as  stated  in  the 
literature,  are  found  to  vary  within  rather  wide  limits,  due,  no  doubt,  to  the 
fact  that  so-called  tribasic  calcium  phosphate  is  apparently  a  solid  solution  of 
the  dibasic  salt  and  calcium  oxide,  and  therefore  analyses  of  individual  samples 
may  show  an  excess  of  either  lime  or  phosphoric  acid.  When  placed  in  contact 
with  water,  more  PO4  ions  enter  solution  than  Ca  ions,  the  resulting  solution 
being  acid  in  reaction  and  the  solid  phase  richer  in  lime  than  it  was,  previous  to 
being  added  to  the  water.  For  material  having  a  composition  approximating 
closely  that  represented  by  the  formula  Ca3(PO4)2  the  amount  which  is  dissolved 
by  CO2  free  water  at  the  ordinary  temperature,  as  calculated  from  the  calcium 
determination,  is  o.oi  to  o.io  gram  per  liter,  depending  upon  the  conditions  of 
the  experiment.  Water  saturated  with  CO2  dissolves  0.15  to  0.30  gram  per 
liter. 

A  list  of  references  to  papers  on  this  subject  is  given  by  Cameron  and  Hurst  — 
J.  Am.  Chem.  Soc.,  26,  903, 1904;  see  also  Cameron  and  Bell,  Ibid.,  27,  1512, 1905. 


211 


CALCIUM  PHOSPHATE 


CALCIUM    PHOSPHATE    (Dibasic)    CaHPO4.2HaO. 
SOLUBILITY  IN  WATER. 

(Cameron  and  Seidell  —  J.  Am.  Chem.  Soc.  26,  1460,  '04;  see  also  Rindell  —  Compt.  rend.  134,  iza,  'oaj 
Magnanini  —  Gazz.  chim.  ital.  31,  II,  544,  *oi.) 

i  liter  of  CO2  free  water  dissolves  0.136  gram  CaHPO4  at  25°. 

i  liter  of  water  sat.  with  CO2  dissolves  0.561  gram  CaHPO4  at  25°. 

SOLUBILITY  OF  Di  CALCIUM  PHOSPHATE  AND  OP  MONO  CALCIUM  PHOS- 
PHATE IN  AQUEOUS  SOLUTIONS  OF  PHOSPHORIC  ACID  AT  25°. 

(Cameron  and  Seidell  —  J.  Am.  Chem.  Soc.  27,  1508,  '05;  Causse  —  Compt.  rend.  114,  414,  '92.) 


Grams  per  Liter  of 
Solution. 

Gms.  per  Liter 
Calc.  from  CaO  Found. 

PaO5  per  Liter 
in  Excess  of              e  rj  t>v. 
that  combined             Sohd  Phase- 

CaO. 

P205. 

with  Ca. 

I  .71 

4.69 

4-J5 

CaHP04 

2-53 

CaHP04.2ILO 

"•57 

36.14 

28.05 

" 

21.5 

u 

23  -31 

75-95 

56-53 

tt 

46-45 

ft 

39.81 

139.6 

97-Qi 

" 

89.0 

tt 

49.76 

191.0 

120.7 

tt 

128.0 

tf 

59-40 

234.6 

144.1 

u 

159-4 

tt 

70-31 

279.7 

170.6 

tt 

190.7 

tt 

77.00 

317.0 

(  174.2 
(321.3 

CaHPO,  or 
CaH4(P04)2 

226.0 

122.2 

CaHPO4.2H 
CaH4(PO  )r! 

.0+ 

E^O 

72.30 

35J-9 

301.6 

CaH4(P04)2 

169.0 

CaH4(P04)2.: 

Hp 

69-33 

361.1 

289-3 

a 

186.1 

M 

59  98 

419.7 

250.2 

tt 

267.9 

tl 

53-59 

45J-7 

223-7 

ft 

316.1 

tt 

44-52 

505-8 

185.8 

tt 

393-1 

ft 

39-89 

538.3 

166.4 

tt 

437-4 

tt 

Density  of  the  solution  in  contact  with  both  salts  at  25°  =  1.29. 

SOLUBILITY  OF  CALCIUM  PHOSPHATES  IN  AQUEOUS  SOLUTIONS  OF  PHOSPHORIC 
ACID  AT  DIFFERENT  TEMPERATURES. 

(Bassett,  Jr.,  1908,  1917.) 

Results  at  25°.  Results  at  40°.  Results  at  50.7°. 


Gms.  per  100 
Gms.  Sat.  Sol.      Solid  Phase. 

Gms.  per  100 
Gms.  Sat.  Sol. 

Solid  Phase. 

Gms.  F 
Gms.  S 

S-  too 
.  Sol. 

Solid  Phase. 

CaO. 

P206. 

CaO. 

P2O5. 

CaO. 

p2o6: 

3.088 

36.11  CaHiPjjOs.HiO 

1.768 

42.42 

CaH*P208.H20 

0.336 

62.01 

CaH*P208+ 

4.908 

28.34 

3.584 

36.79 

" 

CaHiPjOg-aO 

5.809 

24.20 

+CaHPO* 

5-755 

27.25 

"  +CaHPO* 

0.635 

58.08 

CaH*PjO».H2O 

5.523 

22.90Ca 

HPO* 

4.813 

21.67 

CaHPO* 

1.428 

50.25 

" 

4-499 

17.55 

3.810 

16.35 

2.974 

41.92 

" 

2.638 

9.100 

2.536 

9-905 

4.880 

33.18 

•« 

1.878 

6.049 

1.847 

6.979 

5.725 

29.61 

"  +CaHPO* 

0.826 

2.387 

1.267 

4.397 

3.507 

15.48 

CaHPO* 

0.165 

0.417  (  '  CaHPO*. 

0.576 

1.819 

2.328 

9.465 

» 

0.07 

0.166  1         2H2O 

0.156 

0.426 

" 

I.563 

6.157 

» 

O.o6 

0.140 

0.0592 

0.158 

" 

0.692 

2.281 

" 

0.05 

0.118            " 

0.0508 

0.128 

Ca3P208.HjO 

0.0596 

0.1527 

CaHPO*.aHjO 

0.04 

0.093 

0.0098 

0.0262 

" 

0.0514 

0.1331 

CaaPjOs-HjO 

0.03 

0.070!              . 

0.0709 

trace 

Ca*P209.4H20 

0.0351 

0.0942 

" 

0.02 

0.047  f  r  'TXPO^'TT  r\ 

1  0.0814 

" 

" 

0.0106 

0.0309 

" 

O.OI 

0.023J     a          4'2    2 

0.0840 

" 

" 

0.0007 

0.0007 

" 

In  the  case  of  most  of  the  solutions  7-15  weeks  constant  agitation  was  allowed 
for  attainment  of  equilibrium.  For  the  last  seven  results  at  25°,  18  months 
were  required.  Cerasine  bottles  were  used  in  these  cases.  The  solid  phases 
were  determined  by  analysis.  The  quintuple  points  were  found  by  dilatometer 
experiments  at  36°,  21°  and  152°.  (See  next  page.) 


CALCIUM  PHOSPHATES  212 

SOLUBILITY  OF  CALCIUM  PHOSPHATES  IN  AQUEOUS  SOLUTIONS  OF  PHOSPHORIC 
ACID  AT  TEMPERATURES  ABOVE  100°. 

(Bassett,  Jr.,  1908.) 
Cms.  per  100  Cms  Sat.  Sol. 
*°  -Caa  -  '  -  PloT-  SohdPhase, 

100  2.503  53-71  CaH4P208+CaH4P208.H20 

1  15  b.  pt.  5  .  623  43  .  60  CaH4P208.H20+CaHP04 

132         "  4-327  53-43  CaH4P208+CaH4P208.H20 

169        "  4-489  63.95  CaH*P208 

The  quintuple  points  for  the  system  determined  by  dilatometer  experiments 
are  as  follows: 

5.60  53    ;  CaH4P208+CaH4P208H20+CaHP04 


152 
21 
36 


5.81 
0.0514 


23.5 
0.14 


CaH4P2Os.H20+CaHP04+CaHP04.2H20 
CaHPO4+CaHP04.2H2O+Ca3P2Os.H2O 


Salt  in  Aq.  Solvent. 


Gms.  Salt 


For  additional  data  on  the  solubility  of  calcium  phosphates  in  water,  see 
Cameron  and  Bell,  1905  and  1910. 

Data  for  the  four  component  system,  lime,  phosphoric  acid,  sulfuric  acid  and 
water,  the  essential  constituents  of  "superphosphates,"  are  given  by  Cameron 
and  Bell  (1906). 

One  liter  of  aqueous  0.005  n  potassium  bitartrate  solution  sat.  with  calcium 
phosphate,  contains  0.08  gm.  Ca  and  0.181  gm.  HaPO4  at  25°.  (Magnanini,  1901.) 

SOLUBILITY  OF  CALCIUM  PHOSPHATE  IN  AQUEOUS  SALT  SOLUTIONS  UNDER  2 
ATMOSPHERES  PRESSURE  OF  CO2  AT  14°. 

(Ehlert  and  Hempel,  1912.) 

Gm 

Salt  in  Aq.  Solution. 

Solventi 

70.95      1.777 

cone. 
K2SO4  74-5 

cone. 
NaCl  50 

"  cone. 

NaNOs  72.7 

Cone. 
Na2SO4.ioH2O  137.7 

conc- 


per 
Gms. 


Water 

NH4C1 

45-74 

a 

cone. 

(NH4)2S04 

56.5 

« 

cone. 

MgCl2.6H2O 

86.9 

11 

cone. 

MgS04.7H20 

105.3 

u 

cone. 

MgCl2.KC1.6H2O 

79.2 

(i 

cone. 

MgSO4.K2SO4.MgCl2.6H2O 


2.491 
4.904 

4.765 
1.321 
0.641 

1.583 
0.864 
2.491 
3-227 


Gms.  Salt 

per  ioo 
Gms.  HaO. 

0.228 

I-37I 
1.293 

2.413 

5-885 

1.287 

2.892 

1.9728 

3.6001 

1-577 
I.I54 

Data  for  the  solubility  of  calcium  phosphate  in  aqueous  saturated  solutions  of 
carbon  dioxide  containing  ammonia  are  given  by  Foster  and  Neville,  1910. 

CALCIUM  PELARGONATE   (Nonate)   Ca[CH3(CH2)7  COO]2.H2O. 

CALCIUM  PROPIONATE   Ca(CH3.CH2COO)2.H2O. 
SOLUBILITY  OF  EACH  IN  WATER. 

(Lumsden,  1902;  Krasnicki,  1887.) 

Calcium  Pelargonate. 

Gms. 

t".  Ca[CH3(CH2)7COOla 

per  ioo  Gms.  H-iO. 


0 
20 
40 
00 
80 

90 
ioo 


O.l6 
0.  14 
0.13 
0.12 
0.15 

0.18 
0.26 


Calcium  Propionate. 

Gms.  Ca(CH3.CH2COO)2  per  ioo  Gms. 

Water. 
42.8O 

39-85 
38.45 
38.25 
39.85 
42.15 
48.44 

Solution. 
29.97 
28.48 
27.76 
27.67 
28.48 
29.66 
32.63 

213  CALCIUM  SALICTLATE 

CALCIUM  SALICYLATE  Ca(C6H4.OHCOO)2.3H2O. 

100  grams  of  the  saturated  aqueous  solution  contain  2.29  grams  of  the  an- 
hydrous salt  at  15°  find  35.75  grams  at  IOO°.  (Tarugi  and  Checchi,  1901.) 

CALCIUM     SELENATE    CaScO4. 

SOLUBILITY  IN  WATER 

(Etard  —  Ann.  chim.  phys.  [7]  2,  532,  '94.) 
t°.  -i°.          +5°.  20°.  37*.  67°. 

Gms.  per  ioo  gms.  sol.  7.4        7.3        7.6        6.8        5.1 

The  accuracy  of  these  results  appears  questionable. 

CALCIUM    SILICATE    CaSiO3. 
SOLUBILITY  IN  WATER  AND  IN  AQUEOUS    SUGAR  SOLUTIONS  AT  17°. 

(Weisberg  —  Bull.  soc.  chim.  [3]  15,  1097,  '96.) 

The  sample  of  calcium  silicate  was  air  dried. 

Grams  per  ioo  cc.  Saturated  Solution. 

Solvent.  At^i?0.  After  Boiling  and  Filtering  Hot. 

CaO(det-)      '  CaSiO3(calc.)  CaO(det.)         CaSiOs(calc.) 

Water  0.0046        0.0095 

i o%  sugar  sol.  0.0065        0.0135  0.0094        0.0195 

20%  sugar  sol.  0-0076        0-0157  0-0120        0-0249 

FREEZING-POINT  DATA  (Solubility,  see  footnote,  p.  i)  ARE  GIVEN  FOR  THE 
FOLLOWING  MIXTURES  OF  CALCIUM  SILICATE  AND  OTHER  COMPOUNDS. 

CaSiOs  +  CaS  (Lebedew,  1911.) 

-j-  CaTiOs  (Smolensky,  1911-12.) 

-j-  Li2Sip3  (Wallace,  1909.) 

+  MgSiO3  (Allen  and  White,  1911;  Ginsberg,  1906.) 

+  MnSiO3  (Ginsberg,  1908,  1909.) 

+  Na2SiO3  (Wallace,  1909;  Kultascheff,  1903.) 

CALCIUM  SUCCINATE  Ca(C2H202)2. 

CALCIUM  (Iso)  SUCCINATE  CaCH3.CHC2O4.H2O. 

SOLUBILITY  OF  EACH  IN  WATER. 

(Miczynski,  1886.) 

Calcium  Succinate.  Calcium  Iso  Succinate. 

Gms.  w                        Gms.  Gms.  Gms. 

to          Ca(C2H202)s               to       Ca(C2H2Oi)2  t»       Ca(CjH«Oi)i  t»  Ca(C2H2O2)j 

per  ioo  Gms.                  '     per  ioo  Gms.  '     per  ioo  Gms.  per  ioo  Gms. 

H20.                                     HzO.  H.O.  H£>. 

o   1.127     50   1.029      o   0.522     50   0.440 

10    1.220       60    0.894       10    0.524       60     0.396 
2O    1.276       70    0.770       2O    0.517       7O     0.342 

40       1.177  80      0.657  4°      °-475  8°        0.279 

ioo  cc.  H2O  dissolve  1.424  gms.  CaC4H4O4.H2O  at  18°  and  1.436  gms.  at  25° 

(Partheil  and  Hubner,  1903.) 

ioo  gms.  H2O  dissolve  1.28  gms.  CaC4H4O4  at  15°  and  0.66  gms.  at  100°. 

(Tarugi  and  Checchi,  1901.) 

Results  for  calcium  succinate  in  water,  varying  considerably  from  the  above  and 
indicating  an  increase  of  solubility  with  temperature,  are  given  by  Cantoni  and 
Diotalevi  (1905)  but  the  terms  used  for  expressing  the  results  are  not  stated. 

ioo  cc.  95%  alcohol  dissolve  0.00136  gm.  CaC4H4O4.H2O  at  18°  and  0.00136  gm. 
at  25°.  (Parheil  and  Hubner,  1903.) 


CALCIUM  SULFATB  214 

CALCIUM  SULFATE  CaSO4.2H20. 

SOLUBILITY  IN  WATER. 

(Hulett  and  Allen,  1902;  for  references  to  other  determinations  see  Hulett  and  Allen,  also  Euler,  1904. 
For  data  by  the  electrolytic  conductivity  method,  see  Holleman,  Kohlrausch  and  Rose,  1893,  1908.) 


Gms.  CaSO* 
t°.      per  100  cc. 

Solution. 

Millimols 
per  Liter. 

Density  of 
Solutions. 

Gms.  CaSO4 
t°.         per  loo  cc. 
Solution. 

Millimols 
per  Liter. 

Density  of 
Solutions 

O 

o, 

1759 

12 

.926 

I.OOI97 

40 

o. 

2097 

15 

•413 

0.99439 

10 

o, 

,1928 

14 

.177 

I.OOI73 

55 

o. 

2009 

14 

.765 

0.98796 

18 

0. 

,2016 

14 

.817 

I  .  OOO59 

65-3 

0. 

1932 

14 

.2OO 

0.98256 

25 

0. 

,2080 

15 

.235 

0.99911 

75 

o. 

1847 

13 

•575 

0.97772 

30 

o, 

,2090 

15 

.361 

0.99789 

IOO 

o. 

1619 

II 

.900 

35 

o, 

,2096 

15 

•4°S 

0.99612 

107 

II 

•390 

SOLUBILITY  OF  CALCIUM  SULFATE  ANHYDRITE  AND  OF  SOLUBLE  ANHYDRITE 

IN  WATER.      (Melcher,  1910.) 


to  MiUimols  PCr  GmS'LiteSr°4  ***  Solid  Phase' 

loo  11.65  1-586  CaSO4.2H20 

loo  11.4  i  .55  2  Soluble  anhydrite 

100                 4.6  0.626  Anhydrite 

•    156                  3.2  0.436  Soluble  anhydrite 

156                  1.35  0.184  Anhydrite 

218                  °-35  -    0.048  " 
Data'  for  the  solubility.'of  calcium  sulfate  in  sea  water  are  given  by  Manuelli,  1916. 

SOLUBILITY  OF  CALCIUM  SULFATE  IN  .AQUEOUS^SOLUTIONS  OF  AMMONIUM 
ACETATE  AT  25°.    (Harden,  1916.) 

Cms.  CH3COONH4  per  ,  Cms.  CaSO4  per 

loo  Gms.  Solution.  100'  Gms.  Sat.  Solution. 

o  I  0.2085 

2.13  1.005  0.454 

5.34  I.  012  0.752 

10.68  1.024  1.146 

21-37  1-045  1.755 

SOLUBILITY  OP  CALCIUM  SULPHATE  IN  AQUEOUS  SOLUTIONS  OP  HYDRO- 
CHLORIC, NITRIC,  CHLOR  ACETIC,  AND  FORMIC  ACIDS. 

(Banthisch  —  J.  pr.  Chem.  29,  52,  '84;  Lunge  —  J.  Soc.  Chem.  Ind.  4,  32,  '85.) 

In  Hydrochloric.  In  Nitric.    In  Chlor  Acetic.  In  Formic. 


Grams  Acid      Grams  CaSO4  per 
per  TOO  cc.            i°o  cc.  Sol. 

Gms.  CaSO4  per 
loo  cc.  Solution 

Gms.  CaSO4  per 

IOO  CC.  Sol. 

Gms.  CaSO4  per 
loo  cc.  Soi. 

Solution. 

at  25°. 

at 

I026. 

at  25°. 

at  25°. 

at  25°. 

0 

O 

.208 

o, 

,160 

O 

.208 

O.2O8 

0.208 

I 

0 

.72 

I. 

38 

0 

•56 

2 

I 

.02 

a. 

38 

0 

.82 

3 

I 

•25 

3 

20 

I 

•  O2 

4 

I 

•  42 

3.; 

64 

I 

.20 

0.22 

0.24 

6 

I 

•65 

4' 

1  6^ 

I 

.48 

.  .  . 

8 

I 

•74 

. 

I 

.70 

10 

. 

I 

.84 

0.25 

12 

. 

.  . 

, 

.  . 

I 

.08 

.  .  . 

.  .  . 

Data  for  the  solubility  of  mixtures  of  CaSO4(NH4)2  SO4.H2O  +  (NH4)2SO4  and  of 
CaSp4(NH4)2SO4.4H2O  +  CaSO4.2H2O  at  various  temperatures  between  3°  and  100° 
are  given  by  Barre,  1909  and  1911.  Additional  data  for  this  system,  including  re- 
sults for  the  pentacalcium  salt,  (NH4)2Ca6(SO4)6.H2O,  are  given  by  D'Ans,  1909. 


215 


CALCIUM  SULFATE 


SOLUBILITY  OF  CALCIUM  SULFATE  IN  AQUEOUS  SOLUTIONS  OF  AMMONIUM 

SALTS. 


(In  NH4C1  and  NH4NO3,  Cameron  and  Brown  —  J.  Physic.  Chem.  g,  210,  '05  ;  In  (NH4)2SO4  at  25°, 
Sullivan  —  J.  Am.  Chem.  Soc.  27,  529,  '05;  In  (NKO-jSCu  at  50°,  Bell  and  Tabor  —  J.  Physic.  Chem.  10, 

InNH4Cl     InNH4NO3                 In  NH4C1  In  NH4NO3 

at  25°. 

at  25°. 

at  25°. 

at  25°. 

Gms.  Ammo- 
nium Salt 

G.CaSO4 
Dissolved 

G.  CaS04 
Dissolved 

Gms.  Ammo- 
nium Salt 

G.  CaS04 
Dissolved 

G.  CaSO4 
Dissolved 

per  Liter. 

per  Liter. 

per  Liter 

per  Liter. 

per  Liter. 

per  Liter. 

O 

2.08 

2.08 

300 

IO.IO 

10.80 

2O 

5-oo 

3-70 

375 

7-40 

40 

7-00 

5-10 

400 

11.40 

60 

8.00 

6.05 

600 

12.15 

80 

8.50 

7-00 

800 

12  .IO 

IOO 

9-10 

7-65 

1000 

• 

ii.  81 

J5o 

10.30 

8.88 

1400 

10-02 

200 

10.85 

9-85 

sat. 

7-55 

In 

(NH4)2S04at25°. 

In  (NH^SO,  at 

5o°. 

Grams  per  Liter  Sol.         Wt.  of  ioo  CC. 

Grams  per 

Liter  Sol. 

Sp.  Gr. 

(NH^SO 

4.     CaS04. 

Sat.  Sol. 

'(NH4)2S04. 

CaSO4.  '     of  Solutions. 

O 

2.08 

99.91 

0 

2.168 

.  .  . 

0.129 

2.O4 

99.91 

I5-65 

1.609 

1.0026 

0.258 

1.99 

99.92 

30-67 

1-750 

I.OII3 

0.821 

1.81 

99-95 

91  .6 

2.542 

1.0440 

1.643 

1.66 

99.99 

160.4 

3.402 

.0819 

3.287 

1.54 

100.10 

221.6 

4.068 

.II08 

6-575 

1.44 

100.34 

340.6 

5.084 

•1653 

1.46 

100.82 

416.5 

5-354 

.1964 

26.30 

1.62 

101.76 

428.4 

4.632 

.2043 

84.9 

2.33 

105.34 

530.8 

2  .152 

•2437 

169.8 

3-33 

110.32 

566 

1.  08 

1.2508 

339-6 

4-50 

119.15 

566.7 

0 

I.25IO 

SOLUBILITY  OF  CALCIUM  SULFATE  IN  AQUEOUS  SOLUTIONS  OF  CALCIUM  SALTS 


AT  25 


(Cameron  and  Seidell  — J.  Physic.  Chem,  5.  643.  'or,  Seidell  and  Smith  —  Ibid.  8,  493,  '04;  Cameron 
and  Bell  —  J.  Am.  Chem.  Soc.  28,  1220,  '06.) 


In  Calcium 
Chloride. 

Grams  per  Liter  Sol. 

In  Calcium 
Nitrate. 

Gms.  per  Liter  Sol. 

Wt.of 

In  Calcium  Hydroxide  and 

vice  versa. 

Gms.  per  Liter  Sol.                Solid 

"    CaCl2. 

CaS04.  " 

Ca(N03)2. 

CaS04. 

x 

cc.  Sol. 

Ca07~ 

CaS04. 

Phase. 

o.oo 

2 

.06 

o.o 

2.08 

0 

•998 

0 

.0 

2 

.126 

CaS04.2H,0 

7-49 

'z 

.24 

25    - 

1.24 

:z 

.014 

0 

.062 

2 

.030 

« 

II  .96 

I 

.18 

50 

1.20 

z 

.032 

O 

.176 

I 

.918 

a 

25-77 

Z 

.10 

IOO 

I.I3 

z 

.067 

O 

•349 

Z, 

853 

tt 

32-05 

I 

.08 

200 

o-93 

z 

•137 

O 

.61 

z 

.722 

it 

51  .53 

I 

.02 

300 

0.76 

z 

.204 

o 

•939 

I, 

634 

" 

97.02 

0 

.84 

400 

o-57 

i 

.265 

I 

.222 

I. 

588 

1  CaS04.2H2O+ 
!      Ca(OH)3 

192.71 

o 

•47 

500 

0.40 

i 

.328 

I 

.242 

z 

.214 

Ca(OH), 

280.30 

0 

.20 

544 

o-35 

i 

•352 

I 

.150 

0 

.666 

" 

367-85 

0 

•03 

I 

.166 

0 

•  oo 

M 

CALCIUM  SULFATE 


216 


SOLUBILITY  OF  CALCIUM  SULFATE  IN  AQUEOUS  SOLUTIONS  OF  COPPER  SULFATE 


AT  25°. 

(Bell  and  Taber,  1907.) 


Cms,  per  Liter  Sat.  Sol. 


dK  Sat.  Sol. 


Gms.  per  Liter  Sat.  Sol. 


CuS04. 

CaSOi. 

U23  OO.I.  OU1. 

CuSO4. 

CaSOi. 

an  oai.  aoi. 

I.I44               - 

2.068 

1.002 

39-407 

I.7I8 

I.04I 

3-564 

.986 

I.OO5 

49.382 

1.744 

I.05I 

6.048 

•944 

I  .OO7 

58.880 

1.782 

1.061 

7.279 

.858 

1.009 

97-950 

I-93I 

1.098 

14.814 

.760 

1.016 

146.725 

2.048 

1.146 

19.729 

•736 

1.  021 

I96.O2I 

2.076 

1.192 

29-543 

.688 

1.030 

224.916 

2.088 

i.  218 

SOLUBILITY  OF  MIXTURES  OF  CALCIUM  SULFATE  AND  CAESIUM  SULFATE  IN 

WATER. 

(D'Ans,  1908.) 


te. 

25 
60 


Mols.CsjS04.CaS04 

per  1000  Gms. 

Sat.  Sol. 

0.667 
0.607 


Gms.  Cs2SO4.CaS04 

per  1000  Gms. 

Sat.  Sol 

352 
320 


Solid  Phase. 

Dicalcium  Sulfate  +  Gypsum 


SOLUBILITY  OF  CALCIUM  SULFATE  IN  AQUEOUS  SOLUTIONS  OF  MAGNESIUM 
CHLORIDE  AND  OF  MAGNESIUM  NITRATE  AT  25°. 

(Cameron,  Seidell,  and  Smith.) 
In  Magnesium  Chloride.  In  Magnesium  Nitrate. 

Grams  per  Liter  of  Sat.  Solution. 


MgCl2. 

CaS04. 

HzO." 

O 

2.08 

997-9 

8.50 

4.26 

996.5 

I9.I8 

5-69 

994-5 

46.64 

7-59 

989.1 

121.38 

8.62 

972.2 

206.98 

6-57 

949-9 

337 

2.77 

908.7 

441.1 

i-39 

878.6 

warns  per 

L,iter  solution. 

Wt.  of  i  cc. 

Mg(NOs)2. 

CaS04. 

Solution. 

0 

2.08 

0.9981 

25 

5-77 

1.0205 

50 

7.88 

I  .0398 

100 

9.92 

1.0786 

200 

13-34 

1.1498 

300 

14 

I.2I90 

4OO 

14.68 

I.282I 

514 

15.04 

1-3553 

SOLUBILITY  OF  CALCIUM  SULFATE  IN  AQUEOUS  SOLUTIONS  OF  MAGNESIUM 

SULFATE  AT  25°. 

(Cameron  and  Bell,  19063.) 


Grams  per  Lit 

er  Solution.             5 

p.  Gr.  of 
tions  at  f$  °. 

MgSO4. 

CaS04."         Sok 

0 

2.046 

.0032 

3-20 

1.620 

•0055 

6-39 

1.507 

.0090 

10.64 

I.47I 

.OIl8 

21.36 

1.478 

.O226 

42.68 

1-558 

.0419 

64.14 

1.  608 

.0626 

85.67 

1.617 

•0833 

128.28 

1.627 

.1190 

Grams  per  Liter  Solution.            J 

p.  Gr.  of 
itions  at  §f  ° 

MgS04. 

CaS04.        *>« 

149.67 

1-597              1 

•1377 

165.7 

1-549          3 

.1479 

I7I.2 

1.474 

.1537 

198.8 

i  .422 

.1813 

232.1 

1.254 

.2095 

265.6 

1.070 

.2382 

298 

0.860         : 

.2624 

330.6 

0.647        <J 

.2877 

355 

0.501           ,3 

•3023    . 

217 


CALCIUM   SULFATE 


SOLUBILITY  OF  CALCIUM  SULFATE  IN  AQUEOUS  SOLUTIONS  OF   PHOSPHORIC 

ACID  AT  25°. 

(Taber,  1906.) 


Gms.  per  Liter. 

Sp.  Gr.  of 

Gms.  per  Liter. 

Sp.  Gr.  of 

0 

5 

21.4 
46.3 
105-3 

SOLUBILITY  OF 

Grams  HzSO4 
per  Liter  of 
Solution. 

CaS04."          Solutions  at  2f  .                  Pj( 
2.126               0.9991                     145 
3.143                   .002                       205 

3-734             -007                311 
4.456             .016                395 
5.760             .035                494 
7.318             .075 

CALCIUM  SULFATE  IN  AQUEOUS  S 

(Cameron  and  Breazeale,  19 
Results  at  25°. 

)s. 

•I 

j 

..6 

>OLUT 
33.) 

Resu 
Gm 
pe 

CaS04.  '        Solutions  at  §|. 

7.920          1.106 
8.383          1.145 

7.965               I.  221 
6.848               1.280 
5.572               1.344 

IONS  OF  SULFURIC  ACID. 

Its  at  35°.     Results  at  43°. 
s.  CaSO4        Gms.  CaSO4 
r  Liter.             per  Liter. 

Gms.  CaSO4 
per  Liter. 

Wt.  of 
Sol 

I  CC. 

O 

•  00 

2 

.126 

0 

.9991 

grams 

.  .  . 

2 

•145 

O 

.48 

2 

.128 

I 

.0025 

tt 

2 

.209 

2 

•236 

4 

.87 

2 

.144 

I 

.OO26 

(i 

2 

•451 

2 

•456 

8 

.11 

2 

.203 

I 

.0051 

a 

2 

.760 

16 

.22 

2 

.382 

I 

.0098 

n 

3 

.116 

48 

.67 

2 

.727 

I 

.0302 

tt 

3 

•397 

3 

.843 

75 

.00 

2 

.841 

I 

•0435 

tt 

4 

.146 

97 

•35 

2 

•779 

I 

•0756 

(I 

3 

.606 

.  .  . 

146 

•  01 

2 

•571 

t( 

3 

•150 

4 

•139 

194 

•70 

2 

•3*3 

I 

•1134 

ft 

3 

•551 

243 

•35 

I 

.901 

I 

.1418 

tt 

•  •  « 

2 

•959 

292 

.02 

I 

•541 

I 

.1681 

It 

•  •• 

2 

.481 

SOLUBILITY  OF  CALCIUM  SULFATE  IN  AQUEOUS  SOLUTIONS  OF  POTASSIUM 
CHLORIDE,  BROMIDE,  AND  IODIDE  AT  21°. 

(Ditte,  1898.) 

In  KC1  Solutions.  In  KBr  Solutions.  In  KI  Solutions 


Grams  of  the 
Potassium  Salt 
per  Liter. 

Gms.  CaSO4 
per  Liter. 

Gms.  CaSO4 
per  Liter. 

Gms.  CaSO4 
per  Liter. 

0 

2.05 

2.05 

2.05 

10 

3-6 

3-i 

2.8 

20 

4-5 

3-6 

32 

40 

5-8 

4-5 

3-9 

60 

6.6 

5-2 

4-5 

80 

7-2 

5-9 

4-85 

100 

7-5 

6-3 

5-1 

I25 

double  salt 

6-7 

5-45 

150 

... 

7.0 

5-8 

20O 

.  .  . 

7-3 

5-95 

250 

.  «  « 

double  salt 

6.00 

300 

double  salt 

CALCIUM   SULFATE  218 

SOLUBILITY  OF  CALCIUM  SULFATE  IN  AQUEOUS  SOLUTIONS  OF  POTASSIUM 
NITRATE  AND  OF  POTASSIUM  SULFATE  AT  25°. 

(Seidell  and  Smith,  1904;  Cameron  and  Breazeale,  1904.) 

In  Potassium  Nitrate.  In  Potassium  Sulphate. 

Cms.  per  Liter  _,  Cms.  per  Liter 

SohTtion.  Wt.of.icc.  Solution.  Wt.  of  i  cc. 


KNOaT    CaSOi.  fc2SO4.    '    CaSO, 

o.o  2.08  0.9981  o.o  2.08  0.9981 

12.5  3.28  1.0081  4.88  I. 60  1.0036 

25.0  4.08  1.0154  5.09  1.56  1.0038 

50.0  5.26  1.0321  9.85  1.45  1.0075 

ioo. o   6.86    1.0625       19.57   1.49    1.0151 
150    7.91    1.0924       28.35   1.55    1.0229 

200      8.69     I.I224          30.66    1.57     1.0236 

260      syngenite    1.1539  32-47      J-S8* 

*  Solid  phase  syngenite.  Results  for  the  solubility  of  syngenite  in  solutions  of  potassium  sulphate  are 
also  given  in  the  original  paper. 

Data  for  the  solubility  of  syngenite,  K2Ca(SO4)2.H2O,  and  of  potassium  pentacal- 
cium  sulfate,  K2Ca5(SO4)6.H2O,  in  water  at  various  temperatures,  are  given  by 
D'Ans  (1909).  This  author  also  gives  results  for  the  effect  of  the  following  salts 
upon  the  concentration  of  the  boundary  solution  for  gypsum-potassium  syn- 
genite at  25°:  KC1,  KBr,  KI,  KC1O3,  KC1O4,  KNO3,  CH3COOK,  KOH,  K4Fe(CN), 
K3Fe(CN)6,  NaCl,  Nal,  NaNOs,  CH3COONa,  HC1,  HNO3,  H3PO4f  CH3COOH, 
H2SO4,  Ag2SO4  and  cane  sugar. 

Data  for  the  solubility  of  mixtures  of  CaSO4.K2SO4.H2O  +  CaSO4.2H20  and 
CaSO4.K2SO4.H2O  +  K2SO4  in^water  at  temperatures  between  o°  and  99°,  are 
given  by  Barre  (1909,  1911). 

Data  for  mixtures  of  gypsum-rubidium  syngenite  and  of  dicalcium  salt-syn- 
genite,  at  temperatures  between  o°  and  40°,  are  given  by  D'Ans  (1909). 

SOLUBILITY  OF  CALCIUM  SULFATE  IN  AQUEOUS  SOLUTIONS  OF  SODIUM 
CHLORIDE  AT  26°. 

(Cameron,  1901;  also  Orloff,  1902;  Cloez,  1903;  d'Anselme,  1903.) 

Grams  per  ioo  cc.  Solution.          \\rt.  of  i  cc.  Grams  per  ioo  cc.  Solution.        \yt.  of  i  cc. 

'  NaCl.  CaSOT  Solution.  '    NaCl.  CaSOT  Solution. 

O         0.2I2I     0.9998         17.650     0.712     1.1196 

9.115    0.666    1.0644       22.876    0.679    1.1488 

14.399     0.718      1.0981         26.417     0.650     1.1707 
14.834     0.716      I.IOI2         32.049     0.572     1.2034 

SOLUBILITY  OF  MIXTURES  OF  CALCIUM  SULFATE  AND  CALCIUM  CARBONATE  IN 
AQUEOUS  SOLUTIONS  OF  SODIUM  CHLORIDE  AT  23°. 

(Cameron  and  Seidell,  1901  a.) 

Grams  per  Liter  Solution.  Grams  per  Liter  Solution. 

NaCl.  Ca(HC03)2.          CaSCh.  '  NaCl.  Ca(HCO3)2.  CaSO?. 

o  0.060        1.930  79.52          0.060          6.424 

3.63      0.072     2.72O          121.90      0.056      5.272 
11.49      0.089     3.446          I93.8O      0.048      4.786 

39.62          o.ioi        5.156  267.60         0.040         4.462 

Data  for  the  solubility  of  mixtures  of  calcium  sulfate  and  sodium  chloride  at 
o°-09°  are  given  by  Arth  and  Cretien  (1906). 

Data  for  the  equilibrium  CaSO4  +  Na2CQ3  ^  CaCO3  +  Na2S04  at  25°  are 
given  by  Herz  (191  la). 


219  CALCIUM   SULFATB 

SOLUBILITY  OF  MIXTURES  OF  CALCIUM  SULFATE  AND  SILVER  SULFATE  IN 

WATER. 

(Euler,  1904.) 

Per  Liter  of  Solution.  Total  Salt  c     r      t 

i°.  r        Cou  Cms.  Equiv.  per  100  Gms. 

Cms.  Salt.  Sal£  Solution  Solutions. 

'7°igfs°d4     -35 


1:5 

SOLUBILITY  OF  CALCIUM  SULFATE  IN  AQUEOUS  SOLUTIONS  OF  SODIUM 
NITRATE  AND  OF  SODIUM  SULFATE  AT  25°. 

(Seidell,  Smith,  Cameron,  Brea/eale.) 
In  Sodium  Nitrate.  In  Sodium  Sulfate. 

Gms.  per  Liter  Solution.  \yt.  of  T  cc.  Gms.  per  Liter  Solution.  \yt.  of  r  cc. 

'NaNO?.  CaSO4.  '  Solution.  '  Na2SO4.  CaS67  Solution. 

o  2.08  0.9981  2.39  1.65  1.0013 

25  4.25  1.0163  9-54  i-45  1.0076 

50  5.50  1.0340  14.13  1.39  1.0115 

100  7.10  1.0684  24.37  I-47  1.0205 

200  8.79  1.1336  46.15  1.65  1.0391 

300        9.28       1.1916  115.08      2.10      1.0965 

600     7.89    1.3639       146.61    2.23    1.1427 

655  7.24  L3904  257.10  2.65  I.2I2O 

Data  for  the  solubility  of  calcium  sulfate,  sodium  sulfate  glauberite,  sodium 
sulfate  syngenite,  separately  and  mixed,  in  water  at  various  temperatures,  are 
given  by  D'Ans  (1909)  and;'Barre  (1911). 

SOLUBILITY  OF  CALCIUM  SULFATE  IN  AQUEOUS  AND  ALCOHOLIC  MONO- 
POTASSIUM  TARTRATE  SOLUTIONS  AT  20°. 

(Magnanini,  1901.) 

Gms.  CaSO4  Gms.  CaSO< 

•Solvent.  per  100  Gms.  Solvent.  per  100  Gms. 

Solution.  Solution. 

Water  0.2238       10%  alcoholic  N/  200  KHC^Oe        0.0866 

Aq.  N/2oo  KHC^Oe       0.2323       Aq.    N/2oo  KHC2H4O6+s%  tar- 
10%  alcohol  0.0970  taric  acid  0.2566 

10%  ale.  N/4oo  KHC2H406+5% 
tartaric  acid  0.1086 

SOLUBILITY  OF  CALCIUM  SULFATE  IN  AQUEOUS  SUGAR  SOLUTIONS. 

(Stolle,  1900.) 


Per  cent  Concen-                    Gms.  CaSC>4  Dissolved  by  1000  Gms.  of  the  Sugar  Solutions  at: 

Solutions.              30°. 

40°.             50°. 

60°. 

70°. 

80°. 

0 

2.157 

•73° 

1.730 

1.652 

1.710 

10 

2.041 

1.730 

•730 

i-574 

i-574 

1.613 

20 

i.  808 

1.652 

.419 

1.380 

1.419 

1.263 

27 

i-55o 

1.438      M 

.361 

1.283 

1.283 

0.972 

35 

1.263 

1.050 

.088 

1.108 

0.914 

.  .  . 

42 

1.030 

0.777 

0.816 

0.855 

0.729 

49 

.  .  . 

0.564        0.739 

0.564 

0.603 

0.486 

55 

0.486        0.505 

0.486 

0.369 

0.330 

ioogms.glycerolofdi5i.256dissolve5.i7gms.  CaSChat  i5°-i6°.  (Ossendowski,  1907.) 
100  gms.  glycerol  of  d  1.114  dissolve  0.95  gm.  CaSO4  at  ord.  temp.      (Asselin,  1873.) 


CALCIUM   SULFATE  220 

FREEZING-POINT  DATA  (Solubilities,  see  footnote,  p.  i)  ARE  GIVEN  FOR  THE 
FOLLOWING  MIXTURES  OF  CALCIUM  SULFATE  AND  OTHER  SALTS: 

Calcium  Sulfate  +  Lithium  Sulfate  (Mailer,  1910.) 

+  Potassium  Sulfate  (Muller,  1910;  Grahmann,  1913.) 

+  Rubidium  Sulfate  (Muller,  1910.) 

+  Sodium  Sulfate  (Muller,  1910;  Calcagni  and  Mancini,  1910.) 

CALCIUM    SULPHIDE   CaS. 

SOLUBILITY  IN  AQUEOUS  SUGAR  SOLUTIONS. 

(Stolle.) 


Per  cent  Concen- 

trution  of  Sugar     /• 

Grams  CaS  Dissolved  per  Liter  of  the  Sugar  Solutions  at: 

Solutions. 

30°. 

40°. 

50°. 

60°. 

70°. 

80°. 

PC*.' 

0 

i 

.982 

2.123 

I 

•235 

i 

•390 

1.696 

2 

.032 

2.496 

10 

i 

.866 

I.3I6 

I 

.441 

i 

•673 

1.560 

I 

•634 

1-544 

20 

2 

.187 

I  .696 

I 

.802 

i 

•905 

1.879 

I 

.892 

1.930 

27 

2 

.522 

2-097 

2 

•059 

2 

.226 

2.342 

2 

•304 

2-357 

35 

2 

.689 

2.265 

2 

•304 

2 

.406 

2.342 

2 

•857 

2.947 

42 

2 

•342 

2  .136 

2 

.226 

2 

.522 

2-574 

2 

•509 

2.689 

49 

2 

•445 

2.290 

2 

•458 

2 

.638 

2.728 

2 

.8l8 

3-o63 

55 

2 

•509 

2.226 

2 

•340 

2 

.882 

2.766 

2 

.972 

3.616 

CALCIUM   SULFITE   CaSO32H2O. 

SOLUBILITY  IN  WATER  AND  IN  AQUEOUS  SUGAR  SOLUTIONS  AT  18°. 

(Weisberg,  1896.) 

Grams  CaSOa  per  100  cc.  Solution. 

Solvent.  '  At  Too  After  Boiling 

At  l8  '  Solution  2  Hours. 

Water  0.0043  .... 

10  Per  cent  Sugar  o .  0083  o .  0066 

30  Per  cent  Sugar  o .  0080  o .  0069 

RESULTS  AT  HIGHER  TEMPERATURES. 

(Van  der  Linden,  1916.) 

Cms.  CaS03.2H20  per  1000  gms.  Sat.  Solution  at. 


Solvent. 


30°.        40°.        50°.        60°.        70°.        80°.        90°.      b.  pt. 

Water  0.064  0.063   °-°57   0.06  1   0.045  0-031   0.027  o.on 

AqSucroseofi5gms.perioo 


Water+Excess  CaSC>4  0.031    0.029   0.025   0.019   0.012   0.009   0.008   0.006 

0.032   0.022   0.019  0.021   0.017   0.020  0.021 


Aq.  Sucrose,  15  gms.+i-S  gms.  } 

Glucose  per  100  cc.+Excess  >  0.032   0.027   0.022  0.020  0.019  0.019  0.019  0.023 
CaSO4 

CALCIUM  Phenanthrene  SULFONATES. 

SOLUBILITY  IN  WATER. 

(Sandquist,  1912.) 

r«»v.     ,,r.^  Gms.  Anhydrous  Salt 

Compound.  ^  IQQ  g£  ^ 

Calcium-  2-Phenanthrene  Monosulfonate  0.024 

"       -  3-  "  "  -2H20  0.083 

"       -io-  "  "  .2H2O  0.30 


221  CALCIUM  TARTRATE 

CALCIUM  TARTRATE  CaC4H4O6.4H2O. 

SOLUBILITY  IN  WATER. 

(Cantoni  and  Zachoder,  1905.) 

AO     Gms.  CaC«H4O«.4H2O  to      Gms.  CaC^HtOj.^jO          to       Gms.  CaC4H4O8.4HiO 

**          per  ioo  cc.  Sol.  per  ioo  cc.  Sol.  per  ioo  cc.  Sol. 

o  0.0365  30  0.0631  70  0.1430 

10  0.0401  40  0.0875  80  0.1798 

20  0.0475  5°  o.noo  85  0.2190 

25  0.0525  60  0.1262 

ioo  gms.  aq.  Ca.  tartrate  solution  contain  0.0185  gm«  CaC4H4O6.4H2Oat  18°,  and 
0.029489  gm.  at  25°. 

ioo  gms.  95%  alcohol  solution  contain  0.0187  gm.  CaC4H4O6.4H2O  at  18°,  and 
0.02352  gm.  at  25°.  (Partheil  and  Hiibner,  1903.) 

ioo  gms.  aq.  Ca.  tartrate  solution  contain  0.0364  gm.  CaC4H4O6  at  20°. 

ioo  gms.  10%  alcohol  solution  contain  0.0160  gm.  CaC4H4O6  at  20°. 

ioo  gms.  aqueous  5%  tartaric  acid  solution  contain  0.1632  gm.  CaC4H4O6 
at  2O°.  (Magnanini,  1901.) 

SOLUBILITY  OF  CALCIUM  TARTRATE,  CaC4H4O6.4H2O,  IN  AQUEOUS  ACETIC 
ACID  SOLUTIONS  AT  26°-27°. 

(Herz  and  Muhs,  1903;  see  also  Enell,  1899.) 

Normality  of     Gms.  CHsCOOH    Residue  from  Normality  of     Gms.  CHsCOOH  Residue  from 

Acetic  Acid.       per  ioo  cc.  Sol.      50.052  cc.  Sol.  Acetic  Acid.        per  ioo  cc.  Sol.  50.052  cc.  Sol. 

o  o  0.0217  3.80  22.80        0.2042 

0.57        3.42      0.1082         5.70       34.20     0.1844 

1.425     8.55    0.1635      10.09     60.54    0.1160 

2.85        17.10      0.1970         16.505      93.03     0.0337 

The  residue  was  dried  at  70°  C. 

SOLUBILITY  OF  CALCIUM  TARTRATE  IN  AQUEOUS  SOLUTIONS  OF  CALCIUM 
_j         CHLORIDE,  TARTARIC  ACID,  ETC.,  AT  18°. 

(Paul,  1915.) 

(The  determinations  were  made  by  weighing  the  tartrate  remaining  undissolved 
and  calculating  the  amount  dissolved  by  difference.  It  was  found  that  even  a 
small  amount  of  CO2  in  the  water  had  a  distinct  influence  on  the  solubility.  One 
liter  of  pure  CO2  free  water  was  found  to  dissolve  0.380  gm.  CaC4H4O6.4H2O  at 
1 8°  and  one  liter  of  ordinary  distilled  water,  0.410  gm.  at  the  same  temperature.) 

Results  for  Aque-  Results  for  Aqueous  Results  for  Aque-      Results  for  Alcoholic 
ous  Calcium        Dipotassium  Tar-      ous  Tartaric  Tartaric  Acid 


Chloride  Solution. 

'  Gms.  per  Liter. 

trate 

Gms.  per 

Sols. 

Liter. 

Acid  Sols. 

Gms.  per  Liter. 

Sols. 

Gms.  per  Liter. 

CaCU. 

CaQaOe.   kjC4H4O6. 

CaC4H4Oe.   . 
4H20. 

n  TT  n        CaC4H406. 

L4-n.6vJ6*                   TT  f\ 

4rl2U. 

CzHsOH. 

OHeOe. 

CaC4H4O«. 

0.503 

0. 

202 

0.392 

0.166 

i 

0 

.910 

50 

0 

0.263 

1.005 

o. 

179 

•  2 

•139 

0.160 

2 

I 

.162 

(4 

4 

I.I07 

3.518 

0. 

166 

2 

•352 

o.i57 

4 

I 

•5" 

(4 

16 

i.8S 

4.523 

0. 

154 

2 

.614 

0.150 

6 

I 

.776 

80 

O 

0.205 

o. 

154 

4 

•705 

0.223 

8 

I 

.972 

tt 

4 

0.867 

7-538 

0. 

171 

23 

•524 

0.263 

10 

2 

.205 

u 

16 

1.506 

IO.O5 

0. 

177 

47 

.048 

0.305 

12 

2 

.380 

IOO 

o 

0.190 

25.125 

o. 

182 

14 

2 

.514 

u 

4 

0.766 

50.25 

0. 

224 

16 

2 

.643 

14 

16 

1.297 

Data  for  the  effect  of  potassium  chloride  and  of  potassium  acetate  upon  the 
solubility  of  calcium  tartrate  in  aqueous  0.5  normal  acetic  acid  solutions  at  25°, 
and  also  for  the  effect  of  potassium  monochloracetate  upon  the  solubility  of  the 
salt  in  0.5  normal  chloracetic  acid  solutions  at  25°,  are  given  by  Henderson  and 
Taylor  (1916). 


CALCIUM  TARTRATE 


222 


SOLUBILITY  OF  CALCIUM  TARTRATE  IN  AQUEOUS  SOLUTIONS  OF  AMMONIUM, 
POTASSIUM  AND  SODIUM  CHLORIDES  AT  SEVERAL  TEMPERATURES. 

(Cantoni  and  Jolkowsky,  1907.) 

NOTE.  —  (The  authors  refer  in  all  cases  to  their  determination  of  the  amount  of 
decomposition  of  the  tartrate  by  the  aqueous  chloride  solutions.  Constant  agita- 
tion and  temperature  were  maintained.) 


Cms.  Chloride  per 
Liter  Solvent. 

5 
10 

30 
IOO 
2OO 

Cms.  Ca  Tartrate  Dissolved  at 
16°  per  Liter  of  Aq.: 

ta. 

16 

30 

55 
70 

85 

Cms.  Ca  Tartrate  per  Liter  of 
7%  Aqueous: 

NH4C1.           KC1.            NaCl 
0.701      0.643      0.680 

0.861     0.822    0.840 

I.28l       I.lSo       1.305 

1.897     J-753     i  -860 

2.305      2.  110      2.163 

NH4C1.          KC1.           NaCl. 
1.676      1.504      1.637 
2.417      2.031       2.275 
3.712      2.154      3.579 
5.080      2.546      4.148 
6.699      4.264      6.305 

CALCIUM    BITARTRATE     CaH2(C4H4O6)2. 

SOLUBILITY  IN  WATER  AND  IN  AQUEOUS    SOLUTIONS  OP  ACIDS  AND 

OF  SALTS. 

(Warington  —  J.  Chem.  Soc.  28,  946,  '75.) 

In  Hydrochloric  Acid.       In  other  Acids  and  in  Salt  Solutions  at  14°. 

Acid  or  Salt.        GmsAcidorSalt  Gms.CaH2(C4H4O6)a 
per  loo  cc.  Sol.      per  100  cc.  Sol. 

Acetic  Acid 
Tartaric  Acid 
Citric  Acid 
Sulphuric  Acid 
Hydrochloric  Acid 
Nitric  Acid 
Potassium  Acetate 
Potassium  Citrate 


Cone,  of  HC 
Gms.  per 
loo  Gms.  Sol 

1      Gms.  CaH2(C4H4O6)2 
per  100  Gms.  Solvent. 

•       At  22°. 

At  80°. 

O 

O.6OO 

4-027 

0.68 

3-01 

5-35 

2.15 

6.88 

"•35 

4.26 

11.19 

20.23 

8.36 

22.75 

40.93 

16.13 

48.31 

80.12 

0.81 

0.422 

1.03 

0.322 

0.84 

0.546 

0.685 

1.701 

0.504 

1.947 

0.845 

1.969 

1-387 

0.744 

1-397 

0.843 

CALCIUM   THIOSULFATE   CaS2O,.6H2O. 

SOLUBILITY  OF  CALCIUM  THIOSULFATE  IN  AQUEOUS  SOLUTIONS  OF  SODIUM 
THIOSULFATE  AT  9°  AND  25°  AND  VICE  VERSA. 

(Kremann  and  Rodemund,  1914.) 


Results  at  9°. 


Gms.  per  100  Gms.                                                        Gms.  per  100  Gms. 

Sat.  Sol 

Solid  Phase.                          Sat.  Sol. 

NazSzOj. 

CaSzOa.                                                    NazSzOs. 

CaSzO. 

0 

29.4    CaS2O3.6H2O               o 

34-7 

II  .04 

22.64      "                              9.24 

29.69 

25.21 

15  .84      "+Na2S2O3.5H2O  15  .67 

21.41 

31.01 

7.70  Na2S2O3.5H2O            18.34 

25.18 

28.24 

21  .14 

30.19 

20.33 

31.24 

18.43 

35-04 

ii.  61 

Results  at  25°. 


Solid  Phase. 

CaS2O3.6H2O 


Data  are  also  given  for  the  quaternary  systems,  CaS2O3+Na2S2O3+NaNO3 
+H2O  and  CaS203+Ca(NO3)2+NaNO3+ H2O  at  9°  and  25°.  A  triple  salt  of  the 
composition  CaNa^SzOs^NOa.iiHaO  was  obtained. 


223 


CALCIUM  VALERATE 


CALCIUM  VALERATE  Ca[CH3(CH2)3coo]2.H2o. 

CALCIUM  (Iso)  VALERATE    Ca[(CH3)2.CH.CH2.COO]2.3HaO. 
SOLUBILITY  OF  EACH  IN  WATER. 

(Lumsden  —  J.  Chem.  Soc.  81,  355,  '02;  see  also  Furth  —  Monatsh.  Chem.  9,  313,  '88;  Sedlitzky — 

Ibid,  8,  566,  '87.) 


Calcium  Valerate. 

Gms.  CaCCsHoO^a 

40^            per  TOO  Gms.                t  °. 

Water. 

Solution. 

O 

9.82 

8.94 

o 

IO 

9'25 

8-47 

10 

20 

8.80 

8.09 

20 

30 

8.40 

7-75 

30 

40 

8.05 

7-45 

40 

5° 

7-85 

7.28 

45 

57 

7-75 

7.19 

5° 

60 

7.78 

7.22 

60 

70 

7-80 

7.24 

70 

80 

7-95 

7-36 

80 

90 

8.20 

7.58 

90 

100 

8.78 

8.07 

TOO 

Calcium  Iso  Valerate. 

Gms.  Ca(CsH9O2)2 

per  100  Gms. 

bond 
Phase. 

'Water. 

Solution. 

26.05 

2O.66 

(XC.H.O.VaH.O 

22.70 

18.50 

ti 

21.  80 

17.90 

tt 

21.68 

17.82 

" 

22.00 

18.18 

" 

22.35 

18.42 

" 

19-95 

16.63 

GKC.H.O.kH.O 

18.38 

I5-52 

" 

17.40 

14.82 

tt 

16.88 

14.44 

11 

16.65 

14.28 

" 

l6-55 

14.20 

" 

CAMPHENE   Ci0H16. 

Freezing-point  data  (solubility,  see  footnote,  p.  i)  are  given  by  Kurnakov  and 
Efrenov  (1912)  for  mixtures  of  camphene  +  methylmustard  oil,  camphene-f- 
naphthalene  and  camphene  +  phenanthene. 

CAMPHOR  C10H16O  d  and  /. 

APPROXIMATE  SOLUBILITY  OF  d  CAMPHOR  IN  SEVERAL  SOLVENTS  AT  ORDI- 
NARY TEMPERATURE.     (U.  S.  P.,  Squires;  Greenish  and  Smith,  1903.) 

Parts  Camphor 

Solvent.  per  100  Parts  Solvent. 

Solvent. 

o . 08-0 . 14 

100 


Parts  Camphor  per 
100  Parts  Solvent 


Water 

90%  Alcohol 
95%  Alcohol 
Ether 


125 
173 


Carbon  Disulfide    Readily  Soluble 


Chloroform 
Olive  Oil 
Turpentine 
Glacial  Acetic  Acid 
Lanolin 


300-400 

25-33 
66 

200 
12-5  (Klose,ioo7). 

Saturated  solutions  of  d  camphor  and  of  /  camphor  in  turpentine  of  ap  =4.38 
(in  a  10  cm.  tube  at  18°)  were  found  to  have  di&  =  0.9028  and  0.9030  respectively; 
the  <XD  in  a  10  cm.  tube  were  +23.07  and  —16.52  respectively.  (Jones,  1907-08.) 

SOLUBILITY  OF  CAMPHOR  IN  CONCENTRATED  AQUEOUS  HYDROCHLORIC 

ACID.     (Zaharia,  1899.) 

(The  dissolved  camphor  could  not  be  determined  by  evaporating  and  weighing  the 
residue  on  account  of  volatility;  polarimetric  methods  could  not  be  used  on  account 
of  the  interference  of  the  HC1.  The  author,  therefore,  determined  the  densities 
(H2O  at  4°  in  each  case)  of  the  pure  solvent  and  saturated  solution  in  each  case, 
and  assumed  that  the  difference  represented  the  weight  of  camphor  dissolved. 
The  saturated  solutions  were  prepared  by  stirring  the  several  mixtures  with  a  glass 
stirring  rod,  at  intervals,  during  6  hours.) 

Densities  at  o°.  Densities  at  10°.          Densities  at  20°.  Densities  at  40°. 


Solvent.     Sat.  Sol.      Solvent.      Sat.  Sol.      Solvent.     Sat.  Sol.       Solvent.     Sat.  Sol. 

27.2  %HC1 

.145        I  .  143 

.140        I  .  138        I  .  135 

•133 

.125 

.123 

30.6 

.164 

•159 

.158 

•153 

•153 

.148 

.  142 

•138 

33  9 
34.98 

] 

.181 
.187 

.  167 
.158 

•175 
.181 

•163 
.160 

.169 
175 

•159 
.158 

•'57 
.163 

•149 
•153 

35-74 

.IQI 

.  140 

•185 

.148 

.179 

153 

.167 

153 

36.38 

'   3 

•195 

.126 

.189 

•134 

.182 

.140 

.170 

•153 

36.68 

.197 

.Il6 

.190 

.124 

.184 

•134         

CAMPHOR 


224 


RECIPROCAL  SOLUBILITY  OF  CAMPHOR  AND  PHENOL,  DETERMINED  BY  THE 
FREEZING-POINT  METHOD. 

(Wood  and  Scott,  1910.) 

(The  freezing-point  was  determined  in  most  cases  by  measuring  the  rate  of 
cooling  of  the  mixtures  and  ascertaining  the  point  at  which  the  rate  changed.  The 
experiments  were  made  with  very  great  care.) 


Cms.                                                   Cms. 
t"of      Camphor      Solid               f.    f          Camphor 

FinT   GnTMix-  **-•          Breezing.     <££  j~. 
ture.                                                     ture. 

Solid          -     t'of 
Phase.           Freezing. 

Cms. 

Sms.  Mix- 
ture. 

Solid 
Phase. 

174 

5 

IOO 

.0     CjoHwO     -13 

.8 

7i.48C10HM0      -22 

.6 

52 

52 

i.i 

158 

95 

.98 

-26 

•4,  -32 

70.12 

"+i.i  -23 

.6 

44 

90 

" 

140 

92 

•55 

-15 

•9 

69.32 

i.i            —28 

-30.5 

40 

35 

"+C6H60H 

112 

88 

.86 

—  20 

.1 

67.76 

-15 

•  7 

38 

57 

CsHjOH 

80 

82 

.88 

-19 

•3 

66.64 

-3 

34 

So 

" 

50 

7 

79 

•73 

-18 

•  7 

62.21 

+5 

30.31 

29 

5 

76 

.58       "        -18 

.  6  m.  pt. 

16 

.1 

25 

40 

" 

—  O 

i 

73 

.37        "        -20 

.1 

61.51 

25 

20 

31 

» 

~I3 

S 

72 

.24          "            —  20 

55-8o 

36 

.1 

6 

8? 

" 

i 

i  =  CicHieO.CeH 

Data  for  the  above  system  obtained  by  the  method  of  determination  of  the 
temperature  of  disappearance  of  the  last  crystal,  are  given  by  Kremann,  Wischo 
and  Paul  (1915).  The  results  are  not  in  good  agreement  with  the  above.  These 
authors  also  give  similar  determinations  for  the  systems  camphor  -j-resorcinol  and 
camphor +/S  naphthol. 

Data  for  the  systems  camphor  +  phenol  +  water,  camphor  +  n  butyric  acid  -f- 
water,  camphor  +  succinic  acid  nitrile  -f-  water  and  camphor  +  triethylamine  + 
water  are  given  by  Timmermans,  1907. 

Freezing-point  data  (solubilities,  see  footnote,  p.  i)  are  given  for  the  following 
mixtures  of  camphor  and  other  compounds. 


Camphor  +  Borneol 

+  Hydroquinone 

+  Menthol 

-j-  «  Naphthol 

+  0  Naphthol 

+  a  Mononitronaphthalene 

+  Naphthalene 

+  /3  Naphthylamine 

+  Nitric  Acid 

+  Phosphoric  Acid 

+  Pyrocatechol 

+  Pyrogallol 

-j-  Resorcinol 

+  Salol 

-j-  Sulfur  Dioxide 

-j-  a  Trinitrotoluene 

4-  p  Toluidine 

-f-  i?  other  compounds 

BenzolCAMPHOR  Enol  and  keto  forms. 

Solubility  data  have  been  used  by  Dimroth  and  Mason  (1913)  for  determining 
the  transition  of  the  tautomeric  forms  into  each  other.  Results  are  given  for  the 
solubility  of  each  form  in  ether,  acetone,  ethylacetate,  ethyl  alcohol  and  methyl 
alcohol. 

One  liter  benzene  dissolves  256  gms.  enol  benzoylcamphor  at  5°,  by  freezing- 
point  method.  (Sidgwick,  1915.) 


(Vanstone,  1909.) 
(Efremov,  1912,  1913.) 
(Pawlewski,  1913.) 
(Caille,  1909.) 
(Caille,  1909.) 
Gourniaux,  1912.) 


(Zukow  and  Kasatkin,  1909.) 

«(  <C 

(Efremov,  1912,  1913.) 

Gourniaux,  1912.) 

(Caille,  1909;  Efremov,  1912,  1913.) 

(Caille,  1909.) 

(Bellucci  and  Grassi,  1913,  1914.) 

(Giua,  1916.) 

(Efremov,  1915,  1916.) 


225  BromoCAMPHOR 

BromoCAMPHOR  a  Ci0Hi5OBr. 

APPROXIMATE  SOLUBILITY  IN  SEVERAL  ORGANIC  SOLVENTS  AT  ORDINARY  TEMP. 

(U.  S.  P.;  Squires;  Beilstein;  results  in  alcohol  by  Miiller,  1893.) 

<ir,l^A«t          Parts  Bromo  Camphor  Solvent  Parts  Br<>mo  Camphor  per 

Solvent.         per  IOQ  parts  Solvent>  I00  Parts  Solv;nt.  ^ 

Alcohol          12.  i  at  15°        Ether  50 

"  19.7  "  25°        Chloroform  143 

130.0  "  50°        Olive  Oil  12.5 

"  705.0"  61°        95%  Formic  Acid  13.6  (Aschan,  1913.) 

Freezing-point  data  (solubility,  see  footnote,  p.  i)  are  given  for  mixtures  of  /bromo- 

camphor  +  d  chlorocamphor  by  Padoa  (1904)  ;  for  mixtures  of  d  bromocamphor  + 

/  bromocamphor  by  Padoa  and  Rotondi  (1912);  for  mixtures  of  bromocamphor  -j- 

stearine  by  Batelli  and  Martinetti  (1885);  /3  bromocamphor  +  salol  by  Caille,  1909. 

CAMPHOROXIME   Ci0H16  :  NOH  d  and  /. 

100  gms.  turpentine  dissolve  8.68  gms.  d  oxime  at  18°,  dn  =  0.8784,  ap  =  2.30 
in  10  cm.  tube. 

100  gms.  turpentine  dissolve  8.69  gms.  /  oxime  at  18°,  du  =  0.8782,  an  =  18.24 
in  10  cm.  tube. 

aD  of  the  turpentine  =  4.38  in  a  10  cm.  tube  at  18°. 

In  the  case  of  results  in  /  amyl  bromide  the  d^  =  1.199  in  both  cases  and  the 
OD  was  —3.55  (10  cm.  tube)  for  the  d  oxime  and  +  11.48  for  the  /  oxime.  The  etj> 
of  the  amyl  bromide  was  +4.6  in  10  cm.  tube  at  18°.  The  results  show  that  the 
solubility  and  rotatory  power  of  the  d  and  /  isomerides  are  identical  in  an  optically 
active  as  well  as  in  an  inactive  solvent. 

Freezing-point  data  are  given  for  mixtures  of  d  and  /  camphoroxime  by  Beck 
(1904)  and  Adriani  (1900). 

CAMPHORIC  ACID   C8H14(COOH)2. 

loo  gms.  of  water  dissolve  0.8  gm.  C8Hi4(COOH)2  at  25°,  and  10  gms.  at  the  b.  pt. 

(U.S.P.) 
SOLUBILITY  OF  CAMPHORIC  ACID  IN  AQUEOUS  SOLUTIONS  OF  ALCOHOL  AT  25°. 

(Seidell,  1908,  1910.) 


Wt.  %  C2H5OH         <fes  of         Gms.  C8Hi4(COOH)2    Wt.  %  CzIfcOH  <fe  of        Gms.  CeHu  (COOH)a 

in  Solvent.          Sat.  Sol.     per  100  Gms.  Sat.  Sol.       in  Solvent.  Sat.  Sol.     per  100  Gms.  Sat.  Sol. 

o  i  0.754  6o  i  45 

10  i  i.  60  70  i    ,  49 

20  i  6.30  80  0.995  51.20 

30  i  14  90  0.980  51.40 

40  i  26  96.3  0.970  50.37 

50  i  31  100  0.960  50.10 

SOLUBILITY  OF  CAMPHORIC  ACID  IN  SEVERAL  SOLVENTS. 

Gms.  d&  of  Gms. 


Solvent.  t°.        Sat.  C8Hu(COOH)2  per      Solvent.  t°.  Sat.  C8H14(COOH)2per 

Sol.    100  Gms.  Solvent.  Sol.  too  Gms.  Solvent. 

Amyl  Alcohol(iso)  25      0.907       50(3)         Carbon  Bisulfide  25  1.258      0.020(3) 

Butyl  Alcohol(iso)22.5     ...         54.1(1)      Chloroform  25       ...         0.153(3) 

Ethyl  Alcohol          o         ...         84.7(1)      Cumene  25  0.890      0.197(3) 

15.1     ...       112(2)         Ether  (abs.)  25  0.922     91.40(3) 

62.5     ...       147(2)         95%  Formic  Acid  18.5  ...         8.68(4) 

Methyl  Alcohol     o  ...       116.3(1)      Ligroin  25  0.714      0.007(3) 

22.5     ...       131.1(1)      Nitrobenzene  25  1.2          0.5(3) 

Propyl  Alcohol      o  ...         42.2(1)      Spts.  Turpentine  25  0.852       1.74(3) 

22.5     ...         61     (i)     Toluene  25  0.862      0.15(3) 

Benzene  25      0.873        0.008(3)  Xylene  25  0.859      0.23(3). 

(i)  Timofeiew  (1914);  (2)  Beilstein;  (3)  Seidell  (1910);  (4)  Aschan,  (1913). 

Data  for  the  distribution  of  camphoric  acid  between  water  and  ether  at  25°  are 
given  by  Chandler  (1908).  Data  for  the  freezing  points  of  mixtures  of  d  and  / 
camphoric  acid  and  d  and  /  isocamphoric  acid  are  given  by  Centnerszwer  (1899). 

CAMPHORIC  ANHYDRIDE   C10HuO3  d  and  /. 

One  liter  of  benzene  dissolves  37.5  gms.  d  camphoric  anhydride  at  5°,  deter- 
mined by  depression  of  the  freezing-point.  (Sidgwick,  1915.) 


CANTHARIDINE  226 

APPROXIMATE  SOLUBILITY  IN  SEVERAL  SOLVENTS  AT  ROOM  TEMP. 

(Self  and  Greenish,  1907.) 

Cms.  Cantharidine  Cms.  Cantharidine 
Solvent.                 per  100  Cms.                       Solvent.  per  100  Gms. 

Solvent.  Solvent. 

Aq.  25%  Acetone    0.02        Aq.  10%  Acetic  Acid         0.14 
"     50%       "          °-10          "    45%  Formic   "  0.12 

"     75%        "          °-45        Carbon  Tetrachloride         0.04 

Lanolin  4.4  (Kiose,  1907.) 

CAOUTCHOUC. 

SOLUBILITY  IN  ORGANIC  SOLVENTS.    (Hanausek,  1887.) 

Gms.  Caoutchouc  Dissolved  per  100  Gms.  Solvent. 

Solvent.  / *—m ; N 

Ceara.  Tete  Noire.        Sierra  Leone. 

Ether  2.5  3.6  4.5 

Turpentine  4.5  5  4.6 

Chloroform  3  3.7  3 

Petroleum  1.5  4.5  4 

Benzene  4.4  5  4.7 

Carbon  Bisulfide  0.4  o  o 

SOLUBILITY  OF  CAOUTCHOUC  IN  MIXTURES  OF  BENZENE  AND  ALCOHOL.  (Caspari,  1915.) 
(Freshly  prepared  solutions  of  deresinified  caoutchouc  in  benzene  were  titrated 
with  alcohol  to  appearance  of  two  phases.  The  end  point  is  sharp  to  within  one 
drop  of  precipitant,  especially  at  low  cones,  of  caoutchouc.  For  purposes  of 
converting  the  weights  of  caoutchouc  to  volume,  the  factor  0.91  may  be  taken.) 

Results  at  20°. 


Gms. 
Caoutchouc. 

cc.  CVHe. 

cc.  Abs.        Gms. 
C2HsOH.  Caoutchouc 

cc.  CeHe. 

cc.  9i< 

70            Gms.        rr  -„       cc.92<? 
a.     Caoutchouc.  cc          5>    CzHsOI 

0.032 

40 

17 

0.206 

40 

II 

o, 

,80 

40 

9.6 

0.080 

40 

15 

8 

0.81 

40 

IO 

.8 

2 

,OI 

40 

8.8 

0.405 

40 

14, 

,8 

2.01 

40 

10 

.2 

O 

.20 

40 

8.1 

2.404 

40 

14 

•5 

3.22 

40 

9 

.8 

4.061 

40 

13 

,8 

Results  at  40°.  Results  at  60°. 

Gms.  Caoutchouc,  cc.  C«H«.    cc.  Abs.  CzHsOH.  Gms.  Caoutchouc,    cc.  CeHe.    cc.  Abs.  CjHsOH, 

0.2  40  18.8  0.2  40  N2i.6 

i.o  40  18.1  i  40  23.3 

2  40  17.4  2  40  24.4 

SOLUBILITY  OF  CAOUTCHOUC  IN  MIXTURES  OF  BENZENE  AND  ACETONE.  (Caspari,  1915.) 
Results  at  20°.  ;  Results  at  40°.  Results  at  60°. 

Gms.  r-  TT  ~  cc.  Gms.  ^  TT  cc.  Gms.  r  TT  cc. 

Caoutchouc.    <*•  UH*'    (CHs^CO.  Caoutchouc.  cc'  UH(>-    (CH3)2CO.  Caoutchouc.  cc     6H6'    (CH3)2CO. 

o.n       20          i$-7      o.io      20          19.6      o  10       20          23 

0.80       20  15.0      0.98       20  17.6       i.oi       20  26.4 

1.86       20          14-7 
CARBAMIDES. 

SOLUBILITY  IN  SEVERAL  SOLVENTS.    (Walker  and  Wood.  1898.) 

as  Methyl  phenyl  carbamide  (m.  pt.  82°),  benzyl  carbamide  (m.  pt.  149°). 
o  tolyl  carbamide  (m.  pt.  185°)  and  p  tolyl  carbamide  (m.  pt.  173°). 

Gms.  Each  Carbamide  Separately  per  100  cc.  Sat.  Solution. 

Solvent.  t°.    / * v 

as  Methyl  Phenyl.          Benzyl.  p  Tolyl.  o  Tolyl 

Water  45  74  1.71  0.307          0.251 

Acetone         23  29.4  3-io  2.66  0.462 

Ether  22.5         2.28  °-°53          0.062          0.0162 

Benzene         44-2         12.4  0.0597         °-°43          °-OI5S 

100  gms.  chloroform  dissolve  0.6-0.7  gm-  diiododithio  carbamide  (CSN-jH^Iz 
at  temp,  not  stated.  (Werner,  1912.) 


227  CARBAZOLE 

CARBAZOLE    (Diphenylene  imide)    (C6H4)2NH. 

100  grams  abs.  alcohol  dissolve  0.92  gm.  (C6H4)2NH  at  14°,  and  3.88  gms.  at 
b.  pt. 

loo  gms.  toluene  dissolve  0.55  gm.  (C6H4)2NH  at  16.5°,  and  5.46  gms.  at  b.  pt. 

Freezing-point  data  are  given  for  mixtures  of  carbazole  and  phenanthene  by 
Garelli  (1894). 

CARBINOL  CH3OH,  see  Methyl  alcohol,  p.  435. 

Trimethyl  CARBINOL  (CH3)3COH,  Triphenyl  CARBINOL  (C6H5)3COH. 

Freezing-point  data  (solubilities,  see  footnote,  p.  i)  are  given  for  mixtures  of 
trimethyl  carbinol  and  water  by  Paterno  and  Mieli  (1907).  Results  for  tri- 
methyl carbinol  +  phenol,  trimethyl  carbinol  +  thymol  and  trimethyl  carbinol  + 
bromotoluene  are  given j^by  Paterno  and  Ampola  (1897).  Results  for  triphenyl 
carbinol  +  phenol  are  given  by  Yamamoto  (1908). 

CARBON  DIOXIDE   CO2. 

SOLUBILITY  IN  WATER. 

(Bohr,  1899;  Geffcken,  1904;  Just,  1901.) 
Solubility  in  Water. IlNaCl%  ^NaCl^ 

*°*    ' ~       ~^ft~       ~T^  V  ft. ' 

o        0.335        I-7I3          •••  1-234  0.678 

5        0.277        1.424          ...  1.024  0.577 

10        0.231        1.194          •••  0.875  0.503 

15        0.197        1.019        1.070  0.755  0.442 

20        0.169        0.878          ...  0.664  0.393 

25 —   0.145        0.759        0.826  0.583  0.352 

30        0.126        0.665          ...  0.517  0.319 

40        0-097        °-S3°          •••  0.414  0.263 

50        0.076        0.436          ...  0.370  0.235 

60        0.058        0.359          ...  0.305  0.183 

q  •=  wt.  of  gas  dissolved  by  i  oo  grams  of  solvent  at  a  total  pressure  of  760  mm. 

ft  =  the  Bunsen  Absorption  Coefficient  which  signifies  the  volume  (v)  of 

the  gas  (reduced  to  o°  and  760  mm.)  taken  up  by  unit  volume  (V)  of  the  liquid 

when  the  pressure  of  the  gas  itself  minus  the  vapor  tension  of  the  solvent  is 

760  mm.  _  v 

*  ~  V(i  +  0.00367  /) ' 

/  =  the  Ostwald  Solubility  Expression  which  represents  the  ratio  of  the 
volume  (v)  of  gas  absorbed  at  any  pressure  and  temperature,  to  the  volume 

(V)  of  the   absorbing  liquid,  i.e.  I  =  —-      This  expression  differs  from  the 

Bunsen  Absorption  Coefficient,  ft,  in  that  the  volume  (v)  of  the  dissolved  gas 
is  not  reduced  to  o°  and  760  mm.  The  solubility  /  is  therefore  the  volume 
of  gas  dissolved  by  unit  volume  of  the  solvent  at  the  temperature  of  the 
experiment.  The  two  expressions  are  related  thus: 


0.00367  /),      ft  = 


,     A 
(i  +  0.00367  0 

SOLUBILITY  IN  WATER  AT  PRESSURES  ABOVE  ONE  ATMOSPHERE. 

(Wroblewski  —  Compt.  rend.  94,  1335,  '82.) 

pressure     Coefficient  of  Saturation*  at:  .Pressure    Coefficient  of  Saturation  *  at  : 

in  Atmos-      ,  -  -  —  —  •  -  -  —  >  m  Atmos-    .  -  -  -  •  - 

Dheres.  °  •  I2-4  •  pheres.  0°-  12.4°. 

i  1-797  i.  086  20  26.65  17.11 
5  8.65  5.15  25  30.55  20.31 
10  16.03  9-65  3°  33-74  23.25 

*  Coefficient  of  absorption  is  no  doubt  intended. 


CARBON  DIOXIDE 


228 


SOLUBILITY  OF  CARBON  DIOXIDE  IN  WATER  AT  HIGH  PRESSURES.  (Sander,  1911-12.) 

NOTE.  —  The  pressures  varied  from  25  to  170  kilograms  per  square  centimeter. 
The  results  are  expressed  in  terms  of  the  volume  of  CC>2,  reduced  to  I  kg.  per  sq. 
centimeter,  dissolved  by  unit  volume  of  liquid  at  the  temperature  and  pressure 
of  the  experiment.  A  Caillet  apparatus,  provided  with  the  well-known  Caillet 
tube,  was  used.  The  experiments  were  made  with  very  great  care.  In  general, 
the  procedure  consisted  in  compressing  CO2  above  mercury  in  the  closed  milli- 
meter graduated  end  of  the  Caillet  tube  and  taking  many  readings  on  the  scale 
at  various  pressures  and  temperatures.  The  volumes  thus  found  were  compared 
with  similar  readings  made  after  a  known  amount  of  solvent  had  been  introduced 
above  the  layer  of  mercury,  by  means  of  a  graduated  pipet  with  turned-up  end. 
The  differences  show  the  volume  of  CO2  dissolved  at  given  temperatures  and 
pressures. 

Two  series  of  determinations  were  made.  In  the  case  of  the  results  marked  (a) 
the  used  volume  of  water  was  0.210  cc.  and  for  those  marked  (6)  the  volume  was 
0.102  cc.  The  volumes  of  CO2  used,  varied  from  60  to  76  cc. 


20 


35 

a 


60 

tt 


SOLUBILITY  OF  CARBON  DIOXIDE  IN  WATER  EXPRESSED  IN  TERMS  OF  THE  FAHR- 
ENHEIT SCALE  OF  TEMPERATURE  AND  POUNDS  PER  SQUARE  INCH  PRESSURE. 

(Heath,  1915;  Anthony,  1916,  see  also  Riley,  1911.) 

(The  existing  data  were  calculated  to  this  form,  particularly  for  use  in  the 
bottling  industry.) 

Volumes  of  CCfe  Gas  Dissolved  by  One  Volume  of  Water  at: 


Pressure  in 
Kg.  per 
Sq.  Cm. 

cc.  of  COa  (Reduced  to 
i  Kg.  per  Sq.  Cm.)  Dis- 
solved by    i  cc.  HzO. 

r. 

Pressure  m 
Kg.  per 
Sq.  Cm. 

,     Cc.  CO2  (Reduced  to  i  Kg. 
per  Sq.  Cm.)  Dissolved 
by  i  cc-  H2O. 

(a) 

(ft) 

(a) 

(6) 

25 

.  .  . 

17.77 

60 

90 

22.74 

21.  l6 

30 

.  .  . 

19.77 

u 

100 

26.22 

27.85 

40 

... 

21  .52 

It 

110 

28.92 

28.79 

50 

.  .  . 

28.09 

tl 

120 

30.20 

33-90 

55 

.  .  . 

29-75 

100 

00 

8.97 

.  .  . 

30 

11.77 

13-57 

tt 

70 

IO.II 

6.40 

40 

14.82 

20 

n 

80 

11.05 

9-59 

5o 

18.96 

24.64 

tt 

90 

12.62 

10.85 

00 

22  .90 

22  .50 

a 

100 

I3-63 

12.40 

70 

27.18 

27.62 

it 

no 

14.88 

16.31 

80 

.  .  . 

32.85 

tt 

120 

16.40 

15-78 

40 

10.88 

9.80 

tt 

130 

17-93 

16.89 

50 

12.24 

I3-72 

tt 

I4O 

19.56 

17.71 

60 

14.46 

15.28 

tt 

150 

20.58 

17.49 

70 

16.80 

17.46 

tt 

160 

22.07 

80 

19.74 

22.67 

tt 

170 

22.78 

Inch 

Pressure 

32°. 

36°. 

40°. 

44°. 

48°. 

55°. 

60°. 

65°. 

70°.      75°- 

80°. 

85°.     90°. 

is 

3.46 

3-iQ 

2.93 

2.70 

2tso 

2.  2O 

2.02 

1.86 

I.7I     1.58 

1.84 

4-35    *-27 

20 

4.04 

3-73 

3.42 

3-15 

2^2 

2-57 

2.36 

2.17 

2            1.84 

1.69 

1.58    1.48 

25 

4.58 

4.27 

3.92 

3.61 

3-35 

2.04 

2.69 

2.48 

2.29     2.IO 

i-93 

1.80    1.70 

30 

5.21 

4.81 

4.41 

4.06 

3-77 

3.31 

3.03 

2.80 

2.58     2.37 

2.18 

2.03    1.91 

35 

5.80 

5-35 

4.91 

4-52 

4.19 

3-69 

3-37 

3-11 

2.86    2.63 

2.42 

2.26    2.13 

40 

6.37 

5-89 

5-39 

4.97 

4.61 

4.05 

3.71 

342 

3.15  2.89 

2.67 

2-49    2.34 

45 

6.95 

6.43 

5.88 

5-43 

5.03 

4-43 

4.06 

3-74 

3-44   3-i6 

2.91 

2.72    2.56 

5° 

7-53 

6-95 

6.36 

5-89 

5-45 

4.80 

4.40 

4.05 

3-73   3-42 

7.16 

2.94    2.77 

55 

8.ii 

748 

6.86 

6-34 

5.87 

5.17 

4-74 

4.37 

4.02    3.69 

3-4° 

3.17    2.99 

60 

8.71 

8.02 

7-35 

6.79 

6.  20 

>53 

5.08 

4.68 

4-31    3-95 

3-64 

3-39   3-20 

70 

9.86 

9.09 

8.33 

7.70 

7-13 

6.27 

5-76 

5-30 

4.89   4.49 

4.14 

3-86    3-63 

80 

1  1.  02 

10.17 

9.3i 

8.6  1 

7.98 

7 

6-43 

5.92 

5.46    5.02 

4.62 

4.31    4.06 

00 

12.  18 

11.25 

10.30 

9-52 

8.82 

7.74 

7.11 

6-54 

6.04    5.55 

5.12 

4-77    4-49 

100 

13-34 

12.33 

11.29 

10.43 

9.66 

8-4 

7.79 

7.18 

6.62    6.08 

<.6o 

5.22    4-91 

SOLUBILITY  OF  CO2  IN 

229                           CARBON  DIOXIDE 

AQUEOUS  SOLUTIONS  OF  ACIDS  AND  SALTS. 

(Geffcken.) 

Aq. 

Gms.  Acid       C02  Dissolved,  /  at: 

Aq. 

Gms.  Salt 

CO2  Dissolved,  /  at: 

Solvent. 

per  Liter. 

15°- 

25°- 

Solvent 

per  Liter. 

15°. 

25°. 

HC1 

18.23          I 

.043 

0.806 

CsCl 

84.17 

I  .OO6 

0 

.781 

" 

36.46         I 

.028 

0.799 

KC1 

37-30 

0.976 

0 

•759 

tt 

72.92          I 

.000 

0-795 

]£C1 

74.60 

0.897 

o 

.700 

HN03 

3I-52          I 

.078 

0.840 

KI 

83.06 

0.992 

0 

•775 

" 

63-05          I 

.086 

0-853 

KI 

166.12 

0.923 

o 

.727 

Cl 

126.10         I 

.100 

0.877 

KBr 

59-55 

0.986 

o 

.768 

H2SO4 

24.52          I 

.018 

0.794 

KBr 

119.11 

0.914 

0 

•713 

tt 

49  .  04       o 

.978 

0.770 

KNO3 

50.59 

1.005 

o 

.784 

t( 

.98.08      o 

.917 

0.730 

KN03 

101.19 

0.946 

o 

•749 

n 

147.11       o 

.870 

0.698 

RbCl 

60.47 

0.989 

0 

.769 

n 

196.15       o 

.828 

0.667 

RbCl 

120.95 

0.921 

o 

.788 

SOLUBILITY  IN 

AQUEOUS  SOLUTIONS  OF  SALTS.     (Mackenzie,  1877.) 

Salt  in 

Gms.  Salt  per 

Density  of 

Absorption  Coefficient  a  at: 

Solution. 

100  Gms.  Solution.        Solution  15".              '     go 

15°. 

22°. 

KC1 

6.05 

i  .021 

0.988 

o-777 

o 

.670 

tt 

8.646 

1-053 

0.918 

0.777 

o 

.649 

" 

11.974 

1.080 

0.864 

0.720 

o 

•597 

tt 

22.506 

1-549 

0.688 

o-57i 

o 

.480 

NaCl 

7.062 

1.038 

0.899 

(6.4°) 

o-735 

it 

12.995 

1.080 

0.633 

(6.4°) 

o.557 

o 

.482 

11 

17.42 

1.123 

0.518 

(6.4°) 

0.431 

0 

•389 

tt 

26.00 

I-I95 

o-347 

(6.4°) 

0.297 

o 

•263 

NH4C1 

6.465 

i  .021 

1.023 

0.825 

o 

.718 

" 

8.723 

1.047 

1.  000 

0.791 

0 

.702 

" 

12.727 

1-053 

0.922 

0.798 

o 

.684 

tt 

24.233 

i  .072 

0.813 

(10°) 

0.738 

0 

.600 

8°. 

16-5°. 

22°. 

30°. 

BaCl2 

7.316 

.068 

0.969 

0.744 

0.680 

0 

.566 

tt 

9-753 

.092 

I  .O2I 

0.645 

0.607 

0 

•543 

tt 

14.030 

•137 

.  .  . 

0.618 

0.524 

o 

.467 

tt 

25-215 

•273 

0-495 

0.618 

0.383 

0 

•315 

SrCl2 

9.511 

.087 

0-779 

0.663 

0 

-508 

tt 

12.325 

•1159 

0-737 

0.586 

0.507 

o 

•539 

n 

17.713 

•173 

0.606 

o-473 

0.444 

0 

•367 

" 

3i-i94 

•343 

0.285 

0.245 

0.247 

o 

.223 

CaCl2 

4-365 

.036 

0.942 

0-759 

0.673 

0 

•596 

tt 

5-739 

I 

.049 

0-855 

0.726 

0.616 

0 

•527 

tt 

8.045 

I 

.068 

0.838 

0.674 

0.581 

0 

.500 

tt 

15-793 

I 

•*39 

0.632 

0.520 

0.471 

0 

.400 

Data  for  the  solubility  of  CO2  in  sea  water  are  given  by  Hamberg  (1885). 

According  to  Fox  (19093.),  analyses  of  sea  water  all  show  an  excess  of  base  over  acid,  that  is,  when  COi 
Is  left  out  of  account.  This  COz  (about  50  cc.  per  liter)  is,  of  course,  in  equilibrium  with  the  excess  of  base, 
which  is  actually  equal  to  about  40  rngs.  OH  per  liter.  The  partial  pressure  of  COz  very  seldom,  if  ever, 
exceeds  6  in  10,000.  For  the  determination  of  the  absorption  coefficient  of  COz  there  are,  consequently, 
four  independent  variables  to  be  considered;  influence  of  alkalinity,  a  chemical  influence  in  addition  to  the 
purely  physical  influences  of  temperature,  pressure  and  salinity.  For  convenience,  the  dissolved  COz  may 
be  considered  as  made  up  of  two  parts,  about  i  %  dependent  upon  physical  influences  alone  and  a  far  larger 
part  dependent  upon  the  alkalinity,  pressure  and  temperature,  but  independent  of  salinity.  Extensive 
experimental  determinations  are  described. 

A  critical  review  of  the  literature  on  the  solubility  of  carbon  dioxide  in  water 
and  in  sea  water  is  given  by  Coste  (1917). 


CARBON  DIOXIDE 


230 


SOLUBILITY  OF  CARBON  DIOXIDE  IN  AQUEOUS  SOLUTIONS  OF  SALTS 

(Setschenow,  1892.) 

(Results  expressed  in  terms  of  cc.  CO2  (at  o°  and  760  mm.)  dissolved 
sat.  solution.) 


Salt. 

Cms. 
Salt  per 

Dis- 
solved 

Salt. 

Cms. 
Salt  per 

Dis- 
solved 

Salt. 

Cms. 
Salt  per 

Dis- 
solved 

Liter. 

C02. 

Liter. 

C02. 

Liter. 

C02. 

NH4C1 

I 

1.005 

LCI 

16.72 

1-035 

NaCl 

12.9 

0.978 

M 

IO 

0.985 

i 

50.15 

0.808 

« 

64 

0.760 

tt 

51.6 

0.941 

t 

125.4 

0.596 

t 

128 

0.580 

tt 

172 

0.819 

i 

250.8 

0.497 

t 

192 

0.466 

tt 

258 

0.770 

i 

501.5 

O.  I2O 

NaBr 

II5.I 

0-775 

NI^NOa 

2.8 

1.013 

MgS04 

26.5 

O.9OI 

1 

460.3 

0.364 

' 

II.  2 

I.OO2 

a 

79-5 

0.669 

( 

690.4 

O.22I 

< 

55 

0.989 

it 

159 

0.441 

NaNOa 

89.3 

0-835 

i 

IOI 

0.962 

n 

3i8 

0.188 

u 

J25 

0.762 

t 

202.  i 

0.9II 

KBr 

83-9 

0.908 

M 

208.4 

0.621 

i 

404-3 

0.807 

" 

167.7 

0.819 

U 

416.8 

0.385 

t 

810.4 

0.612 

u 

25*.  5 

0.748 

ft 

625.2 

0.244 

(NH4)2S04 

72.2 

0.712 

tt 

503.1 

0-579 

NaClO3 

233-3 

0.625 

u 

144.4 

0.575 

KI 

3*9-  1 

0-777 

<l 

349-9 

0.506 

Ba(N03) 

62.7 

0.922 

tt 

478.6 

0.688 

n 

699.8 

0.257 

Ca(N03)2 

41 

0.923 

tt 

957-3 

0.506 

Na2S04 

14.2 

0.950 

Citric  Acid 

12 

1.007 

KSCN 

326 

0.691 

tt 

94.8 

0.620 

49 

0.975 

tt 

489 

0.590 

tt 

284.4 

0.234 

99 

0.950 

it 

978 

0.387 

ZnSO4 

38.3 

0.903 

198 

0.893 

KN03 

58.8 

0-959 

n 

76.7 

0.783 

298 

0.841 

u 

II7-5 

0.890 

tt 

230 

0.474 

595 

0.719 

tt 

235-1 

0.781 

(< 

460 

O.2O9 

Cms.          *    .     Solubility 

Cms. 

Salt  per       Lf   ofCO2,Ost- 
100  cc.        g~V      wald  Ex- 

Salt. 

Salt  per 
too  cc. 

Solution,                pression  l^. 

Solution. 

0.825 

Fe(S04)(NH4)2SO4.6H2O 

9-51 

2.35      1.005      0.791 

a 

10.26 

5.05      1.013      0.754 

it 

22.47 

IO.O2 

.022       0.732 

KC1 

1.84 

17.09 

.045       0.665 

u 

3-05 

2.80 

.Ol8      0.789 

tt 

4-58 

5.81 

.040      O.74I 

ft 

7.46 

8.15 

.054      0.710 

Sucrose 

2.63 

9-97 

.070      0.676 

tt 

5.16 

5-o8 

.019       0.8l5 

tt 

9.68 

10.12 

.041       0.795 

tt 

12.33 

Several  determinations  at  other  temperatures  are  also  given. 
SOLUBILITY  OF  CARBON  DIOXIDE  IN  AQUEOUS  SALT  SOLUTIONS  AT  25°. 

(Findlay  and  Shen,  1912.) 

,    r    Solubility 

<jalf              salt  per      ^.     oiuu2,  use-                    cn  u                        bait  per      ^  f  ofCO2,Ost- 
oalt.  ,^  ^         oat.      mn-\j  v^_  t>ait.  5_        bat.    wai<|  j?x_ 

„  '  pression /2B. 

Water  alone        0.825    Fe(SO4) (NH4)2SO4.6H2O    9.51     1.052    0.641 

NH4C1  2.35     1.005     0-791  10.26     1.057    0.629 

.124    0.460 
.008    0.792 

--.-.,  „  „  -017     0.764 

BaCl2  2.80       .018    0.789  4.58       .026    0.749 

.044    0.701 
.009    0.813 

....  .  „  .018    0.798 

Chloral  Hy-    (    5.08       .019     0.815  9-68       .038    0.767 

drate          }  10.12       .041    0.795  I2-33       -051    0.744 

Data  for  KC1  solutions  at  higher  pressures  are  given  by  Findlay  and  Creighton, 
1910. 

Data  for  the  influence  of  colloids  and  fine  suspensions  upon  the  solubility  of 
carbon  dioxide  in  water  at  25°  and  at  various  pressures  are  given  by  Findlay,  1908; 
Findlay  and  Creighton,  1910,  1911;  Findlay  and  Shen,  1911,  1912;  Findlay  and 
Williams,  1913;  Findlay  and  Howell,  1915. 

The  solubility  of  CO2  increases  slightly  with  increasing  concentrations  of 
Fe(OH)8l  gelatine,  silicic  acid,  aniline  (chem.  combination  occurs),  methyl  orange, 
blood,  serum,  peptone,  protopeptone,  and  commercial  hemoglobin.  The  solu- 
bility diminishes  slightly  with  increasing  concentrations  of  arsenious  sulfide, 
dextrine,  soluble  starch,  glycogen  (?),  egg  albumen  and  serum  albumen.  No 
appreciable  effect  is  produced  by  suspensions  of  charcoal  or  silica. 

^When  the  solubility  is  increased  by  a  given  substance,  the  solubility  curve  falls 
with  increase  of  pressure;  when  it  is  lessened,  the  curve  rises  with  increasing  pres- 
sure. In  the  case  of  starch  and  other  neutral  colloids,  the  solubility  passes  through 
a  minimum  with  increase  of  pressure. 

Data  for  the  influence  of  colloids  and  suspensions  on  the  evolution  of  COj  from 
supersaturated  solutions,  are  given  by  Findlay  and  King,  1913-14. 


231 


CARBON  DIOXIDE 


SOLUBILITY  OF  CARBON  DIOXIDE  IN  AQUEOUS  SALT  SOLUTIONS  AT  15.5°  AND 

760  MM.  PRESSURE. 

(Christoff,  1905.) 

A  gravimetric  method  was  used.  A  stream  of  CO2  was  passed  through  the 
weighed  salt  solution  and,  after  saturation,  the  solution  again  weighed  and  the  dif- 
ference taken  to  represent  absorbed  CO2.  The  loss  of  water  from  the  solution 
was  prevented  by  first  passing  the  CC>2  through  a  series  of  U-tubes  containing  some 
of  the  same  solution.  Constant  temp,  was  not  employed,  but  corrections  of  the 
results  were  made  for  the  slight  variations  in  temp,  which  occurred.  Absorption 
flasks  of  special  shape,  graduated  to  hold  75  cc.,  were  used. 


Salt  in  Aq.  Solution. 

Water  Alone 
(NH4)2SO4 


K2A12(S04)4.24H20 

NH4HB2O4 

CuSO4 

LiCl 


KBr 

KC1 

KI 

KNO3 

K2HAsO4 

KH2As3O4 

KH2PO4 

K2HPO4 


Gms.  COiz 

Gms.  CO» 

Cone,  of        Absorbed 

Salt  in  Aq. 

Cone,  of       Absorbed" 

Aq.  Sol.        per  75  cc. 

Solution. 

Aq.  Sol.        per  75  cc. 

Solvent. 

Solvent. 

0.1382 

K.P4012 

i      normal     0.1237 

i        normal  o  .  1093 

KHSO4 

0.66 

O.IO2O 

i 

0.0991 

u 

2. 

O.  IOOO 

i 

o  .  1054 

K2S04 

0.66 

0.1140 

0.25 

0.7672 

" 

i 

0.1002 

2 

0.0751 

Na4B4(>7 

0.025 

0.2205 

I 

0.1087 

" 

o.  125 

0.5317 

0-5 

0.1209 

" 

0.25 

O.85II 

I 

O.  IO2O 

M 

sat.  sol. 

1.8285 

2 

O.O662 

H 

"  -f-crysts.  3.2240 

4 

0.0527 

NaBO2 

0.25  normal  0.8122 

i 

0.1280 

NaCl 

i 

o.  1050 

i 

O.I2I3 

Na3PO4.i2H2O 

i 

0.5828 

i 

O.I2O4 

Na4P2O7.ioH2O 

i 

o  .  8463 

i 

O.I23I 

Na4P4Oi2 

i 

0.0700 

0.5 

O.  IIIO 

ZnSO4 

2 

0.0720 

i 

0.0812 

Sugar 

O.I 

o.  1225 

i 

0.0860 

" 

0-5 

o.  1089 

0.5        '          o.490o(?) 

u 

i 

0.0931 

SOLUBILITY  OF  CARBON  DIOXIDE  IN  AQUEOUS  SOLUTIONS  OF  SULFURIC  ACID. 


Results  at  15.5°. 

Per  cent          Cms.  CO2 
H2SO4        Absorbed  per 
in  Solvent.    75  cc.  Solvent. 

2.5          0.1282 

5           0.1079 
10           0.0833 

20                0.0755 
30                0.0751 

(Christoff, 

Per  cent 
H2S04 
in  Solvent. 

40 

45 
70 
90 

1905.) 

Cms.  CO2 
Absorbed  per 
75  cc.  Solvent. 
0.0713 
0.0725 
0.0918 
0-1433 

Results  at  20°.    (Christoff,  1906.) 


Per  cent 

H2SO4 

in  Solvent. 

o 

35.82 
6l.62 
95.6 
96 


Solubilit 
Ostwald  Expres- 


0.9674 

0.6521 
0.7191 
0.9924 
j8  =  0.926  (Bohr,  1910.) 


SOLUBILITY  OF  CARBON  DIOXIDE  IN  AQUEOUS  SOLUTIONS  OF  CHLORAL  HYDRATE 
AND  OF  GLYCEROL  AT  15°. 

Results  in  terms  of  the  Bunsen  absorption  coefficient  0,  and  also  the  Ostwald 

(von  Hammel,  1915.) 


solubility  expression  /  (see  p.  227). 
In  Aq.  Chloral  Hydrate. 


In  Aq.  Glycerol. 


CC1,.CH(OH)2  per     Abs-Coef., 
100  Gms.  Aq.  Sol.            ft5' 

Solubility,       (CH^CHOH  per  Aba.  Corf., 
100  Gms.  Aq.  Sol. 

Solubility, 

17.7 

0.885 

0-935 

0 

1.008 

I  .064 

31.6 

0.803 

0.848 

26.11 

0-785 

0.829 

38.3 

0.781 

0.825 

43-72 

0.639 

0.675 

49-8 

0.760 

0.802 

62.14 

0.511 

0.540 

57-i 

0.765 

0.808 

77-75 

0.430 

0-454 

68.8 

0.797 

.  0.842 

90.74 

0.404 

0.427 

79-4 

0.903 

0-953 

99.26 

0.410 

0.438 

CARBON  DIOXIDE 


232 


SOLUBILITY  OP  CARBON  DIOXIDE  IN  ALCOHOL. 

(Bohr  —  Wied.  Ann.  Physik.  [4]  IP  247,  'oo) 

In  99  per  cent  Alcohol.  In  98.7  per  cent  Alcohol. 

cc.  COg  (at  o°  and^  760  mm.)  per  i  cc.       cc.  COz  (at  o°  and^?6o  mm.)  per  r  cc. 


b    . 

'Alcohol. 

Sat.  Solution. 

-65 

38.41 

35-93 

—  2O 

7-51 

7.41 

—  10 

5-75 

5-69 

0 

4.44 

4.40 

+  10 

3-57 

3-55 

20 

2.98 

2  .96 

25 

2.76 

2-74 

30 

2-57 

2.56 

40 

2.20 

2.19 

45 

2  .01 

2.00 

Alcohol. 

39  -89 
7-25 
5-43 
4-35 


Sat.  Solution. 

37-22 

7.l6 

5-38 

4-31 


SOLUBILITY  IN  AQUEOUS  ALCOHOL  AT  20°. 

(Muller,  1889;  Lubarsch,  1889.) 


Density  of                  Per  cent        Abs.  Coef.             Density  of 

Per  cent           Abs.  Coef. 

Alcohol.              Alcohol  by  Wt.    of  COz,  a.                Alcohol. 

Alcohol  by  Wt.      of  COz,  a. 

0.998                     1.07        0.861      0.922 

49.O              0.982 

0.969                           22.76            0.841         0.870(18.8 

i°)          7I.I               1.293 

0.960(22.4°)        28.46           0.792         0.835(16°) 

85.3          1-974 

0.956                  3I-I7        0.801      0.795(19°) 

99-7          2.719 

o.935(i70)         42.15        0.877 

SOLUBILITY  IN  AQUEOUS  ALCOHOL 

AT  25°. 

(Findlay  and  Shen,  1911.) 

Results  for  alcohol,                Results  for  alcohol, 

Results  for  alcohol, 

of  df|  =  0.9931                       of  dft  =  0.9929 

of  dft  =  0.9834 

(2.95  gms.  per  100  cc.).         (3.01  gms.  per  100  cc.). 

(8.83  gms.  per  100  cc.). 

Pr««             Solubility  of  COz,           Prpc<              Solubility  of  COz, 
mm   H          OstwaldExpres-           mm  H           Ostwald  Expres- 
sion /25.                                                                   Sion  /2o. 

Pressure      Solubffity  of  COz, 
mmSHge.     °StW^0dntpreS- 

737            0-812                745            0.814 

747          0.786 

836            0.813               937            0.815 

942          0.784 

1073             0.811              1083            0.813 

1090         0.785 

1338            0.811              1357            0.812 

1360         0.788 

These  authors  also  showed  that  the  solubility  of  COz  in  wort  containing  13  gms. 
solids  per  100  cc.  is  less  than  in  water;  also  that  the  solubility  of  CO2  in  beer  is  less 
than  in  aqueous  alcohol  solutions  of  alcohol  content  equal  to  that  of  the  beer. 

SOLUBILITY  OF  CARBON  DIOXIDE  IN  AQUEOUS  SOLUTIONS  OF  NON- 
ELECTROLYTES  AT  20°. 

Results  in  terms  of  the  Bunsen  Absorption  Coefficient  /3,  see  p.  227.    (Usher,  1910.) 


Aqueous  Solu- 
tion of: 

Gm.        , 
Mols.per  d 
Liter. 

20  of  Aq. 

Absorp- 
tion 
Coef.  0. 

Aqueous  Solu- 
tion of: 

Liter. 

20  OI  AQ. 

Absorp- 
tion 
Coef.  0. 

Water  Alone 

0.877 

Resorcinol 

0-5 

.0096 

0.901 

Sucrose 

0.125 

.0152 

0.846 

Catechol 

o-S 

.0107 

0.868 

" 

o.  25 

•0313 

0.815 

Urethan 

0.5 

.0037 

0.869 

« 

0.50 

•0637 

0.756 

Carbamide 

0.5 

.0072 

0.864 

" 

I 

.1281 

0.649 

Thiocarbamide 

.0092 

P-859 

Dextrose 

0.5 

.0328 

0.792 

Antipyrine 

0.5 

•  0134 

0.859 

Mannitol 

0.5 

•0303 

0.782 

Acetamide 

0.5 

.0005 

0.879 

Glycine 

o-S 

.0141 

0.843 

Acetic  Acid 

0.5 

.0026 

0.868 

Pyrogallol 

0-5 

.0172 

0-853 

n  Propyl  Alcohol 

o-S      c 

>-9939 

0.869 

Quinol 

0-5         ^ 

:.oo95 

0.887 

233 


CARBON  DIOXIDE 


SOLUBILITY  OF  CARBON  DIOXIDE  IN  ORGANIC  SOLVENTS  AT  Low  TEM- 
PERATURES AND  PRESSURES.    (Stem,  1912-13.) 

Very  accurate  determinations  with  an  elaborate  apparatus.  The  results  are 
expressed  in  terms  of  K'  =  the  number  of  cc.  of  CO2,  reduced  to  o°,  absorbed  at  the 
indicated  pressure  by  I  gram  of  liquid.  This  number  differs  from  the  Bunsen 
absorption  coefficient  only  by  a  constant  factor  which  is  the  density  d  of  the  liquid. 
Therefore  Bunsen  coef.  /3  =  K'd.  The  results  are  also  expressed  in  terms  of  the 
Ostwald  solubility  expression  /  (see  p.  227). 


-78 


-59 


SOLUBILITY  OF  CARBON  DIOXIDE  IN  ORGANIC  SOLVENTS  AT  HIGH  PRESSURES. 
(See  Note,  p.  228.)  (Sander«  I9"-"-) 


Solvent,  CjHsOH.  Solvent,  CHsOH. 
Pressure      d=  0.872.          d-Jlt  =  0.884- 
mi£:m'       <*J=  0-856.          ij  =  0.866. 

Solvent, 
(CHj)zCO. 
d-ja  =  0.900 

d-£9  =  0.879- 

Solvent, 
CHsCOs.OHs. 
d_p  =  1.017. 
<*-j9  =  0.994 

Solvent. 
CHjCOjCHj. 
d-p=  1.056. 

d-|9=  1.032. 

K1. 

/. 

K1. 

/. 

K'. 

/. 

K'. 

/. 

K'. 

/. 

5° 

107 

194 

120.5 

3" 

196.6 

250.2 

177-5 

304.9 

224.1 

100 

iii.S 

68.4 

195 

119.6 

322 

I98.I 

255-6 

177.1 

315 

224.3 

200 

115-7 

69.5 

202.9 

1  20.  1 

344-5 

201.5 

271.8 

179.2 

337.4 

223.1 

400 

123.8 

71.4 

221.5 

122.2 

400 

208.8 

310.9 

183.2 

389.3 

225.6 

700 

138.6 

74.7 

260 

126.8 

545-5 

IOO 

40.85 

27.27 

63 

42.5 

97-8 

67.2 

85.3 

65.6 

94-3 

75-8 

2OO 

41 

27.16 

64.2 

42.7 

IOI.2 

68 

86.3 

65-3 

98.45 

77.1 

400 

42.35 

27.65 

66.3 

43-i 

106.6 

72.8 

91.6 

66.7 

103.6 

77-6 

700 

44.15 

28.10 

69 

43-35 

II8.8 

72.8 

IOI.5 

69.7 

112.9 

79 

Pres- 
sure in 

perSq 
Cm. 

Cc.  of  COj  (Reduced  to  i  Kg  per  Sq.  Cm.)  Dissolved  at  the  Temp,  and  Pressure  of  Experi- 
ment by  i  cc.  of  Sat.  Solution  in: 

.  ClHjOH     aHrOH    (CjHOzO 
(0.093  cc.)  (0.103  cc.)  (0.131  cc.) 

CHsCOOCzHs     QHs       CeHsCl      OHsBr     OHsNOi 
(0.155  cc.)     (0.08  cc.)  (0.106  cc.)  (0.113  cc.)  (0.164  cc.) 

OHsCHa 
(o.ii4cc.) 

Results  at  20°. 

20 

. 

56.16 

. 

71.16 

62.61 

50.83 

57-12 

57-91 

30 

104.8 

86.62 

188.2 

125-3 

95-22 

82.29 

92.50 

103-3 

40 

149.7 

122.  1 

227.9 

192.4 

137.3 

121.  1 

"5.9 

155-9 

50 

188.8 

174.6 

264.3 

187.5 

1  60 

155-9 

235-8 

Results 

at  35°- 

20 

40 

.  .  . 

48.65 

46.66 

43.38 

44.48 

49-6 

40 

113.1 

98.16 

188.4 

138.3 

101.5 

90-43 

94-39 

118.8 

60 

173 

159-9 

241.3 

219.8 

243-1 

168.3 

.146 

145.1 

192.1 

80 

269.6 

233-9 

227 

Results 

at  60°. 

2O 

24-73 

.  .  . 

34-57 

35.86 

30.58 

31-38 

40 

72.82 

64-65 

140.5 

88.71 

73-69 

62.64 

52.26 

78.67 

60 

122.5 

111.5 

195-4 

186.7 

156.6 

118.1 

98.73 

72-15 

128.1 

80 

167.9 

159.2 

221.4 

223.4 

215 

149-3 

i3J-4 

85-03 

171.9 

IOO 

195-7 

213.9 

248.7 

284.4 

169.7 

210 

Results  at  100°. 

30 

33.65 

30.56 

41.09 

28.68 

40 

26.5 

80.70 

46.52 

48.16 

41.49 

50-36 

49-25 

60 

66.05 

74.51 

IOI 

132 

91.27 

77-24 

72.64 

70.85 

85.98 

80 

III.  2 

107.7 

142.8 

162.3 

155-8 

103 

92.86 

86.86 

II7.6 

IOO 

145-7 

144.7 

175.4 

i9i-5 

212.9 

121.5 

118 

.  .  . 

149 

1  20 

174.6 

175.4 

258.2 

140.7 

140.7 

.  .  . 

I7I.8 

130 

182.6 

146.8 

178.2 

The  figures  in  parentheses  immediately  below  the  formulas  of  the  solvents  in  the 
above  table,  show  the  volumes  of  solvent  used  for  the  series  of  determinations  in 
each  case.  The  volumes  of  CO2  varied  from  about  55  to  77  cc.  in  the  several 
cases.  The  increasing  content  of  COa  in  the  solvents  at  increasing  pressures 
caused  a  considerable  increase  in  volume  of  the  solvent.  This  was  determined 
and  the  proper  calculation  of  the  readings  to  the  saturated  solution  were  made. 
All  necessary  figures  to  show  the  extent  of  the  applicability  of  Henry's  Law  in  the 
present  case,  are  given. 


CARBON  DIOXIDE 


234 


SOLUBILITY  OF  CARBON  DIOXIDE  IN  ORGANIC  SOLVENTS. 

(Just,  1901.) 


The  determinations  are  described  in  great  detail. 
of  the  Ostwald  solubility  expression  /  (see  p.  227). 


Results  are  given  in  terms 


Solvent. 

fc 

*». 

b. 

Solvent. 

b. 

/20- 

/«. 

Water 

0.8256 

Benzene 

2.425 

2.540 

2.710 

Glycerol 

0.0302 

.  .  . 

Amylbromide 

2-455 

2.638 

2.803 

Carbon  Bisulfide 

0.8699  0.8888 

0.9446 

Nitrobenzene 

2.456 

2.655 

2.845 

lodobenzene 

1.301 

I-37I 

1.440 

Propyl  Alcohol 

2.498 

Aniline 

1.324 

1-434 

I-53I 

Carvol 

2.498 

2.69O 

2.914 

o  Toluidine 

1.381 

1-473 

1-539 

Ethyl  Alcohol  (97%) 

2.706 

2.923 

3.J30 

m 

1.436 

1.581 

1.730 

Benzaldehyde 

2.841 

3-057 

3-304 

Eugenol 

1-539 

I-653 

1.762 

Amylchloride 

2.910 

3.127 

3-363 

Benzene  Trichloride 

1.643 

Isobutylchloride 

3-I°5 

3-388 

3-659 

Cumol 

1.782 

1.879 

1.978 

Chloroform 

3-430 

3-681 

3-956 

Carven 

1.802 

1.921 

2.030 

Butyric  Acid 

3-478 

3.767 

4.084 

Dichlorhydrine 

1.810 

1.917 

2.034 

Ethylene  Chloride 

3-525 

3-795 

4.061 

Amyl  Alcohol 

1.831 

1.941 

2.058 

Pyridine 

3-656 

3.862 

4.291 

Bromobenzene 

1.842 

1.964 

2.092 

Methyl  Alcohol 

3-837 

4-205 

4.606 

Isobutyl  Alcohol 

1.849 

1.964 

2.088 

Amylformate 

4.026 

4.329 

4.646 

Benzylchloride 

1.938 

2.072 

2.180 

Propionic  Acid 

4.078 

4407 

4.787 

Metoxylol 

2.090 

2.216 

2.346 

Amyl  Acetate 

4.119 

4.411 

4.850 

E  thylenebromide 

2.157 

2.294 

2.424 

Acetic  Acid  (glacial) 

4.679 

5.129 

5-6i4 

Chlorobenzene 

2.265 

2.420 

2.581 

Isobutyl  Acetate 

4.691 

4.968 

Carbontetrachloride 

2.294 

2.502 

2.603 

Acetic  Anhydride 

5-206 

5.720 

6.218 

Propylenebromide 

2.301 

2.453 

2.586 

Acetone                »> 

6.295 

6.921 

.  .  . 

Toluene 

2-305 

2.426 

2-557 

Methyl  Acetate 

6.494 

SOLUBILITY  OF  CARBON  DIOXIDE  IN  ETHYL  ETHER,  f  RESULTS  IN  TERMS  OF  THE 
OSTWALD  SOLUBILITY  EXPRESSION  /. 

(Christoff,  1912.) 


k  =  7-330. 


/io  =  6.044. 


Data  for  the  solubility  of  carbon  dioxide  in  mixtures  of  acetic  acid  and  carbon 
tetrachloride  and  of  ethylene  chloride  and  carbon  disulfide  are  given  by  Christoff, 
1905. 

Data  for  the  adsorption  of  CO2  by  p  azoxyphenetol  at  temperatures  below  and 
above  its  melting  point,  show  that  no  adsorption  or  solution  occurs  while  the 
material  is  in  the  solid  (unmelted)  condition,  but  after  the  first  melting,  absorp- 
tion takes  place  and  as  soon  as  the  isotropic  liquid  phase  is  reached,  a  second  very 
well-marked  increase  in  absorption  is  observed.  After  this,  expansion  and  de- 
crease of  solubility  proceed  regularly  with  rise  of  temp.  (Homfray,  1910.) 
'The  absorption  coefficient  ft  of  CO2  in  Russian  petroleum  was  found  by 
Gniewosz  and  Walfisz  (1887)  to  be  1.17  at  20°  and  1.31  at  10°. 

Data  for  the  absorption  of  CO2  by  rubber  and  carbon  are  given  by  Reychler 
(1910). 

Data  for  the  absorption  of  CO2  by  hemoglobin  are  given  by  Jolin  (1889). 

Data  for  the  distribution  of  CO2  between  air  and  H2O,  air  and  aq.  H2SO4  and 
air  and  toluene  at  various  temperatures,  are  given  by  Hantzsch  and  Vagt  (1901). 

Data  for  the  freezing-points  of  mixtures  of  CO2  and  methyl-ether  and  for  CO2 
and  methyl  alcohol  are  given  by  Baume  and  Perrot  (1911,  1914). 


235 


CARBON  BISULFIDE 


CARBON  BISULFIDE   CSa. 

SOLUBILITY  IN  WATER. 

(Chancel  and  Parmentier,  1885;  Rex,  1906.) 


Grams  CSz  per  100 


cc. 

[Solution. 


O 

5 

10 

IS 

20 

25 


Cms.  H2O 
(Rex). 

0.258 


0.239 

... 
0.217 


30 

35 
40 

45 
49 


Grams  CS2  per  100 

cc. 
Solution. 

Cms.  H2O 
(Rex). 

O.IS5 

0.195 

0.137 

O.III 

0.070 

0.014 

0.204 
0.199 
0.194 
0.187 
0.179 
0.169 

,100  cc.  H2O  dissolve  0.174  cc.  CS>2  at  22°;  Vol.  of  solution  =  100.208,  Sp.  Gr.  = 
0.9981. 

100  cc.  CS2  dissolve  0.961  cc.  H2O  at  22°;  Vol.  of  solution  =  100.961,  Sp.  Gr.  = 
1.253.  (Herz,  1898.) 

SOLUBILITY  OF  CARBON  DISULFIDE  IN: 


Aq.  Solutions  of  Ethyl  Alcohol  at  17°. 

(Tuchschmidt  and  Folleuins,  1871.) 


Wt.  per  cent 
Alcohol. 

cc.CS, 

per  100  cc. 
Solvent. 

Wt.  per  cent 
Alcohol. 

cc.  CSj 

per  100  cc. 
Solvent. 

t°. 

100 

CO 

91-37 

50 

IO 

98.5 

182 

84.12 

30 

20 

98.15 

132 

76.02 

20 

25 

96-95 

100 

48.40 

2 

30 

93-54 

70 

47.90 

0 

35 

Methyl  Alcohol. 

(Rothmund,  1898.) 
Wt.  per  CS2  in: 


CHiOH 

CSa     ' 

Layer. 

Layer. 

45.1 

98.3 

50.8 

97.2 

54-2 

96.4 

58.4 

95-5 

64 

93-5 

40.5  (crit.  temp.)  80.5 
SOLUBILITY  OF  CARBON  BISULFIDE  IN  ETHYL  ALCOHOL.    (Guthrie,  1884.) 


Gms.  CSz  per  100 
Cms.  CS2+C2H5OH. 

Appearance  on  Cooling  in  Ice  and 
Salt  Mixture. 

94.94 

Remains 

clear 

down  to 

-18.4 

89-54 

Becomes 

turbid  at  —  14  . 

4 

84.89 

it 

"       "    -15- 

9 

79.96 

(t 

tt 

'   -16 

. 

i 

65.11 

tt 

(t 

"   -17 

. 

7 

59.58 

Remains 

clear 

down  to 

—  20 

29.92 

it 

ii 

a      (( 

M 

CARBON 

MONOXIDE  CO. 

SOLUBILITY 

IN  WATER.      (Winkler,'"i9oi.) 

a     < 

'  Absorp. 

/SY'Solu-. 

t  . 

0,  "Absorp. 

0',  "Solu- 

* •              Coef."  ' 

bility." 

<7- 

Coef." 

bility." 

9* 

0 

0. 

03537 

0.03516 

o 

.0044 

40 

0.01775 

0.01647 

0. 

0021 

5 

O. 

03149 

0.03122 

0 

.0039 

50 

0.0l6l5 

O.OI42O 

O. 

0018 

10 

0. 

028l6 

0.02782 

0 

•0035 

60 

0.01488 

O.OII97 

0. 

0015 

15 

0. 

02543 

0.02501 

0 

.0031 

70 

O.OI44O 

o  .  00998 

0. 

0013 

20 

0. 

02319 

0.02266 

0 

.0028 

80 

0.01430 

O.OO702 

0. 

0010 

25 

0. 

02142 

O.O2O76 

o 

.0026 

90 

O.OI42O 

0.00438 

0. 

0006 

30 

o. 

01998 

O.OI9I5 

o 

.0024     100 

O.OI4IO 

O.OOOOO 

O. 

oooo 

0  = 

vol. 

of  CO  absorbed  by 

I 

volume  of  the  liquid  at  a  partial  pressure 

of  7& 

mm.     See  p.  227. 

ft'  =  vol.  of  CO  (reduced  to  o°  and  760  mm.)  absorbed  by  I  volume  of  the  liquid 
under  a  total  pressure  of  760  mm. 

q  =  grams  of  CO  dissolved  by  100  grams  H20  at  a  total  pressure  of  760  mm. 


CARBON  MONOXIDE  236 

SOLUBILITY  OF  CARBON  MONOXIDE  IN  WATER  AND  AQUEOUS  SOLUTIONS. 

The  solubility  in  water,  in  terms  of  the  Ostwald  solubility  expression  (see  p. 
227),  was  found  by  Findlay  and  Creighton  (1911)  to  be  l^,  =  0.0154. 

Data  for  the  solubility  of  CO  in  water  at  high  pressures  are  given  by  Cassuto, 


Data  for  the  solubility  of  CO  in  aq.  NaOH  solutions  are  given  by  Fonda,  1910. 

Results  for  the  solubility  of  CO  in  aq.  H2SO4  at  20°  are  given  in  terms  of  the 
Ostwald  solubility  expression  /  by  Christoff  (1906)  as  follows: 
/25  for  H2O  =  0.02482,    /25  for  35.82%  H2SO4  =  0.0114,    /«  for  61.62%  H2SO4  = 
0.00958,  /25  for  95.6%  H2SO4  =  0.02327  and  0.02164. 

Data  for  the  solubility  of  CO  in  ox  blood  and  ox  serum  at  25°  are  given  by 
Findlay  and  Creighton,  1910-11. 

Data  for  the  influence  of  time  on  the  absorption  of  CO  by  blood  are  given  by 
Grehaut  (1894).  The  author  passed  air  containing  from  one  part  CO  per  1000 
to  one  part  CO  per  60,000,  through  100  cc.  portions  of  blood  and  found  that  the 
maximum  absorption,  18.3  cc.  CO  per  100  cc.  of  blood  (for  the  I  :  1000  mixture) 
occurred  in  three  hours. 

Data  for  the  solubility  of  CO  in  aqueous  hemoglobin  solutions  are  given  by 
Hiifner  (1895)  and  Hiifner  and  Kulz  (1895). 


SOLUBILITY  OF  CARBON  MONOXIDE  IN  AQUEOUS  ALCOHOL  SOLUTIONS 
AT  2O°  AND  760  MM.  PRESSURE. 

(Lubarsch,  1889.) 

Wt.  %                       Vol.  %                         Wt.  %  Vol.  % 

Alcohol.                 Absorbed  CO.                  Alcohol.  Absorbed  CO. 

o                     2.41                  28.57  1.50 

9-09                      1-87                         33.33  1.94 

16.67                       1.75                         50  3.20 

23.08  1.68 


SOLUBILITY  OF  CARBON  MONOXIDE  IN  ORGANIC  SOLVENTS. 

Just,  1901.) 

Results  in  terms  of  the  Ostwald  Solubility  Expression,  see  p.  227. 


Solvent. 

/25. 

fe 

Solvent. 

fe. 

b. 

Water 

o  .  02404 

0.02586 

Toluene 

0.1808 

0.1742 

Aniline 

0.05358 

0.05055 

Ethyl  Alcohol 

o.  1921 

O.I9OI 

Carbon  Bisulfide 

0.08314 

o.  08112 

Chloroform 

O.I9S4 

0.1897 

Nitrobenzene 

0.09366 

0.09105 

Methyl  Alcohol 

O.I95S 

0.1830 

Benzene 

0.1707 

o.  1645 

Amyl  Acetate 

0.2140 

0.2108 

Acetic  Acid 

0.1714 

0.1689 

Acetone 

0.2225 

0.2128 

Amyl  Alcohol 

0.1714 

0.1706 

Isobutyl  Acetate 

0.2365 

0.2314 

Xylene 

0.1781 

0.1744 

Ethyl  Acetate 

0.2516 

0.2419 

100  volumes  of  petroleum  absorb  12.3  vols.  CO  at  20°,  and  13.4  vols.  at  10°. 

(Gniewosz  and  Walfisz,  1887.) 


SOLUBILITY  OF  CARBON  MONOXIDE  IN  ETHYL  ETHER. 

(Christoff,  1912.) 

Results  in  terms  of  the  Ostwald  solubility  expression,  see  p.  227. 
/o  =  0.3618.  /io  =  0.3842. 


237 


CARBON  MONOXIDE 


SOLUBILITY  OF  CARBON  MONOXIDE  IN  MIXTURES  OF  ACETIC  ACID  AND 
OTHER  SOLVENTS  AT  25°. 

(Skirrow,  1902.) 

Results  in  terms  of  the  Ostwald  solubility  expression,  see  p.  227. 


Mixture  of            Wt.  %               rr>                                 Mixture  of 

wt.  % 

f*s\ 

Acetic  Ac.        CHaCOOH            V~'                                 Acetic  Ac. 

CHjCOOH 

,co. 

and:             in  Mixture.                                                     and: 

in  Mixture. 

*». 

Aniline       100            0.173              Chloroform 

56.4 

0.196 

86.5        o.no 

O 

0.206 

"              58.3        0.070             Nitrobenzene 

78.4 

0.156 

"              17.8        0.058 

49 

0.130 

o             0.053 

0 

0.093 

Benzene      67.5        0.199             Toluene 

74-7 

0.191 

33-S        o.I98 

56.9 

0.195 

19.2               0.190 

20.5 

0.190 

o             0.174 

0 

0.182 

V 

SOLUBILITY  OF  CARBON  MONOXIDE  IN  MIXTURES  OF 

ACETONE 

AND 

OTHER  SOLVENTS  AT  25°. 

(Skirrow.) 

Mixture  of  Acetone     ^(M%£°        CO.                 Mixture  of  Acetone 
j                     in  iviiXLurc.            ?                                    __  j. 

By  Wt.              ks' 

%(CH,)2CO 
in  Mixture. 
By  Wt. 

CO. 

In. 

AniHne                 100           0.238          Chloroform 

66.6 

0.226 

79.2        0.179 

26.5 

0.212 

44.9        o.i  10 

O 

O.2O7 

"                           o            0.053          /3  Naphthol 

86 

0.190 

Carbon  Bisulfide   82            o  .  236 

73.1 

0.169 

"                 50.5        0.227          Nitrobenzene 

78.4 

0.207 

26            0.187 

46.8 

0-157 

14.5        0.144 

0 

0.093 

o            0.096          Phenanthrene 

87.2 

0.205 

Naphthalene          86.7        0.199                   " 

75 

0.183 

72.6        0.187 

SOLUBILITY  OF  CARBON  MONOXIDE  IN  MIXTURES  OF 

BENZENE 

AND 

OTHER  SOLVENTS  AT  25°. 

(Skirrow,  1902.) 

The  solubility  of  the  CO  given  in  terms  of  the  Ostwald  expression, 

see  p.  227. 

Mixture  of  Benzene      ^/^^^           CO.                      Mixture  of  Benzene 

%C»H6in 
Mixture. 

CO. 

and:                     ByWt."              fe'                                   and: 

By  Wt. 

k&- 

Naphthalene        100         0.174           Aniline 

87-3 

0.156 

88.5        0.164              " 

71.7 

0.131 

66.2        0.141 

42.6 

0.095 

Phenanthrene      89.5        0.144              " 

21.2 

0.068 

72.6        0.127 

0 

0-053 

a  Naphthol          96  .  5        o  .  149           Nitrobenzene 

71.8 

0.152 

87.9        0.139 

0.127 

j8  Naphthol           97.9        0.158 

0 

0.093 

95  .  6        o  .  149           Ethyl  Alconol 

47-7 

0.181 

0 

0.192 

CARBON  MONOXIDE  238 

SOLUBILITY  OF  CARBON  MONOXIDE  IN  MIXTURES  OF  TOLUENE  AND 
OTHER  SOLVENTS  AT  25°. 

(Skirrow,  1902.) 

Mixture  of  Tol-  CgHsCHa  in  Mixture.      CO.  Mixture  of  Tol-    frl&CIfr  in  Mixture.    Co. 

uene  and:  wt.  %.    Mol.  %.         Ais-  uene  and:  \vt.  %.     Mol.  %.        k&. 

Aniline            100  100  0.182  a  Naphthol          95.5  97.1  0.171 

"                    93-4  93- S  0.169  91.2  94.2  0.162 

80. i  80.3  0.148  Nitrobenzene       81.7  85.7  0.160 

55.4  55.6  0.115  So.8  58.1  0.131 

25.4  25.6  0.077  2.3.7  29.3  0.108 

o            o  0.053  °  °  0-093 

Naphthalene    92.9  94.8  0.169  Phenanthrene      94.4  97  0.170 

84.9  88.7  0.161  88.8  93.9  0.161 

77.3  82.5  0.153  78.4  87.5  0.147 

SOLUBILITY  OF  CARBON  MONOXIDE  IN'  MIXTURES  OF  ORGANIC  SOLVENTS  AT  25°. 

(Skirrow.) 

%  of  Latter  in  Mixture.          CO 
Mixture  Composed  of:  'By  Wt.    '    By  Moll  £ 

Chloroform  and  Methyl  Alcohol  o.o  0.207 

"  "  13.0  0.202 

100  0.196 

Carbon  Bisulphide  and  Ethyl  Di  Chloride  100  o .  147 

75  0.157 

51  0.160 

18.4  0.140 

'o.o  0.083 

Methyl  Alcohol  and  Glycerine  o.o          o.o  o .  196 

."  39.6        30.1  0.096 

60.5        50.1  0.052 

77.1        68.9  0.025 

loo.o       100.0  very  small 

NOTE.  —  From  the  results  shown  in  the  preceding  five  tables,  it  is 
concluded  that  the  solubility  of  carbon  monoxide  in  various  mixtures 
of  organic  solvents  is,  in  general,  an  additive  function. 

CARBON  OXYSULFIDE  COS. 

SOLUBILITY  OF  CARBON  OXYSULFIDE  IN  WATER. 

(Winkler,  1906.) 

o    1-333    O-356       20    0.561    0.147 
5    1.056   0.281      25   0.468   0.122 

10  0.836  0.221  30  0.403  0.104 

15  0.677  0.179 

For  /?  and  q  see  Carbon  Dioxide,  p.  227. 

SOLUBILITY  OF  CARBON  OXYSULFIDE  IN  SEVERAL  SOLVENTS. 

Solvent.  t°.        CC'^5ohrent  Authority. 

Water  13.5  80  (Hempel,  1901.) 

2O  54  (Stock  and  Kuss  1917.) 

Alcohol  22          800  "  " 

Toluene  22         1500  M  " 

HC1  Solution  Of  CuCl  13.5  20  (Hempel,  1901.) 

i  gm.  KOH+2CC.H2O+2CC.C2H5OH  13 .5     7200 
Pyridine  ...  4.4  « 

Nitrobenzene  12.0  " 


239          CARBON  TETRACHLORIDE 

CARBON  TETRACHLORIDE  CC14. 

SOLUBILITY  IN  WATER.    (Rex,  1906.) 

t°.  o°.  10°  20°  30° 

Gms.  CCLj  per  100  gms.  H2O  0.097    0.083    0.080    0.085 

RECIPROCAL  SOLUBILITY  OF  CARBON  TETRACHLORIDE,  ALCOHOL  AND  WATER. 

(Curtis  and  Titus,  1915.) 

Alcohol  was  added  from  a  weight  buret  to  mixtures  of  weighed  amounts  of 
CCU  and  H2O,  stirred  vigorously  at  19.75°,  until  the  mixture  became  homogeneous. 
Per  cent  Per  cent  Per  cent 

CCU.  CzHfiOH.  H20. 

41.94  43.19  14.89 

33.07  47.68  19.25 

25.46  50.50  24.04 

17.00  51.95  31.05 

14.02  51.56  34.42 

10.53  50.97  38.50 

In  order  to  determiae  the  effect  of  temperature  upon  the  mutual  solubility,  one 
component  was  added  to  a  known  mixture  of  the  other  two,  and  the  critical 
solubility  temperature  determined  by  raising  and  lowering  the  temp,  through  the 
critical  point  several  times.  A  further  amount  of  the  third  component  was  then 
added  and  the  critical  solubility  temperature  again  determined. 


**c3B 

^g  =  0.5048. 

"Rltin        ^^    '         —  _  .£  .     T>~4.!~        V^v^  4          —   ^  ^ 

Ratio  CCl4 

=  1.0922. 

Jxaiio  „  „  , 

-JTT               i.WU^. 

""CsHsC 

>xl 

ltl°  H20 

Per  cent 

Crit.oSol." 

Per  cent 

Crit^Sol. 

Per  cent 

Crit.  Sol. 

Per  cent 

Crit.  Sol. 

H2O. 

HzO. 

H20. 

24.25 

-i'.8 

12.47 

2.03 

6.84 

12.7 

47-43 

44-5 

24.61 

+3-6 

13-95 

23-9 

7-16 

21-55 

47-83 

39-5 

25.13 

10.6 

14-45 

29.8 

7-35 

27.2 

48.6 

30.6 

25.64 

17 

14.85 

35-4 

7-54 

31-3 

49.61 

19.9 

26.14 

24-5 

15-3 

39-55 

7.84 

36.8 

50.07 

14.6 

27.15 

31-45 

I5-67 

42.75 

8.02 

39-75 

50.50 

9.15 

28.52 

35-  5(?) 

16.02 

45-5 

8.28 

44.1 

51.06 

1.6 

The  results  show  that  temperature  has  very  little  effect  on  the  mutual  solubility 
of  the  three  components.  Extensive  series  of  determinations  of  refractive  indices 
and  densities  of  the  mixtures  are  also  given. 

Freezing-point  data  for  CCU+C1  are  given  by  Waentig  and  Mclntosh  (1916). 

CARMINE. 

loo  gms.  H2O  dissolve  0.13    gm.  carmine  at  20-25°.       (Dehn,  1917.) 

pyridine  "        3.34  gms.       "        "       " 

50%  aq.  pyridine        "        2.03     " 

CARVACROL   (CH3)2CH.C6H3(CH3)OH. 

MISCIBILITY  OF  AQ.  ALKALINE  SOLUTIONS  OF  CARVACRQL  WITH  SEVERAL 
ORGANIC  COMPOUNDS  INSOLUBLE  IN  WATER.    (Sheuble,  1907.) 

To  5  cc.  portions  of  aq.  KOH  solution  (250  gms.  per  liter)  were  added  the  given 
amounts  of  the  aq.  insoluble  compound  from  a  buret  and  then  the  carvacrol,  drop- 
wise  until  solution  occurred.     Temperature  not  stated. 
Composition  of  Homogeneous  Solutions. 


Aq.  KOH. 

Aq.  Insol.  Compd. 

Carvacrol. 

5CC. 

2  cc.  (=  1.64  gms.)  Octyl(i)  Alcohol 

1.8  gms. 

5" 

5  cc.  (=  4.1    gms.) 

2.6      " 

5" 

2  cc.  (=  1.74  gms.)  Toluene 

4        " 

5" 

3  cc.  (=  2.61  gms.)        " 

4-8    " 

5" 

2  cc.  (=  1.36  gms.)  Heptane 

4.6    « 

the  normal  secondary  octyl  alcohol,  i.e.,  the  so-called  capryl  alcohol,  CHj(CH»)t.CH(OH)CHj. 


CARVOXIME 


240 


CARVOXIME   Ci0H4:NOH   d,  I  and  i. 

SOLUBILITY  IN  AQUEOUS  ALCOHOL  OF  dn.6  =  0.9125  (51.6  PER  CENT 

C2H6OH).      (Goldschmidt  and  Cooper.  1898.) 

The  determinations  were  made  by  the  synthetic  method.  On  account  of  the 
slow  rate  at  which  melted  carvoxime  solidified  on  cooling  below  the  melting  point, 
in  the  tubes  containing  the  synthetic  mixtures,  it  was  possible  to  obtain  results 
which  show  the  solubility  curve  for  liquid  carvoxime,  in  addition  to  the  curves  for 
dextro  and  inactive  carvoxime.  The  curves  for  these  latter  intersect  the  curve 
for  liquid  carvoxime  respectively  at  51.7°,  the  m.  pt.  of  dextro,  and  70.5°  the  m.pt. 
of  inactive  carvoxime. 


Gms.                      Gms.           Mols.  Carvoxime 
Carvoxime.             Solvent,   per  100  Gms.  Solvent. 

t°  of  Solution. 

Solid  Phase. 

Solid. 

Liquid. 

0.0668             1.0868 

0.0373 

38.4 

13-9 

d  Carvoxime 

0.1232             1.0830 

o  .  0689 

45-8 

31-9 

" 

0.2026              I.  02l8 

0.1202 

50-3 

49-8 

" 

0.4040              I.  O2l8 

0.2396 

.  .  . 

79.6 

" 

0.4128             0.8130 

0.3077 

.  .  . 

94-5 

<t 

0.0657             1.0980 

0.0363 

54-2 

i  Carvoxime 

O.I2I2              I.0l6l 

0.0723 

62.5 

33-7 

M 

0.2715              I.OI29 

0.1625 

69.25 

61.3 

u 

°-3755          1-0384 

0.2192 

76.6 

tt 

0.4496         0.7768 

0.3409 

... 

102.9 

tt 

SOLUBILITY  IN  d  LIMONENE. 

(Goldschmidt  and  Cooper,  1898.) 

Gms.  Ci0H4:NOH 

Gms.  CioH4:NOH 

t8.            per  100  Gms. 

Solid  Phase. 

t°. 

per  100  Gms. 

Solid  Phase. 

d  Limonene. 

d  Limonene. 

24.6              44.6              I 

Carvoxime 

48 

198.7 

/  Carvoxime 

30             59-2          I 

a 

49.4 

199.7 

d 

30.3              63.3               d 

tt 

55.1 

325-I 

I 

38.4            104.3               I 

u 

55-9 

346.6 

d 

39.3        103.1          d 

it 

58.8 

560 

d 

43.1            130.8               / 

it 

63.2 

1269.3 

d 

Freezing-point  data  are  given  for  mixtures  of  d  and  /  carvoxime  by  Adriani, 
1900  and  by  Beck,  1904. 

CASEIN. 

100  gms.  H2O  dissolve  2.01  gms.  casein  at  20-25°.  (Dehn,  1917.) 

loo  gms.  pyridine  dissolve  0.09  gm.  casein  at  20-25°.  " 

100  gms.  aq.  50%  pyridine  dissolve  0.56  gm.  casein  at  20-25°.  " 

Data  for  the  solubility  of  casein  in  aqueous  NaCl  solutions  are  given  by  Ryd 
(1917).  An  abstract  of  experiments  on  the  solubility  of  casein  in  dilute  acids  is 
given  by  Van  Slyke  and  Winter  (1913).  Results  for  the  solubility  of  casein  in 
aqueous  solutions  of  KOH,  LiOH  and  Ca(OH)2  at  various  temperatures,  are  given 
by  Robertson,  1908. 

CATECHOL  oC6H4(OH)2. 

Freezing-point  data  (solubilities,  see  footnote,  p.  i)  are  given  for  mixtures  of 
catechol  and  picric  acid,  catechol  and  a  naphthylamine  and  catechol  and  p  tolui- 
dine  by  Philip  and  Smith,  1905. 

CEPHAELINE 


Salts. 

SOLUBILITY  IN  WATER.      (Carr  and  Pyman,  1914.) 
Salt.  Formula.  t°. 


Gms.  Hydrated  Salt 
per  zoo  cc.  Sat.  SoL 

Cephaeline  Hydrochloride  C28H38O4N2.2HC1.7H2O    17-18  26.5 

acid  C28H38O4N2.5HC1  18    about  50 

Hydrobromide  C28H3sO4Na.2HBr.7H2O    1 7-18  5 . 4  (dried  at  100°) 


24I 


CERIUM  ACETATE 


CERIUM    ACETATE,  BUTYRATE,  FORMATE,  etc. 
SOLUBILITY  IN  WATER. 

(Wolff  —  Z.  anorg.  Chem.  45,  102,  '05.) 

Grams  Anhydrous  Salt  per  100  Cms.  Solution  at: 


Salt.  Formula. 

Acetate  Ce(C2H3O2)3.i$H2O 

Butyrate  Ce(C4H7O2)3,  and3H2O 

Iso  Butyrate  Ce(C4II7O2)3.3H2O 

Formate  Ce(GHO2)3 

Propionate  Ce(C3H6O2)3.H2O,  and  3H2 


3-544 


15°. 

19.61 

3.406 

6.603(20.4°) 

0-398(13°) 
18.99 

76°. 
12.97 
1.984 

3-39 
0-374(75-3°) 
15-93 

CERIUM    AMMONIUM    NITRATE    (Ceri)   Ce(NO3)4.2NH4NO8. 
SOLUBILITY  IN  WATER. 

(Wolff.) 


Gms.  per  100  Gms. 
t  o                                Solution. 

Atomic                 Gms.Ce<NO3)4.2NH4NOa 
Relation.                           per  100  Gms. 

' 

NH*. 

Ce. 

NH*      :       Ce. 

Solution. 

Water". 

25 

4 

.065 

15 

.16 

2 

.08 

i 

58 

•49 

140 

•9 

35-2 

4 

•273 

16 

•  1C 

2 

.06 

i 

61 

•79 

161 

-7 

45-3 

4 

.489 

16 

•69 

2 

.08 

i 

64 

•51 

174 

•9 

64-5 

4 

-625 

Us 

•  4oCe 
.o3CeIV 

2 
2 

.06 
•39 

iCe 
iCelV 

66 

.84 

201 

.6 

85.6 

4 

•778 

1*5 

.i6Ce 
.79CeIV 

2 
2 

.04 
•34 

iCe 
iCe  IV 

69 

.40 

226 

.8 

(22 

.82  Ce 

2 

.08 

iCe 

112 

6 

•117 

.22CeIV 

2 

95 

iCelV 

88 

•03 

735 

•4 

CERIUM  AMMONIUM  NITRATE    (Cero)  Ce(NO3)3.2N#4ttO,.4H3O. 

SOLUBILITY  IN  WATER. 

(Wolff.) 


Gme.  per  too  Gms. 
t<\                   Solution. 

NH4. 

Ce. 

8-75 

4.787 

18.56 

£•5.0 

5-°9 

19.80 

45-o 

5-53 

21  -06 

60-0 

6.01 

22-77 

65.06 

6.  ii 

23.42 

AtomicRe,ation. 


NIL,       :  C 

e>        '  Solution. 

Water.' 

1.999  : 

7O.2 

235-5 

1-995  : 

74-8 

296.8 

2.037  • 

80.4 

4IO.2 

2.054  : 

c          87.2 

681.2 

2.  022  : 

89.1 

817.4 

CERIUM    AMMONIUM    SULPHATE    Ce2(SO4)3.(NH4)2SO4.8H2O. 

SOLUBILITY  IN  WATER. 

(Wolff.) 

Gms. 


Gms. 
Ce2(S04)3.(NH4)2S04 
1   •           per  100  Gms. 

Solid 
Phase. 

.8H2O 

M 

It 

22.3 

35-i 

45-2 

Solution. 
5.06 

4-93 
4.76 

Water". 

5-33 

S.l8 

4-99 

Ce2(SO4)s  .(NH4)2SO4 
*   •             per  ipo  Gms. 

Solid 

Phase. 

Solution. 

Water. 

45  -° 

2.91 

2-99 

Anhydride 

55-25 

2  .l6 

2.21 

u 

75-4 

I  .46 

1.48 

u 

85-2 

I.I7 

1.18 

n 

CEROUS   CHLORIDE 


242 


CEROUS   CHLORIDE  CeCl,. 

100  cc.  anhydrous  hydrazine  dissolve  3  gms.  CeCls,  with  evolution  of  gas,  at 
room  temp.  (Welsh  and  Broderson,  1915.) 

CERIUM  CITRATE  2(CeC6H607).7H2O. 

100  gms.  of  aq.  citric  acid  solution  containing  10  gms.  citric  acid  per  100  cc., 
dissolve  0.3  gm.  Ce(C6H6O7)  at  20°.  (Holmberg,  1907.) 

CERIUM  COBALTICYANIDE  Ce2(CoC6N6)2.9H2O. 

100  gms.  aq.  10%  HC1  (di$ '=  1.05)  dissolve  1.075  Sms.  of  the  salt  at  25°. 

(James  and  Willand,  1916.) 

CERIUM  FLUORIDE   CeF3. 

Freezing-point  lowering  data  are  given  for  mixtures  of  CeF8  +  KF  by  Puschin 
and  Baskow,  1913. 

CERIUM   GLYCOLATE  Ce(C2H3O3)3. 

One  liter  H2O  dissolves  3.563  gms.  of  the  salt  at  2O°.  (Jantsch  and  Grunkraut,  1912-13.) 

CERIUM  IODATE  Ce(IO3)3. 

Oneliter  sat.  aqueous  solution  contains  1.456  gms.Ce(IO3)3,  determined  by  achem- 
ical  method,  and  1.636  gms.  determined  electrolytically.  (Rimbach  and  Schubert,  1909.) 

CERIUM  MALONATE   Ce2(C3H2O4)3  +  6H2O. 

c  i  AO   Gms.  Ce2(C3H2O4)3  per 

Solvent-  t  *  '     loo  Grams.  Solvent. 

Aq.  Ammonium  Malonate,  containing  10  gms.  per  100  cc.        20  0.2 

Aq.  Malonic  Acid,  containing  20  gms.  per  100  cc.  20  0.6 

(Holmberg,  1907.) 

CERIUM   Magnesium,  etc.,  NITRATES. 

SOLUBILITY  IN  CONG.  AQ.  HNO3  (dy  =  1.325 =51. 59'Gms.  HNO3  per  100  cc.)  AT  16°. 

(Jantsch,  1912.) 

Cerium  magnesium  nitrate,  i  liter  sat.  solution  contains  58.5  gms.[Ce(NOs)6]Mg3.24H20. 
"      nickel  "  "  "        75-3    "  "        Ni3       " 

"      cobalt  "  "  "  "      103.3    "  "        Co,      " 

"       zinc  "  "  "  "      111.7    "  "         Zn3      " 

"       manganese      "  "      178.8    "  "         Mn?     " 

CERIUM  OXALATE  Ce2(C2O4)3.9H2O. 

One  liter  H2O  dissolves  0.00041  gm.  Ce2(C2O4)3  at  25°,  determined  by  the  elec- 
trolytic method.  (Rimbach  and  Schubert,  1909.) 

SOLUBILITY  OF  CERIUM  OXALATE  IN  AQUEOUS  SOLUTIONS  OF  SULFURIC 
ACID  AND  OF  OXALIC  ACID  AT  25°. 

(Hauser  and  Wirth,  1908;  Wirth,  1912.) 


Cone  of    Gms.  per  100  Gms. 

Gms.  per  100  Gms. 

Aqueous             Sat.  Sol. 

Phase              Conc>  of  Aq>  Acid' 

Sat.  Sol. 

Solid 
Phase. 

Acid.        CeO^  Ce2(C204)3. 

' 

CeO2=  Ce2(C2O4)s. 

O.IWH2SO4  0.0136     0.0215  Ce(C204)3.9H2Oo.m(COOH)2 

0.0020     o.oo32Ce2(C2O4)3-9H2O 

0-5 

0.0524    0.0828 

0-5 

0.0083     0.0131 

" 

i.o 

0.114      0.1802 

I.O 

0.0040     0.0063 

" 

1-445 

0.1764    0.2788 

3-2 

(sat.) 

0.0019     0.0030 

" 

2-39 

0.3083    0.4871 

0.05 

+.O5«H2S( 

)4o.oo3O     0.0047 

" 

2.9 

0.4724    0.7467 

*         0.05 

+•5 

0.0025     0.0039 

it 

3-9 

0.6300    0.9957 

0.25 

+-25      " 

0.0046     0.0073 

" 

4-32 

0.7502     1.  1860 

0.50  "    +.05 

0.0105     0.0166 

" 

5.3             0.9019     1.4250 

0.50  "    +.50 

o.ooio    0.0016 

" 

CERIUM   Dimethyl  PHOSPHATE   Ce2[(CH3)2PO4]6.H2O. 

100  gms.  H2O  dissolve  79.6  gms.  Ce2[(CH3)2PO4]6  at  25°  and  about  65  gms.  at 
95°»  (Morgan  and  James,  1914.) 


.243 


CERIUM   SELENATE 


CERIUM  SELENATE  Ce2(SeO4)8.iiH2O. 
SOLUBILITY  IN  WATER. 

Gms. 

t°.     Ce2(Se04)3  per  Solid  Phase.  t°. 

loo  Gms.  HzO. 

39-55      Ce2  (SeC^s.  1 2H2O      60 

37.0  60.8 

36.9 

33.84 

33-22 

33-15 
32.16 


(Cingolani,  1908.)  ] 

Gms. 

Ce2(SeO4)» 

per  100  Gms. 

H.O. 


Solid  Phase. 


78.2 
80.5 
91 

95-4 


13.68      Ce2(SeO4)3.8H2O 
13.12 

5.53 
4-56 


Ce2(Se04)3.7H20 


o 
n. 6 

12.6 

26 

28.8 

34.2 

45 

45-9     31-89 
CERIUM  SULFATE  Ce2(SO4)3. 

SOLUBILITY  OF  THE  SEVERAL  HYDRATES  IN  WATER. 

(Koppel,  1904;  the  previous  determinations  by  Muthman  and  Rolig,  1898,  and  by  Wyrouboff,  1901, 
are  shown  by  Koppel  to  be  inaccurate.) 


2.02 

I 
I 


100 


536 
785 

2.513 


Gms. 


Mols. 


Gms. 


Solution. 


H20. 


O 

14.20 

0-525 

18.8 

14.91 

o-555 

19.2 

15.04 

0.561 

0 

J7-35 

0.665 

15 

10.61 

0.376 

21 

8.863 

0.308 

31-6 

6.686 

0.227 

45-6 

4-910 

0.164 

5o 

4-465 

0.148 

60 

3-73 

0.123 

65 

3-47 

0.114 

o 

15-95 

0.605 

IS 

9-95 

o.35o 

Ce2(S04)3.oH20 


Solution. 

mv. 

20.5 

8.69 

0.302 

40 

5-6l3 

0.188 

60 

3.88 

0.129 

45 

8.116 

0.280 

60 

3  .145 

0.103 

80 

1.19 

0.0382 

100.5 

0.46 

0.0149 

35 

7.8 

0.27 

40 

5  -71 

0.19 

50 

3  .31 

o.n 

65 

1-85 

0.06 

82 

0.98 

0.032 

100.5 

0.42 

0.014 

Solid  Phase. 


062(504)3^20 


Ce2(S04)3.5H30 


Ce2(S04)3.8H20 


SOLUBILITY  OF  CERIUM  SULFATE  IN  AQUEOUS  SOLUTIONS  OF  ALKALI 

SULFATES.      (Barre,  1910.) 


In  aq.  sols,  of 
K2SO4  at  16°. 

In  aq 

Na2SC 

isols.  of 
4  at  19°. 

In  aq.  sols,  of 
(NH4)2SO4  at  16°. 

Gms.  per  too  Gms.  H2O. 

Gms.  per  100  Gms.  HzO. 

Gms.  per  100  Gms.  H2O. 

KzSO4. 

Ce2(SO4)3. 

'Na2S04. 

Ce2(SO4)3. 

(NH4)2SO4 

.          CC2(SO4)l. 

0 

10.747 

0 

9.648 

0 

10.747 

0.178 

0.956 

0.328 

0.637 

3.464 

1.026 

0.510 

0.432 

0.684 

0.259 

9-323 

0.782 

0.726 

0.250 

I.09I 

0.0937 

19  .  240 

0.748 

I.29O 

0.042 

1.392 

0.0570 

29-552 

0.701 

0 

6.949  (at  33°) 

1.699 

0.0303 

45.6l6 

0.497 

2.640 

0.0120 

55-083 

0.194 

3-589 

0.0065 

63.920 

0.090 

5.660 

0.0046 

72.838 

0.035 

7.710 

0.0037 

The  following  double  salts 

•were  found. 

Ce2(S04)3, 

,K2SO4.2H2O, 

2Ce2(S04),. 

3K2S04.8H20,    Ce2(S04)3.5K2S04,    Ce2(SO4)3.Na2SO4.2H2O,    Ce2(SO4)3(NH4)2SO4. 
8H20  and  Ce2(SO4)8.5(NH4)2SO4. 


CERIUM   SULFATE 


244 


SOLUBILITY  OF  CERIUM  SULFATE  IN  AQ.  SOLUTIONS  OF  SULFURIC  ACID  AT  25°. 

(Wirth,  1912.) 


Normalit 
of  Aq. 
IfcSO*. 

v     Gms.  per 
Sat 

zoo  Gms. 
.  Sol.                      Solid 

TlU-«« 

Normality 
of  Aq. 
HzSO4. 

Gms.  per  100  Gms. 
Sat.  Sol. 

Solid 
Phase. 

CeCfe    = 

=  Ce2(S04)3: 

CeO2     = 

Ce2(S04)3. 

0.0 

4 

.604 

7 

.60       CezCSO^a-SH 

zo     4 

•32 

2 

3' 

.301 

Ce2(S04)3.8H2O 

O.I 

4 

.615 

7 

.6l8 

6 

.685 

0 

.9115 

i. 

505 

" 

I.I 

3 

.64 

6 

" 

9 

.68 

0 

•4439 

o 

733 

" 

2.16 

3 

.04 

5 

.Ol8 

15 

•15 

O 

•145 

o 

239 

" 

CERIUM  SULFONATES. 

SOLUBILITY  IN  WATER. 

Name. 


(Holmberg,  1907;  Katz  and  James,  1913.) 


Formula. 


Gms.  Anhy- 
drous Salt 

per  100 
Gms.  H2O. 

25-5 
5.89 


Cerium  m  Nitrobenzene  Sulfonate        Ce[C6H4(NO2)SO3]3.6H2O  15 

Cerium  Bromonitrobenzene  Sulfonate  Ce[C6H3Br(NO2)SO3i.4.2]3.8H2O  25 

CERIUM  TARTRATE   Ce2(C4H4O6)34sH2O,  also  6H2O. 
SOLUBILITY  IN  WATER  (Rimbach  and  Shubert,  1909,  by  electrolytic  method) 

AND  IN  AQ.   SOLUTIONS.      (Holmberg,  1907.) 


Solvent. 


Gms.    An- 

hydrous Salt 

per  100  Gms. 

Sat.  Sol. 


Solid  Phase. 


25 

20 

20 
20 
2O 


0.005 

0.7 

2 

0.4 

O.2 


Water 

Aq.  Am.  Tartrate,  10  Gms.  per  100  cc. 
Aq.  Am.  Tartrate,  20  Gms.  per  100  cc. 
Aq.  Tartaric  Acid,  20  Gms.  per  100  cc. 
Aq.  Tartaric  Acid,  40  Gms.  per  100  cc. 

CERIUM  TUNGSTATE   Ce2(WO4)3. 

Freezing-point  lowering  data  for  mixtures  of  Ce2(WO3)3  and  PbWO4  are  given 
by  Zambonini,  1913. 

CETYL  ALCOHOL   Ci6H33OH. 

100  gms.  methyl  alcohol  dissolve    96.9  gms.  Ci6H3OH  at  23.9°.       (Timofeiew,  1894.) 

ethyl  "         102.2     "  "     " 

«  <i          ii  37 

propyl         "  "        405        "  "  39 

CHLORAL  HYDRATE   CC13.CHO.H2O. 
.  SOLUBILITY  IN  WATER,  ETHYL  ALCOHOL,  CHLOROFORM,  AND  IN  TOLUENE. 

(Speyers,  1902.) 

Calculated  from  the  original  results,  which  are  given  in  terms  of  gram  molecules 
of  chloral  hydrate  per  100  gram  mols.  of  solvent. 


In  Water. 


In  Alcohol. 


In  Chloroform. 


In  Toluene. 


•>  . 

w. 

s". 

'w. 

s.  ' 

w. 

s. 

w. 

s: 

o 

1-433 

189 

•7 

I 

.11 

123.3 

i 

•530 

3-7 

0.898 

3-2 

5 

1.460 

233 

.0 

I 

.16 

130.0 

i 

•5*5 

4.0 

0.900 

4-0 

10 

1.485 

275 

•  o 

I 

•23 

140.0 

i 

.5!0 

5  .0 

0.910 

7.0 

15 

1.510 

•  o 

I 

•30 

160.0 

i 

•505 

9.0 

0-915 

II.  0 

20 

J-535 

383 

•  0 

I 

.36 

185.0 

i 

.510 

19-0 

o-94 

21.0 

25 

'•555 

433 

•  0 

I 

.42 

215.0 

i 

.  34-o 

0.97 

36.0 

30 

1.580 

480 

.0 

I 

.49 

245.0 

i 

•540 

56.0 

1.02 

56.0 

35 

i-59 

516 

.0 

I 

•55 

280.0 

i 

•570 

80.0 

I  .13 

80.0 

40 

1.605 

.  ' 

I 

.60 

320.0 

i 

•590 

IIO.O 

1-40 

IIO-O 

45 

1.620 

. 

. 

W  =  wt.  of  i  cc.  saturated  solution,  S  =  Gms.  C2HC13.H2O  per  100 
grams  solvent. 


245  CHLORAL  HYDRATE 

SOLUBILITY  IN  SEVERAL  SOLVENTS. 

f0  Cms.  CChCOH.HzO  sl      .  t.         Gms.  tCbCOH.HjO 

Solvent.  t  .  per  IOQ  Gms  Soivent.  t  .          IOQ  Gmg  Solvent 

50%  Aq.  Pyridine  20-25  374        (Dehn,  1917.)  Ether          ord.  t.  200  (Squires.) 

Pyridine  20-25  80.9  Oil  tur-     (cold  10       " 

Carbon  Bisulfide  ord.  t.  i  .  47  (Squires.)             pentine  (  hot  20 

Glycerol  ord.  t.  200  Olive  Oil     ord.  t.  100       " 

Freezing-point  data  (solubility,  see  footnote,  p.  i)  are  given  for  mixtures  of 
chloral  and  water  by  van  Rossem  (1908)  ;  for  mixtures  of  chloral  and  ethyl  alcohol 
by  Leopold  (1909);  for  mixtures  of  chloral  hydrate  and  menthol  by  Pawlewski 
(1893)  and  for  mixtures  of  chloral  hydrate  and  salol  by  Bellucci  (1912,  1913). 

DISTRIBUTION  OF  CHLORAL  HYDRATE  BETWEEN  WATER  AND  ORGANIC 

SOLVENTS. 


Immiscible  Solvents.  t.       Dist.  Coef  .  c^nOrg.  Solvent.       Authoritv- 

Water  and  Ether          0-30°  0.235       (Hantzsch  and  Vagt,  1901.) 

Water  and  Benzene  ...  ...  (Bubanovk,  1913.) 

Water  and  Olive  Oil       ord.  4.9  (Baum,  1899.) 

"          "  "  30°  4-3  (Meyer,  1901;  1909.) 

3  16.7  (Meyer,  1901.) 

"          "      Toluene  O-200  58-74.5  (Hantzsch  and  Vagt,  1901.) 

CHLORAL  FORMAMIDE   CC13.CH(OH).NH.CHO. 

100  gms.  H2O  dissolve  5.3  gms.  CC13CH(OH).NHCHO  at  25°.  (U.  S.  P.) 

100  gms.  95%  alcohol  dissolve  77  gms.SCCl3CH(OH).NHCHO  at  25°. 


L.U-ttJ.1 

*Ci    14* 

SOLUBILITY  IN 

(Winkler,  1912;  Roozeboom 

WATER. 

,  1884,  1885,  1888.) 

t°. 

0'. 

9. 

f  . 

Gms.  Cl  per 
100  Gms.  HjjO. 

Solid  Phase. 

0 

4.6lO 

I  .46 

—  0.24 

0.492 

Ice  +  C1.8  aq. 

3 

3-947 

1-25 

o 

0.507-0.560 

C1.8  aq. 

6 

3.411 

1.  08 

2 

3.644 

" 

9 

3-031 

0.96 

4 

0.732 

a 

9.6 

2.980 

0.94 

6 

0.823 

u 

12 

2.778 

0.88 

8 

0.917 

(C 

10 

3-095 

0.980 

9 

0.965-0.908 

tc 

15 

2-635 

0-835 

20 

1.85 

u 

20 

2.260 

0.716 

28.7 

3-69 

"  +  2  layers 

25 

1.985 

0.630 

30 

1.769 

0.562 

40 

1.414 

0.451 

50 

1.204 

0.386 

60 

i.  006 

0.324 

70 

0.848 

0.274 

80 

0.672 

0.219 

90 

0.380 

0.125 

[OO 

c 

0 

ft'  =  vol.  of  Cl  .(reduced  to  o°  and  760  mm.)  absorbed  by  i  vol.  H2O  at  total  pres- 
sure of  760  mm. 

q  =  Gms.  Cl  per  100  gms.  H2O  at  a  total  pressure  of  760  mm. 

The  coefficient  of  solubility  of  chlorine  at  15°,  determined  by  an  aspiration 
method,  is  given  as  51.7  for  carbon  tetrachloride,  39.6  for  acetic  anhydride,  36.7 
for  99.84%  acetic  acid,  25.3  for  90  vol.  %  acetic  acid,  16.43  for  75  vol.  %  acetic 
acid  and  13.43  for  65  vol.  %  acetic  acid.  (Jones,  1911.) 


CHLORINE  246 

SOLUBILITY  IN  WATER. 

(Goodwin,  1882.) 

•  ,.    • 

The  saturated  aqueous  solution  of  the  chlorine  was  cooled  until  chlorine  hydrate 
separated;  the  temperature  was  then  gradually  raised  and  portions  withdrawn  for 
analysis  at  intervals.  The  chlorine  was  determined  by  iodometric  titration  and 
the  results  calculated  to  volume  of  chlorine  dissolved  by  unit  volume  of  solvent 
at  the  given  temperature  and  760  mm,  pressure.  Slightly  different  results  were 
obtained  for  solutions  in  contact  with  much,  little,  or  no  chlorine  hydrate.  The 
following  results  are  taken  from  an  average  curve:  , 

to  Solubility  fo  Solubility  ,0  Solubility 

Coefficient.  .  Coefficient.  Coefficient. 

2.5  1.76  ii  3  25  2.06 

5  2  12.5          2.75  30  1.8 

7-5  2.25  15  2.6  40  1.35 

IO  2.7  20  2.3  50  I 

SOLUBILITY  OF  CHLORINE  IN  AQUEOUS  SOLUTIONS  OF  HYDROCHLORIC 
ACID  AND  OF  POTASSIUM  CHLORIDE. 

(Goodwin.) 
Coefficient  (^Solubility  in: ^  Results  at  21°.     (Mellor,  1901.) 

*°-          HC1.  HC1  HC1  KC1  Cms.  HClper    Solubility  of  Cl. 

(i.o46Sp.Gr.).  (i.oSSp.  Gr.).  (1.125  Sp.Gr.).  (20 g. per  xoocc.)       1000  cc.    (Ostwald/,  seep.  227.) 

o        4.1  6.4  7.3  1.5  o.  2.2799 

5        5-i  S-2  6-7  2  3.134        1.6698 

10  4.1  4.5  6.1  2.2  9.402  I-50I3 

15  3.5  3.9  5.5  1.6  12.540  1.5292 

20  3  3.4  4-7  I-2  31-340  1-8033 

25  2.5  3  4  i  125.360  2.4473 

30  2  2.4  ...  -0.9  219.380  3-I3*2 

40  1.25  1.6  ...  ...  3I3-4oi  3.8224 

Goodwin  also  gives  results  for  solutions  of  NaCl,  CaCl2,  MgCl2,  SrCl2,  Fe2Cl2, 
CoCl2,  NiCl2,  MnCl2,  CdCl2,  LiCl,  and  in  mixtures  of  some  of  these,  but  the  con- 
centrations of  the  salt  solutions  are  not  stated. 


SOLUBILITY  OF  CHLORINE  IN  AQUEOUS  SOLUTIONS  OF  SODIUM  CHLORIDE. 

(Kumpf,  1882;  Kohn  and  O'Brien,  1898.) 

Coefficient  of  Solubility  in: 
9-97%  NaCl.          16.01  %  NaCl.          19.66%  NaCl.          26.39%  NaCl. 

o  2.3  1.9  1.7  0.5 

5  2  1.6  1.4  0.44 

10  1.7  1.3  1.15  0.4 

15  1.4  i. 06  0.95  0.36 

20  1.2  0.9  0.8  0.34 

25  0.94  0.75  0.65  0.3 

50  ...  ...  ...  0.2 

80  ...  ...  ...  0.05 

100  cc.  of  6.2  per  cent  CaCl2  solution  dissolve  0.245  Sm-  Cl  at  12°. 
100  cc.  of  6.2  per  cent  MgCl2  solution  dissolve  0.233  gm.  Cl  at  12°. 
loo  cc.  of  6.2  per  cent  MnCl2  solution  dissolve  0.200  gm.  Cl  at  12°. 
For  coefficient  of  solubility  see  p.  227. 


247  CHLORINE 

Freezing-point  data  (solubility,  see  footnote,  p.  i)  are  given  for  the  following 
mixtures  containing  chlorine. 

Chlorine  +  Chloroform  (Waentig  and  Mclntosh,  1916.) 

+  Ethyl  Alcohol  "  " 

-j-  Methyl  Alcohol  " 

-j-  Ethyl  Acetate  (Waentig  and  Mclntosh,  1916;  Maass  and  Mclntosh,  1912.) 

+  Methyl  Acetate  (Waentig  and  Mclntosh,  1916.) 

+  Ether 

-j-  Hydrochloric  Acid  (Maass  and  Mclntosh,  1912.) 

-j-  Iodine  (Stortenbecker,  1888,  1889.) 

+  Sulfur  (Ruff  and  Fischer,  1903.) 

-j-  Sulfur  Dioxide  (Smits  and  Mooy,  1910;  Van  der  Goot,  1913.) 

-j-  Sulfuryl  Chloride  (SO2C12)  (Van  der  Goot,  1913.) 

+  Sulfur  Dioxide 

-j-  Stannic  Chloride  (Waentig  and  Mclntosh,  1916.) 

-j-  Toluene  (Waentig  and  Mclntosh,  1916;  Maass  and  Mclntosh,  1912.) 

-j-  Nitrosyl  Chloride  (NOC1)  (Boubnoff  and  Guye,  1911.) 

DISTRIBUTION  OF  CHLORINE  BETWEEN  CC14  AND  GASEOUS  PHASE  AND 
BETWEEN  CC14  AND  WATER. 

(Jakowkin,  1899.) 


Results  for  CC14  + 
Gaseous  Phase. 

MillimolsCl  per  Liter. 

Results  for  dist.  between  CC14  and  H2O. 
ist  Series.                                    2nd  Series. 

Millimols  per  Liter.                                  Millimols  per  Liter. 

H2OI,ayer. 

ecu. 

Layer. 

803.3 
464.6 
222.5 
52.93 

HzO  Layer. 

ecu. 

Layer. 
864.2 

335-1 

311-3 

202.7 

Gaseous 
Phase. 

O.IIOQ 
O.2666 

O-SS^S 
0.8800 

ecu 

Phase. 
8.908 
22.46 
44.14 

75  -°9 

Total 
Cl. 
58.21 

38.36 
23.08 
10.10 

•  Unhydro- 
lized  Cl. 

39-67 
22.97 
II  .12 
2.707 

Total 
Cl. 

61.73 
42.62 
28.98 
21.70 

Unhy- 
drolized  Cl. 

42.55 
26.36 
15.24 

9-94 

Data  for  the  effect  of  HC1  upon  the  distribution  between  H2O  and  CC14  are 
also  given. 

CHLORINE  DIOXIDE  C1O2.8H2O  ±  iH2O. 

SOLUBILITY  IN  WATER. 

(Bray,  1905-06.) 

*°        SrlS?        Solid  Phase.  t°.  ^ClO,  Solid  Phase. 

— 0.79  Eutec.  26.98       ClO2.8H2O+Ice  15.3  87.04    ClOj.SHjOiiHjO 

0  27.59       ClO2.8H2O±iH2O        I0.7tr.pt.  107.9          "  +  liquid  CIO, 

1  29.48  "  14  more  than  >  107.9      liquid  CIO, 
5-7               42.10                    "                      10.7  116.7 

10  60.05  "  I  more  than  >  108.6  " 

The  exact  composition  of  the  hydrate  could  not  be  determined  on  account  of 
manipulative  difficulties. 

Data  for  the  distribution  of  C1O2  between  H2O  and  CCU  at  o°  and  25°  are  given, 
also  some  results  showing  the  effect  of  H2SO4,  KC1OS  and  of  KC1  on  this  distribu- 
tion. 

CHLORINE  MONOXIDE  C12O. 

100  volumes  of  water  at  o°  absorb  200  volumes  of  C12O  gas. 
CHLORINE  TRIOXIDE  C12O3. 

SOLUBILITY  IN  WATER  AT  APPROX.  760  MM.  PRESSURE. 

(Brandan,  1869.) 
t°.  8.5°.  14°.  21°.  93°. 

Cms.  C^Oa  per  ioo  gms.  H2O       4.765        5.012        5-445        5.651 

Garzarolli  and  Thurnbalk,  1881,  say  that  C12O5  does  not  exist,  and  above 
figures  are  for  mixtures  of  C12O  and  Cl. 


CHLOROFORM  248 

CHLOROFORM  CHC13. 

SOLUBILITY  IN  WATER. 

(Chancel  and  Parmentier,  1885;  Rex,  1906.) 

AO  Cms.  CHCls  per  Density  of  f0         Gms.  CHCls  per 

Liter  of  Solution.  Solutions.  •     100  Cms.  HjO  (Rex). 

O  9.87  1.00378 

3.2       8.90  ...  O       1.062 

17.4  7.12  1.00284  .10  0-895 
29.4  7-O5  1.00280  20  0.822 
41.6  7.12  1.00284  30  0.776 
54-9  7-75  1.00309 

S'IQO  cc.  H2O  dissolve  0.42  cc.  CHC13  at  22°;  Vol.  of  sol.  =  100.39  cc.,  Sp.  Gr.  = 
1.0002. 

100  cc.  CHC13  dissolve  0.152  cc.  H2O  at  22°;  Vol.  of  sol.  =  99.62  cc.,  Sp.  Gr.  = 

1.4831.  (Herz,  1898.) 

SOLUBILITY  OF  CHLOROFORM  IN  AQUEOUS  ETHYL  ALCOHOL,  METHYL 
ALCOHOL,  AND  ACETONE  MIXTURES  AT  20°. 

(Bancroft,  1895.) 

In  Ethyl  Alcohol.  In  Methyl  Alcohol.  In  Acetone. 

Per  5  cc.  CzHsOH.  Per  5  cc.  CHsOH.  Per  5  cc.  (CH3)2CO 


cc.  H2O.  cc.  CHCls.  cc.  HjO.  cc.  CHCls.  cc.  H2O..  cc.  CHCb. 

10                   0.20  10  o.io  5  0.16 

8                    0.3                         5  0.48  4  0.22 

6                    0.515                     4  0.8  3  0.33 

4  1-13  24  2  0.58 

2                    2.51                        1.49  7  i  0.955 

i                   4.60                      1.35  8  0.79  i. 12 

0.91              5                            i. 12  10  0.505  i. 60 

0.76  6  0.30  2.50 

0.55  8  0.21  3.50 

0.425  10  0.19  4 

0.20  20  0.16  5 

O.I25  3O.24  O.I2  IO 

Data  for  the  system  chloroform,  ethyl  ether  and  water  are  given  by  Juttner, 
1901. 

Experiments  by  Schachner  (1910)  show  that  various  fats  (olive  oil,  sheep  suet, 
goose  fat)  in  an  atmosphere  containing  0.55%  CHCla  vapor,  dissolve  0.96-0.98 
per  cent  CHC13  at  38.5°. 

Data  for  the  properties  of  solutions  of  CHC13  in  water,  saline  solution,  serum, 
hemoglobin,  etc.,|in  their  relation  to  anesthesia  are  given  by  Moore  and  Roaf, 
(1904)  and  Waller  (1904-05). 

Freezing-point  lowering  data  (solubility,  see  footnote,  p.  i)  are  given  for  the 
following  mixtures  of  chloroform  and  other  compounds. 

Mixture.  Authority. 

Chloroform  +  Hydrobromic  Acid  (Maassand  Mclntosh,  1912.) 

+  Hydrochloric  Acid  (Baume  and  Borowski,  1914.) 

+  Methyl  Alcohol 

4-  Methyl  Ether  (Baume,  1914, 1909.) 

p  nitrophenyl  chloroform  +  m  nitrophenyl  chloroform  (Holleman,  1914.) 

CHOLESTEROL  CwHaOH.HzO. 

100  gms.  H2O  dissolve   0.26  gm.  cholesterol  at  20-25°.  (Dehn.igr;.) 

pyridine  "       68.10  gms. 

50%  aq.  pyridine  i.io     " 

loo  cc.  HzO  dissolve  0.0006  gm.  cholesterol-digitonide  at  b.  pt.       (Mueller,  1917.) 
100  cc.  ether  dissolve  0.0007  gm.  cholesterol-digitonide  at  room  temp.          " 

Freezing-point  lowering  data  (solubility,  see  footnote,  p.  i)  are  given  for  mix- 
tures of  cholesterol  acetate  and  phytosterol  a  and  /3  by  Jaeger,  1907.  Data  for 
mixtures  of  cholesterol  and  oleic  acid,  cholesterol  and  palmitic  acid  and  cholesterol 
and  stearic  acid  are  given  by  Partington,  1911. 


249 


CHOLESTEROL 


SOLUBILITY  OF  STEARIC  ACID  ESTER  OF  CHOLESTEROL  IN  OILS  AT  37°  AND 

VICE  VERSA.      (Filehne,  1907.) 

The  determinations  were  made  by  adding  small  weighed  amounts  of  the  ester 
to  the  oil  at  60°  and  cooling  to  36-37°  while  stirring  continually.  The  additions 
of  the  ester  were  repeated  until  a  clouding  just  appeared  at  36-37°.  In  the  case  of 
the  solubility  of  the  oils  in  cholesterol,  the  composition  of  the  sat.  solution  was 
estimated  by  means  of  the  specific  gravity  and  the  melting  point. 


Solvent. 


t°  of 
Clouding. 


ms.  Ester 

Gms.  Oil  or  Acid  per  100 
0  ,                           Gms.  Sat.  Solution  in 

per  loo 

Solute.                         Ester, 

Bet.  by: 

'Sp.  Gr. 

M.  pt. 

3-35 

Olive  Oil                    25.5 

33-8 

0.26 

Oleic  Acid                 37 

40 

4.11 

Castor  Oil                   5 

1.85 

o-33 

Ricinic  Acid              20 

16 

0.85 

Pseudo  Ricinic  Acid  10 

12 

0.87 

Crotonic  Acid            (5) 

5 

Olive  Oil  37.6 

Castor  Oil  37.6 

Oleic  Acid  37.5 

Ricinic  (Oil)  Acid      37 
Pseudo  Ricinic  Acid  36 . 2 
Crotonic  (Oil)  Acid   36 . 5 

CHOLINE   PERCHLORATE  and  its  Nitric  Ether. 

100 gms.  H2O  dissolve  about  290 gms.  (CH3)3N(ClO4)CH2CH2.OHat  i5°.)(Hofmann 
100  gms.  H2O  dissolve  o.62'gm.  (CH3)3N(C1O4)CH2.CH2.ONO2  at  15°.  \  HJjJld 
100  gms.  H2O  dissolve  0.82  gm.  at  20°.  J    1911.)' 

CHROMIUM  ALUMS. 

SOLUBILITY  OF  CHROMIUM  ALUMS  IN  WATER  AT  25°.    (Locke,  1901.) 

Per  loo  cc.  Water. 
Formula. 


Grams          Grams  Gram 

Anhydrous.  Hydrated.        Mols. 

Potassium  Chromium  Alum   K^C^SO^^H^O   12.51     24.39    0.0441 
Tellurium  Chromium  Alum    Te2Cr2  (804)4.  24H2O  10.41     16.38    0.0212 

CHROMIUM   CHLORIDES   CrCl3.6H2O. 

SOLUBILITY  OF  THE  GREEN  AND  THE  VIOLET  MODIFICATIONS  IN  WATER  AT  25°. 

(Olie  Jr.,  1906.) 

The  solubility  of  hydrated  chromium  chloride  depends  upon  the  inner  com- 
position of  the  solution,  that  is,  the  relative  amounts  of  the  green  and  the  violet 
modification  of  the  salt  present  in  the  saturated  solution.  These  are  determined 
by  precipitating  with  silver  nitrate.  A  freshly  prepared  solution  of  the  green 
chloride  yields  only  one-third  of  its  chlorine  in  the  cold,  hence  the  composition  of 
this  modification,  according  to  Werner,  is  represented  by  the  formula'  [Cr(H2O)4Cl2] 
C1.2H2O.  The  violet  chloride  is  considered  to  have  the  composition,  [Cr(H2O)e]Cl3. 
A  determination  of  the  amount  of  each  present  involves  precipitating  one  portion  of 
the  solution  at  o°  with  silver  nitrate  and  another  portion  (for  total  Cl)  at  the  boiling 
point.  Experiments  were  first  made  with  aqueous  solutions  of  different  percentage 
composition  of  the  two  modifications.  These  were  agitated  at  25°  and  analyzed  at 
intervals  until  equilibrium  was  reached.  The  time  for  equilibrium  varied  from  18 
to  40  days  according  to  the  concentrations  present.  The  effect  of  temperature 
and  of  the  presence  of  HC1  on  the  transition  of  the  green  chloride  was  also  studied. 

The  equilibrium  in  saturated  solutions  at  25°  was  determined  by  rubbing  the 
hydrated  chromium  chloride  with  a  little  water  previously  cooled  to  o°  to  a  thin 
mush.  This  was  then  agitated  at  25°  and  portions  removed  at  successive  inter- 
vals of  time  and  analyzed.  The  results  show  the  total  chloride  and  per  cent 
present  as  the  green  modification. 


25  Gms.  Green  Salt 
+  10  Gms.  H2O. 

Time  of     Gms.  CrCls     Per  cent 
\gita-     per  100  Gms.    of  Green 


25  Gms.  Violet  Salt       25  Gms.  Violet  Salt  +  locc. 
+  10  Gms.  H2O.       of  35%  Sol.  of  the  Green  Salt. 

Time  of    Gms.  CrCla  Per  cent 
Agita-    per  100  Gms.  of  Green 

Sat.  Sol. 

61.99 

63.88 

70.68 

72.11 

70.62 

In  a  later  paper  Olie  Jr.  (1907)  gives  additional  results  at  29°,  32°  and  35°. 
loocc.anhydr.  hydrazine  dissolve  I3gms.  CrCU  at  room  temp.  (Welsh&Broderson.'is.) 


tion.          Sat.  Sol. 
Ihr.          58.36 
4hrs.         63.27 
i    day       68  .  50 
3    days      68  .  95 
19  days      68  .  58 

Salt.           tion. 

91-7       fchr. 
75.2       i  day 
62.36    4    days 
57-22     7       " 
57-38     26     « 

Salt. 
i-53 
8.46 
30.89 
37.28 
Si-54 

tion. 

ifchr. 
2   days 

5     " 
8      " 

12      " 

Sat.  Sol. 

65.49 

70.47 

76.38 
73.26 
71.14 

Salt. 

15-95 
26.81 

39-34 
34-20 
58-60 

CHROMIUM  TRIOXIDE  250 

CHROMIUM  TRIOXIDE   CrO3. 

SOLUBILITY  IN  WATER. 

(Buchner,  and  Prins,  1912-13;   Kremann,  Daimer  and  Bennesch,  1911;  Koppel  and  Blumenthal,  1907; 
and  Mylius  and  Funk,  1900.) 

,.,  Gms.  CrO3        c  Ud  I  Gms.  CrO3        s  M 

OilQ  4.0  -v«-   ,-.-   f^mf  OOllCl  AO  r^^w  -r^^  C*mo          oOUQ 


-   O.Q          3.6         Ice       -   43-5  49-1        Ice  50          64.55          CrO, 

—  1.9        7-8        "      -  60      53.3  65        64.83 

—  3.7      ii. s        "      -155      60.5       "  +CrO,        82        66 

—  4.8        14.1  "        —    20        61.7  CrO,  90          68.5  " 

—  10.95     24.9        "  o      62.24          "  100        67.4  " 

—  11.7      25.2        "      +  18      62.45          "  115        68.4 
-18.75     33-5         "            24.8  62.88           «  122         70.7 

—  25.25      39.2  "  40        63.50  193-196   IOO         [decomposition 

Density  of  solution  sat.  at  18°  =  1.705. 

100  cc.  anhydrous  hydrazine  dissolve  I  gm.  CrO8  with  evolution  of  gas  and 
production  of  a  black  precipitate  at  room  temp.  (Welsh  and  Broderson,  1915.) 

CHROMIUM  DOUBLE  SALTS. 

SOLUBILITY  IN  WATER. 

Qorgensen,  1879,  1884,  1890;  Struve,  1899.) 

Gms.  per 

Name  of  Salt.  Formula.  t°.       100  Gms. 

H20. 

Chlorotetraamine  Chromium  Chlo- 
ride                                               CrCl(NH3)4(OH2)Cl2             15  6.3 
Chloropurpureo  Chromium  Chloride  CrCl(NH3)5Cl2                       16  0.65 
Luteo  Chromium  Nitrate                     Cr(NH3)6(NO3)3                       ?  2.6 
Chloropurpureo  Chromium  Nitrate    CrCl(NH3)5(NO3)2                 17.5  1.4 
Chromic  Potassium  Molybdate          3K2O.Cr203.i2Mo03.2oH2O  17  2.5 

CHROMIUM  SULFATES   (ous  and  ic). 

SOLUBILITY  IN  WATER. 

Salt.  Gms.  pg^oo  Gms.  Solid  Phase.  Authority. 

Chromous  i2.35(ato0)  CrSO4.7H20  (Moissan,  1882.) 

Chromic  120       (at?0)  Cr2(S04)3.i8H20       (Etard,  1877.) 

CHROMIUM  THIOCYANATE  Cr(CNS)8. 

Data  for  the  distribution  of  Cr(CNS)3  between  water  and  ether  at  o°-3O°  are 
given  by  Hantzsch  and  Vagt,  1901. 

CHRYSAROBIN  CjoHzeOy. 

SOLUBILITY  IN  SEVERAL  SOLVENTS. 

(U.  S.  P.) 

c  ,  Gms.  per  100  Gms.  Solvent  at:  Gms.  per  too  Gms. 

'     as».  8o°.  SolVent>  Solvent  at  25°. 

Water          0.021          0.046                      Chloroform  5.55 

Alcohol        0.324          0.363  (60°)             Ether  0.873 

Benzene       4                   ...                        Amyl  Alcohol  3.33 

Carbon  Bisulfide  o .  43 
CHRYSENE  Ci8Hi2. 

SOLUBILITY  IN  TOLUENE  AND  IN  ABS.  ALCOHOL. 

(v.  Becchi.) 

loo  gms.  toluene  dissolve  0.24  gm.  Ci8Hi2  at  18°,  and  5.39  gms.  at  100°. 
100  gms.  abs.  alcohol  dissolve  0.097  Sm*  CisHi2  at  16°,  and  0.170  gm.  at  boiling 
point. 


251 


CINEOLE 


CINEOLE   (Eucalyptole)   Ci0Hi8O. 

Freezing-point  lowering  data  (solubility,  see  footnote,  p.  i)  for  mixtures  of 
cineole  and  each  of  the  following  compounds  are  given  by  Bellucci  and  Grassi, 
(1913);  phenol,  a.  and  ft  naphthol,  o,  m  and  p  crespl,  o,  m  and  p  nitrophenol, 
o,  m  amidophenol,  pyrocatechol,  resorcinol,  hydroquinone,  guaiacol,  o,  m  and  p 
oxybenzoic  acid,  methyl  salicylate,  phenyl  salicylate,  naphthalene  and  thymol. 

CINCHONA  ALKALOIDS. 

SOLUBILITY  OF  CINCHONINE,  CINCHONIDINE,  QUININE,  AND  QUINIDINE  IN 

SEVERAL   SOLVENTS.      (Muller,  1903;  see  also  Prunier,  1879.) 

Grams  of  the  Alkaloid  per  100  Grams  Solution. 


Solvent.                                                                                                   Quinine 
Cinchonine    Cinchonidine                CjoHwNjO,.                  Quinidine 

f~>       TT       -»T    /-\          f*      TI       XT    C\                                                            A                                                       /"«       IT        KT    f\ 

-19 

23    a    • 

19    n 

Hydrate. 

Anhydride. 

Ether 

0 

.10 

0.211 

I.6l9 

0.876              0.776 

Ether  sat.  with  Hp 

o 

.123 

0-523 

5.6l8 

2.794              1.629 

HjO  sat.  with  Ether 

0 

.025 

0.0306 

0.0667 

0.0847            0.031 

Benzene 

o 

•0545 

0.099 

0.2054 

1.700              2.451 

Chloroform 

o 

.6979 

9.301 

100  + 

100+                100  + 

Acetic  Ether 

0 

.0719 

0.3003 

4.65 

2.469           1.761 

Petroleum  Ether 

0 

•0335 

0.0475 

0.0103 

O.O2II            O.O24I 

Carbon  Tetra  Chloride  o 

.0361 

0-0508 

0.203 

0.529               0.565 

Water 

o 

.0239 

0.0255 

o-574 

0.0506           O-O2O2 

Glycerine  (15^°) 

o 

•50 

0.50 

...                     ... 

SOLUBILITY  OF  CINCHONINE  AND 

CINCHONIDINE'  IN  SEVERAL  SOLVENTS. 

Gms.  Alkaloid  per  100 

Solvent. 

t°. 

Gms 

.  Solvent. 

Authority. 

Cinchonine.    Cinchonidine. 

Water 

ord.  temp 

.     0.0043 

(Hatcher,  1902.) 

u 

20 

0.0131 

(Scholtz,  1912.) 

" 

25 

O.OII3 

0.021 

(Schaefer,  1910.) 

Aq.  10%  Ammonia 

20 

0.025 

... 

(Scholtz,  1912.) 

Aq.  85%  C2H50H+io%  Am. 

20 

0.41 

... 

« 

Aniline 

20 

1.6 

« 

Pyridine 

20 

1.4 

7*78 

(Scholtz,  1912;  Dehn,  1917.) 

50%  Aq.  Pyridine 

20-25 

10 

(Dehn,  1917.) 

Aq.  85%  C2H5OH  (^20=0.832) 

20 

0.86 

.  .  . 

(Scholtz,  1912.) 

C2H5OH  (95%) 

2O 

0.80 

5 

(Wherry  and  Yanovsky.igiS.) 

C2H5OH  (prob.  92.3  wt.  %) 

25 

0.62 

(Schaefer,  1913.) 

Abs.  QjHsOH 

19 

0.874 

(Timofeiew,  1894.) 

Abs.  C2H5OH 

25 

0.89 

(Sill,  1905.) 

Benzene 

25 

0.057 

0.127 

(Schaefer,  1913.) 

Acetone 

25 

0.091 

(Sill,  1905.) 

Chloroform 

17 

0.014 

(Oudemans,  1872.) 

" 

25 

0.606 

19 

(Schaefer,  1913.) 

u 

SO 

0-565 

(Kohler,  1879.) 

Ether 

25 

0-055 

(Sill,  1905.) 

" 

32 

0.264 

(Kohler,  1879.)  » 

Isoamyl  Alcohol  ' 

25 

I.IO 

(Sill,  1905.) 

Isobutyl  Alcohol 

1.09 

. 

(Timofeiew,  1894.) 

Methyl  Alcohol 
Piperidine 

25 
20 

0.785-1. 
3-5 

17       7-39 

(Schaefer,  1913;  Sill,  1905.) 
(Scholtz,  1912.) 

Diethyl  Amine 

2O 

" 

Results  for  the  solubility  of  cinchonine  and  Cinchonidine  in  mixtures  of  ethyl  and 
methyl  alcohols  with  benzene  and  with  chloroform  are  given  by  Schaefer  (1913). 

It  is  pointed  out  by  Schaefer  (1910),  that  if  the  saturated  solution  is  analyzed 
by  shaking  out  with  chloroform  or  ether,  variable  results,  depending  on  the  age 
and  method  of  manufacture  of  the  alkaloid,  will  be  obtained. 

Except  in  the  case  of  the  results  by  Sill  in  the  above  table,  the  saturated  solu- 
tions were  obtained  by  agitating  at  intervals,  instead  of  constantly  at  the  given 
temperature. 


CINCHONA  ALKALOIDS 


252 


SOLUBILITY  OF  CINCHONINE,  CINCHONIDINE  AND  CINCHOTINE  SALTS  IN  WATER. 

Cms.  per  100  Cms.  H2O. 


Salt. 
Hydrobromide 

*"•    Cinchonine    Cinchoni-  Cinchotine                          Authority. 
Salt.        dine  Salt.       Salt. 
25        1.7              I  •  66          ...     (Schaefer,  1910.) 

Bihydrobromide 

25 

55-5          14-3 

Hydrochloride 

25 

4  .  S1             4  .  82        2  .  1  23  (Schaefer,  1910;  Forst  and  Bohringer,  1881.) 

Bihy  drochloride 

25 

62.5             ...     (Schaefer,  1910.) 

Sulfate 

25 

I  .  IT4           I  .o85      3  .  286  (Schaefer,  1910;  Forst  and  Bohringer,  1881.) 

Sulfate 

80 

3.1              4.8            ...     (U.S.  P.) 

Bisulfate 

2S 

66.6          IOO                 ...     (Schaefer,  1910.) 

Perchlorate 

12 

0.3(solvent  =aq.6%  HCIOJ  (Hofmann,  Roth,  Hobold  and  Metzler,  1910.) 

Salicylate 

25 

0.17            0.075        •••     (Schaefer,  1910.) 

Tannate 

2S 

0.091          0.055 

Tartrate 

25 

3  .  127         ...             1  .  768  (Schaefer,  1910;  Forst  and  Bohringer,  1881.) 

Bitartrate 

16 

0.99           ...             1.28    (Forst  and  Bohringer,  1  88  1.) 

Oxalate 

20 

0.96         ...           1.16          "                 " 

i  4.16  at  10°.     *  4  at  15°, 

,     »  at  10°.     *  1.52  at  13°.      •  i  at  15°.      •  at  13°.      T  3  at  16°.      «  at  16°. 

SOLUBILITY  OF  CINCHONINE  SULFATE  AND  OF  CINCHONIDINE  SULFATE  IN 
ALCOHOL  AND  OTHER  SOLVENTS. 

Gms.  per  100  Gms.  Solvent. 
Solvent.  t°. 


Ethyl  Alcohol  (92.3  wt.  %) 
«  «  « 

Methyl  Alcohol 
Chloroform 
Ether 
Glycerol 


25 
60 

25 
25 
25 
15 


(CJBaNjO)r 

H2S04.3H,0. 
0.85  (1.4) 
...     (3-1) 
35-9 

O.I   (O.ll) 
O.O2 


Authority. 


(Schaefer,  1913;  U.  S.  P.) 
(U.  S.  P.) 

(Schaefer,  1913;  U.  S.  P.) 
(Schaefer,  1913;  U.  S.  P.) 
(U.  S.  P.) 


4.2 

9.8  (10) 
...  (19.2) 
83.9 

0.66(1.45) 
0.04 
6.7 

Results  for  mixtures  of  alcohol,  chloroform  and  benzene  are  given  by  Schaefer,  '13. 
Very  carefully  determined  data  for  the  solubility  of  Cinchonine  in  ethyl  alco- 
hol, methyl  alcohol,  amyl  alcohol  and  acetone  solutions  of  various  concentra- 
tions of  a  large  number  of  organic  acids  and  of  phenols  are  given  by  Sill,  1905. 

CINNAMIC  ACID   C6H6CH:CH.COOH. 

loo  gms.  H2O  dissolve  0.0495  gm.  C6H6CH:CHCOOH  at  25°.  (De  Jong,  1909.) 
loo  gms.  H2O  dissolve  0.0607  gm.  C«HiCH:CHCOOH  at  25°.  (Sidgwkk,  1910.) 
loo  cc.  0.5  n  sodium  cinnamate  solution  dissolve  0.155  gm.  C6H5CH:CHCOOH 

at  25°  (Sidgwick,  1910.) 

loo  cc.  sat.  sol.  in  petroleum  ether  (b.  pt.  3O°-7o°)  contain  0.095  Sm-  C6H6CH: 

CH.COOH  at  26°. 

100  cc.  sat.  sol.  in  carbon  tetrachloride  contain  2.172  gms.  C6H6CH:CH.COOH 

at  26°.  (De  Jong,  1909.) 

loo  cc.  sat.  sol.  in  95%  formic  acid  contain  3.76  gms.  C6H6CH  :CH.COOH  at  20°. 

(Aschan,  1913.) 

SOLUBILITY  OF  CINNAMIC  ACID  (Melting  point,  133°)  IN  ALCOHOLS.  (Timofeiew,  1894.) 

Gms.  Cinnamic  Acid  per  100  Gms.  Sat.  Solution  in: 

-18 
-12.5 
o 

+  19-5 
SOLUBILITY  OF  CINNAMIC  ACID  IN  ORGANIC  SOLVENTS  AT  25°.  (Herz  and  Rathmann,  1913.) 


So.ven, 


CH3OH. 

C^OH. 

C3H7OH.         (CH^CH.CHjOH. 

8.1 

6.74 

4-3 

.  .  . 

9-3 

8 

5-5 

.  .  . 

13 

n-3 

8.2 

.  .  . 

22.5 

18.1 

13-4 

8.6 

loo  cc.  Sat.  Sol.  CHC13 


Chloroform  1 2 . 09 

Carbontetrachloride  i .  75 
Trichlorethylene  6 . 04 
Tetrachlorethylene  2.55 
Tetrachlorethane  11.05 
Pentachlorethane  5 . 54 


IOO      C 

C.+      0      CC 

80 

+    20 

50 

+  So 

33-3 

+  66.6 

20 

+  80 

0 

-f-ioo 

n^VTVil 

>cc.Sat. 

Ft  FrrF 
Sol.  l^nC 

\»        C2HC15 

12.09 

IOO      C 

C.+      0      CC. 

9.86 

80 

+    20        " 

6.61 

So 

+    50        " 

4-50 

33-3 

+  66.6" 

3.32 

20 

+  80      " 

1-75 

o 

+  IOO 

per  i  oo  cc. 
Sat.  Sol. 
6.04 
5-91 
5-85 
5-82 
5-70 

5-54 


253  CINNAMIC  ACID 

OINNAMIO   ACID   C6H5CH:CH.COOH. 

SOLUBILITY   OF   CINNAMIC   ACID  IN  AQUEOUS   SOLUTIONS  OF  SODIUM 
ACETATE,  BUTYRATE,  FORMATE,  AND  SALICYLATE  AT  26.4°. 

(Philip  —  J   Chem.  Soc.  87,  992,  '05.) 

Calculated  from  the  original  results,  which  are  given  in  terms  of 
molecular  quantities  per  liter. 


Gms.  NaSalt 

Urns.  (J 

per  Liter  in  bolutio 

us  of: 

per  Liter. 

CH3COONa. 

C3H7COONa. 

HCOONa. 

Ce^.OH.COONa, 

O 

0.56 

0.56 

0.56 

0.56 

I 

1.50 

1-30 

0.92 

0.62 

2 

2.12 

1.85 

1.  12 

0.70 

3 

2.52 

2.25 

1.27 

o-73 

4 

2-85 

2.60 

1.40 

0.77 

5 

3-05 

2.90 

1.47 

0.80 

5  ...  ...  ...  0.90 

i  liter  of  aqueous  solution  contains  0.491  gm.  C6H6CH  :CH.COOH 
at  25°  (Paul). 

SOLUBILITY  OF  'CINNAMIC  ACID  IN  AQUEOUS  SOLUTIONS  OF  ANILIN 
AND  OF  PARA  TOLUIDIN  AT  25°. 

(Lowenherz  —  Z.  physik.  Chem.  25,  394,  '98.) 

Original  results  in  terms  of  molecular  quantities  per  liter. 

In  Aqueous  Anilin.  In  Aqueous  p  Toluidin. 

Grams  per  Liter.  Grams  per  Liter. 


CeHfiCH  :  CHCOOH.  CeH^CHsNIfc.    QHeCH  :  CHCOOH. 

0  0.49  o  0.49 

1  1.20  I  1.52 

2  1.65  2  2.  2O 

3  2.02  3  2.83 

4  2.35  4  3.35 
6                   2.92                           5  3  .80 

"Freezing-point  data  for  mixtures  of  cinnamic  acid  and  dimethylpyrone  and 
for  hydrocinnamic  acid  and  dimethylpyrone  are  given  by  Kendall,  1914. 

BromoCINNAMIC  ACIDS. 

SOLUBILITY  OF  a  AND  OF  /3  BROMOCINNAMIC  ACIDS  IN  WATER  AT  25°. 

(Paul,  1894.) 

Per  looo  cc.  Sat.  Solution. 
Gms.  Millimols. 

a  C6H5CH:  CBrCOOH  3.9325  17.32 

/3C6H5CBr:  CHCOOH  0.5255  2.315 

SOLUBILITY  OF  a  I  so  BROMOCINNAMIC  ACID  IN  AQUEOUS  SOLUTIONS  OF 
OXANILIC  ACID  (Melting  point  =  120°)  AT  25°. 

(Noyes,  1890.) 
Normality  of  Solutions.  Grams  per  Liter. 

C,H5NHCO-  C6H5CH-  QHsNHCO-  QHjCH- 

COOH.  CBrCOOH.  COOH.  CBrCOOH. 

o         0.0176         o        3-995 

0.0275     0.0140       4.54     3.178 
0.0524     0.0129         8.65      2.928 


CINNAMIC  ACIDS 


254 


Allo  CINNAMIC  ACIDS    (Unstable  Isomers  of  Cinnamic  Acid). 
SOLUBILITY  OF  EACH  OF  THE  THREE  ISOMERIC  ALLOCINNAMIC  ACIDS  AND  OF 

THE  MELTS  OF  THE  THREE  ISOMERS  IN  WATER. 

Results  for: 

(Meyer, 

1911.) 

Allocinnamic  Acid     Allocinnamic  Acid 

Allocinnamic  Acid 

Melted 

Allocin- 

of  M.  pt.  68°. 

of  M.  pt.  58°. 

of  M.  pt.  42°. 

namic  Acid. 

(Natural  Isocinnamic  Acid.) 

(Artificial  Isocinnamic  Acid.) 

fco    "  Cms.  Acid 

AO   ~    Gms.  Acid 

+o        Gms.  Acid 

AO         Gms.  Acid 

per  Liter. 

1  '         per  Liter. 

per  Liter. 

i  . 

per  Liter 

18         6.88 

18        7.62 

18        8.95 

18 

I3-63 

25         8.45 

25        9-37 

25       11-03 

25 

14.44 

35       H-I4 

35       I2-39 

35       14-61 

35 

16.05 

45       14.46 

45       16.09 

45 

i8.ii 

55       18.45 

55 

20.55 

These  curves 

intersect  that  for  the  melted  acid  at  the 

65 

23-43 

melting  points  of 

the  solid  isomers. 

75 

27.69 

The  results  show  that  the  three  isomers  are  polymorphic  modifications  of  the 
cis  acid. 

loo  gms.  ligroi'n  (b.  pt.  60-70°)  dissolve  more  than  16  gms.  isocinnamic  acid. 

(Liebermann,  1903.) 

IOO  gms.  ligroi'n  (b.  pt.  60-70°)  dissolve  approx.  2  gms.  allocinnamic  acid.    ' 
SOLUBILITY  OF  a  CHLOROCINNAMIC  ACID,  ETC.,  IN  BENZENE. 

(Stoermer  and  Heymann,  1913.) 


Gms. 

Gms. 

Name  of  Compound. 

M.pt. 

t°. 

Cmpd.  per 
loo  Gms. 

Name  of  Compound. 

M.pt. 

tf. 

Cmpd.  per 
loo  Gms. 

C6H6. 

C6H6. 

a 

Chlor- 

137 

2O 

2.6 

ft  Brom- 

*35 

jo 

1.58 

Allo  a 

Allo  a 
0 

Brom- 
Chlor- 

cin- 
namic 
Acid 

in 

120 
142 

21 
2O 

17 

II 
5-17 

5    6.9 
1.94 

Allo 

cis 
trans 
cis 

Dichlor- 
u 

Dibrom- 

cin- 
namic 
Acid 

159-5 

121 
101 
IOO 

14 
13 

14 
14 

0.86 
6.1 

21.2 
26.9 

Mo  ft 

u 

132 

16 

3-i7 

trans 

" 

136 

14 

10.6 

FREEZING-POINT  DATA  (Solubility,  see  footnote,  p.  i)  FOR  MIXTURES  OF  CIN- 
NAMIC ACID  AND  OTHER  COMPOUNDS,  AND  OF  CINNAMIC  ACID  DERIVATIVES 
AND  OTHER  COMPOUNDS. 

(Bruni  and  Gorni,  1899.) 
(de  Kock,  1904.) 

a  Monochlorcinnamic  Aldehyde  +  a  Monobromcinnamic  Aldehyde     (Kiister,  1891.) 
Cinnamylidine  +  Diphenylbutadiene  (Pascal,  1914.)' 

+  Diphenyldiacetylene  " 


Cinnamic  Acid  +  Phenylpropionic  Acid 
p  Methoxycinnamic  Acid  +  Hydroquinone 


CITRIC  ACID   (CH2)2COH(COOH)3.H20. 

SOLUBILITY  OF   HYDRATED  AND   OF   ANHYDROUS   CITRIC  ACID,   DETERMINED 
SEPARATELY,  IN  AQUEOUS  SOLUTIONS 'OF  ETHYL  ALCOHOL  AT  25°. 

(Seidell,  1910.) 
Results  for  Hydrated  Citric  Acid.  Results  for  Anhydrous  Citric  Acid. 


Wt   °7  C.H  OH         rL  nf        Gms-  (CHo^COH-       Wf   „  r  „  ^u       j      t          Gms.  (CH2)2COH- 
inlS™       Sal!  Sol.  C^^ffi^°        inloS°H    Sats°ol.   (C°°^ll^GmS' 

0 

•311 

67-5 

20 

1.297 

62.3 

20 

.286 

66 

40 

I  .246 

59 

40 

•257 

64-3 

60 

I.I9O 

54-8 

50 

•237 

63-3 

70 

1.160 

52.2 

60 

.216 

62 

80 

i  .120 

48.5 

70 

.192 

60.8* 

90 

1.065 

43-7 

80 

.163 

$8.1* 

IOO 

i  .010 

38.3 

90 

.125 

54.7* 

IOO                  J 

.068 

49-8* 

*  Solid  phase  dehydrated  more  or  less  completely. 

255 


CITRIC  ACID 


SOLUBILITY   OF   HYDRATED  AND   OF   ANHYDROUS   CITRIC  ACID,   DETERMINED 
SEPARATELY,  IN  SEVERAL  ORGANIC  ACIDS  AT  25°.     (Seidell,  1910.) 
Results  for  Hydrated  Citric  Acid.  Results  for  Anhydrous  Citric  Acid. 

GmscoHl2)2"  Gms' 

sf?°Sfol(COOH)3-H°0          Solvent.  <£  §f       <ggsgJH 

•       per  loo  sat.  bol.  periooGms< 

Gms.  bat.  Sol.  Sat.  Sol. 

0.8917  5.980  Amyl  Acetate      0.8861  4.22 

0.8774  *5-43Q  Ether  (abs.)         0.7160  1.05 

0.9175  5.276  Chloroform          1.4880  o 

0.7228  2.174  C6H6,  CS2 

i  .  4850  o  .  007  CCU  or  CeHsCHa  ...  o 


Solvent. 

Amyl  Acetate  of  ^20=0.8750 
Amyl  Alcohol  of  ^20=0.8170 
Ethyl  Acetate  of  d25=  0.89  1  5 
Ether  (abs.)  of  ^22=0.7110 
Chloroform  of  d&  -  1  .  476 

loo  gms.  95%  formic  acid  dissolve  12.25  gms.  citric  acid  at  20°.      (Aschan,  1913.) 
I  oo  gms.  dichlorethylene  dissolve  o.oosgm.  citric  acid  at  15°.  (Wester  &  Bruins,  '14.) 

trichlorethylene  0.012    '  "   . 

"          methyl  alcohol         "      197         gms.      "       "     "19°.        (Timofeiew,  1914.) 

propyl  alcohol         "62.8 

DISTRIBUTION  OF  CITRIC  ACID  BETWEEN  WATER  AND  ETHER.     (Pinnow,  1915.) 


Results  at  15°. 

Mols.  Citric  Acid  per  Liter. 


. 


In  H2O  Layer.  In  Ether  Layer. 

0.902  0.0077 

0.460  0.0036 

O.22O  O.OOI7 

0.297  0.0023 

COBALT  AMINES. 

SOLUBILITY  IN  WATER  AT  ORDINARY  TEMPERATURE. 


IZ7 
128 

I29 

129 


Results  at  25.5°. 

Mols.  Citric  Acid  per  Liter. 

Dist  Coef. 
114 
155 
155 
158 

In  H2O  Layer. 

°v9l75 
0.481 
0.241 

0.315 

In  Ether  Layer. 
0.0063 
0.0031 
0.00155 
0.0020 

(Lai  De,  1917.) 


Name  of  Isomeride. 


Formula. 


Triamine  Cobalt  Nitrate  [(NH3)3Co(NO2)3] 

1.2    Dinitrotetraamine     cobaltitetranitrodi-  ["„  (NO^al'^ 

amine  cobaltiate 
1.6     Dinitrotetraamine 

amine  cobaltiate 
Hexa-amine  cobaltihexanitrocobaltiate 


Gms.  Isom- 

eride  per 

liter  Sat.  Sol. 

2.882 


cobaltitetranitrodi- 


r 

LC° 


(NH,) 


"  "  0.398 

[Co(NH3)6]m—  [Co(NO2)6]I1i       0.0215 


COBALT    DOUBLE    SALTS. 

SOLUBILITY  IN  WATER. 

(Jorgensen  —  J.pr.Chem.  [2]  18,  205,  '78;  19,  49,  '79;  Kurnakoff  —  J.  russ.  phys.  chem.  Ges.  24,  629, 


'92.) 


Name. 


Formula. 


Co(NH3)6Cl3 


Chloro  purpureo  cobaltic  bromide     CoCl(NH3)5Br2 

Bromo  purpureo  cobaltic  bromide     CoBr(NH3)5Br 

Chloro  tetra  amine  cobaltic  chloride 

Chloro  purpureo  cobaltic  chloride    CoC^NH^gCL, 

Chloro  purpureo  cobaltic  chloride    CoCl(NH3)5C 

Chloro  purpureo  cobaltic  chloride 

Luteo  cobaltic  chloride 

Luteo  cobaltic  chloride 

Roseo  cobaltic  chloride 

Roseo  cobaltic  chloride 

Chloro  purpureo  cobaltic  iodide 

Chloro  purpureo  cobaltic  nitrate 

Chloro  purpureo  cobaltic  sulphate 

Nitrato  purpureo  cobaltic  nitrate 


Co(NH3)5(OH2)CI3 
Co(Nttl(C*gC£ 

CoCl(NH3)5I2 

CoCl(NH3)5(NO3)2 

CoCl(NH3)5SO4.2H2O 

Co(NO3)(NH3)(NOa)2 


14.3 
16 


o 

15.5 
46  6 

o 
46-6 

o 

16.2 
19.2 
15 

17.3 
16 


Gms.  Salt 

per  100 

Gms.  H2O. 

0.467 

0.19 

2  .  50 

0.232 

0.41 

i  .03 

4-26 

12  .  74 

16  .  12 

24.87 

2.0 

i  .  25 

o  .75 

o  .36 


COBALT  ACETATE  256 

COBALT  ACETATE  Co(CH3COO)2. 

100  cc.  anhydrous  hydrazine  dissolve  I  gm.  cobalt  acetate  with  evolution  of 
gas'  at  room  temp. 

COBALT   BROMIDE   CoBr2. 

SOLUBILITY  IN  WATER. 

(Etard,  1894.) 


(Welsh  and  Broderson,  1915.) 


59°. 

66  7 


7S°- 

66.8 


97°. 

68.1  (blue) 


Cms.  CoBr2  per  100  gms.  solution 

100  gms.   methyl  acetate    (di*  =  0.935)   dissolve    10.3    gms.   CoBr2  at   18°, 


sat.  solution  =  1.013. 

COBALT  CHLORATE  Co(ClO3)2. 

SOLUBILITY  IN  WATER. 


(Naumann,  1909.) 


Gms. 
to          Co(C103)2 
per  100  Gms. 

Mols. 
Co(C103)2 
per  100 

(Meusser,  1902.) 
Solid  Phase.        t°. 

Solution. 

Mols 

.  H20. 

— 

12 

29 

•97 

3 

.41 

Ice 

18 

— 

21 

53 

•30 

9 

.08 

Co(C103)2.6H20 

21 

— 

19 

53 

,61 

9 

.20 

« 

35 

0 

57 

•45 

10 

•75 

" 

47 

10-5 

61 

•83 

12 

.90 

H 

61 

Gms. 

Mols. 

t°. 

Co(ClO3)2 
per  100  Gms. 

Co(rc!S!2   Solid  phase- 

Solution. 

Mols.  H2O. 

18 

64.19 

14.28     Co(C103)2.4HjO 

21 

64.39 

TACT                     " 

35 

67.09 

16.10 

47 

69.66 

18.29 

61 

76.12 

25-39 

Density  of  solution  saturated  at  1 8°  =  1.861. 
COBALT   PerCHLORATE   Co(ClO4)2.9H2O. 

SOLUBILITY  IN  WATER. 

(Goldblum  and  Terlikowski,  1912.) 
Gms.  Gms. 


r>. 

UKL, 

Gms. 

roo 
H20. 

Solid  Phase. 

t° 

£ 

.tensity  ( 
at.  Sol. 
< 

JU(UUJ2 
per  loo 
5ms.  H2O 

Solid  Phase. 

—  10 

•9 

32 

.67 

Ice 

0 

•564 

IOO 

CoCClO^.sHjO 

-30 

-7 

58 

.16 

" 

7-5 

.566 

101.9 

" 

-62 

.  2  Eutec. 

Ice+Co(C104)2.9H20 

18 

.567 

103.8 

« 

-30 

-7 

83 

.2 

Co(C104)2.9H20 

26 

•581 

113-4 

H 

—  21 

•3 

QO 

.6 

M 

45 

.588 

115 

H 

COBALT    CHLORIDE 


SOLUBILITY  IN  WATER. 

(Etard  —  Compt.  rend.  113,  699,  '91;  Ann.  chim.  phys.  [7]  2,  537,  '94.) 


t°. 

Gms. 
CoCl2  per 
loo  Gms. 

Solid 
Phase. 

t°. 

Gms. 
CoCl2  per                  Solid 
zoo  Gms.                 Phase. 

Solution. 

Solution. 

—  10 

27.0 

CodydHjO  (red) 

35 

38.0    CoC^.Hp  (violet) 

0 

29-5 

14 

40 

41.0 

+  10 

31-5 

«« 

So 

47-o 

20 

33-5 

U 

60 

47-5     CoCL^O  (blue) 

25 

34-5 

it 

80 

49-5 

30 

35-5 

(( 

TOO 

51.0 

SOLUBILITY  OF  COBALT  AMMONIUM  CHLORIDES  IN  WATER. 

(Kurnakoff  —  J.  russ.  phys.  chem.  Ges.  24,  629,  '93;  J.  Chem.  Soc.  64,  ii,  509,  '93.) 

Grams  per  100  Grams  H2O  at: 
o°.  16.9°.  46.6°- 


,,  . 


CoCl3.5NH3.H2O 
CoCl^NH, 


0.232 
16.12 
4.26 


24.87 


1.031 
... 
12.74 


257 


COBALT  CHLORIDE 


SOLUBILITY  OF  COBALT  CHLORIDE  IN  AQUEOUS  HYDROCHLORIC 
ACID  SOLUTIONS  AT  o°. 

(Engel  —  Ann.  chim.  phys.  [6]  7,  355,  '89.) 


Milligram  Mols. 
per  10  cc.  Sol. 

Sp.  Gr.  of 

gQpnftlflBB. 

Gms.  per  100  Gms. 
Solution. 

Gms.  per  100  cc. 
Solution. 

iCoCl2. 

HCL 

CoCl2. 

HCl. 

CoCl2. 

HCl. 

62.4 

O 

I 

•343 

30 

•17 

0 

.00 

40 

•5 

0 

58-52 

3 

•7 

I 

.328 

28 

.62 

0 

.102 

38 

.0 

0-135 

50.8 

ii 

•45 

I 

•299 

25 

•39 

0 

.321 

33 

.0 

0.417 

37-25 

25 

.2 

I 

.248 

19 

•43 

0 

•738 

24 

.2 

0.919 

12.85 

55 

•  O 

I 

.167 

7 

•JS 

z 

.718 

8 

•34 

2.OO 

4-75 

74 

•75 

I 

.150 

2 

.68 

2 

•369 

3 

.08 

2.72 

12.0 

104 

•5 

I 

.229 

6 

•34 

3 

.099 

7 

•79 

3-8i 

25.0 

139 

•o 

I 

•323 

12 

.27 

3 

.829 

16 

.24 

5-07 

SOLUBILITY  OF  COBALT  CHLORIDE  IN  AQUEOUS  ALCOHOL 
AT  11.5°. 

(Bodtker  — Z.  physik.  Chem.  22,  509,  '97.) 

10  gms.  of  CoCl2.6H2O  were  added  to  20  cc.  of  alcohol  and  in  addition 
the  amounts  of  CoCl2  shown  in  the  second  column.  The  solutions  were 
shaken  2  hours,  5  cc.  withdrawn,  and  the  amount  of  dissolved  CoCl, 
determined  by  evaporation  and  weighing. 


Vol.  % 

Gms.  CoCl2 

Gms.  per  5  cc.  Solution. 

Vol. 

% 

Gms.  CoCl2 

Gms.  per  5  cc.  Sol. 

Alcohol. 

Added. 

H20. 

CoCl2. 

Alcohol. 

Added. 

H20. 

CoCl2. 

9x-3 

0 

.0 

I 

•325 

1.168 

99 

•3 

0.612 

0 

.764 

1-459 

98-3 

O 

.0 

I 

•  134 

1.214 

99 

•3 

0.813 

0 

.688 

1.568 

98-3 

O 

•  O 

I 

.068 

1.181 

99 

•3 

I  .022 

o 

•634 

i-7i3 

99-3 

0 

.0 

I 

•045 

1.199 

99 

•3 

I  .240 

0 

•553 

1.831 

99-3 

O 

.194 

O 

.899 

1.204 

99 

•3 

1.446 

o 

•483 

1-943 

99-3 

0 

.400 

O 

.829 

1-325 

99 

•3 

1.650 

o 

.500 

2.183 

100  gms.  sat.  solution  in  alcohol  (6.792  Sp.  Gr.)  contain  23.66  gms. 

CoCL,  So.  Gr.  =   I.OI07.  (Winkler  —  J.pr. Chem. 91.  207, '6*0 


SOLUBILITY  OF  COBALT  CHLORIDE  IN  ORGANIC  SOLVENTS. 


Solvent. 


Acetone 


Ethyl  Acetate 

Ether,  Abs. 

Glycol 

Acetonitrile  18 

Methyl  Acetate         18 

95%  Formic  Acid      20 . 5 

Anhy.  Hydrazine   ±15 


Gms.  per  100  Gms.  Solvent. 

' 

'  CoCl2. 

CoCl2.2H2O. 

0 

9.II 

I7.I6 

22.5 

9.28 

17.06 

25 

8.62 

18 

2-75 

14 

0.08 

.  .  . 

79 

0.26 

... 

0.021 

0.201 

10. 7  (per  100  g.  sol.) 
4.08 
0.369*         ... 

6.2 

I  ... 

dja  sat.  sol.  =  0.938. 


Authority. 

(von  Laszczynski,  1894.) 
(von  Laszczynski,  1894.) 
(Krug  and  McElroy,  1892.) 
(Naumann,  1904.) 

(von  Laszczynski,  1894.) 
« 

(Bodtker,  1897.) 

(de  Coninck,  1905.) 

(Naumann  and  Schier,  1914.) 

(Naumann,  1909.) 

(Aschan,  1913.) 

(Welsh  and  Broderson,  1915.) 


COBALT  CHLORIDE 


258 


SOLUBILITY  OF  COBALT  CHLORIDE  IN  PYRIDINE. 

(Pearce  and  Moore,  1913.) 


r. 

Gm.  CoCl2 
per  too  Gms 
Sat.  Sol. 

Solid 
Phase. 

t° 

p^oo^p^l          t°. 

Gm.  CoCl2 
per  100  Gms 
Sat.  Sol. 

Solid 
•  Phase. 

48 

.2 

0 

C6H5N 

34 

6 

0.749  1.4         74.8 

2. 

037 

1.2 

50 

•  3 

Eutec.  ... 

"+  1.6 

.37 

6 

0.754                78.2 

2. 

276 

" 

45 

0.4185 

1.6 

44 

6 

0.950    '            79.8 

2. 

428 

H 

30 

0.4205 

" 

47 

2 

.O2O 

88 

3- 

284 

" 

.6 

0.4208 

" 

.no 

90  tr. 

Pt.    .. 

"  +CoCl, 

10 

0.4310 

" 

55 

.192 

96.5 

7- 

251 

CoCl2 

0 

0.4307 

« 

60 

.324 

98.8 

7- 

936 

" 

15 

tr 

.  pt.       ... 

1.6+1.4 

64 

2 

.460 

106 

12. 

540 

M 

23 

0.569 

1.4 

68 

.572                 no 

14. 

165 

• 

25 

0-575 

" 

70 

tr. 

pt     .  .  .            "    +1.2 

1.6  =  CoCl2.6CsHsN.      1.4  =  CoCl2.4CsHiN.      1.2  =.CoCl2.2C5H5N. 
COBALT  CITRATES. 


Salt. 


Formula. 


IN  WATER. 

(Pickering,  1915.) 

Gms.  per  TOO  cc.  Sat.  Sol. 
t°.          ~    _         Salt 

Co  ~  (anhydrous). 

Cobalt  Citrate  (normal)     Co3[(COO.CH2)2C(OH)COO]2.2H2O  10  0.08       0.267 

Cobalt  Hydrogen  Citrate  CoH[(COO.CH2)2C(OH)COO]  10  0.20        0.906 

Cobalt  Potassium  Citrate  KCof(COO.CH2)2C  (OH)  COO].  4H2O  10  1.05        5.11 

Cobalt  Potassium  Citrate  K4Co[(COO.CH2)2C(OH)COO]2  10  3.04  31 

COBALT  FLUORIDE  CoF2.4H2O. 

100  gms.  sat.  solution  in  water  contain  2.23  gms.  of  cobalt  fluoride  of  a  variety. 
loo  gms.  sat.  solution  in  water  contain  2.32  gms.  of  cobalt  fluoride  of  0  variety. 

(Costachescu,  1910.) 

OOBALT   IODATE   Co(IO3)2. 

SOLUBILITY  IN  WATER. 

(Meusser  —  Ber.  34,  2435,  '01.) 
Solid  Phase  : 

Co(IO3)2.2H2O. 


Co(IO3>.4H2O. 


Co(IO3)2. 


G. 

o-54 
0.83 
1.03 
1.46 
1.86 
2.17 


M. 

O.O28 
0.038 
0-046 
0.065 
0.084 
0-098 


G. 

M. 

G. 

M. 

0.32 

O.OI4 

o-45 

0.020 

1.03 

0.046 

0.52 

0.023 

0.89 

0.040 

0.67 

0.030 

0.85 

0.030 

O 

18 

30 
So 
60 

65 
75 
100 

G  =  Gms.   Co(IO3)2  per   100  gms.   solution. 
per  100  Mols.  H2O. 

OOBALT   IODIDE   CoI2. 

SOLUBILITY  IN  WATER. 

(Etard  —  Compt.  rend.  113,  699,  '91;  Ann.  chim.  phys.  [7]  2,  537,  *g4<) 

The  accuracy  of  these  results  is  doubtful. 


0.84 

1.02 


0.038 
0.045 


o-7S 
0.69 


0-033 
0-031 


M  =  Mols.  Co(IO8)8 


Gms.  CoI2 

f. 

per  100  Gms. 
Solution. 

-10 

55-5 

O 

58.0 

10 

61-5 

15 

63.2 

20 

65-2 

2$ 

67 

Solid  Phase. 


25 
30 
40 

50 
80 

no 


Gms.  CoI2 

per  100  Gms. 

Solution. 

67-5 
7O.O 

75-o 
79.0 
80.0 
81.0 


Solid  Phase. 

(olive) 

ii 

CoI2.H20  (yellow) 


259  COBALT  MALATE 

COBALT  MALATE  Co(COO.CH2.CHOHCOO).2H2O. 

ioo  cc.  sat.  solution  in  water  contain  0.14  gm.  Co  =  0.453  gm-  anhydrous  salt 
at  10°.  (Pickering,  1915.) 

COBALT  MALONATES. 

SOLUBILITY  OF  COBALT  MALONATES  IN  WATER. 

(Lord,  1907.) 

Gms.  Anhy- 
Satt.  FomuJa.  f.        ££**.. 

Sat.  Sol. 

Cobalt  Malonate  CoCH2(COO)2.2H2O  18  1.353 

"      Ammonium  Malonate         Co(NH4)2[CH2(COO)2]2.4H2O         18  10.61 

"      Caesium  "  CoCs2[CH2(COO)2]2.4H2O  18  14.23 

"      Potassium  "  CoK2[CH2(COO)2]2.4H2O  18  4.26 

OOBALT    NITRATE   Co(NO3)2. 

SOLUBILITY  IN  WATER. 

(Funk  —  Wiss.  Abh.  p.  t.  Reichanstalt  3,  439,  *oo.) 
Gms.  Mols.  Gms.  Mols. 

*' •  PS°Sf^.(52^>     **""-•         •'•  P£»S.  C^S  *»«*- 

Solution.     Mols.H2O.  Solution.       Mols.H2O. 

—  26          39-45        6.40      Co(NO3)2.QH2O  41      55.96        12.5      Co(NO3)2.6H2O 

-20.5    42-77      7-35  "  56    62.88      16.7 

—  21  41-55        6-98      Co(NO3)2.6HaO  55      61.74        15.8      Co(NOa)2.3HaO 

—  io        43.69      7.64  "  62    62.88      16.7 
-  4        44.85       7.99             "  70    64.89       18.2 

o        45-66      8.26  "  84    68.84      21.7 

+  18        49.73      9.71  91     77-21      33-3 

Density  of  solution  saturated  at  18°  =  1.575. 

SOLUBILITY  OF  COBALT  NITRATE  IN  GLYCOL. 

(de  Coninck,  1905.) 

ioo  grams  saturated  solution  contain  80  gms.  cobalt  nitrate. 
COBALT  RUBIDIUM  NITRITE   Rb3Co(NO2)6.H2O. 

ioo  gms.  H2O  dissolve  0.005  Sm-  of  the  salt.  (Rosenbladt,  1886.) 

COBALT  OXALATE  Co(COO)2. 

ioo  gms.  95%  formic  acid  dissolve  0.04  gm.  Co(COO)2  at  19.8°.     (Aschan,  1913.) 
COBALT  SULFATE  CoSO4.7H2O. 

SOLUBILITY  IN  WATER. 

(Mulder;  Tobler,  1855;  Koppel,  Wetzel,  1905.) 


Gms.  CoSO4  per 
t°.                    ioo  Gms. 

Mols.  CoSO4. 
per  ioo 

Gms.  CoSO4  per 
t°.                       ioo  Gms. 

Mols.  CoSO, 
per  ioo 

Solution. 

Water.' 

Mols.  H2O 

Solution. 

Water. 

Mols.  H2O. 

0 

20-35 

25-55 

2.958 

35 

31.40 

45-80 

5-31 

5 

21.90 

28.03 

3-25I 

40 

32.81 

48.85 

5.664 

10 

23.40 

30-55 

3-540 

50 

35.56 

55-2 

15 

24.83 

33-05 

3.831 

60 

37.65 

60.4 

20 

26.58 

36.21 

4.199 

70 

39-66 

65-7 

25 

28.24 

39-37 

4.560 

80 

41.18 

70 

... 

30 

29.70 

42.26 

4.903 

IOO 

45-35 

83 

•  •  • 

IOO  gms.  H2O  dissolve  37.8  gms.  CoSO4  at  25°.  (Wagner, '1910.) 

Freezing-point  data  (solubility,  see  footnote,  p.  i)  for  mixtures  of  CoSC>4  + 

Li2SO4,  CoSO4  +  K2S04  and  CoSO4  +  Na2SO/are  given  by  Calcagni  and  Marotta 

(1913). 


COBALT   SULFATE 


260 


SOLUBILITY  OP  MIXTURES  OP  CoSO4.7H2O  AND  Na2SO4.ioH2O 

IN  WATER. 

(Koppel;  Wetzel.) 


Gms.  per 
^o^            ioo  Gms.  Solution. 

Gms.  per 
ioo  Gms.  H2O. 

Mols.  per 
ioo  Mols.  H2O. 

Solid  Phase. 

'CoSO4.        Na2SO4. 

rCoS04. 

Na2SO4. 

CoSO4. 

Na2SO4. 

0 

5 

16 
17 

•56 
.46 

9-59 

21.85 
23-94 

10 

•07 

2 

2 

•54 

•77 

I 
I 

•27 
.67 

CoS04.7H20  + 
Na2S04.ioH2O 

10 

.90 

n-73 

25-41 

16 

•67 

2 

•94 

2 

.11 

.. 

20 

17 

•59 

16.43 

26.65 

24 

.91 

3 

.09 

3 

.15 

CoNa2(S04)2.4H20 

25 

17 

.06 

I5-70 

25.36 

23 

•32 

2 

•95 

2 

•97 

" 

30 

J5 

•94 

14-93 

23  -!5 

21 

.61 

2 

•7o 

a 

•74 

«« 

35 

15 

•73 

14.52 

22.54 

20.85 

2 

.62 

2 

.64 

" 

40 

14 

•87 

14.22 

20.98 

2O 

•05 

2 

.46 

2 

•53 

» 

18-5 

18 

•75 

15.61 

28.61 

23 

.82 

3 

•32 

3 

.02 

CoNa2(SO4)2.4H2O 

20 

19 

•30 

15.10 

29.42 

23 

.01 

3 

.41 

2 

.92 

+  CoSO4.7H2O 

25 

20.30 

13.60 

30-74 

20 

•58 

3 

•56 

2 

.61 

30 

21 

.67 

12.05 

32.70 

18 

•17 

3 

•79 

2 

•30 

„ 

35 

22 

.76 

10.43 

34.06 

15 

.61 

3 

•95 

I 

.98 

M 

40 

24 

•05 

9.16 

35-oi 

13 

.72 

4 

.81 

I 

•74 

" 

18.5 

16 

.87 

16.97 

25-50 

25 

•65 

2 

.96 

3 

•25 

CoNa2(S04)2.4H2O 

20 

15 

.41 

18.12 

23.18 

27 

.26 

2 

.69 

3 

•45 

+Na2S04.ioH2O 

25 

10 

•63 

23.26 

16.07 

35 

17 

I 

.86 

4 

.46 

lt 

30 

6 

.01 

28.67 

9.20 

43 

•74 

I 

.07 

5 

•54 

M 

35 

4 

•56 

32.14 

7.19 

50 

79 

O 

•835 

6 

•44 

CoNa2(SO4)2.4H2O 

40 

4 

.72 

3I-78 

7-45 

So- 

10 

o 

.864 

6 

•34 

+  Na2SO4 

SOLUBILITY  OF  COBALT  SULPHATE  IN  METHYL  AND  ETHYL  ALCOHOL 

AND  IN  GLYCOL. 


Solvent. 


Methyl  Alcohol  (abs.) 


3 
15 
18 

(93-5%)  3 

(50%)  3 

Ethyl  Alcohol  (abs.)  3 

Glycol 


Gms.  per  100  Gms. 
Solvent. 


Observer. 


CoSO4.      CoSO4.7H2O. 

.  .  „  42  .8      (deBruyn — Z.  physik.Ch.  10,  784,  '92.) 

50.9 

1-04          54-5 
i3-3 
1.8 
2.5 

o  .  (per  100  gmS.  (de  Coninck—  Bull. acad.  roy .  Belgique, 

solution)  3 .  i          359.  '05-) 


COBALT  SULFIDE  CoS. 

One  liter  water  dissolves  0.00379  Sm-  CoS  at  18°  (electrolytic  conductivity 
method,  assuming  complete  dissociation  and  hydrolysis).  (Weigel,  1906.) 


261 


COCAINE 


COCAINE  C17H21N06. 

SOLUBILITY  IN  SEVERAL  SOLVENTS. 


Solvent. 


Water 


50%  Glycerol 


Gms.  CnH21NO, 
t°.             per  zoo  Gms.                      Authority. 

Solvent. 

2O 

0.028 

(Zalai,  1910.) 

±20 

0.140 

(Baroni  and  Barlinetti,  1911.) 

25 

0.17 

(U.  S.  P.) 

80 

0.38 

« 

±20 

8 

(Baroni  and  Barlinetti,  1911.) 

25 

2O 

(U.  S.  P.) 

25 

26.3 

" 

18-22 

n.  6 

(Muller,  1903.) 

l8-22 

34 

» 

18-22 

0.254 

" 

20 

76 

(Scholtz,  1912.) 

2O 

31-94 

(Gori,  1913.) 

18-22 

100  + 

(Muller,  1903.) 

18-22 

100 

» 

18-22 

59 

«• 

18-22 

2-37 

" 

20-25 

80+ 

(Dehn,  1917;  Scholtz,  1912.) 

20 

56 

(Scholtz,  1912.) 

20 

36 

" 

20 

4-34* 

(Zalai,  1910.) 

25 

8-3 

(U.  S.  P.) 

25 

7.1 

" 

*  Per  too  cc. 

3  Cms.  H3BO3  in  A< 
Alcohol  (92.5  Wt.  %) 

Ether 

« 

Ether  sat.  with  H2O 

Water  sat.  with  Ether 

Aniline 

Carbon  Tetrachloride 

Chloroform 

Benzene 

Ethyl  Acetate 

Petroleum  Ether 

Pyridine 

Piperidine 

Diethylamine 

Sesame  Oil 

Olive  Oil 

Oil  of  Turpentine 


COCAINE  HYDROCHLORIDE  C17H21NO4.HC1. 

100  gms.  H2O  dissolve  250  gms.  of  the  salt  at  25°  and  1000  gms.  at  80°.  (U.  S.  P.) 

100  gms.  92.3%  alcohol  dissolve  38  gms.  salt  at  25°  and  71  gms.  at  60°.  (U.  S.  P.) 

100  gms.  chloroform  dissolve  5.4  gms.  salt  at  25°.  (U.S. P.) 

100  gms.  glycerol  dissolve  25  gms.  salt  at  15°.  (B.  P.) 

COCAINE  PERCHLORATE   C17H2iNO4.HClO4. 

100  gms.  H2O  (containing  8%  free  HC1O4)  dissolve  0.26  gm.  perchlorate  at  6°. 

(Hofmann,  Roth,  Hobold  and  Metzler,  1910.) 

CODEINE   Ci8H21NO3.H2O. 

CODEINE  PHOSPHATE   Ci8H2iNO3.H8PO4.2H2O. 

CODEINE   SULFATE    (Ci8H2iNO3)2.H2SO4.5H2O. 

SOLUBILITY  OF  EACH  SEPARATELY  IN  SEVERAL  SOLVENTS. 

Gms.  per  100  Gms.  Solvent. 

e. 

(U.  S.  P.;  Baroni  and  Barlinetto, 

(Zalai.  1910.)  [1911-) 

(U.  S.  P.) 

(Schaeffer,  1913;  U.  S.  P.) 

(U.  S.  P.) 

(Schaeffer,  1913.) 


Solvent. 


Water 


Alcohol  (92.3  Wt.  %) 


25 

20 
80 

25 
60 

25 
25 
20 

25 
25 

Codeine, 
o  .  80-1  .  7 
0.84 
1.70 

63.7 
108.7 
62.8 

2.94-1.33 
8 
11.4 

12 

C.  Phos- 
phate. 

44-9 

227 

0.383 
1.03 

O.OI5 
0.075 

C. 

Sulfate. 

3-3 
16" 

O.I 

0.27 
0.56 
0.007 

Insol. 

Authority. 


Methyl  Alcohol 

Chloroform 

Carbon  Tetrachloride 

Ether 

Benzene 

Trichlorethylene 

3  Gms.  HsBOs  per  100  cc. 

aq-  50%  Glycerol  ord.  t. 

loo  gms.  trichlorethylene  dissolve  0.014  £m-  codeine  hydrochloride  at  15°. 

(Wester  and  Bruins,  1914.) 

Data  for  the  solubility  of  codeine  and  codeine  sulfate  in  mixtures  of  alcohols, 
benzene  and  chloroform  are  given  by  Schaeffer  (1913). 


0.007  (Schaeffer,  U.  S.  P.) 

(Gori,  1913;  Beilstein,  Suppl.) 
(U.  S.  P.) 
(Schaeffer,  1913.) 
(Wester  and  Bruins,  1914.) 

(Baroni  and  Barlinetto,  1911.) 


COLCHICINE 


262 


COLCHICINE  C22H25N06. 

SOLUBILITY  IN  SEVERAL  SOLVENTS. 

(Mliller,  1903;  U.  S.  P.) 
Gms. 

Solvent. 


Solvent. 


Gms. 


Water 


Ether 


sat.  with  H2O 


18-22 

25 

80 

82 

18-22 

25 
1 8-2  2 


per  100  Gms. 

Solvent. 

9.6 

4-5 


0.13 
0.64 
0.18 


Water  sat.  with  Ether  18-22 

Benzene  18-22 

Benzene  25 

Chloroform  18-22 

Carbon  Tetrachloride  18-22 

Ethyl  Acetate  18-22 

Petroleum  Ether  18-22 


per  100  Gms. 
Solvent. 
12.05 
0.94 

I  -IS 
IOO+ 
O.I2 

'•34 
0.06 


Beilstein. 


COLCHICINE  SALTS. 

Name. 


Formula. 


Solvent. 


Colchicine  lodohydrate         C22H25NO6.HI     Water 
Iso  Colcnicine  lodohydrate 


Gms.  Salt 
per  Liter 
Sat.  Sol. 


30 
30 


Authority. 
(Pfannl,  1911.) 


0.84 

3-86 

o .  083    (Jensen,  1913.) 

0.007  " 


COLLIDINE    (2.4.6  Trimethyl  Pyridine)  C6H2N(CH8)8. 
SOLUBILITY  IN  WATER. 

(Rothmund,  1898.) 
Gms.  Collidine  per  100  Gms. 
Aq.  Layer.     Collidine  Layer. 

5.7  crit.  t.  17.20 

7.82          41.66 

54.92 
62.80 


Gms.  Collidine  per  100  Gms. 


10 
20 

30 
40 
60 


3.42 
2.51 
1.93 
1.76 


70.03 
80.19 


Aq.  Layer. 

Collidine  Layer. 

80 

i-73 

86.12 

100 

i!78 

88.07 

120 

1.82 

88.98 

I4O 

2.19 

89.10 

160 

2-93 

87.2 

180 

3-67 

... 

COLLIDINE    (1.3.5  Trimethyl  Pyridine)  C6H2N(CH3)3. 

DISTRIBUTION  BETWEEN  WATER  AND  TOLUENE. 

(Hantzsch  and  Vagt,  1901.) 


G.  Mols.  Collidine  per  Liter. 


G.  Mols.  Collidine  per  Liter. 


t°. 

H20  Layer. 

Toluene 
Layer. 

Dist.  Coef. 

t°. 

H2O  Layer 

Toluene 
Layer. 

Dist.  Coef. 

o 

0.0035 

0.0580 

0.0603 

50 

0.0017 

0.0596 

0.0285 

10 

O.OO26 

0.0587 

0.0443 

70 

O.OOI5 

0.0597 

0.0251 

20 

O.OO22 

0.0588 

0.0374 

90 

0.0013 

0.0598 

0.0218 

30 

0.0020 

0.0594 

0.0337 

CONGO   RED   [C6H4.N:N.CioH6(NH2)SO3Na]2. 

100  gms.  H2Q  dissolve  n.6  gms.  congo  red  at  2O°-25°.  (Dehn,  1917.) 

100  gms.  pyridine  dissolve  0.29  gm.  congo  red  at  20-25°. 

100  gms.  aq.  50%  pyridine  dissolve  7.32  gms.  congo  red  at  20-25°.  " 

CONIINE    (aPropyl  Piperidine)    C8HnN. 

100  gms.  H2O  dissolve  1.83  gms.  coniine  at  20°.  (Zalai,  1910.) 

COPPER  ACETATE  Cu(C2H3O2)2H2O. 

100  gms.  glycerol  (d^  =  1.256  =  96%)  dissolve  10  gms.  copper  acetate  at 
I5°-l6°.  (Ossendowski,  1907.) 


263  COPPER  ACETATE 

SOLUBILITY  OF  ANHYDROUS  COPPER  ACETATE  IN  PYRIDINE. 

(Mathews  and  Benger,  1914.) 


t°.  per  100  Gms.         Solid  Phase.  t°.         per  100  Gms.         Solid  Phase 

Sat.  Sol.  Sat.  Sol. 


—  1  1.  6  0.37       CutQHsOz^CsHsN  45.2  4.17 

+    2  0.6  "  34.8  3.75        Cu(C5H302)2.CsH6N 

13  I-°3  55-7  4-13 

26.45          Z-6I  64-3  4.48  " 

37-4  2.83  "  76.2  4.83 

41.9  3.12  83.3  5.40 

43-2  3-39  95-4  6.31 

Transition  point  =  44.7°. 

COPPER  ^BROMIDE    (ous)   Cu2Br2. 

SOLUBILITY  OF  CUPROUS  BROMIDE  IN  AQUEOUS  SOLUTIONS  OF  POTASSIUM 
BROMIDE  AT  i8°-2O°. 

(Bodlander  and  Storbeck,  1902.) 
Millimols  per  Liter.  Grams  per  Liter. 


KBr. 

Total  Cu. 

Total  Br.       Cu  (ic). 

Cu  (ous). 

KBr. 

Total  Cu. 

Cu  (ic). 

Cu  (ous). 

0 

O 

•3157 

0.4320    o 

.2096 

0.1061 

0 

O.O2OI 

O 

•0133 

0.0067 

25 

0 

.119 

0 

.012 

0.107 

2 

.98 

O.OO76 

0 

.0007 

0.0068 

40 

0.200 

.'  .  .            0 

•013 

0.187 

4 

.76 

O.OI27 

0 

.0007 

O.OII9 

60 

O 

.310 

0 

•025 

0.285 

7 

•15 

O.OI97 

0 

.0015 

O.OlSl 

80 

0 

•423 

0 

.012 

0.411 

9 

•53 

O.0266 

0 

.0007 

O.026l 

IOO 

0 

•584 

.  .  . 

0.584 

ii 

.91 

0.0371 

.  .  . 

0.0371 

120 

0 

•693 

.  .  . 

0.693 

14 

.29 

0.0441 

0.0441 

500 

8 

.719 

.  .  . 

8.719 

59 

•55 

0-5540 

0.5540 

loo  gms.  acetonitrile  dissolve  3.86  gms.  Cu2Br2  at  18°. '  (Naumann  and  Schier,  1914.) 
Freezing-point  lowering  data  for  mixture  of  CuBr  +  KBr  are  given  by  de 
Cesaris,  1911. 

COPPER  BROMIDE    (ic)  CuBr2. 

IOO  gms.  acetonitrile  dissolve  24.43  £ms'  CuBr2  at  18°.     (Naumann  and  Schier,  1914.) 
ioo  gms.  95%  formic  acid  dissolve  0.16  gm.  CuBr2  at  21°.  (Aschan,  1913.) 

COPPER   CARBONATE   Basic. 

SOLUBILITY  IN  AQUEOUS  CO2  SOLUTIONS  AT  30°. 

(Free,  1908.) 

Aq.  0.5  n  Na2COs  and  0.5  n  CuSCX  were  mixed  and  the  precipitate  washed  and 
suspended  in  H2O  containing  CO2  at  a  pressure  slightly  above  atmospheric,  for 
3  days.  The  filtered  precipitate  was  kept  in  water  ready  for  use.  In  the  fresh 
condition  or  dried,  the  molecular  ratio  of  the  constituents  was  found  to  be  iCuO: 
0.515  CO2:  0.61  H2O.  For  the  solubility  determinations,  about  2  gms.  of  the 
precipitate  were  suspended  in  600  cc.  of  H2O  and  CO2  passed  in  to  the  desired 
concentration.  The  mixture  was  shaken  frequently  for  3  days.  The  total  COg 
in  the  sat.  solution  was  determined  and  the  free  CO2  calc.  by  difference,  assuming 
that  the  amount  combined  to  the  Cu  was  in  the  molecular  ratio  2CuO:iCO2. 

Parts  per  Million.  Parts  per  Million. 

Free  CO2.  Metallic  Cu.  Free  CO2.  Metallic  Cii. 

o  =  pure  H^O  i .  5  859       28 

157  8.3  961       31 

277  13-7          1158       33-7 

348  17  1224       34.8 

743  25.7  1268-1549  35-3-39-7* 

*  Saturated  with  CO2  at  i  +  atmosphere. 

Results  practically  identical  with  the  above  were  obtained  for  a  NaCl  solu- 
tion containing  ioo  parts  per  million.  Data  for  other  concentrations  of  NaCl 
and  for  other  salts  are  also  given.  Salts  with  a  common  ion  depress  the  solubil- 
ity. Those  with  no  common  ion  increase  it  slightly.  A  recalculation  of  the 
results  of  Free  is  given  by  Seyler  (1908). 


COPPER  CARBONATE  264 

SOLUBILITY  OF  MIXTURES  OF  COPPER  CARBONATE  AND  POTASSIUM 
CARBONATE  IN  WATER  AT  25°. 

(Wood  and  Jones,  1907-08.) 

ioo  gms.  H2O  dissolve  3.15  gms.  CuCO3  +  105  gms.  K2CO3  at  25°  when  the 
solid  phase  in  contact  with  the  solution  is  CuCO3.K2CO3  +  K2CO3. 

Additional  points  on  the  curves  were  determined  but  the  analytical  data  are 
not  given.  The  following  approximate  values  were  read  from  the  curve  for  the 
double  salt,  CuCO3.K2CO3: 

Gms.  per  ioo  Gms.  H2O. 

, • —• %  Solid  Phase. 

K2CO3.  CuCO3. 

105  3.15  KgCOrf  CuCO3.K2CO3 

.100  3.20  CuCO3.K2CO3 

90  3.40 

85  3-6o 

The  triple  point  for  double  salt  +  CuCO3  could  not  be  determined  since 
CuCO3  is  not  capable  of  existing  alone  and  decomposes  into  CO2  +  Cu(OH)a. 

COPPER  CHLORATE    (ic)   Cu(ClO3)2.4H2O. 

SOLUBILITY  IN  WATER. 

(Meusser,  1902.) 

Gms.  Mols.  Gms.  Mols. 

t°.  Cu(ClO3)2       Cu(ClO3)2     Solid  Phase.  t°.  '  Cu(ClO3)2       Cu(ClO3)2    Solid  Phase, 

per  ioo  Gms.  per  ioo  Mols.  per  ioo  Gms.  per  ioo  Mols.    ^ 
Solutions.           H2O.  Solutions.  H26. 

-12  30.53  3.43  Ice  l8          62.17          12.84  CuCClO,),.^© 

-3i          54-59          9-39    Cu(ClO3)2.4H2O      45        66.17        15.28 

-21  57.12  10.41  "  59.6      69.42  17.73  " 

-f  0.8      58.51        11.02  ."  71        76.9         25.57  1 

Density  of  solution  saturated  at  18°  =  1.695. 

COPPER   CHLORIDE   (ic)   CuCl2.2H2O. 

SOLUBILITY  IN  WATER. 

(Reicher  and  Deventer,"  1890;  see  also  Etard,  1894.) 

Gms.  CuCl2  Gms.  CuCl2  Gms.  CuClj 

t°.  per  ioo  Gms.  t°.  per  ioo  Gms.  t°.  per  ioo  Gms. 

Solution.  Solution.  Solution. 

—  40  Eutec.     36.3  20  43.5  50  46.65 

o  41.4  25  44  60  47.7 

10  42.45  30  44.55  80  49.8 

17  43-°6  40  45-6  ioo  51.9 

Density  of  solution  saturated  at  o°  =  1.511,  at  17.5°  =  1.579. 
ioo  gms.  sat.  solution  in  water  contain  43.95  gms.  CuCl2  at  30°,  solid  phase, 
CuCl2.2H2O.  (Schreinemakers,  1910.) 

COPPER   CHLORIDE   (ous)   CuCl. 

ioo  gms.  H2O  dissolve  1.52  gms.  CuCl  at  25°.  (Noss,  1912.) 

SOLUBILITY  OF  CUPROUS  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  HYDROCHLORIC 
ACID  CONTAINING  CuCl2  AT  25°. 

(Poma,  1909,  1910.) 

Results  for  i  n  HC1.  Results  for  2  n  HC1.  Results  for  4  n  HC1. 

Mols.  per  Liter.  Mols.  per  Liter.  Mols.  per  Liter. 


CuCl,  • 
Added. 

CuCl2+CuCl.  Phase. 

Added.      CuCl2+CuCl.  Phase.         C 

dded.    CuCla+CuCl. 

SOlld 

.  Phaser 

0 

0.0862      CuCl 

0 

o 

.  2365      CuCl 

0 

0 

.7704 

CuCl 

0 

.1 

0.2017 

O 

.094 

0 

.3528    " 

0 

•095 

0 

.9044 

" 

0 

.2 

0.3256         « 

o 

.188 

0 

.4766     " 

0 

.189 

I 

.0370 

M 

0 

•4 

0.5707         « 

0 

•  235 

0 

•5385    " 

o 

•379 

I 

.3040 

" 

o 

•  5 

0.6924 

o 

.282 

0 

.6038     " 

0 

•473 

I 

.4380 

« 

265 


COPPER  CHLORIDE 


SOLUBILITY  OP  CUPROUS  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OP  HYDRO- 
CHLORIC ACID. 

(Engel  —  Ibid.  [6]  17.  372,  '89;  Compt.  rend.  121,  529,  '95.) 


Milligram  Mols.  jjer  10  cc.  Sol. 

iCu2Cl2. 

HCl. 

Results  at  o°. 

o-475 

8-975 

i-5 

17-5 

2.9 

26.O 

4-5 

34-5 

8.25 

47-8 

15-5 

68.5 

104.0 

Results  at 

i5°-i6°. 

7-4 

54-4 

10.8 

68.9 

12.8 

75-o 

16  o 

92.0 

Sp.  Gr.  of 
Solutions. ' 


Gms.  per^ioo  cc.  Sol. 
'Cu2Cl2/ HCL 


Cms,  per  100  Cms.  Sol. 
'      HCL 


I 

•05 

0.471 

0 

•327 

o 

.448 

0 

.312 

I 

.049 

i 

.486 

0 

.638 

i 

.418 

0 

.608 

I 

.065 

2 

.872 

0 

.948 

2 

.697 

0 

•932 

I 

.080 

4 

•457 

I 

•257 

4 

.127 

I 

.!64 

I 

•135 

8 

.172 

I 

•743 

7 

.199 

i 

I 

.261 

15 

•7 

2 

•497 

12 

.46 

i 

^80 

I 

•345 

32 

.68 

3 

.827 

24 

•30 

2 

•845 

I 

.19 

7 

•33 

I 

•983 

6 

•159 

I 

.666 

I 

.27 

10 

.69 

2 

•5" 

8 

.422 

I 

•977 

I 

.29 

12 

.68 

2 

•734 

9 

.826 

2 

.119 

I 

•38 

J5 

.84 

3 

•346 

ii 

.48 

2 

•424 

SOLUBILITY  OF  CUPRIC  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OP  HYDRO- 
CHLORIC ACID  AT  o°. 

(Engel  —  Ann.  chim.  phys.  [6]  17,  351,  '89.) 
Milligram  Mols.  per  10  cc.  Sol.        Sp  Gr.  of          Gms.  per  100  cc.  Sol.          Gms.  per  100  Gms.  Sol. 


iCud2. 

HCl.                    Solutions. 

CuCl2. 

HCl. 

CuCl2. 

HCI: 

91 

•75 

O 

1.49 

61 

.70 

o. 

0 

41 

•  41 

o.o 

86 

.8 

4 

•5              *-475 

58 

•37 

I. 

64 

39 

•58 

1  .11 

83 

.2 

7 

.8 

.458 

55 

•95 

2. 

84 

38 

•37 

1  .95 

79 

•35 

10 

•5 

•435 

53 

•37 

3- 

83 

37 

.19 

2.67 

68 

•4 

20 

•25 

•389 

46 

.01 

7- 

38 

33 

.11 

50 

•  o 

37 

•3*9 

33 

.62 

13- 

67 

25 

•5o 

10.37 

22 

.8 

70 

•25 

.231 

15 

•33 

25- 

61 

12 

.46 

20.80 

23 

•5 

102 

.288 

.81 

37- 

36 

12 

.27 

29.00 

26 

•7 

128 

•  O 

•323 

17 

.96 

46. 

66 

13 

•57 

35  -26 

29 

•  o 

Sat 

.HCl 

COPPER  CHLORIDE,  AMMONIUM  CHLORIDE  MIXTURES  IN  AQUEOUS 
SOLUTION  AT  30°. 

(Meerburg  —  Z.  anorg.  Chem.  45,  3,  '05.) 


Grams  per  100 
Gms.  Sat.  Solution. 

CuCl2. 
0 

NEUCl.' 

29-5 
28.6 

3-6 
10.5 

25-9 
I6.5 

19.9 

9-4 

29.4 

4-9 

41.4 

2.1 

43-2 

2-0 

43-9 

0 

Grams  per  100 
Gms.  Solid  Phase. 

'CuCl2. 


6.0 
37-o 
21.7 
28.5 
35-i 
43-1 


48.2 

34-9 
23-1 
18.4 

15-3 

13-3 

6.6 


Solid  Phase. 

NH^Cl 
NH«C1  +  CuCl2.2NH4Cl.2H2O 


Cud8.2NH4Cl.aH20 + Cud2.iH,O 


Additional  determinations  for  the  ammonia  end  of  this  system  at  25°  are 
given  by  Foote,  1912. 


COPPER  CHLORIDE 


266 


COPPER  AMMONIUM  CHLORIDE   CuCl2.2NH4C1.2H2O. 


•io. s 
-10.8 
•ii 
•io 
o 

12 
20 


per  100  Gms. 
Solution. 

3.87 
2O.  12 
20.3 
20.46 
22.O2 
24.26 
25-95 


SOLUBILITY  .IN  WATER. 

(Meerburg,  1905.) 


Solid  Phase. 

Ice 

< 

Ice+CuCl2.2NH4C1.2H2O 
CuCl,.2NH4C1.2H2O 


30 
40 

50 
60 
70 
80 


Gms. 

CuCl2.2NH4Cl 

per  100  Gms. 

Solution. 

27.70 

30.47 
33-24 
36.13 
39-35 
43.36 


Solid  Phase. 


.SOLUBILITY  OF  CUPROUS  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OP  CUPRIC 

SULFATE  AT  ABOUT  2O°. 
(Bodlander  and  Storbeck,  1902.) 


Millimols  per  Liter. 


Grams  per  Liter. 


CuSO4. 

Total  Cu. 

Total  Cl. 

Cu  (ic). 

Cu  (ous). 

CuSCv 

Total  Cu. 

Total  Cl. 

Cu(ic). 

Cu  (ous). 

o 

2 

.880 

5-312 

2.25$ 

O.622 

O 

0.183 

O.lSS 

0.143 

'   0.040" 

0.987 

3 

.602 

4.908 

3-145 

0-457 

o. 

158 

0.229 

0.174 

O.2OO 

0.029 

1-975 

4 

553 

4.687 

4-I3I 

0.422 

o. 

315 

0.290 

0.166 

0.263 

0.027 

2.962 

5 

193 

4.256 

4.625 

0.509 

o. 

473 

0.330 

0.151 

o.  292 

0.032 

4.937 

7 

276 

4.329 

6.546 

0.730 

0. 

788 

0.463 

0.154 

0.4l6 

o  .  046 

SOLUBILITY  OF  CUPROUS  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF 
POTASSIUM  CHLORIDE  AT  ABOUT  20°. 

(Bodlander  and  Storbeck,  1902.) 


Millimols  per  Liter. 

Grams  per  Liter. 

KC1. 

Total  Cu. 

Total  Cl. 

Cu  (ic). 

Cu  (ous). 

KC1. 

Total  Cu. 

Total  Cl. 

Cu  (ic). 

Cu  (ous). 

0 

2 

851 

5.416 

2.222 

0.629 

0 

o. 

181 

0.193 

0.141 

O.O4O 

2. 

5     i 

955 

6.015 

I.42I 

0-534 

0.186 

0.124 

0.213 

0.090 

0.034 

5 

i 

,522 

7.525 

1.008 

0.5H 

0-373 

o. 

097 

0.267 

0.069 

0.033 

10 

i 

.236 

"•735 

0-475 

0.761 

0.746 

o. 

079 

0.416 

0.030 

0.048 

20 

i 

,446 

21.356 

0.324 

1.  122 

1.492 

o. 

092 

0-759 

O.O2I 

O.O7I 

50 

2 

,411 

notdet. 

0.1088 

2.302 

3-730 

o. 

153 

not  det. 

O.OO7 

0.146 

IOO 

4 

,702 

« 

O 

4.702 

7.460 

0. 

299 

tt 

O 

0.299 

2OO 

9 

485 

M 

O 

9-485 

14.920 

0. 

603 

t( 

0 

0.603 

1000 

97 

« 

O 

97 

74.60 

6. 

170 

u 

0 

6.170 

2000 

384 

t( 

0 

384 

149.2 

24- 

42 

it 

0 

24.420 

The  results  in  the  3d,  7th,  8th  and  last  line  of  this  table  are  at  16°. 


SOLUBILITY  OF  COPPER  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  SODIUM 

CHLORIDE. 

(Hunt,  1870.) 
Gms.  CuClg  per  too  cc.  Solution  of: 


f. 

Sat.  NaCl. 

iS%NaCl. 

S%NaCL 

II 

8-9 

3-6 

40 

11.9 

6 

I.I 

90 

16.9 

10.3 

2.6 

267 


COPPER  CHLORIDE 


SOLUBILITY  OF  CUPROUS  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  FERROUS 
CHLORIDE  AT  21.5°  AND  VICE  VERSA. 

(Kremann  and  Noss,  1912.) 

In  order  to  ascertain  the  composition  of  the  solid  phase,  the  experiment  was 
made  by  mixing  together  weighed  amounts  of  H2O,  CuCl  and  FeCl2  and  agi- 
tating in  a  thermostat  at  constant  temperature.  A  weighed  portion  of  the 
clear  saturated  solution  in  each  case  was  analyzed  and  the  composition  of  the 
solid  phase  calculated  by  difference. 


Cms.  per  100  Cms.  H2O. 

FeCl2. 

CuCl.   ' 

O 

i-53 

6.02 

i-33 

11.62 

i.  80 

16.30 

3-n 

26.30 

7.12 

29-35 

8.06 

33-12 

9-S6 

Solid  Phase. 

CuCl 

M 


Gms.  per  100  Cms.  H2O. 


FeCl2. 

CuCl.    " 

43-75 

12.42 

CuCl 

54 

17.04 

« 

66.40 

21.6 

u 

73-20 

23.20 

71.90 

21.65 

F( 

69.30 

11.9 

65.10 

O 

Solid  Phase. 


+FeCl2.4H20 
FeCl2.4H20 


SOLUBILITY  OF  CUPROUS  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  SODIUM 
CHLORIDE  AT  26.5°  AND  VICE  VERSA. 

(Kremann  and  Noss,  1912.) 


(See  remarks  above.) 


'NaCl. 
0 

10.8 

CuCl.' 

i-55 

OUJ1U.    i  IltlbC. 

CuCl 

20.7 

27 
36.48 

7-30 
40.60 
49.10 

M 

Gms.  per  100  Gms.  H2O. 


Solid  Phase. 


'  NaCl. 

CuCl.  ' 

44.14 

57-21 

CuCl 

55-io 

44.10 

NaCl 

56.80 

41.70 

" 

50.90 

18.70 

u 

SOLUBILITY  OF  CUPROUS  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  POTASSIUM 
CHLORIDE  AT  22°  AND  VICE  VERSA. 

(Bronsted,  1912.) 


Gms.  per  100  Gms.       _  ,. 
Sat.  Sol.               Solid 

Gms.  per  100  Gms.           _  ... 
Sat-Sol.                   lohd 

Gms.  per  TOO  Gms. 
Sat.  Sol. 

Solid 
Phase. 

KC1. 

CuCl.' 

'  KC1. 

CuCl. 

'  KC1. 

CuCl. 

3-87 

0 

.115    CuCl 

21 

.64 

13 

.32        CuCl 

24, 

04 

4 

•53 

CuCl.aKCl 

6.56 

0 

•405    " 

23 

.84 

17 

-23 

25 

03 

3 

.14 

" 

8.24 

O 

.861    " 

25 

.24 

21 

•47 

26 

,28 

a 

.20 

" 

n-33 

2 

.19     " 

23 

.87 

15 

.48    CuCLaKCl 

27 

,06 

i 

.60 

" 

I5-30 

4 

.80     " 

23 

•57 

13 

•99 

26 

.68 

-i 

.21 

KC1 

17-47 

7 

.19     " 

23 

II 

•39 

26 

32 

0 

-58 

" 

20.31 

10 

.21          " 

23 

-49 

7 

•35 

25 

.68 

0 

** 

COPPER  CHLORIDE  268 

SOLUBILITY  OF  CUPRIC  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  MERCURIC 
CHLORIDE  AT  35°  AND  VICE  VERSA. 

(Schreinemakers  and  Thonus,  1912.) 


'  HgCl2. 

CuCl2. 

auiiu  r  iia.se. 

HgCl2. 

CuCl2.     " 

ooiiu  rnase. 

O 

44-47 

CuCl2.2H2O 

52-54 

18.46 

HgCl2 

21.03 

33-5 

« 

52.81 

18.06 

u 

37-30 

26.07 

tt 

51.03 

14-73 

(( 

44-47 

23-31 

tt 

49-50 

5-94 

It 

50-47 

21  .50 

"  +HgCl2 

23.87 

2.64 

tl 

52-44 

19.40 

HgCl2 

8.51' 

0 

tt 

SOLUBILITY  OF  COPPER  CHLORIDE  AND  POTASSIUM  CHLORIDE  DOUBLE 
SALTS  AND  MIXTURES  IN  WATER. 

(Meyerhoffer  —  Z.  physik.  Chem.  5,  102,  '90.) 

Cl  per  i  Gram  Solution.  Mols.per  iooMols.H2O. 

* Solid 

Phase. 

CuCl2.2KC1.2H20  +  KCl 


CuCl2.KCl  +  KC1 
CuCl2.2KC1.2H2O  +  CuCl2.2H2O 
« 

CuCl2.KCl  +  CuCl2.2H2O 
ii 

CuCl2.2KC1.2H2O  +  CuCl2.KCl 
CuCl2JCCl 


SOLUBILITY  OF  CUPRIC  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  SODIUM 
CHLORIDE  AT  30°  AND  VICE  VERSA. 

(Schreinemakers  and  de  Baat,  1908-09.) 

Gms.  per  100  Gms.  Sat.  Sol.  Gms.  per  TOO  Gms.  Sat.  Sol. 

,    ^. • — — — >         Solid  Phase.  . — ; • — — >        Solid  Phase. 

MaCl.  CuCl2.  NaCl.  CuCl2. 

o  43-95  CuCl2.2H2O                 12.25  32.40         NaCl 

3.10  41.14  13.54  28.64 

4.28  41.06  15-40  23.72 

6.41  39.40  "                              18.44  16.98             " 

10.25  36.86  "  +NaCl                20.61  11.03 

12.02  32.38  NaCl                  26.47  °                  " 


t<>. 

Present  as 
CuCl2. 

Present  as 
KC1. 

CuCb. 

KCl. 

39-4 

0.120 

0.107 

5.56 

9-93 

49.9 

0.129 

O.II5 

6-39 

11.4 

60.4 

0.142 

0.125 

7.71 

13.6 

79.1 

0.168 

O.I42 

n.  i 

18.8 

0.188 

0.154 

14.9 

24.4 

93-7 

0.194 

0.156 

16.2 

26.0 

98.8 

0.197 

O.l62 

17-5 

28.7 

o 

0.214 

O-02I 

9.84 

i-94 

39-6 

0.232 

O.O49 

12.9 

5-44 

50.1 

0.233 

0.059 

13-7 

6.90 

0.241 

0.062 

14.8 

7-63 

60.2 

0.246 

O-o66 

15-8 

8-49 

72.6 

0-255 

0.063 

16.8 

8-35 

64.2 

14.9 

ii.  6 

72-5 

... 

... 

14.8 

15.0 

26$ 


:  COPPER  CHLORIDE 


SOLUBILITY  OF  CUPRIC  CHLORIDE?  itf  AQUEOUS  ALCOHOL  AT^II.S". 

(Bodtker,  1897.) 

10  gms.  of  CuCl22H2O  and  the  indicated  amounts  of  CuCl2  were  added  to 
20  cc.  portions  of  alcohol.  The  solutions  shaken  two  hoursjand  5  cc.  portions 
withdrawn. 


Vol.  % 

Gms.  CuCl2 

Gms.  per  5 

cc.  Solution.  ' 

Vol. 

% 

Gms.  CuClj 

Gms.  per  5  cc. 

Solution. 

Alcohol. 

Added." 

'   H2O. 

CuCl2.   " 

Alco] 

hoi. 

Added.  , 

>  H20. 

CuCl2.  " 

89.3 

o 

0.794 

LI37 

99 

•3 

0.223 

0.330 

I-29S 

92.3 

o 

0.648 

1.090 

99 

•3 

0.887 

0.247 

1.639 

96.3 

0 

0.478 

1.116 

99 

•3 

I.S40 

0.191 

2.086 

99-3 

o 

0.369 

1.208 

99 

•3 

1-957 

0.164 

2.400 

SOLUBILITY  OF  CUPRIC  CHLORIDE  IN  SEVERAL  SOLVENTS. 

(Etard  —  Ann.  chim.  phys.  [7]  2,  564,  '94;  de  Bruyn  —  Z.  physik.  Chem.  10,  783,  '92;  de  Coninck  — 
Compt.rend.  131,  59,  'oo;  St.  von  Laszczynski —  Ber.  27,  2285,  '94.) 

Grams  CuCl2  per  100  Grams  Sat.  Solution  at: 


ooiveni. 

0°. 

15°. 

20°. 

40°. 

80°. 

Methyl  Alcohol 

36 

40.5  (deB.) 

36.5 

37-o 

Ethyl  Alcohol 

32 

35.0  (deB.) 

35-7 

39-0 

Propyl  Alcohol 

29 

30-5 

30-5 

.  .  . 

Iso  Propyl  Alcohol 

.  .  . 

16.0 

30.0 

n  Butyl  Alcohol 

1^ 

.  .  . 

J5-3 

16.0 

16.5 

Allyl  Alcohol 

23 

.  .  . 

23.0 

.  .  . 

Ethyl  Formate 

10 

9.0 

8.0 

Ethyl  Acetate 

.  .  . 

... 

3-0 

2-5 

i.3(720) 

Acetone  (abs.) 

8.86* 

8.92f 

2.88 

(18°)    ... 

1.40(56°) 

Acetone  (80%) 

.  .  . 

18.9$ 

Ether 

0.043  (IJ°) 

o.n 

*  (CuCl2.2  Aq.) 

t(CuCl2.2Aq.) 

*  (23°  CuCl2.2  Aq.) 

For  the  solubility  of  cupric  chloride  in  mixtures  of  a  number  of 
organic  solvents,  see  de  Coninck. 

Gms. 

Solvent.  V.        g^T 

Sat.  Sol. 

Acetonitrile  18        1.57 

Ethyl  Acetate  18        0.4 

Methyl  Acetate  18        0.55 


Sp.  Gr. 
Sat.  Sol. 


Authority. 


(Naumann  and  Schier,  1914.) 
0.9055   (Naumann,  1904.) 
O  .  939      (Naumann,  1909.) 


AnhydrOUS  Hydrazine    Ord.  temp.    5  (decomp.)   .  .  .         (Welsh  and  Broderson,  1915.) 

SOLUBILITY  OF  CUPROUS  CHLORIDE  IN  ACETONITRILE.     (Naumann  and  Schier,  1914.) 
loo  gms.  acetonitrile  of  boiling  point  81.6°  dissolve  13.33  gms«  CuCl  at  18°. 

SOLUBILITY  OF  CUPRIC  CHLORIDE  IN  PYRIDINE. 

:(Mathews  and^Spero,  1917.) 
Gms. 

to  CuCl2  per 

100  Gms. 
Sat.  Sol. 


0.140 
0.195 
0.295 


—  12. 1 

—  IO 

—  8.9  tr.  pt.  0.270 
+  2  0.275 

10  0.293 

25  0.348 

35  0.382 


Gms. 

Solid  Phase. 

t° 

CuCl2  per 

Solid  Phase. 

too  Gms. 

Sat.  Sol. 

:i,.6C5HBN 

45 

0.422 

CuClj-aCjHjN 

53 

0-493 

it 

(unstable) 

60 

0.565 

"  (unstable) 

+CuCl2.2C5H6N 

62 

0.616 

"           " 

CuCl2.2C6H5N 

58  tr.  pt. 

.  .  . 

"  +2CUC1J.3C5HSN 

" 

63 

0-543 

2CUC12.3C5H6N 

(i 

75 

0.631 

« 

M 

95 

0.917 

M 

COPPER  CHLORIDE  270 

DISTRIBUTION  OF  CUPRIC  CHLORIDE  BETWEEN  AQ.  HC1  AND  ETHER 
When  i  gm.  of  copper  as  chloride  is  dissolved  in  100  cc.  of  10%  HC1  and  shaken 
with  loo  cc.  of  ether,  0.05%  of  the  metal  enters  the  ethereal  layer.     (Mylius,  1911.) 

COPPER  Ammonium  CHLORIDE   CuCl2.NH4Cl. 

SOLUBILITY  IN  ABSOLUTE  ALCOHOL  AT  25°.    (Foote  and  Walden,  1911.) 

Gms.  per  100  Gms.  Sat.  Sol. 
— • Solid  Phase. 


4.7  not  det.  NH4C1+  CuCl2.] 

6.45  "  CuCl2.NH4Cl 

12.90 

34-7  "  +CuCl2.C2H5OH 

COPPER   Potassium  CHLORIDE   CuCl2.KCl. 

SOLUBILITY  IN  ABSOLUTE  ALCOHOL  *ANDJN  ACETONE  AT  25°.  (Foote  and  Walden,  191 1) 
In  Absolute  Alcohol.  In  Acetone. 

Gms.  per  100  Gms.  Sat.  Sol.  Gms.  per  100  Gms.  Sat.  Sol. 

_   -. " ^7- .  Solid  Phase.  TT-rr " — TTTT, •         Solid  Phase. 

CuCl2.  KC1.  CuCl2.  KC1. 

1.40  0.28  KCl+CuCl2.KCl  0.34  0.38          KCl+CuCl2.KCl 

2.15       not.  det.  Cud2.KCi  0.48      not  det.  CuCi2.Kd 

5.25  "  «•  1.50 

30.16  "  2.06 

34.45  0.21  "  H-CuClz.QHBOH         2.40  0.27          "  +CuCl2.C3H«O 

33.97  O  CuCl,.CfH,OH 

Freezing-point  data  (solubility,  see  footnote,  p.  i)  are  given  for  the  following 
mixtures  of  cuprous  chloride  and  other  chlorides. 

CuCl  +  CuCl2  (Sandonnini,  1912  (a)). 

+  FeCls  (Hermann,  1911.) 
+  PbCl2 

-j-  LiCl  (Sandonnini,  1911,  1914;  Korreng,  1914.) 

-\-  RbCl  (Sandonnini,  1914;  Sandonnini  and  Aureggi,  1912.) 

+  AgCl  (Sandonnini,  1911,  1914;  Poma  and  Gabbi,  1911,  1912.) 

-j-  KC1  (Sandonnini,  1911,1914;  Korreng,  1914;  Sackur,  1913;  Poma  and  Gabbi,  1911, 1912.) 

+  NaCl  (Sandonnini,  1911,  1914;  Korreng,  1914;  Sackur,  1913;  de  Cesari,  1911.) 

+  T1C1  (Sandonnini,  1911,  1914.) 

+  SnCl2  (Hermann,  1911.) 

+  ZnCl2 

Freezing-point  lowering  data  for  mixtures  of  CuCl  +  Cu2O  and  CuCl  +  Cu2S 
are  given  by  Truthe,  1912. 

COPPER  Potassium   CITRATE   CuK4[(COOCH2)2C(OH)COO]2. 

100  cc.  sat.  solution  in  H2O  contain  43.3  gms.  of  the  salt  at  10°.  (Pickering,  1915.) 
COPPER  CYANIDE  (ous)  Cu2(CN)2. 

Freezing-point  data  for  Cu2(CN)2  +  KCN  and  Cu2(CN)2  +  NaCN  are  given 
by  Truthe  (1912). 

COPPER  HYDROXIDE   (ic)   Cu(OH)2. 

SOLUBILITY  IN  AQUEOUS  SOLUTIONS  OF  AMMONIA  AT  18°.     (Dawson,  1909.) 

Mols.  NH3  per        Gm.  Atoms  Cu  per  Mols.  NH3  per      Gm.  Atoms  Cu  per 

Liter.  Liter.  Liter.  Liter. 

0.2  0.00054  3  0.0548 

0.5  0.0033  4  0.0784 

1  0.0109  5  0.1041 
1.5  0.0204  6  0.1254 

2  0.0314  8  0.1599 
2.5  0.0442  9.96  0.1787 

Three  series  of  results  at  25°,  somewhat  higher  than  the  above,  are  given  by 
Bonsdorff,  1904. 

Data  showing  the  effect  of  increasing  amounts  of  (NH4)2SO4,  Ba(OH)2,  NaOH 
and  of  Na2SO4  upon  the  solubility  of  cupric  hydroxide  in  aqueous  ammonia 
solution  at  18°,  are  given  by  Dawson,  1909  a. 


271 


COPPER  IODATK 


COPPER  IODATE   (ic)   Cu(IO3)2H2O. 

One  liter  sat.  aqueous  solution  contains  1.36  gms.  Cu(I03)2  at  25°,  determined 
by  measurement  of  single  potential  differences  against  a  o.i  n  calomel  electrode. 

(Spencer,  1913.) 

COPPER  IODIDE   (ic)   CuI2. 

One  liter  sat.  aqueous  solution  contains  11.07  gms.  CuI2  at  20°. 

(Fedotieff,  ign-ia.) 
COPPER  IODIDE   (ous)   Cu2I2. 

SOLUBILITY  OF  CUPROUS  IODIDE  IN  AQUEOUS  SOLUTIONS  OF  AMMONIUM 
BROMIDE  AND  OF  POTASSIUM  BROMIDE. 

(Kohn,  1909;  Kohn,  and  Klein,  1912.) 

Results  for  Aq.  NH4Br  at  20°.  Results  for  Aq.  KBr  Solutions. 

Normality    Gms.  Cu2I2  Normality  Gms.  Cu2I2  Normality    Gms.  Cu2I, 

NHiBr       per  1000  cc.  t°.          of  KBr    per  1000  cc.     t°. 

Sol.  Sat.  Sol.  Sol.          Sat.  Sol. 

2  1.9068  19.5  2  1.467      23 

3  3-6540  24  2  1.558      22 

4  6.0588  19.5        3        3.409     22 


of  KBr    per  1000  Gms. 
Sol.  Sat.  Sol. 


3-595 
7.126 
6.977 


SOLUBILITY  OF  CUPROUS  IODIDE  IN  AQUEOUS  SOLUTIONS  OF  IODINE  AT  20° 

AND  VICE  VERSA.      (Fedotieff,  1910-11.) 


Gms.  per  Liter.        Solid           Gms.  per  Liter. 

Solid 

Cu. 

I.        Phase.     '  Cu. 

i. 

Phase. 

0.285 

0 

.5848    Cul      0.964 

5 

.0854 

Cul 

0.482 

I 

•3053      " 

.032 

5 

.6854 

" 

0.583 

I 

.9218      " 

.090 

6 

.2816 

" 

0.678 

2 

•5573     " 

.112 

6 

•5301 

" 

0.756 

3 

.  2042     " 

.232 

7 

.6529 

"  +1 

0.844 

3 

•9539    " 

.040 

6 

.4440 

I 

0.898 

4 

•4359    "      0.898 

5 

•5941 

" 

Gms.  per  Liter. 


Solid 
Phase. 


Cu.  I. 

0.748  4.7112   I 

0.6o6  3.8562 

0.448  2.9493   " 

0.300  2.0689 

0.159  I-2304   " 

at   o°= 0.925     5.4609  Cui+i 
at  40°= i. 658    11.3658     " 

_  Constant  agitation  and  temperature.     Iodine  determined  by  thiosulfate  titra- 
tion;  copper,  electrolytically. 

Additional  data  for  the  solubility  of  cuprous  iodide  in  aqueous  solutions  of 
iodine  in  presence  of  acids  and  salts  at  25°,  are  given  by  Bray  and  MacKay 
(1910).  These  authors  state  that  cuprous  iodide  is  difficultly  soluble  in  water, 
but  in  the  presence  of  iodine  a  considerable  amount  dissolves,  owing  to  the 
formation  of  cupric  iodide  and  tri-iodide. 

100  gms.  acetonitrile  dissolve  3.52  gms.  Cu2I2  at  18°.       (Naumann  and  Schier,  1914.) 
Freezing-point  lowering  data  for  mixtures  of  Cul  +  Agl  are  given  by  Quercigh,  '14. 

COPPER  NITRATE   (ic)   Cu(NO3)2. 

SOLUBILITY  IN  WATER. 


Gms. 
to       Cu(N03)2 
'    per  100  Gms. 

Mols. 
Cu(NO3)2 
per  too 

Solid  Phase. 

Solution. 

•Mols.  H2O. 

-23 

36.08 

5-42 

Cu(NO3)2.9H2O 

—  20 

40.92 

6-65 

• 

—  21 

39-52 

6.27 

Cu(NO3)2.6H2O 

0 

45 

7.87 

M 

+  10 

48.79 

9-15 

« 

18 

53-86 

11.20 

II 

(Funk,  1900.) 
Gms. 


Mols. 


r. 


per  100  Urns.      per 
Solution.      Mols.  H2O. 


scud  Ph- 


55.58 


Cu(NOJ),.3H10 


20 
26.4 

25 
40 
60 
80 

II4-5 

Density  of  solution  saturated  at  18°  =  1.681. 

100 gms.  H2O dissolve  127.4 gms. Cu(Np3)2at2O0,<f20sat. sol.  =  1.688.  (Fedotieff ,  1911-12.) 

Data  for  the  solubility  of  copper  nitrate  in  aq.  ammonia  solutions  are  given 
by  Stasevich,  1913.  , 

Data  for  the  solubility  of  copper  nitrate  in  aq.  solutions  of  copper  sulfate 
and  of  sodium  nitrate  at  20°  are  given  by  Massink,  1916  and  1917. 

100  cc.  anhydrous  hydrazine  dissolve  I  gm.  copper  nitrate,  with  decomposi- 
tion, at  room  temp.  (Welsh  and  Broderson,  1915.) 


60.  01 
6I.5I 
64.17 
67-5I 

77-59 


12 

I6.7 

14.4 

15.2 

17.2 

2O 

33-3 


Cu(NO3)j.6H,O 


COPPER   OXALATE 


272 


COPPER  OXALATE   (ic)   CuC2O4.£H2O. 

One  liter  H2O  dissolves  0.02364  gm.  CuC2O4  at  25°,  determined  by  the  con- 
ductivity method.  (Schafer,  1905.) 

COPPER   OXIDE    (ic)   CuO. 

SOLUBILITY  IN  AQUEOUS  SOLUTIONS  AT  25°. 

(Jaeger,  1901.) 

In  Aq.  HF  +  KF. 

Gm.  Atoms 
Cu  per  Liter. 

0.0356 

0.06437 

0.1442 


In  Aq.  Hydrofluoric  Acid. 

Normality        Gm.  Atoms 
Cu  per  Liter. 

0.0307 

O.II64 

0.2494 

0.388 

0.463 


In  Aq.  HN03  and  CH3COOH. 


ofHF. 
0.12 
0.28 

o-57 
i. 08 
2.28 


Normality 
of  HF. 


Solvent. 


i  n  CHaCOOH 
i  n  HNO3 


Gm.  Atoms 
Cu  per  Liter. 


0.1677 
0.4802 


Cu  determined  electrolytically. 


0.12 
0.28 

0-57 

I. II  O. 

2.17        o. 

COPPER   OXIDE   (ous)   Cu2O. 

SOLUBILITY  IN  AQUEOUS  AMMONIUM  SOLUTIONS  AT  25°. 

(Donnan  and  Thomas,  1911.) 

The  cuprous  oxide  was  prepared  by  adding  KOH  solution  to  a  mixture  of 
equal  weights  of  CuSO4.sH2O  and  sucrose  dissolved  in  water,  until  nearly  all  the 
precipitate  had  redissolved.  The  solution  was  kept  at  70°  until  the  cuprous 
oxide  had  separated.  Two  batches  were  prepared.  The  first,  No.  I,  obtained 
from  the  more  dilute  solution,  was  bulky  and  dark  red  in  color,  Cu  =  88.62%. 
The  second,  No.  II,  was  bright  red,  Cu  =  88.59%.  The  solubility  determina- 
tions were  made  with  extreme  care.  A  special  apparatus  was  used.  By  means 
of  this,  the  constituents  of  the  mixtures  were  introduced  into  the  bottles  in  an 
atmosphere  of  hydrogen  and  every  precaution  taken  to  prevent  oxidation.  The 
bottles  were  sealed  and  rotated  for  2-4  weeks  at  constant  temperature.  In 
case  the  slightest  tinge  of  blue  developed  in  a  bottle  (indicating  oxidation),  it 
was  rejected. 

Results  for  Preparation  No.  I.  Results  for  Preparation  No.  II. 

Gms.  per  1000  Gms.  Sol.    Mols.  per  1000  Gms.  Sol.    Gms.  per  1000  Gms.  Sol.     Mols.  per  1000  Gms.  Sol. 


Cu. 

NH3. 

Cu. 

NH3. 

Cu. 

NH3. 

Cu. 

NH3. 

0-3593 

3 

.91 

0 

.00566 

0.23 

0.4229 

7 

.82 

0 

.00665 

0.46 

0.6869 

13 

•77 

0 

.01080 

0.81 

0.6678 

8 

.16 

0 

.01050 

0.48 

I.OI44 

27 

•°3 

o 

•01597 

i-59 

o  .  9890 

22 

.61 

o 

•01555 

i-33 

I  .  0462 

32 

.64 

o 

.01645 

1.92 

1.0494 

28 

•39 

o 

.01650 

1.67 

1.3229 

68 

.68 

0 

.02081 

4.04 

1.3528 

54 

•15 

0 

.02127 

3-i9 

1.4882 

74 

.12 

0 

.02340 

4-36 

I  .  5048 

72 

.08 

o 

.02366 

4.24 

1-6313 

98 

•52 

o 

•02565 

5-56 

1.5963 

78 

.20 

o 

.02510 

4.60 

1.6981 

122 

.40 

0 

.02670 

7.20 

1-6555 

102 

•05 

0 

.02603 

6 

COPPER   SULFATE   CuSO4.sH2O. 

SOLUBILITY  IN  WATER. 

(Etard,  1894;  Patrick  and  Aubert,  1874;  at  15°,  Cohen,  1903;  at  25°,  Trevor,  1891.) 


Gms.  CuSO4  per  100  Gms. 


O 
10 
20 

25 
30 
40 
50 


Solution. 
12-5 
I4.8 

Water. 
14.3 
17-4 

17.2 

20.7 

18.5 

22.7 

20 
22.5 

25 
28.5 

25 

33-3 

to 

Gms.  CuSO4  per  100  Gms. 

• 

Solution. 

Water. 

60 

28.5 

40 

80 

35-5 

55 

100 

43 

75-4 

120 

44 

78.6 

140 

44-5 

80.2 

160 

44 

78.6 

180 

43 

75-4 

SO  at 

16°  =  1.193. 

(Greenish, 

1902.) 

Sp.  gr.  of  sat.  solution  of  CuSO4.sH2O  in  H2O  at  16°  =  1.193. 

100  gms.  sat.  solution  in  H2O  contain  20.32  gms.  CuSO4at  30°.    (Schreinemakers,  1910.) 


273 


COPPER   SULFATE 


SOLUBILITY  OF  COPPER  SULFATE  IN  AQUEOUS  SOLUTIONS  OF  AMMONIUM 

SULFATE  AT  o°. 

(Engel,  1886.) 


Milligram  Equiv.  per 
10  cc.  Solution. 

Sp.  Gr.  of 

Grams  per 
too  cc.  Solution. 

(NH4)2S04. 

CuSO. 

ions. 

(NH4)2S04. 

CuSO4. 

0 

18.52 

I.I44 

0 

14.79 

5-45 

20.15 

I.I90 

3.61 

16.09 

7 

10.5 

1.108 

4.63 

8.38 

7-4 

9.1 

1.099 

4.90 

7.26 

8-45 

6.425 

I.08I5 

5-59 

5-13 

n-35 

3-7 

I.07I 

7.51 

2.95 

18.6 

1.178 

1.082 

12.31 

0.94 

31-2 

i 

1.116 

20.65 

0.80 

SOLUBILITY  OF  MIXTURES  OF  COPPER  AMMONIUM  SULFATE  AND  NICKEL 
AMMONIUM  SULFATE  IN  WATER  AT  i3°-i4°: 

(Fock,  1897.) 

CuSO4.(NH4)2SO4.6H2O  +  NiSO4.(NH4)2SO4.6H2O, 


Mol.  %  in  Solution. 

Mols.  per  top  Mols.  H2O. 

Mol.  %  in  Solid  Phase. 

Cu  Salt. 
0 

33-34 
56-05 
73.89 
79-92 

100 

Ni  Salt. 
IOO 

66.66 

43-95 
26.20 
20.08 

0 

Cu  Salt. 
0 
0.1476 
0.2664 
0.4165 
0.4785 
I-0350 

Ni  Salt." 
0.521 
0.295 

o  .  2089 

0.1449 
0.1202 
O 

Cu  Salt. 
0 
10.29 

30.59 
52.23 

78.80 
IOO 

Ni  Salt. 
IOO 

89.71 
69.41 

47-77 

21.  2O 
0 

SOLUBILITY  OF  MIXTURES  OF  COPPER  AMMONIUM  SULFATE  AND  ZINC 
AMMONIUM  SULFATE  IN  WATER  AT  i3°-i4°. 

(Fock,  1897.) 


CuSO4.(NH4)2SO4.6H2O  +  ZnSO4.(NH4)2SO4.6H2O. 


Mol.  %  in  Solution. 


Mols.  per  100  Mols.  H2O. 


Mol.  %  in  Solid  Phase. 


'  Cu.  Salt 

Zn  Salt] 

Cu  Salt. 

Zn  Salt. 

"Cu  Salt. 

Zn  Salt. 

4-97 

95  .03 

O.O422 

0.8069 

2-39 

97.61 

10.65 

89-35 

0.0666 

0-5638 

4-52 

95-48 

19.24 

80.76 

0.1218 

0.5H5 

9°-3 

90.97 

30.19 

69.81 

0.2130 

0.4924 

14.67 

85-33 

44-44 

55-56 

0.3216 

0.4022 

22.62 

77.38 

IOO 

o 

1-035 

0 

IOO 

0 

SOLUBILITY  OF  COPPER  SULFATE  IN  AQUEOUS  SOLUTIONS  OF  MAGNESIUM 

SULFATE  AT  o°. 

(Diacon.  1866.) 


Gms.  per  100  Gms.  H2O. 
CuSO4.  MgSO4. 

o  26.37 

2.64  25.91 

4-75        25.30 

9.01  23 . 30         MgS04.6H,0+CuS04.sHzO 


Solid  Phase. 
MgS04.6H20 


Gms.  per  too  Gms.  H2O. 


CuSCv 
12.03 
I3.6I 
14.99 


MgS04. 

I5-67 
8.64 
O 


Solid  Phase. 
CuS04.sH,0 


COPPER  SULFATB 


274 


SOLUBILITY  OF  COPPER  SULFATE  IN  AQUEOUS  SOLUTIONS  OF  COPPER 
CHLORIDE  AT  30°. 

(Schreinemakers,  1910.) 


Cms.  per  100  Gms. 
Sat.  Sol. 


CuSO4. 

20.32 

13.62 
8.93 

4-77 


o 

6.58 
15.68 

25.67 


Solid  Phase. 


CuS04.5H2O 


Gms.  per  100  Gms. 
Sat.  Sol. 


CuCl2. 
39-48 
42.62 

43-25 

43-95 


CuS04. 
3.21 
2.90 
I.I4 
O 


Solid  Phase. 

CuSO4.sH2O 
"+CuCl2.2H2O 
CuCl2.2H20 


DATA  FOR  EQUILIBRIUM  IN  COMPLEX  SYSTEMS  CONTAINING  COPPER  SULFATE. 

System.  Authority. 

CuSO4  +  CuCl2  +  (NH4)2SO4  +  NH4C1  +  H2O  (Schreinemakers,  1910.) 

"        +       "       +  K2SO4  +  KC1  -f  H2O  (Schreinemakers  and  deBaat,  1914  a.) 

"        +       "        +  Na2SO4  +  NaCl  +  H2O  (Schreinemakers,  1911.) 

"        +  Li2SO4  +  (NH4)2SO4  +  H2O  (Schreinemakers,  1909.) 


SOLUBILITY  OF  COPPER  SULFATE  IN  AQUEOUS  SOLUTIONS  OF  LITHIUM 
SULFATE  AT  30°. 

(Schreinemakers,  1908,  1909.) 


Gms.  per  too  Gms. 

Sat.  Sol. 

'Li2S04. 
O 


3-54 

6.08 

11.94 

I5-72 


CuSO4. 
20.32 

17-59 

16.10 

13-55 
12.14 


Solid  Phase. 

CuSO4.5H2O 


Gms. 


>er  loo  Gms. 
it.  Sol. 


Li2S04. 
17.92 

20-55 
22.23 

23-59 
25.24 


CuSO4. 
II  .04 
IO.O5 

6.41 

3-39 
o 


Solid  Phase. 

CuSO4.5H2O 
"  +Li2SO4.H2O 
Li2SO4.H2O 


SOLUBILITY  OF  COPPER  SULFATE  IN  AQUEOUS  SOLUTIONS  OF  LITHIUM  AND 
OTHER  CHLORIDES  AT  25°. 

(Herz,  1910.) 


In  Lithium 
Chloride. 

Gms.  per  100  cc. 
Sat.  Sol. 

In  Potassium 
Chloride.' 
Gms.  per  100  cc. 
Sat.  Sol. 

In  Rubidium 
Chloride. 

Gms.  per  100  cc. 
Sat.  Sol. 

In  Sodium 
Chloride. 

Gms.  per  too  cc. 
Sat.  Sol. 

LiCl.            CuS04. 
3.10       20.06 

5-93      18.78 

12                17.03 

KC1.            CuS04. 
4.19         23.89 
8.75         24.92 
17.50         29.03 

'  RbCl.         CuS04, 

o           22.34 

13.22       25.02 

.   NaCl.         CuSO4. 
2.10      22.41 
7.72       22.76 
14.79      24.05 

SOLUBILITY  OF. COPPER  POTASSIUM  SULFATE  CuK2(SO4)2.6H20  IN  WATER  AT  25°. 
loo  gms.  H2O  dissolve  11.14  Sms-  CuK2(SO4)2.  (Trevor,  1891.) 

Additional  data  for  the  system  Copper  sulfate  -f  Potassium  sulfate  +  H2O  are 
given  by  Meerburg,  1909. 

Data  for  the  solubility  in  water  of  mix-crystals  of  copper  sulfate  and  man- 
ganese sulfate  at  o°  and  17°,  and  of  copper  sulfate  and  zinc  sulfate  at  12°,  18°, 
25°i  35°»  40°  and  45°,  are  given  by  Hollemann,  1905-06. 


275 


COPPER   SULFATE 


COPPER  SULFATE,  MANGANESE  SULFATE,  MIXED  CRYSTALS  AT  25°. 

(Stortenbecker,  1900.) 
Cms,  per  100  Gms.  HaO.  Mols.  per  100  Mols.  H2O, 


CuSCv  MnSO4. 

Tridinic  Crystals  with  sH2O. 


20.2 
19.76 

I3-65 

ii.  61 

9-39 
6-47 


o 
3-69 

St'S* 
39-4i 

46.77 
53-39 
58-93 


o.o          61.83 

Monoclinic  Crystals  with  7H2O. 


9-39 
6-47 
o.o 


46.77 
53-39 


Cu. 

2.282 

2.23 

1-54 

I-31 

i. 06 

o-73 
0.34 
o.o 

i. 06 

o-73 
o.o 


Mn. 

O 

0.44 

3-76 

5-59 
6-37 
7-03 
7-375 

5-58 
6-37 
8±* 


Mol.  %  Cu 
in  Solution. 


Mol.  %  Cu 
in  Crystals. 


100 

100 

90-5 

83.5 

99-3 

74.1 

97-3 

57-7 
31-0 

*l'.l 

29.0 
26.1 

21.8 

70.4 

21.2 

42.6 

20.0 

34-4 

13-45* 

22.9 

15  .2* 

10.27 

10-5 

4-6 

4.9 

2.31 

2.15 

o.o 

IOO.O 

20.  o 


10.27 
4,6* 
o.o 


28.2 
23-5 

20.8 

16.0 
5-8* 
100 


*  Indicates  points  of  labil  equilibrium. 


COPPER  SULFATE,  ZINC  SULFATE,  MIXED  CRYSTALS  IN  WATER  AT  18°. 

(Stortenbecker,  1897.) 


Triclinic  Crystals  with 


Monoclinic  Crystals  with  7H2O. 


Rhombic  Crystals  with  7H2O. 


Mols.  per  100  Mols.  H2O. 

Mol.  %  Cu 

Mol.  %  Cu 

Cu. 

Zn. 

in  Solution. 

in  Crystals. 

2.28 

0 

100 

100 

-83 

2.08 

46.8 

94.9 

-41 

3-60 

28.1 

.19 

5-01 

19.2 

77-9 

.86 

3-36 

36.2 

40.4 

.22 

4-45 

21-5 

29-5-3I-9 

.01 

4.72 

17.6 

24.1-28. 

0.82 

5-03 

14.0 

19.0-22. 

0.51 

5-59 

8.36 

12.4-14-9 

0.30 

5-56 

4.87 

7.02 

o.o 

6.42 

o.o 

0 

1.19 

5.01 

19.2 

5.01 

0.51 

5-59 

8.36 

1.97 

0.267 

5-77 

4.42 

i-i5 

o.o 

5-94 

o.o 

0-00 

COPPER  SULFATE 


276 


SOLUBILITY  OF  COPPER  SULFATE,  SODIUM  SULFATE  MIXTURES  IN  WATER. 

(Koppel,  1901-02;  Massol  and  Maldes,  1901.) 


Solid  Phase. 


CuS04.5H20+Na«SO4.ioH2O 


CuSO4.NajSO<2H2O 


CuS04.Na2S04.2H20+CuS04.sH20 


Gms.  per  100  Gms. 
t»t                      Solution. 

Mols.  per  100  Mols. 
H20. 

"  CuSO4. 

NajSO,. 

CuSO4. 

NajSO4. 

O 

13.40 

6.23 

1.88 

0.98 

IO 

14.90 

9.46 

2.23 

1.56 

15 

15.18 

11.64 

2-34 

2.02 

17.7 

14-34 

13-34 

2.24 

2-34 

23 

14.36 

12.76 

2.23 

2.21 

40.15 

13-73 

12.26 

2.10 

2.10 

17.7 

14.99 

I3-48 

2-37 

2-39 

23 

16.41 

n-35 

2-57 

1.99 

40.15 

20.56 

8 

3-25 

1.47 

18 

13-53 

13.84 

2.10 

2.41 

20 

n-34 

I5-70 

I.76 

2-73 

25 

6.28 

21.20 

0.98 

3-70 

30 

2.607 

28.38 

0-43 

5-2i 

33-9 

1-475 

32.30 

0.25 

6.18 

37-2 

1-494 

31.96 

0.25 

6.08 

30 

5-38 

22.17 

30.1 

3  -69 

25-37 

30 

i-57 

32.09 

« 

CuS04.Na2S04.2H20  +increasing 


Data  tor  the  system  copper  sulfate,  sodium  sulfate,  water,  at  20°  and  35* 
are  given  by  Massink,  1916,  1917. 


SOLUBILITY  OF  COPPER  SULFATE  IN  AQUEOUS  SOLUTIONS  OF  SULFURIC 

ACID  AT  0°.         (Engel,  1887.) 


Milligram 

Eqvnv. 
H,0. 

per  10  Gms. 

Sp.  Gr.  of 
Solutions. 

I.I44 

Grams  per  100  Grams 
H20. 

H2S04. 
0 

CuSO4. 

18.6 

H2S04. 
0 

cuso4: 
14-85 

4.14 
14.6 

17.9 
19.6 

I 
I 

-143 
.158 

2 

7 

•03 
.16 

14.29 
15-65 

54-2 
56-25 
71.8 

12.4 
8.06 

7-75 
5 

I 
I 
I 
I 

.170 

•195 
.211 

.224 

15 
26 

27 
35 

.20 

•57 
•57 

.2 

9.90 

6.43 
6.19 

3-99 

SOLUBILITY  OF 

COPPER  SULFATE  IN  AQUEOUS 

AT  25°.      (Bell  and  Taber,  1908; 

SOLUTIONS 

Foote,  1915.) 

OF   SULFURIC 

ACID 

Gms.  per  100  Gms. 
Sat.  Sol. 

Solid  Phase. 
CuSO4.sH20 

<  Gms.  per  100  Gms. 
Sat.  Sol. 

Solid  Phase. 

CuSO4.3H2O+CuSO 
CuS04.H20 

H20 

H2S04. 
0 
11.14 

CuSO4. 
18.47 
12.62 

H2S04. 
55-72 
61.79 

CuS04. 
2.13 

o-95 

25 
36 
42 

47 
49 

•53 
•77 

.66 

5 
3 

2 
2 
2 

.92 
•25 
-63 

•59 
-83 

M 

"  +CuSO4.sH2O 

77 
83 
85 
85 
86 

•93 
.29 
.46 
.76 
.04 

0.17 

0-15 
0.19 

0-43 
0.40 

u 
If 

"  +CuS04 
CuS04 

50 
54 

•23 

.78 

2 
2 

.70 
.19 

CuSO4.3H2O 

92 

.70 

0.19 

277 


COPPER   SULFATE 


SOLUBILITY  OF  COPPER  SULFATE  IN  METHYL  AND  ETHYL  ALCOHOL,  ETC. 

(de  Bruyn,  1892;  de  Coninck,  1905.) 


Solvent. 

Methyl  Alcohol  Abs. 

"       93-5% 
"       50% 
"  "       Abs. 

Ethyl  Alcohol  Abs. 
Glycol 
Glycerol 
Glycerol 

95%  Formic  Acid 
Anhy.  Hydrazine 


Cms,  per  ioo  Gms.  Solv.    SOLUBILITY    IN   AQUEOUS 


i8 
18 
18 

3 

3 
14.6 

15-5 
15-16 


CuS04.  CuS04.sH20. 

1.05          15.6 
0-93 
0.40 
...          13.4 


ALCOHOL  AT  15°. 

(Schiff,  1861.) 


Alcohol 


Gms.  CuSO4.sH2O 
per  ioo  g.  Solvent. 


IO 
20 
40 


I.I 

7-6* 
30 

36  . 3      (Ossendowski,  1907.) 


15-3 
3-2 
0.25 


ord.  t.  2 

*  Per  ioo  gms.  solution. 


O'O5 
.  .  .  t 


(Welsh  and  Broderson,  1915.) 
t  decomp. 


Data  for  the  solubility  of  copper  sulfate  in  methyl  alcohol  are  given'  by  Carrara 
and  Minozzi,  1897. 

COPPER   SULFIDE   (ic)   CuS. 

1    One  liter  of  water  dissolves  0.00033  gm.  CuS  at  18°,  determined  by  the  conduc- 
tivity method.  (Weigel,  1906;  see  also  Bruner  and  Zawadski,  1909.) 
ioo  cc.  sat  aq.  sodium  sulfide  solution  (of  d  =  1.225)  dissolve  0.0032  gm.  CuS. 

(Holland,  1897.) 

SOLUBILITY  OF  COPPER  SULFIDE  IN  AQUEOUS  SUGAR  SOLUTIONS. 

(Stolle,  1900.) 


insolvent. 
10 

30 
50 

Gms.  CuS  p< 

:r  Liter  of  Aq.  Sugar 

1  Solution  at: 

17.5°- 
0.5672 
0.8632 
0.9076 

45°- 
0-3659 
0.7220 
1.0589 

75°.  ' 
I-I34S 
1.2033 
I  .  2809 

COPPER  SULFIDE   (ous)   Cu2S. 

Freezing-point  lowering  data  (solubility,  see  footnote,  p.  i)  for  mixtures  of 
Cu2S  +  Ag2S,  Cu2S  +  PbS  and  Cu2S  +  ZnS  are  given  by  Friedrich,  1907-08. 
Results  for  Cu2S  +  Sb2S3  are  given  by  Chikashigi  and  Yamanchi,  1916.  Data 
for  Cu2S  +  FeS  are  given  by  Shad  and  Bornemann,  1916. 


COPPER  SULFONATES. 

100  gms.  H2O  dissolve  0.25  gm.  copper    2-phenanthrene  monosulfonate  at  20°. 

0^26   "         "       10-  " 


COPPER  TARTRATE  CuC4O6H4.3H2O. 

SOLUBILITY  IN  WATER. 

(Cantoni  and  Zachoder,  1905.) 


(Sandquist,  1912.) 


t°. 

Gms. 
per  ioo  cc. 

t°. 

Gms. 
CuC406H4.3H20 
per  ioo  cc. 

t°. 

Gms. 
CuC4OfH4.3H2O 
per  ioo  cc. 

Solution. 

Solution. 

Solution. 

15 

0.0197 

40 

0.1420 

65 

0.1767 

20 

0.0420 

45 

0.1708 

70 

0.1640 

25 

o  .  0690 

O.I92O 

75 

0.1566 

30 

o  .  0890 

55 

0.2124 

80 

0.1440 

35 

0.1205 

60 

0.1970 

85 

0.1370 

COPPER  THIOCYANATE 


278 


NH3. 

Cu(SCN)2. 

0.79 

2-45 

1.98 

4.08 

2.50 

5.11 

4.26 

5.96 

5-35 

6.22 

6-39 

6-59 

9-93 

7.98 

16.55 

11.24 

21.47 

15.22 

COPPER  THIOCYANATE    (ic)   Cu(SCN)2. 

SOLUBILITY  IN  AQUEOUS  AMMONIA  SOLUTIONS  AT  25°  AND  AT  40°. 

(Horn,  1907.) 

Results  at  25°.  ,  Results  at  40°. 

dv,         Gms.  per  100  Gms.  Sat.  Sol.      ^.^  ^^^         Gms.  per  100 
Sat. 

1.0082  0.70  2.4S      Cu(SCN)2.2NH3 

I.OI66 
I .O2I3 
I.OI7I  4.26  ^.Q6  Cu(SCN)2.4NH3 

1.0151 
1.0134 
1.0070 

0.9987 
0.9985 

COUMARIN  C9H6O2. 

100  gms.  water  dissolve  o.oi  gm.    coumarin  at  2O°-25°.  (Dehn,  1917.) 

"         pyridine  87.7    gms. 

50%  aq.  pyridine  60. i 

"         chloroform  49.4  "  25°.    (Osaka,  1903-08.) 

Freezing-point  lowering  data  for  mixtures  of  coumarin  and  sulfuric  acid  are 
given  by  Kendall  and  Carpenter,  1914. 

CRESOLS   C6H4(OH)CH3  o,  m  and  p. 

SOLUBILITY  OF  EACH  SEPARATELY  IN  WATER. 

(At  20°,  Vaubel,  1895;  Sidgwick,  Spurrell  and  Davies,  1915.) 

Determinations  by  synthetic  method;  melting-point  of  o  =  29.9°,  of  m  =  4°, 
of  p  =  33-8°.  Triple  point  for  o  =  87  and  2.5  gms.  per  100  gms.  sat.  sol.  at 
8°;  triple  point  for  p  =  86  and  2  gms.  per  100  gms.  sat.  sol.  at  8.7°. 


NH3. 

Cu(SCN)2. 

»     ooiiu  rnase. 

0.94 

2.81 

Cu(SCN)2.2NH3 

1.77 

4.18 

" 

2-57 

6.55 

" 

3-52 

8.76 

« 

4-35 

11.78 

Cu(SCN)2.4NH3 

5-50 

12.07 

" 

7-58 

12.99 

« 

13.98 

16.58 

" 

18.02 

19.76 

• 

Gms.  per  100  Gms.  Sat.  Solution. 

20 
40 

o  Cresol. 

2-45 
3.08 

m  Cresol. 
2.18 

2.51 

p  Cresol. 
1-94 
2.26 

50 
60 

3.22 
3-40 

2.72 
2.98 

2-43 
2.69 

70 
80 
90 

3-74 
4.22 
4.80  • 

3-35 
4-43 

3-03 
3-52 
4.16 

100 

5-30 

5-47 

5.10 

no 

<  .80 

5-SO 

^0                   Gms.  per  too  Gms.  Sat.  Solution. 

o  Cresol. 

m  Cresol. 

P  Cresol. 

120 

6.22 

7 

6.58 

I30 

6.70 

8.86 

9 

I4O 

7.67 

12.3 

15-9 

143.5  crit-  *. 

.  .  . 

.  .  . 

CO 

147  crit.  t. 

00 

150 

II.  I 

160 

23-7 

162.  8  crit.  t. 

00 

One  liter  aqueous  I  normal  solution  of  the  sodium  salt  of  o  cresol  dissolves 
7.57  gms.  o  cresol  at  25°,  8.32  gms.  at  40°,  9.84  gms.  at  60°  and  13.62  gms.  at  80° 

(Sidgwick,  1910.) 

MISCIBILITY  OF  AQUEOUS  ALKALINE  SOLUTIONS  OF  m  CRESOL  WITH  SEVERAL 
ORGANIC  COMPOUNDS  INSOLUBLE  IN  WATER. 

(Sheuble,  1907.) 

To  5  cc.  portions  of  aq.  KOH  solution  (250  gms.  per  liter)  were  added  the 
given  amounts  of  the  aq.  insoluble  compound  from  a  buret,  and  then  the  m  cresol 
dropwise,  until  solution  occurred.     Temp,  not  stated. 
Composition  of  Homogeneous  Solution. 


cc.  Aq.  KOH. 

Aq.  Insol.  Cmpd. 

m  Cresol. 

5 

2 

CC. 

(I 

.64 

gms, 

.)  Octyl  Alcohol* 

I 

.1 

gms. 

5 

5 

tt 

(4 

.1 

tt 

)      " 

I 

.8 

tt 

5 

2 

" 

(i 

•74 

tt 

)  Toluene 

4 

•4 

" 

5 

3 

tt 

(2 

.61 

it 

\       a 

5 

.1 

" 

5 

2 

" 

(I 

.36 

tt 

)  Heptane 

6 

•4 

n 

the  normal  secondary  alcohol,  the  so-called  capryl  alcohol,  CH3(CH2)sCH(OH)CHa. 


279 


CRESOL 


DISTRIBUTION  OF  CRESOL  BETWEEN  WATER  AND  ETHER.    (Vaubel,  1903.) 

Composition  of  Solvent.  Gms-  ^jj  'm  H2°           ln  Ether  Layer. 

200  cc.  H20+ioo  cc.  Ether  0.0570               i  .0760 

200  cc.  H2O+200  cc.  Ether  0.0190               i  .1144 

FREEZING-POINT  LOWERING  DATA  (Solubility,  see  footnote,  p.  i)  FOR  MIX- 
TURES OF  o,  m  AND  p  CRESOL  (each  determined  separately)  AND  OTHER 
COMPOUNDS. 

Mixture.  Authority. 

o,  m  and  p  Cresol  +  Dimethylpyrone  (Kendall,  1914.) 

-j-  Picric  Acid  (Kendall,  1916.) 

"                            +  Pyridine  (Hatcher  and  Skirrow,  1917.) 

0  and  p                        +  (Bramley,  1916.) 

+  Sulfuric  Acid  (Kendall  and  Carpenter,  1914.) 

4-  Urea  (Kremann,  1907.) 


o,  m  and  p  ,    

Trinitrocresol  +  Naphthalene 


(Saposchinikow  and  Gelvich,  1903,  1904.) 


CROTONIC  ACIDS  a.  ^CHsCHrCHCOOH,  0  =  HCH3C:CHCOOH. 
FREEZING-POINT  LOWERING  DATA  FOR  MIXTURES  OF  CROTONIC  ACIDS  AND  OF 
CROTONIC  ACID  AND  OTHER  COMPOUNDS. 

Mixture.  Authority. 

a  Crotonic  Acid  +  ft  Crotonic  Acid  (Morrell  and  Hanson,  1904.) 

"     +  Dimethylpyrone  (Kendall,  1914.) 

+  Sulfuric  Acid 

Chlorocrotonic  Acid  +  Dimethylpyrone 
"     +  Sulfuric  Acid 


(Kendall  and  Carpenter,  1914.) 

(Kendall,  1914.) 

(Kendall  and  Carpenter,  1914.) 


Methyl   CRYPTOPINES,    A,  B  and  C  forms,  C22H25O5N. 

The  solubilities  of  the  three  forms  in  benzene,  determined  by  lowering  of  the 
freezing-point,  are:  5  gms.  A  form  per  liter  at  5°,  30  gms.  B  form  and  no  gms.  C 
form.  (Sidgwick,  1915.) 

CUMINIC  ACID   C3H7C6H4.COOH    (p  Isopropyl  Benzole  Acid). 

SOLUBILITY  IN  WATER  AT  25°.    (Paul,  1894.) 
looo  cc.  sat.  solution  contain  0.1519  gm.  or  0.926  millimol  cuminic  acid. 

PseudoCUMIDINE  (CH3)3.C6H2.NH2  (s,  5  Amino,  i.  2.  4,  Trimethyl  Benzene). 
SOLUBILITY  IN  WATER. 

(Lowenherz,  1898.) 
t°.  19.4°.  23.7°.  28.7°. 

Gms.  \l/  Cumidine  per  liter  H2O     i .  198  i  .330  i  .498 

CYANAMIDE   CN.NH2. 

SOLUBILITY  IN  WATER,  DETERMINED  BY  FREEZING-POINT  METHOD. 

(Pratolongo,  1913.) 

Gms.  " 


Gms. 

fc°  of  Congealing. 

CN.NH2  per 
100  Gms. 

Solid  Phase. 

Sat.  Sol. 

—    0.62 

2.58 

Ice 

-    3.96 

9.42 

" 

-     7.58 

18.40     . 

"  . 

—  12.72 

30-9 

<( 

—  i6.6Eutec. 

37-8 

"  +CN.NH, 

-15-6 

38.75 

CN.NH2 

f  of  Congealing. 


Sat.  Sol. 

-14-39 

40.19 

-  2.49 

56.80 

+14.50 

77.20 

25.6 

87-I5 

37-90 

96.77 

42.9 

100 

Solid 
Phase.' 

CN.NH, 


Similajata  forCN.NHi  +  urea  and^CN.NHa  +  dicyandiamide  are  also'  given. 

DiCYANDIAMIDINE    Perchlorate   C2H6N4OHC1O4. 
'"loo'gms.  H2O  dissolve  9.97  gms.  of  the  salt  at  17°  (d  sat.  sol.  =  1.039).  (Carlson,  1910.; 


CYANOGEN  280 

CYANOGEN   (CN)2. 

SOLUBILITY  IN  WATER  AND  OTHER  SOLVENTS. 

(Berthelot,  1904.) 

The  determinations  were  made  over  mercury  with  exclusion  of  air.  The 
mercury  was  not  attacked  by  the  (CN)2.  On  account  of  polymerization,  the 
solubility  increased  with  time  of  contact  and  amount  of  agitation  of  the  mixture. 

One  volume  of  H2O  at  30°  dissolves  3.5  vols.  (CN)2  after  2  hours,  and  9.7  vols. 
after  97  hours. 

One  volume  of  abs.  alcohol  at  20°  dissolves  26  vols.  (CN)2  immediately;  39 
vols.  after  4  hours;  89  vols.  after  48  hrs.  and  223  vols.  after  4  days. 

One  volume  glacial  acetic  acid  dissolves  42  vols.  of  (CN)2  immediately  and 
50.5  vols.  after  3  days. 

One  volume  of  chloroform  dissolves  about  19  vols.  (CN)2  immediately  and 
29-30  vols.  with  time. 

One  volume  of  benzine  finally  dissolves  28  vols.  (CN)2. 

One  volume  of  rectified  turpentine  dissolves  9-10  vols.  of  (CN)2. 

One  volume  of  ether  dissolves  5  vols.  (CN)2  at  20°.  (Gay  Lussac.) 

CYCLOHEXANE    (Hexamethylene,  Hexahydrobenzene)  CH2  <  (CH2.CH2)2  > 
CH2. 

Freezing-point  data  (solubility,  see  footnote,  p.  i)  for  mixtures  of  cyclo- 
hexane  and  ethylene  bromide  are  given  by  Baud  (i9i3b).  Results  for  mix- 
tures of  cyclohexane  and  methyl  alcohol  are  given  by  Lecat  (1909).  Results 
for  mixtures  of  cyclohexane  and  piperidine  are  given  by  Mascarelli  and  Con- 
stantino (1909,  1910). 

CYCLOHEXANOL  (CH2)5.CHOH. 

100  gms.  H2O  dissolve  5.67  gms.  cyclohexanol  at  11°.  (de  Forcrand,  1912.) 

loo  gms.  cyclohexanol  dissolve  11.27  Sms-  H2O  at  11°. 

RECIPROCAL  SOLUBILITY  OF  CYCLOHEXANOL  AND  WATER,  DETERMINED  BY 
THE  FREEZING-POINT  METHOD. 

(de  Forcrand,  1912.) 

Gm.  (CH2)5.CHOH  Gm.  (CH2)5CHOH 

t°  of  Solidification.  per  100  Gms.  t°  of  Solidification.  per  100  Gms. 

Mixture.  Mixture. 

+  22.45  loo                       -57.4Eutec.  95-°3° 

17.48  99-767                -43-2  93-I50 

—  1.40  98.817                -33  91.962 

—34.10  96.868                —18.50  90.980 

-46.80  95-910                -14-58  9°-36 

-55.70  95-I70  .     -12.05  88.73 

Freezing-point  data  for  mixtures  of  cyclohexanol  and  phenol  are  given  by 
Mascarelli  and  Pestalozza,  1908,  1909. 

CYCLOHEXANONE  (CH2)6:CO. 

Freezing-point  data  for  mixtures  of  cyclohexanone  and  phenol  are  given  by 
Schmidlin  and  Lang,  1910. 

CYTISINE    (Ulexine)    CUH16N2O   (m.  pt.  I5i°-I5i.5°). 

SOLUBILITY  IN  SEVERAL  SOLVENTS  AT  15°. 

(Van  de  Moer,  1891.) 

Q0iv<,nf  Gms.  CuHiRN2O                                 QniWnt  Gms-  CuHwNjO  per 

bolvent.  per  ipo  Gms.  Sat.  Sol.                              Solvent.  100  Gms.  Sat.  Sol. 

Water  soluble  in  all  proportions  Benzine  1.26 

Alcohol  "          "              "  Petroleum  Ether  insol. 

Chloroform  "                         "  Amyl  Alcohol  0.303 

Ether  (d  0.725)  0.302  Carbon  Disulfide  insol. 

Ether,  abs.  insol.  Ethyl  Acetate  very  soluble 


28l 


DEXTRIN 


DEXTRIN  CuH»Qio. 

SOLUBILITY  IN  WATER.     (Lewis,  1914.) 

"  In  the  case  of  dextrin,  however,  no  matter  how  small  an  amount  of  water  be 
employed,  under  no  condition  does  the  concentration  of  the  solution  remain  con- 
stant, while  on  the  other  hand  the  addition  of  further  solvent,  never  fails  to 
dissolve  additional  dextrin,  although  the  use  of  no  amount  of  water,  however 
large,  will  dissolve  the  whole  of  the  sample." 


100  gms.  pyridine  dissolve  65.44  gms.  dextrin  at  20-25°. 

100  gms.  aq.  50%  pyridine  dissolve  102  gms.  dextrin  at  20-25°. 


(Dehn,  1917.) 


DIACETYL   TARTARIC   ETHER    (m.    pt.    104°)    DIACETYL   RACEMIC 
ETHER    (m.  pt.  84°). 

Freezing-point  lowering  data  for  each  of  these  compounds  in  ethylene  bromide 
and  in  p  xylene  are  given  by  Bruni  and  Finzi,  1905. 

DIBENZYL   C6H5.CH2.CH2.C6H5. 

Freezing-point  lowering  data  for  mixtures  of  dibenzyl  and  stilbene  are  given  by 
Garelli  and  Calzolari,  1899. 


DIDYMIUM  Ammonium  NITRATE   Di(NO3)3.2NH4NO3. 
100  gms.  H2O  dissolve  292  gms.  of  the  salt  at  15°. 


(Holmberg,  1907.) 


DIDYMIUM  SULFATE  Di2(SO4)3. 

SOLUBILITY  IN  WATER. 

Gms. 


(Marignac,  1853.) 


t°. 

per  100 

Solid  Phase. 

Gms.  H2O. 

12 

43.1 

Di2(S04)3 

18 

25.8 

tt 

25 

20.  6 

tt 

38 

13 

t( 

50 

ii 

tt 

19 
40 

So 

100 

per  100 
Gms.  H2O. 

II.7 
8.8 
6-5 

1.8    • 

Solid  Phase. 

Di2(SO4)3.6H2O 
Di2(SO4)3.8H2O 

DIDYMIUM  POTASSIUM   SULFATE   K2SO4.Di2(SO4)3.2H2O. 
100  gms.  H2O  dissolve  1.6  grams  of  the  double  salt  at  18°. 

DIDYMIUM  SULFONATES. 

SOLUBILITY  IN  WATER. 


Salt. 


Didymium  Benzene  Sulfonate 

'        m  Nitro  Benzene  Sulfonate 


m  Chloro 

m  Bromo       "  " 

Chloro  Nitro  " 

a  Naphthalene  Sulfonate        Di(Ci0H7SO3)3.6H2O 

1.5  Nitro  "  "  Di(CioH6(N02)SO3)3.6H2O 

1.6  " 

1.7  "  " 


(Holmberg,  1907.) 
Formula.  t°. 

Di(C6H5SO3)3.9H2O  15 

Di(C6H4(NO2)SO3)3.6H2O  15 

Di(C6H4ClS03)3.9H2O  15 

Di(C6H4BrSO3)3.9H2O  15 

Di(C6H4Cl(N02)S03*)3.i6H2O    15 

IS 
15 

Di(CioH6(N02)S03)3.9H2O  15 

Di(Ci0H6(NO2)SO3)3.9H2O  15 


(Marignac.) 


Gms. 

Anhydrous 
Salt  per  100 
Gms.  H20. 

S3-I 
47-8 
12.7 

14-3 


0.52 
0.18 


*  (SO3:NO2:C1  -  1.3.6.) 

DIETHYLAMINE   see  ETHYLAMINE,   page  294. 

DIONINE    (Ethyl  Morphine)    Ci9H23NO3. 

100  cc.  H2O  dissolve  0.2613  gm.  Ci9H23NO3  at  20^. 
loo  cc.  oil  of  sesame  dissolve  0.5144  gm. 


at  20°. 


(Zalai,  1910.) 


DIPHENYL  282 

DIPHENYL   CeHs-CeHfi. 

100  grams  absolute  methyl  alcohol  dissolve  6.57  grams  at  19.5°. 

100  grams  abs.  ethyl  alcohol  dissolve  9.98  grams  at  19.5°.  (de  Bruyn,  1892.) 

Freezing-point  data  (Solubility,  see  footnote,  p.  i)  are  given  for  mixtures  of 
diphenyl  +  naphthalene  by  Washburn  and  Read  (1915)  and  by  Vignon  (1891). 
Results  for  diphenyl  -f-  phenanthrene  and  for  diphenyl  +  triphenylmethane  are 
given  by  Vignon  (1891). 

DIPHENYLAMINE   (C6H6)2NH. 

RECIPROCAL  SOLUBILITY  OF  DIPHENYLAMINE  AND  WATER,  BY  SYNTHETIC 

I  [METHOD. 

(Campetti  and  del  Grosso,  1913.)  ' 

Cms.  (C6H5)2  NH  Cms.  (C6H5)2NH  Cms.  (C6H5)2NH 

t°.  per  100  Gms.  t°.          per  ipo  Gms.  t°.  per  ipo  Gms. 

Mixture.  Mixture.  Mixture. 

231  1.48  305crit.  t.  47.5  239  88.28 

264  3.49  304  62.52  229  90.23 

275  5.62  299  73.07  210  92.93 

297  16.50  289  82.08  152  97-19 

303  45.16  249  86.73 

Similar  data  for  the  systems  diphenylamine  +  ether  and  diphenylamine  -f- 
isopentane  are  given  by  Campetti,  1917. 

SOLUBILITY  OF  DIPHENYLAMINE  IN  SEVERAL  SOLVENTS. 

Solvent.  f.  pe^gMLt.  Authority. 

Water  20-25  0.03  (Dehn,  1917.) 

Methyl  AlCOhol  14.5  45  .  2  (Timofeiew,  1894.) 

"  "  19-5  57-5  (de  Bruyn,  1892.) 

Ethyl  Alcohol  14  .  5  39.4  (Timofeiew,  1894-) 

"  "  19.5  56  (de  Bruyn,  1892.) 

Propyl  Alcohol  14.5  29.4  (Timofeiew,  1894.) 

Pyridine  20-25  302  (Dehn,  1917.) 

Aq.  50%  Pyridine         20-25        two  layers  formed 

SOLUBILITY  OF  DIPHENYLAMINE  AND  ALSO  OF  TRIPHENYLAMINE  IN  CARBON 

DlSULFIDE.      (Arctowski,  1895.) 
NH(C6H^)2  in  CS,  N(C6H5)3  in  CS,. 


t°. 

Gms.  per  100 
Gms.  Solution. 

t°. 

Gms.  per  100 
Gms.  Solution. 

-88J 

0.87 

-83 

I.9I 

-117 

0-37 

-91 

1.56 

—  102 

1.24 

—  II3| 

0.98 

SOLUBILITY  OF  DIPHENYLAMINE  IN  HEXANE  AND  IN  CARBON  DISULFIDE. 

(Etard,  1894.) 

Gms.  NH(C«HE)j  Gms.  NH(CfiHR)2 

$».            per  IPO  Gms.  Sol,  in;  t°t  per  100  Gms.  Sol,  in: 

Hexane.  CS^T*  Hexane.  CS2.  ' 

-60        ...            1.3  o  2.6        33.7 

—  50           ...                 2.2  +10  3.8            46.8 

—  40           ...                 3.8  20  6.7            60.9 
-30            0.5               7.2  30  13.8            76 

—  20        0.8        12.5  40  47 

—  io        1.4        21.6  50  94 


283 


DIPHENYLAMINE 


FREEZING-POINT  DATA  FOR  MIXTURES  OF  DIPHENYLAMINE  AND  OTHER 

COMPOUNDS. 


Diphenylamine 


Diphenylmethylamine 


+  Acetyldiphenylamine 
4-  Ethylene  Bromide 
-j-  Naphthalene 
+  a  Naphthylamine 
+  Nitronaphthalene 
+  a  and  /3  Naphthol 
-j-  Paraffin 
+  Phenanthrene 
+  Phenol 
-j-  Resorcinol 
-j-  p  Nitrotoluene 
-{-2.4  Dinitrotoluene 
-j-  a  Trinitrotoluene 
-j-  p  Toluidine 
+  Urethan 
Phenol 


(Boeseken,  1912.) 

(Dahms,  1895.) 

(Roloff,  1895;  Vignon,  1891.) 

(Vignon,  1891.) 

(Battelli  and  Martinetti,  1885.) 

'Vignon,  1891.) 

(Palazzo  and  Battelli,  1883.) 

(Narbutt,  1905.) 

(Philip,  1903.) 

(Vignon,  1891.) 

(Giua,  1915.) 


+  o  Chlorophenol 
Hexanitrodiphenylamine    +  a  Trinitrotoluene 

DIPHENYLAMINE   BLUE. 

SOLUBILITY  IN  SEVERAL  SOLVENTS  AT  23°. 


(Vignon,  1891.) 

(Pushin  and  Grebenschikov,  1913.) 

(Bramley,  1916.) 

(Giua,  1915.) 


Solvent. 

Methyl  Alcohol 

Ethyl 

Amyl 


(Szathmary  de  Szachinar,  1910.) 


Gms.  Diphenylamine  Blue 
per  100  Gms.  Sat.  Sol. 


0.385 
0.230 
o  .  049 


Acetone 
Aniline 


Diphenylamine  Blue 
per  100  Gms.  Sat.  Sol. 

°-i77 
°-395 


DIPHENYL  SULFIDE   (C6H5)2S,  etc. 

Freezing-point  lowering  data  for  mixtures  of  (CeHs^S  +  (C6H5)2Se, 
(C6H6)2Te,  (C6H6)2S  +  (C6H6)2O,  (QH.),Se+(G,H.),Tef  are  given  by  Pascal  (1912). 

DYES. 

Data  for  the  distribution  of  12  dyes  between  water  and  isobutyl  alcohol  at  25°, 
are  given  by  Reinders  and  Lely,  Jr.  (1912). 

DYSPROSIUM  OXALATE   Dy2(C2O4)3.ioH2O. 

100  cc.  aq.  20%  methylamine  oxalate  dissolve  0.276  gm.  Dy^QjOOs-  | (Grant  and 
"         ethylamine  "  "        1.787     "  \    James, 

triethylamine       "  "       1.432  )    Wl) 

EDESTIN  and  Edestin  Salts. 

SOLUBILITY  IN  AQ.  SALT  SOLUTIONS  AT  25°. 

(Osborne  and  Harris,  1905.) 

The  determinations  were  made  by  shaking  an  excess  of  the  air-dry  preparation 
with  20  cc.  of  the  salt  solution,  allowing  the  globulin  to  settle  and  determining 
nitrogen  in  10  cc.  of  the  clear  supernatant  solution.  The  edestin  or  edestin  salt 
was  calculated  from  the  N.  The  results  are  given  in  the  form  of  curves.  The 
following  figures  were  read  from  the  curve  for  the  solubility  of  neutral  edestin  in 
aq.  NaCl. 

Gms.  NaCl per  20  cc.  Solvent     — »  0.468    0.585    0.702    0.818    0.935 
Gm.  Edestin  per  20  cc.  Sat.  Sol. —>  0.25      0.55      0.92       1.25      1.45 

Curves  are  also  given  for  the  solubility  of  edestin  in  aqueous  solutions  of  many 
other  salts  and  of  the  solubility  of  edestin  chloride,  bichloride  and  sulfate  in  aq. 
sodium  chloride  solutions. 

100  gms.  pyridine  dissolve  0.07  gm.  edestin  at  20-25°.  (Dehn,  1917.) 

ioo  gms.  aq.  50%  pyridine  dissolve  9.05  gm.  edestin  at  20-25°. 


ELATERIN  284 


ELATERIN 

ibo  cc.  90%  alcohol  dissolve  0.09  gm.  elaterin  at  15-20.    (Squire  and  Caines,  1905.) 
100  cc.  chloroform  dissolve  4  gms.  elaterin  at  15-20.  "  " 

EMETINE  and   Salts. 

SOLUBILITY  IN  WATER. 

(Carr  and  Pyman,  1914.) 

c  I*  •p^rrv.nio  *°         Gms.  Hydrated  Salt 

Salt-  Formula.  t.         per  I00  cc.  Sat.  Sol. 

Emetine  Hydrochloride  C29H4oO4N2.2HC1.7H20  18                13  .  i 

"     Hydrobromide    C29H4oO4N2.2HBr.4H2O  17-18             1.9 

"      Nitrate                C29H4oO4N2.2HNO3.3H2O  17-18            3.7 

"      Sulfate                C29H4oO4N2.H2S04.7H2O  17-18  more  than  100 

ERBIUM   OXALATE   Er2(C2O4)3.i4H2O. 

SOLUBILITY  IN  AQ.  SULFURIC  ACID  AT  25°. 

(Wirth,  1912.) 

Solid  Phase. 

Er2(C204)3.i4H20 


Normality  of 
Aq.  H2SO4. 

Gms.  per  100  Gms.  Sat.  Sol. 

'  Er203- 

Er2(QA)3. 

2.l6 

0.329 

0.5144 

3-n 

0-493 

0.7708 

4-32 

0.7036 

1.  10 

6.I7S 

I  .IO 

1.72 

ERBIUM   Dimethyl  PHOSPHATE   Er2[(CH3)2PO4]6. 

IOO  gms.  H2O  dissolve  1.78  gm.  Er2[(CH3)2PO4]6  at  25°.     (Morgan  and  James,  1914.) 

ERBIUM   SULFATE   Er2(SO4)3.8H2O. 

SOLUBILITY  IN  WATER  AND  Aq.^H2S04  AT  25°. 

(Wirth,  1912.) 

[Gms.  per  ioo  Gms. 

Solid  Phase. 


Normality 
of  H2S04. 

Gms.  per 

Sat. 

ioo  Gms. 
Sol.                Solid  Phase 

Normality 
•      of  H2SO4. 

[Gms.  per 
Sat. 

ioo  Gms. 
Sol. 

Er203. 

Er.CSO,);,. 

'  Er203. 

Er2(S04)3: 

Water  alone  7 

•339 

II 

.94    ErzCSO^.SHzO       2 

.16 

3 

.98 

6. 

473 

O 

.1 

7 

•389 

12 

.02                " 

6 

•175 

0 

•9352 

i  , 

52i 

0 

•505 

6 

.249 

10 

.  164 

12 

.6 

0 

.0852 

0 

,1386 

I 

.1 

5 

.256 

8 

•549 

ERBIUM  Bromonitrobenzene  SULFONATE  Er(C6H3Br.NO2.SO3, 1.4.2)3. 12H2O. 

ioo  gms.  sat.  solution  in  water  contain  6.056  gms.  anhydrous  salt  at  25°. 

(Katz  and  James,  1913.) 

ERUCIC  ACID   C8H17CH:CH(CH2)nCOOH. 

SOLUBILITY  IN  ALCOHOLS. 

(Timofeiew,  1894.) 

Gms.  Erucic  Gms.  Erucic 

Alcohol.  t°.          Acid  per  ioo  Alcohol.  t°.          Acid  per  ioo 

Gms.  Sat.  Sol.  Gms.  Sat.  Sol. 

Methyl  Alcohol      —   2  2.25  Ethyl  Alcohol  '+21.4  63.4 

+  18  60.4  Propyl  Alcohol  -   2  10.2 

21.4  62                 "             "  +18  60.5 

Ethyl  Alcohol         -   2  8.24                                        21.4  63 

ERYTHRITOL   (CH2OH.CHOH)2. 

ioo  gms.  H2O  dissolve  61.5  gms.  erythritol  at  20-25°.  (Dehn«  *9i7) 

ioo  gms.  aq.^0%  pyridine  dissolve  8.47  gms.  erythritol  at  20-25°. 

ioo  gms.  pyridine  dissolve  2.50  +  gms.  erythritol  at  20-25.  (Dehn.Jigi?;  Holty,  1905.) 


285 


ETHANE 


uinr,  ^2n6.        SOLUBILITY  IN  WATER. 

(Winkler,  1901.) 

t°. 

/9. 

/S'. 

3. 

t°. 

0. 

/?'. 

j. 

O 

0 

.0987 

o 

.0982 

0 

.0132 

40 

0 

.0292 

o  0271 

0.0037 

5 

0 

.0803 

0 

.0796 

0 

.0107 

50 

o 

.0246 

0.0216 

0.0029 

10 

0 

.0656 

0 

.0648 

0 

.0087 

60 

0 

.0218 

0.0175 

0.0024 

15 

0 

•0550 

0 

.0541 

0 

.0073 

70 

0 

.0195 

0.0135 

0.0018 

20 

0 

.0472 

0 

.0462 

o 

.0062 

80 

o 

.0183 

0.0097 

0.0013 

25 

0 

.0410 

0 

.0398 

0 

.0054 

90 

0 

.0176 

0.0054 

0.0007 

30 

0 

.0362 

o 

•0347 

0 

.0049 

100 

o 

.0172 

o.oooo 

o.oooo 

/?  =  Absorption  coefficient,  i.e.,  the  volume  of  gas  (reduced  to  o° 
and  760  mm.)  absorbed  by  i  volume  of  the  liquid  when  the  pressure 
of  the  gas  itself  without  the  tension  of  the  liquid  amounts  to  760  mm. 

ft'  =  Solubility,  i.e.,  the  volume  of  gas  (reduced  to  o°  and  760  mm.) 
which  is  absorbed  by  one  volume  of  the  liquid  when  the  barometer 
indicates  760  mm.  pressure. 

q  =  the  weight  of  gas  in  grams  which  is  taken  up  by  100  grams  of 
the  pure  solvent  at  the  indicated  temperature  and  a  total  pressure 
(that  is,  the  partial  pressure  of  the  gas  plus  the  vapor  pressure  of  the 
liquid  at  the  absorption  temperature)  of  760  mm. 

Freezing-point  data  for  mixtures  of  ethane  and  hydrochloric  acid  are  given  by 
Baume  and  Georgitses,  1912,  1914. 

SOLUBILITY  OF  ETHANE  IN  SEVERAL  ALCOHOLS  AND  OTHER  SOLVENTS. 

(McDaniel,  1911.) 
Solvent. 

Methyl  Alcohol  (99%)  22.1 
"  "  30.2 

40 
49.8 

Ethyl  Alcohol  (99.8%)  22,2 

«          « 

(I  U 

Isopropyl  Alcohol 


Abs.  coef.  A  =  vol.  of  ethane  absorbed  by  unit  volume  of  solvent  at  the  temp,  stated. 
For  definition  of  Bunsen  Coef.  B,  see  /3  above,  and  also  carbon  dioxide,  p.  227. 
Additional  data  for  the  solubility  of  ethane  in  amyl  alcohol  are  given  by  (Friedel 
and  Gorgeu,  1908). 

ETHYL  ACETATE   CH3COOC2H5. 

SOLUBILITY  OF  ETHYL  ACETATE  IN  WATER  AND  VICE  VERSA. 

(Merriman,  1913,  see  also  Seidell,1 1910.) 

Results  for  Ethyl  Acetate  in  Water.  Results  for  Water  in  Ethyl  Acetate. 

Gms.  H2O  per  100 


t°. 

Abs. 
Coef.  A. 

"  Bunsen                c/o™,,*             *° 
Coef.  B.               Solvent.           t  . 

Abs. 
Coef.  A. 

Bunsen 
Coef.  B. 

22.1 

0.4436 

0.4102       Amyl  Alcohol  22 

0.4532 

0.4196 

30.2 

0.4278 

0.3883                      "        30.1 

0.4444 

0.4002 

40 

0.3938 

0.3436       Benzene           22.1 

0.4954 

0.4600 

49.8 

0.2695 

0.2278 

35 

0.4484 

0.3976 

22.2 

0.4628 

0.4282 

40.1 

0.4198 

0.3661 

30-r 

0.4503 

0.4051 

49.9 

0-3645 

0.3081 

40 

0.4323 

0.3771       Tol 

ene           25 

0.4852 

0.4450 

21.5 

0.4620 

0.4275 

3° 

0.4778 

0.4300 

29.9 

0.4532 

0.4081 

40.1 

0.4675 

0.4080 

40 

0.4400 

0.3837 

50.2 

0-4545 

0.4013 

60.3 

0.4244 

0.3478 

60 

0.4502 

0.3690 

t°. 

d£  of  Sat.  Sol. 

Gms.  CH3COOC2H5 
per  100  Gms.  H2O.| 

0 

5 

*  1.  0034 
1.0022 

II.  21 
10.38 

10 

I  .  OOOQ 

9.67 

15 
20 

25 

0.9995 
0.9979 
0.9962 

9-°5 
8-53 
8.08 

30 

0.9943 

7.71 

40 

0.9901 

7.10 

t°. 

d^  of  Sat.  S< 

o 

10 

0.9280 
0.9164 

20 

0.9054 

25 

3° 

40 

O.9OO2 
0.8953 
0.8863 

50 
60 

.  .  . 

2.34 

2.68 
3-07 
3-30 
3-52 
4.08 
4.67 
5-29 


ETHYL  ACETATE 


286 


SOLUBILITY  IN  WATER  AND  IN  AQUEOUS  SALT  SOLUTIONS  AT  28°, 

(Euler  —  Z.  physik.  Chem.  31,  365,  '99;  49,  306,  '04.) 


Cone,  of  Salt 
Solution. 

CHgCOOCjiHs 

per  Liter. 

Solvent.            *  -.    /  

Cone,  of  Salt 
Solution. 

CH3COOC2H» 
per  Liter. 

^olvent. 

Nor-   Gms  per 
mality.    Liter. 

Gram 
Mols. 

Grams. 

Nor-  Gms.  per    Gram 
nudity.    Liter.      Mols. 

Grams. 

Water 

0 

O 

0. 

825 

75.02 

NaCl(at  18°) 

i 

14.62 

0.76 

67.0 

KNOa 

i 

5° 

•59 

O. 

77 

67.81 

«           « 

i 

29-25 

0.67 

59-o 

M 

I 

101 

.19 

0. 

72 

63.40 

«           « 

i 

58.5 

°-5I 

45-o 

It 

2 

202 

.38 

O. 

625 

55-04 

Na2S04 

i 

71.08 

0.465 

40.96 

KC1 

i 

18 

•4 

0. 

747 

65-79 

"      (at  18°) 

i 

35-54 

0.61 

54-0 

« 

i 

36 

.8 

0. 

685 

65-33 

((           (t 

i 

71.08 

0.42 

37-o 

M 

I 

73 

.6 

O. 

575 

50.64 

MgS04 

1 

16.30 

o-733 

64.55 

«    . 

2 

147 

.2 

0. 

41 

36.  ii 

a 

i 

32.6 

0-655 

57.68 

Nad 

\ 

14 

.62 

0. 

745 

65.61 

(i 

i 

65.21 

0-505 

44-47 

M 

i 

29 

•25 

0. 

677 

59.62 

ZnSO4 

1 

20.18 

0-733 

64.55 

« 

I 

58 

•5 

0. 

545 

47-99 

« 

i 

40.36 

0-653 

57-50 

M 

2 

117 

.0 

O. 

3J5 

27.74 

u 

i 

80.73 

0.500 

44-03 

Additional  data  for  the  influence  of  salts  upon  the  solubility  of  ethyl  acetate  in 
water  are  given  by  Lundin,  1913. 

SOLUBILITY  OF  ETHYL  ACETATE  IN  AQUEOUS  SOLUTIONS  OF  ETHYL  ALCOHOL  AT  25°. 

(Seidell,  1910.) 


cc.  CH3COOC2H5  Gms.  CH3COOC2H, 
per  TOO  Gms. 
Solvent. 

8.6 


10.9 

13-3 
19.6 

37-o 
66.7 

00 

SOLUBILITY  OF  ETHYL  ACETATE  IN  AQUEOUS  ETHYL  ALCOHOL,  METHYL 
ALCOHOL,  AND  ACETONE  MIXTURES  AT  20°. 

(Bancroft  —  Phys.  Rev.  3,  122,  131,  '95-' 96.) 

In  Ethyl  Alcohol.  In  Methyl  Alcohol.  In  Acetone. 

Per  i  cc.  C2H6OH. 


Wt.  « 
in! 

70  C2H5OH 
Solvent. 

d&  of  Sat. 
Sol. 

cc.  CH3COO( 
per  100  cc 
Solvent. 

0 

o-999 

10 

5 

0-993 

10-5 

10 

0.986 

12 

15 

0-974 

15 

20 

0.960 

27 

25 

0-945 

44 

30 

0.931 

70 

35 

0.918 

125 

40 

CO 

cc-HaO*     , 

:H3COOC2H6.t 

10 

0.25 

8 

0.27 

4 

0-35 

2 

1.02 

1.  06 

2.50 

0.65 

5-0 

0-54 

7.0 

0.44 

10.  0 

Per  i 

cc.  CH3OH. 

Per  i 

cc.  (CH3)2CO. 

cc.  H2O. 

CHaCObc-zHB. 

cc.  H2O. 

CH3COOC2H8. 

10 

1.  08 

10 

1.  01 

3 

0.68 

5 

O.6o 

*•$ 

1.69 

2 

o-43 

1.29 

2.50 

I  .5 

0.47 

1.0 

4-9 

I  .O 

0.63 

0.98 

7-o 

0.8 

o-74 

I  -O 

8.0 

0.51 

1.  00 

1.03 

10.  0 

0.25 

2.00 

0.29 

5.00 

1  acetate.                     t  Saturated  with  water. 

Data  for  the  distribution  of  ethyl  acetate  between  petroleum  and  water,  ben- 
zene and  water,  and  benzene  and  a  large  number  of  aqueous  solutions,  at  various 
temperatures,  are  given  by  Philip  and  Bramley,  1915. 


287 


ETHYL  ALCOHOL 


RECIPROCAL  SOLUBILITY  OF  ETHYL  ALCOHOL  AND  WATER  AT  Low  TEM- 
PERATURES, DETERMINED  BY  THE  FREEZING-POINT  METHOD. 

(Pictet  and  Altschul,  1895;  Pickering,  1893.) 
Cms. 


t°.  of 
Freezing. 

Sp.  Gr.    C2HBOH  per  Solid 
Sat.  Sol.      100  Gms.    Phase. 

Sat.  Sol. 

—    I 

0.9962 

2.5        Ice 

—    2 

0.9916 

4.8          « 

-  3 

0.9870 

6.8       " 

-  5 

0.9824 

11.3 

-  6.1 

0.9793 

13-8       " 

-  8.7 

0.9747 

17.5       " 

-  9.4 

0.9732 

18.8 

—  10.6 

0.9712 

20.3 

—  12.2 

o  .  9689 

22.1 

-14 

0.9662 

24  .  2 

-16 

0.9627 

26.7      •• 

—  18.9 

0.9578 

29.9 

t°.  of               Sp.  Gr. 
Freezing.            Sat.  Sol. 

Gms. 
QHjOHper        Solid    . 
100  Gms.         Phase. 

Sat.  Sol 

-23.6      o 

.9512 

33-8 

Ice 

—28.7      o 

.9417 

39 

H 

-  33-9      o 

.9270 

46.3 

" 

—  41          o 

.9047 

56-1 

" 

-   50 

68 

" 

-  60 

.  .  . 

75 

H 

-   70 

.  .  . 

80 

« 

-  80 

.  .  . 

83-5 

" 

—  100 

.  .  . 

89-5 

" 

—  uSEutec. 

.  .  . 

93-5 

"   +C2H6OH 

"~II5 

96 

QH6OH 

—  110.5 

.  .  . 

100 

" 

The  result  for  the  eutectic  and  for  the  f.-pt.  of  C2H5OH  are  by  Puschin  and 
Glagoleva,  1914,  1915;  the  other  data  for  concentrations  of  C2HsOH  above  70% 
were  obtained  by  exterpolation.  Additional  data  for  the  freezing-point  lowering 
are  given  by  Rozsa  (1911). 

Freezing-point  lowering  data  for  mixtures  of  ethyl  alcohol  and  hydrochloric 
acid  are  given  by  Maass  and  Mclntosh,  1913. 

The  distribution  coefficient  of  ethyl  alcohol  between  amylalcohol  and  water 
was  found  by  Fontein  (1910)  to  be  1.13  at  15.5°  and  1.21  at  28°. 


MISCIBILITY  OF  ETHYL  ALCOHOL  WITH  MIXTURES  OF: 
Benzaldehyde  and  Water  at  o°. 

(Bonner,  1910.) 
Composition  of  Homogeneous  Mixtures. 


Benzene  and  Water  at  15°. 

(Bonner,  1910.)     (See  also,  p.  125.) 

Composition  of  Homogeneous  Mixtures. 


Gms. 

Gms. 

Gms. 

Sp. 

Gr.  of 

Gms. 

Gms. 

Gms. 

Sp.  Gr.  of 

QH5CHO. 

H20. 

C2H5OH. 

Mixture.                        C6H6. 

H20. 

C2H5OH. 

Mixture. 

0-957 

0.043 

0 

•  159 

I 

.02 

O 

.987 

o 

.013 

0.170 

0.86 

0.898 

O.  IO2 

O 

.283 

I 

.OI 

0 

•937 

0 

.063 

0.356 

0.87 

O.SOO 

0.200 

0 

.420 

0 

•99 

*0 

.900 

0. 

100 

0.500 

0.86 

0.700 

0.300 

O 

•  550 

O 

.98 

o 

.800 

o 

.200 

0.860 

0.86 

^0.598 

O.4O2 

O 

.601 

0 

•97 

0 

.700 

o 

,300 

0.910 

0.88 

0.430 

0 

.610 

0 

.600 

o, 

.400 

1.07 

0.87 

0.496 

0.504 

o 

•643 

o 

.96 

o 

.500 

o 

.500 

1.18 

0.87 

0-394 

0.606 

o 

.681 

0 

•95 

o 

.400 

o 

.600 

I  .22 

0.88 

0.298 

0.702 

0 

.701 

0 

•95 

0.300 

o 

,700 

I.  21 

0.89 

0.200 

0.800 

0 

.670 

o 

•95 

o 

.201 

o, 

799 

I-I3 

0.89 

O.IOO 

O.9OO 

o 

.610 

0 

.96 

o 

.100 

o 

.900 

0.97 

0.92 

0.031 

0.969 

0 

.461 

o 

•97 

0 

.020 

o 

.980 

o-59 

0.94 

NOTE.  —  The  determinations  were  made  by  gradually  adding  ethyl  alcohol  to 
the  mixtures  of  the  given  amounts  of  water  and  the  other  constituent  until  a 
homogeneous  solution  was  obtained.  The  results  give  the  binodal  curve  for  the 
system.  The  author  also  determined  "tie  lines"  showing  the  compositions  of 
various  pairs  of  liquids  which  may  exist  in  equilibrium.  As  the  two  layers 
approach  each  other  in  composition,  the  tie  line  is  gradually  shortened  and  finally 
reduced  to  a  point,  designated  as  the  "plait  point"  of  the  binodal  curve.  This 
point  is  indicated  by  a  *  in  the  above  tables.  The  mixtures  above  and  below  the 
*  correspond,  according  to  their  Sp.  Gr.,  to  the  upper  and  lower  layers  of  the 
system.  See  also,  last  table  p.  289. 

The  distribution  coefficient  of  ethyl  alcohol  between  benzene  and  water  at  25° 
was  found  by  Morgan  and  Benson  (1907)  to  be  1.16.  Additional  data  for  this 
system  are  also  given  by  Bubanovic,  1913  and  by  Taylor  (1897). 


ETHYL  ALCOHOL 


288 


'MISCIBILITY  OF  ETHYL  ALCOHOL  (see  Note,  p.  287)  WITH  MIXTURES  OF: 

Bromobenzene  and  Water  at  o°.  Nitrobenzene  and  Water  at  15°. 

(Bonner,  1910.)  (Bonner,  1910.) 

Composition  of  Homogeneous  Mixtures.  Composition  of  Homogeneous  Mixtures. 


Cms.              Cms.           Cms.         Sp.  Gr. 

Gms.           Gms.           Gms.           Sp.  Gr. 

QH5Br.            H2O.         C2H5OH.     Sat.  Sol. 

C6H8NO2.        H2O.        C2H5OH.       Sat.  Sol. 

0.99       o.oio    0.115     I-34 

0.965      0.035      0.248         I.  08 

*o.96       0.040    0.32 

*o.9i       0.09      0.49         ... 

0.90       o.io      0.65       1.07 

0.90      o.io      0.53         i.  02 

0.80          0.20         I                 0.96 

0.80      0.20      0.86        0.97 

0.70          0.30         I.I9         0.96 

0.70         0.30         1.09            0.94 

o  .  60       o  .  40      i  .  30      o  .  98 

0.594      0.406       1.238         0.93 

0.50      0.50      1.39     0.95 

0.50         0.50         I.3I            0.92 

0.40       0.60      1.43      0.91 

0.40      0.60       1.34         0.92 

0.30      0.70     1.43     0.92 

0.30      0.70       1.30        0.91 

O.2O          O.8O         1.36         0.93 

0.194      0.8o6       I.  212         0.92 

o.io       0.90      1.16      0.93 

o.io      0.90      0.98        0.93 

0.024     0.976    0.803     °-92 

0.02      0.98      0.601      0.95 

MISCIBILITY  OF  ETHYL  ALCOHOL  (see 

Note,  p.  287)  AT  o°  WITH  MIXTURES  OF: 

Benzyl  Acetate  and  Water.  (Bonner,  1910.) 

Benzyl  Alcohol  and  Water.  (Bonner,  1910.) 

Composition  of  Homogeneous  Mixtures. 

Composition  of  Homogeneous  Mixtures. 

Cms.  CH3.-        Cms.           Cms.         Sp.  Gr. 

Gms.            Gms.            '  Gms.           Sp.  Gr. 

CO2.CH2.QH5.     H2O.        C2H5OH.     Sat.  Sol. 

C6H5CH2OH.     H2O.        Q,H5OH.        Sat.  Sol. 

0.977        0.023      0.120      1.05 

0.90      o.io      0.13         1.03 

0.901    0.099  o-a1?   i-°3 

0.80         0.20         0.26            I 

O.8O          O.2OO      0.46         0.99 

0.70         0.30         0.35            0.98 

0.70          0.300      0.58         0.97 

0.60         0.40         0.39            0.98 

*o.68       0.32      0.60 

0.50         0.50         0.40            0.97 

0.60        0.40       0.69       0.95 

0.40         O.6O         0.41            0.97 

0.50        0.50       0.78       0.94 

*o.38      0.62      0.42 

0.40       0.60       0.85       0.94 

0.379    0.621     0.417      0.98 

0.30       0.70      0.88      0.93 

0.30      0.70      0.41        0.97 

0.20       0.80      0.88      0.93 

0.194    0.806    0.388      0.97 

o.io       0.90      0.80      0.94 

o.io      0.90      0.35        0.98 

0.041     0.959    0.665     °-95 

0.04      0.96      0.139      0.99 

MISCIBILITY  OF  ETHYL  ALCOHOL  (see 

Note,  p.  287)  AT  o°  WITH  MIXTURES  OF: 

Benzylethyl  Ether  and  Water. 

(Bonner,  1910.) 

Carbon  Tetrachloride  and  Water. 

(Bonner,  1910.) 

Composition  of  Homogeneous  Mixtures. 

Composition  of  Homogeneous  Mixtures. 

Cms.           Cms.           Cms.        Sp.  Gr. 

Gms.            Gms.            Gms.           Sp.  Gr. 

CeHsCHj.O.QHs.  H2O.        CjHjOH.    Sat.  Sol. 

CCU.            H2O.         C2H5OH.       Sat.  Sol. 

0.971      0.029    0.189    °-94 

0.961       0.039      0.224         1.36 

0.90       o.io      0.37       0.92 

0.928      0.072      0.347          1.23 

0.80          0.20         0.54         0.92 

*o«92      0.08      0.39 

0.70          0.30         0.67         0.91 

0.90      o.io      0.45         i.  20 

*o.67       0.33       0.71 

O.8O         O.2O         0.67             I  .15 

0.60        0.40       0.78       0.91 

0.70         0.30         0.82             1.07 

0.50       0.50      0.87      0.91 

o  .  60      o  .  40      o  .  94         i  .  03 

0.40       0.60      0.93      0.92 

0.499    °-5O1     1.04         i 

0.30       0.70       0.96       0.92 

0.40      0.60      i              °-97 

0.198     0.802    0.952  ,0.92 

0.25      0.75       1.105      °-9S 

o.io       0.90      0.86       0.93 

o.io      0.90      i              0.92 

0.08       0.92       0.793     °-94 

0.032     0.968    0.745      0.93 

289  ETHYL  ALCOHOL 

DISTRIBUTION  OF  ETHYL  ALCOHOL  AT  25°  (Bugarszky,  1910)  BETWEEN: 

Bromobenzene  and  Carbon  Tetrachloride  and        Carbon  Disulfide  and 

Water.  Water.  Water. 

Cms.  C2H5OH  per  Liter.  Cms.  C2H5QH  per  Liter.  Cms.  QHsOH  per  Liter. 

C6H5Br  Layer*     H2O  Layer'.  'CO,  Layer.      H2O  Layer."  'CSj  Layer.        H2O  Layer. 

0.72  18.5  0.45  18.7  0.27  IQ.I 

1-36  36-9  o-93          36-5  1-87          37- 

2.68  68.2  2.55          68.1  10.23          69.3 

MISCIBILITY  OF  ETHYL  ALCOHOL  (see  Note  p.  287)  AT  o°  WITH  MIXTURES  OF: 
Chloroform  and  Water.  (Bonner,  1910.)  Diethylketone  and  Water.  (Bonner,  1910.) 

Composition  of  Homogeneous  Mixtures.  Composition  of  Homogeneous  Mixtures. 


Cms. 

Cms. 

Cms. 

Sp, 

Gr. 

Cms. 

Cms. 

Cms. 

Sp.  Gr. 

CHC13. 

H20. 

C2H6OH. 

Sat 

.Sol. 

i- 

H20. 

Sat.  Sol. 

0.907 

O 

•093 

0.434 

I. 

19 

0. 

938  ' 

0 

.062 

0.136 

0.85 

0.90 

0 

.10 

0-45 

I  . 

18 

0. 

900 

O 

.10 

O.I9 

0.85 

0.80 

O 

.20 

0.60 

I. 

12 

O. 

895 

O 

•  105 

0.201 

0.86 

0.70 

0 

•3° 

0.68 

I  . 

07 

0. 

800 

0 

.20 

0.31 

0.87 

0-593 

0 

•407 

0.726 

I. 

04 

0. 

781 

O 

.219 

0.317 

0.87 

0.501 

O 

•499 

0.729 

I  . 

03 

0. 

702 

0 

.298 

0.356 

0.88 

"0.420 

0 

•58 

0.73 

.  . 

. 

0. 

600 

0 

.400 

0.392 

0.89 

0.404 

O 

•596 

0-733 

I  . 

01 

O. 

547 

O 

•453 

O.4IO 

0.90 

0.300 

O 

.70 

0.70 

O. 

99 

0. 

499 

0 

.501 

0.4II 

0.91 

0.197 

0 

.803 

0.672 

0. 

98 

O. 

458 

O 

•542 

0.415 

0.92 

O.IOO 

O 

.90 

0.61 

O. 

98 

0. 

407 

0 

•593 

0.404 

0.91 

0.088 

0 

.912 

0.608 

0. 

98 

Additional  data  for  the  miscibility  of  alcohol  with  chloroform  +  water  mixtures 
are  given  by  Miller  and  McPherson,  1908. 

MISCIBILITY  OF  ETHYL  ALCOHOL  WITH  MIXTURES  ^OF  ETHYL  ETHER  AND 

WATER  AT  O°.     (Corliss,  1914;  Bonner,  1910;  see  also  Kremann,  igioa.) 
Composition  of  the  Lower  Layer.  Composition  of  Upper  Layer. 


Cms. 
(C2H5)20. 
0.10 

Cms. 
H20. 

0.90 

Cms. 
C2HBOH. 

0.163 

Sp.  Gr. 
Sat.  Sol. 

0.970 

Cms. 
(C2H6)20. 

Cms. 
H20. 

Cms. 

Sp.  Gr. 
Sat.  Sol. 

0.957 

0 

•043 

O.I5I 

0-757 

0.16 

0.84 

O, 

297 

O 

•951 

O 

.902 

0 

.098 

0.230 

0.778 

0.178 

0.822 

O, 

.318 

O 

•945 

O 

•87 

O 

•  13 

0.26 

0.788 

0.192 

0.8o8 

0, 

332 

0 

.941 

0 

.85 

O 

•  15 

0.275 

0.794 

0.204 

0.796 

O 

•34 

O 

•937 

O 

.825 

0 

•  175 

0.292 

0.800 

0.227 

0-773 

O, 

352 

0 

•932 

O 

•79 

O 

.210 

0.313 

0.808 

0.250 

o-75 

0, 

36 

0 

.926 

0 

•759 

O 

•243 

0.33 

0.815 

0.293 

0.707 

O, 

37 

O 

.916 

0 

•70 

0 

•30 

0-35 

0.827 

0-335 

0.665 

0, 

375 

0 

.906 

O 

•645 

O 

•355 

0.366 

0.839 

0.422 

0.578 

O, 

385 

O 

.886 

0 

•562 

O 

•438 

0.385 

0.857 

"0.49 

0.51 

0 

•385 

O 

.874 

0 

•49 

0 

•51 

0.385 

0.874 

The  data  for  the  binodal  curve  given  by  Corliss  and  by  Bonner  agree  closely. 
The  Sp.  Gr.  determinations  of  Corliss  were  made  on  larger  amounts  of  solution 
and  appear  to  be  the  more  accurate.  In  addition,  Corliss  gives  the  specific  gravi- 
ties of  each  layer  of  a  series  of  liquids  in  contact  with  each  other,  and  from  these 
and  the  binodal  curve,  the  above  data  for  the  composition  of  the  several  con  jugate 
layers  have  been  calculated.  Data  are  also  given  by  Corliss  for  the  distribution 
of  colloidal  arsenious  sulfide  between  the  two  layers  of  the  system. 

Data  for  the  distribution  of  ethyl  alcohol  between  ether  and  water  and  between 
ether  and  molten  CaCl2.6H2O  are  given  by  Morgan  and  Benson  (1907). 


ETHYL  ALCOHOL 


290 


MISCIBILITY  OF  ETHYL  ALCOHOL  WITH  MIXTURES  OF  ETHYL  ETHER  AND 
WATER  AT  25°.    (Horiba,  1911-12.) 

Composition  of  Lower  Layer.  Composition  of  Upper  Layer. 


Gms. 

Gms. 

(QH5)20. 

H20. 

Gms.  QH5OH. 

5-77 

94-23 

0 

6-3 

85-7 

8 

7.2 

79-2 

13-6 

8 

76 

16 

9-7 

70.4 

19.9 

13-3 

62.8 

23-9 

22.1 

50.6 

27-3 

28.4 

43-4 

28.2 

*3i-6 

40 

28.4  (Plait  point; 

Gms. 

Gms. 

Gms. 

H20. 

QH5O2H. 

98/72' 

1.28 

0 

94-5 

2.2 

3-3 

88.5 

3-7 

7-8 

84-4 

4-9 

10.7 

75.1 

8.4 

I6.5 

60.8 

iS-5 

23-7 

43-8 

28.1 

28.1 

35-8 

35-6 

28.6 

31-6 

40 

28.4 

The  binodal  curve  was  determined  in  the  usual  way  (see  Note,  p.  287).  A  series 
of  conjugate  liquids  was  then  prepared  and  the  Sp.  Gr.,  refractive  index  and 
viscosity  of  each  layer  determined.  From  specially  prepared  curves  for  variations 
of  physical  constants  with  composition  of  mixture,  the  composition  of  the  several 
conjugate  liquids  was  ascertained.  The  results  thus  obtained,  are  given  in  the 
above  table. 

Data  for  the  miscibility  of  ethyl  alcohol  with  mixtures  of  water,  ethyl  ether  and 
sulfuric  acid  at  o°  and  with  mixtures  of  ethyl  ether,  water  and  ethylsulfuric 
acid  at  o°  are  given  by  Kremann,  19103. 

MISCIBILITY  OF  ETHYL  ALCOHOL  (see  Note  p.  287)  AT  o°  WITH  MIXTURES  OF: 
Ethyl  Acetate  and  Water.  (Bonner,  1910.)         Ethyl  Bromide  and  Water.  (Bonner,  1910.) 

Composition  of  Homogeneous  Mixtures. 


Composition  of  Homogeneous  Mixtures. 

Gms. 

Grns. 

Gms. 

Sp.  Gr. 

CHjCOOQHs. 

H20. 

C2H5OH. 

Sat.  Sol. 

0.92 

0.080 

0.100 

0.91 

0.90 

O.IO 

0.13 

0.91 

0.799 

O.2OI 

0.228 

o-93 

0.699 

O.3OI 

0.265 

0.92 

0.60 

0.40 

0.29 

o-95 

0.50 

0.50 

0.30 

o-95 

*o.48 

0.52 

0.30 

0.40 

O.6O 

0.31 

0.96 

0.30 

O.7O 

0.31 

0.96 

0.197 

0.803 

0.282 

o-97 

0.102 

0.898 

0.143 

o-99 

Gms. 

Gms. 

Gms. 

Sp.  Gr. 

C2HBBr. 

H20. 

C2H5OH. 

Sat.  Sol. 

0.967 

0.033 

O.24O 

1.23 

0.90 

O.IO 

0-37 

I-I5 

*o.83 

0.17 

0.45 

0.80 

O.2O 

0-51 

1.09 

0.70 

0.30 

0.64 

1.  06 

0.60 

0.40 

0-754 

1.03 

0.50 

0.50 

0.83 

I 

0.40 

O.6O 

0.89 

o-99 

0.30 

0.70 

0.89 

o-97 

O.IO 

0.90 

o-73 

0-97 

0.017 

0.983 

0.182 

o-99 

MISCIBILITY  OF  ETHYL  ALCOHOL  (see  Note  p.  287)  AT  o°,  WITH  MIXTURES  OF: 
Ethyl  Buty rate  and  Water.  (Bonner,  1910.)    Ethyl  Propionate  and  Water.  (Bonner,  1910.) 


Composition  of  Homogeneous  Mixtures. 


Composition  of  Homogeneous  Mixtures. 


Gms. 


0.97 
0.90 
0.80 
0.70 
0.599 
0.494 
*o.46 
0.40 
0.297 
0.193 
O.JO 


Gms. 
H20. 

0.030 

o.io 

0.20 

0.30 

0.401 

0.506 

0.54 

0.60 

0.703 

0.807 

0.90 


Gms.    '      Sp.Gr. 
C2H5OH.     Sat.  Sol. 

0.166    0.96 

0.32 

0.483 

0.567 

0.628 

0.659 

0.67 

0.69 

0.693 


0.88 
0.89 
0.90 
0.91 


Gms.  Gms. 

CjHjCOOQNj.    H2O. 
0.977      0.023 

0.90      o.io 

0.80 

0.695 
0.60 


Gms. 


0-684 
0.63 


0.92 
o-93 
o-94 
0.94 


0.50 
*o.46 
0.398 
0.30 
0.201 
o.io 


0.20 

°-3°5 

0.40 

0.50 

0.54 

0.602 

0.70 

0.799 

0.90 


0.138 

0.27 

0.38 

°-453 

0.49 

0.52 

0.53 

0.532 

0.55 

°-5I7 
0.46 


Sp.  Gr. 
Sat.  Sol. 

0.90 

0.90 

0.90 

o-92 
0.91 
0.92 

0.93 
0.94 

°-95 
0.96 


291 


ETHYL  ALCOHOL 


MISCIBILITY  OF  ETHYL  ALCOHOL  (see  Note,  p.  287)  AT  o°  WITH  MIXTURES  OF  ; 


Ethylene  Chloride  and  Water. 

(Bonner,  1910.) 
Composition  of  Homogeneous  Mixtures. 

Cms.             Cms.            Cms.  Sp.  Gr. 

CH2C1.CH2C1.      H2O.         CjH.,OH.  Sat.  Sol. 

O.pyi   0.029   0.191  I.I5 

0.90   o.io   0.42  i.  08 

*O . 88     O  .  1 2    0 . 46  ... 

0.792     0.208    0.670  i. oi 

O.7O          0.30         O.8O  0.98 

O.6O          0.40         0.93  0.96 

0.50          0.50         0.99  0.95 

0.40       0.60      i.oi  0.94 

0.30       0.70      0.99  0.94 

O.2O           O.8O         0.95  0.94 

O.O95        0.905       0.842  0.96 

0.02           0.980      0.514  0-97 


Ethylidene  Chloride  and  Water. 

(Bonner,  1910.) 
Composition  of  Homogeneous  Mixtures. 

Cms.            Cms.            Cms.  Sp.  Gr. 

CH3.CHCI2.      H20.        QHjOH.  Sat.  Sol. 

0.985  0.015  0.226  i. 10 

0.90   o.io   0.43  1.03 

0.805  °-I95  0.586  i.oi 

O.yO         0.30         0.69  0.98 

*o.67      0.33      0.72 

0.60      0.40      0.77  0.96 

0.50      0.50      0.82  0.95 

0.437    0-563    o-857  0.94 

0.30      0.70      0.88  0.93 

0.20      0.80      0.86  0.93 

o.io      0.90      0.79  0.94 

0.03      0.97      0.576  0.95 


MISCIBILITY  OF  ETHYL  ALCOHOL  (see  Note,  p.  287)  AT  o°  WITH  MIXTURES  OF: 


Heptane  and  Water.    (Bonner,  1910.) 

Composition  of  Homogeneous  Mixtures. 


Cms. 
Heptane.* 


Gms.  Gms.  Sp.  Gr."| 

H20.  C,H5OH.  Sat.  Sol. 

0.962        0.038  0.704  0.79 

0.90       o.io  1.44  0.80 

0.798        0.202  2.375  0.82 

0.70       0.30  2.82  0.81 

0.60          0.40  3.06  0.82 

0.50          0.50  3.16  0.83 

o .  40   o .  60  3 . 1 7  o .  84 

0.30   0.70  3.10  0.85 

0.196   0.804  2.96  0.87 

0.093  0.907  2.305  0.88 


Hexane  and  Water.    (Bonner,  1910.) 

Composition  of  Homogeneous  Mixtures. 


Gms. 
Hexane. 


Sp.  Gr. 
Sat.  Sol. 


Gms.  Gms. 

H2O.  C2H8OH. 

0.97         0.03  0.59 

0.90      o.io  1.30  0.77 

0.80         0.20  2.04  0.79 

0.70      0.30  2.45  0.81 

0.60      0.40  2.73  0.82 

0.50     0.50  2.93  0.83 

o . 40      o . 60  3 . oo  o . 83 

0.20         0.80  2.75  0.85 

o.io      0.90  2.23  0.86 

0.014    0.986  1.056 


Kahlbaum's  Heptane  and  Hexane  "aus  Petroleum  "  were  used. 


MISCIBILITY  OF  ETHYL  ALCOHOL  (see  Note,  p.  287)  AT  o°  WITH  MIXTURES  OF: 


Isoamyl  Alcohol  and  Water. 

(Bonner,  1910.)  , 

Composition  of  Homogeneous  Mixtures. 

Gms.  (CH3)2-      Gms.  Gms.  Sp.  Gr. 

CH(CH2)2OH.     H20.         C2H5OH.  Sat.  Sol. 

0.903      0.097     0.116  0.84 

0.90          O.IO         O.I2  0.84 

0.797        O.2O3       0.258  0.85 

0.694     0.306    0.396  0.86 

0.602     0.398    0.427  0.88 

0.497     °-5°3     °-449  0.89 

0.399     0.601     0.453  0.90 

0.294     0.706    0.434  0.92 
*o.27        0.73       0.43 

0.196     0.804    0.411  0.94 

o.io       0.900    0.369  0.96 


Isobutyl  Alcohol  and  Water. 

(Bonner,  1910.) 
Composition  of  Homogeneous  Mixtures. 


Gms.  (CH,),-     Gms. 
CH.CH2OH.     H20. 


Gms. 


Sp.  Gr. 
Sat.  Sol. 


0.70  0.30  0.13  0.87 

0.589  0.4II  0.177  0.89 

0.502  0.498  0.194  0.90 

0.50  0.50  0.20  0.90 

0.40  O.6O  O.2O  0.92 

0.387  0.613  0.204  0.92 

*o.35  0.65  0.21 

0.304  0.696  0.205  0.94 

0.30  0.70  O.2I  0.94 

O.2O  O.8O  O.2O  °-95 

0.132  0.868  0.189  0.96 


ETHYL  ALCOHOL 


292 


MISCIBILITY  OF  ETHYL  ALCOHOL  (see  Note,  p.  287)  AT  o°  WITH  MIXTURES  OF: 


Isoamyl  Bromide  and  Water.  (Bonner,  '10.) 
Composition  of  Homogeneous  Mixtures. 


Iso butyl  Bromide  and  Water.  (Bonner,  '10.) 

Composition  of  Homogeneous  Mixtures. 


Gms.             Cms.            Cms.         Sp.  Gr. 

Gms.  (CH3)r      Gms.           Gms.            Sp.  Gr. 

CsHuBr.          H2O.         QH6OH.     Sat.  Sol. 

CHCH2Br.        H2O.        CjH6OH.        Sat.  Sol. 

0.975     0.025    0-251     i-io 

0.976    0.024    0.200      1.18 

*o  .  96       o  .  04      0.36 

*o.93      0.07      0.42 

0.90       o.io      0.68       i.oi 

0.90      o.io      0.52         1.09 

0.80          0.20         1.09         0.96 

0.80         0.20         0.83            I.OI 

0.70          0.30         1.37         0.94 

0.70         0.30             .05            0.98 

0.60       0.40      1.57      0.93 

O.6O         0.40             .21            0.96 

0.498     0.502       .676    0.91 

0.501     0.499       -3°        °-94 

0.40       0.60         .75      0.91 

0.40     0.60       .35      0.93 

0.30       0.70         .75      0.91 

0.30     0.70       .36      0.93 

O.2O           O.8O             .71          0.91 

O.2O         O.8O             .32            0.92 

o.io       0.90         .46      0.92 

o.io      0.90         .20        0.93 

0.022        0.978          .027      0.93 

0.047   0.953   0.937     0.94 

MISCIBILITY  OF  ETHYL  ALCOHOL  (see 

Note,  p.  287)  AT-O°  WITH  MIXTURES  OF: 

Isoamyl  Ether  and  Water.    (Bonner,  '10.) 

Mesitylene  and  Water.    (Bonner,  '10.) 

Composition  of  Homogeneous  Mixtures. 

Composition  of  Homogeneous  Mixtures. 

Gms.  f(CH3)2.-    Gms.           Gms.         Sp.  Gr. 

Gms.            Gms.          Gms.           Sp.  Gr. 

CH.CH2CHd2O.   H20.        C2H5OH.     Sat.  Sol. 

C6H3(CHa)3.       HjO.        CjHjOH.       Sat.  Sol. 

0.958     0.042    0.368    0.81 

*o.97      0.03      0.48 

0.90       o.io      0.70      0.82 

0.963     0.037     o-S1^      0.86 

*o  .  89       o  .  1  1      o  .  74         ... 

0.90      o.io      1.09        0.85 

0.879       O.I2I      0.793      0-82 

o  .  80      o  .  20      i  .  66        o  .  84 

0.80          0.20         1.20         0.83 

0.70      0.30      2.04        0.85 

0.702        0.298       1.573      0.83 

0.60      0.40      2.32        0.85 

0.594       0.406       1.876      0.84 

0.50      0.50      2.52        0.85 

0.50          0.50         1.98         0.84 

0.40      0.60      2.64        0.86 

0.40          0.60         2.19         0.85 

0.30      0.70      2.68        0.87 

0.302     0.698     2.24      0.86 

0.199    0.801     2.49        0.87 

0.20       0.80      2.14      0.87 

o.io      0.90      2.28        0.89 

o.io       0.90      1.87      0.89 

0.051     0.949     1.615      0.90 

MISCIBILITY  OF  ETHYL  ALCOHOL  (see 

Note,  p.  287)  AT  o°  WITH  MIXTURES  OF: 

Methyl  Aniline  and  Water.  (Bonner,  '10.) 

Phenetol  and  Water.    (Bonner,  '10.) 

1  '  Composition  of  Homogeneous  Mixtures. 

Composition  of  Homogeneous  Mixtures. 

Gms.            Gms.            Gms.        Sp.  Gr. 

Gms.            Gms.            Gms.           Sp.  Gr. 

CHjNHQHj.      H20.        QHsOH.    Sat.  Sol. 

QHsOCzHs.       H2O.         C2H5OH.       Sat.  Sol. 

0.959     0.041     0.218    0.96 

0.992     0.18      0.157      0.96 

0.90       o.io      0.37      0.95 

*o.9o      o.io      0.55         ... 

0.795        0-205      0.555      0.93 

0.897      0.103      0.554         0.93 

0.70       0.30      0.68       0.93 

0.798      0.202       0.916         0.90 

*o.66       0.34      0.72 

0.70         0.30             .l8            0.90 

0.60       0.40      0.76      0.93 

O.6O         O.4O             .39            0.89 

0.50       0.50      0.84      0.93 

0.495    °-5°5       •51^      0-89 

0.40       0.60      0.89      0.93 

0.399    0.601       .560      0.89 

0.30       0.70      0.91       0.93 

0.30      0.70         .54        0.90 

0.20       0.80      0.87       0.94 

0.198    0.802       .449      0.91 

0.098     0.902     0.734     0.95 

O.IO         0.90             .21             0.92 

0.041      0.959    0-581     0.96 

0.082    0.918       .156      0.93 

293 


ETHYL  ALCOHOL 


MISCIBILITY  OF  ETHYL  ALCOHOL  (see 
Pinene  and  Water.     (Bonner,  1910.) 

Composition  of  Homogeneous  Mixtures. 


Note  p.  287)  AT  o°  WITH  MIXTURES  OF: 

Propyl  Bromide  and  Water.     (Bonner,  1910.) 
Composition  of  Homogeneous  Mixtures. 


Cms.              Cms.            Cms.         Sp.  Gr.  ' 

Gms.              Gms.          Gms.           Sp.  Gr. 

C,0H,,.             H20.        QH6OH.     Sat.  Sol. 

CH3.CH2.CH2Br.     H2O.        QH6OH.       Sat.  SoL 

0.99       o.oio    0.268    0.87 

0.975         0.025      0.190         1.26 

*o.985     0.015     0.47 

*o.92         0.08      0.42 

0.897     0.103     1.595     0.85 

0.90           O.IO        0.50           1.  12 

0.795     0.205     2.268    0.84 

O.8O           O.2O         0.72            I.  06 

0.70       0.30      2.67      0.84 

0.70        0.30      0.88        1.02 

0.60       0.40      2.94      0.85 

0.60        0.40      i.oi        0.99 

0.493     °-5°7     3-!35    0-85 

0.50        0.50       i.io        0.98 

0.393     0.607     3.126    0.86 

0.40        0.60      1.15        0.96 

0.293     0.707     3.038    0.86 

0.30       0.70      1.14       0.95 

0.194     0.806     2.799    0-87 

O.2O4         0.796       I.  12            0.94 

0.094     0.906     2.331     0.89 

0.096         0.904       1.02            0.94 

0.035     0.965     1.639    0-91 

0.027         0.973      0.687         0.95 

MISCIBILITY  OF  ETHYL  ALCOHOL  (see 

Note  p.  287)  AT  b°  WITH  MIXTURES  OF: 

Toluene  and  Water.     (Bonner,  1910.) 

o  Toluidine  and  Water.     (Bonner,  1910.) 

Composition  of  Homogeneous  Mixtures. 

Composition  of  Homogeneous  Mixtures. 

Gms.             Gms.           Gms.         Sp.  Gr. 

Gms.               Gms.           Gms.           Sp.  Gr. 

C6H5CH3.        H20.         QHsOH.    Sat.  Sol. 

CH3.C6H4.NH2.      H2O.         QHsOH.       Sat.  Sol. 

0.948        0.052      0.388      0.87 

0.954         0.046      0.025         I-°I 

0.90       o.io      0.61      0.86 

0.90           O.IO         O.2I            0.93 

0.80       0.20      0.95      0.86 

0.80            0.20         0.32            0.97 

0.70       0.30         .21       0.86 

0.70           0.30         0.41            0.96 

0.60       0.40         .41      0.86 

0.60           O.40         0.455         O-Q^ 

0.50       0.50         .53      0.87 

0.50            0.50         0.48            0.96 

0.40       0.60         .59      0.87 

0.40            O.OO         0.50           0.96 

0.30       0.70         .56      0.88 

0.30            0.70         0.50           0.96 

0.20       0.80         .44      0.89 

0.20            0.80         0.49            0.96 

o.io       0.90         .23      0.91 

0.098         O.9O2      0.462         0.98 

0.028     0.972    0.817    0.94 

0.027      0-973     0.262 

MISCIBILITY  OF  ETHYL  ALCOHOL  (see 

Note  p.  287)  AT  o°  WITH  MIXTURES  OF: 

Bromotoluene  (b.  pt.  182-3)  and  Water. 

p  Nitrotoluene  and  Water. 

(Bonner,  1910.) 

(Bonner,  1910.) 

Composition  of  Homogeneous  Mixtures. 

Composition  of  Homogeneous  Mixtures. 

Gms.              Gms.            Gms.         Sp.  Gr. 

Gms.             Gms.           Gms.           Sp.  Gr, 

BrC6H4.CH3.       H2O.         CjHsOH.     Sat.  Sol. 

NO2.C6H4.CH3.     H2O.         QH6OH.       Sat.  Sof. 

o  .  98       o  .  02      o  .  33 

0.978         0.022      0.253          I.  08 

0.951        0.049      O.522       I.OQ 

*o«95        0.05      0.50 

0.90       o.io      0.87       i.  06 

0.90        o.io      0.84        0.97 

0.80          0.20             .28         0.97 

O.8O           O.2O         1.29            0.96 

O.yO          0.30             .54         0.94 

0.70            0.30         1.57            0.92 

O.6O          O.40             .71         0.93 

0.00           0.40         1.73            0.91 

O.5O          O.50             .8l         0.92 

0.506         0.494       1.782         0.91 

O.4O          O.6O             .89         0.91 

0.398      0.602     1.868      0.91 

O.30          O.70             .89         0.90 

0.294      0.706     1.816      0.91 

O.20         0.80            .78         0.90 

0.20        0.80      1.63        0.91 

o.io      0.90        .533    0.91 

o.io        0.90      1.30        0.92 

0.033       0.967      1.307      O.Q2 

0.056      0.944     1.105      0.93 

ETHYL  ALCOHOL 


294 


MISCIBILITY  OF  ETHYL  ALCOHOL  (see  Note  p.  287)  AT  o°  WITH  MIXTURES  OF: 


o  Xylene  and  Water.     (Bonnet,  1910.) 

Composition  of  Homogeneous  Mixtures. 


m  Xylene  and  Water.     (Bonner,  1910.) 
Composition  of  Homogeneous  Mixtures. 


' 

Gms. 

Gms. 

Gms. 

Sp.  Gr. 

Gms. 

Gms.           Gms. 

Sp.  Gr. 

o  C,H4(CH3),. 

H20. 

QH6OH. 

Sat.  Sol. 

Hn  C^g-tl^v^ji^g.          H^O.             C^HsOH. 

Sat.  Sol. 

0.971 

0.029 

0-352 

0.89 

0. 

967 

0. 

033    0.388 

0.88 

4 

0.04 

o-53 

.  .  . 

0. 

90 

O. 

10      0.81 

0.87 

0.90 

O.IO 

0-93 

0.87 

o. 

80 

O. 

20 

-30 

0.85 

0.786 

0.214 

•32 

0.87 

0. 

70 

0. 

30 

.61 

0.86 

0.70 

0.30 

•53 

0.87 

0. 

60 

O. 

40 

•77 

0.86 

O.6O 

0.40 

.72 

0.87 

0. 

50 

0. 

50 

.90 

0.87 

0.50 

0.50 

.87 

0.87 

0. 

40 

0. 

60 

.98 

0.87 

0.40 

0.60 

.96 

0.88 

o. 

30 

o. 

70 

.01 

0.88 

0.30 

0.70 

•94 

0.88 

0. 

20 

0. 

86 

•87 

0.89 

O.2O 

0.80 

.81 

0.89 

0. 

10 

0. 

9° 

•53 

0.90 

O.O3I 

0.969 

.19 

0.03 

o. 

023 

o. 

977 

.168 

O.O2 

Additional  data 

for  the  system  ethyl  alcohol, 

m  xylene, 

water  at  o°, 

19°,  41°, 

63 

0  and  1  00°  are  given  by  Holt  and 

Bell,  1914. 

p  XYLENE  AND  WATER.    (Bonner,  1910.) 


Composition  of  Homogeneous  Mixtures. 


Composition  of  Homogeneous  Mixtures. 


Gms. 

Gms. 

Gms. 

Sp.  Gr. 

Gms. 

Gms. 

Gms. 

Sp.  Gr. 

P  C6H4(CHa)2.       H20. 

C2H5OH. 

Sat 

.Sol. 

*C6H4(CH3)2.      H20. 

QH5OH. 

Sat.  Sol. 

0.966 

0.034 

O. 

.306 

O, 

84 

0 

•5° 

O 

•50 

1.68 

0.86 

*0.92 

0.08 

0. 

57 

0 

.40 

O 

.60 

1.77 

0.86 

0.90 

O.IO 

0, 

65 

0, 

•8S 

0 

.292 

0 

.702 

1-743 

0.87 

0.80 

0.20 

I, 

°5 

o 

•8S 

O 

•  193 

o 

.807 

1.625 

0.88 

0.70 

0.30 

I, 

•35 

o 

.85 

0 

.100 

o 

.90 

i-39 

0.89 

0.60 

T*t-  - 

0.40 

ft*.      .                        . 

J  ( 

A 

0 

•85 

0 

1          t  1 

.015 

_       _    1            1  A 

0 

•985 

0.863 

0-93 

The  coefficient  of  distribution  of  ethyl  alcohol  between  olive  oil  and  water  is 
O.026  at  3°  and  0.047  at  30°.  (Meyer,  1901;  1909.) 

100  gms.  cottonseed  oil  (0.922  Sp.  Gr.)  dissolve  22.9  gms.  ethyl  alcohol  at  25°. 
100  gms.  ethyl  alcohol  dissolve  11.75  gms.  cottonseed  oil  at  2 5°.    (Wroth  and  Reid, '16.) 

DISTRIBUTION  OF  ETHYL  ALCOHOL  BETWEEN  COTTONSEED  OIL  AND 

WATER  AT  25°.     (Wroth  and  Reid,  1916.) 
Gms.  C2H5OH  per  100  cc. 


Oil  Layer. 

H20  Layer." 

JXCLLiU* 

o  .  2083 

6.147 

29-5 

0.2251 

6.738 

29.9 

0.25I5 

6-835 

27.1 

0.2783 

6.876 

24.7 

°/3°1I7.,. 

8.682 

f          ,   1           1           t            1 

28.7 

Data  for  the  reciprocal  solubility  of  ethyl  alcohol  and  turpentine  are  given  by 
Vezes  and  Mouline,  1904,  1905-06. 

Data  for  the  system  ethyl  alcohol,  water,  petroleum  are  given  by  Rodt  (1916). 

ETHYLAMINES   C2H5.NH2,  (C2H6)2NH,  (C2H6)3N. 

Freezing-point  data  (solubility,  see  footnote,  p.  i)  for  mixtures  of  ethylamine  + 
water,  diethylamine  +  water,  and  triethylamine  +  water  are  given  by  Guthrie, 
1884  and  by  Pickering,  1893. 

The  solubility  of  ethylamine  and  of  diethylamine  in  water  at  60°,  calculated 
from  the  vapor  pressures  determined  by  an  aspiration  method,  are  given  by  Doyer, 
(1890)  as  follows: 

A     •  Vapor  Pressure  in      Ostwald  Solubility      Bunsen  Absorption 

mm.  Hg.  Ex.  /  (see  p.  227.)        Coef.  (see  p.  227.) 

C2H5NH2  64.5  321  263 

(C2H6)2NH  233  89  73 

Data  for  the  solubility  of  triethylamine  in  water  at  high  pressures  are  given  by 
Kohnstamm  and  Timmermans,  1913. 


295 


ETHYL  AMINES 


SOLUBILITIES  OF  Di  ETHYL 
AMINE  AND  WATER.* 

(Lattey  —  Phil.  Mag.  [6]  10,  398,  '05.) 


Gms.  NH(C2H5)2 
per  100  Gms. 

0 

Aqueous 

Amine 

' 

Layer. 

Layer. 

155 

21.7 

59-O 

150 

23-6 

55-5 

148 

24.8 

53-5 

146 

26.3 

51.0 

145 

28.0 

49.0 

144 

31.0 

45  -° 

DISTRIBUTION  OF  TRI  ETHYL  AMINE 
BETWEEN  WATER  AND  AMYL 
ALCOHOL  AT  25°. 

(Herz  and  Fischer  —  Ber.  37,  4751,  '04.) 

Cms.  N(C2H5)3  •  Millimols  N(C2H6)» 

per  100  cc.  per  10  cc. 


Aqueous 
Layer. 

Alcoholic 
Layer. 

Aqueous 
Layer. 

Alcoholic 
Layer. 

0.0885 
0.1683 
0.1866 
0.2502 

2.299 

4-457 
4.922 
6.491 

0-0875 
0.1664 
0.1846 
0.2474 

2.273 
4-408 
4.868 
6.418 

143.5  (crit-  *•)    37-4 


TriethylAMINE   N(C2H5)3. 


t°. 

1 8. 6  (crit.  temp.) 

20 

25 

30 

35 


SOLUBILITY  IN  WATER.* 

(Rothmund,  1898.) 
Gms.  NCCjH^s  per  100  Gms.  f0 


Gms.  N(C2H5)3  per  100  Gms. 


Aq.  Layer. 

Amine  Layer. 

Aq.  Layer. 

Amine  Layer 

>•) 

51-9 

40 

3^5 

96.48 

14.24 

72 

50 

2.87 

96.4 

7-3° 

95.l8 

55 

2-57 

96.3 

96.60 

60 

2.23 

96.3 

4.58 

96.5 

65 

1.97 

96.3 

SOLUBILITY  OF  TRIETHYLAMINE  IN  WATER  AND  IN  AQ.  ETHYL  ALCOHOL 
AT  DIFFERENT  TEMPERATURES.* 

(Meerburg,  1902.) 


Water. 


13-33%  Alcohol.         28.98%  Alcohol.         38.84%  Alcohol.          60.16%  Alcohol. 


din.  ^((^2x15)3 

(jrHl.  ^((^2X15)  3 

Gm.N(C2Hfi)3            Gm.N(C2H5j3                Gm.N(C2H5) 

t°.        per  100           t°. 

Gms.  Sol.                  < 

per  zoo 
jms.  Sol. 

t  .        per  loo 

Gms.  Sol. 

t  .        per  loo               t°.       per  loo 
Gms.  Sol.                      Gms.  Sol. 

69.2 

I 

•7 

38. 

3 

8.2 

54- 

5 

22 

.8 

73-4 

31.2       76-77     71.2 

30.8 

5 

.6 

3i- 

7 

13-9 

45 

29 

.8 

65-4 

33-3      74-75     75 

23.1 

8 

5 

28 

21.6 

33 

4 

51 

.1 

51.6 

40.6      72-73    80 

I8.7 

25 

.8 

26. 

4 

30.6 

3i 

4 

63 

•7 

42.1 

50.6 

I8.7 

37 

.2 

24. 

9 

40-5 

30 

3 

68 

•5 

40.9 

54-7 

19-5 

.8 

24. 

2 

49.8 

28, 

•5 

82 

.2 

34-2 

70.6 

20.5 

68 

.6 

24. 

I  , 

60.7 

35 

91 

.8 

33 

77-5 

20.5 

84 

24 

69.7 

34-7 

88 

20.5 

89 

•7 

23- 

5 

76.6 

40-5 

91.3 

21.2 

92 

•4 

24 

81.5 

25.8 

95 

•5 

24. 

2 

87.4 

- 

26.5 

96 

.1 

25 

92 

NOTE.  —  Results  for  triethylamine,  water  and  ethyl  ether,  and  for  triethyl- 
amine,  water  and  phenol  are  also  given  by  Meerburg. 

100  gms.  abs.  methyl  alcohol  dissolve  57.5  gms.  NH(C6H5)2  at  19.5°. 
100  gms.  abs.  ethyl  alcohol  dissolve  56  gms.  NH(C6H5)2  at  19.5°. 

(de  Bruyn,  1892.) 

*  Determinations  made  by  "Synthetic  Method,"  see  Note,  p.  16. 


Results 

at  1  8°. 

Results 

at  25°. 

Results  at 

32.35°. 

Cms.  Equiv. 
per  Liter 
Aq.  Layer. 

Partition 
Coef. 

Gms.  Equiv. 
per  Liter 
Aq.  Layer. 

Partition 
Coef. 

Gms.  Equiv. 
per  Liter 
Aq.  Layer. 

Partition 
Coef. 

0.0756 

26.09 

O.II59 

I9-I3 

0.1287 

14.76 

0.0886 

26.14 

0.0999 

19.11 

0.2479 

14.79 

o  .  0484 

2.14 

0.0483 

i-59 

0.1200 

1.093 

0.0503 

2.14 

O.O4l6 

i-59 

O.IIO4 

1.095 

0.0189 

O.I3I 

O.OIO4 

0.099 

0.0132 

0.069 

O.OI9I 

O.I3I 

O.OI3I 

0.099 

0.0133 

0.069 

ETHYLAMINES  296 

DISTRIBUTION  OF  ETHYLAMINES  BETWEEN  WATER  AND  TOLUENE. 

(Moore  and  Winmill,  1912.) 


Amine. 

(C2H5)NH2 

a 

(C2Hs)2NH 
(C2H5)3N 

Similar  data  for  triethylamine  at  25°  and  at  other,  temperatures  are  given  by 
Hantzsch  and  Sebaldt,  1899,  and  by  Hantzsch  and  Vagt,  1901. 

Data  for  ternary  systems  composed  of  triethylamine,  water  and  each  of  the 
following  compounds:  naphthalene,  cane  sugar,  KC1,  K2CO3,  K2SO4  and  KSCN, 
are  given  by  Timmermans  (1907). 

ETHYL,   DiETHYL  and  TriETHYLAMINE  HYDROCHLORIDES,  etc.  v 
SOLUBILITY  OF  EACH  IN  WATER  AND  IN  CHLOROFORM  AT  25°. 

* '  (Peddle  and  Turner,  1913.) 

Solubility  in  Water.  Solubility  in  CHC13. 

Amine  Salt.  Formula.  Gms.  Amine  Salt      Gms.  Amine  Salt 

per  loo  Gms.  H2O.  per  100  Gms.  CHC13. 

Ethylamine      Hydrochloride    C2H5.NH2.HC1  279.9  0.17 

Diethylamine  "  (C2H5)2NH.HC1  231.7  29.45 

Hydrobromide  (C2H5)2NH.HBr  311.6  46 . 65 

"  Hydroiodide      (C2H5)2NH.HI  377.2  71.56 

Triethylamine  Hydrochloride  (C2H5)3N.HC1  137  17.37 

Hydrobromide  (CjjHs^N.HBr  150.6  23 . 44 

Hydriodide       (CjjHysN.HI  370  92.2 

ETHYL   BROMIDE   C2H6Br. 

SOLUBILITY  IN  ETHER.    (Parmentier,  1892.) 

t°.  —13°.  O.  12.  22.5.  32. 

Gms.  C2HsBr  per  ioo  gms.  Ether  632        561        462        302        253 
SOLUBILITY  OF  ETHYL  BROMIDE,  ETC.,  IN  WATER. 

(Rex,  1906.) 

Grams  per  100  Grams  H2O  at: 
Dissolved  Substance.  t * N 


o  .  10  .  20°.  30°. 

Ethyl  Bromide  i .  067  o .  965  o .  914  o .  896 

Ethyl  Iodide  0.441  0.414  0.403  0.415 

Ethylene  Chloride  0.922  0.885  0.869  0.894 

Ethylidene  Chloride  0.656  0.595  °-55°  0.540 

ETHYL  BUTYRATE   C3H7COOC2H5. 

SOLUBILITY  IN  WATER  AND  IN  AQUEOUS  ETHYL  ALCOHOL  MIXTURES  AT  20°. 
100  g.  H2O  dissolve  0.5  g.  ethyl  butyrate  at  22°.  (Traube,  1884.) 

100  cc.  H2O  dissolve  0.8  cc.  ethyl  butyrate  at  20°.  (Bancroft,  1895.) 

100  cc.  ethyl  butyrate  dissolve  0.4  —  0.5  cc.  H2O  at  20°. 

Per  5  cc.  (cc.  H2O  10          6          4          2.96    2.10 

Ethyl  Alcohol j  cc.  C3H7COOC2H5       o .  34    o .  96     2 . 47    4          6 

ETHYL   CARBAMATE   (Urethan)   CO(OC2H5)NH2.     See  also  p.  741. 
SOLUBILITY  IN  SEVERAL  SOLVENTS  AT  25°.    (U.  s.  P.  vin.) 

Solvent.  Water.          Alcohol.  Ether.      Chloroform.     Glycerol. 

Gms.  CO(OC2H5)NH2       ) 
per  100  gms.  solvent     }     I00+         l66          IO°          77  33 


297 
ETHYL  ETHER   (C2H6)2O. 

RECIPROCAL  SOLUBILITY  OP  ETHER 


ETHYL  ETHER 


AND  WATER. 


(Klobbie— Z.physik.Chem.  24,  619,  '97$  Schuncke  —  Ibid.  14,334.  '94;  St. ToUoczko  —  Ibid. 20, 407, 

•96.) 


Solubility  of  Ether  in  Water, 
Lower  Layer  —  Aqueous. 

Gms.(C2H5)2O  per  100  Cms. 

Solubility  of  Water  in  Ether. 
Upper  Layer  —  Ethereal. 

Gms.  H2O  per  100  Gms. 

Water.          Solution. 

o        13-12        ii.  6 
5        11.4          10.2 
10          9.5            8.7 
15          8.2            7.6 

I 

^ther.         So 
.01            ] 
.06 
.12            ] 
.16 
,».20  ] 

lution. 
•  O 

•05 
.12   (2.6, 

•*5 

S.) 

Jii 

25          6-oS          5-7 
30          54           5-1 
*4o          4-7            4-5 
*5°          4-3            4-i 
*6o          3-8            3-7 
*7o          3-3            3-2 
*8o          2.9            2.8 

.26 

•33 
•52 
•73 
•83 
J.04        j 

J.25            i 

.26 
•32 
•50 

•7 
.8 

J.O 
}  .2 

*  Indicates  determinations  made  by  Synthetic  Method,  for  which  see  page  16, 

ioo  cc.  H2O  dissolve  8.11  cc.  ether  at  22°;  vol.  of  solution,  107.145  cc.,  Sp. 
Gr.  0.9853. 

ioo  cc.  ether  dissolve  2.93  cc.  HzO  at  22°;  vol.  of  solution,  103.282  cc.;  Sp..Gr. 

0.7164.  (Herz,  1898.) 

More  recent  determinations  of  the  solubility  of  ethyl  ether  in  water,  agreeing 

closely  with  the  above  data,  are  given  by  Osaka,  1910. 

Data  for  the  temp.-pressure  diagram  of  ether-water  are  given  by  Scheffer,  19123. 

SOLUBILITY  OF  ETHER  IN   AQUEOUS   SOLUTIONS   OF   HYDROCHLORIC 

ACID. 

(Schuncke  — Z.  physik.  Chem.  14,  334,  '94;  in  38-52%  HC1,  Draper— Chem.  News,  35,  87,  '77.) 


In 

38.52  %HC1.             In  31.61  %H 

Cl.                     In  20  %  HC1. 

-6 
o 
+  6 

cc.  Ether              cc.  Ether             Gms.  per  i 
per  ioo  cc.            per  ioo  cc. 
Solvent.                 Solvent.                    HC1- 

181            149                   0.4622 
177.5         T42                    0.4622 
172.5        I3I-5                0.4622 

Gram  H2O.         cc.  Ether   Gms.  per  i  g.  H2O. 
(C2H5)2O.         Solvent.       HC1.        (C^g)^. 
.387              67.2      0.253      0-5637 
.308              58.3      0.253      0-4863 

.2075        51-1    o-253    0.4231 

15 

163            121.7(14°)      0.4622 

•1075        40-5    0.253    0.3299 

20 

158            in  .9  (20.8°)  0.4622 

•0005        33.1    0.253    0.2688 

26 

135            104.2                0.4622 

0.9360            27.5      0.253      0.2221 

In  i2.58%HCl. 

In  3.65  %HC1. 

to 

cc.  Ether  per       Gms.  per  i  Gram  H2O. 

cc.  Ether  per        Gms.  per  i  Gram  H2O. 

• 

ioo  cc.  Solvent.         HC1.        (C2H5)2O. 

ioo  cc.  Solvent.         HC1.          (C2Hfi)2O. 

-6 

26.45        0.144    0.2106 

19.23           0.0308      0.1454 

o 

22.  19           O-I44      0.1748 

... 

+6 

19.18           0-144      0-1503 

14.31           0.0308      0.1070 

15 

I5.6l            0.144      0-I2IO 

11.83           0-0308      0.0868 

20 

13.76           0-144      0.1059 

10.52           0-0308      0-0769 

26 

12.70           0.144      0.0970 

9.24           0-0308      0-0673 

The  above  data  are  recalculated  and  discussed  by  Juttner,  1901. 


ETHYL  ETHER 


298 


Data  for  the  solubility  of  ethyl  ether  in  carbon  dioxide  at  high  pressures  are 
given  by  Sander  (1911-12).  The  determinations  were  made  by  using  quite  small 
amounts  of  ether  and  observing  the  pressure  at  which  a  drop  of  liquid  just 
appeared  or  disappeared  in  a  mixture  of  known  weight  per  cent  composition. 
The  results  give  the  "gas  curve"  for  constant  temperature  and  when  plotted  in 
connection  with  the  "  liquid  curve"  (see  CO2,  p.  233),  give  the  complete  pressure 
—  concentration  diagram. 

Freezing-point  lowering  data  for  mixtures  of  ethyl  ether  and  hydrochloric  acid 
are  given  by  Maass  and  Mclntosh  (1913). 

SOLUBILITY  OF  ETHER  IN  AQUEOUS  SALT,  ETC.,  SOLUTIONS  AT  18°. 

(Euler,  1904.) 

Aq.  Solu- 
tion of: 


Aq.  Solu- 
tion of: 

vjms.  per 
Liter  Added 
Salt. 

oms.  (.L^tii 
per  100  c 
Solvent, 

Water 

0 

7.8 

KN03 

lOI.ig 

5-4 

KC1 

73-6 

4-7 

LiCl 

42.48 

5-2 

NaCl 

58-5 

4-5 

Mannite 
H2S04 


Gms.  per 
Liter  Added 

Gms.  (CjHs^O 
per  100  cc. 

Salt. 

Solvent. 

59-54 

3-7 

91  .06 

6.7 

49 

6.6 

122.5 

5-65 

245- 

4-55 

SOLUBILITY  OF  ETHYL  ETHER  IN  AQ.  SALT  SOLUTIONS  AT  28°. 

(Thorin,  1915.) 


Gms. 
S^vent.         £*£0 

Solvent. 

Gms.                                                                Gms. 

(CtfM>            Solvent                       (QH5)20 

per  100  cc.                                                       per  100  cc. 

Solvent. 

Solvent. 

Solvent. 

Water 

5-85 

o.s«Na3PO4 

4- 

17 

o.5«NaSuccinate 

4 

.68 

0.5  wNal 

5-70 

o  .  5  n  Na3  AsO4 

4- 

20 

o.  5  wNa  Citrate 

4 

.19 

o  .  5  n  NaBr 

4.68 

o.S«Hg(CN)2 

5- 

7i 

o.  5  wNa  Acetate 

4 

•IS 

o.swNaCl 

4.48 

o  .  5  n  NHUNOs 

5- 

37 

o  .  5  n  Na  Tartrate 

4 

.12 

o  .  5  n  NaF 

4-iS 

o  .  5  n  FeCls 

5- 

09 

o.s«NaPhthalate 

5 

.88 

o.swNa2SO4 

4-30 

o  .  5  n  Na2Cr2O7 

4- 

84 

o  .  5  n  Na  Cinnamate 

6 

.29 

0.5  wNa2CrO4 

4.22 

o.s«FeSO4 

4- 

33 

o.5«NaBenzoate 

5 

•99 

o  .  5  n  Na2MoO4 

4-39 

o.5wAl2(S04)3 

3- 

95 

o.5«NaSalicylate 

6 

•44 

o.5wNa2WO4 

4.12 

o  .  5  n  Am.  Oxalate  4  . 

74 

o  .  5  n  Na  Benzene  Sulf  onate 

6 

•°S 

SOLUBILITY  OF  ETHYL  ETHER  IN  0.91  PER  CENT  (PHYSIOLOGICAL  NORMAL 
SALINE)  AQUEOUS  NaCl  SOLUTION. 

'    (Bennett,  1912.) 

Determinations  made  by  freezing-point  method.     Ether  of  di6  =  0.720  used. 


t". 

Gms.  (QH^O 
per  100  Gms. 

cc.  (C2H5)20 
(at  15  )  per  100 

Aq.  NaCl. 

cc.  Aq.  NaCl. 

0 

13.08 

18.27 

5 

11.15 

I5-58 

10 

9-45 

13.20 

15 

8.10 

11.31 

20 

6.87 

9.60 

25 

5.96 

8.33 

30 

5-30 

7.40 

Purified  ether  prepared  from  methylated  spirit  gave  slightly  higher  results. 
SOLUBILITY  OF  ETHYL  ETHER  IN  AQ.  SULFURIC  ACID  AT  o°. 

(Kremann,  igioa.) 


Gms.  per  too  Gms.  Homogeneous  Mixture. 


Gms.  per  100  Gms.  Homogeneous  Mixture. 


(C2H5)20. 
24.2 
24.8 

43-9 
34 


H20. 

34-5 
35-4 
15.7 
26.1 


H2S04. 
41-3 

39-8 
40.4 

39-9 


(C2H6)20. 

16.1 
6.1 

53-8 


H20. 
42-7 
78 
8-5 


H2S04. 
41.2 

15-9 

37-7 


Data  for  the  system  ethyl  ether,  ethyl  alcohol,  water,  sulfuric  acid  at  o°  are  also 
given. 


299  ETHYL  ETHER 

SOLUBILITY  OF  ETHER  IN  AQUEOUS  ETHYL  ALCOHOL  AND  IN  AQUEOUS 
METHYL  ALCOHOL  MIXTURES  AT  20°. 

(Bancroft,  1895.) 

In  Ethyl  Alcohol.  In  Methyl  Alcohol. 

Per  5  cc.  QHsOH.  Per  5  cc.  QHjOH.  Per  i  cc.,  CHaOH.  Per  i  cc.  CH3OH. 


'cc.  H2O.* 

cc.  (Q 

.VCC.HA*  cc. 

(QH6)20.f 

cc.  H2O. 

cc.  (C2HB)2O. 

cc.  H20. 

cc.  (C2HB),0. 

50 

I  . 

30 

4.45 

7 

10 

I.I3 

0.83 

I. 

80 

25 

I. 

70 

4 

7 

,8 

7 

0.85 

0.64 

3 

10 

2. 

3-87 

8 

4 

0.60 

0.52 

5 

8 

3- 

35 

3.10 

10 

2 

•5 

0.56 

0.44 

10 

6 

5- 

10 

2.08 

15 

I 

.8 

0.63 

0-45 

IS 

5.21 

6 

1.77 

17 

•5 

I 

1.23 

*  Saturated  with  ether. 

f  Saturated  with  water. 

THE  SYSTEM  ETHYL  ETHER-MALONIC  ACID- WATER  AT  15°.    (Kiobbie,  1897.) 

Results  for  Conjugated  Liquid  Layers  Formed    Results  for  the  Liquid  Layers  in 
when  Insufficient  Malonic  Acid  to  Satu-  Contact  with  Excess  of 


rate  the 

Gms.  per  100  Gms 
Layer. 

Solutions  Was  Present. 

.  Lower        Gms.  per  100  Gms. 
Layer. 

Upper 

Gms 

Malonic  Ac 

,  per  100  Gms. 
Liquid. 

id. 

Solid  Phase. 

Malonic  Add 
« 

« 
tt 
tt 
tt 
tt 
it 

Malonic 
Acid. 
0 
4-63 
II.  60 
20.45 
27-43 
33-63 
34-17 
3I.II 

H20. 
92.23 

87.42 
79.92 

69-S5 
60.57 

47-45 
35-8i 
26.76 

Ethyl 
Ether. 

7-77 
7-94 
8.48 
9.99 

12 

18.80 
30.02 
42.12 

Malonic 
Acid. 
o 
0.72 
2.19 
5.01 
9-52 
21.89 

3°  -44 
31.11 

HA 

1.  2O 

i-54 
1.99 
3-o8 
5-i9 
13-42 
25-37 
26.76 

Ethyl 
Ether. 
98.80 

97-74 
95-82 
91.91 
85.29 
64.91 
44.19 
42.12 

Malonic 
Acid. 
8 
9.96 
19.41 
27.22 

35-51 
46.48 
51-33 
57-37 

H20. 
0 
0.42 
2-79 
5-23 
10.73 
20.86 
26.30 
39.10 

Ethyl. 
Ether. 
92 
89.61 
77.80 
67-54 
53-75 
32.66 
22.36 
3-52 

Data  for  the  system  ethyl  ether,  succinic  acid  nitrile  and  water  are  given 
by  Schreinemakers,  1898. 

Data  for  the  extraction  of  formic  acid  from  water  by  ether  are  given  by  Dakin, 
Janney  and  Wakemann,  1913. 

ETHYL  FORMATE  HCOOC2H6. 

100  grams  water  dissolve  10  grams  ethyl  formate  at  22°.  (Traube,  1884.) 

ETHYL  METHYL  KETONE  CH3.CO.C2H6. 

SOLUBILITY  IN  WATER.    (Rothmund;  1898.) 
By  synthetic  method,  see  Note,  page  16. 

,0          Gms.  Ketone  per  100  Gms.  Gms.  Ketone  per  100  Gms. 

Aq.  Layer.  Ketone  Layer.  Aq.  Layer.  Ketone  Layer. 

-io  34.5  89.7  90          16.1        84.8 

+  10  26.1  90  no          17.7        80 

30  21.9  89.9  130          21.8        71.9 

50  17.5  89  140         26          64 

70  16.2  85.7  i5i.8(crit.  temp.)  44. 2 

The  accuracy  of  Rpthmund's  data  is  questioned  by  Marshall  (1906)  and  the 
following  new  determinations  given. 

t'.  64.7°.          65.5°-         73-6°.        91-0°.  15°.  73-6°. 

Wt.  %  Ketone  in  Mixture     18.15     18.08      18      18.08    88.2    85.05 

Data  for  the  reciprocal  solubility  of  ethyl  methyl  ketone  and  water,  containing 
J-5%  ethyl  alcohol,  are  given  by  Bruni  (1899,  1900).  This  system  is  of  interest 
particularly  on  account  of  having  both  an  upper  and  a  lower  critical  point. 

Freezing-point  data  for  mixtures  of  ethylmethyl  ketone  and  water  are  given  by 
Timmermans  (1911)  and  by  Bruni,  1899,  1900. 


ETHYL  KETONE  300 

DiETHYL  KETONE   (Propione)  (C2H6)2CO. 

SOLUBILITY  IN  WATER.     (Rothmund,  1898.) 

The  determinations  were  made  by  Synthetic  Method,  see  p.  16.  The  critical 
temperature  could  not  be  reached  and  high  accuracy  is  not  claimed  for  the  results. 

Cms.  Diethyl  Ketone  Cms.  Diethyl  Ketone 

t».  per  IPO  Gms.  t°.  per  ioo  Cms. 

Aq.  Layer.    Ketone  Layer.  Aq.  Layer.    Ketone  Layer. 

20  4.60  ...  loo      3.68        93 .10 

40  3-43  97-42  120        4.05  QO.lS 

60    3.08   96.18       140  4.76   87.01 
80     3.20    94.92        160   6.10    83.33 

ETHYL  PROPIONATE  C2H6COOC2H5. 

SOLUBILITY  IN  WATER  AND  IN  AQUEOUS  ETHYL  ALCOHOL  MIXTURES. 

(Pfeiffer,  1892;  Bancroft,  1895.) 

.     4i™v,r,i  cc.  H2O  to  Cause  Separation  of  a  Second  Phase  in 

F  M-  ?  Mixtures  of  the  Given  Amounts  of  Alcohol 

and  3  cc.  Portions  of  Ethyl  Propionate. 

3  2.32 

6  6.87 

9  12.35 

12  IQ-I? 

15  27.12 

18  36.84 

21  50.42 

24  CO 

100  grams  H2O  dissolve  1.7  grams  ethyl  propionate  at  22°.  (Traube,  1884.) 

DiETHYL   Diacetyl  TARTRATE    (CHOCOCH3)2(COOC2H6),. 

Freezing-point  lowering  data  (solubility,  see  footnote,  p.  i)  for  mixtures  of 
diethyl  diacetyl  tartrate  and  each  of  the  following  compounds  are  given  by 
Scheuer  (1910);  m  nitrotoluene,  ethylene  bromide,  phenol  and  naphthalene. 
Results  for  diethyl  diacetyl  tartrate  and  naphthalene  are  also  given  by  Palazzo 
and  Batelli  (1883). 

ETHYL  VALERATE  C4H9COOC2H6. 

ETHYL   (Iso)   VALERATE   (CH3)2.CH.CH2COOC2H6. 

SOLUBILITY  OF  EACH  IN  WATER  AND  IN  AQUEOUS  ALCOHOL  MIXTURES  AT  20°. 

(Pfeiffer,  1892;  Bancroft,  1895.) 

ioo  cc.  water  dissolve  0.3  .cc.  ethyl  valerate  at  25°. 
100  cc.  water  dissolve  0.2  cc.  ethyl  iso  valerate  at  20°. 
ioo  cc.  ethyl  iso  valerate  dissolve  0.4+  cc.  water  at  20°. 

Mixtures  of  Ethyl  Alcohol,  Mixtures  of  Ethyl  Alcohol, 

Ethyl  Valerate  and  Water.  Ethyl  Iso  Valerate  and  Water. 

Per  5  cc.  Ethyl  Alcohol. 

CC.Alcohol*    cc.H20.f    cc.Alcohol*    cc.H2O-t  ' 177 "Cc  Ethyl     ' 

CC'H2°-     Iso  Valerate. 

10  0.15 
8  0.23 
6  0.46 

5          o-72 
4          1.23 

*  cc.  Alcohol  in  mixture. 

t  cc.  H2O  added  to  cause  the  separation  of  a  second  phase  in  mixtures  of  the  given  amounts  of  alcohol 
and  3  cc.  portions  of  ethyl  valerate. 


3 

1.42 

39 

53-13 

9 

7.18 

45 

63.60 

15 

14-13 

57 

90-53 

21 

22.40 

72 

131.0 

27 

31.62 

81 

180.0 

33 

41  .62 

ETHYLENE  C2H4. 

301                                       El 

SOLUBILITY  IN  WATER  AND  IN  ALCOHOL. 

(Bunsen  and  Carius;  Winkler,  1906.) 

t°. 
O 

0 

0. 

.226 

O 

q- 
.0281 

Solubility 

in  Alcohol. 

5 

O 

.191 

0 

.0237 

t°.     I(^c 

Vol^AlcSd. 

10 

0 

.162 

o 

.0200 

0 

359-5 

15 

0 

•139 

0 

.0171 

4 

337-5 

20 

0 

.122 

0 

.0150 

10 

308.6 

25 

0 

.108 

o 

.0131 

15 

288.2 

30 

o 

.098 

0 

.0118 

20 

271-3 

ETHYLENE 


O.I. 

0.25. 

0.5. 

0.75. 

X.O. 

0.154 

0.144 

0.130 

0.118 

o  .  1056 

0.153 

0.144 

0.128 

0.114 

O.IOI 

0.157 

0.156 

o.i55 

0.154 

0.1525 

0.1425 

0.127 

0.109 

0.093 

For  ft  and  q  see  Ethane,  p.  285. 
SOLUBILITY  OF  ETHYLENE  IN  AQUEOUS  SOLUTIONS  OF  ALKALI  HYDROXIDES, 

ETC.,  AT   15°.      (Billitzer,  1902.) 

Results  in  terms  of  the  Ostwald  Solubility  Expression  /.     See  p.  227. 

Solubility  1K  in  Aq.  Solution  of  Normality: 
Aqueous  Solution  of: 

KOH 

NaOH 

NH40H 

|  Na2SO4 

In  HzO  alone     o .  1593 

SOLUBILITY  OF  ETHYLENE  IN  METHYL  ALCOHOL  AND  IN  ACETONE.    (Levi,  1901.) 
Results  in  terms  of  the  Ostwald  Solubility  Expression  /.     See  p.  227. 

t°.        In  Methyl  Alcohol.       In  Acetone.  t".       In  Methyl  Alcohol.        In  Acetone. 

o    3-3924     4-0652      30    1.8585     1.8680 
10    2.8831     3-358°      40    1-3432     1.0852 

20      2.3718       2.6278         5O      0.8259       0.2772 

25  2.1154  2.2500  60         0.3506 

The  formulas  from  which  the  above  figures  were  calculated  are: 

In  Methyl  Alcohol,        I  =  3 .3924  —  0.05083  /  —  o.ooooi  ^. 

In  Acetone,  /  =  4.0652  —  0.06946  /  —  0.000126  P. 

SOLUBILITY  OF  ETHYLENE  IN  SEVERAL  SOLVENTS.    (McDaniel,  1911.) 

qnlvwi  *°        Abs- Coef-       Bunsen  Qnlv^nt        t «  Abs-  Coef-  Bunsen 

Solvent.         t.  A  Coef.0.  solvent.       t.  A  Coef .  0. 

Benzene  22  3.010  2.786  Heptane  22.4  3-463  3.207 

35  2.655  2.353  35  3-186  2.824 

50  2.482  2.100  39  3.110  2.722 

Hexane  22  3.038  2.8141  Acetone  20  2.571  2.290 

35  2.826  2.505  35  2.308  2.046 

?     "  45        2.586        2.219          Limonene   22        no  constant  equilibrium 

Abs.  Coef.  A  =  vol.  of  ethylene  absorbed  by  unit  vol.  of  solvent  at  temp,  stated. 

For  definition  of  Bunsen  Coef.  ft,  see  carbon  dioxide,  p.  227. 

The  Coef.  of  Abs.  ft  of  ethylene  in  Russian  petroleum  is  o.  1 64  at  I  o°  and  o.  1 42  at  20°. 

(Gniewosz  and  Walfisz,  1887.) 

Freezing-point  data  (solubility,  see  footnote,  p.  i)  for  mixtures  of  ethylene  and 
methyl  ether  are  given  by  Baume  and  Germann,  1911,  1914. 

ETHYLENE  BROMIDE  C2H4Br2. 

F.-PT.  DATA  FOR  MIXTURES  OF  ETHYLENE  BROMIDE  AND  OTHER  COMPOUNDS. 

Ethylene  Bromide  +  Naphthalene  (Baud,  1912;  Dahms,  1895.) 

44         +  ft  Naphthol  (Bruni,  1898.) 
•  "        -j-           "      +  Picric  Acid  (Bruni,  1898.) 

-j-  Paraldehyde  (Paterno  and  Ampola,  1897.) 

-j-  Phenol  (Dahms,  1895;  Paterno  and  Ampola,  1897.) 

-j-  Toluene  (Baud,  1912.) 

"         +  Bromotoluene  (Paterno  and  Ampola,  1897.) 
"-             "        +£Xylene 


ETHTLENE  CYANIDE  302 

ETHYLENE   CYANIDE  C2H4(CN)2. 
DISTRIBUTION  BETWEEN  WATER  AND  CHLOROFORM.    (Hantzsch  and  Vagt,  1901.) 


Gm.  Mols.  QjH^CCN);;  per  Liter.  .      Cl. 

*  •  /     T  r^-w-rf^i  -T  Ivatio.  ~—  • 

Aq.  Layer,  c\.         CHClj  Layer,  c%.  c2. 

o      0.0786      0.0464     1.69 
10      0.0787      0.0463      1.70 

20       0.0791        0.0459       1.72 

Additional  data  for  the  influence  of  KOH,  KC1  and  HC1  on  the  above  distri- 
bution are  also  given. 

DiETHYLENE  ETHER   (CH2OCH2)2. 

Freezing-point  data  (solubility,  see  footnote,  p.  i)  are  given  for  mixtures  of 
diethylene  ether  and  water,  by  Unkovskaja,  1913. 

Tetraphenyl  ETHYLENE    (C6H5)2C:C(C6H5)2. 

Freezing-point  data  for  tetraphenyl  ethylene  +  silicotetraphenyl  are  given  by 
Pascal  and  Normand  (1913). 

0  EUCAINE   Ci5H21NO2  and  Salts. 

100  cc.  H2O  dissolve  0.296  gm.  anhydrous  ft  eucaine  at  20°.  1     (Zalai, 

100  cc.  oil  of  sesame  dissolve  3.49  gms.  anhydrous  ft  eucaine  at  20°.     )     1910.) 

100  cc.  aniline  oil  dissolve  66.6  gms.  anhydrous  /3  eucaine  at  20°. 

100  cc.  H2O  dissolve    2.5  gms.  /3  eucaine  hydrochloride  at  15-20° 


(Squire  and 
Caines, 
1905.) 


ioo  cc.  90%  alcohol  9 

100  cc.  H2O  "  25  "  lactate 

ioo  cc.  90%  alcohol  "  12.5  " 

loocc.  CHC13  "  20  " 

EUROPIUM   Bromonitrobenzene  SULFONATE  Eu[C6H3Br(i)N02(4)SO3(2)]j.- 

ioH2O. 
ioo  gms.  sat.  solution  in  water  contain  6.31  gms.  anhydrous  salt  at  25°. 

(Katz  and  James,  1913.) 

FATS. 

SOLUBILITY  OF  THE  FATTY  ACIDS  OBTAINED  FROM  SEVERAL  SOURCES  IN 
ALCOHOL  AND  IN  BENZENE.     (Dubois  and  Fade,  1885.) 


Crude  Fatty 

Gms.  Fat  j 

>er  ioo  Gms.  Ab; 

5.  Alcohol  at: 

Gms.  Fats  per  ioo 

Acid  of: 

r  o°. 

10°. 

26°. 

Gms.  Benzene  at  1  2°, 

Mutton 

2.48 

5.02 

67.96 

14.70 

Beef 

2.51 

6.05 

82.23 

15.89 

Veal 

5 

13.78 

137.10 

26.08 

Pork 

5-63 

11.23 

118.98 

27.30 

Butter 

10.  61 

24.81 

158.2 

69.61 

Margarine 

2-37 

4-94 

47.06 

13-53 

MlSCIBILITY  OF  FATS  AND  90  VOL.  PER  CENT  ALCOHOL  AT  37°.     (Vandevelde,  1911.) 

Mixtures  of  fats  and  alcohol  in  various  proportions  were  shaken  twice  daily  for 

8  days  and  the  volume  of  each  layer,  as  well  as  its  composition,  determined. 


Composition  of  Mixture- 
Mixture.             .  —  *  . 
cc.  Alcohol        cc.  Fat 

Alcohol  +  Cocaline        25               5 

Volume  after  Agitation. 

Gms.  Fat  per  Gms.  Alcohol 
ioo  Gms.      per  ioo  Gms. 
\lcohol  Layer    Fat  Layer. 

4-9              19-4 

cc.  Alcohol 
25-4 

cc.  Fat     , 
4-6 

« 

(1 

2O 

IO 

19 

.2 

10.8 

5 

.6 

16 

,2 

it 

u 

is 

IS 

13 

17 

7 

.2 

13 

5 

N 

(( 

10 

20 

6 

•7 

23 

•3 

9 

.1 

12 

,2 

ft 

ll 

5 

25 

i 

.1 

28 

•9 

13 

II, 

4 

Alcohol  + 

Butter  Fat 

25 

5 

25 

.r 

4 

•9 

3 

•  5 

17 

4 

" 

" 

20 

IO 

19 

.2 

IO 

.8 

3 

•5 

14 

i 

" 

" 

IS 

IS 

13 

17 

4 

14 

i 

" 

** 

10 

20 

7 

.  i 

22 

9 

S 

•  7 

" 

" 

5 

25 

2 

28 

14 

.1 

9 

5 

Alcohol  + 

Olive  Oil 

25 

S 

24 

•  7 

5-3 

2 

•3 

ii 

2 

" 

" 

20 

IO 

19 

.2 

IO 

.8 

2 

•4 

8 

.7 

'* 

" 

IS 

15 

13 

17 

2 

•  4 

8 

7 

N 

« 

10 

20 

7 

-5 

22 

•  5 

2 

•  5 

•      8 

8 

H 

M 

5 

25 

2 

.2 

27 

.8 

7 

7 

,6 

For  other  data  on  the  solubility  of  fats  see  Ewers  (1910)  and  Louise  (1911). 


303  FLUORENE 

FLUORENE   (Diphenylenemethane)  C6H4.CH2.C«H4. 

Freezing-point  data  (solubility,  see  footnote,  p.  i)  are  given  by  Kre*mann  (1911) 
for  mixtures  of  fluorene  and  each  of  the  following  compounds:  o,  m  and  p  dintro- 
benzene,  1.3.5,  trinitrobenzene,  dinitrophenol,  dinitrotoluene,  trinitrotoluene  and 
picric  acid. 

FLUORESCEIN 


100  gms.  H2O  dissolve  0.005  Sm«  fluorescein  at  20-25°  (Dehn,  1917.) 

100  gms.  pyridine  dissolve  13.29  gms.  fluorescein  at  20-25°  " 

100  gms.  aq.  50%  pyridine  dissolve  37.22  gms.  fluorescein  at  20-25°  " 

FORMALDEHYDE,    Solid   Polymers   (CH2O)n. 

SOLUBILITY  OF  THE  Six  WELL-DEFINED  SOLID  POLYMERS  OF  FORMAL- 

DEHYDE IN  WATER.     (Auerbach  and  Barschall,  1908.) 

Name.  Formula.  m.  pt.       Gms.  per  100  cc.  Sat.  Solution  in  Water. 

Paraformaldehyde      (CH2O)n+#H2O       150-160     20-30  gms.  at  18° 
a  Polyoxymethylene     (CH2O)n  163-8        n  gms.  at  18-25° 

/3  Polyoxymethylene     (CH2O)n  163-8        3.3  gms.  at  18°,  about  4  at  25° 

7  Polyoxymethylene     (CH2O)n  ^S~5        less  than  o.i  at  18°,  o.i  gm.  at  25° 

8  Polyoxymethylene     (CH2O)n  169-70      practically  insoluble 

a  Trioxymethylene        C3H6O3  63-4        17.2  at  18°,  21.1  at  25° 

All  are  insoluble  in  alcohol  and  ether  except  trioxymethylene. 
SOLUBILITY  OF  TRIOXYMETHYLENE  IN  AQ.  SODIUM  SULFITE  SOLUTIONS  AT  15°. 

(Lumiere  and  Seyewetz,  1902.) 

Gms.  Na2S03  per  100  cc.  H2O  5        10        20        25      28  (sat.) 

Gms.  CsHeOs  per  100  cc.  sat.  sol.      22        24        26        27      27 
Data  are  also  given  for  the  solubility  of  various  mixtures  of  trioxymethylene 
and  sodium  sulfite  in  water  at  15°. 

The  distribution  coefficient  of  formaldehyde  between  water  and  ether  is  8.5  at 
O°  and  9.23  at  2O°.  (Hantzsch  and  Vagt,  1901.) 

FORMAMIDE  HCONH2. 

SOLUBILITY  IN  WATER,  DETERMINED  BY  THE  FREEZING-POINT  METHOD. 

(English  and  Turner,  1915.) 

Gms.  Gms.  Gms. 

t°  of      HCONH2    Solid     t°  of       HCONH2       <,  r  ,  p,    ^  t°  of        HCONH2   ~  ,.  .  p. 

Solidif.       per  100     Phase.  Solidif.      per  100          Solid  Phase.  Solidif         per  IQQ  2   Solid  Phase. 
Gms.  H2O.                             Gms.  H2O.  Gms.  H2O. 

—  o           o  Ice    —31.1  116.4  Ice  —37-6  267        HCONHa 

-2.7       9.93  "  -42.5  169  -29.4  369-8 

-5.7      17.87  "  -45-4  187-8  HCONH2.H2O      -21.9  540.3 

-ii         35.45  "  -40.4  218.3  "                -14-5  836.8 

-23.6      81.93  -40  241.4  -  6.4  1780 

Similar  data  are  also  given  for  formamide  +  formic  acid  and  formamide  -h 
propionic  acid. 

o  and  p  ChloroFORMANILIDES   C1.C6H4NH.CHO. 

Freezing-point  lowering  data  for  mixtures  of  o  and  p  chloroformanilide  are 
given  by  King  and  Orton,  1911. 

FORMIC  ACID  HCOOH. 

SOLUBILITY  IN  WATER,  DETERMINED  BY  FREEZING-POINT  METHOD.    (Faucon,  1910.) 

to  f     Gms.  HCOOH        «,  .      Gms.  HCOOH      to  of    Gms.  HCOOH 


o  o 

-5  12.5 

—  10  23 

—  15  32 

—  20  39.2 
-25  46.5 

Similar  data  for  mixtures  of  97.4%  formic  acid  and  water  are  given  by  Kremann, 
1907. 


-30 

53 

-40 

74.2 

-35 

57-6 

-30 

79 

-40 

62.5 

—  20 

84.2 

-45 

66.5 

—  10 

89.4 

—49  Eutec. 

70 

0 

95 

-45 

71.7 

+8.51 

TOO 

FORMIC  ACID  304 

DISTRIBUTION  OF  FORMIC  ACID  BETWEEN  WATER  AND  BENZENE  AT  13-15°. 

(v.  Georgievics,  1913.) 

A  small  separatory  funnel  was  used  and  the  acid  in  each  layer  titrated  with  o.i 
n  NaOH,  using  phenolphthaleine  as  indicator. 

Cms.  HCOOH  Found  per:  Cms.  HCOOH  Found  per: 


25  cc.  H2O  Layer. 

isocc.  C6H6  Layer. 

25  cc.  H2O  Layer. 

iSoce.  C6H6  Layer. 

1.016 

0.016 

2.365 

0.035 

1-539 

0.031 

3.826 

O.O62 

1.800 

0.024 

5^74 

O.II4 

2.  112 

0.031 

7.836 

0.138 

p__ 

The  distribution  ratio  of  formic  acid  between  water  and  benzene  was  found  by 
King  and  Narracott  (1909)  to  be  I  to  0.0242  at  room  temp. 

Freezing-point  lowering  data  (solubility,  see  footnote,  p.  i)  are  given  for  mix- 
tures of  formic  acid  and  dimethylpyrone  by  Kendall,  1914. 

FUMARIC  ACID  COOH.CH:CH.COOH. 

MALEIC  ACID   COOH.CHrCH.COOH.     (See  also  p.  398.) 
SOLUBILITY  IN  WATER.    (Vaubel,  1899.) 

loo  gms.  water  dissolve  0.672  gm.  fumaric  acid  at  165°. 

100  gms.  water  dissolve  50  grams  maleic  acid  at  100°. 

Data  for  the  distribution  of  fumaric  acid  between  water  and  ether  at  25°  are 
given  by  Chandler,  1908. 

FURFUROL  C4H3OCHO. 

SOLUBILITY  IN  WATER.    (Rothmund,  1898.) 
Determinations  by  Synthetic  Method,  for  which  see  p.  16. 

Gms.  C4H3OCHO  per  100  Gms.  Gms.  C4H3OCHO  per  100  Gms. 

Aq.  Layer.       Furfurol  Layer.  Aq.  Layer.       Furfurol  Layer. 

40  8.2  93.7  ioo          18.9  83.5 

50  8.6  93  no          24  78.5 

60  9.2  92  115          28  74.6 

70  10.8  90.7  120          34.4  68.1 

80  13  89  122.7  (crit.  t.)  51 

90  15.5  86.6 

GADOLINIUM  CobaltiCYANIDE  GdiCCoCeNe^HjO. 

looo  gms.  aq.  10%  hydrochloric  acid  dissolve  1.86  gms.  of  the  salt  at  25°. 

(James  and  Willard,  1916.) 

GADOLINIUM  GLYCOLATE  Gd2(C2H3O3)3.2H2O.  , 

IOOO  CC.  H2O  dissolve  14.147  gms.  of  the  salt  at  2O°.     (Jantsch  and  Grunkraut,  1912-13.) 

GADOLINIUM   Magnesium  NITRATE,   etc. 

SOLUBILITY  OF  DOUBLE  NITRATES  OF  GADOLINIUM  AND  OTHER  METALS  IN  CONC. 
NITRIC  ACID  OF  dy  =  1.325  (  =  51.59  GM.  HNO3  PER  ioo  cc.)  at  16°.  (Jantsch,  1912.) 

Gms.  Hydrated 

Salt.  Formula.  Salt  per  Liter 

Sat.  Solution. 

Gadolinium  Magnesium  Nitrate       [GdCNOa^feMga^I^O        352 .3 

Nickel  "  "          Ni3      "  400.8 

Cobalt  "  "          Co3     "  451-4 

Zinc  Zn3     "  472.7 

GADOLINIUM  OXALATE  Gd2(C2O4)3.ioH2O. 

SOLUBILITY  IN  AQUEOUS  SOLUTIONS  OF  SULFURIC  ACID  AT  25°.    (Wirth,  1912.) 

Normality  of         Gms.  per  ioo  Gms.  Sat.  Sol. 
Aq-H2S04.         — Gd^ Gd2(CA)3. 

2.16  0.1883  0.3005      Gd2(C204)3.ioH2O 

3.11  0.3010  0.4803 

4-32  0.4359  0.6956 

6.175  0.707  1.128 


305  GADOLINIUM   OXALATE 

SOLUBILITY  OF  GADOLINIUM  OXALATE  IN  AQUEOUS  20%  SOLUTIONS  OF 
METHYLAMINE  OXALATE,  ETHYLAMINE  OXALATE  AND  TRIETHYLAMINE  OXALATE. 

(Grant  and  James,  1917.) 


. 

Aq.  20%  Methylamine  Oxalate  0.069 

"         Ethylamine  0.360 

"         Triethylamine      "  0.883 

GADOLINIUM   Dimethyl  PHOSPHATE   Gd2[(CH3)2PO4]6, 

100  gms.  H2O  dissolve  23  gms.  Gd2[(CH3)2PO4]6  at  25°  and  6.7  gms.  at  95°. 

(Morgan  and  James,  1914.) 

GADOLINIUM  SULFATE  Gd2(SO4)3.8H2O. 

SOLUBILITY  IN  WATER.    (Benedicks,  1900.) 

t<>.  ,        Gms-  era8  H2bPef  I0°  Solid  Phase' 

•      o  3.98'  '  Gd2(SO4)3.8H2O 

10  3-3 

14  2.8 

25  2.4 

34.4          2.26 

SOLUBILITY  OF  GADOLINIUM  SULFATE  IN  AQUEOUS  SOLUTIONS  OF: 
Sodium  Sulfate  at  25°.    (Bissell  and  James,  1916.)        Sulf  uric  Acid  at  25°.    (Wirth,  1912.) 

Gms.  per  100  Gms.  H2O.  Normality  Gms.  P61"  I0°  Gms-  Sat-  So1- 

' 


NasS04. 
O 

Gd2(SO4) 
2.15 

Gd2 

UUU    i  1UIOC. 

(SO4)3.8H2O 

ofH 
0 

'    Gd203  = 
1-793 

2, 

Igsl* 

Gd2(S04)3.8H20 

0.43 

2.06 

it 

0 

I 

1.98 

3 

.291 

M 

0.47 

0.76 

Gd2(SO4)3.Na2SO4.2H2O 

o. 

505 

2-365 

3- 

931 

M 

1.26 

0.17 

11 

I, 

I 

2.29 

v5 

.807 

€( 

3-01 

0.07 

ti 

2 

.16 

1.789 

2 

974 

tl 

7.46 

0.05 

(i 

6. 

175 

0.528 

0.8777 

it 

27.40 

0.05 

(i 

12. 

6 

0.0521 

O. 

,0867 

ft 

GADOLINIUM  SULFONATES. 

SOLUBILITY  IN  WATER.  Gms 

Salt.  Formula.  *°-&SK?S    Authority- 

Gms.  H2O. 


xS    43.8 
Gd[CtH3Br(N02)SOs(I.4.2)],IoH20  ,S      6.3. 


GALACTOSE   C6Hi2O6.     See  also  Sugars,  pages  695-7. 

100  gms.  saturated  solution  in  pyridine  contain  5.45  gms.  C6Hi2O6  at  26°, 

density  of  solution  =  1.0065.  (Holty,  1905.) 

100  gms.  H2O  dissolve  68.3  gms.  galactose  at  20-25°.  (Dehn,  917.) 

100  gms.  aq.  50%  pyridine  dissolve  6.83  gms.  galactose  at  20-25°.  " 

GALLIC  ACID  3.4.5,    (OH)3C6H2COOH.H2O. 

SOLUBILITY  IN  AQUEOUS  ETHYL  ALCOHOL  AT  25°. 

(Seidell,  1910.) 

Wt.  PerCent  fnT^nntPfr  n       Wt.  Per  Cent  rniS"™™?'*?  O 

CjHsOHm       ^Sat-So..     <°^™GH*»°         &H£H  in      ^of  Sat.  Sol.      «*>*%$£? 
Solvent.  Sat.  Sol.  Solvent.  Sat  ^ 

o  1.002  1.15  60  0.957  16 
10  0.992  2  70  0.946  18 
20  0.983  4.2  80  0.933  I9-9 

30       0.977       7.5  90       0.919       21.2 

40     0.972    10.6        95     0.911     21.6 

50  0.965  13.4  IOO  0.902  22.2 

IOO  gms.  H2O  dissolve  0.95  gm.  gallic  acid  at  15°.  (Greenish  and  Smith,  1903.) 

loo  gms.  H2O  dissolve  33.  3  gms.  gallic  acid  at  100°.  (U.  S.  P.  VIII) 


GALLIC  ACID  306 

SOLUBILITY  OF  GALLIC  ACID  IN  ORGANIC  SOLVENTS  AT  25°. 

(Seidell,  1910.) 

^    «f  Qof  Gms-  CfiH2(OH)j 

Solvent.  Density  of  Solvent.  Solution  COOH.H2O  per  100 

Gms.  Sat.  Sol. 

Acetone  du>  =  0.797  0.941  25-99 

Amylalcohol  (iso)        ^0=0.817  o .  834  5.39 

Amylacetate  ^20  =  0.875  0.878  2.72 

Benzene  d&  =  0.873  °-&7S  0.022 

Carbon  Bisulfide         di  =  1.258  1.262  0.042 

Ether  (abs.)  ^20  =  0.711  0.718  i-37° 

Ethylacetate  d&  =  0.892  0.911  3.610 

The  amount  of  gallic  acid  dissolved  by  carbon  tetrachloride,  chloroform  and 
toluene  was  too  small  for  estimation. 

100  gms.  glycerol  dissolve  8.3  gms.  C6H2(OH)3CpOH.H2O  at  25°.  (U.  S.  P.  VIII.) 
loo  gms.  95%  formic  acid  dissolve  0.56  gm.  gallic  acid  at^!9.4°.        (Aschan,  1913.) 

GERMANIUM  DIOXIDE  GeO2. 

loo  gms.  H2O  dissolve  0.405  gm.  GeO2  at  20°,  and  1.07  gms.  at  100°.  (Winkler,  1887.) 

GERMANIUM  (Mono)  SULFIDE  GeS 
GERMANIUM  (Di)  SULFIDE  GeS* 

100  gms.  H2O  dissolve  0.24  gm.  GeS 

loo  gms.  H2O  dissolve  0.45  gm.  GeSa.  (Winkler,  1887.) 

GLASS. 

For  data  on  the  solubility  of  glass  in  water  and  other  solvents,  see: 

(Cowper,  1882;  Emmerling,  1869;  Bohling,  1884;  Kreusler  and  Herzhold,  1884;    Kohlrausch,   1891; 
Forster,  1892;  Mylius  and  Forster,  1889;  1892;  Wartha,  1885;  Nicolardot,  1916.) 

GLOBULIN    (Serum). 

SOLUBILITY  IN  AQUEOUS  MAGNESIUM  SULFATE  SOLUTIONS. 

(Galeotti,  1906;  Scaffidi,  1907.) 

The  precipitated  globulin  (from  oxblood)  was  not  dried,  but  pressed  between 
filter  paper,  and  an  excess  introduced  into  each  MgSC>4  solution.  After  constant 
agitation  for  12  hours,  the  saturated  solution  was  filtered,  weighed  and  evaporated 
to  constant  weight,  the  coagulated  globulin  then  washed  to  disappearance  of  SO4 
and  dried  and  weighed. 
Results  for  10°.  Results  for  25°.  Results  for  40°.  Results'for  55°.  Results  for  70°. 

Gms.  per  ido  Gms.  Gms.  per  100  Gms.  Gms.  per  100  Gms.  Gms.  per  100  Gms.  Gms.  per  100  Gms. 
Sat.  Sol.         Sat.  Sol.         Sat.  Sol.         Sat.  Sol.         Sat.  Sol. 


MgS04. 

Globulin. 

MgS04. 

Globulin. 

MgS04. 

Globulin. 

MgS04. 

Globulin. 

MgS04. 

Globulin. 

0.06 

0.07 

0.06 

0.07 

0.06 

0.42 

0.40 

1.14 

0.71 

o-34 

0.18 

0-34 

O.2I 

0.61 

0.31 

1.42 

0.88 

2.14 

2.52 

o-55 

0.65 

I.63 

0.63 

2.  2O 

0.61 

5-39 

i.  60 

3-34 

4-74 

1.14 

2.  II 

3-35 

2.28 

5.56 

1.92 

8.31 

S-64 

5-06 

6.83 

1.17 

4-32 

4-42 

3-35 

6.07 

5-40 

8.63 

10.81 

3.10 

9.22 

1.76 

I3-63 

2.60 

16 

4-03 

14.72 

3 

13-84 

2.  II 

13.29 

i 

20.86 

0.37 

21.30 

o-95 

18.47 

i.  02 

17.90 

0.69 

15.38 

0-37 

24.18 

0.18 

25-47 

0.03 

27.03 

O.OI 

17.67 

0.07 

The  coagulation  curve  and  freezing-point  curve  are  also  given. 

GLUCOSE  d  C6Hi2O6.H2O.    See  also  Sugars,  pages  695-7. 

100  gms.  H2O  dissolve  82          gms.  glucose  at  20-25°.       (Dehn,  1917.) 

100  gms.  pyridine  7.62       " 

100  gms.  aq.  50%  pyridine        "       49.17       "          "  "  " 

100  gms.  trichlor  ethylene  0.006     "  15° 

(Wester  and  Bruins,  1914.) 

GLUTAMINIC  ACID  C3H5NH2(COOH)2. 

Data  for  the  solubility  of  glutaminic  acid  in  aq.  salt  solutions  are  given  by 
Wiirgler  (1914)  and  Pfeiffer  and  Wurgler  (1916). 


307  GLUTAMINIC  ACID 

GLUTAMINIC  ACID  HYDROCHLORIDE   C3H6NH2(COOH)2.HC1. 

SOLUBILITY  IN  WATER.     (Stoitzenberg,  1912.) 
(The  following  results  were  taken  from  the  diagram  given  by  the  author.) 

Cms.  Glutaminic  Acid.  Cms.  Glutaminic  Acid. 

t°.  HC1  per  100  cc.  t°.  HC1  per  100  cc. 

Sat.  Sol.  Sat.  Sol. 

o  3i-5  60  57 

10  34.5  70  62 

20  38  80  67.5 

30  42-5  90  74 

40  47  100  81 

50  52  20  1.4  (sol.  sat.  with  HC1) 

GLUTARIC  ACID    (Pyrotartaric)  (CH2)3(COOH)2. 

SOLUBILITY  IN  WATER.    (Lamouroux,  1899) 

t°.  o°.  15°.  20°.  35°.  50°.  65°. 

Cms.  (CH2)3(COOH)2 

per  100  cc.  solution  42.9     58.7     63.9     79.7     95.7     ni.8 

100  gms.  95%  formic  acid  dissolve  55.62  gms.  glutaric  acid  at  18.6°.  (Aschan,  1913.) 
Data  for  the  distribution  of  glutaric  acid  between  water  and  ether  at  25°  are 
given  by  Chandler,  1908. 

F.  pt.  data  for  glutaric  acid  +  sulfuric  acid.  (Kendall  and  Carpenter,  1914.) 

GLYCINE    (Glycocoll)   CH2.NH2.COOH. 

loo  gms.  H2O  dissolve  51  gms.  CH2.NH2.COOH  at  20-25°.  (Dehn,  1917.) 

100  gms.  pyridine  dissolve  0.61  gm.  CH2.NH2.COOH  at  20-25°. 
100  gms.  aq.  50%  pyridine  dissolve  0.74  gm.  CH2.NH2.COOH  at  20-25°.     " 
SOLUBILITY  OF  GLYCINE  IN  WATER  AND  IN  AQ.  SALT  SOLUTIONS  AT  20°. 

(Pfeiffer  and  Wurgler,  1915,  1916.) 
Mnlc  Sal*     Gms.  Glycine  ,»  ,    colf    Gms.  Glycine 


Water  only              1.962  LiCl        0.96        4.188 

BaCl2        0.5          2.375  LiBr        0.97        4.245 

BaBr2       0.5          2.954  SrCl2       0.25        2.129 

SrCl2         0.5          2.362  0.50        2.331 

SrBr2        0.49        2.440  i              2.605 

CaCl2        0.57        4.848  2              3.301 
CaBr2        0.51        4-994 

10  cc.  sat.  aq.  solution  contains  1.8  gms.  glycine  +  2.7  gms.  KC1  at  20°  when 

both  are  present  in  the  solid  phase.  (Pfeiffer  and  Modelski,  1912.) 

GLYCOLIC  ACID  CH2OH.COOH. 

SOLUBILITY  IN  WATER.     (Emich,  1884.) 

t°.  20°.  60°.  80°.  100°. 

Gms.  CH2OH(COOH) 

per  100  gms.  H2O  0.033        0.102        0.235        0.850 

PhenylGLYCOLIC  ACID   dextro  and  racemic.     CH.C6H5.OH.COOH. 
SOLUBILITY  OF  DEXTRO  AND  OF  RACEMIC  PHENYL  GLYCOLIC  ACID  IN  CHLOROFORM. 

(Holleman,  1898.) 

Gms.  Detro  Acid  Gms.  Racemic 

t°.  per  loo  Gms.  t°.  Acid  per  100 

CHC13.  Gms.  CHClj. 

IS  0.952  IS  0.877 

25  1.328  25  1.07 

35  i-95o  35  1-6° 

GLYCYRRHIZIC  ACID. 

100  gms.  sat.  solution  in  H2O  contain  0.575  gm.  glycyerrhizicacid  at  15°.  (Capin,  '12.) 
IOO  gms.  sat.  solution  in  H2O  contain  0.152  gm.  Am.  glycyrrhizate  at  o°  and 
0.225  gm-  at  15°.   '  (Capin,  1912.) 

PhenylGLYOXAL   Phenyl  hydrazone   C6H5.CO.CH.N.NH.C6H6. 

One  liter  C6H6  dissolves  52.6  gms.  of  the  A  form  at  5°.  (Sidgwick,  1915  ) 

One  liter  CeHe  dissolves  2.9  gms.  of  the  B  form  at  5°.  " 


GOLD  308 

GOLD  Au. 

SOLUBILITY  OF  GOLD  IN  POTASSIUM  CYANIDE  SOLUTIONS.     (Maclaurin,  1893.) 
Gold  disks  were  placed  in  Nessler  tubes  with  aqueous  KCN  solutions. 
Gms.  Au  Dissolved  in  24  Hours  in  Nessler  Tubes: 


rer  cent 
KCN. 

Full. 

£  Full. 

Oxygen. 
Passed  in. 

Oxygen  + 
Agitation. 

O.I 

I 

5 

O.OOI95 
O.OOI62 
0.0032 

0.00331 
O.OO4I8 
0.0046 

o  .  00845 

0.01355 

0.0472 

20 

5° 

O.OOI2 
O.OOO43 

0.00305 
O.OOO26 

O.OII5 
0.00505 

0.0314 
O.OIO8 

The  following  data  for  more  dilute  KCN  solutions  are  given  by  Christy  (1901). 
Gold  strips  2  X  |  inch  were  rotated  for  24  hrs.  in  aq.  KCN  solutions  and  the 
loss  in  weight  determined. 

1  Per  cent  Mgs.  Au  Per  cent         Mgs.  Au  Per  cent         Mgs.  Au 

KCN.  Dissolved.  KCN.         Dissolved.  KCN.          Dissolved. 

o  o.oio  0.002          0.44  0.016        74-96 

0.0005  0.043-0.07     0.00325  1.77     0.0325  150.54 

o.ooi       0.10-0.23  0.004          4-29  0.065       168.12 

0.0016     0.16  0.008        48.43 

Data  are  also  given  for  48  hour  periods  and  for  solutions  containing  Oa. 
One  liter  of  cone.  H  NOs  dissolved  o.  66  gm.  Au  on  boiling  for  two  hours.  (Dewey,  '10.) 
Data  for  the  rate  and  limit  of  solubility  of  Au  in  cone.  HC1  solutions  of  iron 
alum  and  of  cupric  chloride  are  given  by  McCaughey,  1909. 

GOLD   CHLORIDE   (Auric)   AuCl3. 

100  gms.  HaO  dissolve  68  gms.  AuCla. 

When  i  gm.  of  gold  as  chloride  is  dissolved  in  aq.  HC1  of  different  strengths  and 
the  solutions  shaken  with  100  cc.  portions  of  ether,  the  following  percentages  of 
the  gold  enter  the  ethereal  layer.  With  20%  HC1,  95%;  10%  HC1,  98%;  5%  HC1, 
98%;  11%  HC1,  84%  and  0.18%  HC1,  40.3%  of  the  gold. 

Distribution  results,  indicating  considerable  variation  in  the  constitution  of  the 
dissolved  substance  in  the  two  layers,  are  also  given.  (Mylius,  1911.) 

GOLD    PHOSPHORUS    TRI   CHLORIDE    (Aurous)    AuClPCl3. 
100  gms.  PC13  dissolve  i  gram  at  15°,  and  about  12.5  grams  at  120°. 

(Lindet  —  Compt.  rend.  101,  1492,  '85.) 

GOLD  ALKALI  DOUBLE  CHLORIDES. 

SOLUBILITY  OF  SODIUM  GOLD  CHLORIDE,  LITHIUM  GOLD  CHLORIDE, 
POTASSIUM  GOLD  CHLORIDE,  RUBIDIUM  GOLD  CHLORIDE,  AND 
CAESIUM  GOLD  CHLORIDE  IN  WATER. 

(Rosenbladt  —  Ber.  19,  2537,  '86.) 

Grams  Anhydrous  Salt  per  100  Grams  Solution. 

10 
20 
30 

40 

50 
60 

70 
80 
90 

100 

100  gms.  glycerol  (di6  =  1.256)  dissolve  0.21  gm.  AuK(CN)2.5H2O  at  15-16°. 

(Ossendowski,  1907  ) 


NaAuCU. 

LiAuCU. 

KAuCU. 

RbAuCU- 

CsAuCU. 

58.2 

53  -1 

27.7 

4-6 

o-5 

60.2 

57-7 

38.2 

9-0 

0.8 

64.0 

62.5 

48.7 

13-4 

i  .7 

69.4 

67-3 

59-2 

17.7 

3-2 

77-5 

72.0 

70-0 

22.2 

5-4 

90.0 

76.4 

80.2 

26.6 

8.2 

81.0 

3I.O 

12  .O 

85-7 

35-3 

16.3 

39-7 

21-7 

44.2 

27-5 

309  GUAIACOL 

GUAIACOL  C6H4(OH)OCH3(7. 

GUAIACOL  CARBONATE  [C6H4(OCH3)O]2CO. 

SOLUBILITY  IN  WATER,  ALCOHOL,  ETC.   (u.  s.  P.  vra.) 

Cms.  per  100  Cms.  Solvent. 


Solvent.  t°. 


Guaiacol.  Guaiacol  Carbonate. 

Water  25  1.89 

Alcohol  25  ...  2.08 

Chloroform  25  ...  66.6 

Ether  25  ...  7.69 

Glycerol  25  100 

The  coefficient  of  distribution  of  guaiacol  carbonate  between  olive  oil  and  water 

at  25°  is  given  as  Sr  =  3.7  by  Boeseken  and  Waterman,  1911,  1912. 

Freezing-point  lowering  data  (solubility,  see  footnote,  p.  i)  are  given  for  mix- 
tures of  guaiacol  and  a.  naphthylamine  by  Pushin  and  Mazarovic,  1914;  for  mix- 
tures of  guaiacol  and  picric  acid  by  Philip  and  Smith,  1905;  and  for  mixtures  of 
guaiacol  and  salol  by  Bellucci,  1912,  1913. 

a  Tri  PhenylGUANIDINE   CeH.N:C(NHCaHO,. 

SOLUBILITY  IN  MIXTURES  OF  ALCOHOL  AND  WATER  AT  25°.  (HollemanandAntusch,'94.) 

Gms.  Gms. 

Vol.  %     C6H5N:C(NHC6Hfi)2       Density  Vol.  %      C«H5N:C(NHC6H5)2       Density 

Alcohol.  per  100  Gms.  of  Solutions.  Alcohol.          per  100  Gms.          of  Solutions. 

Solvent.  Solvent. 

ioo  6.23  0.8021  80  i.  06  0.8572 

95  3.75  0.8158  75  0.67  0.8704 

90  2.38  0.8309  70  0.48  0.8828 

85  1.58  0.8433  6o  °-22  0.9048 

See  remarks  under  a  Acetnaphthalide,  p.  13. 

Freezing-point  lowering  data  for  mixtures  of  triphenylguanidine  and  triphenyl 
methane  and  for  triphenylguanidine  and  phthalide  are  given  by  Lautz,  1913. 

HEMOGLOBIN. 

ioo  gms.  H2O  dissolve  15.16  gms.  hemoglobin  at  20-25°.  (Dehn,  1917.) 

ioo  gms.  pyridine  dissolve  0.15  gm.  hemoglobin  at  20-25°.  " 

ioo  gms.  aq.  50%  pyridine  dissolve  0.77  gms.  hemoglobin  at  20-25°.        " 

HELIANTHIN  (Methyl  Orange,  Tropaeolin). 

ioo  cc.  H2O  dissolve  0.0055  to  0.0225  gm.  helianthin.  (Dehn,  igiya.) 

ioo  cc.  pyridine  dissolve  0.75  gm.  helianthin.  " 

ioo  cc.  50%  aq.  pyridine  dissolve  62.5  gms.  helianthin.  " 

Results  for  other  solvents  and  observations  on  the  state  of  colored  compounds 
in  solution  are  given. 

HELIUM  He. 

SOLUBILITY  IN  WATER,     (von  Antropoff,  1909-10.) 

t°.  Coef.  of  Absorption. 

o  0.0134 

IO  O.OIOO 
20  0.0138 

30  0.0161 
40  0.0191 
50  0.0226 

The  coef.  of  absorption  adopted  for  the  present  results  is  that  of  Bunsen  as 
modified  by  Kuenen.  The  modification  consists  in  substituting  unit  of  mass  in 
place  of  unit  of  volume  of  water,  in  the  formula. 


HELIUM 


310 


HELIUM    He. 


to 


SOLUBILITY  IN  WATER. 

(Estreicher  —  Z.  physik.  Chem.  31,  184,  '99.) 

Absorption  Coefficient. 


Cor.  Barometic  Vol.  of 
Pressure.       Water. 

Vol.  of 
He. 

fl. 

At  Bar.  Pressure 
Minus  H2O 
Vapor  Tension. 

At  760  mm. 
Pressure. 

o 

.000270 

O 

.0150 

>  764 

.0 

73 

•584 

I 

•093 

O 

.0149 

O 

.0149 

758 

.0 

73 

•578 

I 

.062 

0 

.000260 

0 

.0144 

o 

.0146 

758 

.0 

73 

•597 

I 

.046 

0 

•000255 

0 

.0142 

O 

.0144 

757 

.8 

73 

.641 

I 

.008 

0 

.000246 

o 

.0137 

0 

.0140 

758 

•4 

73 

.707 

0 

.996 

0 

.000242 

0.0135 

O 

.0139 

762 

•3 

73 

•793 

0 

•983 

0 

.000238 

o 

•0133 

o 

.0137 

764 

•4 

73 

.897 

0 

•985 

0 

.000238 

o 

•0133 

o 

.0138 

764 

•5 

74 

.0167 

0 

.972 

0 

.000234 

0 

.0131 

0 

.0138 

762 

.0 

74 

.147 

o 

•957 

o 

.000232 

o 

.0129 

0.0139 

76l 

•7 

74 

.294 

0 

•947 

0 

.000229 

o 

.0127 

o 

.0140 

760 

•9 

74 

.461 

0 

.920 

0 

.000223 

o 

.0124 

0 

.0140 

5 
10 

IS 

20 

25 
30 

35 
40 

45 
5o 
For  q  and  also  absorption  coefficient,  see  Ethane,  p.  285. 

HEPTANE  n  CH3(CH2)5CH3. 

F.-pt.  lowering  data  for  mixtures  of  heptane  and  phenol  are  given  by  (Campett 
and  Delgrosso,  1913). 

HEPTOIC  ACID  CH3(CH2)6COOH. 

100  gms.  H2O  dissolve  0.241  gm.  heptoic  acid  at  15°.  (Lumsden,  1905.) 

HEXAMETHYLENE  (Hexahydrobenzene) .    See  Cyclohexane,  p.  280. 
HEXAMETHYLENE  TETRAMINE    (CH2)6N4. 

100  gms.  H2O  dissolve  81.32  gms.  (CH2)6N4  at  12°.  (Delepine,  1895.) 

ioo  gms.  abs.  alcohol  dissolve  3.22  gms.  (CH2)6N4  at  12°.  " 

IOO  CC.  90%  alcohol  dissolve  12.5  gms.  (CH2)6N4  at  I5-2O0.  (Squire  and  Caines,  1905.) 

T r\ri   ^-»-v-« <-.      /^t-1^1      *r1«si/i^1-«r«~k    Q  ^-w\    ^v, -.-»,.      //~*LT    \    XT      *•»•*-    -r/-»O  /T^.I : _o«^\ 


ioo  gms.  CHC13  dissolve  8.09  gms.  (CH2)6N4  at  12°. 
HEXANE   C6Hi4. 

SOLUBILITY  IN  METHYL  ALCOHOL. 

(Rothmund,  1898.) 

Determined  by  synthetic  method,  see  p.  16. 
t°. 


(Delepine,  1895.) 


Gms.  Hexane  per  100  Gms. 


10 

20 
30 


Alcoholic 
Layer. 

26.5 
31.6 
38.3 


Hexane 
Layer. 

96.8 

95-9 
93-7 


F.-pt.  data  for  hexane  +  phenol. 


Gms.  Hexane  per  ioo  Gms. 

t°-  Alcoholic  Hexane 

Layer.  Layer. 

35  43-6  9i-2 

40  52-7  85.5 

42.6    (crit.  t.)  68.9 

(Campetti  and  Delgrosso,  1913.) 


HIPPURIC  ACID  C6H6CO.NH.CH2COOH. 

SOLUBILITY  IN  SEVERAL  SOLVENTS. 

Solvent 

Water 

Methyl  Alcohol 
Ethyl  Alcohol 
Propyl  Alcohol 
50%  Aqueous  Pyridine 


t°.          C6H5CO.NHCH2COOH                 Authority, 
per  ioo  Gms.  Solvent. 

20-25 

0.42 

(Dehn,  1917.) 

22 

9.80 

(Timofeiew,  1894.) 

22 

5.20 

" 

23 

2.80 

" 

20-25 

88 

(Dehn,  1917.) 

3H  HIPPURIC  ACID 

SOLUBILITY  OF  HIPPURIC  ACID  AT  25°  IN  AQUEOUS  SOLUTIONS  OF: 

Formic  Acid.  (Kendall,  1911.)  Sodium  Hippurate.  (Sidgwick,  1910.) 

Normality      Cms.  Hippuric  Normality  Cms.  Hippuric       Normality  of      Cms.  Hippuric 

of  Aq.  Acid  per  of  Aq.  Acid  per  Aq.  Sodium  Acid  per 

HCOOH.  Liter.  HCOOH.  Liter.  Hippurate.  Liter. 

o  3.67  5  4-08  o  6.Q9(?) 

1.25          3.61  10  4.77  i  13-9700 

2-5  3-72 

HIPPURIC   ACID   C6H6CONH.CH2COOH. 

SOLUBILITY  IN  AQ.  POTASSIUM  HIPPURATE  SOLUTIONS  AT  20*. 

(Hoitsema  —  Z.  physik.  Chem.  27»  3i?t  '98.) 

Density       Gram  Mols.  per  Liter  Sol.                Grams  per  Liter  Solution.  Solid 

of  Solutions.     C9H9N03.    KCgHgNCV             C9H9NO3.   'KC9H8NO3.'  Pnase- 

.002         0.0182      O                                 3-276           0.0  CoHoNO, 

.003       0.0163     o.on  2.919        2.39 

.008    0.0183   0.071         3-278    15.43 

.022      0.0234    0.254  4-191      55-lS 

.114         0-064         1.36  11-47         295.4 

.l82         O.I3I          2.21  23.46         480.1 


192         0.147         2.32  26.32         504.1  iCeHjjNOg-f 

195        0.153         2.40  27.40        52I.4J     C9H^03.KC9H8N03.H»0 


.201  0.133  2.50  23.82  543.1 

.239  0.084  3.01  15.04  654.0 

.282  0.068  3.57  1  2.l8  775-7 

.282  0.065  3.58  II.  60  777-8)     +KC9H8N03 

1.276  0.031  3.56  5.55  773.4  KQtfsNOs 

1.277  o.on       3.55  1.917     771.3 
1.277      o-oo        3-56  •••       773-4 

HOLOCAINE  HYDROCHLORIDE. 

loo  gms.  H2O  dissolve  2  gms.  holocaine  hydrochloride  at  15-20°. 

(Squire  and  Caines,  .1905.) 

HOMATROPINE  HYDROBROMIDE   Ci6H21NO3.HBr. 

SOLUBILITY  IN  WATER,  ETC. 
(U.  s.  P.  vni.) 

loo  gms.  water  dissolve  17.5  gms.  salt  at  25°. 

100  gms.  alcohol  dissolve  3.08  gms.  salt  at  25°,  and  11.5  gms.  at  60°. 

100  gms.  chloroform  dissolve  0.16  gm.  salt  at  25°. 

HYDRASTINE      C21H2iNO6.  HYDRASTININE      HYDROCHLORIDE 

CiiHnNO2.HCl. 

SOLUBILITY  IN  SEVERAL  SOLVENTS. 

(U.  S.  P.  VIII;  at  i8°-22°,  Miiller,  1903.) 

Gms.  C2iH21NO«  per  100  Gms.  Gms.  per  100  Gms.  Solution 

Solvent.  _  Solution.  _  Solvent.  at  i8°-22°. 

'  At  i8°-22°.  At  80°.    '  Q1H21NOI^C11H11N02.HC1. 

Water  0.033  0.025  Ether  0.51      0.078(25°) 

Alcohol  0.74(25°)  5.9(60°)  Ether+H2O  o.8o 

Benzene  8.89  ...  Chloroform  loo-f-     0.35    (25°) 

Ethyl  Acetate      4.05  ...  CCU  0.123  ... 

Petroleum  Ether  0.073 


HYDRAZIDES  312 

HYDRAZIDES. 

SOLUBILITY  OF  THE  TAUTOMERIC  FORMS  OF  HYDRAZIDES  IN  BENZENE  AT  5°. 
Determined  by  the  freezing-point  method.     See  also  p.  487.          (Sidgwick,  1915.) 

Cms.  Compound 

Compound.  Formula.  Dissolved  per 

Liter  Benzene. 

form        5.5 


Phthalylphenylhydrazide  Ce^  <?  ^  >  N.NH.C6H5   !   •„*** 

^  CO  '  )   C  form 


i.i 


/C0\ 


Phthalylphenylmethylhydrazide  Ce^  \  CQ  /  N.N(CH3)C6H6,  A  form     124 

HYDRAZINE  NH2.NH2. 

DISTRIBUTION  OF  HYDRAZINE  BETWEEN  WATER  AND  BENZENE. 

(Georgievics,  1915.) 
Cms.  NH2.NH2  per:  Gms.  NH.NH,  per: 

25  cc.  H2O  Layer.    75  cc.  C6H6  Layer.  25  cc.  H2O  Layer.     75  cc.  C6H6  Layer. 

0.4137  O.O27  1.7601  0.0626 

0.6676  0.0335  2.3336  o.noi 

1.0862  0.0355  4-75  0-J37 

HYDRAZINE  PerCHLORATE  N2H4(HC1O4)2.3H2O. 

SOLUBILITY  IN  WATER.    (Carlson,  1910.) 

,o  Sp.  Gr.  Gms.  N2H4(HC1O4)2 

Sat.  Sol.  per  100  cc.  Sat.  SoL 

18  1.264  41-72 

35  I-3QI  66.9 

HYDRAZINE   MonoNITRATE  N2H4.HNO3. 

SOLUBILITY  IN  WATER.     (Sommer,  1914.) 

Gms.  N2H4HNp3  per  100  Gms.  Gms.  N2H4.HNp3  per  100  Gms. 

' Sat.  Sol.  Water.  Sat.  Sol.  Water. 

10  63.63  174.9  40.02  85.86  607.2 

15  68.47  217.2  45-02  88.06  737-6 

20.01  72.70  266.3  5°-01  91.18  1034 

25.01  76.61  327.5  55.01  93.58  1458 

30.01  80.09  402.2  60.02  95.51  2127 

35.01  83.06  490.3 

HYDRAZINE  SULFATE  N2H4.H2SO4. 

loo  grams  water  dissolve  3.055  gms.  N2H4.H2SO4  at  22°.      (Curtius  and  Jay,  1889.) 

Phenyl  HYDRAZINE  and  other  substituted  hydrazines.     See  page  486. 

HYDRIODIC  ACID  HI. 

SOLUBILITY  IN  WATER,  DETERMINED  BY  FREEZING-POINT  METHOD. 

(Pickering,  i893a.) 

Gm.  HI  Gms.  HI 

t°.          per  100  Gms.     Solid  Phase.                                   t°.  per  100  Gms.     Solid  Phase. 

Sat.  Sol.  Sat.  Sol. 

—  IO  20.3       Ice  —60  52.6      HI.4H2O 

-20         29.3      "  -40  59 

-30         35.1      «  about-35.5m.pt.      64 

-40         39          «  -40  65.5 

—  50  42  "  —49  66.3  +HI.3H2O 

—  60         44.4      "  —48m.pt.          70.3     Hi.3H2o 

-70  46.2         "  -56  73.5  "  +HI.2H20 

—  80  47.9         "    +HI.4H2O  —52  74  HI2H2O 

F.-pt.  data  for  HI  +  H2S  (Bagster,  191 1),  HI  +  (CH3)2O.  (MaassandMclntosh,  1912.) 


HYDROBROMIC  ACID 


HYDROBROMIO    ACID    HBr. 

SOLUBILITY  IN  WATER. 

(Roozeboom  —  Z.  physik.  Chem.  2,  454,  '88;  Rec.  trav.  chim.  4,  107,  '85;  5.  358,  '86;  see  also  Pickering 
—  Phil.  Mag.  [5]  36,  119,  '93.) 


Gms.HBr  Dissolved(at  760-765111111.) 
per  100  Gms. 


Water. 

Solution. 

255-0 

7I-83 

239.0 

70.50 

221  .2 

68.85 

6II.6 

210-3 

67.76 

581.4 

2O4.O 

67.10 

193.0 

65.88 

532-1 

171  .5 

63.16 

468.6 

I50-5 

60.08 

406.7 

130.0 

56.52 

344-6 

Gms.  HBr  Dissolved  at 

Lower  Pressures  per  100 

Gms.  H2O. 

175.0  (10  mm.) 


-  2.5 

-15 

o 

+  10    210.3    67.76     581.4     108 . 5  (5  mm.) 
15 
25 
50 

75 
100 

For  0  see  ethane,  p.  285. 

F.-pt.  data  for  HBr  +  H2S  (Bagster,  1911);  HBr  +  (CH3)2O,  HBr  +  CH3OH, 
HBr  +  CzHsOH,  HBr  +  CH3COOC2H6  and  HBr  +  C6H6CH3. 

(Maass  and  Mclntosh,  1912.)     (Reid  and  Mclntosh,  1916.) 

HYDROCHLORIC  ACID  HC1. 

SOLUBILITY  IN  WATER  BY  THE  FREEZING-POINT  METHOD. 

(Composite  curve  from  results  of  Roloff,  1895;  Pickering,  1893 (a);  Roozeboom, 
1884,  1889  and  Rupert,  1909.) 


Gms.  HC1 
t°.              per  loo  Gms 

Solid  Phase.                      t°. 

Gms.  HC1 
per  loo  Gms.    Solid  Phase. 

Sat 

Sol. 

Sat.  Sol. 

—  I  .  706 

I 

.66 

Ice 

— 

18 

•4 

48.6 

HC1.2H,O 

-14.97 

10 

.02 

" 

— 

17 

.7m. 

Pt. 

50.3 

" 

-28.84 

14 

•5i 

• 

— 

18 

•7 

52.85 

" 

-40 

17 

.40 

" 

— 

19 

•4 

54-i 

M 

-60 

21 

•30 

" 

— 

20 

.8 

55-7 

« 

-80 

24 

.20 

" 

— 

21 

•  3 

56.5 

« 

-86Eutec. 

24 

.8 

"    +HC1.3H20       — 

23 

.2 

57-3 

« 

—  50 

30 

.1 

HC1.3H20 

— 

23 

-5Eutec. 

" 

+HC1.H20 

-40 

32 

•7 

M 

— 

21 

•5 

58^2 

HC1.H,O 

-30 

36 

•5 

« 

— 

20 

•7 

59.1 

• 

—  24.9m.pt. 

40 

•3 

" 

— 

18 

•4 

61.1 

" 

-27-5 

44 

"  +HC1 

.aH2O 

— 

17 

•4 

62.4 

" 

-23.8 

45 

•7 

HC1.2H20          — 

15 

-4 

65-4 

'« 

—  21.2 

45 

•9 

" 

— 

15 

•35 

66.8 

" 

At  about  —15.35 

two  liquid  layers  are  formed.     Data  for  these  are 

as  follows: 

HC1  layer. 

H2O 

layer. 

t°of 
Saturation 

Gms.  H2O                    Gms.  HC1 
per  100  Gms.    t°.       per  100  Gms. 
Sat.  Sol.                        Sat.  Sol. 

d.  of  Sat.  Sol.     t°. 

Gms.  HC1 
per  100  Gms. 
Sat.  Sol. 

d.  of  Sat.  Sol. 

Below  —50 

O 

.008 

—  2O 

67. 

65 

•  279 

IS 

64 

70 

.231 

"     -50 

o 

.017 

~~I5 

67. 

29 

.269 

20 

64 

19 

.228 

Bet.  -15  and  o° 

o 

.077 

—  10 

66. 

.260 

30 

63.21 

.229 

Above  45 

0 

.021 

-5 

66. 

44 

•  255 

35 

62 

00 

.227 

" 

0 

.052 

0 

65- 

85 

.247 

40 

62 

27 

.218 

" 

0 

.11 

+5 

65- 

48 

.245 

45 

61.76 

.212 

" 

0 

•13 

10 

65- 

18 

.240 

So 

61 

65 

.2IQ 

For  additional  data  on  this  system  see  Baume  and  Tykociner,  1914. 


HYDROCHLORIC  ACID  314 

HYDROCHLORIC    ACID    HC1. 

SOLUBILITY  IN   WATER  AT  DIFFERENT  TEMPERATURES  AND 
PRESSURES. 


o 
8 

12 
14 

18 
23 
30 
40 

f 
60 


ioscoe  and  Dittmar  —  Liebig's  Ann.  112,  334,  '59;  betow  o°,  Roozeboom-  —  Rec.  trav. 
chim.  3,  104,  '84.) 

At  Different  Temperatures  and  760  mm.  Pressure.          At  Different  Pressures  and  o° 

_A                                                                                                                                                                                                                JL                                                     — 

cc.  HClper 
ioocc.H2O. 

Density.      ' 

^SoF 

r  Gms.  HC1  per 
100  g.  H2O. 

Pressures.* 

Gms.  HC1  per 
100  g.  H2O 

525-2 

1.2257 

45  •I5 

82.31 

60 

61-3 

497  7 

I  .2265 

44-36 

79  73 

100 

65-7 

480.3 

1.2185 

43  83 

78.03 

150 

68.6 

47J-3 

I.2I48 

43-28 

76.30 

200 

70.7 

462  4 

1.2074 

42.83 

74-92 

300 

73-8 

451.2 

I  .  2064 

42-34 

73-4i 

4OO 

76.3 

435-o 

I.20I4 

41  .54 

71.03 

500 

78.2 

40.23 

67-3 

600 

80.0 

38.68 

63-3 

750 

82.4 

.  .  . 

.  .  . 

37-34 

59-6 

IOOO 

85.6 

... 

35-94 

56-1 

1300 

89-5 

*  Pressures  in  mm.  Hg  minus  tension  of  H2O  vapor. 


SOLUBILITY  IN  WATER  AT  TEMPERATURES  BELOW  o". 

At  a  pressure  of  760  mm.  At  pressures  below  and  above  760  mm. 

t°.  q.  t°.  q.  t°.         mm.  Pressure.        q. 

-24  IOI.2      -15      93.3  -23.8  ...  84.2 

—  21        98.3       —io    89.8  —2i  334        86.8 

—  18.3    96          —  5    86.8  —19  580        92.6 
— 18        95.7            o    84.2              — 18            900        98.4 

-17.7      1073      101.4 

For  definition  of  q,  see  Ethane,  p.  285. 

The  eutectic  is  at  —86°  and  33  gms.  HC1  per  100  gms.  H2O. 


SOLUBILITY  OF  HYDROCHLORIC  ACID  GAS  IN  METHYL  ALCOHOL,  ETHYL 
ALCOHOL,  AND  JN  ETHER  AT  760  MM.  PRESSURE. 

(dc  Bruya— Rec.  tray.  chim.  u,  129,  '92;  Schuncke  —  Z.  physik.  Chem.  14*  336.  *94-) 
Grams  HC1  gas  per  100  Grams  Solution  in: 


CH3OH.  C2H6OH.  (C2H6)2O. 

-10  54-6  ...  37-5I(-9-2°) 

-  5 
o 

+  5 
io 

'5 

30 
25 
30 


5I-3 

45-4 

35-6 

44.2(6.5°) 

42.7(11-5°) 

30.35 

27  .62 

47-o(i8°) 

41.0 

24.9 

40.2  (23.5°) 

22.18 

43-o(3i.7°) 

38-1(32°) 

19.47 

315  HYDROCHLORIC  ACID 

SOLUBILITY  OF  HYDROCHLORIC  ACID  GAS  IN  AQ.  SULFURIC  ACID  SOLUTIONS. 

(Coppadoro,  1909.) 


Results  at  17°. 

Gms.  per  100  Cms. 
1  of  Sat.                 Sat.  Sol. 

Results  at  40°. 

Gms.  per  100  Gms. 
d  ol  Sat.              Sat.>l. 

Results  at  70°. 

,    ,  _          Gms.  per  100  Gms. 
d  °cL?at'               Sat:  S01- 

Sol. 

H,S04. 

HCl.  ' 

oOl. 

H2S04. 

HCl.  ' 

SoL 

H2SO4.- 

HCl.' 

.211 

0 

42.7 

1.185 

3 

-56 

35-6 

1.145 

I 

.61 

32.7 

.220 

I. 

86 

39-9 

i-i95 

5 

.86 

34-8 

1.150 

3 

-38 

3I-I 

.220 

4- 

75 

39-2 

I.  210 

8 

.90 

32-4 

1.160 

4 

.80 

30-5 

•235 

8. 

04 

36-9 

1-255 

16 

.80 

27.6 

1.180 

7 

•93 

28.9 

.260 

12. 

80 

33-2 

1-255 

18 

.8 

25-9 

1.225 

18 

•9 

22.8 

•305 

2O. 

9 

28.5 

1.340 

28 

.6 

18.5 

1.230 

20 

22-3 

•355 

30. 

8 

22.6 

I  .400 

44 

.2 

"•5 

1.315 

36 

.2 

13-2 

•430 

44- 

6 

15 

1.520 

61 

.1 

3-35 

1.380 

48 

6.99 

•545 

59- 

4 

6.26 

1-575 

66 

•4 

1.17 

1.510 

62 

•7 

1.56 

.580 

65- 

4 

3-25 

1.650 

73 

.2 

0.17 

1.560 

67 

.6 

0-54 

i.  660 

73- 

7 

0.62 

1-725 

79 

•4 

0.081 

1.700 

80 

•7 

0.05 

1-735 

77- 

5 

O.II 

i-755 

81 

•4 

0.032 

1-745 

83 

0-035 

1.815 

89 

0.068 

1.770 

83 

•5 

0.029 

1-745 

83 

-4 

0.032 

Phenol  Rich  Layer. 

^ 

%  HCl.        %  Phenol". 

o              72 

0.09            78 

0.2          80  .  3 
0.36       82.6 
0.52      84.5 

%  Water. 
11.22 

84.5 
80.38 

72.43 
60.25 

%  HCl.      %  Phenol. 

o          88.78 

IO.7           4.8 
15.64        3.98 
24-37         3-2 

36-25      3-5 

MISCIBILITY  OF  HYDROCHLORIC  ACID  WITH  MIXTURES  OF  WATER  AND 
PHENOL  AT  12°. 

(Schreinemakers  and  van  der  Horn  van  der  Bos,  1912.) 

Composition  of  the  Reciprocally  Composition  of  the  Solutions  in 

Saturated  Liquid  Pairs.  Contact  with  Solid  Phenol. 

Water  Rich  Layer. 
%HC1.    '  %  Phenol 

o  7-45 

3.1  6.6 

6.6  5-3 

8  5-1 

10.7  4.8 

Additional  data  for  this  system  are  given  by  Krug  and  Cameron,  1900. 

FREEZING-POINT  DATA  (Solubility,  see  footnote,  p.  i)  FOR  MIXTURES  OF 
HYDROCHLORIC  ACID  AND  OTHER  COMPOUNDS. 

Hydrochloric  Acid  +  Hydrogen  Sulfide  (Baume  and  Georgitses.  1912, 1914.) 

11  i    A/Toi-t,,,!   Al~~t,~|   f   (Baume  and  Borowski,  1914;   Baume  and  Pamfil, 

-  Methyl  Alcohol  {       igil   I9u;  Maass  and  Mclntosh,  1913-) 

+  Methyl  Chloride  (Baume  and  Tykociner,  1914.) 

+  Methyl  Ether  (Maass  and  Mclntosh,  1912;  Baume,  1911, 19x4.) 

+  Propionic  Acid  (Baume  and  Georgitses,  1912,  1914.) 

-j-  Sulfur  Dioxide  (Baume  and  Pamfil,  1911, 1914.) 

HYDROCYANIC  ACID  HCN. 

DISTRIBUTION  BETWEEN  WATER  AND  BENZENE. 

(Hantzsch  and  Sebalt,  1899;  Hantzsch  and  Vagt,  1901.) 

t.  Mol.  HCN  per  Liter;  c  Mol.  HCN  per  Liter:  c 

H2O  Layer  (c).   CeH6  Layer  (c').       7''  '     H2O  Layer  (c) .  CgR*  Layer  (cO-~        ?' 

6     0.00625      0.00325     1.923          7      0.0574        0.0148      3.88 
16     0.00593      0.00363     1-634        20      0.0572        0.0154      3.72 
25     0.00580      0.00375     1.547 
Data  for  the  effect  of  HCl  and  of  KC1  on  the  distribution  are  also  given. 

HYDROFLUORIC  ACID   HF. 

100  grams  H2O  dissolve  in  grams  HF  at  —35°.  (Metzner.  1894.) 


HYDROGEN  316 

HYDROGEN  H.  SOLUBILITY  IN  WATER. 

(Winkler  —  Ber.  24,  99,  'gx;  Bohr  and  Bock  —  Wied.  Ann.  44,  318,  '91;  Timofejew  —  Z.  physik. 

Chem.  6,  147,  oo.) 

t°.  ft'.  _  /.  _  ft.  q. 

a  0.0214  ...      ...  0.0214  0.000193 

5  0.0203  0.0209  —  0.0241  0.0204  0.000184 

10  0.0193  0.0204  —  0.0229  0.0195  0.000176 

15  0.0185  0.0200  —  0.0217  0.0188  0.000169 

20    0.0178   0.0196  -  0.0205     0.0182     0.000162 

25      0.0171    0.0193  —  0.0191  0.0175        0.000156 

30      0.0163        ...              ...  0.0170       0.000147 

40      0.0153       ...              ...  0.0164       0.000139 

50      0.0141        ...               ...  0.0161        0.000129 

60      0.0129        ...               ...  0.0160        0.000119 

80      0.0085        ...               ...  0.0160        0.000079 

100      o.oooo        ...               ...  0.0160        o.oooooo 

I  =  Ostwald  Solubility  Expression,  see  p.  227.  For  0',  /3,  and  q,  see  Ethane,  p.  285. 

Data  for  the  solubility  of  hydrogen  in  water  at  pressures  up  to  I  o  atmospheres 
are  given  by  Cassuto,  1913. 

SOLUBILITY  OP  HYDROGEN  IN  AQUEOUS  SOLUTIONS  OF  ACIDS  AND 

BASES  AT  25°. 

(Geffcken  —  Z.  physik.  Chem.  49,  268,  '04.) 


_  Solubility  of  H  (/a  =  Ostwald  Expression)  in  Solutions  of; 


peter.        HCL  HN°3'        *H2SO4.  CHaCOOH.  CH2C1COOH.    KOH.        NaOH. 

o.o  0.0193  0.0193  0.0193  0.0193  0.0193  0.0193  0.0193 

0.5  0.0186  0.0188  0.0185  0.0192  0.0189  0.0167  0.0165 

i.p  0.0179  0.0183  0.0177  0.0191  0.0186  0.0142  0.0139 

2.0  0.0168  0.0174  0.0163  0-0188  0.0180       ...  0.0097 

3.0  0.0159  0.0167  0.0150  0.0186       ...           ...  0-0072 

4.0       ...  0.0160  0.0141  0.0186       ,..           ...  0.0055 

The  above  figures  for  the  concentrations  of  acids  and  bases  were  calculated  to 
grams  per  liter,  and  these  values  with  the  corresponding  1&  values  for  the  solubility 
of  hydrogen,  plotted  on  cross-section  paper.  From  the  resulting  curves,  the  follow- 
ing table  was  read  : 


Grams  Acids 
and  Bases 
per  Liter. 

0 
20 

40 

00 

80 

100 

150 

2OO 
250 

Solubility  of  H  (/25  = 

Ostwald  Expression)  in  Solutions  of: 

0 
0 
O 
0 
O 
O 

HCL 
.0193 
.0185 
.0179 
.0173 
.0167 
•  Ol6o 

HNO3. 
0.0193 
0.0189 

0.0186 
0.0183 
0.0180 
0.0179 
0.0171 
0.0165 
0.0160 

*H2S04. 

0.0193 

0.0186 
0.0180 
0.0174 
0.0168 
0.0162 
0.0148 
0.0140 

CH3COOH. 
0.0193 
0-0192 
O.Oigi 
0.0190 
0.0189 
0.0189 
0.0188 

0.0186 
0.0184 

CH2C1COOH 
0.0193 
0.0191 
O.OI9O 

o.o  i  88 
0.0187 
0.0185 
0.0182 
0.0179 

0 
0 

o 

0 

KOH. 
.0193 
.OI72 

•0135 

NaOH. 
0.0193 
0.0165 
O.OI4O 
O.OII7 
0.0097 
0.0082 
0,0058 

For  Ostwald  Solubility  Expression  /,  see  p.  227. 

THE  SOLUBILITY  OF  HYDROGEN  IN  CONC.  H2SO<  AT  20°. 

(Christoff,  1906.) 

%H2S04       o  35.82  61.62  95.6 

4o  0.0208        0.00954        0.00708        0.01097 


317 


HYDROGEN 


SOLUBILITY  OF  HYDROGEN  IN  AQUEOUS  SOLUTIONS  OF  AMMONIUM 

NITRATE  AT  20°. 

(Knopp —  Z.  physik.  Chem.  48,  103,  '04.) 


*' 

Normality 
(per  1000  Gins.' 
H20. 

Molecular 
Concentra- 
tion. 

Absorption 
Coefficient 
of  Hydrogen. 

Density 
•A  Solutions. 

o.oo 

O-OO 

o.oo 

0.0188 

1.037 

0.1308 

0.002352 

0.01872 

.0027 

2.167 

0.2765 

0.004956 

0.01845 

.0072 

3-378 

0.4363 

0.007799 

0.01823 

•  OI22 

4.823 

0.6333 

O.OII280 

0.01773 

.0182 

6.773 

0.9069 

0.016447 

0.01744 

.0262 

/  /  v/ 

"•550 

1.6308 

0.028525 

0-01647 

.04652 

SOLUBILITY    OF    HYDROGEN    IN    AQUEOUS    SOLUTIONS    OF    BARIUM 

CHLORIDE. 

(Braun  —  Z.  physik.  Chem.  33,  735,  'oo.) 


Gms.BaClu 
per  100  Gms. 
Solution. 

o.oo 

3-29 

3-6 

6-45 
7.00 

Coefficient  of  Absorption  of  Hydrogen  at  : 

5°. 
0.0237 

0.02II 
O.O2O9 
0-0196 
0.0194 

10°. 

0-0221 
0.0198 
0.0197 

0.0186 
0.0183 

15°. 
0.0206 

0.0l85 
O.Ol84 
0.0173 
0.0172 

20°. 
O.OI9I 
0.0172 
O.OI7O 

0.0161 
0.0159 

2S°- 

0.0175 
0-0157 
0.0156 
0.0147 
0.0146 

SOLUBILITY  OF  HYDROGEN  IN  AQUEOUS  SOLUTIONS  OF  CALCIUM  CHLOR- 
IDE, MAGNESIUM  SULPHATE,  AND  LITHIUM  CHLORIDE  AT  15°. 

(Gordon  —  Z.  physik.  Chem.  18,  14,  '95.) 

Coefficient  of  Absorption  of  hydrogen  in  water  at  15°  =  0.01883. 
In  Calcium  In  Magnesium  In  Lithium 


Chloride. 


Sulphate. 


Chloride. 


Gms. 
CaCl2 

G.M. 
CaCl2 

Absorption 
Coefficient 

Gms. 
MgSO4 

G.M. 
MgSO4 

Absorption 
Coefficient 

Gms. 
LiCl 

G.M. 
LiCl 

Absorption 
Coefficient 

per 
too  g.  Sol 

per 
.    Liter. 

of  H. 

per 
100  g.  Sol. 

per 
Liter. 

of  H. 

per 
100  g.  Sol. 

Ltter. 

of  H. 

3-47 

0. 

32I 

0. 

01619 

4- 

97 

0-433 

O.OI5OI 

3-48 

0.835 

0.01619 

6.10 

0. 

578 

0. 

01450 

10. 

19 

0.936 

0.01159 

7-34 

1.800 

0.01370 

"•33 

I. 

122 

0. 

01138 

23- 

76 

2.501 

0.00499 

14.63 

3-734 

0.0099 

17-52 

I. 

1827 

0. 

00839 

26.34 

2. 

962 

0. 

00519 

For  definition  of  Coefficient  of  Absorption,  see  page  227, 


SOLUBILITY   OF   HYDROGEN   IN  AQUEOUS   SOLUTIONS   OF   POTASSIUM 
CARBONATE,  CHLORIDE,  AND  NITRATE  AT  15°. 

(Gordon.) 

In  Potassium                  In  Potassium                   In  Potassium 
Carbonate.                          Chloride.                            Nitrate. 

Gms. 
K2C03 
per 
100  g.  Sol. 

2.82 
8.83 
16.47 

24.13 
4I.8l 

G.M. 
K-jCOa 
per 
Liter. 

0.209 
0.690 
1.376 
2.156 
4.352 

Absorption 
Coefficient 
of  H. 

0.01628 
0.01183 
0.00761 
0.00462 
0.00l6o 

Gms. 
KC1 
per 
100  g.  Sol. 

3.83 
7.48 
12.13 
19.21 
22.92 

G.M. 
KC1 
per 
Liter. 

0.526 
1.051 

1-755 
2.909 

3-554 

Absorption 
Coefficient 
of  H. 

0.01667 
0.01489 
0.01279 
O.OIOI2 
0.00892 

Gms. 
KNO3 
per 
100  g.  Sol. 

4-73 
8.44 
16.59 
21.46 

G.  M. 
KNO3 

Liter. 
0.482 
0.879 
1.820 
2.430 

Absorption 
Coefficient 
of  H. 

0.01683 
0.01559 
0.01311 
O.OIlSo 

HYDROGEN 


318 


SOLUBILITY  OP   HYDROGEN   IN  AQUEOUS   SOLUTIONS   OP   POTASSIUM 
CHLORIDE  AND  NITRATE  AT  20°. 

(Knopp  —  Z.  physik.  Chem.  48,  103,  '04.) 


In  Potassium  Chloride. 

In 

Potassium  Nitrate. 

P> 

Normality 
(per  1000 
g.H20). 

Absorption 
Coefficient. 

Density 
of 
Solutions. 

P- 

Normality 
(per  looo 
g.H20). 

Absorption         &*&? 

Coefficient.       c  .  °? 
Solutions. 

1.089 

0.1475 

o 

.01823 

I 

.0052 

I 

.224 

0 

.1245 

0.01835 

.0059 

2.123 

0.2907 

0 

•01757 

I 

.OIl8 

2 

.094 

O 

.2114 

o.  01818 

.0113 

4.070 

0.5687 

0 

.01661 

I 

.0243 

4 

.010 

0 

.4127 

0.01785 

.0236 

6-375 

0.9127 

o 

•01531 

I 

•0394 

5 

•925 

0 

.6225 

0.01743 

•0359 

7.380 

1.0682 

0 

.01472 

I 

.0460 

7 

.742 

o 

.8293 

0.01667 

.0477 

13.612 

2.1222 

0 

•01255 

I 

.0875 

13 

.510 

I 

•5436 

0.01436 

.0865 

SOLUBILITY   OP   HYDROGEN   IN   AQUEOUS   SOPIUM   CARBONATE   AND 
SULPHATE  SOLUTIONS  AT  15°. 

(Gordon.) 


In  Sodium  Carbonate. 

Gms.  NazCOa      G.M.  Absorption 

per  loo  Gms.      Na2CO»  Coefficient 

Solution.        per  Liter.  of  H. 

2.15     0.207  0.01639 

8.64     0.438  0.01385 

11.53        1.218  0.00839 


In  Sodium  Sulphate. 

Gms.  Na2SO4  G.  M.  Absorption 

per  loo  Gms.  Na2SO4  Coefficient 

Solution.  per  Liter.  of  H. 

4-58  o-335  0.01519 

8.42  0.638  0.0154 

16.69  I-364  0.00775 


SOLUBILITY  OP  HYDROGEN  IN  AQUEOUS  SOLUTIONS  OP  SODIUM 

CHLORIDE. 

(Braun;  Gordon.) 


Gms.NaCl 
per  ioo  Gms. 
Solution 
1.25 
3-80     . 
4.48 

6.00 
14-78 
23.84 

Coefficient  of  Absorption  of  Hydrogen  at: 

5°. 

0.0218 
0.0198 
0.0192 
0.0184 

10°. 

O.O2O5 

0.0188 
0.0182 
0.0175 

15°. 
O.OI9I 
0.0176 
O.OI7I 
O.Ol64 
0.0093 
0.00595 

20°. 
0.0177 
0.0162 
0.0159 
0.0153 

25°. 

0.0162 
0.0148 

0.0143 
0.0138 

SOLUBILITY  OP  HYDROGEN  IN  AQUEOUS  SOLUTIONS  OP  SODIUM 

NITRATE. 
In  Sodium  Nitrate  at  20°.  In  Sodium  Nitrate  at  15°. 

(Knopp.)  (Gordon.) 


Normality 

Absorption 

Density 

Gms.  NaNO3 

G.M. 

Absorption 

p. 

(per  1000 
Gms.  H20). 

Coefficient 
of  H. 

of 
Solutions. 

per  TOO  Gms. 
Solution. 

NaNOa 
per  Liter. 

Coefficient 
of  H. 

1.041 

0.1236 

0.01839 

I  .0052 

5-57 

0.679 

0.01603 

2.192 

0.2634 

0.01774 

I.OI30 

ii  .16 

I-4I3 

0.0137 

4-405 

0.5416 

0.01694 

1.0282 

19.77 

2.656 

0.01052 

6.702 

o  .  8442 

O.OI5I8 

I  .04411 

37-43 

5-7II 

0.00578 

12.637 

J-7354 

0.0130 

I  .08667 

319  HYDROGEN 

SOLUBILITY  OF  HYDROGEN  IN  AQUEOUS  SOLUTIONS  OF  VARIOUS  SALTS  AT  15°. 

(Steiner,  1894.) 

Salt  in  Aq  Bunsen  Absorption  Coefficient  0  (Xio4)  in  Aq.  Solution  of  Normality. 

Solution. 

LiCl 
KNO3 


KC1 
NaNO3 


NaCl 
iMgS04 
|ZnSO4 
iNa2SO4 


0. 

I. 

2. 

3- 

4- 

5- 

6.     7-      9- 

1883 

1^74 

132^ 

II2I 

040 

1883 

1^24 

1276 

IO76 

1883 

1221 

QQ3 

810 

667 

--0 

1883 

I  f)O2 

1217 

006 

820 

1883 

I4O6 

I2OI 

984 

808 

667 

^42 

1883 

140? 

line 

0^8 

780 

trio 

1883 

I478 

1144 

880 

699 

573 

1883 

1451 

II2O 

856 

659 

499 

...   ...   ... 

1883 

1446 

III3 

852 

667 



1883 

I37O 

001 

7IO 

*-3  /  w 

yvyj. 

/  xv 

1883 

1338 

967 

700 

508 

372 

273   206   158 

1883 

I7AO 

6OO 

1883 

1280 

731 

|Na2CO3 

Cane  Sugar 
SOLUBILITY  OF  HYDROGEN  IN  ALCOHOL.     (Timofeiew,  1890;  Bunsen-Heurich,  1892.) 

Coef.  of  Absorp-  Coef.  of  Absorp-  Coef.  of  Absorption 

t°.  tion  in  98.8%  t°.  tion  in  7%  t°.  in  Pure  Alcohol 

'     Alcohol.  Alcohol.  (Bunsen). 

o  0.0676  4  0.0749  i  0.06916 
6.2  0.0693  18.8  0.0740  5  0.06847 

.13.4  0.0705  11.4  0.06765 

23.7  0.06633 

SOLUBILITY  IN  AQUEOUS  ALCOHOL  SOLUTIONS  AT  20°  AND  760  MM.  PRESSURE. 

(Lubarsch,  1889.) 
Wt.  %  Alcohol.  Vol.  %  Absorbed  H.         Wt.  %  Alcohol.        '.Vol.  %  Absorbed  H. 

o  1.93  28.57  1.04 

9-09  i-43  33-33  i-i7 

16.67  I-29  50  2.02 

23.08  I.I7  66.67  2.55 

SOLUBILITY  OF  HYDROGEN  IN  AQ.  SOLUTIONS  OF  CHLORAL  HYDRATE. 

(Miiller,  C.  1912-13.) 
Cms.  Chloral  Absorption  Coefficient. 

j.o  Hydrate   per  d^  of  Aq.  , * \ 

100  Gms.  Aq.  Solution.  ft.  fto. 

Sol. 

19.4  15-5  1.0722  0.01732  0.01724 

17.4  28.3  I.I43  0.01569  0.01540 
18.7  46.56  1.2505  0.01388  0.01375 

16.5  52  1.2870  0.01314  O.OI28O 
17  63  I-37I  0.01270  0.01243 

17.9  68  1.4097  0.01286  0.01270 

18.3  78.4  1-4993  0.01398  0.01380 

SOLUBILITY  OF  HYDROGEN  IN  CHLORAL  HYDRATE  SOLUTIONS  AT  20°.  (Knopp,  1904.) 

A  Normality  (per  Molecular  Absorption  Density 

1000  Gms.  H2O).          Concentration.  Coefficient  of  H.  of  Solutions. 

4.91  0.310  0.005594  0.01839  1.0202 

7.69  0.504  0.008992  0.01802  1.0320 

14.56  I.O3O  O.OI8223  O.OI7I2  1.0669 

29.50  2.530  0.043601  0.01542  I.I466 

38.42  3-770  0.063647  0.01440  1.1982 

49-79  6  0.097493  0.01353  1.2724 

63.90  10.700  o. 161660  0.01307  1.3743 

For  definition  of  Bunsen  Absorption  Coef.,  see  p.  227. 


HYDROGEN 


320 


SOLUBILITY  OF  HYDROGEN  IN  AQUEOUS  SOLUTIONS  OF  GLYCEROL. 

Results  at  14°  and  21°.  (Henkel,  1905,  1912.)         Results  at  25°.    (Drucker  and  Moles,  1910.) 


Wt.  % 

Absorp.  Coef. 

t  . 

Glycerol. 

0  (See  p.  227-) 

14 

O 

0.0193 

M 

2.29 

0.0189 

u 

5-32 

0.0186 

u 

8-57 

0.0182 

ft 

10.83 

0.01815 

u 

15-31 

0.01765 

21 

0 

0.0184 

« 

2.29 

0.0181 

It 

5.68 

0.0177 

11 

6.46 

0.0176 

11 

10.40 

0.0171 

u 

18.20 

0.0160 

Wt.  % 
Glycerol. 

%  Sat.  Sol. 

/zs  (Ostwald 
Expression)  . 

0 

I 

0.0196 

4 

I.OIOI 

0.0186 

10.5 

1.0260 

O.OI78 

22 

1.0542 

0.0154 

49-8 

1.1290 

o  .  0099 

50-5 

1.1300 

0.0097 

52-6 

1-1365 

o  .  0090 

67 

1.1752 

0.0067 

80 

1.2113 

0.0051 

82 

1.2159 

0.0051 

88 

1.2307 

o  .  0044 

95 

1.2502 

0.0034 

Aqueous  Solution  of: 

.  Water  alone 
Dextrose  (Grape  Sugar) 


Additional  data  for  this  system  are  given  by  Miiller,  C.  1912-13. 
SOLUBILITY  OF  HYDROGEN  IN  AQUEOUS  SOLUTIONS  OF  SEVERAL  COMPOUNDS. 

(Hiifner,  1906-07.) 
Cone,  of 
Solvent  Gms. 
per  Liter. 

O 

41-45 
87-3 
174 
60 

59 
89 

75 

SOLUBILITY  OF  HYDROGEN  IN  AQUEOUS  SOLUTIONS  OF  CANE  SUGAR  AND 
OF  GRAPE  SUGAR.     (Mulier,  c.  1912-13.) 


Urea 

Acetamide 
Alanine 
Glycocol 


t. 

Absorption  Coef.  0. 

20.  1  1 

O.OlSl 

20 
20.25 
20.28 

0.0176 

0.0166 
0.0152 

20.17 
20.11 

0.0170 
0.0180 

20.08 
20.  l6 

0.0156 
0.0158 

Wt.  % 
Cane 
Sugar. 

Sp.  Gr. 
Sat.  Sol. 

Abs.  Coef.            to 

015- 

Wt.  % 
Grape 
Sugar. 

Sp.  Gr. 
Sat.  Sol. 

Abs.  Coef. 

5-04 

di5    =1 

.019 

O 

.0173 

19 

3 

0 

0.0184 

14-7 

du  =i 

.060 

O 

.0151 

20 

5 

12 

,2 

^20=1 

.048 

0.0160 

20.26 

du  =  i 

.084 

0 

.0146 

20 

•5 

2O 

•7 

d%Q  =  I 

.084 

0.0145 

29.86 

di3  =  i 

.128 

0 

.0126 

21 

.1 

32 

•56 

^20=  I 

.130 

0.0125 

31-74 

dn  =i 

.138 

o 

.0119 

21  , 

,8 

45 

8 

^20=1 

.199 

O.OIO2 

39.65 

</i.3.5=  i 

•  175 

0 

.0103 

21 

,2 

59 

^0=1 

.266 

0.0078 

42.94 

^12-5=  I 

•  195 

0 

.0094 

15-2 

ii. 6 

12 
12.7 

ii. 8 
13-3 

12.6 

SOLUBILITY  OF  HYDROGEN  IN  AQUEOUS  SUGAR  SOLUTIONS  AT  15°.  (Gordon,  1895.) 

Gms.  Sugar  per  Gm.  Mols.  Sugar  Absorption 

100  Gms.  Solution.  per  Liter.  Coefficient  of  H. 

16.67  °-52o  0.01561 

30.08  °-993  0.01284 

47.65  1.699  0.00892 

SOLUBILITY  OF  HYDROGEN  AT  25°  (Findlay  and  Shen,  1912)  IN  AQ.  SOLUTIONS  OF: 


Dextrin. 

Starch. 

Gelatin. 

<ms.  Dextrir 
per  100  cc. 

1     Sp.  Gr. 

1* 

Gms 
per 

Starch     cn  r>~ 
100  cc.      Sp'  Gr" 

i             Gms. 
'**•            per 

Gelatin         , 

100  CC. 

3-98 

1.  012 

0 

.0194 

2 

.OI 

I 

.005 

0.0194 

I 

•53 

0.0194 

8.58 

I.Oig 

0 

.0191 

3 

-56 

I 

.Oil 

0.0189 

2 

.69 

0.0189 

8.12 

1.028 

0 

.0188 

7 

•13 

i 

.024 

O.OlSl 

4 

•74 

0.0185 

19.20 

1.066 

0 

.0174 

9 

.29 

I 

.032 

0.0182 

5 

•7i 

0.0182 

321 


HYDROGEN 


SOLUBILITY  OF  HYDROGEN  IN  AQUEOUS  PROPIONIC  ACID  SOLUTIONS. 

(Braun,  1900.) 


Cms.  QHsCOOH 

per  100  Cms. 

Solution. 

2.63 

3-37 
5-27 
6.50 
9.91 


Coefficient  of  Absorption  of  Hydrogen  at: 


5°. 

10°. 

15°. 

20°. 

25°. 

O.  02  245 

O.O2I4 

0.0200 

0.0188 

0.0172 

0.0222 

0.0212 

0.0199 

0.0187 

O.OI7I 

O.O224 

O.O2I2 

0.0198 

O.Ol84 

O.OI7I 

0.0218 

o  .  0209 

0.0193 

0.0183 

0.0169 

0.0213 

o  .  0203 

O.OI9I 

0.0178 

0.0160 

SOLUBILITY  OF  HYDROGEN  IN  RUSSIAN  PETROLEUM. 

(Gniewasz  and  Walfisz,  1887.) 

Coefficient  of  absorption  (see  p.  227)  at  20°  =  0.0582,  at  10°  =  0.0652. 


SOLUBILITY  OF 
Results  in  terms  of 

Solvent. 

Water 
Aniline 
Amyl  Alcohol 
Nitrobenzene 
Carbon  Bisulfide 
Acetic  Acid 
Benzene 
Acetone 


HYDROGEN  IN  WATER  AND  IN  ORGANIC  SOLVENTS. 

the  Ostwald  Expression,  see  p.  227.  (Just,  1901.) 

Solvent.  /25-                ly\. 

Amyl  Acetate  0.0774    0.0743 

Xylene  0.0819    0.0783 

Ethyl  Acetate  0.0852    0.0788 

Toluene  0.0874    0.0838 

Ethyl  Alcohol  (98 .8 %)  o .  0894    o .  0862 

Methyl  Alcohol  0.0945    0.0902 

Isobutyl  Alcohol  0.0976    0.0929 


fa. 

0.0199 
0.0285 
0.0301 

0.0371 
0.0375 
0.0633 
0.0756 
0.0764 

fc. 

0.02OO 
0.0303 
0.0353 
0.0353 
0.0336 
0.0617 
O.O7O7 
0.0703 

SOLUBILITY  OF  HYDROGEN  IN  ETHYL  ETHER. 

(Christoff,  1912.) 

Results  in  terms  of  the  Ostwald  Solubility  Expression  I  (see  p.  227). 
k  =  0.1115,     h  =  0.1150,     /io  =  0.1195,     As  =  0.1259. 

Data  tor  the  solubility  of  hydrogen  in  metals  are  given  by  Sieverts  and  co- 
workers,  1909,  1910,  1912. 


HYDROGEN  PEROXIDE  H2O2. 

DISTRIBUTION  OF  HYDROGEN  PEROXIDE  BETWEEN  WATER  AND  AMYL  ALCOHOL 


AT  O°  AND  AT  25°. 


(Calvert,  1901;  Joyner,  1912.) 


Results  at  O°.     (Calvert,  Joyner.) 
Mok.  HA  per  Liter.  jp 

A 

6.76 
6.66 
6.63 
6  .  66 
6.71 


Results  at  25°. 

Mols.  H2O2  per  Liter. 


(Calvert.) 


H2O  layer  (fl 
0.146 
0.200 
0.407 

0-749 
1.970 


Alcohol  Layer  (A). 

0.0216 

0.030 

0.061 

0.113 

0.293 


H2O  Layer  (JF).  Alcohol  Layer  (4). 
0.094  0.013 

0.194  0.028 

0.297  0.042 

o . 670  o . 095 

0.913  0.130 


7.01 
6.91 
7.08 
7.09 
7.01 


Data  are  also  given  for  the  distribution  of  hydrogen  peroxide  between  aqueous 
sodium  hydroxide  solutions  and  amyl  alcohol  at  o°  and  at  25°. 


HYDROGEN  PEROXIDE 


322 


DISTRIBUTION  OF  HYDROGEN  PEROXIDE  BETWEEN  WATER  AND  ORGANIC  SOLVENTS. 

(Walton  and  Lewis,  1916.) 

Different  amounts  of  perhydrol  (30%  H2O2  solution)  were  added  to  various 
mixtures  of  water  and  organic  solvents  and,  after  constant  agitation  for  about 
i  hour,  the  H2O2  in  each  layer  was  determined. 


Solvent 

Ethyl  Acetate 
Isobutyl  Alcohol 
Amyl  Acetate 
Acetophenone 
Ether 
Ether 
Aniline 

t°. 

25 
25 
25 
25 
25 

0 

25 

Ratio, 
Cone.  aq. 

Solvent. 

Methyl  Iodide 
m  Toluidine 
Phenol 

Quinoline 
it 

u 

t°. 

25 
25 
25 

0 

25 
40 

Ratio, 
Cone.  aq. 

Cone.  org.  solvent 
3.92-  4.II 
2.58-    2.63 

13         "13-2 
5.82-   6.06 
8.28-   Q.II 
5-72-    5.85 
4.08-  4.IO 

Cone.  org.  solvent 

Approx.  200 
Approx.      5 

4-35  -5-55 
0.276-0.391 
0.365-0.642 
0.516-0.602 

The  following  approximate  values,  determined  at  room  temp.,  are  quoted  from 
the  dissertation  of  A.  Braun,  Univ.,  Wisconsin,  1914. 

Ratio,  Ratio,  Ratio, 

Solvent.  Cone.  aq.  Solvent.  Conc-  aq.  Solvent.  Cone.  aq. 


Conc.  org.  solvent  Conc.  Org.  solvent  Conc.  Org.  solvent 

Ethyl  Acetate  f  Ethylisovalerianate  ^  Isobutyl  Alcohol  £ 
Nitrobenzene  ^  Isoamyl  Propionate  T\  Propyl  Formate  | 
Acetophenone  £  Chloroform  ^fa  Isobutyl  Butyrate  ^ 

Amyl  Acetate       |        Benzene  jfo      Propyl  Butyrate      ^ 

The  distribution  ratio  of  hydrogen  peroxide  between  water  and  ether  at  17.5° 
varies  with  concentration  from  13.9  to  17.4.  (Osipoff  and  Popoff,  1903.) 

HYDROGEN  SELENIDE  H2Se 

SOLUBILITY  IN  WATER. 

(de  Forcrand  and  Fonzes-Diacon,  1902.) 

4°  9-65 

3-77 


Vol.  H2Se  (at  o°  and  760  mm.)  dissolved 
per  i  vol.  H2O 


13-2 


3-45 


22.5 
2.70 


HYDROGEN  SULFIDE  H2S. 

SOLUBILITY  IN  WATER. 

(Winkler,  1906,  1912.) 
t°.       Abs.  Coef.  0.        q. 

o  4.621  0.699 

5  3-935  0.593 

10  3.362  0.505 

15  2.913  0.436 

20  2.554  0.380 

SOLUBILITY  IN  WATER  AND  IN  ALCOHOL  AT  t°  AND  760  MM.  PRESSURE. 

(Bunsen  and  Carius;  Fauser,  1888.) 
In  Water.  In  Alcohol. 


t°. 

Abs.  Coef.  /9 

'.         q. 

t°.     Abs.  Coef.  0.        q. 

25 

2.257 

0-334 

60 

1.176 

0.146 

30 

2.014 

0.295 

70 

1.  010 

0.109 

35 

1.811 

0.262 

80 

0.906 

0.076 

40 

1.642 

0.233 

90 

0.835 

0.041 

So 

1.376 

0.186 

100 

0.800 

0 

t°. 

i  Vol.  H20  Absorbs. 

0. 

Q- 

i  Vol.  Alcohol  Absorbs. 

o 

4-  37  Vols. 

H2S  (at  o°  and  760  mm.) 

4- 

686 

0. 

710 

17.89 

Vols.  H2S  (at  o°  and  760  mm.) 

5 

3-97 

" 

4- 

063 

0. 

615 

14.78 

« 

IO 

3-59 

« 

3- 

520 

0. 

530 

11.99 

M 

15 

3-23 

" 

3- 

056 

0. 

458 

9-54 

«« 

20 

2.91 

« 

2. 

672 

0. 

398 

7.42 

M 

25 

2.61 

" 

. 

5-96 

(24°) 

M 

30 

2-33 

« 

m 

f 

t 

35 

2.08 

« 

m 

40 

1.86 

« 

For  /3  and  q 
The  PT  and 

see  Ethane,  page  285. 
the  Px  curves  for  the  system  H2S  +  H2O  are  given 

by  Scheffer, 

1911. 

323 


HYDROGEN   SULFIDE 


SOLUBILITY  OF  HYDROGEN  SULFIDE  IN  AQUEOUS  SOLUTIONS  OF  HYDRIODIC 
ACID  AT  25°  AND  760  MM.  TOTAL  PRESSURE. 

(Pollitzer,  1909.) 

Cms,  per  Liter. 
HI.  HJST 


Mols. 

per  Liter. 

Gms.  per  Liter. 

Mols.  per  Liter. 

'IH']. 

[HI]. 

[H2S]. 

HI. 

H2S. 

IH']. 

[HI]. 

[H2S]: 

O.2O 

O 

o. 

1040 

O 

3-54 

4.71 

4 

-38 

O. 

163 

1.23 

I 

.01 

0. 

III 

129.2 

3-78 

5-33 

5 

.005 

0. 

165 

1.74 

1 

•51 

0. 

113 

193.2 

3-85 

6.06 

5 

-695 

O. 

181 

2.18 

I 

•93 

0. 

125 

246.9 

4.26 

7-33 

6 

•935 

O. 

197 

2.Q2 

2 

.64 

0. 

138 

337-8 

4.70 

.9-75 

9 

.21 

O. 

267 

3-71 

3 

.42 

0.142 

437-5 

4.84 

560.4 
640.3 
728.6 
887.2 
1179 


5-55 
5-62 
6.17 
6.71 
9.10 


Data  for  the  solubility  of  hydrogen  sulfide  in  liquid  sulfur  are  given  by  Pela- 
bon,  1897. 

Freezing-point  lowering  data  for  mixtures  of  H2S  and  CH3OH  and  H2S  and 
(CH3)2O  are  given  by  Baume  and  Perrot,  1911,  1914. 


SOLUBILITY  OF  HYDROGEN  SULFIDE  IN  AQUEOUS  SALT  SOLUTIONS  AT  25°. 

(McLauchlan,  1903.) 

NOTE.  —  The  original  results  are  given  in  terms  of  •=-  which  is  the  iodine  titer  (I) 

of  the  H2S  dissolved  in  the  salt  solution,  divided  by  the  titer  (/o),  of  the  H2S  dis- 
solved in  pure  water.  These  figures  were  multiplied  by  2.61  (see  25°  result  in 
last  table  on  page  322)  and  the  products  recorded  in  the  following  table  as 
volumes  of  H2S  absorbed  by  i  vol.  of  aqueous  solution. 


Solution. 

wNH4Br 


iw(NH4)2S04 
«NH4C2H3O2 
n  (NH2)2CO 


Grams  Salt 

I          Vols.  H2S 

per  Liter. 

k      Per 

i  Vol.  Sol. 

98 

I 

2.61 

53-4 

0.96 

2.40 

80 

0.99 

2.58 

33 

0.82 

2.14 

16.5 

0.91 

2.37 

77.1 

1.09 

2.84 

60.  i 

I.  O2 

2.66 

18.22 

0-975 

2-54 

24-52 

0.905 

2.36 

150 

0.944 

2.46 

45° 

0.858 

2.24 

1000 

0.863 

2.26 

Solution. 

wKBr 
wKCl 


wKI 

wNaBr 

wNaCl 


n 

SnCAOe 
Pure  C3H5(OH)3  1000 

Similar  data  are  also  given  for  the  solubility  of  H2S  in  aq.  C2H6OH  solutions 
and  in  aq.  CH3COOH  solutions  at  25°. 


Gms.  Salt" 

i 

Vols.  H,S 

per  Liter. 

£'   per  i  Vol.  Sol. 

119 

O 

•945 

2.47 

74-5 

0 

•853 

2.22 

IOI 

0 

•913 

2.38 

43-5 

0 

.78 

2.04 

21.7 

0 

•89 

2.32 

166 

0 

•98 

2.56 

103 

0 

•935 

2.44 

58-5 

0 

•847 

2.21 

29.2 

0 

•93 

2.42 

•    85 

o 

•893 

2.32 

*    35-5 

0 

•73 

1.90 

i    17-8 

0 

•855 

2.23 

HYDROQUINOL  (Hydroquinone)  C6H4(OH)2  p. 

100  gms.  sat.  solution  in  water  contain  6.7  gms.  hydroquinol  at  20°,  Sp.  Gr.  of 
sol.  =  1. 012.  (Vaubel,  1899.) 

100  gms.  95%Jormic  acid  dissolve  6.07  gms.  hydroquinol  at  20.2°.    (Aschan,  1313.) 


HYDROQUINOL  324 

SOLUBILITY  OF  HYDROQUINOL  IN  SULFUR  DIOXIDE  IN  THE  CRITICAL  VICINITY. 

(Centnerswer  and  Teletow,  1903.) 

Determinations  made  by  the  Synthetic  Method,  for  which  see  Note,  p.  16. 

-0         Cms.  Hydroquinol  *<>  Gms.  Hydroquinol  j.0  Gms.  Hydroquinol 

per  100  Gms.  SO2  per  100  Gms.  SO2  per  100  Gms.  SO2 

63        0.89          II7.6      4.46         136.7       10.31 
73.5      1.22          123.3      5.66         I4I.4       13-3 
89.2      2.l8          134.2      8.31         145         14.9 

DISTRIBUTION  OF  HYDROQUINOL  BETWEEN  WATER  AND  ETHER  AT  15°. 

(Pinnow,  1911.) 
Cone.*  Hydroquinol  in:  Cone.  Hydroquinol  in: 


H2O  Layer.  Ether  Layer.  H2O  Layer.  Ether  Layer. 

0.00502  o.oin  0.0502  0.1275 

0.01196  0.0249  0.0818  0.2343 

0.0128  0.0274  0.1105  °-3543 

0.0236  0.0552  0.1411  0.5300 

0.0455  0.1148  0.1502  0.5604 

*  The  terms  in  which  the  cone,  is  expressed  are  not  stated. 

FREEZING-POINT  DATA  (Solubility,  see  footnote,  p.  i)  ARE  GIVEN  FOR  THE 
FOLLOWING  MIXTURES: 

Hydroquinol  and  Naphthalene.  (Kremann  and  Janetzky,  1912.) 

1    Pyrocatechol.  Qaeger,  1907.) 

"   Resorcinol. 

"    £Toluidine.  (Philip  and  Smith,  1905.) 

Monochlorohydroquinol  and  Monobromohydroquinol.        (Kuster.iSgi.) 
Diacetylmonochlorohydroquinol  and  Diacetylmonobromohydroquinol. 

(Kuster,  1911.) 

HYDROXYLAMINE  NH2(OH). 
HYDROXYLAMINE  HYDROCHLORIDE  NH2(OH).HC1. 

SOLUBILITY  OF  EACH  IN  SEVERAL  SOLVENTS. 

(de  Bruyn,  1892.) 

Gms.  NH2OH  Gms.  NH2(OH).HC 

Solvent.  t°.  per  too  Gms.  t°.  per  too  Gms. 

Solution.  Solvent. 

Methyl  Alcohol  (abs.)  5  35  iQ-75  16.4 

Ethyl  Alcohol  (abs.)  15  15  19.75  4.43 

Ether  (dry)  (b.  pt.)  1.2 

Ethyl  Acetate  (b.  pt.)  1.6 

For  densities  of  NH2(OH).HC1  solutions,  see  Schiff  and  Monsacchi,  1896. 

PhthalylHYDROXYLAMINE   C6H4<CO         >  O. 

One  liter  benzene  dissolves  0.33  gm.  of  the  A  form  of  melting  point  22O°-226°. 

(Sidgwick,  1915.) 

HYOSCYAMINE  Ci7H23N03. 

SOLUBILITY  IN  SEVERAL  SOLVENTS  AT  i8°-22°. 

(Muller,  1903.) 

Gms.  C17H21NO,  Gms.  C17H21NO, 

Solvent.  per  100  Gms.  Solvent.  per  100  Gms. 

Solution.  Solution. 

Water                            0.355  Chloroform  100+ 

Ether                              2 . 02  Acetic  Ether  4 . 903 

Ether  sat.  with  H2O      3 . 913  Petroleum  Ether  o .  098 

Water  sat.  with  Ether  3.125  Carbon  Tetrachloride  o .  059 
Benzene                         o .  769 


325 


HYOSCINE 


HYOSCINE   (Scopolamine)   HYDROBROMIDE,   etc. 

SOLUBILITY  IN  SEVERAL  SOLVENTS  AT  25°.  (U.  S.  P.  VIII.) 

Grams  per  too  Grams  Solvent. 


Solvent.                       Hyoscine 
Hydrobromide 
C17H21NO4HBr.3H2O. 

Water                   66.6 
Alcohol                    6  .  2 
Ether 
Chloroform             o  .  133 

Hyoscyamine 
Hydrobromide 
CnHzsNOa.HBr. 

very  soluble 

50 
0.062 
40 

Hyoscyamine 
Sulfate 
(C17H23N03)2.H2S04 

very  soluble 

15.6 

0.04 
0.043 

Nitro  INDAN  Carboxylic  Acids. 

Freezing-point  lowering  data  for  mixtures  of  /  nitroindan-2-carboxylic  acid 
and  d  nitroindan-2-carboxylic  acid  are  given  by  Mills,  Parker  and  Prowse,  1914. 

CO 
INDIGO  (C6H4<NH>C:)2. 

100  gms.  95%  formic  acid  dissolve  0.14  gm.  indigo  at  19.8°.  (Aschan,  1913.) 

INDIUM  IODATE   In(IO,)8. 

IOO  gms.  H2O  dissolve  0.067  gm-  In(IO3)3  at  2O°.      (Mathers  and  Schluederberg,  1908.) 

IsoINOSITOL   C6Hi2O6. 

loo  gms.  H2O  dissolve25.i2  gms.  C6Hi2O2at  i8°and43.22  gms.  at  100°.  (Muller,  1912.) 

IODIC  ACID   HIO3. 

SOLUBILITY  OF  IODIC  ACID  IN  WATER.    (Groschuff,  1906.) 


-  0.3 

1.69 

Ice 

16            71.7 

mos 

—     1.  01 

6.81 

it 

40            73-7 

« 

-  2.38 

26.22 

« 

60            75.9 

H 

-  4.72 

51.42 

« 

80            78.3 

U 

-  6.32 

57-6i 

K 

85            78.7 

u 

—  12.25 

67.40 

" 

101            80.8 

« 

-14 

69.10 

"  +HI03 

no            82.1 

HI03+HI308 

-J5 

70 

(unstable)  Ice 

125            82.7 

HI308 

-19 

72 

«         «, 

140         83.8 

" 

0 

70.3 

HI03 

160            85.9 

u 

SOLUBILITY  OF  IODIC  ACID  IN  NITRIC  ACID.     (Groschuff.) 

Gms, 

.  HIO3  per  100  Gms. 

*"•                 '     Aq.                   27.73  %HN03          40.88%  HNQ,' 
Solution.                   Solution.                   Solution. 

0 

74.1 

18                      9 

20 

75-8 

21                             10 

40 

77-7 

27                    14 

60 

80 

38                    18 

IODINE   I2 

SOLUBILITY  OF  IODINE  IN  WATER.    (Hartley,  1908.) 

j.o  Gms.  I  per  1000  Gms. 

H20. 

18  0.2765 

25  0-3395 

35  0.4661 

45  0.6474 

55  0.9222 

The  above  determinations  were  made  with  great  care.  Results  for  single 
temperatures  in  good  agreement  with  the  above  are  given  by  Dietz,  1898; 
Jakowkin,  1895;  Noyes  and  Seidensticker,  1898;  Sammet,  1905;  Bray  and 
Connolly,  1910,  1911;  Herz  and  Paul,  1914  and  Fedotieff,  1911-12. 


IODINE 


326 


SOLUBILITY  OF  IODINE  IN  AQUEOUS  MERCURIC  CHLORIDE  AND  IN  AQUEOUS 
CADMIUM  IODIDE  SOLUTIONS  AT  25°. 

In  Aq.  HgCl2. 

(Herz  and  Paul,  1914.) 

Gms.  per  Liter. 


Millimols  per  Liter. 


o 

94-44 
124.42 
iQS-42 
334-6o 


1-3.4 
12.94 
14.60 
18.06 
25-43 


HgCl2. 
o 

25.64 
33-78 
54-29 
90.84 


I. 

0.340 
3-285 
3.706 
4-583 
6.454 


In  Aq.  CdI2. 

(Van  Name  and  Brown,  1917.) 
Gms.  per  Liter. 


CdI2. 

3-66 

45.78 

91.56 

183.12 


I. 

2.072 

9.056 

11.386 

14.040 


SOLUBILITY  OF  IODINE  IN  VERY  DILUTE  AQUEOUS  SOLUTIONS  OF  POTASSIUM 

IODIDE. 

(Determinations  made  with  very  great  care.) 


Results  at  o°. 

Results  at  25°. 

Results 

at  25°. 

(Jones  and  Hartman,  igiS-) 

(Bray  and  MacKay,  1910.)     (Noyesand  Seidenstricker,  1898.) 

Normality           A 

Gms.  I  per 

Normality 

Millimols  I2 

Normality 

Millimols  I2 

KIAs2i.           Sallol. 

ioo  Gms. 
Sat.  Sol. 

of  Aq. 
KISol. 

per  Liter  j 
Sat.Sol. 

of  Aq. 
KISol. 

per  Liter 
Sat.  Sol.~ 

O.OOO992 

.OOO2 

0.0282 

0 

1-333 

O 

1.342 

O.OO2OO 

.OOO4 

0.0409 

0.001 

1.788 

0.00083 

1.814 

0.00500 

.OOIO 

o  .  0760 

O.OO2 

2.266 

0.00166 

2-235 

O.OIOOO 

.OO2O 

0.1356 

0.005 

3.728 

0.00664 

4.667 

0.01988 

.0044 

0-2533 

O.OIO 

6.185 

0.01329 

8.003 

O.O500                3 

.OIO9 

0.609 

O.O2O 

11.13 

0.02657 

4.68 

0.09993 

.O2I9 

1.199 

0.050 

25-77 

0.05315 

28.03 

0.100 

51-35 

0.1063 

55-28 

SOLUBILITY  OF  IODINE  IN  AQUEOUS  SOLUTIONS  OF  POTASSIUM  IODIDE  AT 
25°  AND  VICE  VERSA. 

(Parsons  and  Whittemore,  1911.) 
(Time  of  rotation  6  mos.  or  longer.    Duplicate  determinations  at  different  lengths  of  time,  were  made.) 

Solid 


Sp.  Gr. 
Sat.  Sol. 

Gms.  per  ioo  Gms. 
Sat.  Sol. 

KI                    I 

1-349 

16.03            18.49 

1.516 

19.70            26.16 

1.769 

22.88          36.06 

1.910 

23.55       40.52 

2.403 

24.78       53.60 

2.904 

25           63.12 

3.082 

25.18          66.04 

3-3*6 

26             68.09 

Solid 

Sp.  Gr. 

Gms.  per  ioo  Gms. 
Sat.  Sol. 

Phase. 

Sat.  Sol. 

KI                    I 

dine 

3-246 

27.92          66.45 

29.71          62.81 

2.665 

35.80          49.61 

2-539 

38.09          44.58 

2.216 

44.82          31.01 

2.066 

49.04          23.08 

1.888 

54.41          11.63 

+KI 

1-733 

60.39            o 

KI 


Additional  data  for  this  system  are  given  by  Bruner,  1898;  Hamberger,  1906; 
and  Lami,  1908. 

Data  for  the  solubility  of  iodine  in  aq.  40%  ethyl  alcohol  and  aq.  60%  ethyl 
alcohol  solutions  of  potassium  iodide  at  25°,  are  given  by  Parsons  and  Corliss, 
1910.  The  solid  phases  were  identified  in  each  case  and  it  was  demonstrated 
that  no  polyiodides  of  potassium  exist  in  the  solid  phase  or  in  solution  at  25°. 

An  extensive  series  of  determinations  of  the  simultaneous  solubility  of  iodine 
and  potassium  iodide  in  nitrobenzene  and  in  other  organic  solvents,  as  well  as 
in  mixtures  of  nitrobenzene  and  other  solvents  are  given  by  Dawson  and  Gawler, 
1902,  and  Dawson,  1904.  The  determinations  were  made  to  obtain  information 
on  the  formation  of  polyiodides  in  solution.  The  molecular  ratio  of  dissolved 
I2/KI  was  found  to  be  I  or  more  in  all  cases.  (See  also  p.  537.) 

Freezing-point  lowering  data,  determined  by  time-cooling  curves,  for  mixtures 
of  iodine  and  potassium  iodide  are  given  by  Kremann  and  Schoulz,  1912.  Data 
for  this  system  are  also  given  by  Olivari  (1908). 


327  IODINE 

SOLUBILITY  OF  IODINE  IN  AQUEOUS  SOLUTIONS  OF  POTASSIUM  BROMIDE 
AND  OF  SODIUM  BROMIDE  AT  25°. 

(Bell  and  Buckley,  1912.) 


In  Aq.  KBr 

Solutions. 

In  Aq.  NaBr 

Solutions. 

Cms.  KBr 

Gm.  Atoms  I 

Gms.  NaBr 

Gm.  Atoms  I 

per  Liter. 

per  Liter. 

per  Liter. 

per  Liter. 

60.6      ty 

0.0176 

2,^       96.4 

0.0266 

106.9 

0.0278 

I87.7 

0.0425 

175-9 

0.0415 

271.8 

0.0538 

229.8 

0.0532 

357-4 

0.0598 

281.9 

0.0628 

422.21 

0.0638 

33°  -6 

0.0717 

499.1  • 

o  .  0648 

377-1 

0.0797 

569-9 

o  .  0644 

411 

0.0864 

632 

0.0622 

461.7 

o  .  0948 

679.7 

0-0595 

509.8 

0.1006 

750-5 

0.0551 

567.9  sat. 

0.1094 

756.1  sat. 

0.0550 

SOLUBILITY 

OF  IODINE  IN 

AQUEOUS  SOLUTIONS  OF  ACIDS. 

Aqueous  Acid. 

Mols.  I  per  Liter       Gms.  I  per  Liter 
Sat.  Sol.                    Sat.  Sol. 

Authority. 

o.ooi  wHCl 

0.001332 

°  •  338            (Bray  and  MacKay,  1910.) 

o.iorcHNOs 

0.001340 

0  .  340            (Sammet,  1905.) 

o  .  10  n  H2SOi 

O.OOI342 

0.341 

« 

SOLUBILITY  OF  IODINE  IN  AQUEOUS  SODIUM  IODIDE  SOLUTIONS. 
(Gill,  1913-14.)       i 

Aqueous  Nal  solutions  were  prepared  by  dissolving  the  stated  amounts  of  the 
salt  in  water  and  diluting  to  100  cc.  An  excess  of  iodine  was  added  to  each  of 
these  solutions,  the  mixtures  heated  to  60°  and  shaken  for  several  minutes. 
They  were  then  allowed  to  cool  in  a  thermostat  at  25°  for  four  hours.  The 
dissolved  iodine  in  weighed  amounts  of  the  saturated  solutions  was  titrated  with 
thiosulfate.  The  densities  of  the  Aq.  Nal  mixtures  and  also  of  the  solutions 
after  saturation  with  iodine  were  determined. 

Gms.  Nal  &*  of  d25  of  Aq.  Nal  Gms.  I  Dissolved 

per  zoo  cc.  Aq.  Nal  after  Saturation          at  25°  per  100  Gms. 

Aq.  Solution.  Solution.  with  I.  of  the  Sat.  Sol. 

5  1.0369  1.0698  4.99 
10  1.0720  1-1415  9.96 
15  1.1072  1.2162  J4-93 

20  I.I458  1.2998          20.02 

Determinations  at  other  temperatures  were  made  in  an  apparatus  which  per- 
mitted constant  stirring  of  the  solutions  at  the  several  temperatures.  Results, 
interpolated  from  the  original,  are  as  follows: 

Gms.  I  Dissolved  per  100  Gms.  Gms.  I  Dissolved  per  100  Gms. 

0  Sat.  Solution  in  Aq.  Nal  of:  Sat.  Solution  in  Aq.  Nal  of: 

10  Gms.  per        20  Gms.  per  10  Gms.  per        20  Gms.  per 

100  cc.  100  cc.  100  cc.  loo  cc. 

10     8.9     17.6        30     10.3     20.5 
15     9-3     l8-3        40     10.9     22 

20       9.6       19  50       11.7       23.4 

25     10      19.4        60     12.6     24.9 


IODINE 


328 


SOLUBILITY  OF  IODINE  IN  AQUEOUS  SALT  SOLUTIONS  AT  25°. 

(McLauchlan,  1903.) 


Q,.                Gms.  Salt 
per  Liter. 

NaaSO4          29.77 
KaSO4            43.5 
(NH4)2SO4     33 

Gms.  Dissolved 
I  per  Liter. 

0.160 
0.238 
0.246 

.  Salt. 

NH4C1 
NaBr 
KBr 

Gms.  Sak. 
per  Liter. 

53-4 
103 
119 

Gms.  Dissolved 
I  per  Liter. 

0-735 
3-29 
3.801 

NaNO3 

85 

0.257 

NHjBr 

98 

4.003 

KN03 

IOI.2 

0.266 

NH4C2HsO2 

77-i 

0.440 

NHiNOs 

80 

0-375 

(NH4)2C204 

86.9 

0.980 

NaCl 

S8.5 

0-575 

HaBOs 

55-8 

0.300 

KC1 

73-6 

0.658 

SOLUBILITY  OF  IODINE  IN  NITROBENZENE  SOLUTIONS  CONTAINING  VARIOUS 
IODIDES  AT  ROOM  TEMPERATURE.    SOLUTIONS  SAT.  WITH  I  IN  EACH  CASE. 

(Dawson  and  Goodson,  1904.) 


Iodide. 

Gms.  per  Liter. 

Iodide. 

Iodine. 

Potassium  Iodide 

12-35 

112.7 

«             « 

45-56 

295-7 

«             « 

115.8 

698.2 

«             « 

155-2 

943-6 

Sodium  Iodide 

13-55 

125 

«          « 

57-7 

393 

«           a 

log:  I 

738 

«           « 

228 

1251 

Rubidium  Iodide 

85.4 

421 

Rubidium  Iodide 

217-5 

1060 

Lithium  Iodide 

84.1 

642 

Iodide. 

Caesium  Iodide* 
Caesium  Iodide 
Ammonium  Iodide 
Ammonium  Iodide* 
Aniline  Hydriodide 
Dimethylaniline  Hydriodide 
Tetramethylammonium  Iodide 
Tetramethylammonium  Iodide 
Strontium  Iodide 
Barium  Iodide 
Barium  Iodide 


*  Solvent  =  o  nitrotoluene  instead  of  nitrobenzene. 


Gms.  per  Liter. 


Iodide. 
48.2 

223 
69.5 
94-3 

164 

160 
49-3 
51-4 

106.5 
42.2 

158.5 


Iodine. 
213 
858 
482 
669 
721 
626 
266 
280 
599 
237 
809 


Similar  results  are  also  given  for  solutions  containing  KI  in  addition  to  the 
other  iodide,  and  one  series  for  the  simultaneous  solubility  of  KBr  and  I  in  nitro- 
benzene. It  is  considered  that  the  increased  solubility  is  most  easily  explained 
on  the  assumption  that  periodides  are  formed  in  solution. 


SOLUBILITY  OF  IODINE  IN  AQUEOUS  ETHYL  AND  NORMAL  PROPYL  ALCOHOL 
SOLUTIONS  AT  15°. 

(Bruner,  1898.) 


In  Aq.  Ethyl  Alcohol. 


In  Aq.  (n.)  Propyl  Alcohol. 


Vol.  % 
C,H5OH 
insolvent. 

Gms.  I  per 
100  cc. 
Solution. 

Vol.  % 

r1  TT  f\tr 
\*2  iL^Jti. 

in  Solvent. 

Gms.  I  per 

100  CC. 

Solution. 

Vol.  % 
CaH7OH 
in  Solvent. 

Gms.  I  per 
100  cc. 
Solution. 

Vol.  % 
CSH7OH 
in  Solvent. 

Gms.  I  per 

ICO  CC. 

Solution. 

10 

0.05 

60 

I.I4 

IO 

0.05 

60 

2.71 

20 

0.06 

70 

2-33 

20 

O.II 

70 

4.10 

30 

0.10 

80 

4.20 

30 

0.40 

80 

6.05 

40 

0.26 

90 

7-47 

40 

o-94 

90 

9.17 

50 

0.88 

100 

15-67 

50 

1.64 

100 

14-93 

329  IODINE 

SOLUBILITY  OF  IODINE  IN  AQUEOUS  ETHYL  ALCOHOL  AND  IN  AQUEOUS  ACETIC 
ACID  SOLUTIONS  AT  25°. 

(McLauchlan,  1903.) 

In  Aq.  C2H6OH  Solutions.  In  Aq.  CH3COOH  Solutions. 


Gms.  I  per 

ioo  cc.  Sat. 

Gms.  CH3COOH 
per  too  Gms. 

Gms.  I  per 
ioo  cc.  Sat. 

Solution. 

Solvent. 

Solution. 

0.034 

0 

0.034 

0.039 

20      . 

0.076 

0.172 

39-5 

0-173 

0-955 

61.1 

0.510 

6.698 

80.7 

I-363 

24.548 

IOO 

3.l62 

Cms. 
per  100  Gms. 
Solvent. 

O 

4-55 
28.48 
44.41 

72-51 
100 


SOLUBILITY  OF  IODINE  IN  AQUEOUS  GLYCEROL  SOLUTIONS  AT  25°. 

(Herz  and  Knoch,  1905.) 

Density  of  glycerine  at  25°/4°  =  I-2555'»  impurities  about  1.5%. 

Wt.%  Glycerine        Millimols  I              Grams  I  per  Density  of 

inSolvent.      per  100  cc.  Solution.      loocc.  Solution.  Solutions  at  25  °/4°. 

o                    0.24                0.0304  0.9979 

7.15        0.27         O.O342  1.0198 

20-44        0.38         0-0482  I.047I 

31.55        0-49         0.0621  1.0750 

40.95        0.69         0.0875  1.0995 

48.7               1.07               0.135  1.1207 

69.2                        2.20                        0.278  LI765 

ioo.  o               9.70                1-223  1.2646 


ioo  gms.  glycerol  (du  =  1.256)  dissolve  2  gms.  iodine  at  i5°-i6°. 

(Ossendowski,  1907.)  > 

SOLUBILITY  OF  IODINE  IN  BENZENE,  CHLOROFORM,  AND  IN  ETHER. 

(Arctowski  —  Z.  anorg.  Chem.  n,  276,  '95-'96.) 

In  Benzene.  In  Chloroform.  .    In  Ether. 


t°. 

Gms.  I  per  ioo 
Gms.  Solution. 

A  o            Gms.  I  per  ioo              ^  0             Gms.  I  per  ioo 
Gms.  Solution.                               Gms.  Solution. 

4.7 

8.08 

-49 

0.188            -83          15.39 

6.6 

8.63 

-55* 

0.144            —90          14-58 

10.5 

9.60 

-60 

0.129            —  108        15-09 

10-44 

—  69  J 

0.089 

16^3 

11.23 

-73i 

0.080 

+  10 

i  .  76  per  ioo  gms.  CHC13 

(Duncan  —  Pharm.  J.  Trans.  22,  544,  'pi-' 

SOLUBILITY  OF  IODINE  IN  BROMOFORM,  CARBON  TETRACHLORIDE,  AND  IN 
CARBON  DISULFIDE  AT  25°. 

(Jakowkin,  1895.) 

I  liter  of  saturated  solution  in  CHBr3  contains  189.55  gms.  I. 
i  liter  of  saturated  solution  in  CC14  contains  30.33  gms.  I. 
I  liter  of  saturated  solution  in  CSa  contains  230  gms.  I. 


IODINE 


330 


—  100 

-  80 

-  63 

—  20 

—  10 


SOLUBILITY  OF  IODINE  IN  CARBON  BISULFIDE. 

(Arctowski,  1894.) 


Gms.  I  per  100 
Gms.  Solution. 

0.32 
0.51 
1.26 
4.14 
S-S2 


O 
10 

15 

20 


Gms.  I  per  100 
Gms.  Solution. 

7.89 
10.51 

12-35 
14.62 
10.92 


3° 
36 
40 
42 


[Gms.  I  per  100 
Gms.  Solution. 

19.26 
22.67 
25.22 
26.75 


SOLUBILITY  OF  IODINE  IN  SEVERAL  SOLVENTS  AT  25°. 

(Herz  and  Rathmann,  1913.) 
Iodine 
Solvent. 

Chloroform 

Carbon  Tetrachloride 

Tetrachlorethylene 

One  liter  sat.  solution  of  iodine  in  nitrobenzene  contains  50.62  gms.  I  at  i6°-i7°. 

(Dawson  and  Gawler,  1902.) 
IOO  gms.  hexane  dissolve  1 .32  gms.  iodine  at  25°.    (Hildebrand,  Ellefson  and  Beebe,  1917.) 

100  gms.  sat.  solution  of  iodine  in  anhydrous  lanolin  (melting  point  46°),  con- 
tain 5.50  gms.  iodine  at  45°.  (Klose,  1907.) 


Iodine  per  Liter  of 
Sat.  Sol. 

Solvent. 

Trichlorethylene 
Tetrachlorethane 
Pentachlorethane 

Iodine  per  Liter  of 
Sat.  Sol. 

Mols. 
0-352 
0.237 
0.241 

Gms. 
44.68- 
30.08 
3°  -59 

Mols. 
0.312 
0.244 
0.272 

Gms. 
39.61 
30-97 

34-53 

SOLUBILITY  OF  IODINE  IN  MIXTURES  OF  CHLOROFORM  AND  ETHER  AT  25°. 

(Harden  and  Dover,  1916.)  ', 

Gms.  CHC13  per  100        Gms.  Iodine  per  100 
Gms.  CHC13+(C2HB)2O.  Gms.  ~ 

O 


10 
20 

30 
40 

5° 


3S-i 
29.6 
24.8 

20.2 

I6.3 
12.7 


Gms.  CHC13  per  100      Gms.  Iodine  per  100  Gms. 
Gms.  CHC13+(C2H5)2O.        CHC13+(C2 

60  9.83 


80 

90 

loo 


7-5 

5-73 

4.31 

3.10 


loo  cc.  of  a  mixture  of  CHC13  +  CSa  (3:1)  dissolve  7.39  gms.  iodine  (t°  ?.) 
The  addition  of  S  even  up  to  the  point  of  saturation  does  not  affect  the  amount 
of  iodine  held  in  solution.  (Olivari,  1908.) 

Diagrammatic  results  for  mixtures  of  iodine  and  each  of  the  following  com- 
pounds are  given  by  Olivari,  1911:  CHI3,  p  C6H4Br2,  [C6H4]N2,  p  C6H4(NO2)2, 
(C6H6CO)2O  and  C6H6COOH.  ' 


SOLUBILITY  OF  IODINE  IN  MIXED  SOLVENT 

(Stromholm,  1903.) 

Gms.  I 
Solvent.                             per  Liter                               SoK 
Sat.  Sol. 
Ether                                                 206  .  3      Ether+  20.96  grr 
Carbon  Bisulfide                               178.5      Ether+4i.9 
Ether+3.96  gms.  H2O    per  liter      221          CS2    +22.5 
'     +7.91  gms.  H2O                       235.7       CSa     +45.1 
'    +excessH2O                            251.4      Ether+47.63 
1    +9.79  gms.  C2H6OH  "            219.1      CS2    +50.06 
"    +19.6    "          "         "            231.5      Ether+8o.3 
'    +294    "           "         "            243-9      Ether+77.8s 
"    +39.2    "          "         «            254.4      CS-j    +62.2 

S   AT    1  6.6°. 

ent. 

is.  CS2  per  liter 
CS2 
ether 
ether 
CHCU 
CHCU 
C6H6 
CH3I 
S 

Gins.  I 
per  Liter 
Sat.  Sol. 
202.3 
217.2 

189.3 
201.  I 
195-2 
172.8 
204.1 
22O.2 
189.4 


One  liter  sat.  solution  in  ether  contains  167.3  Sms.  I  at  o°.         (StrSmholm,  1903.) 


331  IODINE 

SOLUBILITY  OF  IODINE  IN  MIXTURES  OF  CHLOROFORM  AND  ETHYL  ALCOHOL, 
CHLOROFORM  AND  NORMAL  PROPYL  ALCOHOL,  CHLOROFORM.  AND  BENZENE, 
AND  CHLOROFORM  AND  CARBON  DISULFIDE  AT  15°. 

(Bruner,  1898.) 

Vol  °f  CHCI  ^ms'  *  Dissolved  per  100  cc.  of  Mixtures  of: 

insolvent.  3 

O 
10 
20 

30 
40 

50 

60 

70 

80 
'QO 
IOO 

SOLUBILITY  OF  IODINE  IN  MIXTURES  OF  CARBON  TETRACHLORIDE  AND  BEN- 
ZENE AND  IN  MIXTURES  OF  CARBON  TETRACHLORIDE  AND  CARBON  DISUL- 
FIDE AT  I 


CHC13+C2H5OH. 

CHC13+C3H7OH. 

CHC13+C6H6. 

CHClj+CSs. 

I5-67 

14-93 

10.40 

17.63 

9-43 

13.16 

9.84 

15.93 

8.69 

11.20 

8.78 

14.20 

7.80 

8.98 

7-74 

12.  l6 

7.09 

8.09 

6.96 

IO.2O 

6.62 

7.82 

6.20 

9.08 

6.24 

7.09 

5-34 

7.72 

5-77 

6.42 

4.89 

6.42 

5-06 

5-54 

4-53 

5-27 

4-34 

4-52 

4.07 

4.32 

3.62 

3.62 

3.62 

3.62 

1898.) 

Vrti   of  rr\     Gms.  I  per  100  cc.  of  Mixture  of:  v  i   o/  rn     Gms.  I  per  100  cc.  of  Mixture  of: 

VOl.    /Q  V^^i4  -^_,^ _Ai  -  _  VOI.    /o  l_,l_J4  ji  

*»  Solvent.      '  CCU+CeHe.         CCU+CS,.   '  in  Solvent.        'ca+C^.        CCU+CS,/ 

o  10.40  17.6  60  4.90  5-55 

10  9.44  14.44  70  4.09  4.50 

20  8.53  12.33  80  3.41  3.37 

30  7.77  10.34  90  2.74  2.60 

40  6.63            8.60  loo  2.06  2.06 

50  5.70           6.83 

In  the  case  of  the  above  determinations  the  volume  change  occurring  on  mixing 
the  solvents  was  neglected.  The  temperature  was  not  accurately  regulated  and 
the  mixtures  not  shaken  during  the  saturation.  The  curves  plotted  from  the 
results  are  not  smooth. 

DISTRIBUTION  OF  IODINE  BETWEEN  WATER  AND  BROMOFORM^  WATER  AND  CAR- 
BON BISULFIDE,  AND  WATER  AND  CARBON  TETRACHLORIDE  AT  25°. 

Qakowkin,  1895.) 

The  original  results  were  plotted  on  cross-section  paper  and  the  following  table  made  from  the  curves. 
Jakowkin  points  out  that  the  results  of  Berthelot  and  Jungfleisch,  1872,  are^incorrect  on  account  of  the 
presence  of  HI. 

Gms.  I  per  Liter  Gms.  I  per  Liter  of: 

of  H2O  Layer 
in  Each  Case. 

0.05 
0.10 

0-15 
0.20 
0.25 

A  theoretical  discussion  of  the  results  of  Jakowkin  is  given  by  Schiikarew  (1901). 


CHBr3  Layer. 

CSj  Layer. 

CCU  Layer. 

20 

30 

4 

45 

60 

8.5 

71 

91 

13 

IOO 

126 

17-5 

130 

160 

22 

IODINE 


332 


DISTRIBUTION  OF  IODINE  BETWEEN  CARBON  DISULFIDE  AND 
AQ.  POTASSIUM  OXALATE. 

(Dawson  — Z.  physik.  Chem.  56,  610,  '06;  Dawson  and  McRae  —  J.  Chem.  Soc.  81,  1086,  '02.) 


Concentration 

flf 

Gms.  I  per  Liter  of 

Aq.  K2C204. 

Aq.  Layer.      CS2  Layer. 

.0  Equiv. 

2.408            10.82 

.0          " 

3-555        l6-32 

.0          " 

5.766            27.91 

.0          " 

6.861        34-01 

.2           " 

3-525        J7-o7 

Vol.  of  Solution 

which  Contains 

i  Mol.  I. 


Fraction  of  I 
Uncombined 
in  Solution. 


105.3      0.005495 
71.37     0.00561 

43-99  0.005915 
36.98  0.006055 
71.97  0.005645 

DISTRIBUTION  OF  IODINE  BETWEEN  AMYL  ALCOHOL  AND  WATER  AND 

BETWEEN  AMYL  ALCOHOL  AND  AQUEOUS  POTASSIUM  IODIDE 

SOLUTIONS  AT  25°. 

(Herz  and  Fischer  —  Ber.  37,  4752,  '04.) 

The  original  results  were  plotted  on  cross-section  paper,  and  the 
following  tables  made  from  the  curves. 

Millimols  I  per  10  cc.  of  H2O  and  of  Aq.  KI  Layers. 


Amyl  Alcohol  Layer 

' 

N 

2N 

3N 

4N 

ioN 

in  Each  Case. 

H-jO. 

—  K.I. 

—  KI. 

-  —  KI. 

'  —  K  I 

•  KI. 

10 

10 

10 

IO 

IO 

2-5 

O.OI2 

0-135 

0.160 

0.170 

0.170 

O.OI4 

0.150 

0.185 

O.2OO 

O-2OO 

0.160 

4.0 

O.OlS 

0.180 

0.235 

0.255 

O.27O 

O.24O 

5 

O.O2I 

O.2IO 

0.280 

0.340 

0.315 

6 

O.025 

0.230 

0-330 

0-375 

0.410 

0.390 

7 

O.O29 

0.250 

0-375 

0.430 

0.480 

0.470 

8 

.  .  . 

0.26o 

0.420 

0.490 

0-550 

o-555 

9 

0.270 

0.450 

0-550 

O.62O 

0-640 

10 

.  .  . 

0.280 

0.470 

0.605 

0.690 

0.720 

12 

.  .  . 

.  .  . 

0.490 

0.700 

0.830 

0.900 

14 

0.510 

0.790 

0.980 

1.200 

20 

... 

0-575 

Grns.Iperioocc. 
Amyl  Alcohol  Layer 

Gms.  I  per 

ioo  cc.  of  H2O  and  of  KI 

Layers. 

/J 

N 

aN 

N 

N 

N       ""* 

in  Each  Case. 

H20. 

—  KI. 

—  KI. 

—  KL 

—  KI. 

—  —  KI. 

10 

10 

10 

10 

IO 

3 

O.OI4 

0.164 

O.2O 

0.21 

0.21 

4 

c  016 

0.196 

O.24 

O.26 

O.26 

0.21 

6 

^•026 

0.252 

o-34 

0.38 

O.4O 

o-37 

8 

o*-o33 

0.297 

0.43 

0.49 

0-54 

0.51 

10 

0.040 

0.328 

0.51 

0.61 

0.67 

0.69 

12 

0.341 

0.58 

o-73 

0.81 

0.84 

14 

0.60 

0.83 

o-95 

1.  00 

16 

0.63 

0.91 

1.09 

1.20 

18 

0.64 

25 

0.71 

The  original  figures  for  sN/io  and  loN/io  KI  solutions  give  prac- 
tically identical  curves. 

Results  for  the  distribution  of  Iodine  between  N/io  KI  solutions  on 
the  one  hand,  and  mixtures  in  various  proportions  of  C6H64-  CS3, 
C6H6CH3+CS2,  C6H6  +  C6H6CH3,  C6H6  +  ligfft  petroleum,  CS2  +  light 
petroleum,  CS3+CHC13,  CHC13+  CCH6,  CC14  +  CS2  and  CC14+  C6H6CH, 
on  the  other  hand,  are  given  by  Dawson  —  J.  Chem.  Soc.,  81,  1086,  '02, 


333 


IODINE 


DISTRIBUTION  OF  IODINE  BETWEEN  WATER  AND  IMMISCIBLE  ORGANIC  SOLVENTS. 

Results  for  Water  Results  for  Water    Results  for  Water    Results  for  Water 
-f  Carbontetra-        +  Nitrobenzene      +  Carbon  Disul-       +  Chloroform 
chloride  at  18°.  at  18°.  fide  at  15°.  at  25°. 

(Dawson,  1908.)  (Dawson,  1908.)  (Dawson,  1902.)          (Herz  &  Kurzer,  1910.) 

Mols.  Iodine  per  Liter.        Mols.  Iodine  per  Liter.      Gins.  Iodine  per  Liter.     Mols.  Iodine  per  Liter. 


'H2O  Layer.  CCU  Layer. 
0.000416      0.0344 
0.000535      0.0443 

Results  for  Water 
+  Trichlorethyl- 
ene  at  25°. 

(Herz  &  Rathmann,  '  13.) 
Mols.  Iodine  per  Liter. 

H2O  Layer.  CeHsNOz  Layer 
0.00019       0.0333 
o  .  00050      o  .  0854 
0.00133     0.2275 
0.00189      0.3328 

Results  for  Water 
+  Tetrachlor- 
ethylene  at  25°. 
(Herz  &  Rathmann,;  13.) 
Mols.  Iodine  per  Liter. 

.H2O  Layer.  CSj  Layer. 
0.0452        27.85 
0.0486        30.09 
0.0486        30.31 

Results  for  Water 
+  Tetrachlor- 
ethane  at  25°. 

(Herz  $;  Rathmann,  '13.) 
Mols  Iodine  per  Liter. 

H20  Layer.  CHC1,  Layer." 
0.00025       0.0338 
0.00120       0.1546 
0.00184       0.2318 
0.00259       0-3439 

Results  for  Water 
+  Pentachlor- 
ethane  at  25°. 
(Herz  &  Rathmann,  '13.) 
Mols.  Iodine  per  Liter. 

'       H2O          CHC1.CC12 
Layer.             Layer. 
0.00046        0.0543 
O.oooyo        0.0778 
O.OOII2        0.1275 
0.00236        0.2672 

'      H20          CC12.CC12 
Layer.            Layer. 
O.OOO88        0.0653 
O.OOI27        0.0932 
0.00172        0.1285 

0.00281      0.2161 

•     H20             CiH,(V 
Layer.            Layer. 
0.00119       O.lioi 
0.00145       0.1247 
0.00159       0.1479 
0.00217       0.2103 

H20           C2HC151 
Layer.          Layer. 
0.00092     0.0848 
0.00117     0.1067 
0.00160     0.1434 
o  .  00204    o  .  1963 

Data  for  the  distribution  of  iodine  between  water  and  mixtures  of 
at  25°  are  given  by  Herz  and  Kurzer,  1910. 

Data  for  the  distribution  of  iodine  between  carbon  disulfide  and  aqueous  solu- 
tions of  each  of  the  following  iodides  at  25°  are  given  by  van  Name  and  Brown, 
1917.  Cadmium  iodide,  cadmium  potassium  iodide,  lanthanum  iodide,  nickel 
iodide,  strontium  iodide,  zinc  iodide  and  zinc  potassium  iodide.  Results  for  the 
distribution  of  iodine  between  carbon  tetrachloride  and  aq.  mercuric  potassium 
iodide  are  also  given. 

Results  for  distribution  between  CS-5  and  aq.  BaI2  sols,  are  given  by  Herz  and 
Kurzer,  1910. 

Data  for  the  distribution  of  iodine  between  carbon  disulfide  and  aqueous  solu- 
tions of  potassium  iodide  at  15°  and  at  13.5°,  and  between  carbon  disulfide  and 
aqueous  solutions  of  hydriodic  acid  at  13.5°,  are  given  by  Dawson,  1901  and  1902. 

Data  for  the  distribution  of  iodine  between  carbon  tetrachloride  and  aqueous 
solutions  of  mercuric  bromide  and  of  mercuric  chloride  at  25°  are  given  by  Herz 
and  Paul,  1914. 

DISTRIBUTION  OF  IODINE  BETWEEN  CARBON  DISULFIDE  AND  AQ. 
t;  ETHYL  ALCOHOL  AT  25°.    (Osaka,  1903-08.) 


Gms.  C2H5OH 

Gms.  Iodine  per  Liter: 

Gms.  CsHfiOH    Gms.  Iodine  per  Liter: 

per  100  cc. 
Aq.  Alcohol. 

CSz  Layer 
c. 

Aq.  Alcohol 
Layer  c'. 

c'' 

per  100  cc. 
Aq.  Alcohol. 

CSz  Layer 
c. 

Aq.  Alcohol 
Layer  c'. 

c' 

7.6 

O, 

,072 

35-86 

O 

.0020 

I9.I 

0.330 

97 

o, 

0034 

7-6 

O, 

211 

107.79 

o 

.0020 

22.9 

O.II5 

23-78 

Q 

,0048 

ii.  4 

o 

077 

32.93 

0 

.0023 

22.9 

0.418 

89.61 

o 

0047 

ii.4 

o 

,280 

133.22 

0 

.0021 

26.7 

0.0756 

9-8 

o 

.0077 

15-3 

o 

075 

25.61 

0 

.0029 

26.7 

0-495 

65.10 

o 

.0076 

iS-3 

o 

315 

115-34 

0 

.0027 

30.5 

o  .  0636 

4.90 

0 

.0130 

19.1 

o 

•045 

I3-42 

0 

.0034 

30.5 

0.546 

42.27 

o 

.0129 

DISTRIBUTION  OF  IODINE  BETWEEN  ETHER  AND  ETHYLENE  GLYCOL.   (Landau,  1910.) 

Results  at  25°. 

Gms.  Iodine  per  Liter: 


Results  at  o°. 

Gms.  Iodine  per  Liter: 

a 

r 

.48 
.80 

.75 
.76 

•75 
.80 

(C2H5)20 
Layer  (c). 
2.139 
7.820 
16.620 
20.564 
3L785 
79-950 

(CH2OH)2 
Layer  (b), 

1-449 
4-347 
9.486           1 
11.685 

18.135 
44.460 

(C2H5)20 
Layer  (a). 

(CH2OH), 
Layer  (b). 

r 

2.208 

1.449 

•52 

4-255 

2.541 

.60 

7.728 

4-347            J 

.78 

16.200 

9.120 

.78 

30.322 

17.062 

.78 

78.195 

44-460           3 

.76 

IODINE 


334 


DISTRIBUTION  OF  IODINE  BETWEEN  GLYCEROL  AND  BENZENE  AND  BETWEEN 
GLYCEROL  AND  CARBON  TETRACHLORIDE. 

(Landau,  1910.) 


Results  for  Glycerol  and  Benzene. 

Grams  Iodine  per  Liter:                   /M 

Results  for  Glycerol  and  CC14. 

Gms.  Iodine  per  Liter:                  /M 

t°-       Glycerol  Layer 
(o) 

Benzene  Layer. 

(b)      ' 

to' 

t  •      Glycerol  Layer 
(a) 

CC14  Layer. 
(b) 

(a) 

25° 

0.407 

I 

.922 

4 

.72 

25° 

0.365 

0 

.565        1 

•55 

ft 

0.676 

4 

.086 

6 

.04 

u 

0 

.684 

I 

.224          ] 

.78 

tt 

1.470 

10 

.212 

6 

•95 

" 

I 

.416 

2 

.652       : 

.87 

n 

2.622 

20 

.102 

7 

.67 

" 

5 

.064 

9 

.888       'i 

•95 

n 

5.280 

42 

.458 

8 

.04 

" 

7 

.636 

14 

.766          3 

•93 

40° 

0-459 

2 

.168 

4 

.72 

40° 

o 

.322 

0 

•575 

•79 

It 

0.658 

3 

.911 

5 

•94 

tl 

o 

.690 

I 

.169        1.74 

It 

1.584 

II 

.244 

7 

.10 

tl 

i 

.224 

2 

.772        1.69 

11 

3.048 

24 

.104 

7 

.91 

" 

2 

.832 

6 

.444        2.26 

11 

46 

.960 

8 

•44 

" 

6 

•854 

15 

.410        2.25 

50° 

0.467 

2 

.194 

4 

.70 

So° 

0 

.299 

0 

.653        2.19 

It 

0.642 

3 

.864 

6 

.02 

It 

0 

•  570 

I 

.270        2.23 

" 

1.463 

II 

.196 

7 

•65 

" 

I 

•  5" 

3 

•457        2.29 

tl 

2.391 

19 

.872 

8 

•31 

It 

2 

.664 

6 

.468        2.43 

" 

46 

.782 

8 

.69 

It 

6 

.348 

16 

.008        2.52 

DISTRIBUTION  OF  IODINE  BETWEEN  GLYCEROL  AND  CHLOROFORM. 


Results  at  25°. 

(Herz  &  Kurzer,  1910.) 

Results  at  30°. 

(Hantzsch  &  Vagt,  1901.) 

Results  at  Dif.  Temps. 
(Hantzsch  &  Vagt,  1901.) 

Mols.  Iodine  per  1000 
Gms. 

c 

Mols.  Iodine  per  Liter: 

c 

Mols.  I  per  Liter: 

C 

Glycerol 

CHC13 

c' 

Glycerol 

CHC13 

c' 

Glycerol 

CHClj 

c' 

Layer  c. 

Layer  c'. 

Layer  c. 

Layer  c'. 

Layer  c. 

Layer  c'. 

0.0244 

0.0564 

O 

•43 

0.00097 

0.00172 

0.056 

O 

0.0119 

0.0177 

0.675 

0.0397 

0.0919 

0 

•43 

O.OO2O4 

0.00412 

0-495 

20 

0.0084 

0.0213 

0.400 

0.0500 

O.II5I 

0 

•43 

0.00418 

0.00898 

0.465 

40 

0.0077 

O.O22I 

0-349 

0.00782 

0.0216 

0.362 

50 

0.0074 

O.O226 

0.330 

Data  are  also  given  by  the  above  named  investigators  for  the  distribution  of 
iodine  between  aqueous  glycerol  solutions  and  chloroform  at  several  temperatures. 

DISTRIBUTION  OF  IODINE  BETWEEN  GLYCEROL  AND  ETHYL  ETHER. 

(Hantzsch  &  Vagt,  1901.) 
Mols.  Iodine  per  Liter: 


O 
30 
30 

Glycerol  Layer 
(c). 
0.00566 
0.00544 
0.00100 

Ether  Laver 
(0- 
O.027O 
0.0272 
O.OO5I 

?* 

0.21 
O.2O 
0.20 

FREEZING-POINT  DATA  (Solubility,  see  footnote,  p.  I)FOR  MIXTURES 
IODINE  AND  OTHER  ELEMENTS. 


Iodine  and  Selenium 
"    Sulfur 
44   Tellurium 
44   Tin 


(Pellini  and  Pedrina,  1908.) 

(Olivari,  1908;  Smith  and  Carson,  1908.) 

(Jaeger  and  Menke,  1912.) 

(van  Klooster,  1912-13;  Remders  and  de  Lange,  1912-13.) 


SOLUBILITY  OF  IODINE  IN  ARSENIC  TRICHLORIDE.  (Sloan  and  Mallet,  1882.) 

t°.  o°.  15°.  96°. 

Gms.  I  per  ico.gms.  AsCl3  8.42  u.88  36.89 


335  IODOEOSINE 


IODOEOSIN    (Sodium  tetra  iodofluorescein) 

loo  gms.  H2O  dissolve  90  gms.  iodoeosin  at  20-25°.  (Dehn,  1917.) 

100  gms.  pyridine  dissolve  4.63  gms.  iodoeosin  at  20-25°. 

IOO  gms.  aq.  50%  pyridine  dissolve  71.6  gms.  iodoeosin  at  20-25°. 

IODOFORM   CHI3,   IODOL   C4I4NH    (Tetraiodopyrrol). 
SOLUBILITY  IN  SEVERAL  SOLVENTS. 

(U.  S.  P.  VIII;  Vulpius,  1893.) 

Gms.  per  100  Gms.  Solvent. 
Solvent.  t°.  , * — 


Water  25  0.0106  0.0204 

Alcohol  25  2.14(1.43  gms.  (V.))        u.i 

Alcohol  b.  pt.  (10     gms.  (V.)) 

Ether  25  19.2    (16.6  gms.  (V.))        66.6 

Chloroform  25  ...  0.95 

Pyridine  20-25  I73-1    ODehn,  1917.) 

Aq.  50%  pyridine  20-25  22-4 

Lanolin  (30%  H20)  46  5.2    (Kiose,  1907.) 

IRIDIUM   CHLORIDE   IrCU. 

When  i  gm.  iridium  as  chloride  is  dissolved  in  100  cc.  of  10%  HC1  and  shaken 
at  1 8°  with  100  cc.  of  ether,  0.02  per  cent  of  the  metal  enters  the  ethereal  layer. 
When  20%  HC1  is  used  5%  of  the  metal  enters  the  ether.  When  dissolved  in  i  % 
HC1  or  in  water  approximately  o.oi  per  cent  of  the  metal  enters  the  ethereal  layer. 

(Mylius,  1911.) 

IRIDIUM  Ammonium  CHLORIDE   IrCl4.2NH4Cl. 
SOLUBILITY  IN  WATER. 

(Rimbach  and  Korten,  1907.) 
Gms.  IrCU-aNEUCl  per  100  Gms.  Gms.  IrCU.aNH^Cl  per  100  Gms. 


I    . 

Water.             Sat.  Sol. 

Water.             Sat 

.Sol. 

' 

14.4 

o  .  699        o  .  694 

52.2 

I  . 

608             I. 

583 

26.8 

o  .  905        o  .  899 

61.2 

2  . 

I3O            2. 

068 

39-4 

1.226            I.I24 

69-3 

2. 

824            2. 

746 

IRIDIUM 

DOUBLE    SALTS 

v 

SOLUBILITY  IN  WATER. 

(Palmaer  —  Ber.  23,  3817;  24,  2090,  '91.) 

Double  Salt. 

Formula. 

t°. 

Gnu 

per 

Irido 

Pentamine  Bromide 

Ir(NH3)5Br3 

12.5 

O. 

W 

<i 

U 

Bromonitrate 

Ir(NH3)sBr(N03)3 

18 

5. 

58 

« 

It 

Tri  Chloride 

Ir(NH3)5Cl3 

i5-i 

6. 

53 

U 

11 

Chloro  Bromide 

Ir(NH3)5QBr2 

15 

0. 

47 

n 

« 

Chloro  Iodide 

Ir(NH3)5ClI2 

15 

0. 

95 

K 

U 

Chloro  Nitrate 

Ir(NH3)5Cl(N03)2 

15-4 

i. 

94 

it 

tt 

Chloro  Sulphate 

Ir(NH3)5ClSO4.2H2O 

15.0 

0. 

74 

ft 

tt 

Nitrate 

Ir(NH3)5(N03)3 

16 

0. 

28 

« 

Aquo  Pentamine  Bromide 

Ir(NH3)6(OH2)Br3 

ord.  temp. 

25.0 

« 

« 

Chloride 

Ir(NH3)5(OH2)Cl3 

ord.  temp. 

74. 

7 

« 

tt 

Nitrate 

Ir(NH3)5(OH2)(N03)3 

i? 

IO. 

o 

IRON   BROMIDE    (Ferrous)    FeBr2.6H2O. 

SOLUBILITY  IN  WATER. 

(Etard  —  Ana.  chim.  phys.  [7]  2,  537,  '94.) 


A  o             Gms.  FeBr2           A  o 
*  '        per  loo  Gms.  Sol. 

Gms.  FeBr2             t  0             Gms.  FeBrs 
per  loo  Gms.  Sol.                     per  100  Gms.  Sol. 

—  20 

47-0 

30 

55-o 

60 

59-o 

0 

50-5 

40 

56.2 

80 

61.5 

20 

5,3-5 

IOO 

64.0 

IRON  CARBONATE  336 

IRON   CARBONATE   (Ferrous)   FeCO3. 

SOLUBILITY  OF  FERROUS  CARBONATE  IN  AQUEOUS  SALT  SOLUTIONS,  BOTH 
WITH  AND  WITHOUT  THE  PRESENCE  OF  CARBON  DlOXIDE. 

(Ehlert  and  Hempel,  1912.) 

(Each  mixture  was  1000  cc.  in  volume  and  was  rotated  constantly  for  24  hours. 
Temp.,  probably  5-8°.) 


SOLUBILITY  IN  PRESENCE 

OF   CO2  (2  atmospheres  pressure). 


SOLUBILITY  IN  ABSENCE 
OF  CO2. 


Aqueous  Solution  of: 

r~ 
Cms.  Salt  per 
1000  Cms.  H2O. 

Cms.  FeCO3  per 
1000  cc.  Solvent. 

Cms.  Salt  per        Cms.  FeC03  per 
1000  Cms.  H2O.      1000  cc.  Solvent.. 

Water  alone 

0 

6.I9I 

NaCl 

.  .  . 

351-2 

0-350 

MgCl2.6H2O 

86.9 

5.840 

« 

700 

4-555 

tt 

1150 

4-459 

.  .  . 

.  .  . 

tt 

1437-5 

4-693 

.  .  . 

.  .  . 

n            * 

1725 

5.398 

.  .  . 

.  .  . 

tt 

2300 

9.052 

2300 

4-205 

Na2S04.ioH20 

137-7 

7-943 

137-7 

0.701 

a 

Sat.  at  14° 

9-578 

Sat.  at  14° 

0-934 

MgSO4.7H2O 

ioS-3 

6.242 

io5-3 

1.467 

tt 

Sat.  at  14° 

7-392 

Sat.  at  14° 

2-933 

IRON  BICARBONATE   (Ferrous)   Fe(HCO3)2. 

SOLUBILITY  OF  FERROUS  BICARBONATE  IN  CARBONATED  WATER  AT  30°. 

(Smith,  H.  J.,  1918.) 

Pure  white  ferrous  carbonate  was  prepared  by  heating  to  100°  for  several 
days  in  a  steel  bottle,  an  aqueous  solution  of  ferrous  sulfate,  sodium  bicarbonate 
and  carbon  dioxide  (introduced  at  400  Ibs.  pressure).  The  crystalline  product 
was  similar  to  the  mineral  siderite  and  was  probably  isomorphous  with  calcite. 
Fifty  to  one  hundred  gram  portions  were  placed  in  a  two- liter  steel  bottle,  coated 
on  the  inside  with  a  mixture  of  beeswax  and  Venice  turpentine.  Water  was  added 
and  CO*  introduced  through  a  needle  valve  from  a  cylinder  of  the  liquefied  gas. 
The  pressure  was  read  on  a  gauge.  The  bottle  was  rotated  at  constant  tempera- 
ture for  several  days  or  until  equilibrium  was  reached.  The  portion  of  the 
saturated  solution  for  analysis  was  withdrawn  through  a  brass  tube  attached  to 
the  valve  on  the  inside  of  the  bottle  and  packed  with  cotton  to  act  as  a  filter.  The 
filtered  portion  was  received  in  a  tared  evacuated  flask,  containing  a  few  cc.  of 
cone.  HjSCX  The  CO2  was  determined  by  absorption  and  the  iron  by  precipitation, 
resolution,  reduction  and  titration  with  permanganate.  The  results  show  that 
the  decomposition  tension  of  Fe(HCO3)2  is  greater  than  25  atmospheres  at  25°. 


Cms.  Mols.  per  Liter. 

Cms.  per  Liter. 

Cms.  Mols.  per  Liter. 

Cms.  per  Liter. 

•H2C03. 

Fe(HC03)2. 

'H2C03. 

Fe(HCO3)2. 

H2C03. 

Fe(HC03)2. 

H2C03. 

Fe(HCO3)2. 

0.1868 

0 

.00245 

II 

-58 

0.436 

0.3294 

0 

.00311 

20 

•43 

0-553 

0.1985 

0 

.00256 

12 

•3i 

0-455 

0-3745 

0 

•00315 

23 

•23 

0.560 

0.2168 

0 

.00262 

13 

•45 

0.466 

o  .  4046 

o 

.00332 

25 

.09 

0.590 

0.2327 

0 

.00274 

14 

•43 

0.487 

0.4750 

o 

.00348 

29 

•45 

O.6l9 

o  .  2960 

0 

.00303 

18 

•35 

0-539 

o  .  6600 

0 

.00402 

40 

•93 

0.715 

0.3116 

o 

.00304 

19 

•32 

0.541 

0.7154 

0 

.00418 

44 

•36 

0.744 

0.3153 

0 

.00318 

19 

•55 

0.566 

0.7600 

o 

•00434 

47 

•13 

0.772 

IRON   CHLORIDE   (Ferrous)   FeCl2.4H2O. 

100  gms.  sat.  sol.  in  water  contain  17.54  gms.  Fe  =  39.82  gms.  FeCl2  at  22.8°. 
loo  gms.  sat.  sol.  in  water  contain  18.59  gms.  Fe  =  42.8    gms.  FeCl2  at  43.2°. 

(Boecke,  1911.) 


337 


IRON  CHLORIDE 


IRON  CHLORIDE   (Ferrous)   FeCl2.4H2O.     SOLUBILITY  IN  WATER. 

(Etard.) 


10 

IS 
25 
30 
40 

50 


Gms.  FeCl2 

per  100  Gms. 

Solution. 

39-2 

4O.O 

41-5 
42.2 

43-6 
45-2 


Solid  Phase. 


t°. 

60 
80 

87 
90 

100 
120 


Gms.  FeCl2 

per  100  Gms. 

Solution. 

47-o 
50.0 

51.2 
51-4 

51.8 


Solid  Phase. 


FeCl2.4H2O+FeCl8 


SOLUBILITY  OF  IRON  CHLORIDE 

(Roozeboom  —  Z.  physik. 


Mols.F< 

t°.   per  100  Mols, 
H20. 


Cms.  FeCla  per  100 
Cms. 


(FERRIC)  Fe2Cl6  IN  WATER. 

Chem=  10,  477,  '92.) 

Gms.  FeCla  per  too 


Mols. 
per  100 


ols. 


_,    -- 
Gms. 


H7O.       Solution. 
Solid  Phase,  Fe2Cl6.i2H2O. 

-55  2.75  49-52  33-J2 

-27  2.98  53.60  34-93 

o  4-13  74-39  42-66 

+  20  5.10  91.85  47.88 

30  5.93  106.8  51.64 

37  8.33  150-0  60. 01 

30  i i. 20  201.7  66.85 

20   12.83   231.1    69.79 

8     13.7      246.7      71.15 

Solid  Phase,  Fe2Cl6.7H20. 

20      11-35      204.4  67.14 

32      13.55      244.0  70.92 

30      15.12      272.4  73.13 

25      15.54      280.0  73.69 

Solid  Phase,  Fe2Cl6.sH2O. 

12      12.87      231.8  69.87 

27      14.85      267.5  72.78 


35 

50 
55 
55 


j.          H2O.        Solution. 
Solid  Phase,  FesCla-sHsO  (con.). 

15.64  281.6  73.79 

17.50  315.2  75.91 

19.15  344.8  77.52 

20.32  365.9  78.54 


Solid  Phase,  Fe2Cl6.4H2O. 
50        19.96      359.3      78.23 


55      20.32  365.9 

60        20.70  372.8 

69  21.53  387.7 

73-5  25-0  450-2 

70  27.9  502.4 
66      29.2  525.9 

Solid  Phase,  Fe2Cl&. 

66   29.2  525.9 

75   28.92  511.4 

80   29.20  525.9 

100   29.75  535-8 


78.54 
78.86 

79-50 
81.81 

83.41 
84.03 

84.03 
83.66 
84.03 
84.26 


SOLUBILITY  OF   FERRIC  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF 
AMMONIUM  CHLORIDE  AT  25°,  35°,  AND  45°. 

(Mohr  —  Z.  physik.  Chem.  27,  197,  '98.) 


Results  at  25°.     Results  at  35°.     Results  at  45°. 


Mols.  per 
100  Mols.  H2O. 

Mols.  per 
100  Mols.  H2O. 

Mols.  per 
100  Mols.  H2O. 

NH4C1. 

FeCl3. 

NH4C1. 

Fed,. 

NH4C1. 

FeCla. 

O 

10.98 

O 

J3-36 

0-0 

33-4 

!-57 

10-74 

I.4I 

13-05 

2.48 

9-02 

3-08 

9.28 

4.08 

9-58 

5-28 

7-73 

6.98 

7-64 

.  .  . 

9-59 

6-77 

10.76 

6.70 

13.09 

6^31 

9-83 

6.70 

II.  60 

6-52 

13-54 

6.28 

9-65 

6.07 

12.28 

6.08 

12.91 

5-49 

9-93 

5-23 

n-57 

3-98 

13-49 

4.84 

9-92 

3-97 

11.89 

3-38 

13.46 

4.99 

10.31 

2.05 

13-23 

1-38 

I3-30 

0-0 

14-79 

o-o 

i6!28 

0-0 

Solid  Phase 
in  Each  Case. 

Fe2Cl«.i2H20(5.H2Oat4S0) 
Hydrate  +  Double  Salt 
Double  Salt 


Double  Salt  +  Mixed  Ciystals 
Mixed  Crystals 


IRON  CHLORIDE 


338 


SOLUBILITY  OF 

FERRIC  CHLORIDE   IN  AQUEOUS  SOLUTIONS 

OP 

AMMONIUM  CHLORIDE  AT  15°. 

(Roozeboom  —  Z.  physik.  Ch. 

10,  148,  '92.) 

Mols.  per  100  Mols.H2O. 

Grams  per  ipo  Gms.HjO. 

Solid 

NH4C1. 

FeCl3. 

'NHjCl.            FeCl3> 

Phase. 

o.o 

9-30 

o.o          83.88 

Fe2Cl«.i2H2O 

1.09 

9-57 

3.24           86.32 

44 

1.36 

9-93 

4.03           9I.6l 

Fe2Cl6.i2H20  -f  Double  Salt 

2-OO 

9.27 

5.92            83.64 

Double  Salt 

2-79 

8.71 

8.3I            78.77 

" 

4-05 

8.09 

12.  08            73.  2O 

" 

6.41 

7.18 

19.12            64.83 

«4 

10.78 

6.21 

32.04            56.00 

" 

7.82 

6-75 

23.21            60.83 

Mixed  Crystals  containing  7.29% 

FeCJ, 

7.62 

5-94 

22.63            53.47 

5.55 

" 

7.70 

5-03 

22.90            45-42 

4-4 

M 

7.8l 

4-34 

23.23            39-I3 

"                   M              3-8 

It 

S-52 

2.82 

25-33            25.43 

1.64 

<( 

10.95 

0.68 

32.55               6-15 

"                   "              0.31 

II 

u.88 

o.o 

35-30         o.o 

NILC1 

SOLUBILITY  OF  FERRIC  CHLORIDE  IN  AQUEOUS  HYDROCHLORIC  ACID 
SOLUTIONS  AT  DIFFERENT  TEMPERATURES. 

(Roozeboom  and  Schreinemaker  —  Z.  physik.  Chem.  15,  633,  '94.) 


Mols.  per  TOO 
H,0. 

Mols. 

Gms.  per  100  Gms.                   Mols 
H20.                  Solid 

.  per  100  Mols 
H20. 

.    Gms.  per  100  Gms. 
H20.                Solid 

HC1. 

FeCl3. 

HC1. 

FeCl8.    *****'        HC1.         FeCl3: 

'HC1. 

FeCl3.    Phase 

Results  at  o°. 

Results  at  25°  (con.). 

O 

8 

•25 

0 

74 

3° 

0. 

0 

29.00 

0.0 

26l.I 

7-52 

6 

•51 

15.22 

58 

62 

7. 

5 

29.75 

15.18 

267.9 

Fe2Cl6 

13.37 

6 

-33 

27.06 

57 

01 

19. 

35.25 

39-46 

317.4 

•5    2M 

16.80 

8 

-70 

33-99 

78 

34 

19. 

5 

35-25 

39-46 

3I7-4 

18.45 

10 

•23 

37-34 

92 

10 

FeaCl«      20, 

6 

35-34 

41.68 

20.40 

15 

.40 

41.28 

138 

7 

.i2H203I> 

34 

41.58 

63.42 

374-4 

^|u) 

20.10 

16 

.00 

40.67 

144 

i 

33- 

00 

43-0° 

66.77 

387.3 

19.95 

17 

•70 

40.37 

159 

4 

34- 

65 

44-80 

70.11 

403.4 

19.00 

22 

•75 

38.45 

204 

8 

40. 

4i 

40.25 

81.77 

362.4 

1  FeCl« 

18.05 

23 

.41 

36-53 

210. 

8  . 

39- 

03 

41.38 

78.98 

372.7 

[  C2.2HC1 

18.05 

23 

.40 

36-53 

2IO. 

8 

^fflzO  35< 

74 

45-24 

72-33 

407.4 

J    +  4H2O 

19.50 

25 

•93 

39-55 

233-5    J 

Results  at  AO°. 

24.  12 
26.0O 
26.00 
34.60 

37-27 
34.60 

30 
32 
32 

36 
38 

.04 
.16 
.16 
.11 
.60 
.11 

48.81 
52.60 
52.60 
70.01 

75-41 
70.01 

270. 
289. 
289. 

343- 
329. 
343- 

i 

6 

2 

6 

2 

F^fc>^4 

Fe2HCl    2o  ° 

-fW)  2° 

32.4 
37.45 
37-45 
50.80 
58.0 
50.8 

0.0 

27.11 

27.11 
54.64 

o.o 

54.64 

291.7 
337-3 
337-3 
457-5 
522.3 
457-5 

1   Ferf* 

Results  at  25°. 

42. 

01 

48.64 

85.00 

438.  oj 

O.O 

IO 

.90 

o.o 

98 

IS^\            42. 

50 

47-52 

86.72 

428.0 

)  Fe2Cl« 

2-33 

23 

.72 

4.715 

213 

6  r  j  2  jf  o  42  • 

OI 

48.64 

85.00 

438-0 

i    +4H2O 

0.0 

24 

•5 

0.0 

220 

7  J  '' 

0.0 

2.33 
7.50 

23 
23 
29 

•5 
.72 

-75 

o.o 

4.715 
15.18 

211. 
267! 

6  i                    Results  for  other  temperatures 
4  1  Fe2ci«        are  also  given   in  the  original 

g    f      .yHaO      paper. 

0.0 

31 

•50 

0.0 

283. 

6  J 

339 


IKON   CHLORIDE 


RESULTS  FOR  THE  SYSTEM  FERRIC  OXIDE,  HYDROCHLORIC  ACID,  WATER  AT  25°. 

(Cameron  and  Robinson,  1907.) 

(Excess  of  ferric  hydroxide  was  added  to  aq.  ferric  chloride  solutions  and  agi- 
tated for  3  months.) 


Gms.  per  100  Gms. 
Sat.  Sol. 

Solid  Phase.              o  f?  £, 

Gms.  per  too  Gms. 
Sat.  Sol. 

Solid  Phase. 

Fe2O3.              HCl.                                                                         FejOs. 

HCL  ' 

34 

.61 

59 

.88 

FeCl3.HC1.2HtO                1.485 

21 

.84 

29 

-33  { 

FeCl3.6H20+ 
Fe203.*HCl.H2O 

33 

•27 

60 

•23 

" 

•349 

16 

.82 

22 

•55 

Fe2Oa.itHCl.H2O 

32 

•78 

54 

+  FeCl3 

.321 

15 

•83 

21 

.10 

" 

•95 

58 

.20 

FeCV+FeCU^HjO 

.284 

14 

.62 

19 

•53 

« 

34 

.42 

54 

.12 

FeCl3.2HjO 

.242 

12 

•59 

16.61 

35 

.22 

59 

.28 

" 

.220 

II 

.76 

15 

.28 

• 

34 

.07 

55 

.71 

I.I95 

10 

•56 

13 

.76 

• 

34 

.21 

55 

•47 

+FeCl3.2jH20     1.158 

8 

.60 

II 

.24 

" 

34 

•44 

51 

.11 

FeCl3.3JH20+  "              I.H5 

6 

•47 

8 

•39 

• 

33 

.04 

46 

.72 

"  +FeCl3.6H2O            1.070 

4 

.04 

5 

•36 

(C 

24 

.42 

33 

.40 

FeCU.6H20              1  .  047 

2 

•85 

3 

.66 

" 

Data  for  the  systems  FeCl2  +  MgCl2  +  KC1  +  H2O  at  22.8°  and  for  FeCl2  + 
KC1  +  NaCl  are  given  by  Boeke,  1911. 

100  gms.  abs.  acetone  dissolve  62.9  gms.  FeCl3  at  18°.  (Naumann,  1904.) 

100  gms.  anhydrous  lanolin  (m.  pt.  about  46°)  dissolve  4.17  gms.  FeCl3  at  45°. 

(Klose,  1907.) 

DISTRIBUTION  OF  FERRIC  CHLORIDE  BETWEEN  WATER  AND  ETHER  AT  18°. 

(Mylius,  1911.) 

One-gram  portions  of  iron  as  chloride  were  dissolved  in  100  cc.  of  aq.  HCl  of 
different  concentrations  and  shaken  with  100  cc.  of  ether  in  each  case.  The  per- 
centage of  iron  in  the  ethereal  layer  was  determined  after  separation  of  the  two 
layers. 

Per  cent  cone,  of  Aq.  HCl  i        5        10      15      20 

Per  cent  of  Iron  Extracted  by  Ether          (o.oi)    o.i      8      92      99 

Fusion-point  curves  (solubility,  see  footnote,  p.  i)  for  mixtures  of  FeCl3  +  PbCl2 
and  FeCl3  +  ZnCl2  are  given  by  Herrmann,  1911,  and  for  mixtures  of  FeCl3+TlCl 
by  Scarpa,  1912. 


SOLUBILITY  OF  THE  SALT  PAIR  FeCl3.NaCl  IN  WATER  AT  21°. 

(Hinrichsen  and  Sachsel,  1904-05.) 


Gms.  Used. 

Gms.  per  100  Gms. 
Solution. 

G.  Mols. 
per  100  Mols.  H2O. 

Solid  Phase. 

FeCl3. 

NaCl.' 

FeCl3. 

NaCl. 

FeCl3. 

NaCl.  " 

0 

3-6 

0 

36.10 

0 

II.  2 

NaCl 

1.8 

3 

24.27 

9.10 

2.69 

2.8 

Mix  Crystals 

3-6 

2-5 

25.40 

8-45 

2.81 

2.6 

tt 

5-5 

2 

26.40 

5-25 

2.93 

2-54 

« 

7.2 

i-5 

38.15 

3.90- 

4-23 

1.22 

tt 

9 

i 

45.38 

2-45 

5-03 

o-75 

u 

10.8 

o-5 

46.75 

2.  II 

5-i8 

0.65 

tt 

10.8 

0 

83.39 

0 

9-3 

o 

FeCla 

IRON  CHLORIDE 


340 


SOLUBILITY  OF  THE  SALT  PAIR  FeCl3.KCl  IN  WATER  AT  21°. 

(Hinrichsen  and  Sachsel,  1904-05.) 


Cms.  Used. 


Fed,. 

O 
13 

18 

23 
28 


KCl. 

35 
28 

21 


16 


36.2       9 

46.5       6 

155  o 


Gms.  per  100  Gms. 
Solution. 

Gms.  Mols.  per  100 
Mols.  H20. 

Solid  Phase. 

FeClj. 
O 

13-44 
23.18 
28.05 

KCl.  ' 

34-97 
24-45 
16.54 
11.69 

FeCl3. 
0 
1.49 
2-57 

3-« 

KCl. 

8-45 
5-90 

3-99 
2.82 

KCl 

Mix  Crystals 

35-72 

11.68 

3-96 

2.82 

" 

36.62 

11.19 

4.06 

2.70 

FeCl3.2KCl.H20 

37-35 

13.67 

4.14 

3-30 

a 

51.69 

7-54 

5-73 

1.82 

a 

83-89 

0 

9-3 

0 

.      FeCl3 

SOLUBILITY  OF  THE  SALT  PAIR  FeCl3.CsCl  IN  WATER  AT  21°. 

(H.  and  S.) 


Gms.  Used. 

Gms.  per  100  Gms. 
Solution. 

Gms.  Mols.  per  100 
Mols.  H,0. 

Solid  Phase. 

FeCl3. 

CsCl. 

'  FeCl3. 

CsCl. 

FeCl3. 

CsCl.  ' 

O 

65 

0 

65 

0 

6-95 

CsCl 

0.6 

ii.  6 

0-45 

55-18 

0.05 

5-9 

FeCl3.3CsCl.H2O 

1-4 

10.2 

2.1 

52.38 

0.23 

5-6 

ts 

2.2 

8.8 

5-24 

5J-44 

o-57 

5-5 

(( 

2 

74 

7-8 

47.70 

0.86 

5-i 

FeCl3.2CsCLH2O 

3-8 

6 

8-93 

4i-i5 

0.99 

4-4 

u 

4-6 

4-6 

15-34 

25-25 

1.70 

2.7 

n 

5-4 

2.8 

21.65 

14.96 

2.40 

1.6 

(i 

6.2 

1.4 

27.96 

8.42 

3.10 

0.9 

ti 

35 

0.2 

48.71 

0.94 

5-40 

O.I 

n 

35 

0 

83-89 

o 

9-3 

o 

FeCla 

IRON  FORMATE   (Ferric)   Fe3(OH)2(HCOO)7.4H2O. 

SOLUBILITY  IN  WATER  AND  IN  ABSOLUTE  ALCOHOL. 

(Hampshire  and  Pratt,  1913.) 


15 
20 

25 

30 

35 


Solubility  in  Water. 
Gms.  Salt 

per  100  Gms.  Solid  Phase. 

H20. 

Fe3(OH)2(HCOO)74H2O 


Solubility  in  Abs.  Alcohol. 

Gms.  Salt 

t°.  per  100  Gms. 

QH6OH. 


5-08 

5-52 
6.10 
6.78 
7-52 


19 

22 
23 


4-59 
6.25 
7.62 


(The  sat.  solutions  are  not  stable.) 


341 


IRON  HYDROXIDE 


IRON  HYDROXIDE   (Ferric)   Fe(OH)3. 
SOLUBILITY  OF  FERRIC  HYDROXIDE  IN  AQ.  OXALIC  ACID  SOLUTION  AT  25°. 

(Cameron  and  Robinson,  1909.) 

The  solutions  were  constantly  agitated  for  3  months.  The  solubility  is  directly 
proportional  to  the  concentration  of  the  oxalic  acid  and  no  definite  basic  ferric 
oxalate  is  formed. 

Gms.  per  100  Gms.  Sat.  Sol. 
Fe2O3.  CA 

0.48        0.61 

0.95  1.23 

1.86        2.45 


Gms.  per  100  Cms.  Sat.  Sol. 


Sat.  Sol. 


1.007 
I.OI5 
I.03I 


Sat.  Sol. 
1.040 
1.050 
1.064 


2-33 

2.98 
3.62 


5.17 


IRON  NITRATE   (Ferric)   Fe(N03)3.9H20. 

EQUILIBRIUM  IN  THE  SYSTEM,  FERRIC  OXIDE,  NITRIC  ACID  AND  WATER  AT  25°. 

(Cameron  and  Robinson,  1909.) 

Solutions  of  ferric  nitrate  of  varying  concentrations  were  shaken  with  freshly 
precipitated  ferric  hydroxide  at  const,  temp.,  25°,  for  4  months.  The  acid  branch 
of  the  curve  was  studied  in  a  similar  manner  by  starting  with  ferric  nitrate  and 
various  concentrations  of  nitric  acid.  No  definite  basic  nitrates  of  iron  were 
formed. 


^25  Of  | 

Gms 

.  per  100  Gms. 
Sat.  Sol.                  solid  Phase.  •       c. 

dys  of 
it    Sol 

Gms.  per  100  Gms. 
Sat.  Sol.     • 

Solid  Phase. 

Fe2O3.        N2O5. 

,t.    OUl. 

'  FeA. 

NA.: 

.032 

I 

.78 

2 

.21   FeA  m  NA  n  H2O 

I 

•452 

12 

.14 

33- 

5 

FeA.3NA.i8HjO 

:°79 

3 

•99 

5 

.61 

I 

•434 

9 

•95 

36. 

3 

" 

.127 

5 

•79 

9 

" 

I 

.417 

7 

•25 

40. 

3 

" 

.177 

7 

.22 

12 

.31 

I 

.404 

5 

.02 

47- 

5 

" 

.264 

9 

.70 

16 

.60 

I 

.428 

3 

•55 

51. 

5 

" 

.368 

12 

.48 

22 

.70 

I 

•450 

4 

.51 

52 

* 

•435 

14 

.62 

28 

•13 

I 

•465 

4 

•19 

55- 

2 

" 

.498 

15 

.40 

29 

.52 

I 

.407 

3 

•93 

47- 

2 

FeA.4NAi8H20* 

.496 

15 

.22 

30 

.50  FeA.3N205.i8H20 

I 

.419 

3 

•52 

49- 

6 

" 

This  salt  was  obtained  accidentally  and  its  preparation  could  not  be  repeated. 


IRON  NITRATE   (Ferrous)   Fe(NO3)2.6H2O. 

SOLUBILITY  IN  WATER. 

(Funk,  1900.) 


t°. 

27 
21.5 

19 
15.5 

Gms. 
Fe(NOs)2 
per  100 
Gms. 
Sol. 

35-66 
36.10 
36.56 
37-17 

Mols. 
Fe(NO3)2 
per  100 
Mols. 
H20. 

5-54 
5-64 
5-76 
5-9i 

Solid  Phase. 


Gms. 

Mols. 

Fe(N03)2 

Fe(NO^ 

t°. 

per  100 

Gms. 

per  100 
Mob 

Sol. 

H20 

-9 

39-68 

6.$7 

0 

4L53 

7.10 

18 

45-14 

8.23 

24 

46.51 

8.70 

Solid  Phase. 


Fe(NOl)2.6HlO 


60.5      62.50      16.67 


Density  of  solution  saturated  at  18°  =  1.497. 


IRON    OXALATE  342 

IRON   OXALATE   (Ferrous)   FeC204.2H2O. 

SOLUBILITY  IN  WATER>T  25°  DETERMINED  BY  THE  CONDUCTIVITY  METHOD. 

(Schafer,  1905.) 

The  sat.  solution  contains  5.38.  10-*  gm.  mols.  C2O4  per  liter. 
IRON   OLEATE. 

100  gms.  glycerol  (d  =  1.114)  dissolve  0.71  gm.  iron  oleate.  (Asselin,  1873.) 

IRON    OXIDES,    HYDROXIDE   and   SULPHIDE. 

SOLUBILITY  IN  AQUEOUS  SUGAR  SOLUTIONS. 

(Stclle  —  Z.  Ver  Zuckerind.  50,  340,  'oo.) 

%  <?IIMT  One  Liter  of  Sugar  Solutions  Dissolves  Milligrams  of: 

te  Sol-          Feg(OH)6  at;  Fe?O3  at:          _  Fe3O4  at:  _  FeSatt 

vent.     i7.4<>.      ^        5?.        17.5°.'         4!*      '  17.5°-       45^          75°^      17-5°.         ^      7?T 

10  3.4  3-4  6.1  1.4  2.0  10.3  10.3  12.4  3.8  3.8  5.3 
30  2.3  2.7  3.8  1.4  ...  12.4  10.3  12.4  7.1  9.1  7.2 
50  2.3  1.9  3.4  0.8  i.i  14.5  10.3  14-5  9-9  19-8  9.1 

IRON    PHOSPHATE    Fe2(PO4)3. 

THE  ACTION  OF  WATER  AND  OP  AQUEOUS  SALT  SOLUTIONS  UPON 
FERRIC  PHOSPHATE. 

(Lachowicz  —  Monatsh.  Chem.  13,  357,  '92;  Cameron  and  Hurst  —  J.  Am.  Chem.  Soc.  26,  888,  '04.) 

The  experiments  show  that  the  ordinary  precipitation  methods  for 
the  production  of  ferric  phosphate  give  products  which  do  not  conform 
to  the  formula  Fe2(PO4)3.  By  digesting  such  samples  with  water 
very  little  is  dissolved,  but  the  material  is  decomposed  to  an  extent 
depending  upon  the  relative  amounts  of  solid  and  solvent  used.  The 
amount  of  PO4  dissolved  per  gram  of  Fe2(PO4)3  varies  from  about 
0.0026  gram  removed  by  5  cc.  H2O  to  0.0182  gram  removed  by  800  cc, 
H2O  at  the  ordinary  temperature. 

SOLUBILITY  FERRIC  PYROPHOSPHATE  IN  AQ.  AMMONIA  AT  o°.    (Pascal,  1909.) 
The  solutions  containing  an  excess  of  salt  were  agitated  violently  every  half 

hour  for  seven  hours  and  filtered  at  o°.     The  sat.  sol.  was  analyzed  for  ammonia 

and  for  residue  obtained  by  evaporation. 


Gms.NH3        F<.{??n  Gms.NH3 

P^Sol"13'  Pe^ioo^s.  Solid  Phase.  P^gms.  pem's.         Solid  Phase. 

0.884  5.606                 Fe«(PA)i  •••5*92  14-71        viscous  black  deposit 

1.59  9-75                         "  8.26  13.89       chamois  colored  lumps 

3.71  14-85                          "  10.55            7.40 

4.72  15.94  15.96            2.52 
5.93  I3-92  viscous  black  deposit  18.83           °-445 
7.91  14.61 

SOLUBILITY  OF  FERRIC  PHOSPHATE  IN  AQ.  PHOSPHORIC  ACID  SOLUTIONS  AT  25°- 

(Cameron  and  Bell,  1907.) 

Solid  ferric  phosphate  of  unknown  composition  was  constantly  agitated  with 
aq.  phosphoric  acid  solutions  of  concentrations  up  to  5%  for  4  months.      Analy 
of  the  sat.  solutions  and  solid  phases  were  made. 


ses 


^of 

Gms.  per  100  Gms.  Sat.  Sol. 

Solid  Phase. 

Sat.'  Sol. 
.0074 
.0162 
.0244 
.0310 
•0383 

FeA-                  PA.    ' 
O.OIO5            0.942 
0.0205            1-984 
0.0384            2.838 

0.0611        3.770 
0.0849        4.706 

Solid  Solution 
it 

343 


IRON  SULFATB 


SOLUBILITY  OF  FERROUS  SULFATE 

IN  WATER. 

(Fraenckel,  1907.) 

Gms.  FeSO4 

Gms. 

f 

per  100            Solid  Phase. 
Gms.H2O. 

t°.         FeSO4penoo           Solid  Phase. 
Gms.  H2O. 

—  o. 

172 

I.OI56                Ice 

45 

.18 

44 

•32 

FeSO4.7H2O 

—  o. 

566 

4.2^2 

50 

.21 

48 

.60 

" 

—  I  . 

063 

8.7054 

52 

50 

.20 

" 

—  I  . 

511 

12.713 

54-03 

S2 

.07 

" 

—  I. 

771 

14.511 

56 

.56  ti 

r.  pt«54  . 

58 

(1       I   T7|»Cf\      . 

H,0 

—  I  . 

82Eutec 

.17.53         Ice+FeS04.7H20 

60 

.OI  / 

54 

•95 

FeS04.4H2O 

0 

15.65               FeS04.7H20 

65 

55 

•59 

"      unstable 

+  10 

20.51 

70 

.04 

56 

.08 

"            " 

15- 

25 

23.86 

64 

.8tr. 

Pt. 

.  .       FeSO4.4H2O+FeSO4.H2O 

20. 

13 

26.56 

68 

.02 

52 

•31 

FeSO4.H2O 

25- 

O2 

29.60 

77 

1 

45 

.90 

" 

30. 

03 

32.93 

80 

.41 

43 

-58 

" 

35-07 

36.87 

85 

.02 

40 

.46 

" 

40. 

05 

40  .  2O                       " 

90 

-13 

37 

.27 

" 

<Zl6.6 

of  sat. 

sol.  =  1.219] 

(Greenish  and  Smith, 

1903.) 

SOLUBILITY  OF  FERROUS  SULFATE  IN  AQ.  SOLUTIONS  OF  LITHIUM  SULFATE  AT  30°. 

AND  VICE  VERSA.      (Schreinemakers,  1910.) 


Cms.  per  100  Cms.  Sat.  Sol." 

'    FeS04. 
24.87 

Li2SO4. 
0 

FeSO4.7H2O 

24-45 

4 

tt 

21.15 

5-58 

(i 

18.79 

ii.  16 

a 

16.51 

15.81 

u 

16.11 

16.50 

11  +Li2S04. 

Gms.  per  100  Cms.  Sat.  Sol. 


FeSO4. 

15-39 
12.68 

5-32 

3-74 
o 


Li2S04. 

16.80 

18.31 
22.15 

23-I5 
25.1 


Solid  Phase. 

Li2SO4.H2O 


EQUILIBRIUM  IN  THE  SYSTEM  FERRiCiOxiDE,  SULFURIC  ACID  AND  WATER  AT  25°. 

(Cameron  and  Robinson,  1907.) 

(Excess  of  freshly  precipitated  ferric  hydroxide  was  added  to  ferric  sulfate  solu- 
tions of  varying  concentrations  and  the  mixtures  constantly  shaken  for  4  months.) 


d 

c~ 

25  Of 

t    Snl 

Gms.  per  100  Gms. 
Sat.  Sol. 

Solid 

Phasp 

Gms.  per 
Sat. 

100  Gms. 
Sol. 

Solid 
Phase. 

OU 

L.  OOl. 

Fe203. 

S03/ 

jrnase. 

Fe2O3.           SO3. 

I 

.001 

0 

.07 

o 

.11 

Solid  Solution 

20 

.48 

26. 

18 

Fe2O3.3SOs.  ioH20 

I 

.Oil 

O 

.62 

0 

-94 

" 

*9 

•77 

28. 

93 

it 

I 

•045 

2 

•03 

2 

-65 

u 

10 

.87 

31. 

35 

Fe2O3.4S03ioH2O 

I 

.131 

6 

.18 

7 

.40 

t( 

0 

.16 

tt 

I 

.217 

IO 

•03 

ii 

.84 

0.07 

41. 

19 

u 

I 

.440 

15 

.90 

20 

.70 

M 

I 

•05 

42. 

43 

t( 

SOLUBILITY  OF  FERRIC  SULFATE  AND  OF  FERROUS  SULFATE  IN  AQ. 
SOLUTIONS  OF  SULFURIC  ACID  AT  25°.     (Wirth,  1912-13.) 

Results  for  Ferric  Sulfate.  Results  for  Ferrous  Sulfate. 


Normality  of 
used  Acid. 

2.25 
6.685 
19.84 

Gms.  per  100  Gms.  Sat. 
Sol. 

Normality  o 
used  Acid. 

2.25 
10.2 
12.46 

I5-I5 
19.84 

,  Gms.  per  100  Gms.  Sat. 
f                    Sol. 

Solid  Phase. 

FeSO4.7H2O 

a 

FeS04.H2O 
tt 

« 

FeA 

9-99 

5-82 
O.O2 

=  Fe2(S04)3. 
25.02 
14.58 
0.05 

FeA      = 
IO 

5-414 
3.8l6 
2.  II 

0.08 

FeS04. 
19.03 
10.30 
7.26 
4.015 
0.1522 

IRON   SULFATE 


344 


EQUILIBRIUM  IN  THE  SYSTEM  FERRIC  OXIDE-SULFUR  TRIOXIDE- WATER  AT  25°. 

(Wirth  and  Bakke,  1914.) 

(The  mixtures  were  shaken  for  3-4  weeks.) 


Gms.  pe 
Si 

;r  100  Gms. 
t.  Sol. 

Solid  Phase, 
not  det. 

prob.  Fe2(S04)3.H2S04.9H20 
+Fe2(S04)3.H2S04.3H20 
Fe2(SO4)3.H2SO4.8H2O 
"  +Fe(S04)3.H2S04.3H20 
Fe(S04)3.H2SO4.8H2O 

unstable 

Gms 

.per 
Sat. 

100  Gms. 

Sol. 

Ft 
O 

3 
6 
9 

12 
13 
13 

.24 

•53 

•65 
•39 
•03 
•27 
.68 

S03. 

7I-23 
56.84 

»  1 

32.15 
31-54 

3I-84 
31-78 

Fe2( 
14. 

20. 

9- 
II. 

13- 

16' 

49 

21 

39 

06 
88 

07 

S03. 

31-45 
31.88 

3I-30 

31-54 

29-43 
28.33 
27.92 
27.98 

Solid  Phase, 
unstable 


Fe2(SO4)3.H2S04.8H2O+ 

Fe2(S04)3.9H20 


Results  are  also  given  for  the  two  forms  of  yellow  ferric  sulfate  (a  copiapite  and 
0  copiapite)  also  for  ferric  hydroxide  and  sulfate  solutions. 

It  was  found  that  a  saturated  solution  of  Fe2(SO4)3.H2SO4.8H2O  in  abs.  alcohol 
at  25°  contained  8  gms.  Fe2O3  +  17.18  gms.  SO3  (Ratio,  1 14.235)  per  100  gms.  sat. 
sol. 

The  yellow  ferric  sulfate  Fe2(SO4)3.9H2O  is  less  soluble  in  alcohol.  After  4 
weeks  shaking  at  25°,  100  gms.  of  the  sat.  solution  in  abs.  alcohol  contained  4.497 
gms.  Fe2Os  and  6.779  Sms-  SOs  (Ratio,  1:3.006).  Thus  the  alcoholic  solution, 
just  as  the  aqueous,  is  considerably  more  acid  than  the  solid  phase  with  which  it 
is  in  equilibrium. 

loo  grams  sat.  solution  in  glycol  contain  6  gms.  FeSO4  at  ordinary  temperature. 

(de  Coninck.) 

100  gms.  anhydrous  hydrazine  dissolve  I  gm.  ferrous  sulfate  at  room  temp, 
with  decomposition.  (Welsh  and  Brodeison,  1915.) 

SOLUBILITY  OF  MIXTURES  OF  FERROUS  SULPHATE  FeSO4.7H2O  AND 
SODIUM  SULPHATE  Na2SO4.ioH2O  IN  WATER. 

(Koppel  —  Z.  physik.  Chem.  52,  405,  '05.) 


Solid  Phase. 

FeS04.7H20  +  Na2S04.ioH«0 
FeNa2(S04)24H20 

M 
M 

FeNaaCSOOz^HsO  +  FeSO4.7H20 


t°. 

Gms.  per  100  Gms, 
Solution. 

Gms.  per  100  Gms. 
If20. 

FeSO4. 

Na2S04. 

FeSO4. 

Na2SO4. 

0 

14 

•54 

4 

•93 

18 

.06 

6 

.11 

15-5 

17 

.76 

II 

•32 

25 

•05 

15 

•97 

21.8 

16 

•57 

15 

24 

•34 

22 

•51 

24.92 

16 

.21 

1$ 

.13        23.62 

22 

.04 

35 

16 

•35 

14 

.98 

23 

.91 

21 

•83 

40 

16 

•37 

15 

.42 

24 

.01 

22 

.62 

18.8 

18 

•13 

I3.8 

26 

•63 

2O 

.28 

23 

19 

•58 

12 

•5 

28 

.82 

18 

•4 

27 

20 

•97 

II 

•3 

30 

•95 

16 

.64 

31 

22 

.91 

9 

.71 

33 

•99 

14 

.41 

35 

23 

•85 

9 

.26 

35 

.66 

13 

•85 

40 

26 

•32 

7 

•85 

39 

.98 

II 

.92 

18.8 

18 

•23 

14 

•83 

27 

•23 

22 

.16 

23 

13 

•83 

18 

.04 

20 

•31 

26 

.48 

28 

7 

.66 

24 

.41 

ii 

.28 

35 

•94 

31 

4 

•58 

29 

•5° 

6 

•95 

44 

•75 

35 

4 

.04 

30 

•49 

6 

.16 

46 

•58 

40 

4 

.10 

30 

.60 

6 

.27 

46 

•99 

FeNa2(SO4)24H2O  +  N 


FeNa3S044H20  -f  NajSO* 


345  IRON  SULFATE 

IRON  Potassium  SULFATE   (Ferrous)   FeSO4.K2S04.6H2O. 
SOLUBILITY  IN  WATER.    (Tobier,  1855.) 

f0  Gms.  K2Fe(SC>4)2  t»  Gms.  K2Fe(SO4)2 

per  100  Gms.  H2O.  per  100  Gms.  H20. 

o  19-6  35  41 

10  24.5  40  45 

14-5  29.1  55  56 

16  30-9  65  57.3 

25  36-5  70  64.2 

IRON   SULFIDE   (Ferrous)   FeS. 

One  liter  of  water,  saturated  at  18°  with  precipitated  ferrous  sulfide,  contains 
70.I.IO"6  mols.  FeS  =  0.00616  gm.,  determined  by  conductivity  method. 

(Weigel,  1906,  1907.) 

Additional  data  for  the  solubility  in  water  are  given  by  Bruner  and  Zawadzki. 
loo  gms.  anhydrous  hydrazine  dissolve  9  gms.  FeS  at  room  temp,  with  decom- 
position. (Welsh  and  Broderson,  1915.) 
Fusion  diagrams  for  mixtures  of  FeS  +  PbS  and  for  FeS  +  ZnS  are  given  by 
Friedrich,  1907,  1908. 

IRON  SULFONATES. 

SOLUBILITY  OF  IRON  PHENANTHRENE  SULFONATES  IN  WATER  AT  20°. 

(Sandquist,  1912.)  Gms  Anhydrous  Salt 

Salt'  per  100  Gms.  H2O. 

Iron    2-Phenanthrene  Monosulfonate    sH^O  o .  044 

"      3-  "  "  5H20  0.20 

"     lo-  6H2O  0.16 

IRON   THIOCYANATE   (Ferric)   Fe(CNS)3-3H2O. 

DISTRIBUTION  BETWEEN  WATER  AND  ETHER.     (Hantzsch  and  Vagt,  1901.) 
Results  at  25°.  Results  at  Several  Temperatures. 

Gm.  Mols.  Fe(CNS)3  per  Liter.  c  Gm.  Mols.  Fe(CNS)3  per  Liter.  ,. 

H2O  Layer  (c).  Ether  Layer  (cO-  c>  H2O  Layer  (c).    Ether  Layer  (c1) .          c' 

0.0202  0.0108  1.87  o  0.0089  0.0167  °-532 
0.0119  0.0034  3.51  10  0.0127  0.0128  0.995 
0.0066  0.00093  7-°7  20  0.0165  0.0091  1.814 
0.0035  0.00025  J3-95  3°  0.0196  0.0059  3.303 

35        0.0207        0.0048        4.32 
Results  for  the  effect  of  HNO3  upon  the  distribution  at  25°  are  also  given. 

ITACONIC  ACID   CH«:C(COOH)CH,COOH. 

Data  for  the  distribution  of  itaconic  acid  between  water  and  ether  at  25°  are 
given  by  Chandler,  1908. 

KERATIN. 

100  gms.  H2O  dissolve  8.71  gms.  keratin  at  20-25°.  (Dehn,  1917.) 
100  gms.  aq.  50%  pyridine  dissolve  16  gms.  keratin  at  20-25°.  " 

Pyridine  mixes  with  keratin  in  all  proportions  at  20-25°.  " 


'    SOLUBILITY  IN  WATER,    (von  Antropoff,  1909-10.) 
(Results  in  terms  of  coefficient  of  absorption  as  defined  by  Bunsen,  see  p.  227,  and 
modified  by  Kuenen  in  respect  to  substituting  mass  for  volume  of  water  involved.) 
t°.  Abs.  Coef.  (First  Series).       Abs.  Coef.  (Second  Series). 

o         0.1249          0.1166 
10         0.0965          0.0877 

20  0.0788  0.0670 

30  0.0762  0.0597 

4O  O.O74O  0.0561 

50  0.0823  0.0610 

The  cause  of  the  differences  between  the  first  and  second  series  of  results  was 
not  ascertained  by  the  author. 


LACTIC  ACID 


346 


LACTIC  ACID   (t)   CH3CHOHCOOH. 

DISTRIBUTION  BETWEEN  WATER  AND  ETHER. 

(Pinnow,  1915.) 

Results  at  27.5°. 


Results  at  15°. 
Gm.  Mols.  Acid  per  Liter: 


Gm.  Mols.  Acid  per  Liter: 


(w) 


HjO  Layer  (w). 

Ether  Layer  (e). 

e 

H20  Layer  (w). 

Ether  Layer  (e). 

(«) 

I.98 

0.215 

9.19 

1-354 

0.130      - 

10.42 

I-3SI 

0-133 

10.15 

0.3203 

0.0278 

11.52 

0.297 

0.0246 

12.  08 

0-1855 

0.0156 

11.89 

0.1448 

O.OIlS 

12.27 

0.0548 

O.0046 

11.88 

F.-pt.  data  for  mixtures  of  trichlorolactic  acid  and  dimethylpyrone  are  given  by 
Kendall,  1914. 

LACTOSE   (see  sugars,  pages  695-7). 

LANTHANUM  BROMATE  La(BrO3)s.9H2O. 

100  gms.  H2O  dissolve  28.5  gms.  lanthanum  bromate  at  15°.  (Marignac.) 

LANTHANUM  CITRATE  2(LaC2H6O7).7H2O. 

100  gms.  aq.  citric  solution  containing  10  gms.  citric  acid  per  100  cc.,  dissolve 
0.8  gm.  La(C6H6O7)  at  20°.  (Holmberg,  1907.) 

LANTHANUM  CobaltiCYANIDE  La2(CoC6N6)2.9H2O. 

100  gms.  aq.  10%  HC1  (dm  =  1.05)  dissolve  10.41  gms.  salt  at  25°. 

(James  and  Willand,  1916.) 

LANTHANUM  GLYCOLATE  La(C2HsO3)3. 

One  liter  H2O  dissolves  3.328  gms.  La(C2H3O3)3  at  20°.  (Jantsch'and  Grunkraut,  1912-13.) 

LANTHANUM  IODATE  La(I03)3. 

SOLUBILITY  IN  WATER  AND  IN  AQ.  SALT  SOLUTIONS  AT  25°. 

(Harkins  and  Pearce,  1916.) 

1000  gms.  H2O  dissolve  0.6842  gm.  La(IO3)3  at  25°,  dap  sat.  sol.  =  0.99825. 


•"  ~ 

Cone,  of 

Gms. 

^     of 

Cone,  of 

Gms. 

,      f 

Salt. 

Salt,  Milli- 

Li(IO3)3 

Salt.         Salt,  Milli- 

*!  - 

Nonnal. 

per  Liter. 

Sat.  Sol. 

Normal. 

per  Liter. 

Sat.  Sol. 

La(NO,), 

2 

0-5595 

0.99732 

NaNO3         25 

0.86901 

.00250 

" 

5 

0.5288 

0.99807 

So 

0.99040 

.00385 

ti 

10 

0.5194 

0.99859 

IOO 

I  .  1603 

.00742 

" 

50 

0.5522 

I.  00212 

200 

I-385 

.01290 

u 

IOO 

0.6214 

I.  OO66I 

400 

1.636 

.02422 

'n 

200.52 

0.7431 

I.OI533 

800 

2.  156 

.04677 

KIO, 

0.0990 

0.6290 

I.OOO3O 

I6OO 

2.859 

.09005 

14 

0.4957 

0.5633 

1.00027 

"               32OO 

3.030 

.17243 

It 
K 

0.9914 

1.9828 

0.4970 
0.3738 

1.00030 
I.0003I 

^N^O  1    26^4 

0.631 

.00112 

NalO, 

0.0913 

0.63538 

I.0006o 

52.68 

0-674 

.00355 

" 

0.4560 

o  .  56466 

I.OOO59 

105.36 

0-754 

.00971 

1C 

0.9130 

0.50835 

1.00065 

158.04 

0.816 

.01608 

u 

I  .  8260 

0.39938 

1.00065 

196.83 

0.867 

.02183 

U 

3.6530 

0.19736 

1.00069 

393.67 

1.063 

.04343 

u 

4.5326 

0.13393 

1.00083 

787.35 

1-364 

.08286 

(i 

6.7989 

0.09733 

I.OOI3O 

I574-70 

1.923 

.16652 

According  to  Rimbach  and  Schubert  (1909),  one  liter  H2O  dissolves  1.681  gms. 
Li(IO3)3  at  25°,  determined  chemically,  and  1.871  gms.  determined  electrolytically; 
solid  phase,  2La(IO,)3.3H2O. 

LANTHANUM  MALONATE  La2(C3H2O4)3.5H2O. 

100 gms.  aq.  Am.  malonate  sol.  (10  gms.  per  100  cc.)  dissolve  0.2  gm. )  La2(C3H2O4)s 
loo  gms.  aq.  malonic  acid  sol.  (20  gms.  per  loocc.)  dissolve  0.6  gm.  f     at  20°. 

(Holmberg,  1907.) 


347 


LANTHANUM  MOLYBDATE 


LANTHANUM  MOLYBDATE   La2(MoO4)3. 

One  liter  H2O  dissolves  0.0179  gm-  La2(MoO4)3  at  25°  and  0.0332  gm.  at  85°. 

(Hitchcock,  1895. 
LANTHANUM  Ammonium  NITRATE   La(NO3)3.2NH4NOs. 

100  gms.  H2O  dissolve  181.4  gms.  La(NO3)3.2NH4NO3  at  15°.       (Holmberg,  1907.) 
LANTHANUM j  Double.  NITRATES. 
SOLUBILITY  OF  LANTHANUM  DOUBLE  NITRATES  IN  CONC.  HNO3(dia  =  1.325) 

AT   1 6°.      (Jantsch,  1912.) 


Salt. 

Lanthanum  Magnesium  Nitrate 
Nickel 
Cobalt 
Zinc 
"  Manganese       " 


Formula. 


[La(N03)6]2Mg3.24H20 

Co3  " 
Zn3  " 
Mn3  " 


Gms.  Hydrated  Salt 

Dissolved  per 

Liter  Sat.  Sol. 

63-8 

80.3 

109.2 

124.1 


LANTHANUM  NITRATE  La(NO3)3. 

SOLUBILITY  OF  LANTHANUM  NITRATE  IN  AQUEOUS  SOLUTIONS  OF  LANTHANUM 

OXALATE  AT  25°  AND  VICE  VERSA.       (James  and  Whittemore,  1912.) 
Gms.  per  ioo  Gms.  Sat.  Sol. 


Solid  Phase. 


Gms.  per  100  Gms.  Sat.  Sol. 


La2(C204),.3H20 


O 

0.67 

2.IO 

2.23 

2.26 

2-34 

2-47 

2-59 

2.68 
not  det.     not  det. 


La;(C204)3. 

La(NO3)3.  ' 

ooiia  rnase. 

not  det. 

not  det. 

La2(C204)3.5H20 

3-32 

42.27 

La2(C204)3.8H20 

2.80 

38-50 

" 

2.51 

35-57 

" 

2.21 

31-53 

ft 

2.01 

28.63 

«* 

I.46 

22.15 

« 

1.18 

17.99 

H 

0.50 

9.89 

« 

0.28 

5-o6 

H 

La(N03)3. 
60.17    LatNOa), 

59-91 
59-03         " 
59-03 
58.22 

55-20 

52-74 
49.84 
45-26 

La2(C204)3.SH20 

LANTHANUM  OXALATE  La2(C2O4)3.9H2O. 

One  liter  water  dissolves  0.00062  gm.  La2(C2O4)3  at  25°,  determined  by  electroly- 
tic method.  (Rimbach  and  Schubert,  1909.) 

ioo  gms.  aq.  10.2%  HNO3  (d  =  1.063)  dissolve  0.80  gm.  La2(C2O4)3  at  15°. 

(v.  Scheele,  1899.) 

ioo  gms.  aq.  19.4%  HNO3  (d  =  1.116}  dissolve  2.69  gms.  La2(C2O4)3  at  15°. 

(v.  Scheele,  1899.) 

SOLUBILITY  OF  LANTHANUM  OXALATE  IN  AQ.  SOLUTIONS  OF  SULFURIC 

ACID  AT  25°.      (Hauser  and  Wirth,  1908;  Wirth,  1908;  Wirth,  1912.) 

Normal-    Gms.  per  ioo  Gms.  Normal-  Gms-  P61"  Joo  Gms. 

ity  of  Sat.  Sol.  Solid  Phase.  ity  of  Sat.  Sol.  Solid  Phase. 

H*SO4.        La2O3  =  La2(C204)3.  H2SO4.     La2O3 

o.i       0.0208    0.0346  La2(C2O4)3.9H2O      2 
0.5      0.0979    0.1629 


La2(C2O4)3. 

0.4417  0.7344    La2(C2O4)3.9H20 

3.09    0.680  1.1306 

4.32    0.880  1.4630 

5.6      1.092  1.8155  " 


0.2383    0.3962 
c.S       0.319      0.5304 

SOLUBILITY  OF  LANTHANUM  OXALATE  IN  AQ.  SOLUTIONS  OF  OXALIC  ACID 

AT  25°.      (Hauser  and  Wirth,  1908.) 
Normality  of  Aq.  Gms.  per  ioo  Gms.  Sat.  Sol.  Solid  phase 


La2(C204)3. 


Oxalic  Acid. 

o .  i  unweighable 

i.o  0.00032  0.00053 

3.2  (sat.)         0.00045  0.00075 

Results  are  also  given  for  the  solubility  in  mixtures  of  sulfuric  and  oxalic  acids, 
ioo  cc.  aq.  20%  triethylamineoxalate  dissolve  approx.  0.032  gm.  La2(C2O4)3. 

(Grant  and  James,  1917.) 


LANTHANUM  PHOSPHATE 


348 


LANTHANUM  Dimethyl  PHOSPHATE  La2[(CH,)jPO4]6.4HjO. 

100  gms.  H2O  dissolve  103.7  gms.  La2[(CH3)2PO4]6  at  25°.  (Morgan  and  James,li9t4.) 

LANTHANUM  SULFATE  La2(SO4)3.9H2O. 

SOLUBILITY  IN  WATER.        (Muthmann  and  Rolig,  1898.) 
Gms.  La2(SO4)3  per  100  Gms. 
Solution.        Water. 

2.91        3 
2.53        2.6 


Gms.  La2(SO4)3  per  100  Gms. 
Solution/         Water. 


o 
14 

30 


1.86 


1.9 


5° 

75 

100 


o-95 
0.68. 


0.96 
0.69 


SOLUBILITY  OF  LANTHANUM  SULFATE  IN  AQ.  SOLUTIONS  OF  AMMONIUM 
SULFATE,  POTASSIUM  SULFATE  AND  SODIUM  SULFATE.     (Ban-e,  1910,  1911.) 

In  Aq.  (NH4)2SO4  at  18°.     In  Aq.  K2SO4  at  16.5°.       In  Aq.  Na2SO4  at  18°. 


Gms.  per  100  Gms.  H2O.        Solid 

Gms.  per  100  Gms.  H2O.      Solid      Gms.  per  100  Gms.  H2O. 

Solid 

(NH4)2SO4.     La2(S04)3.       phase- 

K2SO4.      La2(SO4)3.      Muse.        NazSCv     La2(SO4)3. 

Phase. 

4.01 

0.393         I.I-2 

o            2.198     1.0.9     °            2.130 

1.0.9 

8-73 

0.279 

0.247      0.727        1.  1.2       0.395      0.997 

I.I.  2 

18.24 

0-253 

0.496    0.269                 0.689    0-353 

11 

27.89 

0.476*          " 

0.846    0.185                 0-774    0.299 

(t 

36.11 

0.277*          " 

1.029    0.054      1.5       1.136    0.129 

ti 

47-49 

0.137          2.5 

1.156    0.022        "        2.480    0.044 

" 

53-82 

0.067          1.5 

3.802    0.019 

it 

65.29 

0.0117 

5.548    0.016 

" 

73-78 

.    0.0033 

*  =  unstable  equilibrium. 

1.0.9 
KorN; 

=  La2(S04)3.9H20, 
a),    2.5  =  2La2(S04) 

1.  1.2  =  La2(SO4)3.*2SO4.2H2O    (where   X  = 
3.5(NH4)2S04,  1.5  =JLa2(S04)3.5*2S04. 

(NHO, 

SOLUBILITY  OF  LANTHANUM  SULFATE  IN  AQUEOUS  SOLUTIONS  OF  SULFURIC 

ACID  AT  25°.      (Wirth,  1912.) 


Normality 
of  Aq. 
H2S04. 

Gms.  per  100  Gms. 
Sat.  Sol. 

pS.      Ng-ty 

Gms.  per  100  Gms. 
Sat.  Sol.                     ^Solid 

1^03  = 

La2(S04)3. 

La203  = 

=  La2(S04)3. 

Water 

I 

•43 

2 

•483 

La2(S04)3.9H20       4 

.321 

I 

.11 

I 

.927      LajCSOJs.gl 

o 

•505 

I 

.69 

2 

•934 

6 

.685 

0 

•531 

0 

.9217 

i 

.10 

I 

.796 

3 

.118 

9 

.68 

O 

.266 

O 

.4617 

2 

.16 

I 

.818 

3 

•156 

12 

.60 

0 

.214 

o 

•371 

3 

•39 

I 

.42 

2 

-465 

15 

•15 

0 

.177 

0 

•307 

Data  for  the  solubility  of  lanthanum  sulfate  in  aq.  H2SO4  in  presence  of  solid 
oxalic  acid  at  25°  are  given  by  Wirth,  1908. 

LANTHANUM  SULFONATES. 

SOLUBILITY  OF  EACH  IN  WATER. 


Sulfonate. 


Lanthanum  Benzene  Sulfonate 

m  Nitrobenzene  Sulfonate 
'  m  Chlorbenzene  Sulfonate 
m  Brombenzene         " 


Gms. 

Anhydrous 
Formula.  Sulfonate       Authority. 

per  too 
Gms.  H2O. 

63 . 1   (Holmberg,  1907.) 
16 


La[C«H6SO3]3.9H2O 
La[C6H4NO2SO3]3.6H2O 
LafCjH4Cl.SO3ls.9H2O 
LalC6H4Br.SO3l3.9H2O 


I3-I 
12.9 

'  (6)  Chloro  (3)  Nitrobenzene  (i)  )Sulfo-j  La[C6H3Cl(NO2)SO3]3.8H2O  24 . 5  " 

'  (i)  Bromo  (4)  Nitrobenzene  (2)  {  nate  \  LalCgHjBrNOzSO^.SHzO     5     (Katz  &  James,  '13.) 
*'  a  Naphthalene  Sulfonate  La[C10H7SO3]3.6H2O  5 . 2  (Holmberg,  1907.) 

"  1.5  Nitronaphthalene  Sulfonate        La[CioH8(NO2)SO3l3.6H2O     0.55  " 

"1.6  "  "  «  .9H.D     0.21 

"  1.7  "  "  "  .9IW)     i.i 


349  LANTHANUM  TARTRATE 


LANTHANUM  TARTRATE  La2(C4H4Oe 

One  liter  H2O  dissolves  0.059  gm.  La2(C4O4O6)3  at  25°  (solid  phase  La2(C4H4O6)3. 
3H2O).  Determined  by  electrolytic  method.  (Rimbach  and  Schubert,  1909.) 

SOLUBILITY  OF  LANTHANUM  TARTRATE  IN  AQ.  TARTARIC  ACID  AND  AMMONIUM 
TARTRATE  SOLUTIONS  AT  20°. 

(Holmberg,  1907.) 

In  Aq.  Tartaric  Acid.  In  Aq.  Ammonium  Tartrate. 

Gms.  Tartaric  Acid  per   Gms.La^C^O^sper  •      Gms.  Am.  Tartrate  per  Gms.  La^C^O^s  per 
100  cc.  Solvent.  too  Gms.  Sat.  Sol.  100  cc.  Solvent.  100  Gms.  Sat.  Sol. 

20  0.6  10  0.2 

40  1.2  20  0.6 

LANTHANUM  TUNGSTATE  La2(WO4)3. 

One  liter  H2O  dissolves  0.0117  gm.  La2(WO4)3  at  27°  and  0.0236  at  65°. 

u  (Hitchcock,  1895.) 
LAURIC  ACID   Ci2H23COOH. 

SOLUBILITY  IN  ALCOHOLS. 

(Timofeiew,  1894.) 

Alcohol  t°     Gms.CuH-aCOOHDer  Alcohol  t°    Gms.  C,2H23COOH  per 

Alcohol.  t  .       IQO  Gms  Sa(.  Sol  Alcohol.  t  .       IQQ  Gms  Sat  sd 

Methyl  Alcohol      o  14.8        Propyl  Alcohol       o          21.5 

21  58.6  21          52.6 

Ethyl  Alcohol        o  20.5        Isobutyl  Alcohol    o          18.4 

21  57.3  21          49.7 

LEAD  Pb. 

An  extensive  investigation  of  the  solubility  of  lead  in  the  water  passing  through 
lead  pipes  is  described  by  Paul,  Ohlmiiller,  Heise  and  Auerbach,  1906.  ^  The 
solubility  is  increased  by  oxygen,  CO2,  sulfates  and  perhaps  other  salts;  it  is  de- 
creased by  hydrocarbonates. 

SOLUBILITY  OF  LEAD  IN  LIQUID  AMMONIA-SODIUM  SOLUTIONS  AT  —33°. 

(Smith,  F.  H.t  1917.) 

Gm.  Atoms  Sodium       Gm.  Atoms  Pb  Gm.  Atoms  Na  Gm.  Atoms  Pb 

per  Liter  of  Liquid    Dissolved  per  Gm.  per  Liter  of  Liquid     Dissolved  per  Gm. 

Ammonia.  Atom  Na.  Ammonia.  Atom  Na. 

0.078  1-95  0.13  2.17 

0.093  2-20  °-I4  2-12 

0.094  2.03  0.33  1.83 

o.no  2.24  0.34  1.73 

0.12  1.78 

LEAD  ACETATE  Pb(C2H3O2)2.3H2O. 

loo  gms.  H2O  dissolve  55.04  gms.  Pb(C2H3O2)2  at  25°.  (Jackson,  1914.) 

EQUILIBRIUM  IN  THE  SYSTEM  LEAD  OXIDE,  ACETIC  ACID,  WATER  AT  25°. 

(Sakabe,  1914.) 
Gms.  per  100  Gms.  Sat.  Sol.  „  .. .  _.  Gms.  per  100  Gms.  Sat.  Sol. 

(C2H302)(HO)Pb-f- 


PbO. 

CH3COOH. 

•»              oouu  jrnase.             .  / 

PbO. 

CHjCOOI 

4.18 

2*-53 

Pb(C2H302)2.3H20 

> 

3.80 

16.78 

« 

7-I5 

7.20 

3.16 

13.07 

" 

5.20 

5-61 

2.64 

5-49 

« 

3-78 

4.17 

3-34 

5-36 

M 

2.89 

2-5i 

4-38 

7-30 

« 

i-45 

1.03 

5.18 

7.92 

"  +(0,11302)  (HO)Pb 

i  .05 

0-54 

5-59 

7.72 

(QHAXHOJPb 

1.07 

0.48 

6.51 

7-79 

" 

i 

0.20 

PbO 


Equilibrium  was  attained  quickly  in  the  acid  solutions  but  2-3  days  were  required 
in  case  of  the  basic  salts.     Both  sat.  solutions  and  solid  phases  were  analyzed. 


LEAD  ACETATE  35O 

EQUILIBRIUM  IN  THE  SYSTEM  LEAD  ACETATE,  LEAD  OXIDE,  WATER  AT  25°. 

(Jackson,  1914.) 


^26  Of 

Gms.  per  too  Gms.  Sat.  Sol.      Solid 

djsof    Gms.  per  ioo  Gms.  Sat.  Sol.       Solid 

Sat.  Sol. 

'    PbO. 

Pb(C2H302)2. 

Phase. 

Sat.  Sol. 

PbO.     Pb(C2H3Oo)2.         Phase. 

I  .326 

—  0 

.27* 

35-19 

i-3 

2 

.280 

24 

•74 

49 

.21 

3.1.3+1.2.4 

1-334 

'+0 

.IO 

35-60 

« 

2 

.048 

23 

•59 

43 

•17 

1.2.4 

1.367 

I 

.OI 

37-14 

it 

I 

•951 

22 

.78 

40 

.78 

(( 

1.422 

3 

.38 

38.93 

a 

I 

•657 

19 

-63 

3i 

.40 

ii 

1-531 

6 

.01 

41-95 

(( 

I 

•599 

18 

•73 

29 

-63 

tt 

1.658 

9 

•47 

44.71 

(C 

I 

.382 

14 

.62 

20 

.96 

tt 

.  .  . 

14 

.22 

47.88 

(( 

I 

.348 

13 

.41 

19 

-65 

ft 

1.852 

14 

-44 

47.92 

(( 

I 

.229 

10.66 

12 

•99 

tt 

.  .  . 

15 

.89 

48.951 

.3+3-1.3 

I 

.157 

8 

•47 

8 

.64 

tt 

1.930 

IS 

.90 

48.42 

3.1.3 

I 

.119 

7 

.87 

5 

•27 

tt 

1.942 

16 

•25 

48.85 

(( 

I 

.117 

7 

•79 

5 

•25 

ft 

1.956 

16 

-65 

49.04 

(( 

4 

•17 

Pb(OH)2 

2.024 

18 

-83 

48.71 

tt 

I 

.100 

6 

'•*4 

4 

•3i 

n 

2.161 

22 

•23 

48.52 

(( 

I 

•095 

6 

•54 

4 

•25 

tt 

2.193 

22 

•94 

48.96 

ft 

I 

-085 

5 

.91 

3 

.82 

tt 

23 

.28 

49.14 

ft 

I 

•075 

5 

.29 

3 

.40 

tt 

2.22O 

23 

•53 

49.01 

{( 

o 

.20 

0 

.11 

<t 

In  this  case  the  acidity  is  expressed  in  terms  of  PbO. 

i.3  =  Pb(C2H302)2.3H20,  3.1.3  =  3Pb(C2H302)2.Pb0.3H20,  1.2.4  «Pb(C,HA)r 
2PbO.4H2O. 

The  above  results  show  the  solubility  of  lead  acetate  in  aqueous  solutions 
containing  increasing  amounts  of  lead  hydroxide.  The  mixtures  were  constantly 
agitated  for  periods  varying  from  2  to  7  days.  Both  the  saturated  solutions  and 
the  solid  phases  were  analyzed.  The  basic  lead  in  a  given  sample  was  determined 
by  measuring  the  volume  of  standard  acid  neutralized  by  it.  The  neutral  lead 
acetate  was  determined  by  precipitation  of  the  lead  as  sulfate  or  as  oxalate. 

SOLUBILITY  OF  LEAD  ACETATE  IN  AQ.  SOLUTIONS  OF  POTASSIUM  ACETATE  AT  25°. 

(Fox,  1909.) 

Gms.  per  ioo  Gms.  Sat.  Sol. 
CHaCQOK.        '  (CH3COO),Pb.  Solid  Phase. 

o  35.9  (CH3COO)2Pb.3H20 

13-87  38.05 

15.40  36.90 

SOLUBILITY  OF  LEAD  ACETATE  IN  AQUEOUS  SOLUTIONS  OF  ETHYL  ALCOHOL  AT  25°. 

(Seidell,  1910.) 
Wt.%^      ^of        £ms-pb  Wt-%         ^  of         H^'Pb 

Solvent.        So1'        Sat.  Sol.    '  Solvent.         SoL        Sat.  Sol. 

o  -343      36.5  (CaHaOa^Pb.sH-jO    70        0.955       12.4     (C2H3O2)2Pb.3H20 

10  -275      32.3  80        0.907        9.4 

20  .215       28.6  81        0.905        9 

30  .157       25  "  85        0.855        4  (C2Ha02)2Pb 

40  -105      21.9  90        0.826        1.6 

50  .055       18.7  95        0.806        0.6 

60  .002       15.6  ioo        0.790        0.4 

ioo  gms.  95%  formic  acid  dissolve  o.99(?)  gm.  Pb(C2H3O2)2  at  19.8°.  (Aschan,  1913.) 
ioo  gms.  anhydrous  lanolin  (m.  pt.46°)  dissolve  i  .1  gm.  Pb(C2H3O2)2at45°.  (Klose,  '07.) 
ioo  gms.  glycerol  dissolve  about  20  gms.  Pb(C2H3O2)2  at  15°.  (Ossendowski,  1907.) 

LEAD  ARSENATE   PbHAsO4. 

Two  gm.  portions  of  amorphous  dilead  arsenate  were  agitated  at  32°  with  90  to 
1 80  cc.  portions  of  0.0338  normal  aqueous  ammonia  for  two  days.  The  saturated 
solutions  were  found  to  contain  only  traces  of  lead  but  amounts  of  As2O6  varying 
from  1.956  to  1.429  gms.  per  liter.  (McDonnell  and  Smith,  1916.) 


351  LEAD  BENZOATE 

LEAD  BENZOATE  Pb(C7H6O2)2.H2O. 

SOLUBILITY  IN  WATER. 

(Pajetta,  1906.) 
t°.  18°.  40.6°.  49°. 

Cms.  PbCCrHsC^  per  100  gms.  sat.  sol.       0.149        0.249        0.310 

LEAD   BORATE   Pb(BO2)2.H2O. 

100  cc.  anhydrous  hydrazine  dissolve  about  2  gms.  Pb(BO2)2  at  room  temp. 

(Welsh  and  Broderson,.i9is.) 

LEAD  BROMATE   Pb(BrO3)2.H2O. 

'b(BrO3)2  at  K, 

(Rammelsberg,  1841;  Bottger,  1903.) 


100  gms.  water  dissolve  1.32  gms.  Pb(BrO3)2  at  19.94°. 

(Rammelst 


LEAD    BROMIDE    PbBr2. 

SOLUBILITY  IN  WATER. 

(Lichty  —  J.  Am.  Chem.  Soc.  25,  474,  '03.) 


t°. 

Density 
of  Solutions, 
H2O  at  o°. 

Gms.  PbBr2  per  too 

Milligram  Mols.  PbBr2  per  100 
cc.  Solution.        Gms.  H2O. 

cc.  Solution. 

Gms.  H2O. 

o 

I  .0043 

0-4554 

0-4554 

1.242 

1.242 

15 

1-0053 

0.7285 

0.7305 

1.987 

1.989 

25 

I  .Oo6l 

0.9701 

0-9744 

2.646 

2.655 

35 

I  -0060 

I.3I24 

1.3220 

3-577 

3-603 

45 

I  .0059 

I-7259 

1-7457 

4.705 

4-760 

55 

I  .0046 

2  .IO24 

2.1376 

5-731 

5.827 

65 

I  .0028 

2.516 

2-574 

6.859 

7.016 

So 

I  -OOOO 

3-235 

3-343 

8.819 

9.113 

95 

0-9995 

4-1767 

4-3613 

11.386 

11.890 

100 

4-550 

4-751 

12.40 

12.94 

SOLUBILITY  OF  LEAD  BROMIDE  IN  AQUEOUS  HYDROBROMIC  ACID 

AT  IQ°. 

100  grams  H2O   containing   72.0   grams  HBr  dissolve   55.0  grams 
PbBr2  per  100  gms.  solvent,  and  solution  has  Sp.  Gr.  2.06. 

(Ditte  —  Compt.rend  92,  719,  '81.) 

SOLUBILITY  OF  LEAD  BROMIDE  IN  PYRIDINE. 

(Heise,  1912.) 
j.o  Gms.  PbBrz  per  c  i-j  -ni.  *o        Grns.  PbBr2  per     c  IM  -D^ 

100  Gms.  Pyridine.         Solld  Phase"  *  '    100  Gms.  Pyridine.  Solld  Phase' 

—  26  I.  O2          PbBrz.aCsHjN  45  O.66l         PbEr^CsHsN 

— 10  0.89  "  64  0.800      " 

-  5  0.84  "  77  0.969 

o  0.80  95  1.33 

+  13  0.661  "  loo  1.44       " 

I9tr.pt.  ...  "  +PbBr2.2C5H6N         105  1.56 

26  0 . 583  PbBr2.2C5H6N 

FREEZING-POINT  DATA  (Solubility,  see  footnote,  p.  i)  ARE  GIVEN  FOR  THE 
FOLLOWING  MIXTURES  OF  LEAD  BROMIDE  AND  OTHER  COMPOUNDS. 

Lead  Bromide  +  Lead  Chloride  (Monkemeyer,  1906.) 

+  Lead  Iodide 

"         +  Lead  Fluoride  (Sandonnini,  1911.) 

"          +  Lead  Oxide  (Sandonnini,  1914.) 

-j-  Mercuric  Bromide  (Sandonnini,  1912, 1914.) 

"  "        -j-  Silver  Bromide  (Matthes,  1911.) 


LEAD  BROMIDE 


352 


LEAD 
LEAD 


Dicyclohexyl   DiBROMIDE   (C6Hn)2PbBr2. 

Dicyclohexyl   DiCHLORIDE   (C6Hn)2PbCl2. 

SOLUBILITY  OF  EACH  IN  SEVERAL  SOLVENTS  AT  22.5°. 

(Gruttner,  1914.) 

Grams  per  100  Grams  Solvent. 


Solvent. 

Benzene 

Carbon  Tetrachloride 

Chloroform 

Alcohol  +  Pyridine  (i :  i) 


O.OI4 
O.OO4 
0.078 
2.560 


(C6Hn)2PbCl2. 

0.016 
0.004 
0.083 
2.904 


Similar  results  are  also  given  for  lead  tetracyclohexyl,  PbCCeHiOi,  lead  tetra- 
phenyl,  Pb(C6H8)4,  and  lead  diphenyldicyclohexyl,  Pb(C6H6)a(C6Hn)j. 

Gms.  per  100  Gms.  Solvent. 
Solvent. 

Alcohol 

Benzene 

Carbon  Tetrachloride 

Ethyl  Acetate 

LEAD  CAPROATE,  CAPRYLATE,  CAPRATE,  etc. 

SOLUBILITY  OF  EACH  IN  ETHER  AND  IN  PETROLEUM  ETHER. 

(Neave,  1912.)  / 

Solubility  in  Ethyl  Ether.     Solubility  in  Pet.  Ether. 

Gms.  Salt  per  100  cc.  Sat.  Sol.     Gms.  Salt  per  100  cc.  Sat.  Sol. 


Pb(C6Hn)4. 

Pb(C6H5)4. 

Pb(C6H6)2(C6H11)2. 

O.OIO 

O.O2O 

0.324 

1.068 

I-I45 

2.298 

0.244 

0.303 

0.845 

0.030 

0.123 

0.231 

Pb 

« 

a 
tt 
tt 
n 
n 
(i 
tt 

Caproate 
Heptylate 
Caprylate 
Nonylate 
Caprate 
Myristate 
Laurate 
Palmitate 
Stearate 

73-74 
90.5-91. 

83.5-84- 
94-95 

IOO 

107 

103-104 

112 
125 

At  20°.      At  B.  pt.  of  Sat.  Sol.     At  20°.       At  B.  pt.  of  Sat.  Sol. 

i  .  364              ...              o  .  0608 
5      0.2397          1.490           0.020           0.0528 
5       0.0938           0.546     practically  insol.     0.0384 
0.1115           0.2404                                0.0450 
0.0290          0.4285                                0.0170 
practically  insol.     0.0555                                 0.0210 
"                0.0205               "         practically  insol. 
0.0261 
practically  insol.       "                 0.0170 

The  ethyl  ether  was  distilled  over  sodium.  Petroleum  ether  distilling  between 
4O°-6o°  was  used.  The  solutions  were  stirred  constantly  at  20°.  A  definite  volume 
of  the  sat.  solution  was  evaporated  to  dry  ness  and  residue  weighed  in  each  case. 

LEAD  CARBONATE  PbCO3. 

SOLUBILITY  IN  WATER  BY  ELECTRICAL  CONDUCTIVITY  METHOD. 

(Kohlrausch  and  Rose,  1893;  Bottger,  1903.) 

I  liter  of  water  dissolves  0.0011—0.0017  gni-  PbCO3  at  20°. 

SOLUBILITY  OF  LEAD  CARBONATE  (NEUTRAL)  IN  AQUEOUS  SOLUTIONS  OF 
CARBON  DIOXIDE  AT  18°. 

(Pleissner,  1907.) 
Millimols  per  Liter.  Milligrams  per  Liter. 


CO2. 

o 

0.064 

0.123 

0.328 

0.592 

0.988 

2.40 


o 
2.8 

5-4 
14.4 
26 

43-5 
106 


Pbc3. 

1.75 
6 


7 
8.2 


0.008 
0.029 
0.034 
0.040 

0.048  2  9.9 

0.053  43-5  10.9 

0.076  106  15.4 

A  determination  of  the  solubility  of  basic  lead  carbonate  in  water  gave  1.6  mg. 
Pb3(CO3)2(OH)2  per  liter  =  1.3  mg.  Pb  or  0.006  millimol  Pb. 


353  LEAD  CARBONATE 

Data  for  equilibrium  in  the  system  composed  of  K2COs  +  PbCO3  +  K2CrO4 
+  PbCrO4  at  25°  are  given  by  Goldblum  and  Stoffella,  1910. 

Data  for  equilibrium  by  lead  carbonate  precipitation  in  aq.  solutions  of  sodium 
salts  at  25°  are  given  by  Herz,  1911. 

LEAD  CHLORATE  Pb(ClO3)2.H2O. 

100  grams  H2O  dissolve  151.3  gms.  Pb(QO3)2,  or  100  gms.  sat.  solution  con- 
tain 60.2  gms.  Pb(ClO3)2  at  18°.  Density  of  solution,  1.947.  (Mylius  and  Funk,  1897.) 

100  gms.  H2O  dissolve  440  gms.  Pb(ClO3)2  at  18°,  dn  =  1.63.         (Carlson,  1910.) 


LEAD  CHLORIDE   PbCl3. 

SOLUBILITY  IN  WATER.       (Lichty;  see  also  Formanek,  1887;  Bell,  1867;  Ditte,  1881.) 

to 

Density 

Gms.  PbCl2 

per  100 

Milligram  Mols. 

PbCl2  per  TOO 

. 

of  Solutions, 
H2O  at  o°. 

cc.  Solution. 

Gms.  H2O. 

cc.  Solution. 

Grams  H2O." 

0 

I  .0066 

0.6728 

0.6728 

2.421 

2.421 

15 

1.0069 

0.9070 

0.9090 

3  -265 

3.272 

25 

1.0072 

I  .0786 

I  .0842 

3.882 

3-903 

35 

I  .0060 

i  -3*50 

1.3244 

4-733 

4-767 

45 

I  .OO42 

1.5498 

I-5673 

5-579 

5-644 

55 

I  .0020 

1.8019 

1.8263 

6.486 

6-573 

65 

0-9993 

2.0810 

2.1265 

7-490 

7-65I 

80 

0.9947 

2.5420 

2.6224 

9.150 

9-439 

95 

0.9894 

3-0358 

3-I654 

10-926 

n-394 

100 

3.208 

3-342 

11.52 

12  .01 

SOLUBILITY 

OF  LEAD 

CHLORIDE  IN 

AQUEOUS  'SOLUTIONS  OF 

ACETIC  ACID 

AT   25°. 

(Hill,  1917.) 

Normality 

Dissolved  PbCl2. 

Normality 

Dissolved  PbCl2. 

of  Acetic 

Gms. 

Equiv. 

of  Acetic 

Gms. 

Equiv. 

Acid. 

per  Liter. 

per  Liter. 

Acid. 

per  Liter. 

per  Liter. 

O 

10.77 

0-07753 

0.465 

IO.27 

0.07392 

0.05 

10.82 

0.07782 

0.929 

9-45 

o  .  06803 

O.IO 

10.85 

0.07717 

1.845 

7.90 

o.os686 

O.2O 

10.70 

0.07703 

3-680 

5.26 

0.03788 

SOLUBILITY  OF  LEAD  CHLORIDE  IN  AQUEOUS  AMMONIUM  CHLORIDE  AT  22°. 

(Bronsted,  1911.) 

Gm.  Equivalents  per  Liter.  Gm.  Equivalents  per  Liter. 

'  NH.C1.       '        Pbd..    '  SoMPhaSe'  'NH.C!.        '      PbCl..  ***»"• 


O  0.0749        PbCl,  0.8  0.0087 

o.i  0.0325          "  i  0.0080          " 

0.2  0.0194  1.5  0.0073 

0.4  0.0138  2.5  0.0092 

0.5  0.0130  "                                  4  0.0182           " 

0.52  0.0127  "  +NH«a.2PbCl1             6  0.0473 

0.55  0.0123  NH4Cl.2PbCl2                  7.29  0  .  0898             "•  +NH4C1 

0.65  0.0105  "                            7.29  O                          NHiCl 

For  additional  results  at  25.2°  see  von  Ende,  1901. 

SOLUBILITY  OF  LEAD  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  HYDROCHLORIC 

ACID. 

Results  at  l8°.      (Pleissner,  1907.)  Results  at  25.2°.      (von  Ende,  1901.) 

Normality          Gms.  PbClj  Normality         Millimols        Normality        Millimols 

ofHCl.  per  Liter.  of  HC1.     PbCl2  per  Liter,     of  HC1.      PbCl,  per  Liter. 

o  9-34  o  38.8     .     1.026  4.41 

o.oooi  9-305  0.0045        37-35        2.051  5.18 

0.0002  9.300  O.OI5I  33.75  3.085  7.78 

0.0005     9-243         0.0452    25.46    5       19.38 
0.00102    9.200         0.1850    10.25    7-5      65.86 

0.0102       8.504  0.5142      5.37    12.05      164.30 


LEAD  CHLORIDE  354 

SOLUBILITY  OF  LEAD  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OP  HYDRO- 

CHLORIC  ACID. 

(At  o°,  Engel  —  Ann.  chim.  phys.  [6]  17,  359,  '89;  at  25°,  Noyes  —  Z.  physik.  Chem.  9, 623,  '92;  at  differ- 
ent temperatures,  Ditte  —  Compt.  rend.  92,  718,  '81;  see  also  Bell  —  J.  Chem.  Soc.  21,  350,  '68.) 


Cms.  HC1 
Liter. 

Cms.  PbCl2  per 
Liter  at: 

Cms.  HC1 
per  100 
Cms.  H2O. 

Cms.  PbCl2  per  100  Gms.  Solution  at: 

0°. 

25°. 

o0.'" 

20°. 

40°. 

55°. 

80°. 

0 

3-83 

10 

•79 

O 

8.0 

II  . 

8 

17.0 

21  . 

0 

31.0 

o-5 

4-5 

9 

•  O 

100 

1.2 

I. 

4 

3-2 

5 

5 

12.0 

1.0 

3-6 

7 

.6 

J5o 

i-5 

2. 

o 

5-o 

7 

,5 

16.0 

2.0 

2.2 

6 

.0 

200 

3-5 

5- 

o 

8.2 

ii 

•7 

21-5 

3-o 

1.6 

5 

.0 

250 

6-5 

8. 

0 

13.0 

16 

,2 

28.5 

6 

1.4 

3 

.1 

300 

10.7 

12. 

5 

17-5 

22 

.0 

3S-o 

10 

I  .2 

i 

.8 

400 

21-5 

24. 

0 

... 

•  • 

•    . 

... 

100 

1.2 

2OO 

5-2 

. 

.. 

250 

10-5 

• 

300 

17-5 

. 

400 

40-0 

. 

SOLUBILITY  OF  LEAD  CHLORIDE  IN  AQUEOUS  SALT  SOLUTIONS 

AT  25°. 

(Noyes;  in  HgCl2  solutions  at  20°,  Formanek  —  Chem.  Centralb.  270,  '87.) 

In  Aqueous  Solutions  of: 


HCl,  KC1,  MgCl2,  CaCl2,  MnCl2         In  CdCl2 
and  ZnCl2  Gram  Equivalents         Gram  Equiv. 
per  Liter  of:                          per  Liter. 

In  HgCl2 
Gram  Equiv. 
per  Liter. 

InPb(N03)2 
Gram  Equiv. 
per  Liter. 

'Salt.           PbCl2.               CdG2.        PbCl2. 

o.o      0.0777        °-°°    0.0777 
0.05    0.050          0.05     0.0601 
o.io    0.035          0<I°    0.0481 

0-20      0-021              0-20      0.0355 

HgCl2.      PbCl2. 

o.o    0.0777 
o.i     0.0992 

Pb(N03)2.        PbCl2. 

o.o        0.0777 

O-2           0.0832 

The  above  results  were  calculated  to  grams  per  liter  plotted  on  cross- 
section  paper,  and  the  figures  in  the  following  table  read  from  the 
curves. 


Gms. 

Salt 

Grams  PbCl2  per  Liter  in  Aqueous  Solutions  of: 

per 
Liter. 

HCl. 

KC1. 

MgCl2. 

CaCl2. 

MnCl2. 

ZnCl2. 

CdCl2. 

HgCl2.          Pb(N03)a 

o 

I 

10.79 
8-5 

10.79 
9-3 

10.79 
7-7 

10.79 
8.7 

10.79 
9-5 

10.79 

10.79 

10.2 

io-79( 

II  .0 

N)  9-7i(F) 
9.8 

10.79 

10.8 

2 

6-5 

8.2 

6-5 

7.6 

8-3 

.  .  . 

9-7 

11.4 

IO.O 

10.85 

3 

5-2 

7-2 

5-7 

6.7 

7-3 

9.2 

11,7 

10.3 

10.87 

4 

4-3 

6-5 

5-2 

6.0 

6-3 

•  •  • 

8.6 

12.0 

10.5 

10.90 

6 

3-2 

5-3 

4.4 

4.8 

5-° 

... 

7-7 

12.7 

II.  O 

10.95 

8 

4-5 

3-9 

4.1 

.  .. 

7.0 

13-3 

ii.  6 

II  .00 

10 

2.1 

3-9 

3-3 

3-5 

.  .  , 

6-3 

14.0 

12.2 

11.05 

14 

2.8 

3-o 

5-4 

I3.2 

11.15 

20 

14.8 

1  1  .  20 

40 

IQ-0 

11.70 

355 


LEAD   CHLORIDE 


SOLUBILITY  OF  LEAD  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  LEAD  NITRATE  AT  25°. 
Results  by  Harkins,  1911.  Results  by  Armstrong  and  Eyre,  1913. 


Gms.  per  Liter  Sat.  Sol. 

dmm  of  Sat. 

V  Sol. 

Pb(N03)2.                    PbCl2. 

o                    10.  81 

I  .  0069 

3.31           10.67 

1.0095 

8.28           10.65 

I.OI39 

16.56             10.84 

I.  02  10 

33-12               11.57 

... 

Aq.  Pb(N03)2 
Sol.,  Gms.  per 
1000  Gms.  H2O. 

Gms.  PbCU  per 
1000  Gms. 
Sat.  Sol. 

0 

10.89 

3-31 

10.96 

6.62 

i°-53 

33-12 

11.15 

82.80 

12.95 

SOLUBILITY  OF  LEAD  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  POTASSIUM 
CHLORIDE  AT  25.2°.       (von  Ende,  1901.) 


Normality 
of  KC1. 

0 
0.001 

Gm.  Equiv.  PbClj 
per  Liter. 

0.07760 
0.07664 

0.0025 

0.07570 

0.0049 
O.OO99 
0.0200 

0.07404 
0.07056 
0.06432 

0.0599 

0.04524 

Normality 

Gm.  Equiv.  PbCl2 

of  KC1. 

per  Liter. 

0.0999 

0.02380 

0.5006 

0.01480 

0.7018 

0.01476 

0.9991 

o  .  00980 

I.50I8 

0.00996 

2.OO24 

O.OIII2 

3.0036 

0.01948 

SOLUBILITY  OF  LEAD  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  POTASSIUM 
CHLORIDE  AT  20°.     (Bronsted,  1912.) 


Gm.  Equivalents  per 
1000  Gms.  Solution. 

"KC1. 
O.IQ5 

PbCl2. 
0.01900 

0.299 

0.01452 

0-375 
0.483 

0.01324 
0.01236 

0.510 

0-575 
0-639 

0.0125 
0.01068 
0.00954 

0.930 
I  .224 

1-575 

1.884 

0.00770 
0.00736 
0.00786 
0.00894 

Solid  Phase. 


Gm.  Equivalents  per 
1000  Gms.  Solution. 


Solid  Phase. 


PbCl2 


KC1. 
2.10 
2.  2O 
2.29 

2.36 


+2PbCl2.KCl 
aPbCVKCl 


2.45 
2.66 
2.77 
2.91 
3-05 


2PbCl2.KCl 


2PbCl2.KCl+PbCl2.KCl.|H2O 
PbCl,.KCl.JH20 


PbCl2. 
0.01022 
O.OIO6O 
O.OII84 
O.OI3OO 
0.01308 
0.01396  ' 
0.01476 
0.01550 
0.01656 
0.01780 

4.57*    0.0280* 
Gm.  equivalents  per  1000  Gms.  H^O. 

Data  for  the  solubility  of  lead  chloride  in  aqueous  KC1  and  aqueous  NaCl  are 
given  by  Demassieux,  1914. 
SOLUBILITY  OF  LEAD  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  ALCOHOL  AND  OF 

MANNITOL  AT  25°.       (Kernot  and  Pomilio,  1912.) 

Results  for  Aqueous  Ethyl  Alcohol.     Results  for  Aqueous  Mannitol. 


+KC1 


Gms.  per  Liter  .Solution. 


C2H5OH. 


5.75 

11.51 
23.02 
46.05 
92.10 
184.20 


10 


PbCl2. 

IO-75 
16 

9.36 
9.14 
8.25 
7.12 
4.76 


Gms.  per  Liter  Solution. 
(CH2OH)2(CHOH)T 


PbCl2. 

IO-75 
10.42 

10.67 
10.64 
10.91 
ii.  16 
11.29 
SOLUBILITY  OF  LEAD  CHLORIDE  IN  GLYCEROL.  (Presse,  1874.) 

I  part  glycerol  +  7  parts  H2O  dissolve  0.91  per  cent  PbCl2. 

I  part  glycerol  +  3  parts  H2O  dissolve  1.04  per  cent  PbCl2. 

I  part  glycerol  +  i  part  H2O  dissolves  1.32  per  cent  PbCl2. 

Pure  glycerol  dissolves  2  per  cent  PbCl2. 


2.84 

5.69 
11.38 
22.76 
45.53 
91.06 


LEAD   CHLORIDE 


356 


SOLUBILITY  OF  LEAD  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  SEVERAL 

COMPOUNDS  AT  25°.    (Armstrong  and  Eyre,  1913.) 


Gms.  PbCl2 

Gms.  PbCl2 

Aqueous 
Solution  of: 

per  1000 
Gms.  H2O. 

per  1000 
Gms.  Sat. 
Sol. 

Aqueous 
Solution  of: 

Gms.  C^mpd. 
per  1000 
Gms.  H2O. 

per  1000 
Gms.  Sat. 
Sol. 

Water  alone 

0 

10.89 

Ethyl  Alcohol 

11.51 

10.43 

Glycol 

15.51 

10-75 

Glycerol 

23.01 

10.98 

tt 

62.04 

10.90 

Propyl  Alcohol 

I5.OI 

10.08 

Acetaldehyde 

II.OI 

10.54 

a           it 

60.06 

9-37 

" 

33-03 

9.82 

Methyl  Acetanilide 

29.82 

10.25 

Paraldehyde 

II.OI 

10.50 

Hydrochloric  Acid 

9-12 

4-23 

u 

33-02 

9.96 

n              it 

18.23 

3.60 

ioo  cc."  anhydrous  hydrazine  dissolve  3  gms.  PbCl2  at  ord.  temp,  with  decom- 
position. (Welsh  and  Broderson,  1915.) 

SOLUBILITY  OF  LEAD  CHLORIDE  IN  PYRIDINE.  (Heise,  1912.) 


to 

Gms.  PbCljs 
per  ioo  Gms. 

Solid  Phase. 

Pyridine. 

—  20 

0.303 

PbCl2.2C5H5N 

0 

0.364 

tt 

+  22 

0-459 

n 

44 

0-559 

11 

65 

0.758 

tt 

76 

90 

94 

IO2 


Gms.  PbCl2 

per  ioo  Gms. 

Pyridine. 

0.893 
1.07 
I. 12 


Solid  Phase. 

PbCl2.2C5H5N 

it 


FREEZING-POINT  DATA  (Solubility,  see  footnote,  p.  i)  ARE  GIVEN  FOR 
THE  FOLLOWING  MIXTURES  OF  LEAD  CHLORIDE  AND  OTHER  COMPOUNDS. 

Lead  Chloride  +  Lead  Fluoride 
+  Lead  Iodide 
+  Lead  Oxide 
-j-  Lead  Sulfide 
+  Lithium  Chloride 
+  Magnesium  Chloride 
+  Manganese  Chloride 
-j-  Potassium  Chloride 
-J-  Rubidium  Chloride 
+  Silver  Chloride 
-f  Strontium  Chloride 
-j-  Sodium  Chloride 
-j-  Thallium  Chloride 
-j-  Tin  Chloride 


(Sandonnini,  1911.) 

(Monkemeyer,  1906.) 

(Ruer,  1906.) 

(Truthe,  1912.) 

(Tries,  1914.) 

(Menge,  1911.) 

(Sandonnini,  1911,  1914.) 

(Tries,  1914;   Lorenz  and  Ruckstuhl,  1906.) 


(Matthes,  1911;  Tries,  1914.) 

(Sandonnini,  1911,  1914.) 

(Tries,  1914-) 

(Korreng,  1914;  Sandonnini,  1913.) 

(Hermann,  1911;  Sandonnini,  1911,  1914.) 

(Herrmann,  1911.) 


+  Zinc  Chloride 
LEAD   CHLORIDE   (Basic). 

SOLUBILITY  OF  BASIC  LEAD  CHLORIDES  IN  WATER  AT  18 


(Pleissner,  1907.) 


Compound 

Basic  Lead  Chloride 


Formula. 


Gms.  per  Liter  Sat.  Aq. 
Solution. 


Pb 

0.079 
0.021 


Pb  Salt. 
0.099 
0.025 


PbCl2.PbO.H2O 

J     "  PbCl2.3PbO.H2O 

LEAD  FluoroCHLORIDE   PbFCl. 
SOLUBILITY  OF  LEAD  FLUOROCHLORIDE  IN  WATER  AND  IN  AQUEOUS  SOLUTIONS. 

(Stark,  1911.) 

Solubility  in  Water.  Solubility  in  Aq.  Solutions  at  25°. 


t. 

Gms.  PbFCl 
per  ioo  Gms. 

A,.So,u,ion           G-£FC> 

H,0. 

Ot: 

Sat.  Sol. 

0 

0.02II 

o  .  00996  n  PbCl2 

0.0030 

18 

0.0325 

0.0195    n 

O.OOOS 

25 

0.0370 

0.0392    n     " 

0.0005 

IOO 

O.IOSI 

Aq.  Solution 
of: 


Gms.  PbFCl 

per  ioo  cc. 

Sat.  Sol. 


o.o535wHCl  0.0758 

0.1069^    "  0.1006 

0.0518  n  CH3COOH    0.0512 


O.I055/J 


0.0561 


357  LEAD   CHROMATE 


LEAD  CHROMATE  PbCrO4. 

SOLUBILITY  OF  LEAD  CHROMATE  IN  WATER. 


t°.         "*     G™rffi°'  Method.  Authority. 


Normality 

Milligrams  * 

'b  per  100  cc.  b; 

it.  SQL  at: 

Normality 

of  HC1. 

18°. 

25°- 

37°. 

HNOj. 

O.I 

3.86 

4.96 

7.40 

O.I 

0.2 

8-15 

10.  06 

15.40 

0.2 

o-3 

I3-56 

I7-38 

27.30 

°-3 

0.4 

22.14 

27.78 

43.60 

0.4 

0.5 

32.30 

42.60 

68 

o-5 

0.6 

46.60 

61.06 

97.20 

0.6 

l8  3.0.IO"7  O.OOOIO  Solution  equilibrium  (Beck  and  Stegmiiller,  1910.) 

1  .4.  1  0~7  0  .  00004  (Auerbach  and  Pick.) 

1  8  3.2.IO"7  O.OOOIO  Conductivity  (Kohlrausch,  1908.) 

20  2.I.IO"7  0.00007  Radio  Indicators  (v.  Hevesy  and  Rona,  1915.) 

SOLUBILITY  OF  LEAD  CHROMATE  IN  AQUEOUS  SOLUTIONS  OF  HYDROCHLORIC 

AND  OF  NITRIC  ACIDS.     (Beck  and  StegmiUler,  1910,  1911.) 
Solubility  in  Aq.  HC1.  Solubility  in  Aq.  HNO3  at  18°. 

Milligrams  Pb  per 
100  oc.  Sat.  Sol. 

2;  67 
4.70 
6.46 

8.3I 
10.31 
12.39 

Results  are  also  given  for  the  solubility  of  mixtures  of  lead  chromate  and 
lead  sulfate  in  aqueous  hydrochloric  acid  at  25°  and  37°. 

SOLUBILITY  OF  LEAD  CHROMATE  IN  AQUEOUS  POTASSIUM  HYDROXIDE  SOLUTIONS. 

(Lacland  and  Lepierre,  1891.) 

t°.  Grams  KOH  per  loo  cc.    Grams  PbCrO4  per  icocc. 

15  2.308  I.Ip 

60  2.308  1.62 

80  2.308  2.61 

102  2.308  3.85 

LEAD    CITRATE   Pb(C6H5O7)2.H2O. 

SOLUBILITY  IN  WATER  AND  IN  ALCOHOL. 

100  gms.  H2O  dissolve  0.04201  gm.  Pb(C6H5O7)2.H2O  at  18°,  and 
0.05344  gm.  at  25°. 

100  gms.  alcohol  (95%)  dissolve  0.0156  gm.  Pb(C6H6O7)2.H2O  at 

1  8°,  and  0.0167  gm-  at  25°-  (Partheil  and  Httbner  —  Archiv.  Pharm.  241,  413,  '03.) 

LEAD    DOUBLE    CYANIDES. 

SOLUBILITY  IN  WATER. 

(Schuler  —  Sitzber.  Akad.  Wiss.  Wien,  79,  302,  '79.) 
Double  Salt.  Formula.  t°.    ^^Q00 

Lead  Cobalticyanide                    Pbg[Co(CN)6]2.7H2O                     18  56.5 

Lead  Cobalticyanide                    PbJCo(CN)6]2.7H2O                     19  61.3 

Lead  Potassium  Cobalticyanide  PbKCo(CN)6.3H2O                      18  14.8 

Lead  Cobalticyanide  Nitrate       Pb3fCo(CN)6]2.Pb(NO3)2.i2H2O  18  5.9 

Lead  Ferricyanide  Nitrate          PbjFe(CN)6]2.Pb(NO3)2.i2H2O   16  7.5 

Lead  Potassium  Ferricyanide      PbKFe(CN)6.3H2O                      16  21.0 

LEAD  FLUORIDE   PbF2. 

One  liter  of  water  dissolves  0.6  gm.  PbF2  at  9°,  0.64  gm.  at  18°,  and  O.68  gm.  at 
26.6°  (conductivity  method).  (Kohlrausch,  1908.) 

ipo  cc  anhydrous  hydrazine  dissolve  6  gms.  PbF2  at  room  temp,  with  decom- 
position. (Welsh  and  Broderson,  1915,) 

Freezing-point  data  (solubility,  see  footnote,  see  p.  i)  for  mixtures  of  PbF2  and 
PbI2  are  given  by  Sandonnini  (1911);  for  mixtures  of  PbF2  +  PbO  by  Sandon- 
nini  (1914);  for  mixtures  of  PbF2  +  Pb3(PO4)2  by  Amadari  (1912),  and  for 
PbF2  +  NaF  by  Puchin  and  Baskow  (1913). 


LEAD  FORMATE 


358 


LEAD  FORMATE   Pb(HCOO)2. 

SOLUBILITY  OF  LEAD  FORMATE  IN  AQUEOUS  SOLUTIONS  OF  BARIUM  FORMATE  AT  25°. 

(Fock,  1897-) 


Mol.  %  in  Solution. 

Grams  per  Liter. 

Sp.  Gr.  of 

In  Solid  Phase  Mol.  %  of 

Pb(HCO2)2. 

Ba(HCO2)2. 

'  Pb(HC02)2. 

Ba(HCO2)2. 

Solutions. 

Pb(HCO2)2. 

Ba(HC02)2.' 

O 

IOO 

28.54 

1.2204 

0 

IOO 

0.2Q 

99.71 

I  .IO4 

28.65 

I.22I3 

1.72 

98.28 

0.74 

99.26 

2.803 

28.90 

I  .2251 

5-29 

94.71 

1.24 

98.76 

5-3°9 

32.24 

1.2529 

11.94 

88.06 

2.91 

97.09 

ii  .42 

29.29 

I.234I 

24.81 

75-19 

5-92 

94.08 

23.11 

28.13 

1-2355 

56.54 

43-46 

IOO 

0 

28.35 

I  .0911 

IOO 

0 

LEAD  HYDROXIDE   Pb(OH)2. 

SOLUBILITY  OF  LEAD  HYDROXIDE  IN  AQUEOUS  SOLUTIONS  OF  SODIUM  HYDROXIDE. 

(Moist  Lead  Hydroxide  used,  temperature  not  given.) 

(Rubenbauer,  1902.) 

Grams  per  100  cc.  Solution. 


Amount  of  Na 

Amt.  of  Pb 

Mol.  Dilution 

in  20  cc. 

in  20  cc. 

of  NaOH. 

o  .  2024 

O.IOI2 

2.27 

0.3196 

0.1736 

1.44 

0.5866 

0-3532 

0.785 

0.9476 

o  .  407  i 

0.485 

1.7802 

0.5170 

0.258 

NaOH. 

1-759 
2.778 

5-1° 
8-235 

I5-470 


Pb(OH)2. 
0.590 
I  .OIO 
2.056 
2.370 
3.010 


LEAD  IODATE   Pb(IO3)2. 

One  liter  of  water  dissolves  0.0134  gm.  Pb(IO3)2  at  9.2°,  0.019  gm.  at  18°  and 

O.023  gm.  at  25.8°.  (Kohlrausch,  1908;  Bottger,  1903.) 

One  liter  H2O  dissolves  0.0307  gm.  Pb(IO3)2  at  25°.     (Harkins  and  Winninghoff,  1911.) 

SOLUBILITY  OF  LEAD  IODATE  IN  AQUEOUS  SALT  SOLUTIONS  AT  25°. 

(H.  and  W.,  1911  ) 


Gms.  per  Liter. 
KNO3. 
0.202 
I  .Oil 

5-055 
20.220 


Gms.  per  Liter. 


Gms.  per  Liter. 


Pb(I03)2. 
0.0318 
0.0363 
0.0567 
0.0708 


LEAD   IODIDE   PbL 


o 
15 
25 
35 
45 
55 
65 
80 

95 

IOO 


Density. 
(H2O  at  o°.) 

I.  0006 
0.9998 

o  .  9980 

0.9951 
0.9915 
0.9872 


0-9745 

o  9671 


KIO3. 
O.OII3 
0.0227 
Pb(N03)2. 
0.0165 
0.165 

SOLUBILITY 

(Lichty, 
Grams  PbI2 

Pb(IO3)2. 
0.0199 
0.0122 

0.0242 
O.OII5 

IN  WATER. 
1903.) 

per  100. 

cc.  Solution. 
O.O442 
0.0613 
0.0762 
0.1035 

o  .  1440 

0.1726 
0.2140 
0.2937 
0.3814 
O.42O 

Grams  H,O. 
0.0442 
O.O6I3 
0.0764 
0.1042 
0-1453 
0.1755 
0.2183 
0.3023 
0.3960 
0.436 

Pb(N03)2. 

1.656 

16.561 

82.805 

496.83 


Pb(I03)2. 
O.OO52 
0.0045 
0.0078 
0.0418 


Millimols  PbI2  per  100. 


cc.  Solution. 
0.096 

0.133 
0.165 
0.224 
0.312 

0-374 
0.464 
0.637 
0.828 
0.895 


Grams  H2O. 
0.096 

0.133 

0.166 
0.226 

0-315 
0.381 

0-473 
0.656 
0.859 
0.927 


^  Data  for  the  solubility  of  lead  iodide  in  water  by  the  conductivity  method  are 
given  by  Bottger,  1903;  Kohlrausch,  1904-05;  Denham,  1917. 


359  LEAD  IODIDE 

SOLUBILITY  OF  MIXTURES  OF  LEAD  IODIDE  AND  POTASSIUM  IODIDE  IN  WATER. 

(Ditte,  1881;  Schreinemakers,  1892.) 

Gms.  per  1000  Gms.  H2O. 

PbI2.  KT 

5  ...  163      Double  Salt +PbI2    50  526.7  1906  Double  Salt  +KI 

20  9          260  64  789.3          2161 

28  25          325  83.5     1,108.6          2434 

39  45          449  92         1,273  2566 

67  255          751  137        2,382  3278 

80  731        1186  165        4,187  4227 

80  569.9      976.4  218      10,303 

104.5      1411         1521  241       12,803  7998  " 

120          2151        1812  "  242       12,749  ...  " 

137          2874        2097  250      15,264 

175          5603        2947  157        5, 218  gms.  Pbl,.2Kl  >bl2.2Kl.2iHso 

189  ...       3339  "  172        6,489    ' 

9  96.6     1352  '    +KI   186        7,903 

13  114.3     1384  "     194        9,266    ' 

23  186.3     I3I°  "     201       11,320    ' 

Ordinary  solubility  method  used  for  temperatures  below  boiling-point  of  the 
solution  and  sealed  tube  (with  constriction  in  middle)  method  used  for  tem- 
peratures above  boiling  point. 

One  liter  sat.  aqueous  solution  of  iodine  dissolves  0.0021 6  gm.  mols.  PbI2  (0.996 
gms.)  at  2O°.  (Fedotieff,  1911-12.) 

SOLUBILITY  OF  LEAD  IODIDE  IN  ACETONE,  ANILINE  AND  AMYL  ALCOHOL. 

(von  Laszczynski,  1894.) 

AO  Gms.  PbL  per  ioo 

Gms.  Solvent. 

59  0.02 

13  °-5o 

184  i. 10 

C5H7OH  133.5  0-02 

SOLUBILITY  OF  LEAD  IODIDE  IN  PYRIDINE. 

(Heise,  1912.) 

Gms.  PbI2  Gms.  Pbl, 

t°.                   per  ioo  Gms.  Solid  Phase.                        t°.         periopGms.   Solid  Phase. 

Pyridine.  Pyridine. 

—  43 . 5  f  .-pt.             ...  Pblj.sCjHjN                        35             O.l88      Pblj^CsHjN 

—37        0.166        "          57    0.190 

—  20        0.175        "          77    0.228     "  • 

—  9        0.186        "          92    0.200     " 
o        0.200        "          98    0.340     " 

+  3         0.215        "          105    0.370 

6tr.pt.          0.225    Pbiz.aCjHsN+Pbiz^CsH^        108          0.410  " 

15  O.2O8  Pblz^CsHsN  112  0.445  " 

ioo  gms.  95%  formic  acid  dissolve  0.25  gm.  PbI2  at  19.8°.  (Aschan,  1913.) 

ioo  cc.  anhydrous  hydrazine  dissolve  2  gms.  PbI2  at  room  temp,  with  decom- 
position. (Welsh  and  Broderson,  1915.) 
Freezing-point  data  for  mixtures  of  lead  iodide  and  silver  iodide  are  given 
by  Matthes  (1911). 

T.F.AD  MAT.ATE  Pb.C4H4O5.3H2O. 

SOLUBILITY  IN  WATER  AND  ALCOHOL. 

(Partheil  and  Hubner,  1903.) 

ioo  gms.  H2O  dissolve  0.0288  gm.  PbC4H4Os.3H2O  at  18°,  and  0.06504  gm.  at 
25°. 

ioo  gms.  95%  alcohol  dissolve  0.0048  gm.  PbC4H4O6.3H2O  at  i8°-25°. 
Density  of  alcohol  employed  =  0.8092. 


LEAD  LAURATE  360 

LEAD  LAUEATE,  MYRISTATE,   PALMITATE  and  STEARATE. 

SOLUBILITY  OF  EACH  IN  SEVERAL  SOLVENTS. 

(Jacobson  and  Holmes,  1916.) 
(See  Lithium  Laurate,  p.  375,  for  formulas  and  other  details.    See  also  p.  362.) 


Solvent. 


Cms.  of  Each  Salt  (Determined  Separately)  per  too  Gms. 
Solvent. 


Pb  Laurate. 

Pb  Myristate. 

Pb  Palmitate. 

Pb  Stearate. 

35 

O.OOQ 

0.005 

O.OO5 

0.005 

So 

0.007 

0.006 

0.007 

0.006 

25 

O.OOg 

O.OO4 

0 

O 

35 

0.032 

O.OO4 

O.OOI 

O.OOI 

5° 

0.264 

0.052 

0.012 

0.004 

15-5 

0.061 

0.056 

0.051 

0.039 

25 

0.096 

0.078 

0.069 

0.051 

35 

0.113 

0.082 

0.076 

0.062 

5<> 

0.280 

O.II9 

0.093 

0.083 

14-5 

O.OIO 

0.013 

O.OIO 

0.007 

14 

0.017 

O.OIO 

0.009 

0.007 

35-5 

0.035 

0.015 

0.009 

0.008 

50 

O.2OI 

0.077 

0.033 

O.O2O 

15 

O.OII 

O.OIO 

0.009 

0.008 

Water 

Abs.  Ethyl  Alcohol 

u        u          <( 

tt        tt          (( 
Methyl  Alcohol 


Ether 

Ethyl  Acetate 
(t          u 

tt          tt 
Benzene 

LEAD  NITRATE  Pb(NO8)2. 

SOLUBILITY  IN  WATER. 

(Mulder;  Kremers,  1854;  at  15°,  Michel  and  Kraft,  1854;  at  17°,  Euler,  1904.) 
Grams  Pb(N03)2  per  100  Gms.  Grams  Pb(NO3)2  per  100  Gms. 


V  . 

O 
10 

17 

20 

25 
30 

Water. 

Solution. 
27.33^) 
3L6 
34-2 
35.2 
36.9 
38.8 

Water. 

Solution. 
41.9 

45 
47-8 
52.7 
57-1 
34-54 

36 

44 
50 
52 
56 
60 

•4 

•3 
•4 

•7 

L>       38.  8  W 

48.3 

54 

56.5 
60.6 

66 

40 
50 
60 
80 
IOO 
17 

69 

78 

88 
107 
127 
52 

•4 

•7 

.6 
.76* 

75 
85 
95 

138.8 

*  Euler. 
(i)  Mulder,  (2)  Kremers,  (3)  Average  of  M  and  K. 


Density  of  saturated  solution  at  17°  =  1.405. 
loo  gms.  H2O  dissolve  55.8  gms.  Pb(NO3)2  at  20°. 
Pb( 


(Euler.) 

F(LeBlanc  and  Noyes,  1890.) 
b(NO3)2  +  KNO3  at  20°  dissolve  95.39  gms.  Pb(NO3)2. 

+61.05  gniS.  KNO3.  (LeBlanc  and  Noyes,  1890.) 

loo  gms.  H2O  sat.  with  Pb(NO3)2  -f  NaNO3  at  20°  dissolve  38.42  gms.  Pb(NO3)2 

+84.59  Sms-  NaNO3.  (Le  Blanc  and  Noyes,  1890.) 

SOLUBILITY  OF  LEAD  NITRATE  IN  AQUEOUS  SOLUTIONS  OF  COPPER  NITRATE 

AT  20°. 

Fedotieff,  1911-12.) 
Gms.  per  100  Gms.  H2O. 


0 

-55  -ii2         J 

1   OttL.   O 
.419 

7-7 

39-34 

•354 

15.04 

27.80          ] 

.322 

24.63 

19.05          i 

.321 

33-25 

14.70 

•343 

Cu(NO3)o. 

Pb(NO3)2." 

1*20  ui  00.1.  hjvsi. 

37.96 

13.08 

1.360 

60.32 

8.19 

I.45I 

83.11 

5-37 

1.546 

100.29 

3-53 

1.622 

127.70* 

2.33* 

1.700 

*  Solid  phase  in  contact  with  this  solution  =  Pb(NO,),  +  Cu(NO,)2.6H,O. 


361 


LEAD  NITRATE 


SOLUBILITY  OF  LEAD  NITRATE  IN  CONCENTRATED  AQUEOUS  SOLUTIONS  OF  SODIUM 
NITRATE  AND  VICE  VERSA,  DETERMINED  BY  SYNTHETIC  METHOD. 

(Isaac,  1908.) 

(The  several  mixtures  were  enclosed  in  sealed  tubes  and  lieated  until  only 
one  or  two  very  small  crystals  remained  undissolved.  The  temperature  was 
then  determined  at  which  the  edges  of  these  crystals  just  showed  a  change  from 
sharp  to  round  or  vice  versa.) 


Results  for  Lead  Nitrate  as 
Solid  Phase. 

Cms,  per  100  Cms.  Sat.  Sol. 


Results  for  Sodium  Nitrate  as 
Solid  Phase. 


t°  Of 

Saturation. 
32 

35-5 
39-5 
44 
49.1 

55 
58 
62 
65 

SOLUBILITY  OF  MIXED  CRYSTALS  OF  LEAD  NITRATE  AND_STRONTIUM  NITRATE 

IN  WATER  AT  25°. 

(Fock,  1897-) 


'  NaNO3. 

Pb(N03)2. 

34-42 

19.69 

34-15 

20.33 

33-71 

21-35 

33-35 

22.  19 

32-94 

23.15 

32.60 

23-93 

32.47 

24.24 

32-33 

24-57 

32.19 

24-89 

t°  of 

Saturation. 

21 

26.5 

3i 

38.8 

41 

44.25 

51 


Cms,  per  100  Gms.  Sat.  Sol. 


NaNOj. 

Pb(NOa)2." 

40.97 

13.62 

42.04 

13.38 

43-18 

12.88 

44.63 

12.78 

45  -11 

12.94 

46.03 

12-45 

47.28 

12.50 

49-03 

11.76 

49.92 

11.56 

Mol.  per  cent  in  Solution. 

Gms.  per  ioo  cc.  Solution. 

Pb(NO3)2. 

Sr(N03)2. 

Pb(N03)2. 

SrCNO-O,. 

IOO 

0 

46-31 

O 

87.41 

12.39 

50-47 

4.56 

78.68 

21.32 

53-92 

8.14 

56.39 

43-61 

45-34 

17.81 

60.29 

39-71 

44.48 

18.74 

33-70 

36.30 

25-23 

35.03 

24.58 

75-42 

19-13 

37-54 

o 

IOO 

o 

71.04 

Sp.  Gr.  of 
Solutions. 


.4472 
.4336 
.4288 
,4263 

4245 
.4468 
.4867 

.5141 


Mol.  per  cent  in  Solid  Phase. 

'  PKNO^.   *    Sr(NO»)j.   " 

ioo 

99-05 
98.11 
97.02 
96.06 
83-84 


32.88 
o 


o 

0.95 
1.89 
2.98 
3.94 
16.16 
67.12 
ioo 


SOLUBILITY  OF  LEAD  NITRATE  IN  ETHYL  AND  METHYL  ALCOHOL. 


Solvent. 


Gms.  Pb(NOj)2  per  ioo  Gms.  Solvent  at: 


. 

Aq.  C2H5OH  (Sp.  Gr.  0.9282)   4.96 
Abs.  C2H5OH 
Abs.  CHsOH 


50°. 

14.9      (G) 
(deB) 


8°.  22°.  40°. 

5.82      8.77  12. 

0.04(20.5°) 
1.37       " 

(Gerardin,  1865;  de  Bruyn,  1892.) 

ioo  cc.  anhydrous  hydrazine  dissolve  52  gms.  lead  nitrate  at  room  temper- 
ature with  formation  of  a  yellow  precipitate.  (Wekh  and  Broderson,  1915.) 


SOLUBILITY  OF  LEAD  NITRATE  IN  PYRIDINE. 

(Walton  and  Judd,  1911.) 


Gms.  Pb(NO,)2 
t°.            per  ioo  Gms. 

Solid  Phase. 

Pyridine. 

-19.4 

2-93        Pfc 

.(NQ^C.H 

-14-5 

2.14 

" 

•IO 

1.90 

" 

o 

3-54 

" 

5.4 

3-93 

M 

8.7 

5-39 

M 

14.72 

6.13 

(« 

19.97 

6.78 

" 

24.75 

8.56 

• 

30.03 

10.96 

M 

34.97 

13.20 

« 

40.03 

16  94 

« 

Gms.  Pb(NOj) 

t°. 

per  ioo  Gms. 
Pyridine. 

45 

22.03 

49-97 

29-37 

51  tr.  pt. 

59-52 

36.70 

70 

47.29 

80 

61.60 

89-93 

90.21 

94  94 

128.06 

96  tr.  pt. 

. 

99.89 

143-36 

104.90 

152 

109.90 

163.80 

Solid  Phase. 


+Pb(NO,)2.3CsHlN 


+3Pb(N03)1.2C6HlN 
3Pb(NO,),.2C»H|N 


LEAD  NITRATE  362 

SOLUBILITY   OF   LEAD   NITRATE-NITRITE,    Pb(NO3)2.Pb(NO2)2.2Pb(OH)2.2H2O, 
IN  AQUEOUS  SOLUTIONS  OF  ACETIC  ACID  AT  13.3°. 

(Chilesotti,  1908.) 

Normality  of          Gms.  PbO  per  100  Normality  of        Cms.  PbO  per  100  cc. 

Acetic  Acid  cc.  Sat.  Sol.  Acetic  Acid.  Sat.  Sol. 

o  0.601  0.25  5-45° 

0.0$  1.323  0.50  9.690 

o.io  2.185  °-75  IJ5-874 

LEAD    OXALATE    PbC2O4. 

One  liter  of  water  dissolves  0.0015  gni.  PbC2O4  at  18°  (conductivity 

method).  (Bottger  —  Z.physik.  Chem.  46,  602,  '03;  Kohlrausch  —  Ibid.  50,  356,  W-'os.) 

LEAD    OXIDES.  SOLUBILITY  IN  WATER. 

(Bottger;  Ruer  —  Z.  anorg.  Chem.  50,  273,  '06.) 
No.  Description  of  Oxide.  G£r!S'     pe?LUer. 

1.  Yellow  Oxide,  by  boiling  Pb  hydroxide  with  10%  NaOH  i .  03  X  io~*  o.  023 

2.  Red  Oxide,  by  boiling  Pb  hydroxide  with  cone.  NaOH  0.56X10"*  0.012 

3.  Yellow  Oxide,  by  heating  No.  i  to  630°  1.05X10"*  0.023 

4.  Yellow  Oxide,  by  heating  No.  2  to  740°  1.00X10"*  0.022 

5.  Yellow  Oxide,  by  heating  com.  yellow  brown  oxide  to  620°  i .  09  X  io~*  o.  024 

6.  Yellow  Brown  Oxide  commercially  pure  i.ioXio"*  0.024 

7.  Yellow  Brown  Oxide,  by  long  rubbing  of  No.  5.  i.  12X10"*  0.025 

Bottger  gives  for  three  samples  of  lead  oxide,  0.017,  0.021,  and  0.013 
gm.  per  liter  respectively. 

One  liter  H2O  dissolves  0.068  gm.  PbO  at  18°,  solid  phase  PbO  and  0.1005  Sm- 
PbO  at  1 8°,  solid  phase  Pb3O2(OH)2.  (Pleissner,  1907.) 

Results  for  the  solubility  of  hydrated  lead  oxide  in  water  and  dilute  H2SO4 
solutions  are  given  by  Sehnal  (1909).*  The  results  are  considerably  higher  than 
the  above,  viz.  0.1385  gm.  Pb  per  1000  cc.  H2O  at  20°;  with  increase  of  H2SO4 
the  solubility  decreases  rapidly. 

100  cc.  anhydrous  hydrazine  dissolve  i  gm.  lead  oxide  (red)  at  room  temp. 

(Welsh  and  Broderson,  1915.) 

Freezing-point  lowering  data  for  mixtures  of  PbO  +  PbSO4  are  given  by 
Schenck  and  Rassbach,  1908.  Data  for  mixtures  of  PbO  +  SiO2  are  given  by 
Weiller,  1911,  and  by  Cooper,  Shaw  and  Loomis,  1909. 

LEAD  PerOXIDE  PbO2. 

The  two  forms  of  lead  superoxide,  (a)  amorphous  and  (&)  crystalline,  differ 
in  their  solubilities  in  sulphuric  acid.  One  liter  of  very  concentrated  H2SO 
dissolves  about  o.oio  mol.  PbO2  (&)  at  22°.  One  liter  of  cone.  H2SO4  contain- 
ing 1720  gms.  per  liter,  dissolves  0.0995  mol-  PbO2  (a)  at  22°.  The  solid  phase 
is  slowly  converted  to  Pb(SO4)2.  One  liter  of  H2SO4  containing  1097  gms.  HjSO* 
per  liter  dissolves  0.004  mol.  PbO2  at  22°.  The  solid  phase  is  converted  more 
quickly  to  Pb(SO4)2.  In  more  dilute  H2SO4  solutions  no  solubility  can  be  de- 
tected. (Dolezalek  and  Finckli,  1906.) 

LEAD  PALMITATE,   LEAD  STEARATE.    See  also  p.  360. 

100  cc.  absolute  ether  dissolve  0.0138  gm.  palmitate  and  0.0148  gm.  stearate. ' 

(Lidoff,  1893.) 
LEAD  TetraPHENYL  Pb(C6H6)4. 

Freezing-point  data  for  Pb(C6H6)4  +  Si(C6H6)4  are  given  by  Pascal  (1912). 

LEAD  PHOSPHATE   (Ortho)   Pbs(PO4)2. 

One  liter  water  dissolves  0.000135  gm.  lead  phosphate  at  20°  by  conductivity 

method.  (Bottger,  1903.) 

One  liter  of  4.97  per  cent  aqueous  acetic  acid  solution  dissolves  1.27  gms. 
Pba(PO4),.  (Bertrand,  1868.) 


363  LEAD   SUCCINATE 

LEAD  SUCCINATE  PbC4H4O4. 

SOLUBILITY  IN  WATER  AND  IN  ALCOHOL. 

(Partheil  and  Hiibner,  1903.) 

ioo  gms.  H2O  dissolve  0.0253  gm.  PbC4H4O4  at  18°,  and  0.0285  gm.  at  25°. 
100  gms.  95%  alcohol  dissolve  0.00275  gm«  PbC4H4O4  at  18°,  and  0.003  Sm» 
at  25°. 

Density  of  alcohol  used  =  0.8092. 

SOLUBILITY  OF  LEAD  SUCCINATE  IN  WATER. 

(Cantoni  and  Diotalevi,  1905.) 
t°.  10°.  21°.  32°.  39°.  50°. 

Gms.  PbC4H404  per  ioo  cc. 
sat.  sol.  0.015    0.019    0.024    0.027    0.029 

LEAD   SULFATE   PbSO4. 

SOLUBILITY  IN  WATER. 

(Average  curve  from  gravimetric  results  of  Dibbits  (1874),  Beck  and  Steg- 
miiller  (1910)  and  Pleissner  (1907)  and  conductivity  results  of  Bottger  (1903) 
and  Kohlrausch  (1904-05). 

t°.          Gms.  PbSO4  per  Liter.  t°.  Gms.  PbSO4  per  Liter. 

o       0.028         20       0.041 

5      °-°3i        25      0.045 

10      0.035         3°      °-049 

15      0.038         35      0.052 

18       0.040         40      0.056  . 

Results  considerably  higher  than  the  above  are  reported  by  Sehnal  (1909). 
This  author  finds  0.082  gm.  PbSO4  per  liter  at  18°  and  claims  that  the  presence 
of  H2SO4  in  the  PbSO4  reduces  the  solubility  very  greatly.  His  results  for  the 
solubility  in  presence  of  small  amounts  of  H2SO4  are: 

Gms.  H2SO4  per  1000  cc.  solu- 

tion o  0.0098    0.0196    0.0980    0.4900    0.9800 

Gms.  dissolved  PbSO4  per  1000 

cc.  solution  at  20°  0.082    0.051      0.025      0.013      0.006      o 

Sehnal  also  gives  results  showing  that  the  solubility  in  water  and  dilute  HjSO* 
solutions  is  exactly  the  same  at  100°  as  at  20°. 

Data  for  the  solubility  of  PbSO4  precipitates  are  given  by  deKoninck,  1907. 

SOLUBILITY  OF  LEAD  SULFATE  IN  AQUEOUS  SOLUTIONS  OF  AMMONIUM  ACETATE 
AND  OF  SODIUM  ACETATE. 

(Noyes  and  Whitcomb,  1905;  Dunnington  and  Long,  1899;  Dibbits,  1874.) 

In  Ammonium  Acetate.  In  Sodium  Acetate. 

At  25°  (Nand  W.).  '  At  100°  (D.  and  L.).  (D.). 


Millimoh  per  Liter.            Gms.  per  Liter.          G.  NHiCaHad  G.  PbSO4    Gms.  per  ioo  Cms.  H2O. 

NH.C.H.Q,.         PbSO»."  '  NHAHA.    PbS04:      *§£££  ShltS*'      NaC2H,O2.'     PbSO4.    ' 

o            0.134        o          0.041        28  7.12        2.05      0.054 

103.5             2.10              7.98      0.636           32  9.88           8.2           0.853 

207.1         4.55        15.96     1.33          37  10.58      41          11.23 

414.1       10.10        31.92     3.02          45  ii.  10 

SOLUBILITY  OF  LEAD  SULFATE  IN  AQUEOUS  SOLUTIONS  OF  AMMONIUM 
ACETATE  AT  25°. 

(Harden,  1916.) 

Gms.  per  1000  Gms.  Sat.  Sol.  Gms.  per  rooo  Gms.  Sat.  Sol. 

NH«CiH,0*.                PbS04.                         NH4C,H,0,.  PbSO4.  " 

7.96                  0.636                               53.4  5.60                  1.  012 

15.91             i-37°                    106.8  16.8              1.024 

31.70             3.04                      213.7  3S-9              1-045. 


Milligrams  Pb  per  100  cc.  Solution. 

Normal- 

Mgm.  Pb 

Normal- 

Mgm.  Pb 

At  18°. 

At  25°. 

At  37°. 

HNO3. 

So?. 

N»CL 

per  100  cc. 
Sol. 

I      2.6O 

3 

3.80 

O.I 

10.48 

O.I 

11.19 

19 

22.18 

28.04 

O.2 

17.48 

0.2 

18.73 

35-70 

42.88 

54-50 

0-3 

23.4I 

o-3 

26.51 

55-37 

65-15 

84.04 

0.4 

29.84 

0.4 

33-76 

75-27 

88.80 

I  I  I  .  9O 

LEAD   SULFATE  364 

SOLUBILITY  OF  LEAD  SULFATE  IN  AQUEOUS  SOLUTIONS  OF  POTASSIUM  ACETATE 

AND  OF  SODIUM  ACETATE  AT  25°.     (Fox,  1909.) 
In  Aq.  Potassium  Acetate.  In  Aq.  Sodium  Acetate. 

Gms.  per  100  Gms.  Sat.  Sol.  Gms.  per  100  Gms.  Sat.  Sol.  c  ... 

, * x         Solid  Phase.  , *- ^  |°hd 

CH3COOK.  (CH3COO),Pb.  CH,COONa.  (CH3COO)2Pb.      Na^SO,.  Phase' 

4.33              2.54  PbSO.+PbKjCSO^j             6.69             0.78               0.34  PbSO, 

9-°3  3-55  6.95          0.81  0.35 

17.81  5.43  11.76        2.73          1.26 
26.58         9.83  16.90         5.70  2.49 

28.82  11.40  19.92          8.24  3.60 
28.93         19-41                                         21.51         10.75  4-68 

In  the  case  of  the  CH3COOK  solutions,  the  double  salt  PbK2(SO4)2  is  formed 
and  no  SO4  ions  enter  the  solution. 

SOLUBILITY  OF  LEAD  SULFATE  IN  AQUEOUS  SOLUTIONS  OF  HYDROCHLORIC  AND 
OF  NITRIC  ACIDS  AND  OF  SODIUM  CHLORIDE. 

.(Beck  and  Stegmiiller,  1910.) 

T_  A  ur1!  In  Aq.  HNOa          In 

In  Aqueous  HL1.  ^  Tft0 

Normality 
of  HCl. 

o(  =  pureH20) 

O.I 
0.2 

0-3 

0.4 

SOLUBILITY  OF  LEAD  SULFATE  IN  AQUEOUS  SOLUTIONS  OF  SULFURIC  ACID 

AT   1 8°.     (Pleissner,  1907.) 
(  See  also  Sehnal,  preceding  page.) 

Gms.  per  Liter.  Millimols^  per  Liter.  Gms.  per  Liter.  Millimols  per  Liter. 

HtSO4.  PbSO4. "      'H2SO4.         PbSO4".  '  H2SO4. PbSO4.  '       H2SO4. PbSO4.' 

o  0.0382      o  0.126  0.0245      0.0194      0.25      0.064 

0.0049      0.0333      °-°5      o.no  0.0490      0.0130      0.50      0.043 

0.0098      0.0306      o.io      o.ioi  0.4904      0.0052       5  0.017 

SOLUBILITY  OF  LEAD  SULFATE  IN  CONCENTRATED  AQUEOUS  SOLUTIONS  OF  ACIDS. 

(Schultz,  1861;  Rodwell,  1862.) 
In  Aq.  H2SO4.  In  Aq.  HCl.  In  Aq.  HNO3. 

(a)  (b)  (c)  (a)  (b)  (c)  (a)  (b)  (c) 

1.540  63.4  0.003  I-°5  IO-6  0.14  i. 08  ii. 6  0.33 

1-793  85.7  o.on  i. 08  16.3  0.35  1. 12  17.5  0.59 

1.841  97  0.039  i-n  22  0.95  1.25  34  0.78 

1.14  27.5  2. ii  1.42  60  i. 01 

1.16  31.6  2.86 

(a)  Sp.  Gr.  of  Aq.  Acid,     (b)  Gms.  Acid  per  100  Gms.  Solution,     (c)  Gms.  PbSO4  per  100  Gms.  Solvent. 

SOLUBILITY  OF  LEAD  SULFATE  IN  CONC.  SOLUTIONS  OF  SULFURIC  ACID. 

(Donk,  1916.) 

Gm«.  per  100  Gms.  Gms.  per  100  Gms.'     , 

t«.  Sat.  Sol.  Solid  Phase.  t°.  Sat.  Sol.  Solid 

H2S04.  PbS04:  "H2S04.          PbS04. 

O  51.2  O  PbS04  IOO  6l.2  O  PbSO4 

O  89.4  O  "    +H5SO4.HeO  IOO  72.5  O.I 

o         97  o  H2so4  loo        96.3          0.2 

O  97.2  0.3  "     +PbSO4  IOO  99.1  0.9 

50         -50.4          o  PbSO4  200        79  o  " 

50        '86.7          o.i  200        88.8          o.i 

50         95-i          0.2  200        95.5          0.3 

50          99.3          0.6  200        98.9  i.i 

Additional  data  for  highly  concentrated  solutions  of  H2SO4  are  given  by  Ditz 
and  Kanhauser  (1916). 


365 


LEAD  SULFATE 


SOLUBILITY  OF  BASIC  LEAD  SULFATES  IN  WATER  AT  18°. 

(Pleissner,  1907.) 


Compound. 

\  Basic  Lead  Sulfate 
f  Basic  Lead  Sulfate 

LEAD   PerSULFATE 


Formula. 


One  Liter  Sat.  Solution  Contains: 


Mg.  Lead  Salt  =  Mg.  Pb  =  Millimols  Pb. 

PbSO4.PbO  13.4          10.6 

PbSO4.3PbO.H2O      26.2          22 

Pb(S04)2. 
SOLUBILITY  IN  AQUEOUS  SULFURIC  ACID  AT  22°. 


0.050 
0.106 


(Dolezalek  and  Finckli,  1906.) 


Gms.  per  Liter. 


"H2S04. 
948 

Pb(SO4)2. 
0 

1014 

1081 
1098 

0.719 
1.198 
1-557 

1130 
1180 

2.115 
5-749 

1217 

9-303 

Solid  Phase. 
PbOS04.H,0 


Gms.  per  Liter. 


H2S04. 

Pb(S04)2. 

1253 

14.85 

1352 

16.17 

1470 

9-30 

1532 

9.46 

1631 

19.80 

l698 

33-34 

1703 

35-22 

Solid  Phase. 
PbOSO4.H2O 

Pb(S04), 


The  solid  phase  at  concentrations  of  acid  up  to  1352  gms.  per  liter  is  the  white 
basic  salt  of  the  composition  PbOSO4.H2O.  In  the  concentration  limits  of 
about  1470-1703  gms.  H2SO4  per  liter  the  original  yellow  color  of  the  solid  phase 
remains  unchanged. 

Freezing-point  data  (solubility,  see  footnote,  p.  i)  for  mixtures  of  PbSO4-HLi2SO4, 
PbSO4  +  K2SO4  and  PbSO4  +  Na2SO4  are  given  by  Calcagni  and  Mariotta  (1912). 
Results  for  mixtures  of  PbSO4  +  K2SO4  are  also  given  by  Grahmann,  1913. 

LEAD   (Hypo) SULFATE. 

SOLUBILITY  OF  MIXTURES  OF  LEAD  HYPOSULPHATE  AND  STRONTIUM 
HYPOSULPHATE  AT  25°. 

(Fock  —  Z.  Kryst.  Min.  28.  389,  '97.) 


Mol.  per  cent  in  Solution. 

Grams  per  Liter.                 Rn  nr  nf 

Mol.  per  cent  in  Solid  Phase. 

PbSjO, 

SrSzCV 

PbS2O6. 

SrS2Oe.               Solutions. 

PbS208 

SrS20(j 

4H20. 

•4H20. 

.4H20. 

.4H20. 

0.0 

100.  0 

o.o 

145.6 

.1126 

0-0 

IOO-O 

1.05 

98-95 

2-97 

I5I.2 

.1184 

0.30 

99-7 

I5-3I 

84.69 

40.82 

152.5 

•1503 

3-87 

96.13 

46.80 

53-20 

149-2 

II4-5 

.2147 

9.84 

90.16 

62.30 

37-70 

256.1 

85.0 

.2889 

19.26 

80.74 

75-75 

24.25 

3Io-3 

67.0 

•3252 

23-73 

76.27 

78.09 

21  .91 

373-7 

70-8 

.3726 

32.24 

67.76 

88.29 

11.71 

509-5 

45-6 

.4671 

49-97 

50-13 

100.  0 

o.oo 

374-3 

o.o 

.6817 

0-00 

0-00 

LEAD  SULFIDE  PbS. 

One  liter  H2O  dissolves  3.6.10"*  gm.  Mols.  =  0.00086  gm.  PbS  at  18°,  (Weigel,  1907.) 
Determined  by  conductivity  method.  See  also  Bruner  and  Zawadzki  (1909). 
Fusion  diagrams  for  PbS  +  ZnS  and  PbS  +  Ag2S  are  given  by  Friedrich 

(1908).     Results  for  PbS  +  Sb2S3  are  given  by  Wagemmann  (1912). 

LEAD  SULFONATES. 


SOLUBILITY  IN  WATER. 

Name.  Formuta.  *•.%£!£&. 

Lead  2.5  Diiodobenzenesulfonate     C^HgOs^S-sPb^HzO  20  0.77    (Boyle,  1909.) 

Lead  ft  Naphthalene  Sulfonate         (C10H7SO3)2Pb.H2O    25  0.4      (Witte, '15;  Euwes, '09.) 

"      «  (doHvSOjJjPb.aHaO  24.9  4 . 195  (Euwes,  1909.) 

Lead  2  PhenanthreneMonosulfonate         iH,O  20  0.014  (Sandquist,  1912.) 

5  3H2O  20  0.08 

"  10  4H,0  20  0.14 


LEAD   TARTRATE 


366 


LEAD    TAETRATE    PbC4O6H4. 

SOLUBILITY  IN  WATER. 

(Caatoni  and  Zachoder  —  Bull.  soc.  chim.  [3]  33,  751,  '05;   Partheil  and  HQbner  —  Arckiv.  Pharm.  241. 

' 


A  o         Gms.  PW^OeJ^  per  .  0 

ioo  cc.  Solution. 

l8  O.OIO     (P.andH.)    50 

25  0.0108  "  55 
35  0.00105  60 
40  0.0015  65 


'03.) 

Gms.  PbC4O(jH4  per 
ioo  cc.  Solution. 

O.OO225 
O.OO295 
0.00305 
0.00315 


Cms 

IOO  CC 


70 

75 
80 

85 


PbC406H4  per 
cc.  Solution. 


0.0032 
0.0033 
0.0038 
0.0054 


NOTE.  —  The  positions  of  the  decimal  points  here  shown  are  just 
as  given  in  the  original  communications. 

ioo  gms.  alcohol  of  0.8092  Sp.  Gr.  (about  95%)  dissolve  0.0028  gm 
PbC4O6H4at  18°,  and  0.00315  gm.  at  25°.  (P  ^  H) 

LECITHIN 


ioo  gms.  of  sat.  solution  in  aqueous  5%  bile  salts  contain  4.5  gms.  lecithin  at 
I5°-2O°  and  7  gms.  at  37°.     Lecithin  is  practically  insoluble  in  water. 

(Moore,  Wilson  And  Hutchinson,  1909.) 

LEUCINE   CH3(CH2)3CH(NH2)COOH. 

ioo  cc.  H2O  dissolve  2.2  gms.  leucine  at  18°. 

ioo  cc.  alcohol  dissolve  0.06  gm.  leucine  at  17°. 

Data  for  the  solubility  of  leucine  in  aqueous  solutions  of  salts  at  20°  are  given 
by  Wiirgler ,  1914,  and  Pfeiffer  and  Wiirgler,  1916: 

LIGNOCERIC   ACID. 

Data  for  the  freezing-points  (solubility,  see  footnote,  p.  i)  of  mixtures  of 
lignoceric  acid  and  other  compounds  are  given  by  Meyer,  Brod  and  Soyka,  1913. 

LIGROIN. 

ioo  cc.  H2O  dissolve  0.341  cc.  ligroin  at  22°,  Vol.  of  solution  =  100.34,  Sp.  Gr. 
0.9969. 

ioo  cc.  ligroin  dissolve  0.335  cc.  H2O  at  22°,  Vol.  of  solution  =  100.60,  Sp.  Gr. 

0.6640.  (Herz,  1898.) 

LITHIUM   Li. 

One  gm.  atom  Li  dissolves  in  3.93  gm.  mols.  NHS  at  —80°,  at  —50°.  at  —25°, 

and  at  O°.  (Ruff  and  Geisel,  1906.) 

LITHIUM  ACETATE   CH3COOLi.2H2O. 

Freezing-point  data  for  mixtures  of  lithium  acetate  and  acetic  acid  are  given 
by  Vasilev,  1909. 

LITHIUM  SulfoANTIMONATE  Li3SbS4.ioH2O. 

SOLUBILITY  IN  WATER  AND  IN  AQUEOUS  ALCOHOL. 


In  Water.     (Donk,  1908.) 

Gms.  Li,SbS4 
t°.         per^ioo^Gma.  Solid  Phase.            t°. 

In  Aqueous  Alcohol  at  10°  and  30°. 

Gms.  per  ioo  Gms. 
Sat^Sol.              Solid  Phase.          Authority. 

i 

i 

—    i 

7 

2 

•j 
12 

SOL 

I                 Ice 
8                " 

IO 
IO 

CjHjOH. 
10.7 
26.2 

Li,SbS4. 
41  .  8      Li,SbS4.icHiO    (Donk,  1908.) 
36.5 

; 

—     c 

I 

17 

5 

" 

10 

66.2 

20 

.6 

—  IO 

8 

23 

2 

" 

30 

13-3 

46 

.  3      Li,SbS4.8iHtO 

—  *5 

9 

28 

5 

" 

30 

51-9 

30 

.7        " 

-26 

2 

35 

•2 

" 

30 

54-8 

29 

•9 

(Schreine- 

—42 

40 

4 

Ice+Li,SbS4.ioHzO 

30 

58.4 

30 

.8        " 

makers  and 

0 

45 

5 

LisSbS4.ioH,O 

30 

58.6 

32 

.3        "  +Li,SbS« 

Jacobs, 

+  10 

46 

9 

•« 

30 

65.26 

29 

.31         Li,SbS4 

1910.) 

30 

So 

i 

u 

30 

74-3 

24 

.  I 

SO 

5i 

3 

M 

30 

79-5 

20 

•  5 

LITHIUM  BENZOATE 


LITHIUM  BENZOATE   C6H6COOLi. 

SOLUBILITY  IN  AQUEOUS  ALCOHOL  SOLUTIONS  AT  25°. 

(Seidell,  1910.) 

Gms.  Q,H5COOLi 

per  zoo  Gms. 

Sat.  Sol. 

27.64 

28.60 

28.50 

27.80 

26.20 

23.60 

100  gms.  H20  dissolve  about  40  gms 

100  gms..  alcohol  dissolve  about  10  gms.  CeHsCOOLi  at  the  b.  pt. 

LITHIUM  BORATE  LizQBA. 

SOLUBILITY  IN  WATER. 

t°  o        10        20        30        40         45 

Gms.  Li2OB20s  per  100  Gms.  HjO     0.7      1.4      2.6      4.9     11.12    20 

(Le  Chatelier,  1897.) 

EQUILIBRIUM  IN  THE  SYSTEM  LITHIUM  OXIDE,  BORIC  OXIDE,  WATER  AT  30°. 

.'  (Dukelski,  1907.) 

nor  fnn  rime    Qa+    ^rtl 

Solid  Phase. 


Per  cent 
CjHsOH  in           s 
Solvent. 

JMof 
at.  Sol. 

0 
IO 

.103 

.088 

20 

.072 

30 

.052 

40 

.030 

50 

.003 

Per  cent 
QHjOH  in 
Solvent. 

da  of 
Sat.  Sol. 

Gms.  C«H6COOLi 
per  zoo  Gms. 
Sat.  Sol. 

60 

0.970 

19-80 

70 

0.932 

15.40 

80 

O.SOO 

IO.7O 

QO 

0.847 

6.40 

95 

0.823 

4-50 

100 

0.799 

2.6o 

I5COOLi  at 

the  b.  pt. 

(U.S.  P.) 

Li20. 

B203. 

OULLU  jruoac. 

7.01 

LiOH.H20 

7-51 

2.98 

" 

7.71 

3.38 

"  +Li2O.B2O3.i6H2O 

7.68 

3.56 

Li2O.B2O3.i6H2O 

5-40 

2.78 

" 

3-47 

2.42 

" 

2.94 

2-51 

" 

1.58 

3-27 

<« 

2.17 

6.90 

« 

3-66 

14.78 

« 

5-25 

22 

« 

5-63 

23-8 

" 

K.8l 

6.  20 

Li2O.2B203.*H2O 

Gms.  per  100  Gms.  Sat.  Sol. 

1.32 

0.86 

B203. 
3.36 
2.47 

0.53 

2.47 

2.17 

2.61 

5.08 

13.12 
16.39 
30.81 

4.10 

27.07 

3-22 

15.40 

i-55 

15.40 

1.30 
0.96 
0.63 

14.14 
11.47 
4.85 

o 

3-54 

Li20.5B20,.ioH20 


B(OH), 


Freezing-point  data  (solubility,  see  footnote,  p.   i)  for   mixtures  of  LiBOj 
+  NaBO2,  and  LiBO2  +  Li2SiO3  are  given  by  van  Klooster,  1910-11. 

LITHIUM  BROMATE  LiBrO3. 

100  gms.  H2O  dissolve  153.7  gms.  LiBrO3  at  18°,  or  100  gms.  saturated  solu- 
tion contain  60.4  gms.     Sp.  Gr.  of  sol.  =  1.833.  (Mylius  and  Funk,  1897.) 

LITHIUM  BROMIDE  LiBr.2H2O. 

SOLUBILITY  IN  WATER. 

(Kremers,  1858;  Bogorodsky,  1894;  Jones,  1907.) 


IO 

20 

30 
40 

44 
SO 
60 
80 

IOO 

159 


—  0.46 

Gms.  LiBr  per 
100  Gms.  H2O. 
1.058 

Solid  Phase. 
Ice(J) 

-1.94 
-  4.27 
-10.3 

4.274 
8.678 
17.80 

m 

-30.5 

37-^4 

" 

~45 
-30 

50 

80 

"  +LiBr.3l 
LiBr.3H2O 

—  10 

122 

" 

o 

+  4 

143 

160 

"  (K) 

"    +UET.2W 

1  66 

177 
191 
205 
209 
214 
224 

245 
266 


LiBr.2H20  (K) 


+LiBr.H20  (B) 
LiBr.  H2O  (K) 


LiBr.H20+LiBr  (B) 


Freezing-point  data  for  LiBr  +  LiOH  (Scarpa,  1915),  for  LiBr  +  AgBr. 

(Sandonnini  and  Scarpa,  1913.) 

loo  gms.  glycol  dissolve  60  gms.  LiBr  at  14.7°.  (de  Coninck,  1905.) 


LITHIUM   CAMPHORATE  368 

DiLITHIUM   d  CAMPHORATE   Ci0Hi4O4Li». 

SOLUBILITY  IN  AQUEOUS  SOLUTIONS  OF  CAMPHORIC  ACID  AT  i3.5°-i6° 
AND  VICE  VERSA. 

(Jungfleiscb  and  Landrieu,  1914-) 
Gms.  per  100  Gms.  Sat.  Sol. 
, » s  Solid  Phase. 


C6H14(COOH)2.  C10HuO4Li2. 

0.621  o  Camphoric  Acid  C6Hi4(COOH)2 

2.02  3.77 

3.25  10.63        Monolithium  Tetracamphorate 

3.51  12.61 

3.99  20.56  Dicamphorate         CioHi5O4.Li.CioHi604 

3-43  24.69  "      , 

2.87  37  .16  Camphorate  CioHi5O4Li 

o  40  .  80        Dilithium  Camphorate 


The  mixtures  were  kept  in  a  cellar  at  nearly  constant  temperature  and  shaken 
from  time  to  time  until  equilibrium  was  reached.  Additional  results  at  i7°-23° 
are  also  given. 

LITHIUM  CARBONATE  Li2CO3. 

SOLUBILITY  IN  WATER. 

(Bevade,  1885;  Fluckiger,  1887;  Draper,  1887.) 

An  average  curve  was  constructed  from  the  available  results  and  the  following 
table  read  from  it. 

Gms.  LigCOa  per  100  Gms.  Gms.  Li2C(\per  100  Gms. 


*0- 

Water. 

Solution. 

1;      * 

Water. 

Solution. 

0 

i-54 

1.52 

40 

I.I7 

1.16 

10 

i-43 

I.4I 

50 

1.  08 

1.07 

20 

i-33 

I-3I 

60 

1.  01 

1.  00 

25 

i  .29 

1.28 

80 

0.85 

0.84 

30 

1.25 

1.24 

IOO 

0.72 

0.71 

Density  of  saturated  solution  at  o°  =  1.017;  at  J5°  = 

SOLUBILITY  OF  LITHIUM  CARBONATE  IN  AQUEOUS  SOLUTIONS  OP 
ALKALI  SALTS  AT  25°. 

(Geffcken  —  Z.  anorg.  Chem.  43,  197,  '05.) 

The  original  results  were  calculated  to  gram  quantities  and  plotted 
on  cross-section  paper.  The  figures  in  the  following  table  were  read 
from  the  curves. 

Gms  Salt  Grams  Li2CO3  per  Liter  in  Aqueous  Solutions  of: 


per  Liter. 

KC1O3. 

KN08. 

KC1. 

NaCl. 

K2S04. 

Na2SO4. 

NH4C1. 

(NH4)2S04. 

O 

12.63 

12  .63 

12.63 

12.63 

12  .63 

12.63 

12.63 

12.63 

IO 

12.95 

I3-°5 

13  .IO 

13-4 

13.9 

14.0 

16.0 

2O-7 

20 

13.10 

13-3 

J3-5 

13  .9 

14.7 

15.0 

19.2 

25.0 

30 

13.25 

13.6 

13-8 

14-3 

IS-4 

16.0 

21.5 

28.2 

40 

13.40 

13-8 

14.0 

14.6 

16.0 

16.6 

23-3 

30.8 

<5o 

13.8 

14.2 

14-5 

16.9 

17.8 

26.0 

35-2 

80 

13-6 

14.0 

14.4 

17.7 

18.6 

27  .6 

38.5 

IOO 

J3-5 

13.9 

14.2 

18.2 

19.4 

28.4 

41.0 

120 

*3-3 

13-7 

14.0 

19.9 

28.7 

42.6 

140 

13.0 

J3-3 

.  .  . 

.  .  . 

20.4 

28.8 

43-5 

I7O 

12  .6 

28.0 

/ 

200 

12.2 

y 
20-0 

... 

loo  gms.  aq.  alcohol  of  0.941  Sp.  Gr.  dissolve  0.056  gm.  Li2CO3  at  15.5°. 
One  liter  sat.  sol.  in  water  contains  0.1722  gm.  mols.  =  12.73  gms-  Li2CO3  at  25°. 

(Ageno  and  Valla,  1911.) 


369 


LITHIUM  CARBONATE 


SOLUBILITY  OF  LITHIUM  CARBONATE  IN  AQUEOUS  SOLUTIONS  OF  ORGANIC  COM- 
POUNDS AT  25°. 

(Rothmund,  1908,  1910;  see  also  Traube,  1909.) 

The  solubility  in  H2O  =  0.1687  mols.  Li2CO3  per  liter  =  12.47  gms.  at  25°. 

Gm.  Mols.  LijCOs  per  Liter  in  Aq.  Solution  of: 
Aqueous  Solution  of: 

Methyl  Alcohol 

Ethyl  Alcohol 

Propyl  Alcohol 

Amyl  Alcohol  (tertiary) 

Acetone 

Ether 

Formaldehyde 

Glycol 

Glycerol 

Mannite 

Grape  Sugar 

Cane  Sugar 

Urea 

Thiourea 

Dimethylpyrone 

Ammonia 

Diethylamine 

Pyridine 

Urethan 

Acetamide 

Acetonitrile 

Mercuricyanide 

Freezing-point  data  for  mixtures  of  Li2CO3  '+  Li2SO.4  (Amadori,  1912.) 

Li2CO3  +  K2CO3.  (Le  ChateUer,  1894.) 


0.125 

0.25 

0.5 

i 

Normality. 

Normality. 

Normality. 

Normality. 

.  .  . 

0.1604 

0.1529 

0.1394 

O.l6l4 

0-1555 

O.I4I7 

0.1203 

0.1604 

0.1524 

0.1380 

0.1097 

0.1564 

0.1442 

0.1224 

o  .  0899 

0.1600 

O.I5I5 

0.1366 

o  .  i  104 

0.1580 

0.1476 

0.1300 

.  .  . 

0.1668 

0.1653 

0.1606 

O.I53I 

0.1660 

0.1629 

0.1565 

0.1472 

0.1670 

0.1647 

0.1613 

0.1532 

0.1705 

0.1737 

0.1778 

0.1702 

0.1728 

0.1752 

0.1778 

0.1693 

0.1689 

0.1661 

0.1557 

0.1686 

0.1673 

0.1643 

0.1605 

0.1667 

0.1643 

0.1600 

0.1523 

0.1562 

o  .  1460 

0.1280 

0.0992 

0.1653 

0.1630 

0.1577 

o  .  1466 

0.1589 

O.I48l 

0.1283 

0.0937 

0.1592 

0.1503 

0.1347 

0.1091 

0.1604 

0.1525 

0.1377 

0.1113 

.  .  . 

O.l6l4 

0.1520 

0.1358 

0.1618 

0.1556 

0.1429 

0.1178 

0.1697 

0.1704 

LITHIUM   (Bi)   CARBONATE  LiHCO,. 

100  gms.  H2O  dissolve  5.501  gms.  LiHCO3  at  13°. 


(Bevade,  1884.) 


LITHIUM  CHLORATE  LiClO3. 

loo  gms.  H2O  dissolve  213.5  gms.  LiClO3  at  18°,  or  100  gms.  sat.  solution  con- 
tain 75.8  gms.     Sp.  Gr.  of  sol.  =  1.815.  (Mylius  and  Funk,  1897.) 
ioo  gms.  H2O  dissolve  483^13.  LiClO3  at  1 5°,  di6  of  sat.  sol.  =  i  .82.    (Carlson,  1910.) 


LITHIUM  CHLORAURATE  LiAuCU. 


10 
20 
30 


Gms.  LiAuCl4  per 
ioo  Gms.  Solution. 


57-7 
62.5 


SOLUBILITY  IN  WATER. 

(Rosenbladt,  1886.) 

to         Gms.  LiAuCU  per 
ioo  Gms.  Solution. 


40 
50 


67.3 
72 


60 
70 
80 


Gms.  LiAuCli  per 
ioo  Gms.  Solution. 

76.4 

81 
85-7 


LITHIUM   CHLORIDE 


370 


LITHIUM  CHLORIDE  LiCl. 
SOLUBILITY  IN  WATER. 

Cms.  LiCl  per  100  Gms. 


(Average  curve  from  results  of  Gerlach,  1869.) 

Gms.  LiCl  per  100  Gms. 


»  . 

Water. 

Solution. 

0 

67 

40.1 

10 

72 

41.9 

20 

78-5 

44 

25 

Bi.S 

44.9 

3° 

84-5 

45-8 

I  . 

Water. 

Solution^ 

40 

90.5 

47-5 

50 

97 

49.2 

60 

103 

SI.Q 

80 

"5 

53-5 

100 

127.5 

56 

Density  of  saturated  solution  at  o°,  1.255;  at  15°,  1.275. 


SOLUBILITY  OF  LITHIUM  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  HYDROCHLORIC 

ACID. 

Results  at  25°.     (Here,  1911-12.) 

Gms.  per  100  cc.  Sat.  Sol. 
LiCl.  HC1.' 


Results  at  o°.     (Engel,  1888.) 

Gms.  per  100  cc.  Sat.  Sol. 


LiCl. 

HC1. 

»0  IN  oat.  i 

51 

0 

1.255 

41-4 

8.2 

1.243 

28.5 

24.1 

I..  249 

24.6 

29-5 

L25I 

57-4 
56.87 

53-64 
51.98 


o 

2.30 
3-84 
6.43 


SOLUBILITY  OF  LITHIUM  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  ALCOHOL  AT  25°. 

(Pinar  de  Rubies,  1913-1914.) 

'  The  LiCl  was  determined  by  titration  with  AgNOs.  Solutions  saturated  by 
constant  agitation  for  many  hours.  Solid  phase,  LiCl.r^O  for  all  mixtures. 
The  anhydride,  LiCl,  separates  only  from  the  most  highly  concentrated  alcohol 
solutions. 


Gms.  per  100  Gms.  Sat  Sol. 


Gms.  per  100  Gms.  Sat.  Sol. 


CiH6OH. 

O 
IO 
20 

30 
40 


LiCl. 
44.9 
40.9 
37-25 

33-3 
29.4 


QH5OH. 

50 
60 

70 

75 
80 


LiCl. 

25-75 
21.6 
21. 1 
20.8 
20.75 


SOLUBILITY  OF  LITHIUM  CHLORIDE  IN  ETHYL  ALCOHOL  AT  DIFFERENT 

TEMPERATURES.       (Turner  and  Bissett,  1913.) 
o          Gms.  LiCl  per  100 
Gms.  QjH6OH. 


Solid  Phase. 


Solid  Phase. 


O 

5 
10 

i5 
17 


Solvent. 


14.42          LiC1.4C2H5OH 

15-04 
16.77 
18.79 
20.31 

SOLUBILITY  OF  LITHIUM  CHLORIDE  IN  SEVERAL  SOLVENTS. 

Gms.  LiCl 


20 

24.28 

LiCl 

30 

25.10 

« 

40 

25-38 

n 

50 

24.40 

M 

60 

23.46 

ft 

Gms.  LiCl 

per  100 

Gms. 

Solvent. 


Authority. 


Solvent.       t° 


per  100 

Gms. 

Solvent. 


Authority. 


9-03 

10-57* 
4.32* 
1-93* 


(Turner  &  Bissett,  1913.) 
(Andrews  &  Ende,  1895.) 
(Patten  &  Mott,  1907.) 


Alcohol:  Alcohol: 

Methyl    25  42.36    (Turner  &  Bissett,  1913.)  Amyl  25 

Ethyl        25  2 . 54*  (Patten  &  Mott,  1904.)          "  ? 

Propyl      25  16.22     (Turner  &  Bissett,  1913.)       "  25 

?  15.86     (Schkmp,  1894.)  Butyl  25 

25  3.86*(P*tten&Mott,  1904.)     Glycerol  25 

Allyl        25  4.38*  Phenol  53 

*  Fused  LiCl  used  for  these  determinations. 

loo  cc.  anhydrous  hydrazine  dissolve  16  gms.  LiCl  at  room  temp. 

(Welsh  and  Hroderson,  1915.) 


371 


LITHIUM  CHLORIDE 


t°. 

8 
28 
40 
60 
80 

IOO 


SOLUBILITY  OF  LITHIUM  CHLORIDE  IN  SEVERAL  SOLVENTS. 

(Laszczynski,  1894;    deConinck,  1905.) 


In  Acetone.  (L.) 


In  Pyridine.  (L.)        In  Glycol.  (de  C.) 


Gms.  LiCl 

Gms.  LiCl 

f. 

per  100  Gms. 

t°. 

per  100  Gms. 
(CH,)2CO. 

0 

4.60 

46 

3-76 

12 

4.41 

53 

3-12 

25 

4.II 

58 

2.14 

"t°. 

15 


Cms.  Lid 
per  too  Gms. 
C6H5N. 

7-78 
14-26 


Cms.  Lid 
t°.    per  100  Gms. 
Sat.  Sol. 

15         ii 


SOLUBILITY  OF  LITHIUM  CHLORIDE  IN  PYRIDINE. 

(Kahlenberg  and  Krauskopf,  1908.) 

In  97%  Pyridine 


In  Anhydrous  Pyridine. 


Gms.  LiCl  f>er  100  Gms. 

Solid  Phase. 

LiC1.2CfiH6N 
tt 

u 

tt 
tt 

'  Sat.  Sol.          Solvent. 
11.31           12.71 
11.87           13.47 
I  I.  60           I3.IO 
11.38           12.84 
11.71           13.27 
13.01           14.98 

tr.  temp,  about  28°. 


K-     V,  3%HS° 

by  Volume. 

.„          Gms.  LiCl  per  TOO  Gms. 

Sat.  Sol. 

22  12.50 

32  13-79 

45        15-58 

58  16.72 

72  17.12 

97        i8.35 


Solvent. 
14.31 
15.98 
18.46 
2O.O8 

20.66 
22.48 


SOLUBILITY  OF  LITHIUM  CHLORIDE  AT  25°  IN  MIXTURES  OF: 


Acetone  and  Benzene. 

(Marden  and  Dover,  1917.) 


Ethyl  Acetate  and  Benzene. 

(Marden  and  Dover,  1917.) 


Gms.  Acetone     Gms.  LiCl 
per  100  Gms.    per  100  Gms. 
Solvent.  Solvent. 


Gms.  Acetone       Gms.  LiCl 
per  loo  Gms.    per  100  Gms. 


IOO 
00 
80 
60 


2.30 
1.69 
0.966 
0.234 


Solvent. 

40 

2O 

IO 

O 


Solvent. 
0.088 
O.OI9 
0.009 
O 


Gms.  Ethyl  Acetate 

per  100  Gms. 

Solvent. 

IOO 


70 


Gms.  LiCl 
per  loo  Gms. 
Solvent. 
I.78 

0.147 
0.028 
0.005 


DISTRIBUTION  OF  LITHIUM  CHLORIDE  BETWEEN  WATER  AND  AMYL 
ALCOHOL  AT  30°. 

(Dhar  and  Datta,  1913.) 


Mols.  LiCl  per  Liter.  Cl 

H2O  Layer  c\.  Alcohol  Layer  Cj.  ** 

3.24                0.0347  93.37 

3.06                0.0325  94.15 

2.93                0.0300  97-70 

2.82                O.0275  102.58 

2.76               O.O250  IIO.40 


Mols.  LiCl  per  Liter.  ft 

H2O  Layer  c\.  Alcohol  Layer  c^.              ** 

2.68  0.0240  in.  66 

2.58  0.0275  H3.40 

2.34  O.020O  117 

1.84  0.0125  147-2 

0.65  O.003O  2l6.66 


Freezing-point  data  (solubility,  see  footnote,  p.  i)  are  given  for  the  following 
mixtures  of  lithium  chloride  and  other  compounds. 

Lithium  Chloride  +  Lithium  Hydroxide  (Scarpa,  1915.) 

-j-  Magnesium  Chloride  (Sandonnini,  1913,  1914.) 

+  Manganese  Chloride  (Sandonnini  and  Scarpa,  1913.) 

+  Potassium  Chloride  (Richards  and  Meldrum,  1917.) 

"          +'NaCl  (Richards  and  Meldrum,  1917.) 

+  Rubidium  Chloride  (Richards &Meldrum,'i7;  Zemcznzny  &Rambach,'lo.) 

+  Silver  Chloride  (Sandonnini,  191  ia,  1914.) 

-j-  Sodium  Chloride  (Zemcznzny  and  Rambach,  1910.) 

-j-  Strontium  Chloride  (Sandonnini,  1911,  191  ia,  1914.) 

-j-  Thallium  Chloride  (Sandonnini,  1911,  1914.) 

"  -j-  Tin  Chloride  (ous)  (Rack,  1914.) 


LITHIUM  CHROMATE  372 

LITHIUM   CHROMATE  Li2CrO4.2H2O. 


LITHIUM    BICHROMATE    Li2Cr2O7.2H2O. 

SOLUBILITY  IN  WATER  AT  30°. 

(Schreinemaker  —  Z.  physik.  Chem.  55,  79,  '06;  at  18°,  Mylius  and  Funk  —  Ber.  30,  1718, '97.) 
Composition  in  Weight  per  cent: 


Of  Solution.  Of  Residue. 

%Cr03.  %Li20.  %Cr03.  %Li2O. 

o.o  7.09 

6.986  7.744  4.322  18.538 

16.564  8.888  10.089  19.556 

25.811  10.611  15.479  21.106 

33.618  12.886  24.365  19-398 

37.411  14-306  44-555  i7-4ii 

37.588  14.381  36.331  18.552 

37-495  13-3"  5*-o75  16.384 

40.280  10.858 

43.404  11.809  53-793  14-070 

45-I3o  9-5I5  56-085  10.190 

47-945  7-951  58-029  9.238 

57.031  6.432  65.560  8.733 

67-73I  5-7I3  71-687  8.513 

67.814  5.689  80.452  3.780 

65.200  4.661 

63.257  2.141  85.914  0.758 

62.28 


Solid 
Phase. 


LiOH.H2O 


LiOH  JI20  +  Li2Cr04.2H20 


Li2CrO4.2H2O 


Li2CrO4.2 


Li2Cr2O7.2H2O 


Li2Cr207.2H20  +  CrOg 


CrO, 


A  saturated  aqueous  solution  contains: 

.49-985  Per  cent  Li2CrO4,  or  100  grams  H2O  dissolve  99.94  grams 
Li2CrO4  at  30°  (S.). 

56.6  per  cent  Li2Cr2O7,  or  100  grams  H2O  dissolve  130.4  grams 
Li2Cr2O7  at  30°  (S.). 

52.6  per  cent  Li2CrO4,  or  100  grams  H2O  dissolve  110.9  grams 
LiCrO4  at  18°  (M.  and  F.). 

Sp.  Gr.  of  sat.  solution  at  18°  =  1.574. 

LITHIUM  CITRATE  C3H4(OH)(COOLi)3.4H2O. 

100  gms.  HjO  dissolve  61.2  gms.  Li  citrate  at  15°.     d^  sat.  sol.  =  1.187. 

(Greenish  and  Smith,  1902.) 


SOLUBILITY  IN  AQUEOUS  ALCOHOL  AT  25°. 

'    (Seidell,  1910.) 


Wt    Of 

Gms. 

Gms. 

wt.  % 

.CjHuoH 

in  Solvent. 

<*25  of            C3H4OH(COOLi)3.- 
Sat.  Sol.         4H2O  per  100  Gms. 
Solvent. 

Wt.  % 
C2H6OH 
in  Solvent. 

<Z.E  of          C3H4OH(COOLi)3.- 
Sat.  Sol.        4HjO  per  icx»  Gms. 
Solvent. 

o 

1.216 

74-50 

50 

0-933 

4-93 

10 

I.I5O 

49-30 

60 

0.897 

2.25 

20 

1.083 

32.10 

70 

0.867 

0.60 

30 

1.025 

18.80 

80 

0.838 

0.30 

40 

0.976 

9-65 

100 

0.788 

O.O2 

373  LITHIUM  FLUORIDE 

LITHIUM  FLUORIDE  LiF. 

100  gms.  H2O  dissolve  0.27  gm.  LiF  at  18°.     Sp.  gr.  of  sol.  =  1.003. 

(Mylius  and  Funk,  1897.) 

F.-pt.  data  for  LiF  +  LiOH  and  for  LiOH  +  Lil  are  given  by  Scarpa,  1915. 
LITHIUM  FORMATE  HCOOLi. 

SOLUBILITY  IN  WATER. 

(Groschuff,  1903.) 

Gms.  Mols.  Gms.  Mols. 

to          HCOOLi        HCOOLi         «....  p.  to          HCOOLi        HCOOLi       «,,..  p. 

*•      per  100  Gms.  per  100  Mols.     Solid  Phase.         t.      per  I00  Gms.  per  100  Mols.    Solld  Phase> 
Solution.  H20.  H,0.  H^O. 

—  20  21.14  9-28  HCOOLi.H2O      91  54.16  40.90    HCOOLi.H2O 

o  24.42  ii.  18  98  57.05  45-99        HCOOLi 

18  27.85  13.36  104  57-64  47-n 

49-S  35-<5o  19-14  120  59.63  51.13 

74  44.91  28.22 

Sp.  gr.  sat.  sol.  at  .18°  =  1.142. 

SOLUBILITY  OF  NEUTRAL  LITHIUM  FORMATE  IN  ANHYDROUS  FORMIC  ACID. 

(Groschuff,  1903.) 


Gms.  HCOOLi 

Mols.  HCOOLi 

t°. 

per  loo  Gms. 
Solution. 

per  loo  Mols. 
LHCOOH. 

Solid  Phase. 

0 

25-4 

30 

HCOOLi 

18 

25-9 

30-9 

tt 

39 

26.4 

31-75 

tt 

60 

26.9 

32.6 

" 

79 

27.8 

34 

*' 

LITHIUM  HIPPURATE  C6H6CO.NHCH2COOLi. 

100  gms.  H2O  dissolve  about  40  gms.  of  the  salt  at  15-20°. 

(Squire  and  Caines,  1905.) 
LITHIUM  HYDROXIDE  LiOH.H2O. 

SOLUBILITY  IN  WATER. 

(Dittmar,  1888;  Pickering,  1893.) 


Gms.  per  100  Gms.         Gms.  LiOH 
t°.                           Solution.                per  100  Gms.      t°. 

Gms.  per  too  Gms.         Gms.  LiOH 
Solution.                per  I00  Cms- 

Li20       = 

.      LiOH.  '            HiO. 

Li20      = 

LiOH. 

H20. 

-10.5 

.  . 

7- 

23 

. 

30 

7-05 

II 

.27 

12.9 

—  1  8  Eutec. 

ii 

.  2 

.  . 

. 

40 

7.29 

II 

.68 

13 

0 

6 

.'67 

10 

.64 

12 

•  7 

50 

7.56 

12 

.12 

13-3 

10 

6 

•74 

IO 

.80 

12 

•7 

60 

7.96 

12 

.76 

13-8 

20 

6 

.86. 

10 

•99^ 

12 

.8 

80 

8.87 

14 

.21 

15-3 

25 

6 

•95 

II 

.14 

12 

•9 

100 

10.02 

16 

.05 

17.5 

SOLUBILITY  OF  LITHIUM  HYDROXIDE  IN  AQUEOUS  SOLUTIONS  OF  LITHIUM 
SULFOANTIMONATE  AT  30°  AND  VlCE  VERSA. 

(Donk,  1908.) 

Gms.  per  100  Gms.  Gms.  per  100  Gms. 

Sat.  Sol.  Solid  Phase.,,                           Sat.  Sol.                              Solid  Phase. 

EiOIL                Li3SbS4.  LiOH.               Li3SbS4. 

II.4                  O  LiOH.HjO                    2.1                48.3             LiOH.H20 

9.1                   8.3  2.1                52.1                 "  +Li3SbS4.ioHI0 

2.3                 29.9  1.4                 51.8                   LUSbS4.ioH,Q 

O  51-3 

Data  for  equilibrium  in  the  system  lithium  hydroxide,  phenol,  water  at  25°  are 
given  by  van  Meurs,  1916. 


LITHIUM   IODATE 


374 


LITHIUM   IODATE   Li(IO3).£H2O. 

100  gms.  H2O  dissolve  80.3  gms.  LiIO3  at  18°,  or  100  gms.  solution  contain 
44.6  grams.     Sp.  gr.  of  sol.  =  1.568.  (Mylius  and  Funk,  1897.) 

LITHIUM  IODIDE  LiI.3H2O. 

SOLUBILITY  IN  WATER; 

(Kremers,  1858,  1860;  ice  curve,  Jones,  1907.) 


I  . 

Water. 

Sat.  Sol. 

OU11U  JTUctiC. 

V    . 

Water. 

Sat.  Sol. 

ooiia  rnase. 

—0.296 

1 

.08 

1.  06 

Ice 

20 

165 

62. 

2 

LiI.3H2O 

—  1.218 

A 

.36 

4.19 

a 

25 

I67 

62. 

6 

« 

-2.70 

8 

•71 

8.02 

« 

30 

171 

63- 

i 

« 

-  6.14 

17 

.69 

15-03 

it 

40 

179 

64- 

2 

M 

-16.2 

38 

3i 

27.70 

ii 

50 

187 

6$. 

2 

M 

-25 

48 

.67 

32.72 

tt 

60 

202 

66. 

9 

« 

~59 

85 

!3 

46 

u 

70 

330 

69. 

7 

M 

—69  Eutec. 

93 

48.2 

Ice+LiI.3H2O 

75 

263 

72. 

5 

H 

-60 

IOO 

50 

LiI.3H20 

75 

m.  pt. 

«« 

—40 

118 

54.13 

M 

85 

m.  pt. 

.  .  . 

LiI.2H20 

—  20 

134 

57-27 

<( 

80 

435 

81. 

| 

LiI.H2O 

o. 

151 

60.2 

it 

IOO 

481 

82. 

8 

(( 

10 

157 

61.1 

(i 

1  20 

590 

85- 

$ 

a 

SOLUBILITY  OF  LITHIUM  IODIDE  IN  SEVERAL  SOLVENTS. 


Solvent. 

t°. 

Methyl  Alcohol 

25 

Ethyl  Alcohol 

25 

Propyl  Alcohol 

25 

Amyl  Alcohol 

25 

Glycol 

Furfurol 

25 

Nitromethane 

O 

n 

25 

*  Solid  phase  = 

LiI.4C3H7OH. 

Gms.  Lil  per 
100  Gms.  Solvent. 

Authority. 

343-4 

(Turner  and  Bissett, 

1913.) 

250.8 

"                  " 

47.52* 

«                  « 

112.5 

"                  " 

38-9 

(de  Coninck,  1905.) 

45  -9t 

(Walden,  1906.) 

I.22f 

« 

2.52 

" 

f  =  gms.  per  100  cc.  sat.  solution. 
F.-pt.  data  for  Lil  +  Agl  are  given  by  Sandonnini  and  Scarpa,  1913. 

LITHIUM  IODOMERCURATE   2LiI.HgI2.6H2O. 

100  gms.  sat.  solution  of  lithium  iodomercurate  in  water  prepared  by  cooling  a 
hot  solution  and  allowing  to  stand  at  24.7°  for  3  months,  contained  1.30  gms.  Li, 
27.4  gms.  Hg,  58  gms.  I  and  13.3  gms.  H2O;  Sp.  Gr.  of  the  sat.  sol.  =  3.28. 

(Duboin,  1905.) 

LITHIUM   LAURATE,   MYRISTATE,   etc. 
SOLUBILITY  IN  WATER  AND  IN  ALCOHOL  OF  d  =  0.797,  AT  18°  AND  AT  25°. 

(Partheil  and  Ferie,  1903.) 

Gms.  Salt  per  100  cc.  Sat.  Solution  in: 


Salt. 

Formula. 

Water  at 

Alcohol  at 

18°. 

25°- 

18°. 

25°. 

Stearate 

CnH^COOLi 

O.OIO 

O.OII 

0.041 

0.0532 

Palmitate 

C15H3iCOOLi 

O.OII 

0.018 

0.0796 

0.0956 

Myristate 
Laurate 
Oleate 

Ci3H27COOLi 
CnH23COOLi 
CnH-aCOOLi 

0.0232 

0.158 
0.0674 

0.0234 
0.1726 

0.1320 

0.184 
O.4l8 

o  .  9084 

0.2100 
0.4424- 
I.OIO 

375 


LITHIUM  LAURATE 


LITHIUM  LAURATE,   MYRISTATE,   PALMITATE   and   STEARATE. 

SOLUBILITY  OF  EACH  OF  THESE  SALTS,  DETERMINED  SEPARATELY,  IN 
SEVERAL  SOLVENTS. 

(Jacobson  and  Holmes,  1916.) 

Li  laurate  =  CnH23COOLi.  Li  myristate  =  CisH^COOLi,  Li  palmitate  = 
CH3(CH2)uCOOLi  and  Li  stearate  =  CH3(CH2)16COOLi. 

Excess  of  salt  shaken  with  solvent  for  2  hrs.  in  all  cases.  The  sat.  sol.  was 
analyzed  by  evaporating  to  dryness  and  weighing  residue. 

Gms.  of  Each  Salt  (determined  separately)  per 

100  Gms.  Solvent. 
Solvent. 


Abs.  -Ethyl  Alcohol 


Methyl  Alcohol 

«  « 

a  a 

ti  (i 

Water 
tt 


Ether 
a 


•>  . 

Li 

Li 

Li 

Li 

Laurate. 

Myristate. 

Palmitate. 

Stearate. 

20 

0.403 

0.194 

0.096 

0.072 

25-4 

0.447 

O.224 

O.II8 

0.089 

35 

0.546 

0.278 

0.142 

0.106 

5o 

0.782 

0-435 

0.248 

0.200 

65 

I.I49 

0.669 

0.391 

0-333 

15-2 

3-159 

1.346 

0.616 

0-349 

25 

3-773 

i.  680 

0.771 

0-439 

34-6 

4-597 

2.193 

i.  086 

0.658 

50 

6.088 

3.281 

1.652 

1-057 

16.3 

0.154 

0.027 

O.OIO 

0.009 

25 

0.187 

0.036 

0.015 

O.OIO 

35 

0.207 

0.042 

0.015 

O.OIO 

50 

0.280 

0.062 

15-8 

O.OII 

0.013 

0.007 

O.OII 

25 

0.006 

0.004 

0.007 

O.OII 

16 

0.073 

0.029 

0.019 

O.OII 

25-7 

6.  in 

0*046 

0.032 

0.028 

35 

0.126 

0.062 

0.033 

0.031 

49-2 

0.203 

0.109 

0.069 

0.060 

15.2 

0.006 

0.004 

0.004 

0.004 

14-5 

0.068 

0.037 

0.038 

0.034 

25 

0.064 

0.034 

0.024 

0.029 

35 

0.061 

0.044 

0.037 

0.031 

50 

0.061 

0.045 

0.036 

0.044 

24-5 

0.026 

0.013 

0.015 

0.012 

15 

0.300 

0.413 

0.434 

0.571 

25 

0.376 

0.447 

0.508 

0.706 

35 

0.430 

0.502 

0-537 

0.663 

Amyl  Alcohol 


Chloroform 
Amyl  Acetate 


Methyl  Acetate 

Acetone 
tt 


^  The  above  lithium  salts  were  prepared  by  adding  the  calculated  amount  of 
lithium  acetate  to  the  alcoholic  solutions  of  the  respective  fatty  acids.  The 
resulting  precipitates  were  dissolved  in  boiling  alcohol  and  the  solutions  allowed 
to  stand  over  night  in  a  cool  place.  The  salts  so  obtained  were  washed  and 
dried. 

LITHIUM  TetraMOLYBDATE   Li2O.MoO3.2H2O. 

100  cc.  sat.  aqueous  solution  contain  43.13  gms.  Li2O.MoO3.2H2O  at  20°.    d» 
of  sat.  sol.  =  1.44.  (Wempe,  1912.) 


LITHIUM  NITRATE  376 

LITHIUM   NITRATE   LiNO3.3H2O. 

SOLUBILITY  IN  WATER.      (Donnan  and  Burt,  1903.) 

Gms.  LiNO,  Cms.  LiNOj 

t°.         per  100  Cms.  Solid  Phase.  .  t°.  per  100  Cms.  Solid  Phase. 

Solution.  Solution. 

o.i          34.8         LiNO3.3H2O  29.87        56.42          LiNO3.3H2O 

10.5         37-9  29.86        56.68 

12.  i         38.2  29.64        57.48 

13-75        39-3  29.55        58.05 

19.05        40.4  43.6          60.8  LiN03.|H2O 

22.1         42.9  50.5          61.3 

27-55        47-3  55  63 

29-47        53.67  60  63.6 

29.78        55.09  64.2          64.9  LiNO3 

70.9          66.1 

The  eutectic  Ice  +  LiNO3.3lI2O,  is  at  -17.8°  and  about  33  gms.  LiNO3  per 
100  gms.  sat.  sol.     Transition  points,  29.6°  and  61.1°. 

Data  for  die  system  LiNO3+Li2SO4+H2O  at  o°,  30°  and  70°  are  given  by 
Massink,  1916. 

A  sat.  solution  of  lithium  nitrate  in  acetone  contains  0.343  gm.  mols.  =  23.67 

gms.  per  liter  at  about  2O°.     ^  (Roshdestwensky  and  Lewis,  1911.) 

Freezing-point  data  for  LiNOs  +  KNO3  and  LiNO3  +  NaNO3  are  given  by 

Carveth,  1898.     Results  for  LiNOa  +  KNO3  are  also  given  by  Harkins  and  Clark, 


Results  for  LiNO3  +  Li2SO4  are  given  by  Amadori,  1913. 
LITHIUM  NITRITE  LiNO2.H2O. 

SOLUBILITY  IN  WATER.    (Oswald,  1914.) 

Gms.  Gms. 

r.        JSSST  solid  Phase.  t.     ™°d,£r 

Sat.  Sol.  Sat.  Sol. 

-    7.5  II.  I  Ice                               38.5  55.5       LiN02.H,0 

-II.7  15  42  56.9 

—  21  21.2  49  60.6 

—  28.8  29  49.5  6l.2               "  +LiNCMH2O 

—  31.3  29.4  "  +LiN02.H20           65  63.8               LiN02.*H,0 
-19.3  33-9  LiN02.H20                  81.5  68.7 

O  41-5  91  72.4 

+  19  48.90*19=1.3186.)  96  91.8 

25          50-9  92.5      94-3 

100  gms.  H2O  dissolve  10.5  gms.  AgNO2  +  78.5  gms.  LiNO2  at  14°.     (Oswald,  1914.) 

LITHIUM   OXALATE   Li2C2O4. 

SOLUBILITY  OF  MIXTURES  OF  LITHIUM  OXALATE  AND  OXALIC  ACID  IN 

WATER  AT  25°.      (Foote  and  Andrew,  1905.) 

Mixtures  of  the  two  substances  were  dissolved  in  water,  and  the  solutions  cooled 
in  a  thermostat  to  25°. 

Gms.  per  100  Gms.  Solution.  Mols.  per  100  Mols.  H20. 

"     HsCA.     '    Li2C204.  H2C204.     '     Li2C2O4.  '  P  aS6' 

10.20         ...  2.274         ...  H2C2O4.2H2O 

2'457        °'622  H2C204.H20  and  HLiC204.H20 


808        3.18          1.823        0.633 
2  60        «;  o*          o  tc6^        o  062  \ 

'2  )  =39-2H2C204  and 

0.469        1.273  HLiC204.H20  and  Li2C204 

5-87  ...  1.901  Li2C2O4 

100  gms.  aqueous  solution,  simultaneously  saturated  with  lithium  oxalate  and 
ammonium  oxalate  at  25°,  contain  5.75  gms.  Li2C2O4  +  4.8  gms.  (NH4)2C2O4. 

(Foote  and  Andiew,  1905.) 


377  LITHIUM  PHOSPHATE 

LITHIUM  PHOSPHATE  Li3PO4. 

100  gms.  H2O  dissolve  0.04  gm.  Li3PC>4.  (Mayer,  1856.) 

LITHIUM    (Hypo)   PHOSPHATE   Li4P2O6.7H2O. 

100  gms.  H2O  dissolve  0.83  gm.  hypophosphate  at  brd.  temp.  (Rammelsberg,  1892.) 

LITHIUM  PERMANGANATE  LiMn04.3H2O 

100  gms.  water  dissolve  71.4  gms.  permanganate  at  16°.  (Ashoff.) 

LITHIUM  SALICYLATE   C6H4OHCOOLi.|H2O. 

SOLUBILITY  IN  AQUEOUS  ALCOHOL  SOLUTIONS  AT  25°. 

(Seidell,  1909,  1910.) 


Gms.                                                  Gms.                      Gms. 
CzHjOHper                 ^B  of      C6H4OHCOOH.iH2O   C2H5OH  per 
looGrns.                  Sat.  Sol.          per  100  Gms.            100  Gms. 

Gms. 
<Z25  of        C6H4OHCOOH.iH2O 
Sat.  Sol.            oer  too  Gms. 

'Solvent. 

Sat.  Sol. 

Solvent. 

Sat.  Sol. 

0 

.209 

56 

60 

I.I04 

5I-I 

10 

•  195 

55-9 

70 

1.083 

49-5 

20 

.180 

55-4 

80 

I  .056 

47-5 

30' 

.163 

54-7 

90 

1.026 

45-8 

40 

.144 

53-7 

92.3 

I  .O2O 

45-6 

50 

.124 

52.5 

IOO 

1.027 

48.2 

100  gms.  propyl  alcohol  dissolve  18.7  gms.  Li  salicylate  (temp.?).  (Schlamp,  1895.) 
LITHIUM  SULFATE  Li2SO4.H2O. 

SOLUBILITY  IN  WATER. 

(Average  curve  from  Kremers,  1855;  Etard,  1894.) 


t°. 

Gms.  Li2SO4  per 
100  Gms.  Solution. 

t°. 

'    Gms.  Li2SO4  per 
zoo  Gms.  Solution. 

t°. 

Gms.  Li2SO 
loo  Gms.  So 

—  20 

18.4 

20 

25-5 

50 

24-5 

—  10 

24.2 

25 

25-3 

60 

24.2 

0 

26.1 

30 

25.1 

80 

23-5 

10 

25-9 

40 

24.7 

IOO 

23 

per 
ution. 


SOLUBILITY  OF  LITHIUM-POTASSIUM  SULFATE  IN  WATER. 

(Spielrein,  1913.) 

Gms.  per  100  cc.  Gms.  per  100  cc. 

t°.            Sat.  Sol.                   Solid  Phase.  t°.  gSat.  Sol.                   Solid  Phase.  - 

Li2S04.  K2S04.  Li2S04.  K2SO4. 

20     35.6      3.6    Li2SO4.K2SO4+Li2SO4  60  10.6     16.3    Li2SO4.K2SO4+K2SO4 

20     13.3     13.1                          +K2SO4  98  30.2      9.3              "           +Li2SO4 

60     32.5      6                             +Li2SO4  98  9        23                             +K2SO4 

SOLUBILITY  OF  LITHIUM-SODIUM  SULFATES  IN  WATER. 

(Spielrein,  1913.) 

Gms.  per  TOO  cc.  Gms.  per  100  cc. 

^t0.    ^      Sat.  Sol.  SoUd  Phase.  t8.         Sat.  Sol.  ,      Solid  Phase. 

Li2SO4.  Na2SO4.  Li2SO4.  NaiSO4. 

O         31.4       5.9    Li2S04.Na2S04.siH20+Li2S04  33.5   25.8    13. 

°        18.5     11.4  "+Na2S04  33-5  13-9    21.8 

7.5    20.4     11.17  (triple  pt.)  53       28        16  6  +Li2S04 

16        32  9-3  -S3       16.7    27.3  '  +Na2S04 


24         26          14.9    Li2SO4.Na2S04.i2H2O+Li2SO4   99        27.4    14.4 


+Li2S04 
+Na2S04 


24        16.5     21.4  "  +Na2SO4         99       14.4    25.1 

32         20         16.8  (triple  pt.) 

There  is  some  uncertainty  as  to  whether  all  of  the  above  results  are  in  terms 
of  grams  per  100  cc.  or  per  100  gms.  of  sat.  solution. 

SOLUBILITY  OF  LITHIUM  SULFATE  IN  ABSOLUTE  SULFURIC  ACID. 

(Bergius,  1910.) 

io  cc.  sat.  solution  in  abs.  H2SO4  contain  2.719  gms.  Li2SO4  and  the  crystalline 
solid  phase  has  the  composition  Li2SO4.7H2SO4  and  melts  at  about  12°. 


LITHIUM  SULFATE  378 

SOLUBILITY  OF  LITHIUM  SULFATE  IN  AQ".  H2S04  AT  30°.    (van  Dorp,  1910.) 

Cms.  per  100  Cms.  Sat.  Sol.         _  ...  _,  Cms.  per  100  Cms.  Sat.  Sol. 

'     H.£..      '       ItfCV    '        S°'"mMe-  '    H.SO..       '      L1.SO..    '  S°MPhaSe- 

5.05  22.74      Li2SO4.H20          55 .08        13-69  LiSC>4 
12.23        20.45                                 61.46        17.10 

16.60  19.10  62.49        18.89      Li2S04.H2SO4 
32.70        13.37  69.40        13.75 

42.98        10.57  78-23        11.64 

52.72        H.44  83.43        15.65 

SOLUBILITY  OF  LITHIUM  SULFATE  IN  AQUEOUS  ALCOHOL  AT  30°. 

(Schreinemakers  and  van  Dorp,  Jr.,  1906.) 

Cms.  per  100  Cms.  Sat.  Sol.  Cms.  per  100  Cms.  Sat.  Sol. 

'    QH.OH.    '      Li,S04.     '  SohdPhaSe'  '  C,H5OH.     '       Li,SO4.    '  S°Ld  P^' 

o  25.1          Li2SO4.H20        47.28        3.04          Li2SO4.H2O 

11.75       16.16  58.59        1.22 

21.19       n-S2  69.39        0-396 

29.40         8.17  80.74        o 

33.31         6.66  ,94-n        o 

F.-pt.  data  for  Li2SO4  +  MnSO4  are  given  by  Calcagni  and   Marotta,  1914: 

Results  for  Li2SO4  +  SrSO4  are  given  by  Calcagni  and  Marotta,  1912.  Results 
for  Li2SO4  +  Na2SO4  and  Li2SO4  +  K2SO4  are  given  by  Nacken,  1907;  results  for 
Li2SO4  +  Ag2SO4  are  given  by  Nacken,  i9O7b. 

LITHIUM  SILICATE  Li2SiO3. 

Fusion  point  data  for  Li2O  +  SiO2  and  Li2SiO3  +  ZnSiOs  are  given  by  van 
Klooster,  1910-11.     Results  for  Li2SiO3  +  MgSiO3,  Li2SiO3  +  Na2SiO3,  Li2SiO3  + 
K2SiO3  and  Li2SiO3  +  SrSiO3  are  given  by  Wallace,  1909. 
LITHIUM   TARTRATES. 

SOLUBILITY  IN  WATER. 

Cms.  Salt 
Salt.  Formula.  t°.    per  too  Cms.        Authority. 

Sat.  Sol. 

Lithium  Dihydroxytartrate  Li2C4H4O8.2^H2O      o        0.079    (Fenton,  1898.) 

Lithium  Sodium  Racemic  Tartrate  LiNaC^Oe^H^O  20      19.97      (Schlossberg,  1900.) 

"      Dextro          "  "  20      22.55 

"       Potassium  Racemic    "        LiKC^A.I^O      20      55.19 
"       Dextro  20      37.82 

MAGNESIUM  Mg.     F.-pt.  data  for  Mg+Hg.  (Cambi  and  Speroni,  1915.) 

MAGNESIUM  ACETATE   Mg(CH3COO)2.4H2O. 

EQUILIBRIUM  IN  THE  SYSTEM  MAGNESIUM  OXIDE-ACETIC  ACID-WATER  AT  25°. 

(Iwaki,  1914.) 
Cms.  per  too  Cms.  Cms.  per  100  Cms. 

Sat,  Sol.  Solid  Phase.  Sat,  Sol.  Solid  Phase. 

CHjCOOH.        MgO.  CHsCOOH.          MgO. 

3.36          1. 73  MgO  31.37  7.99(CH3COO)2Mg.4H20 

5.65          2.93      "  36.23  8.l8  "  +2.3.3 

8.06  4.21  "  '35-77    8-J7     2-3-3 

12.46  6.54  "  ,,;      40.87  7.42 

15 . 46   8 . 24  "  +(CH,coo)2Mg.4H2o  47 . 86   6 . 74 

15.38    8.31   (CH,COO)2Mg.4H20     56.16     5.81 

14.25   7.24     "       61.59   4.68 

20.19   7-47      "        69.13    3.75 
22.93   7 -60      "        75.93    2.85 

26.61  7.74      "        82.90  ,  2.23 

2.3.3  =  2(CH3COO)2Mg.3CH3COOH.3H2O.  More  careful  work  in  the  region 
of  the  double  salt  showed  that  a  second  double  salt  of  the  composition  5(CH3COO)2 
Mg.ioCH3COOH.7H2O  was  obtained.  This  compound  usually  separated  from 
the  more  concentrated  acetic  acid  solutions. 


379  MAGNESIUM   BENZOATE 

MAGNESIUM   BENZOATE   Mg  (Ce^COOJ^HjO. 

100  gms.  H2O  dissolve  6.16  gms.  Mg(C6H6COO)2  at  15°  and  19.6  gms.  at  100°. 

(Tarugi  and  Checchi,  1901.) 
IOO  gms.  H2O  dissolve  3.33  gms.  MgCCgHsCOO^  at  I5-2O.    (Squire  and  Caines,  1905.) 

MAGNESIUM    BROMATE    Mg(BrO3)2.6H2O. 

TOO  cc.  sat.  solution  contain  42  grams  Mg(BrO3)2,  or  0.15  grammols. 
at  1 8°. 

(Kohlrausch  —  Sitzb.  K.  Akad.  Wiss.  (Berlin),  i,  90,  '97.) 

MAGNESIUM    BROMIDE    MgBr2.6H2O. 

SOLUBILITY  IN  WATER. 

(Menschutkin  — -  Chem.  Centrb.  77,  I.  646,  '06;  at  18°,  Mylius  and  Funk  — Ber.  30,  1718,  '97.) 
o       Grams  MgBr2  per  100  Gms.  Grams  MgBr2  per  100  Grams. 

Solution.  Water.  Solution.        Water. 

—  io        47.2          89.4  40          50.4         101.6 

o  47-9  91-9  5°  51-0  I04-i 

io  48-6  94-5  60  51.8  107.5 

18  49.0  96.1  80  53.2  113.7 

18  50.8  103 . 4  (M.  and  F.)    100  54.6  120.2 

20  49-i  96-S  I2°  56-°  I27-5 

25  49-4  97-6  140  58-°  I38-1 

30  49.8  99.2  160  62.0  163.1 

Density  of  saturated  solution  at  18°  =  1.655  (M.  and  F.) 
Etard  —  Ann.  chim.  phys.    [7]  2,  541,  '94,  gives  solubility  results 
which  are  evidently  too  high. 

MAGNESIUM   BROMIDE    ETHERATES,  ALCOHOLATES,  ACIDATES, 
ETC. 

SOLUBILITIES  RESPECTIVELY  IN  ETHER,  ALCOHOL,  ACIDS,  ETC.,  AT 
VARIOUS  TEMPERATURES. 

(Boris  N.  Menschutkin.  Monograph  in  the  Russian  language  entitled  "  On  Etherates  and  Other  Molec- 
ular Combinations  of  Magnesium  Bromide  and  Iodide."  St.  Petersburg,  1907,  pp.  267  and  XLVIII. 
Also  published  in  the  Memoirs  of  the  St.  Petersburg  Polytechnic  Institute,  Vols.  1-7,  1904-1907,  and 
in  condensed  form  in  Vols.  49-62  of  the  Zeit.  anorg.  Chem.,  1906-1909.) 

Preparation  of  Material.  The  dietherate  of  magnesium  bromide, 
MgBr2.2(C2H5)2O  (Z.  anorg.  Chem.,  49,  34,  '06)  was  prepared  by  the  very  gradual 
addition  of  bromine  to  a  cold  mixture  of  magnesium  powder  and  dry  ether. 
It  is  very  hygroscopic  and  is  stable  only  under  its  ethereal  solution.  It  is  decom- 
posed by  water  and  reacts  with  very  many  organic  compounds  as  alcohols, 
acids,  ketones,  esters,  aldehydes,  etc.  The  addition  products  thus  formed  con- 
stitute the  material  employed  in  the  author's  succeeding  studies.  The  mono- 
etherate  of  magnesium  bromide,  MgBr2.(C2H6)2O,  was  prepared  just  as  the 
dietherate,  but  the  temperature  during  crystallization  was  kept  above  30°,  at 
which  point  the  dietherate  is  converted  to  monoetherate.  It  is  also  precipitated 
by  dry  ligroin. 

Method  of  Determination  of  Solubility.  At  temperatures  below  30°  the 
determinations  were  made  by  agitating  an  excess  of  the  salt  with  the  solvent  and 
analyzing  the  saturated  solution.  At  the  higher  temperatures  the  synthetic 
(sealed  tube)  method  of  Alexejeff  (Wied.  Ann.,  1885)  was  used. 

See  also  p.  391. 


MAGNESIUM   BROMIDE 
ETHERATES 


380 


SOLUBILITY  OF  MAGNESIUM  BROMIDE  DIETHERATE,  MgBr2.2(C2H6)2O,  AND  OF 
MAGNESIUM  BROMIDE  ETHERATE,  MgBr2(C2H3)2O,  IN  ETHYL  ETHER,  (C2H5)2O, 
AT  VARIOUS  TEMPERATURES. 

(Menschutkin.    See  preceding  page.) 


Solubility  of  the  Dietherate 
in  Ether. 


Solubility  of  the  Monoetherate 
in  Ether. 


^0        Gms.  per  100  Gms.  Sat.  Sol. 

Mols.  MgBr,. 
2(C2H5)2O  per          t<, 
100  Mols. 
Sat.  Sol. 

Gms.  per  100  Gms.  Sat.  Sol.  (£ 

ols.  MgBr2, 
2H5)20  per 
:oo  Mols. 
Sat.  Sol. 

'     MgBr2.2(C2H5)2O.    MgBr,. 

MgBr2.(C2H6)20.  MgBr2.    '     ' 

-  8 

1.  08 

0.6 

0 

.24 

0 

68 

.8 

49 

.1 

28.1 

o 

1.44 

0 

.8 

O 

•32 

20 

67 

.2 

47 

•9 

27.1 

+  10 

2-3 

i 

.27 

0 

3° 

66 

•5 

47 

•3 

26.6 

14 

2-95 

i 

.64 

0 

•67 

40 

65 

•5 

46 

•7 

26.1 

16 

i 

•93 

o 

.80 

60 

63 

.8 

45 

•5 

25-1 

18 

4.14 

2 

•3 

0 

.96 

80 

62 

.1 

44 

•3 

24.2 

20 

4.86 

2 

•7- 

I 

•125 

100 

60 

•7 

43 

•3 

23-5 

22. 

.8     6.3 

3 

•5 

I 

.6 

120 

59 

.6 

42 

•5 

22.9 

Two  liquid  layers  separate  between  these  con- 

I4O 

58 

•5 

41 

•7 

22.3 

centrations  of  MgBr2.2(C2Hjj)2O. 

158 

57 

•5 

41 

21-9 

23 

72.3 

40 

.1 

36 

.8 

Two  liquid  layers  separate  between  these  con- 

24 

75-3 

41 

.8 

40 

•5 

centrations  of  MgBr2.(C2H6)2O. 

26 

79-5 

44 

.1 

46 

.6 

158 

5 

.8 

4 

.15 

1.6 

28 

5     84.2 

46 

•7 

54 

.2 

158 

4 

.8 

3 

•4 

1.36 

30 

85.5 

47 

•4 

56 

•9 

159 

i 

.96 

i 

•4 

0.56 

l62 

0 

.38 

o 

.27 

O.II 

170 

0 

.18 

0 

•13 

0.05 

At  22.8°  and  158°  the  saturated  solutions  of  the  dietherate  and  monoetherate, 
respectively,  separate  into  two  liquid  layers  which  have  at  the  intervening  tem- 
peratures the  following  composition.  Determinations  of  the  specific  gravity  of 
the  lower  layer  gave  d#  =  1.1628  and  d%$  =  1.1492. 


Gms.  per  100  Gms.  Solution. 


t°.                              Lower  Layer. 

Upper  Layer. 

MgBr2.2(C2H3)2O. 

MgBr2. 

MgBr2.2(C2H3)2O. 

MgBr2. 

—  10 

75-75 

42 

3-2 

1.8 

0 

73-9 

41 

4.1 

2-3 

+  IO 

72.2 

40.1 

5 

2.8 

20 

70.8 

39-3 

5-9 

3-3 

30 

69.8 

38.7 

6.8 

3-8 

40 

68.8 

38.2 

7-7 

4-3 

50 

68 

37-8 

8.5 

4-7 

60 

67.7 

37-6 

9.2 

5.1 

70 

67.7 

37-6 

9-7 

5-4 

80 

68 

37-8 

10 

5-6 

90 

68.6 

38.1 

10.2 

5-7 

100 

69.4 

38.5 

10.4 

5-8 

120 

71 

39-3 

10.  1 

5-6 

140 

72.4 

40.15 

9.2 

5.1 

158 

74 

41 

7.8 

4-3 

unstable 


stable 


38i  MAGNESIUM  BROMIDE 

ALCOHOLATES 

SOLUBILITY  OF  ETHYL,  METHYL,  PROPYL,  ETC.,  ALCOHOLATES  OF  MAG- 
NESIUM BROMIDE  IN  THE  RESPECTIVE  ALCOHOLS.     (Menschutkin,  1907.) 
These  compounds  were  all  prepared  by  the  action  of  magnesium  bromide 
dietherate  upon  the  several  alcohols.     The  ether  was  expelled  and  the  new  alco- 
holate  addition  product  recrystallized  from  the  respective  alcohol.     The  solubility 
determinations  were  made  by  the  synthetic  method. 


Solubility  of                 Solubility  of                Solubility  of             Solubility  of 

MgBr2.6CH3OH          M 
in  Methyl  Alcohol.       in 

gBr2.6C2H5OH        MgBr2.6C3H7OH  MgBr2.6IsoC4H9OH 
Ethyl,  Alcohol,      in  Propyl  Alcohol,  in  IsoButyl  Alcohol. 

Gms.  MgBr2. 
t»               6CH3OH           to 

Gms.  MgBr2. 
6C2H6OH              to 

Gms.  MgBr2.                    Gms.  MgBr2. 
6C3H7OH          to            6C4H9OH 

per  ioo 

per  ioo 

per  ioo                               per  ioo 

Gms.  Sat.  Sol. 

Gms.  Sat.  Sol. 

Gms.  Sat.  Sol.                   Gms.  Sat.  Sol. 

o             42.6               o 

17.2               o 

77-9              o                55-8 

20                44.6                 10 

24.9             10 

81.5             10                60.5 

40              46  .  7               20 

32.7                 20 

85.1             20                65.2 

60              48  .  9              30 

40-3                 30 

88.5            30                69.8 

80              51.4              40 

47.8                 40 

92                40                74.3 

ioo              55.5              60 

62.2              43 

93                50               78.5 

I2O                  60.7                   80 

73-8             46 

94.3            60               82.4 

140              66  .  8              90 

78.7         48 

95-8           65               84.2 

160             74               ioo 

86.7          50 

97.8           71              88 

180             84.5            103 

90                 52m.pt.  ioo                75               92 

185             88               106 

94-4 

77               94-6 

i90m.pt.   ioo               108 

.5m.pt.  ioo 

8om.pt.    ioo 

Solubility  of 
MgBr2.6  Iso  C5HnOH 
in  IsoAmyl  Alcohol. 

Solubility  of 
MgBr2.4(CH3)2CHOH 
in  Dimethyl  Carbinol. 

Solubility  of 
MgBr2.4(CH8)3COH 
in  Trimethyl  Carbinol. 

Gms.  MgBr2. 
t»              6C5HUOH  per 

Gms.  MgBr2. 
to              4(CH3)2CHOH 

Gms.  MgBr2. 
to                    4(CH3)3COH 

ioo  Gms. 

per  ioo  Gms. 

per  ioo  Gms. 

Sat.  Sol. 

Sat.  Sol. 

Sat.  Sol. 

i    o               70.2 

o               40 

24.7m.  pt.  of  (CH3)3COH 

10               75-6 

2O                     42  .  2 

24.4Eutec.      0.06 

20                     80.2 

40                     45 

25              I 

30           84.5 

60                     48.5 

35                    9-5 

35               86.7 

80                53-3 

45                   19-1 

38               88.7 

ioo                59 

55                   32.2 

40               90 

120               67.3 

60                  40.5 

42               92 

130                74 

70                   62.5 

44               94-2 

136                83.6 

75                   77 

46  m.  pt.  ioo 

138                90 

79                   91-5 

139  m.  pt.  ioo 

80  m.  pt.      ioo 

MAGNESIUM  BROMIDE  ANILINATES. 

SOLUBILITY  OF  MAGNESIUM  BROMIDE  ANILINATES  IN  ANILINE  AT 

DIFFERENT  TEMPERATURES.    (Menschutkin,  1907.) 

The  compounds  were  formed  by  the  action  of  aniline  on  magnesium  bromide 
dietherate.  The  three  compounds  were:  MgB^CeHsNH-j,  MgBr2.4C6H4NH2 
and  MgBr2.2C6H5NH2. 


Gms.  MgBr2. 
to                          4C6HSNH2 
per  ioo  Gms. 

Sat.  Sol. 

IO 

3-2 

50 

5-i 

70 

7-5 

QO 

12.8 

IOO 

18.5 

103.5 

27-5 

103  tr.  pt. 

24 

1  20 

24-3 

140 

24-3 

Solid  Phase. 


MgBr2.6C6H5NH2 


MgBr2.4C6H5NH, 


Gms.  MgBr2. 
4C6H8NH2 

t  . 

per  ioo  Gms. 

Sat.  Sol. 

160 

26 

180 

28.3 

200 

33-5 

2  2O 

45 

230 

55 

237  tr.  pt. 

76.3 

250 

77-3 

260 

78.1 

270 

79 

Solid  Phase. 


MgBrI.4C6H4NH1 


MAGNESIUM  BROMIDE  382 

MAGNESIUM  BROMIDE  PHENYLHYDRAZINATES. 

SOLUBILITY  OF  MAGNESIUM  BROMIDE.     PHENYLHYDRAZINATES  IN  PHENYL- 

HYDRAZINE. 

(Menschutkin,  1907.) 

(Approximate  determinations.) 

Gms.  MgBr2. 
5NHNH2 


2O 
40 
60 
80 
99 


Cms.  MgBr2. 

6QH6NHNH2 

per  too  Gms. 

Sat.  Sol. 

3 

7 

16.4 
33 
54-8 


Solid  Phase. 


MgBrj.GCeHsNHNH, 


IOO  tr.  pt. 
140 

180 

200 


Sat.  Sol. 
54-8 
60.8 
68.4 

73-4 


MgBr2.4QHjNH.NH2 


MAGNESIUM  BROMIDE  COMPOUNDS  with  Benzaldehydeand  with  Acetone- 
SOLUBILITY  RESPECTIVELY  IN  BENZALDEHYDE  AND  IN  ACETONES. 

(Menschutkin,  1907.)' 

The  compounds  were  prepared  by  the  action  of  benzaldehyde  and  of  acetone  on 
magnesium  bromide  dietherate.  On  account  of  the  nature  of  the  compounds  the 
results  are  only  approximately  correct. 

Solubility  of  MgBr2.3C6H5COH 
in  Benzaldehyde. 


Solubility  of  MgBr2.3CH3.CO.CH3. 
in  Acetone. 


Gms.  MgBr2. 
«            3QH6COH            to 
per  ioo  Gms. 

Gms.  MgBr2. 
3C6H5COH 
per  ioo  Gms. 

Gms.  MgBr2.           •           Gms.  MgBr2. 
to         3CH3.CO.CH3       to            3CH3COCH3 
per  ioo  Gms.                        per  ioo  Gms. 

Sat. 

Sol. 

Sat.  Sol. 

Sat.  Sol. 

Sat.: 

Sol. 

O 

0 

•7 

140 

I7.8 

0 

0.2 

75 

50 

, 

30 

I 

.3 

145 

37-5 

30 

0.8 

76 

71 

.6 

60 

I 

•9 

146 

65 

60 

i-45 

80 

83 

•3 

IOO 

3 

•4 

148 

84-5 

70 

2 

84 

89 

.8 

120 

6 

153 

93-2 

73 

5-5 

88 

95 

.2 

130 

9 

•5 

I5pm.pt. 

IOO 

74 

14 

92m.  pt. 

IOO 

MAGNESIUM  BROMIDE  COMPOUNDS  with  Methylal,  Ortho  Ethylformate, 
Formic  Acid  and  Acetic  Acid. 

(Menschutkin,  igo7a.) 

The  compounds  were  prepared  by  the  action  of  methylal,  ortho  ethylformate* 
and  absolutely  dry  formic  and  acetic  acids  on  magnesium  dietherate.  In  the  case 
of  the  latter  compounds  the  results  are  only  approximately  correct,  due  to  their 
extreme  hygroscopicity. 

Solubility  of  Solubility  of  Solubility  of  Solubility  of 

MgBr2.2CH,(OCH3)2  MgBr2.2CH(OC2H6)3  MgBr2.6HCOOH   MgBr2.6CH3COOH 


in  Methylal. 

in  Orthoethylformate.  in  Formic  Acid. 

in  Acetic 

Acid. 

Gms.  MgBr2.                      Gms.  MgBr2.                    Gms.  MgBr2. 
t»                  2CH2(OCH3),     to              2CH(OC2H6)3    to               6HCOOH 
per  ioo  Gms.                       per  ioo  Gms.                    per  ioo  Gms. 
Sat.  Sol.                              Sat.  Sol.                            Sat.  Sol. 

Gms.  MgBr2. 
to              6CH3COOH 
'             per  ioo  Gms. 
Sat.  Sol. 

20 

o-3 

0 

n.  i 

o 

49-8 

17 

o-3 

40 

0.45 

20 

12.5 

20 

57-5 

3° 

i  .  5 

60 

0.6 

40 

14.8 

40 

65-1 

50 

4-5 

80 

0-75 

60 

18.6 

60 

73-i 

60 

7-9 

IOO 

0.9 

80 

25-7 

70 

78.1 

70 

16.2 

106 

i.i 

90 

35 

80 

86 

80 

38.5 

2  liquid  layers  here 

95 

86 

95 

90 

57-7 

106 

86.2 

IOO 

50 

88  m.  pt. 

IOO 

IOO 

71.8 

108 

90.8 

105 

66 

105 

80 

no 

95-4 

no 

88.5 

no 

89.5 

112  m.  pt. 

IOO 

114  m.  pt. 

IOO 

112  m.  pt. 

IOO 

383 


MAGNESIUM  BROMIDE 


MAGNESIUM  BROMIDE  COMPOUNDS  with  Acetamide,  Acetanilide  and 

Acetic  Anhydride.  (Menschutkln,  1909.) 

The  compounds  were  prepared  by  reaction  with  magnesium  bromide  dietherate. 


Solubility  of 
MgBr2.6CH3CONH2 
"in  Acetamide. 

Gms. 
MgBr2.6CHr 
te.           CONH2            Solid  Phase, 
per  ioo  Gms. 
Sat.  Sol. 

Solubility  of                    Solubility  of 
MgBr2.6CH3CONHC6H5  MgBr2.6(CH3CO)8O 
in  Acetanilide.            in  Acetic  Anhydride. 

Gms.                                                                 Gms. 
MgBr2.6CHr                                                         MgBr2. 
t°.      CONHQHs         Solid  Phase.           t°.       6(CH3COO)2O 
•  per  ioo  Gms.                                                    per  ioo  Gms. 
Sat.  Sol.                                                          Sat.  Sol. 

82  m.pt.ofCH3CONH2  CH3CONH2 

112  m.  pt.  of  CHsCONHQHj                        o 

26 

4 

80 

3 

I 

no 

3- 

7 

CHsCONHQHs          2O 

28 

7 

70 

21 

7                     " 

108 

7- 

7 

40 

31 

6 

60 

40 

" 

-*     n 

"+MgBr2CH3-        60 

35 

7 

ff\ 

CH3CONH2+MgBr2 

107. 

5      9 

CONHQH6   80 

i 

50-5* 

50 

CH3CONH2 

L20 

13- 

i 

MgBr2.CH,CONHC6H6  ioo 

48 

4 

70 

57 

8     MgBr2.CH,CONH2 

140 

19. 

3 

"                    1  2O 

57 

8 

90 

60 

5 

160 

25- 

5 

I30 

69 

8 

1  10 

65 

180 

35- 

3 

133 

77 

130 

5 

200 

59- 

5 

135 

85 

150 

80 

205 

73- 

2 

136.  5t 

1  60 

85 

207 

82. 

5 

" 

165 

90 

209 

ioof 

" 

i69f 

IOO 

4.    

MAGNESIUM   BROMIDE    COMPOUNDS  with  Urethan  and  with  Urea.  • 

(Menschutkin,  1909.) 

Solubility  of  Magnesium  Bromide              Solubility  of  Magnesium  Bromide 
Urethan  Compounds  in  Urethan.                     Urea  Compounds  in  Urea. 

Gms.                                                                                    Gms. 
TMgBr2.4C2H5O-                                                                   MgBr,.4CO- 
t°.           CONH2                     Solid  Phase.                        t°.           (NH,)2               Solid  Phase, 
per  ioo  Gms.                                                                       per  iooj3ms. 

Sat.  Sol. 

bat.  bo 

i. 

49m. 

pt.  of  urethan 

C2H3OCONH2 

132 

m.  pt.  of  urea           COCNHj), 

45 

18.5 

" 

126 

9-5 

" 

36-5 

" 

120 

17.2 

« 

35* 

43-3 

"  +MgBr2.6C2H3OCONH2 

114 

21.8 

» 

So 

45-6 

MgBr2.6CjH3OCONH2 

108. 

5*     24.2 

CCKNH,),  +MgBr2.6CO(NHj), 

70 

51  -3 

"5 

29.8 

MgBrj.GCOCNHzJj 

80 

56-2 

120 

35 

"          t 

90 

66.5 

127 

45-5 

" 

75-5 

130 

60 

" 

9It 

69.4 

+MgBr2.4C,H,OCONH, 

i3°t 

58 

"  +MgBr2.4CO(NH2), 

IOO 

73-8 

MgBr2.4CjH3OCONH, 

145 

60.7 

MgBrj^COCNH,), 

no 

80 

« 

1  60 

67.2 

" 

"5 

84.1 

" 

165 

71.4 

" 

120 

90 

" 

170 

83-7 

M 

123 

IOO 

" 

171 

96 

« 

*  Eutec. 

t  tr.  pt. 

MAGNESIUM   CAMPHORATE   CioH14O4Mg.i4H2O. 

SOLUBILITY  OF  MAGNESIUM  CAMPHORATE  IN  d  CAMPHORIC  ACID  AT  15° 
AND  VICE  VERSA. 

Qungfleisch  and  Landrieu,  1914.) 

Gms.  per  ioo  Gms.  Sat.  Sol 
'    Ci0H1404.    C10H1404Mg. 

3.16  10.30 

3-5  16.5 

3.6         16.7 
1.91        15-1 

o  14.25 


Gms.  per  ioo  Gms.  Sat.  Sol.    _ 
C10Hlg04.       '      C10H14Q^g.So 

0.622  (13.5°)    o  CioH16O4 

I . 20  I . 29 

1-98  3-53 

2.36  5-66 

2.85  8.19 


Solid  Phase. 

CioHlo04 

"  +CioH1404Mg.i4H20 
CioH,404Mg.i4H20 


MAGNESIUM  CARBONATE  384 

MAGNESIUM  CARBONATE  MgCO,.3H2O. 

SOLUBILITY  IN  WATER  IN  PRESENCE  OF  CARBON  DIOXIDE  AT  15°. 

(Treadwell  and  Reuter  — Z.  anorg.  Ch.  17,  200,  '98.) 


cc.  CO2  per  too  cc. 
Gas  Phase  (at  o° 

and  760  mm.). 

Partial 
Pressure  of  COa 
in  mm.  Hg. 

Grams  per 

TOO  cc.  Solution. 

Free  CO2. 

MgC03. 

Mg(HC03)2. 

Total  Mg. 

1  8.  86 

143-3 

O.IIQO 

.  .  . 

I.2I05 

0.2016 

5-47 

41  .6 

0.0866 

I  .2IO5 

0.2016 

4-47 

33-8 

0.0035 

I  .2105 

0.2016 

i-54 

11.7 

0.0773 

I  .0766 

0.2016 

J-3S 

10.3 

.  .  . 

0.0765 

0.7629 

0.1492 

1.07 

8.2 

... 

0.0807 

0-5952 

0.1224 

0.62 

4-7 

.  .  . 

O.O7OI 

0-3663 

0.0865 

0.60 

4.6 

0-0758 

0.3417 

0.0788 

o-33 

2-5 

0-0748 

0.2632 

0.0655 

0.21 

1.6 

0.0771 

O.2229 

0.0594 

0.14 

i  .1 

0.0710 

0.2169 

0.0566 

0.03 

o-3 

0.07II 

0.2036 

0.0545 

0.0685 

0.2033 

0-0536 

0.0702 

0-1960 

0.0529 

0.0625 

0.2036 

O.O52O 

0.0616 

0.1954 

0.05II 

... 

... 

0.0641 

0.1954 

O.O5l8 

Therefore  at  o  partial  pressure  of  CO2  and  at  15°  and  mean  barometric  pressure, 
one  liter  of  saturated  aqueous  solution  contains  0.641  gm.  of  MgCO3  plus  1.954 
gms.  Mg(HCO3)i. 

It  is  pointed  out  by  Johnston  (1915)  that  although  Treadwell  and  Reuter  made 
very  painstaking  analyses,  their  mode  of  working  did  not  secure  equilibrium  con- 
ditions, a  fact  which  is  borne  out  by  the  lack  of  constancy  of  the  calculated  solu- 
bility-product constant. 

SOLUBILITY  OP  MAGNESIUM  CARBONATE  IN  WATER  CHARGED  WITH  CAR- 
BON DIOXIDE  AT  PRESSURES  GREATER  THAN  ONE  ATMOSPHERE. 

(Engel  and  Ville  —  Compt.  rend.  93,  340,  '81;  Engel  —  Ann.  chim.  phys.  [6]  13,  349,  '88.) 


Pressure  of 
C02in 
Atmospheres. 

G.  MgCO3? 

per  Liter. 

Pressure  of 
CO2in 

Atmospheres  o 

G.  MgC03*  per  Liter. 

At 

12°. 

At  19°. 

At 

12°. 

At  19°. 

o-5 

20. 

5 

. 

4 

•  o 

42 

.8 

I.O 

26. 

5 

25 

.8 

4 

•7 

43-5 

2.0 

34- 

2 

33 

.1(2 

,i  At.) 

6 

.0 

50 

.6 

48.5(6 

2  At.) 

3-o 

39- 

O 

37 

•2(3 

.2  At.) 

9 

.0 

56.6 

SOLUBILITY  IN  WATER  SATURATED  WITH  CO3  AT  ONE  ATMOSPHERE. 

(Engel.) 

f.  o  Gms.  MgCO>* 

per  Liter. 

60  II 

80  5 

100  O 

Dissolved  as  Mg(HCO3)a. 


t<>. 

Gms.  MgCO3* 
per  Liter. 

±y         Gms.MgCO3* 
per  Liter. 

5 

36 

30 

21 

10 

31 

40 

17 

20 

26 

385 


MAGNESIUM  CARBONATE 


Data  for  the  system  magnesium  carbonate-carbonic  acid- water  at  20°,  25°,  30°, 
34°  and  39°  are  given  by  Leather  and  Sen  (1914).  In  connection  vith  these  results, 
it  is  pointed  out  by  Johnston  (1915),  that  it  is  questionable  whether  equilibrium 
was  really  obtained  and  furthermore,  the  accuracy  of  the  analytical  results  cannot 
be  trusted  since  the  ratio  of  total  amount  of  CO2  in  solution,  to  the  magnesia  ia 
very  irregular.  The  results  when  plotted  directly  show  great  inconsistencies. 

THE  CALCULATED  SOLUBILITY  OF  MgCO3.3H2O  IN  WATER  AT  18°  IN  CONTACT 
WITH  Am  CONTAINING  PARTIAL  PRESSURES  OF  CO2  FROM  0.0002  TO  0.0005 
ATMOSPHERES. 

(Johnston,  1915.) 

It  is  shown  that  if  the  CO2  pressure  is  kept  constant  at  P  and  the  water  evapo- 
rated off  so  slowly  at  18°  that  equilibrium  conditions  are  continuously  maintained, 
the  following  amounts  of  Mg(OH)2  or  of  MgCO3.3H2O  will  be  obtained. 


Partial  Pressure  P 
of  CO2  in  Atms. 

O 


Mols. 


Cms.  per  Liter. 

0.0087    Mg(OH)2 


I3 
29 
45 
60 
97 
05 

12 


Total  Mg 

p 

0.00015 
0.01934 
O.O22I8 
0.02486 
0.02742 
0.02868 
0.02924 
0.02976 

SOLUBILITY  OF  MAGNESIUM  CARBONATE  IN  NATURAL  WATERS. 

(Wells,  1915.) 

(In  all  cases  the  solutions  were  in  equilibrium  with  atmospheric  air  at  20°.) 

Milligrams  per  Liter  of  Sat.  Solution. 
Mixture. 


MgC03.3H20 


0.00020 
0.00025 
0.00030 
0.00035 
0.00040 
0.00045 

0.00050 


Mg.  Free  COj. 

Natural  Magnesite  in  Distilled  H2O  0.018  trace  0.065 

in  Aq.  NaCl  (27.2  g.  per  1.)         0.028  trace  0.086 

MgCOs^BkO  (equilibrium  from    bicarbonate  end)  0.038  0.28  COc  as  carbonate  0.83 

MgCO3.3H2O(  '    under  saturation ")  0.034  0.32  CO2"  0.59 

SOLUBILITY  OF  MAGNESIUM  CARBONATE  IN  AQUEOUS  SOLUTIONS  OF 
POTASSIUM  BICARBONATE. 

(Auerbach,  1904.) 

The  conditions  necessary  for  preventing  changes  in  equilibrium  due  to  hy- 
drolysis and  loss  of  CO2  are  discussed.     The  mixtures  were  shaken  from  1-4  days. 

The  sat.  sol.  analyzed  for  total  alkali  (  K  -\ J  by  titration  with  standard  HC1 

using  methyl  orange  as  indicator.  The  neutralized  solution  was  boiled  to  expel 
CO2  and  then  excess  o.  i  n  NaOH  added  and  the  filtrate  from  magnesium  precipi- 
tate back  titrated  with  o.i  n  HC1.  The  — -  was  calculated  from  the  used  O.I  n 
NaOH  and  the  K  obtained  by  difference. 


Results  at  15°. 

Mols.  per  Liter. 

Results  a 

Mols.  per  Liter. 

t25°. 
Solid  Phase. 
MgC03.3H20 

« 
"  (labil) 
"  +1.1 
i.i 

« 

Results  at 

Mols.  per  Liter. 

35°. 
Solid  Phase. 
MgCO^HjO 

"  (labil) 

"    +X.X 

i.i 
«< 

KHC03.     MgOV"0 
o               0.0095  MgCOs.3HzO 
0.0992     0.0131           " 
0.1943     0.0167           " 
0.3992      O.O2II            "(labil) 
0.2681      0.0192           "  +1.1 
0.5243      0.0097          LI 
0.6792      0.0074           " 
0.981        0.0028           " 
i.i  =  MgCO3.KHCO3.4H2O. 

KHCO3. 
O 

0.0985 

O.22IO 

0-3434 
0.4985 
0.3906 

0-5893 
0.6406 
I.I25 

MgCO3. 
0.0087 
0.0115 
0.0149 
0.0181 
0.0217 
0.0196 
0.0128 
0.0117 
0.006  1 

KHCO3. 
O 

0.1092 
0.2811 

0.4847 
0.5807 
0.5088 
0.6231 
0.8535 

MgCO3. 
0.0071 
0.0098 
0.0142 
0.0177 
0.0198 
0.0184 
0.0153 
0.0119 

Additional  data  for  this  system  are  given  by  Nanty,  1911. 

Data  for  the  solubility  of  MgCO3  in  aq.  NaCl  and  other  salt  solutions,  deter- 
mined by  prolonged  boiling  and  subsequent  cooling  of  the  solution  out  of  contact 
with  air,  are  given  by  Gothe  (1915). 


MAGNESIUM   CARBONATE  386 

SOLUBILITY  OF  MAGNESIUM  CARBONATE  IN  AQUEOUS  SOLUTIONS  OP 
SODIUM  CARBONATE  AT  25°.  The  solutions  being  in  equilibrium 
with  an  atmosphere  free  from  CO2. 

(Cameron  and  Seidell  — J.  Physic.  Ch.  7,  588,  '03.) 
Wt.  of  i  Liter  Grams  per  Liter.  Reacting  Weights  per  Liter. 


of  Solution. 

Na2C03. 

Mgco3: 

Na2C03. 

MgC03. 

996.8 

o.oo 

0.223 

o.ooo 

O.OO266 

1019-9 

23.12 

0.288 

O.22O 

0.00344 

1047-7 

50-75 

0.510 

0.482 

o  .00620 

1082.5 

86.42 

0.879 

O.82O 

0.01027 

1118.9 

127.3 

1-314 

1.209 

0.01570 

1147.7 

160.8 

1.636 

I  .526 

0.01955 

1166.1 

181.9 

1.972 

1.727 

0.02357 

1189.4 

213.2 

2.317 

2.024 

0.02770 

SOLUBILITY  OP  MAGNESIUM  Bi  CARBONATE  AND  OF  MAGNESIUM  CAR- 
BONATE IN  AQUEOUS  SOLUTIONS  OF  SODIUM  CHLORIDE  AT  23°.  The 
solutions  being  in  equilibrium  with  an  atmosphere  of  CO2  in  the 
one  case,  and  in  equilibrium  with  air  free  from  CO2  in  the  other. 

(C.  and  S.) 
In  Presence  of  CO2  as  Gas  Phase.  In  Presence  of  Air  Free  from  CO2. 


Cms.  NaCl 
per  Liter. 

Gms.  Mg(HCO3)2 
per  Liter. 

Wt.  of  i 
Liter. 

Gms.  NaCl 
per  Liter. 

Gms.  MgCO3 
per  Liter. 

7-0 

30.64 

996.9 

o.o 

0.176 

5^5 

30.18 

IOI6.8 

28.0 

0.418 

119.7 

27.88 

1041  .  I 

59-5 

0.527 

163.9 

24.96 

1070.5 

106.3 

0.585 

224.8 

20.78 

1094.5 

147.4 

0-544 

306.6 

iQ-75 

1142.5 

231.1 

0.460 

II70.I  . 

272.9 

o-393 

II99-3 

331-4 

0.293 

SOLUBILITY  OP  MAGNESIUM  CARBONATE  IN  AQUEOUS  SOLUTIONS  OF 
SODIUM  SULPHATE  AT  24°  AND  AT  35.5°.  The  solutions  being  in 
equilibrium  with  an  atmosphere  free  from  CO2. 

(Cameron  and  Seidell.) 

Results  at  24°.  Results  at  35.5.° 

Wt.  of        Gms.  Na2SO4      Gms.  MgCO8  Wt.  of          Gms.  Na2SO«     Gms.  MgCO3 

i  Liter.  per  Liter.          per  Later.,  i  Liter.  per  Liter.          per  Liter. 

007-5  o.oo        0.216  995-1  0.32        0.131 

I02I.2      25.12     0.586          1032.9      41.84     0.577 

1047.6    54-76   0.828      1067.2    81.84   °-753 


1080.9  95-68 

1133.8  160.8 

1157.3  191.9 

1206.0  254.6 

1242.0  305.1 


.020  1094.8  116.56  0.904 

.230  II20-4  148.56  0.962 

.280  "S1-?  186.7  1-047 

.338  1179.8  224.0  I. 088 

.388  1236.5  299.2  1-130 


MAGNESIUM   CHLORATE 


MAGNESIUM   CHLORATE   Mg(ClO3)2.6H2O. 

SOLUBILITY  IN  WATER. 

(Meusser  —  Ber.  35,  1416,  '02.) 


Mg(003)2  Mg(C103)j 
per  100  Gms.   per  100 
Solution.    Mols.H20. 


Solid 
Phase. 


Gms.  Mols. 

Mg(C103)2    Mg(C10a)a 
per  100  Gms.     per  100 
Solution .      Mols .  H2O . 


-18 

o 

18 

29 

35 


51.64 

53-27 
56.50 
60.23 
63-65 


10.05 
10.73 

12.22 
14.25 
16.48 


Mg(C108)2-6H30 


42 
65-5 

39-5 
61  .o 
68 


63.82 
69.12 

65-37 
69.46 
70.69 


93       (73 -71) 


16.60 
20.08 
17.76 
21.40 
22.69 
(26.38) 


Solid. 
Phase. 

Mg(C108)a.4H,0 


Mg(C10a)a.3H30 


Sp.  Gr.  of  saturated  sol.  at  +  18°  =  1.564. 


MAGNESIUM  CHLORIDE  MgCl2. 

SOLUBILITY  IN  WATER. 

(van't  Hoff  and  Meyerhoff er,  1898;  Engel;  Lowenherz.    Results  quoted  from  Landolt  and  BCrnstein,  191 2-) 


„  Gms.  MgCbper  too  Gins              SoHd 

t°. 

Gms.  MgCljperioo  Gms*  Solid 

t  • 

Solution. 

Water.                     Phase- 

Solution 

.    Water. 

Phase. 

—  10 

n.  i 

12 

•5         Ice 

O 

34 

•5 

52 

.8 

MgCl2.6HaO 

—  2O 

16.0 

19 

.0 

IO 

34 

•9 

53 

•5 

" 

-30 

19.4 

24 

.0 

20 

35 

•3 

54 

•5 

—  33- 

6 

20.  6 

26 

O           Ice  +  MgCl2.i2H2O 

22 

35 

.6 

55 

.2 

" 

—  20 

26.7 

36 

.  5           MgCl2.i2H2O 

25          36.2 

56 

•7 

" 

-16. 

4 

30.6 

44 

.04f.pt. 

40 

36 

•5 

57 

•5 

44 

-16. 
-17- 

8 
4 

3i-6 
32-3 

46 
47 

.2 

6* 
* 

MgCl2.i2H2O  + 
MgCl2.8H2O  a 
MgCl2.i2H20-f 
MgCl2.8H2O/3 
MgCl2.i2H2O  + 

60 
80 
100 

37 
39 
42 

•9 

.8 

.2 

61 
66 

73 

.0 

.0 

.0 

44 

44 

-19 

4 

33-3 

49 

9 

116 

•7  46 

.2 

85 

•5 

f  MgCl2.6H2O  + 
|     MgCl2.4H2G 

-  9- 
-  3- 

6 

4 

33-9 
34-4 

51 

3* 
•3 

M!gC^l2.8H2O  p 
+  MgClo.6H2O 
MgCl2.8H20  a  + 
MgCl2.6H2O      about 

152 
181 

6  49 

5  55 

.1 

.8 

96 
126 

•4 

.0 

MgCl2.4H2O 
(  MgCl2.4H2O  + 
\     MgCl2.2H2O 

1  86 

56 

.1 

128 

.0 

MgCl2.2H20 

*  =  Unstable. 

SOLUBILITY   OP   MAGNESIUM   CHLORIDE   IN   AQUEOUS   SOLUTIONS   OP 
HYDROCHLORIC  ACID  AT  o°. 

(Engel —  Compt.  rend.  104,  433,  '87.) 


Milligram  Mols.  p^er  10  cc.  Solution. 

Sp.Gr.of 

Grams  per  Liter  of  Solution. 

HC1. 

iMgd2. 

Solutions. 

HC1. 

MgClz. 

o.o 

99-55 

I  .362 

o.o 

474.2 

4-095 

95-5 

1-354 

14-93 

454-8 

9-5 

90.0 

1-344 

34.63 

428.6 

17.0 

82.5 

1.300 

61.97 

393-o 

20.5 

79-o 

1.297 

74-74 

376-2 

28.5 

71.0 

1.281 

103.9 

338-3 

42.0 

60.125 

286.4 

58.75 

46.25 

214.2 

2204.3 

76.0 

32-0 

277.1 

152.0 

sat.  HC1  (Ditte)       6.5 

100  gms.  H2O  dissolve  52.65  gms.  MgCl2  at  3.5°,  55.26  gms.  at  25°  and  58.66 
gms.  at  50°.  (Biltz  and  Marcus,  1911.) 


MAGNESIUM   CHLORIDE 


388 


SOLUBILITY  OF  BASIC  MAGNESIUM  CHLORIDE  IN  WATER  AT  25°. 

(Robinson  and  Waggaman,  1909.) 

An  excess  of  MgO  was  shaken  with  each  of  20  MgCl2  solutions  at  25°  for  six 
months  and  the  supernatant  clear  solutions  and  solid  phases  with  adhering  liquid, 
analyzed.  The  solutions  were  titrated  with  0.02  n  HC1  for  dissolved  MgO 
(present  as  Mg(OH)2).  The  composition  of  the  solid  phase  in  each  case  was 
ascertained  by  plotting  the  analytical  results  on  a  triangular  diagram. 


Solid  Phase. 


2MgO.HCl.SH2O 


SOLUBILITY  OF  MIXTURES  OF  MAGNESIUM  CHLORIDE,  POTASSIUM  CHLORIDE 

AND  OF  MAGNESIUM  POTASSIUM  CHLORIDE  (CARNALLITE)  IN  WATER  AT 

VARIOUS  TEMPERATURES. 

(van't  Hoff  and  Meyerhoffer,  1899,  1912.) 


Sat.  Sol. 

Gms.  per  100  Gms. 
Sat.  Sol. 

Solid  Phase.'       gjfc^ 

Gms.  per  100  Gms. 
Sat.  Sol. 

MgCl*. 

MgO.    ' 

MgCl2. 

MgO. 

I 

019 

2 

•36 

0 

00008 

Indefinite 

.141 

17-53 

0 

.0024 

•I 

038 

4 

•47 

o 

00028 

Solid  Solution 

.162 

18.52 

0 

.0025 

i 

056 

6 

•79 

o  .  00048 

.192 

22.04 

0 

.00245 

I 

075 

9 

.02 

o 

00080 

(C 

.245 

26.88 

0 

.0025 

VI 

13 

•  14 

0 

00115 

l( 

.274 

29.80 

0 

.0024 

.321 

34-22 

o 

.0030 

Gms.  per  100 
t°.             Gms.  H2O. 

Solid  Phase. 

Kind  of  Point  on  Curve.1 

MeCl,. 

KC1. 

—    II 

i 

.  . 

; 

24 

6 

Ice  +KC1 

Cryohydric  of  KC1 

-  33 

6 

26 

"  +MgCl2.i2H20 

MgCl2 

i2H2O 

—  34 

3 

22 

7 

I 

24 

"  +KCl+MgCl2.i2H2O 

+KC1 

—    21 

34 

9 

2 

03  Carnawte+MgCl2.I2H2O+KCl 

Formation  Temp,  of 

Carnallite 

—       O 

35 

5 

3-02 

+KC1 

Point  on  Curve 

25 

38 

4 

4.76            +    " 

U                  (( 

50 

42 

6 

17 

4-  " 

((             (I 

(Uhlig, 

1913 

61 

5 

42 

6 

7 

20 

+  " 

((           11 

*54 

5 

65 

5 

14 

07 

H~  " 

(I             « 

167 

5 

88 

i 

26 

-f  " 

M.  pt.  of  Carnallite 

25 

55 

5 

0.83 

"  +MgClj.6H,O 

Point  on  Curve 

50 

59 

13 

o 

50 

"  +         " 

K                       It 

(Uhlig, 

1913-) 

80 

65 

i 

24 

U     _J_                   « 

1C                      it 

"5 

7 

85 

6 

i 

66 

"  +        "        +MgCl2.4H2O  Transition  Point 

[Carnallite 

152 

5 

105 

7 

9-93 

"  +MgCl2.4H20+KCl 

Upper  Formation  Temp,  of 

176 

126 

9 

16 

97  MgCl2.4H2O+MgCl2.2H2O+KCl  Transition  Point 

186 

126 

9 

26 

i 

MgCl2.2H2O+KCl 

Point  on  Curve 

Carnallite  =  MgKCl3.6H2O. 
SOLUBILITY  OF  MIXTURES  OF  MAGNESIUM  CHLORIDE  AND  OTHER  SALTS  IN 


Mixture. 

MgCl2.6H2O+MgSO4.6H2O 
MgCl2.7H2O+MgSO4.6H2O 


WATER  AT  25°. 

(Lowenherz,  1894.) 
Gms.  Mols.  per  1000  Mols.  H2O. 


104  MgCl2+i4  MgSO4 
73       "     +15       " 
MgCl2.6H2O+MgCl2.KC1.6H2O  106  Cl2-f-i  K2+io5  Mg 


Gms.  per  Liter  of  Solution. 

i •*" 

25.  Cl+4.4  SO4 

19.5  Cl+5-3  S04 

26.9Cl+o.3K+45.7S04 


Results  for  all  possible  combinations  of  magnesium  sulfate  and  potassium 
chloride  and  of  magnesium  chloride  and  potassium  sulfate  are  also  given. 

100  cc.  anhydrous  hydrazine  dissolve  2  gms.  MgCl2  at  room  temp.     A  flocculant 

ppt.  separates  on  Standing.  (Welsh  and  Broderson,  1915.) 

Freezing-point  data  (solubility,  see  footnote,  p.  i)  for  mixtures  of  MgCl2  and 
KC1,  NaCl,  AgCl,  ZnCl2  and  SnCl2  are  given  by  Menge  (1911).  Data  for  mixtures 
of  MgCl2  +  SrCl2  and  MgCl2  +  MnCl2  are  given  by  Sandonnini  (1912,  1914). 
Data  for  MgCl2  +  MgSO4  are  given  by  Jaenecke  (1912).  Data  for  MgCl2+TlCl 
are  given  by  Korreng  (1914)  and  data  for  MgCl2+KCl  and  MgCl2-f  HC1  are  given 
by  Dernby  (1918). 


MAGNESIUM  CINNAMATE 


MAGNESIUM   CINNAMATE   (C6H6.CH.CH.COO)2Mg.H2O. 

100  gms.  sat.  solution  in  water  contain  0.85  gm.   (C6H6CH.CHCOO)2Mg  at 
15°  and  1.94  gms.  at  IOO°.  (Tarugi  and  Checchi,  1901.) 

MAGNESIUM  CHROMATE   MgCrO6.7H2O. 

100  grams  H2O  dissolve  72.3  grams  MgCrO<  at  18°,  or  100  grams  solution  con- 
tain 42.0  grams.     Sp.  Gr.  =  1.422.  (Mylius  and  Funk,  1897.) 

MAGNESIUM    POTASSIUM    OHROMATE   MgCrO4.K2CrO4.2H2O. 
100  grams  H2O  dissolve  28.2  grams  at  20°,  and  34.3  grams  at  60°. 

(Schweitzer.) 

MAGNESIUM    PLATINIC    CYANIDE 


SOLUBILITY  IN  WATER. 

(Buxhoevden  and  Tamman  —  Z.  anorg.  Ch.  15,  319  '97.) 

Gms.MgPt(CN)4                                                              Gms.  MgPl(CN)* 
t°.          per  100  Gms.             Solid  Phase.                        t°.         penooGms.           Solid  Phase. 
Solution.                                                                              Solution  . 

—  4.12               24.90     MgPt(CN)4.6.8-8.iH2O             48.7            40-89         MfcPt(CN)4.4H2O 

O 

•5 

26 

•9 

"        (Red) 

55 

41 

•33 

• 

5 

•5 

28 

•65 

" 

58 

.1 

42 

.15 

14 

18 

.0 

32 

.46 

it 

69 

.0 

43 

.40 

41 

36 

.6- 

39 

•53 

it 

77 

.8 

44 

,90 

• 

45 

.0 

41 

•33 

it 

8? 

•4 

45 

•52 

M 

46 

.2 

42 

.0 

•« 

90 

.0 

45 

•65 

14 

42 

.2 

40 

.21 

MgPt(CN)4.4H2O 

93 

.0 

45 

.04 

It 

46 

•3 

39 

•85 

14    (Bright  Green) 

96 

•4 

44 

•33 

MgPt(CN)4.2H20 

100 

•  0 

44 

.0 

" 

(White) 

MAGNESIUM  FerroCYANIDES. 

SOLUBILITY  IN  WATER  AT  17°. 

(Robinson,  1909.) 

One  liter  sat.   sol.  contains   1.95  gms.   magnesium  potassium  ferrocyanide, 
MgK2FeC6N6. 

One  liter  sat.  sol.  contains  2.48  gms.  magnesium  ammonium  ferrocyanide, 

Mg(NH4)2FeC6N6. 

MAGNESIUM  FLUORIDE   MgF2. 

One  liter  of  water  dissolves  0.076  gm.  MgF2  at  18°  by  conductivity  method. 

(Kohlrausch,  1905.) 

One  liter  water  dissolves  0.087-0.090  gm.  MgF2  at  0.3°  and  0.084  gm.  at  27° 
by  conductivity  method.  (Kohlrausch,  1908.) 

MAGNESIUM  HYDROXIDE   Mg(OH)2. 

One  liter  of  water  dissolves  0.008  —  0.009  Sm-  Mg(OH)2  at  18°  by  conductivity 

method.  (Dupre  and  Brutus,  1903.) 

One  liter  of  water  dissolves  0.009  Sm-  Mg(OH)2  at  18°  by  conductivity  method 
(Kohlrausch  and  Rose,  1893),  0.012  gm.  (Tamm,  1910). 

SOLUBILITY  OF  MAGNESIUM  OXIDE  IN  AQUEOUS  SOLUTIONS  CONTAINING 
SODIUM  CHLORIDE  AND  SODIUM- HYDROXIDE. 

(Maigret,  1905.) 

Gms.  MgO  per  Liter  Solution  with  Added: 

Gms.  NaCl  ,  *  ^ 

per  Liter.  0.8  g.  NaOH  4.0  g.  NaOH 


125 
140 

160 


per  Liter. 
0.07 
0.045 

none 


per  Liter. 
0.03 

none 


MAGNESIUM  HYDROXIDE  390 

SOLUBILITY  OF  MAGNESIUM  HYDROXIDE  IN  AQUEOUS  SOLUTIONS  OP 
AMMONIUM  CHLORIDE  AND  OF  AMMONIUM  NITRATE  AT  29°. 

(Herz  and  Muhs  —  Z.  anorg.  Ch.  38,  140,  '04.) 

NOTE.  —  Pure  Mg(OH)2  was  prepared  and  an  excess  shaken  with 
solutions  of  ammonium  chloride  and  of  ammonium  nitrate  of  different 
concentrations. 

..Concentration  of        ^Sg^d  Normality  of;  Grams  per  Liter 

^Wo?™^    °'^™^r     'Mg(OH),    NH.C1'.  •IWOH^HH.O: 

.7  (NH4C1)  0.09835  0.156  0.388  4.55  20.86 
0.466  "  O.IIOS  0.108  0.250  3.15  13.39 
0.35  "  0-09835  0.089  O.I72  2.6o  9-21 

0.233   "     0.1108     0.0638  0.106      1.86   5.67 
0.175   "     0.1108     0.049  0-0771      i-43   4-i3 

0.35   (NIL^NOs)   O.IIoS       0.0833  O .  l834(NH*NOt)2  -43   14 -69  (NIL^NOs) 
0.175    "       O.IIOS       0.04950-076     "    1.45    6.09 

MAGNESIUM    IODATE    Mg(IO3)a. 

SOLUBILITY  IN  WATER. 

(Mylius  and  Funk  —  Ber.  30,  1722,  '97;  Wiss.  Abh.  p.  t.  Reichanstalt  3,  446,  foo.) 

Gms.  Mols.  Gms.  Mols. 

to  Mg(I03)2         Mg(I03)2  Solid  to         Mg(I03)2    Mg(I03)2  Solid 

per  ioo        per  TOO  Mols,  Phase.  per  100     per  100  Mols,       Phase. 

Gms.  Solution.      H2O.  Gms.  Solution.      H2O. 

O  3-1  0.15      MgaQs^.ioHjjO  o  6.8  0.34      Mg(IOa)2.4H2O 

20  10.2  0-55  10  6.4  0.30 

30        17.4          i. oi                               18  7.6  0.40 

35        2I-9          I-35                             20  7.7  0.40 

50        67.5        10.0                               35  8.9  0.47 

63  12.6  o .  69            M 

ioo  19.3  1.13 

Sp.  Gr.  of  solution  sat.  at  18°=  1.078. 
MAGNESIUM  IODIDE  MgI2.8H2O. 

SOLUBILITY  IN  WATER.     (Menschutkin,  1905, 1907.) 

The  salt  was  prepared  by  the  action  of  water  upon  magnesium  iodide  dietherate 
(see  p.  391)  by  which  the  octrahydrate  and  not  the  hexahydrate  is  formed.  The 
crystals  of  this  hydrate  melt  at  43.6°.  The  solubility  determinations  were  made 
by  the  synthetic  method. 

Gms.  per  100  Gms.  Sat.  Solution. 

Solid  Phase. 

MgI2.8H2O 

1 '  (Mylius  and  Funk,  1897.) 

u 

(( 


MgI2.6H20    = 

=       Mgl,. 

O 

76 

54-7 

18 

59.7    W-i.909) 

20 

81 

58.3 

40 

88 

63.4 

43.5tr.pt. 

90.8 

65-4 

43 

89.8 

64.7 

80 

90-3 

65 

120 

90.9 

65-4 

160 

91.7 

66 

200 

93-4 

67.2 

215 

94-3 

67.9 

"    +MgI2.6H20 
MgI2.6H2O 


391  MAGNESIUM   IODIDE 

MAGNESIUM  IODIDE  ETHERATES,  ALCOHOLATES,  ACIDATES,  etc. 

SOLUBILITIES  RESPECT/VELY  IN  ETHER,  ALCOHOL  AND  ACID  SOLVENTS  AT 
VARIOUS  TEMPERATURES. 

Boris  N.  Menschutkin.  Monograph  in  the  Russian  Language  entitled  "On  Etherates  and  Other  Molec- 
ular Combinations  of  Magnesium  Bromide  and  Iodide,"  St.  Petersburg,  1907,  pp.  267  -+-  XL VIII. 
Also  published  in  "Memoirs  of  the  St.  Petersburg  Polytechnic  Institute,"  vols.  1-7,  1904-07  and  in 
condensed  form  in  vols.  49-67  of  the  Zeit.  anorg.  Chem.,  1906-09. 


Preparation  of  Material.    The  dietherate  of  magnesium  iodide,  MgI2.2C4Hi0O, 

was  prepared  by  the  very  gradual  addition  of  iodine  to  a  mixture  of  magnesium 
and  dry  ether.  The  reaction  is  not  so  violent  as  that  which  takes  place  during 
the  preparation  of  the  magnesium  bromide  dietherate  (see  p.~379).  Two  liquid 
layers  are  present  at  the  end  of  the  reaction  and  by  slight  cooling  beautiful  white 
needle-like  crystals  separate  from  the  lower  one.  The  growth  of  these  crystals 
is  also  accompanied,  as  in  the  case  of  the  magnesium  bromide  compound,  by  an 
evolution  of  ether  droplets.  Magnesium  iodide  dietherate  is  very  hygroscopic, 
it  is  less  stable  than  magnesium  bromide  dietherate,  and  becomes  yellowish  even 
after  several  hours,  and  brown  after  a  day,  owing  probably  to  separation  of 
iodine.  As  in  the  case  of  the  magnesium  bromide  compound  it  reacts  with  very 
many  organic  compounds  as  alcohols,  acids,  ketones,  etc.,  with  liberation  of  ether 
and  formation  of  addition  products.  These  latter  constitute  the  material  used 
for  the  following  solubility  studies. 


Method  of  Determination  of  Solubility.    The  synthetic   (sealed  tube) 
method  of  Alexejeff  (Wied.  Ann.,  1885)  was  used  almost  exclusively. 


Explanation  of  Results.  As  is  seen*  from  the  following  table,  the  solubility 
increases  much  more  rapidly  with  temperature  than  in  the  case  of  magnesium 
bromide  dietherate,  especially  in  the  vicinity  of  the  melting  point  of  Mgl2.2C4H:oO 
under  its  ethereal  solution,  which  is  at  23.6°.  At  this  temperature  there  appears 
two  layers,  the  lower  one  of  which  may  be  considered  as  a  solution  of  ether  in 
dietherate,  and  the  upper  one  as  a  solution  of  the  lower  layer  in  ether.  By  in- 
crease of  temperature  a  point  is  reached,  at  which  both  layers  are  miscible  in  all 
proportions  (critical  point).  In  the  case  of  magnesium  bromide  dietherate  no 
such  critical  point  could  be  obtained.  Both  layers  may  be  cooled  below  23.6°, 
but  only  to  about  +  15°  since  here  spontaneous  crystallization  of  the  dietherate 
almost  always  occurs,  and  the  temperature  rises  to  23.6°.  The  great  tendency 
to  crystallize  is  probably  due  to  the  difference  between  the  composition  of  the 
lower  layer  and  of  the  saturated  solution  of  the  dietherate.  The  determinations 
in  the  vicinity  of  the  critical  point  were  quite  difficult  to  make  on  account  of  the 
considerable  opalescence  which  occurred  and  also  the  formation  of  a  white 
substance,  the  nature  of  which  was  not  ascertained.  The  critical  concentration, 
as  determined  by  means  of  the  law  of  straight  averages  of  Cailletet  and  Mathias, 
was  approximately  40.3  per  cent  MgI2.2(C2H5)2O;  the  temperature,  38.5°.  At 
concentrations  of  MgI2.2C4HioO  greater  than  54  per  cent,  a  single  liquid  is  again 
formed  and  the  solubility  curve  can  be  followed  up  to  the  melting  point  of  the 
dietherate  at  51°. 


MAGNESIUM  IODIDE 


392 


SOLUBILITY  OF  MAGNESIUM  IODIDE  DIETHERATE  IN  ETHER  AT  DIFFERENT 
TEMPERATURES.     (Menschutkin,  1906.) 

Cms.  per  100  Cms.  Mols.  MgI2.2(C2H6)2O 

per  I00  Mols. 


t°.  Sat,  Sol.  per  loo  Mols.  Solid  Phase. 

5-4  2.2  1.45  0-39  MgI2.2(C2H5)2O 

ii. 8 
iS-6 
18.1 
20.4 

22.2 

23-6 

Between  these  two  concentrations  of  MgI2.2(C2H6)2O  two  liquid  layers  separate 
(see  below). 

23-6  54.4  35-5  J7-l 

25  73 


^gIZ.2(CjH6)2 

O    =     MgI2. 

Sat.  Sol. 

2.2 

I  .45 

0.39 

3-7 

2-43 

0.66 

5-3 

0.96 

8.3 

5-4 

1.55 

n.  6 

7-55 

2.24 

17-3 

11.28 

3.56 

22 

14.4 

4.67 

30 
35 
40 

45 
5i.Sm.pt. 


82.5 
87 

89.6 

93-5 

IOO 


47.6 

54 

57 

58.6 

61.2 

65.2 


42.9 

53-4 
60.4 

71-4 
100 


At  23.6°  the  saturated  solution  separates  into  two  liquid  layers  which  have 
the  following  composition  at  different  temperatures. 

Cms.  per  100  Cms.  Solution. 


unstable 

u 

stable 

« 

u 

it 


MAGNESIUM   IODIDE  ALCOHOLATES  and  ANILINATE. 

SOLUBILITY  OF  EACH  IN  THE  RESPECTIVE  ALCOHOLS  OR  ANILINE.  (Menschutkin.) 


4.0                                         Lower  Layer. 
MgI2.2(QH6)20  =  MgI2. 

Upper  Layer. 
Mgl^CQH-^O  =  Mgl,. 

15 

54-4 

35-5 

20.5 

13-4 

2O 

54-4 

35-5 

21-5 

I4.I 

25 

54-4 

35-5 

22.5 

14.7 

30 

54-4 

35-5 

23-5 

15-4 

35 

54-1 

35-3 

26 

17 

36 

53-5 

34-9 

27 

17.7 

37 

52.2 

34-2 

28.5 

lS.1 

38 

So-5 

33-i 

32 

21 

38  .  5  cnt.  temp. 

40.3 

26.3 

40-3 

26.3 

MgI2.6CH3OH 
in  Methyl  Alcohol 

Gms. 
to       MgI2.6CH3OH 
per  loo  Gms. 

MgI2.6C2H5OH 
in  Ethyl  Alcohol. 

Gms. 
to         MgI2.6C2H5OH 
per  100  Gms. 

MgI2.6C6H5NH2 
in  Aniline. 

Gms. 
to       MgI2.6C8H5NH2 
per  100  Gms. 

MgI2.6(CH3)2CHOH 
in  Dimethyl  Carbinol. 

Gms. 
to         MgI2.6(CHj)r 
*  '        CHOH  oer  100 

Sat.  Sol. 

Sat.  Sol. 

Sat.  Sol. 

Gms.  Sat.  Sol. 

O 

49.6 

0 

21.9 

0 

3-3 

10 

57.1 

20 

52.6 

2O 

33-2 

60 

3-9 

30 

60 

40 

55-3 

40 

44-4 

IOO 

5 

50 

63.3 

60 

58.8 

60 

55-3 

130 

8.5 

70 

67 

80 

60.6 

80 

65.5 

150 

17-5 

90 

71.2 

IOO 

63.3 

IOO 

74-7 

170 

38 

no 

76.2 

1  20 

66.2 

120 

82.7 

180 

S2 

120 

79-4 

140 

69.5 

130 

87.2 

i88J 

64-5 

130 

84.8 

160 

73-2 

I4O 

93-3 

200 

65.9* 

136 

91.7 

180 

77.1 

143 

96 

210 

67.2* 

I38f 

IOO 

200 

8i.S 

146.  st 

IOO 

230 

69.8* 

Solid  Phase,  Mgl^HjNH,.       f  M.  pt.        I  Tr.  pt. , 


393 


MAGNESIUM  IODIDE 


MAGNESIUM   IODIDE   COMPOUNDS. 

SOLUBILITY  OF  MAGNESIUM  IODIDE  COMPOUNDS  WITH  BENZALDEHYDE, 
ACETONE,  ACETAL,  AND  ACETIC  ACID  IN  EACH  OF  THESE  LIQUIDS. 

fc(Menschutkin.) 


MgI2.6C6H5COH     MgI2.6CH3COCH3        MgI2.2CH3CH-         MgI2.6CH3COOH 
in  Benzaldehyde.           in  Acetone.            (OC2H6)2  in  Acetal.        in  Acetic  Acid. 

Gms.  MgI2.-                           Gms.  MgI2.-                          Gms.  MgI2.-                         Gms.  Mglj.- 
to            6C,H5COH       to                 6CH3COCH3          to        2CH3CH(OC2H6)2     fa           6CH3COOH 
per  loo  Gms.                        per  100  Gms.                       per  100  Gms.                     Der  100  Gms- 

Sat.  Sol. 

Sat.  Sol. 

Sat.  Sol. 

Sat.  Sol. 

0 

3-2 

0 

4-9 

20                0.15 

20 

0.6 

20 

3-8 

30 

6.7 

60                 0.45 

40 

2 

40 

5-3 

50 

8-3 

77            0.60 

60 

5 

60 

7-7 

60 

10.2 

(Between  these  two  con- 

70 

9-5 

80 

n 

70 

15-2 

centrations    the    mix- 

80 

18.5 

IOO 

18.5 

80 

28.6 

ture  separates  into  two 

95 

42 

no 

26.5 

85 

40 

liquid  layers.) 

105 

54-5 

120 

40 

90 

59-2 

77          92 

65 

125 

53 

95 

80 

79          93-7 

125 

73-8 

130 

74-5 

IOO 

92-5 

81          95-5 

85 

136 

94.2 

105 

98.5 

83          97-3 

140 

94 

I39m.pt.  IOO  Io6.5m.pt.  IOO  86m.pt.  IOO  I42m.pt.  IOO 

^On  account  of  the  properties  of  these  molecular  compounds,  their  great  hygro- 
scopicity,  etc.,  the  solubility  determinations  are  not  strictly  accurate  in  all  cases. 

SOLUBILITY  OF  MAGNESIUM  IODIDE  COMPOUNDS  WITH  FORMIC  AND  ACETIC  ACID 
ESTERS  IN  THE  RESPECTIVE  ESTERS. 

(Menschutkin.) 


in  Ethyl  Formate,  in  Methyl  Acetate. 

in  Ethyl  Acetate.      in  Propyl  Acetate. 

Gms.  MgI2.-                        Gms.  MgI2.- 
to             6HCOOC2H5       to           6CH3COOCH, 

Gms.  MgI2.-                        Gms.  Mgl,.- 
to             eCHsCOOQHj         to       6CH3COOC3H7 

per  loo  Gms.          '            per  100  Gms. 

per  too  Gms.                       per  100  Gms. 

Sat.  Sol.                             Sat.  Sol. 

Sat.  Sol.                              Sat.  Sol. 

o             15.1          o            0.4 

o               3.2            o           4.1 

10             17.4        60            0.75 

20                      4.8              20                 5.4 

20                   20.5            90                 0.9 

40               8.6          30            6.5 

30             25           loo            1.8 

50              13-7          35            7-8 

40           31.8      103           2.4 

55              21.5          40          19 

50                 44               (Two  layers  here.) 

60             38             45          46 

60             68          103          74.2 

65              63.5          50          72.5 

7o.5m.pt.  loo          no          81.7 

70              90.5          55          88.2 

120               98 

75              92-7          6°          96 

I2Im.pt.  IOO 

78.5m.pt.  IOO                   65m.pt.  IOO 

MgI2.6CH3COO  (iso)  C4H9 
in  Isobutyl  Acetate. 

MgI2.6CH3COO  (iso)  C6HU 
in  Isoamyl  Acetate. 

Gms.  MgI2.6CHr 
t°.                     COO  (iso)  C4H9 
per  loo  Gms.  Sat.  Sol. 

Gms.  MgIv6CHr 
te.                   [COO  (iso)  CSHU 
per  loo  Gms.  Sat.  Sol. 

o                    10.5 

o                     7.7 

20                            13.6 

20                           II.5 

40                            17.6 

40                   20  .  9 

60                    24  .  9 

45                   25.5 

70                   33-7 

5°                   33-2 

80                   52 

55                   47-8 

85              <     89 

57-5                63 

87.5m.pt.           IOO 

6om.pt.              IOO 

MAGNESIUM  IODIDE 


394 


MgI2.6CH3CN 
in  Acetonitrile. 

MgI2.6CH3CONH2 
in  Acetamide. 

Gms.  MgI2.- 
to      6CH.,CNper    *o 

Gms.  MgI2.- 
^CH3  CONHj       Solid  Phase 

t°  6: 

ioo  Gms. 

per  ioo  Gms. 

*  .1 

Sat.  Sol. 

Sat.  Sol. 

0 

37-2 

82m 

.  pt.  of  acetamide 

49  n 

30 

49.8 

70 

28      CHjCONH, 

45 

50 

58.2 

58 

46.7     " 

39 

70 

67.9 

49* 

56  .  5     '  +MgI2.6CHaCONH2  32* 

75 

71.7 

80 

63.4      Mglj  6CH3CONH, 

40 

80 

76.5 

130 

76 

60 

85 

83 

160 

85-5 

80 

89 

170 

90.8 

86 

i77t 

IOO 

87! 

*  Eutec. 

t  m.  ] 

SOLUBILITY  OF  MAGNESIUM  IODIDE  COMPOUNDS  WITH  ACETONITRILE,  ACETAMIDE 
AND  URETHAN  IN  THESE  LIQUIDS.    (Menschutkin.) 

MgI2.6NH3COOC2H6 

in  Urethan. 
Gms.  MgI2.- 

™°GS?'       ^id  Phase. 
Sat.  Sol. 
pt.  of  urethan 
27.5NH3COOQH5 

45 

51.8      "  +MgI2.NH3COOC2H5 
55  MglvNHsCOOCjHj 

64.7 
78.8 
92.5 
IOO 

t. 

MAGNESIUM  IODOMERCURATE  MgI2.2HgI2.7H2O. 

The  sat.  solution  in  water  at  17.8°  has  the  composition  MgI2.i.29HgI2.n.o6H2O 
and  Sp.  Gr.  2.92.  (Duboin,  1906.) 

MAGNESIUM   DiLACTATE   Mg(C6H8O6).6H2O   racemic,   Mg(C6H8O6).3H2O, 

inactive. 
SOLUBILITY  OF  RACEMIC  AND  OF  INACTIVE  MAGNESIUM  DILACTATE  IN  WATER. 

(Jungfleisch,  1912.) 

ioo  gms.  H2O  dissolve  7  to  8  gms.  racemic  and  2.28  gms.  inactive  lactate  at  15°. 

MAGNESIUM  LAURATE,  MYRISTATE,  PALMITATE  and  STEARATE. 

SOLUBILITY  OF  EACH  IN  SEVERAL  SOLVENTS,    (jacobson  and  Holmes,  1916.) 

Gms.  Each  Salt  Determined  Separately  per  ioo,Gms.  Solvent. 
Solvent. 

Water 
tt 

u 
tt 


Abs.  Ethyl  Alcohol 


Methyl  Alcohol 


Ether 

Ethyl  Acetate 


Amyl  alcohol 


Amyl  Acetate 
u 

tt 

tt 


t°. 

Mg  Laurate 

Mg  Myristate 

Mg  Palmitate 

Mg  Stearate 

(C11H23COO)Z 

Mg. 

•    (CnHtfCOO),- 
Mg. 

(CH3(CH2)M- 
COO)2Mg. 

(CHs(CHj)r 
COO)2Mg. 

15 

O.OIO 

0.006 

0.005 

0.003 

25 

0.007 

O.OO6 

O.OOS 

O.OO4 

35 

O.OIO 

O.OO7 

0.006 

O.OO7 

So 

0.026 

0.014 

o  .  009 

0.008 

0.519 

0.158 

0.034 

O.OI7 

25 

0.591 

0.236 

0.058 

O.O23 

35 

0.805 

0-373 

0.085 

0.031 

50 

1.267 

0-577 

O.I5I 

.  .  . 

15 

1.095 

0.571 

0.227 

0.084* 

25 

1.108 

0.763 

0.36 

O.IOO 

S1^ 

0.50 

0.166 

25 

0.015 

O.OIO 

O.OO4 

0.003 

15 

0.004 

0.004 

0.004 

0.004 

35 

O.OII 

O.OIO 

0.007 

0.008 

50 

0.024 

O.O2I 

0.013 

15 

0.191 

0.086 

0.043 

0.014 

25 

0.236 

0.145 

0.066 

0.018 

35 

1.481 

0.438 

O.IO4 

0.039 

50 

4.869 

1.893 

0.263 

0.105 

15 

0.119 

0.063 

0.039 

0.029 

25 

0.162 

0.073 

0.045 

0.030 

34-6 

0.259 

O.IO5 

0.057 

0.046 

50 

1-939 

0.605 

0.216 

0.115 

395 
MAGNESIUM    NITKATE   Mg(NO3)2. 


MAGNESIUM   NITRATE 


SOLUBILITY  IN  WATER. 

(Funk  —  Wiss.  Abh.  p.  t.  Reichanstalt  3,  437,  'oo.) 


t° 

Gms. 
Mg(N03)2 
per  100  Gms. 

Mols. 
Mg(N03)2 
per  100  Mo] 

,             Solid 
is.           Phase. 

Gms. 
Mg(N03)2 
t   .     per  100  Gms. 

Mois. 
Mg(NOs 
per  loo  Ik! 

,)2          Solid 
lols.       Phase. 

Solution. 

H20. 

Solution. 

H20. 

-23 

35 

•44 

6 

.6 

Mg(N03)2.9H20 

40 

45 

.87 

10. 

3 

Mg(NOa)2^] 

-20 

36.19 

7 

.0 

" 

80 

.69 

14. 

6 

" 

-18 

38 

•03 

7 

•4 

" 

90 

57 

.81 

16. 

7 

" 

-18 

38 

•03 

7 

•37 

Mg(NO3)2.6H2O 

89 

63 

.14 

20. 

9 

) 

~   4 

•5  39 

•50 

7 

.92 

" 

77-5 

65 

.67 

23- 

2 

U 

0 

8 

.08 

" 

67 

6? 

•55 

25- 

I 

+18 

42 

•33 

8 

•9 

" 

* 

Reverse  curve- 

Sp.  Gr.  of  solution  saturated  at  18°  =  1.384. 

The  eutectic  is  at  —29°  and  34.6  gms.  Mg(NO3)2  per  100  gms.  sat.  solution. 
Fusion-point  data  for  Mg(NOs)2  +  Zn(NOs)2  are  given  by  Vasilev   (1909.) 
Results  for  Mg(NO3)2  +  HNO3  are  given  by  Dernby  (1918). 

MAGNESIUM   OLEATE   (CH3(CH2)13CH:;CH.CH2COO)2Mg. 

One  liter  H2O  dissolves  about  0.23  gm.  oleate  (soap).  (Fahrion,  1916.) 

100  gms.  glycerol  (d  1.114)  dissolve  0.94  gm.  oleate.  (Asselin,  1873.) 

MAGNESIUM  OXALATE   MgC2O4.2H2O. 

One  liter  of  water  dissolves  0.3  gm.  MgC2O4  at  18°  (conductivity  method). 

(Kohlrausch,  1905.) 

MAGNESIUM^  OXIDE   MgO. 

Fusion-point  data  (quenching  method)  for  MgO  +  SiOg  are  .given  by  Bowen 
and  Anderson,  1914. 

MAGNESIUM  PHOSPHATE   MgHPO4.3H2O. 

SOLUBILITY  OF  MAGNESIUM  PHOSPHATE  IN  AQUEOUS  SOLUTIONS  OF  PHOSPHORIC 

ACID  AT  25°.     (Cameron  and  Bell,  1907.) 

The  mixtures  were  constantly  agitated  for  two  months  and  the  clear  solutions 
analyzed  for  magnesia  and  phosphoric  acid. 


^25  Of 

Sat.  Sol. 

Gms.  per  Liter.             c  VJ 

Phase.     Sa^  °JL 

Gms.  p 

er  Liter. 

Solid  Phase. 

MgO. 

P206. 

MgO. 

P2O5. 

0.207 

0.486  MgHPO4.3H2O 

109.5 

439       MgHPO4-3H2O 

0.280 

0.732 

1.470 

122.6 

498 

.  .  . 

0-553 

1.917 

129.9 

546.5       " 

1.438 

4-85 

140 

584 

.006 

2.23 

7-35 

1-595 

146.8 

623.3 

.017 

4-73 

16.84 

147-3 

625.9 

.042 

11.19 

38.59 

.  .  . 

150.3 

645.8 

.069 

17-33 

61.21 

.  .  . 

155-5 

680.7 

V 

.109 

26.09 

93-09 

.  .  . 

1  60 

700 

+MgH4(P04)2.XH20 

.144 

37-40 

130.7 

1.626 

87.1 

779.6 

MgH4(PO4)2.XH2O 

.285 

75-5 

281.8 

1.644 

77.1 

809/6 

" 

1.654 

7O.6 

835.1 

" 

MAGNESIUM   (Hypo)   PHOSPHATE   Mg2P2O6.i2H2O. 

One  liter  of  water  dissolves  0.066  gm.  hypophosphate.  (Salzer,  1886.) 

One  liter  of  water   dissolves   5   gms.  magnesium  hydrogen  hypophosphate, 

MgH2P2O6.4H2O.  (Salzer.) 

MAGNESIUM  SALICYLATE   Mg(C7H6O3)2.4H2O. 

loo  gms.  sat.  solution  in  water  contain  20.4  gms.  salicylate  at  15°  (14.3  gms. 

Squire  and  Caines,  1905),  and  79.7  gms.  at  100°.  (Tarugi  and  Checchi,  1901.) 

loo  gms.  90%  alcohol  dissolve  0.6  gm.  salicylate  at  I5°-2O°.  (Squire  and  Caines,  1905.) 


MAGNESIUM  SILICATE  396 

MAGNESIUM   SILICATE   MgSiO,. 

Fusion-point  data  for  mixtures  of  MgSiOs  +  MnSiOs  are  given  by  Lebedew 
(1911).     Results  for  MgSiO3  +  Na2SiO3  are  given  by  Wallace  (1909). 


MAGNESIUM  FLUOSILICATE   MgSiF6.6H2O. 

One  liter  of  water  dissolves  652  gms.  of  the  salt  at  17.5°. 
=  1-235. 


Sp.  Gr.  of  solution 
(Stolba,  1877.) 


MAGNESIUM   SUCCINATE   C4H4O4Mg.5H2O. 

100  gm£.  sat.  solution  in  water  contain  24.35  gms.  succinate  at  15°  and  66.36 
gms.  at  I  OO°.  (Tarugi  and  Checchi,  1901.) 


MAGNESIUM  SULFATE   MgSO4.7H2O. 

SOLUBILITY  IN  WATER. 

(Results  by  several  investigators.    4th  Ed.  Landolt>nd  Bornstein,  "  Tabellen," 
1912.) 


Gms.  MgSO4 

Gms.  MgSO4 

t°.        per  100  Gms.                  Solid  Phase. 

t°.         per  100  Gms.             Solid  Phase. 

Sat.  Sol. 

Sat.  Sol. 

Unstable  Portions  of  Curve. 

—  2.9      13.9    (i)           ice 

-8.4      23.6     (l)    Ice 

—3.9       19.       (2)               "  +MgSO4.i2H2O 

—  5          19       (12)     "  -fMgSO4.7H2O  rhomb. 

+  1.8       21.  1     (2)    MgSO4.i2H20+MgS04.7H2O 

o          20  .  6     (3)    MgSO4.7H2O  rhomb. 

10            23  .  6     (3)       MgSO4.7H2O  (rhombic) 

o          25.8     (3)             "           0  hexagonal 

20            26  .  2       ; 

0 

+10         27.9      3 

25            26.8      t 

[ 

20         30          3 

30            29        .   % 

0 

o         29          3 

MgS04.6H,0 

40       31-3  (s) 

10         29  .  7    (3 

« 

48          33        (< 

)                    +MgSO4.6H,O 

20         30.8    (3 

50          33-S    (' 

7         MgS04.6H2O 

30         31.2    (7 

55          34-3    ( 

1 

70        37-3    (5 

60          35-5    (5) 

80        39-i    (S) 

68          37        (8)               "  +MgS04.H,0 

90        40.8    (5) 

80          38.6    (7)                MgS04.H20 

100        42.5    (5) 

83          40.2    (9) 

99.4-     40.6(10) 

164          29.3  (n) 

188           20.3  (n) 

.  (i)  de  Coppet,  1872;  (2)  Cottrell  et  al,  1901;  (3)  Loewel,  1855;  (4)  Basch,  1901;  (5)  Mulder; 
(6)  Van  der  Heide,  1893;  (7)  Smith,  1912;  (8)  Van't  Hoff,  1901;  (9)  Geiger,  1904;  (10)  Meyerhoffer, 
1912;  (n)  Etard,  1894;  (12)  Guthrie,  1876.  See  also  Tilden,  1884. 

Data  for  densities  of  aq.  MgSO4  solutions  are  given  by  Barnes  and  Scott,  1898. 

SOLUBILITY  OF  MAGNESIUM  SULFATE  IN  AQUEOUS  SOLUTIONS  OF  POTASSIUM 
SULFATE  AT  25°  AND  VICE  VERSA. 

(Van  Klooster,  1917.) 

rime     r\fir    Tnr*   Clmc     Qof      Qrtl  /~lr*-»p     r\av    Y  ^/-*    Clrrtv     Qnf      Q/-»1 

Solid  Phase. 


MgS04. 

K2S04. 

•»                    DOI1U   1  IKISC. 

MgS04. 

K2S04. 

26.76 

0 

MgS04.7H,0 

13.26 

10.34 

26.67 

1.68 

" 

12.88 

IO.5I 

26.57 

2-34 

" 

12.68 

10.70 

26.36 

3-76 

« 

12.06 

10.77 

26.39 

4.02 

"  +MgK2(S04)2.6H20 

10.69 

10.84 

18.76 

7.02 

MgK,(SO«),.6H|Q 

7.8 

II  .IO 

16.36 

8-43 

" 

4 

11.03 

I4.27 

9-63 

" 

o 

10.77 

loo  gms.  95%  formic  acid  dissolve  0.34  gm.  MgSO4  at  19°. 


+K2S04 
K2S04 


(Aschan,  1913.) 


397  MAGNESIUM   SULFATE 

SOLUBILITY  OF  MAGNESIUM  SULFATE  IN  METHYL  AND  ETHYL  ALCOHOLS 

(de  Bruyn,  1892.) 

Solvent.          t°.  Per  100  Cms.  Solvent.  Solvent.  t°.      Per  100  Gms.  Solvent. 

Abs.  CHaOH  18  1.18  gms.  MgSO4  93%  Methyl  Ale.  17    9.7  gms.  MgSO4.7H,O 

17  41          "      MgS04.7H,0  50%        "          "  3-4  4.1     " 

3-4  29        "  "  Abs.  CijHsOH  3     1.3    " 


SOLUBILITY  IN  AQUEOUS  ETHYL  ALCOHOL. 

(Schiff,  1861.) 

Weight  per  cent  Alcohol  10  20  40 

Gms.  MgSO4.7H2O  per  100  gms.  solvent  64.7        27.1        1.65 

SOLUBILITY  OF  MAGNESIUM  SULFATE  IN  SATURATED  SUGAR  SOLUTION  AT  31.25°. 

(Kohler,  1897-) 

ioo  gms.  saturated  aqueous  solution  contain  46.52  gms  sugar  +  *4  Sms. 
MgS04. 

ioo  gms.  water  dissolve  119.6  gms.  sugar  +  36  gms.  MgSO4. 

Data  for  the  system  magnesium  sulfate,  phenol,  and  water  are  given  by  Tim- 
mermans,  1907. 

Fusion-point  data  for  mixtures  of  MgSO4  +  K2SO4  are  given  by  Ginsberg, 
1906;  Nacken,  i9O7a  and  Grahmann,  1913.  Results  for  MgSO4  +  NajSO4 
are  given  by  Nacken  iox)7b. 


MAGNESIUM  POTASSIUM  SULFATE   MgK2(SO4)2.6H2O. , 
SOLUBILITY  IN  WATER. 

(Tobler,  1855.) 

t°-  o°       20°          30°        45°        60°        75° 

Gms.  MgK2(SO4)2  per 
icogms.  H2O  14.1       25          30.4      40.5      50.2      59.8 

ioo  gms.  H2O  dissolve  30.52  gms.  MgK2(SO4)2.6H2O  at  15°.  (Lothian,  1909.) 


MAGNESIUM   SULFITE   MgSO3.6H2O. 

10  gms.  cold  water  dissolve  1.25  gms.  sulfite;  ioo  gms.  boiling  water  dissolve 

0.83  gm.  (Hager,  1875.) 

IOO  gms.  H2O  dissolve  I  gm.  sulfite  at  15°.  (Squire  and  Caines,  1905.) 


MAGNESIUM    SULFO  NATES. 

SOLUBILITY  IN  WATER  AT  20°. 

(Sandquist,  1912.) 

r  A  Gms.  Anhydrous  Salt 

Compound.  p^  JQO 


Magnesium  -2-Phenanthrene  Monosulfonate  6H2O  0.051 

-3-  "  "  4H2O  0.116 

-10-  "  "  5H2O  0.22 


MALAMINIC  ACID 


398 


MALAMINIC  ACID  CH2(OH)COOH:jCH2CONH2,  CH2COO.NH3.CHCOOH. 

SOLUBILITY  IN  WATER  AT  18°.    (Lutz,  1902.) 


Compound. 

d  |8  Malaminic  Acid 


M,p,. 

149 

U9 
148 


7.52 

7-5° 
4.02 


+9  .  70 
-9-33 


MALEIC  ACID   COOHCHfCH.COOH   (see  also  p.  304). 

SOLUBILITY  IN  SEVERAL  ALCOHOLS.    (Timofeiew,  1894.) 


Alcohol. 

f. 

Gms. 
(CHCOOH)2 
per  100  Gms. 

Alcohol. 

f 

Gms. 
(CHCOOH)j 
per  loo  Gms. 

Sat.  Sol. 

Sat.  Sol. 

Methyl  Alcohol 

22. 

5 

41 

Propyl  Alcohol 

0 

2O 

Ethyl  Alcohol 

O 

30.2 

u 

22  , 

5 

24-3 

u 

22  . 

5 

34-4 

Isobutyl  Alcohol 

0 

14.2 

" 

22, 

•5 

17-5 

Data  for  the  distribution  of  maleic  acid  between  ether  and  water  at  25°  are 
given  by  Chandler,  1908. 

Freezing-point  data  for  mixtures  of  maleic  acid  and  /  mandelic  acid  are  given 
by  Centnerszwer,  1899. 


MALIC  ACID  I  COOH.CH2CHOHCOOH. 

100  gms.  methyl  alcohol  dissolve  1 24.8     gms.  malic  acid  at    oc 

167.7 
91.4 
54 


ethyl 
propyl  ' 
dichlorethylene 
trichlorethylene 


0.009 

O.OIO 


o 

15°. 

15°. 


(Timofeiew,  1894.) 


(Wester  &  Bruins,  1894.) 


DISTRIBUTION  OF  MALIC  ACID  BETWEEN  WATER  AND  ETHER.    (Pinnow,  1915.) 

Results  at  25.5°. 

Gm.  Mols.  Acid  per  Liter. 


Results  at  15°. 

Gm.  Mols.  Acid  per  Liter: 

H2O  Layer.          Ether  Layer. 

0.564  0.0091 

o . 288  o . 0045 

O.I5I       O.OO24 
0.967       0.0157 


Dist.  Coeff. 
62 
64 

62.9 
6l.6 


t2O  Layer. 
I.I79 
0.582 

Ether  Layer. 
0.0172 
O.OO82 

68.4 
71 

0.293 

0.0040 

73 

0.142 

0.0020 

71 

Freezing-point  data  for  i  malic  acid  -f- 1  mandelic  acid  are  given  by  Cent- 
nerszwer, 1899. 

MALONIC  ACID  CH2(COOH)2. 

SOLUBILITY  IN  WATER. 

(Klobbie,  1897;  Miczynski,  1886;  Henry,  1884;  Lamouroux,  1898,  1899.) 


Gms.  CH2(COOH)2  per  100. 


Gms.  CH2(COOH)2  per  100. 


Gms.  Solution.* 

cc.  Solution  (L.). 

0 

52 

61 

10 

56.5 

67 

20 

60.5 

73 

25 

62.2 

76.3 

30 

64 

80 

40 

68 

86.5 

t>  . 

Gms.  Solution.* 

cc.  Solution  (L.). 

So 

71 

-  93 

60 

74-5 

IOO 

70 

106 

80 

82  " 

•  •  • 

IOO 

89 

132  m.  pt.  loo 

*  Average  curve  from  results  of  K.,  M.,  and  H. 

ioo  gms.  95%  formic  acid  dissolve  22.42  gms.  malonic  acid  at  19.5°.  (Aschan,  1913.) 


399 


MALONIC   ACID 


Alcohol. 


Methyl  Alcohol       - 


SOLUBILITY  OF  MALONIC  ACID  IN  ALCOHOLS. 

(Timofeiew,  1894.) 
Gms. 
A.Q  OH.2(C^OOri)j  Alpnhftl 

^Sa^Sol!"8' 

42 . 7        Ethyl  Alcohol 
43 . 5        Propyl  Alcohol 


CH,( 
perioo 


Ethyl  Alcohol 


-i5 
o 

+19 

+19.5 

-18.5 

-15 

o 
+  19 


47-3 

52.5 

53-3 

30 

30.7 

35-3 

40.1 


Isobutyl  Alcohol 


+  19-5 
-18.5 
-IS 
o 

+19 
+  19-5 
o 

19 


Sat.  Sol. 
41-3 
19.5 
20.2 

24-3 
29-5 
30-7 
17.5 
21.2 


SOLUBILITY  OF  MALONIC  ACID  IN  ETHER. 

(Klobbie,  1897.) 


t°. 

Cms.  CH,(COOH). 
per  loo  Gms. 

t°. 

Gms.  CH2(COOH), 
per  100  Gms. 

Solution. 

Solution. 

0 

6.25 

30 

10.5 

IP 

7-74 

80 

33 

20 

9 

00 

39 

25 

9-7 

Gms.  CH2(COOH), 

t8. 

per  100  Gms. 
Solution. 

100 

46 

no 

56 

1  20 

70 

132  m. 

pt.          100 

100  ems.  saturated  solution  of  malonic  acid  in  pyridine  contain  14.6  gms.  at  26°. 

(Holty,  1905.) 

SOLUBILITY  OF  SUBSTITUTED  MALONIC  ACIDS  IN  WATER. 

(Lamouroux,  1899.) 
Gms.  per  100  cc.  Saturated  Aqueous  Solution. 


O 
15 
25 
30 

DISTRIBUTION  OF  MALONIC  ACID  BETWEEN  ETHER  AND  WATER  AT  25°. 

(Chandler,  1908.) 
Mols.  Acid  per  Liter. 


Malonic 

Methyl 
Malonic 

Ethyl 
Malonic 

«  Propyl 
Malonic 

n  Butyl 
Malonic 

Iso  Amyl 
Malonic 

Acid. 

Acid. 

Acid. 

Acid. 

Acid. 

Acid. 

61.1 

44-3 

52.8 

45-6 

ii.  6 

38.5 

70.2 

58.5 

63-6 

60.  i 

30.4 

51-8 

76.3 

67.9 

71.2 

70 

43-8 

79-3 

92.6 

91.5 

90.8 

94-4 

79-3 

83-4 

H2O  Layer. 
0.1478 
O.II2I 
0.0862 
0.0331 

MANDELIC  ACID 


Solvent. 

Water 


Ether  Layer. 
0.0135 
O.OIO2 
0.0076 
O.OO27 


Coef. 


Cone.  H2O 


10.94 
11.07 
11.28 
12.22 


Dist.  Coef. 

corrected  for 

lonization. 

9.86 

9-79 
9.86 
9.82 


Methyl  Alcohol 
«  «( 

Ethyl  Alcohol 
«  « 

Propyl  Alcohol 

«  « 

95%  Formic  Acid 


C6H5.CH(OH)COOH  i  and  d. 
SOLUBILITY  IN  SEVERAL  SOLVENTS. 

t»  Gms.  C«H5CHOHCOOH 

per  iQOiGms.  Sat.  Sol. 
15.95     (inactive  acid) 
19.17    (dextroacid) 
5I.I       (inactive  acid) 


20 

20 
O 

16.5 
O 

16.5 

o 

16.5 
19 


64.9 
46.7 

53-6 
35 
43 
40 


Authority. 

(Schlossberg,  1900.) 
« 

(Timofeiew,  1894.) 


(Aschan,  1913.) 


MANDELIC  ACID 


400 


FREEZING-POINT  DATA  (Solubility,  see  footnote,  p.  i)  ARE  GIVEN  FOR  THE  FOL- 
LOWING MIXTURES  OF  MANDELIC  ACID  AND  OTHER  COMPOUNDS. 


d  Mandelic  Acid  +  /  Mandelic  Acid 


(Adrian!,  1900.) 
(Centnerszwer,  1899.) 


«          i    /  «  « 

Methylester  +  I  Mandelic  Methylester 

Isobutylester  +  /  Mandelic  Isobutylester 

Acid  +  Dimethylpyrone 

/  Menthylester  +  d  Mandelic  /  Menthylester    (Findky  and  Hickmans,  1907. 


(Kendall,  1914.) 


Menthyl  MANDELATES. 

SOLUBILITY  IN  ETHYL  ALCOHOL. 

(Findlay  and  Hickmans,  1909.) 


Solvent.              t°. 

Gms. 
Gms. 

per  100 
Solvent. 

Solid 
Phase. 

Solvent.          t°. 

Gms.  per  100 
Gms.  Solvent. 

Solid 
Phase. 

L. 

D. 

L. 

D. 

80% 

Alcohol 

35 

1.  08 

D 

80%  Alcohol     10 

0.287 

D 

«* 

35 

3 

.19 

L 

IO 

0-595 

L 

it 

35 

0 

.80 

0.80 

R 

IO 

0.184 

0.184 

R 

tt 

35 

0 

•544 

i-35 

D+R 

IO 

0.404 

o.  291 

D+R 

tt 

35 

2 

•83 

0.60 

L+R 

IO 

0.505 

0.088 

L+R 

" 

25 

0-595 

D 

Abs.  ^ 

Jcohol      o 

1.  06 

D 

tt 

25 

I 

.64 

L 

0 

J-93 

L 

it 

25 

0 

.448 

0.448 

R 

'               o 

0.625 

0.625 

R 

tt 

25 

o 

.321 

0.882 

D+R 

o 

0-535 

0.915 

D+R 

tt 

25 

I 

.192 

0.267 

L+R 

o 

1.03 

0-54 

L+R 

*  d&  =  0.8517. 

D  =1  menthyl  d  mandelate,  [a]^17-5  =  —9.45°  in  alcohol. 
L  =  I  menthyl  /  mandelate  [ct]Dzo  =  — 140.92°  in  alcohol. 
R  =  I  menthyl  r-mandelate  [a]^11-3  =  —75.03  in  alcohol. 

MANGANESE  BORATE   MnH4(BO,)2. 

SOLUBILITY  IN  WATER  AND  IN  AQUEOUS  SALT  SOLUTIONS. 

(Hartley  and  Ramage  —  J.  Ch.  Soc.  63,  137,  '93.) 

per  Liter  in  Solutions  of: 


f. 

H20  + 
trace 
Na2S04. 

Na2SO<              Na2S04 
(0.2  Gms.          (20  Gms. 
per  Liter).         per  Liter). 

NaCl 
(20  Gms. 
per  Liter). 

CaClj 
(20  Gms. 
per  Liter). 

14 

0-94 

I  .7 

. 

.  . 

18 

.  .  . 

.  .  . 

0 

•77 

I  .31 

2 

.91 

40 

0.50 

0.69(52°) 

O 

•65 

.  .  . 

2 

•44 

60 

O 

•36 

0.6o 

2 

•25 

80 

0.08 

... 

0 

.12 

0.29 

I 

MANGANESE  BROMIDE   MnBr2. 

SOLUBILITY  IN  WATER. 

(Etard,  1894.) 


t«. 

Gms.  MnBrj 
per  100  Gms. 
Solution. 

Solid 
Phase. 

—  20 

52-3          ] 

SdnBra^H 

—  10 

O 
10 

54-2 
56.0 

57-6 

M 

20 

25 
30 

59-5 
60.2 
61.1 

M 

M 

t-. 

Gms.  MnBr3 
per  loo  Gms. 
Solution. 

Solid 
Phase. 

40 

62.8 

MnBr2.4HaO 

50 

64.5 

• 

60 

66.3 

» 

70 

68.0 

M 

80 

69.2 

MnBr.2HsO 

90 

69.3 

" 

IOO 

69-5 

•i 

us  MnCl2  p 

er  ioo  Grams 

Mols.  MnCJ3              Solid 
per  ioo  Mols.  H2O.       Phase. 

Water. 

Solution. 

53-8 

35-o 

MnCl£.4lIj 

58-7 

37-o 

" 

63-4 

38.8 

... 

68.1 

40-5 

it 

73-9 

42-5 

M 

77.18 

43-55 

II.OS 

80.71 

44.68 

n-55                ** 

88.59 

46.96 

12.69               " 

98.15 

49-53 

14.05 

105.4 

51  .33 

15.10 

108.6 

52.06 

15-55           MnCl2.2H. 

no.  6 

52-52 

I5-85 

112.7 

52.98 

16.14 

114.1 

53-2 

•    .    •                                                " 

iiS-3 

53-5 

•    •    •                                                ** 

118.8 

54-3 

... 

II9-5 

55-o 

...                                                 M 

401  MANGANESE  CARBONATE 

MANGANESE   CARBONATE  MnCO8. 

One  liter  water  dissolves  5.659.io~4  mols.  MnCOs  =  0.065  Sm-  at  25°- 

(Ageno  and  Valla,  1911.) 

MANGANESE  CHLORIDE  MnCl2. 

SOLUBILITY  IN  WATER. 

(Etard;  Dawson  and  Williams  —  Z.  physik.  Chem.  31,  63,  '99.) 

4.  •  Sp.  Gr.  of 

*  •  Solutions. 

—  20 

—  10 

O 

+  10 
20 

25         I .4991 
30        I-5049 

40  L5348 

50  1-5744 
57.65         1.6097 

60  i.  6108 

70  1-6134 
80 
90 

100 
120 

I4O 

One  liter  of  water  dissolves  87.0  grams  MnCl2.    One  liter  of  sat.  HC1 
dissolves  19.0  grams  MnCl,  at  12°.  (Ditte  —  Compt.  rend.  92, 242,  '81.) 

EQUILIBRIUM  IN  THE  SYSTEM  MANGANESE  CHLORIDE,  POTASSIUM  CHLORIDE 
AND  WATER.    (Suss,  1913.) 

Cms  per  100  Gnu.  Gms.  per  100  Gms. 

f.             Sat.  Sol.              Solid  Phase.           t°.  Sat.  Sol.  Solid  Phase. 

MnClj.       KC1.  MnCl,.        KC1. 

6          40.23       ...     MnCWHjO  52.8  50.14       6.0lMnCl2.4H2O+MnCl2.2H2O+i.i.2 

6          35-94       9-41     "  +I.I.2+KC1  58.3  51.72       ...         MnCl2.4H2O+MnCl2.2H2O 

6             ...        23.06             KC1  62.6  51.86       ...                    MnCl2.2H2O 

28.4     44.46       ...     MnClz^H-jO  62.6  49.95        6.67                          "  -fi.i.2 

28.4     43.28       8.66     "  +1.1.2  62.6  44.05      12.49       i.i.2+MnCl2.2KCl.3H2O 

28.4     38.65      13.79     "  +I.2.2+KC1  62.6  36,85      18.77  MnCl,.2KC1.2H2O+MnCl,.4KCl 

28.4        ...        26.91            KC1  62.6  ...        31.57                        KC1 

1.1.2  =  MnCkKC1.2H2O.      1.2.2  =  MnCl22KC1.2H2O 

100  cc.  anhydrous  hydrazine  dissolve  13  gms.  MnCl2  at  room  temp. 

(Welsh  and  Broderson,  1915). 

Fusion-point   data  for   MnCl2  +  SnCl2   (Sandonnini,   1911),    MnCl2  +  SnClj 
(Sandonnini  and  Scarpa,  1911),  MnCl2  +  ZnCl2  (Sandonnini,  1912  and  1914). 

MANGANESE   CINNAMATE   (C6H6CH:CHCOO)2Mn. 

100  gms.  H2O  dissolve  0.26  gm.  manganese  cinnamate  at  26°.        (De  Jong,  1909.) 

MANGANESE  FLUOSILICATE   MnSiF6.6H2O. 

100  gms.  H2O  dissolve  140  gms.  salt  at  17.5°.     Sp.  Gr.  of  solution  =  1.448. 

(Stolba,  1883.) 
MANGANESE  HYDROXIDE   Mn(OH)2. 

One  liter  H2O  dissolves  2.I5.IO"6  gms.  mols.  Mn(OH)2  at  18°. 

(Sackur  and  Fritzmann,  1909.) 

One  liter  H2O  dissolves  2.10.10""*  gms.  mols.  Mn(OH2)  at  18°.          (Tamm,  1910.) 
The  determination  of  S.  &  F.  was  made  by  the  neutralization  method  of  Kuster, 
that  is,  by  determining  the  conductivity  minimum  on  adding  Ba(OH)2  to  MnSO< 
solution  and  calculating  the  Mn(OH)2  remaining  in  solution. 


MANGANESE  HYDROXIDE 


402 


SOLUBILITY  OF  MANGANESE  HYDROXIDE  IN  AQUEOUS  SOLUTIONS  OF 
ORGANIC  SALTS. 

(Tamm,  1910.) 

(25  cc.  of  the  neutral  salt  solution  +  25  cc.  of  aqueous  suspension  of  Mn(OH)» 
were  shaken  different  lengths  of  time.     Temp,  not  stated.)  ^ 

100  cc.  sat.  solution  in  I  n  sodium  tartrate  solution  contain  0.052  gm. 
100  cc.  sat.  solution  in  I  n  sodium  malate  solution  contain  0.032  gm. 
IOO  cc.  sat.  solution  in  I  n  sodium  citrate  solution  contain  0.095  Sm* 

MANGANESE  IODOMERCURATE  3MnI2.5HgI2.2oH2O. 

A   saturated   solution   of    the   salt   in   water   at    17°   has 
1.4  MnI2.HgI2.io.22H2O  and  density  2.98. 

MANGANESE  NITRATE  Mn(NO3)2. 

SOLUBILITY  IN  WATER. 

(Funk  —  Wiss.  Abh.  p.  t.  Reichanstalt  3,  438,  'oo.) 


the    composition 
(Duboin,  1906.) 


to 

Gms.           Mols. 
Mn(N03)2  Mn(NO3)2                Solid 

• 

per  loo 
Gms.  Sol. 

per  loo                Phase. 
Mols.  H2O. 

-29 

42 

.29 

7 

.37      Mn(NO3)2.6H2O. 

-26 

43 

7 

•63 

—  21 

44 

•30 

8 

•  O                      " 

-16 

45 

•52 

8 

•4 

-  5 

48 

.88 

9 

.61 

o 

50 

•49 

10 

.2 

•fn 

54 

•50 

12 

.O                       " 

t  °. 

Gms. 
Mn(NO3)2 

Mols. 
Mn(N03)2 

Solid 

per  loo 
Gms.  Sol. 

per  loo 
Mols.H2O. 

Phase. 

18 

57-33 

13.5 

Mn(N03)2.6H20. 

25 

62.37 

I6.7 

" 

27 

65.66 

19.2 

Mn(N03)2.3H20. 

29 

66.99 

2O-4 

** 

30 

67.38 

20-7 

" 

34 

7I-31 

24-9 

H 

35-5 

76.82 

33-3 

M 

Sp.  Gr.  of  solution  saturated  at  18°  =  1.624. 
The  Eutec  is  at  —36°  and  40.5  gms.  Mn(NO3)2  per  100  gms.  Sat.  Sol. 

MANGANESE   OXALATE   MnC2O4.2H2O. 

SOLUBILITY  IN  AQUEOUS  SOLUTIONS  AT  25°. 

(Hauser  and  Wirth,  1909.) 

In  Oxalic  Acid     In  Ammonium  Oxalate  In  Sulfuric  Acid 

Solutions.  Solutions.  Solutions. 

Per  1000  Gms.  Sat.  Sol.     Per  1000  Gms.  Sat.  Sol.        Per  1000  Gms.  Sat.  Sol. 


G.  Mols. 

Gms. 

G. 

Mols. 

Gms. 

Normality 

Gms.                  Solid  Phase. 

(COOH)2. 

Mn(COO)2.(NH<)2(COO)5 

.  Mn(COO)2. 

H2S04. 

Mn(COO)2. 

O 

O 

.312 

O, 

005 

O 

•338 

O, 

025 

I 

.825           MnCA.2H2O 

0 

.0125 

0 

•759 

0 

.025 

0 

•479 

0 

.24 

8 

.850 

0 

.025 

0 

•930 

0, 

,050 

0 

.761 

I 

25 

•955 

0 

.050 

I 

.080 

O, 

125 

I 

.789 

2 

•389 

51 

.080 

o 

•125 

I 

•396 

O, 

245 

3 

.970 

2 

.987 

60 

.  109  MnCA.2H20+(COOH), 

0 

•  25 

I 

.708 

0, 

245 

4 

.005 

o 

•952 

73 

.200 

0 

•49 

2 

.081 

o, 

,28l 

4 

.650 

4 

.500 

82 

.401                      " 

Results  are  also  given  for  the  solubility  of  MnC2O4.2H2O  in  aq.  solutions  of 
H2SO4  containing  also  about  0.25  gm.  mols.  free  oxalic  acid  per  liter  at  25° 

MANGANESE   OXIDE   MnO. 

Fusion-point  data  for  mixtures  of  manganese  oxide  and  silicic  acid  are  given  by 
Doernickel,  1907. 

MANGANESE   (Hypo)   PHOSPHITE   Mn(PH2O2)2H2O. 

100  gms.  H2O  dissolve  15.15  gms.  salt  at  25°,  and  16.6  gms.  at  b.  pt.     (U.  S.  P.) 

MANGANESE   SILICATE   MnSiO3. 

Fusion-point  data  for  mixtures  of  manganese  silicate  and  titanate  are  given  by 
Smolensky,  1911-12. 


403 


MANGANESE   SULFATE 


MANGANESE  SULFATE  MnSO4. 

SOLUBILITY  IN  WATER. 


(Cottrell  —  J.  Physic.  Ch.  4,  651,  '01;  Richards  and  Fraprie  —  Am.  Ch.  J.  26,  77,  *oi.    The  results 
of  Lmebarger  —  Am.  Ch.  J.  15,  225,  '93,  were  shown  to  be  incorrect  by  Cottrell,  and  this  conclusion 
was  confirmed  by  R.  and  F.) 

Grams  MnSO4  per                                                         Grams  MnSO4  per 
t».                zoo  Gms.               Solid  Phase.                t°.                  100  Cms.             Solid  Phase 

J   Water. 

Solution. 

Water. 

Solution. 

—  10 

47 

.96 

32 

.40      MnS04.7H20 

16 

63 

•94 

38 

•99 

MnS044H20 

0 

53 

•23 

34 

•73 

18, 

5 

64 

.19 

39 

.10 

" 

5 

56 

.24 

35 

•99 

25 

65 

•32 

39 

•53 

44 

9 

59 

•33 

37 

.24 

3° 

66 

•44 

39 

•93 

'* 

12 

61 

•77 

38 

.19 

39 

9 

68 

.81 

40 

•77 

M 

14-3 

63 

•93 

39.00 

49 

9 

72 

•63 

42 

.08 

44 

5 

58 

.06 

36 

.  69      MnSO4.sH2O 

41 

4 

60 

•87 

37 

.84 

MnSO4.H2O 

9 

59 

.19 

.18 

5° 

58 

•17 

36 

.76 

« 

15 

61 

.08 

37 

.91 

60 

55 

.0 

35 

•49 

44 

25 

64 

.78 

39 

.31 

70 

52 

.0 

34 

.22 

44 

67 

.76 

40 

.38 

80 

48 

.0 

32 

•43 

44 

35-5 

71 

.61 

4i 

•74 

90 

42 

•5 

29 

•83 

44 

IOO 

34 

.0 

24 

.24 

44 

SOLUBILITY  OF  MANGANESE  SULFATE,  COPPER  SULFATE  MIXED  CRYSTALS 
IN  WATER  AT  18°. 

(Stortenbecker,  1900.) 


Mola.  per  TOO  Mols. 
H,0. 

Mol.  per  cent 
Cuin: 

Mols.  per  100  Mols. 
H20. 

Mol.  per  cent 
Cuin: 

"Cu. 

Mn.  " 

Solution. 

Crystals. 

'Cu. 

Mn.  " 

Solution. 

Crystals. 

Solid  Phase,  CuMnSO4.sH2O, 

Triclinic. 

Solid  Phase, 

CuMnSO4.sH2O. 

Triclinic. 

2.282 

O 

IOO 

IOO 

[0-73 

6. 

37 

IO 

•27 

10.5] 

00 

•5 

. 

. 

5 

.0 

4.9 

2.23 

0-44 

83 

•5 

0-34 

7- 

03 

4 

.60 

74 

.1 

97 

•3 

. 

2 

•31 

2-15 

.  i  . 

57 

•7 

95 

.1 

7- 

375 

0 

.0 

o.o 

... 

... 

•  o 

81 

•3 

Solid 

Phase 

.  CuMnSO4.  Monoclinic.  jH- 

i-54 

3-76 

4.70 

29 

26 

21 

.0 

.1 

.8 

70 

•4 

[1.06 

5- 

58 

20 
15 

•4 
•9 

28.2* 
23-5] 

21 
20 

.2 
•  O 

42 
34 

.6 

•4 

[o-73 

6. 

37 

12 
10 

•45 
•27 

20.8 

16.0] 

[1.06 

5-58 

15 
13 

•9 
•9 

\J  • 

22 

15 

A 

±8 

4 

0 

.60 
•  o 

5.8* 
o.o 

*  Indicates  meta  stabil  points. 

CuMnSO4>5H2O  =  100-90.8  and  2.11-0  mol.  per  cent  Cu. 
=  37.8-4.92  mol.  per  cent  Cu. 


SOLUBILITY  OF  MANGANESE  SULFATE  IN  GLYCOL. 
:ioo  gms.  saturated  solution  contain  0.5  gm.  MnSO*-.  (de  Coninck,  1905.) 


MANGANESE  SULFATE 


404 


SOLUBILITY  OF  MANGANESE  SULFATE  IN  AQUEOUS  SOLUTIONS  OF 
AMMONIUM  SULFATE  AT  25°  AND  50°    AND  VICE  VERSA. 

(Schreinemakers,  1909.) 


Results  at  25°. 


Results  at  50°. 


Cms.  per  100  Gins. 
Sat.  Sol. 


MnSO4. 

39.3 

38.49 

33.44 

22.06 

9.O2 

2.91 

1.75 

1.77 

O 

D6  = 


Solid  Phase. 


MnSO4.sH2O 

"      +D, 
D, 


O 

3.64 

4.91 

9.65 
20.36 
37-42 
42.58 
43.  24 
43-4 

MnSO4.(NH4)2SO4.6H2O. 


+(NH4)2S04 
(NH4)2SO4 


Gms.  per 

ioo  Gms. 

Sat 

.Sol. 

Solid  Phase. 

MnSO4. 

(NH^SO, 

36.26 

O 

,             MnSd.HjO 

35-35 

2-95 

"  +DM 

30.57 

5-14 

DM 

16.86 

17.62 

" 

6.92 

35.98 

" 

6.29 

39-71 

" 

5-70 

43-24 

3-49 

44.02 

(NH^O, 

0 

45-7 

" 

D2.i  = 

=  (MnSO4 

)2(NH4)2S04. 

SOLUBILITY  OF  MANGANESE  SULFATE  IN  AQUEOUS  SOLUTIONS  OF  SODIUM 
SULFATE  AT  35°  AND  VICE  VERSA. 

(Schreinemakers  and  Provije,  1913.) 


Gms.  per  ioo  Gms. 
Sat.  Sol. 

MnSO4. 

NajSO,. 

39-45 

0 

33-92 

5-23 

33-06 

7-97 

32.92 

7.42 

3L05 

9.20 

27.67 

10.76 

22.14 

14.28 

14.58 

20.01 

Solid  Phase. 


MnSO4.HjO 


+(MnS04)9.(Na2S04)IO 


(MnS04)9.(Na2S04)io 


Gmis.  per  too  Gms. 
Sat.  Sol. 

MnSO4. 

Na2SO4. 

13.96 

21.91 

12.19 

22.49 

10.45 

23-4I 

7-43 

26.58 

5-69 

29.31 

5-n 

30.52 

2.96 

31-33 

0 

33 

;  Solid  Phase. 
(MnSO4)9.(NajSO4)io 


+MnS04(Na2SO4), 


+Na2S04 


Data  for  the  solubility  of  mix  crystals  of  manganese  and  zinc  sulfates  between 
o°  and  39°  are  given  by  Sahmen,  1905-06. 


SOLUBILITY  OF  MANGANESE  SULFATE  IN  AQUEOUS  ETHYL  ALCOHOL. 

(Schreinemakers,  1909;  Schreinemakers>nd  Deuse,  1912.) 

.   .'    Results  at  50°. 

Gms.  per  ioo  Gms.  Sat.  Sol. 
MnS04. 
36.26 
28.12 
18-75 


Results  at  25°. 

Gms.  per  ioo  Gms.  Sat.  Sol. 

QHjOH.          MnSO4. 

O  39-3 

6.8l  33-72- 

liquid  layers  separate  here 

53-09  1-23 

57.39  0.56 

76.70          o 


Solid  Phase. 
MnS04.SH20 


MnS04.H20 


C2H5OH. 
O 
6.67 

16.02 

22.63 
36.47 


Solid  Phase. 
MnS04.H;O 


12-54 
4.12 


Composition  of  the  liquid  layers. 

Water  rich  Layer.  QH5OH  rich  Layer. 


The  following  reciprocally  saturated  meta- 
stable  solutions  were  obtained  at  50°. 


Water  rich  Layer. 


C2H5OH  rich  Layer. 


%C2H5OH. 

%MnS04. 

•%QH6OH. 

%MnSO4. 

%  C2H5OH. 

%  MnS04. 

%  C2H5OH. 

%  MnS04." 

6.81 

33-72* 

53-09 

1.23* 

5-68 

34-95 

53.64 

0.97 

8.48 

31.51 

49.76 

1.83 

7.69 

30.99 

45.83 

2.19 

15.02 

22.  6l 

32.75 

8.01 

8.70 

29.20 

41-93 

11.85 

24.84 

35-15 

5-95 

*  These  liquids  in  contact  with  MnSO4.sH2O. 

Similar  data  are  also  given  for  30°  and  for  35°.     Both  stable  and  metastable 
liquid  pairs  were  obtained  at  these  intermediate  temperatures. 
Additional  data  for  this  system  are  also  given  by  Cuno,  1908. 


405  MANGANESE   SULFATE 

SOLUBILITY  OF  MANGANESE  SULFATE  IN  AQUEOUS  ETHYL  ALCOHOL  (CON.). 
Composition  of  the  conjugated  liquids  in  contact  with  excess  of  solid  salt. 

C2H5OH  rich  Layer.  Aqueous  rich  Layer. 

%C2H5OH.  %  MnS04".  %  QHjOH.  %  MnSO4'. 

10  37.06  5.44  13-78  25.25          MnSO4.sH2O 

15  44-56  2.79  9.25  29.79 

17.  47-11  2.22  8.53  30-88 

21  53.55  i. 10  6.10  35.05 

25  53-09  1-23  6-8i  33-72 

30  45.20  2.49  8.69  30.15          MnSO4.H2O 

31  43.90  2.74  8.47  30.10 
35  41.71  3.44  9.24  28.61 
37  38-26  4.84  11.03  26.47 

41  34.01  5.86  11.93  24.97 

42  32-37  6.89  13.57  23.09 

43  3*-42  8.51  14.33  22.01 

Data  for  the  solubility  of  manganese  sulfate  and  potassium  iodate  in  methyl 
alcohol  are  given  by  Karplus,  1907. 

SOLUBILITY  OF  MANGANESE  SULFATE  IN  AQUEOUS  ETHYL  AND  PROPYL 
ALCOHOL  SOLUTIONS  AT  20°. 

(Linebarger,  1892;  Snell,  1898.) 

Gms.  MnS04  per  100  Gms.  Aq. 
Ethyl  Ale.          Propyl  Ale. 

3-3  i-9 

2.2  1.4 

1.4  i.i 

100  cc.  anhydrous  hydrazine  dissolve  about  I  gm.  MnSO4  at  room  temp. 

(Welsh  and  Broderson,  1915.) 

Fusion-point  data  for  mixtures  of  MnSO4  +  K2SO4,  and  MnSO4  +  Na2SO4  are 
given  by  Calcagni  and  Marotta,  1914. 

MANGANESE   SULFIDE   MnS. 

One  liter  sat.  solution  in  water  contains  7i.6.io~6  mols.  MnS  =  0.00623  gm. 
per  liter  at  18°  by  conductivity  method.    (Weigel,  1907;  see  also  Bruner  and  Zawadzki,  1909.) 

MANGANESE   Potassium  VANADATE   MnKV6Oi4.8H2O. 

100  gms.  H2O  dissolve  1.7  gms.  salt  at  18°.  (Radan,  1889.) 

MANNITOL  CH2OH(CHOH)4CH2OH. 

SOLUBILITY  IN  WATER. 

(Findlay,  1902.) 

to     Gms.  CH2OH(CHOH)4CH2OH  *„     Gms.  CH2OH(CHOH)4CH2OH 

per  roo  Gms.  H2O.  per  100  Gms.  H2O. 

o  7-59  40  35-4 

IO  1 1  . 63  (13-94  gms.  Campetti,  1901)'  $O  .  8  46  . 69 

2O  Z7-71  (18.98  gms.  Campetti,  1901)  60  6o.OI 

24,5  20.96  70  74-5 

30  25.4  80  91.5 

35.8  29.93  I0°  I33-I 

100  gms.  alcohol,  Sp.  Gr.  0.905,  dissolve  1 .56  gms.  mannitol  at  14°.  (Krusemann,  1876.) 
Data  for  the  solubility  of  mannitol  at  high  pressures  are  given  by  Cohen, 

Inouye  and  Euwen,  1910. 

100  gms.  sat.  sol.  in  pyridine  contain  0.47  gm.  mannitol  at  26°.  (Holty,  1905.) 
100  gms.  aq.  50%  pyridine  dissolve  2.46  gms.  mannitol  at  20-25°.  (Dehn,  1917.) 
Data  for  the  ternary  systems  mannitol  -f-  succinic  acid  nitrile  -f-  water  and 

mannitol  +  triethylamine  +  water,  are  given  by  Timmermans,  1907. 


Cone,  of  Alcohol 

Gms.  MnS04  per 

zoo  Gms.  Aq. 

Cone,  of  Alcohol 

in  Wt.  per  cent. 

Ethyl  Ale. 

Propyl  Ale. 

in  Wt.  per  cent. 

34 

9-5 

6 

44 

36 

7.2 

4.6 

48 

38 

5-8 

3-5 

52 

40 

4-7 

2.8 

MERCURY  ACETATE 


406 


MERCURY  ACETATE  (ic)  Hg(C2H3O2)2,  (ous)  Hg2(C2H3O2)2. 

100  gms.  water  dissolve  25  gms.  mercuric  acetate  at  10°. 

loo  gms.  water  dissolve  0.75  gm.  mercurous  acetate  at  13°. 

loo  cc.  anhydrous  hydrazine  dissolve  about  2  gms.  mercurous  acetate  at  room 
temp,  with  precipitation  of  Hg.  (Welsh  and  Broderson,  1915.) 

MERCURY  BENZOATE   (ic)    (C6H6COO)2Hg.?H2O. 

100  gms.  H2O  dissolve  1.2  gms.  mercuric  benzoate  at  15°  and  2.5  gms.  at  100°. 

(Tarugiand  Checchi,  1901.) 


(ic)   HgBr2. 
SOLUBILITY  IN  WATER. 


MERCURY  BROMIDE 


Q  I  .06  (Lassaigne,  1876.) 

25     .  0.6l  (SherrUl,  1903.) 

ICO  2O-25  (Lassaigne.) 

Mercurous  bromide.    One  liter  sat.  aq.  solution  contains  0.000039  Sm-  Hg2Bri 
at  25°.  (Sherrill,  1903.) 

EQUILIBRIUM  IN  THE  SYSTEM  MERCURIC  BROMIDE,  AMMONIA,  WATER  AT  8°-io°. 

(Gaudechon,  1910.) 

The  mixtures  were  shaken  intermittently  for  21-48  hrs.     Both  the  clear  sat. 
solution  and  the  separated  and  dried  solid  phases  were  analyzed. 


Initial  Mixture. 
Gms.  Mols.  per  Liter. 

Sat.  Solution. 
Gms.  Atoms,  per  Liter. 

Solid  Phase 

HgBr2. 

NH3. 

NH«Br. 

Hg. 

Br. 

N. 

OOIIQ  Jrnasc. 

o, 

0125 

o. 

0250 

o 

trace 

0. 

0154 

0.0185 

(NHg2Br)4HgBr2 

0 

0166 

0. 

0332 

o 

0.00032 

0. 

0172 

O.O2O2 

36% 

"  +64%  NHg2BrNH4Br 

o 

,025 

o 

050 

0 

0.00078 

0. 

0241 

O.O25I 

NH&Br.NH^Br 

0 

.050 

0 

,100 

o 

0.0019 

0. 

0525 

0.0514 

o 

.0125 

o 

,025 

o. 

0375 

0.00178 

o. 

0497 

0.0497 

" 

o 

.025 

o 

.050 

0. 

075 

0.0041 

0.103 

0.108 

« 

o 

.0328 

o 

.0656 

0 

0984 

0.0061 

o. 

133 

0-133 

93% 

"  +6%  NHgBr.3NH4Br 

0 

•0365 

0 

•073 

0 

1095 

0.0060 

0. 

132 

0.133 

36% 

"  +64%  NHgBr.3NH«Br 

0 

.050 

0 

.  IOO 

o 

150 

0.007 

o. 

170 

o.  169 

NHg2Br.3NH«Br 

0 

.  IOO 

0 

.200 

o 

.300 

0.0124 

o. 

333 

0.338 

" 

o 

.ci8o 

o 

.036 

o, 

.01875 

O.OOI 

0.0315 

0.0318 

NHgjBr.NI^Br 

0.050 

0.100 

0.006 

0.0057 

0. 

1172 

0.1178 

" 

0 

.050 

o 

.100 

o 

150 

0.0071 

0. 

169 

0.168 

NHg2Br.3NH4Br 

0 

.  IOO 

0 

.200 

o 

.160 

0.0083 

0. 

184 

0.187 

" 

0 

•  125 

0 

.250 

o 

.306 

0.0160 

o. 

393 

« 

SOLUBILITY  OF  MERCURIC  BROMIDE  IN  AQUEOUS  SALT  SOLUTIONS  AT  25°. 

(Herz  and  Paul,  1913.) 


(The  mixtures  were  constantly  agitated  for  eight  days.) 
In  Aq.  BaBr2.      In  Aq.  CaBr2.      In  Aq.  KBr.       In  Aq.  NaBr. 

Mols.  per  Liter.          Mols.  per  Liter.         Mols.  per  Liter.         Mols.  per  Liter. 

In  Aq.  SrBr2. 

Mols.  per  Liter. 

BaBr2. 
0 
0.274 
0.396 

0-579 
1.096 

HgBr2. 
0.017 
0-370 
0.540 

0-759 
1.478 

CaBr2. 
0.072 
0.645 
1.892 
2.479 
3-754 

HgBr2. 
o.  117 
0.676 
1.358 
2.766 
3.666 

"[KBr. 
0 
O.  209 
0.770 
2.380 
3-470 

HgBr2.' 
0.017 
0.098 
0.472 
1.360 
1.930 

NaBr. 
O.II8 
0.596 
1.142 
2.448 
5.246 

HgBr2. 
0.078 
0.285 
0.540 
1.276 
2.306 

SrBr2. 
0.062 
0.328 
0.668 
1.401 
1.872 

HgBr2. 
0.104 
0.471 
0.902 
1.770 
2.238 

The  following  slightly  higher  results  for  KBr  solutions  are  given  by  Sherrill 
(1903). 

Mols.  KBr  per  liter       o  0.05      o.io      0.5          0.866     234 

Mols.  HgBr2  per  liter    0.017     O-O55     0.088     0.0359     0.611     1.407     2.096     2.339 

Data  for  equilibrium  in  the  system  HgBr2  +  KOH  +  H20  at  25°  are  given  by 
Herz  (1910). 


407 


MERCURY  BROMIDE 


SOLUBILITY  OF  MERCURIC  BROMIDE  IN  AQUEOUS  SOLUTIONS  OF  METYHL 
ALCOHOL,  ETHYL  ALCOHOL  AND  OF  ETHYL  ACETATE  AT  25°. 

(Herz  and  Anders,  1907.) 

In  Aq.  Methyl  Alcohol.        In  Aq.  Ethyl  Alcohol.        In  Aq.  Ethyl  Acetate. 


wt.  % 

CH,OH 
in 

Sat  Sr.1 

Gms. 
HgBr2  per 

IOO  CC. 

Wt   °7 
in 

.                 Gms.            Wt.  % 
d»foi     HgBr.perCHjCC^QHj 
Sat.  Sol.     ioo  cc.               in 

Solvent. 

Sat.  Sol. 

Solvent. 

Sat.  Sol. 

Solvent. 

10.6 

o 

9857 

0.72 

O 

I 

.0022 

0.6o 

0 

30.77 

o 

9588 

1.29 

20, 

18 

0 

.9717 

0.67 

4 

•39 

47.06 

o 

94oi 

2.52 

40, 

69 

0 

-9435 

i-59 

96 

.76 

64 

o 

9386 

6.85 

70. 

01 

0 

.9214 

6.58 

IOO 

78.05 

o 

9744 

14.66 

IOO 

0 

•9873 

22.81 

IOO 

I, 

2275 

50.25 

loo  gms. 

sat.  sol.  in  95% 

CjHftOH 

(di6  = 

0.8126) 

contain  i 

0°,  16.53 

gms.  at 

25    and  22.63  Sms 

i.  at  50°. 

<**50f 

Sat.  Sol. 

I.OO22 
I.OOlS 
I.II59 
I.OII3 


Gms. 
HgBr2  per 

IOO  CC. 

Sat.  Sol. 
0.6o 

0-574 
26.69 


(Reinders,  1900.) 


SOLUBILITY  OF  MERCURIC  BROMIDE  IN  ALCOHOLS. 

(Timofeiew,  1894.) 


In  Methyl  Alcohol.      In  Ethyl  Alcohol.     In  Propyl  Alcohol.    In  Isobutyl  Alcohol 


t°. 

Gms.  HgBr2 
per  ioo  Gms. 

t°. 

Gms.  HgBr2 
per  ioo  Gms. 

r. 

Gms.  HgBr2 
per  ioo  Gms. 

to 

Gms.  HgBr2 
per  ioo  Gms. 

CHjOH. 

CjHsOH. 

C3H7OH. 

C4H,OH. 

0 

4LI5 

0 

25.2 

0 

14.6 

o 

4.6l 

10 

49-5 

10 

26.3 

10 

15-6 

10 

5^3 

19 

66.3 

19 

29.7 

19 

15-5 

23 

6.65 

22 

60.9 

39 

31-9 

39 

20.8 

39 

9-58 

39 

71  .3 

65 

44-5 

65 

31-3 

65 

15.80 

65 

90.8 

89 

66.9 

86.5 

42.7 

97 

139.1 

SOLUBILITY  OF  MERCURIC  BROMIDE  IN  MIXTURES  OF  ALCOHOLS  AT  25°. 


In  Mixtures  of  Methyl 

(Herz  and  Kuhn,  1908.) 
In  Mixtures  of  Methyl 

In  Mixtures  of  Ethyl  and 

and  Ethyl  Alcohols. 

and  Propyl  Alcohols. 

Propyl  Alcohols. 

%  CH,OH      d     of 

Gms. 
HgBr2  per 

%C,H7OH 

i 

f«of 

Gms. 
HgBr2  per 

%  C3H7OH 

<*¥of 

Gms. 
HgBr2  per 

Mixture.      Sat-  SoL 

IOO  CC. 

Sat.  Sol. 

Mixture. 

Sat:  Sol. 

IOO  CC. 

Sat.  Sol. 

Mixture. 

Sat.  Sol. 

IOO  CC. 

Sat.  Sol. 

0            0.9873 

22.8 

O 

I 

.227 

50.20 

O 

0.9873 

22.80 

4-37     0.9932 

23.1 

II.  II 

I 

•  1954 

47.28 

8.1 

o  .  9802 

22.25 

10.4 

.009 

25-4 

23-8 

I 

.1524 

41-53 

17-85 

0.9740 

21.  06 

41.02 

.080 

33-3 

65-2 

I 

•0257 

25-30 

56-6 

0.9487 

17.63 

80.69 

-185 

45-7 

91.8 

o 

•9437 

16.35 

88.6 

0.9269 

14.76 

84-77 

•193 

46.8 

93-75 

o 

.9368 

15-86 

91.2 

0.9239 

14.64 

9I-25 

.211 

48.6 

96.6 

0 

•9275 

14.66 

95-2 

0.9227 

14.06 

IOO 

.227 

50.2 

IOO 

o 

.9213 

I3.78 

IOO 

0.9213 

13.78 

SOLUBILITY  OF  MERCURIC  BROMIDE  IN  ORGANIC  SOLVENTS. 


In  Carbon  Disulfide. 

(Arctowski,  1894.) 


In  Other  Solvents  at  i8°-2O°. 
(Sulc.,  1900.) 

Gms.  HgBr 2 

Solvent.  Formula.       per  ioo  Gms. 

Solvent.. 

0.126 

0.679 

0.003 

2.3I 

2.34 

One  liter  benzene  dissolves  6.99  gms.  HgBr2  at  25°.  (Abegg  and  Shemll,  1903.) 


Gms.  HgBr2 
t°.        per  ioo  Gms.  t°. 
Solution. 

Gms.  HgBr2 
per  ioo  Gms. 
Solution. 

—  io     0.049     JS 

0.140 

—  5     0.068     20 

O.l87 

o     0.087     25 

0.232 

+  5     °-ioS    30 

0.274 

10        0.122 

Chloroform  CHC13 

Bromoform  CHBr3 

Carbon  Tetrachloride  CCU 
Ethyl  Bromide  C2H5Br 

Ethylene  Dibromide 


MERCURY  BROMIDE  408 

SOLUBILITY  OF  MERCURIC  BROMIDE  IN  AN  EQUIMOLECULAR  MIXTURE  OF 
ETHYL  ALCOHOL  AND  BENZENE.    (Dukdski,  1907.) 

t°.  o.          10.       20.      30.         40.          50.       60. 

Gms.  HgBr2  per  loo  Gms.  Sat.  Sol.    10.7     12     14     16     17.5     19    21 
100  gms.  of  sat.  sol.  in  acetone  at  25°  contain  34.76  gms.  HgBr2.       (Reinders,  1900.) 
SOLUBILITY  OF  MERCURIC  BROMIDE  IN  ANILINE.     (Staronka,  1910.) 

Gms.  Gms. 

«••       g&?   S?8S!       So*"  Phase.  f-         S&?    SJaST          "Id  Phase. 

C6H5NH2.  C6H5NH2. 

60          4  16.14    HgBr2.2C6HBNH2       IIO*          33.3        193.3     HgBr2.2C«H6NH2 


70  5.8  23.83 

80  8.3  35.04 

QO  12.2  53.80 

IOO  18.8  89.64 

105  23.2  116.9 


109 -7t  33-5  195  "  +HgBr2.CeH6NH, 

US  37.2  229.3         HgBr2.C8H6NH, 

120  42.3  283.8 

124  50  387.2 

123  55.4  480.9 


*  M.  pt.  f  Eutec. 

IOO  gms.  ethyl  acetate  dissolve  13.05  gms.  HgBr2  at  18°.  (Naumann,  1910.) 

IOO  gms.  methyl  acetate  dissolve  21.93  gms-  HgBr2  at  18°  (d18  sat.  sol.  =  1.090). 

(Naumann,  1909.) 

SOLUBILITY  OF  MERCURIC  BROMIDE  IN  PYRIDINE.    (Staronka,  1910.) 

Gms.  Gms. 


C5HSN.  C6H5N. 

10          5              24  HgBr2.2CsH6N     107*  39  291 .5  HgBr-j^CsHsN+HgBrz.CjHjN 

30          8             39-64  no  40.4  309                   HgBrz.CjHsN 

50       ii.  a        57-49  "              120  45.5  381.3                     " 

80        17.5         96.68  I23f  50  455-8 

IOO        22            128.5  I25  51  474-4             sHgBrj.aCBHjN 

no        24.5       147.8  130  54.2  539.4 

«8t     33-3       227-6  I34t  60  683.7 

no       35.5       250.8  133  64  810.4                      " 

*  Eutec.  f  m.  pt. 

SOLUBILITY  OF  MERCURIC  BROMIDE  IN  QUINOLINE.    (Staronka,  1910.) 

0.0  Mol.  %         Gms.  HgBr2  per  c  r  j  TJV, 

HgBr2?        loo  Gms   C^N.  Solld  Phase' 

88  4.4  12.85         HgBr2.2C9H7N 

in  8.9  27.28 

127  14.3  46.58 

134  17.6  61.16 

Data  for  the  solubility  of  mercuric  bromide  in  nitrobenzene,  in  p  nitrotoluene, 
in  m  nitrotoluene,  in  o  nitrotoluene  and  in  a  nitronaphthalene,  determined  by  the 
method  of  lowering  of  the  freezing-point,  are  given  by  Mascarelli,  1906,  and  Mas- 
carelli  and  Ascoli,  1907.  Data  for  HgBr2  +  Se  are  given  by  Olivari,  1912. 

DISTRIBUTION  OF  MERCURIC  BROMIDE  BETWEEN  WATER  AND  BENZENE 
(THIOPHENE  FREE)  AT  25°.    (Shemll,  1903.) 

Mols.  per  Liter.  Mols.  per  Liter. 

H20  Layer.         QH,  Layer".  H2O  Layer.     "      C.H6  Layer. 

0.017  0.194  0.876  0.00634  0.0715  0.89 

0.01147       0.1303  0.88  0.00394        0.0436  0.90 

0.00953       0.1074  0.89  0.00320        0.0353  °-9° 

e  Data  are  also  given  for  the  distribution  between  aqueous  potassium  iodide  solu- 
tions and  thiophene  free  benzene  at  25°. 

Data  for  the  solubility  of  mix  crystals  of  HgBr2  -f-  HgI2  in  acetone  at  25°  and 
in  ethyl  alcohol  of  di6  =  0,8126  =  95%  at  o°,  25°  and  50°  are  given  by  Reinders 
(1900).  In  the  case  of  acetone,  the  ratio  of  HgBr2  in  the  solution  increases  with 
increase  of  per  cent  of  HgBr2  in  the  solid  phase.  In  the  case  of  the  alcohol  solu- 
tions the  ratio  in  solution  does  not  show  such  regular  variations  with  change  of 
per  cent  of  MgBr2  in  the  solid  phase. 


409 


MERCURY  CHLORIDE 


MERCURY  CHLORIDE   (ic)   HgCl2,   (ous)   Hg2Cl2. 

SOLUBILITY  OF  MERCURIC  CHLORIDE  IN  WATER. 

Average  curve  from  results  of  Etard,  1894;  Foote,  1903;  Osaka,  1903-08; 
Herz  and  Paul,  1913;  Greenish  and  Smith,  1903;  Schreinemakers  and  Thonus, 
1912;  Sherrill,  1903;  Morse,  1902. 

to      Gms.  HgCl2  per 
'   ioo  Gms.  Sat.  Sol. 


o  3-5 

10  4.6 

15-5  5-3 

20  6.1 


1.047) 


f. 

Gms.  HgClj  per 
ioo  Gms.  Sat.  Sol. 

to           Gms.  HgClj  per 
ioo  Gms.  Sat.  SoL 

25 

3° 

6.9 

7-7 

80 
IOO 

23.1 

38 

40 
60 

9-3 
14 

120 

59 

78.5 

20 


SOLUBILITY  OF  MERCUROUS  CHLORIDE  IN  WATER. 


Gms.  Hg2Cl2 

per  100  Gms. 

Sat.  Sol. 


Authority. 


0.5     O .  OOOI4O  (Conductivity,  Kohlrausch,  1908.) 

l8          O.OOOO75  (Indirect,  Behrend,  1893.) 

1 8          O .  OOO2 1  (Conductivity,  Kohlrausch,  1908.) 

0 . 000038  (Ley  and  Heimbucher,  1904.) 


t". 

Gms.  Hg2Cl2 
per  100  Gms. 
Sat.  Sol. 

Authority. 

24.6 

O.OOO28 

(Kohlrausch,  1908.) 

25 

0.000047 

(Sherrill,  1903.) 

43 

O.OOO7O 

(Kohlrausch,  1908.) 

SOLUBILITY    OF    MERCURIC    CHLORIDE    IN   AQUEOUS    SOLUTIONS    OP 

SODIUM  CHLORIDE. 

(Homeyer  and  Ritsert  —  Pharm.  Ztg.  33,  738,  '88.) 


Per  cent  Concentration                                           3  ^™s' 

of  NaCl  Solutions.                'IS<> 

65° 

100° 

0.5                      10 

13 

44 

i.o                       14 

18 

48 

5.0               30 

36 

64 

10.  o                        58 

68 

no 

25.0                               120 

142 

196 

26.0  (saturated)  128 

152 

208 

SOLUBILITY    OF    MERCURIC    CHLORIDE    IN    AQUEOUS    SOLUTIONS    OP 

HYDROCHLORIC  ACID  AT: 
o°.  20-25°  (?). 

(Engel  —  Ann.  chim.  phys.  [6]  17,  362,  '89.)  (Ditte  —  Ibid.  [5]  22,  551,  '81.) 


{.  Mob.  per 
HC1. 

ioo  cc.  Sol. 
iHgCl. 

Gms.  pe 
HC1. 

r  ioo  cc.  Sol. 
HgCl2. 

Sp.  Gr.  of 

Solutions. 

Farts  riU 
per  ioo 
Parts  H2O. 

Parts  Hg( 
per  ioo 
Parts  Solu 

4-3 

9-7 

i-57 

13.11 

I.II7 

o.o 

6.8 

99 

19.8 

3.6l 

18.04 

1.238 

$•« 

46.8 

17.8 

35-5 

6.49 

32-44 

1.427 

IO.I 

73-7 

26.9 

55-6 

9.81 

49.04 

1.665 

13-8 

87.8 

32-25 

68.9 

II  .76 

58.80 

I  .$11 

21.  1 

127.4 

34-25 

72.4 

12.48 

62.40 

1.874 

31.0 

141.9 

4i-5 

85  5 

iS-^ 

75-65 

2.023 

50.0 

148.0 

48.1 

88  6 

17-54 

87.70 

2.066 

68.0 

154.0 

70-9 

95-7 

25.84 

129.20 

2.198 

One  liter  of  o.i  n  Hg(NO3)2  solution  dissolves  105  gms.  HgCl2  at  25°. 

(Morse,  1902.) 

This  result,  together  with  distribution  experiments,  show  that  complexes  of 
HgCl2  and  Hg(NO3)j  are  formed. 


MERCURY  CHLORIDE 


410 


SOLUBILITY  OF  MERCURIC  CHLORIDE  IN  AQUEOUS  SALT  SOLUTIONS  AT  25°. 

(Herz  and  Paul,  1913-) 


In  Aqueous  Ba- 
rium Chloride. 

In  Aqueous  Cal- 
cium Chloride. 

In  Aqueous  Lith- 
ium Chloride. 

In  Aqueous  Mag- 
nesium Chloride. 

Mols.  per  Liter. 

Mols.  per  Liter. 

Mols.  per  Liter. 

Mols. 

per  Liter. 

1 

HgCl2. 

CaCl2. 

HgCl2. 

LiCl. 

HgCl2. 

MgCl2. 

Hg(V 

0 

0.265 

O 

.190 

0.364 

0.414 

0 

.351 

0.168 

0-374 

o 

.385 

0.697 

o 

,402 

0.766 

0.835 

0 

.666 

0.415 

0.719 

0 

•572 

1.167 

0, 

656 

1.108 

I.27I 

I 

.021 

o.57o 

I.I3I 

0 

.776 

1.620 

o 

,964 

1.811 

L738 

I 

.678 

0.997 

1.864 

I 

-336 

2.645 

I 

429 

2.645 

2.265 

2 

.214 

1.320 

2.569 

3 

•030 

5.348 

I, 

723 

3.304 

3.091 

2 

.896 

1.728 

3.206 

In  Aqueous  Potas- 

In  Aqueous  Sodium 

In  Aqueous  Strontium 

sium  Chloride. 

Chloride. 

Chloride. 

Mols. 

per  Liter. 

Mols. 

per  Liter. 

Mols.  per  Liter. 

'   KC1. 

HgCl2. 

'  NaCl. 

Hg(V 

'SrCl2. 

HgCl2/ 

O 

0.265 

O.20I 

0.372 

0.164 

O 

•315 

O.I 

0.381 

(Sherrill,  1903.) 

0.416 

0.508 

0.3II 

0 

.563 

0.174 

0-355 

0.671 

0.748 

0.519 

o 

.829 

0.221 

0.381 

I-I53 

1.192 

0.724 

I 

-342 

0.25 

0.542 

(Sherrill,  1903.) 

I.94I 

2.022 

1.046 

I 

.776 

0.683 

0.836 

3.162 

3-434 

1.384 

2 

.293 

SOLUBILITY  OF  MERCURIC  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  POTASSIUM 
CHLORIDE  AT  20°  AND  VICE  VERSA. 

(Tichomirow,  1907;  see  also  results  by  Foote  and  Levy  on  next  page.) 
Gms.  per  100  Gms.  H2O. 


KC1. 

HgCl2.  • 

ouuu  i  lutse. 

0 

7-39 

HgOa 

1.  12 

11.63 

tt 

2-39 

15.72 

tt 

4-05 

22.17 

tt 

4.84 

25.16 

"  +2HgCl2.KCl 

5.60 

25-13 

2  HgCl2.KCl 

6.71 

25.66 

" 

7-39 

26.41 

"  +HgCl2.KCl 

7.46 

24.70 

HgCl2.KCl 

8.95 

19-93 

tt 

15 

22.87 

" 

17.57 

26.12 

" 

Gms.  per  100  Gms.  H2O.         -  c_,:  J  Wl_ 

KC1. 

HgCl2. 

20-35 

29      HgCl2.KCl 

26.31 

34.83    " 

30-32 

39-10    " 

34-12 

42.82     "  +HgCl2.2KCl 

34.18 

39.34    HgCl2.2KCl 

34-34 

35-i6    " 

35-54 

30.63 

37.72 

24.3° 

41-33 

19.33    «  +KC1 

39.66 

15.76           KC1 

37.87 

10.28             " 

35-32 

2.1 

100  gms.  i  n  aq.  NaCl  solution  dissolve  25.08  gms.  HgCl2  at  25°. 

(Osaka,  1903-08.) 
Data  for  the  solubility  of  mercuric  chloride  in  aqueous  solutions  of  glycerol, 

sucrose,  tartaric  and  citric  acids  at  25°  are  given  by  Moles  and  Marquina,  1914. 
Data  for  equilibrium  in  the  system  HgCl2  +  KOH  +  H2O  at  25°  are  given  by 

Herz,  1910. 
Similar  data  for  mercurous  chloride  +  KOH  +  H2O  at  25°  are  given  by  Herz, 

1911. 


411 


MERCURIC  CHLORIDE 


SOLUBILITY  OP  MIXTURES  OF  SODIUM  AND  MERCURIC  CHLORIDE  IN 

WATER  AT  25°. 

(Foote  and  Levy  —  Am.  Ch.  J.  35,  239,  '06.) 


Gms.  per  100  Gms.  Solution.    Gms.  per  100  Gms.  Undissolved  Residue. 


NaCl. 

HgCl2. 

NaCl. 

HgCl2. 

H26. 

26.5 

none 

100 

none 

none 

18.66 

51-35 

.  .  . 

16.39 

...   ] 

18.71 

21.98 

... 

18.64 

51.42 

.  .  . 

65.42 

... 

18.87 

51  .26 

.  .  . 

71-25 

...   J 

14.97 

57-74 

16.38 

74.18 

9-44  ' 

14.03 

59.69 

16.36 

74-21 

9-43 

13  .25 

62  .16 

16.16 

74-70 

9.14 

13.17 

62.59 

15.96 

74-76 

9-28 

12.97 

62.50 

78.20 

... 

I3-I4 

62.48 

.  .  . 

88.64 

.  .  . 

62-55 

90.83 

•  •  •   , 

Two  determinations  made  at 

10.3°  gave: 

19.46 

46.49 

67.46 

29.19 

3-35 

19.48 

46.50 

22.83 

68.85 

8.32 

Solid 
Phase. 


NaCl 


NaCl  and 
NaCl.HgCl2.aHaO 


Double  Salt 

NaCl.HgCl2.2H2O 
Calc.  Comp.  =  16.01%  NaCl 

74-14%  HgCl.g.85%  HaO 


and 


SOLUBILITY  OF  MIXTURES  OF  POTASSIUM  AND  MERCURIC  CHLORIDES 
IN  WATER  AT  25°. 

(Foote  and  Levy.) 


Composition  of  Solution. 
Grams  per  100  Grams 

Percentage  Composition 
of  Undissolved 

Solid 

Solution. 

Residue 

Phase. 

J    KC1. 

HgCl2. 

KC1. 

HgCl2. 

H20. 

26.46 

none 

100 

none 

KC1 

26.24 

15.04 

.  .  . 

3-63 

:::  i 

| 

26.43 

15.02 

.  .  . 

26.15 

...  i 

KC1  and 

26.33 

15  .02 

52.01 

...  i 

2KCl.HgCl3.H20 

26-33 

14.92 

6  1  .04 

...  j 

23-74 

18.91 

34.6l 

61.66 

3-731 

2KCl.HgCl2.H2O 

22.36 
21.39 

21.39 
23.88 

34-77 
34-8o 

62.02 
61.84 

3-2i 
3-35  J 

Calc.  Composition 
34-05%  KC1,  61.84% 
4.11%  H20 

20.32 
20.26 

27  .62 
27.38 

65-24 
73-98 

:::! 

2KCl.HgCl2.H20  and 
KCl.HgCl2.H2O 

I7-85 

25-34 

21.89 

75-io 

3  -on 

9.26 

18.95 

21  .02 

73-36 

5.62 

iKCl.HgC!2.H2O 

'6.84 

19.56 
22.81 

20.76 
20-75 

73.06 
74-54 

6.18 

4-71 

Calc.  Composition 
20.52%KC1,  74-53%  1 
4-95%  H20 

6.66 

24.32 

20.54 

73-99 

5-47J 

'. 

6.52 
6.64 

25.16 

76.46 
80.60 

:::] 

1          KCl.HgCl2.H2O  and 
KC1.2HgCl2.2H2O 

I 

6.27 

5-77 

25.11 
24-73 

12  .09 
11.87 

83.20 
83.18 

4-71 

4-95  ! 

,  KC1.2HgCl2.2H2O 
Calc.  Composition 

4.68 

24-75 

.  .  . 

84.46 

...  l 

I 

4.66 

25-J7 

.  .  . 

93-68 

I 

I          KCl.aHgCl2.aH30  ai 

4.69 

24.82 

98.50 

:::  j 

I 

none 

6.90 

none 

100.  OO 

none 

HgCla 

HgCl2, 


MERCURIC  CHLORIDE 


412 


SOLUBILITY  OF  MIXTURES  OF  MERCURIC  AND  RUBIDIUM  CHLORIDES  IN 
WATER  AT  25°. 

(Foote  and  Levy,  1906.) 


Composition  of  Solution. 
Cms.  per  100  Gms.  Solution. 


Percentage  Composition  of 
Undissolved  Residue. 


Solid  Phase. 


RbCl. 

HgCl» 

RbCl. 

HgCl2. 

H20. 

48.57 

none 

100 

none 

none   Rbci 

46.76 

9.18 

88.04 

11.24. 

0.72 

47-54 
47-55 

9-49 
9-39 

60.33 
56.59 

37-51 
40.75 

2.16 
2.66 

RbCl  and  2RbCl.HgCl2.H20 

47-3 

9-47 

46.73 

49-38 

3-88 

47-65 
35  -16 

iQ-35 
19.58 

46.50 
45-98 

50.92 
50.80 

2-58 

3-22 

2RbCI.HgCI2.H20  Calc.   Com- 
position 45-55%  RbCl.  51  .05% 
HgCl2.3.4%  H20 

34-77 

19.94 

43-07 

52-44 

4-49 

2RbCl.HgCl2.H20  and  3RbCl. 

34.76 

20.  10 

41.10 

55-36 

3-54 

2HgCl2.2H2O 

30.27 
29.20 
27.38 

20.17 

20.55 
20.63 

39-07 
39.10 

38.67 

57-34 
'   57'-47 
57-40 

3-59 
3-43 
3-93 

3RbCl.2HgCl2.2H20 
Calc.  Composition 
38.55%  RbCl,  57.62  %HgCl2. 
3.82  %H20 

26.83 

20.87 

38.48 

57-36 

4.16 

3RbCl.2HgCl2.2H2O  and 

27.09 

20.97 

31.40 

64.35 

4-25 

RbCl.HgCl2.H2O 

26.15 

20.58 

30-34 

65.48 

4.18 

RbCl.HgCl2.H2O 

23.81 

18.71 

30.87 

65.10 

4-03 

Calc.  Composition 

18.10 

14.25 

29.87 

65.28 

4-85 

29-49%  RbCl,    66.11  %HgCl2, 

10.87 

10.42 

29-33 

66.15 

4-52 

4.40%  H2O 

10.68 

10.56 

28.59 

67-99 

3-42 

RbCl.HgCl2.H2O  and  3RbCl 

10.50 

10.05 

26.22 

72.20 

1.58 

4HgCl2.H20 

10.  06 

9.86 

25.28 

73-38 

0.84 

8.48 
8.46 

8.71 
8.80 

25-30 
25-44 

73-15 
73-67 

!-55 
0.89 

3RbCl.4HgCl2.H2O 
Calc.  Composition 
24.76%  RbCl,    74-01%  HgCl2, 

5.68 

8.70 

25.09 

73-46 

1-45 

i.23%H20 

5-io 

8-33 

24.92 

73-93 

i-i5 

3-43 

8.25 

22.79 

75-72 

i-49 

3RbCl.4HgCl2.H20   and   RbCl 

3-38 

8 

12.68 

86.74 

0.58 

5HgCl2 

2.98 

7.71 

8.40 

91.24 

1.89 
1.50 

7.64 
7-55 

8-38 
8.30 

.  91.78 
91.81 

RbCl.sHgCl2 
Calc.  Composition 
8.20%  RbCl,  91.8%  HgCl, 

1.  10 

7.21 

8.07 

91.58 

„  .  . 

0.79 
0.84 

7.16 
7.42 

6.91 

2.27 

93-15 
97.09 

... 

RbCl.sHgCl2  and  HgCl2 

none 

6.90 

none 

100 

HgCl2 

20 

30 
40 
50 
60 


SOLUBILITY  OF  MERCURIC  CHLORIDE  IN  ACETIC  ACID. 

(Etard,  1894.) 


Gms.  HgCU 

per  roo  Gms. 

Solution. 

2-5 

3-5 
4-7 
6 

7.2 


te. 

70 
80 

90 
100 


Gms.  HgCl2 

per  i  oo  Gms. 

Solution. 

8-5 
9-7 
ii 

12.4 


no 

120 
130 

140 

160 


Gms.  __„„, 

per  100  Gms. 

Solution. 

I3.6 

16.5 
20.7 
25.2 

34-8 


413 


MERCURY  CHLORIDE 


SOLUBILITY  OF  MERCUROUS  CHLORIDE  (CALOMEL)  IN  AQUEOUS  SOLUTIONS  OF 
SODIUM  CHLORIDE,  BARIUM  CHLORIDE,  CALCIUM  CHLORIDE  AND  OF  HYDRO- 
CHLORIC ACID  AT  25°. 

(Richards  and  Archibald,  1902.) 

Solid  phase  in  each  case.     Calomel  +  about  o.i  gm.  of  mercury. 


In  Aqueous  NaCl. 


In  Aqueous  BaCl2. 


p.  Gr.  of 

Gms.  per  Liter. 

Sp.  Gr.  of 

Gms.  per  Liter. 

olutions. 

'  NaCl.       .             HgCl. 

Solutions. 

BaClz.    a             HgCl. 

.  .  . 

5.85              O.C04I 

1.  088 

104.15               0.044 

.040 

58.50              0.041 

I-I34 

156.22               0.088 

.078 

IIQ                      O.I2Q 

I.I74 

208.30              0.107 

•093 

148.25              0.194 

1.263 

312.54              0.231 

.142 

222.3                 0.380 

.188 

292.5                 0.643 

In  Aqueous  CaCl2. 


In  Aqueous  HC1. 


p.  Gr.  of 

Gms.  pe 

•  Liter.                           Sp.  Gr.  of 

Gms.  per  Liter. 

olutions. 

'    CaCl2. 

HgCl.  "                  Solutions. 

HCl.j 

HgCl.  ' 

39-96 

O.O22 

31.69 

0.034 

.  .  . 

55-5 

0.033 

36.46 

0.048 

.064 

in 

O.oSl 

.042 

95-43 

0.207 

.105 

I38-75 

0.118 

.069 

158-4 

0-399 

•151 

I95-36 

0.231 

.091 

209.2 

0.548 

.205 

257-52 

0.322 

.114 

267.3 

0.654 

•243 

324.67 

0.430 

.119 

278.7 

0.675 

•315 

432-9 

0.518              1.132 

3I7-3 

0.670 

•358 

499-5 

0.510              1.153 

-364-6 

0.673 

loo  gms.  bromoform,  CHBr3,  dissolve  0.055  8m-  HgCl  at  i8°-2O°.     (Sulc.,  1900.) 
SOLUBILITY  OF  MERCURIC  CHLORIDE  IN  AQUEOUS  ETHYL  ALCOHOL  AT  25°. 

(Abe,  1912.) 


'QH6OH. 

HgCl2.  " 

ociiiu  .rjua.sc. 

C2H5OH. 

HgCl2. 

ouuu  rna.be. 

0 

6.80 

HgCk 

45-84 

I5-36 

HgCfe 

5-08 

0.65 

u 

49.86 

18.18 

M 

14.49 

6.41 

1C 

53-61 

21.40 

(I 

21 

6-55 

It 

57.26 

24.51 

tt 

26.25 

7-31 

ft 

60.55 

27.67 

It 

31-53 

8.51 

tf 

63-95 

29.86 

tt 

36.85 

10.32 

(( 

67-39 

32.40 

tt 

41.36 

12.64 

It 

SOLUBILITY  OF  MERCURIC  CHLORIDE  IN  AQ.  ETHYL  ALCOHOL  AT  25°. 

(Herz  and  Anders,  1907.) 


t.  %  CjHsOH 
in  Solvent. 

dy,  of  Solvent. 

d^  of  Sat.  Sol. 

Gms.  HgCV] 
100  cc.  Sat.  £ 

0 

0.9971 

I-0565 

7.22 

20.  l8 

0.9665 

I.02I4 

6-76 

40.69 

0.9302 

I.OlSo 

10.69 

70.01 

0.8632 

I.  O6l6 

23.60 

100 

0.7856 

I.I067 

36.86 

MERCURY  CHLORIDE 


414 


SOLUBILITY  OF  MERCURIC  CHLORIDE  IN  AQUEOUS  METHYL  ALCOHOL  AT  25°. 

(Herz  and_Anders,  1907.) 


Wt.  %  CHjOH 
in  Solvent. 

J,«  of  Solvent.           d^ 

of  Sat.  Sol. 

Cms.  HgCl2  per 
100  cc.  Sat.  Sol. 

10.60 

0.9792 

.0441 

7.00 

30-77 

0.9481 

.0420 

11.31 

37.21 

0.9369 

.0507 

13-43 

47.06 

0.9186 

.0809 

19.71 

64 

0.8800 

.2015 

38-44 

78-05 

0.8489                 ] 

c-33*4 

57-17 

100 

0.7879                 ] 

[.2160 

48.62 

loo  cc.  90%  ethyl  alcohol  dissolve  27.5  gms.  HgCl2  at  15.5°,  rfis  sat.  sol.  =  1.065. 

(Greenish  and  Smith,  19030 

loo  gms.  00.2  %  ethyl  alcohol  dissolve  33.4  gms.  HgCU  at  25°.  (Osaka,  1903-8.) 

abs.         "  "  "     •  49.5 (de  Bruyn,  1892.) 


methyl 


49-5 
52.9 


1       at  19.5°  and  66.9  gms.  at  25°. 
(de  Bruyn,  1892.) 
1.2    "         "      at  the  crit.  temp. 

(Centnerszwer,  1910.) 

SOLUBILITY  OP  MERCURIC  CHLORIDE  IN  METHYL,  ETHYL  PROPYL, 
n  BUTYL,  Iso  BUTYL  AND  ALLYL  ALCOHOLS. 

(Etard  —  Ann.  cliim.  phys.  [7]  2,  563,  '94.) 

NOTE.  —  For  the  solubility  in  Me,  Et,  and  propyl  alcohols  at  room 
temperature,  see  Rohland —  Z.  anorg.  Ch.  1-8,  328,  '98;  at  8.5°,  20°  and 
38.2°,  see  Timofejew  —  Compt.  rend.  112,  1224,  '91;  in  Me  and  Et 
alcohols  at  25°,  see  de  Bruyn  —  Z.  physik.  Ch.  10,  783,  '92.  The  deter- 
minations of  these  investigators  agree  well  with  those  of  Etard,  which 
are  given  below. 

Grams  HgCl2  per  100  Grams  Saturated  Solution  in: 


fc    . 

CHaOH. 

C2H6OH. 

CsH7OH.     CH3(CH2)3OH.  (CH3)2CHCH2OH.  CH2.CH.Cl£oH. 

-30 

14-5 

15.0 

—  20 

20.1 

15-7 

*3-5 

21.0 

—  10 

IS-2 

26.5 

I6.5 

i3-7 

25-5 

O 

20.1 

29.8 

17.4 

14.0 

5-2 

30.0 

+  10 

26.3 

30.6 

18.0 

14-3 

6.0 

37-5 

20 

34-o 

32.0 

18.8 

14.6 

6.8 

46-5 

25 

40.0 

32-5 

19-5 

i5-S 

7-2 

30 

44-4 

33-7 

20.  o 

16.5 

7-5  ' 

40 

58.6 

35-6 

23.0 

19.6 

9-7 

60 

62.5 

41.2 

29.8 

26.5 

17.0 

.  .  . 

80 

66.0 

47-5 

36.8 

33-o 

24.9 

100 

70.1 

54-3 

43-8 

3i-7 

120 

73-5 

61.5 

50.6 

.  .  . 

39-2 

'SO 

78-5 

... 

... 

... 

SOLUBILITY  OF  MERCURIC  CHLORIDE  IN  AQ.  ETHYL  ACETATE  AT  25°.  ^ 

(Herz  and  Anders,  1907.)  ^ 

Wr  t.  %  CHjCOOCjHg  j        ^r  c    \.        f 

in  Solvent.  d*£  ol 

o  0.9971 

4-39* 

96.76t 
loot  0.884 

Almost  sat.  with  ethyl  acetate.       t  Ethyl  acetate  almost  sat.  with  H,O.       J  (b.  pt.  =  75.77°.) 


t  of  Sat.  Sol. 

Gms.  HgClj  per 
100  cc.  Sat.  SoL 

1-0565 
1.0581 

7-22 
7-38 

I.237I 
I  .1126 

41-55 
26.42 

415 


MERCURY  CHLORIDE 


SOLUBILITY  OF  MERCURIC  CHLORIDE  IN  WATER-ETHER  MIXTURES  AT  25°. 

(Abe,  1912.) 
Cms.  per  100  Cms.  Sat.  Sol. 


HgCl2. 

Ether. 

H2O. 

ouiiu  rua.sc. 

6.92 

87.86 

5-22* 

HgCl2 

S-2 

1.2 

93-6 

u 

4-3 

5-2 

90-5 

(I 

2.8 

5-4 

91.8 

tt 
tt 

5-4 

*  (Solvent,  ether  sat.jwith  H20.) 

SOLUBILITY  OF  MERCURIC  CHLORIDE  IN  MIXTURES  OF  ETHER  AND  ETHYL 
ALCOHOL  AT  25°.    (Abe,  1912.) 


Gms.  per  100  Cms.  Sat.  Sol. 


HgCl2. 
32.43 
35-50 

37-39 
37 -96 
38-24 
37-75 


C2H6OH. 
67-57 
58.59 
51.02 

44-79 
38.69 

32.84 


Gms.  per  100  Gms.  Sat.  Sol. 

'     5gC£  QH6OH.  ' 

36.29  27.16 

34.08  22.48 

28.55  I5-2Q 

20.67  8.97 

5-49  o 


SOLUBILITY  OF  MERCURIC  CHLORIDE  IN  MIXTURES  OF  ALCOHOLS  AT  25°. 

(Herz  and  Kuhn,  1908.) 

In  Mixtures  of  Ethyl  and   In  Mixtures  of  Ethyl  and    In  Mixtures  of  Methyl  and 
Methyl  Alcohols.  Propyl  Alcohols.  Propyl  Alcohols. 


%  CH3OH 

da.  Of 

Gms.HgCl,  %C3H7OH     fl 

Uof 

Gms.  HgCl2  %  C3H7OH     a 

'     of     Gms.  HgCfc 

in 

Solvent. 

Sat.  Sol. 

per  100  cc. 
Sat.  Sol. 

in 

Solvent. 

Sat.  Sol. 

per  too  cc. 
Sat.  Sol. 

in 
Solvent. 

_  TT           per  loo  cc. 
Sat.  Sol.       Sat.  Sol. 

0 

I.IO7 

36.86 

O 

I 

,1070 

36.86 

O 

I 

.2l6o 

48.62 

4-37 

I.I30 

39-43 

8. 

i 

I 

,0988 

36.67 

II.  II 

I 

.2278 

50-34 

10.40 

I-I57 

42.61 

17- 

85 

I 

,0857 

34.06 

23.80 

I 

.2848 

57-14 

41.02 

1.294 

58.37 

56. 

6 

I 

,0272 

27.11 

65.20 

I 

.1568 

42.28 

80.69 

I.32I 

61.67 

88. 

6 

0 

9854 

21.66 

91.80 

I 

.0090 

25.09 

84.77 

1.288 

57-82 

91. 

2 

o 

.9824 

21.60 

93-75 

I 

.0029 

23-23 

91-25 

1.254 

53.85 

95- 

2 

o 

.9772 

20.87 

96.6 

0 

.9851 

21.52 

100 

1.216 

48.62 

IOO 

o 

,9720 

20.03 

IOO 

0 

.9720 

20.03 

SOLUBILITY  OF  MERCURIC  CHLORIDE  IN  MIXTURES  OF  ETHYL  ALCOHOL  AND  BEN- 
ZENE AND  OF  ETHYL  ALCOHOL  AND  CHLOROFORM  AT  DIFFERENT  TEMPERATURES. 

(Dukelski,  1907.) 


In  a  Mixture  of 
one  mol.  C2H6OH 
+  one  mol.  CeHe. 

Gms.  HgCl2 
t°.          per  loo  Gms. 

In  a  Mixture  of       In  a  Mixture  of          In  a  Mixture  of 
two  mols.  C2H6OH    one  mol.  C2H6OH     two  mols.  C2H6OH 
+  one  mol.  CeHe.     +  one  mol.  CHsCl.    +  one  mol.  CHCla. 
Gms.  HgCl2                       Gms.  HgCl2                       Gms.  HgCl2 
t°.         per  loo  Gms.          t°.         per  100  Gms.            t°.     per  100  Gms. 

Sat. 

Sol. 

Sat.  Sol. 

Sat.  Sol. 

Sat.  SoL 

-2.5 

15 

.20 

-5 

.2 

19-45 

—  20, 

1  5 

3-82 

—  20 

-5 

6.60 

O 

15 

.40 

0 

20.13 

—  12 

4-43 

0 

7.69 

6 

16 

.38 

9 

.1 

21.65 

O 

4-89 

8 

8.96 

20.5 

18 

.40 

20 

•9 

23-57 

8 

5-37 

23 

10.66 

20.65 

18 

-50 

24 

-4 

24.19 

23 

7.12 

38 

•5 

12.50 

'  24.5 

19 

•33 

36 

•5 

26.53 

38, 

5 

8.51 

44 

.2 

14.40 

34-5 

21 

•34 

53 

-7 

31.27 

44 

,2 

9-51 

54-4 

24 

-84 

74 

38.74 

45 

,6 

9.98 

54-5 

24 

.42 

Some  of  the  determinations  were  made  by  the  direct  method  of  saturating  the 
solution  at  a  given  temperature  and  determining  the  dissolved  material  by  evap- 
orating and  weighing.  Others  were  made  by  the  synthetic  method  of  Alexejew. 


MERCURY   CHLORIDE 


416 


SOLUBILITY  OF  MERCURIC  CHLORIDE  IN  MIXTURES  OF  METHYL  ALCOHOL  AND 
CHLOROFORM,  METHYL  ALCOHOL  AND  CARBON]  TETRACHLORIDE,  AND  METHYL 
ALCOHOL  AND  DICHLORETHANE  AT  DIFFERENT  TEMPERATURES. 

(Dukelski,  1907.) 


In  a  Mixture  of 
one  mol.  CH3OH 
4-  one  mol.  CHC13. 

Gms.  HgClj 
t°.        per  100  Gms 

In  a  Mixture  of 
two  mols.  CH3OH 
+  one  mol.  CHC13. 

Gms.  HgClj 
t°.           per  loo  Gms. 

In  a  Mixture  of        In  a  Mixture  of 
two  mols.  CH3OH   two  mols.  CH3OH 
+  one  mol.  CC14.  +  one  mol.  C2H4C12. 

Gms.  HgCl2                         Gms.  HgCl2 
t°.        per  100  Gms.           t°.          periooGms. 

Sat.  Sol. 

Sat.  Sol. 

Sat.  Sol. 

Sat.  Sol. 

—  12 

I  .73 

—  12 

3-33 

0 

5-20 

O 

13-33 

O 

3-51 

O 

6-73 

7-7 

6.69 

12.5 

21.30 

8 

5-63 

8 

8.21 

24-9 

14.06 

20.8 

29.23 

23 

IO.I5 

23 

16.56 

30.6 

19.40 

25-3 

34.78 

24.9 

10.71 

24-9 

18.45 

35-5 

20.50 

30.2 

36.87 

30.6 

11.40 

30.6 

19.70 

36.1 

21.  80 

37-4 

37-95 

38.5 

12.  02 

38.5 

20.83 

48.5 

21.90 

45-9 

39-36 

SOLUBILITY  OF  MERCURIC  CHLORIDE  IN  MIXTURES  OF  METHYL  ALCOHOL 
AND  BENZENE  AT  DIFFERENT  TEMPERATURES. 

(Timofeiew,  1894.) 


In  a  Mixture  of  one  mol. 
CH3OH  +  one  mol.  C6H6. 


*'• 

O 

21-25 
30 
37 


Gms.  HgCl2  per  roo 
Gms.  Sat.  Sol. 

8 

23-9 
27-3 
28.1 


In  a  Mixture  of  one  mol. 
CH3OH  +  two  mols.  C6H6. 

to  Gms.  HgCls  per  100 

1  '  Gms.  Sat.  Sol. 


O 

21-25 
30 

37 


4-8 
17.1 
18 
18.4 


SOLUBILITY  OF  MERCURIC  CHLORIDE  IN  BENZENE,  IN  DICHLORETHANE 
AND  IN  ETHYLACETATE  AT  DIFFERENT  TEMPERATURES. 

(Dukelski,  1907.) 


In  C6H6. 


In  C2H4C12. 


f  „           Gms.  HgCl2  per 
loo  Gms.  Sat.  Sol. 

6-5 

0.26 

18 

o-53 

34-i 

0.64 

54-i 

i  .02 

69 

i-39 

to           Gms.  HgClj  per 
100  Gms.  Sat.  Sol. 

O 

i-33 

12.5 

i-55 

25-3 

i-73 

33 

2.05 

45-9 

2.42 

In  CH3COOC2H6. 

xo  Gms.  HgClo  per 

*         100  Gms.  Sat.  Sol. 


6.5 


26 

38 

45 


22.9 
22.7 

22.8 

23-5 
26.4 


SOLUBILITY  OF  MERCURIC  CHLORIDE  IN  MIXTURES  OF  BENZENE  AND  ETHYL- 
ACETATE,  CHLOROFORM  AND  ETHYL  ACETATE  AND  OF  CARBO.N  TETRACHLORIDE 
AND  ETHYL  ACETATE. 

(Dukelski,  1907.) 


In  a  Mixture  of  one  mol. 

CeHe  +  one  mol. 

CH3COOC2H6. 


In  a  Mixture  of  one  mol. 

CHCls  +  one  mol. 

CH3COOC2H5. 


In  a  Mixture  of  one  mol. 
CCU  +  two  mols. 
CH3COOC2H6. 


fo              Gms.  HgCl2  per 
100  Gms.  Sat.  Sol. 

O 

9.62 

6-5 

9.62 

25-7 

9.78 

27.6 

9.98 

35-5 

10.81 

45-3 

13.69 

Gms.  HgCl2  per 
zoo  Gms.  Sat.  Sol. 


O 

26.1 
36.1 
46 

48.5 


3-34 
4.07 
4.78 

5-38 
5.10 


to           Gms.  HgCli  per 
100  Gms.  Sat.  Sol. 

O 

9-24 

10.3 

9-05 

25-7 
27.6 

38.5 

9-32 
.9-50 
-9-89 

45-3 

11.70 

417 


MERCURIC   CHLORIDE 


SOLUBILITY  OF   MERCURIC   CHLORIDE  IN  ETHYL  ACETATE  AND  IN 

ACETONE. 

(Etard,  1894;  von  Laszcynski,  1894;  Krug  and  McElroy,  1892;  Linebarger,  1894;  Aten,  1905-06.) 

NOTE.  —  The  results  obtained  by  the  above-named  investigators  were  calcu- 
lated to  a  common  basis  and  plotted  on  cross-section  paper.  The  variations 
which  were  noted  could  not  be  satisfactorily  harmonized,  consequently  all  the 
results  are  included  in  the  following  table: 


SOLUBILITY. 


In  Ethyl  Acetate. 


In  Acetone. 


Grams  HgCk  per  100  Grams  Solution. 


Gms.  HgCl2  per  too  Gms.  Solution. 


•  •  /  
Laszcynski. 

Aten.     Linebarger. 

Etard  .     K  and  McE  .  Laszcynski  . 

Aten. 

Etard. 

—  10 

. 

23.0 

. 

.  . 

40 

...          ... 

44.0 

* 

57 

.0 

0 

22 

•  O 

23.2 

32 

.0 

40 

49-7 

43-o 

* 

61 

•7 

+  10 

22 

.2 

23-5 

32 

•5 

40 

52.0  5 

i.o  *~5 

8.9 

>t  61 

•7 

20 

22 

•5 

23-4 

32 

40 

54 

58.5 

t 

61 

•7 

25 

22 

•7 

23-5 

33 

.0 

40 

37-4      55-2 

S8.2 

t 

61 

•7 

30 

23 

.0 

33 

.2 

40 

61 

•7 

40 

23 

•5 

33 

•5 

40 

...         ... 

61 

•7 

50 

24 

.0 

33 

•5 

41 

...          ... 

. 

61 

•7 

60 

24 

•7 

.  .  . 

42-5 

...         •  *  . 

61 

•7 

80 

26 

.0 

. 

45-2 

...         ... 

61 

•7 

100 

.  . 

. 

.  .  . 

. 

48.0 

...          ... 

,  » 

120 

. 

. 

50.8 

... 

>  • 

150 

. 

. 

55-o 

... 

.. 

•  • 

(*) 

Solid  phase  HgCl2(CH3)2CO. 

(t)  Solid  Phase  HgCl,. 

loo  gms.  absolute  acetone  dissolve  143  gms.  HgC^  at  18°. 


(Naumann,  1904.) 


100  gms.  ethyl  acetate  (dig.  =  0.8995)  dissolve  48.8  gms.  HgCl2  at  18°. 

(Naumann,  1910.) 

100  gms.  methyl  acetate  (dig  =  0.935)  dissolve  42.6  gms.  HgCl2  at  18°. 

(Naumann,  1909.) 


SOLUBILITY  OF  MERCURIC  CHLORIDE  IN  SEVERAL  SOLVENTS. 

(Arctowski,  1894;  von  Laszcynski,  1894;  Sulc,  1900.) 


In  Carbon  Bisul- 
phide (A.). 


In  Benzene 
(von  L.). 


In  Several   Solvents 
at  18-20°  (S.). 


Gms.  HgCl2 

Gms.  HgCl2 

Gms.  HgCl2 

t°. 

per  100  Gms. 

t°.              per  100  Gms. 

Solvent. 

per  100  Gms. 

Solution. 

Solution. 

Solvent. 

—  10 

O.OIO 

15            o-537 

CHBrs 

0.486 

o 

O.OlS 

41            0.616 

CHC13 

0.106 

IO 

O.O26 

55            0.843 

CC14 

0.002 

15 

0.032 

84            1-769 

C2H5Br 

2.010 

20 

O.O42 

C2H4Br, 

1-530 

25 

0-053 

30 

0.063 

MERCURY   CHLORIDE 


418 


SOLUBILITY  OF  MERCURIC  CHLORIDE  IN  MIXTURES  OF  ACETONE  AND  BENZENE, 
ETHER  AND  CHLOROFORM  AND  OF  ETHYL  ACETATE  AND  BENZENE  AT  25°. 

(Harden  and  Dover,  1917.) 


In  Mixtures  of 
CH3COCH3  +  C6H6. 

Gms.CH3COCHj     Cms.  HgCl2 
per  100  Gms.       per  100  Gms. 


Mixture. 

Mixed  Solven 

100 

140 

90 
80 

117 
96.5 

70 
60 

77 
60 

50 

45 

40 

3i-4 

30 

20 

20 

10.7 

10 
0 

3-9 
0.66 

In  Mixtures  of 
(C2H5)20  +  CHC13. 


Gms.  CHC13 
per  100  Gms. 
Mixture. 

Gms.  HgCl2 
per  100  Gms. 
Mixed  Solvent. 

0 
IO 

6-95 
5-85 

20 

4-73 

30 
40 

3-7° 
2.80 

SO 
60 

2.IO 
I.48 

70 
80 
QO 
100 

o-95 
0.657 
0.328 
0.128 

In  Mixtures  of 
CH3COOC2H6  +  C6H6. 

Gms.  CH3COOC2H5      Gms.  HgCl2 
per  100  Gms.          per  100  Gms. 
Mixed  Solvent. 


Mixture. 
100 
90 
80 
70 
60 

40 

30 
20 
IO 
O 


49-3 
26 

22.1 
I8.I 
14.2 
II 

8 

5-4 

3-i 

1.6 

0.66 


SOLUBILITY  OF  MERCURIC  CHLORIDE  IN  BENZENE. 

(Average  curve  from  results  of  Linebarger,  1895;  Sherrill,  1903;  and  Marden  and  Dover,  1917.) 


O 
10 
20 


Gms.  HgCl2  per 
zoo  Gms.  CaH«. 

O.2O 

0-39 
0.56 


25 
30 
40 


Gms.  HgCl2  per 
100  Gms.  CjHg. 

0.64 


0.84 


SOLUBILITY  OF  MERCURIC  CHLORIDE  IN  ABSOLUTE  ETHYL  ETHER. 

(Etard,  1894;  Laszcynski,  1894;  Kdhler,  1879.) 


fc 

-2O 

O 

20 


Gms.  HgCl2  per 
100  Gms.  Solution. 

6 
6 
6 


60 
70 
80 


Gms.  HgCl2  per 
loo  Gms.  Solution. 

6 
6-4 

7 


90 
100 
no 


Gms.  HgCl2  per 
100  Gms.  Solution. 

7-5 
8 

8-5 


SOLUBILITY  OF  MERCURIC  CHLORIDE  IN  CHLORINATED  HYDROCARBONS  AT  25°. 

(Hoffmann,  Kirmreuther  and  Thai,  1910.) 


Solvent. 


Formula. 


Solvent. 


Gms. 

HgCl2per 

loo  Gms. 

Solvent. 

Ethylene  Chloride  CH2C1.CH2C1  1.229      Dichlorethylene 


Formula. 


Tetrachlorethane  C2H2Cl4 
Chloroform  CHCU 

Pentachlorethane  C2HCl6 


0.090 
o.  101 


Trichlorethylene 
Tetrachlorethylene 


0.0193     Carbontetrachloride    CC14 


Gms. 
HgCl2per 
100  Gms. 
Solvent. 

CHC1.CHC1  0.114 
CHC1.CC12     0.0274 
CC12.CC12       0.0072 
trace 


(Aschan,  1913.) 


100  gms.  95%  formic  acid  dissolve  2.1  gm.  HgCl2  at  19°. 

100  gms.  95%  formic  acid  dissolve  0.02  gm.  Hg2Cl2  at  16.5°. 

100  cc.  anhydrous  hydrazine  dissolve  I  gm.  HgCl2  with  decomp.  at  room  temp. 

(Welsh  and  Broderson,  1915.) 
loo  cc.  anhydrous  hydrazine  dissolve  I  gm.  Hg2Cl2  with  decomp.  at  room  temp. 

(Welsh  and  Broderson,  1915.) 
IOO  gms.  glycerol  dissolve  80  gms.  HgCl2  at  25°.  (Moles  and  Marquina,  1914.) 

ioo  gms.  glycerol  dissolve  8  gms.  HgCl2  ?  Hg2Cl2  at  15-16°.      (Ossendowski,  1907.) 
loo  gms.  anhydrous  lanolin  (m.  pt.  about  46°)  dissolve  1.55  gms.  HgCl2  at  45°. 

(Klose,  1907.) 


419 


MERCURY  CHLORINE 


Gms. 


SOLUBILITY  OF  MERCURIC  CHLORIDE  IN  PYRIDINE. 

(McBride,  1910.) 

The  determinations  at  the  lower  temperatures  were  made  by  stirring  an  excess 
of  HgCl2  with  pyridine  and  analyzing  the  sat.  solution.  Those  at  the  higher  tem- 
peratures were  made  by  the  synthetic  method. 

Cms. 
*"•        SPoT/  Solid  Phase. 

Sat.  Sol. 

—32.6   2.76  HgCl2.2C6HjN 
—  21.75   7.86   " 
0.02  13.14   " 
12.58  17.34   " 
18.78  19.78   " 
27.23  22.65   " 
31.05  24.46   " 
40.90  29.29   " 
50.10  34.94   " 
60.03  40.36 
70.15  46.44 
76      ... 
80.02  51.52 
89     56.45 
94.1   60.09 


t°.  Solid  Phase. 

Sat.  Sol. 

94-7     60.72     HgCl2.2CBHBN+3HgCl2.2CBH6N 
74.7     48.38     HgCl2.C6H6N(unstable) 
(stable) 


50.53 
53-41 
56.45 
57-84 
60.72 
63.06 


"  +HgCl2.C6H6N 
HgCl2.2CBHBN  (unstable) 


83.5 

90.4 

97 

IOO-5 
104.2 
107 
106.2 

95-2  60.77 
106.4  61.93 
109.8  62.58 
114  63.18 
65 
69.66 


(unstable) 
+3HgCl2.2CsH5N 
3HgCl2.2C6H6N  (unstable) 
"  (stable) 


124.2 
145-5 


Data  for  this  system  are  also  given  by  Staronka  (1910). 

Data  for  the  solubility  of  HgCl2.2C6H6N  and  of  Hg(NO3)2.2C5H6N.2H2O  in 
aqueous  solution  of  pyridine  at  i8°.i  are  given  by  Stromholm  (1908). 

Data  for  the  solubility  of  diamine  mercuric  chloride,  (NH3)2HgCl2  —  NH2HgCl, 
in  aqueous  solutions  of  ammonia  at  17.5°  are  given  by  Stromholm  (1908). 

SOLUBILITY  OF  MERCURIC  CHLORIDE  AND  OF  DOUBLE  MERCURIC  AND 
TETRA  METHYL  AMINE  CHLORIDE   (CH3)4NC1.6HgCl2  IN  AQ.  ETHER 

AT    1  7°.        (Stromholm  —  J.  pr.  Ch.  [2]  66,  443,  '02;  Z.  physik.  Chem.  44,  64,  '03.) 


Molecular  Concentration  per  Liter. 


Grams  per  Liter  of  Solution. 


H20. 

HgCl2  (*). 

HgCl2  (f). 

O-O 

0-I5I5 

0.0342 

0.0656 

0-1795 

0-0428 

0.1311 

o  .  2069 

0-0516 

0.1956 

0.2339 

0-0603 

0.2611 

o  .  2489 

0-0690 

0.3267 

o  .  2849 

0.0779 

0.3922 

0.3100 

0.0866 

H2O. 

HgCl2  (*). 

HgCl2  (f). 

O 

41  .16 

9.26 

1.18 

48.64 

II  .60 

2.36 

56.08 

14.00 

3-52 

63-38 

16.34 

4.70 

70.16 

18.70 

5.88 

77-20 

21  .IO 

7.06 

84.02 

23.48 

(*)  Results  in  this  column  are  for  solutions  in  contact  with  the  Solid  Phase  HgClj.     (t)  Results  in 
this  column  are  for  solutions  in  contact  with  the  Solid  Phase  (CH3)4NC1.6HgCl2. 


SOLUBILITY  OF  MERCURIC  CHLORIDE  AND  OF  DOUBLE  MERCURIC  AND 
TETRA  METHYL  AMINE  CHLORIDE  IN  ALCOHOL-ETHER  SOLUTIONS 


AT  17 


(Stromholm.) 


.  . 

Grams  CaHsOH  per  Liter.    Grams  HgCl2  (*)  per  Liter.  Grams  HgCl2  (t)  per  Liter. 

o.o  41.16  9.26 

50.00  11.87 

58.76  14.38 

66.96  16.90 


o.o 

4.58 

9.16 

13.74 


MERCURY   CHLORIDE 


420 


SOLUBILITY  OF  DOUBLE  MERCURIC  CHLORIDES  IN  AQUEOUS  AND  PURE 
ETHER  AT  16.6°. 

(Stromholm,  1902,  1903.) 
Mol.  Cone,  of  HgCl2  per  Liter  of:  Cms.  HgCl2  per  Liter  of: 


Aq. 
Ether 


Pure         Aq.  Aq.  Aq.  Pure      Aq.          Aq. 

Ether.  Ether       Ether  Ether  Ether.    Ether  Ether 

(i).     (2).     (3).          (4).    (5).    (6). 

0.1515  0.2387  0.2647  0.3196  41.04  64.69  71.71  86.58 

0.0673  0.1157  0.1293  0.1617  18.23  3i-4i  35-05  43-79 

0.0404  0.0720  0.0835  0.1034  10.95  *9  -51  22-6i  28.01 

0.0342  ...   0.0706   ...  9.26   ...  19.10   ... 

0.0264  ...   0.0568  ...    7.14   ...  15.39   ••• 

0.0209  0.0400  0.0460  0.0594  5.66  10.83  12.48  16.10 

0.0063  •••   0.0144  •••    1-70   ...  3.90   ... 


Solid  Phase. 


HgCl2 


(CH3)4NC1.6HgCl2 

(C2H5)3SC1.6HgCl2 

(CH3  C2H6)2SC1.6HgClj 

(CHs)2.H2NCl.2HgCl2 


(i)  containing  0.21055  mol.  H2O  per  liter.     (2)  0.2756  mol.  H2O  per  liter.     (3)  0.421  mol.  H2O  per  liter. 
(4)  containing  3.79  gms.  H2O  per  liter.     (5)  4.97  gms.  H2O  per  liter.     (6)  7.59  gms.  H2O  pe 


SOLUBILITY  OF  MIXTURES  OF  MERCURIC 
Absolute  Alcohol.     (Foote,  1910.) 

Gms.  per  100  Gms. 
Sat.  Solution. 


KC1. 
0.21 
0.28 
O.22 
0.28 
0.25 
0.17 
0.38 


HgCl2. 
33.69 
33-80 
24.84 
6.21 

1.65 

i. 57 
1.03 


Solid  Phase. 
HgCl2+5KC1.6HgCl2.2C2H6OH 
sKC1.6HgCl2.2C2H5OH 


7-59  gms.  H2O  per  liter. 

AND  POTASSIUM  CHLORIDES  AT  25°  IN: 
Acetone.     (Foote,  1910.) 

Gms.  per  100  Gms. 
Sat.  Solution. 


KC1. 
1.27 

1-39 
2-58 
2.78 

2-93 
2.52 

3-34 
2.92 


HgCl2. 
61.87 
60.68 
55-85 
54-41' 
48.13 
18.04 
13.26 
ii 


Solid  Phase. 

HgCl2+KCl.sHgCl2.(CH,)2CO 
KCl.5HgCl2.(CH3)2CO 


+5.6.2 


5.6.2 


+KC1 


100  gms.  of  sat.  abs.  alcohol  solution 
HgCl2  and  3.01  gms.  NaCl  at  25°. 


5.6.2=  5KC1.6HgCl2.2(CH8)aCO. 
of  HgCl2  +  NaCl  contain  46.85  gms. 

(Foote,  1910.) 


SOLUBILITY  OF  MERCURIC  CHLORIDE  AND  SODIUM  CHLORIDE  IN  ETHYL 

ACETATE  AT  40°. 

(Linebarger  —  Am.  Ch.  J.  16,  214,  '94.) 

Solid 


Mols.  per  too  Mols. 
Acetate. 

Gms.  per  too  Gms. 
Acetate. 

Gms.  per  100  Gms. 
Solution. 

NaCl. 

HgCl2. 

NaCl. 

HgCl2". 

NaCl. 

HgCl2. 

0.8 

12.9 

0.53 

39-7 

o-53 

28.4 

2-3 

12.4 

I  .53 

38-15 

27.61 

4-3 

16.4 

2.85 

50-44 

2  '.78 

33-54 

9.1 

22.85 

6.05 

86.14 

46.28 

18.5 

34-9 

12.29 

107.4 

10-95 

5J-76 

20.  o 

40.0 

13.29 

123.0 

II  -73 

55.18 

HgCl3 


HgCl2  +  NaCl 


The  double  salt  (HgCl2)2.NaCl  is  formed  under  proper  conditions. 


DISTRIBUTION  OF  MERCURIC  CHLORIDE  BETWEEN  WATER  AND  BENZENE. 

(Linhart,  1915.) 

Results  at  40°. 

Mols.  HgCl2  per  Liter:    •  Cone,  in  H2O 

me.  in  C6H« 
13.07 
12. 08 


Results  at  25°. 

Mols.  HgCl2  per  Liter;  Cone,  in  H2O 

Cone,  in  C6Hg 
I3-65 
12.91 

12-35 


C«Hg  Layer. 

O.O2IOO 

O.OI224 

0.005244 

0.00o6l8 

0.000310 

0.000155 


H20  Layer. 
0.2866 
0.15777 
0.064756 


0.007382 
o  .  003696 
0.001845 


11.90 
11.90 


C8H6  Layer. 

0.02647 

0.015296 

0.011774 

0.008041 

0.004140 

0.000847 


H2O  Layer. 

0.34600 

0.18470 

0.138228 

0.091959 

o  .  04586 

0.009153 


11.74 
11.44 
II.  08 
I0.8I 


421 


MERCURY  CHLORIDE 


DISTRIBUTION  OF  MERCURIC  CHLORIDE  BETWEEN  WATER  AND  ETHER. 

(Hantzsch  and  Sebalt,  1899.) 

50  cc.  ether  +  50  cc.  sat.  aqueous  HgCl2  solution  were  shaken  together  at 
different  temperatures  and  after  equilibrium  was  established  the  HgCl2  in  each 
layer  determined. 


I/  . 

H20  Layer  (cO- 

(C2H5)2O  Layer  (<:*). 

c* 

0 

0.0056 

O.OI4O7 

0.391 

10 

O.OO66 

O.OI4I5 

0.467 

17-5 

o  .  0090 

0.02150 

0.419 

25 

O.OO95 

O.O2O76 

0.429 

Determinations  by  Skinner  (1892)  at  room  temp,  using  concentrations  of 
HgCl2  in  the  aqueous  layer  varying  from  1.4  to  5.9  per  cent,  gave  a  distribu- 

tion coefficient,  —  =  approximately  0.23. 

DISTRIBUTION  OF  MERCURIC  CHLORIDE  BETWEEN  AQUEOUS  HC1  AND  ETHER 

AT    18°.      (Mylius,  1911.) 

When  I  gm.  of  Hg  as  HgCl2  is  dissolved  in  100  cc.  of  H2O  or  aqueous  HC1  and 
shaken  with  100  cc.  of  ether,  the  percentage  of  the  Hg  which  goes  into  the  ethe- 
real layer  is  as  follows: 

Percentage  Cone,  of  Aq.  HC1        o  (=H20)         i  10  20 

Per  cent  Hg  in  Ether  Layer        69.4  13  0.4          0.2 

DISTRIBUTION  OF  MERCURIC  CHLORIDE  BETWEEN  WATER  AND  TOLUENE  AT  24°. 

(Brown,  1898.) 
Gms.  HgCJ2  per  100  cc.  Cms.  HgClg  per  TOO  cc. 

H2O  QsHsCHs  H2O 

Layer.  Layer.  Layer. 

0.442  0.0270  1.816 

0.732         0.0488         3-766 

0.780      0.0542      3-754 
1.192      0.0812      6.688* 

*.This  solution  saturated. 
Results  at  Dif.  Temperatures.  Results  at  25°. 


yer. 

0.130 

0.292 

0.298 
0.528* 


(Hantzsch  and  Vagt,  1901.) 

Mols.  HgCl2  per  Liter: 
H2O  Layer  fa) .  C6H5CH3  Layer  (<*) . 


£i. 


O 
10 
20 
30 
50 


0.0578 
0-0575 
0.0576 
0.0574 
0.0573 


o . 0047 
o . 0050 
0.0050 
0.0051 
0.0052 


12.35          0.18410  0.01590  ii. 6 

ii. 60          0.09193  0.00807  XI-4 

11.40          0.04593  0.00410  n.  i 

ii. 20          0.02289  0.00211  10.8 

11.25          0.01142  0.00108  10.5 

0.00573  0.00057  10 

Data  for  the  effect  of  Hg(NO3)2  upon  the  distribution  are  given  by  Morse 
(1902).     Results  for  the  effect  of  ZnCl2  are  given  by  Drucker  (1912). 

FREEZING-POINT  DATA  (Solubilities,  see  footnote,  p.  i)  ARE  GIVEN  FOR  THE 

FOLLOWING  MIXTURES: 

Mercuric  Chloride  +  Mercuric  Iodide  (Padoa  and  Tibaldi,  1903.) 

+  Selenium  (Olivari,  1909.) 

+  Sulfur 

+  Nitrobenzene  (Mascarelli,  1906.) 

-j-  o  m  and  p  Nitrotoluene  (Mascarelli,  1906, 1907, 1909.) 

+  Urethan  (      "         1908, 1909.) 

+  a  Nitronaphthalene  (      "         1906, 1907.) 
+  p  Nitrotoluene          (      "         1908.) 
+  «  Nitronaphthalene  (      "         1906, 1907.) 

+  p  Nitranisole  (      "         1906.) 


MERCURY   CINNAMATE 


422 


MERCURY  CINNAMATE   (ic)    (C6H5CH.CHCOO)2Hg.?H2O. 

100  gms.  H2O  dissolve  about  0.03  gm.  mercuric  cinnamate  at  25°.    (De  Jong,  1906.) 
loogms.  H2O  dissolve  about  o.  53  gm.  Hg  cinnamateat  100°.    (Tarugi&  Checchi,  1901.) 

MERCURIC  CYANIDE 


Hg(CN)2. 
SOLUBILITY  IN  WATER. 

Gms.  Hg(CN),  per  100: 
cc.  Sat.  Sol." 


Authonty. 


Gms.H20. 

—  o.45Eutec.  about  u 

13.5  9-3 

15  12  .  5 
2O  ..." 

25  ... 

25  11.27 

IOI.I  53-8S 

One  liter  5.2%  aqueous  NH3  solution  dissolves  204.3  Sms-  Hg(CN)2  at  about  20°. 

(Konowalow,  1898.) 

SOLUBILITY  OF  MERCURIC  CYANIDE  "IN  AQUEOUS  POTASSIUM  CYANIDE  SOLU- 


9-3 
II.  12 

IO.  95  (<Jj,£ 


(Guthrie,  1878.) 

(Timofeiew,  1894.) 

(Marsh  and  Struthers,  1905.) 

(Konowalow,  1898,  1899.) 

(Sherrill,  1903.) 

(Herz  and  Anders,  1907.) 

(Griffiths.) 


TIONS  AT  25 

Mols  per  Liter. 


(Sherrill,  1903.) 

Gms.  per  Liter. 


Hg(CN)2. 
122.6 


'  KCN.  Hg(CN),'.  'KCN. 

0.0493  0.4855  3.21 

0.0985  0.5350  6.41         135.2 

O.I97O  0.6270  12.83         158.4 

The  regularity  of  the  increase  in  solubility  proves  that  the  complex  Hg(CN)j. 
KCN  is  formed  at  the  given  concentrations. 

Data  are  also  given  for  the  distribution  of  Hg(CN)2  between  aqueous  solu- 
tions of  KCN  and  ether  at  25°. 


SOLUBILITY  OF  MERCURIC  CYANIDE  IN  AQUEOUS  SOLUTIONS  OF  METHYL  ALCOHOL, 

(Herz  and  Anders,  1907.) 

In  Aq.  Ethyl  Acetate. 


ETHYL  ALCOHOL  AND  OF  ETHYL  ACETATE  AT  25° 
In  Aq.  Methyl  Alcohol.         In  Aq.  Ethyl  Alcohol. 


Wt.  % 
CH3OH  in 
Solvent. 

Sat.  Sol. 

Gms. 
Hg(CN)2 
per  100  cc. 
Sat.  Sol. 

Wt.  % 
C2H6OH  in 
Solvent. 

<*«of 
Sat.  Sol.  I 

Gms. 
Hg(CN)2  ( 

wt.  % 

ZHsCOOQH 

8  Sat.  Sol. 

Gms. 
Hg(CN), 
oer  100  cc. 
Sat.  Sol. 

10.6 

I 

.0640 

11.02 

0 

I. 

0813 

10-95 

O 

I.oSlO 

10.95 

30.77 

I 

.0484 

12.46 

2O. 

18 

I. 

0339 

8.76 

4-39 

1.0798 

10.83 

47.06 

I, 

,0426 

16.37 

40. 

69 

I. 

0006 

9-O2 

96.76 

1-9374 

2.66 

64 

I 

.0441 

20.48 

70. 

OI 

O. 

9419 

9-57 

IOO 

0.9097 

i.  80 

78.05 

I 

.0484 

24.58 

IOO 

0. 

8552 

8.19 

IOO 

I. 

0762 

34.29 

SOLUBILITY  OF  MERCURIC  CYANIDE  IN  ETHYL  ALCOHOL,  METHYL  ALCOHOL 
AND  IN  MIXTURES  OF  THE  Two. 


In  Ethyl  Alcohol. 

(Timofeiew,  '94;  de  Bruyn,  '92; 

Herz  and  Kuhn,  1908.) 


In  Methyl  Alcohol. 

Trwr  -v 
1907.) 


In  CH3OH+C2H6OH  at  25°. 

(Herz  and  Kuhn,  1908.) 


t°. 

Gms.  Hg(CN)2 
per  loo  Gms. 

t°. 

Gms.  Hg(CN)2 
per  zoo  Gms. 

%  CH3OH 
in 

rfj^fiOf 

Gms.  Hg(CN), 
per  loo  cc. 

Sat.  Sol. 

Sat.  Sol. 

Mixture. 

Sat.  Sol. 

Sat.  Sol. 

0 

8-3 

0 

26.10 

4-37 

0.8618 

9.02 

IO 

8.8 

14-17 

29.17 

10.4 

0.8707 

10.  IO 

20 

9-25 

23-4 

32.01 

41.02 

0.9267 

16.70 

25 

9-53* 

27-4 

31-77 

80.69 

1.024 

28.20 

30 

9-8 

31-7 

32-53 

84.77 

1.034 

29.60 

40 

10.3 

38.1 

33-29 

91-25 

1.052 

30 

*  d. 

,8=0.8552 

44-5 

34-05 

IOO 

1.076 

34-30 

ioo  gms.  of  a  sat.  solution  of  Hg(CN)2  in  a  mixture  of  equimolecular  amounts 
of  CH3OH  and  C6He  contain  10.2  gms.  Hg(CN)2  at  10°,  13  gms.  at  30°  and  15 
gms.  at  50°.  (Dukelski,  1907.) 


423 


MERCURY  CYANIDE 


SOLUBILITY  OF  MERCURIC  CYANIDE  IN  MIXTURES  OF  PROPYL  AND  METHYL 
ALCOHOLS  AND  PROPYL  AND  ETHYL  ALCOHOLS  AT  25°.     (Herz  and  Kuhn,  1908.) 


In  C3H7OH+CH3OH. 


In  C3H7OH+C2H6OH. 


%  C3H7OH 
in  Mixed 
Solvent. 

O 
II. II 

23.80 
65.20 
91.80 

93-75 
96.60 
ioo 


rf«of 
Solvent. 

0.7878 
0.7894 
0.7907 

0.7954 
0.7992 

0-7995 
0.7999 
0.8OO4 


rfyof 
Sat.  Sol. 

I . 0760 
1.0327 
0.9891 
0.8800 
0.8376 
0.8335 
0.8322 
0.8283 


Hg(CN)2 


34-3 

29.52 

24.48 

10.48 

5-04 

4.23 

3.98 

3-44 


o 
8.1 

I7-85 

56.6 

88.6 

91.2 

95-2 

IOO 


0.7867 
0.7886 
0.7902 
0.7926 
0.7973 
0.7979 

0.7986 
0.8004 


rfy  Of 

Sat.  Sol. 

0.8552 
0.8549 
0.8527 
0.8386 
0.8311 
0.8306 
0.8293 
0.8283 


Gms. 

Hg(CN), 

per  ioo  cc. 

Sat.  Sol. 

8.91 

7.90 

7-30 

5-21 

3-87 

3.84 

3.64 

3-44 


ioo  gms.  propyl  alcohol  dissolve  3.79  gms.  Hg(CN)2  at  13.5". 
ioo  gms.  acetonitrile  (b.  pt.  81.6°)  dissolve  9.58  gms.  Hg(CN)s 


(Timofeiew,  1894.) 
>2  at  18°. 
(Naumann  and  Schier,  1914.) 

ioo  gms.  benzonitrile  (b.  pt.  190-1°)  dissolve  1.093  Sms.  Hg(CN)2  at  18°. 

(Naumann,  ^914.) 

SOLUBILITY  OF  MERCURIC  CYANIDE  IN  ANILINE.    (Staronka,  1910.) 


t°  of  Solidification 
Mol.  %  Hg(CN)2  in  sat. 
Solution 


41°       49        58.5    65        77        83.5     84        88.5 


3.7       5.7       7.7       9        14.2     is. 2     19.7     23.4 

The  solid  phases  are  the  unstable  Hg(CN)2.4C6H6NH2  and  the  stable  Hg(CN)2. 
2C6H6NH2  (m.  pt.  about  90°). 
One  liter  sat.  solution  in  ethyl  ether  contains  2.53  gms.  Hg(CN)2  at  25°. 

(Abegg  and  Sherrill,  1903.) 
ioo  gms.  glycerol  dissolve  27  gms.  Hg(CN)2  at  15.5°. 

SOLUBILITIES  OP  MERCURIC  CYANIDE  DOUBLE  SALTS  IN  WATER  AND 

IN  ALCOHOL. 


Double  Salt. 


cold 

1° 


Hg(CN)2.2KCN 
Hg(CN)2.2TlCN 

Hg(CN)2.2TlCN  10° 
2Hg(CN)2.CaBr2.5H2O  cold 
2Hg(CN)2.CaBr2.5H2O  boiling 

Hg(CN)2.KCl.H20  18° 

Hg(CN)2.KBr.2H20  18° 

Hg(CN)2.KBr.2H20  boiling 
Hg(CN)2.BaI2.4H2O      cold 

Hg(CN)2.BaI2.4H2O  boiling 
Hg(CN)2.KI  cold    • 

Hg(CN)2.NaI.2H2O  18° 

Hg(CN)2.SrI2.6Ha6  '18° 


Gms.  per  ioo  Grams. 
Water.       'Alcohol.  " 

22.7 
12.6 

9-7 

100.0 

400.0 

14.81 

7-49 
ioo.o-f 

6.42 
250.0 

6.2 
22.2 


50.0 
IOO.O 


Observer. 
(Fromuller  —  Ber.  u,  oa,  *78.) 

14  41 

(Custer.) 
(Brett.) 


4.42  (Custer.) 

62.5     (00%  Ale.) 

1. 04  (34° B  Ale.)  (Caillot.) 

15.4     (90%  Ale.)          (Custer.) 

25.0    (90%  Ale.) 


14-3 

SOLUBILITY  OF  MECURIC  CYANIDE  IN  ORGANIC  SOLVENTS  AT  i8°-2o°. 

(Sulc,  1900.") 

G.  Hg(CN)2per 
ioo  Gms.  Solvent. 

0.005 
O-OOI 
0.013 
0:001 


Solvent. 

Bromoform 
Carbon  Tetra  Chloride 
Ethyl  Bromide 
Ethylene  Di  Bromide 


Formula. 

CHBr3 
CC14 
C2H5Br 
C2H4Br2 


Data  for  the  ternary  system,  mercuric  cyanide,  phenol,  water  are  given  by 
Timmermans,  1907. 


MERCURY  CYANIDE 


424 


SOLUBILITY  OF  MERCURIC  CYANIDE  IN  PYRIDINE.    (Staronka,  1910.) 

Mols. 

t°.  per  foo  Mols.  Solid  Phase. 
(CN)2+ 


9  7-1 

ii  8.7 

12.2  10.4 

13  II-3 

13-5  12.9 

14-5  13-8 

16.5  15.8 

20.5  15.9 


Mols. 
Hg(CN) 
t°.  per  zoo  M 

22.5      17.3 
28.5      18.4 
32          19-3 

38        20.6 

5ls.  Solid  Phase. 
Hg(CN),.2C8H,N 

Mols. 

t°.  per  100  Mols.  Solid  Phase. 
Hg(CN)2+ 
C5H5N 
56.5     26.6  2Hg(CN)2.3C5H5N 
68          27.5     Hg(CN)2.C6H6N 
70          27.7 
86         29 

42 

22.3 

in 

32 

46 

23 

7 

" 

122.5 

33 

O 

53 

25 

3 

;2Hg(CN)2.3C6H5N 

125 

34 

4 

54-5 

26 

" 

141 

38 

3 

•  O       *3  'V  irT '  J 

100  gms.  pyridine  dissolve  64.8  gms.  Hg(CN)2  at  18 


(Schroeder,  1905.) 


SOLUBILITY  OF  MERCURIC  CYANIDE  IN  QUINOLINE.    (Staronka,  1910.) 


Mols.  Hg(CN)2 

per  100  Mols.  Solid  Phase.               t°. 
Hg(CN)2+C9H7N. 

4.2  Hg(CN)2.3C9H7N           137 

6  "  tr.  pt.  60°          161 

89(61°)             8.2  180 

99(61)               9.2  192 


Mols.  Hg(CN)2 
>  Me 


Solid  Phase. 


45 


per  100 
Hg(CN)2+C9H7N. 

13.2  Hg(CN)2.2C«H7N(?) 

17.4 
22.5 
27.1  « 


MERCURY  FULMINATE  C2HgN2O2. 

One  liter  of  solution  in  water  contains  0.70  gm.  C2HgN2O2  at  12°  and  1.76 
gms.  at  49°.  (Holleman,  1896.) 

MERCURIC  IODIDE  HgI2. 

SOLUBILITY  IN  WATER. 

t°.  Gms.  HgI2  per  Liter.  Observer. 

18  o .  0004  (conductivity  method)        (Kohlrausch,  1904-  05.) 

17.5  0.040  (Bourgoin,   1884.) 

22  0.054  (Rohland,  1898.) 

25  0.0591  (Morse,  1902.) 

SOLUBILITY  OF  MERCUROUS  IODIDE  IN  WATER  AT  25°.     (Sherrill,  1903.) 

One  liter  sat.  solution  contains  2  X  io~7  gms.  Hg2l2,  determined  by  indirect 
method. 

Data  for  the  solubility  of  mercurous  iodide  in  aq.  KI  solutions  at  25°  are  also 
given  by  Sherrill. 

SOLUBILITY  OF  MERCURIC  IODIDE  IN  AQUEOUS  SOLUTIONS  AT  25°. 

(Herz  and  Paul,  1913.) 


In  Aq.  Bal2. 

Mols.  per  Liter. 
'Bal^ H^lT 
0.099  °-°59 
0.748  0.742 
0.978  0.897 
1.508  1.462 


In  Aq.  CaI2. 

Mols.  per  Liter. 


In  Aq.  Nal. 

Mols.  per  Liter. 


CaI2. 
0-053 
0.252 
0.468 
1.799 


HgI2. 
0.050 
0.261 
0.440 
1.706 


Nal. 
0.794 

1.385 
2.225 


HgI2. 
0.412 
0.622 
0-945 


In  Aq.  SrI2. 

Mols.  per  Liter. 
"Sr£ HgTT. 
0.254  0.212 

0.355  0.320 

0-539  0.582 

o . 608         o . 694 


SOLUBILITY  OF  MERCURIC  IODIDE  IN  AQUEOUS  SOLUTIONS  OF  POTASSIUM 

IODIDE  AT  25°.      (Sherrill,  1903;  Herz  and  Paul,  1913.) 
Mols.  per  Liter.  Gms.  per  Liter.  Mols.  per  Liter.  Gms.  per  Liter. 

"KL  HiiT            ICL         Hgi2. '  TL  '  Hgi2.  '         To!  Hgi2.  ' 

0.05  0.025                8.3          11.4  i  0.50  166  227.2 

o.io  0.05                16.6          22.7  1.5  0.75  249  340.8 

0.20  o.io                33.2          45-4  2  i  332  454.5 

0.50  0.25    '           83            113.6  2.5  1.25  415  578 

Data  for  the  distribution  of  mercuric  iodide  between  aq.  KI  solutions  and 

benzene  at  25°  are  given  by  Sherrill,  1903. 


425  MERCURY  IODIDE 


EQUILIBRIUM  IN  THE  TERNARY  SYSTEM  MERCURIC  IODIDE,  POTASSIUM 
IODIDE,  WATER  AT  20°  AND  30°.     (Dunningham  1914.) 

Results  at  20°. 

Results  at  30 

9 

Gms.  per 

zoo  Gms.  Sat.  Sol. 

Gms.  per 

TOO  Gms.  Sat.  Sol. 

Solid  PJia«a» 

KI. 

55* 

KI. 

Hgl,. 

ooiiu  i  nase. 

50-9 

19.3                KI 

60.6 

KI 

44-4 

32-4 

40 

53 

"  +KHgI3 

39 

48 

39-6 

52-7 

KHgla 

37-4 

53.6                "  +KHgj3 

40 

52.2 

" 

37-8 

52.6                 KHglj 

4O.2 

51-2 

" 

35.1 

52-2 

39-3 

50.3 

M 

35-5 

512            KHgI3.H2O 

33-7 

49-8 

" 

26.7 

50.3                   "  +UeT* 

33 

52 

" 

26.6 

49-4                   HgI2 

3!-4 

5i-7 

KHglj.HzO 

23-7 

40  .  2                       " 

29.1 

52.2 

" 

14.9 

22.5 

EQUILIBRIUM  IN  THE  TERNARY  SYSTEM  MERCURIC  IODIDE,  POTASSIUM 
IODIDE,  ETHYL  ETHER  AT  20°.     (Dunningham,  1914.) 

Two  liquid  layers  with  compositions  as  follows,  are  formed: 

Gms.  per  100  Gms.  Upper  Layer.         Gms.  per  100  Gms.  Lower  Layer. 

,  s  , " v  Solid  Phase. 

KI.  Hgl,.  KI.  HgI2. 

i.i  2.8  None  Ki+KHgS 

I.I  2.4  17.6  53.2  KHgl, 

0.8  2.5  16.5  56.1  HgL, 

None  17  58.2  KHgi3+Hgi2 

Data  are  also  given  for  the  four  component  system,  HgI2  +  KI  +  (C2H5)2O  + 
H2O  at  20°.     The  results  are  of  special  interest  since  3  liquid  layers  are  formed. 

SOLUBILITY  OF  MERCURIC  IODIDE  IN  AQUEOUS  ETHYL  ALCOHOL: 


At  1  8°.' 

(Bourgoin.) 

(Herz  and  Knoch 

At  25°. 

—  Z.  anorg.  Ch.  45,  266, 

'05.) 

Solvent. 

Gms.  HgI2 
per  Liter. 

Wt.%  Alcohol 
in  Solvent. 

Hgl2  per  100  cc.  Solution. 

Sp.  Gr.  of 
Solutions  25°/4° 

Millimols. 

Grams. 

Abs.  Alcohol 

11.86 

100 

3 

86 

I 

•754 

O 

•8033 

H2O  +  8o% 

90°  Ale. 

2.857 

95 

.82 

2 

56 

I 

.162 

O 

.8095 

H20+io% 

90°  Ale. 

0.086 

92 

•44 

j 

,92 

0 

•873 

0 

•8154 

86 

•74 

I 

38 

O 

.623 

O 

.8300 

78 

•75 

O 

935 

0 

•425 

O 

.8465 

67 

•63 

o-45 

0 

.204 

0 

.8721 

SOLUBILITY  OF  MERCURIC  IODIDE  IN  AQUEOUS  METHYL  ALCOHOL  AND  IN 
AQUEOUS  ETHYL  ACETATE  AT  25°.    (Herz  and  Anders,  1907.) 

In  Aq.  Methyl  Alcohol.  In  Aq.  Ethyl  Acetate. 

rJS^Z0-  d** of  <*M  of        Gms" Hgl2     wt-  %  CHr  4« of          Gms'  Hgl« 

CHjOH  in  0  ¥  o  -¥  ^  per  zoo  cc.          COOC2H5  i8     ,  per  100  cc. 

Solvent.  SoFvent.  Sat.  Sol.          Sat.  Sol.  in  Solvent.  Sat.  Sol.  Sat.  Sol 

47.06  0.9186  0.9187  0.044  4-36  0-9973  0-013 

64  0.8800  0.8834  0.158  96.74  0.9063  1.87 

78.05  0.8489  0.8519  0.445  I0°  0.9011  1.09 

100  0.7879  0.8155  2.590 

100  gms.  sat.  solution  in  95%  alcohol  (dis  =  0.8126)  contain  0.72  gm.  HgI2 
at  O°,  1. 06  gms.  at  25°  and  2.15  gms.  at  50°.  (Reinders,  1900.) 


MERCURIC  IODIDE 


426 


Alcohol. 

Methyl 


tt 

Ethyl 


Propyl 

Amyl 
tt 

u 

Isopropyl 
Isobutyl 


SOLUBILITY  OF  MERCURIC  IODIDE  IN  ALCOHOLS. 

Formula. 

<in  Pr  nf  Gms.HgI2per 
*°-                  Solution.        I??(im,s-         Observer. 

CHsOH 

15-20 

0.799 

nwuuufe 

3  .  24       (Rohland.) 

" 

19 

3  •  7          (Timofeiew.) 

tt 

19-5 

3.16       (de  Bruyn.) 

11 

23 

3  .  98       (Beckmann.) 

" 

66  (b.  pt.) 

... 

6.512     (Sulc.) 

CjjHsOH 

15-20 

O.SlO 

1  .  42       (Rohland.) 

tt 

18 

1  .  48       (Bourgoin.) 

t( 

19 

1  .  86       (Timofeiew.) 

u 

19.5 

.... 

2  .  09       (de  Bruyn.) 

" 

25 

0.803 

2  .  19       (Herz  and  Knoch.) 

u 

78  (b.  pt.) 

. 

4.325     (Sulc.) 

CsH7OH 

15-20 

0.816 

0.826    (Rohland.) 

" 

19 

1.25       (Timofeiew.) 

C&HnOH 

13 

0  .  66       (Laszcynski  .) 

tt 

71 

... 

3-66 

(i 

IOO 

5-30 

tt 

133.5 

... 

9-57 

(CH3)2CH.OH 

81  (b.  pt.) 

... 

2.266    (Sulc.) 

(CH3)2CHCH2OH 

22.5 

.  .  . 

0.51       (Timofeiew.) 

(i 

105-107  (b. 

Pt.)     .  .  . 

2-433     (Sulc.) 

SOLUBILITY  OF  MERCURIC  IODIDE  IN  MIXTURES  OF  ALCOHOLS  AT  25°. 

(Herz  and  Kuhn,  1908.) 

In  CH3OH+C2H6OH.          In  C3H7OH+CH3OH.        In  C3H7OH+C2H5OH. 


Per  cent 

d      of 

Gms.HgI2  Percent 

d     of 

Gms.  Hglj,    Percent 

A__  nf      Gms.  Hel, 

CH3OH  in 
Solvent. 

-3L5 

Sat.  Sol. 

per  loo  cc 
Sat.  Sol. 

C3H7OH  in 
Solvent. 

Sat.  Sol. 

per  loo  cc 
Sat.  Sol. 

.  C3H7OHin        fr          perioocc 
Solvent.       Sat-  So1-       Sat.  Sol. 

O 

0.8038 

I 

.80 

O 

0.8156 

3.l6 

0 

0 

8038 

.80 

4 

•37 

0.8039 

I 

•93 

II.  II 

8.1 

0 

8036 

•73 

IO 

.40 

0.8046 

2 

.08 

23.80 

0.8155 

3.04 

17-85 

0 

8043 

•65 

41 

.02 

0.8077 

2 

•32 

65.20 

56.6 

0 

8057 

•55 

80 

.69 

0.8131 

2 

.89 

91.80 

O.SlOI 

i.6g 

88.6 

84 

•77 

0.8140 

2 

.96 

93-75 

O.SlIO 

1.67 

91.2 

0 

8099 

.52 

91 

.25 

0.8146 

2 

•98 

96.60 

0.8108 

1-53 

95-2 

0 

8108 

•  44 

IOO 

0.8156 

3 

.16 

IOO 

0.8116 

1.42 

IOO 

0 

8116 

.42 

SOLUBILITY  OF  MERCURIC  IODIDE  IN  ACETONE  IN  ETHYL  ACETATE 
AND  IN  BENZENE. 

(Sulc;  Krug  and  McElroy  —  J.  Anal.  Ch.  6,  186,  '92;  Laszcynski  —  Ber.  27,  2285,  '94.) 


In  Acetone. 


In  Ethyl  Acetate.  In  Benzene. 


t°. 

Cms.  HgI2 
per  loo  Gms. 
(CH3)2CO. 

Gms.  HgI2 
t°.           per  100  Gms. 
CH3COOC2H6. 

I 

2.83 

—  20 

1.49 

18 

3-36 

+17-5 

1-56 

25 

2.09  (K.andMcE.) 

21 

1.64 

40 

4-73 

40 

2.53 

58 

6.07 

55 

3-i9 

56  (b.pt.)  3.  249  (Sulc.) 

76 

4-31 

74-78  (b.pt.)  4. 20  (Sulc.) 


Gms.  HgI2 
per  loo  Gms. 


15  0.22 

60  0.88 

65  0-95 

84  1.24 

8o(b.pt.)o.825(SulcO 


427 


MERCURY  IODIDE 


100  gms.  acetone 
benzene 
chloroform 
acetone 


dissolve  2.04  gms.  HgI2  at  23°.       (Beckmann  and  Stock,  1895.) 
0.25     ' 
0.07 


ethyl  acetate 


2 

3-09 

1.47 


(red)  at  25°. 
(yellow)  at  25°. 
at  1 8°. 


(Reinders,  1900.) 
(Naumann,  1910.) 


One  liter  sat.  solution  in  benzene  contains  2.24  gms.  HgI2  at  25°. 

(Abegg  and  Sherrill,  1903.) 


Gms.  Hglj 
t°.             per  100  Gms. 
Aniline. 

-11.48* 

...    c 

-    6-5 

23-35 

+    0-4 

28.69 

I7.8 

42.85 

21.  1 

47-55 

26.9 

55-47 

30.1 

62.05 

36.2 

75-8o 

42.9 

96.49 

46.  8f 

SOLUBILITY  OF  MERCURIC  IODIDE  IN  ANILINE. 

(Pearce  and  Fry,  1914.) 
Solid  Phase. 


+HgI2(red) 


Gms.  HgI2 
t°.          per  zoo  Gms. 

Aniline. 

48.8 

128.1 

63.6 

163.8 

70.82 

184.1 

76.2 

2OI  .6 

95-9 

246.7 

io8f 

"5-7 

281.8 

137.2 

285.2 

181.1 

297.9 

199.1 

863.2 

Solid  Phase. 
HgI2  (red) 


"  +HgI2  (yellow) 
HgI2  (yeUow) 


*  Eutec. 


t  Tr.  pt. 


Additional  data  on  this  system  are  also  given  by  Staronka,  1910. 

Data  for  the  solubility  of  mercuric  iodide  in  nitrobenzene  and  in  p  nitrotoluene, 
determined  by  the  synthetic  (sealed  tube  method),  are  given  by  Smits  and  Bak- 
horst  (1915).  The  transition  point  of  HgI2,  red  to  yellow,  was  found  to  be  at 
1.68  mol.  per  cent  HgI2  and  127.5°  m  nitrobenzene  and  1.81  mol.  per  cent  HgI2 
and  128°  in  p  nitrotoluene.  The  interesting  part  of  the  investigation  is  the 
characteristic  prolongation  of  the  melting  line  above  the  transition  point.  Similar 
data  for  the  solubility  of  mercuric  iodide  in  nitrobenzene,  m  nitrotoluene,  p  nitro- 
toluene and  in  nitronaphthalene,  determined  by  the  freezing-point  method, 
using  a  Beckmann  apparatus,  are  given  by  Mascarelli  (i9o6a).  Observations 
on  the  appearance  and  color  changes  of  the  HgI2  are  given. 


SOLUBILITY  OF  MERCURIC  IODIDE  IN  CARBON  DISULFIDE. 

(Linebarger,  1894;  Arctowski,  1894,  1895-96.) 


116 

93 

86.5 

10 


Gms.  HgI2 

per  100  Gms. 

Solution. 

O.OI7 
0.023 
0.024 
0.107 


-  5 
o 

+  s 

10 


Gms.  Hgl, 

per  100  Gms. 

Solution. 

O.I4I 
0.173   ' 
0.207 
0.239 


15 
20  • 

25 
30 


Gms.  Hgl, 

per  100  Gms. 

Solution. 

0.271 
0.320 
0.382 
0-445 


One  liter  sat.  solution  of  mercuric  iodide  in  CS-j  contains  3.127  gms.  at  15° 

(Dawson,  i 

One  liter  sat.  solution  of  mercuric  iodide  in  CCU  contains  0.170  gm.  at  18 

(Dawson,  i 

Data  are  also  given  by  Dawson  for  the  distribution  of  HgI2  between  aqueous 
solutions  of  KI  and  CS-j  at  15°  and  aqueous  solutions  of  KI  and  CCU  at  18°. 

100  cc.  anhydrous  hydrazine  dissolve  69  gms.  HgI2  with  precipitation  of  Hg 
at  room  temp.  (Welsh  and  Broderson,  1915.) 


MERCURY  IODIDE 


428 


SOLUBILITY  OF  MERCURIC  IODIDE  IN  SEVERAL  ORGANIC  SOLVENTS. 

(Sulc  —  Z.  anorg.  Ch.  25,  401,  'oo.) 
Solvent. 

Chloroform 

Chloroform 

Bromoform 

Tetra  Chlor  Methane 

Tetra  Chlor  Methane 

Ethyl  Bromide 

Ethyl  Bromide 

Ethylene  Di  Bromide 

Ethyl  Iodide 

Ethylene  Di  Chloride 

Iso  Butyl  Chloride 

Methyl  Formate 

Ethyl  Formate 

Methyl  Acetate 

Acetal 

Epi  Chlor  Hydrine 

Hexane 


Formula. 

+  o                         Gms.Hgl2peric 
Gms.  Solvent. 

CHC13 

18-20 

O.O4O 

CHC13 

61  (b.  pt.) 

O.l63 

CHBr3 

1  8-20 

0.486 

CC14 

18-20 

0.006 

CC14 

75  (b.  pt.) 

0.094 

C2H5Br 

18-20 

0.643 

C2H5Br 

38°  (b.  pt.) 

o-773 

C2H4Br2 

18-20 

0.748 

C2H5I 

18-20 

2.041 

G.UA 

8S.S0  (b.  pt.) 

i.  200 

(CH3)0.CHCH2C1 

69 

0.328 

HCOOCH3 

36-38     " 

1.166 

HCOOC2H5 

5^-55     " 

2.150 

CH3COOCH3 

56-59     " 

2.500 

CH3CH(OC2H5)2 

i°S 

2.OOO 

CHg.O.CH.CItjCl 

117         " 

6.II3 

C,H14 

67 

0.072 

SOLUBILITY   OP   MERCURIC   IODIDE   IN   ETHER  AND   IN   METHYLENB 

IODIDE. 

In  Methylene  Iodide. 


In  Ether. 

(Sulc;  Laszcynski.) 


t°. 


Cms.  H 
Cms. 


o  0.62 

36  0.97 

35  (b.pt.)  0.47  (Sulc) 


(Retgers  —  Z.  anorg.  Ch.  3,  253,  '93.) 


15 

IOO 

180 


Gms.  Hgl2  per  i< 
Cms.  CH2Ia. 

2-5 

16.6 
58.0 


SOLUBILITY  OF  MERCURIC  IODIDE  IN  FATTY  BODIES. 

(Mehu  —  J.  pharm.  chim.  [5]  12,  249,  '85.) 

t-o      Gms.  HgI2  per 
•  '  100  Gms.  Solvent. 


Solvent. 

Bitter  Almond  Oil 
Bitter  Almond  Oil 
Castor  Oil 
Castor  Oil 
Nut  Oil 


25 

100 

25 

100 

ioo 


1.3 
4.0 

20.  0 

1.3 
ioo  grams  oil  of  bitter  almonds  dissolve  5.0  grams  HgI2.KI  at  25°. 


Solvent. 

to        Gms.  HgI2  p 
*     ioo  Gms.  Solve 

Vaseline 

25 

0.025 

Vaseline 

IOO 

0.20 

Poppy  Oil 

25 

1-0 

Olive  Oil 

25 

0-4 

Carbolic  Acid 

IOO 

2-0 

on. 


SOLUBILITY  OF  MERCURIC  IODIDE  IN  OILS. 

(Anon,  1903,  1904.) 


Oil 


Castor 
Walnut 
Linseed       " 
Cod  Liver  " 


Gms.  Hgl, 

per  too  cc. 

Oil. 

I.QO 
1.29 
1.23 

Q-545 


oa. 

Peanut  OU 
Olive      " 
Almond  " 
Vaseline 


Gms.  Hglj 
per  IOQCC. 

oa. 
0.52 


0.26 


429  MERCURY  IODIDE 

SOLUBILITY  OF  MERCURIC  IODIDE  IN  PYRIDINE. 

(Determinations  from  —50°  to  98.5°  made  by  saturating  the  solvent  at  con- 
stant temperatures  are  given  by  Mathews  and  Ritter  (1917).  Measurements  of 
the  points  of  solidification  of  various  mixtures  of  the  two  components,  covering 
the  range  from  IO°  to  135°,  are  given  by  Staronka  (1910). 

Cms.  Hgl,  Cms.  HgI2 

t°.  per  100  Cms.  Solid  Phase.  t°.  penooGms.      Solid  Phase. 

Sat.  Sol.  Sat.  Sol. 

—  50  1.93      HgI2.2C5H6N  90.08  61.43    Hg 

-31.5  4.27  "  ioo  65.72  " 

'-lo  10.28  "  105  6^.89  " 

.  —  o.i  14-85  "  io7m.pt.  72.09  " 

-f-  8.83  18.42  «  105  75.67  " 

20.02  24.40  "  ioo  79-73 

25.55  27-9°  "  9°  84.16  " 

40.08  37-64  "  87  EutCC.          85.17        "  +HgI2.C6H5N 

50.02  43-15  "  IOO  86  Hgl-j.CsHsN 

60.07  48.29  "  120  87.16 

80.05   57.60   "    135      88.78 

SOLUBILITY  OF  MERCURIC  IODIDE  IN  QUINOLINE. 

(Staronka,  1910.) 

Mols.  HgI2  K  Mols.  HgI2' 

t°.  per  ioo  Mols.        Solid  Phase.  t°.  rper  ioo  Mols.  "  Solid  Phase. 

HgI2+C,H7N.  HgI2+C9H7N. 
IOO                       4.7         ,HgI2.2C,H7N                   l6o  37.7          HgI2.C»H7N 

115.5  9-i  J65  4i-6 

133-5  13-2  165  43 

138  23.1  170  48.8 

145  26.7         Hgi2.c,H7N  169.5  49-5 

153     .          3*-4  166.5  54-4 

Fusion  point  data  for  mixtures  of  HgI2  +  I  are  given  by  Olivari,  1908. 

MERCURIC   IODIDE   Diamine   (NH3)2HgI2. 

Data  for  the  solubility  of  diamine  mercuric  iodide  in  aqueous  ammonia  solu- 
tions at  20°  are  given  by  Francois  (1900).  The  solid  is  not  stable  in  solutions 
containing  less  than  48  gms.  NH3  per  liter. 

MERCURY  NITRATE   (ic)   Hg(NO3)2,  (oils)  Hg2(NO3)2. 

ioo  gms.  anhydrous  lanolin  (m.  pt.  about  46°)  dissolve  1.15  gm.  Hg(NO3)2 
at  45°.  (Klose,  1907.) 

ioo  cc.  anhydrous  hydrazine  dissolve  about  2  gms.  Hg2(NO3)2  with  precipita- 
tion of  Hg  at  room  temp.  (Welsh  and  Broderson,  1915.) 

MERCURY  OXIDE  HgO. 

SOLUBILITY  IN  WATER. 

(Schick,  1903.) 
t°.  Gms.  per  1000  cc.  Solution. 


25  0.0518  yellow  HgO  0.0513  red  HgO 

ioo  0.410    yellow  HgO  0.379  red  HgO 

At  25°  the  mixtures  were  constantly  agitated  for  4  days  or  longer.  At  100° 
the  solutions  were  boiled  and  stirred  for  5  hours.  A  longer  period  would  prob- 
ably have  caused  better  agreement  between  the  red  and  yellow  HgO. 

One  liter  H2O  dissolves  0.05  'gm.  HgO  (red,  large  grains)  at  25°.      (Hulett,  1901.) 
One  liter  H2O  dissolves  0.15  gm.  HgO  (red,  finest  grains)  at  25°. 


MERCURY  OXID.B 


430 


SOLUBILITY  OF  MERCURIC  OXIDE  IN  AQUEOUS  HYDROFLUORIC  ACID  AT  25°. 

(Jaeger,  1901.) 

Cms.  Hg  per 
9.6  cc.  Sat.  Sol. 

0.12  O.O242 

0.24  0.0475 

0.57  O.I2IO 


Normality 
of  HF. 


I. II 
2.17 


0.2247 
0.4976 


Gm.  Atoms  Hg 
per  Liter. 

O.OI258 

0.0247 

0.0629 

0.1168 

0.2586 


MERCURY  DiPHENYL  Hg(C6H5)2. 

Fusion-point  data  for  mixtures  of  Hg(C6H6)2  +  Sn(C6H5)4  are  given  by  Cambi 
(1912). 

MERCURY  SELENITE  HgSeO3. 

SOLUBILITY  IN  AQUEOUS  $9DiuM  SELENITE  SOLUTIONS  AT  25°. 

(Rosenheim  and  Pritze,  1909.) 


Normality 

of  Na,SeOj 

Solution. 

0.0625 

0.125 

0.25 


Cms.  HgSeO3 

per  100  Cms. 

Sat.  Sol. 

0.18 

0.32 

o-53 


Normality 

NajSeO,  of 

Solution. 

o-S 

i 

2 


Cms.  HgSeOj 

per  100  Gms. 

Sat.  Sol. 

0.70 

1-39 
2-73 


MERCURY  SULFATE   (ic)   HgSO4. 
EQUILIBRIUM  IN  THE  SYSTEM,  MERCURY  OXIDE,  SULFUR  TRIOXIDE,  WATER 

(Hoitsema,  1895.) 

Results  expressed  in  molecules  per  sum  of  100  molecules  of  the  three  com- 
ponents of  the  system.     The  mixtures  were  rotated  for  3  hours  or  longer. 


Results  at  25°. 


Results  at  50° 


H20. 

S03. 

HgO. 

ouuu  niase. 

H20. 

S03. 

HgO. 

98 

•5 

I 

.24 

o-33 

3HgO.SO, 

98 

•9 

0 

.96 

0 

•  17 

96 

.6 

2 

•49 

0.92 

* 

96 

3 

•05 

o 

•93 

94 

•4 

3 

•93 

i.6S 

" 

93 

.2 

4 

.92 

I 

.90 

93 

•9 

4 

.24 

1  '85  I 

3HgO.SOs  and 

92 

.8 

5 

.10 

2 

.09 

94 

•4 

4 

•52 

2.12) 

3HgO.2SO3.2H2O 

92 

.8 

5 

.16 

2 

.06 

93 

•4 

4 

•65 

1.94 

3HgO.2SOj.2HjO 

92 

•5 

5 

•34 

2 

.12 

92 
92 

•9* 
•9 

4 
5 

.81 
.11 

2.29 
1.98 

3HgO.SO, 
3Hg0.2S03.2H20 

92 

.2 

5 

•57 

2 

.20 

92 

•3* 

5 

.20 

2-54 

3HgO~SO3 

92 

.1 

5 

•75 

2 

.11 

92 

•3 

5 

•58 

2.09 

3Hg0.2S03.2HjO 

92 

5 

.80 

2 

.16 

92 
91 

.1 
•9 

5 
5 

.81 
•97 

2.08 
2.90 

3HgO.S03 

QI 

.2* 

6 

•27 

2 

•56 

QI 
QI 

•9 
•3 

6.15 
6.54 

2.05 
2.13 

3Hg0.2S03.2H20 

QI 

•5 

6 

•34 

2 

.19 

91 

.2 

6 

•77 

2.02 

HgO.SOj.HjO 

QI 

•3* 

6 

•37 

2 

•30 

QI 

•3 

6 

.90 

1.  80 

« 

QI 

.6 

6 

.69 

I 

•75 

QI 

•3 

7 

.67 

1.  01 

" 

QI 

.1 

8.32 

0 

•57 

QI 

•3 

7 

.84 

0.89 

HgO.SO,.HjO  and 

90 

•5 

9 

.11 

0 

•4 

QI 

8 

•36 

0.69 

HgO.SO, 

89 

.6 

10 

.2 

0 

•23 

QO 

•5 

8 

•95 

o-53 

" 

86 

•7 

13 

.2 

0.06 

89 

.2 

10 

.6 

O.22 

HgO.SO, 

31 

.6 

68 

•4 

0 

•03 

75 

.8 

24 

.2 

trace 

" 

39 

.2 

60 

•7 

trace 

M 

. 

Solid  Phase. 
sHgO.SO, 


(  3HgO.S03  and 
j     3HgO.2SOa.2HjO 
3HgO.2S03.2HjO] 

3HgO.SO3  and 

HgO.SO, 

(  3HgO.2SOj.2HjO 
(      and  HgO.SO, 
HgO.SO, 


Indicates  unstable  equilibrium 


431  MERCURY   SULFATE 

MERCUROUS   SULFATE  HglSO4. 

SOLUBILITY  IN  WATER,  IN  SULFURIC  ACID  AND  IN  POTASSIUM  SULFATE  AT  25°. 

(Drucker,  1901;  Wright  and  Thomson,  1884-85;  Wilsmore,  1900.) 
Solvent.  HgsSO.perLfter. 


I  Gm.  Mol.  Gms. 

Water  11.71  io~4  o .  58   (o.47  w.  and  T.,  0.39  w.) 

Aq.  H2SO4  (  i  .96  gms.  per  liter)  8.31     "  0.41 

Aq.  H2S04  (  4  •  90  gms.  per  liter)  8.78  o .  44 

Aq.  H2SO4  (  9.80  gms.  per  liter)  8.04  0.40 

Aq.  K2SO4  (34-87  gms.  per  liter)  9 . 05  o .  45 

SOLUBILITY  OF  MERCUROUS  SULFATE  IN  WATER  AT  DIFFERENT  TEMPERATURES. 

(Barre,  1911.) 

Gms.  per  100  Gms.  Sat.  Sol. 

Solid  Phase. 


Hg2S04. 

16.5        o-°55      0.008 
33         0.060      0.018       " 
50         0.065      °-°37 
75         0.074      0.063 
100         0.092      0.071 

The  mixtures  were  kept  at  constant  temp,  but  not  constantly  agitated.  By 
successive  treatment  of  a  given  amount  of  Hg2SO4  with  HjO,  it  is  gradually 
converted  to  an  almost  insoluble  basic  salt,  Hg2O.Hg2SO4.H2O. 

SOLUBILITY  OF  MERCUROUS  SULFATE  IN  AQUEOUS  POTASSIUM  SULFATE 

SOLUTIONS.       (Barre,  1911.) 

Results  at  15°.  Results  at  33°.  Results  at  75°.* 

Gms.  per  100  Gms.  Sat.  Sol.     Gms.  per  100  Gms.  Sat.  Sol.  ,    Gms.  per  100  Gms.  Sat.  Sol. 


K2S04. 

Hg2S04.- 

H2SO4(free).     K,SO4. 

HgtS04.  H2S04(free). 

K,S04. 

HfcSO*.  HjSO^freej" 

2.90 

0.0475 

O. 

0080 

2.94 

O 

.0677 

0.0250 

3 

.10 

0.1344 

0.1684 

5-70 

0.0703 

0. 

0093 

5-68 

0 

.1015 

0.0350 

5 

•75 

O.2I2O 

0.2135 

8.22 

0.0912 

0. 

0098 

8.30 

o 

.1364 

0.0441 

8 

•So 

0.2951 

0.2514 

8.77 

0.0994 

10.70 

0 

.1724 

0.0438 

13 

.20 

0.4610 

0.2503 

9-44, 

'0.1080 

0. 

OIIO 

11.90 

0 

.1902 

0.0420 

I? 

•30 

o  .  6440 

0.2225 

MERCURY  SULFIDE  HgS. 

One  liter  H2O  dissolves  0.054  X  IO"6  m°l«-  HgS  =  0.0000125  gm.  at  18°. 

(Weigel,  1906,  1907.     See  also  Bruner  and  Zawadzki.) 

Hexamethyl  MELLITIC  ACID   Ester  C6(COOCH3)6. 

Data  for  the  ternary  system  hexaniethyl  mellitic  acid  ester,  phenol  and  water 
are  given  by  Timmernians  (1907). 

MENTHOL   Ci0H19OH. 

One  cc.  of  95%  alcohol  dissolves  about  5  gms.  menthol  at  room  temp. 

(Greenish  and  Smith,  1903.) 

FREEZING-POINT  DATA  (Solubility,  see  footnote,  p.  i)  ARE  GIVEN  FOR  THE 
FOLLOWING  MIXTURES. 

Menthol  +  Ethylene  bromide  (Dahms,  1895.) 

"        +  Menthane  (Vanstone,  1909.) 

"        +  Methyl  urethan.  (Scheuer,  1910.) 
"        -j-  Naphthalene 

+  p  Toluidine  (Pawlewiki,  1893.) 

SOLIDIFICATION  POINTS  OF  MIXTURES  OF  MENTHOL  AND  SALOL.  (BeUu«ci,i9i2,i9i3.) 

t°  of  Solidification  42    30 . 5     28     28.5    32.5    41.9 

Gm.  Salol  per  100  Gm.  Mixture       100    80        60    40        20         o 


METHANE 
METHANE  CH4. 

432 

SOLUBILITY  IN  WATER. 

(Winkler,  1901.) 

t° 

0. 

0'. 

q. 

t°. 

0. 

0'. 

q. 

0 

0 

•05563 

0.05530 

0 

.00396 

40 

0 

.02369 

o 

.02198 

0.00159 

5 

O 

.04805 

0.04764 

O 

.00341 

50 

0 

.02134 

0 

.01876 

0.00136 

10 

0 

.04177 

0.04127 

0 

.00296 

60 

o 

.01954 

0 

.01571 

O.OOII5 

15 

0 

.03690 

0.03628 

O 

.00260 

70 

0 

.01825 

o 

.01265 

0.00093 

20 

o 

.03308, 

0.03233 

0 

.OO232 

80 

0 

.01770 

0 

.00944 

0.00070 

25 

0 

.03006 

0.02913 

0 

.00209 

90 

o 

•01735 

0 

•00535 

o  .  00040 

30 

0 

.02762 

0.02648 

O 

.00191 

100 

0 

.01700 

o 

0 

For  the  values  of  /3,  /3'  and  q  see  Ethane,  page  285. 


SOLUBILITY  OF  METHANE  IN  METHYL  ALCOHOL  AND  IN  ACETONE. 

(Levi,  1901,  1902.) 

In  methyl  alcohol  /  (Ostwald  expression,  see  page  227)  =  0.5644  —  0.0046  /  — 
0.00004  f2. 

In  acetone  /  (Ostwald  expression)  =  0.5906  —  0.00613  t  —  0.000046  P. 
From  which  are  calculated  the  following  values: 


In  Methyl  Alcohol.                                             In 

o        0.5644             40       0.3164             o       0.5906 
10       0.5144             50       0.2344           10       0.5247 

20          0.4564                 60         0.1444               2°         0.4496 
30          0.3904                 70         0.0464              30         0.3653 

SOLUBILITY  OF  METHANE  IN  SEVERAL  ALCOHOLS  AND 

(McDaniel,  1911.) 
Solvent.                      f.       AbskCoef'      Bunsen        SolveQt             <.„ 

Acetone. 

40       0.2718 
50       0.1691 
60       0.0572 

OTHER  SOLVENTS. 

Abs.  Coef.      Bunsen 
A.             Coef.0. 

Alcohol: 

Methyl  (99%) 

22 

.  i 

0.4436 

o. 

4102 

Toluene 

40. 

I 

0 

•4675 

o  .  4080 

" 

30 

.  2 

0.4278 

o. 

3883 

u 

So. 

2 

0 

•4545 

0.4013 

" 

40 

0.3938 

0. 

3436 

tt 

60 

0 

.4502 

0.3690 

" 

49 

.8 

0.2695 

0. 

2278 

m  Xylene 

21. 

I 

0 

.5146 

0.4778 

Ethyl  (99.8%) 

22 

.2 

0.4628 

0. 

4282 

tt 

30. 

5 

0 

.5028 

0.4529 

" 

30 

.1 

0.4503 

0. 

4051 

tt 

50 

0 

•4972 

0.4203 

n 

40 

0.4323 

0. 

3771 

(l 

60 

0 

.4870 

0.3992 

Isopropyl 

21 

•  5 

0.4620 

0. 

4275 

Hexane 

22. 

2 

0 

•6035 

0.5585 

" 

29 

•9 

0.4532 

o. 

4081 

11 

40. 

2 

0 

•5320 

0.4639 

" 

40 

0.4400 

0. 

3837 

n 

49- 

7 

0 

.5180 

0.4380 

tt 

60 

•3 

0.4244 

o. 

3478 

" 

60 

0 

•4964 

0.4068 

Amyl 

22 

0.4532 

0. 

4196 

Heptane 

22. 

2 

0 

•7242 

0.6720 

tt 

30 

.1 

0-4444 

o. 

4002 

" 

30. 

I 

0 

.6906 

0.6221 

Benzene 

22 

.1 

0.4954 

0. 

4600 

11 

40 

0 

.6675 

0.5820 

" 

35 

0.4484 

0.3976 

Pinene* 

20 

0 

.4888 

0.4565 

" 

40 

.  i 

0.4198 

0. 

3661 

" 

30. 

X 

0 

.4620 

0.4163 

" 

49 

•9 

0-3645 

0.3081      " 

39- 

I 

0 

•4472 

0.3914 

Toluene 

25 

0.4852 

o. 

4450 

' 

45 

0 

.4440 

0.3811 

" 

0.4778 

o. 

4300 

" 

55- 

2 

0 

•3694 

0.3076 

*  b.  pt.  155-160*. 

Abs.  coef.  A  =  vol.  of  methane  absorbed  by  unit  vol. 
stated. 

For  definition  of  Bunsen  abs.  coef.  /3  see  carbon  dioxide, 


of  solvent  at  temp 
p.  227. 


433 


METHANE 


SOLUBILITY  OF  METHANE  IN  ETHYL  ALCOHOL. 

(Bunsen,  1877,  1892.) 
t°.  2°.  6.4°.  11°.  15°.  19°.  23.5°. 

Abs.  coef.  /3  (found)  0.51721  0.50382  0.49264  0.48255  0.4729  0.4629 

from  which  the  following  formula  was  calculated. 

Bunsen  abs.  coef.  /3  for  methane  =  0.522745  —  0.00295882  t  —  0.0000177  /*. 

The  solubility  of  methane  in  aq.  H2SO4  (Christoff,  1906)  in  terms  of  the  Ostwald 
solubility  expression  fa.  In  95.6%  H2SO4,  ko  =  0.03303;  in  61.62%  H2SO4, 
/2o  =  0.01407;  in  35. 82%  H2SO4,  fa  =  0.01815;  in  H2O,  /20  =  0.03756. 

The  solubility  of  methane  in  ethyl  ether,  in  terms  of  the  Ostwald  Solubility 
Expression  /  (see  p.  227),  is  1.066  at  o°  and  1.028  at  10°.  (Christoff,  1912.) 

The  coef.  of  absorption  /3  (Bunsen)  of  methane  in  petroleum, (Russian)  is  0.144 

at  10°  and  O.I3I  at  2O°.  (Gniewosz  and  Walfisz,  1887.) 

Fusion-point  data  are  given  for  diphenyl  methane  +  naphthalene  by  Miolati, 
(1892)  and  for  diphenyl  methane  +  phenol  by  Paterno  and  Ampola  (1897). 

Triphenyl  METHANE   CH(C6H6)3. 

SOLUBILITY  IN  ANILINE. 

(Hartley  and  Thomas,  1906.)  / 


By  synthetic  method,  see  page  16. 

Gms. 
CH(C6H5)3  Mol.  per                  o  r  . 
t°.      per  100         cent                     pg££                     t° 
Gms.  So-  CH(CeHfi)3. 

Gms. 

CH(C6H5); 

per  loo 
Gms.  So- 

*  M-r    Ps£ 

CH(C«H6)3.         Pnase' 

lution. 

lution. 

23.0 

5 

•4 

i 

•85 

CH(C6H5)3.CaH6NH2 
rhombs 

7i 

•3 

67 

•9 

44 

.6    OT<q»fcCgiNHj 

35-3 

9 

•5 

3 

.8 

7i 

.6 

71 

•7 

49 

.1 

43-o 

13 

•5 

5 

.6 

M 

7i 

.2 

76 

.3 

55 

I                     " 

S^-i 

21 

•9 

9 

•7 

" 

70 

.6 

78 

•3 

57 

•9 

61  .4 

36 

•5 

.8 

•I 

7i 

.6 

82 

.1 

63 

.  5  CH(CflH6)3  monoclinic 

66.0 

47 

.2 

25 

•4 

M 

74 

•3 

84 

•9 

68 

.2 

68.7 

54 

.8 

3i 

.6 

w 

82 

.1 

9i 

•7 

80 

•9 

70.1 

64 

.6 

40 

•9 

M 

87 

•3 

96 

.1 

90 

.2 

SOLUBILITY  OF  TRI  PHENYL  METHANE  IN  BENZENE. 


(Linebarger  —  Am.  Ch.  J.  ij*  45,  '93.) 

Gms. 

r  Solid  Phase. 


(Hartley  and  Thomas.) 


Gms. 


Mol. 


CeH6. 

Solution. 

3 

•9 

3 

.90 

CflH6+CH(CaH6)3.C6He     33 

12 

.6 

4 

•4 

4 

•  o 

4 

.06 

CH(C6H6)3.C0H6                  49 

•4 

24 

.0 

8 

.8 

12 

•5 

5 

.18 

65 

.6 

38 

•9 

17 

.2 

16 

.1 

6 

•83 

73 

.8 

57 

•5 

30 

.2 

19 

•4 

7 

.24 

77 

.1 

67 

•4 

39 

•7 

23 

.1 

8 

•95 

77 

•9 

76 

•3 

So 

•7 

37 

•  5 

10 

.48 

(Cft?3H(cS             77 

•5 

80 

.2 

56 

•4 

42 

.0 

*9 

.61 

T  v^rn,Mi"5/3                            > 

CH(CoH6)3                            7° 

.2 

84 

.1 

62 

.8 

44 

.6 

22 

.64 

74 

.6 

87 

•5 

69 

.i 

5° 

.1 

30 

.64 

76 

.0 

89 

.0 

72 

.2 

55 

•5 

40 

•51 

78 

.8 

90 

•5 

75 

•3 

71 

.0 

140 

.00 

82 

•3 

93 

.1 

81 

•3 

76 

.2 

319 

.67 

86 

.6 

95 

•7 

87 

.8 

monoclinic 


Hartley  and  Thomas  call  attention  to  the  inaccuracy  of  Linebarger's  results  and 
to  the  correctness  of  the  determinations  of  Kuriloff  (18973).  According  to 
Kuriloffthetr.pt.  (CeHg^CH.CeHe  +  C6H6  is  at  4.2°  and  1.25  mol.  %  (CeHs^CH, 
the  m.  pt.  of  (C6H5)3CH.C6H6  is  78.2°  and  the  tr.  Pt.(C6H6)3CH.C6H6  +  (C6H6)3.CH 
is  at  74°  and  69.4  mol.  %  (C6HB)3CH.  <* 


Triphenyl  METHANE 


434 


SOLUBILITY  OP  TRI  PHENYL  METHANE  IN  CARBON  BISULPHIDE. 

(Etard  —  Ann.  chim.  phys.  [7]  2,  5701  '94;  below  —  80°,  Arctowski  —  Z.  anorg.  Ch.  II,  273,  '95.) 


40 
50 
60 
70 

So 


Gms.  CHCQsHs. 

t°. 

per  100  Gms. 

Solution. 

-113 

•5        0-98 

—  102 

1.24 

-    91 

1.56 

-    83 

I.9I 

-    00 

3-4 

t°. 

Gms.  CH(C6HS)3 
per  100  Gms. 
Solution. 

-40 

7-5 

—  20 
0 
+  10 

13-7 
25-8 
38.7 

20 

43-2 

30 

52-9 

Cms. 
per  100  Gms. 
Solution. 

63.7 
72.4 
78.6 
85.6 

92.2 


SOLUBILITY  OF  TRI  PHENYL  METHAKE  rv  HEXANE  AND  IN 
CHLOROFORM.     (Eurd.) 


Gms.  CHtCeH-Oa  per  100  Gms. 
Solution  in: 


Gms.  CH(CeH5)3  per  100  Gi 
Solution  in: 


Hexane. 

Chloroform. 

-So 

10.5 

—30 

I  .2 

15.2 

—  20 

1.6 

19.0 

—  10 

2.2 

23-5 

0 

3-5 

28.9 

+  10 

5-6 

35-o 

20 

8-3 

41-5 

Hezane. 

Chloroform. 

30 

12-5 

48.8 

40 

20.  o 

56.1 

50 

25.8 

63.8 

60 

45-7 

71.7 

70 

62.0 

79-8 

80 

785 

87.2 

90 

97.0 

SOLUBILITY  OF  TRI  PHENYL  METHANE  IN: 

(Hartley  and  Thomas.) 

Thiophene. 

Gms.  Mol. 


Gms. 

Pyrrole. 

Mol. 

to     CH(QjH5)3       per                    Solid 
'  per  100  Gms.     cent                  Phase. 
Sol.        CHCCeHsV 

24 

.6 

24 

•3 

8 

_i 

29 

.0 

29 

.8 

10 

.4              "    fl 

31 

•5 

33 

•4 

12 

.1 

36 

.8 

40 

.6 

J5 

.8      CHCCTOs 

42 

•7 

49 

.1 

20 

•9            "  n 

46 

•9 

56 

•  0 

25 

•9 

53 

.2 

63 

9 

32 

.8 

60 

•  0 

72 

•3 

41 

.8 

63 

9 

76 

•7 

47 

•4 

68 

•5 

81 

•9 

55 

.6 

71 

.1 

84 

•4 

59 

.8 

80 

.0 

91 

5 

74 

.8 

89 

.2 

97 

.6 

9i 

Q'                            M 

t 

o     CH(C«H5)3      per                  Solid 
*  per  i  oo  Gms.    cent                  Phase. 
Solution.  CH(C6H5)3. 

2f 

•  7 

26 

.0 

10 

.8 

CHCQHJs.C^S 

*^ 

i 

„     rhombs 

33 

•5 

31 

-I 

13 

•5 

44 

0 

43 

.6 

21 

.1 

'• 

47 

.6 

48 

•4 

24 

•4 

1C 

53 

-5 

58 

•7 

32 

9 

•• 

57 

•4 

70 

2 

44 

•7 

•* 

57 

.6 

74 

.8 

50 

6 

• 

62 
67 

•7 
.0 

78 
81 

•7 
9 

56 

60 

.0 

.8 

CH(C«H5)3 
„   monoch'nic 

67 

.2 

82 

i 

6r 

3 

" 

74 

.2 

87, 

4 

70 

5 

" 

79 

.0 

90. 

\J 

76 

3 

M 

87 

,2 

96. 

2 

89 

9 

" 

F.-pt.  data  for  triphenylmethane  +  naphthalene  are  given  by  Vignon  (1891). 
SOLUBILITY  OF  TRIPHENYL  METHANE  IN  PYRIDINE.    (Hartley  and  Thomas,  1906.) 
Synthetic  method  used,  see  note,  p.  16. 


t 

0 

Gms. 
CH(C,H5), 
per  TOO  Gms, 
Solution. 

Mol.  per 
cent           Solid  Phase. 
CH(C6H6)3. 

t' 

Gms. 
CH(C6H5), 
per  TOO  Gms. 
Solution. 

Mol.  per 
cent        Solid  Phase. 
CH(C6HS)8. 

22 

.8 

46 

.2 

22 

CH(C6HB), 

59 

•3 

75-6 

50-3 

CHCQHs), 

31 

•7 

53 

•3 

27. 

2          "  monoclinic 

67 

.8 

81.9 

59-7 

" 

37 

•9 

57 

.6 

30- 

7 

72 

.8 

85-7 

66.4 

" 

48 

•7 

66 

.6 

39- 

5          " 

80 

.6 

9i-5 

77.2 

(4 

53 

.1 

70 

.1 

43- 

5       " 

86 

.8 

95-8 

88.1 

M 

435 


Sulfon  METHANES 


Ethyl  and  Methyl  Sulfon  METHANES. 

SOLUBILITY  IN  WATER  AND  IN  90%  ALCOHOL. 

Compound.  Formula.  f          Gms.  Cmpd.  per  too  cc.:  Authority. 

Water.  90%  Alcohol 

Sulfonal  (CH3)2C(SO2C2H6)j  15.5  0.22  1.25      (Greenish  and  Smith,  1903.) 

Tetronal  (C2H5)2C(SO2C2H5)2  IS-2O          O.l8  8.33      (Squire  and  Caines,  1905.) 

Trional  (CH3)(C2H6)C(SO2C2H5)2    15-20        0.31         9.0 


DISTRIBUTION  BETWEEN  WATER  AND  OLIVE  OIL  AT  ROOM  TEMP. 

(Baum,  1899;  Meyer,  1909.) 

Gms.  Cmpd.  per  100  cc. 
Compound.  Formula. 


Dimethyl  Sulfon  Dimethyl  Methane  (CH3)2C(SO2.CHS)1 

Diethyl  Sulfon  Methane 

Sulfonal 


Trional 
Tetronal 

METHYL  ACETATE  CH3COOCH3. 

loo  gms.  H2O  dissolve  25  gms.  CH3COOCH3  at  22°. 


(CHMC.HOCCSCfe.CiHs),  0.0404    0.1646 


Ratio 
M. 

0.103 
O.I5I 
0.979 
4.074 
0.0462  0.1446  3.756 


HjO  Layer    Oil  Layer 

(w) ,      (0) . 
0.6072  O.O622 
0.092 
0.0686 


0.610 
0.070 


(Traube,  1884.) 


More  recent  data  for  the  solubility  of  this  compound  in  water  are  given  by 
(Herz,  1917). 


METHYL  ALCOHOL  CH3OH. 

FREEZING-POINTS  OF  MIXTURES  OF  METHYL  ALCOHOL  AND  WATER. 

(Pickering,  1893;  Baumfi  and  Borowski,  1914.) 


Gms. 

,0 

CH3OH 

Solid 

t  . 

per  100 

Phase. 

Gms.  Sol. 

—  IO 

14-5 

Ice 

—  20 

25 

" 

-30 

33 

" 

-40 

40 

" 

-50 

47 

" 

-60 

52-6 

Gms. 

Gms. 

*° 

CH3OH 
per  loo 
Gms.  Sol. 

Solid 
Phase. 

t°. 

CH3OH 
per  loo  Gms. 
Mixtures. 

Solid  Phase. 

-70 

58-3 

Ice 

-130 

75-5 

Ice 

-80 

62.6 

" 

-138.5 

Eutec.    77 

"     +CH,OH 

-90 

65-7 

" 

-130 

82 

CH,OH 

—  IOO 

68.8 

" 

—  120 

86.5 

M 

—  no 

71.5 

" 

—  no 

92 

" 

—  1  20 

74.0 

" 

-95-7 

IOO 

" 

In  the  vicinity  of  the  eutectic  the  solutions  become  vitreous  and  direct  determina- 
tions of  the  f  .-pt.  cannot  be  made.    The  above  results  were  obtained  from  the  curve. 


MISCIBILITY  OF  METHYL  ALCOHOL  (see  Note,  p.  287)  AT  o°  WITH 

MIXTURES  OF: 
Carbon  Tetrachloride  and  Water.  (Bonner,  1910.)  Chloroform  and  Water.  (Bonner,  1910.) 


Composition  of  Homogeneous  Mixtures. 


Composition  of  Homogeneous  Mixtures. 


Gms. 
00* 

Gms. 
H20.            ( 

Gms. 

:HSOH. 

Sp.  Gr.  of 
Mixture. 

Gms. 
CHC1,. 

Gms. 
HA 

Gms. 
CH,OH. 

Sp.  Gr.  of 
Mixture. 

"0.935 

0.015      c 

).2I5 

.  .  . 

0.979 

0.021 

0.161 

.  .  . 

0.974 

0.026      c 

>.328 

1.30 

0.90 

O.IO 

0-35 

•17 

0.90 

O.IO           < 

>-74 

I-I3 

0.80 

0.2O 

0.49 

.12 

0.80 

0.20 

.10 

1.04 

*o.73 

0.27 

o-57 

.  .  . 

0.70 

0.30           ] 

.40 

I 

0.70 

0.30 

0.60 

.08 

0.60 

0.40           ] 

.68 

0.97 

0.60 

0.40 

0.70 

•05 

0.50 

0.50 

•7i 

o-9S 

0.50 

0.50 

0.77 

.02 

0.40 

0.60 

•77 

o-93 

0.40 

O.6O 

0.83 

0.20 

0.80           ] 

.88 

0.92 

0.20 

0.80 

0.84 

0.97 

O.IO 

0.90           1 

.90 

0.92 

O.IO 

0.90 

0.74 

0.96 

O.O26 

0.974 

•045 

o-93 

0.013 

0.987 

0.267 

0.98 

METHYL  ALCOHOL 


436 


,MISCIBILITY  OF  METHYL  ALCOHOL  (see  Note,  p.  287)  AT  o°  WITH 
MIXTURES  of: 


Brombenzene  and  Water.  (Bonner,  1910.) 

Composition  of  Homogeneous  Mixtures. 


Ethyl  Bromide  and  Water.    (Bonner,  1910.) 

Composition  of  Homogeneous  Mixtures. 


Cms. 

Cms. 

Cms. 

Sp.  Gr.  of 

Gms. 

Gms. 

Gms. 

Sp.  Gr.  of 

C6H6Br. 

H20. 

CH3OH. 

Mixture. 

C2H5Br. 

H20. 

CH3OH. 

Mixture. 

0.991 

0.009 

0.230 

o-973 

O.O27 

0.202 

1.27 

0.985 

O.OI5 

0.314 

1.24 

0.950 

0.05 

o-33 

*0.98 

O.O2 

0.40 

0.936 

0.064 

o-393 

1.18 

0.90 

0.10 

1.  01 

1.04 

0.90 

O.IO 

o.54 

1.14 

0.80 

0.20 

1-50 

0.98 

0.80. 

0.20 

0.86 

1.05 

O.yO 

0.30 

1.84 

o-95 

0.70 

0.30 

i  .04 

1.  01 

0.60 

0.40 

2.065 

0.94 

0.60 

0.40 

1.18 

o-99 

0.50 

0.50 

2.24 

0.91 

0.50 

0.50 

1.26 

0.97 

0.40 

O.6O 

2.30 

0.90 

0.40 

O.6O 

i-3i 

0.96 

0.30 

0.70 

2.28 

0.89 

O.2O 

0.80 

I.  21 

0.94 

0.20 

0.80 

2.20 

0.89 

O.IO 

0.90 

0.94 

0.94 

0.095 

0.905 

1.927 

0.90 

0.022 

0.978 

1.94 

0.98 

0.016 

0.984 

1-332 

0.91 

MISCIBILITYTOF  METHYL  ALCOHOL  (see  Note,  p.  287)  AT  o°  WITH 
MIXTURES  OF: 

Hexane  and  Water.    (Bonner,  1910.)  Heptane  and  Water. 


Composition  of  Homogeneous  Mixtures. 


(Bonner,  1910.) 
Composition  of  Homogeneous  Mixtures. 


Gms. 

Gms. 

Gms. 

Sp.  Gr.  of 

Gms. 

Gms. 

Gms. 

Sp.  Gr.  of 

Hexane(i). 

H20. 

CH3OH. 

Mixture. 

Heptane(i). 

H20. 

CH3OH. 

Mixture. 

0-973 

0.067 

4.280 

0.966 

0.034 

4.78 

.  .  . 

0.90 

O.IO 

4.69 

0.80 

0.90 

O.IO 

5-55 

0.80 

0.80 

0.20 

5.26 

0.80 

0-793 

0.207 

6.36 

0.82 

0.691 

0.309 

5-710 

0.82 

0.70 

0.30 

7-30 

0.82 

0.60 

0.40 

6.17 

0.81 

0.60 

0.40 

8.22 

0.82 

0.491 

0.509 

6.365 

0.83 

0.50 

0.50 

8.76 

0.82 

0.40 

0.60 

6.33 

0.83 

0.40 

0.60 

8.65 

0.83 

0.30 

0.70 

6.13 

0.84 

0.30 

0.70 

7.78 

0.83 

0.20 

0.80 

5-49 

0.85 

0.198 

0.802 

6.7I 

0.84 

O.IO 

0.90 

4.01 

0.86 

O.IO 

0.90 

4.40 

0.87 

0.016 

0.984 

i-759 

0.91 

0.038 

0.962 

2.96 

0.91 

(i)  The  hexane  and  heptane  used  were  Kahlbaum's  "aus  Petroleum." 
loo  cc.  cotton  seed  oil  (^25  =  0.922)  dissolve  4.84  gms.CK^OH  at  25°. 

(Wroth  and  Reid,  1916.) 

100  cc.  methyl  alcohol  dissolve  6.74  gms.  cotton  seed  oil  at  25°.     " 
DISTRIBUTION  OF  METHYL  ALCOHOL  BETWEEN"  WATER  AND  COTTON  SEED 

OIL  AT  25°.      (Wroth  and  Reid,  1916.) 


Oil  Layer. 
0.199 

HjO  Layer. 
17.28 

jxauu. 

86.6 

0.253 
0.298 
0.264 

23-34 
25-73 
24-I5 

92.2 
86.2 
9i-3 

Gms.  CHsOH  per  100  cc. 

Oil  Layer.        H2O  Layer. 
0.275  23.48 

Q.258  24.44 

0.284  23.06 


Ratio. 
85.2 

94 
81.4 


Freezing-point  curves  (solubility,  see  footnote,  p.  i)  are  given  for  the  following 
mixtures:  CH3OH  +  SO2,  CH3OH  +  C2H5COOH,  (CH3OH.HC1)  + 
C2H6COOH,  (C2H5COOH.HC1)  +  CH3OH  (Baume  and  Pamfil,  1914); 
CH3OH-f  NH3  (Baume  and  Borowski,  1914);  CH3OH  +  CH3I  (Baume  and 
Tykociner,  1914). 


437 


METHYL  AMINES 


METHYL  AMINES  CH3NH2,  (CH3)2NH,  (CH8)8N. 

Freezing-point  data  (solubility,  see  footnote,  p.  i)  for  mixtures  of  CH3NH2  -f- 
H2O,  (CH3)2NH  +  H2O  and  (CH8)«N  +  H2O  are  given  by  Pickering  (1893). 

The  solubility  of  methylamine  and  of  dimethylamine  in.water  at  60°,  calculated 
from  the  vapor  pressures  determined  by  an  aspiration  method  are  given  by  Doyer 
(1890)  as  follows: 


Aminc. 

CH3NH2 

(CH3)2NH 

Vapor  Pres- 
sure in 
mm.  Hg. 

40.6 
90-3 

Ostwald  Solu- 
bility CoefJ. 
(see  p.  2  2  7). 

5" 

230 

Bunsen  Abs. 
Coef  .  0. 
(see  p.  227). 

419 

188 

SOLUBILITY  OF  TRIMETHYL  AMINE  IN  VARIOUS  SOLVENTS  AT  25°. 

(v.  Halban,  1913.) 

The  measurements  were  made  according  .to  the  dynamic  method  in  the  form 
developed  by  R.  Abegg  and  his  collaborators  (Gaus,  1900;  Abegg  and  Riesenfeld, 
1902).  The  calculations  of  the  partial  pressures  of  the  trimethylamine  were  made 
according  to  the  Abegg  and  Riesenfeld  method. 

E  =  calc.  partial  pressure  of  (CH3)3N  above  a  I  normal  solution,  based  on 

Henry's  Law. 

i 

}\  =  solubility,  i.e..  the  quotient  of  the  concentration  in  the  solution  and  in  the 
,          .  mois.  (CH3)3N  per  liter  X  RT  X  760 

gas  phase:  X  =  —, f  ,~..  >  ,T  . ^- .  Rl  X  760  =  18,590. 

partial  pressure  of  (CH3)3N  in  mm.  Hg ' 


Solvent.         E. 
Methyl  Ale.  26.1 
Ethyl       "      —  - 
Propyl 
Amyl 
Benzyl 
Acetone 


39-5 
39-4 
48-3 
14.2 

243 


711 

471 

472 

385 

1308 

76. 


Solvent.  E. 

Acetophenone  321 
Ether  349 

Acetonitrile  292 
Nitromethane  329 
o  Nitrotoluene  340 
Nitrobenzene  350 


x. 

57-9 

53-3 
63-7 
56.5 
54-7 


Solvent.  E.          X. 

Ethyl  Acetate  220  84.5 
Ethyl  Benzoate  244  76.2 
Chloroform  31.1  598 

:  Bromnaphthalene  409       47 


Hexane 
Benzene 


248 
172 


75 
109 


Two  determinations  are  also  given  for  triethyl  amine: 

X25  in  hexane  =  2160.        X25  in  nitromethane  =  400. 


METHYL  AMINE  AND  TRI  METHYL 
Water  and  Amyl  Alcohol. 

(Herz  and  Fischer  —  Ber.  37,  4751,  '04.) 

Cms.  NH2(CH3)             Mfflimok  NH2(CH3) 
per  ipo  cc.                             per  10  cc. 

AMINE,  DISTF 
Water 

(Herz  and  Fis 

Cms.  N(CHa)3 
per  100  cc. 

Aq.        Alcoholic                Aq.         Alcoholic 
Layer.       Layer.               Layer.         Layer. 

0-37      0-12               I.I5S      0-3804 

0-94    0.33          3-°36     1-070 
J-57    0.54         5.054    1.759 
1.89    0.69         6.083    2.219 

2.00      0.72              6.429      2.315 

2-53    0.92          8.126    2.981 
3.30    1.24       10.613    3.974 

Aq.            QjHfl 
Layer.        Layer. 

0-345      0.174 

0.812     0.396 

1-075      0-545 
1.462      0.731 
2.139      1.077 

2-757     i-376 
3.292    1.683 
3.996    2.053 
6.582    3.465 

Millimok  N(CHa)3 
per  10  cc. 


Aq. 
Layer. 

0.584 

1-377 
1.819 
2.474 
3.619 
4-663 
5-568 
6.760 
H-I3S 


QH5 

Layer. 
0.295 
0.670 
0.921 
1.237 
1.823 
2.328 
2.847 

3-474 
S-86I 


METHYL  AMINES  438 

DISTRIBUTION  OF  METHYLAMINE  BETWEEN  WATER  AND  CHLOROFORM  AND  DI- 
METHYL AND  TRIMETHYL  AMINES  BETWEEN  WATER  AND  TOLUENE. 

(Moore  and  Winmill,  1912.) 


Results 

at  1  8°. 

Results 

at  25°. 

Results  at  32. 

35°. 

A™;«»       Gm.  Equiv.  per      Partition 

6m. 

Equiv.  per 

Partition 

Gm.  Equiv.  per 

Partition 

Amme'     Liter  Aq.|Layer.        Coef.         Liter  Aq.  Layer.        Coef.        Liter  Aq.  Layer. 

Coef. 

(CH3)NH2 

0.0817 

8 

.496 

O 

.  1  2O3 

7.965 

0 

.1399 

5 

•99 

u 

0.0809 

8 

•477 

0 

.1312 

8 

0 

.0959 

6 

(CHa)2NH 

0.0759 

23 

.28 

0 

.1203 

19.013 

0 

.1003 

13 

.38 

tt 

0.0975 

23 

.29 

O 

.IOIO 

19.05 

O 

.1043 

13 

•36 

(CH3)3N 

0.0688 

3 

.297 

0 

.0677 

2.291 

O 

.1182 

I 

•815 

•u 

0.0791 

3 

.290 

0 

.0641 

2.297 

0 

.1248 

I 

.820 

Similar  data  for  the  distribution  of  trimethylamine  between  water  and  toluene 
at  25°  and  at  other  temperatures  are  given  by  Hantzsch  and  Sebalt  (1899)  and 
Hantzsch  and  Vagt  (1901). 

DiMETHYL  AMINE  HYDROCHLORIDE   (CH,),NH.HC1. 

IOO  gms.  H2O  dissolve  369.2  gms.  (CH3)2NH.HC1  at  25°.     (Peddle  and  Turner,  1913.) 

ioo  gms.  CHCls  dissolve  16.91  gms.  (CH3)2NH.HC1  at  25°. 

Phenyl  METHYL  AMINE  HYDROCHLORIDE   (CH3)(C6H6)NH.HC1. 
ioo  gms.  H2O  dissolve  378.8^1113.  (CH3)(C6H5)NH.HClat25°.  (Peddle  and  Turner,  '13.) 

Di  and  TriMETHYL  AMINE  CHLOROPLATINATES,     (CH3)2NH.H2PtCl8, 
(CH3)3N.H2PtCl6. 

SOLUBILITY  OF  EACH  IN  AQ.  ALCOHOL  AT  o°.    (Bertheaume,  1910.) 

Gms.  Each  Compound  (Determined  Sepa- 
Sol  ent  rately)  per  ioo  Gms.  Solvent. 

(CH3)2NH.H2PtCl6.       (CH3)N.H2PtClfi. 

Absolute  Alcohol          o .  0048  o .  003  6 

90°  o.i 10  0.070 

80°  0.325          0.243 

70°          0-558      0-391 
60°         0.996     0.766 

METHYL  BUTYRATE  C3H7COOCH3. 

ioo  gms,  H2O  dissolve  1.7  gms.  C3H7COOCH3  at  22°.  (Traube,  1884.) 

More  recent  data  for  the  solubility  of  methyl  toutyrate  in  water  are  given  by 

Herz,  1917. 

METHYL  BUTYRATE,   METHYL  VALERATE. 

SOLUBILITY  OF  EACH  IN  AQUEOUS  ALCOHOL  MIXTURES. 

(Bancroft,  1895;  from  Pfeiffer,  1892.) 

ioo  cc.  H2O  dissolve  1.15  cc.  methyl  butyrate  at  20°. 

cc.  Alcohol  cc.  H20  Added.*  <Cc.  Alcohol    cc.  H2O  Added.* 

in  Mixture.      Butyrate.  Valerate.  i°  Mixture.          Valerate. 

3            2.34  1.66  27  44.15 

6            6.96  5.06  30  52.37 

9  12.62  9.03  33  62.25 

12  19.45  13.40  36  74.15 

15  28.13  18.41      ,  39  91.45 

18  38.80  24  42               oo 

21  55.64  30.09 

24             oo  36.72 

*  cc.  HjO  added  to  cause  the  separation  of  a  second  phase  in  mixtures  of  the  given  amounts  of  ethyl 
alcohol  and  3  cc.  portions  of  methyl  butyrate  and  of  methyl  valerate  respectively. 

METHYL  ETHER   (CH3)20. 

F.-pt.  curves  are  given  for  (CH3)20  +  H2O  (Baume  and  Perrot,  1914) ;  (CH3)2O  -f 
C2H2,  (CH3)2O  +  SO2  (Baume,  1914);  (CH3)2O  +  NO  (Baume and  Germann,  1914); 
(CH3)2O  +  CO2  (Baume  and  Borowski,  1914). 


439  METHYL  IODIDE 

METHYL   IODIDE,  Methylene  Chloride  and  Methylene  Bromide. 
SOLUBILITY  OF  EACH  IN  WATER.    (Rex,  1906.) 

Gms.  per  100  Gms.  H2O. 


CH3I.  CH2C12. 

o  1.565        2.363        1.173 

10  1.446     2.122     1.146 

20  I-4I9     2          I.I48 

30  1.429     1.969     1.176 

Fusion-point  data  for  methyl  iodide  +  pyridine  are  given  by  Aten  (1905-06)  A 

METHYL   ORANGE   H2NC6H4.N2.C6H4SO3Na. 

100  gms.  H2O  dissolve    0.02  gm.  methyl  orange  at  20-25°.]  (Dehn,  1917.) 

pyridine  1.80    "  " 

aq.  50%  pyridine  51.5 

METHYL   OXALATE   (CH3)2C2O4. 

loo  gms.  H2O  dissolve   6.18  gms.  (CH3)2C2O4  at  20-25°.  (Dehn,  1917.) 

pyridine  "^       4.8 

aq.  50%  pyridine        "       93.1 

95  %  formic  acid  22.58  at  20.2°  (Aschan,  1913.) 

F.-pt.  data  for  (CH3)2C2O4  +  H2O  are  given  by  Skrabal  (1917). 

METHYLENE  BLUE   (CH,),N.C.H,(NS)C.H,:N(CH,),C1. 

100  gms.  H2O  dissolve  4.36'gms.  methylene  blue  at*2O-25°.  (Dehn,  '17.) 

pyridine  "       0.26     " 

aq.  50%  pyridine  0.74 

Data  for  the  distribution  of  methylene  blue  between  aniline  and  water  are 
given  by  Pelet-Jolivet  (1909). 

METHYL  PROPIONATE   C2H4COOCH3. 

100  gms.  H2O  dissolve  5  gms.  C2H6COOCH3  at  22°.  (Traube,  1884.) 

More  recent  data  for  the  solubility  of  methyl  propionate  in  water  are  given  by 

Herz  (1917). 

METHYL   SALICYLATE   C6H4OH.COOCH3. 

100  cc.  H2O  dissolve  0.074  Sm-  C6H4OH.COOCH3  at  30°.  (Gibbs,  1908.) 

100  cc.  o.i  n  H2SO4  dissolve  0.077  gm.  C6H4OH.COOCH3  at  30°. 

SOLUBILITY  OF  METHYL  SAHCYLATE  IN  AQUEOUS  ALCOHOL  AT  25°.  (Seidell,  1910.) 


Wt.  % 
C2H5OH 
in  Solvent. 

<*«of 
Sat.  Sol. 

Gms.  CgHjiOH.- 
COOCH3  per 
loo  Gms.  Sat.  Sol. 

Wt.  % 
in  Solvent. 

<*25  Of 

Sat.  Sol. 

Gms.  C6H4OH.- 
COOCH3  per 

0 

I 

0.12 

60 

0.923 

°  iT.oo'  ° 

30 

0.958 

O.6O 

65 

0.929 

30.50 

40 

0.940 

2.30 

70 

0-943 

39-40 

50 

0.925 

6.  20 

75 

0-974 

58.50 

55 

0.922 

10 

80 

1.050 

72 

SOLUBILITY  OF  METHYL  SALICYLATE  IN  AQUEOUS  ALCOHOL  AT  DIFFERENT 
TEMPERATURES.  (Seidell,  1910.) 

Wt.  %  C2HSOH  Gms.  QI^OH.COOCHs  per  100  cc.  Solvent  at: 

in  Solvent. 

O 
30 
40 
50 

55 
60 

65 
70 

75 
80 


15°. 

20°. 

25°. 

30°. 

(about)  o.i 

O.I 

O.I 

O.I 

0.3 

0.4 

0.5 

0.6 

0.8 

1  .1 

1.8 

2.4 

3-5 

5 

6 

4.2 

6 

7-8 

9-5 

7-7 

10 

12.5 

15-5 

13 

16.5 

20.2 

24.5 

22 

28 

33 

40 

43 

52 

62 

72 

92 

135 

180 

230 

METHYL  StTLFATE  440 

METHYL  SULFATE   (CH,)2SO4. 

RECIPROCAL  SOLUBILITY  OF  METHYL  SULFATE  AND  OIL  OF  TURPENTINE. 

The  determinations  were  made  by  the  synthetic  method  (sealed  tubes). 

The  dz5  of  the  oil  of  turpentine,  CioHie,  was  0.8602,  its  absolute  index  of  refraction 
for  yellow  light  at  25°  was  1.467  and  its  rotation  in  a  loo-mm.  tube  was  —32.25°. 

Cms.  (CH3)2S04  per  100  Gms.  Gms.  (CH3)2SO4  per  100  Cms. 


t°.  (CH3)2S04  CwHw,  .  '  (CH3)jS04  C10H16  ' 

Rich  Layer.         Rich  Layer.  Rich  Layer.         Rich  Layer. 

30  95  4  80  87  13 

40  93  5  90  84  17 

50  92  6  ico  76  27 

60  91  8  105  68  37 

70  89  10  108  .  2  (crit.  t.)  50  .  5 

The  results  are  influenced  appreciably  by  the  age  and  purity  of  the  products 
and  by  the  length  of  time  the  mixtures  are  kept  in  the  sealed  tubes.  Somewhat 
different  results  were  obtained  with  a  sample  of  turpentine  containing  5  vol.  %  of 
white  spirit. 

MICHLER'S    KETONE    (Tetramethyl-pa-diamidobenzophenone)   CO[C6H4(4)- 

N(CH3)2]2. 

100  gms.  H2O  dissolve  0.04  gm.  of  ketone  at  20-25°.     (Dehn,  1917  ) 

pyridine*  "       9.92    " 

aq.  50%  pyridine        "       3-59    " 

MOLYBDENUM   TRIOXIDE    (Molybdic  acid  dihydrate)   MoO3.2H2O. 

SOLUBILITY  IN  WATER.     (Rosenheim  and  Bertheim,  1903.) 
Gms.  MoO3  per  1000  Gms.  Gms.  MoO3  per  1000  Gms. 

Sat.  Solution.          H2O. 

18  1-065  i.  066  59 

23  1.822  1.856  60 

30  2.570  2.638  66 

40  4.541  4.761  70 

48  5.980  6.360  74.4 

50.2  6.431  6.873  75 
54  7.283  7.855  79 

When  a  solution  of  the  dihydrate  is  held  at  40-50°,  considerable  amounts  of  crys- 
tals, designated  by  the  authors  as  a  molybdic  acid  monohydrate,  separate.  They 
differ  from  the  /8  molybdic  acid  monohydrate  obtained  by  direct  conversion  of  the 
dihydrate  at  70°,  in  being  better  crystals  and  in  yielding  solutions  which  can  be 
filtered. 

SOLUBILITY  OF  a  MOLYBDIC  ACID  MONOHYDRATE  IN  WATER. 

(Rosenheim  and  Davidsohn,  1903.) 
Gms.  MoO3  per  1000  Gms.  Gms.  MoO3  per  1000  Gms. 

Sat.  Solution.          H2O.  Sat.  Solution.          H2O. 

14.8   2.  112    2.117       45    3.648   3.661 
24.6   2.612    2.619       52    4-I67   4.184 

30.3  2.964    2.973       6°   4.665   4.685 

36.8  3.284   3.295      70   4.213   4.231 
42   3.434   3.446      80   5.185   5.212 

SOLUBILITY  OF  MOLYBDIC  ACID  DIHYDRATE  IN  AQ.  AMMONIUM  SALT 

SOLUTIONS.      (R.  and  D.,  1903.) 

Gms.  MoO3  per  1000  Gms. 

t°.  Solvent.  .  -  -*  - 

Sat.  Solution.       Solvent. 

29.6     10%  (NH4)2SO4          18.91        19.27 
31.5     io%NH4HS04  26.79        27.53 

4i-8  33.22        34.36 

49-7  36-32        37-69 

Fusion-point  data  for  MoO3  +  Na2MoO4  are  given  by  Groschuff  (1908). 


441 

MORPHINE  C17Hi9N03.H20. 

SOLUBILITY  IN  SEVERAL  SOLVENTS. 

(U.  S.  P.;  Muller,  W.,  1903.) 


MORPHINE 


Solvent. 


Cms.  Morphine  per  100  Cms. 
Solution. 


Solvent. 


Cms.  Morphine  per  too  Cms. 
Solution. 


At  l8°-22 

Water                0.0283 
Alcohol 
Ether                 0.0131 
Ether  sat.  with 
H2O               0.0094 
H2O  sat.  with 
Ether             0.0447 
Benzene             0.0625 
Water                0.0254 
Chloroform        0.0504 
Water                0.0288 
Acetone             0.128 
Aq.  50  Vol.  % 
Acetone          0.132 
Water                0.0217 
Water               0.0192 

°.     At  25°.         At  80°. 
0.030      0.0961 
0.600        1.31  (60°) 
0.0224 

(20°)  (Winterstein,  1909.) 

(20°) 

(15°)  (Guerin,  1913.) 
(15°) 

(15°) 
(20°)  (Zalai,  1910.) 
(20°)  (Guild,  1907.) 

At   i8°-22°.          At  25°. 
Chloroform        0.0655           0.0555 
Amyl  Alcohol        .  .  .             0.8810 
Ethyl  Acetate    0.1861           0.1905 
Petroleum 
Ether             0.0854             ... 
Carbon  Tetra- 
chloride          0.0156          0.032  (17°) 
Glycerol             0.45  (15.5°) 
CCL,                   0.025  (20°)  (Gori,  1913.) 
Aniline               6.1    (20°)  (Scholtz,  1912.) 
Pyridine           16       (20°) 
Piperidine        39.8    (20°) 
Diethylamine     7.41  (20°) 
50%  Aq.            1                     J(Baroniand 

3%  HaBOs    J     *              [    1911-) 

SOLUBILITY  OF  MORPHINE  IN  SEVERAL  SOLVENTS  AT  25°. 


Solvent. 

Ethyl  Alcohol 
Methyl  Alcohol 
Chloroform 
Benzene 


Cms. 

C17H19N03.H20 

per  loo  cc. 

Solvent. 

0.388 

6.66 

0.04 

insol. 


(Schaefer,  1913.) 


Cms. 


Solvent. 


i  Vol.  C2H5OH+4  Vols.  CHClg 
+4  Vols.  C6H6 

i  Vol.  CHsOH  +4  Vols.  CHCla 
+4  Vols.  C6H6 


per  100  cc. 
Solvent. 

0.66 

0.2 

4-54 
2-5 


SOLUBILITY  OF  MORPHINE  IN  ETHYL  ETHER  AT  5.5°. 

(Marcbionneschi,  1907.) 


Solvent. 


Washed  and  Distilled  Ether 

Ether  Purified  by  Distillation  over  Na 


Gms.  Morphine 

per  100  Gms. 

Sat.  Sol. 

0.049 
0.263 
0.56 


Solid 


Ci7H19NO3.H2O 

a 

C17H19N03 


SOLUBILITY  OF  MORPHINE  IN  AQUEOUS  SOLUTIONS  OF  SALTS  AND  BASES  AT 
ROOM  TEMPERATURE,  SHAKEN  EIGHT  DAYS. 

(Dieterich,  1890.) 

In  N/io  Salt  or  Base.  In  N/i  Salt  or  Base. 

Grams  per  Liter.  Grams  rjer  Liter. 


[.  oau  or  liase.            /- 

Salt  or  Base. 

Morphine. 

Salt  or  Base. 

.Morphine  • 

NH4OH 

3-51 

O.2O 

35-08 

0-505 

(NH4)2C03 

4-80 

0.031 

48.03 

0.040 

KOH 

4.62 

2.78 

46.16 

.  .  . 

K2C03 
KHCO3 

6.92 
10.02 

O.2O 
O.O24 

69.15 

ioo.  16 

0-379 
0-040 

NaOH 

4-OO 

3-33 

40.05 

.  .  . 

Na2CO3 
NaHC03 

5-30 
8.41 

0.09 
0.032 

53-03 
84.06 

0.14 
0.044 

Ca(OH),  (sat.) 

i  .00  (25°) 

Acetate. 

Hydroc 

5-8l 
2.4 

20.  Of 
*  60°. 

hloride. 
80°. 

20O.O 
2.8* 

Sulphate. 

Apo  M.  Hydrochloride. 

25°. 
44.9 

4.6 

0.21 
19.2 

80°.  ' 

50.0 
40.0* 

'25°. 

6-53 
0.22 

80° 

166. 

0. 

25°. 
6           2.53 

53*    2.  62 
0.026 
A"     0.053 

8o°/ 
6.25 
3-33 

t.*! 

>-5°' 

MORPHINE  442 

i 

MORPHINE  ACETATE  CH3COOH.C17H19NO3.3H2O,  Morphine 
Hydrochloride  HC1.C17H19NO3.3H2O,  Morphine  Sulphate  H2SO4. 
(C17H10NO3)2.5H2O,  and  Apo  Morphine  Hydrochloride  HC1.C17 
H17N02. 

SOLUBILITY  IN  SEVERAL  SOLVENTS. 

(U.  S.  P.) 

Grams  per  100  Grams  of  Solvent. 
Solrent. 

Water 
Alcohol 
Chlorof 
Ether 


100   gms.  H2O  dissolve  1.69  gms.  apo  morphine  hydrocloride  at  15.5°,  and  2.04 
gms.  at  25°. 

100  gms.  90%  alcohol  dissolve  1.96  gms.  apo  morphine  hydrochloride  at  about 
15.5°.  (Dott,  1906.) 

100  gms.  H2O  dissolve  4.17  gms.  morphine  hydrated  sulfate  .5H2O  at  15°. 

(Power,  1882  ) 

MORPHINE   SALTS   (con.) 

SOLUBILITY  IN  WATER  AND  IN  90%  ALCOHOL  AT  ORD.  TEMP. 

(Squire  and  Caines,  1905.) 

Gms.  Salt  per  IPO  cc.  Gms.  Salt  per  100  cc. 

Morphine  Salt.  9o%  Morphine  Salt.  '     90% 

H2°-       Alcohol.  H2°'  Alcohol. 

Morphine  Acetate  ...        i  Diacetyl  Morphine  (Heroine)     o.n      2.5 

"        Hydrochloride   ...        2  "       -  HC1        50  9.1 

"        Sulfate  ...        0.143      Ethyl  Morphine  HCl(Dionin)  14.3      20 

"        Tartrate  10        0.172 

100  gms.  4%  HC1O4  solution  dissolve  0.44  gm.  morphine  perchlorate  at  15°. 

(Hofmann,  Roth,  Hobald  and  Metzler,  1910.) 

SOLUBILITY  OF  MORPHINE  SALTS  IN  SEVERAL  SOLVENTS  AT  25°. 

(Schaeffer,  1913.) 

Gms.  of  Each  Salt  Separately  per  100  cc.  of  Each  Solvent. 
• 


Morphine       Morphine  Diacetyl 

Hydrochloride.     Sulfate.  Morphine.      HC            HC1 

95%  Ethyl  Alcohol                      0.606      0.2  3          9.1        4 

85%  Ethyl  Alcohol                      1.2          0.4  ......... 

80%  Ethyl  Alcohol                      2              0.77  ......... 

Methyl  Alcohol                                ...           ...  4         n.i       66.  6 

Chloroform                                  Insol.       Insol.  66.6    33.3      0.526 

Benzene                                        Insol.        Insol.  12.5     Insol.     Insol. 

i  Vol.  C2H5OH+4  Vols.  CHC13   0.18        0.0164  66.6      4-5        5 

"            +4  Vols.  C6H6      0.089      °-OI33  25          Q-71     I-I4 

i  Vol.  CH3OH  +4  Vols.  CHC13      ...        0.22  66.6     20        20 

+4  Vols.  C6H6      0.253      0.066  25          6.6      8.33 

Ethyl  MORPHINE   Ci,HHON(OH)(OC,H,).  J 

100  cc.  H2O       dissolve    0.208  gm.  CnHi7OH(OH)(OC2H5)  at  25°.    (Schaeffer,  1912.) 

"      alcohol        "         1.33    gms.                      "  " 
"      ether           "       66.6 


443  Ethyl  MORPHINE 

Ethyl    MORPHINE    HYDROCHLORIDE    C17H17NO(OH)(OC2H5).HC1.2H2O 
(Dionin)  (see  also  on  preceding  page). 

SOLUBILITY  IN  WATER  AND  IN  ALCOHOL.    (Schaeffer,  1912.) 

Cms.  Ethyl  Morphine  HC1 
per  100  cc. 

t°.  'Water.  Alcohol.^ 

IS  8-7  3-85 

25  12.5  5 

40  25  12. 1 

50  40  20 

These  results  differ  from  similar  data  for  commercial  samples  of  Dionin. 
The  differences  are  believed  to  be  due  to  the  impurities  (amorphous  salts  of  the 
by-products  of  the  ethylation)  in  commercial  products. 

100  cc.  H2O  dissolve  10  gms.  ethyl  morphine  hydrochloride  at  ord.  temp.  (Dott,  19x2.) 

MUSTARD   OIL  Allyl  Isothiocyanic  Ester  CS:NC3H5. 

SOLUBILITY  IN  SULFUR  BY  SYNTHETIC  METHOD.     (See  Note,  p.  16.) 

(Alexejew,  1886.) 

Gms.  Mustard  Oil  per  loo'Gms. 

Sulfur  Layer.    Mustard  Oil  Layer. 

90  10  72 

100  12  67 

tuo  15  62 

120  23  51 

124  (crit.  temp.)  35 

Freezing-point  data  for  allyl  isothiocyanate  +  aniline  are  given  by  Kurnakov 
and  Solovev  (1916).  Results  for  methyl  isothiocyanate  -j-  phenanthrene  and 
methyl  isothiocyanate  +  naphthalene  are  given  by  Kurnakov  and  Efrenov 
(1912). 

MYRISTIC  ACID   C13H27COOH. 

SOLUBILITY  IN  ALCOHOLS.    (Timofeiew,  1894.) 

Gms.  Gms. 

Alcohol  t°          CjjH^COOH  Alrnhnl  t°  CuH^COOH 

AicohoL  l  '       per  TOO  Gms.  Alcohol.  t  .  IOQ  Gms> 

Sat.  Sol.  Sat.  Sol. 

Methyl  Alcohol         o  2.81     Propyl  Alcohol         o  5.6 

21          21.2          "  "  2i  31.2 

31-5      59-2          "  "  36.5        55-3 

Ethyl  Alcohol  o  7.14    Isobutyl  Alcohol       o  6.4 

21          31  21  28 

Freezing-point  data  for  myristic  acid  +  palmitic  acid  are  given  by  Heintz  (1854). 

NAPHTHALENE   d0H8. 

1000  cc.  H2O  dissolve  0.019  g™'  Ci0H8  at  o°  and  0.030  gm.  at  25°.       (Hilpert,  1916.) 
SOLUBILITY  IN  ACETIC  AND  OTHER  ACIDS.    (Timofeiew,  1894.) 


Acid                       *•         Gms.  CioHg  per                     A  _:  j 

f0        Gms.  CioHg] 

i 

:oo  Gms.  Acid, 

/\C1U. 

*  '           3 

too  Gms.'Ac 

Acetic  Acid 

6-75 

6.8 

Isobutyric  Acid 

6.75 

12.3 

U                  (I 

21-5 

i3-i 

Propionic  Acid 

6-75 

13-9 

{(             (I 

42.5 

3i-i 

U                    (t 

21-5 

23-4 

11             t( 

51-3 

53-5 

t(             <( 

50 

7Q.8 

(I             (I 

60 

in 

Valeric  Acid 

6-75 

9-5 

Butyric  Acid 

6.75 

13.6 

«          n  • 
t 

21-5 

17.7 

«          « 

21.5 

22.1 

65 

167.4 

«         ti 

60 

I3I.6 

NAPHTHALENE  444 

SOLUBILITY  OF  NAPHTHALENE  IN  AQUEOUS  AMMONIA. 

(Hilpert,  1916.) 

Gms.  CigHg  per  1000  Gms. 
Solvent.  Solvent  at: ^ 

o°.  25°. 

Aq.  5%NHs  0.030  0.044 

Aq.  10%  NHs  0.042  0.074 

Aq.  25%NHa  0.064  0.162 

100%  NHs  33  120 

Aq.  2%  Pyridine  0.082  0.245 

SOLUBILITY  IN  METHYL,  ETHYL,  AND  PROPYL  ALCOHOLS. 

(Speycrs — Am.  J.  Sci.  [4]  14,  294,  '02 ;  at  19.5°,  de  Bruyn  —  Z.  physik.  Chem.  10,  784,  '92  ;  at  11°,  Timo 
feiew  —  Compt.  rend.  112*  11371  '91.) 

The  original  results  were  calculated  to  a  common  basis,  plotted  on 
cross-section  paper,  and  the  following  table  read  from  the  curves. 

In  Methyl  Alcohol.  In  Ethyl  Alcohol.  In  F-opyl  Alcohol. 


t'. 

Wt 

Sc 

.  of  i  c< 

Gms.  C10H8 

Wt.  of  i  cc. 
Solution. 

Gms.  C10H8 
per  100  Gms. 
C2H6OH. 

Wt.  of  i  cc. 
Solution. 

Gms.  Cjo-^s 
per  loo  Gms. 
C3H7OH. 

0 

o. 

8194 

3 

.48 

O 

•8175 

5.0 

0.8285 

4-45 

10 

o. 

812 

5 

.6 

O 

.814 

7-0 

0.824 

5-6 

20 

0.807 

8 

.2 

o 

.810 

9.8 

0.821 

8.2 

25 

o. 

805 

9 

.6 

o 

.809 

ii  -3 

0.820 

9.6 

30 

o. 

804 

ii 

.2 

o 

.809 

13-4 

O.82O 

11.4 

40 

o. 

805 

16 

.2 

o 

.812 

19-5 

0.823 

16.4 

50 

0.813 

26 

•  O 

0 

.822 

35-o 

0.837 

26.0 

60 

o. 

837 

So 

•  O 

o 

•855 

67.0 

0.867 

50.0 

65 

o. 

870 

o 

.890 

96.0 

0.897 

80.0 

70 

o. 

9023 

(68°)  : 

o 

•930 

179.0 

0-933 

134.1  (68 

•5°) 

EQUILIBRIUM  IN  THE  SYSTEM  NAPHTHALENE,  ACETONE,  WATER. 

(Cady,  1898.) 

An  excess  of  naphthalene  was  added  to  each  of  a  series  of  mixtures  of  water  and 
acetone  and  the  temperature  determined  at  which  a  second  liquid  phase  first 
appeared.  Since  an  excess  of  naphthalene  was  present,  the  amount  dissolved  was 
not  known.  The  following  supplementary  experiment  was,  therefore,  required  to 
ascertain  the  composition  of  the  saturated  solution  in  each  case.  "A  weighed 
quantity  of  naphthalene  was  added  to  a  known  weight  of  the  mixed  liquids,  the 
amount  being  just  sufficient  to  cause  the  formation  of  two  liquid  phases.  The 
consolute  temperature  of  the  system  was  then  determined  and  the  experiment  re- 
peated several  times  with  different  amounts  of  naphthalene.  If  the  results  are 
plotted,  using  the  weights  of  naphthalene  in  a  constant  quantity  of  the  mixed 
liquids  as  abscissas  and  the  temperatures  as  ordinates,  we  shall  get  a  series  of 
curves.  The  composition  of  the  liquid  phase  at  the  moment  when  the  system 
passes  from  solid,  solution  and  vapor  to  solid,  two  solutions  and  vapor  is  given  by 
the  point  at  which  the  prolongation  of  the  curve  for  that  particular  mixture  of 
acetone  and  water,  cuts  the  ordinate  for  temperature  at  which  the  change  takes 
place.  This  me^iod  requires  no  analysis  and  is  of  advantage  in  this  case  where 
ordinary  quantitative  analysis  would  be  very  difficult."  Considerable  difficulty 
was  experienced  in  determining  the  consolute  temperatures-.  It  was  necessary 
on  account  of  the  extreme  volatility  of  the  acetone  to  seal  the  mixtures  in  tubes. 

The  table  of  results,  calculated  with  the  aid  of  the  determinations  made  as  de- 
scribed above,  is  given  on  the  following  page. 


445 


NAPHTHALENE 


TABLE  SHOWING  THE  TEMPERATURES  AT  WHICH  SOLUTIONS  OF  THE  GIVEN  COM- 
POSITIONS BEGIN  TO  SEPARATE  INTO  Two  LAYERS  IN  PRESENCE  OF  SOLID 
NAPHTHALENE.  (Cady,  1898.) 

(Calculated  as  described  on  preceding  page.) 

Cms.  per  100  Gms.  Solution. 
f. 
65.5 

53-3 
45 
38 
32.2 

28.5 
28.2 

The  isotherms  for  intervals  of  10°  lie  so  close  together  that  they  are  practically 
indistinguishable  for  the  greater  part  of  their  length. 

SOLUBILITY  OF  NAPHTHALENE  IN  LIQUID  CARBON  DIOXIDE. 

(Buchner,  1905-06.)     (Synthetic  Method  used.) 


Acetone. 

Water. 

Naphthalene. 

10 

89.92 

0.08 

ig.QI 

80 

0.09 

29.92 

69.67 

0.41 

4O.8l 

58.22 

o  97 

48.67 

48.68 

2.65 

57-43 

36.64 

5-93 

60.43 

25-75 

13.82 

Crit.  Temp. 

34-8 

64 

80 


Gms.  CnHg  per 
100  Gms.  Sat.  Sol. 

8 
54 

IOO 


loo  gms.  95%  formic  acid  dissolve  0.30  gm.  naphthalene  at  18.5°.      (Aschan,  1913.) 
100  gms.  95  %  formic  acid  dissolve  3.44  gms.  a  nitronaphthalene  at  18.5°.        " 
Data  for  equilibrium  in  the  systems:  naphthalene,  phenol,  water  and  naphtha- 
lene, succinic  acid  nitrile,  water,  determined  by  the  synthetic  method,  are  given 
by  Timmermans  (1907). 

SOLUBILITY  OF  NAPHTHALENE  IN; 


Chloroform. 

(Speyers;  Etard.) 

Carbon  Tetra        Carbon     Di 
Chloride,                Sulphide. 

(Schroder  —  Z.  physik.  (Arctowski  —  Compt 
Ch.  ii,  457/93.)    rend.  121,  123/95;  Etard.) 

ft0               Wt.  of  i  cc. 
Solution. 

Gms.  C10H8  per 
100  Grama 
CHCJa. 

Gms.  CioH8  per 
too  Gms.  SaL 
Solution, 

Oms.  C-iQrig  per 
too  Gms.  Sat. 
Solution. 

-108 

• 

... 

0.63 

-82 

.  1  . 

1.38 

~~~  5° 

23 

-30 

8.8 

6.6 

—   10 

15-6 

... 

14.1 

0 

•393 

19-5 

9-0 

19.9 

+   10 

•355 

25-5 

I4-O 

27-5 

20 

.300 

31.8 

20-0 

36-3 

25 

.280 

35-5 

23-0 

41  -o 

30 

•255 

40.1 

26.5 

46.0 

40 

.205 

49-5 

35-5 

57  -2 

50 

.150 

60.3 

47-5 

67.6 

60 

.090 

62.5 

79-2 

70 

.040 

87^2 

80.0 

9°  -3 

NOTE.  —  Speyers'  results  upon  the  solubility  of  C10H8  in  CHC13, 
when  calculated  to  grams  per  100  grams  of  solvent,  agree  quite  well 
with  Etard's  (Ann.  chim.  phys.  [712  570,  '94  figures,  reported  on  the 
basis  of  grams  C10H8  per  100  grams  saturated  solution. 


NAPHTHALENE 


446 


Benzene. 


SOLUBILITY  OF  NAPHTHALENE  IN: 

(Schroder;  Etard;  Speyers.) 

Chlor  Benzene.     Hexane. 


50 
20 
O 
10 
20 
25 
30 
40 

50 
60 

70 
80 


Gms.  CioH8 

per  100  Gms. 

Solution. 


27 

36 
40 

45 
54 
65 
77 


88.0 


Gms.  CioHg 

per  100  Gms. 

Solution. 


24.0 
31.0 


39-o 
48.0 

57-5 
70-5 
85.0 


Gms.  C10H8 

per  loo  Gms. 

Solution. 

o-3 
1.9 

5-5 

9.0 
14.0 
17-5 

21  .0 
30.8 

43-7 
60.6 
78.8 


Toluene. 


wt.  of  i  cc. 

Solution. 


0.9124 
0.9126 
0-9I35 
0-9I55 
0.9180 
0.9250 
0.9350 
0-9475 

o . 9640 

0.9770 


Gms.  CioH8 

per  100  Gms. 

C6H5.CH3. 


15-0 
28.0 
36.0 
42.O 
56.0 

69-5 
83.0 

97-5 

III.O 


Freezing-point  data  (solubility,  see  footnote,  p.  i)  are  given  for  mixtures  of 
naphthalene  and  each  of  the  following  compounds: 


ttNaphthol.  (Crompton  &  Whitely,  1895;    Kuster, 

'95;  Vignon,  '91 ;  Miers  &  Isaac,  'o8a.) 

ft  Naphthol.  (Crompton  &  Whitely,  1895;  Vignon, 

iSgirlsaac,  1908.) 

a  Naphthylamine.       (Vignon,  1891.) 
0 

Dihydronaphthalene.  (Kuster,  1891.) 
Nitronaphthalene.       (Palazzo  &  Battelli,  1883.) 
Palmitic  Acetic  Ester.  (Batelli  &  Martinetti,  '85.) 
Paraffin.  (Palazzo  &  Battelli,  1883.) 

Phenanthrene.         (Vignon,  1891;  Miolati,  1897.) 

Phenol.  (Yamamoto,  '08;  Hatcher  &  Skirrow,  '17.) 
0  Nitrophenol.  (Saposchinikow,  '04 ;  Kremann,  '04.) 
p  Nitrophenol.  (Kremann,  1904.) 


2.4  Dinitrophenol.  ( (Saposchinikow,  1904; 
Picric  Acid.  (      Kremann,  1904.) 

Pyridine.  (Hatcher  &  Skirrow,  1917.) 

Pyrocatechol.  (Kremann  &  Janetzky,  1912.) 
Resorcinol.         (Vignon,  1891;    Kremann  & 

Janetzky,  1912.) 

Stearic  Acid.  (Gourtonne,  1882.) 

Sulfur.  (Bylert,         .) 

Nitrotoluene.  (Kremann,  1904.) 

i.2.4Dinitrotoluene.  " 

1 .2 .6  "         (Kremann  &  Rodinis,  1906.) 

1.34 

I.3;5 

Trinitrotoluene.         (Kremann,  1904.) 

P  Toluidine.  (Vignon,  1891.) 

Thymol.  (Roloff,  1895.) 


F.-pt.  data  are  also  given  for  the  following  mixtures: 

Nitronaphthalene  +  Paraffin.  (Campetti  &  Delgrosso,  1913;  Palazzo  &  Batelli,  1883.) 

a  Nitronaphthalene  +  Urethan.  (Mascarelli,  1908.) 

a  Nitronaphthalene  +  «  Naphthylamine.      (Tsakalotos,  1912.) 


NAPHTHALENE  SULFONIC  ACID  C10H7SO3H. 

SOLUBILITY  IN  AQUEOUS  HYDROCHLORIC  ACID  AT  30°. 

(Masson,  1912.) 


dyoi  Sat. 

Solution. 
.1925 
•1653 

•1553 
.1115 
.1197 
.1569 


Mols.  per  Liter  Sat.  Sol. 


HC1. 

C10H7SO,H. 

0 

3  •  263 

I.29I 

2.470 

1.826 

2.117 

4.017 

0.762 

7.232 

0.089 

0.88 

0.063 

Gms.  per  Liter  Sat.  Sol. 


HC1. 

C10H7S03H. 

O 

679 

47.08 

5H 

66.59 

440.6 

146.5 

158.6 

263.7 

I8.5 

300.3 

I3-I 

447  NAPHTHOIC  ACID 

0  NAPHTHOIC  ACID  Ci0H7COOH. 

One  liter  of  aqueous  solution  contains  0.058  gm.  Ci0H7COOH  at  25°. 

(Paul,  1894.) 
Dihydro  p  NAPHTHOIC  ACIDS  Ci0H9COOH  (118°  and  161°  isomers). 

SOLUBILITY  OF  EACH  ISOMER,  DETERMINED  SEPARATELY,  IN  WATER. 

(Derick  and  Kamra,  1916.) 

cc.  o.oi  n  Ba(OH)2  Solution  Required 
AO  per  10  cc.  of  the  Sat.  Solution  of  the: 


118°  Isomer. 

161°  Isomer. 

0 

0-39 

O.I9 

20 

0.56 

o-34 

40 

1-34 

0.69 

55-56 

2.89 

i-45 

71-72 

6.7 

3.48 

80 

9-3 

4.68 

00 

14.6 

8 

96-97 

20.1 

io-5 

P  NAPHTHOL  CioHyOH. 

SOLUBILITY  IN  WATER. 

Gms.0C10H7OH 

t°.  per  100  cc.  Authority. 

Sat.  Sol. 

12.5  0 . 044  (Kuriloff,  1897.) 

25.1  0 . 074  (Kttster,  1895.) 

29.5  0.0876  (Kuriloff,  1898.) 

Data  for  the  solubility  of  isomorphous  mixtures  of  0  naphthol  and  naphthalene 
in  water  at  25.1°  are  given  by  Kiister  (1895). 

SOLUBILITY  OF  /3  NAPHTHOL  IN  AQUEOUS  SOLUTIONS  OF  PICRIC  ACID  AT  29°. 

(Kuriloff,  1898.) 
Mols.  X  lo6  per  100  cc.  Solution.  Gms.  per  100  cc.  Solution. 


QH2.OH(N02)3. 

C,0H7OH. 

C6H2OH(N02)3. 

Ci0H7OH. 

Solid  Phase. 

0 

609 

O 

0.0877 

0  Naphthol 

54 

615 

0.0124 

0.0886 

" 

68.5 

62O 

0.0157 

o  .  0894 

"  +/3  Naphtholpicrate 

69 

607 

0.0158 

0.0875 

0  Naphtholpicrate 

69 

597 

0.0158 

0.0860 

• 

88 

494 

O.O2I2 

O.O7I2 

• 

100 

390 

0.0229 

0.0562 

" 

196 

180 

O.O449 

0.0259 

« 

308 

105 

o  .  0706 

O.OI5I 

« 

933 

8 

0.2138 

O.OOII 

"  +PicricAcid 

928 

0 

O.2I26 

0 

Picric  Acid 

Data  are  also  given  for  the  distribution  of  0  naphthol  between  water  and  ben- 
zene. The  mean  of  the  cone,  in  C6H6  layer  divided  by  cone,  in  H2O  layer  is  given 
as  67.  The  temperature  is  not  given.  The  determination  of  the  ft  naphthol  was 
made  by  an  iodine  titration  method. 

The  coefficient  of  distribution  of  /3  naphthol  between  H2O  and  CHClj  at  25°  is; 
cone,  in  H2O  -5-  cone,  in  CHCls  =  0.0171.  (Marden,  1914.) 

Data  for  the  solubility  of  /9  naphthol,  picric  acid  (naphthol  picrate)  and  their 
mixtures  in  benzene,  determined  by  the  synthetic  (sealed  tube)  method,  are  given 
by  Kuriloff  (i897a). 

100  cc.  90%  alcohol  dissolve  about  55  gms.  /3  Ci0H7OH  at  15.5°. 

(Greenish  and  Smith,  1903.) 

100  gms.  95%  formic  acid  dissolve  3.11  gms.  /3  C10H7OH  at  18.6°.    (Aschan,  1913.) 


NAPHTHOL  448 


SOLIDIFICATION  TEMPERATURES  OF  MIXTURES  OF  ft  NAPHTHOL  AND  SALOL. 

(Bellucci,  1912.) 

t°  of  Cms.  0  CioH7pH  per  t°  of  Cms.  0  C10H7OH  per 

Solidification.  100  Cms.  Mixture.  Solidification.  100  Gms.  Mixture. 

121.7  ioo  80  40 

116.5  9°  68  30 

in  80  52.5  20 

105  70  34  Eutec.  10 

97-5  °°  38.5  5 

88  -  -    50  42  o 

FREEZING-POINT  DATA  (Solubility,  see  footnote,  p.  i)  ARE  GIVEN  FOR  THE 
FOLLOWING  MIXTURES: 

a  Naphthol  +  a.  Naphthylamine.  (Vignon,  1891.)  ^ 

+  ft 

+  Dimethylpyrone.  (Kendall,  1914.) 

-j-  Resorcinpl.  (Vignon,  1891.) 

+  p  Toluidine.  (Vignon,  1891;  Philip,  1903.) 

ft  Naphthol  +  a  Naphthol.  (Vignon,  1891;  Crompton  and  Whiteley,  1895.) 

"  +  a  Naphthylamine  (Vignon,  1891.) 

+  /3. 

+  Dimethylpyrone  (Kendall,  1914.) 

+  Picric  Acid.  (Kendall,  1916.) 

-j-  Sulfonal  (Bianchini,  1914.) 

+  p  Toluidine.  (Vignon,  1891.) 

a  NAPHTHYLAMINE  p  Sulfonic  Acid,  1.4  a.  Ci0H6NH2.SO3H. 
a  NAPHTHYLAMINE  o  Sulfonic  Acid,  1.2  a  doHeNHi.SOsH. 
SOLUBILITY  OF  EACH  SEPARATELY  IN  WATER. 

(Dolinski,  190?  "* 
Gms.  per  ioo  Gms.H2O.  Gms.  per  ioo  Gms.  H2O. 


t°. 

p  Sulphonic 

o  Sulphonic 

t°. 

p  Sulphonic 

o  Sulphonic 

Ac. 

Ac. 

Ac. 

Ac. 

0 

0.027 

0.24 

50 

0.059 

0.81 

10 

O.O29 

0.32 

60 

0-075 

I  .01 

20 

0.031 

0.41 

70 

0.097 

i  .37 

30 

0.037 

0.52 

80 

0.130 

1.  80 

40 

0-048 

0.65 

90 

0.175 

2  .40 

IOO 

0.228 

3-19 

The  coefficient  of  distribution  of  ft  naphthylamine  between  benzene  and  watei 
at  25°  is;  cone,  in  C6H6-:-  cone,  in  H2O  =  279.  The  coefficient  for  a  naphthyla 
mine,  similarly  determined,  is  252.  (Farmer  and  Warth,  1904 ) 

FREEZING-POINT  DATA  ARE  GIVEN  FOR  THE  FOLLOWING  MIXTURES: 

a  Naphthylamine  +  Phenol.  (Philip,  1903.) 

+  Quinol.  (Philip  &  Smith,  1905.) 

+  Resorcinpl.  (               "                ;  Vignon,  1891.) 

+  p  Toluidine.  (Vignon,  1891.) 

ft  Naphthylamine  -j-  Phenol.  (Kremann,  1906.) 

-j-  Rescorcinol.  (Vignon,  1891.) 

+  p  Toluidine. 

P  NAPHTHYL   BENZOATE   C6H5COOC10H7. 

ioo  gms.  95%  formic  acid  dissolve  0.25  gm.  CeHsCOOCioHr  at  18.6°. 

(Aschan,  1913.) 

NARCEINE   C23H27N08  +  3H2O. 

ioo  gms.  H2O  dissolve  0.076  gm.'narceine  at  13°;  ioo  gms.  80%  alcohol  dissolve 
0.105  gm.  at  13°. 

ioo  gms.  CC14  dissolve  o.on  gm.  narceine  at  17°  (Schindelmeiser,  1901);  0.002 
gm.  at  20°  (Gori,  1913). 


449 


NARCOTINE 


NARCOTINE   C20H23NO7. 

SOLUBILITY 

IN 

SEVERAL  SOLVENTS. 

Solvent. 

t°. 

Gms.  Narcotine  per 
100  Gms.  Solvent. 

Authority. 

Water 

15 

0    I* 

(Guerin,  1913.) 

Water 

20 

O.OO445 

(Zalai,  1910.) 

Acetone 

15 

41.96* 

(Guerin,  1913.) 

Aq.  50  Vol.  %  Acetone 

15 

0.7* 

« 

Aniline 

20 

25 

(Scholtz,  1912.) 

Pyridine 

2O 

2-3 

« 

Piperidine 

20 

« 

Diethylamine 

2O 

0.4 

« 

Carbon  Tetrachloride 

2O 

1.04 

(Gori,  1913-) 

Trichlor  Ethylene 

15 

6.5 

(Wester  and  Bruins,  1914.) 

Oil  of  Sesame 

2O 

0.086 

(Zalai,  1910.) 

*  Per  100  cc.  solvent. 

NEODYMIUM   CHLORIDE   NdC1.6H2O. 

SOLUBILITY  IN  WATER.     (Matignon,  1906,  1909.) 
Method  of  obtaining  saturation  not  stated. 

Cms.  NdCl3  per  100  Cms.  Cms.  NdCl3.6HoO  per  100  Gms. 


jj 

Sat.  Sol. 
1.74 


Sat.  Sol.  Water.  Sat.  Sol.  Water. 

13  1-74  49-67  98.68  71.12  246.2 

100  ...  ...  140 

100  gms.  abs.  alcohol  dissolve  44.5  gms.  (anhydrous)  NdCl3  at  20°.     Saturation 
was  obtained  by  spontaneous  evaporation  of  the  solution  over  H2SO4. 

(Matignon,  1906.) 

100  gms.  anhydrous  pyridine  dissolve  1.8  gms.  anhydrous  NdCl3  at  about  15°. 
Saturation  obtained  by  daily  agitation  of  the  solution  for  some  weeks.  (Matignon,  '06.) 

NEODYMIUM  COBALTICYANIDE  Nd2(CoC6N6)2.9H2O. 

looogms.aq.  io%HCl  (di5  =  1.05)  dissolve  4. 19  gms.  salt  at  25°.  (James  &  Willand,  '16.) 

NEODYMIUM   GLYCOLATE   Nd(C2H3O3)3. 

One  liter  H2O  dissolves  4.609  gms.  salt  at  2O°.  (Jantsch  &  Grimkraut,  1912-13.) 

NEODYMIUM  MOLYBDATE   Nd2(MoO4)3. 

One  liter  H2O  dissolves  0.0186  gm.  salt  at  28°  and  0.0308  gm.  at  75°.     The 
mixtures  were  frequently  stirred  at  constant  temperature  during  only  two  hours. 

(Hitchcock,  1895.) 

NEODYMIUM   Double  NITRATES. 

SOLUBILITY  IN  AQ.  HNO3  OF  d^=  i.325(  =  51.59  GMS.  HNO3  PER 

100  CC.)    AT    16°.     (Jantsch,  1912.) 

Gms.  Hydrated 

Double  Salt.  Formula.  Double  Salt  per 

100  Gms.  Sat.  Sol 

Neodymium  Magnesium  Nitrate  [Nd(NO3)6]2Mg3.24H2O         97.7 

Nickel  "  "         Ni3        "  116.6 

Cobalt  "  "         CO3      "  151.6 

Zinc  "  "         Zn3       "  177 

Manganese        "  Mn3      "  296 

NEODYMIUM   OXALATE   Nd2(C2O4)3.ioH2O. 

SOLUBILITY  IN  WATER  AT  25°  BY  ELECTROLYTIC  DETERMINATION. 

(Rimbach  and  Schubert,  1909.) 

One  liter  sat.  solution  contains  0.0053  mg-  equivalents  of  anhydrous  salt  =  0.49 
milligram. 

SOIJUBILITY  IN  AQUEOUS  20%  SOLUTIONS  OF  METHYL,  ETHYL  AND  TRIETHYL 
AMINE  OXALATBS,  ROUGHLY  DETERMINED.    (Grant  and  James,  1917.) 

100  cc.  aq.  20%  methyl    amine  oxalate  dissolve  0.027  gm.  neodymhim  oxalate. 
"       ethyl  "  "  "       ai07    " 

"       triethyl        "  ^  "       0.065    "-  " 


NEODYMIUM   OXALATE  450 

SOLUBILITY  OF  NEODYMIUM  OXALATE  IN  AQUEOUS  SOLUTIONS  OF 

NEODYMIUM   NITRATE  AT  25°.      (James  and  Robinson,  1913.) 

(The  mixtures  were  constantly  agitated  at  constant  temperature  for  twelve 
weeks.) 
Gms.  per  100  Gms.  Sat.  Sol.  Gms.  per  100  Gms.  Sat.  Sol. 

Solid  Phase. 


Nd2(C204)3. 

Nd2(NO3)6. 

Nd2(C204)3. 

Nd2(N03)6. 

0.18 

6.46       Nd2(C204)3.nH20 

2.07 

47.64 

0-54 

12.23 

2-54 

50-52 

0.76 

17.78 

2.89 

52.82 

0.85 

22.67 

3-17 

54.67 

0.96 

27-43 

2.21 

56.48Pr. 

1.28 

3I-36                     " 

1.44 

59.68 

1.38 

1.33 

59-67 

1.66 

38^0 

I.  21 

59-70 

1.88 

42.13 

0.96 

59-75 

1.96 

44.82 

60.46 

1.2^.24 
Nd2(NO3)6(?H20) 


4)3.2|Nd2(N03)6.24H20. 

NEODYMIUM   Dimethyl  PHOSPHATE   Nd2[(CH3)2PO4]6. 

100  gms.  H2O  dissolve  56.1  gms.  Nd2[(CH3)2PO4]6  at  25°  and  about  22.3  gms. 

at  95°-  (Morgan  and  James,  1914.) 

NEODYMIUM  SULFATE   Nd2(SO4)3. 

SOLUBILITY  IN  WATER. 

(Muthmann  and  Rolig,  1898.) 

Gms.  Nd2(SO4)^  per  100  Gms.  Gms.  Nd2(SO4)3  per  TOO  Gms. 

Solution.  Water.  Solution.  Water. 

o          8.7  9.5  50          3.5  3.7 

16          6.6  7.1  80          2.6  2.7 

30          4.7  5  108          2.2  2.3 

NEODYMIUM   SULFONATES. 

SOLUBILITY  IN  WATER. 

Gms.  Anhy- 
Sulfonate.  Formula.  t°.  dr™Qs  Q^f61      Authority. 

H2O. 
Neodymium : 

m          (Nitrobenzene  Nd[C6H4(NO2)SO3]3.6H2O  15     46.1       (Holmberg,  1907.) 

Bromo}      Sulfonate      Nd[C6H3Br(i)NO2(4)SO3(3)]3.8H2O  25         7.25       (Katz& James,  1913.) 

NEODYMIUM   TUNGSTATE   Nd2(WO4)3. 

One  liter  H2O  dissolves  0.0190  gm.  Nd2(WO4)3  at  22°,  0.0168  gm.  at  65°  and 
0.0152  gm.  at  98°.  The  mixtures  were  not  constantly  agitated  and  only  two 
hours  were  altowed  for  saturation.  (Hitchcock,  1895.) 

NEON   Ne. 

SOLUBILITY  IN  WATER. 

(v.  Antropoff,  1909-10.) 
t°.  o.  10.  20.  30.  40.  50. 

Coef.  of  Absorption /?    0.0114   0.0118   0.0147   0.0158   0.0203    0.0317 

The  results  are  in  terms  of  the  coefficient  of  absorption  as  defined  by  Bunsen 
(see  p.  227)  and  modified  by  Kuenen,  in  respect  to  substitution  of  mass  of  H2O 

for  volume  of  H2O  in  the  formula      Absorp.  coef.  Kuenen  =  — ~rrrv>  vx  r>* 

mass  of  H2O  X  P 

NEURINE  PERCHLORATE   CH2.CH.N(CH3)3ORHC1O4. 

100  gms.  EUO  dissolve  4.89  gms.  of  the  salt  at  14.5°         (Hofmann  &  Hobold,  1977.) 


451 
NICKEL  BROMATE   Ni(BrO3)2.6H2O. 

100  gms.  cold  water  dissolve  27.6  gms.  nickel  bromate. 


NICKEL   BROMATE 


NICKEL  BROMIDE 


NiBr2.6H2O. 

SOLUBILITY  IN  WATER. 

(Etard,  1894.) 


t°. 
-20 

—  io 
o 

+  10 
20 


Gms.  NiBrt 

per  100  Gms. 

Solution. 


47. 

50. 
53 
55 
56. 


t°. 

25 

30 
40 
50 
60 


Gms.  NiBr, 

per  100  Gms. 

Solution. 

57.3 

58 

59.1 
60 
60. 


t°. 

80 

ioo 
120 
140 


NICKEL  CARBONATE  NiCO3. 

One  liter  H2O  dissolves  7.?8<)\X  io~*  mols.  NiCO3 

NICKEL   CARBOXYL. 


Gms.  NiBrj 

per  100  Gms. 

Solution. 

60.6 

60.8 
60.9 
6  1 


0.0925  gm.  at  25°. 

(Ageno  and  V 


(Ageno  and  Valla,  1911.) 


ioo  gms.  of  the  aqueous  solution  saturated  at  9.8°  contain  2.36  cc.  of  the  vapor 
6.43  milligrams  Ni.     In  blood  serum  it  is  2  \  times  as  soluble.          (Armit,  1907.) 


NICKEL    CHLORATE    Ni(ClO3)2. 

SOLUBILITY  IN  WATER. 

(Meusser  —  Ber.  35,  1419,  '02.) 


48 

55 

65 

79-5 
-13-5 
—  9  26.62 

Sp.  Gr.  of  solution  saturated  at  +  18  =  1.661. 

According  to  Carlson  (1910)  ioo  gms.  sat.  sol.  in  H2O  at  16°  contain  64.1  gms. 
Ni(ClO3)2  and  du  of  sat.  sol.  =  1.76. 


Gms. 

Mols. 

t° 

Ni(ClO3)2 

Ni(C103)2 

Solid 

per  ioo  Gms, 
Solution. 

.     per  ioo 
Mols.H2O 

Phase. 

-18 

49-55 

7.84 

Ni(ClO3)2.6H2O 

-  8 

5J-52 

8.49 

" 

o 

52.66 

8.88 

" 

+  18 

56-74 

10-47 

" 

40 

64.47 

15.35 

it 

Gms.           Mols. 
Ni(ClO3)2    Ni(ClO3)2 
per  ioo  Gms.      per  ioo 

Solid 
Phase. 

Solution.      Mols.  H2O. 

67.60         16.65 

Ni(C103)24H,0 

68.78         17.59 

•4 

69.05         iS.OI 

« 

75.50         24.68 

• 

3J-85        3-73 

Ice 

2.90 


NICKEL  PerCHLORATE   Ni(ClO4)2.9H2O. 

SOLUBILITY  IN  WATER. 

(Goldblum  and  Terlikowski,  1912.) 
Gms 


O 

10.9 
21.3 

30.7 

49 

30.7 


H20. 

O 

33.19 
46.68 

70 

.. 

90 


Ice 


Ice  +  Ni(ClO4)3.9H2O 


—21.3 

9 
7-5 

18 

26 

45 


Gms. 


H20. 

..  92.5["Ni(ClO4)s9H»0 

573  104.6    Ni(ClO4),.sH,Q 

576  1  06.  8    Ni(C10<)3.sH,0 

576  no.i 

584  112.  2 

594  1  18.  6 


NICKEL  CHLORIDE 


452 


NICKEL   CHLORIDE   NiCl2.6H2O. 

SOLUBILITY  IN  WATER. 

(Etard,  1894.) 


t-. 

Gms.  NiCU 
per  ioo  Gms. 
Solution. 

«-. 

Gms.  NiClj 
per  ioo  Gms. 
Solution. 

t°. 

Gms.  NiCl2 
per  ioo  Gms. 
Solution. 

-17 

29.7 

25 

40 

60 

45.1 

o 

35 

30 

40.8 

70 

46 

+  10 

37-3 

40 

42.3 

78 

46.6 

20 

39  -1 

50 

43-9 

IOO 

46.7 

1000  cc.  sat.  HC1  solution  dissolve  4  gms.  NiCl2  at  12°.  (Ditte,  1881.) 

100  gms.  abs.  alcohol  dissolve  10.05  Sms-  NiCl2  at  room  temperature. 

100  gms.  abs.  alcohol  dissolve  53.71  gms.  NiCl2.6H2O  at  room  temperature. 

(Bodtker,  1897.) 

100  gms.  abs.  alcohol  dissolve  2.16  gms.  NiCl2.7H2O  at  17°,  and  1.4  gms.  at  3°. 

(de  Bruyn,  1892.) 

100  gms.  saturated  solution  in-glycol  contain  16.2  gms.  NiCl2  at  room  tem- 
perature, (de  Coninck,  1905.) 

loo  cc.  anhydrous  hydrazine  dissolve  8  gms.  NiCl2  at  room  temp,  and  solu- 
tion is  colored  violet.  (Welsh  and  Broderson,  1915.) 

ioo  gms.  95%  formic  acid  dissolve  5.9  gms.  NiCl2  at  20.5°.  (Aschan,  1913.) 

When  i  gm.  of  nickel,  as  chloride,  is  dissolved  in  ioo  cc.  of  10%  aq.  HC1  and 
shaken  with  ioo  cc.  of  ether,  o.oi  per  cent  of  the  Nickel  enters  the  ethereal  layer. 

(Mylius,  1911.) 

NICKEL  CITRATE  Ni3[(COOCH2)2C(OH)COO]2.2H2O. 

'ioo  cc.  sat.  solution  in  water  contain  0.28  gm.  Ni  =[0.94  gm.  anhydrous 
salt  at  IO°.  (Pickering,  1915.) 

NICKEL   Potassium   CITRATE   K4Ni[(COOCH2)2COHCOO]2. 

ioo  cc.  sat.  sol.  in  water  contain  3.9  gms.  Ni  =  41  gms.  salt  at  10°. 

(Pickering,  1915.) 

NICKEL  HYDROXIDE  Ni(OH)2. 

Aqueous  ammonia  solutions  of  nickel  hydroxide  were  evaporated  in  a  vacuum 
desiccator  and  samples  withdrawn  at  intervals  for  analysis.  The  results  obtained 
in  duplicate  series  yielded  different  curves.  For  2  n  NHs  the  gms.  Ni  per  liter 
varied  from  0.17  to  0.83.  For  4  n  NH3,  the  gms.  Ni  per  liter  varied  from  0.36 
to  1.8.  (Bonsdorff,  1904.) 


NICKEL   IODATE    Ni(IO3)24 
SOLUBILITY  IN  WATER. 

(Meusser  —  Ber.  34,  2440,  *oi.) 

Gms.              Mols.                                                            Gms.              Mols. 
to       Ni(IO3)2        Ni(IO3)2               Solid                     to        Ni(IO3)2        Ni(IO3)2              Solid 
'    per  ioo  Gms.  per  ioo  Mols.        Phase.                         '  per  ioo  Gms.  per  ioo  Mols.        Phase. 
Solution.           H2O.                                                           Solution.           H2O. 

0        0-73         0.033       Ni(I03)24H20             18        0.55         0.0245     Ni(IOa)2.2H20  (a) 

18 

I  -01 

0.045 

50      0.81 

0-035 

1C 

30 

1.41 

0.063 

75 

•03 

0.045 

tc 

O 

o-53 

0.023 

Ni(I03)2.2H20  (i)       80 

.12 

O.O49 

It 

18 

0.68 

0.030 

30 

•135 

O.05O 

Ni(I03)2 

30 

0.86 

0.039 

.07 

0-046 

" 

50 

1.78 

0.080 

75 

.02 

0.045 

" 

8 

0.52 

0.023 

Ni(I03)2.2H2O  (2)       90        0.988 

0.044 

M 

(i)  a  Dihydrate. 


(2)  /3  Dihydrate. 


453 


NICKEL  IODIDE 


NICKEL  IODIDE   NiI2.6H2O. 


—  20 

O 

IO 

20 


Gms.  NiI2  per 
100  Gms.  Solution 

52 

55-4 
57-5 
59-7 


IN  WATER.    (Etard,  1894.) 

xo           Gms.  Nil2  per 
loo  Gms.  Solution. 

to            Gms.  NiI2  per 
100  Gms.  Solution. 

25 

60.7 

60 

64.8 

30 

61.7 

70 

65 

40 

63.5 

80 

65.2 

50 

64.7 

90 

65-3 

By  interpolation  the  tr.  pt.  for  NiI2.6H2O  +  NiI2.4H2O  is  at  43°. 

NICKEL  MALATE   Ni[CH2CHOH(COO)]2.3H2O. 

loo  cc.  sat.  solution  in  water  contain  0.02  gm.  Ni  =  0.06  gm.  salt_at  ip°. 

NICKEL   NITRATE   Ni(NO3)2. 

SOLUBILITY  IN  WATER. 

(Funk  —  Wiss.  Abh.  p.  t.  Reichanstalt,  3,  439,  *oo.) 


(Pickering,  1915.) 


Gms.  Mols. 

Ni(NO3)2      Ni(N03)2  Solid 

per  100  Gms.  per  100  Mols.       Phase. 
Solution.         H2O. 


Ni(NO3)2.9H2O 


Ni(N03)2.6H20 


-23 

39 

.02 

6-31 

—  21 

39 

.48 

6-43 

—  10 

•5  44 

•13 

7-79 

—  21 

39 

•94 

6-55 

—  12 

•5  4i 

•59 

7.01 

—  10 

42 

.11 

7.16 

-  6 

43 

.00 

7-44 

O 

44 

•32 

7.86 

+  18 

48 

•59 

9-3 

Gms.  Mols. 

Ni(N03)2      Ni(NO3)2  SoUd 

per  100  Gms.  per  100  Mols.        Phase. 


Ni(NOa)2.6H2O 


Ni(N03)3.3H20 


Solution. 

H2O. 

20 

49.06 

9-49 

41 

55-22 

12.  1 

S^ 

•7    62.76 

I6.7 

58 

61.61 

J5-9 

60 

61.99 

16.0 

64 

62.76 

16.6 

70 

63-95 

17.6 

90 

70.16 

23.1 

95 

77.12 

33-3 

100  gms.  sat.  solution  in  glycol  contain  7.5  gms.  Ni(NO3)2  at  room  temperature. 

(de  Coninck.) 
100  cc.  anhydrous  hydrazine  dissolve  3  gms.  Ni(NO3)2  at  room  temp. 

(Welsh  and  Broderson,  1915.) 

NICKEL   OXALATE   Ni(COO)2. 

100  gms.  95%  formic  acid  dissolve  o.oi  gm.  at  19.8°.  (Aschan,  1913.) 

NICKEL  SULFATE   NiSO4.7H2O. 

SOLUBILITY  IN  WATER.      (Steele  and  Johnson,  1904;  see  also  Tobler,  Etard  and  Mulder.) 


Grams  NiSO4  per 
*o                    zoo  Gms.                     Solld 

*      •                                                    *                                                      T>U««« 

t° 

Grams  NiSO4  per 
100  Gms. 

Solid 
Phase. 

Solution. 

Water.' 

Solution. 

Water. 

-5 

20 

•47 

25 

.  74      NiSO4.7H2O 

33 

•  O 

30 

•25 

43 

•35 

NiSO4.6H2O 

0 

21 

.40 

27 

.22 

35 

.6 

30 

•45 

43 

•79 

•      (blue) 

9 

23 

•99 

31 

•55 

44 

•7 

32 

•45 

48 

•05 

" 

22  .6 

27 

.48 

37 

.90 

5° 

.0 

33 

•39 

5° 

.15 

" 

30 

29 

•99 

42 

.46 

53 

.0 

34 

•38 

52 

•34 

" 

32-3 

30 

•57 

44 

•  O2                " 

54 

•5 

34 

•43 

52 

•50 

NiSO4.6H2O 

33 

31 

•38 

45 

•74 

57 

.0 

34 

.81 

53 

.40 

"  (green) 

34 

31 

.20 

45 

•5 

60 

35 

•43 

54 

.80 

" 

32-3 

30.35 

43 

.57      NiSO4.6H2O 

7° 

37 

•29 

59 

•44 

" 

33  -° 

30 

•25 

43 

•35            "    <blue> 

80 

38 

.71 

63 

•17 

M 

34-o 

30 

•49 

43 

•83 

99 

43 

.42 

76 

•71 

M 

Transition  points,  hepta  hydrate  <=±  hexa  hydrate  =  31.5* 
Hexa  hydrate  (blue)  ^±  hexa  hydrate  (green)  =  53.3°. 


NICKEL   SULFATE 


454 


SOLUBILITY  OF  MIXTURES  OF  NICKEL  SULPHATE  AND  COPPER  SULPHATE. 


Results 

at  35°. 

Gms.  per  100  Gms.  H^. 

Mol.  per  cent  in  Solution. 

Mol.  per  cent  in  Solid  Phase.       Crystal 

CuSO4. 

NiSO4.  * 

CuS04. 

NiSO4/ 

'CuS04. 

NiSO4. 

Form. 

9.62 

583-9 

1.57 

98.43 

o-35 

99-65 

Rhombic 

41.66 

484.4 

7.69 

92.31 

2.12 

97.88 

" 

75-39 

553-5 

11.66 

88.34 

4.77 

95-23 

Tetragonal 

106.40 

506-5 

16.92 

83.08 

6-52 

93-48 

" 

172.0 

483.8 

25-63 

74-37 

13.88 

86.17 

" 

186.9 

468.0 

27.90 

72.IO 

(I8.77 
(94.91 

81-23 

5-09 

Tetragonal 
Triclinic 

Results 

at  67°. 

20.04 

729-3 

2.65 

97-35 

o-93 

99.07 

Monociinic 

66.01 

706.2 

8.3I 

91.69 

2.86 

97.14 

" 

88.08 

501.6 

86.45 

3-92 

96.08 

•« 

47-94 

675.0 

16.39 

83.61 

6.66 

93-34 

» 

249-9 

747-8 

24.46 

75-54 

22.32 

77.68 

f  Monociinic 
I  Triclinic 

SOLUBILITY  OF  MIXTURES  OF  NICKEL  SULPHATE  AND  SODIUM  SUL- 
PHATE, ETC. 

(Koppel;  Wetzel  —  Z.  physik.  Chem.  52,  401,  '05.) 


Gms.  per  100 
t°.                Gms.  Solution. 

Gms.  per  100 
Gms.H2O. 

Mols.  per  100 
Mols.  H2O. 

SoKd 

Dl  

NiS04. 

Na8S04. 

NiS04. 

Na2S04. 

'NiS04.      Na2S04.  '         fudx' 

O 

16 

•94 

7 

.61 

22 

.46 

10 

.09 

2 

.61     1.28  " 

. 

5 

17 

•99 

IO 

•85 

25.28 

J5 

.24 

2 

•94       1-93 

NiS04.7H20  + 
Na2SO4.ioH2O 

10 

18 

•97 

I3-85 

28 

.26 

20 

.64 

3 

.29       2.61 

20 

18 

.76 

17 

.21 

29 

•3i 

26 

.87 

3 

.410    3.404 

NiNa2(S04)24HaO 

25 

17 

•85 

16 

•54 

27 

•33 

25 

•33 

3 

.181    3.208 

« 

30 

16 

•74 

15 

•34 

24 

.64 

22 

•58 

2 

.868     2.861 

it 

35 

16 

.28 

14 

.91 

23 

.66 

21 

.67 

2 

•753     2.744 

- 

40 

15 

•35 

14.49 

21 

.88 

20 

•65 

2 

.546     2.616 

i* 

18.5 

'9 

.61 

16 

•49 

30 

.70 

25 

.80 

3 

•S6      3-27  * 

20 

20 

•i3 

16 

•IS 

•59 

25 

•35 

3 

.67      3.21 

25 

21 

.20 

14 

•77 

33 

.11 

23 

.06 

3 

.85      2.92 

f  NiNa2(SO4)2.4H2O  H- 

30 

22 

.60 

12 

.80 

34 

.98 

19 

.82 

4 

.07      2.59 

NiSO4.7H2O 

35 

23 

.62 

10 

.78 

36 

.01 

16 

•43 

4 

.19      2.08 

40 

24 

.92 

9 

•39 

37 

•93 

14 

.29 

4 

.41      1.81   - 

18.5 

16 

.80 

18 

•93 

26 

.14 

29 

•45 

3 

.04      3-72   " 

20 

15 

.48 

20 

.18 

24 

.06 

31 

•37 

2 

.80      3.97 

25 

10 

.92 

24 

.12 

16 

.81 

37 

•13 

I 

.96      4.70 

a 

30 

6.40 

28 

•71 

9 

.87 

I 

.15      5.60  - 

35 

4 

•54 

3i 

•65 

7 

•13 

49 

•59 

O 

.838    6.28 

NiNa2(S04)2.4H20  + 

40 

4 

•63 

3i 

•37 

7 

.24 

49 

•03 

o 

.843     6.21 

j      Na2S04 

455  NICKEL  SULFATE 

SOLUBILITY  OF  NICKEL  POTASSIUM  SULFATE  NiK2(SO4)2.6H2O  IN  WATER. 

(Tobler,  1855;  v.  Hauer,  1858.) 

Cms.  NiK2(SO4)2  per  100  Gms.  H2O.  o          Cms.  NiK^SOQa  Per  100  Cms.  H2O. 

(Tobler.)  (v.  Hauer.)  (Tobler.)  (v.  Hauer.) 

o  5.3  ...  50  30 

10         .     8.9  ...  60  35.4  20.47 

20  13.8  9.53  70  42 

30  18.6  ...  80  46  28.2 

40  24  14.03 

SOLUBILITY  OF  NICKEL  SULFATE  IN  AQUEOUS  SOLUTIONS  OF  METHYL 
ALCOHOL  AT  14°. 

(de  Bruyn,  1903.) 

Small  test  tubes  of  4-6  cc.  capacity'were  used.  They  were  almost  completely 
filled  with  the  salt  and  solvent  and  placed  in  the  bath  in  an  inclined  position 
with  salt  occupying  the  upper  part  of  the  tube.  This  caused  a  "spontaneous 
circulation  of  the  solvent."  The  solutions  were  analyzed  by  precipitating  NiO 
with  KOH  at  the  boiling  point,  in  porcelain  vessels. 


Wt.  Per  cent 

VJII 

is.  rNio»~»4  per  100  vjiii 

s.  oai.  oui.  111  \_uuuitt  \ 

mtun 

CH3OH 
in  Solvent. 

NiSO4.7H2O  as 
Solid  Phase. 

NiSO4.6H2O  a  as 
Solid  Phase. 

NiSO4.6H2O  /3  as 
Solid  Phase. 

NiSO4.4H2O  as 
Solid  Phase. 

o  (H20) 

26.4 

26  (low) 

27.2 

25.1 

10 

19.7 

22(?) 

20-4 

20 

14.7 

14 

14.8 

30 

6^8 

6.6 

7-5 

.  .  . 

40 

2.8 

2.4 

3.1 

50 

1.3 

i 

1.4 

1.4 

60 

0.8 

0.4 

0.6 

70 

0.6 

0.2 

0.4 

80 

0.65 

0.2 

0.4 

0.66 

85 

*-5 

°-3 

0.7 

90 

5-7 

1.2 

2-5 

95 

ii 

6 

9  (?) 

.  .  . 

100 

16.8 

12.4  (low) 

15.7  (low) 

7-38 

NiSO4.6H2O  a  is  greenish  blue.     NiSO4.6H2O    is  more  greenish  than  the  a  salt. 
SOLUBILITY  OF  NiSO4.3CH3OH.3H2O  IN 'AQUEOUS  CH8OH  AT  14°. 

(de  Bruyn,  1903-) 


Wt.  Per  cent 
CH3OH. 

Gms.  NiSO4  per 
100  Gms.  Sat.  Sol. 

Wt.  Per  cent 
CH3OH. 

Gms.  NiSO4  per 
100  Gms.  Sat.  Sol. 

85 

I  .93 

90 

0.70 

86 

I  .73 

92-5 

0.50 

87 

1.48 

95 

0-455 

88 

1-25 

97-5 

0-77 

89 

1.  01 

100 

3-72 

Approximately  two  hours  were  allowed  for  attainment  of  equilibrium. 

In  solutions  containing  more  than  15%  H2O  the  salt  is  gradually  transformed 
toNiSO4.6H2O0. 

100  gms.  absolute  ethyl  alcohol  dissolve  1.4  gm.  NiSO4-7H2O  at  4°  and  2.2 
gms.  at  17°.  (de  Bruyn,  1892.) 

100  gms.  sat.  solution  in  glycol  contain  9.7  gms.  NiSO4  at  room  temp. 

(de  Coninck,  1905.) 
NICKEL  SULFIDE   NiS. 

One  liter  H2O  dissolves  39.9  X  lO"6  gm.  mols.  NiS  =  0.0036  gm.  at  18°,  by 

conductivity  method.  (Weigel,  1906.) 

Fusion-point  data  for  Ni2S-fNa2S  and  Ni3S2+Na2S  are  given  by  Friedrich  (1914). 


NICOTINE 
NICOTINE  Ci0Hi4N2. 


456 
SOLUBILITY  IN  WATER. 

(Hudson,  1904.) 


Determinations  made  by  Synthetic  Method,  for  which  see  Note,  page  16. 
Below  60°  and  above  210°  both  liquids  are  miscible  in  all  proportions;  likewise 
with  percentages  of  nicotine  less  than  6.8  and  above  82  per  cent  the  liquid  does 
not  show  two  layers  at  any  temperature.  Below  94°  the  upper  layer  is  water. 
Above  94°  the  upper  layer  is  nicotine.  The  curve  plotted  from  the  following 
results  makes  a  complete  circle. 


Percentage  of 

Nicotine 
in  the  Mixture. 

6.8 

7.8 
10.0 
14.8 
32.2 
49.0 
66.8 
80.2 
82.0 


Temperature  of 
Appearance  of 


Temperature  of 


94 
89 

75 


64 
72 

87 
129 


95 
155 

200 
210 
205 
190 
170 
I30 


Additional  data  for  the  above  system  are  given  by  Tsakalotos  (1909).  The 
values  for  the  temperatures  of  saturation  are  in  general,  from  i°  to  5°  lower  than 
those  of  Hudson. 

NIOBIUM   Potassium  FLUORIDE   NbK2F7. 

SOLUBILITY  IN  WATER  AND  IN  AQUEOUS  HF  AND  AQUEOUS  KF  SOLUTIONS. 

(Ruff  and  Schiller,  1911.) 

'  The  determinations  were  made  in  platinum  vessels.  The  mixtures  were 
shaken  for  3  hour  periods  at  constant  temperature  and  the  saturated  solutions 
filtered  through  platinum  funnels. 

Gms.  per  100  Cms.  Sat.  Solution. 


NbF6. 

KF. 

HF. 

ooiiu  .ruase. 

Water 

16 

5-IQ 

2.98 

o-35 

K2NbOF6.H2O 

a 

16 

7.07 

5-33 

4-35 

K2NbOF5.H2O+K2NbF7 

Aq.  10.95%  HF 

16 

4-33 

2.32 

10.43 

K2NbF7 

"      7-4i%KF 

16 

1.16 

5-54 

0.13 

K2NbOF5.H2O 

"      7-39%  EF 

16 

2.67 

6.04 

5-39 

K2NbOFs.H2O+K2NbF7 

Water 

85 

30-39 

14.68 

0-35 

K2NbOFs.H20(?) 

Aq.  4.8i%KF 

80 

11.66 

10.  08 

i-53 

" 

NITRIC  ACID  HNO3. 

DISTRIBUTION  OF  NITRIC  ACID  BETWEEN  WATER  AND  ETHER  AT  25°., 

(Bogdan,  1905,  1906.) 
Mols.  HNO3  per  Liter  of:  Mols.  HNO,  per  Liter  of: 


H2O  Layer. 
0.9145 
0.4811 

o . 2644 

0.1392 


Ether  Layer. 
0.0855 
0.0278 

o . 00894 

O.OO278 


H2O  Layer. 
0.09005 
0.04749 
0.02760 
0.02462 


Ether  Layer. 
O.OOlSl 
0.00064 
0.00029 
0.00025 


457 


NITRIC   ACID 


RECIPROCAL  SOLUBILITY  OF  NITRIC  ACID  AND  WATER,  DETERMINED  BY  THE 
FREEZING-POINT  METHOD. 

(Kiister  and  Kremann,  1904;  see  also  Pickering,  1893.) 


Gms.  HN03 
t°.                     per^ioopms.       Solid  Phase.            t°. 

Gms.  HNO3 
per  100  Gms.        Solid  Phase. 

bat.  bol. 

Sat.  Sol. 

—  10 

13.9    Ice 

-40 

69.7 

HNO3.3H2O 

—  20 

22.9      " 

—42  Eutec. 

70.5 

"  +HN03.H20 

-30 

27.8      « 

-40 

72.5 

HNO3.H2O 

-40 

3I-5    " 

-38m.pt. 

77-75 

" 

—43  Eutec. 

32.7     "+HN03.3H20 

-40 

82.4 

" 

-40 

34  .  1          HN03.3H20 

-50 

86.5 

" 

-30 

40 

-60 

88.8 

« 

—  20 

49.2 

—  66.3  Eutec. 

89-95 

"  +HN03 

—  18  .  5  m.  pt. 

53-8 

-60 

91.9 

HNO, 

—  20 

58.5 

-5o 

94-8 

" 

-30 

65-4 

—4i.2m.pt. 

100 

• 

NITROGEN  Na. 


SOLUBILITY  IN  WATER. 


(Winkler  —  Ber.  24,  3606,  '91;  Braun  —  Z.  physik.  Chem.  33,  732,  'oo;  Bohr  and  Bock  —  Wied.  Ann, 

44,  318,  '91.) 


t° 

L/oemcien 

t  01  ADsorptic 

A, 

in     p. 

"  Solubility  "  B'. 

?• 

0 

0.0235* 

...t 

0.0233* 

O.OO239* 

5 

0.0208 

0.0215 

0.0217 

O.O2O6 

O.OO259 

10 

0.0186 

0-0196 

O.O2OO 

0.0183 

0.00230 

15 

0.0168 

0.0179 

0.0179 

0-0165 

0.00208 

20 

0.0154 

0-0164 

O.Ol62 

O.OI5I 

0.00189 

25 

0.0143 

O.OI5O 

0.0143 

0.0139 

0.00174 

30 

0.0134 

0-0138 

.  .  . 

O.OI28 

o.  00161 

35 

0-0125 

0.0127 

.  .  . 

O.OIlS 

0.00148 

40 

0.0118 

O-OIlS 

O-OIIO 

0.00139 

50 

0.0109 

0.0106 

.  .  . 

0.0096 

0-OOI2I 

60 

0.0102 

O-OIOO 

.  .  . 

0.0082 

O.OOIO5 

80 

0.0096 

0.0051 

0.00069 

100 

0.0095 

o.oioo 

o.oooo 

o.ooooo 

*w. 

t  B.  and  B. 

tB. 

For  values  of  ft,  ft',  and  q,  see  Ethane,  p.  285. 

Single  determinations  of  the  solubility  of  nitrogen  in  water  reported  by  Hiifner 
(1906-07),  Bohr  (1910),  Muller  (1912-13)  and  von  Hammel  (1915),  are,  on 
the  average,  about  2-3  units  in  the  fourth  place  higher  than  the  above  figures 
of  Winkler  for  the  absorption  coefficient  ft.  Drucker  and  Moles  (1910),  give  an 
extensive  review  of  the  literature  and  present  results  which,  they  state,  are  in  very 
satisfactory  agreement  with  previous  determinations.  A  critical  review  of  the 
literature  of  the  solubility  of  nitrogen  in  water  and  in  sea  water  is  given  by 
Coste  (1917). 

Data  for  the  solubility  of  the  nitrogen  of  air  in  water  are  given  by  Fox  (iQOQa). 
The  oxygen  was  removed  from  air  and  the  solubility  of  the  residual  N  +  1.185% 
argon  was  determined.  After  making  correction  for  the  argon,  the  following 
formula  for  the  solubility  of  pure  nitrogen  in  water  was  deduced : 

1000  X  coef.  of  abs.  ft  =  22.998  —  0.5298 1  -f  0.009196  £  —  0.00006779  **• 

Data  for  the  solubility  of  nitrogen  in  water  at  pressures  up  to  10  atmospheres 
are  given  by  Cassuto  (1913).  The  solubility  was  found  to  increase  at  a  some- 
what slower  rate  than  proportional  to  the  pressure. 


NITROGEN  458 

SOLUBILITY  OF  NITROGEN  IN  SEA  WATER. 

(Fox,  igoga). 

Before  using  the  sample  of  sea  water  for  the  solubility  determinations  it  was 
found  necessary  to  add  acid,  otherwise  the  CO2  could  not  be  boiled  out  or  the 
precipitation  of  neutral  carbonates  prevented.  The  very  small  amount  of  acid 
was  titrated  back,  using  phenolphthaleine  as  indicator. 

The  results  are  in  terms  of  number  of  cc.  of  nitrogen  (containing  argon)  ab- 
sorbed by  1000  cc.  of  sea  water  from  a  free  dry  atmosphere  of  760  mm.  pressure. 

The  calculated  formula  expressing  the  solubility  is: 

1000  a  =  18.639  —  04304 1  +  o-o°7453  **  —  0.0000549  & 
—  Q  (0.2172  —  0.007187  /  -f  0.0000952 12). 


imorine         t°-n°           A° 

r  looo. 

8°. 

12 

°. 

16°. 

20°. 

24°. 

28°. 

O 

18 

-64 

17.02 

15.63 

14. 

45 

13-45 

12, 

•59 

11.86 

11.25 

4 

17 

•74 

16.27 

14.98 

88 

12.94 

12 

15 

11.46 

10.89 

8 

16 

.90 

15-51 

I4.32 

13. 

30 

12.44 

II 

,70 

11.07 

10.52 

12 

16 

•03 

14-75 

13-66 

12. 

72 

H-93 

II 

•25 

10.67 

10.  16 

16 

15 

.18 

14 

13 

12. 

15 

n-73 

10, 

,81 

10.27 

9.80 

20 

14 

.31 

13.27 

12.34 

II. 

57 

10.92 

10, 

36 

9.87 

9-44 

A  recalculation  of  Fox's  determinations  to  parts  per  million,  with  correction 
for  vapor  pressure,  is  published  by  Whipple  and  Whipple  (1911). 

SOLUBILITY  OF  NITROGEN  IN  AQUEOUS  SOLUTIONS  OF  SULFURIC  ACID 

Results  at  21°.     (Bohr,  1910.)  Results  at  20°.  (Christoff,  1006.) 

Normality  of  Absorption  Coef .  Normality  of  Absorp.  Coef.  Per  cent        Ostwald  Solubility 

Aq.  H2SO4.         0  (Bunsen).         Aq.  H2SO4.      0  (Bunsen).  H2SO4.  Expression  1M. 

o      0.0156     24.8    0.0048        o       0.01537 

4.9      O.009I       29.6     O.O05I  35-82      0.008447 

8.9    0.0072     34.3    o.oioo       61.62    0.006144 
10.7    0.0066     35-8*   0.0129       95-6     0.01672 
20.3    0.0049 

*  =  about  96%. 

For  definitions  of  Absorption  Coef.  (Bunsen)  and  Solubility  Expression  (Ost- 
wald), see  p.  227. 

SOLUBILITY  OF  NITROGEN  IN  AQUEOUS  SALT  SOLUTIONS. 

(Braun.) 
Coefficient  of  Absorption  of  N  in  Barium  Chloride  Solutions  of: 


i  . 

13.83  Per  cent 

11.92  Per  cent. 

6.90  Per  cent. 

3.87  Per  cent.        3.33  Per  cent. 

5 

O.OI27 

0.0137 

0.0160 

O.OlSo 

0.0183 

10 

O.OII7 

0.0125 

0.0147 

0.0166 

0.0168 

15 

O.OI04 

O.OII4 

0.0132 

0.0148 

0.0150 

20 

0.0092 

0.0098 

0.0118 

0.0132 

0.0135 

25 

0.0078 

0.0086 

0.0104 

O.OII4 

0.0119 

Coefficient  of  Absorption  of  N  in  Sodium  Chloride  Solutions  of: 

' 

11.73  Per  cent. 

8.14  Per  cent. 

6.4  Per  cent. 

2.12  Per  cent.        0.67  Per  cent. 

5 

O.OIO2 

O.OI27 

0.0138 

O.OI79 

0.0200 

10 

0.0093 

O.OII3 

O.OI26 

0.0164 

0.0185 

15 

O.OOSl 

O.OIOI 

O.OII3 

O.OI47 

0.0l64 

20 

0.0066 

0.0087 

0.0098 

O.OI3I 

O.OI48 

25 

O.OO47 

0.0075 

0.0083 

O.OII3 

0.0130 

SOLUBILITY  OF  NITROGEN  IN  ALCOHOL. 

(Bunsen.) 

t°.  o°.  5°.          10°.          15°.         20°.         24°. 

Vols.  N  *  dissolved 
by  i  Vol.  Alcohol.         0.1263    0.1244    0.1228    0.1214    0.1204    0.1198 

*  At  o°  and  760  mm. 


459 


NITROGEN 


SOLUBILITY  OF  NITROGEN  IN  MIXTURES  OF  ETHYL  ALCOHOL  AND  WATER 

AT  25°. 

(Just,  1901.) 

Results  in  terms  of  the  Ostwald  solubility  expression,  see  p.  227. 

Dissolved 

Nfe). 

0.01634 
0.01536 


Vol.  %  H2O  in 
Mixture. 

Vol.  %  Alcohol'in 
Mixture. 

100 

0 

80 

20 

67 

33 

0 

100  (99-8% 

SOLUBILITY  OF  NITROGEN  IN  SEVERAL  SOLVENTS  AT  20°  AND  25°. 

(Just.) 


Solvent.  ^25. 

Water  0.01634 

Aniline  o .  03074 

Carbon  Disulfide  0.05860 

Nitro  Benzene 

Benzene 

Acetic  Acid 

Xylene 

Amyl  Alcohol        0.1225 


0.06255 
0.1159 
o. 1190 
o.  1217 


0.01705 
0.02992 
0.05290 
0.06082 

o. 1114 
o.  1172 
o. 1185 
0.1208 


Solvent.                        /25- 

Toluene                    0.1235 
Chloroform                0.1348 
Methyl  Alcohol         o.  1415 
Ethyl  Alcohol  (99-8%)  o.  1432 
Acetone                     0.1460 
Amyl  Acetate            0.1542 
Ethyl  Acetate           0.1727 
Isobutyl  Acetate       o.  1734 

*20. 
O.II86 
0.1282 
0.1348 
O.I40O 
0.1383 

o.  1512 

0.1678 
0.1701 

SOLUBILITY  OF  NITROGEN  IN  PETROLEUM.     COEFFICIENT  OF  ABSORPTION  AT 
10°  =  0.135,  AT  20°  =  0.117. 

(Gniewasz  and  Walfisz,  1887.) 


SOLUBILITY  OF  NITROGEN  IN  AQUEOUS  PROPIONIC  ACID  AND  UREA 

SOLUTIONS. 

(Braun.) 
Coefficient  of  Absorption  of  N  in  C2H5COOH  Solutions  of: 


I/  . 

11.22  per  cent. 

9.54  per  cent. 

6.07  per  cent. 

4.08  per  cent. 

3.82  per  cent. 

5 

10 

i5 

20 

0.0195 
0.0178 
'0.0159 
0.0146 

0.0204 
0.0182 
0.0l63 
0.0147 

0.0208 

0.0186 
0.0164 
0.0148 

O.O2IO 
0.0192 
0.0169 
0.0154 

O.O2O9 
O.OI9I 
O.Ol67 
0.0155 

25 

0.0130 

0.0134 

0.0134 

0.0137 

0.0137 

Coefficient  of  Absorption  of  N  in  CO(NHs),  Solutions  of: 


15-65 

per  cent. 

11.9  per  cent. 

9.42 

per  cent. 

6.90  per  cent. 

5.15  per  cent. 

2.28  per  cent. 

5 

10 

i5 

20 

0. 
O. 
0. 
0. 

0175 
Ol62 
0150 
OI4O 

o 

0 
O 
O 

.0179 
.0167 
.0149 
.0139 

O, 

o 
o 
o 

OI9O 
,0176 
0158 
,0146 

0 
O 
0 
0 

.0198 
.0183 
.0165 
.0151 

0 
O 
0 
0 

.0197 
.0182 
•0165 
.0151 

0.0199 
0.0l84 
O.OI7I 
0.0155 

25 

o. 

0130 

0 

.0130 

o 

0133 

O 

.0137 

0 

•0135 

0.0139 

NITROGEN 


460 


SOLUBILITY  OF  NITROGEN  IN  AQUEOUS  SOLUTIONS  OF  CHLORAL  HYDRATE  AT  15°. 


Results  by  Miiller,  C  (1912-13.) 

Gms. 


Results  by  von  Hammel  (1915). 
Gms. 


CC1S.CH(OH), 

</2o  of  Aq. 

Absorp.  Coef. 

CC13CH(OH)2 

Abs.  Coef. 

Solubility  L* 

per  ioo  Gms. 

•      Sol. 

/Sat  15°. 

per  ioo  Gms. 

0  at  15°. 

(Ostwald). 

Aq.  Sol. 

Aq.  Sol. 

0 

I 

0.0170 

0 

0.0170 

0.01796 

15-8 

1.0738 

0.0158 

15 

0.0152 

0.0160 

28.2 

I.I422 

0.01422 

26.1 

O.OI4I 

0.0149 

37-25 

I  .  1946 

O.OI3OO 

37-6 

0.0123 

O.OI3O 

47 

1-2535 

0.01275 

48.9 

O.OII5 

O.OI2I 

56.52 

1.3225 

O.OI245 

61.3 

O.OII4 

O.OI2O 

71.5 

I.44I 

0.01420 

70.9 

0.0131 

0.0138 

78.8 

1.503 

0.01492 

79.1 

0.0156 

0.0165 

SOLUBILITY  OF  NITROGEN  IN  AQUEOUS  SOLUTIONS  OF  GLYCEROL. 
Results  of  Miiller,  C.        Results  of  von  Hammel       Results  of  Drucker 
(1912-13).  (1915).  and  Moles  (1910). 

Gms.  Gms.  Gms. 


IOO  ( 

Aq. 

Sol.' 

1 

1   ' 

ioo  Gms. 
Aq.  Sol. 

p 

1  5  ' 

Aq-  sSS' 

25 

.061 

0 

.01266 

15-7 

o 

01400 

0 

0 

0.0156 

42 

2 

.108 

0 

.00976 

29.9 

o 

01087 

16 

I. 

0392 

0.0103 

51 

5 

•133 

0 

.00759 

46.6 

0 

00840 

29.7 

I. 

0744 

0.0067 

58 

.151 

0 

.00703 

57-6 

o 

00698 

48.9 

I. 

1263 

0.0052 

80 

25 

.212 

0 

.00530 

67.1 

0 

00635 

74-5 

I  . 

1931 

0.0025 

90 

.240 

o 

.00583 

77 

0 

00527 

84.1 

I. 

2213 

0.0024 

95 

.249 

0 

.00716 

88.5 

0 

00536 

99-25 

0 

00524 

Solubility  of  Nz  in  pure  isobutyric  acid  of  fa  =  0.9481,  IM  (Ost«vaH)  =  0.1651. 

(Drucker  and  Moles,  1910.) 

Solubility  of  N2  in  aq.  37.5%  isobutyric  acid  of  fa  —  0.9985,  4s  (Ostwald) 
=  0.0396.  (Drucker  and  Moles,  1910.) 

Solubility  of  N2  in  aq.  37.5%  isobutyric  acid  of  fa  =  0.9985,  ^  (Ostwald) 

=  0.0384,  (Drucker  and  Moles,  1910.) 

SOLUBILITY  OF  NITROGEN  IN  AQUEOUS  SOLUTIONS  OF  SEVERAL  COMPOUNDS. 

(Huiner,  1906-07.) 

Cone,  of  Aq.  Solution. 

t°.  Abs.  Coef.  0. 


Aq.  solution  01: 

Normality. 

Gms.  per  Liter. 

Glucose 

I 

180 

" 

0-5 

90 

" 

O.25 

45 

Alanine        («  Aminopropionic  Acid) 

I 

89 

GlyCOCol      (Aminoacetic  Acid) 

I 

75 

Aribinose 

I 

150 

Levulose 

I 

180 

Erythritol 

I 

122 

Urea 

I 

60 

Acetamide 

I 

59 

20.18 

2O.  21 
20.2 

0.01215 
0.01380 
0.01480 

2O.I9 

20.  16 

0.01213 

O.OI2I2 

2O.  21 

O.OI203 

2O.25 

O.OI22I 

20.25 
20.  l8 

O.OI32I 
0.01477 

20.22 

0.01475 

SOLUBILITY  OF  NITROGEN  IN  AQUEOUS  SOLUTIONS  OF  CANE  SUGAR  AT  15°. 

(Miiller,  C.,  1912-13.) 


per  ioo  Urns. 
Aq.  Solution. 

11.38 
2O 


Abs.  Coef. 
at  15°. 


Gms. 

per  ioo  Gms. 
Aq.  Solution. 


Aq.  Sol. 
I.I29 


Abs.  Coef.  0 
at  15°. 


Aq.  Sol. 

1.050  0.61480  30.12  I.I29  O.OIO90 

1.082  O.OI280  47.89  1.220  0.00785 

29.93  I.I28  O.OI053  48.57  1.223  0.00700 

Data  for  the  solubility  of  nitrogen  in  defibrinated  ox-blood  and  ox  serum  under 
pressures  varying  760-1400  mm.  Hg  are  given  by  Findlay  and  Creighton  (1910-11). 
Data  for  the  solubility  of  nitrogen  in  liquid  oxygen  are  given  by  Erdman  and 
Bedford  (1904)  and  Stock  (1904.) 


46l 


NITROGEN 


SOLUBILITY  OF  NITROGEN  IN  METHYL  ALCOHOL  SOLUTIONS  OF  POTASSIUM 
IODIDE  AND  OF  UREA. 

(Levi,  1901.) 

Solubility  of  N  (in  terms  of  the  Ostwald  Solubility  Expression  /)• 


Solvent. 

Cms.  KI  or  of  Urea 


At  s°. 


At  15°. 


At  25°. 


is  of  Solvent.         /».        du  of  Solvent.       /u. 


O  %(=pureCH£)H) 

2.152   KI 

3-053     " 
10.939     " 
2.738  Urea 
4.841      " 

7-377     " 


a*  of  Solvent.        J*. 
0.7937      0.1649 
0.8019     0.1524 
O.SlOI 
0.8801 
0.7997 
0.8o8o 
0.8350     0.1878     0.8241      O.l6oo     0.8193 


O.8o8o      0.2154     0.7980     0.1923 

0.8171  0.2028  0.8070  0.1802 

0.1756 

0.1464 
0.2030 

0.1951 


0.8249  0.1966 
0.8930  0.1676 

0.8148 
0.8231 


0.8015 

0.8841 
0.8050  0.1823 

O.8I22   O.I75O 


0.1466 
0.1258 
O.I56l 
O.I49I 
0.1444 


SOLUBILITY  OF  NITROGEN  IN  ETHYL  ETHER. 

(Christoff,  1912.) 

Results  in  terms  of  the  Ostwald  expression  /  (see  p.  227),  IQ  =  0.2580,  /w  =  0.2561. 


WTTROGEN  OXIDE  (ic) 

NO. 
SOLUBILITY  IN  WATER. 

(Winkler,  1901.) 

t°. 

0- 

v. 

?• 

t°. 

ft. 

p. 

g- 

0 

0.0738 

0 

•0734 

O 

.00984 

40 

0.0351 

o 

•0325 

o 

.00440 

5 

0.0646 

0 

.0641 

0 

.00860 

50 

0.0315 

o 

.0277 

o 

•00376 

10 

0.0571 

o 

.0564 

o 

•00757 

60 

0.0295 

o 

.0237 

c 

-00324 

15 

0.0515 

o 

.0506 

0 

.00680 

70 

0.0281 

o 

•0195 

o 

.00267 

20 

0.0471 

o 

.0460 

o 

.00618 

80 

0.0270 

o 

.0144 

.0 

.00199 

25 

0.0430 

o 

.0419 

0 

.00564 

00 

0.0265 

o 

.0082 

o 

.00114 

30 

0.0400 

ro 

.0384 

o 

•00517 

100 

0.0263 

o 

.0000 

6 

.00000 

For  values  of  /3,  £'  and  q,  see  Ethane,  page  285. 

SOLUBILITY  OF  NITRIC  OXIDE  IN  AQUEOUS  SULPHURIC  Aero  SOLUTIONS 

AT  18°. 

(Lunge,  1885;  Tower,  1906.) 


(0.035, 


Wt.  per  cent  H*SO4 
in  Solution. 

Sp.Gr. 
at  15°. 

98                     ] 

.84 

00                     ] 

.82 

80                     ] 

•733 

70                   .  ] 

.616 

60                     1 

•503 

50                   '] 

•399 

Tension  of          Solubility  Coefficient 
HjO  Vapor.                 of  NO  at  iS°. 

0.0227 

O.I  mm. 

0.4  ;; 

0.0193 

0.0117 

n 

0.0113 
0.0118 

6.2      " 

O.OI2O 

(0.017,  L.) 


*  Volume  of  NO  (at  760  mm.)  per  i  volume  of  aqueous  HjSO4. 

SOLUBILITY  OF  NITRIC  OXIDE  IN  ALCOHOL. 

(Bunsen.) 


0° 
0.316 


5° 

0.300 


10" 

0.286 


15° 

0.275 


20° 
0.266 


24° 
0.261 


Vols.  NO* 

absorbed  by  i  vol.  Ale. 

*  At  o°  and  760  mm. 

Data  for  the  solubility  of  nitric  oxide  in  aqueous  solutions  of  FeSO4,  NiSO4r 
CoSO4  and  MnCl2  at  20°  are  given  by  Usher  (1908);  Hufner  (1907)  and  Man- 
chot  and  Zecheulmayer  (1906). 

The  abs.  coef.  0  for  N  in  sat.  aq.  NiSO4  at  20°  is  0.0245;  for  sat.  CoSO4  it  is 
0.0288  and  for  sat.  aq.  MnClj  it  is  0.0082. 


NITROGEN   OXIDE  462 

NITROUS   OXIDE   N2O. 

SOLUBILITY  IN  WATER. 

(Bunsen;  Roth,  1897;  Knopp,  1904;  Geffcken,  1904.) 
Coefficient  of  Absorption  ft 

t     *  A 


(B.) 

(R.) 

«. 

(R.) 

(K.) 

(G.) 

5 

1.0954 

I  .  1403 

0.205 

1.161 

.  .  . 

-    1.067 

10 

0.9196 

0-9479 

0.171 

0.9815 

.  .  . 

0.9101 

15 

0.7778 

0.7896 

0.143 

0-8315 

0.7784 

20 

0.6700 

0.6654 

O.I2I 

0.7131 

0.6739 

0.6756 

2^ 

0.5961 

0.5752 

O.IO4 

0.6281 

0.5942 

*  Calculated  by  Geffcken. 
For  definitions  of  /8  and  g,  see  p.  285;  for  /,  see  p.  227. 

NOTE.  —  Knopp  and  also  Geffcken  call  attention  to  the  fact  that 
Roth  in  making  his  determinations  used  a  rubber  tube  between  the 
gas  burette  and  the  shaking  flask,  and  give  this  as  an  explanation  of 
the  high  results  which  he  obtained. 

SOLUBILITY  OP  NITROUS  OXIDE  IN  AQUEOUS  SULPHURIC  ACID. 

(Lunge  —  Ber.  14,  2188,  '81;  see  also  Geffcken 's  results.) 

Sp.  Gr.  of  H2SO4  1.84          i. 80          1.705          1.45          1.25 

Vols.  N2O  dissolved 
by  loo  vols.  H2SO4         75.7          66.0          39.1  41-6          33.0 

100  vols.  of  KOH  solution  of  1.12  Sp.  Gr.  absorb  18.7  vols.  N2O. 
100  vols.  of  NaOH  solution  of  i.io  Sp.  Gr.  absorb  23.1  vols.  N2O. 


SOLUBILITY  OF  NITROUS  OXIDE  IN  AQUEOUS  SOLUTIONS  OF  ACIDS. 

(Geffcken.) 

Results  in  terms  of  the  Ostwald  Solubility  Expression  (/).    See  p.  227. 
In  Hydrochloric  Acid.       In  Nitric  Acid.         In  Sulphuric  Acid. 

Cms.  HCl       N2O  Dissolved     Qms.  HNO3    N2O  Dissolved       Gms.  H2SO4    N2O  Dissolved 
per  Liter.        /16.  /^         per  Liter.         /15.     *      fa.  per  Liter.        ;18.  J^ 

18.22    0.755    o-577      36.52    °-777    0.597      24.52  0.734  0.566 

36.45    0.738    0.568      63.05    0.777    0.602      49.04  0.699  °-543 

72.90    0.716    0.557    126.10    0.775    0.611      98.08  0.645  0.509 

147.12  0.602  0.482 

196.16  0.562  0.463 

SOLUBILITY  OF  NITROUS  OXIDE  IN  AQUEOUS  SOLUTIONS  OF: 

(Roth.) 

Phosphoric  Acid.  Oxalic  Acid. 


*• 

s 

10 

^5 

20 
2$ 

Coefficient  of  Abs. 

in  H3PO4  Solutions  of: 

Coefficient  of  Abs.  in 
(COOH)2  Solutions  of; 

'  0.812%.          3-70%. 
I.I450      I.I094 
0.9526      0.9264 
0.7940      0-7745 
0.6694      0.6538 
0.5784      0.5643 

3-38%. 

^OST 
0.8827 
0.7388 
0.6253 
0.5427 

i 

0 
0 
0 
0 

4.72%. 

•0365 
.8665 

•7258 
.6147 

•5329 

0 
0 
0 
0 
0 

8.84%. 
.9883 
.8296 
.6977 
.5926 

•5I43 

9-89%. 

0-9635 
0.8101 
0.6826 
0.5810 
0-5054 

0 

o 
o 

0 
0 

13.35%. 

.9171 

.7711 
•6505 

•5555 
.4860 

463 


NITROUS   OXIDE 


SOLUBILITY  OP  NITROUS  OXIDE  IN  AQUEOUS  SOLUTIONS  OP  PROPIONIC 

ACID  AT  20°. 

(Knopp.) 


Cms.  C2H5COOH 
per  liter  *5-*5        60.42 

Coef.  of  Absorp- 
tion of  N2O  0.6323      0.6369 


158.4          176.6          344.0 
0.6504        0.6534        0.7219 


SOLUBILITY  OF  NITROUS  OXIDE  IN  AQUEOUS  SALT  SOLUTIONS. 


Results  by  Geffcken 
page  227. 

Salt. 

Ammonium  Chloride 
Ammonium  Chloride 
Caesium  Chloride 
Lithium  Chloride 
Lithium  Chloride 
Potassium  Bromide 
Potassium  Bromide 
Potassium  Chloride 
Potassium  Chloride 
Potassium  Iodide 
Potassium  Iodide 
Potassium  Hydroxide 
Potassium  Hydroxide 
Rubidium  Chloride 
Rubidium  Chloride 


in  terms  of  the  Ostwald  expression  (/).      See 


Cone,  of  Salt  per  Liter. 

Solubility  of  N20. 

ormu  a. 

Gram  Equiv. 

Grams. 

/is- 

fe 

NH4C1 

o-5 

26.76 

0.730 

o-557 

NH4C1 

I  .0 

53-52 

0.691 

0.529 

CsCl 

o-5 

84.17 

0.710 

0-544 

LiCl 

o-5 

21.24 

0.697 

o-535 

LiCl 

I  .0 

42.48 

0.623 

0.483 

KBr 

o-5 

59-55 

0.697 

o-536 

KBr 

I.O 

119.11 

0.627 

0.485 

KC1 

o-5 

37-3 

0.686 

0.527 

KC1 

i  .0 

74-6 

0.616 

o-475 

KI 

o-5 

83.06 

0.702 

0.541 

KI 

I.O 

166.12 

0-633 

0.492 

KOH 

o-5 

28.08 

0.668 

0.514 

KOH 

I  .0 

56.16 

o-559 

0.436 

RbCl 

o-5 

60.47 

0.695 

o-533 

RbCl 

I  .0 

120.95 

0.625 

0.483 

Results  by  Knopp,  in  terms  of  the  coefficient  of  absorption.     See 


page  227 

Salt.  Formula. 

Potassium  Nitrate     KNO3 


Sodium  Nitrate         NaNO3 


Cone,  of  Salt 

per  Liter. 

Coef.  of  Absorption 

Normality. 

Grams. 

of  N2O  at  20°. 

0.1061 

10.74 

0.6173 

0.2764 

27.94 

0.60O2 

0.5630 

56-97 

0-57*3 

1.1683 

118.2 

0.5196 

0.1336 

n-37 

o  .  6089 

0.3052 

25-97 

0.5876 

0.6286 

53-5o 

0-5465 

I  .1200 

95-30 

0.4926 

Results  by  Roth,  in  terms  of  the  coefficient  of  absorption. 


Grams  NaCl  per 
100  Grams 
Solution. 

O.Q9 
1.  808 
3.886 
5-865 

Coefficient  of  Absorption  of  N2O  at: 

<?. 
1.0609 
1.0032 
0.9131 
0.8428 

10°. 

0.8812 
0.8383 
0.7699 
0.7090 

15°. 

0-7339 
0.7026 

0.6495 
0.5976 

90°. 
O.OIQI 

0.5962 
0.5520 
0.5088 

fi£?. 

O.S363 
0.5190 

0-4775 
0.4424 

NITROUS   OXIDE 


464 


SOLUBILITY  OF  NITROUS  OXIDE  IN  AQUEOUS  SALT  SOLUTIONS. 
Results  by  Gordon  in  terms  of  coefficient  of  absorption.    See  p.  227. 


Concentration  of  Salt. 


Coefficient  of  Absorption 


Grams  per         Gram 
100  Grams        Mols. 
Solution.       per  Liter. 

5-79        0.547 

o 

5°. 

.819 

10°. 

0.697 

0 

15°. 

•591 

0 

20°- 

•500 

9 

.86 

0 

.964 

o 

.668 

0.586 

0 

•509 

0 

•435 

13 

•99 

i 

.416 

o 

.510 

0 

.441 

0 

.380 

0 

.328 

i 

•35 

0 

•319 

o 

.986 

0 

.831 

0 

.700 

0 

•594 

3 

•85 

0.928 

0 

.878 

0 

•743 

0.629     0.536 

ii 

.48 

2 

.883 

o 

,606 

0 

.512 

0 

•437 

0 

•382 

2 

•37 

O 

.219 

o 

934 

0 

.792 

0 

.670 

0 

•569 

5 

.46 

O 

.521 

o 

795 

o 

.665 

0 

•557 

0 

•474 

8 

•56 

O 

.836 

0 

.646 

o-555 

0 

•477 

o 

•4i5 

5 

.90 

0.521 

o 

.766 

o 

.664 

0 

.561 

o 

.471 

7 

.66 

O 

.687 

o 

.708 

0 

.586 

0 

.488 

0 

.414 

10 

•78 

O 

•997 

o 

•569 

0 

.491 

o 

.417 

0.346 

4 

.90 

0 

.676 

0 

.879 

0 

•751 

0.643 

o 

•555 

7 

.64 

I 

•037 

o 

•799 

0 

•693 

o 

591     0.494 

14 

•58 

2 

.147 

o 

•654 

0 

•574 

0 

•500 

0 

•430 

22 

.08 

3 

.414 

o 

•544 

o 

•459 

0 

•390 

o 

•339 

2 

.62 

o 

•154 

o 

.986 

0.831 

0 

.701 

0 

.605 

4 

.78 

0.285 

o 

.918 

0 

•763 

0 

•637 

0 

•542 

6 

.20 

I 

.107 

o 

.800 

x> 

.682 

0 

•585 

0 

•509 

8 

.88 

I 

.614 

o 

.713 

0 

.603 

0 

0 

•434 

12 

•78 

2 

•391 

0 

•634 

0 

•532 

0 

•449 

0.386 

5 

.76 

O 

•427 

o 

.808 

0.677 

0 

•584 

0 

•495 

8 

•53 

O 

.646 

o 

.692 

o 

•574 

0 

.482 

0 

.416 

12 

•44 

O 

•974 

o 

•559 

0 

.486 

0 

•417 

o 

•354 

3 

.31 

O 

•215 

o 

.928 

0 

.788 

0 

.671 

0 

•578 

5 

•73 

o 

-380 

0 

.848 

0 

.709 

0 

.610 

o 

13 

.24 

o 

•939 

o 

.644 

0 

•547 

0 

•463 

0 

•39° 

Salt. 

Calcium  Chloride 

u 

Lithium  Chloride 

a 
Lithium  Sulphate 

Magnesium  Sulphate 

ii 

Potassium  Chloride 

tt 

n 
(i 

Potassium  Sulphate 

Sodium  Chloride 

tt 

Sodium  Sulphate 


Strontium  Chloride 
a 


SOLUBILITY  OP  NITROUS  OXIDE  IN  ALCOHOL  AND  IN  AQUEOUS  CHLORAL 
HYDRATE  SOLUTIONS  AT  2cr. 

(Bunsen;  Knopp  —  Z.  physik.  Ch.  48,  106,  '04.) 


In  Alcohol  (B.). 


In  Aq.  Chloral  Hydrate  (K.). 


Vols.  N20 
t  °.       (at  o°  and  760  mm.) 
per  i  Vol.  Alcohol. 

Normality 
C2HCl3O.H2O. 

Cms. 
C2HC13O.H20 
per  Liter. 

Coef.  of 
Abs.  of  NjO. 

0 

4.178 

0.184 

30-43 

0.618 

5 

3-844 

0-445 

73.60 

0-613 

10 

3-541 

0.942 

155-8 

0.596 

IS 

3.268 

I  .165 

192.7 

0.589 

20 

3-025 

1-474 

243-8 

o-579 

24 

2.853 

i  .911 

316.4 

0.567 

SOLUBILITY  OP  NITROUS  OXIDE  IN  PETROLEUM. 
ABSORPTION  AT  10°  =  2.49,  AT  20° 


COEFFICIENT  OF 
=  2. ii. 


(Gniewasz  and  Walfisz  — Z.  physik.  Ch.  i,  70,  '87.) 


465  NITROUS   OXIDE 

SOLUBILITY  OF  NITROUS  OXIDE  IN  AQUEOUS  SOLUTIONS  OF  GLYCEROL  AND  OF  UREA. 

(Roth,  1897.) 
Coefficient  of  Absorption  of  N2O  in  Glycerol  Solutions  of: 


3.46  Per  cent. 

6.73  Per  cent.      12. 

12  Per  cent. 

16.24  Per  cent. 

5 

i 

.097 

i 

•055 

O 

•999 

0 

•959 

10 

0 

.917 

0 

.887 

0 

.841 

O 

.810 

*5 

0 

.767 

0 

•745 

0 

.710 

o 

.686 

20 

0 

.647 

0 

.630 

0 

.605 

0 

•58S 

25 

0 

•556 

o 

•542 

0 

•527 

o 

•508 

Coefficient  of  Absorption  of  N2O  in 

Urea  Solutions  of: 

3.31  per  cent. 

4.97  per  cent. 

6.37  per  cent. 

7.30  per  cent. 

9.97  per  cent. 

I 

.104 

I  . 

096 

i.  088 

I  .IOI 

1.069 

0 

.921 

o. 

92O 

0.909 

0.921 

o. 

901 

0 

.771 

o. 

773 

0.761 

0.772 

o. 

76l 

o 

•653 

o. 

6S6 

0.644 

0-655 

o. 

65* 

0 

•569 

o. 

567 

0-559 

0.570 

o. 

5<*> 

5 
10 

15 

20 
25 

SOLUBILITY  OF  NITROUS  OXIDE  IN  AQUEOUS  SOLUTIONS  OF  GLYCEROL. 

(Henkel,  1905,  1912.) 

Results  at  15°.  Results  at  20°. 

Per  cent  Glycerol.      Absorption  Coef.  a.  Per  cent  Glycerol.      Absorption  Coef.  a. 

o  0.7327  o  0.6288 

2.49  0.7181  2.36  0.6131 

3.28  o\7io3  4.88  0.5993 

7.17  0.6844  6.88  0.5903 

10.52  0.6668  9.86  0-5633 

14.05  0.6410  15.82  °-53I5 

17.08  0.6229 

Data  for  the  influence  of  colloids  and  fine  suspensions  on  the  solubility  of  ni- 
trous oxide  in  water  at  25°  are  given  by  Findlay  and  Creighton  (1910),  and  Find- 
lay  and  Howell  (1914). 

Results  for  solutions  of  ferric  hydroxide,  dextrin,  arsenious  sulfide,  starch, 
gelatin,  glycogen,  egg  albumen,  serum  albumen,  silicic  acid  and  suspensions  of 
charcoal  and  of  silica  are  given. 

Data  for  the  solubility  of  nitrous  oxide  in  blood  are  given  by  Siebeck  (1909) 
and  by  Findlay  and  Creightonf  (1910-11).  • 

NITROGEN   TETROXIDE   NO2. 

Data  for  the  solubility  of  nitrogen  tetroxide  in  ferrous  bromide  solutions  are 
given  by  Thomas  (1896). 

Freezing-point  data  (solubility,  see  footnote,  p.  i),  are  given  for  mixtures 
of  NO2  +  NO  by  v.  Wittorff  (1904),  and  for  mixtures  of  NO2  +  o  Nitrotoluene 
by  Breithaupt. 

NITROCELLULOSE    (Soluble  Pyroxylin,  Tetra  and  Penta  Nitrate). 
SOLUBILITY  IN  ETHER-ALCOHOL  MIXTURES. 

(Matteoschat,  1914;  see  also  Stepanow,  1907.) 

A  sample  of  gun  cotton  containing  12.95%  N  was  used.  The  compound  was 
first  covered  with  alcohol  and  then  the  amount  of  ether  to  yield  the  desired  com- 
position of  solvent  was  added.  Lower  results  were  obtained  with  ready  prepared 
ether-alcohol  mixtures. 

Ratio  of  Gms.  Gun  Cotton  Dissolved  per  100  Cms.  Solution  in  Mixtures  Prepared  with: 


r  :  Alcohol. 

99-5  Vol.  %  Alcohol. 

95  Vol.  %  Alcohol. 

90  Vol.  %  Alcohol. 

80  Vol.  %  Alcohol. 

i  :  2 

34-4 

i  :  i 

52-3 

42-3 

28.7 

14.2 

2  :  i 

40.5 

52-4 

53-9 

45 

3:1 

25 

42.4 

53 

57-5 

NOVOCAINE  466 

NOVOCAINE   (base)   CH2(C6H4NH2COO)CH2[N.(C2H6)2].2H2O. 

100  cc.  H2O  dissolve  0.333  gm-  anhydrous  novocaine  at  20°.  (Zalai,  1910.) 

100  cc.  oil  of  sesame  dissolve  4.29  gms.  anhydrous  novocaine  at  20°. 

NOVOCAINE    (Hydrochloride)   CH2(C6H4NH2COO).CH2[N(C2H6)2].HC1. 
loo  gms.  H2O  dissolve  about  100  gms.  of  the  salt  at  room  temp. 
100  gms.  alcohol  dissolve  about  3  gms.  of  the  salt  at  room  temp. 

OCTANE  CH3(CH2)6CH3. 

RECIPROCAL  SOLUBILITY  OF  OCTANE  AND  PHENOL. 

(Campetti  and  Del  Grosso,  1913.) 

AC  Gms.  Phenol  per  ^  0  Gms.  Phenol  per 

loo  Gms.  Mixture.  100  Gms.  Mixture. 

22.55  13.28  49.501!.  t.  52.2 

37.85  22.74  49.35  52.37 

38-15  23-S3  44.7  7i-i4 

44.70  32.85  30.65  82.01 

47-75  41-72  19-65  85.99 

OLEIC  ACID   C8Hi7CH:CH(CH2)7COOH. 

SOLUBILITY  OF  OLEIC  ACID  IN  AQUEOUS  ALCOHOL  SOLUTIONS  AT  25°. 

(Seidell,  1910.) 

Oleic  acid  of  d<&  =  0.8935  and  containing  99.5%  acid,  determined  by  titration, 
was  used.  It  was  found  that  the  addition  of  as  little  as  one  drop  of  this  acid 
to  aq.  alcohol  solutions  containing  up  to  50  wt.  %  C2H6OH  caused  an  opalescence 
on  shaking,  therefore,  indicating  a  solubility  of  less  than  about  0.05  gm.  acid  per 
100  cc.  water  or  of  aq.  alcohol.  With  solutions  containing  more  than  50  wt.  % 
C2H6OH  the  following  results  were  obtained: 

Wf  Pot- ,  cc-  Oleic  Acid  per 

r  w  nw  I0° cc-  Aq.  Alcohol  to  Remarks. 

CjHjUH.  produce  cloudiness. 

51  O  .  08  —  0 .  2  Cloudiness  gradually  increased. 

58.2  0.2    —0.4 

65  -5  '           O  .  3    —  0 .  6  Cloudiness  disappeared  when  about  5.5  cc.  acid  had  been  added. 

70.2  O.6    —  I                     "                   "              "         "      4-5  cc.     "       "       " 

81.4  CO  No  cloudiness  appeared  at  all. 

It  was  found  that  although  the  end  points  obtained  by  addition  of  oleic  acid 
to  aq.  alcohol  mixtures  are  not  sharp,  they  become  so  when  the  procedure  is 
changed  to  addition  of  H2O*to  mixtures  of  oleic  acid  and  alcohol.  By  this  method 
perfectly  clear  liquid  may  be  transformed  by  one  drop  of  the  H2O  to  an  opa- 
lescent mixture  which,  after  standing  a  few  minutes,  separates  into  two  liquid 
layers.  Determinations  made  in  this  way  gave  the  following  observed  and  cal- 
culated quantities. 

Gms.  of  Constituents  to  Yield  Results  Calculated  from  the 

Opalescent  Mixtures.  Plotted  Curve. 

Alcohol  +  Oleic  Acid  Mixture.        H2O  Added  Wt.  Per  cent    cc.  Oleic  Acid  Gms.  Oleic  Acid 

to  Cause  Qh^OH  in         per  100  cc.        per  100  Gms. 


CjH6OH.  Oleic  Acid.          Separation.  Aq.  Alcohol.      Aq.  Alcohol.  Sat.  Sol. 

15.30     1-794.    10.4       57       •••  o 
15-30     3-588    10.2       58.5      o      5 

15.30     4.485     9.8       60      n  12.3 

I5-3°     7-175     9-25      62.5     30  20 

15.30     n. 210     8.05       65      49  3°-5 

24.42     22.420    10.10       67.5     69  40 

15.30     20.810     6.50       70      91  50 

1.195     8.969     0.321      75.5     ...  68.5 

80       ...  88 

Alter  standing  24  hours  the  opalescent  mixtures  separated  into  layers  which 
on  analysis,  gave  the  results  shown  in  the  following  table: 


467  OLEIC  ACID 

COMPOSITION  OF  UPPER  AND  LOWER  LAYERS  OBTAINED  BY  THE  ADDITION  OF 
WATER  TO  MIXTURES  OF  AQUEOUS  ALCOHOL  AND  OLEIC  ACID  AT  25°.  (Con. 
from  p.  466). 

Composition  of  Original  Mixture.  After  Separation  into  Two  Layers: 


rwt.  %  * 

cc.  Aq. 

cc. 

cc.  H2O                  Lower  Layer. 

Upper  Layer. 

in  Aq. 
Ale.  Used. 

Alcohol 
Mixture. 

Oleic 
Acid. 

to  Cause  /  * 
Separa-     cc.  Total 
tion.           Vol. 

Sp.  Gr. 

cc.  Oleic 
Acid. 

cc.  Total 
Vol. 

Sp.  Gr. 

cc.  Oleic 
Acid. 

70.2 

25 

2 

3-9° 

29 

0.893 

1.48 

I 

0-35 

70.2 

25 

4 

3-70 

26 

0.890 

1.89 

6 

0.875 

1.98 

65.5 

26.5 

5 

1-75 

22.7 

0.891 

i-93 

9-3 

0.875 

2.78 

70.2 

25 

8 

2-75 

16 

0.893 

0.98 

19 

0.876 

6-59 

70.2 

25 

12.5 

1-55 

6 

0.890 

0.37 

33-2 

0.878 

11.87 

70.2 

35 

.  25 

i 

4-5 

.     1             1 

0.28 

55-5 

0.877 

f 

24.14 

50  cc.  Aq.  Alcohol 

50  cc.  Benzine  Layer. 

Dist.  Coef. 

Layer. 

Layer. 

0.277 

0.723 

2.6l 

O.II2 

0.888 

7-93 

0.025 

o-97S 

39 

O.OO6 

0.994 

166 

0.002 

0.998 

499 

The  C2H5pH  in  the  two  layers  could  not  be  determined  on  account  of  excessive 
foaming  during  distillation   of  the  neutralized  solution.     Some  losses  occurred 
in  transferring  the  original  mixtures  to  the  graduated  cylinders  and  differences 
between  final  amounts  and  those  originally  present  are  due  to  these  losses. 
SOLUBILITY  OF  OLEIC  ACID  IN  AQUEOUS  SOLUTIONS  OF  BILE  SALTS. 

(Moore,  Wilson  and  Hutchinson,  1909.) 

<""-.  ^iS'tr100 

Water  less  than  o .  i 

5%  Aq.  Solution  of  Bile  Salts  about    o.  5 

5%  Aq.  Solution  of  Bile  Salts-f-i  %  Lecithin  .  4 

DISTRIBUTION  OF  OLEIC  ACID  BETWEEN  AQUEOUS  ALCOHOL  AND  BENZINE.  (Holde.'io.) 

Strength  of  Aq.  Gm.  (Approx.)  of  Oleic  Acid  in; 

Alcohol  in  Vol. 
Per  cent. 

84.1 
76.9 
63.7 
50.5 
42.4 

SOLIDIFICATION-POINTS  OF  MIXTURES  OF  OLEIC  AND  STEARIC  ACIDS.  (Meldrum,  '13.) 

Solidification 
Temp. 

O 
IO 
20 
30 
4O 

Additional  data  for  the  above  system  as  well  as  for  mixtures  of  oleic  and 
palmitic  acids  and  for  the  ternary  system  oleic,  palmitic  and  stearic  acids  are 
given  by  Carlinfante  and  Levi-Malvano  (1909).  Results  for  Oleic  Acid  +  Stearic 
acid  are  also  given  by  Fokin  (1912). 

TriOLEIN   (C18H33O2)3C3H5. 

SOLIDIFICATION- POINTS  OF  MIXTURES  OF  TRIOLEIN  AND  OTHER  FATS. 

(Kremann  and  Schoulz,  1912.) 

Triolein  +  Tripalmitin.        Triolein  +  Tristearin.       Tripalmitin  +  Tristearin. 
t°.  Wt.  Per  cent  f0  Wt.  Per  cent.  f <,  Wt.  Per  cent 

Triolein.  Triolein.  .  Tristearin. 

—  7      loo      +28       95.2       60.4      90 
+25       93-9       44       85.3       58       75 

48.2    78.5     50.7    76.7     57.8  .   69.4 

50       73.9       56       68.8       56       60.2 
56.9      53        64-3      47-2       57.2      53 
60.9      27.2       64.3      25.4       55.1      43-8 
62.6       o        56        o        54.5      31.2 

60 . 4  8.4 

Data  for  the  ternary  system,  triolein.  tripalmitin  and  tristearin  are  also  given. 


Per  cent  Oleic  Aci'd 

Solidification 

Per  cent  Oleic  Acid 

in  Mixture. 

Temp. 

in  Mixture. 

54-8 

50 

44-7 

53-3 

60 

41.2 

51-6 

70 

36.6 

49-7 

80 

30-5 

47.6 

OILS 


468 


OILS.     (See  also  Fats,  p.  302.) 

SOLUBILITY  OF  SEVERAL  OILS  IN  ALCOHOL  (di5  =  0.795)  AT  I4~I50- 

(Davidsohn  and  Wrage,  1915.) 
f)-i  Gms.  Oil  per  100  Gms. 

Sat  Sol. 

Linseed  Oil  3.32 

Rape  Oil  i .  36 

Cotton  Seed  Oil  3.61 

Olive  Oil  2.25 

Results  are  also  given  for  the  solubility  of  mixtures  of  oils  and  fatty  acids  in 
alcohol.  The  following  results  at  22°,  in  terms  of  approx.  volume  of  oil  dissolved 
by  100  volumes  of  80%  alcohol,  are  given  by  Aubert  (1902).  Nigella  oil,  4.3; 
oil  of  boldo  leaves,  more  than  100;  matico  oil,  about  20;  cascarilla  oil,  5;  weld- 
mint  oil,  66. 

^  Miscibility  curves  for  various  oils  with  acetone,  petroleum  and  aniline  are 
given  by  Louise  (1911).  The  use  of  this  data  for  the  identification  of  oils  and 
the  detection  of  adulterants  in  them  is  described. 

An  extensive  series  of  observations  on  the  solubility  of  water  in  oils  and  on  the 
water  content  of  various  oils  is  given  by  Umney  and  Bunker  (1912). 

Freezing-point  data  for  oil  of  helianthus  annus  +  stearic  acid  are  given  by 
Fokin  (1912). 

OSMIC   ACID  OsO4,  100  gms.  H2O  dissolve  5.88  gms.  Osmic  Acid  at  about  15°. 

(Squire  and  Caines,  1905.) 

OXALIC  ACID   H2C204.2H20. 

SOLUBILITY  IN  WATER. 

(Koppel  and  Cahn,  1908;  for  older* data  see  Alluard,  Miczynski,  1886;  Lamouroux,  1899.) 


—  0.064 

0.1805 

—  0.152 

0.452 

-  0.533 

I.  -820 

-  0.936 

3.291 

-  i.5o 

5.836 

-  o.9S 

3.302 

o 

3.416 

+  10 

-  5.731 

Ice  20  8.69  HjQC^HjO 

30  12.46 

40  17.71 

50  23.93 

60  30. 71 

70  37.92 

80  45 . 80 

90.2  54.67  " 

H2C2O4.2H2O  melts  in  its  H2O  of  crystallization  at  98°. 

SOLUBILITY  OF  OXALIC  ACID  IN  AQUEOUS  HC1.AND  IN  AQUEOUS  HNO3  AT  30°. 

(Masson,  1.912.) 


In  Aq.  Hydrochloric  Acid. 

In  Aq.  Nitric  Acid. 

G.  Mols. 

G.  Mols. 

Gms. 

G.  Mols. 

G.  Mols. 

Gms. 

HC1           <*™Sat. 

(COOH)2 

(COOH)2 

HNO3         < 

fag  Sat. 

(COOH)2 

(COOH)2 

per  liter            Sol 

per  liter 

per  liter 

per  liter 

Sol. 

per  liter 

per  liter 

Sat.  Sol. 

Sat.  Sol. 

Sat.  Sol. 

Sat.  Sol. 

Sat.  Sol. 

Sat.  Sol. 

0 

-0594 

1.479 

I33-I 

0.478      1.0648 

1.268 

114.  1 

0.503 

•  0561 

I.I90 

107.1 

I.  606      1.0932 

1.039 

93.48 

0.970 

•0577 

1.032 

92.85 

4.224 

.1666 

0.790 

71.09 

1-939 

.0654 

0.821 

73-88 

9-590 

•3074 

0.639 

57-50 

2-959 

•0757 

0.675 

60.74 

13.62 

•3938 

0.847 

76.23 

4-528 

•0957 

0-555 

49-95 

14.12 

.4060 

0.966 

86.94 

6.026 

.1165 

0.525 

47-25 

15-59 

•43J9 

1  .  114 

IOO.  2 

7.907 

.1494 

0.607 

54.63 

16.92 

•4443 

0.840 

75-6 

9.680 

.  1843 

0.871 

78.38 

20.84 

.4819 

0.524 

47-iS 

21.63       L49I7 

0-553 

49.76 

SOLUBILITY  OF  OXALIC  ACID 

IN  AQUEOUS 

SOLUTIONS  OF  H2SO4  AT  25°. 

(Wirth,  '08.) 

ACQ0nHS°o    ^°'fSat- 

Gms.  per  100  Gms.  Sat.  Sol. 

Cone,  of     3 

An     TT  ^O      *** 

B  of  Sat     Gms'  per  I0°  Gms'  Sat'  Sol- 

No*rrnSuy4.          So1' 

S03. 

(COOH)2. 

Aq.  Xlgov^ 

Normality. 

5  Sol. 

S03. 

(COOH)2. 

o              1.047 

O 

10.23 

4.85 

I-I57 

14 

3-92 

I                   I  .  064 

2.98 

8.03 

5.67 

I.I77 

16.44 

3-51 

2  .  39         i  .  140 

7.30 

6.02 

6-45 

1.220 

17.84 

3.12 

4.36         1.146 

12.57 

4.26 

8.9 

1.280 

25.92 

2-37 

469  OXALIC  ACID 


SOLUBILITY  OF  OXALIC  ACID  IN  SEVERAL  ALCOHOLS. 

(Timofeiew,  1894.) 

Gms.  (COOH),                                                                Gms.  (COOH), 
Alcohol.                     t°.          per  zoo  Gms.                   Alcohol.                         t°.          per  100  Gms. 
Sat.  Sol.                                                                              Sat.  Sol. 

Methyl  Alcohol 

—  1.5 

34-2 

Propyl  Alcohol          —  1.5 

12.2 

«            « 

+  20.2 

39-8 

+  18.5 

16.7 

Ethyl  Alcohol 

-  i-5 

22.4 

20.2 

«           a 

+  I8.5 

26.2 

Isobutyl  Alcohol           20  .  2 

10.9 

u              tt 

20.2 

26.9 

SOLUBILITY  OF  OXALIC  ACID  IN  ABSOLUTE  AND  IN  AQUEOUS  ETHER  AT  25°. 

(Bodtker,  1897;  Bourgoin.) 

100  gms.  absolute  ether  dissolve  1.47  gms.  (COOH)2.2H2O. 
100  gms.  absolute  ether  dissolve  23.59  gms.  (COOH)2. 

In  Aqueous  Ether  Solutions. 
Gms.  Solid  Acid  Added  per  100  cc.  Ether  Solution.  Gms.  per  100  cc.  Ether  Solution. 

(COOH)2.2H2O.  (COOH)2.  HA  (COOH)2/ 

(1)  5  o  1.250  0.742 

(2)  5  o  0.788  0.720 
5  o  0.418  1.044 
5  2.44  0.360  3.388 
5  4.82  0.484  6.038 
5  7-i4  0.558  8.538 
5  9.42  0.632  10.996 
5  11-63  0.676  13-316 
5  13-79  0.760  15.684 
5  18.18  0.816  17.818 
5  22.73  0.816  17.818 

(i)  Ether  saturated  with  water.  (2)  Ether  containing  0.694  Per  cent  water. 

100  gms.  glycerol  dissolve  15  gms.  oxalic  acid  at  15.5°.  (Ossendowski,  1907.) 

loo  gms.  95%  formic  acid  dissolve  9.74  gms.  anhydrous  oxalic  acid  at  16.8°. 

(Aschan,  1913.) 

DISTRIBUTION  OF  OXALIC  ACID  BETWEEN  WATER  AND  AMYL  ALCOHOL  AT  20°. 

(Herz  and  Fischer,  1904.) 
Millimols  \  (COOH)2  per  10  cc.  Gms.  (COOH)2  per  100  cc. 

Aq.  Layer.  Alcoholic  Layer.  Aq.  Layer.  Alcoholic  Layer. 

O.68o6                     0.1451  0.306                       0.0653 

2.364                       0.7233  1.064                       0.326 

6.699                        2.550  3.015                        1.148 

10.029  4-300  4-5H  1-934 

Data  for  the  distribution  of  oxalic  acid  between  mixtures  of  amyl  alcohol  + 
ether  and  water  at  25°  are  given  by  Herz  and  Kurzer  (1910). 

DISTRIBUTION  OF  OXALIC  ACID  BETWEEN  WATER  AND  ETHER. 

(Pinnow,  1915.) 

Results  at  15°.  Results  at  27°. 

Gm.  Mols.  (COOH)2  per  Liter.          Dist.  Coef.  of:      Gm.  Mols.  (COOH)2  per  Liter.       Dist.  Coef.  of; 


Water 

Ether 

Total 

Undissoc. 

Water 

Ether 

Total 

Undissoc. 

Layer. 

Layer. 

Acid. 

Acid. 

Layer. 

Layer. 

Acid. 

Acid. 

0-3435 

O.O2945 

II 

.6 

8. 

49 

O, 

,760 

0.0637 

II 

9 

8.18 

0.1885 

0.01395 

13 

•5 

8. 

81 

0, 

56l 

0.0433 

13 

8-37 

O.I24 

0.00845 

14 

.8 

8. 

69 

O 

3575 

0.025O 

14 

3 

8.26 

0.0892 

0.00553 

16 

.1 

8. 

72 

O 

2550 

0.0165 

15 

5 

8.12 

o  .  0470 

0.00248 

19 

8. 

19 

0. 

1754 

0.01025 

17 

i 

7.94 

0.0435 

O.OO22 

19 

.8 

8. 

26 

Data  for  the  effect  of  H2SO4  upon  the  above  distribution  are  also  given. 
Data  similar  to  the  above  for  a  greater  range  of  cone,  at  25°  are  given  by 
Chandler  (1908). 


OXYGEN 


470 


OXYGEN  02. 

SOLUBILITY  IN  WATER. 

*«.     Coef.  of  Absorption  /9.  g. 


(Winkler,  1891;  Bohr  and  Bock,  1891.) 


0 

0.0489* 

0.0496! 

5 

0.0429 

0.0439 

IO 

0.0380 

0.0390 

15 

0.0342 

0.0350 

20 

0.0310 

0.0317 

25 

0.0283 

0.0290 

30 

o.  0261 

0.0268 

0.00695 

0.00607 

0.00537 

0.00480 

0.00434 
0.00393 
0.00359 

*w. 
For  values  of  /3  and  q  see  Ethane,  p.  285. 


cc.  0  per 
Liter  H2O. 
10.187 
8.907 

7.873 
7.038 

6.356 
5.776 
5-255 

t°. 
40 

50 
60 

70 
80 
90 
IOO 

Coef.  of  Absorption  /5.               ?. 

O. 
0. 
O. 
0. 
0. 
0. 
0. 

0231* 
0209 

0195 
0183 
0176 
OI72 
OI7O 

0.0233! 
o.  0207 
0.0189 
0.0178 
0.0172 
0.0169 
0.0168 

0. 

o. 

0. 

o. 

0. 
0. 
0. 

00308 
00266 
00227 
00186 
00138 
00079 

ooooo 

t  B.  and  B. 


According  to  determinations  by  Fox  (igoga),  which  agree  satisfactorily  with  the  above,  the  solubility 
of  oxygen  in  water  is  expressed  by  the  formula: 

1000  X  abs.  coef.  ft  =  49-239  —  i-344°  <  +  0.28752  ft  —  0.0003024  fl. 
References  to  more  recent  papers  on  the  solubility  of  oxygen  are  given  by  Coste  (1917,  1918). 


SOLUBILITY  OF  THE  OXYGEN  OF  AIR  IN  WATER. 

t°.  5-2°.  5-65°.  14-78°. 

Solubility*  8.856  8.744  7.08 

*  cc.  Oxygen  per  1000  cc.  H2O  saturated  with  air  at  760  mm. 


24-8°. 
5.762 


SOLUBILITY  OF  OXYGEN  IN  WATER  AND  IN  AQUEOUS  SOLUTIONS  OF  ACIDS, 

BASES  AND  SALTS.      (Geffcken,  1904.) 


Concentration  per  Liter. 


Solubility  of  Oxygen.* 


Water  alone 
Hydrochloric  Acid 


Nitric  Acid 


Sulphuric  Acid 


Potassium  Hydroxide 
Sodium  Hydroxide 

Potassium  Sulphate 
Sodium  Chloride 


Gram  Equiv, 

,    Grams. 

o-5 

18.22 

I-O 

36-45 

2.0 

72.90 

o-5 

36.52 

i.o 

63-05 

2.O 

I26.IO 

o-5 

24.52 

I.O 

49.04 

2.0 

98.08 

3-o 

I47-I2 

4.0 

196.16 

5-o 

245  .  20 

o-5 

28.08 

I.O 

56.16 

o-5 

20.03 

I.O 

40.06 

2.0 

80.  12 

o-5 

43-59 

I.O 

87.18 

o-5 

29.25 

I.O 

58.5 

2.0 

119.0 

In  terms  of  the  Ostwald  Solubility  Expression. 


0.0363 
0.0344 
0.0327 

0.0299 
0.0348 
0.0336 
0.0315 
0.0338 
0.0319 
0-0335 

0.0256 
0.0233 
0.0213 

0.0291 

0.0234 
0.0288 
0.0231 
0.0152 
0.0294 

0.0237 
0.0308 
.0.0260 
0.0182 

See  page  227. 


0-0308 
0-0296 
0.0287 
0-0267 
0.0302 
0.0295 
0-0284 
0.0288 
0.0275 
0.0251 
0.0229 

o . 0209 

O.OI94 
O.O252 
O.O2O6 
0.0250 
0-0204 
0.0133 
0.0253 
O.O2O7 
O.O262 
0.0223 
0.0158 


SOLUBILITY  OF  OXYGEN  IN  AQUEOUS  POTASSIUM  CYANIDE  SOLUTIONS  AT  20°. 

(Maclaurin,  1893.) 


Cms.  KCN  per  ioo  gms.  sol.       i  10  20 

Coefficient  of  absorption  j3      0.029      0.018      0.013 


30 
0.008 


5<> 
0.003 


471 


OXYGEN 


SOLUBILITY  OF  OXYGEN  IN  SEA  WATER. 

(Fox,  igoga.) 

Before  using  the  sample  of  sea  water  for  the  solubility  determinations,  it  was 
found  necessary  to  add  acid,  otherwise  the  COZ  could  not  be  boiled  out  or  the 
precipitation  of  neutral  carbonates  prevented.  The  very  small  amount  of  acid 
was  titrated  back,  using  phenolphthaleine  as  indicator. 

Results  in  terms  of  cc.  of  oxygen  absorbed  by  1000  cc.  of  sea  water  from  a 
free  dry  atmosphere  at  760  mm.  pressure. 

The  calculated  formula  expressing  the  solubility  is:  1000  a  =  10.291  —  0.2809  t 
-f-  0.006009  P  +  0.0000632  P  —  Cl  (0.1161  —  0.003922  /  +  0.0000631  £). 


Parts  Chlorine 
per  1000. 

t°  = 

o°. 

4°- 

8°. 

12°. 

16°. 

20°. 

24°. 

28°. 

O 

IO. 

29 

9 

.26 

8.40 

7.68 

7.08 

6-57 

6. 

14 

5-75 

4 

9- 

83 

8 

•85 

8.04 

7.36 

6.80 

6-33 

5- 

9i 

5-53 

8 

9- 

36 

8 

•45 

7.68 

7.04 

6.52 

6.07 

5- 

67 

5-3i 

12 

8. 

90 

8 

.04 

7-33 

6.74 

6.24 

5-82 

5- 

44 

5-08 

16 

8. 

43 

7 

.64 

6.97 

6-43 

5-90 

5-56 

5- 

20 

4.86 

20 

7- 

97 

7 

•23 

6.62 

6.  ii 

5-69 

5-31 

4- 

95 

4.62 

A  recalculation  of  Fox's  determinations  to  parts  per  million,  with  correction 
for  vapor  pressure,  is  published  by  Whipple  and  Whipple  (1911). 

Additional  data  on  the  solubility  of  atmospheric  oxygen  in  sea  water  are 
given  by  Clowes  and  Biggs  (1904). 

Data  for  the  solubility  of  oxygen  in  water  under  pressures  up  to  10  atmos- 
pheres are  given  by  Cassuto  (1913).  The  solubility  increases  at  a  somewhat 
slower  rate  than  proportional  to  the  pressure. 


SOLUBILITY  OF  OXYGEN  IN  AQUEOUS  SALT  SOLUTIONS  AT  25°. 

(MacArthur,  1916.) 


Aq.  Salt 
Solution. 

da  Aq. 
Solu- 
tion. 

cc.  oxy- 
gen per 
Liter. 

Aq.  Salt 
Solution. 

dK  Aq.  cc.  Oxy- 
Solu-    gen  per 
tion.      Liter. 

Aq.  Salt 
Solution. 

du  ot     cc.  Oxy- 
Solu-     gen  per 
tion.       Liter. 

Dist.  H20 

I 

5-78 

0.25 

ttKBr 

1.019 

5-29 

O.I25«  NaBr 

1.007 

5-65 

O.I25»  I1 

JH4C1 

I.OOI5 

2.31 

2 

n    " 

1.079 

3.27 

0.25 

n    ' 

1.017 

5-52 

0.25  n 

" 

1.0025 

1.16 

4 

n    " 

1.162 

1.84 

0.50 

n    " 

1.036 

5-15 

i        n 

" 

1.014 

0.07 

O.I25WKC1 

1.003 

5-52 

I 

n     " 

1.075 

4-47 

O.I25«  BaCl2 

1.019 

540 

0.25 

n    " 

1.  0086 

5-30 

2 

n     " 

1.150 

3-37 

0.25  n 

" 

1.042 

5-04 

0.50 

n    " 

I.O2O 

4.98' 

3 

n    " 

1.219 

2-57 

0.50  n 

" 

1.082 

4.27 

I 

n    " 

I.O42 

4.26 

4 

n    " 

I'3°5 

2.O2 

i        n 

" 

I.I77 

3.10 

2 

n    " 

1.086 

3.21 

6 

n     " 

1-455 

1.28 

0.25  nCaCl, 

1.022 

S-o8 

3 

n   " 

I.I34 

2.36 

O.l25«NaCl 

I.OO22 

5.52 

i        n 

" 

1.084 

3-71 

4 

n   " 

I.I70 

1.86 

0.25 

n    " 

1.0067 

5-30 

5        n 

" 

1.34 

2.14 

O.I25«KI 

I.OI3 

5.65 

0.50 

n    " 

I.OI7 

4.92 

0.l25«CsCl 

I.OI4 

5.67 

0.25 

n   ' 

I.O27 

549 

I 

n    " 

1.038 

4.20 

o.i25«LiCl 

I.OOO4 

5.63 

0.50 

n   ' 

1.056 

5-20 

2 

n    " 

1.075 

3.05 

0.50  n 

" 

I.OO9I 

I 

n   ' 

1.116 

4-75 

3 

n    " 

1.  112 

2.24 

i        n 

" 

I.  O2  1 

4-59 

2 

n   ' 

1.23 

3-77 

4 

n    " 

I.I49 

1.62 

2        n 

« 

1.044 

3-63 

5 

n    ' 

1.46 

1.81 

O.I25W  Na2SO4 

I.OI4 

5.04 

3        w 

« 

I.II3 

1.97 

0.25 

MKNO, 

1.015 

5-49 

0.25 

n     " 

1.032 

4.60 

4        w 

" 

1.220 

1.  12 

0.50 

n     " 

1.029 

S-ii 

0.50 

n      " 

1.063 

3-97 

o.i25wMgCl, 

1.  01  1 

5.35 

I- 

n     " 

1.059 

4.61 

I 

n     " 

I.I30 

3 

0.50  w 

« 

1.044 

4.37 

2 

n     " 

i.  no 

3.65 

0.  1  25«  Sucrose 

I.OI5 

540 

i        n 

i 

1.085 

o.i25«  K2.SO4 

1.016 

0.25 

n      " 

1.033 

4.82 

2           « 

i 

1.160 

2.22 

0.25 

n     " 

1.032  . 

4*.66 

0.50 

n     " 

i  -6-i 

1-39 

4        n 

• 

1.284 

0.78 

0.5 

n 

i.  060 

3.89 

I 

n     " 

1.147 

3-20 

5        ** 

' 

1.343 

0-54 

o.i25»RbCl 

1.0094 

5.65 

2 

n     " 

1.336 

1.84 

OXYGEN  472 

SOLUBILITY  OF  OXYGEN  IN  AQUEOUS  SULFURIC  ACID  SOLUTIONS. 
Results  at  21°.     (Bohr,  1910.)  Results  at  29°.  (Christoff,  1906). 


Normality  of 
H2S04. 

Absorp. 
Coef  .  ft. 

Normality  of 
H2SO<. 

Absorp. 
Coef.0. 

Wt.  %        Ostwald  Solubility 
H2SO4.            Expression  /jo- 

0 

0.0310 

24.8 

O.OI03 

0 

0.03756 

4.9 

0.0195 

29.6 

O.OII7 

35-82 

0.0l8l5 

8.9 

0-0155 

34-3 

0.0201 

61.62 

0.01407 

10-7 

0.0143 

35.  8  (=96%) 

0.0275 

95.60 

0.03303 

20.3 

O.OII9 

SOLUBILITY  OF  OXYGEN  IN  ETHYL  ALCOHOL,  METHYL  ALCOHOL  AND 

IN  ACETONE. 

(Timofejew  —  Z.  physik.  Ch.  6,  151,  'oo;  Levi  —  Gazz.  chim.  ital.  3it  II,  513,  'ox.) 


O 

5 
10 

15 

20 

25 
30 
40 

SO 

For  values  of  ft  and  /3',  see  Ethane,  p.  285.  /  =  Ostwald  Solubility  Expres- 
sion. See  p.  227. 

The  formulae  expressing  the  solubility  of  oxygen  in  methyl  alcohol  and  in  ace- 
tone as  shown  in  the  above  table  are  as  follows: 

In  Methyl  Alcohol    /  =  0.31864  —  0.002572  /  —  0.00002866  ^. 
In  Acetone  /  =  0.2997    —  0.00318  /     —  0.000012  P. 

The  formula  expressing  the  absorption  coefficient  of  oxygen  in  ethyl  alcohol 
is  0  =  0.23370  —  0.00074688  t  +  0.000003288  P. 

SOLUBILITY  OF  OXYGEN  IN  AQUEOUS  ALCOHOL  AT  20°  AND  760  MM. 

(Lubarsch, 


i  Ethyl  Alcohol  of  90.7%  (T.). 

In  Methyl 
Alcohol  (L.) 

In  Acetone  (L.) 

0. 

£'• 

0.2337 

0.2297 

0.31864 

0.2997 

0.2301 

0.2247 

0-30506 

0.2835 

O.2266 

0.2194 

o  .  29005 

.     0-2667 

0.2232 

0-2137 

0-27361 

0.2493 

0.2201 

0.2073 

0-25574 

0-2313 

0.2177  (24°) 

0.2017  (24°) 

0.23642 

O.2I27 

.  .  . 

0.21569 

0-1935 

.  .  . 

.  .  . 

0.16990 

0-1533 

0.11840 

0.1057 

Wt.  Per  cent       Vol.  Per  cent  Wt.  Per  cent     Vol.  Per  cent  Wt.  Per  cent    Vol.  Per  cent 

Alcohol.  Absorbed  O.  Alcohol.          Absorbed  O.  Alcohol.         Absorbed  O. 

o  2.98  23.08          2.52  50  3.50 

9.09  2.78  28.57          2.49  66.67       -4-95 

16.67  2-63  33  -33  2.67  80  5.66 

SOLUBILITY  OF  OXYGEN  IN  PETROLEUM.    COEFFICIENT  OF  ABSORPTION  AT 
10°  =  0.229,  AT  2O°  =  0.202. 

(Gniewasz  and  Walfisz,  1887.) 

SOLUBILITY  OF  OXYGEN  ETHYL  ETHER. 

(Christoff,  1912.) 

Results  in  terms  of   the   Ostwald    Solubility  Expression,  A>  =  0.4235,  lw  =* 
0.4215. 


473 


OXYGEN 


SOLUBILITY  OF  OXYGEN  IN  AQUEOUS  SOLUTIONS  OF: 


Chloral.Hydrate  at  20°. 

(Muller,  1912-13.) 

Glycerol  at  15°.    (Muller,  1912-13.) 

Gms. 
CC13.CH(OH)2 
per  loo  Gms. 
Aq.  Sol. 

Aq?Sok 

ArBun°e^  ft        (CH2OH)TcHOH             d  of 
(Bunsen)                       IQQ  Qms                A     Sol 

at  20  •                     Aq.  Sol. 

Abs.  Coef.  0 
(Bunsen) 
at  15°. 

16.9 

1.0798 

0.02795 

20.5 

rfl2.5  =1.0509 

O.O2742 

32 

1.1630 

0.02495 

25 

dtf    = 

.0621 

0.02521 

52.9 

1.2935 

0.02325 

37-3 

dn*  = 

•0957 

0.02022 

61.08 

1-354 

O.O24IO 

45 

^12-5  = 

.Il6l 

O.OI744 

65.5 

1.382 

0.02580 

52 

fi?12  -5  = 

•I35I 

O.OI57O 

71.4 

1.4404 

0.02730 

7i.5 

dl2-b  = 

.1908 

0.00950 

78 

1.46 

0.03280 

88.5 

(/13.5=1.236 

0.00886 

SOLUBILITY  OF  OXYGEN  IN  AQUEOUS  SOLUTIONS  OF: 


Glucose  at  2O°.      (Muller,  1912-13-) 


Cane  Sugar  at  15°.     (Mttlkr,  1912-13-) 


Gms   C  H  O 

Abs,  Coef.  0 

Gms.  QaHaOu 

Abs.  Coef.  0 

per  zoo  Gms. 
Aq.  Sol. 

dzo  of 
f  Aq.  Sol. 

(Bunsen) 
at  20°. 

per  100  Gms. 
Aq.  Sol. 

AqU  Sol. 

(Bunsen) 
at  15°. 

10.84 

I.04I3 

0.02690 

12.  1 

.1.0482 

0.02969 

20-7 

1.0835 

O.O225O 

24.38 

I.  1022 

0.02396 

33-8 

I.I370 

0.0l8l5 

28.44 

I.I205 

o.  02181 

1.2295 

0.01390 

42.96 

I.I938 

0.01600 

58.84 

I  .  2649 

0.01250 

50 

I.23I8 

0.01359 

INFLUENCE  OF  ANESTHETICS  UPON  THE  SOLUBILITY  OF  OXYGEN  IN  OLIVE  OIL. 

(Hamberger,  1911.) 

Name  and  Cone,  of    Solubility  of  Oxygen  in; 
Narcotic  Added  pure       Narcotic 

to  the  Oil.  Solvent.    Solution. 

Sulfonal     (0.8  per  100)    9 . 69      4.55 

9.69 
9.69 
(saturated) 


Trional 


Tetronal     (2  per  100) 

« 

Camphor   (10  per  100) 


9. 10 
9. 10 
9.67 
9.67 
8-53 


5-68 
6.25 

4-55 
5-68 
9. 10 
9. 20 
7.96 


Name  and  Cone,  of 
Narcotic  Added 
to  the  Oil.      . 

Monochlorhydrine  (5 

"     '  (2-5 

(1.25 

(10 
(5 
(5 
(2.5 


D  ichlorhy  drine 
« 

Phenylurethan 


Solubility  of  Oxygen  in; 

Pure  Narcotic 

Solvent.  Solution, 
penoo)   9.10        7.50 
)   9.10        7.50 
)   9.10        7.90 
)   9.10        7.96 
)   9.10        8 
)    8.53        6.25 
)    8.53        7.50 


Data  for  the  solubility  of  oxygen  in  liquid  air  are  given  by  Baly  (1900). 

Data  for  the  solubility  of  oxygen  in  hemoglobin  are  given  by  Jolin  (1889). 

Data  for  the  solubility  of  oxygen  in  defibrinated  ox-blood  and  ox-serum,  at 
pressures  varying  from  760  to  about  1400  ram.  Hg,  are  given  by  Findlay  anc 
Creighton  (1911). 


OZONE  03. 


SOLUBILITY  IN  WATER. 

(von  Mailfert,  1894;  Carius;  Schone,  1873.) 


t°. 

w. 

G. 

R. 

t°. 

w. 

G. 

R. 

0 

39-4 

61.5 

0.641 

27 

13-9 

51-4 

0.270 

6 

34-3 

61 

0.562 

33 

7-7 

39-5 

0.195 

n.  8 

29.9 

59-6 

O.5OO 

40 

4.2 

37.6 

O.II2 

13 

28 

58-1 

0.482 

47 

2.4 

31.2 

0.077 

IS 

25-9 

56.8 

0.456 

55 

0.6 

19.3 

0.031 

19 

21 

55-2 

0.381 

60 

0 

12.3 

0 

W  =  milligrams  ozone  dissolved  per  liter  water.  G  =  milligrams  ozone  in 
one  liter  of  the  gas  phase  above  the  solutions.  R  =  ratio  of  the  dissolved  to 
undissolved  ozone  (W  -J-  G). 


OZONE  474 

The  experiments  of  Schone  (see  preceding  page)  were  repeated  by  Inglis 
(1903).  "The  results  confirm  Schone's  experiments  and  indicate  that  ozone, 
when  passed  through  water,  is  partly  decomposed." 

According  to  Moufang  (1911)  the  solubility  of  ozone  in  distilled  water  ranges 
from  about  10  milligrams  per  liter  at  2°  to  about  1.5  milligrams  per  liter  at  28°. 
The  solubility  is  greatly  affected  by  other  substances  in  solution.  Small  amounts 
of  acids  increase  the  solubility  and  render  the  aqueous  solution  of  the  ozone  more 
permanent.  Alkalis  decrease  the  solubility.  Neutral  salts  (i.e.,  calcium  sulfate) 
increase  the  solubility. 

SOLUBILITY  OF  OZONE  IN  DILUTE  SULFURIC  ACID. 

(Rothmund,  1912.) 

The  explanation  of  the  discrepancies  concerning  the  solubility  of  ozone  in  water  is 
that  the  ozone  quickly  decomposes  as  the  saturation  point  is  reached.  Rothmund, 
therefore,  determined  the  solubility  in  dilute  HaSC^  in  which  decomposition  takes 
place  much  more  slowly  than  in  pure  water.  At  o°  the  absorption  coef.  /3  (Bun- 
sen,  see  p.  227)  in  o.i  n  H2SO4,  is  0.487.  The  coef.  remains  practically  the  same 
when  the  concentration  of  the  ozone  is  changed  over  a  wide  range,  hence  Henry's 
Law  holds  for  ozone.  The  dissolved  ozone  has  the  same  molecular  weight  as  the 
gaseous.  The  solubility  depression  which  ozone  experiences  through  o.i  n 
H2SO4  is  calculated  as  1.5%.  Therefore,  by  extrapolation,  it  is  calculated  that 
the  abs.  coef.  ft  of  ozone  in  H2O  at  o°,  is  0.494. 

PALLADIUM   CHLORIDE   PdCl2. 

When  i  gm.  of  palladium,  as  chloride,  is  dissolved  in  100  cc.  of  H2O  and  shaken 
with  100  cc.  of  ether,  0.02  per  cent  of  the  metal  enters  the  ethereal  layer  at  ord. 
temp.  When  aq.  10%  HC1  is  used/p.oi  per  cent  of  the  metal  enters  the  ethereal 
layer.  (Mylius,  1911.) 

100  cc.  anhydrous  hydrazine  dissolve  i  gm.  PdCl2,  with  evolution  of  gas  and 
formation  of  a  black  precipitate,  at  room  temperature.  (Welsh  and  Broderson,  1915.) 

PALMITIC  ACID  CH3(CH2)14COOH. 

SOLUBILITY  IN  AQ.  AND  ABSOLUTE  ETHYL  ALCOHOL. 

i  (Falciola,  1910.) 

Cms.  CH3(CH2)i4COOH  per  100  cc.: 


Absolute  Aq.  75% 

Alcohol.  Alcohol. 

10  2.8  0.24  0.05 

20  9.2  0.43  0.08 

30  ...  1.19  0.12 

40  31.9  3-59  0-31 

100  cc.  sat.  solution  of  palmitic  acid  in  methyl  alcohol  of  94.4  vol.  %  (d  = 
0.8183)  contain  1.03  to  1.17  gms.  at  0.2°,  equilibrium  being  approached  from  above. 
The  mixtures  were  simply  allowed  to  stand  in  an  ice  chest  for  from  12  to  156 

hours.  (Hehner  and  Mitchell,  1897.) 

SOLUBILITY  OF  PALMITIC  ACID  IN  SEVERAL  ALCOHOLS. 

(Timofeiew,  1894.) 
( 
Alcohol. 

Methyl  Alcohol 
it 

d 
Ethyl  Alcohol 

u 

One  hundred  gms.  of  aq.  5%  solution  of  bile  salts  dissolve  about  o.i  gm.  palmitic 
acid.  100  gms.  aq.  5%  solution  of  bile  salts  containing  i  %  of  lecithin  dissolve  0.6 
gms1.  palmitic  acid.  (Moore,  Wilson  and  Hutchinson,  1909.) 


Gms. 

Gms. 

to      CH3(CH2)14COOH              A,_,_i 

to     CH3(CH2)i4COOH 

per  100  Gms. 

i>  . 

per  loo  Gms. 

Sat.  Sol. 

Sat.  Sol. 

'0 

0.72 

Propyl  Alcohol 

0 

2.92 

21 

5-i 

it 

21 

13.8 

36 

29-5 

Isobutyl  Alcohol 

0 

2.2 

O 

2 

a 

21 

12.8 

21 

10.  I 

475 


PALMITIC  ACID 


Cms.  Stearic  Acid 

t°of 

Gms.  Stearic  Acid 

per  100  Gms. 
Mixture. 

Solidi- 
fication. 

per  loo  Gms. 
Mixture. 

100 

57-2 

55 

90 

56.42 

5o 

80 

56.38 

45 

70 

56.11 

40 

60 

55-62 

36 

t°of  Gms.  Stearic  Acid 

Solidi-  per  100  Gms. 

fication.  Mixture. 

54.85  Eutec. 

55-46 

56.53 

59-3i 

62.62 


30 
25 

20 

10 

O 


SOLIDIFICATION  POINTS  OF  MIXTURES  OF  PALMITIC  AND  STEARIC  ACIDS. 

(De  Visser,  1898.) 

Fifty  gram  samples  of  each  mixture  were  used  and  great  care  taken  to  insure 
accuracy  of  the  determinations. 
t°of 

Solidi- 
fication. 

69.32 
67.02 

64-51 
61.73 
58.76 

Additional  determinations  on  this  system  by  Dubowitz  (1911)  are,  for  the 
most  part,  in  good  agreement  with  the  above.  According  to  Carlinfanti  and 
Levi  Malvano  (1909),  however,  the  eutectic  could^not  be  located  and  there  were 
indications  of  the  existence  of  solid  solutions. 

DATA  ARE  GIVEN  FOR  THE  SOLIDIFICATION  POINTS  OF  THE  FOLLOWING 
MIXTURES: 

Palmit  c  Acid  +  Tripalmitin 

-|-  +  Stearic  Acid. 

4-  4-  Tristearin. 

+  Tristearin  +  Stearic  Acid. 

+  Tristearin. 
Tripalmitin      +  Tristearin  -f  Stearic  Acid. 

-j-  Stearic  Acid. 
Palmitic  Acid  Cetyl  Ester  +  Paraffin. 


(Kremann  and  Klein,  1913.) 
(Kremann  and  Kropsch,  1914.) 


(Kremann  and  Klein,  1913.) 
(Palazzo  and  Battelli,  1883.) 


PAPAVEBINE   C20H21N04. 

IOO  gms.  carbon  tetrachloride  dissolve  0.203  gm.  at  17°.  (Schindelmeiser,  1901.) 

100  gms.  carbon  tetrachloride  dissolve  0.518  gm.  at  20°.  (Gori,  1913.) 

loo  gms.  ethyl  ether  dissolve  0.38  gm.  at  10°. 

100  gms.  of  each  of  the  following  solvents  dissolve  the  stated  amount  of  papaver- 

ine  at  20°.  Aniline,  29  gms.;  pyridine,  8  gms.;  piperidine,  I  gm.;  diethylamine, 

0.4  gm.  (Scholtz,  1912.) 

PARAFFIN. 

.SOLUBILITY  OF  OZOKERITE  PARAFFIN  OF  MELTING  POINT  64°-65°  AND 
SP.  GR.  AT  20°  =  0.917  IN  SEVERAL  SOLVENTS  AT  20°. 

(Pawlewski  and^Filemonowicz,  1888.) 


Gms.  Paraffin  per  100 


Gms.  Paraffin  per  100 


Solvent. 

Carbon  Bisulfide 
Benzine,  boiling  below  75° 
Turpentine,  b.  pt.  i58°-i66° 
Cumol,  com.  b.  pt.  160° 

"       frac.  iso°-i6o° 
Xylene,  com.  b.  pt.  i35°-i43° 

"        frac.  i35°-i38° 
Toluene,  com.  b.  pt.  io8°-no 

frac.  io8°-io9° 
Chloroform 
Benzene 
Ethyl  Ether 
Isobutyl  Alcohol,  com. 

F.-pt.  data  for  paraffin  +  stearin  are  given  by  Palazzo  and  Battelli  (1883). 


Gms. 

cc. 

Solvent. 

Gms. 

cc. 

Solvent. 

Solvent. 

Solvent. 

Solvent. 

12.99 

Acetone 

0.262 

0 

.209 

n-73 

8 

'.48 

Ethyl  Acetate 

0.238 

.  .  . 

6.06 

5 

.21 

"      Alcohol 

0.219 

4.  26 

3 

.72 

Amyl  Alcohol 

O.2O2 

0 

.164 

3-99 

3 

•39 

Propionic  Acid 

0.165 

.  .  . 

3-95 

3 

•43 

Propyl  Alcohol 

o.  141 

4-39 

3 

•77 

Methyl  Alcohol 

O.O7I 

o 

.056 

3     3-88 

3 

•34 

Methyl  Formate 

0.060 

3-92 

3 

.41 

Acetic  Acid 

0.060 

0 

.063 

2.42 

3 

.61 

"      Anhydride 

0.025 

1.99 

1 

•75 

Formic  Acid 

0.013 

0 

.015 

i-95 

Ethyl  Alcohol  75% 

0.0003 

0.285 

o 

.'228 

PENTANE 


476 


Isopentane  Rich 
Layer. 

Phenol  Rich 
Layer. 

4-5 

87 

7 

83-5 

"•5 

80 

18 

75-S 

29-5 

68 

40 

58 

PENTANE   CH3(CH2)3CH8. 

Data  for  the  solubility  of  pentane  in  liquid  carbon  dioxide,  determined  by  the 
synthetic  method,  are  given  by  Biichner  (1906). 

IsoPENTANE   (CH3)2CH.CH2CH3. 

RECIPROCAL  SOLUBILITY  OF  ISOPENTANE  AND  PHENOL.  (Campetti  and  Del  Grosso,  1913.) 

Gms.  Phenol  per  100  Cms. 


20 

30 
40 

50 
60 

65 

66  crit.  temp.  50 

F.-pt.  data  for  mixtures  of  hexachloro-a-keto  7--R-pentene,  C5C16O,  +penta 

chloromonobromo  ex-keto  y-R  pentene,  C5Cl6BrO,  are  given  by  Kiister  (1890,  1891). 

PEPTONE. 

100  gins.  H2O  dissolve  42.2    gms.  peptone  at  20-25°.     (Dehn,  1917.) 

"          pyridine  "         0.22      "  " 

aq.  50%  pyridine        "       12.6       " 

PERCHLORIC  ACID   HC1O4. 

SOLUBILITY  IN  WATER,     (van  Wyk,  1902,  1905.) 

Mixtures  of  HC1O4  and  water  were  cooled  until  crystals  appeared  and  then  very 
gradually  warmed  and  constantly  stirred  while  an  observation  was  made  of  the 
exact  temperature  at  which  the  last  crystal  disappeared.  At  certain  concentrations 
and  temperatures  unstable  solid  phases  were  obtained,  also,  curves  for  two  series  of 
mix  crystals  were  encountered.  The  methods  for  detecting  these  phases  consisted 
in  seeding  the  saturated  solutions  with  the  several  different  crystalline  forms,  and 
observing  the  change  in  rate  of  cooling  during  the  solidification  of  the  mixture. 
The  data  for  the  mix-crystal  curves  I  and  II  are  not  given  in  the  following  table: 


Mols.  HC1O4 
t°.         per  100  Mols.               Solid  Phase.                         t°. 
HC1O4+H2O. 

Mols.  HC104 
per  100  Mols.     Solid  Phase. 
HC104+H2O. 

0 

0 

Ice                           -32 

26 

HC104.2*H20 

—  10 

5 

-29 

.8 

28 

•57 

—  21 

7 

-44 

27 

HC104.2H2O 

-34 

•5 

9 

-41 

27 

.25          «' 

-54 

ii 

-34 

28 

ii 

-50 

•5 

19 

HC104.3iHjO                   —  24 

29 

•9 

-45 

20 

-17 

.8m. 

^•33-3 

-42 

•3 

21 

—  21 

•5 

36 

" 

-41 

•4 

22.22 

-23 

.6 

36 

.5             "  +HClO4.HaO 

-43 

23-5 

—  12 

•5 

37 

HC104.H2O 

-40 

•5 

22.5 

HC104.3H2Oa                   1+3 

38 

-39 

•5 

22.75 

28 

40 

.8 

-37 

.6 

24 

40 

43 

•7 

-37 

•5 

26 

«                                   50  m.  pt 

50 

-38 

.8 

27 

45 

59 

•9 

-47-8 

22.5 

HC104.3H2O/3                         27 

•5 

71 

•5 

-44 

24 

17 

77 

.2 

-43 

•5 

24-5 

+  2 

.2 

83 

•3 

-43 

.2 

25 

"                               —21 

•5 

90 

•7 

-44 

•5 

26 

-40 

94 

-37 

.2 

25 

HClO4.3H2Oa+HC104.2|H2O    —  IO2 

ICO 

477         PETROLEUM  ETHER 

PETROLEUM  ETHER. 

100  cc.  H2O  dissolve  0.005  cc.  petroleum  ether  at  15°.  (Groschuff.  1910.) 

PHENACETIN   (p  Acetphenetidin)  CeH^OC^NHCHaCO  p.   • 
SOLUBILITY  IN  AQUEOUS  ALCOHOL  AT  25°. 

(Seidell,  unpublished.) 


Wt.  %  C2H5OH 
in  Solvent.    __ 

,      f        Cms.  C6H4(OQH5) 
9  t  c£l       NHCH3CO  per  100 
j    Sat.  Sol.     Gms.  Sat.  Solution. 

Wt.  %  OH5OH 
in  Solvent. 

Sa«, 

Cms.  Sat.  Solution. 

o  (water) 

I 

0.0766 

70 

0.879 

6.25 

10 

0.984 

0.14 

80 

0.858 

7.63 

20 

0.968 

0.28 

85 

0.847 

7.88 

30 

0.952 

0.65 

90 

0.834 

7.82 

40 

0-935 

1-50 

92-3 

0.827 

7.70 

50 

0.917 

2.85 

95 

0.821 

7-45 

60 

0.898 

4-55 

100 

0.806 

6.64 

loo  gms.  H2O  dissolve  1.43  gms.  phenacetin  at  "the  b.  pt.  (U.S.  P.,  VIII.) 

ioogms-92.3  wt.  %  alcohol  dissolve  about^o  gms.  phenacetin  at  the  b.  pt.      " 

SOLUBILITY  OF  PHENACETIN  IN  SEVERAL  SOLVENTS. 

(Seidell,  1907.) 

Gms.  Phenacetin  Gms.  Phenacetin 

Solvent.  t°.  per  100  Gms.  Solvent.  t°.  per  100  Gms. 

Sat.  Solution.  Sat.  Solution. 

Acetone  3°~3I  10.68  Benzene       30-31  0.65  (0.873) 

Amyl  Acetate  3°~~3I    2.42  (0.865)  Chloroform     25      4.76 

Amyl  Alcohol  25        3.51  (0.819)  Ether  25      1.56 

Acetic  Acid  (99.5%)    21.5   13.65  (1.064)  Toluene          25      0.30  (0.863) 
Aniline  3°~3I    9-46  (1.025)  Xylene  32.5   1.25  (0.847) 

Benzaldehyde  3°~3I    8.44  (1.063) 

(Figures  in  parentheses  are  Sp.  Gr.  of  Sat.  Solutions.) 

100  cc.  petroleum  ether  dissolve  0.015  gm.  phenacetin  at  room  temp.  (Salkower,  1916.) 
100  gms.  pyridine  dissolve  17.39  gms.  phenacetin  at  20-25°.  (Dehn.igi?.) 

100  gms.  aq.  50%  pyridine  dissolve  28.94  £m$'  phenacetin_at  20-25°.        " 


PHENANTHRAQUINONE 

SOLUBILITY  IN  BENZENE  AND  IN  ETHYL  ACETATE. 

(Tyrer,  1910.) 

Solubility  in  Benzene.  Solubility  in  Ethyl  Acetate. 

,„  Sp  Gr.of        Gms'  (CaHMOW.  s     Gr  of       Gms. 

*°          SatPSolution.  --  *°         SatPSolution. 


10    0.8902     0.412          10   0.9102     0.518 

15     0.8850       0.471  2O     0.9025       0.626 

20     0.8800       0.538  30     0.8906       0.770 

30     0.8698       0.738  40     0.8789       0.995 

40  0.8601  1-032  50  0.8674  1.292 

50  0.8506  x-354  60  0.8561  1.640 

60  0.8415  1.760  65  0.8508  1.902 

70  0.8327  2.687  7°  0-^454  2.215 

80  0.8241  3.770  75  0.8401  2.515 

NOTE.  —  The  Sp.  Gr.  determinations  given  in  the  above  table  and  in  the  tables 
for  anthracene  and  anthraquinone,  pp.  81  and  82,  are  not  included  in  the  original 
paper  of  Tyrer  (1910)  but,  in  response  to  my  request,  have  been  kindly  supplied 
for  the  present  volume.  I  am  also  indebted  to  Dr.  Tyrer  for  the  modified  form 
of  his  original  tables  showing  the  solubilities  of  anthraquinone  and  phenanthra- 
quinone  in  mixed  solvents.  (A.  S.) 


PHENANTHRAQUINONE 


478 


SOLUBILITY  OF  PHENANTHRAQUINONE  IN  MIXTURES  OF  ORGANIC  SOLVENTS. 

(Tyrer,  1910.) 

In  C6H6  +  Hydrocarbons       In  CHC13  +  Pentane     In  CH3COOC2H5  +  Hydro- 


(i)  at  48°. 

Per  cent              Gms 

at  14.5°. 

.  Phenan-        Per  cent            Gms.  Phenan- 

carbons(i)  at  48°. 

Per  cent         Gms.  Phenan- 

Mixe^ 
Solvent 

thraquinone        CHC13  in              thraquinone         CH3COOC2H5       thraquinone 
per  loo  Gms.          Mixed               per  100  Gms.             in  Mixed          per  100  Gms. 
Solvent.             Solvent.                  Solvent.                 Solvent.                Solvent. 

0 

0 

.0708 

0 

0. 

025 

O 

0 

•073 

10 

0 

.088 

10 

o. 

045 

14 

.19 

0 

.126 

20 

o 

.118 

20 

0. 

080 

27 

•37 

O 

.207 

30 

0 

.160 

30 

0. 

"5 

39 

•94 

0 

•335 

40 

0 

.228 

40 

0. 

165 

52 

.12 

0 

•494 

50 

o 

.318 

50 

0. 

220 

63 

-56 

0 

-656 

60 

0 

.440 

60 

0. 

330 

74 

.19 

O 

.817 

70 

0 

.588 

70 

0. 

525 

84 

.62 

0 

•993 

80 

0 

•772 

80 

o. 

805 

90 

I 

•073 

90 

I 

.004 

90 

I. 

415 

IOO 

I 

•  230 

IOO 

I 

.288 

IOO 

2. 

402 

(O 

Distilled  from  petroleum,  b.  pt.  -  82' 

'-92 

°.    (See  note,  preceding  page.) 

PHENANTHRENE  Ci4Hi0. 

SOLUBILITY  IN 

ALCOHOL 

AND  IN  TOLUENE 

.* 

(Speyers 

—  Am.J.Sci.[ 

4]  14,  295,  'oa.) 

In  Alcohol. 

In  Toluene. 

Gms.  CwHro  per 

Sp.  Gr.  of 

Gms.  Ci4Hio  per 

Sp.  Gr.  of 

t 

loo  Grams 

Solutions 

loo  G 

rams 

Solutions 

CjzHjiOH.        CHzO  at  4°-) 

QHfi.CHa 

(H20  at  4° 

.) 

0 

3-65 

0.814 

23 

.0 

0.925 

10 

3-80 

0.807 

30 

.O 

0.929 

20 

4.6 

0.801 

42 

•  O 

Q-934 

25 

5-5 

o-7P9 

50 

.O 

0-939 

30 

6.4 

0-797 

58.0 

0-943 

40 

8.2 

o-795 

76 

.0 

o-955 

50 

10.6 

o.794 

95 

.0 

0.971 

60 

15.6 

o-797 

"5 

.0 

0.989 

70 

0.815 

.0 

1.007 

80 

0.865  (76 

-4°)        155-0 

1.027 

•   Calculated  from  the  original  results  which  are  given  in  terms  of  gram  molecules  of  Phenanthrene 
per  loo  gram  molecules  of  solvent,  and  for  irregular  intervals  of  temperature. 

Behrend,  1892,  reports  2.77  gms.  phenanthrene  per  100  gms.  alcohol  at  12.3°, 
and  3.09  gms.  at  14.8°. 

SOLUBILITY  OF  PHENANTHRENE  IN  ORGANIC  ACIDS.    (Timofeiew,  1894.) 

Gms.  Ci4H10  Gms.  CUH10 

Acid.  t°.          per  100  Gms.  Acid.  .!  t°.          per  100  Gms. 

Sat.  Sol.  Sat.  Sol. 

Acetic  Acid         23  8.31      Propionic  Acid 

9.8 


Butyric  Acid 


23 
39 
70 

23 
39 


34-6 

15-6 
21 


23 

39 
62. 

23 


17 
21.4 

40.3 
12.3 
16.6 

(Aschan,  1913.) 


Isobutyric  Acid 
Valeric  Acid 

100  gms.  95%  formic  acid  dissolve  0.46  gms.  CuHio  at  20.8 
F.-pt.  data  for  mixtures  of  phenanthrene  and  each  of  the  following  compounds 
are  given  by  Kremann  et.  al.,  (1908);  1.2.6  dinitrotoluene,  1.2.4.  dinitrotoluene, 
1.3.4  dinitrotoluene,  trinitrotoluene  and  trinitrobenzene.  Results  for  mixtures 
of  phenanthrene  and  2.4  dinitrotoluene  are  given  by  Kremann  and  Hofmeier 
(1910). 


479 


PHENANTHRENE 


SOLUBILITY  OF  PHENANTHRENE  IN  SEVERAL  SOLVENTS  AT  25°. 

(Hildebrand,  Ellefson  and  Beebe,  1917.) 


Solvent. 

Alcohol 
Benzene 
Carbon  Bisulfide 


Cms.  CuHjo  per  100 
Gms.  Solvent. 

4.91 

59-5 
80.3 


Solvent. 

Carbon  Tetrachloride 

Ether 

Hexane 


Gms.  CuHjo  per  too 
Gms.  Solvent. 


26.3 
42.9 

9-15 


SOLUBILITY  OF  PHENANTHRENE  PICRATE  IN  ABSOLUTE  ALCOHOL. 

(Behrend,  1892.) 
Grams  per  100  Grams  Saturated  Solution. 

Picric  Acid    +    Phenanthrene  •=  Phenanthrene  titrate. 
12-3  0.91  O.yi  1.62 

14.3  i  .00  0.78  1.78 

17.5  1.05  0.82  1.87 


SOLUBILITY  OF   PHENANTHRENE   PICRATE   IN  ALCOHOLIC  SOLUTIONS 
CONTAINING  PICRK;  ACID  AND  ALSO  PHENANTHRENE. 

(Behrend.) 

Grams  Added  to  62  cc.  Abs.  Alcohol.  Gms.  per  100  Gms.  Sat.  Solution. 

to.          ,  -  »  -  N  r. 

P.  Picrate  +  Picric  Ac.  +  Phenanthrene.  Pi 

12.3 
12-3 
12  -S 
12-3 
17-5 
17-5 
17-5 
17-5 
17-5 

PHENOL  C6H5OH. 

SOLUBILITY  IN  WATER. 

(Alexejew,  1886;  Schreinemaker,  1900;  Rothmund,  1898.) 

The  determinations  were  made  by  the  "Synthetic  Method,"  for  which, 
Note,  p.  1  6. 

Gms.  Phenol  per  100  Gms. 


\  Picrate  +  Picric  Ac.  +  Phenanthrene 

1-4 

0 

o-5 

1.4 

0.8 

o 

0 

0.9 

2.1 

0.8 

0 

4.0 

•4 

O.I 

0 

•4 

O.2 

0 

•4 

1.0 

0 

•4 

4.0 

o 

•4 

o.o 

2.2 

Picric  Ac. 

+  Phenanthrene  *- 

P.  Picrate 

0-534 

I-4I3 

1-947 

0.409 

2.I4I 

2-550 

o-354 

2-77 

3.124 

0.139 

5.626 

c  .  76? 

I-I59 

o-75 

I  •  Q  I 

1.285 

0.68 

1-97 

2-45 

o-37 

2.82 

6.15 

0.195 

6-345 

0.423 

3.276 

3-699 

i>  . 

Aqueous  Layer. 

Phenol  Layer. 

10 

7-5 

75 

20 

8-3 

72.1 

30 

8.8 

69.8 

40 

9.6 

66.9 

50 

12 

62.7 

55 

I4.I 

59-5 

60 

I6.7 

55-4 

65 

21-9 

49.2 

68.3  (crit.  temp.) 

33-4 

Results  confirming  the  above,  and  also  viscosity  measurements,  are  given  by 
Scarpa  (1904). 

The  complete  T  —  x  data  for  the  system  are  given  by  Smits  and  Maarse  (1911). 
F.-pt.  data  for  the  system  are  given  by  Rozsa  (1911)  and  Paterno  and  Ampola 


Vaubel  (1895)  states  that    ipo  gms.  sat.  aqueous  solution  contain  6.1  gms. 
phenol  at  20°.     Sp.  Gr.  of  solution  =  1.0057. 


PHENOL 


480 


PHENOL. 


SOLUBILITY  OF  PHENOL  IN  AQUEOUS  ACETONE  SOLUTIONS. 

(Schreinemakers,  1900.) 


In  4.24% 
Acetone. 

Grams  Phenol  per 

In  12.2% 
Acetone. 

Gms.  Phenol  per 

In  24.6% 
Acetone. 

Gms.  Phenol  per 

In  59-9% 
Acetone. 

Gms.  Phenol  per 

A0               100  Gms. 

100  Gms. 

100  Gms. 

100  Gms. 

Aq.  Acetone 
Layer. 

Phenol 
Layer. 

Aq  .  Acetone 
Layer. 

Phenol  * 
Layer. 

Aq.  Acetone 
Layer. 

Phenol    ' 
Layer. 

Aq  .  Acetone   Phenol 
Layer.        Layer 

20 

... 

.  .  . 

26.  o       60.  5 

3° 

S-o 

74.0 

4.0 

71.0 

6.0 

69.5 

28.5          57.0 

40 

5-5 

70.0 

32.0          52.0 

5° 

5-7 

67.0 

5-0 

67.0 

8.0 

64.0 

34-  5§       49-  °§ 

60 

6-5 

61.0 

36.51!      46.  5  U 

70 

9.0 

51.0 

7-5 

57-5 

19.0 

57-  ° 

(49-5°)  41-5 

80 

14.  o 

34-0 

10.5 

49-5 

14.0 

52-5 

(84°)  22.5 

20.  4* 

23.  ot 

47.  ot 

(90.3°)  25. 

o 

26.  5t 

44.  o  t 

(90.  5°)  35- 

,  o 

•90° 

t8S° 

t87°.S 

§45° 

!!47°.5 

The  figures  in  the  above  table  were  read  from  curves  plotted  from  the  original 
results.  Similar  data  are  also  given  for  acetone  solutions  of  seven  other  concen- 
trations. 

The  determinations  were  made  by  adding  various  quantities  of  phenol  to  the 
mixtures  of  water  and  acetone  and  observing  the  temperature  at  which  the  two 
layers  became  homogeneous.  The  isothermal  lines  for  30°,  50°,  68°,  80°,  85°  and 
87°  were  located.  The  results  for  30°  and  80°  are  as  follows:  (Schreinemakers,  1900.) 


Results  at  30°. 

Gms.  per  100  Gms.  Mixture.  Gms.  per  100  Gms.  Mixture. 


Results  at  80°. 

Gms.  per  100  Gms.  Mixture. 


H20. 

(CH^CO. 

C6H6OH. 

H20. 

(CH3)2CO. 

C6H6OH. 

H20. 

(CHs),CO. 

C6H5OH. 

92 

0 

8 

18.4 

34-i 

47-5 

83.3 

3-7 

13 

92-3 

i-7 

6 

17.2 

25-8 

57 

82.9 

7-i 

10 

91 

4 

5 

17.9 

81.1 

64 

74-7 

13-8 

"•5 

88.4 

7.6 

4 

19.1 

12.9 

68 

61.8 

20.2 

18 

81 

IS 

4 

21  .1 

9-9 

69 

52-5 

24-5 

23 

70.9 

23.1 

6 

22.6 

7-4 

70 

40.6 

27.4 

32 

62.1 

28.9 

9 

25.2 

4.6 

70.2 

32.2 

21.8 

46 

51.6 

34-9 

13-5 

27.1 

2-3 

70.6 

33-4 

15-6 

5i 

39-8 

40.2 

20 

28.7 

i-3 

70 

35-4 

ii.  6 

53 

28.9 

43-i 

28 

30 

o-5 

69-5 

40-5 

7-5 

S2 

21.8 

40.2 

38 

49-7 

4-3 

46 

62.7 

2.8 

34-5 

SOLUBILITY  OF  PHENOL  IN  BENZENE  AND  IN  PARAFFIN, 

(Schweissinger,  1884-85.) 

Gms.  C6H5OH  per  100  Gms.  Solvent  at: 


Solvent. 

Paraffin 
Benzene 


16°. 

1.66 
2-5 


8-33 


10 


43". 

5 

IOO 


Data  for  equilibrium  in  systems  composed  of  phenol,  water  and  each  of  the  fol- 
lowing compounds  are  given  by  Timmermans  (1907):  NaCl,  KC1,  KBr,  KNO3, 
,  MgSO4,  tartaric  acid,  salicylic  acid,  succinic  acid  and  sodium  oleate. 


48 1 


PHENOL 


MISCIBILITY  OF  AQUEOUS  ALKALINE  SOLUTIONS  OF  PHENOL  WITH  SEVERAL 
ORGANIC  COMPOUNDS  INSOLUBLE  IN  WATER. 

(Scheuble,  1907.) 

To  5  cc.  portions  of  aq.  KOH  solution  (250  gms.  per  liter)  were  added  the  given 
amounts  of  the  aq.  insoluble  compound  from  a  buret  and  then  the  phenol,  drop- 
wise,  until  solution  occurred.  Temperature  not  stated. 

Composition  of  Homogeneous  Solutions. 


cc.  Aq.  KOH. 
5 
5 

5 

5 
5 


cc.  Aq.  Insol.  Cmpd.  Gms.  Phenol. 

2  (=  1.64  gms.)  Octyl  *  Alcohol        2.6 


5  (=  4.1    gms.)  3.9 

2  (=  1.74  gms.)  Toluene  4.9 

3  (=  2.61  gms.)  Toluene  6.7 
2  (==  1.36  gms.)  Heptane  15 

1  =  the  normal  secondary  octyl  alcohol,  i.  e.,  the  so-called  capryl  alcohol,  CH3(CH2)s.CH(OH)CHj. 

SOLUBILITY  OF  PHENOL  IN  AQUEOUS  SOLUTIONS  OF  DEXTRO  TARTARIC 
ACID  AND  OF  RACEMIC  ACID. 

(Schreinemakers,  1900.) 

In  5.093%  Acid.                         In  19.34%  Acid.  In  40.9%  Acid. 

Gms.  Phenol  per  100  Gms.              Gms.  Phenol  per  100  Gms.  Gms.  Phenol  per  too  Gms 


30 
50 
60 

65 

67-5 

69* 


Aq.  Acid 
Layer. 

7-5 


14-5 
19-5 
25 


Phenol 
Layer. 

72.5 
65.5 
58 

53 
48.5 


t°.  ' 

Aq.  Acid      Phenol 

Layer.         Layer. 

50 

10           77 

60 

12.5        72 

70 

19           64 

75 

29           56 

77* 

47 

47-5 


70 
80 

85 
90 

95< 

97" 


Aq.  Acid. 
Layer. 

13 
16.5 

2O 
26.5 

39 


Phenol 
Layer. 


77 
74 

63-5 


54 


*  Critical  temperature. 

Identical  results  were  obtained  with  the  dextro  and  racemic  acids,  showing  that 
both  have  exactly  the  same  influence  on  the  formation  of  layers  in  the  system 
water-phenol. 

DISTRIBUTION  OF  PHENOL  BETWEEN: 
AMYL  ALCOHOL  AND  WATER  AT  25°.         BENZENE  AND  WATER  AT  2o°r 

(Herz  and  Fischer  —  Ber.  37,  4747,  '04.)  (Vaubel  —  J.  pr.  Ch.  [2]  67,  4?6,  'op 


Millimols  Phenol 
per  10  cc. 

Gms.  Phenol 
per  100  cc. 

Alcoholic  Aqueous 
Layer.     Layer. 

0-  75     0-P47 
0.9       0.05 
I.I        0.07 
e.  6      o.  16 
54-1      3-83 
56-3      3-9 

Alcoholic  Aqueous 
Layer.      Layer. 

o.  705     o.  0441 
o.  846     o.  047 
1.035     0.066 
2.445     0.150 
50.88       3.601 
52.93       3.667 

Gms.  Phenol  in1 


Volumes  of  Solvents 

i  Gm.  Phenol  ^5"           . 

Layer.     Layer 

5occ.H2O+  5occ.C6H8  0.286     0.714 

"         -r-ioocc.  "  o.  1188  0.8212 

"         +151000.  u  0.0893  0.9107 

"        *f20occ.  "  0.0893  0.9107 


DISTRIBUTION  OF  PHENOL  BETWEEN  WATER  AND  BENZENE  AT  20°. 

(Philip  and  Bramley,  1915.) 

Gms.  Phenol  per  Liter.  * 

Ratio  -  • 
a 

2.194 
2.189 
2.184 
2.176 

2.181 

Results  are  also  given  for  the  effect  of  NaCl,  KC1  and  of  LiCl  upon  the  above 
distribution. 


Aq.  Layer,  a. 

C6H6  Layer,  b. 

0-945 

2.073 

0.888 

1.944 

0.711 

1-553 

0-594 

0-475 

1.293 
i  036 

lims.  .Fnei 

iol  per  Liter. 

A.                 .... 

Ratio-. 
a 

2.173 

2.175 
2.180 
2.189 

Aq.  Layer,  a. 
0-356 
0.238 
O.II9 

0.0601 

QH6  Layer;  b. 
0.7736 

o.5J77 

0.2594 
O.I3I4 

PHENOL 


482 


DISTRIBUTION    OF    PHENOL    BETWEEN    WATER    AND    BENZENE    AND 
BETWEEN  AQUEOUS  K2SO4  SOLUTIONS  AND  BENZENE  AT  25°. 

(Rothmund  and  Wilsmore  —  Z.  physik.  Ch.  40,  623,  '02.) 

NOTE.  —  The  original  results,  which  are  given  in  terms  of  gram 
jnols.  per  liter,  were  calculated  to  grams  per  liter,  and  plotted  on  cross- 
section  paper.  The  following  figures  were  read  from  the  curves 
obtained. 


Between  H2O  and  C6H«. 


Effect  of  K2SO4  upon  the  Distribution. 


Grams  C8H5OH 
per  Liter  of: 

Gms.  K2SO4 
per  Liter 

(i)  Gms.  CeH6OH 
per  Liter  of: 

GOGms.  C6H5OH 
per  Liter  of: 

fi20 
Layer. 

Layer. 

Aq. 
Solution. 

Aq. 
Layer. 

QjH,, 
Layer. 

Aq. 
Layer. 

Layer. 

5 

10 

L36 

17.08 

59-96 

9-52 

26.28 

10 

28 

2.72 

16.92 

60.63 

9-50 

26.38 

20 

e 

5-44 
10.89 

16.85 
16-44 

60.92 
62.73 

9.46 

9-35 

26.55 
27.06 

C5 

128 

21.79 

15.89 

65.19 

9.09 

28.27 

30 

200 

43-59 

14-85 

69.71 

8.68 

30.21 

35 

300 

87.18 

12.92 

78.00 

r-79 

34.38 

40 

410 

45 

520 

So 

610 

(i)  First  series. 

(2) 

Second  series. 

EQUILIBRIUM  IN  THE  SYSTEM  PHENOL,  BENZENE  AND  WATER  AT  25°. 

(Horiba,  1914-1916.) 

Cms.  per  100  Cms.  Sat.  Sol. 

Solid  Phase. 

Q,H6OH 


C«H6OH. 

C6H6. 

H20. 

81.06 

18.94 

0 

89.78 

7-92 

2.30 

92.31 

4.07 

3.62 

95-14 

o 

4.86 

The  results  for  the  conjugated  liquid  layers  are  as  follows: 


Upper  Layer. 

Cms.  per  100  Gms.  of  the  Liquid. 


Lower  Layer. 

Gms.  per  100  Gms.  of  the  Liquid. 


QHjOH. 

C6H,. 

H20. 

C6H6OH. 

CeHs. 

H2O. 

0 

99-95 

0.05 

O 

0.198 

99  .  802 

4-78 

94-98 

O.24 

i-43 

0.21 

98.36 

17.36 

81.83 

0.81 

2.80 

O.2I 

96.99 

21.15 

77.22 

1.63 

3.01 

O.2I 

96.77 

28.01 

69.81 

2.18 

3-35 

0.21 

96.44 

44-39 

50-56 

5-05 

4.07 

O.I9 

95-74 

55-8o 

36-13 

8.07 

4-58 

0.19 

59-23 

74-5 

3 

22.5 

5-65 

0.17 

94.18 

70.70 

0 

29.29 

8.195 

0 

91-805 

Data  for  this  system  are  also  given  by  Rozsa  (1911). 

The  coefficient  of  distribution  of  phenol  between  olive  oil  and  water  at  25°, 
cone,  in  oil  -*-  cone,  in  H2O,  is  given  by  Boeseken  and  Waterman  (1911)  as  greater 
than  9  and  less  than  10.3.  The  figure  was  obtained  by  dividing  the  solubility  of 
phenol  in  olive  oil  by  the  solubility  in  water,  each  being  determined  separately. 
Results  for  this  system  are  also  given  by  Reichel  (1909). 

According  to  Greenish  and  Smith  (1903),  100  cc.  of  olive  oil  dissolve  about  50 
gms.  of  phenol  at  15.5°.  These  authors  report  that  100  cc.  of  glycerol  dissolve 
about  300  gms.  of  phenol  at  15.5°. 


PHENOL 


DISTRIBUTION    OF    PHENOL    BETWEEN   WATER   AND    CARBON   TETRA 

CHLORIDE  AT  20°. 

(Vaubel  —  J.  pr.  Ch.  [2]  67,  4?6,  '03.) 

Grams  Phenol  in: 
Volumes  of  Solvents. 


Gms.  Phenol 
Used. 


50  cc.  H2O+  10  cc.  CC14 

"       '      +     20  CC. 

+  30  cc. 
+  50  cc. 

+  100  CC. 

"        +  1500:. 

"  +200  CC. 


H2O  Layer. 

CCU  Layer. 

0.8605 

0.1285 

0.7990 

O.I9OO 

0.7275 

0.2615 

0-6435 

Q-3455 

0.4680 

0.5210 

0.3645 

0.6245 

0.3240 

0-6650 

DISTRIBUTION  OF  PHENOL  BETWEEN  WATER  AND  ORGANIC  SOLVENTS  AT  25°. 

(Herz  and  Rathmann,  1913-) 

Results  for: 

H2O  and  Tetrachlor 

Ethane. 
Mols.  C6H5OH  per  Liter. 


H,0  -d  Chloroform. 

Mols.  C6H6OH  per  Liter. 


Mols.  C6H5OH  per  Liter. 


H2O  Layer.          CHC13  Layer. 
0-0737                0.254 
0.163                   0.761 
O.2II                   1.27 
0.330                  3-36 

0.436             5-43 

H2O  and  Pentachlor 
Ethane. 

Mols.  C6H5OH  per  Liter. 

H2O  Layer.           CC14  Layer. 
0.0605               0.0247 
O.I4O                 0.072; 
0.213                  O.I4I 

o-355            o-392 
0.489            1.47 
0.525            2.49 

H2O  and  Trichlor 

Ethylene. 
Mols.  C6H5OH  per  Liter. 

H2O  Layer.       C2H2  C14  Layer. 

0.023            0.061 

0.0345              0.094 
O.oSl                 0.265 
O.II4                 0.406 
0.151                 O.6l7 
0.155                 0.651 

H2O  and  Tetrachlor 
Ethylene. 
Mols.  C6H5OH  per  Liter. 

H2O  Layer.          C2HC16  Layer. 

o  .  0420           o  .  0495 
0.0866           o.no 

0.150                  0.226 
O.222                   0.432 
O.28O                  0.708 

0.333             I-I7o 

H20  Layer.      CHC1:CC12  Layer. 

o  .  044            o  .  046 
o.ioi             0.107 
0.180           0.236 
0.236           0.388 

0-277         0.555 
0.339         0-986 

H20  Layer.     CC12:CC12  Layer. 
0.0653            0.0277 
0.143               0.0650 
0.327               0.198 
0.421               0.4II 

o  .  490          o  .  684 

DISTRIBUTION  OF  PHENOL  AT  25°  BETWEEN: 

(Herz  and  Fischer  — Ber.  38,  1143,  '05.) 

Water  and  m  Xylene. 


Water  and  Toluene. 

Millimols  C6H6OH 

Grams  C6H6OH 

per 

10  CC. 

per  100 

cc. 

CflHgCH; 

Layer. 

j        H20 
Layer. 

C6H5CH3 
Layer. 

H26 
Layer. 

1.244 

0.724 

1.169 

0.681 

3-047 

1.469 

2.865 

1.381 

4.667 

2  .200 

4-389 

2.068 

6.446 

2.861 

6.o6l 

2.691 

14.960 

4-750 

14.07 

4.467 

I7-725 

5-346 

16.69 

5.027 

47-003 

7.706 

44-20 

7.246 

8.087 

50.58 

7.604 

90.287 

9.651 

84.89 

9.074 

Millimols 

per  10  cc 


mC6H4(CH3)2 
Layer. 

1.610 

4.787 
I2.2IO 
22.7l8 
34.827 
51.352 
77.703 


H20  ' 
Layer. 

1.071 

2.726 
5.l68 
6.994 
8.124 
9.123 
10.050 


Grams  C6H6OH 
per  zoo  cc. 

H2O' 
Layer. 


Layer. 

I.5I4 
4.501 
11.22 
21.36 

32.75 

48.28 

73-07 


1.007 

2.563 
4-86(5 

6-57? 
7.640 
8.578 
9-45< 


PHENOL  484 

FREEZING-POINT  DATA  (Solubilities,  see  footnote,  p.   i)  ARE  GIVEN  FOR 
MIXTURES  OF  PHENOL  AND  EACH  OF  THE  FOLLOWING  COMPOUNDS: 

Dimethylpyrone.    (Kendall,  igua.)  Bromotoluene.  (Paterno  and  Ampola,  1897.; 

Phenylhydrazine.  (Cuisa  and  Bernardi,  1910.)       0  Toluidine.        (Kremann,  1906.) 
Picric  Acid.  (Philip,  1903;  Kremann,  1904.)  p  Toluidine.        (Kremann,  1906;  Philip,  1903.) 

Picric  Acid +Other  Cm'p'ds.    (Kremann,  '04.)  Urea    (Kremann  &  Rodenis,  1906;  Philip,  1903.) 
Pyridine.  (Bramley,  1916;  Hatcher &Skirrow,  1917.)  Methyl  Urea.  (Kremann,  1910.) 

Quinoline.  (Bramley,  1916.)  as  Dimethyl  Urea. 

Resorcinol.  (Jaeger,  1907.)  s  Dimethyl  Urea. 

Sulfuric  Acid.        (Kendall  and  Carpenter,  1914.)    Urethan.  (Mascarelli  &  Pestalozza,  1908, 1909.) 
Thymol.  (Paterno  and  Ampola,  1897.)       p  Xylene.  (Paterno  and  Ampola,  1897.) 

m  Xylidene.       (Kremann,  1906.) 

PHENOLATE  of  Phenyl  Ammonium. 

SOLUBILITY  IN  WATER. 

(Alexejew,  1886.) 

The  determinations  were  made  by  the  synthetic  method  (see  p.  16).  The  re- 
sults were  plotted  and  the  following  figures  read  from  the  curve: 

Gms.  Phenolate  per  100  Gms.  Gms.  Phenolate  per  100  Gms. 

t°.          t *- <k  t°.  t * N 

Aq.  Layer.   Phenolate  Layer.  Aq.  Layer.        Phenolate  Layer. 

10  3  94  no  9  76 

30  4  93  120  12  69 

50  5  91  130  17.5  60 

70  6  87.5  140  crit.  temp.  40 

90  7  83 

AminoPHENOLS.     See  last  line  p.  138. 

5  TribromoPHENOL  C6H2Br3OH.      . 

Data  for  the  solubility  of  mixtures  of  symmetrical  tribromophenol  and  symmetri- 
cal trichlorophenol  in  diluted  methyl  alcohol  at  25°  are  given  by  Kiister  and  Wiirfel 
(1904-05).  The  results  are  presented  in  terms  which  are  not  clearly  explained. 

SOLUBILITY  OF  MIXTURES  OF  5  TRIBROMO  PHENOL  AND  5  TRICHLORO  PHENOL 
IN  METHYL  ALCOHOL  AT  25°. 

(Thiel,  1903;  from  Wiirfel,  1896.) 

Molecular  per  cent  CeH2.OH.Bra  n  Solubility  of 

'  In  Solid.  In  Solution. "  C«H2.OH.a3.        C6H2.OH.Br3'. 

o  o  0.204  o  0.204 

4.49  3-59  0.194  0.007  0.201 

10.13  7 -58  0.191  0.016  0.206 

16.28  12.15  0.172  0.024  0.196 

62.44          13.07  0.204          0.031  0.235 

69.88  15-86  0.150  0.028  0.178 

81.76  19.01  0.096  0.023  0-118 

84.66  24.05  0.069  O.O22  O.O9I 

87-53  32-46  0.043  0.021  0.063 

93.62  47*87  O-O2I  O.OI9  O.O4O 

loo. o  loo. o  o-o  0.019  0.019 

NitroPHENOLS   C6H4(OH)NO2  o,  m  and  p. 

100  gms.  sat.  solution  in  water  contain  0.208  gm.  o  nitrophenol  at  20°. 

"       2.14  gms.  m 

1.32  p  (Vaubel,  1895.) 

F.-pt.  data  for  mixtures  of  m  nitrophenol  and  water  and  for  p  nitrophenol  and 
water  are  given  by  Bogojawlewsky,  Winogradow,  and  Bogolubow  (1906). 


NitroPHENOLS 


NitroPHENOLS   C6H4(OH).NO2  o,  m  and  p. 
SOLUBILITY  OF  EACH  SEPARATELY  IN  WATER. 

Gms.  per  100  Gms.  Sat.  Sol. 


(Sidgwick,  Spurrell  and  Davies,  1915.) 
Gms.  per  too  Gms.  Sat.  Sol. 


Ortho. 

Meta. 

Para. 

40 

O 

•330* 

3- 

02* 

3- 

28 

100 

50 

*       O 

.388 

3- 

68 

4- 

22 

no 

60 

o 

•463 

4- 

54 

5- 

53 

120 

70 

0 

.560 

5- 

80 

7- 

50 

120 

80 

o 

.685 

7; 

90 

10. 

85 

140 

90 

0 

.856 

II  . 

69 

21. 

2 

150 

92.8 

crit.  t.    , 

,  .  . 

.  . 

OC 

> 

160 

98.7 

crit.  t. 

CO                 ... 

200+ 

Ortho.         Meta.       Para. 
1.078         

i-59        

2-32        

2  . 90  

3-75 
crit.  t.    oo 

*  in  above  table  indicates  that  a  solid  phase  is  present. 

The  above  determinations  were  made  by  the  synthetic  method.  M.  pt.  of  o  = 
44.9°;  of  m  =  95.1°,  of  p  =  113.8°.  Triple  pt.  for  o  =  43.5°  at  cone.  99.48  and 
0.35;  for  m  =  41.5°  at  cone.  74  and  3.16;  for  p  =  39.6°  at  cone.  71.2  and  3.26. 

One  liter  sat.  solution  in  water  contains  3.89  gms.  o  nitrophenol  at  48°. 

One  liter  sat.  solution  in  i.o  n  o  C6H4(ONa)NO2  contains  9.6  gms.  o  nitrophenol 
at  48°.  (Sidgwick,  'io.) 

SOLUBILITY  OF  o  NITROPHENOL  IN  LIQUID  CARBON  DIOXIDE.    (Buchner,  1905-6.) 


Gms.  o  C,H4(OH)NO2 
t°.               per  100  Gms. 
Sat.  Sol. 

-52 

1.9 

-40 

2-5 

—  20 

3-8 

0 

+  10 

5-2 
7-7 

Gms.0C,H4(OH)NO2 

per  100  Gms. 

Sat.  Sol. 


12.5 

14 

15 
16 
20 


io 

21.2 

33-8 
48.5 
60  .  7 

100  gms.  95%  formic  acid  dissolve"!  6.06  gms.  0C6H4(OH)NO2at  20.8°.  (Aschan,  '13.) 
ioogms.95%formicaciddissolve23.44gms.£C6H4(OH)NO2at  18.6°. 
One  liter  of  sat.  solution  of  the  pale  yellow  form  of  p  nitrophenol  in  benzene, 
contains  7.1  gms.     p  C6H4(OH)NO2  at  5°,  determined  by  the  f.-pt.  method. 

(Sidgwick,  1915.) 

SOLUBILITY  OF  THE  THREE  NITROPHENOLS,  SEPARATELY,  IN  TOLUENE, 
BROMOBENZENE  AND  IN  ETHYLENE  DIBROMIDE.     (Sidgwick,  Spurrell  and  Davies.  1915.) 


f° 

Gms.  o  C6H4(OH)NO2  per  100  Gms.  Sat.  Sol.                 Gms.  p  C6H4(OH)NO2  per  100  Gms.Sat.  Sol. 

l> 

In 

C6H5CH3.      In  C6H6Br, 

,       In  C2H4Br2. 

In  C6H5CH3.  In  C6H6Br. 

InC2H4Br2. 

15 

46.9 

40 

70 

18 

•5 

.  . 

. 

31 

20 

55-2          48-8 

47 

,8 

80 

28 

.1 

32 

•7 

52     \ 

25 

64.6          57.7 

56 

.8 

90 

54 

•  4 

59 

•7 

73-2 

30 

74.6          67.2 

67. 

2 

100 

79 

.6 

80 

.6 

88.5 

35 

84-5          78.3 

79 

IIO 

96 

•3 

96 

•3 

98 

40 

93.1          89.7 

9° 

6 

t< 

Gms.  m  C«H4(OH)NO2 
per  loo  Gms.  Sat.  Sol. 

Gms.  m  C6H4(OH)NO2 
t°.         per  loo  Gms.  Sat.  Sol.           t°. 

Gms.  m  C6H4(OH)NO, 
per  loo  Gms.  Sat.  Sol. 

in  C6H5CH3. 

in  C,H6CH3. 

in  C6H6CH3. 

.39 

.6 

4.63 

64.8 

16.44 

78-5 

70 

•50 

45 

.8 

6 

67-7 

2O.26 

82.3 

79 

•57 

48 

•9 

7-03 

71-5 

33-16 

88.8 

91 

•43 

54 

9.II 

74-5 

46.93 

95.1 

IOO 

58 

11.28 

75-7 

57-71 

DiNitro 

PHENOL  C6H6. 

OH.(N02)2. 

100  gms.  abs.  methyl  alcohol  dissolve  6.3  gms.  C6H3.OH.(NO2)2  at  19.5°. 

100  gms.  abs.  ethyl  alcohol  dissolve  3.9  gms.  C6H3.OH.(NO2)2at  19. 5°.  (deBruyn, '92.) 


PHENOLS 


486 


FREEZING-POINT  DATA  (Solubility,  see  footnote,  p.  i)  ARE  GIVEN  FOR  THE 
FOLLOWING  MIXTURES  CONTAINING  SUBSTITUTED  PHENOLS. 


o  Bromophenol  +  p  Bromophenol. 

o  Chlorophenol  4-  P  Chlorophenol. 

o  lodophenol  +  p  lodophenol. 

5  Tribromophenol  +  s  Trichlorophenol. 

2.4.6  Tribromophenol  +  Acetyl  tribromophenol. 

o  Chlorophenol  +  Quinoline. 

+  Pyridine. 

o  Nitrophenol  +  Acetyl  o  Nitrophenol. 
o  Nitrophenol  +  a  Dinitrophenol. 

+  p  Toluidine. 

p  Nitrophenol  +  p  Nitrosophenol. 
Each  of  o,  m  and  p  Nitrophenol  +  Dimethylpyrone. 

+  Picric  Acid. 

+  Sulfuric  Acid. 

+  Urea. 

2.4  Dinitrophenol  +  Dimethylpyrone. 
PHENOLPHTHALEIN   (Ce^OH^CO.CeKUCO. 
loogms.  H2O  dissolve    0.0175  gm.  phenol phthalein  at  20°. 

(Acree  and  Slagle,  1909.) 

0.04  at 20-25°.    (Dehn.'i?.) 

"      Pyridine  "      796.         gms. 

"      aq.  50%  pyridine      "      300 
PHENYL  ALANINE  «  C6H6NHCH(CH3)COOH. 

Data  for  the  solubility  of  phenyl  alanine  in  aqueous  salt  solutions  at  20°  are 
given  by  Wiirgler  (1914)  and  Pfeiffer  and  Wurgler  (1916). 
PHENYLENE   DIAMINES   o,  m,  and  p.     C6H4(NH2)2. 

SOLUBILITY  IN  WATER  AT  20°.     (Vaubel,  1895.) 

100  cc.  sat.  solution  contain  23.8  gms.  w'CeH^NI^,  d20  of  sat.  sol.  =  1.0317. 
loo  cc.  sat.  solution  contain    3.7  gms.  p  C6H4(NH2)2,  d20  of  sat.  sol.  =  1.0038. 
RATIO  OF  DISTRIBUTION  BETWEEN  WATER  AND  BENZENE  AT  25°. 

(Farmer  and  Warth,  1904.) 


(Holleman  and  Rinkes,  1911.) 


(Kiister  and  Wiirfel,  1904-05.) 
(Boeseken,  1912.) 
(Bramley,  1916.) 

(Boeseken,  1912.) 

(Crompton  and  Whitely,  1895.) 

(Pawlewski,  1893;  Philip,  1903.) 

(Jaeger,  1908.) 

(Kendall,  i<ji4a.) 

(Kremann  and  Rodenis,  1906.) 

(Kendall  and  Carpenter,  1914.) 

(Kremann  and  Rodenis,  1906.) 

(Kendall,  iyi4a.) 


Results  for  o  Phenylene  Diamine. 

conc.  C8Hg 
conc.  H2O 


Results  for  m  Phenylene  Diamine. 


Gms.  o 


>  Ratio 


Gms.  m  C6H4(NH!1)2  per: 


Ratio 


conc.  C«H« 


50  cc.  C«H«.        1000  cc.  H2O.  50  cc.  C6H«.         1000  cc.  H2O. 

0.0273  0.9818  0.556  0.0828  9.088 

0.2040  7-5470  0.541  0.0463  5.260 

PHENYL  HYDRAZINE   C6H6NH.NH2. 

RECIPROCAL  SOLUBILITY  OF  PHENYLHYDRAZINE  AND  WATER,  DETERMINED 
BY  THE  FREEZING-POINT  METHOD.    (Bianksma,  1910.) 


Gms. 

to       C,H6NH.NH2        Soli,  p,e 

per  100  Gms. 

*  - 

Sat.  Sol. 

O               O         Ice 

19.8 

0.3          2.2      " 

20.4 

0.6       3.9    " 

21.8 

0.7          4.6     "  +C«H6NH.NH2.JH2O 

23 

I               4.7       C,HsNH.NH2.iH20 

24.2 

7        6 

26.1 

ii.  6       7 

26.2 

15           8 

25-7 

16.8       9.6 

23-2 

19.6     10.9               " 

i7 

16.6 

Gms. 

QH6NH.NH2 
per  loo  Gms. 

Sat.  Sol. 

60 


Solid  Phase. 


64 
75 
79 
83 


1  C,H6NH.NH,.iH,O 

2  " 

2      " 

7      " 


92-3 

93-7 
97-2 
98.8 

99 


+C6H8NH.NH, 
C6H6NH.NH2 


19.6  m.  pt.  ioo  .  . 

Between  the  concentrations  10.9  and  60. i,  two  liquid  layers  are  formed.     See 
p.  487. 


487  PHENYL  HYDRAZINE 

RECIPROCAL  SOLUBILITY  OF  PHENYL  HYDRAZINE  AND  WATER.  (Con.) 

The  temperatures  of  separation  into  two  liquid  layers  of  mixtures  containing 
from  10.9  to  60  per  cent  C6H6NH.NH2,  are: 

toof         Cms.  C6H5NH.NH2  t«,  Of          Gms^C.HjNH.NH,       t,  Qj         Cms.  C6H5NH.NH2 

19.8  ii. 6          54.6  29.7  50.6  48.9 

34  I3-8  55-1  31-4  50  5!-2 

45  l6-5  55-a.cnt.-t  33-6  46  53-5 

49-4  18.7  55.2  36.9  44.2  54.7 

52.4  21.9  55  39-3  39-6  56.7 

54  25.2  54  41-7  24  59.5 

54.4  28.3  52.6  46  19.8  60.  i 

Additional  data  for  concentrations  of  CeHsNH.NH-j  above  60  per  cent,  are  given 
by  Oddo  (1913)- 

Benzoyl  PHENYL  HYDRAZINE  C6H6NH.NHC7H5O. 

SOLUBILITY  IN  AQUEOUS  ALCOHOL  AT  25°. 

(Holleman  and  Ajitusch,  1894.) 
Cms.  Hydrazine       cn  p-  Vnl   %         Cms.  Hydrazin* 


ico  2.39          0.793  8o  J-59          0.859 

95  2.43          0.814  70  i.  08          0.884 

93  3  °-822  55  0.51          0.917 

90  2.26          0.831  40  0.16          0.946 

The  above  results  give  an  irregular  curve.     See  remarks  under  a  acetnaph- 

thalide,  p.  13. 

XCOV  H 

Phthalyl  PHENYL  HYDRAZIDE  C6H4<        >N.N< 

CO  CeHfi. 

CO^  CH3 

Phthalyl  PHENYL   Methyl  HYDRAZIDE   C6H4<        >  N.N  ( 

^CO'          ^  C6H5. 

Very  careful  determinations  of  the  solubilities  of  the  enantrotropic  forms  of 
these  two  compounds  in  alcohol,  chloroform,  ethyl  acetate,  acetone,  benzene  and 
in  methyl  alcohol  are  given  by  Chattaway  and  Lambert  (1915).  See  also  p.  312. 

Acetone  PHENYL  HYDRAZONE   (CH3)2C.N2HC6H5. 

DATA  FOR  THE  SYSTEM  ACETONE  PHENYL  HYDRAZONE  -f-  WATER  ARE  GIVEN 
BY  BLANKSMA  (1912). 

The  following  results  were  obtained  for  the  solubility  of  (CHs^C. 
in  water. 


t°. 

Cms.  (CH3)2C.N2.HC,HS 
pet  loo  cc.  Solution. 

Solid  Phase. 

0 

0.090 

(CHa)2C.N2  HCeHB.HjO 

15 

0.187 

« 

32.8 

0.412    x 

" 

DibromoPHENYL  SELENIDE  and  TELLURIDE  (Ce 

Data  for  the  solubility  of  mixtures  of  dibromophenyl  selenide  and  dibromo- 
phenyl  telluride  in  benzene  at  21°  are  given  by  Pellini  (1906). 

PHLOROGLTTCINOL   1.2.3  C6H3(OH)3.2H2O. 

ioogms.H2O  dissolve     i.i3gms.phloroglucinolat2O-25°.  (Dehn,  '17.) 

"      pyridine  "       296 

"      aq.  50%  pyridine      "       134 


PHOSPHO  MOLYBDIC  ACID        488 

PHOSPHO  MOLYBDIC   ACID   P2O5.2oMoO3.52H2O. 

SOLUBILITY  IN  ETHER.    (Parmentier,  1887.) 

t°.  o°.  8.1°.         19.3°. 

Cms.  Acid  per  100  gms.  Ether          80 . 6    84 . 7     96 . 7 

PHOSPHORUS   P.  (yellow) 

SOLUBILITY  IN  BENZENE. 

(Christomanos  —  Z.  anorg.  Ch.  45,  136,  ^55.) 


«.o         Gms.  P  per    Sp.  Gr.  of 
*    100  Gms.  C6He.  Solution. 

AO        Gms.  P  per     Sp.  Gr.  of 
'    jooGms.CeHe.    Solution. 

0 

1-5*3 

.  .  . 

23 

3-399 

0.8875 

5 

1.99 

.  .  . 

25 

3-7o 

0.8861 

8 

2.31 

0.8990 

30 

4.60 

10 

2.4 

0.8985 

35 

5-17 

15 

2.7 

0.894 

40 

5-75 

18 

3-i 

0.892 

45 

6.  ii 

20 

3-2 

0.890 

27-4- 
103.9 


32.9°. 
107.9 


Gmi.  P 
100  Gms. 


50 

55 
60 

65 

70 

75 
81 


6.80 

7.32 
7.90 
8-40 
8.90 
9.40 
10.03 


SOLUBILITY  OF  PHOSPHORUS  IN  ETHER. 


10 


(Christomanos.) 

Gms.  P  per 
100  Gms. 
(C2H6)20. 

Sp.  Gr.  of 
Solutions. 

Gms.  P   per  c      f       t 

f.    -a-.;  <&$£ 

Gms.  P  per 
t  °.      zoo  Gms. 
(C2H6)20. 

0-434 

15 

0.90 

0.723 

28 

i  .60 

O.62 

.  .  . 

18 

I  -OI 

0.719 

30 

i  .75 

0.79 

0.732 

20 

1.04 

0.718 

33 

i.  80 

0.85 

0.729 

23 

1.  12 

0.722 

35 

2.00 

25 

i-39 

0.728 

SOLUBILITY  OF  YELLOW  PHOSPHORUS  IN  SEVERAL  SOLVENTS  AT  15°. 

(Stich,  1903.) 

Gms.  P  per 
Solut 


Solvent. 


er  100  Gms. 
lution. 


Almond  Oil  1.25 

Oleic  Acid  i .  06 

Paraffin  1.45 

Water  o .  0003 

Acetic  Acid  (96%)  o .  105 

SOLUBILITY  OF  PHOSPHORUS  IN  CARBON  DISULFIDE. 

(Cohn  and  Inouye,  1910.) 


—  IO 

-7-5 
-5 


Gms.  P 

per  100  Gms. 

Sat.  Sol. 

31.40 
35.85 
41-95 


-3-5 
-3.2 
-2-5 


Gms.  P 

per  100  Gms. 

Sat.  Sol. 

66.14 

71.72 

75 


o 
+5 

IO 


Gms.  P 

per  TOO  Gms. 
Sat.  Sol. 

8l.27 

86.3 

89.8 


The  above  determinations  were  made  with  very  great  care.     The  authors  show 
that  the  previous  determinations  of  Giran  (1903)  are  inaccurate. 

loogms.  alcohol  (d  =  0.799)  dissolve 0.312  gm.  P,  cold,  and  0.416  gm.,  hot.  (Buchner ) 
100  gms.  glycerol  (d^  =  1.256)  dissolve 0.25  gms.  Pat  15-16°.    (Ossendowski,  1907.) 
Red  phosphorus  is  completely  insoluble  in  turpentine  even  up  to  270°  provided 
the  determination  is  made  without  access  of  air  (sealed  tube).     If  air  is  not  ex- 
cluded a  portion  of  the  red  phosphorus  may  be  converted  to  yellow  phosphorus 
which  would  dissolve.  (Colson,  1907.) 


489 


PHOSPHORUS 


RECIPROCAL  SOLUBILITY  OF  PHOSPHORUS  AND  SULFUR,  DETERMINED  BY 
THE  SYNTHETIC  (Sealed  Tube)  METHOD. 

(Giran,  1906.) 

(Mixtures  of  P  and  S  were  sealed  in  small  tubes  and  first  heated  to  about  200° 
to  cause  combination.  They  were  then  cooled  to  the  solidification  point  and 
gradually  heated  to  the  temperature  at  which  the  last  crystal  disappeared.  The 
following  results,  which  were  read  from  the  diagram,  show  the  eutectics  and 
maxima  of  the  curves.) 


Eutectics. 


t°. 

Mols.  %  S  in 
Mixture. 

Selid  Phase. 

-40 

33-5 

P4S3+P2 

+46 

50 

P4S3+P2S3 

230 

67-5 

P2S3+P2S6 

243 

75 

P2S6+PS6 

Maxima  of  Curves. 

«••  MMixt?reSiQ      Solid  Phase. 

+  167  43.6 

296 


60.8 


272 
314 


72.1 

86.1 


P2S3 
P2S5 

PS, 


Additional  data  for  this  system  are  given  by  Boulouch  (1902  and  1906)  and  by 
Helff,  1893. 

PHOSPHORUS   SULFIDES   P4S3,  P4S7,  P4Si0. 

SOLUBILITY  IN  CARBON  DISULFIDE,  BENZENE,  AND  IN  TOLUENE. 


(Stock,  1910.) 


Cms.  P4S3  per  100  Cms.: 


ll  . 

€82. 

CeHs. 

C6H6Cn3. 

—  20 

II  .1 

0 

+17 

80 

27 

100 

2-5 
II.  I 

3-125 

no 

15-4 

Cms.  P4S7_per  100    Cms.  PjS10  per 
Gms.  €82. 


Cms.  CSj. 


0.005 
0.0286 


0.083 
0.182 
0.223 


PHOSPHORIC  ACID    (ortho)   H3PO4. 
SOLUBILITY  IN  WATER. 


(The  sat.  solutions  were  analyzed  by  titration. 
stirred  for  at  least  two  hours.) 


(Smith  and  Menzies,  1909.) 

The  mixtures  were  constantly 


Gms.  H3PO4 

t°.        per  too  Gms.           Solid  Phase. 

Sat.  Sol. 

-81* 

62.9 

Ice+2HsPO4.H2O 

-16.3 

76.7 

aH«PO4.HjO 

+  o-5 

78.7 

" 

14-95. 

81.7 

" 

24.03 

85-7 

" 

27 

87.7 

" 

29-15 

9°-5 

" 

29-35! 

91.6 

" 

28.5 

92-S 

" 

27 

93-4 

" 

25-4 

94.1 

" 

23-5* 

.  .   . 

"  +ioH3PO4.H2O 

24.11 

94.78 

ioH3PO4.H2O 

Gms.  H3PO4 

t°.        per  100  Gms. 

Solid  Ph 

Sat.  Sol. 

24.38         94.80 

ioH8PO4.H2O 

24.40         94.84 

" 

24.81      -94-95 

a 

25.41         95.26 

« 

25-85         95.54 

" 

26.2* 

« 

26  .  23      95  .  90 

H.PC 

27.02      95.98 

K 

29.42      96.15 

M 

29.77      96.11 

" 

37.65      97.80 

" 

39.35      98.48 

« 

42.30!  100 

« 

+H3P04 


*  Eutec.  t  M.  pt. 

NOTE.  —  The  results  of  Giran  (1908),  determined  by  the  freezing-point  method, 
are  shown  to  be  erroneous,  due  to  supercooling  which  would  result  from  failure  to 
induce  crystallization  by  inoculation. 

F.-pt.  data  for  mixtures  of  phosphoric  and  phosphorus  acids  are  given  by  Rosen- 
hejm,  Stadler  and  Jakobsohn  (1906). 


ns.  H4PA  per  ico 
Gms.  Sat.  Sol. 

Solid  Phase. 

59 
86.8 

Ice  +H4PA.i^H20 

88.8 

+H4PA 

100 

IL.PA 

PHOSPHORIC  ACID  490 

PyroPHOSPHORIC  ACID   H4P2O7. 

SOLUBILITY  IN  WATER.      (Giran,  1908;  see  note  on  preceding  page.) 
t°. 

-75 

+26  m.  pt. 

23 

61  m.  pt. 

HypoPHOSPHORIC  ACID   H2PO3.H2O. 

100  gms.  sat.  solution  in  water  contain  81.8  gms.  H2PO3  at  the  m.  pt.,  62°,  of 
the  hydrated  compound,  t^POa.HgO.  (Rosenheim  and  Pritze,  1908.) 

PHTHALIC  ACIDS   C6H4(COOH)2,   o,  m  and  p. 

SOLUBILITY  OF  EACH  IN  WATER.     (Vaubel,  1895,  1899.) 

Acid.  t°.  Gms.  per  100  Gms.  Solution. 

o  Phthalic  Acid  14  o  .  54 

m  =  Isophthalic  Acid  25  0.013 

p  =  Terephthalic  Acid  .  .  .  almost  insoluble 

MELTING  TEMPERATURES  OF  MIXTURES  OF  o  PHTHALIC  ACID  AND  WATER. 

(Flaschner  and  Rankin,  1910.) 

(The  determinations  were  made  by  the  sealed  tube  method  of  Alexejew.) 
Wt.  %Acid  14.4      28.2        39.6        49.3        75      100 

Saturation  Temp.  97°       111.5°     121.2°     130°         162°     231° 

Unstable  boundary  ...         ...  ...         27°          84° 

SOLUBILITY  OF  o  PHTHALIC  ACID  IN  ALCOHOL  AND  IN  ETHER  AT  15°. 

(Bourgoin,  1878.) 

Gms.  C6H4(COOH)2  o  per  100  Gms. 


Solution. 

Solvent. 

Absolute  Alcohol 

9.156 

II  .70 

90  per  cent  Alcohol 

10.478 

IO.O8 

Ether 

0.679 

0.684 

SOLUBILITY  OF  o  PHTHALIC  ACID 

IN  ALCOHOLS.     (Timofeiew,  1894.) 

Gms.  o 

Gms.  o 

Alcohol                       t°          CeH4(COOH)j 

Alcohol. 

to        C6H4(COOH)2 

per  100  Gms. 

per  100  Gms. 

Sat.  Sol. 

Sat.  Sol. 

Methyl  Alcohol    —2          15.1 

Ethyl  Alcohol 

21.4       11.65 

+  19          19.5 

Propyl  Alcohol 

-  3          3-42 

+  21.4      20.4 

«                 « 

+  19          5.27 

Ethyl  Alcohol       -2            8.2 

((                (( 

22               5-54 

+  19          ii 

(i                a 

23               5-70 

DISTRIBUTION  OF  o  PHTHALIC  ACID  AND  OF  m  PHTHALIC  ACID  (ISOPHTHALIC) 
BETWEEN  WATER  AND  ETHER  AT  25°.     (Chandler,  1908.) 

Results  for  o  Phthalic  Acid.  Results  for  m  Phthalic  Acid. 

Mols.  o  C,H4(COOH)2  Ratio  for       Mols.  m  C6H4(COOH)2  Ratio  for 

I**  Liter:  ?-       U°n-  Per  L*er:  U' 


Ratio-  £°n-                    Per  ao- 

HtO  Layer,  a.  Ether  Layer,  6.  Acid.  H2O  Layer,  a.  Ether  LayerA  Acid. 

0.0261          0.0322         0.809  0.637  0.000398       0.0485  0.0821  0.0359 

0.0131          0.0150         0.873  0.645  0.000272       0.0288  0.0943  0.0352 

0.0085          0.0091          0.932  0.667  0.000263       0.0279  0.0944  0.0350 

0.0056          0.0056          I.  006  0.635  0.000252       0.0266  0.0949  0.0341 
Ratio  of  solubilities  of  Phthalic  acids  in  olive  oil  and  water  at  25°. 

(Boeseken  and  Waterman,  1911,  1912.) 

o  Phthalic  acid,  solubility  in  oil  -s-  solubility  in  H2O  =  o.oi. 
p  Phthalic  acid  (Terephthalic),  solubility  in  oil  4-  solubility  in  H2O  =  9.52. 
loo  gms.  95%  formic  acid  dissolve  0.55  gm.  p  phthalic  acid  (Terephthalic)  at 

20.2°.  CAschan,  1913.) 


491  PHTHALIC  ACIDS 

NitroPHTHALIC   ACIDS   o  and  m  (Iso)   C6H3(NO2)(COOH)2. 

SOLUBILITY  OF  THE  SEVERAL  NITRO  PHTHALIC  ACIDS  itf  WATER  AT  25°. 

(Holleman  and  Huisinga,  1908.) 

Gms.  Acid 

Acid.  M.  pt.  per  100  Gms. 

Sat.  Solution. 

a.  Nitro  Ortho  Phthalic  Acid  220  2 .048 

8      "  164-166  very  soluble 

Symmetrical  Nitro  Iso  Phthalic  Acid  (anhy.)       255-256          0.220 

"    (hydrated)  255-256          0.157 

Asymmetrical    "  "  "  245  0.967 

Vicinal  300  0.216 

The  authors  also  give  several  tables  showing  the  solubility  of  one  of  the  above 
compounds  in  aqueous  solutions  of  another.  These  data  are  .made  the  basis  of 
an  ingenious  solubility  method  for  determining  the  composition  of  unknown 
mixtures  of  these  compounds. 

PHTHALIC  ANHYDRIDE   C6H4<£g>O. 

SOLUBILITY  IN  WATER. 

(van  der  Stadt,  1902.) 

All  determinations,  except  first  three,  made  by  the  Synthetic  Method.  See 
p.  16. 


Gms.  C8H4O3  per  100  Gms. 

Mol.  per  cent           to 
C8HA.               *  • 

Gms.  C8H4O3  per 
100  Gms 

Mol. 
percent 
C8H40,. 

Water. 

Solution. 

Water. 

Solution. 

0 

O 

.00295 

O.OO295 

o 

.00036 

189 

•5 

1076 

91 

.66 

56.73 

25 

0 

.6194 

0.6150 

0 

•P754 

188 

.8 

1265 

92 

.68 

60.63 

50 

I 

.630 

1.604 

o 

.198 

187 

.1 

1474 

93 

-65 

64.22 

135-9 

94 

-3 

48.54 

10 

•30 

181 

.8 

2332 

95 

.88 

73-95 

165.4 

210 

67.75 

20 

-36 

176 

.2 

3334 

97 

.07 

80.23 

179.4 

319 

•3 

76.13 

27 

.98 

169 

-4 

5745 

98 

.28 

87.49 

186.2 

449 

.6 

81.81 

35-37 

130 

•9 

37570 

99 

.72 

97.89 

189.6 

546 

.1 

84.50 

39 

•93 

83010 

99 

.86 

99.02 

191 

821 

•5 

89.19 

5o 

131 

.2 

00 

100 

IOO 

190.4 

863 

•4 

89.62 

51 

.24 

SOLUBILITY  OF  PHTHALIC  ANHYDRIDE  IN  CARBON  BISULFIDE. 

(Arctowski,  1895;  Etard,  1894.) 

Gms. 

t°.  per  loo  Gms. 

Solution. 

70       2.3 

90     3-7 
loo     5 
120     8 

140  13-3 
160  20.7 
180  30.2 

100  gms.  95%  formic  acid  dissolve  4.67  gms.  phthalic  anhydride  at  19.8°. 

(Aschan,  1913.) 
loo  gms.  pyridine  dissolve  83.5  gms.  phthalic  anhydride  at  20-25°.    (Dehn,  1917.) 


r. 

Gms.  C8H4O3 
per  loo  Gms. 
Solution. 

f. 

per  100  Gms. 
Solution. 

-112.5 

0.013 

+  10 

0.3 

-93 

-77-5 

0.013 

0.016 

20 
30 

0.7 

0.8 

-40 

—  20 

—  10 

0.03 
0.06 

O.IO 

40 
50 
60 

1.2 

0 

0.20 

PHTHALIMIDE  492 

PHTHALIMIDE   o  C6H4  <  (CO)2  >  NH. 

100  gms.  H2O  dissolve    0.06  gm.    phthalimide  at  20-25°.  (Dehn,  1917.) 

"        pyridine  "       14.15  gms.  " 

"        aq.  50%  pyridine  7-74 

PHTHALONIC  ACID   COOH.C6H4.CO.COOH.2H2O. 

100  gms.  sat.  solution  in  water  contain'64.4  gms.  anhydrous  acid  at  15°,  Sp.  Gr. 
of  sat.  solution  =  1.243.  (Tcherniac,  1916.) 

Amide  of  PHTHALIDECARBOXYLIC  ACID  C6H4<SS(CONH2)  >O  (m.  pt. 

185.5°). 

100  gms.  H2O  dissolve  0.132  gm.  of  the  acid  at  16.2°  and  5.7  gms.  at  b.  pt. 

(Tcherniac,  1916.) 

PHYSOSTIGMINE    (Eserine)    Ci5H21N3O2. 

Water  dissolves  only  traces  of  physostigmine.  ipo  gms.  of  a  solvent  composed 
of  3  gms.  H3BO3  per  100  cc.  of  aq.  50%  glycerol  dissolve  2.5  gms.  Ci5H2iN3O2  at 
room  temp.  (Baroni  and  Borlinetto,  1911.) 

PHYSOSTIGMINE   SALICYLATE   C6H4(OH)COOH.Ci6H21N3O2  and   Physo- 
stigmine Sulfate  H2SO4(Ci5H2iN3O2)2. 

SOLUBILITY  OF  EACH  IN  WATER,  ALCOHOL,  ETC. 

(U.  S.  P.  VIII.) 


Salicylate. 

Sulfate. 

Water 

25                  I-38 

very  soluble 

Water 

80            6.66 

u 

Alcohol 

25            7-87 

(( 

Alcohol 

60          25 

{( 

Chloroform 

25          ii.  6 

(( 

Ether 

25            0.57 

0.083 

Methylphenyl  PICRAMIDES. 

SOLUBILITY 

IN  ETHYL  ALCOHOL 

AT   18°. 

(Hantzsch,  1911.) 

100  cc.  C2H6OH  dissolve  0.32  gm.  of  the  isomer  melting  at  108°. 
100  cc.  C2H6OH  dissolve  0.42  gm.  of  the  isomer  melting  at  128°. 

PICRIC  ACID  C6H2.OH.(NO2)3  1.2.4.6. 

SOLUBILITY  IN  WATER. 

(Dolinski  —  Ber.  38,  1836,  '05;  Findlay  — J.  Ch.  Soc.  81,  1219,  'oa.) 
Gms.  CeHsNsO?  per  100  Grams  Gms.  CeHsNaO?  per  100  Grams 


Solution. 

Water. 

Solution. 

Water. 

0 

0.67    (D.)      0 

.68  (D.)  I 

.05  (F.) 

60 

2 

•  77  (D.)       2.8l(D. 

)  3-i7(F.) 

10 

.80 

o 

.81 

I 

.10 

70 

3 

•35 

3 

•47 

3-89 

20 

1.  10 

I 

.11 

I 

.22 

80 

4 

.22 

4 

.41 

4.66 

30 

1.38 

I 

•  40 

I 

•55 

90 

5 

•44 

5 

.72 

5-49 

40 

I 

.78 

I 

.98 

IOO 

6 

•75 

7 

.24 

6-33 

50 

2.15 

2 

.19 

2 

•53 

.  Dolinski  does  not  refer  to  the  previous  determinations  of  Findlay. 
loo  gms.  H2O  dissolve  1.525  gms.  C6H2.OH.(NO2)3  at  30°  and  1.868  gms.  at  40°. 

(Karplus,  1907.) 

loo  gms.  H2O  dissolve  1.45  gms.  C6H2.OH.(NO2)3  at  20°.  (Sisley,  1902.) 

loo  gms  H2O  containing  5  gms.  H2SO4  per  liter,  dissolve  0.61  gm.  C6H2OH(NO2)3 
at  20°.  (Sisley,  1902.) 

loo  gms.  ethyl  alcohol  dissolve  8.37  gms.  C6H2OH(NO2)3  at  22°.   (Timofeiew,  1894-) 
loo  gms.  methyl  alcohol  dissolve  22.5  gms.  C6H2OH(NO2)3  at  22°. 
loo  gms.  propyl  alcohol  dissolve  3.81  gms.  C6H2OH(NO2)3  at  22°. 
loo  gms.  95%  formic  acid  dissolve  io.83gms.  C6H2OH(NO2)3at  19.8°.  (Aschan,  1913.) 


493 


PICRIC  ACID 


SOLUBILITY  OF  PICRIC  ACID  IN  WATER  AND  IN  AQUEOUS  SALT 
SOLUTIONS  AT  25°. 

(Levin  —  Z.  physik.  Ch.  55,  520,  '06.) 

One  liter  of  aqueous  solution  contains  0.05328  gram  mols.  =  12.20 
grams  C6H2.OH(NO2)3  at  25°. 

Gm  Mols  Salt  Gram  Mols.  Picric  Acid  per  Liter  in  Aq.  Solutions  of: 


per 

Liter. 

'NaCl. 

NaNO3. 

Na2SO4. 

LiCl. 

Li2S04. 

NIL^Cl. 

0 

.01 

0 

•05524 

0.05529 

0-05604 

0.05480 

O 

.05661 

0.05487 

O 

•  O2 

o 

•05559 

0-05872 

0.05872 

0-05558 

0 

.06053 

0.05540 

0 

•05 

o 

.05729 

0.06632 

0.06632 

0.05703 

0 

.06691 

0.05771 

0 

.07 

0 

.05862 

6.07093 

0.07093 

0.05878 

o 

.07013 

0.05865 

O 

.10 

0 

.05902 

0.07670 

0-07670 

0.06132 

o 

•07437 

O 

•50 

o 

.0790 

0 

.123 

I 

.00 

o 

.Il8o 

... 

0 

.149 

Gm. 

,  Mols. 

Grams  Picric  Acid  per 

Liter  in  Aq.  Solutions  of: 

Salt  per  Liter. 

NaCl. 

NaNO3. 

Na2S04. 

;        uci. 

Li2S04. 

NH«C1. 

O 

.01 

12.66 

12.67 

12.83 

12  .55 

12-97 

12-57 

O 

•  O2 

12.74 

13-45 

13-45 

12-74 

I3-87 

12.69 

0 

•05 

13.12 

13.06 

15-33 

13.22 

O 

.07 

13-43 

16.25 

16.25 

13-47 

16.06 

13-44 

O 

.10 

13-52 

17-57 

17-57 

14.05 

17.04 

0 

•50 

18.09 

28.18 

I 

.00 

26.98 

• 

34-14 

Solubility  in  Aq.  Cane  Sugar. 


Solubility  in  Aq.  Grape  Sugar. 


Gm.  Mols. 
Sugar 
per  Liter. 

Picric  Ac.  per  Liter  Solution. 

Sp.  Gr. 

Solution. 

Gm.  Mols. 
Grape  Sugar 
per  Liter. 

Picric  Acid 

£er  Liter  Sol. 

Gm.  Mols. 

Cms. 

G.  Mols. 

Gms. 

O-IO 

0.05202 

II  .92 

I  .OI22 

O.IO 

0.0530 

12.14 

0.25 

0.04978 

11.40 

I.03I9 

0.25 

0.0521 

"•93 

0.50 

0.0482 

II  .04 

I  .0654 

0.50 

0-0509 

11.66 

1.  00 

0.0443 

IO.I5 

I.I294 

I  .OO 

0-0474 

10.86 

SOLUBILITY  OF  PICRIC  ACID  IN  ABSOLUTE  ALCOHOL. 

(Behrend  —  Z.  physik:  Ch.  10,  265,  '92.) 

TOO  gms.  sat.  solution  contain  5.53    grams  CeHgNgOj  at  12.3°,   and 
5.92  grams  at  14.8°.     Sp.  Gr.  of  the  latter  solution  =  0.8255. 

SOLUBILITY  OF  PICRIC  ACID  IN  BENZENE. 


(Findky.) 


Gms. 

Mols. 

t*. 

C6H3N307 

C6H3N3O 

per  100 
Gms.C6H6. 

per  100 
Mols.CsE 

5 

3-70 

1.26 

10 

5-37 

I  .83 

'5 

7-29 

2.48 

20 

9.56 

3-25 

25 

12.66 

4-30 

26.5 

13  -51 

4.60 

35 

21.38 

7.26 

Gms. 


Mols. 


per  100          per  100 
Gms.CeHe.    Mols.  ~  " 


38.4 

26.15 

8.88 

45 

33-57 

ii  .40 

55 

50-65 

17.21 

58.7 

58-42 

19.83 

65 

71  .31 

24.20 

75 

96.77 

32.92 

PICRIC  ACID  494 

SOLUBILITY  OF  PICRIC  ACID  IN  AQUEOUS  SOLUTIONS  OF  HYDROCHLORIC 

ACID  AT  25°. 

(Stepanow,  1910.) 

(The  solutions  were  saturated  by  constant  agitation  at  constant  temperature. 
The  picric  acid  in  the  saturated  solutions  was  determined  by  evaporation  and 
weighing.  The  solubility  passes  through  a  minimum.) 


Mols.  HC1 

C6H2.OH.(] 

\Oz)s  per  Liter. 

Mols.  HC1 

C6H2.OH.(N02)3 

per  Liter. 

per  Liter. 

Mols. 

Cms. 

per  Liter. 

Mols. 

Cms. 

0.25 

0.0116 

2.66 

3^7 

0.0068 

i-SS 

0.50 

0.0079 

i.  80 

4.40 

0.0082 

1.87 

o-7S 

0.0062 

1.42 

5-H 

o  .  0098 

2.26 

i 

0.0054 

1.24 

5-51 

O.OIO5 

2.41 

1.47 

0.0050 

1.14 

5-87 

O.OII5 

2.65 

2.20 

0.0051 

i-i5 

6.24 

0.0123 

2.82 

2.94 

0.0057 

i-3i 

6.61 

O.OI25 

2.86 

SOLUBILITY  OF  PICRIC  ACID  IN  ETHER. 

(Bougault,  1903.) 
Solvent.  t°.        Cms.  CeHjNsOr  per  Liter' 

Ether  of  Sp.  Gr.  0.721  13  10.8        (B.) 

Ether  of  Sp.  Gr.  0.725  (0.8  pt.H2O  per  100)  13  36 .8 

Ether  of  Sp.  Gr.  0.726  (i  pt.  H2O  per  100)  13  40 

Ether  saturated  with  H2O  15  51 .2 

H2O  saturated  with  Ether  15  13.8 

100  parts  of  ether  dissolve  about  2.27  gms.  picric  acid  at  15°.       (S.  1905.) 

chloroform  2 

"        petroleum  ether  0.04    ' 

loo  gms.  sat.  solution  in  pure  ether  contain  5  gms.  picric  acid  at  20°.  (Sisley,  1902.) 
100  cc.  sat.  solution  in  pure  ether  contain  3.7  gms.  picric  acid  at  20°. 
100  gms.  sat.  solution  in  pure  toluene  contain  12  gms.  picric  acid  at  20°. 
100  cc.  sat.  solution  in  pure  toluene  contain  10.28  gms.  picric  acid  at  20°.     " 
100  cc.  sat.  solution  in  pure  amy  1  alcohol  contain  i  .755  gms.  picric  acid  at  20°.    " 

DISTRIBUTION  OF  PICRIC  ACID  AT  25°  BETWEEN: 
Water  and  Amyl  Alcohol.  Water  and.  Toluene, 

(Herz  and  Fischer  —  Ber.  37,  4747.  '04.)  (H.  and  F.  —  Ber.  38,  1142,  '05.) 


Millimols  CeHjjNsOr 
per  10  cc. 

Gms.  CeHaNgOy 
per  100  cc. 

Millimols  CeHgNaOy 
per  10  cc. 

Gms.  QHgNaOr 
per  100  cc. 

Aq. 

Alcohol  " 

Aq. 

Alcohol 

*      Aq. 

Toluene 

Aq. 

Toluene 

Layer. 

Layer. 

Layer. 

Layer. 

Layer. 

Layer. 

Layer. 

Layer. 

0-0553 

0.0930 

0.127 

0.213 

0.075 

0.126 

0.172 

0-289 

0.0920 

0.1850 

O.2II 

0.424 

O.IO9 

0.230 

0.250 

0.527 

O.l6l3 

0.4127 

0.369 

0.946 

0.163 

0.482 

o-374 

I  .IO4 

0.1869 

0.5182 

0-428 

I.I88 

0.244 

I  .026 

o-559 

2-351 

0.3l6l 

1.079 

0.724 

2-473 

0.389 

2-347 

0.891 

5-38o 

0.4471 

1.638 

I  .024 

3-753 

0.496 

3-747 

i-i37 

8.586 

0.5624 

2.189 

1.288 

5-oi7 

0.583 

5-135 

I-336 

11.770 

0.6423 

2-549 

1.472 

5-839 

Additional  data  for  the  distribution  of  picric  acid  between  water  and  amyl 
alcohol  and  water  and  toluene  at  20°  are  given  by  Sisley  (1902).  Very  irregular 
results  were  obtained.  The  fact  that  the  colors  of  the  two  layers  are  different, 
was  taken  to  indicate  that  the  picric  acid  dissolves  in  a  different  molecular  form 
in  the  two  layers. 


495  PICRIC  ACID 

DISTRIBUTION  OF  PICRIC  ACID  AT  25°  BETWEEN: 


Water  and  Bromoform.                       Water  and  Chloroform. 

(Herz  and  Lewy  —  Z.  Electrochem,  n,  820,  '05.)                                          (H.  and  L.) 

MiUimols  CeHsNaOr           Cms.  CeHsNaOr               Mfflimols  QjHsNaOr           Cms.  QHaNsOr 
per  10  cc.                          per  100  cc.                           per  10  cc.                           per  100  cc. 

Aq.      Bromoform             Aq.      Bromoform             Aq.        Chloroform 
Layer.        Layer.              Layer.        Layer.                Layer.        Layer. 

0.321      0.365            0.736      0.836              0.207      0.254 
0-401      0.515            0.919       I.lSo              0.329      0-547 

0-475    °-655        i.  088    1.501          0.488    1.09 
o-575    0.871        1.317     1.995          0.561     1.41 
0.674    1.14          1.545     2.612          0.588    1.53 
DISTRIBUTION  OF  PICRIC  ACID  BETWEEN: 
Water  and  Benzene.     (Kuriloff,  1898.)   Water  and  Ether  at  20°. 
Mols.  Picric  Acid  per  Liter:                       Cms.  Picric  Acid  per  Liter: 

Aq.        Chloroform 
Layer.         Layer. 

0.474      0.582 

o-754     1-253 
1.118     2.498 

1-285    3-230 
1-348  3-505 

(Sisley,  1902.) 
Dist.  Coef. 
2.63 

i-79 
i-34 
0.13 

O.OI 

Aq.  Layer.         C6H6Xayer. 
0.026l            0.0940 
O.O2O8            0.0779 

0.0188        0.0618 
0.0132        0.0359 
0.0097        0.0198     1  L 

Aq.  Layer.      Ether  Layer. 
6.78            17.85 
3.74               6.70 
2.85               3.72 

0.85          o.n 

O.IO              O.OOI 

Data  for  the  distribution  of  picric  acid  between  water  and  mixtures  of  chloro- 
form and  toluene  at  25°,  are  given  by  Herz  and  Kurzer  (1910). 

FREEZING-POINT  DATA  (Solubilities,  see  footnote,  p.  i)  ARE  GIVEN  FOR 

THE  FOLLOWING  MIXTURES: 
Picric  Acid  +  Dirnethylpyrone.        (Kendall,  1914.) 

-j-  Resorcinol.  (Philip  and  Smith,  1905.) 

-J-  Thymol.  (Kendall,  1916.) 

+  a  Trinitrotoluene.      (Giua,  1916.) 
MethylPICRIC   ACID   C6H(CH3)(OH)(NO2)3,  1.3.2.4.6. 

SOLUBILITY  IN  AQUEOUS  SOLUTIONS  AT  25°.    (Kendall,  1911.) 

Normality  of  Normality  of 

A      c  i  Dissolved  A      c  i       «•  Dissolved 

Aq.  Solvent.  Methyl  pkric  Aq.  Solvent.  Methyl  picric 

Acid.  Acid. 

Water  o.oioo      0.01975  n  o  Nitrobenzoic  Acid          0.0080 

"      -f-Ligroin  0.01019    0.00981  n  Salicylic  Acid  0.01063 

"      -(-Toluene  0.01059    0.01393  n        "  0.01072    . 

0.00895 n  HC1  0.00641  H2O+Excess  of  Salicylic  Acid  0.02613* 

0.01593  n  HC1  0.00487 

0.01013  n  Picric  Acid  0.00702 

*  =  normality  of  salicylic  acid  +  inethylpicric  acid. 

PICROTOXIN  C3oH34013. 

loogms.  H2O  dissolve      o.4i+gm.  picrotoxin  at  20-25°.  (Dehn,  1917.) 

pyridine  dissolve  102          gms.  " 

aq-50%pyridine  81 

PIMELIC   ACID    (CH2)5(COOH)2. 

DISTRIBUTION  BETWEEN  WATER  AND  ETHER  AT  25°.    (Chandler,  1908.) 


Mols.  (CH2)5(COOH)j  per  Liter. 

Dist.  Coef.  ? 

1 

0.7095 
0.7170 
0.7195 

o  .  7480 

0.7075 

Dist.  Coef. 
Corrected 

for  lonization. 

0.670 
0.670 
0.663 
0.663 
0-653 

Aq.  Layer,  a. 

o  .  00998 

0.00702 
0.00480 
O.OO284 
O.OOI79 

Ether  Layer,  b, 
O.OI4O7 
0.00979 
0.00667 
0.00380 
0.00253 

PILOCARPINE  496 

PILOCARPINE   CUH16N202. 

100  cc.  oil  of  sesame  dissolve  0.3142  gm.  CnHi6N2O2  at  20°.  (Zalai,  1910.) 

PILOCARPINE    HYDROCHLORIDE    CUH16N2O2.HC1,    Pilocarpine    Nitrate 
CiiHi6N2O2.HNO3,  and  Piperine  Ci7H19NO3  in  Several  Solvents. 

(U.  S.  P.,  VIII.) 

Gms.  per  100  Gms.  Solvent. 

Solvent.  t°.  , » x 

CUH16N202.HC1.      CUH16N202.HN03.        ,C17H19NO,. 

Water  25  333  25  insoluble 

Alcohol  25                4-35  1-66  6.66 

Alcohol  60               9.09  6.2  22.7 

Chloroform  25               0.18  ...  58.8 

Ether  25               ...  ...  2.8 

PINACOLIN  CH3.CO.C(CH3)3. 

SOLUBILITY  IN  WATER  AND  IN  AQ.  ACETONE  AT  15°.    (Deiange,  1908.) 

Per  cent  Acetone  cc.  Pinacolin  Dissolved 

in  Solvent.  per  100  cc.  Solvent. 

o  (=  pure  H2O)  2 .44 

20  3.47 

33  6.06 

50  9.09 

60  14-27 
PINENE  HYDROCHLORIDE   C10H16.HC1. 

IOO  gms.  95%  formic  acid  dissolve  i.2gms.  CioHie.HCl  at  16.8°.  (Aschan,  1913.) 

PIPECOLINE   C5H9(CH3)NH  d  and  /. 

F.-pt.  data  for  mixtures  of  d  and  I  pipecoline  are  given  by  Ladenburg  and 
Sobecki  (1910). 

PIPERIDINE   CH2<(CH2.CH2)2>NH. 

DISTRIBUTION  BETWEEN  WATER  AND  BENZENE  AT  ORD.  TEMP.  (Georgievks,  1915.) 

Gms.  Piperidine  per:  Gms.  Piperidine  per: 


25  cc.  H2O  Layer.  75  cc.  C6H6  Layer.  25  cc.  H2O  Layer.  75  cc.  CeH6  Layer. 
0.1573                    0.4127                               0.891  2.339 

0.256  0.674  1.299  3-589 

0.409  I. 088  I.7I2  4-789 

0.674  1-746 

PIPERIDINE  HYDROCHLORIDE  CH2<(CH2.CH2)2>NH.HC1. 

SOLUBILITY  IN  SEVERAL  SOLVENTS.    (Freundiich  and  Richards,  1912.) 

c,o,ro,  *o          Mols.  Piperidine 

Solvent.  *  •          HC1  per  Liter. 

Water  o  4.87 

25  S-iQ 

Tetrachlor  Ethane  (sat.  with  H20)  o  0.13 

25  0.29 

Nitrobenzene  25  0.00543 

Benzene  25  0.00102 

MethylPIPERIDINES   2-,  3-,  4-,  n  Methyl,  etc. 

Data  for  the  reciprocal  solubility  of  2-methylpiperidine  and  water,  3-methyl- 
piperidine  and  water,  4-methylpiperidine  and  water,  nitrosopiperidine  and  water 
and  for  w-methylpiperidine  and  water,  determined  by  the  synthetic  (sealed  tube) 
method  of  Alexejeff,  are  given  by  Flaschner  and  MacEwan  (1908)  and  by  Flasch- 
ner  (1909)  and  (1908).  Similar  data  for  «-ethylpiperidine  and  water  and  for  n- 
propylpiperidine  and  water  are  given  by  Flaschner  (1908). 


497  PIPERIDINES 

act'  Diphenyl   PIPERIDINES   Ci7Hi9N. 

SOLUBILITIES  OF  THE  ACID  SALTS  OF  ace'  DIPHENYL  PIPERIDINE  AND  OF  I  so  act' 
DIPHENYL  PIPERIDINE  IN  WATER  AT  25°. 

(Scholtz,  1901.) 

Cms.  per  100  Cms.  Sat.  Solution: 
Piperidine  Base.  f  -  •  —  •  -  *  -  \ 

HClSalt.     HBrSalt.       HI  Salt.       H2SO4  Salt. 

a,  a'  Diphenyl  Piperidine,  m.  pt.  7  1°    o  .  85          o  .  90          0.12  6.31 

Iso  a,  a'  Diphenyl  Piperidine,  liquid          3.02          i  0.72    easily  soluble 

PIPERINE   Ci7Hi9N03.     (See  also  under  Pilocarpine,  preceding  page.) 
SOLUBILITY  IN  SEVERAL  SOLVENTS. 


!  Authority. 

Water  20-25  0.01  (Dehn,  1917.) 

Ethyl      Alcohol  9.5  2.9  (Timofeiew,  1894.) 

Methyl       "  9.5  4.4 

Propyl        "  9.5  2.94 

Trichlor  Ethylene  15  9  .  83  (Wester  and  Bruins,  1914-) 

Pyridine  20-25  22.46         (Dehn,  1917.) 

Aq.  50%  Pyridine          20-25  IJ-39 

PLATINUM  ALLOYS. 

SOLUBILITY  OF  PLATINUM  ALLOYS  IN  NITRIC  ACID. 

(Winkler  —  Z.  anal.  Ch.  13,  369,  '74.) 


Appro*.          Grams  Alloy  Dissolved  per  TOO  Grams  HNOs  Solution  of 

Pt^in  Alloy.  ^ 

i.3o8Sp.Gr. 

i.2o8Sp.Gr. 

i.iooSp.Gr. 

i.2o8Sp.Gr4 

IO 

57 

44 

69 

37 

5 

69 

57 

51 

35 

2-5 

62 

61 

69 

I 

75 

70 

76 

10 

46 

27 

II 

51 

5 

36 

34 

14 

4i 

2-5 

51 

40 

30 

i 

52 

41 

37 

.  . 

10 

7 

9 

8 

5 

8 

9 

10 

.. 

2-5 

22 

17 

ii 

21 

18 

23 

.-. 

10 

14 

19 

4 

3 

5 

21 

20 

6 

18 

2-5 

25 

42 

8 

I 

49 

64 

10 

...-.  • 

10 

10 

II 

19 

5 

5 

16 

12 

6 

ii 

2-5 

16 

24 

19 

.. 

i 

20 

32 

37 

Pt  and  Silver 


Pt  and  Copper 


Pt  and  Lead 
n 

M 
II 

Pt  and  Bismuth 


Pt  and  Zinc 
ii 

n 
ii 

PLATINUM    BROMIDE    PtBr4. 

100  grams  sat.  aqueous  solution  contain  0.41  gram  PtBr4  at  20°. 

(Halberstadt  —  Ber.  17,  2062,  '84.) 

PLATINIO    POTASSIUM    BROMIDE    K2PtBr6. 

100  grams  sat.  aqueous  solution  contain  2.02  grams  K2PtBr6  at  20°. 

(HalberstadU 


PLATINUM  CHLORIDES 


498 


PLATINIC    DOUBLE    CHLORIDES    of    Ammonium,    Caesium,    Potassium, 
Rubidium  and  Thallium.     (Data  for  each  separately.) 
SOLUBILITY  IN  WATER. 

(Crookes  —  Chem.  News  9»  37.  205,  '64;  Bunsen  —  Pogg.  Ann.  113,  337,  *6i.) 
Grams  per  100  Grams  Water. 


1". 

(NH^tCle. 

Cs2PtCl6. 

K2PtCl6. 

Rb2PtCl6. 

Tl2PtCl<j. 

0 
10 

0*666(15°) 

O.O24 
0.050 

o-74 
0.90 

0.154 

0.0064(15°) 

20 
25 

30 
40 

... 

0.079 
0.095 
O.IIO 

0.142 

1.  12 
1.26 
I.4I 
I.76 

O.I4I 
0.143 
0.145 

0.166 

... 

£ 
6o 

0.177 
0.213 

2.17 
2  .64 

0.203 
0-253 

.  .  . 

70 

0.251 

3-19 

0-329 

80 

0.291 

3-79 

0.417 

90 

100 

1-25 

0.332 

0-377 

4-45 

0.521 
0-634 

0.050 

SOLUBILITY  OF  POTASSIUM  CHLOROPLATINATE  IN  WATER  AND  IN  AQUEOUS 
SOLUTIONS  OF  POTASSIUM  CHLORIDE  AND  OF  SODIUM  CHLORIDE. 

(Archibald,  Wilcox  and  Buckley,  1908.) 


Solubility  in  Water. 

Gms.  K2PtCl« 
t°.  per  100  Gms. 

H20. 

0.4784 
0.5992 
0.7742 


O 
IO 

20 

30 
40 
60 

80 

100 


355 
444 


In  Aq.  KC1  at  20°. 

Gm.  Mols.        Cms.  K2PtCl« 


5-030 


KCl 

per  zoo  Gms. 

>er  Liter. 

Solvent. 

O.2C 

0.0236 

0.25 

O.O2O7 

0.50 

0.0109 

I 

o  .  0046 

2 

O.OO45 

3 

O.OO43 

4 

0.0042 

sat. 

0.0034 

In  Aq. 

NaCl  at  1  6°. 

Gm.  Mols.       Cms.  K2PtCU 

NaCl 

per  loo  Gms. 

per  Liter 

Solvent. 

0 

0.672 

0.05 

0.700 

0.10 

0.729 

0.25 

0.758 

0.50 

0-775 

o-7S 

0.791 

i 

0.805 

2 

0.834 

SOLUBILITY  OF  POTASSIUM  CHLOROPLATINATE  IN  AQUEOUS  SOLUTIONS  OF 
METHYL  ALCOHOL  AND  OF  &THYL  ALCOHOL  AT  20°. 

(Archibald,  Wilcox  and  Buckley,  1908.) 


Wt.  Per  cent 
Alcohol  in 

Gms.  K2PtCl«  per  100  Gms.: 

Solvent. 

Aq.  CHjOH. 

Aq.  C2H5OH. 

0 

0.7742 

0.7742 

5 

0-535 

0.491 

10 

0.412 

0.372 

20 

0.264 

0.218 

30 

0.1831 

0.134 

40 

O.II65 

0.076 

Wt.  Per  cent 

Alcohol  in 

Solvent. 

50 
60 
70 
80 
90 
100 


Gms.  K2PtCl8  per  100  Gms.: 


Aq.  CH3OH. 

Aq.  C2HSOH. 

0.0625 

0.0491 

0.0325 

0.0265 

0.0l82 

0.0128 

0.0124 

0.0085 

0.0038 

0.0025 

O.OO27 

o  .  0009 

loo  gms.  aq.  8.2%  isobutyl  alcohol  dissolve  0.625  Sm-  K2PtCl6  at  20°. 
loo  gms.  aq.  sat.  isobutyl  alcohol  dissolve  0.318  gm.  K2PtCl6  at  20°. 

(Archibald,  Wilcox  and  Buckley,  1908.) 

One  liter  of  55%  alcohol  dissolves  0.150  gm.  (NH4)2PtCl6at  15-20°.  (Fresenius,  1846.) 
76%       "  "       0.067    " 

95%       "  "       0.0037  " 


499  PLATINUM  CHLORIDES 

DISTRIBUTION  OF  PLATINUM  CHLORIDE  BETWEEN  WATER  AND  ETHER  AT 
ORD.  TEMP.    (Mylius,  1911.) 

When  i  gm.  of  platinum  as  chloride  is  dissolved  in  100  cc.  of  aq.  10%  HC1  and 
shaken  with  100  cc.  of  ether,  o.oi  per  cent  of  the  platinum  enters  the  etheral  layer. 
If  water  is  used  instead  of  10%  HC1,  approximately  the  same  per  cent  of  Pt  enters 
the  ether  layer. 

100  cc.  anhydrous  hydrazine  dissolve  I  gm.  platinic  chloride,  with  formation  of 
a  black  precipitate  at  room  temp.  (Welsh  and  Broderson,  1915.) 

ChloroPLATINATES   of  Hydrocarbon  Sulfines. 

SOLUBILITY  OF  EACH  IN  WATER  AT  16°.     (Stromholm,  1900.) 

Chloroplatinate.  Cms.  Salt  per 

f • • — •* \       100  Gms. 

Name.  Formula.  Sat.  Solution. 


Trimethyl  Sulfine  Chloroplatinate 
Dimethyl  Ethyl  Sulfine  Chloroplatinate 
Methyl  Diethyl  Sulfine  Chloroplatinate 
Triethyl  Sulfine  Chloroplatinate 


(CH3)3S]2PtCl6  0.47 

(CH3)2(C2H5)S]2PtCl6  3-43 

CH3(C2H5)2S12PtCl6  2.42 

(C2H5)3S]2PtCl6  1.98 


Similar  results  for  more  complex  sulfines  are  also  given. 

PLATING  AMINES. 

SOLUBILITY  IN  WATER.    (Cleve,  1866  ?) 

Amine.  Formula.  Gms.  per  100  Gms.  H2O. 


Platino  Semi  Diamine  Chloride  pt<  (NH.),.C1  0. 26  at  0°,  3 . 4    at  100° 

Chloro  Platino  Amine  Chloride  OPt  <  *gjg   o.  14  at  o°,  3        at  100° 

Chloro  Platino  Semi  Diamine  Chloride  Cl3Pt(NH3)2Cl    o .  33  at  o°,  i .  54  at  100° 
PLATINOUS  NITRITE  AMMONIUM   COMPOUNDS. 

SOLUBILITY  IN  WATER.     (Tschugaev  and  Kiltinovie,  1916.) 

When  ammonia  is  added  to  a  cold  solution  of  potassium  platinonitrite  a  copious 
precipitate  of  the  composition  Pt2NH3(NO2)2,  is  obtained.  By  comparison  of 
the  solubility  of  this  precipitate  with  that  of  each  of  three  hitherto  described 
ammonioplatinum  compounds,  it 'was  found  that  the  precipitate  obtained  as  de- 

NH3.          .N02 
scribed,  corresponds  to  the  cis  form  of  dinitro  diammonio  platinum,          /  Pt  ( 

NH3  NO2 

The  results  for  the  solubility  of  cis  and  trans  dinitro  diammonio  platinum  and  of 
tetra  ammonia  platinous  platinonitrite  in  water,  are  as  follows : 

Gms.  Each  Compound  per  100  Gms.  H2O. 


trans  Pt2NH3(NO.,)2.        [Pt4NH3]  [Pt(NOk)4l- 

25  0.083  0.063  o.on 

63  o . 66  o . 49  ... 

74.4  ...  0.81 

95  2.32  1.85 

Determinations  of  the  solubility  of  several  mixtures  of  the  cis  and  trans  com- 
pounds in  water  are  also  given. 

PONCEAU   (Free  Acid)  Ci0HTN:N.Ci0H4(OH)(SQ,H),.9HiO. 

SOLUBILITY  IN  SEVERAL  SOLVENTS  AT  23.°    (Sisley,  1002.) 

Solvent.  Gms.  Ponceau  per  Liter. 

Water  209 . 6 

+5  Gms.  H2SO4  per  Liter  180 

"     Sat.  with  Amyl  Alcohol  195 
Amyl  Alcohol  73 .4 

Ether,  pure  none 

Data  are  also  given  for  the  distribution  of  ponceau  between  water  and  amyl 
alcohol  at  18°. 


POTASSIUM 


500 


POTASSIUM  K2. 

SOLUBILITY  OF  POTASSIUM  IN  LIQUID  AMMONIA.    (Ruff  and  Geisei,  1906.) 

to  Mols.  NH3  to  Dis- 

solve i  Gm.  Atom  K. 

—  loo  4.82 

-So  4-79 

o  4.74 

SOLUBILITY  OF  POTASSIUM  IN  MELTED  KOH.    (von  Hevesy,  1909.) 
Difficulty  was  experienced  due  to  the  failure  of  the  excess  of  K  to  separate  com- 
pletely from  the  saturated  solution.     Time  of  heating,  50  hours. 

t°.  Cms.  K  per  100  Cms.  KOH. 

480  7.8-8.9 

600  3     -4 

650  2      -2.7 

700  0.5-1.3 

POTASAMMONIUM  K?(NH3)2. 

100  gms.  liquid  ammonia  dissolve  99.5  gms.  K2(NH3)2  at  o°  and  97  gms.  at 
+8.44°.  (Joannis,  1906.) 

POTASSIUM  ACETATE  CH3COOK.iiH2O. 

SOLUBILITY  IN  WATER.    (Abe,  1911.) 


•     Gms.  CHsCOOK 
t°.  per  100  Gms.       Solid  Phase. 

H20. 

2CH3COOK.3H2O 


Gms.  CH3COOK 

per  100  Gms. 

H20. 


Solid  Phase. 


O.I  216.7      2CH3COOK.3H2O     41  327-7        2  CH3COOK.3H20 

5  223.9  "  4i.3tr.pt.         ...        "  +2CH3cooK.H2o 

10  233.9  "  42  329  2CH3COOK.H2O 

15  243.1  ««  45  332.2 

20  255.6  50  337.3 

25   269.4    "    60      350 
30    283.8     "     70       364.8 

35    30.1-8      "      80        380.1 

38   314.2    «    90      396.3 
40   323.3        96      406.5 

SOLUBILITY  OF  POTASSIUM  ACETATE  IN  AQ.  ALCOHOL  SOLUTIONS  AT  25°.  (Seideii,  '10.) 

<*25  of     Gms.  CH3COOK  per 
Sat.  Sol.      loo  Gms.  Solvent. 

219.6  70  LI56  Il8.3 

219.6  80  1.085  87.6 

192.4  90  0.990  52.9 

171.8  95  0.922          34.2 

147.5  I0°  0.850          16.3 


Wt.  %  QHjOH 
in  Solvent. 

O 

20 
40 

50 

60 


Sat.  Sol. 
.417 

.363 
.302 
.260 
.210 


Gms.  CH3COOK  per 
100  Gms.  Solvent. 


F.-pt.  data  for  potassium  acetate  +  acetic  acid  (Vasilev,  1909);  potassium 
acetate  +  sodium  acetate  (Baskov,  1915).  (Baskov,  1915.) 


POTASSIUM  SulfoANTIMONATE 

SOLUBILITY  IN  WATER. 

Solid  Phase. 
Ice 


(Donk,  1908.) 


'   i-3 

-  2.6 

-  4 

-  7.2 
— 10.6 

-&.$ 

-28.8 


9-5 
17.1 

24.2 

35-4 
42.9 
48.8 
52.6 
59-6 


t  o               Gms.  K3SbS4  per 
loo  Gms.  Sat.  Sol.       Solid  Phase. 

-34 

62 

Ice+K3SbS4.6H2O 

—  10 

65.5 

K3SbS4.6H20 

-  4.5 

69.1 

" 

0 

75-4 

K3SbS4.sH2O 

+  10 

76.2 

« 

30 

75-i 

« 

50 

77-7 

K8SbS4.3H20 

80 

79.2 

it 

5oi  POTASSIUM  SulfoANTIMONATE 


SOLUBILITY  OF  POTASSIUM  SULFOANTIMONATE  IN  AQ.  SOLUTIONS  OF 
POTASSIUM  HYDROXIDE  AT  30°  AND  VICE  VERSA. 

(Donk,  1908.) 


Gms.  per  100  Gms.  Sat.  Sol. 


K3SbS4. 

75 

68.4 
56.8 
50-9 

37-7 


KOH. 
O 

3-4 
ii 
16.1 

25  5 


Solid  Phase. 

K3SbS4.sH2O 
K3SbS4.3H20 


K3SbS4 


Gms.  per  100  Gms.  Sat.  Sol. 


K3SbS4. 
19.8 

KOH. 
40-5 

•>           OUMU  rua,sc. 

K3SbS4 

"•5 

49.9 

"  +KOH.2H20 

9.4 

0 

49.9 
56.3 

KOH.2H2O 
u 

SOLUBILITY  OF  POTASSIUM  SULFOANTIMONATE  IN  AQ.  ETHYL  ALCOHOL. 

(Donk,  1908.) 


Solid  Phase. 
K3SbS4.sH2O 


Results  at  10°. 

Gms.  per  roopms.  Sat.  Sol. 
'K3SbS4.  QH5OH.  ' 

o  94 

o  90.5 

Two  Liquid  Layers  Formed  Here. 

69 . 2  0.8 

76.1  o 

Composition  of  the  Liquid  Layers. 

Gms.  per  100  Gms. 


Results  at  30°. 

Gms.  per  100  Gms.  Sat.  Sol. 


K3SbS4. 
O 


C2H5OH. 

97 


Solid  Phase. 
K3SbS4.3H2O 


Two  Liquid  Layers  Formed  Here: 


Composition  of  the  Liquid  Layers. 

Gms.  per  100  Gms. 


Alcoholic  Layer. 

Aqueous  Layer. 

K3SbS4. 
0 
2.2 
4.2 
27.4 

C2H5OH. 
85 

54-7 
46.9 
16 

"K3SbS4. 
67.4 

49 
45-6 

C,HBOH. 
I.I 

3-4 
3-8 

Alcoholic  Layer. 

Aqueous  Layer. 

K3SbS4. 

C2H5OH. 

K3SbS4. 

QHBOtf. 

0 

93-i 

70.5 

±0.5 

0 

85.6 

65.2 

I  .2 

2.2 

56.8 

47-8 

5-7 

8.5 

41.1 

37-i 

9-2 

12.7     31-1 

SOLUBILITY  OF  POTASSIUM  SULFOANTIMONATE  IN  AQ.  METHYL  ALCOHOL  AT  15°. 

(Donk,  1908.) 

Composition  of  the  Liquid  Layers. 

Gms.  per  100  Gms. 

Gms.  per  100  Gms.  Sat.  Sol.     Solid  Phase. 
K3SbS4.  CH3OH. 

0.5  99.5  K3SbS4 

0-45  99-5 

i. 5  93-9 

1.8  92 

Two  Liquid  Layers  Formed  Here. 

62.7  7.5         KaSbS^HjO  ...  ...  31.1  31.3 

68.4  3.5  41.1  22.2 

75-5  o  47.2        18.2 

Two  Liquid  Layers  Formed  Here.  ...  ...  57 -2  II. I 

0-5  98.1 

POTASSIUM   (Dihydrogen)   ARSENATE   KH2AsO4. 

100  gms.  sat.  aq.  solution  contain  15.9  gms.  KH2AsO4,  or  100  gms.  H2O  dissolve 
18.86  gms.  at  6°.     Sp.  Gr.  of  solution  =  1.1134.  (Field,  1859.) 

100  cc.  sat.  aq.  solution  contain  28.24  gms.  KH2AsO4  at  about  7°. 

(Muthmann  and  Kuntze,  1894.) 

loo  gms.  glycerol  (d16  =  1.256)  dissolve  50.1  gms.  potassium  arsenate  at  15-16°. 

(Ossendowski,  1907.) 


Alcoholic  Layer. 

Aqueous  Layer. 

'K,SbS4. 

5 
4-9 

13-6 
19.1 

CH3OH.' 
82.5 

76.3 
66.9 

54 
45-5 

62.5 

CH3OH." 
8 

POTASSIUM  BENZOATE  502 

POTASSIUM  BENZOATE   KC7H6O2.3H2O. 

SOLUBILITY  IN  WATER. 

(Pajetta,  1906, 1907.) 
t°-  17-5°          25°  33-3°       50° 

Cms.  KC7H602  per  ioo  Gms.  Solution    41.1        42.4        44         46.6 

POTASSIUM   BORAXES. 

SOLUBILITY  OF  POTASSIUM  BORATES  IN  WATER  AT  30°. 

(Dukelski  —  Z.  anorg.  Chem.  50,  42,  '06,  complete  references  given.) 

Gms.  per  ioo  Gms.  Solution.  Gms.  per  ioo  Gms.  Residue.  Solid 

'     K20.               B203.  *                 K20.               B203.   '  Phase- 

47 . 50              ...                       ...                  ...  KOH.2H2O 

46.36             O.QI                46.13             9-02  K2O.B203.2iH20 
40-51             1-25                41.62             9.71 
36.82             I. 80               39-90           13 .19. 

32-74         3-51  37-22        14.58 

29.63        6.98         35.05      17.92 

24.84         17-63  30.02         21.70  " 

23.30  18.19  26.84          3J-49  K20.2B203.4H20 

16.21        13-10  25.12        33 .18 

11.78          9.82  20.57        26.43 

9.18          8.00  22.38        31-30 

6.22  9.13  20-87  31    06 

7-73  J3'37  22.21  36.24       K20.2B208.4H20+K20.5B203.8H20 

7.81       13.28         17.50      34.18 

7.71  13.21  11.49  34  -8l  K20.5B203.8H20 

7.63       13.28          12.51       4052 
3-42          7-59  10.77        37.35 

I. 80  4.15  5.88  20-00 

0.51         3.19  10.81        40.89 

0-33  4-58  7-72  34-21  K20.5B203.8H20+B(OH)a 

0.31        4-46          3.91      30-68 

3-54  

POTASSIUM   MetaBORATE   KBO2. 

Fusion-point  data  for  potassium  metaborate  +  sodium  metaborate  and  for 
potassium  metaborate  +  potassium  metaphosphate  are  given  by  van  Klooster 
(1910-11). 

POTASSIUM  PerBORATES,   2KB03.H2O,  2KB03.H2O2. 
SOLUBILITY  OF  EACH  IN  WATER. 

(v.  Girsewald  and  Wolokitin,  1909.) 

T>_rat.,  %  Active  O  in          f0         Gms.  Salt  per  ioo 

Borate.  Gms.  Water. 

2KBO3.H2O  14.93  °  i-2S 

14.93          i5  2.50 

2KBO3.H2O2  20.84          15  0.70 

POTASSIUM   (Fluo)   BORIDE  KBF4. 

ioo  gms.  H2O  dissolve  0.44  gm.  KBF4  at  20°,  and  6.27  gms.  at  100°. 

(Stolba,  1889.) 


503 


POTASSIUM  BROMATE 


POTASSIUM  BROMATE  KBrO3. 

SOLUBILITY  IN  WATER. 

(Krcmers  — Pogg.  Ann.  97,  5,  '56;  Rammelsberg  —  Ibid.  55,  79,  '42;  Pohl  —  Sitzber.  Akad.  Wiss 
Wien.  6,  595,  '51-) 


Gms.  KBrOa  per  100  Gms. 


f     m 

'  Water. 

Solutio 

o 

3  -i 

3-o 

10 

4-8 

4.6 

20 

6.9 

6-5 

25 

8.0 

7-4 

30 

95 

8.7 

Gms.  KBrOa  per  100  Gms. 

Water.  Solution. 

40  13.2  II-7 

50  17-5  J4-9 

60  22.  f  18.5 

80  34-0  25.4 

100  50.0  33.3 


Sp.  Gr.  of  solution  saturated  at  19.5°  =  1.05. 


SOLUBILITY  OF  POTASSIUM  BROMATE  IN  AQUEOUS  SOLUTIONS  OP 
SODIUM  NITRATE  AND  OF  SODIUM  CHLORIDE. 

(Geffcken  — Z.  physik.  Chem.  49,  296,  '04.) 


In  Sodium  Nitrate. 

Grams  per  Liter. 

Mols.  KBrO3 

NaNO3.          KBrO3. 

per  Liter. 

o.o          78.79 

0.4715 

42.54           96.01 

0-5745 

85.09       108.6 

0.6497 

170.18      128.3 

0.7680 

255.27       150.9 

0.9026 

340.36     172.3 

1.031 

In  Sodium  Chloride. 

Grams  per  Liter. 
NaCl.  KBr03. 

o.o          78-79 

29  25     82.24 
58.50     93.87 

117.0    100.9 

175-5    IQ4  3 
234.0    106.9 


Mols.  KBrO3 
per  Liter. 

0-47*5 
0.5220 
0.5616 

o . 6042 

0.6244 

o . 6400 


SOLUBILITY  OF  POTASSIUM  BROMATE  IN  AQUEOUS  SOLUTIONS  OF  VARIOUS 
COMPOUNDS  AT  25°. 

(Rothmund,  1910.) 


Solvent,  0.5  Normal       T 
Aq.  Sol.  of: 

Water  alone 

Methyl  Alcohol 

Ethyl' Alcohol 

Propyl  Alcohol 

Tertiary  Amyl  Alcohol 

Acetone 

Ethyl  Ether 

Formaldehyde 

Glycol 

Glycerol 

Mannitol 

Grape  Sugar 

Urea 


IBrcfper 

Gms. 
KBrO3  per 

Solvent,  0.5  Normal 
Aq   Sol  of- 

Mols. 
KBrO3  per 

Gms. 
KBrOj  per 

Liter. 

Liter. 

Liter. 

Liter. 

0.478 

79.84 

Dimethylpyrone 

0.478 

79.84 

0-444 

74.16 

Ammonia 

0.445 

74-33 

0.421 

70-33 

Dimethylamine 

0.384 

64.13 

0.409 

68.31 

Pyridine 

0.415 

69.31 

0.383 

63.97 

Piperidine 

0.396 

66.15 

0.425 

70.99 

Urethan 

0-433 

72.33 

0-395 

65.98 

Formamide 

0-473 

79.02 

0-397 

66.31 

Acetamide 

0-445 

74-33 

0.448 

74.84 

Glycocol 

0.501 

83.68 

0.451 

75-34 

Acetic  Acid 

0.456 

76.17 

0-451 

75-34 

Phenol 

0.426 

7LI5 

0.431 

71.99 

Methylal 

0.405 

67.66 

0-477 

79-68 

Methyl  Acetate 

0.420 

70.15 

POTASSIUM  BROMIDE 


504 


POTASSIUM  BROMIDE  KBr. 

SOLUBILITY  IN  WATER. 

(Average  curve  from  results  of  Meusser  —  Z.  anorg.  Chem.  44,  79,  '05;  Etard  —  Compt.  rend. 
'84;  Ann.  chim.  phys.  [7]  2,  526,  '94;  de  Coppet  —  Ibid.  [5]  30,^16,  '83;  Tilden  and 
Shenstone  —  Phil.  Trans.  175,  23,  '84.) 


98,  1432. 


Grams  KBr  per  100  Grams 


Grams  KBr  per  100  Grams 


I    . 

Solution. 

Water. 

i>  . 

Solution. 

Water. 

-  6.5 

20.  o 

25.0 

30 

41-4 

70.6 

-  8-5 

26.5 

35-7 

40 

43-o 

75-5 

-10.5 

29'5 

41.8 

50 

44-5 

80.2 

-"•5 

31.2 

45-3 

60 

46.1 

85-5 

—  10 

31.8 

46.7 

70 

47-4 

QO.O 

-  5 

33-3 

50.0 

80 

48-7 

95-o 

o 

34-9 

53-5 

90 

49.8 

99.2 

5 

36-1 

56.5 

IOO 

51.0 

104.0 

10 

37-3 

59-5 

no 

52-3 

109.5 

IS 

38-5 

62  .5 

140 

54-7 

120.9 

20 

39-5 

65  .2 

181 

59-3 

145.6 

25 

40.4 

67.7 

SOLUBILITY  OF  MIXTURES  OP  POTASSIUM  BROMIDE  AND  AMMONIUM 
BROMIDE  IN  WATER  AT  25°. 

(Fock  — Z.  Kryst.  Min.  28,  357,  '97-) 


rams  per  Liter  Solution.       Mol.  per  cent  in  S 

>olution.     Sp.  Gr.  of 

Mol.  per  cent 

in  Solid  Phas 

NH 
0 

4Br. 
•  OO 

KBr.    " 
558.1 

N 
O 

.0 

KBr.              Solutions. 
IOO                     L3756 

NHiBr. 

o.oo 

KBr. 
IOO 

6 

•4 

554 

.2 

I 

•38 

98 

.62            1.3745 

O 

.26 

99-74 

24 

.64 

536 

•5 

5 

.29 

94 

•71         1-3733 

I 

•27 

98.73 

51-34 

516.8 

10 

•77 

89 

•23 

•3721 

3 

.02 

96.98 

152 

•9 

441 

.2 

29 

•63 

70 

•37 

•37^1 

8 

.42 

91.58 

262 

.2 

347 

•3 

47 

.84 

52 

.16 

•3715 

17 

.20 

82.80 

347 

.6 

262 

•3 

61 

.69 

38-31 

•3753 

27 

.98 

72  .02 

381 

-4 

260 

•3 

64 

•03 

35 

97        i 

•3753 

32 

•53 

67.47 

417 

.8 

232 

.2 

68 

.61 

31 

39        i 

.3766 

39 

•45 

60.55 

432 

•5 

222 

•3 

70 

•27. 

29 

73        ' 

•3777 

variable 

variable 

480 

.8 

179 

•9 

76 

•47 

23 

53 

.3766 

98 

•53 

1.47 

577 

•3 

0 

.0 

IOO 

.0 

o 

o 

•3763 

IOO 

•o 

o.oo 

SOLUBILITY  OF  POTASSIUM  BROMIDE  AT  25°  IN: 
Aq.  Solutions  of  KC1  and  Vice  Versa.     Aq.  Solutions  of  KI  and  Vice  Versa. 

(Amadori  and  Pampanini,  1911.) 


(Amadori  and  Pampanini,  1911.) 
Cms,  per  100  Cms.  H2O. 


KBr. 

KCl/ 

68.47 

0 

62.26 

5-43 

58.50 

8.46 

52.45 

12.48 

45-42 

17.17 

38.70 

21.23 

26.62 

25.88 

12.94 

31.02 

0 

36.12 

(Seeal 

Iso  next  page.) 

Gms.  per  100  Cms.  H2O. 


KBr. 
53-21 
42.32 

34-14 
30.08 
29.62 
22.15 

21.88 

18-54 
o 


KI. 

35-92 

66.63 

95-36 

119.52 

119 

127.10 
127.31 
I30.6I 
149.26 


505 


POTASSIUM  BROMIDE 


SOLUBILITY  OP  POTASSIUM  BROMIDE  IN  AQUEOUS  SOLUTIONS  OF 
POTASSIUM  HYDROXIDE. 

(Ditte  —  Compt.  rend.  124,  30,  '97.) 


Grams  per  1000  Grams  H2O. 
'     KOH.  KB7 ' 

36-4  558-4 

"3-5  433-6 

177.2  358.1 

231.1  281.2 


Grams  per  1000  Grams  H2O. 
KOH.  KBr. 

277.6  248.1 

434-7  J37-i 

579.6  64.8 

806.9  33.4 


SOLUBILITY  OF  MIXTURES  OP  POTASSIUM  BROMIDE  AND  CHLORIDE  AND 
OF  MIXTURES  OF  POTASSIUM  BROMIDE  AND  IODIDE  IN  WATER. 

(Etard  —  Ann.  chim.  phys.  [7]  3,  275,  '97.) 

Mixtures  of  KBr  and  KC1.         Mixtures  of  KBr  and  KI. 

0  Grams  per  100  Gms.  Solution. 


KBr. 


KCl. 


—  20 

17.5 

10.5 

0 

21-5 

10.8 

10 

23.2 

II  .0 

20 

24.8 

II  .2 

25 

25-5 

"•3 

3° 

26.3 

11.4 

40 

28.0 

"•5 

60 

30.6 

11.  8 

80 

33-4 

12.  1 

100 

35-7 

12  .6 

120 

38.0 

12-9 

150 

40.6 

13-4 

Grams  per  too  Grams  Solution. 

KBr. 
9.2 

KI. 

42-5 

9-9 

10.2 

45-3 
46.6 

10-5 
10-7 
10-9 
II  .2 

47-5 
48.0 
48.6 
49.6 

II-9 
12.6 

I3.2 
14.0 

5*-3 

52-7 
53-8 
54-8 

14.9 

55-5 

SOLUBILITY  OF  POTASSIUM  BROMIDE  IN  AQUEOUS  SOLUTIONS  OF 
POTASSIUM  CHLORIDE,  AND  OF  POTASSIUM  CHLORIDE  IN  AQUEOUS 
SOLUTIONS  OF  POTASSIUM  BROMIDE,  AT  25.2°. 

(Touren — Compt.  rend.  130,  1252,  'oo.) 

KCl  in  Aq.  KBr  Solutions. 


KBr  in  Aq.  KCl  Solutions. 

Mols.  per  Liter.                 Grams  per  Liter. 

KCl. 

KBr. 

KCl. 

KBr. 

0 

.0 

4 

.76! 

0 

.0 

567 

.0 

0 

.67 

4 

.22 

50 

.0 

502 

•5 

0 

.81 

4 

•'5 

60 

•4 

494 

.2 

I 

•35 

3 

.70 

100 

•7 

440 

•7 

I 

.48 

3 

•54 

no 

•4 

421 

.6 

I 

.61 

3 

.42 

120 

.0 

407 

.2 

I 

.70 

3 

•34 

126 

.8 

397 

•7 

2 

.46 

2 

•So 

183 

•5 

297 

•7 

3 

•775 

O 

•525 

28l 

.6 

625 

•3 

Mols.  per  Liter. 

KBr.  KCl. 

o.o  4.18 

0-49  3-85 

0.85  3.58 

I-3I  3-19 

1.78  2.91 

2.25  2.58 

2-69  2-33 


Grams  per  Liter. 
KBr.          KCl. 

o.oo    311.8 

287.2 
267.1 
238.0 
2I7.I 
192.4 
173-8 


58-4 
IOI-3 
156.1 
211  .9 
268.0 
320.4 


POTASSIUM  BROMIDE 


506 


SOLUBILITY  OP  POTASSIUM  BROMIDE  IN  AQUEOUS  SOLUTIONS  OF 
POTASSIUM  NITRATE,  AND  OF  POTASSIUM  NITRATE  IN  AQUEOUS 
SOLUTIONS  OP  POTASSIUM  BROMIDE,  AT  14.5°  AND  AT  25.2°. 

(Touren  —  Compt.  rend.  130,  908,  'oo.) 

KNO3  in  Aq.  KBr  Solutions. 


KBr  in  Aqueous  KNO3  Solutions. 

Mols.  per  Liter.  Grams  per  Liter. 


Mols.  per  Liter. 


Grams  per  Liter. 


KNOs. 
Results  at 

o.o 

KBr. 
14.2°. 

4.332 

KNO3. 
O-O 

KBr. 

5*5-9 

KBr.         KNO3. 
Results  at  14.20°. 

o.o        2.228 

KBr. 

o.o 

KNO3. 
225.4 

0.362 

4.156 

36 

.6 

494 

•9 

0 

.356    2.026 

42 

•4 

205.0 

0-706 

4-093 

71 

•4 

487 

•4 

O 

.784 

•835 

93 

•4 

185-7 

1-235 

3-939 

124 

•9 

469 

.1 

I 

.092 

•730 

130 

.0 

175-0 

I 

-577 

•587 

I87 

.8 

l6o.6 

Results  at 

25.2°. 

2 

•542 

.406 

302 

•7 

142.2 

0-0 

4.761 

O 

•  o 

566 

.2 

3 

•536 

•308 

421 

.i 

132.3 

O.I3I 

4-72 

13 

•3 

561 

O 

Results  at 

25.2°. 

0.527 

4.61 

53-3 

549 

.1 

O 

.0        3.217 

0 

.0 

325-5 

0.721 

4-54 

72 

•9 

540 

.8 

0 

.38      3.026 

45 

•3 

306.2 

1.09 

4-475 

no 

•3 

533 

.0 

0.93     2.689 

no 

.8 

272.0 

I.I70 

4-44 

118 

•4 

528 

.8 

I 

•37       2.492 

163 

.1 

252.2 

I.C04 

4-375 

152 

.2 

521 

.1 

I 

.208     2.216 

143 

.8 

224-3 

2 

.87       1.958 

34i 

.8 

198.1 

3 

•55      1-807 

422 

.8 

182.8 

SOLUBILITY  OP  POTASSIUM  BROMIDE  IN  ALCOHOLS  AT  25°. 

(de  Bruyn  —  Z.  physik.  Chem.  10,  783,  '92;  Rohland  —  Z..  anorg.  Chem.  18,  327,  '98.) 
Grams  KBr  Dissolved  by  100  Gms.  Alcohol  at: 


/iiconoi. 

Methyl  Alcohol 
Ethyl  Alcohol 
Propyl  Alcohol 

Room  Temp.  (R.). 
I  .92 

0.28  (Sp.  Gr. 
0-055 

0.81) 

25°  (de  B.). 

i  .51  Abs.  Alcohol 

o.i3 

SOLUBILITY  OF  POTASSIUM  BROMIDE  IN  AQUEOUS  ALCOHOL. 

(Taylor —  j.  Physic.  Ch.  I,  724,  '9<5-'97.) 


Results  at  30°. 


Results  at  40°. 


Wt.  per  cent  Alcohol 

Gms.  KBr  per 

100  Gms. 

Gms.  KBr  per 

TOO  Gms. 

in  Solution. 

Sat.  Solution. 

Solvent. 

Sat.  Solution. 

Solvent. 

0 

41  .62 

71.30 

43-40 

76.65 

5 

38.98 

67.25 

40.85 

72.70 

10 

36.33 

63.40 

38.37 

69.00 

20 

31.09 

56.40 

33-27 

62.30 

30 

25.98 

50-I5 

28.32 

56-45 

40 

21  .24 

44-95 

23.22 

50.46 

50 

16.27 

38-85 

i8.ii 

44-25 

60 

11.50 

32-50 

13.02 

37-40 

70 

6.90 

24.70 

7  -98 

28.90 

80 

3-09 

15-95 

3-65 

18.95 

90 

0.87 

8.80 

1.03 

10.45 

100  gm.  acetone  dissolve  0.023  gm-  KBr  at  25°. 

(Krug  and  McElroy  —  J.  anal.  Chem.  6,  184,  '93.) 


507 


POTASSIUM  BROMIDE 


SOLUBILITY  OF  POTASSIUM  BROMIDE  IN  DILUTE  AQUEOUS  ETHYL  ALCOHOL. 
Results  at  o°. 

(Armstrong  and  Eyre,  1910-11.) 


Results  at  25°. 

(Armstrong,  Eyre,  Hussey  and  Paddison,  1907.) 


Wt.  %  CjHBOH 
in  Solvent. 

Gms.  KBr  per 
100  Gms.  Sat.  Sol. 

Wt.  %  QH6OH 
in  Solvent. 

Gms.  KBr  per 
100  Gms.  Sat.  Sol. 

<f,g  of  Sat.  Sol. 

O 

34-92 

O 

40.78 

*  1-3824 

I.I4 

34-35 

I.I4 

39.98 

1.3727 

2.25 

32.96 

2.25 

39-54 

1.3634 

4.41 

31-99 

4.41 

38.41 

1-3443 

8.44 

29-43 

12.  14 

34-97 

1.2815 

18-73 

30.91 

1.2322 

100  gms.  methyl  alcohol  dissolve  2.17    gms.  KBr  at  25°.   (Turner  and  Bissett,  1913.) 
ethyl          "  "        0.142  gm. 


propyl 
arayl 


0-035 
0.003 


SOLUBILITY  OF  POTASSIUM  BROMIDE  IN  AQUEOUS  SOLUTIONS  OF  METHYL 
ALCOHOL  AT  25°. 

(Herz  and  Anders,  1907.) 


Wt.%  CH3OH   Gms.  KBr  per       ,     nt  ~. 
in  Solvent.      100  cc.  Sat.  Sol.    d*£  of  Sat" 


VVL.    /o  v^iij^xa       vjrnis.  rvur  per         »          »  c   .     Q-I 

in  Solvent.        100  cc.  Sat.  Sol.    *?  of  Sat  SoL 

o  56.04  1-3797  64  10.35  0.9801 

10.6  46.28  1.300  78.1  5.24  0.8906 

30.8  29.98  .         1.159  98.9  2.74  0.8411 

47.1  19.28  1.058  loo  1.69  0.8047 

The  solubility  of  potassium  bromide  in  methyl  alcohol  at  the  critical  tem- 
perature is  given  by  Centnerszner  (1910),  as  0.2  gm.  KBr  per  100  gms.  sat  solution. 

100  gms.  95%  formic  acid  dissolve  23.2  gms.  KBr  at  18.5°.  (Aschan,  1913.) 

loo  cc.  anhydrous  hydrazine  dissolve  60  gms.  KBr  at  room  temp. 

(Welsh  and  Broderson,  1915.) 

loo  gms.  hydroxylamine  dissolve  about  44.7  gms.  KBr  at  17°-!  8°. 

(de  Bruyn,  1892.) 

SOLUBILITY  OF  POTASSIUM  BROMIDE  AT  25°  IN: 

(Herz  and  Knoch,  1905.) 


Aqueous  Acetone. 

Aqueous 

Glycerol. 

cc.  Acetone 

Per  100  cc.  Sat.  Solution.           c     0 

wt.% 

KBr  per  100  cc.  Sol.       c     ^ 

per  loo  cc. 
Solvent. 

Millimols 
KBr. 

Gms. 
KBr. 

Gms.       Solutions. 
H2O. 

Glycerol 
in  Solvent 

Millimols. 

Gms.        Solutions. 

O 

481.3 

57-3 

80.6 

-3793 

O 

481.3 

57-32      1.3793 

2O 

366.7 

43-67 

69-5 

.2688 

13.28 

444-3 

52.91 

•3704 

30 

310.5 

36.98 

62.97 

.2118 

25.98 

404 

48.11 

.3655 

40 

259 

30.85 

55-60 

.1558 

45-36 

340.5 

40.55 

•3594 

50 

202.9 

24.16 

47.60 

.0918 

54-23 

310.4 

36.98 

.358o 

00 

144-9 

17.22 

39.15      1.0275 

83-84 

219-25 

26.11 

•3603 

70 

95-3 

11.35 

29.78      0.9591 

IOO 

172.65 

20.56      1.3691 

80 

46.5 

5-54 

20.  10    0.8942 

90 

IO.I 

i.  20 

10.15      0.8340 

100  cc.  sat.  solution  of  potassium 
0.139  gm.  KBr  at  25°. 


bromide  in  furfurol  (C^sO.COH)  contain 

(Walden,  1906.) 


FUSION-POINT  DATA  FOR  MIXTURES  OF  KBr  AND  OTHER  SALTS. 


KBr  +  KF 
KBr  +  KCi 
KBr  +  KI 
KBr  +  AgBr 
KBr  +  NaCl 
KBr  +  KOH 


(Kurnakow  and  Wrzesnewsky,  1912;  Ruff  and  Plato,  1903.) 
(Wrzesnewsky,  1912;  Amadori  and  Pampanini,  1911;  Ruff  and  Plato  1903.) 
n  «  <«  «  « 

(Sandonnini,  1912.) 
(Ruff  and  Plato,  1903.) 
(Scarpa,  1915.) 


POTASSIUM  BUTYRATE 


508 


POTASSIUM   BUTYRATE   C3H7COOK. 

100  gms.  water  dissolve  296.8  gms.  CsHyCOOK,  or  100  gms.  sat.  solution  con- 
tain 74.8  gms.  at  31.25°. 

loo  gms.  of  an  aq.  solution  saturated  with  sugar  and  C3H7COOK  contain 
49.19  gms.  sugar  +  34.78  gms.  C3H7COOK  -f  16.03  gms.  H2O  at  31.25°. 

(Kohler,  1897.) 

POTASSIUM   CAMPHORATES. 

SOLUBILITY  IN  AQUEOUS  SOLUTIONS  OF  d  CAMPHORIC  ACID  AT  13.5-16°  AND 

VICE  VERSA. 

(Jungfleisch  and  Landrieu,  1914.) 


Gms.  per  100  Gms.  Sat.  Sol. 

Gms.  per  100  Gms.  Sat.  Sol. 

CsH14(COOH)2.       C10H1404K2. 

C8H14(COOH)2. 

C10H1404K2. 

O                        66  .  65          CWH14O4K2 

2.90 

3  2  .  84      C10H16O4K.CioHi6O4 

0  .  90                69  .  69         Ci0H16O4K 

3-20 

29-39 

I                        69 

3-30 

28.56      CjoHuO.K.aQoHuO, 

I.  io            66.79 

3-20 

27.32 

0.90                66.65       C10HU04K.H2 

o          3  .  20 

22.77 

1.50                62.37 

3.10 

21.66 

2.60                59.34 

2.90 

12.97 

3-20           58-37 

2.90 

11.73 

3-20                58.09 

3.10 

11.59        dQH^COOH), 

3-20                52.71    CioHiAK-QoH 

iA         2.90 

9.66 

3.20               48.43 

2.80 

8.14 

2.80               47.88 

2.50 

6.76 

2.80               42.36 

2.30 

6.07 

3                  35-6o 

2 

4-55 

2-85            34-77 

0.621 

0 

CioH14O4K2  =  Dipotassium  d  camphorate. 
CioHi6O4K  =  Monopotassium  dtcamphorate. 

C10HJ504K.C10H1604  = 

Oi0^i5O4.K..3V^lot*l(jO4  — 

Monopotassium  d  dicamphorate. 
Monopotassium  d  tetracamphorate. 

POTASSIUM  CARBONATE  K2CO3.2H2O. 

SOLUBILITY  IN  WATER. 

(de  Coppet,  1872;  Meyerhoffer,  1905;  Osaka,  1910-12,  Kremann  and  Zitek,  1909;  de  Waal,  1910; 

Mulder,  1864.) 


Gms.  K2CO3 

t°.  per  100  Gms. 

Sat.  Solution. 

—  io  21.3 

-20  31 

-30  36.9 

—  36.5  Eutec.  39.6 

—  6 . 8  tr.  pt.  50 . 9 

0  Si-3 

-fio  52 

20  52.5 

25  •  52-8 

30  53-2 


Solid  Phase. 
Ice 


Gms.  K2 


per 
Sat. 


K2CO3.*H2O+K2C03.2H2O 
K2CO3.2H2O 


40 
50 
60 

70 

80 

90 

100 

no 

120 
130 


100  Gms. 

Solid  Phase. 

..  Solution. 

53-9 

K2CO3.2H20 

54-8 

" 

55-9 

d 

57-i 

« 

58.3 

« 

59-6 

H 

60.9 

u 

62.5 

« 

64.4 

« 

66.2 

11 

Single  determinations,  not  in  good  agreement  with  the  above,  are  given  by 
Kohler  (1897),  by  Engel  (1888),  and  by  Greenish  and  Smith  (1901). 

POTASSIUM   BiCARBONATE   KHCO3. 

SOLUBILITY  IN  H2O.    (Dibbets,  1874.) 

t°.  o        io        20        30        40        60 

Gms.  KHCO3  per  100  Gms.  Sat.  Sol.  18.3     21.7     24.9     28.1     31.2     37.5 
100  gms.  sat.  aqueous  solution  contain  18.7  gms.  KHCO3  at  o°  (d  =  1.127) 
(Engel,  1888);  23.7  gms  KHCO3  at  15°  (Greenish  &  Smith,  1901);  26.3  gms.  at 
20°  (de  Forcrand,  1909). 


509  POTASSIUM   CARBONATE 

SOLUBILITY  OF  POTASSIUM  BICARBONATE  IN  AQUEOUS  SOLUTIONS  OF 
POTASSIUM  CARBONATE  AT  o°.    (Engei,  1888.) 


Milligram  Mols.  per  i    cc.  Solution.        Sp.  Gr.  of 

Grams  per  100  cc.  Soluti 

iKgCOs. 

KHC03    '           Solutions. 

'  K2CO». 

KHCO3. 

O-O 

21.15 

•133 

o.o 

21.2 

17.14 

15.28 

.182 

ii.  8 

15-3 

24.10 

12.65 

.20 

16.7 

12.6 

34-50 

10.25 

.241 

23.8 

10.3 

49-20 

7-55 

.298 

34-o 

7.6 

62  .14 

5.86 

•350 

43  -o 

5-9 

74.60 

4.90 

•398 

51.6 

4-9 

87.50 

3-75 

.448 

60.5 

3-8 

"7-75 

o.o 

•542 

81.4 

o.o 

SOLUBILITY  OF  POTASSIUM  CARBONATE  IN  AQUEOUS  SOLUTIONS  OF  POTASSIUM 
CHLORIDE  AND  OF  POTASSIUM  HYDROXIDE  AT  30°.    (de  Waal,  1910.) 

Results  for  K2CO3  +  KC1.  Results  for  K2CO3  +  KOH. 

Gms.  per  100  Gms.  Sat.  Sol.  Gms.  per  100  Gms.  Sat.  Sol. 

Solid  Phase. 


K2C03. 

KC1. 

OU11U.  JTllit&C. 

K2C03. 

KOH. 

53-27 

0 

K2C03.i*H20 

53.27 

0 

52.22 

1.03 

"  +KC1 

2.50 

53-77 

51-66 

1.07 

KC1 

2.05 

55-14 

1.64 

26.22 

" 

O 

55-75 

0 

28.01 

" 

"  +KOH.2H2O 
•     KOH.2H20 

loo  gms.  H2O  dissolve  10.76  gms.  K2CO3  +  2.66  gms.  KNO3  at  10°  when  both 

salts  are  present  in  excess.  (Kremann  and  Zitek,  1909.) 

IOG  gms.  H2O  dissolve  10.53  gms.  K2CO3  +  6.12  gms.  Na2CO3  at  10°  when 
both  salts  are  present  in  excess  (Kremann  and  Zitek,  1909).  See  also  Potassium 
Sodium  Carbonate,  p.  512. 

Data  for  aqueous  solutions  of  K2CO3  +  KNO3  +  Na2CO3  +  NaNO3,  simul- 
taneously saturated  with  two  or  more  of  the  salts  at  10°  and  at  25°,  are  also 
given  by  Kremann  and  Zitek  (1909). 

Data  for  the  reciprocal  salt  pairs  K2CO3  +  BaSO4  <=*  K2SO4  +  BaCO3  at  25°, 
80°  and  100°  are  given  by  Meyerhoffer  (1905). 

An  aqueous  solution,  simultaneously  saturated  with  K2CO3.2H2O,  K2SO4  and 
BaCO3,  contains  53.1  gms.  K2CO3  +  0.023  gm-  K2SO4  at  25°.  (Meyerhoffer,  1905.) 

EQUILIBRIUM  IN  THE  SYSTEM  POTASSIUM  CARBONATE,  ETHYL  ALCOHOL  AND 

WATER  AT  2^0-260.     (Frankforter  and  Frary,  1913-) 

NOTE.  —  The  binodal  curve  for  the  system  (see  note,  p.  287)  was  very 
carefully  determined  and  tie  lines  were  located  by  estimations  of  K2CO3  in  spe- 
cially prepared  conjugated  liquids.  The  original  results  have  been  plotted  and 
the  following  data  for  the  conjugated  layers  read  from  the  curve: 

Alcohol  Rich  Layer  (Upper)  Water  Rich  Layer  (Lower.) 

Gms.  per  100  Gms.  Solution.  Gms.  per  100  Gms.  Solution. 


K2C03. 

C2H5OH. 

H20. 

K2C03. 

C2H5. 

H20. 

0.095 

90.65 

9-255T 

53-6 

0.28 

46.12! 

0.241 

72.7 

27.059 

39-n 

I 

59-89 

1.72 

53-5 

44.78 

29.62 

4 

66.38 

4.03 

42.6 

53-37 

25-7 

6.4 

67.9 

6.30 

35-5 

58.2 

21.08 

ii 

67.92 

8.29 

31 

60.71 

I9-I5 

13-2 

67.65 

10-35 

27 

62.65 

18.18 

14.7 

67.12 

14.2 

20.5 

65.3 

14.2 

20.5 

65.3* 

*  Plait  point. 

t  Quad,  point. 

The  authors  give  a  complete  summary  of  previous  investigations  of  this  system 
by  de  Bruyn  (1899,  1900);  Bell  (1905);  Cuno  (1908-09). 


POTASSIUM  CARBONATE  510 

Data  for  the  conjugated  liquid  layers  obtained  in  the  system  potassium  car- 
bonate, ethyl  alcohol  and  water  at  17°  and  at  35°  are  given  by  de  Bruyn  (1900) 
and  at  20°,  40°  and  60°  by  Cuno  (1908). 

COMPOSITION  OF  THE  CONJUGATED  LIQUIDS  WHICH  ARE  IN  EQUILIBRIUM  WITH 
SOLID  POTASSIUM  CARBONATE  (QUADRUPLE  POINTS)  AT  VARIOUS  TEMPERATURES. 

(de  Bruyn,  1900.) 
Cms.  per  100  Cms.  Upper  Layer.  Cms.  per  100  Cms.  Lower  Layer. 

K2CO3. C2HBOH.  HA  K2CO3. C2H6OH.  H^T 

— 18          0.03  90.3  9.7  51.2  0.2  48.6 

o         0.04  91.9  8.1  51.3  0.2  48.5 

+  17  0.06  91.5  8.4  52.1  0.2  47.7 

35          0.07  90.9  9  53.4  0.2  46.4 

50         0.09  91.8  8.1  55.3  0.2  44.5 

75          °-12  Qi-4  8.5  57.9  0.2  41.9 

EQUILIBRIUM  IN  THE  SYSTEM  POTASSIUM  CARBONATE,  METHYL  ALCOHOL, 
WATER  AT  23°-26°. 

(Frankforter  and  Frary,  1913.) 

The  authors  give  the  data  for  the  binodal  curve  and  the  quadruple  points 
but  tie  lines,  other  than  for  the  quadruple  points,  were  not  determined. 

Gms.  per  100  Grns.  Homogeneous  Liquid.  Cms.  per  100  Gms.  Homogeneous  Liquid. 


K2C03. 

CH3OH. 

H20. 

K2C03. 

CH3OH. 

H20. 

6.32 

75.85 

17.83* 

21.  6l 

33-43 

44.96 

6.91 

63-I3 

29.97 

23-15 

31.26 

45.60 

8.07 

59.26 

32-67 

28.25 

23-82 

47-94 

IO.I7 

52.64 

35-33 

30.72 

20.57 

48.71 

12.03 

49-97 

37-99 

32.92 

17.27 

49.80 

14.24 

45-74 

40.02 

40.65 

9.26 

50.09 

16.48 

41.76 

41.76 

43-95 

6.96 

49.09 

18.89 

37-76 

43-36 

45-89 

6.42 

47.69 

49-05 

6.1 

44-88t 

*  Upper  quad,  point.  f  Lower  quad,  point. 

The  following  results  for  the  solubility  of  K2CO3  in  concentrations  of  aq. 
CHjOH  above  and  below  those  yielding  liquid  layers  are  also  given. 

Gms.  per  100  Gms.  Sat.  Sol.  Gms.  per  100  Gms.  Sat.  Sol. 

CHjOH.  K2CO3.  fCH3OH.  K2CO3. 

1-03  51.39  85  2.05 

2.22  50.33  89.2  1.56 

6.1  49  .  05   (Lower  quad,  pt.)  91  I  •  98 

Two  Liquid  Layers  Formed  Here.  93-6  2.72 

75.85  6.32   (Upper  quad  pt).  94-3  5-7       (Abs.  CH3OH). 

Data  for  the  binodal  curves  for  this  system  at  17°  and  at  35°  are  given  by 
de  Bruyn  (1900). 

m  This  author  also  gives  the  following  data  for  the  composition  of  the  conjugated 
liquids  in  equilibrium  with  solid  potassium  carbonate  (quadruple  points)  at 
various  temperatures. 

Gms  per  100  Gms.  Upper  Layer.  Gms.  per  100  Gms.  Lower  Layer. 

CH3OH.  H/X 


K2C03. 

CH3OH. 

H20. 

-30 

21.7 

42.2 

36.1 

—  2O 

13-8 

52.1 

34-1 

—  20 

12.4 

.  .  . 

.  .  . 

0 

7.6 

66.3 

26.1 

0 

7-4 

. 

+17 

6.2 

69^6 

24.2 

35 

5 

72.9 

22.1 

44.2  8.2  47.6 

46.3  6.7  47 
46.6  6.6  46.8 
48.3  5.7  46 
51  4.3  44.7 


5ii  POTASSIUM  CARBONATE 

EQUILIBRIUM  IN  THE  SYSTEM  POTASSIUM  CARBONATE,  NORMAL  PROPYL 
ALCOHOL  AND  WATER  AT  22°-26°. 

(Frankforter  and  Frary,  1913.) 

The  authors  give  the  data  for  the  binodal  curve  and  the  quadruple  points 
but  tie  lines  were  not  located. 

Cms.  per  100  Cms.  Homogeneous  Liquid.  Cms.  per  100  Cms.  Homogeneous  Liquid. 


K2C03. 

C3H7OH. 

H20 

K2C03. 

CaH7OH. 

HA 

52.9 
46.98 

O.O2 
0.12 

47-08* 
52-91 

7-45 
5-97 

9-30 
11.07 

83-25 
82.96 

39 

0.20 

60.80 

4-73 

12.71 

82.56 

34-58 

0.20 

65-I5 

3-86 

14.60 

81.54 

3°  -43 

0-45 

69.12 

3-n 

17.17 

79.71 

26.51 

0.78 

72.71 

2.42 

24.71 

72.87 

22.81 

1.32 

75-87 

1.91 

34-90 

63.19 

19.08 

2-31 

78.62 

1.71 

39 

59-29 

16.35 

3-24 

80.41 

i-33 

45-57 

53-09 

13-47 

4.41 

82.12 

0.948 

51-56 

47-49 

10.99 

6.24 

82.77 

0.387 

64.20 

35-41 

8-55 

8-31 

83-14 

0.017 

95-83 

4-i53t 

Lower  quad,  point.  t  Upper  quad,  point. 

EQUILIBRIUM  IN  THE  SYSTEM  POTASSIUM  CARBONATE,  ISOPROPYL  ALCOHOL 
AND  WATER  AT  20°. 

(Frankforter  and  Temple,  1915.) 

NOTE.  —  The  results  for  the  binodal  curve  in  this  and  the  following  system  are 
reported  in  terms  of  gms.  per  100  gms.  solvent  (water  +  alcohol)  instead  of  gms. 
per  100  gms.  of  homogeneous  liquid  (K2COa  +  water  +  alcohol.) 

Gms.  per  100  Gms.  Alcohol  +  Water.  Gms.  per  100  Gms.  Alcohol  +  Water. 


K2C03. 

Alcohol. 

Water. 

K2C03. 

Alcohol. 

Water. 

44.844 

2.911 

97.089 

15.021 

19-445 

80.555 

36.137 

4.783 

95-217 

I3-244 

23.919 

76.081 

28.879 

7-349 

92.651 

6.065 

45-397 

54-603 

24.152 

9-159 

90.841 

3-933 

53-265 

46.735 

17.665 

14-395 

85-605 

2-954 

57-294 

42.706 

EQUILIBRIUM  IN  THE  SYSTEM  POTASSIUM  CARBONATE,  ALLYL  ALCOHOL  AND 

WATER  AT  20°. 

(Frankforter  and  Temple,  1915.) 
Gms.  per  100  Gms.  Alcohol  -{-  Water.  Gms.  per  100  Gms.  Alcohol  +  Water. 


K2CO8.  Alcohol.  Water.  K2CO3.  Alcohol.  Water. 

47.746  2.103  97.897  8.239  30-677  69.323 

33.200  5.267  94-733  5-521  39-337  60.663 

23.486  9-309  90.691  2.020  54-487  45-513 

16.354  15-037  84.963  1.015  62.610  37-390 

11.331  22.454  77-546  0.0853  81.228  18.772 

EQUILIBRIUM  IN  THE  SYSTEM  POTASSIUM  CARBONATE,  ACETONE,  WATER  AT  20°. 

(See  also  Acetone,  p.  1 3) .      (Frankforter  and  Cohen,  1914.) 

The  binodal  curve  was  very  carefully  determined  and,  in  addition,  data  for  the 
quadruple  points  (solid  K2CO3)  and  five  tie  lines  were  located.  These  data  were 
plotted  and  the  following  interpolated  values  for  the  conjugated  liquids  read 
from  the  curve. 

Gms.  per  100  Gms.  Upper  Layer.  Gms.  per  100  Gms.  Lower  Layer. 


K2C03. 

(CH3)2CO. 

H20. 

K2CO3.            (CH3)2CO. 

H20. 

0.0024 

96.4 

3-5+t 

52.4               trace 

47-  6f 

0.039 

64 

35-96 

32-63                 1.2 

66.17 

0.712 

55-3 

43-99 

24-4                  3-7 

71.9 

1.36 

48.5 

50.14 

22.91                 4.7 

72-39 

4-57 

34 

61.43 

16.92               10.2 

72.88 

6-97 

27-5 

6S-53 

14-77               13 

72.23 

10.5 

20 

69-5* 

10.5                       20 

69.5 

*  Plait  point. 

t  Quad,  points. 

POTASSIUM   CARBONATE 


512 


EQUILIBRIUM  IN  THE  SYSTEM  POTASSIUM  CARBONATE,  POTASSIUM  DIPROPYL 
MALONATE  AND  WATER  AT  25°. 

(M 'David,  1909-10.) 

A  series  of  mixtures  of  K2CO3  +  KCuHwOi  +  H2O  were  prepared  and  thoroughly 
mixed.  They  were  placed  in  a  thermostat  at  25°  and  the  two  layers  which  sep- 
arated in  each  case,  were  analyzed. 

Cms.  per  100  Gms.  Upper  Layer.  Cms.  per  100  Cms.  Lower  Layer. 


K2C03. 

KCUH1904. 

H20. 

4-05 

65-1 

30-85 

4-9 

59-8 

35-3 

5-6 

53-5 

40.9 

7.2 

.50-5 

42.3 

8-7 

39-2 

S2.i 

ii 

34-6 

54-4 

14-5 

23-5 

62 

17 

18.6 

64-4 

18.6 

15 

66.4 

K2C03. 

KCUH1904. 

H20. 

42.6 

0.4 

57 

40-7 

0.4 

58-9 

35 

0-5 

64.5 

33-5 

0.9 

65-6 

28.9 

0.7 

70.4 

26.8 

0.8 

72.4 

24.8 

•       3 

72.2 

23-1 

6.05 

70.8- 

21.7 

8-7 

69.6' 

Several  determinations  at  2°  and  at  56°  are  also  given. 

100  cc.  anhydrous  hydrazine  dissolve  I  gm.  K2CO3  at  room  temp. 

(Welsh  and  Broderson,  1915.) 

loo  gms.  aqueous  solution  simultaneously  sat.  with  K2CO3  and  cane  sugar  at 
31.25°  contain  22.24  gms-  K2CO3  and  56  gms.  sugar.  (Ktihler,  1897.) 

Freezing-point  data  for  mixtures  of  K2CO3  +  KC1  and  K2CO3  +  NaCl  (Sackur, 
1911-12).  K2CO3  +  K2SO4  (Amadori,  1912;  Le  Chatelier,  1894);  K2CO3 
+Na2CO3  (Le  Chatelier,  1894).  (Le  Chatelier,  1894.) 

POTASSIUM   Sodium   CARBONATE   K2CO3.Na2CO3.i2H2O. 

SOLUBILITY  IN  WATER  AT  25°. 

(Osaka,  1910-11.) 


Gms.  per  100  Gms.  Sat.  Sol. 


Gms.  per  100  Gms.  Sat.  Sol. 


K2C03. 

Na2C03.  ' 

K2C03. 

Na,C03. 

52.83 

o          K2CO3.2H2O 

25.2 

14.1 

52 

I              " 

22.4 

16.6 

50.7 

2.6 

19.8 

18.7 

.  49-1 

4.6          "  -f-KzCOa.NajCOa.isHzO 

19.1 

19.7 

49 

4  .  6          K2CO3.Na2CO3.i  2H2O 

23.2 

46.5 

4-3                         " 

14.5 

22.8 

46.2 

5-  2 

10.8 

22.7 

41 

6-3 

10.7 

22.4 

37-7 

7 

4-7 

21.9 

31 

10.5 

o 

22.71 

Solid  Phase. 


+Na2CO3.ioH2O 
Na2C03.ioH2O 


The  previous  determinations  of  Kremann  and  Zitek  (1909),  agree  in  general 
with  the  above,  but  these  authors  report  that  the  double  salt  contains  6H2O 
instead  of  I2H2O. 

100  gms.  H2O  dissolve  184  gms.  potassium  sodium  carbonate  at  15°  (d  =  1.366). 

(Stolba,  1865.) 

POTASSIUM  URANYL  CARBONATE  2K2CO3.(UO2)CO3. 

loo  gms.  H2O  dissolve  7.4  gms.  salt  at  15°.  (Ebelmen,  1852.) 

POTASSIUM   CHLORATE   KC1O3. 

SOLUBILITY  IN  WATER. 

Average  curve  from  results  of  Carlson  (1910),  Calzolari  (1912),  and  Tschugueff  and  Chlopin  (1914). 


O 
10 

15 

20 

25 
30 


d  of  Sat.  Sol. 

Gms.  KC1O3  per 
100  Gms.  H2O. 

I.O2I 

3-3 

L 

1.045 

7-4 
8.8 

10.5 

40 

£ 

80 
100 
104  b.  pt. 


d  of  Sat.  Sol. 

Gms.  KC1O3  per 
100  Gms.  H20. 

1.073 

14 

19-3 

1.115 
1.165 

24-5 
38.5 

1.219 
1.230 

57 
60 

For  previous  results  in  good  agreement  with  the  above,  see  next  page. 


513 


POTASSIUM  CHLORATE 


POTASSIUM   CHLORATE   KC1O3.     (See  also  previous  page.) 
SOLUBILITY  IN  WATER. 

(Gay-Lussac,  1819;  Pawlewski,  1899;  above  100°,  Tilden  and  Shenstone,  i88i;'see  also  Blarez, 
1891;  Etard,  1894;  at  99°,  Kohler,  1879.) 


Gms.  KClOg  per  100  Gms. 


O 
10 
20 
25 
30 
40 

50 
60 


Solution. 

w 

ater. 

3-04 

3-i4 

3-3* 

4.27 

4-45 

5  -° 

6.76 

7.22 

7.1 

7-56 

8.17 

8.6 

8.46 

9.26 

10.  1 

ii  .75 

I3-31 

14-5 

15.18 

17-95 

19.7 

18.97 

23.42 

26.0 

t°. 


Gms.  KC1O3  per  100  Cms. 


Solution. 


Water. 


70  22-55 

80  26.97 

90  3I-36 

loo  35-83 

I2O  42.4 

136  49-7 

190  64.6 

330  96.7 
*  Gay  Lussac. 

ioo  gms.  H2O  dissolve  5.06  gms.  KC1O3  at  10°. 

One  liter  of  H2O  dissolves  65.5  gms.  KCJO3  at  about  20' 


29.16   32.5* 


46.11 
55-54 
73-7 
98-5 
183.0 
2930-00 


39-6 

47-5 
56.0 

73-7 

99.0 

183.0 


(Roozeboom,  1891.) 

_  (Konowalow,  iSggb.) 

One  liter  of  5.2  %  NH3  solution  dissolves  52.5  gms.  KC1O3  at  about  20°.       " 

SOLUBILITY  OF  POTASSIUM  CHLORATE  IN  AQUEOUS  SOLUTIONS  OF  POTASSIUM 
HYDROXIDE,  HYDROGEN  PEROXIDE,  AND  MIXTURES  OF  THE  Two  AT  25°. 

(Calvert,  1901.) 

The  mixtures  were  agitated  by  means  of  a  stream  of  air.     Equilibrium  was 
approached  both  from  above  and  below  25°. 

Mols.  KClOj          Gms.  KC1O3 
Dissolved  per         Dissolved  per 
Liter  of  Sat.  Sol.   Liter  of  Sat.  Sol. 


Composition  of  Solvent. 


Water  alone 

Aqueous  o.  125  n  KOH 

0.25    n     " 
Aq.  H2O2       containing  i .  26    mols.  H2O2  per  1. 

1.31 

Aq.  0.25  n  KOH          '          0.015 
0.276 

0-954 
1.073 

SOLUBILITY  OF  POTASSIUM  CHLORATE  IN  AQUEOUS  SOLUTIONS  OF 


0.675 

82.71 

0.625 

76.60 

0.573 

70.23 

erl. 

0.730 

89-45 

« 

0.737 

90.33 

« 

0.578 

70.82 

« 

6.584 

71-57 

1C 

0.616 

75-50 

(( 

0.673 

82.47 

POTASSIUM 

Gms.  per  ioo  Gms. 
Solution. 

BROMIDE  AT  13°. 

Gms.  per  ioo  Gms. 
Solution. 

(Blarez,  i 
Gms. 

per  ioo  Gms. 
Solution. 

'KBr. 
0.20 
0.60 
0.8 

KC103.  " 

5.18 
5.20 
5-06 

'KBr. 
1-0 
2.0 

3-o 
4-0 

KC1O3. 

5-04 
4.60 
4-2 
4-0 

KBr. 
6.0 
8.0 
IO-O 

KC1CV 
3-46 
2.8o 
2.40 

SOLUBILITY  OF  POTASSIUM  CHLORATE  IN  AQUEOUS  SOLUTIONS  OF  OTHER 
POTASSIUM  SALTS  AT  14°-!  5°.    (Blarez, 


K  Salt. 

KC103. 

oaii.        f 

K  Salt. 

KC103. 

KOH 

1-43 

4-47 

KNO3 

2-59 

4-51 

KC1 

1.91 

4-45 

M 

5-i8 

3-88 

" 

3-82 

3-58 

K^SO, 

2.23 

4-7i 

KBr 

3-05 

4.49 

M 

4.46 

" 

6.10 

3.60 

K2C2O4 

2.42 

4.72 

KI 

4-25 

4-59 

" 

4-85 

3-93 

" 

8.51 

3-65 

POTASSIUM  CHLORATE  514 

SOLUBILITY   OF    POTASSIUM   CHLORATE    IN   AQUEOUS   SOLUTIONS   OF 
POTASSIUM  CHLORIDE  AT  20°. 

(Winteler  — Z.  Electrochem.  79  360,  'oo.> 


Sp.  Gr.  of 

Grams  per  Liter. 

Sp.  Gr.  of 

Grams 

F>er  Liter. 

Solutions. 

KC1.                KC103. 

Solutions. 

KC1. 

KC103: 

1.050 

o             71.1 

1.098 

120 

24-5 

1.050 

10            58.0 

I.IOS 

140 

22.5 

1.050 

20                 49-0 

I  .119 

160 

21.0 

1.054 

40            39-5 

I.I30 

180 

20.  o 

I  .064 

60          34.0 

I.I40 

200 

2O  *} 

1-075 

80            30.0 

I.I68 

250 

20.  o 

1.  086 

ioo            27.0 

SOLUBILITY   OF   POTASSIUM   CHLORATE   IN   AQUEOUS   SOLUTIONS   OP 
POTASSIUM  NITRATE. 

(Arrhenius  —  Z.  physik.  Chem.  n,  397,  '93.) 


Results  at  19.85' 


Mols.  per  Liter. 


Grams  per  Liter. 


Results  at  23.87°. 

Mols.  rjer  Liter.  Grams  per  Liter. 


KNO3. 

KC103." 

'KN03. 

KC103"      "  KN03.        KC1O3" 

KN03. 

KC103. 

O 

•  O 

0 

570 

O 

.O 

69. 

88        o.o      0.645 

O 

•  o 

79 

.09 

O 

•125 

o. 

529 

12 

•65 

64- 

86        0.5      0.515 

50 

•59 

63 

.14 

O 

•25 

o 

492 

25 

.29 

60. 

33 

I 

.0 

o 

•374 

IOI 

.19 

45- 

85 

2 

.0 

0 

•328 

2O2 

•38 

40. 

22 

SOLUBILITY  OF  POTASSIUM  CHLORATE: 

(Taylor,  1897;  see  also  Gerardin,  1865.) 


In  Aqueous  Alcohol. 


In  Aqueous  Acetone. 


Wt.  per  cent  „      At3°- 
Alcohol  or    Gms.  KC103per 
of  Acetone         ioo  Gms. 

At  40°. 
Gms.  KClOg  per 
ioo  Gms. 

At  30°. 
Gms.  KC1O3  per 
ioo  Gms. 

At  40°. 
Gms.  KC1O3  per 
ioo  Gms. 

insolvent.  Soiution 

.     Water. 

Solution. 

Water. 

Solution. 

Water. 

Solution. 

Water. 

O 

9-23 

IO 

•17 

12.23 

J3-93 

9 

•23 

10 

•17 

12.23 

13-93 

5 

7-7« 

8 

.80 

10.48 

12  -33 

8 

•32 

9 

•56 

II  .10 

I3.II 

10 

6.44 

7 

•65 

8.84 

10.77 

7 

.63* 

9 

.09 

10.28* 

12  .60 

20 

4-51 

5 

.90 

6.40 

8.56 

6 

.09 

8 

.10 

8.27 

II  .26 

30 

3-21 

4 

•74 

4.67 

7.00 

4 

•93 

7 

.40 

6.69 

10.24 

40 

2-35 

4 

.00 

3-41 

5-88 

3 

.90 

6 

.76 

5-36 

9-45 

50 

i  .64 

3 

•33 

2-41 

4-94 

2 

.90 

5 

.98 

4-03 

8.40 

60 

I  .01 

2 

•53 

I.4I 

3-69 

2 

•03 

c 

•17 

2.86 

7-35 

70 

0-54 

I 

.82 

0.78 

2.63 

I 

.24 

4 

.18 

1.68 

5.68 

80 

0.24 

I 

.22 

o-34 

J-73 

O 

•57 

2 

.88 

o-79 

3-97 

90 

0-06 

0 

.62 

O-I2 

1.17 

0 

.18 

I 

,82 

0.24 

2-45 

*  Solvent,  9.09  Wt.  per  cent  Acetone. 

ioo  gms.  sat.  solution  of  KC1O3  in  glycol  contain  0.9  gms.  KC1O3. 

(de  Coninck,  1905.) 


515 


POTASSIUM  CHLORATE 


SOLUBILITY  OF  POTASSIUM  CHLORATE  IN  AQUEOUS  SOLUTIONS  OF  VARIOUS 

COMPOUNDS  AT  25°.     (Rothmund,  1910.) 

Aqueous  0.5  Normal 
Solution  of: 

Water  alone 
Methyl  Alcohol 
Ethyl  Alcohol 
Propyl  Alcohol 
Tertiary  Amyl  Alcohol 
Acetone 
Ether 
Glycol 
Glycerol 
Urea 
100 gms.  glycerol  (du  =  1 .256)  dissolve  3.54 gms.  KC1O3 at  15-16°.  (Ossendowski,  1907.) 

POTASSIUM   PerCHLORATE  KC1O4. 

SOLUBILITY  IN  WATER. 

(Average  curve  from  results  of  Noyes  and  Sammet  (1903);  Carlson  (1910);  Rosenheim  and  Weinhaber 
(1910-11);  Calzolari  (1912);  Thin  and  Gumming  (1915). 


KC1O3  per  Liter. 

Aqueous  0.5  Normal 

KC1O3  per  Liter. 

Mols. 

Gms. 

Solution  of: 

Mols. 

Gms. 

O. 

1475 

20. 

44 

Ammonia 

O. 

1474 

2O 

•43 

Q- 

1402 

19. 

43 

Dimethylamine 

0. 

1342 

18 

.66 

0. 

1356 

18. 

75 

Pyridine 

0. 

1410 

19 

•54 

0. 

1343 

18. 

61 

Urethan 

O. 

1400 

19 

.40 

0. 

1279 

17- 

72 

Formamide 

0. 

J539 

21.32 

0. 

1451 

20. 

ii 

Acetamide 

0. 

1447 

20 

•05 

0. 

1336 

18. 

51 

Acetic  Acid 

O. 

1462 

2O 

.26 

0. 

1416 

19. 

62 

Phenol 

0. 

1362 

18 

.87 

0. 

1404 

19. 

45 

Methylal 

0. 

1400 

19 

.40 

0. 

1510 

20. 

92 

Methyl  Acetate 

0. 

1429 

19 

.80 

O 
10 
2O 
25 
30 

40 


doi 
Sat.  Sol. 

1.007 


Gms.  KC1O4  per 
ioo  Gms.  H2O. 

0-75 


<f  of 

Gms.  KC1O4  per 

t  . 

Sat.  Sol. 

ioo  Gms.  Sat.  Sol. 

50 

6-5 

60 

1-033 

9 

70 

.  .  . 

ii.  8 

80 

1-053 

14.8 

90 

.  .  . 

18 

IOO 

1.067 

21.8 

01 Oil  I. 80 

1. 012  2.08 
2.6 

1.022  4.4 

SOLUBILITY  OF  POTASSIUM  PERCHLORATE  IN  AQUEOUS  AND  IN  ALCOHOLIC 
SOLUTIONS  OF  PERCHLORIC  ACID  AT  25.2°. 

(Thin  and  Gumming,  1915.) 

In  Alcoholic  HC1O4  Solutions. 

Aqueous  Solvent.  x^S^S&g 

2.085  93.5%  Alcohol  0.051 

1.999  "  +o.2%HC104*  o.OI75 

o.io  1.485  98.8%  Alcohol  +  o.oio 

i  0.527  "  +2%HC1O4*  0.028 


In  Aq.  HC1O4  Solutions. 

Normality  of  Aq.      Gms.  KC1O4 
HC1O4.  loo  Gms.  Sat. 

o  (=  water) 
o.oi 


The  HC1O4  was  added  as  aq.  20%  HC1O4  solution  hence  the  concentration  of  the  alcohol  was  decreased. 


SOLUBILITY  OF  POTASSIUM  PERCHLORATE  IN  AQ.  KC1  AND  AQ.  K2SO4 

SOLUTIONS  AT  25°.      (Noyes  and  Boggs,  1911.) 
In  Aq.  KC1  Solutions. 
Grns^per  100.2  cc.  Sat.  Sol.         wt.  of  100.2  cc. 
of  Solution. 


101.42 

101.45 


In  Aq.  K2SO4  Solutions. 

Gms.  per  100.2  cc.  Sat.  Sol.         \yt.  of  100.2  cc. 
KC1O4.  K2SO4.  of  Solution. 

2.0566        o 

1.8262     0.4339      101.47 
1.6396     0.8665      101-55 


KC1O4.  KC1. 

2  .0566  O 

1.7800  0.3715 

x-5597         0.7421 
ioo  gms.  51.2  Vol.  %  Aq.  C2H6OH  (d  =0.9319)  dissolve  0.754   gpi.  KC1O4  at  25.2°. 

(Thin  and  Gumming,  1915.) 

93-5  (^=0.8219)  0.051    gm.  KC1O4  at  25.2°. 

(Thin  and  Gumming,  1915.) 

98.8  (^  =  0.7998)        "       0.019    gm.  KC1O4  at  25.2°. 

(Thin  and  Gumming,  1915.) 

90    Wt.  %  Aq.  C2H6OH  "      0.036   gm.  KC1O4  at  25.2°. 

4«  « 


97.2 


(Wenze,  1891.) 

0.0156  gm.  KC1O4  at  25.2°. 
(Wenze,  1891.) 


POTASSIUM  CHLORIDE  516 

POTASSIUM    CHLORIDE    KC1. 

SOLUBILITY  IN  WATER. 


(Average  curve  from  the  results  of  Meusser  —  Z.  anorg.  Chem.  44,  79,  '05;  at  31.25°,  Kohler  —  Z. 
Ver.  Zuckerind.  47,  447,  '07;  Andrae  —  J.  pr.  Chem.  [2]  29,  456,   '84;  Gerardin  —  Ann.  chim.  phys. 
[4]  St  i37.  '65;  de  Coppet  Ibid.  [5]  30,  411,  '83;  Etard  Ibid.  [7]  2,526,  '94;  Mulder;  above  100°,  Tilden 
and  Shenstone  —  Proc.  Roy.  Soc.  (Lond.)  35.  345.  '83-) 

to 

Gms.  KC1  per  100  Gms. 

X0   Gms.  KCl  per  ioo  Gms. 

t° 

Gms.  KCl  per  ioo 

Gms. 

Solution. 

Water. 

Solution. 

Water. 

Solution. 

Water. 

-9 

19 

•3 

23 

•9 

40 

28.6 

40 

.0 

147 

41-5 

70.8 

-4' 

5  20 

.6 

25 

•9 

50 

29.9 

42 

.6 

180 

43-7 

77-5 

0 

21 

.6 

27 

.6 

60 

3J-3 

45 

q 

Solid  Phase 

Ice 

5 

22 

•7 

29 

•3 

70 

32.6 

48 

3 

-9 

19-3 

23-9 

10 

23 

•7 

31 

.0 

80 

33-8 

51 

i 

-8 

•     17-7 

21  -5 

15 

24 

•5 

32 

•4 

90 

35  -,1 

54 

.0 

-8 

16.7 

20.0 

20 

25 

•4 

34 

.0 

IOO 

36.2 

56 

•7 

-7 

14.9 

!7-5 

25 

26 

.2 

35 

•5 

130 

39-8 

66 

.0 

-6 

13.6 

15-7 

30 

27 

.1 

37 

.0 

-5 

•5  I2-5 

14-3 

Sp.  Gr.  of  solution  sat.  at  o  =  °i.i5o;  at  15°  =  1.172. 

The  following  determinations  of  the  solubility  of  potassium  chloride  in  water, 
made  with  exceptional  care,  are  reported  by  Berkeley  (1904). 

*o  d  of  Gms.  KCl  per  ioo  «  d  of          Gms.  KCl  per  ioo 

Sat.  Sol.  Gms.  H2O.  t  '  Sat.  Sol.  Gms.  H2O. 

0.70       I.I540  28.29  74.80  1.2032  49.58 

19.55   1-1738    34-37       89.45     1.2069    53-38 
32.80  1.1839    38-32       108  (b.  pt.)  1.2118    58.11 

59.85    1.1980       45.84 

IOO  gms.  H2O  dissolve  36.12  gms.  KCl  at  25°.  (Amadoriand  Pampanini,  1911.) 

F.-pt.  data  for  aq.  KCl  solutions  are  given  by  Roloff  (1895). 
Data  for  equilibrium  in  the  system  potassium  chloride,  arsenic  trioxide  and 
water  at  30°  are  given  by  Schreinemakers  and  de  Baat  (1915). 

SOLUBILITY  OF  POTASSIUM  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  HYDRO- 
CHLORIC ACID  AT  0°  AND  AT  25°. 
(Armstrong,  Eyre,  Hussey  and  Paddinson,  1907;  Armstrong  and  Eyre,  1910-11.) 

Solvent,  Gms.  KCl  per  ioo  Gms.  Sat.  Sol. 

Gms.  HClper  , *- > 

1000  Gms.  H2O.  At  o°.  At  25°. 

O  22.11  26.45 

9.11  20.93  25-J7 

18.22  I9-7I  24.07 

36.45  17.26  21.74 

109-35  •'•  13-47 

182.25  •••  6-93 

SOLUBILITY  OF  POTASSIUM  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  HYDRO- 
BROMIC  ACID  AND  OF  HYDROCHLORIC  ACID  AT  25°.     (Herz,  1911-12.) 

In  Aq.  HBr.  In  Aq.  HC1. 

Millimols  per  10  cc.  Gms.  per  Liter.  Millimols  j>er  10  cc.  Gms.  per  Liter. 

HBr.  KCl.  HBr.  KCl.  HC1.  KCl.  '  HC1.  KCl.' 

o          42.72        o          318.5          5.66  37.49  20.64  279.6 

6.61     37.80      53.5       281.9        I0-20  33-79  37-*9  252 

34.15      19-57     276.4      146  15.91  28.68  57.98  213.9 

20.94  24.74  76.35  146.6 

32.52  17.39  Il8-6  129.6. 


517 


POTASSIUM   CHLORIDE 


SOLUBILITY   OF    POTASSIUM   CHLORIDE    IN   AQUEOUS    SOLUTIONS 
HYDROCHLORIC  ACID  AT  o°. 

(Jeannel  —  Compt.  rend.  103,  381,  '86;  Engel  —  Ann.  chim.  phys.  [6]  13,  377,  '88.) 


OF 


ram  Mols 

per  10  cc. 

Grams  per  ipo  cc.  Solution.     gD-  Qr>  of 

KC1. 

HCI: 

KCl. 

HCI.             Solutions. 

34-5 

o.o 

25-73 

0-0 

•159 

30.41 

3-9 

22  .69 

1.42 

•152 

27-95 

6.6 

20.84 

2.41 

.150 

27-5 

7-i 

20.51 

2.59            ] 

.147 

23-75 

ii  .1 

17.71 

4-05            ] 

•137 

16.0 

23.0 

n-93 

8-39 

.in 

lo.o 

34-o 

7.46 

12.40           3 

.105 

7-5 

41  .0 

5.60 

*4-95 

.105 

2.0 

65-5 

1.49 

23.88 

.121 

2-4 

148.8  (sat.) 

1.52 

54.26 

.224 

100  cc.  saturated  HCI  solution  dissolve  1.9  gms.  KC1  at  17°.  „    (Ditte,  1881.) 

100  gms.  sat.  aq.  HCI  solution  dissolve  1.9  gms.  KC1  at  20°.    (Stoltzenberg,  1912.) 
F.-pt.  data  for  mixtures  of  KC1  and  HCI  are  given  by  Dernby  (1918). 


SOLUBILITY  OF  MIXTURES  OF  POTASSIUM  CHLORIDE  AND  OF  SODIUM  CHLORIDE 
IN  AQUEOUS  HYDROCHLORIC  ACID  SOLUTIONS  AT  25°. 

(Hicks,  1915.) 
Gms.  per  100  Gms.  Sat.  Solutions. 


HCI. 

NaCl. 

KCl. 

0 

19-95 

10.90 

8.61 

10.65 

7-58 

17.16 

3-56 

3.80 

20.65 

2.03 

2.86 

32.78 

0.18 

1.27 

SOLUBILITY  OF  POTASSIUM  CHLORIDE  IN  AQUEOUS  MAGNESIUM 
CHLORIDE  SOLUTIONS. 

(Precht  and  Wittgen  —  Ber.  14,  1667,  '81.) 
Grams  KCl  per  100  Grams  Sat.  Solution  in: 


t°. 

II 
Mg( 

%              15% 

:i2.      MKci2. 

21.2% 

MgCb. 

3°% 

MKC12. 

20%  MgCl2. 

10 

14 

•3 

9 

9 

5-3 

I 

•9 

4 

.2KCl+5.7NaC 

20 

15 

•9 

ii 

,3 

6-5 

2 

.6 

6 

.0 

1   +5-9 

tt 

30 

17 

•5 

12 

•7 

7.6 

3 

•4 

6 

•9 

"   +6.0 

tt 

40 

19 

.0 

14 

.2 

8.8 

4 

.2 

7 

•9 

"   +6.1 

n 

50 

20 

•5 

15 

.6 

IO-O 

5 

.0 

8 

•9 

"   +6-3 

tt 

60 

21 

•9 

17 

•  o 

II.  2 

5 

.8 

9 

•9 

"   +6.4 

tt 

80 

24 

•5 

J9 

•5 

13-6 

7 

•3 

10 

•9 

"   +6.6 

tf 

90 

25 

.8 

20 

.8 

14.7 

8 

.1 

ii 

•9 

"   +6.7 

t( 

100 

27 

.1 

22 

.1 

J5-9 

8 

•9 

13 

.0 

"   +6.9 

u 

More  recent  data  on  the  solubility  of  potassium  chloride  in  aqueous  solutions 
of  magnesium  chloride  are  given  by  Feit  and  Przibylla  (1909). 


POTASSIUM  CHLORIDE  518 

SOLUBILITY  OF  MIXTURES  OF  POTASSIUM  CHLORIDE  AND  POTASSIUM 
BROMIDE  AT  25°. 

(Fock,  1897.) 


Grams  per  Litef 
Solution. 

Milligram  Mols. 
per  Liter. 

M°kcfinCent     Sp.Gr.of 
r-  i     •              Solutions 

Mol.  per  cent 
KCI  in 

KBr. 

KCI: 

KBr. 

KCI. 

Solution. 

Solid  Phase. 

558 

.1 

0 

.00 

4686.2 

O 

.0 

o 

o 

I 

•3756 

o.oo 

.5 

23 

•44 

4462.7 

3*4 

.2 

6 

.16 

I 

.3700 

o.oo 

503 

.6 

46 

•57 

4228.5 

624.3 

12 

.86 

I 

•3648 

8.23 

454 

.6 

82 

.62 

3817.8 

1108 

•  O 

22 

•49 

I 

•3544 

15.68 

379 

.6 

136 

.6 

3I88.I 

1830 

•7 

36 

.48 

I 

•3320 

33-66 

324 

.8 

166 

•9 

2727.6 

2237 

•4 

45 

.06 

I 

•3IJ9 

63-51 

218 

.0 

213 

•9 

1830.2 

2868 

.0 

60 

•30 

I 

.2689 

82.29 

140 

•7 

250 

•9 

1181.1 

3363 

•9 

74 

.01 

I 

•2455 

88.04 

47 

•5 

291 

•7 

398.8 

39" 

•4 

85 

.22 

I 

.1977 

96.98 

o 

.0 

311 

•3 

0-0 

.1 

IOO 

•  OO 

I 

•1756 

100.00 

SOLUBILITY  OF  POTASSIUM  CHLORIDE  IN  AQUEOUS  POTASSIUM 
HYDROXIDE  SOLUTIONS. 

(Engel  — Bull.  soc.  chim.  [3]  6,  16,  '91;  Winteler  — Z.  Electrochem.  7,  360,  'oo.) 


Results  at 

0°. 

Results  at  20°. 

(Engel.) 

(Winteler.) 

Mg.  Mols.  per 
10  cc.  Solution          S>P- 

Gr.  of 

Jution. 

Gms.  per  100  cc. 
Solution. 

Gms.  per  100  cc. 
Solution.          £ 

p.  Gr.  of 

olution. 

KCI. 

KOH. 

KCI. 

KOH. 

KCI.        KOH.  ' 

35-5 

o            1.159 

26.83 

o.o 

29.3       i.o 

.185 

31.0 

2.375       1.146 

23-44 

J-33 

21.  I       IO.O 

•  2IO 

28.3 

4-7        1-153 

21.39 

2.64 

14.8     20.  o 

-245 

23.0 

9.9      1.172 

17-39 

5-56 

IO-4      30.0 

•295 

18.38 

15  1 

•195 

13.89 

8.46 

6.8     40  .  o 

•345 

14-43 

20.  o 

.216 

10.91 

11.23 

4-0     50.0 

•397 

n-43 

24.63 

•239 

8.64 

13-83 

2.2       60  •  O 

•450 

8.98 

29.25 

.261 

6.78 

16.43 

1-4       70.0 

.500 

6.28 

35-*3 

.294 

4-74 

19.72 

I.I       80  .  O 

•550 

0-9      85.0 

.580 

SOLUBILITY  OF  MIXTURES  OF  POTASSIUM  CHLORIDE  AND  POTASSIUM 

IODIDE  IN  WATER. 

(Etard  —  Ann.  chim.  phys.  [7]  3,  275,  '94.) 


Grams  per  TOO  Gms.  Solution 


Grams  per  100  Gms.  Solution. 


*  • 

KCI. 

Kl. 

i  . 

KCI. 

KI. 

o 

3-7 

50-5 

IOO 

6.2 

61  .0 

20 

4.2 

53-o 

140 

7-3 

63-7 

40 

4-7 

55-3 

180 

8-3 

65-5 

60 

5-2 

57-5 

220 

9-4 

66-3 

80 

5-7 

59-4 

245 

IO.O 

66.5 

519 


POTASSIUM   CHLORIDE 


SOLUBILITY  OF  POTASSIUM  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  POTASSIUM 
IODIDE  AT  25°  AND  VICE  VERSA. 

(Amadori  and  Pampanini,  1911.) 


Gms.  per  100  Cms.  H2O. 


KC1. 

KI. 

0 

149  .  26 

4.06 

144.03 

7-63 

137-79 

11.36 

132.60 

11.74 

I33-90 

15.10 

105.91 

Gms.  per  100  Gms.  H2O. 


KC1. 

KI.    ' 

19.64 

68.22 

23-75 

43-89 

29.56 

23-83 

31.38 

14.83 

33-68    ' 

7 

36.12 

o 

SOLUBILITY  OF  POTASSIUM  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  POTASSIUM 
NITRATE  AT  o°  AND  AT  25°. 

(Armstrong  and  Eyre,  1910-11.) 


Solvent,  Gms.  KNO3 

per  1000  Gms. 

H20. 

O 
25.27 

50-55 
IOI.II 

151.66 


Gms.  KC1  Dissolved  per 
zoo  Gms.  Sat.  Solution  at: 


o  . 

22.  IO 
21.71 
21.25 
20.70 


25  • 

26.73 
26.26 
25.61 
24.58 
23-57 


SOLUBILITY  DATA  FOR  THE  RECIPROCAL  SALT  PAIRS  KCl+NaNO3^NaCl+KNO3 

AT   5°,    25°,    50°   AND    IOO°. 

(Reinders,  1914,  1915;  see  also  Uyeda,  1909-10.) 


Results  at  25°. 

Gms.  per  100  Gms.  H20. 

Results  at  50°. 

Gms.  per  100  Gms.  H2O. 

Solid  Phase  in  Each 
Case. 

NaCl 

NaCl+KCl 
KC1 

KC1+KN03 
i                KNO3 

KN03+NaN03 
NaNO, 

NaNOj+NaCl 

NaCl 
NaCl+KCl 
KCl+KNOs 
KNO3+NaNO3 
NaNO3+NaCl    - 
NaCl+NaNO2+KN03 
NaCl+KCl+KNO3 

NaCl.         KC1. 
36  .  04 
32.28     10 
30.27      16.45 
12               26.78 

35-54 
34.92 

IO 
IO 

23.62 
33-90 

24.82        22.2 
21.36        2O 
24-5 

23.8    ::: 

4-5 

NaNO3. 
10 

60 
100.9 
96.06 
77.46 
58.01 

IO 

15-4 

61.3 

82.1 
64 

KNO3. 
IO 

22.79 
31.48 
37-49 
41.87 

46.15 
20 

32-9 

17.2 

43-15 
41.2 

40-3 

NaCl. 
36.72 

28  .'35 

KC1.      NaNO3. 

23.09        ... 
42  .  80 
41-39        ..- 
38.75        .-. 

KN03. 

24.05 
52.54 
85.10 

20.5 
28.4 
34 
12.7 

...      134.9 
...      114.1 

...        84.8 
...       43-9 
13-4 
25-4 

90.2 

24-3 
58.6 

19.2 

12.2 

59-9 

104  .  i 
110.7 
6.1 

27.2 
82.2 
70.9 

31-50 


27.6 


Results  at  5*. 


10.4 
29.84 


82.10 
41.7 


10.14 
18.1 


27.3 


19.2 


Results  at  iooc 


36-2 
41 .6 


233-6 
158 


199 
218 


NaCl+KCl 

KC1+KN03 

KN03+NaNO3 

NaNO3+NaCl 


POTASSIUM  CHLORIDE 


520 


SOLUBILITY  OF  POTASSIUM  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  POTASSIUM 
NITRATE,  AND  OF  POTASSIUM  NITRATE  IN  AQUEOUS  SOLUTIONS  OF  POTASSIUM 
CHLORIDE,  AT  SEVERAL  TEMPERATURES. 

(Touren,  1900;  Bodlander,  1891;  Nicol,  1891;  Soch,  1898.) 


KC1  in  Aq.  KNO3  Solutions  at: 

14-5°  (T.). 

25.2°  (T.). 

20°,  etc.  (N.). 

Gms.  per  Liter  Solution. 

Gms.  per  Liter  Solution. 

Gms.  per  1000  Gms.  HgO. 

KN03.                   KC1. 

'  KNO3.                 KC1. 

KNO3.                  KC1. 

o               288.3 

o              311.8 

o                345-2 

20  .  64             284  .  2 

13.76            306.6 

56.18            342.15 

32.18             282.1 

32.18            303.6 

168.54            334-39 

62.23             276.8 

91.26            293.2 

at  25°  (S) 

82.77             273.5 

122.7               287.2 

225.8        341.3 

II5.9                270.7 

I4I.4               284.2 

at  80°  (S) 

II9.I                268.3 

182.7               276 

1175              402 

123.4                267.2 

KN03  in  Aq.  KC1  Solutions  at: 

14-5°. 

25.2°. 

20°. 

Gms.  per  Liter  Solution. 

Gms.  per  Liter  Solution. 

Gms.  per  1000  Gms.  H2O. 

KC1.                   KNO,. 

KC1.                  KNO3. 

KC1.                   KNO3. 

o               225.4 

o              325.5 

o              311.1 

13.58             219.8 

19.39            312.3 

82.9               256.8 

31.63             208.2 

49-22            288.7 

165.8               221.7 

65.64             185.2 

100.7               254 

248  .  7               202 

132.6                159.5 

155.2               224.4 

310.8               501.6 

164.4                153-3 

207.3               203.9 

196.5                144 

226.8               196.9 

236.9                I37.I 

In  the  case  of  the  results  by  Touren,  constant  temperature  and  agitation  were 

employed. 

KN03  in  Aq.  KC1  at 

20.5°  (B.).                   KC1  in  Aq. 

KN03  at  17.5°  (B.). 

Gms.  per  100  cc.  Solution. 

Sp.  Gr.  of                    Gms.  per  100  cc 

Solution.           •  Sp.  Gr.  of 

'  KC1.                   KN03.  ' 

Solutions.                    "  KNO3. 

KC1.                  Solutions. 

o                27  68 

.1625                 o 

29.39              1-173° 

4.72                24.39 

.1700                        6.58 

27.50         ,     1.1980 

7-74               22.44 

.1765                 8.88 

27.34              I.  2100 

12.23                20.23 

.1895                12.48 

26.53              1.2250 

15.15                18.96 

.1983                14.83 

25.98              1.2360 

I9.6l                17-67 

.2150                15.22 

25.96              1.2300 

22.17                17.11 

.2265                15-49 

25.95              1-2388 

24.96               16.79 

.2400               15.33 

26.24              I.24IO 

In  the  case  of  the  above  results  by  Bodlander,  a  saturated  aqueous  solution  of 
potassium  chloride  was  prepared  and  weighed  amounts  of  potassium  nitrate  were 
added  to  measured  volumes  of  it.  The  mixtures  were  warmed  and  then  allowed 
to  cool  to  the  indicated  temperature  and  frequently  shaken  during  24  hours. 


521 


POTASSIUM   CHLORIDE 


SOLUBILITY  OF  POTASSIUM  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  POTASSIUM 
NITRATE  AND  VICE  VERSA. 

(Leather  and  Mukerji,  1913.) 

Results  at  30°. 


Sp.  Gr. 
Sat.  Sol. 

1.186 
1.219 
1.251 
1.281 
1.258 
1.241 
1.225 


Cms.  per  100  Cms. 


KCl. 
37.58 
36.72 
36.19 
35-42 
28.71 

19.35 

9-44 


H20. 
KN03. 

O 

8.05 
19.36 
26.83 
29.19 

32.34 
38.10 


Results  at  40°. 

Gms.  per  too  Gms.   , 
H?O.              j 

p.Gr. 
at.  Sol. 

.222 

•344 
.486 
•552 
•544 

•545 
.552 

Results  at  91°. 

Gms.  per  100  Gms. 
H20. 

Solid  Phase 
in 
Each  Case. 

KCl 

"  +KNO, 
KNO, 

KCl. 
40.60 

39.11 
37.08 

3749 
32.22 
22.63 
11.58 

KN03."   " 
0 
16.86 

35-45 
39-71 
41.52 
46.31 
52.66 

KCl. 
53.58 
47.85 
43-30 
39-90 
33.25 

J5-56 

0 

KNO?." 
0 

52.75 

114.6 
162.9 

165.6 

181.1 

202.8 

Sp.  Gr. 
Sat.  Sol. 

I.I94 
1.252 
I.305 
I.3I9 
I.3I2 
1.297 
1.279 

Results  are  also  given  for  20°. 


SOLUBILITY  OF  MIXTURES  OF  POTASSIUM  CHLORIDE  AND  SODIUM 
CHLORIDE  IN  WATER. 


Gms.  per  100  Gms.  H2O. 


Gms.  per  100  Gms.  H2O. 


KCl. 

NaCl. 

KCl. 

NaCl. 

O 

II 

.2(l)  11.2(2)  30(1) 

30(2) 

50 

22(1) 

19(2) 

27.7(l) 

32.3(2) 

IO 

12 

•5 

12.3 

29-7 

30.5 

60 

24 

.6 

20.6 

27.2 

32.8 

20 

14 

.7 

13.8 

29.2 

31 

70 

27 

•3 

32.5 

26.8 

34.1 

25 

17 

)  14.5 

29(3) 

31.3 

80 

31 

(3) 

25.2(3) 

26.4(3) 

34 

30 

17 

.2 

15.4 

28.7 

31-5 

90 

32 

•9 

28.4 

26.1 

32.3 

40 

19 

•5 

17 

28.2 

31-9 

100 

34 

•7 

32.3 

25-8 

30.6 

(i)  Precht  and  Wittgen,  1881;  (2)  Etard,  1897;  (3)  at  25°  and  at  80°,  Soch,  1898. 

NOTE.  —  Page  and  Keightly,  Rudorff  and  also  Nicol  give  single  determinations 
which  lie  nearer  the  results  of  Precht  and  Wittgen  than  to  those  of  Etard. 


SOLUBILITY  OF  POTASSIUM  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  SODIUM 
CHLORIDE  AND  VICE  VERSA. 

(Leather  and  Mukerji,  1913;  see  also  Nicol,  1891.) 


Sp.  Gr. 
>at.  Sol. 

.176 
.197 
.213 
•237 
.240 

•233 
.224 

•193 

Results  at  20°. 

Gms.  per  100  Gms.     ( 
H2O.                ^ 

>p.  Gr. 

at.  Sol. 

.194 
.207 

•235 
.248 
.242 
[.247 
.222 
.197 

Results  at  40° 

Gms.  per  100  Gms. 
H20. 

Sp.  Gr. 

1.222 
1.236 
1.262 
1.262 
1.264 

1-235 
1.223 
1.189 

Results  at  91°. 

Gms.  per  100  Gms. 
H20. 

Solid  Phase 
in 
Each  Case. 

KCl 

it 

"  +NaCl 
NaCl 

KCl. 
34.6l 
26.60 
19.65 
14.92 
I5.36 
14.76 
9.70 
O 

NaCl. 
O 
10.13 

20.61 

30.36 

29.61 

30.38 

32.40 
35.63 

KCl. 
40.60 
31.42 

2443 
18.23 
18.74 

19.13 
10.49 

NaCl.  ' 
0 

10.68 

20.99 
30.60 
30.32 

29.92 

32.59 
36.53 

KCl. 

45.01 

35.84 
33.12 

32.45 
27.15 
13 
O 

NaCl. 
O 

10.66 
22.87 
28.12 
28.26 
29.18 

33-93 
38.72 

Results  are  also  given  for  30°. 

100  gms.  40  wt.  per  cent  alcohol  dissolve  5.87  gms.  KCl  +  12.25  gms.  NaCl  at  25°. 
loo  gms.  40  wt.'per  cent  alcohol  dissolve  5.29  gms.  KNO3  +  10.06  gms.  KCl  at  25°. 

(Soch,  1898.) 

100  gms.  abs.  ethyl  alcohol  dissolve  0.034  gm.  KCl  at  18.5°. 
100  gms.  abs.  methyl  alcohol  dissolve  0.5  gm.  KCl  at  18.5°. 

(de  Bruyn,  1892;  Rohland,  1898.) 


POTASSIUM  CHLORIDE  522 

SOLUBILITY  DATA  FOR  THE  RECIPROCAL  SALT  PAIRS  KCl+Na2SO4^K2SO4+NaCl. 

(Meyerhoffer  and  Saunders,  1899.) 
,   ftf  Mols.  per  1000  Mols.  H2O. 

t°.  <Vf  f *- >  Solid  Phase. 

Sat.  Sol.  S04.          K2.  Na,.          C12. 

4.4*         ...  5.42     14-39     Si-83     60.8  K3Na(S04)2+KCl+NaCl 

0.2  ...  3.35      12.78     50.93     60.36  Na4SO4.ioHrf)-fKCl+NaCl 

—   0.4  ...  3.59      16.38     40.75      53.54  NaaSO4.ioH40+KCl+K,Na(SO4)« 

16  ...  4.72      17.58     50.56     63.42  K3Na(SO4)2+KCl+NaCl 

24.8       1.2484  4.37     20.02     48.36     64.01 

16 .  3*         ...  16 .  29       9.16     61 . 06     53  . 93  KsNa(SO4)2+NaCl+Na2SO4.ioH2O+Na2S04 

24.5       1.2625  14.45       9-QO     58.46     53-91  K3Na(SO4)2+NaCl+Na2SO4 

0.3  ...  2.75     25.77      17.93     40.95  K3Na(S04)2+KCl+K2SO4 

25  1.2034  2.94     36.20     14.80     48.06 

17.9*     1.2470  13.84       O  62.54     48.70  Na2SO4.ioH2O+Na2SO4+NaCl 

30.1*     1.289  50.41      10.08     40.33       o  K3Na(SO4)2+Na2SO4.ioH2O+Na2SO4 

*  tr.  pt. 

Curves  are  given  in  the  original  paper  and  a  complete  discussion  of  the  older  work. 

SOLUBILITY  OF  MIXTURES  OF  POTASSIUM  CHLORIDE  AND  POTASSIUM 
SULFATE  IN  WATER. 

Gms.  per  100  Cms.  H2O.  .  0        Gms.  per  too  Gms.  H2O. 

^          '      KCl     +     K.SO..    '  °bSErVer'  '•  KC1      +  K,SO.. 

IO  30 . 9         1.32     (Precht  &  Wittgen.)  40  38-7         I  .  68    (P.  and  W.) 

15.8          28  2.3        (Kopp.)  50  41.3          1.82 

20  33.4         1.43     (P.andW.)  60  43.8         1. 94 

25  34 .76       2.93     (Van't  Hoff  &  Meyerhoffer.)     80  49-2         2.21  " 

30  36.1          1.57     (P.andW.)  100  54.5         2.53 

100  gms.  aq.  solution,  sat.  with  both  salts,  contain  26.2  gms.  KCl  +  1.09  gms. 
K2SO4  at  30°.  (Schreinemakers  and  de  Baat,  1914.) 

SOLUBILITY  OF  POTASSIUM  CHLORIDE  IN  AQUEOUS  SOLUTIONS 'OF  STANNOUS 
CHLORIDE  AT  25°  AND  VICE  VERSA.    (Fujimura,  1914-) 

Gms.  per  100  Gms.  H2O.  Gms.  per  100  Gms.  H2O. 

Solid  Phase.  — ' Sohd  Phase. 


KCl. 

O                       34-73  KC1                      58.48  17.85        SnCl2.KCl.H20 

2.86           32.17  "                  81.78  19.06 

4.37       34.08  "           107.65  17.79 

5-95           3I-76  SnCi2.2KCi.2H2o       170.70  21.26 

5.83        30.65  "           247.50  24.38 

10.24           27.30  337-26  25-5x 

17.42               24.68  "                      290.30  19.66          SnCl2.2H2O 

27.88               24.40  "                      235.50  7.49 

34-28                  5.99  222.5  2-73 

54.19               19.45  SnCl2.KCl.H20           234.05 

SOLUBILITY  OF  POTASSIUM  CHLORIDE  IN  DILUTE  SOLUTIONS  OF  ETHYL 
ALCOHOL  AT  o°  AND  AT  25°. 

(Armstrong,  Eyre,  Hussey  and  Paddison,  1907;  Armstrong  and  Eyre,  1910-11.) 

Wt.  %  Gms.  KCl  Dissolved  per  100  Gms. 

QHsOH  Sat.  Sol.  at:  <%of 

in                             , * s  Sol.  Sat. 

Solvent.  o°.                                   25°. 

O  22.1                             26.44  I.l8l3 

1.14  21.6                   25.91  I.I754 

2.25  20.9  25.29  1.1689 

4.41  19.7  24.21  1.1568 

8.44  ...  22.46  LI357 

12.13  15-5 

18.69  •••             I7-42  1.0847 


523 


POTASSIUM  CHLORIDE 


SOLUBILITY  OF  POTASSIUM  CHLORIDE  IN  AQUEOUS  ALCOHOL. 

(Gerardin  —  Ann.  chim.  phys.  [4]  5,  140,  '65.) 

Interpolated  from  the  original  results. 

Grams  KC1  per  too  Gms.  Aq.  Alcohol  of  Sp.  Gr.: 


t". 

0.9904 

0.9848 

0.9793 

0.9726 

0.9573 

0-939 

0.8967 

0.8244 

Wt.5*. 

wt'f. 

=  13-6 

Wt.%. 

=  19.1 
Wt.%. 

=  30 
Wt.%. 

=  40 

Wt.%. 

=  60 

Wt.%. 

=  90 

Wt.  %. 

o 

23-4 

iQ-5 

I5-S 

"•S 

7.0 

4.0 

i-7 

o.o 

5 

25.0 

21.0 

16.8 

12.8 

8.0 

4.8 

2.2 

0-0 

10 

26.4 

22.5 

18.0 

14.0 

9.0 

5-6 

2-7 

0-0 

15 

26.8 

24.0 

19.2 

15-2 

IO.O 

6.4 

3-i 

0.04 

20 

29.1 

25-3 

20.3 

16.  i 

10.8 

7.2 

3-5 

0.06 

25 

30-4 

26.8 

2i-S 

17.1 

ii.  6 

7-9 

3-9 

0.08 

30 

3!-7 

28.0 

22.6 

18.2 

12.5 

8-5 

4.2 

o.io 

40 

34-3 

30.8 

24.8 

20-0 

14.0 

9-9 

4.8 

O.2O 

50 

37-o 

33-5 

27.0 

21.8 

*5-5 

10.8 

5-2 

0.30 

60 

16.8 

ii.8 

5-5 

0-40 

SOLUBILITY  OF  POTASSIUM  CHLORIDE  IN  AQUEOUS  ALCOHOL  AT: 


(Schiff  —  Liebig's  Ann.  118,  365,  *6i.) 


14-5    • 
(Bodlander  —  Z.  physik.  Ch.  7,  316,  '91.) 


Sp.  Gr. 

Wt. 

G.  KC1  per 

Sp.  Gr. 

of  Sat 

Grams  per  100  cc.  Solution. 

Alcohol. 

per  cent 
Alcohol. 

100  jr.  AQ. 
Alcohol. 

oi  oat. 
Solutions. 

CjjHsOH. 

H20. 

KCI: 

0.984 

10 

19 

.8 

I 

.1720 

.  . 

88 

.10 

29.10 

0.972 

2O 

14 

•7 

I 

.1542 

2 

•79 

85 

.78 

26 

•85 

0.958 

30 

10 

•7 

I 

•J365 

4 

.98 

84 

.00 

24 

.67 

0.940 

40 

7 

•7 

I 

•1075 

10 

•56 

79 

•63 

20 

•56 

0-918 

So 

5 

.0 

I 

.1085 

15 

•57 

75 

.24 

17 

.24 

0.896 

60 

2 

.8 

I 

•0545 

20 

.66 

70 

•S2 

14 

.27 

0.848 

80 

O 

•45 

I 

•0455 

24 

•25 

67 

•05 

13 

•25 

Gerardin  's  results 

at  15°  agree 

0 

•9695 

40 

.42 

5o 

.18 

6 

•35 

well  with 

the  above 

deter- 

0 

•9315 

48 

•73 

40 

.60 

3 

.82 

minations 

. 

O 

.8448 

68 

•63 

15 

•55 

o 

•30 

30°  and  40°. 

(Bathrick  —  J.  Physic.  Chem.  i,  160,  '96.) 


Wt. 

per  cent 
Alcohol. 

Gms.  KCI  per  100  Gms. 
Aq.jUcohol. 

Wt. 
per  cent 
Alcohol. 

Gms.  KCI  per  too  Gnc 

Aq.  Alcohol. 

At  30°. 

At  40°. 

"At  30°. 

At  40°." 

O 

38.9 

41.8 

43.1 

II.  I 

13.1 

5-28 

33-9 

35-9 

55-9 

6.8 

8.2 

9-43 

30.2 

33-3 

65-9 

3-6 

4.1 

16.9 

24.9 

27.6 

78.1 

1.6 

25-1 

19.2 

21.8 

86.2 

0.4 

0-5 

15-6 

17.2 

POTASSIUM  CHLORIDE 


524 


SOLUBILITY  OF  POTASSIUM  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  ETHYL 
ALCOHOL  AT  25°. 

(Mclntosh,  1903.) 


vt.  % 

HsOH, 

Mols.  KC1 
per  Liter. 

Gms.  KC1  per 
ioo  cc.  Sat.  Sol. 

Wt.  % 
QHsOH. 

Mols.  KC1 
per  Liter. 

Gms.  KC1  per 
ioo  cc.  Sat.  Sol. 

0 

4.18 

3I.I8 

60 

0.56 

4.18 

10 

3-21 

23-93 

70 

0-305 

2.27 

20 

2.40 

17.89 

80 

0.125 

o-93 

3° 

1.78 

I3-27 

90 

O.O42 

0.31 

40 

1.26 

9.40 

IOO 

O.OII 

0.08 

50 

0.84 

6.26 

SOLUBILITY  OF  POTASSIUM  CHLORIDE  IN  DILUTE  AQUEOUS  SOLUTIONS  OF 
METHYL  ALCOHOL  AT  o°  AND  AT  25°. 

(Armstrong  and  Eyre,  1910-11.) 


Wt.  % 
PN  OH 

Gms.  KC1  per  ioo  Gms.  Sat.  Sol.  at; 

v^Xl^UXl 

in  Solvent. 

o°. 

25°. 

0 

22.06 

26.69 

0.79 

21.74 

26.42 

i-57 

21.39 

26.OI 

3.10 

20.  6l 

25-25 

8.76 

17.84 

22.82 

SOLUBILITY  OF  POTASSIUM  CHLORIDE  IN  AQUEOUS  METHYL  ALCOHOL  AT  25°. 

(Herz  and  Anders,  1907;  Mclntosh,  1903.) 


Solvent 

flfog   Of 

Gms 

.KCl 

Solve 

:nt. 

j 

oc    Of 

Gms.  KCl 

,,          wt.  % 

d«F          CH3OH. 

Sat.  Sol. 

per  ioo  cc. 
Sat.  Sol.            dap- 

Wt.% 
CH3OH 

Satfsol 

per  ioo  cc. 
Sat.  Sol. 

O, 

,9971 

0 

1.1782 

31 

.13 

0 

.8820 

64 

o. 

9064 

3-44 

o 

,9791 

10.6 

I.I25 

24 

.53 

0 

.8489 

78.1 

0. 

8607 

1-54 

0 

,9481 

30.8 

1.033 

13 

-65 

0 

.8167 

98.  9(? 

)    o. 

8242 

0-75 

o. 

.9180 

47.1 

0.9679 

7 

.6l 

o 

.7882 

IOO 

o. 

7937 

0-43 

ioo  gms. 

methyl 

alcohol  dissolve 

0-53 

gm.  KCl 

at  25°. 

(Turner  and  Bissett,  1913.) 

ti 

ethyl 

11 

11 

0.022 

«       « 

it 

«« 

" 

n 

propyl 

« 

« 

0.004 

«       « 

M 

« 

" 

amyl  "       0.0008 

Potassium  chloride  is  insoluble  in  CHsOH  at  the  crit.  temp.    (Centnerszwer,  1910.) 

SOLUBILITY  OF  POTASSIUM  CHLORIDE  IN  DILUTE  AQUEOUS  SOLUTIONS  OF 
PROPYL  ALCOHOL  AT  o°  AND  AT  25°. 

(Armstrong  and  Eyre,  1910-11.) 


Wt.  % 

C3H7OH 

in  Solvent. 

I 

1.48 
2.91 
5.66 


Gms.  KC1  per  100  Gms.  Sat.  Sol.  at: 


o°. 

22.O6 
21.25 
20.49 
18.97 


25°. 

26.44 
25.94 
25.23 
23.82 


SOLUBILITY  OF  POTASSIUM  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  GLUCOSE  AT  25°. 

(Armstrong  and  Eyre,  1910-11.) 


wt.% 

Gms.  KCl 

C6H1206+H,O 

per  ioo  Gms. 

in  Aq.  Solvent. 

Sat.  Solution. 

0 

26.63 

4.72 

25.86 

9 

25.18 

16.53 

23.89 

37-27 

20.15 

525 


POTASSIUM  CHLORIDE 


SOLUBILITY  OF  POTASSIUM  CHLORIDE  IN  AQUEOUS  ACETONE  SOLUTIONS. 

(Snell,  1898;  at  20°,  Herz  and  Knoch,  1904.) 


Wt.  (see  Note)     _At  20  . 
Percent          KClperioocc. 
Acetone  in             Solution. 

At  30°. 
Gms.  per  100  Gms. 
Solution. 

At  40°. 
Gms.  per  100  Gms. 
Solution. 

At  50°. 
Gms.  per  100  Gms. 
Solution. 

Solvent. 

Millimols. 

Gms. 

Acetone. 

KCl. 

Acetone.         KCl.  ' 

Acetone.         KCl.  " 

0 

410.5 

30. 

62 

0 

27- 

27 

O 

28.69 

0 

30 

Q.I 

351-7 

26. 

23 

6. 

96 

23- 

42 

6. 

79     25.33 

...    • 

.  .  . 

20 

286.6 

21  . 

38 

16. 

22 

18. 

90 

15- 

75     21.28 

.  .  . 

.  .  . 

30 

223.7 

16. 

69 

25- 

45 

15- 

06 

two  layers 

25.67 

14.42 

40 

166.5 

12. 

42 

35- 

52 

II  . 

31 

it 

36.03 

9-93 

50 

II5-4 

8. 

61 

45- 

98 

8. 

04 

t( 

46.46 

7.07 

60 

71.2 

5- 

31 

56- 

9i 

5- 

12 

a 

57-37 

4-38 

70 

38-5 

2. 

87 

68. 

18 

2. 

60 

(i 

68.56 

2.22 

80 

I2.Q 

O. 

96 

79- 

43 

0. 

76 

79 

34      0.58 

79-25 

0.94 

90 

2 

0. 

15 

89. 

88 

O. 

13 

89 

.84      0.16 

±81° 

sat.  sol. 

100 

O 

0 

100 

0 

100 

0 

NOTE.  —  For  the  20°  results  the  per  cent  acetone  in  the  solvent  is  in  terms 
of  volume  instead  of  weight  per  cent,  and  the  concentration  of  the  second  solu- 
tion is  10  per  cent  instead  of  9.1  which  is  the  weight  per  cent  concentration  of  the 
solvent  for  the  corresponding  results  at  the  other  temperatures. 


AT  THE  TEMPERATURE  40°  AND  FOR  CONCENTRATIONS  OF  ACETONE  BETWEEN  20 
AND  8O  PER  CENT  THE  SATURATED  SOLUTION  SEPARATES  INTO  TWO  LAYERS 
HAVING  THE  FOLLOWING  COMPOSITIONS: 


Upper  Layer. 

Gms.  per  100  Gms.  Solution. 


H20. 

(CH3)2CO. 

KCl. 

55-2 

31.82 

12.99 

53-27 

35-44 

11.29 

51-23 

48.50 

10.27 

50-34 

39-88 

9-77 

48.02 

43-i8 

8.79 

46.49 

45-34 

8.17 

58.99 

25.24 

15-77 

Lower  Layer. 

Gms.  per  100  Gms.  Solution. 


rH20. 

(CH3)2CO. 

KCl. 

28.14 

69.42 

2.44 

30.96 

65-97 

3-07 

32.64 

63-79 

3-56 

34-07 

62.01 

3-92 

37-44 

57-67 

4.89 

38.68 

56.17 

5-25 

23.66 

74.91 

i-43 

100  cc.  sat.  solution  of  potassium  chloride  in  furfurol  (C^aO.COH)  contain 
0.085  gm.  KCl  at  25°.  (Walden,  1906.) 


POTASSIUM  CHLORIDE  526 

SOLUBILITY  OF  POTASSIUM  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  GLYCEROL  AT  25°. 

(Herz  and  Knoch,  1905.) 

Sp.  Gr.  of  Glycerol  at  25°/4°  =  1.2555.  Impurity  about  1.5%. 


Wt.  Per  cent 
Glycerol  in 
Solvent. 

KCl  per  ioo  cc. 
Solution. 

Sp.  Gr.  of 

Solutions. 

Wt.  Per  cent 
Glycerol  in 
Solvent. 

KCl  per  ioo  cc. 
Solution. 

Sp.  Gr.  of 
Solutions. 

Millimols. 

Gms. 

Millimols. 

Gms. 

0 

424.5 

31.66 

I 

.180 

54 

23 

238. 

5 

17 

79 

I  .219 

13.28 

383.4 

28.61 

I 

.185 

83 

.84 

149 

II 

.11 

1.259 

25.98 

339-3 

25-3I 

I 

.194 

IOO 

no 

.6 

8 

25 

1.286 

45.36 

271.4 

20.24 

I 

.211 

100  gms.  H2O  dissolve  246.5  gms.  sugar  +  44.8  gms.  KCl  at  31.25°,  or  100  gms. 
of  the  sat.  solution  contain  62.28  gms.  sugar  +  H-33  gms.  KCl.         (Kohler,  1897.) 

SOLUBILITY  OF  POTASSIUM  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  PYRIDINE  AT  10°. 

(Schroeder,  1908.) 

Aq.  Mixture.  Gms.  KCl  Aq.  Mixture.  Gms.  KCl 

, •  —  per  100  Gms. '  — »          per  too  Gms. 

cc.  H2O.          cc.  Pyridine.  Sat.  Sol.  cc-  H2O.       cc.  Pyndine.  Sat.  Sol. 

ioo       o      23.79        40      60      3.33 
90      10      19-76        30      70      1.25 

80        20        16.37  20        80         0.24 

70        30        I3-I9  1°        90         0-04 

60  40     *        10.05  o  ioo  o 

50  50  6-34 

SOLUBILITY  OF  POTASSIUM  CHLORIDE  IN  DILUTE  AQUEOUS  SOLUTIONS  OF 
SEVERAL  COMPOUNDS  AT  25°. 

(Armstrong  and  Eyre,  1913.) 

Gms.  Cmpd.       Gms.  KCl  Gms.  Cmpd.        Gms.  KCl 

Compound.         per  1000  Gms.   per  ioo  Gms.  Compound,     per  1000  Gms.    per  ioo  Gms. 

H2O.  Sat.  Sol.  H2O.  Sat.  Sol. 

Water  alone         ...  26.89  Glycol  I5-5*  26.43 

Acetaldehyde  n.oi  27.05  62.05  25.26 

Paraldehyde  n.oi  26.42  Mannitol      45-53  24.86 

Glycerol  13.01  25.58  136-59  24.46 

ioo  gms.  95%  formic  acid       dissolve  19.4  gms.  KCl  at  19. 7°.      (Aschan,  1913.) 

glycerol  (di6  =  1.256)  3.72     '  "  15-16°.  (Ossendowski,  1907.) 

ioo  cc.     anhydrous  hydrazine      "         9         "       "     "  room  temp. 

(Welsh  and  Broderson,  1915.) 

ioo  gms.  hydroxylamine  12.3  "  17-18°.  (de  Bruyn,  1892.) 

FUSION-POINT  DATA  (Solubilities,  see  footnote,  p.  i)  ARE  GIVEN  FOR  THE 
FOLLOWING  MIXTURES  OF  POTASSIUM  CHLORIDE  AND  OTHER  SALTS. 

vr'ij^irT      \  (Wrzesnewski/ia;  Amadori&Pam-  vr'l-Lircr*     I  (Jaenecke, '12;  Sackur, '11-12; 

«"KL    i      panmi,'n;  Ruff  &  Plato, '03.)  KUHK2bU4.j      Ruff  &  plato/03>) 

KC1  +  KF.         (Ruff  and  Plato,  1903.)  KCl  +  HgCl       (Sackur,  1913.) 

KC1  +  KOH.     (Scarpa,  1915.)  KCl  +  NaCl.      (Sackur, '13;  Ruff  &  Plato,  03.) 

KCl-i-KCrO4.  (Sackur,'ii-i2;Zemcznzny,'o8.)  KCl-i-Na2SO4.  (Sackur,  1913.) 

KCl  +  KPOs.     (Amadori,  1912.)  KCl+SrCl2.       (Vortisch,  '14;  Sackur,  '11-12.) 

KC1+K4P2O7.  "  KC1+T1C1.        (Sandonnini,  J9"J  1914-) 

KC1+K3PO4. 

POTASSIUM  CHLOROIRIDATE  K2IrCl6. 

ioo  gms.  H2O  dissolve  1.25  gms.  of  the  salt  at  18-20°. 

ioo  gms.  H2O  dissolve  9.18  gms.  dipotassium  aquopentachloroiridite,  IrCl6 
(H2O)K2  at  19°.  (Delepine,  1908.) 


527 


POTASSIUM   CHROMATES 


POTASSIUM  CHROMATES  K2CrO4,  K2Cr2O7,  K2Cr3Oi0>  etc. 

EQUILIBRIUM  IN  THE  SYSTEM,  POTASSIUM  OXIDE,  CHROMIC  ACID  AND 
WATER  AT  SEVERAL  TEMPERATURES. 

(Koppel  and  Blumenthal,  1907.) 


Results  at  o°.  Results  at  30°. 


Results  at  60°. 


Gms.  per  100  Gms.  Sat. 
Solution. 

Gms. 

per  too  Gms. 
'  Solution. 

Sat. 

Gms. 

per  too  Gms.  Sat. 
Solution. 

Solid  Phase  at  each 

'   K20. 

Cr03.  ' 

K20. 

Cr03. 

'    KA 

Cr203. 

Temp. 

3I.I8 

. 

46. 

8 

about  50 

KOH.2H2O 

26.06 

0 

•54 

26. 

89 

0. 

94 

32 

.98 

o. 

53 

K2Cr04 

19.31 

4 

•27 

22. 

25 

3- 

06 

21 

.05 

9- 

15 

" 

17.06 

ii 

•77 

18. 

65 

13- 

72 

20 

•25 

14. 

43 

" 

17.62 

18 

.71 

19. 

12 

20. 

30 

20 

.70 

21  . 

97 

" 

17-73 

19 

.04 

19. 

35 

21 

2O 

.61 

23- 

61 

"  +K2CrA 

10.90 

ii 

•93 

15- 

04 

16. 

85 

14-53 

20. 

82 

K2CrA 

1.87 

3 

•13 

II. 

20 

13- 

ii 

IO 

.OI 

21  . 

21 

" 

0.78 

22 

-38 

2. 

42 

28. 

21 

6 

.86 

39- 

64 

" 

i-47 

42 

•95 

2. 

50 

44. 

50 

7 

.06 

49- 

84 

"  +K2CrAo 

1.25 

44 

-52 

4 

.06 

54- 

73 

K2CrAo 

1.17 

46 

.84 

. 

. 

2 

60. 

69 

" 

i-37 

47 

.40 

2. 

35 

49- 

95 

.  . 

.  . 

"  +K2Cr4Oi3 

1.24 

48.23 

I. 

35 

53- 

39 

. 

.  . 

.  . 

. 

K2Cr4O13 

1.16 

56 

•93 

.  . 

. 

.  . 

. 

. 

.  . 

" 

0.64 

61 

•79 

0. 

69 

62. 

81 

I 

.27 

65- 

77 

"  +Cr03 

0 

61 

•54 

. 

62. 

52 

0 

65- 

12 

CrO, 

THE  CRYOHYDRATES  (EUTECTICS)  IN  THE  SYSTEM  K2O  —  CrO3  —  H2O. 

The  points  were  determined  by  adding  to  a  sat.  solution  of  K2Cr2O7  successive 
I  to  2  gm.  portions  of. chromic  acid  and  ascertaining  the  freezing-point  and 
composition  of  the  solution.  At  the  point  of  appearance  of  a  new  solid  phase  an 
additional  amount  of  chromic  acid  does  not  change  the  f.-pt.  since  the  added  CrOa 
goes  into  the  solid  phase.  This  relation  also  holds  at  the  points  where  the  solu- 
tion is  simultaneously  saturated  with  K2Cr2O7  and  K2Cr2Oio  or  K2Cr2Oi0  and 
K2Cr4013. 


t°  of  Equi- 
librium of 
Sat  Sol 

Gms.  per  100  Gms.      Solid  Phase 
Sat.  Solution.       inj£uffitaraiii 

t°  of  Equi- 
librium of 

Cj,  *      Cnl 

Gms.  per  100  Gms. 
Sat.  Solution. 

Solid  Phase 
in  Equilibrium 
with  Sat.  Sol. 

with  Ice. 

K2O. 

CrO3.              and  jce> 

oat.  ooi. 
with  Ice. 

'    K2O. 

CrO3. 

and  Ice. 

-25 

2O 

5 

.  70     K2CrO4 

—  13 

.22 

not  det. 

27 

.26 

K2CrA 

17 

.52 

13 

.89         " 

-14 

•50 

u 

28 

•85 

" 

—  II 

•37 

17 

.12 

18 

.18         «* 

—  22 

.IO 

ft 

35 

.92 

" 

—  II 

•50 

17 

.18 

18 

.11         "  +K2CrA 

—  22 

.11 

0.47 

36 

.14 

" 

-5 

8 

•27 

8 

.  OI           K2CrA 

-26 

•77 

0.88 

39 

.86 

M 

—  o. 

63 

i 

•38 

2 

•93                "      * 

-30 

.20 

1.18 

42 

.31 

~l~K2Cr3Ojo 

—  i  . 

78 

not 

det. 

6 

.81 

-34 

.01 

0-95 

43 

•45 

K2CrA0 

-5- 

5 

tt 

16 

.05                " 

-39 

0.79 

45 

•65 

"  +K2CrA, 

-6. 

43 

0 

•48 

17 

.25 

-49 

not  det. 

49 

.11 

K2Cr4013 

IO. 

25 

o 

•45 

23 

•63 

-61 

•5 

0.61 

53 

•57 

* 

The  viscosity  of  the  solutions  at  the  lower  temperatures  increased  so  much  that 
the  cryohydrate  points  could  not  be  determined.  By  graphic  extrapolation  the 
cryohydrate  temperature  of  chromic  acid  and  of  chromic  acid  +  potassium  tetra- 
chromate  is  near  —80°  and  the  CrO3  content  is  59  gms.  per  100  gms.  sat.  solution. 


POTASSIUM   CHROMATES 


528 


By  interpolation  from  the  data  given  in  the  preceding  tables  the  following 
solubilities  in  water  are  obtained : 

THE  ICE  CURVE  AND  SOLUBILITY  OF  POTASSIUM  CHROMATE  IN  WATER. 


to              Gms.  K2CrO4  per        Solid 
100  Gms.  H2O.         Phase. 

-  o-99          4-53            Ice 

—1.2                  6.12                  " 
-    4.3.             26.99 
—    7.12             42.04 
-10.35             52.41 

Potassium                      Potassii 
Dichromate                  +  Potasi 

Gms.  K2Cr2O7                             I 
t°.         per  100  Gms.               t°. 
H20. 

-0.63*            4.50           -II.5* 

o                 4.65              o 

30                      I8.I3             +30 
60                      45.44                  60 

104.  8f        108.2            io6.8t 

*••                 *£&£%&    SoHd  Phase. 
-11.35  EuteC.        54  .  54           Ice+K2CrO4 
O                                  57  .11                 K2CrO4 

30                65  .  13 
60                    74.60 
io5.8b.pt.         88.8 
im  Dichromate           Potassium  Dichromate 
sium  Chromate.       +  Potassium  Trichromate. 

Gms.  per  100  Gms.  H2O.         f0           Gms'  p£^ms'  Sat 

K2O.           CrO3. 

17.18     i8.ii 

17.73      19.03 
19-35       21 

20.  61     23.61 
24-3      30.5 

-30* 

0 
+  20 

3° 
60 

K20. 

1.18 
1.47 

2.20 
2.50 
7.06 

16.80 

Cr03. 
42.51 
42.99 
43.10 
44-50 
49.84 
59.20 

Eutec. 

Potassium  Trichromate  +  Potassium 
Tetrachromate. 


* 

'  K20. 

Cr03. 

—39  Eutec. 

0.79 

45-69 

0 

i-37 

47.40 

20 

2 

48.46 

30 

2.25 

49-95 

60 

5.01 

54-09 

t  b.  pt. 

Potassium  Tetrachromate-f- 
Chromic  Acid  (CrOs). 

Gms.  per  100  Gms.  Sat.  Sol. 


O 
20 

30 
60 


K20. 

0.64 

O.62 

0.69 

1.27 


Cr03. 
61.79 
62.80 
62.81 


Data  for  boiling  points  in  the  system  K2O  +  CrO3.H2O  determined  by  means 
of  the  Beckmann  apparatus,  are  also  given. 

The  older  data  for  K2CrO4  and  K2Cr2O7  are  as  follows: 

SOLUBILITY  OF  EACH  IN  WATER. 

(Alluard,  1864;  Nordenskjold  and  Lindstrom,  1869;  Etard,  1894;  Kremers,  1854;  Tilden  and  Shen- 
stone,  1884.) 

Potassium  Dichromate. 


Potassium  Chromate. 
Grams  per  100  Grams  Water. 


Grams  per  100  Grams  Water. 


0 

58.2* 

59  -3t 

60.2* 

10 

60-0 

61.2 

62.5 

20 

61.7 

63.* 

64-5 

25 

62.5 

64.2 

64-5 

30 

63-4 

65.2 

66.5 

40 

65.2 

67.0 

68.6 

50 

66.8 

69.0 

70.6 

60 

68.6 

71.0 

72.7 

70 

70.4 

73-o 

74.8 

80 

72.1 

75-o 

76.9 

90 

73-9 

77-o 

79-o 

100 

75-6 

79-o 

82.2 

"5 

79-o 

150 

83.0 

5* 

5§ 

7 

7 

12 

12 

16 

16 

20 

20 

26 

27 

34 

37 

43 

47 

52 

58 

61 

70 

70 

82 

80 

97 

no 

145 

*43 

205 

*  Etard. 


t  Alluard. 


N.  and  L. 


§  A.,  K.,  T.  and  S. 


529 


POTASSIUM   CHROMATES 


SOLUBILITY  OF  POTASSIUM  CHROMATES  IN  WATER  AT  30* 

(Schreinemaker  —  Z.  physik,  Ch.  55,  83,  '06.) 

Composition  in  Wt.  per  cent  of: 

Solid 


The  Solution 
Per  cent  CrO3       Per  cent  K2O . 


The  Residue. 
Per  cent  CrO3.     Per  cent  K2O . 


0 

±47 

.  .  . 

o.o 

47.16 

12.59 

47-54 

0.1775 

34.602 

10-93 

37-47 

I-351 

26.602 

16.482 

32.532 

20.584 

37-I3I 

39.922 

15-407 

19.225 

27.966 

29-377 

20.67 

19.17 

19.096 

17.30 

37.64 

22.61 

7.88 

.  .  . 

.  .  . 

17-93 

3.412 

25-85 

7.82 

43  -51 

3-oi 

49-45 

9.91 

44.46 

3-245 

53-94 

12.40 

46.368 

2.823 

60.314 

12.935 

49-357 

2-353 

63-044 

11.684 

53-215 

1.360 

62.958 

8.002 

62-55 

0.796 

67.944 

6.731 

62.997 

0.621 

70.0 

4.0 

62.28 

Q.O 

.  .  . 

.  .  . 

Phase. 


KOH-zHzO 


K2Cr207 


K2Cr3O10 


K2Cr40,3 

K2Cr4Ol3  +  Cr08 
Cr03 

IOO  gms.  sat.  solution  in  glycol,  C?H4(OH)2.H2O,  contain  1.7  gms.  K2CrO4at  15.4°. 
IOO  gms.  sat.  solution  in  glycol,  C2H4(OH)2.H2O,  contain  6  gms.  K2Cr2O7  at  14.6°. 

(de  Coninck,  1905.) 

IOO  gms.  H2O  dissolve  IO.I  gms.  K2Cr2O7  at  15.5°.  (Greenish  and  Smith,  1901.) 

ioo  gms.  sat.  solution  in  water  contain  5.52  gms.  K2Cr2O7  at  4.81°,  15.17  gms. 

at  30.1°  and  1777  gms.  at  35.33°.  (Le  Blanc  and  Schmandt,  1911.) 

ioo  cc.  sat.  aqueous  solution  contain  11.43  gms.  K2Cr2O7  at  20°. 

(Sherrill  and  Eaton,  1907.) 

SOLUBILITY  OF  POTASSIUM  CHROMATE  IN  AQUEOUS  SOLUTIONS  OF  POTASSIUM 
MOLYBDATE  AT  25°  AND  VlCE  VERSA. 

(Amadori,  191  aa.) 


Gms.  per  ioo  Gms.  H2O. 


K2Cr04. 
64-62 

49-59 
38.90 

33-21 


K2Mo04. 

O 

15-37 
38.79 
50.96 


Gms.  per  ioo  Gms.  H2O. 

'K2CrO4.  K2MoO4. 

14.13  98.72 

10.07  118.8 

10.24  119.9 

7.12  137.8 

6.37  157.2 


Gms.  per  ioo  Gms.  H2O. 
K2Cr04.  K2MoO4. 

4.92  165.4 

2.14  I80.8 

1.70  183 

o  184.6 


SOLUBILITY  OF  POTASSIUM  CHROMATE  IN  AQUEOUS  SOLUTIONS  OF 
POTASSIUM  SULFATE  AT  25°  AND  VICE  VERSA. 

(Amadori,  191 2a.) 


Gms.  per  ioo  Gms.  H2O. 
K2CrO7  K2SO4. ' 

63.09  0.76 

61.39  I.I7 

58.40  1.84 
5I.8I  2.36 


Gms.  per  ioo  Gms.  H2O. 


K2CrO4. 

40.93 
27.36 
20.83 
14.65 


K2S04. 

3.33 
4.82 

5-72 
7.12 


Gms.  per  ioo  Gms.  H2O. 


K2Cr04. 
7.8l 

4.36 
1.94 
O 


K2S04. 

8.98 

IO.25 

10.86 

12.  IO 


IOO  cc.  anhydrous  hydrazine  dissolve  I  gm.  K2CrO4  at  room  temp. )  (Welsh and  Brod- 
100  cc.  anhydrous  hydrazine  dissolve  i  gm.  K2Cr2O7  at  room  temp.  J     erson,  1915.) 


POTASSIUM  CHROMATES  530 

FREEZING-POINT  DATA  (Solubilities,  see  footnote,  p.  i)  FOR  MIXTURES  OF 
POTASSIUM  CHROMATES  AND  OTHER  COMPOUNDS. 

K2CrO4  +  K2Cr2O7.  (Groschuff,  1908.) 

'    K2CrO4    -j-  K2MoO4.  (Amadori,  1913.) 
K2CraO7  -j-  K2Mo2O7. 

K2CrO4    -j-  K2SO4.  (Amadori,  1913;  Groschuff,  1908.) 

K2CrO4    +  K2WO4.  (Amadori,  1913.) 
K2Cr2O7  +  K2W2O7. 

POTASSIUM  CITRATE   (CH2)2C(OH)(COOK)3.H2O. 
SOLUBILITY  IN  WATER. 

(Average  results  of  Seidell,  1910;  Greenish  and  Smith,  1901;  Kohler,  1897.) 
Gms.  (CH2)2C(OH)(COOK)3.H2O  per  ioo  Gms. 

Sat.  Solution.  Water. 

15  6l.8  l62 

20  63.2  172 

25  64.5  l82   (^25  =    L5l8) 

30  66  194 

ioo  gms.  H2O  dissolve  198.3  gms.  (CH2)2COH(COOK)3  +  303.9  gms.  cane 
sugar  at  31.25°-  (Kohler,  1897.) 

SOLUBILITY  OF  POTASSIUM  CITRATE  IN  AQUEOUS  ETHYL  ALCOHOL  AT  25°. 

(Seidell,  1910.) 

When  potassium  citrate  is  added  to  aqueous  alcohol  of  certain  concentrations 
the  mixture  separates  into  two  liquid  layers.  A  series  of  determinations  made  by 
adding  an  excess  of  the  salt  to  10-15  cc.  portions  of  several  aq.  alcohol  mixtures 
at  25°  gave  the  following  results. 


Wt.% 
.  C2HBOH 
in  Solvent. 

d«5  of 
Sat.  Solution. 

'    Wt.  %_ 
C^HsOH  in 
Sat.  Solution. 

Gms.  (CH2)2COH- 
(COOK)3.H2O 
per  ioo  Gms. 
Sat.  Solution. 

8.9 

(a 

lb 

1.4920 

O 

60 

(a 

.  .  . 

... 

0.2 

32 

lb 

1.4930 

0 

6l.6 

iff 

(a 

.  .  . 

65.1 

0.38 

S1 

lb 

62.5 

*7O     "? 

(a 

0.8366 

81 

O.IO 

7O.2 

lb 

... 

62.3 

8l.4 

0/8356 

8l.4 

0.038 

91.6 

0.8139 

91  .6 

0.016 

99-9 

0.7896 

99-5 

0.014 

a  =  upper,  alcohol  rich  layer,     b  =  lower,  water  rich  layer. 

A  series  of  determinations  was  also  made  by  adding  just  enough  potassium 
citrate  to  the  alcohol  solution  to  cause  distinct  clouding  and  then,  after  bringing 
to  25°,  titrating  with  the  aqueous  alcohol  mixture  to  disappearance  of  the  clouding. 
The  results  were  plotted  and  the  following  interpolated  values  obtained. 


Wt.% 
in  Solvent. 

Gms.  (CH2)2COH- 
<*u  of           (COOK)3.H20 
Sat.  Solution.       per  ioo  Gms. 
Sat.  Sol. 

wt.% 

CzHsOH 
in  Solvent. 

Gms.(CH2)2COH- 
duol             (COOK)3H20, 
Sat.  Solution,      per  ioo  Gms. 
Sat.  Sol. 

0 

I.5l8 

64.5 

40 

I  .005 

12.4 

5 

1.400 

52-5 

50 

0-943 

5-6 

10 

I.3IO 

45-5 

60 

0.900 

1.6 

20 

I.I77 

31-5 

70 

0.868 

0.4 

3°  „ 

1.085 

21.5 

80 

0.838 

0.04 

In  one  determination  at  15°,  made  with  alcohol  of  59  Vol.  per  cent,  4.51  gms. 
(CH2)2COH(COOK)s.H2O  were  required  to  just  cause  clouding. 


531  POTASSIUM  CYANATE 

POTASSIUM   CYANATE  KCNO. 

SOLUBILITY  IN  ALCOHOLIC  MIXTURES. 

(Erdmann,  1893.) 

Cms.  KCNO 

Solvent.  per  Liter  Solvent 

at  b.-pt. 

80  per  cent  Alcohol  +  20  per  cent  Water  62 

80  per  cent  Alcohol  +  20  per  cent  Methyl  Alcohol  76 

80  per  cent  Alcohol  +  10  per  cent  Acetone  82 

POTASSIUM  CYANIDE  KCN. 

100  gms.  H2O  dissolve  122.2  gms.  KCN,  or  100  gms.  sat.  solution  contain  55 
gms.  KCN  at  103.3°.  (Griffiths.) 

100  gms.  abs.  ethyl  alcohol  dissolve  0.87  gm.  KCN  at  19.5°. 
100  gms.  abs.  methyl  alcohol  dissolve  4.91  gms.  KCN  at  19.5°.    (de  Bruyn,  1892.) 
100  gms.  glycerol  dissolve  32  gms.  KCN  at  15.5°.  (Ossendowski,  1907.) 

100  gms.  hydroxylamine  dissolve  41  gms.  KCN  at  17.5°.  (de  Bruyn,  1892.) 

F.-pt.  data  for  KCN  +  KC1,  KCN  +  NaCN,  KCN  +  AgCN,  KCN  +  Cu2 
(CN)2  and  for  KCN  +  Zn(CN)2  are  given  by  Truthe  (1912). 

POTASSIUM  CHROMOCYANIDE  K3Cr(CN)6. 

100  gms.  H2O  dissolve  32.33  gms.  K3Cr(CN)e  at  20°. 

(Moissan,  1885;  Christensen,  1885.) 

POTASSIUM  CHROMITHIOCYANATE  K2Cr(SCN)6.4H2O. 

IOO  gms.  H2O  dissolve  139  gms.  salt.  (Karsten,  1864-5.) 

POTASSIUM  CARBONYL  FERROCYANIDE  K3FeCO(CN)6.3^H2O. 

IOO  gms.  H2O  dissolve  148"  gms.  salt  at  16°.  (Muller,  1887.) 

POTASSIUM   FERRICYANIDE  KsFe(CN)8. 

POTASSIUM  FERROCYANIDE  K4Fe(CN)6.3H,O. 

SOLUBILITY  OF  EACH  IN  WATER. 

(Wallace,  1855;  Etard,  1894;  Schiff,  1860;  Michel  and  Krafft,  1858;  Thomsen.) 

NOTE.  —  The  available  determinations  fall  very  irregularly  when  plotted  on 
cross-section  paper,  and  the  following  figures,  which  are  averages,  are  therefore 
hardly  more  than  rough  approximations  to  the  true  amounts.  The  figures  under 
K4Fe(CN)6  show  the  limits  between  which  the  correct  values  probably  lie. 


Gms.  per  100  Gms.  H2O. 

Gms.  per  100  Gms.  H2O. 

0 
10 
2O 

25 
10 

K3Fe(CN)6. 

31 
36 

43 
46 
<o 

K4Fe(CN),.' 

13       ••• 
2O         2O 

25         40 
28         48 

^2       <J7 

40 
60 

80 

IOO 

IO4.4. 

K3Fe(CN)6. 
60 

66 
82.6 

K4Fe(CN),.' 
38         70 
52         83 

66      89 

76         91 

loo  gms.  H2O  dissolve  0.08946  gm.  mols.  =  32.97'gms.  K4Fe(CN)6  at  25°,  da^  of 

sat.  sol.  =  1.0908.  (Harkins  and  Pearce,  1916.) 

One  liter  of  sat.  solution  in  water  contains  319.4  gms.  K4Fe(CN)6.3H2O  at  25°. 

(Grube,  1914.) 

Using  the  Harkins  and  Pearce  figure  for  dap,  this  result  corresponds  to  34.3  gms. 
K4Fe(CN)6  per  100  gms.  H2O. 
One  liter  of  sat.  solution  in  water  contains  385.5  gms.  K3Fe(CN)6  at  25°. 

(Grube,  1916.) 


POTASSIUM   FERRICYANIDE       532 

One  liter  sat.  sol.  in  0.4687  n  KOH|contains'342.7  gms.  K3Fe(CN)6  at  25°.  (Grube,  1914.) 

0.91328  302.3    " 

1.949  "       215.1     " 

100  cc.  anhy.  hydrazine  dissolve  2  gms.  K3Fe(CN)6  at  room  temp. 

(Welsh  and  Broderson,  1915.) 

SOLUBILITY  OF  POTASSIUM  FERROCYANIDE  IN  Aq.  POTASSIUM  HYDROXIDE 
SOLUTIONS  AT  25°.     (Grube,  1914.) 

Gms. 

s  ,  K4Fe(CN)6.3H2O 

bolvent.  per  1000  cc. 

Sat.  Sol. 
308.5  K4Fe(CN)«.3H2O    O.Q4I5WKOH    184.8     K,Fe(CN)e.3H20 

283.5  "  1-395        "         132-1 

247.1  1.883  86.12 

217.4 


Solvent 


0.  09984  W 

0.2496 
0.4963 
0.7036 


Gms. 

K4Fe(CN)6.3H20 

per  1000  cc. 

Sat.  Sol. 


Solid 
Phase. 


Solid 
Phase. 


SOLUBILITY  OF  MIXTURES  OF  POTASSIUM  FERROCYANIDE  AND  FERRICYANIDE 
IN  WATER  AND  IN  AQ.  POTASSIUM  HYDROXIDE  SOLUTIONS  AT  25°.  (Grube,  1914.) 


OU1VCLII. 

K3Fe(CN)6. 

K4Fe(CN)6. 

ouiiu  jriia.se. 

Water 

338.1 

79.02 

K3Fe(CN)6+K4Fe(CN)6.3H2O 

0.4687  wKOH 

309 

66.64 

" 

0.9628 

275-3 

55-19 

«                        « 

1.949 

200.8 

35-95 

«                        « 

SOLUBILITY  OF  POTASSIUM  FERROCYANIDE  IN  AQUEOUS  SOLUTIONS  OF 
SODIUM  FERROCYANIDE  AT  25°  AND  VICE  VERSA.  (Harkins  and  Pearce,  1916.) 


Mols.  per  1000  Gms.  H2O. 

Gms. 
K4Fe(CN)6         <*2A  of 

Mols.  per  1000  Gms.  H2O. 

Gms. 
Na4Fe(CN)6      <*«.<* 

Na4Fe(CN)6. 

K4Fe(CN)6".  Per  1000  Gms.     Sat.  Sol. 
H2O. 

K4Fe(CN)6. 

Na4Fe(CN)6. 

per  i  ooo  Gms.  Sat.  Sol. 
H2O. 

0 

O. 

89459 

329 

•5 

.09081 

0 

0.6818 

205. 

25 

1.0595 

0. 

05072 

0. 

88272 

325 

.  i 

.0990 

0.1327 

0.7056 

2I4. 

47 

1.0199 

O. 

06633 

0. 

88544 

326 

.10039 

o.  1789 

0.7213 

219. 

23 

1.0792 

0. 

12306 

0. 

88088 

324 

•4 

•09350 

0.2115 

0.7253 

220. 

44 

i.  1006 

0. 

25972 

0. 

89116 

328 

•3 

.12796 

o.  2722 

0.7610 

231. 

29 

1.1113 

0. 

4900 

O. 

91600 

337 

•4 

.17241 

0.3532 

0.7814 

237. 

49 

1.1243 

0. 

87034 

0. 

99000 

364 

.6 

.19700 

0.5850 

0.8652 

262. 

97 

1.1567 

O. 

91060 

I. 

01200 

372 

•  3 

.  21190 

o.6m 

0.8712 

264. 

79 

1.1581 

0. 

95879 

I. 

05177 

387 

•5 

.22673 

0.6994 

0.8984 

273- 

05 

1.1830 

I. 

0438 

I. 

H59 

411 

•25789 

1.0578 

0.9588 

291. 

40 

1.2267 

POTASSIUM   ZINC   CYANIDE  K2Zn(CN)4. 

100  cc.  H2O  dissolve  n  gms.  K2Zn(CN)4  at  20°.  (Sharwood,  1903.) 

POTASSIUM  FLUORIDE   KF.2H2O. 

loo  gms.  H2O  dissolve  92.3  gms.  KF,  or  100  gms.  sat.  solution  contain  48  gms. 
KF  at  18°.    Sp.  Gr.  of  solution  =  1.502.  (Mylius  and  Funk,  1897.) 

SOLUBILITY  OF  POTASSIUM  FLUORIDE  IN  HYDROFLUORIC  ACID  AT  21°. 


Gms.  per  TOO  Gms.  EfeO. 


(Ditte,  1896.) 
Gms.  per  100  Gms.  HgQ. 


Gms.  per  TOO  Gms.  H2Q. 


HF. 
0.0 
I  .21 
I.6l 

3-73 
4-03 
6-05 


KF. 

96-3 
72.0 
61  .o 
40.4 
32-5 
30-4 


'  HF. 

KF.' 

HF. 

KF.' 

9-25 

29.9 

20-68 

38-4 

11.36 

29.6 

28.60 

46.9 

12  .50 

30-5 

41-98 

61.8 

13-95 

31  .4 

53-71 

74.8 

15.98 

33-4 

74-20 

105.0 

I7.69 

35  -62 

119.20 

169-5 

533  POTASSIUM  FLUORIDE 

According  to  de  Forcrand  (1911),  a  saturated  solution  of  KF.2H2O  in  water  at 
18°  has  the  composition  I  mol.  KF  +  3.90  mols.  H20  =  45.3  gms.  per  100  gms.  sat. 
solution.  The  solution  in  contact  with  KF.4.H2O  as  solid  phase,  has  the  compo- 
sition i  mol.  KF  +  5.76  mols.  H2O  =  35.96  gms.  KF  per  100  gms.  sat.  solution. 

EQUILIBRIUM  IN  THE  SYSTEM  POTASSIUM  FLUORIDE,  ETHYL  ALCOHOL  AND 
WATER  AT  2^-26°. 

(Frankforter  and  Frary,  1913.) 

The  authors  determined  the  binodal  curve,  the  quadruple  points  and  two  tie  lines. 

Gms.  per  100  Gms.  Upper  Layer.  Gms.  per  100  Gms.  Lower  Layer. 

fKF.  C2H5OH.  H^O?  lEi\  QH6OH.  H^ 

1.23  92.67  6.07*  45.33  0.67  54* 

...  ...  37-82  1.70  60.49 

1.16  83.30  15-54 

28.68  4.47  66.85 

2.86  65.81  31.33 

4-47  57-4  38-13  20.90  11.9  67. af 

5-47  53 -°4  41-49 

18.55  15-6  65.85 

6.93  47-52  45-55 

8.84  41.28  49.88  15.7  21.8  62. 5t 

9-55  38.66  51.79 

13-57  27.27  59.15 

10.52  35.91  53.57 

ii-43  33-23  54-34 

ii  30  59  ii  30  59t 

*  Quad,  points.  t  Tie  line.  J  Plait  point  approx. 

A  method  for  the  determination  of  alcohol  in  unknown  mixtures,  based  upon  the 
above  data,  is  described  by  the  authors. 

THE  BINODAL  CURVE  FOR  THE  SYSTEM  POTASSIUM  FLUORIDE,  PROPYL  ALCOHOL 
AND  WATER  AT  2^-26°. 

(Frankforter  and  Frary,  1913.) 
Gms.  per  100  Gms.  Homogeneous  Liquid.  Gms.  per  100  Gms.  Homogeneous  Liquid. 

KF\  C3H7OH.  H20."  !Ei\ C3H7OH.  H^O? 

0.17  96.78  3.05*  8.15  7.49  84.36 

0.31  78.91  21.19  10  5-97  84.03 

0.62  66.29  33.09  12.21  4.39  83.41 

0.81  59.97  39.22  14.18  3.45  82.37 

1.29  47.46  51.21  18.75  1-89  79-35 

i-77  35-40  62.83  25.83  0.74  73.43 

2.50  19.05  78.45  35-38  0.23  64.38 

5.32  10.64  84.04  47-62  0.039  52-34* 

*  Quad,  point. 

One  tie  line  was  determined.  In  this  case  the  upper  layer  contained  78.91% 
C3H7OH  and  0.31%  KF,  and  the  lower  layer  contained  9.67%  KF. 

In  this  system,  the  effect  of  change  in  temperature  is  more  marked  than  in 
the  preceding  one  in  which  ethyl  alcohol  is  present. 

100  gms.  sat.  solution  of  potassium  fluoride  in  99.6%  propyl  alcohol  contain 

0.34  gm.  KF  at  room  temp.  (Frankforter  and  Frary,  1913.) 

BINODAL  CURVE  FOR  THE  SYSTEM  POTASSIUM  FLUORIDE,  ISOPROPYL  ALCOHOL 

AND  WATER  AT  20°. 

(Frankforter  and  Temple,  1915.) 

Results  in  terms  of  gms.  per  100  gms.  of  solvent,  alcohol  +  water. 

Gms.  per  100  Gms.  Solvent.  Gms.  per  100  Gms.  Solvent. 

'KF.  CH3CHOHCH3.  H2O.                          'KK  CH3CHOHCH3.  H2O/ 

51.826                1.555  98.445  12.385              21.438  78-562 

38.748               2.965  97-035                      5-07I              59-339  40.661 

36.039             6.525  93-475                    3-973            65.455  34-545 

17.813            13.215  87.785                     1.705             82.750  17-250 


POTASSIUM  FLUORIDE  534 

BINODAL  CURVE  FOR  THE  SYSTEM  POTASSIUM  FLUORIDE,  ALLYL  ALCOHOL 
AND  WATER  AT  20°. 

(Frankforter  and  Temple,  1915.) 

The  results  are  given  in  terms  of  grams  per  100  gms.  Alcohol  +  Water  instead 
of  gms.  per  100  gms.  of  the  homogeneous  mixture. 

Gms.  per  100  Gms.  Solvent.  Gms.  per  100  Gms.  Solvent. 


KF.  CH2:CH.CH2OH.          H2O.  KF.          CH2:CHCH2OH.          H2O. 

45.707      2.270    97-730       7.508    35-390    64.610 

38.076       3-983     96.017         6.624     42.011      57.989 
30.675       5.879     94.121         4.813     47-550     52.450 

24.341  7.129  92.871  3.631  54-211  45-789 

20.580  9.691  90-309  2.236  59-948  36.443 

17.371  11.491  88.509  1.931  65.630  34.370 

13.184  17.764  82.236  1-635  68.845  31.155 

10.880  22.537  77-463  1.368  71-395  28.605 

8.873  29.529  70.471  1-066  75-377  24.223 

BINODAL  CURVE  FOR  THE  SYSTEM  POTASSIUM  FLUORIDE,  ACETONE,  WATER 

AT  20°. 

(Frankforter  and  Cohen,  1914.) 

Gms.  per  100  Gms.  Homogeneous  Mixture.  Gms.  per  100  Gms.  Homogeneous  Mixture. 

r  KF. (CH3)2CO.  H2O.  ^  KF.  (CH3)2CO.  H2O. 

46.3  trace  53.7*  9.17  23.53  67.30 

44.24  0.24  55.52  5  38.72  56.28 

33.34  i  65.66  3.06  47.89  46.84 

29.86  i. 60  68.54  1.38  58.06  40.55 

25.74  3.02  71.24  0.979  62.60  36.42 

20.28  5.90  73 .80  0.75  65.41  33.84 

16.31  9.72  73.97  0.50  69.58  29.92 

12.40  15.59  72.01  O  98  2* 

*  Quad,  point. 

Data  for  4  tie  lines  are  also  given  and  the  approximate  position  of  the  plait 
point  is  shown  on  the  diagram. 

Several  points  on  the  binodal  curves  at  temperatures  between  o°  and  35°  are 
also  given. 

A  discussion,  with  examples,  is  given  of  the  applicability  of  the  above  data  to 
the  determination  of  acetone  in  unknown  mixtures. 

BINODAL  CURVE  FOR  THE  SYSTEM  POTASSIUM  FLUORIDE,  METHYL  ETHYL 
KETONE  AND  WATER  AT  20°. 

(Frankforter  and  Cohen,  1916.) 
Gms.  per  100  Gms.  Homogeneous  Mixture.  Gms.  per  too  Gms.  Homogeneous  Mixture. 

/ A >  t A N 

KF.  CHj.CO.C2Hj.  H2O.  KF.  CHS.CO.C2HB.  H2O. 

34.38  0.17  65.45  10.50  4.87  84.63 

23-63  0.50  75.87  5.70  9.93  84.37 

18.62  1.49  79.89  3.96  12.42  83.61 

15.91  2.19  81.90  0.84  21.23  77.93 

13.80  2.98  83.22  0.34  23.55  76.11 

Freezing-point  data  (solubilities,  see  footnote,  p.  i)  for  mixtures  of  KF  +  KI 
are  given  by  Ruff  and  Plato  (1903).  Results  for  KF  +  KOH  by  Scarpa  (1915). 
Results  for  KF  +  KPO3,  KF  +  K4P2O7  and  KF  +  K3PO4  are  given  by  Amadori 
(1912).  Results  for  KF  +  K2SO4  are  given  by  Karandeef  (1909).  Results  for 
KF  +  NaF  are  given  by  Kurnakow  and  Zemcznzny  (1907). 


535 


POTASSIUM  FORMATE 


POTASSIUM  FORMATE  HCOOH. 


SOLUBILITY  OF  POTASSIUM  FORMATE  AND  OF  THE  ACID  SALT  IN  WATER. 


Solid  Phase  :  HCOOK. 

A 

(Groschuff,  1903.) 
Solid  Phase  :  HCOOK.HCOOH. 

Cms. 

Mols. 

Cms.  HCOOK.- 

Cms. 

Cms. 

Mob. 

HCOOK 

HCOOK 

HCOOH 

HCOOK 

HCOOK 

HCOOH 

t°. 

per  too 

per  100 

r. 

per  100 

per  100 

r. 

per  100 

per  i 

Cms. 

Mols. 

Cms. 

Cms. 

Cms. 

Mol. 

Solution. 

HjO. 

Solution. 

Solution. 

Solution. 

HCOOK. 

—     2O 

72.8 

57-4 

o 

6o-4 

39-o 

0 

36.3 

3-21 

+   18 

76.8 

71.0 

25 

69.8 

4S-i 

19-5 

38.2 

2.96 

So 

80.7 

89.8 

50 

79-2 

51.2 

39-3 

40.8 

2.65 

90 

86.8 

141.0 

80 

90.7 

58.6 

60 

44.0 

2-33 

120 

92.0 

247.0 

70 

45-9 

2.16 

140 

96.0 

5ii 

90 

S2-! 

1.68 

157 

IOO.O 

00 

Sp.  Gr.  of  sat.  solution  at  18°  =  1.573. 

NOTE.  —  Since  the  acid  salt  is  less  soluble  at  ordinary  temperatures  than  the 
neutral  salt,  it  can  be  precipitated  from  the  solution  of  the  neutral  salt  by  addi- 
tion of  aqueous  formic  acid.  Proceeding  in  this  way  an  impure  product  is  ob- 
tained, giving  solubility  values  (expressed  in  HCOOK)  as  shown  in  the  last  three 
columns  above. 


POTASSIUM   GERMANIUM  FLUORIDE  K,GeF6. 
SOLUBILITY  IN  WATER. 

(Winkler,  1887;  Kruss  and  Nilson,  1887.) 

100  gms.  H2O  dissolve  173.98  gms.  K2GeF6  at  18°,  and  34.07  gms.  at  100°  (W.). 
100  gms.  H2O  dissolve  184.61  gms.  K2GeF6  at  18°,  and  38.76  gms.  at  100° 
(K.  and  N.). 


POTASSIUM  HYDROXIDE  KOH. 


Gms.  KOH  per 
4°.                   100  Gms. 

Water. 

Solution. 

2.2 

3- 

7 

3 

.6 

20-7 

22. 

5 

18 

•4 

65.2 

44. 

5 

30 

.8 

36.2 

36. 

2 

26 

.6 

32.7 

77- 

94 

43 

.8 

33 

80 

44 

•4 

23-2 

85 

45 

•9 

0 

97 

49 

.2 

10 

103 

50 

•7 

SOLUBILITY  IN  WATER. 

(Pickering,  1893;  at  15°,  Ferchland,  1902.) 


Solid  Phase. 


Ice 


KOH.4H20 

KOH.4HjO+KOH.2H2O 
KOH.2H,0 


Gms.  KOH  per 

t°.                  100  Gms. 

Solid  Phase. 

Water. 

Solution. 

15 

107 

51-7 

KOH.2H2O 

20 

112 

52.8 

it 

30 

126 

55-76 

" 

32-5 

135 

57-44 

KOH.2H2O+ 

50 

I4O 

58.33 

KOH.H,O 

100 

I78 

64.03 

KOH.HjO 

125 

213 

68.06 

" 

143 

3II.7 

75-73 

ii 

Sp.  Gr.  of  sat.  solution  at  15°  =  1.5355. 

100  gms.  sat.  solution  in  H2O  contain  50.48  gms.  KOH  at  15°. 

(de  Forcrand,  1909.) 
ioo  gms.  sat.  solution  in  H2O  contain  53.1    gms.  KOH  at  15°. 

(Greenish  and  Smith,  1901.) 


POTASSIUM  HYDROXIDE  536 

SOLUBILITY  OF  POTASSIUM  HYDROXIDE  IN  AQUEOUS  SOLUTIONS  OF  ETHYL 

ALCOHOL  AT  30°.      (deWaal,  1910.) 
Cms.  per  ioo  Cms.  Sat.  Sol.  Gms.  per  100  Cms.  Sat.  Sol. 


KOH.           QHsOH. 

H20. 

ooiiu  .rnase. 

KOH.         C2H4OH. 

H20. 

soiia  rb&se. 

55 

75 

0 

44-25 

KOH.2H2O 

27. 

67 

69 

92 

2.41 

KOH.2H2O 

54 

,8l 

0.43 

44.76 

" 

27. 

20 

73- 

01 

negative* 

« 

Two  liquid  layers  are  formed  here. 

26. 

25 

81. 

95 

« 

« 

31 

57.50 

11.50 

KOH.2H2O 

28. 

99 

65.07 

5-94 

» 

*  Negative  on  account  of  reaction  KOH+QjHjOH—  ^QHjOK+HjjO. 

Data  for  equilibrium  in  the  system  potassium  hydroxide,  phenol,  water  at  25° 
are  given  by  van  Meurs  (1916). 

Freezing-point  data  for  KOH  +  RbOH  and  KOH  +  NaOH  are  given  by 
von  Hevesy  (1900).  Results  for  KOH  +  KI  are  given  by  Scarpa  (1915). 

POTASSIUM  IODATE  KIO3. 

SOLUBILITY  IN  WATER. 

(Kremers,  i8s6a;  at  30°,  Meerburg,  1904.) 
t°.  0°  20°  30°  40°         60°         80°        100° 

Gms.  KI03  per  ioo  gms.  H2O    4.73    8.13     11.73     I2-8     l8-5     24.8    32.2 
100  gms.  H2O  dissolve  1.3  gms.  potassium  hydrogen  iodate,  KH(IO3)2,  at  15°* 

and  5.4  gms.  at  17°.  (Semllas.) 

ioo  gms.  H2O  dissolve  4  gms.  potassium  dihydrogen  iodate,  KH2(IO3)3,  at  15°. 

(Meineke,  1891.) 

EQUILIBRIUM  IN  THE  SYSTEM  POTASSIUM  IODATE,  IODIC  ACID,  WATER  AT  30°. 

(Meerburg,  1905.) 

Gms.  per  ioo  Gms.  Gms.  per  ioo  Gms. 

Sat.  Sol.  Solid  Phase.                              Sat.  Sol.                             Solid  Phase. 

HI03.            KI03.  "                                                    '  HI03.               KIOT 

O                   9.51  KI03                                      3-47             3-59        KIO3.2HI03  (unstable) 

0.65            9.49  «  +KI03.HIO,                  4-80             2.90 

0.65            8.90  KIOj.HIO,                             6.45             1.35 

0.67            6.6  "                                         9.35             0.64                KIO3.2HIO3 

1.14         4-57  "  12.04          0.44 

1.69         3.63  «  17-50          0-30 

2. 02  3-10  "  31.20  0.52  " 

3.34         2.10  "  53-64          0.68 

5  1.32  "  62.52          0.72 

7.09  I  '«  76.40  0.8o  +HI03 

8.04  0.85  «  +KI03.2HIO3  76.7  O  HI03 

ioo  cc.  anhydrous  Hydrazine  dissolve  I  gm.  KIO3  at  room  temp. 

(Welsh  and  Broderson,  1915.) 

POTASSIUM   PerlODATE   KIO4. 

ioo  gms.  H2O  dissolve  0.66  gm.  KIO4  at  13°,  dig.  of  sat.  solution  =  1.0051. 

(Barker,  1908.) 

POTASSIUM   IODIDE 

SOLUBILITY  IN  WATER,  DETERMINED  BY  THE  FREEZING-POINT  METHOD. 

(Kremann  and  Kershbaum,  1907.) 
Gms.  KI  per  CrtV A  Gms.  KI  per         <-  KJ 

&.<&      %£•  '"•        &.<§£     $2- 

-12.5  38  Ice  -22.5  52.1  KI 

—  15  41.2  "  —20  52.6 

-17-5  44-6  "  -15  53-5 

—  20  48  "  —10  54-5  " 

-22.5  51.2  «  -  5  55.4 

—  23.2Eutec.          51.9  "  +KI  o  56.4  " 


537 


POTASSIUM  IODIDE 


POTASSIUM  IODIDE  KI. 

SOLUBILITY  IN  WATER. 

(Mulder;  de  Coppet,  1883;  Etard,  1894;  Meusser,  1905;  see  also  Tilden  and  Shenstone,  1884; 
Scbreinemakers,  1892.) 


Gms.  KI  per  TOO  Gms. 

Water. 

Solution. 

10 

II5.I 

53-5 

5 

II9.8 

54-5 

i 

122.2 

55  '® 

0 

127.5 

56.0 

10 

136 

57-6 

20 

144 

59-O 

25 

148 

59-7 

30 

152 

60.3 

40 

160 

61.5 

50 

168 

62.7 

60 

176 

63-7 

70 

184 

64.8 

Gms.  KI  per  100  Gms. 


*  . 

Water. 

Solution. 

80 

192 

65.8 

90 

200 

66.7 

100 

208 

6?  5 

no 

215 

68,3 

120 

223 

69.0 

Ice  Curve 

-  5 

25-7 

22    5 

-  7 

42  .6 

29.9 

-  9 

5      5J'5 

34-o 

—  ii 

•5      64.7 

39-3 

-14 

75-8 

42.7 

Sp.  Gr.  of  sat.  solution  at  15.2°  =  1.704.  (Greenish  and  Smith,  1901.) 

Individual  determinations,  in  good  agreement  with  the  above  results,  are  given 
by  van  Dam  and  Donk  (1911),  and  by  Greenish  and  Smith  (1901). 

SOLUBILITY  OF  POTASSIUM  IODIDE  +  IODINE  IN  WATER  AT  25°. 

(Foote  and  Chalker,  1908.) 


Gms.  per 

100  Gms. 

Sat.  Sol. 

Present  in 
Solid  Phase. 

'  KI. 

I. 

I-KI. 

29-45 

64.34 

34.89 

Kland 

28.91 

63.88 

34-97 

KI3 

26.84 
27.18 

66.54 
67.14 

39.70 
39.96 

KI3  and 
KI. 

27.14 

66.00 

39.46 

Bhlf 

Gms.  per 

100  Gms.  Sat.  Sol. 

Present  in 
Solid  Phase. 

'   KI. 

I.             I  —  KI. 

25-88 

68.79        42.91 

KI7  and 

25.57 

69.01        43.44 

Iodine 

27.86 

66.56 

27.27 

66.91 

3 

26.95 

67.17 

KI, 

25.71 

67.91 

JXJ.7 

The  experiments  of  Hamberger  (1906)  are  discussed.     (See  also  p.  326.) 

SOLUBILITY  OF  MIXTURES  OF  POTASSIUM  IODIDE  AND  SILVER  IODIDE  IN 
WATER  AT  o°,  30°  AND  50°. 

(Van  Dam  and  Donk,  1911.) 


Results  at  o°. 

Gms.  per  TOO  Gms.  Sat.  Sol. 


Results  at  30°. 

Gms.  per  100  Gms.  Sat.  Sol. 


Results  at  50°. 


Agl. 

KI. 

O 

56.1 

9 

53 

18 

51-2 

3i.3 

46.6 

37-9 

44 

37-6 

42.7 

38 

41-3 

28.1 

36.4 

26.6 

34-6 

6.5 

26.1 

i-5 

20.5 

0.2 

9.8 

27-5 

48.7 

21 

50.3 

Agl. 

KI. 

O 

60.35 

16 

55-5 

35-8 

46.9 

42.8 

43-9 

44.1 

43-2 

47-7 

40.9 

49-7 

38.6 

42.8 

38.8 

29.4 

37-6 

10 

31-4 

O.I 


IO.2 


jms.  per  100  Gms.  Sat.  So 

I-  Solid  Phase  in 
Each  Case. 

Agl. 

KI. 

0 

62.6 

KI 

10.7 

59-1 

« 

22.8 

55-5 

" 

45 

43-2 

tt 

53-4 

37-6 

"  +AgI.KI 

53-5 

37-1 

AgLKI 

53-5 

36-6 

"  +AgI 

53-5 

36.5 

Agl 

39 

38.1 

28 

36.7 

« 

16 

33-8 

« 

2-5 

24.8 

" 

Agl.aKI+KI 

Agl.aKI 

POTASSIUM  IODIDE 


538 


SOLUBILITY  OF  POTASSIUM  IODIDE  IN  DILUTE  AQUEOUS  SOLUTIONS  OF  ETHYL 


ALCOHOL  AT  25°. 

(Armstrong,  Eyre,  Hussey,  and  Paddison,  1907.) 

Wt.  Per  cent 

d     of 

Gms.  KI 

Wt.  Per  cent 

d      of 

Gms.  KI 

CjHjOH  in 
Solvent. 

SatTSoL 

per  ioo  Gms. 
Sat.  Sol. 

QHsOH  in 
Solvent. 

"25.  ^*L 
Sat.  Sol. 

per  ioo  Gms. 
Sat.  Sol. 

O 

1.7268 

59.80 

4.41 

1.6833 

58.08 

1.  14 

I.7I54 

59-41 

12.14 

I  .  6063 

54-93 

2.25 

I  .  7042 

58-95 

18.73 

1.5420 

52.08 

loo  gms.  aqueous  94%  ethyl  alcohol  dissolve  3.99  gms.  KI  at  17°.      (de  Bruyn,  1892.) 
I oogms.  aqueous  98%  methyl  alcohol  dissolve  17.1  gms.  KI  at  17°. 
ioo  cc.  of  ethyl  alcohol  of  di6  =  0.8292  dissolve  8.83  gms.  KI  at  15°,  dm  of  sat. 
solution  =  0.8989.  (Greenish  and  Smith,  1901.) 

SOLUBILITY  OF  POTASSIUM  IODIDE  IN  ABSOLUTE  ALCOHOLS. 

(de  Bruyn  — Z.  physik.  Ch.  10,  783,  '92;  Rohland  —  Z.  anorg.  Ch.  18,  327,  '98.) 

ioo  gms.  methyl  alcohol  dissolve  16.5  gms.  KI  at  20.5°. 

100  gms.  ethyl  alcohol  dissolve  1.75  gms.  KI  at  20.5°. 

ioo  gms.  propyl  alcohol  dissolve  0.46  gm.  KI  at  i5°-2o°  (R.). 

SOLUBILITY  OF  POTASSIUM  IODIDE  IN: 


Ethyl  Alcohol 

of  0.9496  Sp.  Gr. 

Aqueous  Ethyl  Alcohol  at  18°. 

r 

Gms.  KI  per 

Sp.  Gr. 

Weight 

Gms.  KI 

Sp.  Gr. 

Weight 

Gms.  K! 

t°. 

IOO 

Gms.  Alcohol 

of 
Alcohol. 

per  cent 
Alcohol. 

per  ioo  Gms. 
Alcohol. 

of 

Alcohol. 

per  cent 
Alcohol. 

per  ioo  Gms 
Alcohol. 

8 

67.4 

0.9904 

S-2 

I30.5 

0.9390 

45 

66.4 

13 

69.2 

0.9851 

9.8 

119.4 

0.9088 

59 

48.2 

25 

75-1 

0.9726 

23.0 

IOO.  I 

0.8464 

86 

II.4 

46 

84-7 

0.9665 

29.0 

89.9 

0.8322 

91 

6.2 

55 

87-5 

0.9528 

38.0 

76.9 

62  9° '  ^  (Gerardin  —  Ann.  chim.  phys.  [4]  5,  155,  '65.^ 

SOLUBILITY  OF  POTASSIUM  IODIDE  IN  AQUEOUS  SOLUTIONS  OF  METHYL  ALCOHOL 


Solvent. 


(Herz  and  Anders,  1907.) 
Sat.  Solution.  Solvent. 


Sat.  Solution. 


Wt.  Per  cent       j 

Gms. 

KI 

Wt.  Per  cent 

Gms.  KI" 

*•¥>'           CH3OH. 

"V 

per  ioo  cc.                a^' 

CH3OH. 

«^6- 

per  ioo  cc. 

0.9971 

O 

1.7213 

102. 

9 

0. 

8820 

64 

I 

.185 

40.33 

0.9791 

10. 

6 

1.634 

92. 

12 

O. 

8489 

78.1 

i 

.066 

28.05 

0.9481 

30. 

8 

1.460 

55 

0. 

8167 

93-9 

0 

.9700 

18.76 

0.9180 

47. 

i 

1.325 

55- 

6 

0. 

7881 

IOO 

0 

.9018 

13.28 

SOLUBILITY  OF  POTASSIUM  IODIDE  IN  SEVERAL  ALCOHOLS. 

Alcohol. 

Methyl  Alcohol 


Ethyl 
« 

Propyl 
Amyl 


t°. 

Gms.  KI  per  ioo 
Gms.  Alcohol. 

Authority. 

ii.  4 

13-5 

(Timofeiew,  1894.) 

12.2 

14.6 

" 

13-5 

16 

" 

25 

18.04 

(Turner  and  Bissett, 

I9I3-) 

13.6 

1.63 

(Timofeiew,  1894.) 

25 

2.16 

(Turner  and  Bissett, 

I9I3-) 

12.2 

o.73i 

(Timofeiew,  1894.) 

25 

0-43 

(Turner  and  Bissett, 

1913-) 

25 

0.098 

« 

ioo  cc.  sat.  solution  of  KI  in  ethyl  alcohol  contain  1.585  gms.  KI  at  25°. 

(Laurie,  1912.) 


539 


POTASSIUM  IODIDE 


SOLUBILITY  OF  POTASSIUM  IODIDE  IN  LIQUID  METHYL  ALCOHOL  AT  TEM- 
PERATURES UP  TO  THE  CRITICAL  POINT. 

(Tyrcr,  1910.) 

(Determined  by  the  Sealed  Tube  Method.) 


r. 

15 
5  = 

5  = 
Bo 

ICO 


14-50 

16.20 

18.9 

22.5 

25 


r. 


140 
160 


r.  ioo 


27.2 
29.2 

30.6 

30-7 
29.1 


240 

245 
247 

250 


cnt,  temp.  252.5 


27-5 
24-8 

22.6 

21 

13-8 

7-6 


SOLUBILITY  OF  POTASSIUM  IODIDE  IN  VAPOR  OF  METHYL  ALCOHOL  ABOVE 
THE  CRITICAL  POINT. 

(Tyrer,  1910*.) 
GBS-ODiaohrdprriooGi 


Btai 


:,:  = 


300 


i 

33 

7 


i  cc.  Vapor. 
O.I 
O.2 

0-3 
0.36 

0-4 
0.45 

Data  for  the 

author  gives  the  crit.  temp,  as  266°  and  the  corresponding  concentration  as  8.64 
gms.  KI  per  ioo  gms.  of  the  sat.  solution. 


0-3 

i 

3-7* 

7-6 

ii. 8 

18.1 


i 

3-5 
7-4 
ti-5 


?y~:e~ 


I 

34 
73 
tt-3 

given  by 


I 

3-4 
7-2 
ii 


rszwer  (1910).     This 


SOLUBILITY  OF  POTASSIUM  IODIDE  IN  MIXTURES  OF  ALCOHOLS  AT  25°. 
fliu  •ir^a.  1908.) 

In  Methyl  -f  Ethyl  1 


In  Ethyl  +  Prop>*l 


SfiS*1 

sSsoL 

9SfSSi 

•as* 

S^SoL    ^loT-  CSSL~   S.L.SOL   ] 

per  ioo  a 
Sat-SoL 

0 

0.8015 

i-55 

0 

O.QOlS 

13.16 

0 

0.8015 

1-55 

4  37 

0.8041 

1.91 

n.  ii 

0.8823 

IO.O6 

8.1 

0.7983 

1.46 

10.4 

0.8071 

2.25 

238 

0.8629 

8-54 

17  85 

0.7991 

1-37 

41.02 

0.8295 

4  94 

65.2 

0.8187 

2.62 

56.6 

0.7988 

0-75 

80.69 

0.8794 

10.13 

91.8 

0.8045 

0.60 

88.6 

0.8022 

0-52 

-   -- 

0.8795 

10.72 

96.6 

0.8041 

0.58 

91.2 

0.8027 

0-49 

91.25 

0.8oo8 

11.84 

IOO 

0.8041 

0-43 

95  2 

0.8029 

0-44 

ICO 

O.OOlS 

13.16 

IOO 

0.8041 

0-43 

SOLUBILITY  OF  POTASSIUM  IODIDE  IN  ACETAMIDE. 


t»                    GMS.  KI  per  ioo 

Sofid 

*  - 

OK.Sit.SoL 

}-_>i 

82  m.  pt. 

O 

CHjGOXH- 

78 

6-5 

- 

74 

12.8 

m 

70 

17-8 

" 

66 

21-5 

M 

$ 

26.2 

M 

53  Eutec, 

28.4 

•+n 

7~ 

85 

ioo 

130 
145 

IOO 

175 


Gms.  KI  per  ioo 
G-B.Sat.5oL 

28-75 
29.1 

29  45 
30-15 
30-5 

30-8 


POTASSIUM  IODIDE 


540 


SOLUBILITY  OF  POTASSIUM  IODIDE  IN  ACETONE  AND  IN  PYRIDINE. 

(von  Laszcynski,  1894;  at  25°,  Krug  and  McElroy,  1892.) 
Cms.  KI  per  100  Cms.  Solvent  at: 


Solvent. 

Acetone 
Pyridine 


—  2.5°                    10° 

22° 

2-38 

25° 

2-93 

56° 
I.  21 

119° 

0.26 


O.II 


100  gms.  glycerol  dissolve  40  gms.  KI  at  15.5°.  (Ossendowski,  1907.) 

100  gms.  95%  formic  acid  dissolve  38.2  gms.  KI  at  18.5°.  (Aschan,  1913.) 

100  cc.  anhydrous  hydrazine  dissolve  175  gms.  KI  at  room  temp. 

(Welsh  and  Broderson,  1915.) 

100  gms.  hydroxylamine  dissolve  no  gms.  KI  at  17.5°.  (de  Bruyn,  1892.) 

100  gms.  sat.  solution  in  hydrated  lanolin  (containing  30%  emulsified  water) 

contain  42.5  gms.  KI  at  45°.     (Klose,  1907;)     KI  is  insoluble  in  anhydrous 

lanolin. 


SOLUBILITY  OF  POTASSIUM  IODIDE  IN  SEVERAL  SOLVENTS. 

(Walden,  1906.) 


Solvent. 

Water 

Water 

Methyl  Alcohol 

Methyl  Alcohol 

Ethyl  Alcohol 

Ethyl  Alcohol 

Glycol 

Glycol 

Acetonitrile 

Acetonitrile 

Propionitrile 

Propionitrile 

Benzonitrile 

Nitromethane 

Nitromethane 

Nitrobenzene 

Acetone 

Acetone 

Furfurol 

Furfurol 

Benzaldehyde 

Salicylic  Aldehyde 

Salicylic  Aldehyde 

Anisic  Aldehyde 

Anisic  Aldehyde 

Ethyl  Acetate 

Methyl  Cyanacetate 

Methyl  Cyanacetate 

Ethyl  Cyanacetate 


_                  . 

*«       SD.Gr.of                      oms.^perioo 

1*  orrnula,. 

Solution. 

cc.  Solution.        Gms.  Solution. 

H2O 

o    i  .  6699 

94-05 

56.32 

H2O 

25      I-7254 

IO2  .  70 

59-54 

CH3OH 

o    0.8964 

ii.  61 

12.95 

CH3OH 

25    0.9003 

13.5-14.3 

14.97 

C2H5OH 

o    0.8085 

1.197 

1.479 

C2H5OH 

25    0.7908 

1.520 

1.922 

(CH2OH)2 

0      1-3954 

45-85 

31-03 

(CH2OH)2 

25   1.3888 

47-23 

33-01 

CHgCN 

o    0.8198 

1.852 

2.259 

CH3CN 

24  0.7938 

i-57 

2.003 

C2H5CN 

o    0.8005 

0.34-0.41 

0.0429 

C2H5CN 

25    0.7821 

0.32-0.36 

0.0404 

C6H5CN 

25 

[.0076 

0.051 

0.0506 

CH3NO2 

0 

[.1627 

0.314-0.366 

0.315 

CH3NO2 

25   1.1367 

0.289-0.349 

0.307 

CeHsNC^ 

25 

.  .  . 

0.0019 

(CH3)2CO 

o    0.8227 

1.732 

2.105 

(CH3)2CO 

25    0.7968 

1.038 

1.302 

CAO.COH 

0 

15.  10 

.  .  . 

C4H3O.COH 

25 

.2014 

5.62 

4-94 

C6H5COH 

25 

.0446 

0.343 

0.328 

C6H4.OH.COH 

o 

•  1501 

1.257 

1.093 

C6H4.OH.COH 

25 

•1373 

0.549 

0.483 

C6H4.OCH3.COH 

o 

.1223 

1.520 

1-355 

CeH4.OCH3.COH 

25 

.1180 

0.720 

0.644 

CH3COOC2H5 

25 

.  .  . 

0.0013 

CHoCNCOOCHg 

o 

.1521 

3.256 

2.827 

CH2CNCOOCH3 

25 

.1358 

2.459 

2.165 

CH2CNCOOC2H5 

25 

.0628 

0.989 

0.930 

541  POTASSIUM  IODIDE 

SOLUBILITY  OF  POTASSIUM  IODIDE  AT  20°  IN  SEVERAL  SOLVENTS  CONTAINING 

DISSOLVED  IODINE. 

(Olivari,  1908.) 
Gm.  Mols.  KI  per  Liter  in  Solvent  Containing: 

Solvent.  as  Gm.  Mols.  Ts~Gm.  Mols.  2.5  Gm.  Mols. 

I2  per  Liter.  Ij  per  Liter.  I2  per  Liter. 

Acetic  Acid  0.511                   1.460  2.080 

Ethyl  Acetate  0.490                    1.400  1.980 

Ethyl  Alcohol  0.520                    1.220  1.730 

Nitrobenzene  0.414                   0.960  1.380 

Ethylbromide  0.140                   0.350 

EQUILIBRIUM  IN  THE  SYSTEM  POTASSIUM  IODIDE — ETHYL  ETHER — WATER  AT  20°. 

(Dunningham,  1914-) 

Cms.  per  too  Gms.  Upper  Layer.                          Gms.  per  100  Gms.  Lower  Layer.  Solid 

KL~~       ~~HA            (C2H6)20.                    liL*""  H2O.  (QH^O.  Phase- 

59-2  40.8  ...               KI 

o                    3.9               96.1                       o  93  7  None 

0.4                0.4               99-2                      55-6  40-7  3-7             KI 

O.I                  2.2                97.7                       25  72.1  2.9  None 

DISTRIBUTION  OF  POTASSIUM  IODIDE  BETWEEN  WATER  AND: 
Nitrobenzene  at  1 8°.     (Dawson,  1908.)      Phenol  at  Room  Temp.     (Riesenfeld,  1902.) 

Mols.  KI  per  Liter.                    Dist.                         Gms.  KI  per  100  cc.  Dist. 

CeHfiNOz  Layer"!      H2O  Layer.         Ratio.              C6H6OH  Layer!     Aq.  Layer.'  Ratio. 

O.OOII4      6.05      5300         0.052       0.725  13.2 

0.00108      6.05      5600         0.197       2.42  12.3 

2.09       30.7  14-7 

Freezing-point  data  for  KI  +  K2SO4  and  KI  +  NaCl  are  given  by  Ruff  and 
Plato  (1903).  Results  for  KI  +  Agl  are  given  by  Sandonnini  (i9i2a).  Results 
for  KI  -f-  SO2  are  given  by  Walden  and  Centnerszwer  (1903). 

POTASSIUM   IODOMERCURATE  (Thoulet  Solution). 

A  sat.  solution  at  22.9°,  prepared  by  adding  KI  and  HgI2  in  excess  to  water, 
contained  8.66%  K,  22.49%  Hg,  52.58  (57.7)  %  I  and  10.97  (11.15)%  H2O, 
corresponding  to  0.22  mol.  alkali,  o.n  mol.  Hg  and  0.45  mol.  I.  (Duboin,  1905.) 

POTASSIUM  MOLYBDATE   K2MoO4 

SOLUBILITY  OF  POTASSIUM  MOLYBDATE  IN  AQUEOUS  SOLUTIONS  OF  POTASSIUM 
SULFATE  AT  25°  AND  VlCE  VERSA. 

(Amadori,  igi2a). 

Gms.  per  100  Gms.  H2O.  Gms.  per  100  Gms.  H2O. 

fzSOT K2MoO4:  KjSOT K2MoO4.' 

o                           184.6                              1.50  99-49 

0.46                     180.7                              2-T3  45-89 

0.72                     177                                  3.95  17-48 

0.98                     127.2                             8.55  4-73 

1.27                    JO7.5                          12. 10  o 

Freezing-point  data  for  K2MoO4+  K2SO4,  K2MoO4  +  K2WO4  and  K2Mo2O 
+  K2W2O7  are  given  by  Amadori  (1913). 

POTASSIUM  NITRATE   KNO3. 

SOLUBILITY  ICE  CURVE  AND  SUPERSOLUBILITY  ICE  CURVE. 

(Jones,  1908.) 
Gms.  KNO3  per  100  Gms.  H2O.  Gms.  KNO3  per  100  Gms.  H2O. 

of  Cryst                    Solubility  Supersolubility  o{  Cryst.  Solubility  Supersolubility 

Ice  Curve.  Ice  Curve.  Ice  Curve.  Ice  Curve. 

-I                            3.336  I. Oil  -3                              ...  5.762 

—  2                           7.582  3-S38  —4                             ...  8.694 

—  2.8*                   11.62  5.56  —5                             ....  II. 12 

-5-3*  ...  ".82 

*  Cryohydrate. 


POTASSIUM  NITRATE  542 

SOLUBILITY  IN  WATER. 

(Mulder;  Andrae,  1884;  Gerardin,  1865;  Etard,  1894;  Ost,  1878;  at  31.25°,  Kohler,  1897;  Euler,  1904; 
Tilden  and  Shenstone,  1884;  Berkeley,  1904.) 

Average  Curve. 

9  Gms.  KNOa  per  TOO  Gms.  .  Gms.KNO3  per  TOO  Gms. 

Water.  Solution.  Water.          Solution. 

o  13-3          11.7  70  *38          58  o 

10  20.9          17.3  80  169          62.8 

2O  3I-6  24.O  9O  2O2  66.9 

25  37.3  27.2  ioo  246  71.1 

30  45-8  3J-4  no  300  75.0 

40  63.9  39.0  120  394  79-8 

50  85.5  44-o  125  493  83.1 

60  no.o  52.0 

The  very  carefully  determined  figures  of  Berkeley  are  as  follows: 


dt  of 

Gms.  KNOs  per 

d.oi 

Gms.  KNO3  per 

Sat.  Sol. 

ioo  Gms.  H2O. 

' 

Sat.  Sol. 

ioo  Gms.  HjO. 

0.40 

1.0817 

13-43 

60.05 

I-3903 

111.18 

14.90 

1.1389 

25.78 

76 

1.4700 

156.61 

30.8o 

I.22I8 

47-52 

91.65 

1-5394 

210.20 

44-75 

i-3°43 

74.50 

114  b.  pt. 

1.6269 

311.64 

IOOO  gms.  H2O  dissolve  384.48  gms.  KNO3  at  25°.         (Armstrong  and  Eyre,  1910-11.) 
One  liter  sat.  solution  in  water  contains  2.8  mols.  =  283.11  gms.  KNO3  at  20°. 

(Rosenheim  and  Weinheber,  1910-11.) 

Recent  determinations  of  the  solubility  of  potassium  nitrate  in  water,  agreeing 
satisfactorily  with  the  above  data,  are  given  by  Chugaev  and  Khlopin  (1914). 

SOLUBILITY  OF  MIXTURES  OF  POTASSIUM  NITRATE  AND  BARIUM 
NITRATE  IN  WATER. 

(Euler  —  Z.  physik.  Ch.  49,  313,  '04.) 
t°.          Sp.  Gr.  of  Sat.  Solution.  Grams  per  ioo  Grams  H2O. 

17  1.  120  13.26  KNO3+  6.31  Ba(NO3)2 

21.5  ...  17.00      "     +   7-58 

30  1.191  24.04  +  9-99 

50  ...  49-34  +18.09 

SOLUBILITY  OF  POTASSIUM  NITRATE  IN  AQUEOUS  SOLUTIONS  OF  NITRIC 

ACID  AT  o°. 

(Engel  —  Compt.  rend.  104,  913,  '87.) 


p.  Gr.  of 

olutions. 

Equivalents 

per  10  cc.  Solution. 

Grams  per  ioo  cc.  Solution. 

1.079 

i2.5KN03 

o       HN03 

12.65  KNO3      o.ooHNO8 

9-9      " 

5-87 

H 

IO-O2         " 

3-71 

tt 

•093 

8.28    " 

13-2 

tt 

8.38         " 

8.38 

" 

.117 

7-4      " 

2i-55 

tt 

7-49      " 

13.58 

" 

.144 

7-4      " 

3i-i 

tt 

7-49      " 

19.47 

" 

.202 

7.6      « 

48.0 

tt 

7.68      " 

30.04 

" 

.289 

10.3 

68.0 

tt 

10.42      " 

42.86 

tt 

498 

28.3      " 

120.5 

tt 

28.64      " 

75-95 

" 

Freezing-point  data  for  KNO,  +  HNO3  are  given  by  Dernby  (1918). 


543 


POTASSIUM  NITRATE 


SOLUBILITY  OF  POTASSIUM  NITRATE  AND  OF  ACID  POTASSIUM  NITRATES 

IN  NITRIC  ACID. 

(Groschuff  —  Ber.  37,  1490,  '04.) 

NOTE.  —  Determinations  made  by  the  so-called  thermometric 
method,  i.e.,  by  observing  the  temperature  of  the  disappearance  of 
the  separated,  finely  divided  solid  from  solutions  of  known  concen- 
tration. 


Grams  per  100 
t°.                   Solution. 

Gms. 

Solid 
Phase. 

Gms.  per  100  Gms. 
t  °i              Solution. 

Solid 
Phase. 

KN03. 

HNO3. 

K.N03.      HN03. 

-  6 

24 

•4 

75 

.41 

KNO3.2HNOa  0) 

22.5 

47.2 

52-93 

KN03.HN03 

+  14 

32 

.6 

67 

.42 

"          (stabil) 

23-5 

47.8 

52.11 

"        (stabil) 

17 

34 

.8 

65 

.04 

" 

25-5 

48.6 

51.46 

«' 

19 

•5     37 

.2 

62 

.90 

" 

27.0 

49.4 

50.78 

22 

44 

•5 

55 

.46 

" 

29.0 

50.1 

49.94 

KNO3.HNO3 

21 

•5    47 

.8 

S2 

.11 

KNOs.2HNO3  (0 

30-5 

5o-9 

49-15 

(labil) 

21 

•5    48 

.6 

51 

.46 

(labil) 

21  .0 

49.4 

50.78 

KNO8       (labil) 

20 

So 

•9 

49 

.15 

" 

39-o 

5o-9 

49  -IS 

"       (stabil) 

—   4 

37 

.a 

62 

-8l 

KNO3.HNO3 

5° 

51  .7 

48.32 

-16 

•5    44 

•5 

55 

.46 

(labil) 

c1) 

Solution  in  HNO3. 

0) 

Solution  in 

KNOj. 

CONDUCT 

OF 

ACID  POTASSIUM 

NITRATE  TOWARDS 

WATER. 

Gms.  per  100  Gms. 
t°.            Solution. 

Solid 
Phase. 

t° 

Gms.  per  100  Gms. 
Solution. 

Solid 
Phase. 

KN03. 

HN03. 

KNOg. 

HNO3. 

22 

44 

•5 

55 

•5 

KNO3.2HNOi 

5° 

38. 

7 

48. 

3 

KNO8 

20 

•5     44 

.1 

55 

•  o 

" 

61 

36. 

o 

44- 

8 

" 

18 

43 

.8 

54 

•5 

" 

63 

34- 

5 

43- 

o 

" 

12 

43 

•  0 

53 

.6 

" 

60. 

5    3°- 

39- 

5 

" 

6 

42 

•3 

52 

•7 

" 

56 

27. 

6 

34- 

4 

" 

o 

41 

.6 

51 

.8 

" 

43 

20. 

8 

25- 

9 

" 

12 

41 

•3 

51 

•4 

KNO8 

17 

ii.  7 

14. 

6 

M 

22 

40 

•9 

51 

.0 

it 

-5 

5- 

54      6.91 

40 

39 

•9 

49 

.8 

* 

SOLUBILITY  OF  MIXTURES  OF  POTASSIUM   NITRATE  AND   POTASSIUM 
CHLORIDE  IN  WATER. 

(Etord  —  Ann.  chim.  phys.  [7]  3,  283,  '94;  at  20°,  Riidorff  —  Ber.  6,  482,  '73;  Nicol  —  Phil.  Mag.  [5] 

3  it  385,  '91  •) 


Gms.  per  too  Gms. 
t».             Solution. 

Gms.  per  100  Gms. 
40.             Solution. 

Gms. 
t°. 

per  100  Gms. 
Solution. 

KN03. 

KCI/ 

'KN03. 

KCI: 

KN03. 

KCI. 

0 

5-o 

20.  o 

30 

16 

•  o 

21 

.2 

70 

39 

•5 

17-5 

10 

8.0 

20.8 

40 

21 

.0 

21 

•  O 

80 

45 

^5 

15-8 

20 

12.6 

21  .2 

50 

27 

•  o 

2O 

•  O 

100 

57 

•5 

ii  .6 

25 

14.0 

21.3 

60 

33 

•5 

19 

.0 

120 

69 

•  0 

7-7 

POTASSIUM  NITRATE 


544 


SOLUBILITY  OF  POTASSIUM  NITRATE  IN  AQUEOUS  SOLUTIONS  OP: 

(Touren  —  Compt.  rend.  131,  259,  'oo.) 


Potassium  Carbonate. 

Results  at  14.5°. 


Potassium  Bi  Carbonate. 


Mols.  per  Liter. 

Gms.  per  Liter. 

KzCO*. 

KNOa- 

K2C03. 

KJNU3. 

o.o 

2 

.228 

o.o 

225 

0-48 

I 

•85 

66.4 

188 

1-25 

I 

•39 

172.9 

141 

2.58 

0 

.86 

356-9 

87 

3-94 

o 

.64 

544-9 

65 

Results  at 

*s°. 

o.o 

3 

.217 

o.o 

326 

o-59 

2 

.62 

81.6 

265 

3-35 

I 

•97 

186.7 

199 

2.10 

I 

.46 

290.5 

148 

2.70 

I 

.14 

373-6 

H5 

3-58 

O 

•79 

495  -1 

80 

Results  at 
Mols.  per  Liter. 

14-5°. 
Grams  per  Liter. 

KHC03. 

KN03.          KHC03. 

KN03. 

0-0 

2-33 

o.o 

336 

o-39 

2.17 

39-o 

2  2O 

0.76 

2.03 

76.0 

205 

1.16 

1.92 

116 

194 

i-55 

1.81 

J55 

183 

Results  at 

25°. 

o.o 

3-28 

o.o 

332 

0.89 

2.84 

89 

287 

i-33 

2.65 

133 

268 

1.91 

2-45 

191 

249 

SOLUBILITY  OF  POTASSIUM  NITRATE  IN  AQUEOUS  SOLUTIONS  OF  POTASSIUM 

CARBONATE  AT  24.2°. 

(Kremann  and  Zitek,  1909.) 

Gms.  per  1000  Gms.  H2O. 
KNO3. 


Gms.  per  1000  Gms.  H2O. 


KN03. 
376.8 
285 
161.7 
I4I.8 


K2C03. 
O 

I30-3 
348.4 
371-9 


Solid 
Phase. 


KNO, 


73 
38.8 


K2C03. 

688.1 
878.3 

III2.2 


Solid 
Phase. 


KNO3 


+K2CO, 


looo  gms.  H2O  containing  I  mol.  KC1  (ioi.n  gms.)  dissolve  324.85  gms.  KNO3 

at  25  .  (Armstrong  and  Eyre,  1910-11.) 

Data  for  the  system  potassium  nitrate,  potassium  sulfate,  water  at  35°  are 
given  by  Massink  (1916,  1917). 

SOLUBILITY  OF  MIXTURES  OF  POTASSIUM  NITRATE  AND  POTASSIUM 
SULPHATE  IN  WATER. 

(Euler  — Z.  physik.  Ch.  49,  3i3>  '04-) 
t*.  Sp.  Gr.  of  Sat.  Solution.  Grams  per  100  Grams  Water. 

15  i .  165  24 .12  KNO3  "    5.65  K2SO4 

20  ...  30.10      "  5.58      " 

25  I. 210  36.12         "  5.58         " 


SOLUBILITY  OF  MIXTURES  OF  POTASSIUM  NITRATE  AND  SODIUM 
CHLORIDE  IN  WATER. 


(Etard  —  Ann.  chim.  phys.  [7]  3,  283,  '94 
agree  well  with  those  of  Etard.) 

;  the  older  determinations  of  Riidorff,  Karsten,  Mulder,  ;tc. 

t». 

Gms.  per  100  Gms. 
Solution. 

t°. 

Gms.  per  100  Gms. 

Solution. 

t°. 

Gms.  per  100  Gms. 
Solution. 

KN03.      NaCl.  " 

KNO3.      NaCl." 

KNO3.       NaCl. 

0 

13            24 

40 

3o-5      *9 

120 

73        8.0 

10 

16        23 

So 

36              17 

140 

77        7-o 

20 

2O            22 

60 

42-5         15 

160 

79-5    6-° 

25 

23            21-5 

80 

55          12 

170 

80.5    5-5 

30 

25            20.5 

100 

67       9-5 

545 


POTASSIUM  NITRATE 


100  gmsi  H2O,  simultaneously  sat.  with  potassium  nitrate  and  sodium  chlo- 
ride, contain  41.14  gms.  KNO3  +  38.53  gms.  NaCl  at  25°  and  168.8  gms.  KNO8 
+  39.81  gms.  NaCl  at  80°.  (Soch,  1898.) 

SOLUBILITY  OF  POTASSIUM  NITRATE  IN  AQUEOUS  SOLUTIONS  OF  SODIUM 

CHLORIDE  AND  VICE  VERSA.      (Leather  and  Mukerji,  1913.) 


Sp.  Gr. 

Results  at  20°. 

Gms.  per  100  Gms.  H2O. 

Solid 

Sp.  Gr. 

Results  at  30°. 

Gms.  per  looGms.  H2O. 

Solid 

Sat.  Sol. 

'    KNO3. 

NaCl. 

Phase. 

Sat.  Sol. 

KNO3. 

NaCl. 

Phase. 

1.167 

31 

•49 

0 

KNO, 

I 

.261 

46 

.48 

9.82 

KNO, 

I.22O 

33 

.41 

9- 

94 

« 

I 

•  302 

47 

.08 

20.  l8 

« 

1.267 

34 

•93 

19. 

44 

" 

I 

•343 

47 

.24 

29.86 

« 

I.3II 

36 

.41 

29. 

46 

ii 

I 

•372 

49 

.24 

38.72 

"  +NaCl 

1-344 

37 

•30 

37- 

73 

"   +NaCl 

I 

•342 

38 

•36 

38.55 

NaCl 

1-330 

31 

.41 

37- 

57 

NaCl 

I 

.298 

25 

•32 

38.23 

» 

1.283 

19 

•56 

37- 

" 

I 

.258 

12 

•IS 

37.38 

« 

1-243 

9 

.76 

36. 

73 

" 

I 

.202 

36.30 

" 

Results  at 

40°. 

Results 

at  91°. 

1.288 

64 

•74 

o 

KNO, 

I 

-552 

2O2 

.8 

o 

KNO, 

1.320 

64 

.66 

ii. 

32 

" 

I 

•573 

204 

.2 

12.  8l 

ii 

.  .  . 

64 

•05 

23- 

41 

" 

.601 

208 

.1 

28.45 

« 

1.396 

64 

•13 

35- 

08 

« 

•645 

213 

•3 

37-92 

» 

1.411 

64 

•77 

38. 

79 

"  +NaCl 

.660 

218 

.8 

39-oS 

"  +NaCl 

1.376 

52 

.81 

39- 

51 

NaCl 

.607 

175 

.8 

40.87 

NaCl 

1-323 

34 

•98 

38. 

98 

" 

•517 

126 

•9 

44-33 

.    ii 

1.267 

17 

•33 

37- 

74 

a 

•378 

57 

•53 

42.90 

, 

At  the  higher  temperatures,  results  for  NaNO3  in  certain  solutions  are  reported. 
SOLUBILITY  OF  POTASSIUM  NITRATE  IN  AQUEOUS  SOLUTIONS  OF  SODIUM 

NITRATE  AND  VICE  VERSA.      (Leather  and  Mukerji,  1913.) 


Rei 

Sp.  Gr. 
Sat.  Sol. 

I.3I7 

1.403 
1.472 

1-544 
1.520 
1.481 

I-451 
1.406 

suits  at  30°. 

Gms  per  100  Gms. 
H20. 

Res 

Sp.  Gr. 
Sat.  Sol. 

1.358 
1.428 

I-505 
1-570 
1-573 
1.526 
1.476 
1.421 

mlts  at  40°. 

Gms.  per  100  Gms. 
H20. 

Sp.  Gr. 
Sat.  Sol. 

1.615 
1.674 

I-75I 
1.790 

1-774 
1.695 

1.610 
1.521 

Results  at  91 

Gms.  per  100  Gms. 
H2O. 

o 

Solid  Phase 
in 
Each  Case. 

KNO, 

« 

"  +NaNO, 

NaNO, 

« 

KN03. 

45-73 
47-25 
50.93 
54-34 
47.67 
30.25 
14.30 

0 

NaN03." 
25.90 

52.53 
79.27 

103.3 
103.1 

101.6 
99.10 
95-90 

KN03. 
63.21 
63.86 
66.44 
74.06 
68.72 
43-92 
20.33 
0 

NaN03. 
23.85 

49-79 
79.46 
116.2 
116.7 

112.  2 
109.9 
105.2 

KN03. 
200.8 
207.2 

229-5 
251.8 
2II.7 
128.5 

.55-75 
o 

NaN03." 

43-4   : 
92.90 
156.2 
206.5 

200 

186 

I73.I 
160.8 

Results  at  20°  are  also  given. 

SOLUBILITY  OF  POTASSIUM  NITRATE  IN  AQUEOUS  SOLUTIONS  OF  SODIUM 
NITRATE  AND  VICE  VERSA  AT  20°. 

(Carnelly  and  Thomson  —  J.  Ch.  Soc.  53,  782,  '88;  Nicol  —  Phil.  Mag.  31,  369,  '91.) 

KNO3  in  Aq.  NaNO3  Solutions.        NaNO3  in  Aq.  KNO3  Solutions. 

Grams  per  100  Grams  HaO. 
KNO3. NaNO3. " 
88 
90 
92 

93 


Grams  per  100  Grams  H2O. 
NaNO3.  KN03 

O 
10 
20 

40 

60 
80 


31-6 

30-5 
3I.O 

33-o 
35-5 
41-0 


o 
10 

20 
25 

30 

35 


94 
96 


POTASSIUM  NITEATE 


546 


SOLUBILITY  OF  POTASSIUM  NITRATE  IN  AQUEOUS  SOLUTIONS  OF  SODIUM 
NITRATE  AND  VICE  VERSA  AT  10°  AND  AT  24.2°. 

(Kremann  and  Zitek,  1909.) 


Gms.  per  1000  Gms.  H2O. 


Cms.  per  1000  Gms.  H2O. 


I  . 

KN03. 

NaN03. 

OUUU  JTllitSC. 

* 

KNO3. 

NaN03. 

ouiiu  ruMBi 

10 

208.9 

O 

KNO3 

24.2 

422 

931-3 

KNO, 

IO 

301.9 

848.3 

"  +NaNO, 

24.2 

437 

1019 

"  +NaNO, 

IO 

o 

805 

NaNO, 

24.2 

123.6 

910.6 

NaNO, 

24.2 

377-3 

0 

KNO, 

24.2 

o 

913 

" 

24.2 

390 

346.7 

" 

SOLUBILITY  OF  POTASSIUM  NITRATE  IN  AQUEOUS  SOLUTIONS  OF  SILVER  NITRATE 


Gms.  per  too  Gms.  Sat.  Sol. 


KNO3. 

31-3 

30-45 

29.22 

26.58 

25.02 


AgN03. 
o 

11.51 
23-59 
39-09 
46.38 


AT  30°  AND  VICE  VERSA. 

(Schreinemakers,  1908-09.) 

Solid  Phase. 
KNO, 


"  +AgNOj.KNO3 


KNO3. 

AgN03. 

ounu  rna.sc 

17.38 

57-85 

AgNOj.KNO, 

13-44 

65.08 

« 

11.22 

69.01 

"  -hAgNO, 

5-53 

7I.6S 

AgNO, 

0 

73 

" 

SOLUBILITY  OF  MIXTURES  OF  POTASSIUM  NITRATE  AND  SILVER  NITRATE 


Gms.  per  100  Gms.  Sol. 


o 

10 

20 

25 


KNO3. 

13-5 
19 
23 
25 


AgNO3. 

43 

44-7 
47 
48 


IN  WATER. 

(Etard,  1894.) 
Gms.  per  100  Gms.  Sol. 
'  KNO3.      'AgNO3. 


Gms.  per  100  Gms.  Sol. 


30 
40 


26.8 

29.6 

32 

33-5 


49-4 
Si-5 
54 
54-8 


80 

IOO 
120 
140 


KNO3. 
36-2 

38.3 
40 

41-5 


AgNO,. 

55-1 
55-3 
55-6 
55-8 


SOLUBILITY  OF  MIXED  CRYSTALS  OF  POTASSIUM  NITRATE  AND  SILVER 


Gms.  per  Liter. 


NITRATE  IN  WATER  AT  25°. 

(Herz,  1905;  Fock,  1897.) 
Mg.  Mols.  per  Liter. 


Mol.  Per  cent        Mol.  Per  cent 


AgN03. 

45-9 
110.7 
176.8 
259.6 
365-6 
507-9 
745-9 


KNOj. 

321.8 

322.6 

333-7 

364 

456.4 

387.2 

398.6 


AgNO3. 
270 

65L3 
1040 
1528 
2151 
2988 
4388 


KNO» 
3180 
3184 
3298 
3597 
45" 
3816 
396o 


AgN03  in 

AgNO3  in 

Solution. 

Solid  Phase. 

7.83 

0.2896 

16.96 

0.6006 

23-97 

o  .  9040 

29.81 

1-054 

32.28 

1.604 

43-85 

2-439 

52.70 

8.294 

SOLUBILITY  OF  POTASSIUM  NITRATE  IN  AQUEOUS  SOLUTIONS  OF  STRONTIUM 
NITRATE  AND  VICE  VERSA  AT  20°  AND  AT  40°. 

(Findky,  Morgan  and  Morris,  1914.) 


Gms.  per  100  Gms. 
t°.                 Sat.  Sol.                     Solid  Phase.             t°. 

Gms.  per 
Sat. 

100  Gms. 
Sol. 

Solid  Phase. 

KNOj. 

Sr(NOj)2. 

'    KNOj. 

Sr(NO3)2. 

20 

22 

90 

5.49     KNO, 

20 

12 

-65 

41. 

12 

Sr(N03)2.4H20 

2O 

21 

70 

9.17 

2O 

10 

40. 

70 

" 

2O 

21 

OI 

17.10         ' 

40 

30 

.26 

23- 

70 

KNO3 

20 

19 

60 

31.24 

40 

26 

.90 

38. 

52 

"  +Sr(NOj)2.4H20 

2O 

19 

49 

34-91 

40 

22 

•50 

40. 

22 

Sr(NO,)2.4H20 

2O 

19 

69 

39.56         '    +Sr(N03),.4H20 

40 

II 

.19 

44- 

19 

" 

20 

17 

56 

40.37           Sr(NO3)2.4H2O 

40 

O 

47- 

7 

" 

1000  gms.  H2O,  simultaneously  saturated  with  both  salts,  contain  552  gms. 
KNOi  +  1074  gms,  Sr(NO3)2  at  25°,  (LeBlanc  and  Noyes,  1890.) 


547 


POTASSIUM  NITRATE 


SOLUBILITY  OF  MIXED  CRYSTALS  OF  POTASSIUM  NITRATE  AND  THAL- 


LIUM NITRATE  IN  WATER  AT 

(Fock.) 


*$' 


Grams  per  Liter. 

Mg. 

Mols.  per  Liter. 

Mol.  per  cent      Sp.  Gr. 
T1NO*               of 

Mol.  per  cent 

TINOa 

T1NO3. 

KN03. 

T1N03. 

KNO3 

,             in  Solution.      Solutions,    in  Solid  Phase  . 

O-OO 

351 

.0 

0 

.0 

3468 

.2 

O 

.00 

.2632 

O 

.00 

2-37 

329 

.0 

8 

•9 

3251 

•5 

O 

•43 

.1903 

0 

.08 

6.15 

332 

•4 

23 

.1 

3285 

.1 

0 

.70 

.1956 

0 

.20 

17.64 

333 

•7 

66 

•3 

3298 

.1 

I 

•97 

.2050 

o 

•57 

49-74 

333 

•3 

186 

•9 

3294 

•4 

5 

•37 

.2196 

I 

.78 

63.60 

321 

.0 

239 

.0 

3172 

•4 

7 

.01       1.2436 

2 

.19 

86.18 

330 

•5 

323 

.8 

3265 

.8 

9 

.02       1.2617 

2 

•77 

123.8 

428 

•3 

465 

.2 

4232 

.6 

9 

.90       1.2950 

(27 

.00 

.04 

101.3 

245 

.1 

380.6 

2423 

•3 

13 

.58       1.2050 

93 

•33 

116.1 

o 

.0 

463 

.1 

O 

.0 

100 

.00       i  .0964 

IOO 

.00 

SOLUBILITY  OF  POTASSIUM  NITRATE  IN  AQUEOUS  ALCOHOL  SOLUTIONS, 

(Gerardin  —  Ann.  chim.  phys.  [4]  5,  151,  '65.) 
Grams  KNO3  per  100  Grams  Aqueous  Alcohol  of  Sp.  Gr.: 


t°. 

0.9904 

0.9843 

0.9793 

0.9726 

•09571 

0-939 

0.8967 

0.8429 

=  13-6 

=  19.1 

=  40 

=  60 

=90 

Wt.%. 

Wt.%. 

Wt.%. 

Wt.%. 

Wt.%. 

Wt.%. 

Wt.%. 

Wt.%. 

10 

i7 

13 

10 

7 

4-5 

3 

I 

0-2 

18 

22.5 

18.5 

14-5 

10 

6.2 

4-5 

1.6 

0-3 

20 

24 

20 

16 

ii 

7.0 

5 

2 

o-3 

25 

29 

24-5 

20 

13-5 

9.0 

6-5 

2-5 

0.4 

30 

36 

30 

25 

8 

0.5 

40 

52 

43 

36 

27 

16:5 

ii 

4 

0.6 

5o 

72 

61 

50 

38 

23.0 

16 

6 

0.7 

60 

93 

79 

69 

52 

31.0 

21 

8 

i.i 

SOLUBILITY  OF  POTASSIUM  NITRATE  IN  AQUEOUS  ALCOHOL  AT  18° 

(Bodlander  —  Z.  physik.  Ch.  7.  316,  '91.) 


p.  Gr.  of 

Gms.  per  100  cc.  Solution. 

Sp.  Gr.  of 

Gms.  per  100  cc.  Solution. 

Solution. 

C^OH. 

H2O. 

KN03. 

Solution. 

C2H6OH. 

H20. 

KNOa". 

I  .1480 

. 

89 

.80 

25.0 

I 

.0120 

23-33 

69.81 

8.06 

.1085 

3 

•3o 

87 

•44 

2O-  1  1 

O 

•9935 

28 

.11 

64.74 

6.50 

•  IOIO 

5 

.24 

86 

.26 

18.60 

0 

•9585 

37 

•53 

54-21 

4-II 

.0805 

8 

.69 

83 

.18 

16.18 

o 

•9450 

42 

.98 

48.15 

3-37 

•0755 

9 

.06 

83 

.10 

15  .39 

o 

.9050 

51 

•23 

27.32 

i-95 

•0655 

14 

.08 

77 

•93 

14-54 

o 

.8722 

61 

•65 

24.74 

0.83 

.0490 

16 

.27 

76 

•36 

12.27 

o 

•8375 

69 

.60 

13-95 

O-2O 

•0375 

19 

•97 

72 

•93 

10.8 

SOLUBILITY  OF  POTASSIUM  NITRATE  IN  DILUTE  ETHYL  ALCOHOL  AT  25°. 

(Armstrong  and  Eyre,  1910-11.) 


Wt.%    ' 
QHsOH  in 
Solvent. 

O 


2.25 
4.41 


Gms.  KNOj 
per  100  Gms. 
Sat.  Solution. 

27.77 
26.69 

25-79 
23.81 


POTASSIUM  NITRATE  548 

SOLUBILITY  OF  POTASSIUM  NITRATE  IN  AQUEOUS  ALCOHOL  AND  IN  AQUEOUS 

ACETONE. 

(Batnrick,  1836.) 

In  Aqueous  Alcohol.  In  Aqueous  Acetone  at  40°. 

Wt  Per  cent             Gms.  KN03  per  100  Gms.  Aq.  Alcohol.  Wt.  Per  cent  Gms.  KNO3 

Alcohol.                '      At30o.                             At  40°.      ^  Aceto-  ^XnGtmS- 

o                    45-6                           64.5  o  64.5 

8.25               32.3                           47-i  8.5  51.3 

17                    22.4                           33.3  16.8  38.9 

25.7                 15.1                           24.1  25.2  22.8 

35                    11.4(34-4°)              16.7  34.3  24.7 

44-9                  7                               11.6(44°)  44-1  17 

54-3                  4-5                             7-2(55)  53-9  "-9 

65                      2.7                             4-4  64.8  7.2 

75-6                  1.3                             2      (76.3)  76  3 

88                      0.4                             0.6(88.5°)  87.6  0.7 


100  gms.  H2O  saturated  with  sugar  and  KNO3  dissolve  224.7  E^s.  sugar  -f- 
41.9  gms.  KNO3,  or  100  gms.  of  the  saturated  solution  contain  61.36  gms.  sugar 

+  11.45  gms.  KNO3  at  31.25°.  (Kohler,  1897.) 


SOLUBILITY  OF  POTASSIUM  NITRATE  IN  AQUEOUS  SOLUTIONS  OF  METHYL 
ALCOHOL,  ETHYL  ALCOHOL  AND  MIXTURES  OF  THE  Two  AT  30°. 

(Schreinemakers,  1908-09.) 


In  Aq.  CH3OH.  In  Aq.  C2H5OH.        In  Aq.  v^xi3v^**T^2iX6^ 

Gms.  per  100  Gms.  Sat.  Sol.  Gms.  per  100  Gms.  Sat.  Sol.  Gms.  per  100  Gms.  Sat.  Sol. 

CH3OH.                KNO3.  QHjjOIL                 KNO3.  '(CH3OH +0^011)  KNO3. 

o                    31.3  10. i                20.7  o  31.3 

7.8                    23.3  23.8                    12. 1  12.7  18.9 

17.3                 16.3  32.2                  9  29.2  12.8 

27.8                  ii. 2  43.1                   6.1  41  6.7 

38-4                   7-7  56.9                  3-3  47-8  5-* 

57                      3-8  76-8                  0.88  56.4  3.5 

98.58                0.43  92.3                  0.15  74.8  1.2 

*  The  mixture  contained  51.7%  CH3OH  and  48.3%  C2H5OH. 

loo  gms.  trichlorethylene  dissolve  o.oi  gm.  KNO3  at  15°.    (Wester  and  Bruins,  1914.) 
100  cc.  anhydrous  hydrazine  dissolve  14  gms.  KNO3  at  room  temp. 

(Welsh  and  Brpderson,  1915.) 

100  gms.  aq.  40  weight  %  C2H6OH,  simultaneously  saturated  with  the  two 
salts,  dissolve  13.74  Sms-  KNO3  +  15.78  gms.  NaCl  at  25°.  (Soch,  1898.) 


SIMULTANEOUS  SOLUBILITY  OF  POTASSIUM  NITRATE  AND  SILVER  NITRATE  IN 
AQUEOUS  51.6  PER  CENT  C2H6OH  AT  30°. 

(Schreinemakers,  1908-09.) 

Gms.  per  100  Gms.  Sat.  Solution. 

-KNCV • AiNoT  SoMK— ' 

4-8  o                          KNO3 

4-55  5-15 

4.11  16.47 

4-26  21.28                       "  H-AgNO3.KNO, 

2.62  36.94                   AgN03.KNO3+AgNO, 

o  37                                     AgN02 

Fusion-point  data  (solubilities,  see  footnote,  p.  i),  are  given  for  KNO3  +  KNO2 
by  Meneghini  (1912);  for  KNO3  +  AgNO3  by  Usso  (1904);  for  KNO3  +  NaNO3 
by  Carveth  (1898)  and  by  Hissink  (1900);  for  KNO3  +  Sr(NO3)2  and  KNO3 
+  NaNO3  +  Sr(NO3)2  by  Harkins  and  Clark  (1915);  for  KNO3  +  T1NO3  by 
Van  Eyk  (1899,  1905). 


549 


POTASSIUM  NITRITE 


POTASSIUM  NITRITE  KNO2. 

SOLUBILITY  IN  WATER. 

(Oswald,  1912,  1914.) 
Gms.  KNO2       «,  ,. . 


-  4.1 

-  7-6 
-13.8 
-18.6 

—  24.6 

-30 

—  31.6  Eutec. 


16.1 
24.1 

40.2 
50.1 
61.7 
69.8 
71.8 
73-2 
73-6 


Ice 


"  +KN02 
KN02 

*  dn.i  =  1.6464. 


•    17- 
25 
40 

55 

75 

100 

in 

119 


100  gms.  H2O  dissolve  about  300  gms.  KNO2  at  15.5°. 
The  figure  138.5  gms.  KNO2  per  100  gms.  H2O  at  15°, 
towski  and  von  Roszkowski  (1897),  is  evidently  low. 


Cms.  KNOj 
per  100  Cms. 
Sat.  Sol. 

Solid 
Phase. 

74-5* 

KNOj 

75-75 

" 

77 

« 

77-5 

M 

78.5 

« 

80.5 

« 

80.7 

II 

81.15 

« 

81.8 

« 

(Divers,  1899.) 

given  by  von  Niemen- 


SOLUBILITY   OF   MIXTURES  OF   POTASSIUM   NlTRITE  AND   OF   SILVER   NlTRITE  IN 

WATER. 

(Oswald,  1914.) 


Results  at  13.5°. 

Gms.  per  100  Gms.  H2O. 


Results  at  25°. 

Gms.  per  100  Gms.  H2O. 


kN02. 

18 

276 


AgN02. 
2.36 
26.3 


KN02. 
23.1 
279 


AgN02. 

5-3 
39-3 


Solid  Phase  in  Each  Case. 

AgN02+K2Ag2(N02)4.H20 
KN02+K2Ag2(N02)4.H20 


Of  the  two  layers  obtained  by  mixing  an  equal  volume  or  more  of  96%  ethyl 
alcohol  with  a  nearly  saturated  aqueous  solution  of  KNO2,  the  lower  contains 
71.9%  KNO2  and  the  upper,  alcoholic,  6.9%.  With  methyl  alcohol  there  is  no 
separation  into  two  layers.  (Donath,  1911.) 


POTASSIUM  OXALATE  K2C2O4.4H2O. 

SOLUBILITY  OF  MIXTURES  OF  POTASSIUM  OXALATE  AND  OXALIC  ACID  IN 

WATER  AT  25°. 

(Foote  and  Andrew,  1905.) 


Gms.  per  100  Gms.  Solution. 


H2C204. 

K,Q04. 

IO.2 

10.31 

0.04 

9.26 

0.13 

3-39 

0.63 

2.06 

4.26 

1.16 

11.50 

0.99 

16.93 

0.85 

21.  08 

0.82 

21.49 

0.64 

23-52 

0-57 

24.88 

0-43 

27.52 

27.40 

Mols.  per  100 

Mols.  H2O. 

2.274 

K2C204. 

2.302 
2.046 

0.005 

0.016 

0.707 

0.071 

0.440 
0.266 

0-495 
1.427 

0.240 
0.221 
0.2II 
0.169 
0-153 

2.235 
2.928 
2.998 

3-301 
3.617 

0.122 

4.14 

4.09 

Solid  Phase. 


H2C2O4.2H2O+H3K(C2O4)2.2H2O 
Double  salt  H3K(C2O4)2.2H2O 
H3K(CA)  .2HJO+HKCA 
Double  salt  HKC-A 
HK  CA  +H2K4(C204)3.2H20 

Double  salt  H2K4(C204)8.2H2O 
HSK4(CS04)3  2H2O4-K,C5O4.H2O 


POTASSIUM   OXALATES 


550 


EQUILIBRIUM  IN  THE  SYSTEM  POTASSIUM  OXALATE,  OXALIC  ACID,  WATER  AT 

o°,  30°  AND  60°. 

(Koppel  and  Cahn,  1908.) 


Results  at  o°. 

Gms.  per  100  Gms. 
Sat.  Sol. 

Results  at  30°. 

Gms.  per  100  Gms. 
Sat.  Sol. 

Results  at  60°. 

Gms.  per  100  Gms. 
Sat.  Sol.              Solid  Phase  in  Each  Case 

CA. 
2.72 
2.91 

K20. 
O.226* 

Q03. 

9-97 
10.15 

K20. 
O.IO 

C203. 
24-75 

K20. 

2. 

985 

0 

•342* 

.  . 

2. 

827 

o 

.125 

IO. 

23 

0. 

34 

25 

.70 

O. 

46          "  +KH3(C2O4)2.2H2O 

2. 

345 

o 

•145 

.  . 

. 

.  . 

. 

. 

"                 " 

I. 

47i 

o 

195 

7- 

28 

o. 

33 

25 

.So 

O. 

54      KH3(QO4)2.2H2O 

0.823 

o 

.240 

4 

0. 

4i 

22 

.06 

o. 

58          " 

O. 

799 

o 

454 

3- 

08 

0. 

50 

20 

•  17 

0. 

67          " 

I. 

173 

o, 

.785 

2. 

38 

I. 

002 

14 

•  25 

o. 

90 

I. 

38i 

0 

962 

2. 

98 

I. 

79 

9 

.82 

I. 

48          " 

I. 

545 

I, 

155 

.  . 

6 

•95 

2. 

244       " 

I. 

666 

I, 

273 

4- 

24 

2. 

76 

9 

•17 

5- 

60          "  +KHCA 

I. 

754 

I. 

479 

4- 

26 

3- 

38 

8 

.81 

6. 

37       KHCA 

2. 

627 

2, 

858 

5- 

44 

5- 

43 

10 

•17 

10 

" 

3- 

772 

4. 

422 

6. 

66 

7- 

27 

12 

•36 

13. 

40 

4- 

292 

5 

161 

8. 

64 

IO. 

05 

14 

.10 

16 

" 

4- 

975 

6, 

088 

IO. 

03 

12. 

01 

15 

•35 

17- 

80 

5- 

652 

7 

IO. 

80 

12. 

94 

16 

.07 

18. 

89          "  +(K2C204)2H2C204.2H20 

6. 

27 

7. 

87 

ii. 

47 

14. 

13 

16 

•Si 

19. 

59      (K2C204)2.H2C204.2H20 

7- 

63 

9 

,72 

12. 

16 

15- 

ii 

16 

.80 

20. 

IO 

8. 

66 

ii 

14 

12. 

32 

15-37 

16 

•95 

2O. 

34 

9- 

055 

ii 

58 

12. 

90 

16. 

23 

17 

.14 

20. 

70          "  +K2Q04.H20 

8. 

826 

ii 

52 

12.36 

16. 

14 

16 

2O. 

41                    KzC-A-HijO 

5- 

215 

12, 

33 

8.52 

15. 

03 

15 

•94 

2O. 

II                             " 

2. 

23 

14 

,80 

4- 

53 

«$• 

55 

15 

.06 

19. 

66 

I. 

245 

16 

,82 

I. 

87 

18. 

17 

8 

.82 

19. 

2S 

0. 

871 

18 

4 

0. 

74 

22. 

32 

2 

.04 

23- 

09 

0. 

511 

20 

91 

. 

0 

•434 

29 

" 

0. 

325 

23 

30 

0 

.365 

31- 

40 

0 

4i 

3t 

O 

4o! 

79 

O 

51- 

34                     KOH.H2O 

*  Supersaturated. 

t 

About. 

EQUILIBRIUM  IN  THE  SYSTEM  POTASSIUM  OXALATE,  OXALIC  ACID,  WATER 

AT  25°. 


Gms. 


er  100  Gms. 
it.  Sol. 


(Hartley,  Drugman,  Vlieland  and  Bourdillon,  1913.) 


Solid  Phase. 


Gms.  per  100  Gms. 

Sat.  Sol. 

Solid  Phase. 

Q03. 

K20.  ' 

3-079 

2.052 

KH3(Q04)2.2H20 

3-450 

2.360 

"  +KHCA 

3-793 

3-199 

KHCA 

5-457 

5-9I9 

" 

9.816 

11.96 

"  +2K2C2O4.H2C2O4.2H2O 

12.365 

15.71 

2K2QO4.H2CzO4.2H2O  +K2C2O4.H2O 

11-85 

I5-5I 

K2C2O4.H2O 

QO,.  K,0. 

8.29  o 

8.278  0.045 

7.412  0.064 

2.827  0.238 

2.007  0.346 

1-734  0.567 

2.675  I.7H 

Similar  data  at  15°  for  the  above  system  are  given  by  .Jungfleisch  and  Landrieu 


55i 


POTASSIUM   OXALATES 


SOLUBILITIES  IN  THE  SYSTEM  POTASSIUM  OXALATE,  OXALIC  ACID,  WATER  AT 
THE  CRYOHYDRIC  POINTS. 

(Koppel  and  Cahn,  1908.) 

(Temp,  of  Equilibrium  of  Solution  with  Ice.) 


teoflce 
Separa- 
tion. 

—  0.9S 
—  0.90 
-0.52 
-0.25 
—  0.58 
—  0.78 
-1.50 
—  2.10 
-2.78 

-345 

Gms.  per  100 
Cms.  Sat.  Sol. 

Solid  Phase, 
Ice+: 

H2C204.2H20 
"  +KH3(CA),.2H2O 

KH3(CA)2.2H20 
<< 

"  +KHCA 
KHCA 

"  +(K2CA;2. 
H2CA.2H20 

t°  of  Ice 

Separa- 
tion. 

-   4-45 

-  5-20 

-  5.32 
-  5.97 

-  6.55 

—  8.10 
—  10.30 
—  13.60 
—  17.40 
-23.80 

Gms.  per  100 
Gms.  Sat.  Sol. 

Solid  Phstee, 
Ice+: 

;K2CA)2.H2CA.2H20 

"  -f-K2C204.H20 

K2CA.H,0 
«i 

« 
« 

u 

CA 
2.641 
2.720 
1.672 
0.643 
1.229 
1.648 
2.707 
3.687 
4.576 
5-681 

K20. 

0.0466 
0.0602 

O.2IO 
0.823 
1.234 
2.950 
4.363 
5-50 
7-05 

CA 
6.902 
7.616 
7.696 
8.51 
6.742 
4-999 
3.358 
1.854 
i.  200 
0.606 

K20.  ' 
8.820  ( 
9-74 
9.84 

II.OI 

10.45 
10.86 
11.76 
13.08 

14.55 
16.89 

SOLUBILITIES  IN  THE  SYSTEM  POTASSIUM  OXALATE,  OXALIC  ACID,  WATER  AT 

THE  BOILING  POINTS. 
(Koppel  and  Cahn,  1908.) 


Gms.  per  100  Gms. 
Sat.  Sol. 

Solid  Phase. 
KH3(CA)2.2H20 

"+KHCA 
KHCA 

CA.        K20. 
39.84        5-25 
36.95         5.83 

32.75        5-97 
27.64        9.12 
27.46      11.43 
23.36      10.50 
18.81      12.29 

t°of 
B.pt. 

Gms.  per  100  Gms. 
Sat.  Sol. 

'CA.        K2o.  ' 

102.8 

19.10        18.25 

103.25 

21.  II          21.71 

107.7 

25.19     27.91 

106.35 

22.04      26.45 

106.25 

19.17        25.02 

108.25 

12.73      27.69 

iii.S 

5-35       30.40 

Solid  Phase. 
KHCA 

"  +K2C204.H20 
K2CA.H20 


t°of 
B.pt. 

105.5 
104.9 
104.3 
103.4 
102.9 
102.5 
102.4 

From  the  preceding  tables  the  following  results  for  the  solubilities  of  the 
pure  oxalates  in  water  are  obtained. 

SOLUBILITY  OF  POTASSIUM  OXALATE,  K2C2O<.H2O  IN  WATER. 


t° 

Gms.  per  100  Gms 

Sat.  Sol.            Solid 

A0      Gms.  per 

roo  Gms.  Sat.  Sol.    Solid 

If 

CA  +  K2O  = 

K2CA.            Phase- 

C  A  +  K20  = 

=K2CA-     phase- 

—  0.78    1.31 

1.71 

3.02      Ice 

30 

12.36 

16.14 

28.50     K2C204.H20 

—   I 

49 

2.48 

3-20 

5-68      " 

40 

13.20 

17.22 

30.44 

—    2 

•50 

3-99 

5.20 

9-195    " 

50 

14.14 

18.46 

32.60 

-  3 

.22 

5-iS 

6.705 

11.855    " 

60 

15.06 

19.66 

34.72 

-  5 

.88 

8.429 

II.OI 

19.43       "  +K2CA-H2O 

70 

15-94 

20.81 

36.75 

o 

8.83 

11.52 

20.35          K2CA.H2O 

80 

16.86 

22.02 

38.875 

+  10 

10.48 

13.69 

24.17 

90.2 

17.73 

23.14 

40.90 

20 

11-57 

15.11 

26.675 

106.2* 

19.17 

25.02 

44.19 

*  b.  pt. 

100  gms.  sat.  aq.  sol.  contain  20.62  gms.  K2C2O4  at  o°,  d  =  1.161.    (Engel,  1888.) 
The  results  oL  Hartley,   Drugman,  Vlieland  and   Bourdillon   (1913)  and  of 

Colani  (1916),  for  the  solubility  of  neutral  potassium  oxalate  in  water,  agree 

satisfactorily  with  the  above. 


SOLUBILITY  OF  POTASSIUM  BIOXALATE,  KHC2O4,  IN  WATER. 

(Koppel  and  Cahn,  1908.) 
t°.  Gms.  per  zoo  Gms.  Sal  Sol,  j^  phase. 

C2Oj.  K2O. 

60  8.75  6.50  KHCA 

I02.4b.pt.  18.81  12.29  " 

The  KHC2O4  is  decomposed  to  the  less  soluble  tetroxalate  at  temperatures 
below  50°. 


POTASSIUM   OXALATES 


552 


SOLUBILITY  OF  POTASSIUM  TETROXALATE,  KH3(C2O4)2.2H2O,  IN  WATER. 

(Koppel  and  Cahn,  1908.) 


—  o.  25  cryohydrate 
o 

30 

60 
103.5  b.  pt. 


Gms.  KH3(C2O4)2  per 

100  Gms.  H2O. 

0..99 

1.27 

4-30 

n-95 
72.17 


Solid  Phase. 


SOLUBILITY  OF  MIXTURES  OF  POTASSIUM  OXALATE  AND  OTHER  SALTS  IN 
WATER.    (Coiani,  1916.) 


Results  at  15°. 

Gms.  per  100  Gms.  Sat.  Sol. 


Results  at  50°. 

Gms.  per  too  Gms.  Sat.  Sol. 


Solid  Phase  in 

Each  Case. 
K2C2O4.H2O+KC1 


10.03  K2C2O4+i9.i9  KC1  15.18  K2C2O4+2o.26  KC1 

23.55       "      +  i.82K2SO4  31.06       "      +  i.99K2SO4 

20.39  +11.60  KNO3(i9°)       19.63  +28.29  KNO3  "   +KNO, 

ipo  gms.  aqueous  solution,   simultaneously  saturated  with   potassium  and 
sodium  oxalates,  contain  26.15  gms-  K2C2O4  +  2.44  gms.  Na2C2O4  at  25°. 

(Foote  and  Andrew,  1905). 

POTASSIUM  Telluric  Acid  OXALATE  K2[HdTe06.C2O4]. 


(Rosenheim  and  Weinheber,  1910-11.) 


SOLUBILITY  IN  WATER. 

t° 
Gms.  K2[H6TeO6.C2O4]  per  100  gms.  H2O 

POTASSIUM  PERMANGANATE  KMnO4. 

SOLUBILITY  IN  WATER.     (Baxter,  Boylston,  and  Hubbard,  1906;  Patterson,  1906.) 


O 
2.67 


2O 
5.36 


6.82 


4o~ 
9.07 


5o° 
12.35 


Gms.  KMnO4  per  100: 


Gms.  KMnO4  per  100 : 


I  . 

Gms.  Solution. 

Gms.  H2O. 

cc.  Solution  (P). 

o 

2-75 

2.83 

2.84 

9.8 

4-31 

15 

.  .  . 

5-22 

19.8 

5-96 

6-34 

24.8 

7.06 

7-59 

.  .  . 

29.8 

8.28 

9-03 

8.69 

Gms.  Solution. 

Gms.  H2O. 

34-8 

i             9.64 

10.67 

40 

ii.  16 

12.56 

45 

12.73 

14.58 

50 

14-45 

16.89 

55 

16.20 

19.33 

65 

20.02 

25.03 

Sp.  Gr.  of  saturated  solution  at  15°  =  1.035. 

Determination  by  Worden  (1907),  made  with  extreme  care,  gave  results  in 
very  close  agreement  with  the  above. 


SOLUBILITY  OF  POTASSIUM  PERMANGANATE  IN: 
Water. 

(Voerman,  1906.) 


Aqueous  Acetone  Solutions  at  13°. 

(Herz  and  Knoch,  1904.) 


Gms.  KMn04  per  100  Gms. 

cc.  Acetone 

KMn04  per  100  cc.  Solutit 

A 

' 

Solution. 

Water. 

per  100  cc. 
Solvent. 

Millimols.          Grams. 

—  0.18 

0.58 

0.58                 Ice 

0 

148.5 

4.70 

-  0.27 

0.99 

I.OI                  " 

10 

162.5 

5.13 

-  0.48 

1.98 

2.  02 

20 

177-3 

5-61 

-  0.58 

2.91 

3               Ice+KMnO 

30 

208.2 

6.59 

+10 

4.01 

4.22            KMnO4 

40 

257-4 

8.14 

15 

4-95 

5-20 

50 

289.7 

9.16 

25 

7 

7-53 

60 

316.8 

10.  02 

40 

10.40 

ix.  di 

70 

328 

10.38 

So 

14-35 

16.75         " 

80 

312.5 

9.89 

90 

227 

7.18 

100 

67 

2.14 

553  POTASSIUM   PERMAN- 

GANATE 

SOLUBILITY  OF  POTASSIUM  PERMANGANATE  IN  AQUEOUS  SOLUTIONS  OF 
POTASSIUM  CARBONATE. 

(Sackur  and  Taegener,  1912.) 

Mols.  KMnO4  per  Liter  in: 


t°. 

O.I  ft  ^ivjCAJg. 

i  n  |K2CO3. 

2  n  £K2CO3. 

4  n  iK2C03. 

6  n  iK2C03. 

0 

o.  1462 

0.0629 

o  .  0446 

0.027 

0.0156 

25 

0-4375 

0.2589 

.  .  . 

0.093 

40 

0.7380 

0.5007 

0.3519 

...      v 

SOLUBILITY  OF  POTASSIUM  PERMANGANATE  IN  AQUEOUS  SOLUTIONS  OF 
POTASSIUM  CHLORIDE. 

(Sackur  and  Taegener,  1912.) 
Mols.  KMnO4  per  Liter  in: 


t°. 

o.i  «  KC1. 

0.5  n  KC1. 

i  n  KC1. 

2  n  KC1. 

o 

0.1395 

0.076 

0.0532 

0.0379 

25 

0.4315 

0.306 

0.220 

0.1432 

40 

0.738 

0.584 

0.444 

0.288 

SOLUBILITY  OF  POTASSIUM  PERMANGANATE  IN  AQUEOUS  SOLUTIONS  OF 
POTASSIUM  HYDROXIDE. 

(Sackur  and  Taegener,  1912.) 
Mols.  KMnO4  per  Liter  in: 


t°.     H2O. 

i  »  KOH. 

2  «  KOH. 

4  » 

KOH. 

6« 

KOH. 

8  n  KOH.    10  n  KOH. 

0 

0 

.  176 

0.050 

0 

.031 

0. 

027 

O 

023 

O.OI7 

O.OI2 

10 

o 

,278 

O.  112 

0 

.068 

0. 

048 

0 

.042 

0.028 

0.016 

20 

0 

,411 

0.179 

o 

.119 

0. 

079 

o 

.074(19°) 

0.032 

0.029 

30 

0, 

573 

0.316(32°) 

o 

.213(32°) 

0. 

149(32°) 

0. 

114 

0.062(32°) 

0.040 

40 

o, 

792 

0-439 

0 

.306 

0. 

211 

0 

,161 

0.084 

0.052 

50 

I  , 

154(53°) 

0.638 

0 

.462 

0. 

304 

0 

.219 

O.III 

.  .  . 

70 

I. 

812 

I.I72 

0, 

869 

0. 

572 

o 

390 

0.188 

0.082 

80 

I-5I3 

I. 

190 

0, 

500 

0.231 

.  .  . 

90 

.  .  . 

.  .  . 

0, 

649 

0.297 

SOLUBILITY  OF  POTASSIUM  MANGANATE  IN  AQUEOUS  SOLUTIONS  OF 
POTASSIUM  HYDROXIDE. 

(Sackur  and  Taegener,  1912.) 

(The  KzMnO*  was  prepared  by  boiling  KMnO4  with  very  cone.  KOH,  draining 
by  suction  and  washing  with  ice  cold  K2CO3  solution.  The  impurities  were  of 
no  consequence  since  the  determinations  were  made  in  alkaline  solutions.) 


Mols.  K2MnO4  per  Liter  in: 


O 
10 

15 

20 
30 
40 

45 
50 
60 
70 
80 


2  n  KOH. 

4  n  KOH. 

6  »  KOH. 

8  n  KOH. 

10  n  KOH. 

0.907 

0-554 

0.155 

0.063        • 

0.0145 

I.OI3 

.  .  . 

0.07O 

0.0152 

.  .  . 

0.681  (17°) 

0.224 

.  .  . 

I.I4O 

0-733  (2S°) 

0.26l  (23°) 

0.078 

0.0160 

1.252 

0.772 

0.303 

0.096 

0.0215 

.  .  . 

0.852 

0.362 

o.  119 

0.0305 

1.424 

0.889 

0.388 

0.938  (51°) 

o.  142 

0.0462 

1.003 

0.469 

0.167 

0.062   (63°) 

1.074 

0.528 

0.196 

0.070 

1.143 

0.587 

O.222 

0.083 

TOO  cc.  anhy.  hydrazine  dissolve  2  gms.  KMnC>4,  with  evolution  of  gas  and  for- 
mation of  a  brown  precipitate,  at  room  temp.  (Welsh  and  Broderson,  1915.) 


POTASSIUM  PERMAN- 
GANATE 


554 


SOLUBILITY  OF 

MIXED  CRYSTALS  OF  POTASSIUM  PERMANGANATE  AND 

POTASSIUM 

PERCHLORATE  AT  7°. 

(Muthmann  and  Kuntze 

,  1894;  recalculated  by  Fock, 

1897.) 

MUligram  Mols. 

per  Liter. 
KC103." 

Cms.  per  Liter. 

Mol.  per  cent 
KMnO4  in 
*          Crystals  of  Solid 
Phase. 

KMnO4. 

KMnO4.              KC1O4. 

O 

63.91 

o                 8.86 

0 

29-37 

54.48 

4-65            7-55 

2.84 

67-73 

42.75 

10.71            5-93 

9.78 

79.04 

39-59 

12.50            5.49 

10.  8  1 

99.81 

38.63 

15-79            5-36 

15.96 

122.24 

34-39 

19-34            4-77 

23-56 

119.21 

38.91 

18.84            5.39 

24.28 

128.08 

33-77 

20.26            4.68 

26.40 

144.46 

33-14 

22.86            4.59 

34-32 

167.81 

29-53 

26.55         4.09 

44.42 

183.09 

25-I9 

28.97         3.49 

67-33 

197.82 

20.  16 

.  31.30         2.80 

77-95 

233-75 

28.26 

36.98         3.92 

94-37 

264.27 

o 

41.81            o 

IOO 

SOLUBILITY  OF  MIXED  CRYSTALS  OF  POTASSIUM  PERMANGANATE  AND 
RUBIDIUM  PERMANGANATE  AT  7°. 

(Muthmann  and  Kuntze,  calc.  by  Fock.) 


Milligram  Mols.  per  Liter. 


Cms,  per  Liter. 


KMn04. 

27.04 

75 

120.26 
188.30 
198.36 
205.76 
225.12 

264.27 


22.69 

22.22 

3L29 
38-98 
41.29 
42.50 
26 

o 


KMnO4. 
4-28 

11.84 

I9.03 
29.80 
31.39 
32.56 
35.6l 

41.81 


4.64 

4-54 

6.40 
7.97 
8.44 
8.69 
5.32 

o 


3.50 

13-75 

34.29 

71.45 
92.50 
99.47 
99.32 

ioo 


POTASSIUM  PICEATE  C6H2(NO2)3OK. 

Data  for  the  solubility  of  potassium  picrate  in  aqueous  solutions  of  ethyl 
alcohol,  methyl  alcohol  and  of  acetone  at  25°  are  given  by  Fisher  (1914). 

POTASSIUM  PHOSPHATES 

SOLUBILITY  OF  POTASSIUM  ACID  PHOSPHATE,  KH2PO4.H3PO4,  IN  WATER. 

(Parravano  and  Mieli,  1908.) 

Determinations  by  Synthetic  (sealed  tube)  Method. 

Gms.  Gms. 


Solid  Phase. 


t'. 


Sat.  Sol. 

-o.6 

3-337 

-2.5 

12.13 

-6.7 

29-43 

-  9-2 

36.98 

—  i3  Eutec. 

44 

o(?) 

45-8 

+  10.9 

50-3 

Solid  Phase. 


Ice 


Sat.  Sol. 

65.2 

68.44 

78 

72.43 

87-5 

77-6 

105.5 

85-9 

+KH2PO4 

120  tr.  pt. 

92.1 

KH2PO4 

135 

96.  i 

« 

139 

IOO 

KH2PO4 


+KH2PO4.H3PO< 


One  liter  of  sat.  aq.  solution  contains  249.9  gms.  KH2PO4  at  7°. 

(Muthmann  and  Kuntze,  1894.) 


555 


POTASSIUM  PHOSPHATES 


SOLUBILITY  OF  POTASSIUM  ACID  PHOSPHATE,   KH2PO4.H3PO4,  IN  ANHYDROUS 

PHOSPHORIC  ACID. 

(Parravano  and  Mieli,  1908.) 

Determinations  by  Synthetic  (sealed  tube)  Method. 

•  Gms.  per  100  Cms.  Sat.  Solution. 

KH2P04.H3P04   ^       KH2P04. 
38.5  18.17  10.56 

84  58-42  33-97 

no  77.53  45.08 

126.5  92.26  S1^0 

EQUILIBRIUM  IN 'THE  SYSTEM  POTASSIUM  HYDROXIDE,  PHOSPHORIC  ACID, 

WATER  AT  25°. 

(D'Ans  and  Schreiner,  igioa;  Parker,  1914.) 

The  results  of  these  investigators  agree  satisfactorily  when  plotted  on  cross- 
section  paper.  The  following  figures  were  read  from  the  curves.  Some  uncer- 
tainty exists  in  regard  to  the  solid  phase  in  contact  with  some  of  the  solutions. 


K. 

P04. 

-»                 OU11U  -T1JCI.SC. 

9.62 

0 

KOH.2H2O 

9.76 

0.24 

"  +K3PO4.3H2O 

9-15 

o-5 

K3P04.3H20 

8.2 

i 

" 

7-5 

i-5 

" 

8.2 

2 

« 

7-5 

2-5 

« 

8.8 

2.9 

« 

9-7 

2.9 

"  +K3P04 

9-5 

3 

K3P04 

8-5 

3-4 

" 

8 

3-6 

H 

7-5 

3-75 

" 

Fusion-point  data  for  KPOs  + 
(1908,  1910). 


POTASSIUM    HYPOPHOSPHATE,  etc. 

SOLUBILITY  IN  WATER. 

(Salzer  —  Liebig's  Ann.  211,  i,  82.) 


K. 

P04. 

-»         aoua  rnase. 

7 

4 

K3P04+K2HP04 

6 

3-6 

K2HP04 

5 

3.15 

" 

4 

2.65 

"      or  KH2P04(?) 

3 

2.2 

(?) 

2 

1-7 

"             "        (?) 

I  .5 

1-5 

"             "        (?) 

1.6 

2 

KH2PO4 

2.1 

4 

" 

2-5 

6 

" 

3 

8 

" 

1.65 

6 

KH2P04.H3P04  (Parker) 

*-35 

8 

«                 « 

are  given 

by  Parravano  and  Calcagni 

Salt. 


Formula. 


Gms.  Salt  per  100 
Gms.  H2O. 


Cold. 
400 
20O 

33 

66.6 


Hot. 


Potassium  Hypophosphate  K4P2O6.8H2O 

"          Hydrogen  Hypophosphate  K3HP2O6.3H2O 

Di  Hydrogen  Hypophosphate  K2H2P2O6.3H2O 

"         Tri  Hydrogen  Hypophosphate  KH3P2O6 
"          Penta  Hydrogen  Hypophosphate  K3H5(P2O6)2. 2H2O  40 

"          Hydrogen  Phosphite  KH2PO3  172  (20°)       . . . 

"         Hypophosphite  KH2PO2  200(25°)      333 

«         Hypophosphite  KH2PO2*  14.3  (2S°)    28 

*  Solvent  alcohol. 


IOO 
200 
125 


POTASSIUM  PHOSPHOMOLYBDATE  K3PO4.iiMoO3.i|H20. 


100  gms.  H2O  dissolve  0.0007  gip.  at  30°. 

100  gms.  aqueous  10%  HNO3  dissolve  0.204  Sm-  at  3°°' 


(Donk,  M.  G.,  1905.) 


POTASSIUM   SELENATE  556 

POTASSIUM   SELENATE  K2SeO4 

SOLUBILITY  IN  WATER. 

t°.  -20°.  -S°.          +5°.          18".  97°. 

Cms. K2Se04 per  100 gms. solution    51.5      51.7      52      52.6      54.9 

(Etard,  1894.) 

100  gms.  H20  dissolve  115  gms.  K2SeO4  at  12°.  (Tutton,  1907.) 

POTASSIUM   SILICATE   K2SiO3. 

Data  for  equilibrium  in  the  systems  K2SiO3  +  H2O,  K2Si2O5  +  H2O,  K2SiO3  + 
SiO2,  SiO2  +  H2O  and  K2SiO3  +  SiO2  +  H2O,  at  temperatures  between  200°  and 
1000°  +,  determined  by  the  "  hydrothermal  quenching  method,"  are  given  by 
Morey  (1917). 

POTASSIUM   STANNATE  K2SnO3.3H2O. 

100  gms.  H2O  dissolve  106.6  gms.  at  10°,  and  110.5  Sms.  at  20°.     Sp.  Gr.  at 

10°  =  I.6l8  at  20°  =  1.627.  (Ordway,  1865.) 

POTASSIUM  SULFATE  K2SO4. 

SOLUBILITY  IN  WATER. 

(Mulder;  Andrae,  1884;  Trevor,  1891;  Tilden  and  Shenstone,  1884;  Berkeley,  1904;  see  also  Etard,  1894.) 


Gms.  K,SO4  per  100  Gms.         ^0 

Gms.  K2SO4  per  100  Gms. 

Gms.  K2SO4 

per  loo  Gms. 

' 

Water. 

Solution. 

Water. 

Solution. 

* 

Water. 

Solution. 

0 

7-35 

6.85 

40 

14.76 

12.86 

90 

22.8 

18-57 

10 

9.22 

8.44 

50 

16.50 

14.16 

IOO 

24.1 

19.42 

20 

II  .11 

IO 

60 

18.17 

I5-38 

I2O 

26.  $ 

20.94 

25 

I2.O4 

10-75 

70 

19-75 

16.49 

143 

28.8 

22.36 

30 

12.97 

11.48 

80 

21.4 

17-63 

170 

32.9 

24.76 

Sp.  Gr.  of  solution  saturated  at  18°  =  1.083. 

The  determinations  of  Berkeley  (1904),  which  were  made  with  exceptional  care, 
are  as  follows: 

^.0  Sp.  Gr.  of  Sat.    Gms.  K2SO4  per  f  „  Sp.  Gr.  of  Sat.     Gms.  K2SO4  per 

Solution.          loo  Gms.  H2O.  Solution.  100  Gms.  H2O. 

0.40    '      1.0589  7.47  58.95  1.1089  iS.OI 

15.70          1.0770  IO-37  74-85  I.II57  20.64 

31.45  I.092I  13.34  89.70  I.II94  22.80 

42.75       i.ioio          15.51  ioi.ib.pt.      1.1207          24.21 

Individual  determination  in  good  agreement  with  the  above,  are  given  by  Le- 
Blanc  and  Schmandt  (1911);  Greenish  and  Smith  (1901);  Osaka  (1903-8);  Nacken 
(1910);  Smith  and  Ball  (1917). 

SOLUBILITY  OF  MIXED  CRYSTALS  OF  POTASSIUM  SULFATE  AND  AMMONIUM 

SULFATE  AT  25°. 

(Fock,  1897.) 


Grams 

per  Liter. 

Milligram  Mols.  per  Liter. 

Mol.  per  cent     Sp.  Gr. 
K2SO4  in            of 
Solution.        Solution. 

Mol.  per  cent 
K2SO4  in 
Solid  Phase. 

'  KaSCV 

(NH4)2S04. 

K2S04. 

(NH4)2S04.  ' 

127-9 

o.o 

734 

O-O 

IOO 

1.  086 

IOO 

135-7 

"5-7 

778.5 

874.6 

47-1 

1.149 

91.28 

84.20 

28l.I 

483 

2126 

I8.5 

1  .200 

80-05 

59.28 

355-o 

340 

2685 

11.13 

1  .226 

68.63 

40.27 

482.7 

231 

3650 

5-98 

1  .246 

27-53 

o.oo 

542-3 

o.o 

4100 

0-00 

1.245 

0-00 

Results  are  also  given  for  14°,  15°,  16°,  30°,  46°,  and  47°. 


557 


POTASSIUM   SULFATE 


SOLUBILITY  OF  POTASSIUM  SULFATE  IN  AQUEOUS  AMMONIA  SOLUTIONS  AT  20°. 

(Girard,  1885.) 

Cms.  NH3  per  ioo  cc.  solution       o          6.086     15.37     24.69    31.02 
Gms.  K2SO4  per  loo  cc.  solution  10.80    4.10        0.83      0.14      0.04 

One  liter  sat.  solution  in  water  contains  105.7  Sms.  K2SO4  at  20°. 
One  liter  sat.  solution  in  5.2%  NH3  contains  45.2  gms.  K2SO4  at  20°. 

(Konowalow, 

SOLUBILITY  DATA  FOR  THE  RECIPROCAL  SALT  PAIR 
K2SO4  +  BaCO3  <=*  K2CO3  +  BaSO4. 

(Meyerhoffer,  1905.) 


25 
25 
80 

80 
80 

IOO 

IOO 


Gms.  per  ioo  Gms. 

t8. 

Sat.  Sol. 

Solid  Phase. 

K2S04. 

K2C03. 

25 

10.76 

O 

K2SO4+BaS04 

25 

6.76 

5-85 

"           " 

25 

3-92 

12.6 

<<           «« 

25 

2.485 

17.81 

"+BaC03 

25 

1.72 

22.1 

K2SO4+BaCO3 

25 

0.0886 

28.5 

«            « 

25 

0.023 

53-i 

"  +K2C03.2H20 

25 

O 

53-2 

K2CO3.2H2O+BaCO3 

Gms.  per  ioo  Gms. 
Sat.  Sol. 

Solid  Phase. 

K2S04. 

K2C03. 

O.6O2 

7-35 

BaC03+BaS04 

0.173 

2.85 

" 

0.613 

2.49 

" 

i-39 

4.88 

" 

7-i 

15-33 

"+K2SO< 

0-797 

2-36 

BaC03+BaS04 

1.83 

4-5i 

" 

9.42 

13-6 

"  +K2S04 

SOLUBILITY  OF  MIXED  CRYSTALS  OF  POTASSIUM  COPPER  SULFATE  AND 
AMMONIUM  COPPER  SULFATE  IN  WATER. 


CuS04.K2SO4.6H2O  and  CuSO4(NH4)2SO4.6H2O  at  I3°-I4°. 


(Fock,  1897.) 


Mols.  per  ioo  Mols. 
H20- 

Mol. 

per  cent  K  Salt. 

Mols.  per  too  Mols. 
H20. 

Mol.  per  cent  K  Salt. 

K 

O 
0. 
0. 

o. 

.  Salt. 

0897 
2269 
2570 

NH4  Salt. 
1-035 

0.8618 
o  .  6490 
0.5887 

in  Solution 
0 
5.06 
16.76 
30.40 

.    in  Solid. 
0 
10.34 

33-05 
46.22 

K  Salt. 

o  .  2946 

0-3339 
0.4560 

0-4374 

NH<  Salt. 

o  .  5096 

0.3319 
0.1961 
0 

in  Solution. 
36.63 
50.15 
69-93 
IOO 

lin  Solid. 
58.20 

75-34 
83.86 

IOO 

SOLUBILITY  OF  SOME  POTASSIUM  DOUBLE  SULFATES  IN  WATER  AT  25°. 

(Locke,  1902.) 

Gms.  Anhydrous  Salt 
per  ioo  Gms.  H2O. 

12.88 


Double  Salt. 

Potassium  Cobalt  Sulfate 
Copper       " 
Nickel 
Zinc 


Formula. 

K2Co(SO4)2.6H2O 
K2Cu(SO4)2.6H2O 
K2Ni(S04)2.6H20 
K2Zn(SO4)2.6H2O 


II  .69 

6.88 


SOLUBILITY  OF  POTASSIUM  NICKEL  SULFATE  AND  ALSO  OF  POTASSIUM  ZINC 
SULFATE  IN  WATER,  EACH  SEPARATELY  DETERMINED  AT  DIFFERENT  TEM- 
PERATURES. 


o 
10 

20 

25 
30 


Gms.  per  ioo  Gms.  H2O. 


.6H2O. 

6 

9 
14 
16 
18 


13 
19 
26 

30 
35 


t8. 

40 
50 
60 
70 


Gms.  per  ioo  Gms.  H2O. 


23 
28 

35 
43 


45 
56 

72 

88 


POTASSIUM   SULFATE  558 

SOLUBILITY  OF  THE  THREE  HYDRATES  OF  POTASSIUM  FERROSULFATE 
IN  WATER  AT  DIFFERENT  TEMPERATURES. 

(Kuster  and  Thiel,  1899.) 
KgSCU.FeSp4.6H2G-.  K2SO4.FeSO4.4H2O.  K2SO4.FeSO4.2H2O. 


t«.     cc.N/ioKMnO4  Cms.  K2SO4  cc.N/ioKMnO4  Gms.K2SO4    cc.N/ioKMnO4  Gms.K2SO" 

per  2cc. 
Solution. 

.FeSO4  per 
100  cc.  Sol. 

per  2  cc. 

Solution. 

.FeSO4  per 

100  CC.  Sol. 

per  2  cc. 

Solution. 

.FeSO4  per, 
100  cc.  Sol.4 

o-5 

12-4 

18.36 

*S'S 

22-94 

15-4 

22-79 

17.2 

17.0 

25.16 

18.1 

26.79 

21  .6 

3I-98 

40.1 

24.8 

36.72 

21.9 

32.41 

27.6 

40-86 

60 

29.0 

42-93 

24.1 

35-68 

28.8 

42.63 

80 

30.6 

45-29 

27-3 

40.46 

28.6 

42-34 

90 

.  .  . 

29.6 

43-82 

28.9 

42-73 

95 

... 

29.8 

44.11 

27.7 

41  -or 

SOLUBILITY  OF  MIXTURES  OF  POTASSIUM  AND  LEAD  SULFATES  AND  OF 
POTASSIUM  AND  STRONTIUM  SULFATES  IN  WATER. 

(Barre,  1909.) 

Results  for  K2SO4  +  PbSO4.  Results  for  K2SO4  +  SrSO4. 

Cms.  K2SO4  Cms.  K2S04 

t°.  per  zoo  Cms.  Solid  Phase.  t°.  per  100  Cms.  Solid  Phase. 

Sat.  Sol.  Sat.  Sol. 

7  0.56  PbS04.K2S04  17.5  1.27  K2S04.SrS04+SrSO< 

17  0.62  "                    50  1.88                  " 

50  1.09  "                   75  2.71 

75  i-37  ioo  3.90 

100  1.69 

SOLUBILITY  OF  POTASSIUM  SULFATE  IN  AQUEOUS  SOLUTIONS  OF  POTASSIUM 
CHLORIDE,  BROMIDE,  AND  IODIDE. 

(Blarez,  1891.) 
Interpolated  from  the  original  results. 

Grams  K2SO4  per  too  cc.  in  Aq. 

Grams  Halogen  Solutions  of: 

Salt  per  100 
cc.  Solution. 

O 
2 

4 

6 

8 

10 

12 


SOLUBILITY  OF  POTASSIUM  SULFATE  IN  AQUEOUS  SOLUTIONS  OF  POTASSIUM 

HYDROXIDE  AT  25°. 

(D'Ans  and  Schreiner,  1910.) 


KC1 

KBr 

KI 

at  12.5°. 

at  14°. 

at  12.5°. 

9.9 

10.  16 

9-9 

8-3 

9.1 

9-2 

7.0 

8.2 

8.4 

5-7 

7-4 

7-7 

4.6 

6.6 

7-2 

3-5 

6.0 

6.6 

5-5 

6.0 

Mols.  per  1000  Cms. 
Sat.  Solution. 

Gms.  per  100  Cms. 
Sat.  Solution. 

Mols.  per  1000  Gms. 
Sat.  Solution. 

Gms.  per  100  Gms. 
Sat.  Solution. 

(KOH)2. 
0 
0.258 

0-433 
I-I3 

K2S04.' 
0.6l7 

0-433 
0.280 

0.137 

KOH. 
O 
2.892 
4.854 
12.67 

K2S04. 
10-75 

7-544 
4.878 
2.386 

(KOH)2. 
2.86 
3-42 
4.809 

K2S04. 
0.035 
0.009 
0 

'  KOH. 
32.06 

38.33 
53-51 

K2S04. 

0.61 
0.16 
o 

559 


POTASSIUM  SULFATE 


SOLUBILITY  OF  MIXED  CRYSTALS  OF  POTASSIUM  SULFATE  AND  POTASSIUM 
CHROMATE  AT  25° 

(Fock,  1897.) 


Milligram 

Mols.  per  Liter 

Grams  per  Liter. 

Mol.  pe 

:r  cent         Sp.  Gr.      Mol.  per  cen? 

r\    ;.,                      —  £                     v  o/-\     • 

'   K2S04. 

K2Cr04. 

K2S04. 

K2Cr04: 

K2So4  iu               ui 
Solution.            Solution. 

J\.2O^4  HI 

Solid  Phase. 

618 

i 

O 

•  O 

107 

•7 

O 

.00 

100 

.0           1-083 

IOO.O 

608 

4 

103 

106 

.0 

2O 

.02 

85 

.51      1.092 

99.65 

34i 

.0 

691 

.8 

59 

.46 

134 

•5 

33 

.01         1.141 

97-30 

174 

.8 

1496 

.0 

30 

•47 

290 

•5 

10 

•50 

.231 

91.97 

no 

•7 

2523 

19 

•30 

49° 

•5 

4 

.21            3 

•356 

28.43 

100 

.6 

2687 

17 

•54 

522 

•3 

3 

.60 

•377 

2-41 

0 

0 

2847 

0 

.0 

553 

•5 

0 

•  OO 

•398 

o.oo 

734 

-O 

O 

.0 

127 

•9 

0 

.0 

100 

•O              3 

.0863 

IOO.O 

617 

.0 

103 

•4 

107 

.6 

20 

.1 

85 

.65          3 

•0934 

99.78 

463 

452 

•7 

80 

.72 

88 

.0 

55 

•55 

•I235 

98.49 

279 

948 

.2 

48 

.64 

184 

•4 

22 

.72        1.1700 

96.07 

1469 

26 

.68 

285 

.6 

9 

.41        1-2255 

85-77 

296 

268l 

51 

.61 

521 

.2 

21 

.09        1.3688 

25-73 

o 

.0 

2715 

0 

.00 

527 

.8 

0 

.00         1-3781 

o.oo 

SOLUBILITY  OF  POTASSIUM  SODIUM  SULFATES  IN  WATER. 


Double  Salt. 

3K2S04.Na2SO4 
5K2SO4.Na2SO4 


103-5 
4-4 
12.7 
100 


Gms.  per  100 
Cms.  H2O. 

Authority. 

40.8 

(Penny,  1855.) 

9.2 

(Gladstone,  1854-) 

10.  1 

25 

SOLUBILITY  OF  POTASSIUM  SULFATE  IN  AQUEOUS  SOLUTIONS  OF  SODIUM 

SULFATE. 


Results  at  25°. 

(Smith  and  Ball,  1917.) 
Gms.  per  100  Gms. 


Results  at  34°  and  at  6o°- 
(Nacken,  1910.) 


Na2S04. 
O 

I.78 
3-58 
5.38 
7.19 


K2S04. 
12.05 

12-33 
12.65 
12.89 
13.12 


Gms.  per  100  Gms. 
Sat.  Sol.  at  34°- 

Gms.  per  100  Gms. 
Sat.  Sol.  at  60°. 

Solid  Phase 
at  34°  and  at  60°. 

Na2SO4. 

K2so4: 

'Na2S04. 

K2S04. 

0 

11.9 

0 

15-3 

K2S04 

7.1 

10.7 

6.6 

13-9 

"  +Glaserite 

31-4 

4.3 

27.1 

8.2 

NajSC^+Mix  crystals 

33  •  I 

0 

0 

NajS04 

Additional  data  for  the  above  system  at  15°,  25°,  40°,  50°,  60°,  70°  and  80°  are 
given  by  Okada  (1914).  The  results  show  that  potassium  and  sodium  sulfates 
form  a  double  salt  of  the  composition  "K3N a (SO4)2.  This  double  salt  dissolves 
sodium  sulfate  as  a  solid  solution  but  not  potassium  sulfate. 


POTASSIUM   SULFATE  560 

SOLUBILITY  OF  POTASSIUM  SULFATE  IN  AQUEOUS  SOLUTIONS  OF  SULFURIC 

ACID  AT  1 8°. 


Mols.  per  100  Mols. 
K2S04+H2SQ4+H20. 

K^SOT  H2S04. 

I. 10  O 

i-59  o-95 

2.49  2.70 

2-75  3-17 

2-75  3-74 

2.83  5.08 


(Stortenbecker,  1902.) 


Solid  Phase. 


K2S04 


Mols.  per  100  Mols. 
K2S04+H2S04+H2O. 


K2S04. 
2.80 

2.61 

2.  25 
I. 08 
0.77 
0.44 


H2S04. 

5-79 
5-6i 
6. 19 

7-94 
9.2 
22.7 


Solid  Phase. 

K2SO4.3KHSO4 

K2SO4.6KHSO4 

"  +KHS04 

KHS04 


SOLUBILITY  OF  POTASSIUM  SULFATE  IN  AQUEOUS  SOLUTIONS  OF  SULFURIC 

ACID  AT  o°. 

(D'Ans,  igoga.) 


Mols.  per  1000  Cms. 
Sat.  Sol. 

K2S04.                  H2S04. 

0-53                   < 
0.64                  < 

0.74 

5-37 
3-75 
.08 

0-73 

•13 

0.71 

0.69 

0.69             : 

•44 
.66 
.88 

Solid  Phase. 


K2S04 


"  +K3H(S04), 


+Ka 


SS. 


Sol. 


K2S04. 

0.61 
0-54 
o-53 
0-43 
0.28 

O.I2 

0.09 


H2S04. 
2.12 
2.29 
2.30 
2.48 
3-04 

4-43 
5-27 


Solid  Phase. 

Ka+Kb 
Kb 

"  +KHS04 
KHSO4 


Ka  and  Kb  are  acid  sulfates  between  K3H(SO4)2  and  KHSO4.     Their  composi- 
tions were  not  determined. 


SOLUBILITY  OF  POTASSIUM  SULFATE  IN  AQUEOUS  SOLUTIONS  OF  SULFURIC 

ACID  AT  25°. 

(D'Ans,  igoga,  igia;  see  also  Herz,  ig  11-12.) 


Mols.  per  1000  Gms. 

Sat. 

Sol. 

Solid  Phase. 

K2S04. 

H2SO4.  ' 

.27 

I-3I 

K2S04+K3H(S04)2 

•33 

1.99 

K3H(S04)2+Ky 

.24 

2.03 

Ky 

•13 

2.17 

" 

.04 

2-35 

"   +KHSO4 

.032 

2-345 

KHS04 

0.67 

2.83 

« 

O.22 

4-13 

" 

0.15 

5.36 

« 

K2S04. 

H2SO4+SO3. 

O.I7I 

6.42 

KHS04 

O.I90 

6.60 

« 

0.266 
0.182 

6.91 
7.26 

"  +KH3(SO4)2.H2O 

0.157 

7.62 

0.167 

7-88 

0.201  8 

Ky  =  an  acid  sulfate  between 
position  was  not  determined. 


Mols.  per  1000  Cms. 
Sat.  Sol. 

Solid  Phase. 

K2SO4. 

H2S04+S03. 

0.250 

8.10 

KHsCSO^.HzO 

0.352 

8.15 

" 

0.364 

8.16 

"  -l-KHaCSOO, 

0.341 

8.29 

KHsCSO,), 

0.322 

8.33 

" 

0.325 

8-45 

" 

0.346 

6.62 

« 

0.384 

8-57 

« 

0.412 

8.71 

K 

0.583 

8.82 

« 

0.880 

8.65 

"  +KHS207 

0.899 

8.63 

KHS207  (unstable) 

0.882 

8.70 

« 

0.561 

8.96 

" 

0.365 

9.80 

" 

0-43 

9-78 

(i 

0.665 

9.80 

" 

0-937 

9.66 

« 

and  KHSO4  of  which  the  exact  com- 


56i  POTASSIUM   SULFATE 

SOLUBILITY  OF  POTASSIUM  SULFATE  IN  AQUEOUS  ALCOHOL. 

(Gerardin,  1865;  Schiff,  1861.) 

In  Aq.  Alcohol  of  0.939  In  Alcohol  of  Different 

Sp.  Gr.  =  40  Wt.  %.  Strengths  at  15°. 

,0  Cms.  K2SO4  per  ioo  Weight  per        Cms.  K2SO4  per  too 

Cms.  Alcohol.  cent  Alcohol.  Cms.  Sat.  Sol. 

40  0.16  10  3.90 

80  O.2I  2O  1.46 

60  0.92  30  0.56 

40  0.21 


SOLUBILITY  OF  POTASSIUM  SULFATE  IN  AQUEOUS  ALCOHOL  AT  25°. 

(Fox  and  Gauge,  1910.) 
Cms.  per  ioo  Gms.  Sat.  Solution.  Cms.  per  ioo  Cms.  Sat.  Solution. 


K2SO4.               C2H5OH.                   H20.  K2SO4.               C2H5OH.                H2O. 

9.17             1.35            89.48  2.66            15.26          82.08 

6.90                 4.80                 88.30  1.83                 20.50              77-67 

4.96                  7.80                 87.24  0.97                 26.91               72.12 

4.32                  9.70                 85.98  0.41                 35.97              63.62 

3.57                12.34                 84.09  0.22                 43.90               55.88 

2.71           14.51            82.78  0.016          69.26          30.72 

SOLUBILITY  OF  POTASSIUM  SULFATE  AT  25°  (Fox  and  Gauge,  1910.)  IN: 

Aqueous  Chloral  Hydrate  Solutions.  Aqueous  Glycerol  Solutions. 

Gms.  per  ioo  Gms.  Sat.  Solution.  Gms.  per  ioo  Gms.  Sat.  Solution. 


K2S04.            CC13CH(OH)2.           H2O.  K2SO4.        (CH2OH)2CHOH.          H2O. 

9.13                     6.44              84.43  8.87                    8.96              82.17 

8.41               9.09          82.50  7.69            13-36          78-95 

7.79                  12.38              79.83  6.47                 20-34              73.19 

7.31                  13.20              79.49  5.83                 24.15              70.02 

5.88                  22.07              72.05  4.44                33.73              61.83 

4.54                  33.15              62.31  3.65                 40.40              55.95 

3.36                  44.40              52.24  3.38                 43.52              53.10 

2.92                  47.30              49.78  2.69                 50.18              47.13 

2                  62.82          35-i8  2.07            57-22          40.71 

1.75             70.28          27.97  i-53            67.94          3°-53 

1.40            80.36          18.24  0.98            78.18          20.84 

i. 08             85.26          13.66  0.73            98.28            0.99 

SOLUBILITY  OF  POTASSIUM  SULFATE  AT  25°  (Fox  and  Gauge,  1910.)  IN: 

Aqueous  Acetone  Solutions.  Aqueous  Pyridine  Solutions. 

Gms.  per  ioo  Gms.  Sat.  Solution.  Gms.  per  ioo  Gms.  Sat.  Solution. 


K2SO4.  (CH3)2CO.  H2O.  K2SO4.       CH<(CH.CH)2>N.      H2O. 

7.20  4.92  87.88  7.95  4.23  87.82 

5.02  10. 06  84.92  4.77  13.90  81.33 

2.96  16.23  8o.8l  2.75  24.51  72.74 

1.50  24.31  74.19  1.47  34.19  64.34 

0.47  37.19  62.34  0.45  46.29  53.26 

0.20  46.29  53.51  0.12  55.93  43.95 

0.03  62.40  37-57  0.006  75-QO  24.09 


POTASSIUM  SULFATE  562 

SOLUBILITY  OF  POTASSIUM  SULFATE  AT  25°  (Fox  and  Gauge,  1910.)  IN: 
Aqueous  Ethylene  Glycol  Solutions.  Aqueous  Mannitol  Solutions. 

Gms.  per  100  Gms.  Sat.  Solution.  Gms.  per  100  Gms.  Sat.  Solution. 


K2S04.                (CH2OH)2.               H20.  K2S04.      (CHOH)4(CH2OH)2.        H2O. 

9.67                     3.16              87.17  10.32                 3.20              86.48 

7.69              9.79          82-53  9-61            8-35          82.04 

5.74             18.47          75.79  9.19          11.26          79.55 

3.57             32.11          64.32  8.66          14.30          77.04 

1.83             49-°3          49-14  8.35           17.22          74.43 

SOLUBILITY  OF  POTASSIUM  SULFATE  AT  25°  IN: 

Aq.  Sucrose  Solutions.  Aq.  Potassium  Acetate  Solutions. 

(Fox  and  Gauge,  1910.)  (Fox,  1909.) 

Gms.  per  100  Gms.  Sat.  Solution.  Gms.  per  100  Gms.  Sat.  Solution. 


K2S04.               CuHaOu.                H20.                           K2SO4.           CH3COOK.  H2O. 

9.65             9.56          80.79                  6.65            6.  ii  87.24 

8.65           18.55          72.80*                5.09            8.68  86.23 

7.42           28.16          64.42                 3.99          11.29  84.72 

6.35         37.24        56.41              2.35        15.59  82.06 

5.21                47.55               47.24                          1.23               20.12  78.65 

4.24          57               38.76                 0.39          29.95  69.66 

100  gms.  glycerol  of  d  =  1  .255  dissolve  1.316  gms.  K2SO4  at  ord.  temp.  (Vogel,  1867.) 

SOLUBILITY  OF  POTASSIUM  SULFATE  IN  AQUEOUS  ACETIC  ACID  AND  IN 
AQUEOUS  PHENOL  SOLUTIONS  AT  25°. 

(Rothmund  and  Wilsmore,  1902.) 

In  Aq.  Acetic  Acid.  In  Aq.  Phenol. 

Mols.  per  Liter.  Grams  per  Liter.  Mols.  per  Liter.  Grams  per  Liter. 

'  ' 


taCOOH.      K2S04.        CH3COOH 

.     lv2SO4.       C-gxi^Oii.                    K2SC/4. 

C6H5OH.    K2SO,. 

o.o 

0-6714 

0 

.0 

117 

.0 

0-0 

o 

.6714 

0 

.0 

117.0 

0.07 

0.6619 

4 

.2 

JI5 

•4 

0.032 

o 

.6598 

3 

.01 

115.0 

0-137 

0-6559 

8 

.22 

114 

•4 

0.064 

o 

.6502 

6 

.02 

IJ3-3 

0-328 

0.6350 

19 

.68 

no 

.8 

0.127 

0 

.6310 

II 

•94 

no.o 

0-578 

0.6097 

34 

.68 

1  06 

•3 

0.236 

o 

.6042 

22 

.19 

I05-3 

I.I5I 

o-5556 

69 

.06 

96 

.87 

0.308 

o 

•5834 

28 

•97 

101  .7 

2.183 

0-4743 

128 

•58 

82, 

.70 

0.409 

o 

•5572 

38 

.46. 

97.2 

0.464  0.5480    43  .63       95.5 

0.498  (sat.)  0-5377    46.82      93.8 

100  gms.  water  dissolve  10.4  gms.  K2SO4  +  219  gms.  sugar  at  31.25°,  or  100 
gms.  sat.  solution  contain  3.18  gms.  K2SO4  +  66.74  gms-  sugar.  (Kohler,  1897.) 

loo  gms.  95%  formic  acid  dissolve  36.5  gms.  K2SO4  at  21°.  (Aschan,  1913.) 

100  gms.  95%  formic  acid  dissolve  14.6  gms.  KHSO4  at  19.3°. 
100  cc.  anhydrous  hydrazine  dissolve  5  gms.  K2SO4  at  room  temp. 

(Welsh  and  Broderson,  1915.) 
100  gms.  hydroxylamine  dissolve  3.5  gms.  K2SO4  at  17-18°.  (de  Bruyn,  189*.) 

FREEZING-POINT  DATA  (Solubility,  see  footnote,  p.  i)  ARE  GIVEN  FOR  THE 
FOLLOWING  MIXTURES: 

K2SO4  +  K2WO4.  CAmadori,  1913-) 

•f  Ag2SO4.  (Nacken,  19070.) 

+  NaCl.  (Sackur,  1911-12.) 

H-  Na2SO4.  (Jaenecke,  1908;   Nacken,  1907  (b)  (c);  Sackur,  1911-12). 

+  SrSO4.  (Grahmann,  1913;  Calcagni,  1912,  19124.) 


563  POTASSIUM   BiSULFATE 

POTASSIUM   BiSULFATE  KHSO4. 

SOLUBILITY  IN  WATER. 

(Kremers,  1854.) 
t°.  o°.  20°.  40°.  100°. 

Cms.  KHS04  per  ioo  gms.  H2O  36.3  51.4  67.3          121.6 

See  also  p.  560. 


POTASSIUM   PerSULFATE 

SOLUBILITY  IN  WATER. 

(Tarugi,  1904.) 


+o         Gms.  K-^Og  per  to  Gms.  K^Og  per  f  0  Gms.  I^Og  per 

1  '          ioo  cc.  Sat.  Sol.  ioo  cc.  Sat.  Sol.  ioo  cc.  Sat.  Sol. 

o  1.620  15  3.140(3.7)  30  7.190(7.7) 

5  2.156  20  4-490  35  8.540 

10  2.600  25  5-840  40  9.890 

The  results  in  parentheses  are  the  averages  of  a  large  number  of  determinations 
by  Pajetta  (1906).  This  investigator  employed  constant  agitation  for  various 
lengths  of  time.  Tarugi  approached  equilibrium  from  above  as  well  as  below  but 
stirred  the  solutions  only  at  intervals.  The  determination  of  the  dissolved  per- 
sulfate  was  made  by  boiling  a  measured  volume  of  the  clear  saturated  solution  for 
20  min.  and  titrating  the  H2SOi  liberated,  according  to  the  equation  K2S2O8-f-H2O 
=  K2SO4  +  H2SO4  +  O.  Tarugi  also  reports  that  the  presence  of  a  number  of 
sodium  and  other  salts  in  solution,  does  not  appreciably  alter  the  solubility  of 
K2S2O8  in  water. 

ioo  gms.  H2O  dissolve  1.77  gms.  K2S2Os  at  o°.  (Marshall,  1891.) 

SOLUBILITY  OF  POTASSIUM  PERSULFATE  IN  SATURATED  AQUEOUS  SALT 
SOLUTIONS  AT  12°. 

(Pajetta,  1906.) 

(An  excess  of  the  salt  and  of  K2S2O8  was,  in  each  case,  added  to  water  and  the 
mixture  stirred  at  constant  temperature  for  10  to  20  hours.) 

Salt  Gms.  K2S2O8  per  sl  Gms.  K^Og  per 

balt' 


.  . 

ioo  Gms.  Sat.  Sol.                        balt'  ioo  Gms.  Sat.  Sol. 

Water  alone                    3.196  K2SO4  0.798 

Na2SO4.ioH20                6.238  KHS04  0.336 

NaHS04                          8.842  KNO3  0.904 

Na2HPO4.i2H2O             4.766  K2CO3  0.0146 

Na2B4O7.ioH2O               3.825  KHCO3  0.317 

NaNO3                         19.302  MgSO4.7H2O  2.990 

Na2CO3.ioH2O               5.682  CaSO4.2H2O  3.384 
NaHC03                         5.042 

Additional  determinations  made  with  salt  solutions  of  lower  concentrations 

than  saturation,  gave  the  following  results  at  12.5°. 


Gms.  Salt  per        Gms.  KjSjOg  Gms.  Salt  per      Gms. 

Salt.  ioo  Gms.  per  ioo  Gms.  Salt.  ioo  Gms.          per  ioo  Gms. 

H20.  Sat.  Sol.  H2O.  Sat.  Sol. 

Na2CO3  2.304  4.297  NaHS04         5.218  4.556 

NaHCO3  3.652  4.230  NaNO3  3.696  4.613 

Na2SO4.ioH2O         7  4.554  Na2HP04       3.086  4.446 

POTASSIUM   Ethyl  SULFATE  K(C2H6)SO4. 

SOLUBILITY  IN  WATER. 

(Illingworth  and  Howard,  1884.) 

Gms.  K(C2H5)SO4 
t°.  per  ioo  Gms. 

Sat.  Sol. 
—  14.2  45.01 

O  53-71 

+  15  62.35 


POTASSIUM   Ethyl  SULFATE  564 

SOLUBILITY  OF  POTASSIUM  ETHYL  SULFATE,  POTASSIUM  METHYL  SULFATE  AND 
OF  POTASSIUM  AMYL  SULFATE  IN  WATER,  DETERMINED  BY  THE  FREEZING- 

POINT  METHOD.  (Ulingworth  and  Howard,  1884.) 

Results  for  K(C2H6)SO4        Results  for  K(CH3)SO4      Results  for  K(C6HU)SO4 
+  H2O.  +  H2O.  +  H2O. 

j.o     t        Gms.  xo  -r          Gms.  +o'r         Gms. 

SSL 


—  2.2  10        Ice  —   2.3  10  Ice                        —    1.9  10       Ice 

—  4.9  20  "                        —   3.6  15  —  4.3  20 

—  8.2  30  —  5  20  —  5.4  24        " 

—  12.1  40  —  8  30  "                                                  +K(C6H11)SO4 
-  14.2  45  .  01  "+K(C2HB)S04  -  1  1  .  8  39  .  84  "  +K(CH3)SO4  -  4-8  25          K(C6Hn)SO4 

—  6  50  EXCzHjJSO*      —11.5  40  K(CH3)S04           o       33-44 
o  53-71  o  47.1  +17-3  59-46 

+  15  62.35  +12.3  54.8 

POTASSIUM  Sodium  SULFITE  KNa2H(SO3)2.4H2O. 

100  gms.  H2O  dissolve  69  gms.  of  the  salt  at  15°.  (Schwicker,  1889.) 

POTASSIUM  SULFONATES 

SOLUBILITY  IN  WATER. 

Gms.  Anhy- 
Salt.  t°.    drous  Salt  per  Authority. 

100  Gms.  H2O. 
Potassium  Naphthalene  Monosulfonate4H2O  25       8  .  48*       (Witt,  1915.) 

"  2  Phenanthrene  Monosulfonate.-IHaO      20      0.273       (Sandquist,  1912.) 

3  "  "  .oH20       20      0.342 

10  .iH2O      20      0.84 

"  o  Guaiacol  Sulfonate  (Thiocol)  15-20  16.6        (Squire  &  Caines,  1905.) 

*  d  =  1.029 

loocc.QOvol.  %  alcohol  dissolve  0.25  gm.thiocolat  I5°-2O°.    (Squire  and  Caines,  1905.) 

POTASSIUM   SULFIDE  K2S. 

Fusion-point  data  for  K2S  +  S  are  given  by  Thomas  and  Rule  (1917). 

POTASSIUM   Antimony  SULFIDE,  see  Potassium  Sulfoantimonate,  p.  500. 

POTASSIUM  TARTRATE  (K2C4H4O6)2.H2O. 

100  gms.  H20  dissolve  138  gms.  K2C4H4O6  at  16.6°,  Sp.  Gr.  of  sat.  sol.  =  1.49. 

(Greenish  and  Smith,  1901.) 

POTASSIUM  (Bi)  TARTRATE  (Mono)  KHC4H406,  Cream  of  Tartar. 
SOLUBILITY  OF  MONO  POTASSIUM  TARTRATE  IN  WATER. 

(Afluard,  1865;  Roelofsen,  1894;  Blarez,  1891;  at  20°,  Magnanini,  1901;  at  25°,  Noyes  and  Clement,  1894.) 


Gms.  KHC4H4O6  per  100 
t°.                                         Gms.  Solution.                                               t°. 

A 

Gms.  KHC4H406  per  100 
Gms.  Solution. 

0 

0. 

30  (R.) 

0. 

32  (A.) 

o, 

35  (B.) 

40 

0.96 

I. 

3 

1.29 

IO 

0. 

37 

0. 

40 

o 

42 

50 

1.25 

I, 

8 

i.  80 

2O 

0. 

49 

0. 

53  (M.) 

o, 

60 

60 

2. 

4 

25 

0. 

58 

0. 

654  (N.  and  C.) 

0. 

74 

80 

.  .  . 

4- 

4 

.  .  . 

30 

0. 

69 

0. 

9  (A.) 

0, 

89 

IOO 

6. 

3 

SOLUBILITY  OF  MONO  POTASSIUM  TARTRATE  IN  AQUEOUS  ALCOHOL  AT  25°. 

(Seidell,  1910.) 


Wt.  % 
C2H5OH 
in  Solvent 

du,oi 
Sat.  Sol. 

Gms.  KHC4H4O« 
per  loo  Gms. 
Sat.  Sol. 

Wt.  % 
C2H8OH 
in  Solvent. 

<*25  Of 

Sat.  Sol. 

Gms.  KHC4H4O« 
per  loo  Gms. 
Sat.  Sol. 

0 

I.OO2 

0.649 

50 

0.912 

0.064 

IO 

0.985 

0.358 

00 

0.890 

0.043 

20 

0.970 

0.2IO 

80 

0.842 

0.023 

30 

0-953 

O.I3I 

92.3 

0.807 

O.OI4 

40 

0-933 

0.087 

IOO 

0.789 

O.OIO 

565 


POTASSIUM   BiTARTRATE 


SOLUBILITY  OF  MONO  POTASSIUM  TARTRATE  IN  AQUEOUS  ALCOHOL  AT  18°. 

(Paul,  1917.) 


Cms.  C2H5OH  per  100  cc.  solvent        o  5 

Gms.  KHC4H4O6  per  liter  sat.  sol.       4 . 903      3 . 58 


2.94 


10 
2-57 


Approximate  determinations  at  other  temperatures  are  given  by  Roelofsen 
(1894)  and  by  Wenger  (1892). 

SOLUBILITY  OF  MONO  POTASSIUM  TARTRATE  (KHC4H4O6)  IN  NORMAL 
SOLUTIONS  OF  ACIDS  AT  20°. 

(Ostwald;  Huecke,  1884.) 

Purified  tartrate  was  added  in  excess  to  normal  solutions  of  the  acids,  and,  after 
shaking,  clear  I  cc.  portions  of  each  solution  were  withdrawn  and  titrated  with 
approximately  o.i  n  Ba(OH)2  solution;  I  cc.  normal  acid  requiring  10.63  cc»  of 
the  Ba(OH)2  solution. 


Acid. 

Gms. 
Acid 

cc.  N/io 
Ba(OH)2 

Gms. 
KHC4H4O< 

1           Acid 

Gms.      cc.  N/io      Gms 
Acid     Ba(OH)2  KHC4H4O6 

per  100  cc.    pei 
Solvent.    Sol 

•  i  cc. 

ution. 

per  loo  cc. 
Solution. 

per  100  cc. 
Solvent. 

per  i  cc.  per  ico  cc 
Solution.     Solution" 

HNO3 

6. 

31 

5 

77* 

10. 

21 

C2H5S03H 

II.  O 

5 

.01* 

8.87 

HC1 

3- 

65 

5- 

32 

9- 

42 

HO.(CH2)2SO3H 

12.  6l 

5 

•33 

9-43 

HBr 

8. 

IO 

5- 

38 

9- 

75 

C6H5S03H 

15.81 

5 

•25 

9.29 

HI 

12. 

80 

5- 

43 

9- 

61 

HCOOH 

4.60 

0 

•45 

0.80 

H2S04 

4- 

90 

3- 

97 

7- 

°3 

CH3COOH 

6.00 

0 

.27 

0.48 

HCH3SO4 

ii. 

21 

5- 

58 

12. 

44 

CH2C1COOH 

9-45 

I, 

.01 

1.79 

HC2H5S04 

12. 

61 

9- 

58 

C2H5COOH 

7.40 

0 

.24 

0.42 

HC3H7S04 

14. 

OI 

5. 

21 

9- 

22 

C3H7COOH 

8.81 

0 

•23 

0.41 

*  The  figures  in  this  column  show  the  amount  of  the  Ba(OH>2  solution  in  excess  of  that  which  would 
have  been  required  by  the  normal  acid  solution  alone  in  each  case,  viz.,  10.63  cc.  They,  therefore,  corre- 
epond  to  the  amount  of  KHC^Oo  dissolved  in  i  cc.  of  each  saturated  solution,  and  when  multiplied 
by  i-77give  the  grams  of  KHC4H4Oe  per  100  cc.  solution. 


SOLUBILITY  OF  MONO  POTASSIUM  TARTRATE  (KHC4H4O6)  IN  AQUEOUS 
SOLUTIONS  OF  ELECTROLYTES  AT  25°. 

(Noyes  and  Clement,  1894;  Magnanini,  1901.) 


Electro- 

Gm. Equiv.  per 
Liter. 

Gms.  per 
Liter. 

Electro- 

Gm. Equiv.  per 
Liter. 

Gms.  per 
Liter. 

lyte. 
KC1 

Electro-      KHC4 
lyte.         H4O6. 

0.025    0.0254 

Electro- 
lyte. 

1.86 

KHC4 

HA 

4.788 

lyte. 

CHsCOOK 

Electro- 
lyte. 

0.05 

KHC4* 

HA. 

0.0410 

Electro- 
lyte. 

4.91 

KHC4" 

HA. 
7.718 

" 

0.05 

0.0196 

3 

•73 

3-680 

" 

O.  IO 

o  .  0504 

9.82 

9.486 

u 

O.  IO 

0.0133 

7 

.46 

2.509 

" 

o.  20 

0.0634 

19.63 

II. 

930 

11 

O.2O 

0.0087 

14 

.92 

1.636 

KHS04(2o°) 

O.OI 

0.0375 

1-36 

7- 

06 

KC103 

0.025 

0.0256 

3 

.06 

4.821 

" 

O.O2 

0.0500 

2.72 

9- 

AI 

u 

0.05 

0.0197 

6 

•13 

3.716 

" 

O.  IO 

0.1597 

13.62 

30. 

06 

" 

O.  IO 

0.0138 

12 

.26 

2.601 

KHC2O4*  (20°) 

O.OI 

o  .  0369 

1.28 

6. 

94 

" 

O.2O 

0.0097 

24 

•  52 

1.728 

a 

0.02 

o  .  0424 

2.56 

7- 

98 

KBr 

0.05 

0.0192 

5 

•95 

3.699 

u 

0.10 

O.II32 

12.82 

21. 

30 

" 

0.10 

0.0134 

ii 

.91 

2.517 

HC1 

0.013 

0.0367 

0-45 

6. 

90 

" 

o.  20 

0.0087 

23 

.82 

1.629 

" 

O.O25 

0.0428 

0.91 

8. 

06 

KI 

0.05 

0.0196 

8 

•30 

3.687 

" 

O.O5O 

o  .  0589 

1.82 

ii. 

09 

M 

O.  10 

0.0132 

16 

.61 

2.492 

Nad 

0.05 

0.0376 

2.92 

7- 

08 

u 

o.  20 

0.0086 

33 

.22 

1.619 

tt 

O.IO 

0.0397 

5.85 

7- 

48 

KNO3 

0.05 

0.0195 

5-06 

3.676 

11 

o.  20 

0.0428 

11.70 

8. 

05 

u 

O.  IO 

0.0136 

IO 

.  12 

2.551 

NaC103 

0.05 

0.0382 

5-32 

7- 

18 

" 

o.  20 

0.0090 

20 

.24 

1.696 

M 

O.IO 

o  .  0405 

10.65 

7- 

63 

K2SO4 

0.05 

0.0208 

4 

.36 

3.921 

" 

O.2O 

0.0446 

21.30 

8. 

40 

" 

0.10 

0.0147 

8 

.72 

2.769 

M 

0.20 

O.OIOO 

17 

•44 

1.888 

*  =  acid  potassium  oxalate. 


POTASSIUM  TARTRATE  566 

POTASSIUM  Sodium  TARTRATE.     KNa.C4H4O6.4H2O.     (Rochelle  or  Seig- 

nette  Salt.) 

loo  gms.  sat.  aq.  solution  contain  36.66  gms.  KNaC4H4O6  at  9.7°  and  47.97  gms. 
at  29.5°.  (van't  Hoff  and  Goldschmidt,  1895.) 

loo  gms.  H2O  dissolve  53.53  gms.  KNaC4H4O6  at  15°,  Sp.  Or.  of  sol.  =  1.2713. 

(Greenish  &  Smith,  1901.) 

SOLUBILITY  OF  MIXTURES  OF  POTASSIUM  TARTRATE  AND  OF  SODIUM 
TARTRATE  IN  WATER  AT  SEVERAL  TEMPERATURES. 

(van  Leeuwen,  1897.) 
AB  Gms.  per  100  Gms.  Sat.  Sol.  Gms.  per  roo  Gms.  Sat.  Sol. 

*  •  '-K  rwn    '*r   rwr>  '    Solld  Phase'  *  '  '  y  r  H  n    -    -  —    '       Solld  Phase* 

K2C4H4U6.    J\a2L4Jl4Us.  Js.2^4Al4U6. 


l8  19.2  16.5    KNaCiHiQs^HsiO       26.6        56  4.2    KNaC4H406.4H2O+K2T 

38  26.6  22.8        "  48.3         51.6  13.2 

20.9     ii. 8         28          "  +Na*T  59-7       44-5  25.3 

38  25.8  24.7        "          "  80  39.7  34.7 

50  36.7  23.9        " 

K2T  =  K2C4H4O6.£H2O.     Na2T  =  Na2C4H4O6.2H2O. 


SOLUBILITY  OF  SEVERAL  POTASSIUM  SALTS  OF  TARTARIC  ACIDS  IN  WATER  AT  20°. 

(Schlossberg,  1900.) 
Salt.  Formula.  Q^^sS° 

Potassium  Sodium  Salt  of  Racemic  Acid  KNa(C4H4O6).3H20  62.84 
Potassium  Sodium  Salt  of  d  Tartaric  Acid  KNa(C4H4O6).4H2O  63 . 50 
Potassium  Neutral  Inactive  Pyrotartrate  K^CsHeOe.H^O  56.33 

Potassium  Neutral  Dextropyrotartrate          K^CsHeOe  57-62 

• 
SOLUBILITY  OF  POTASSIUM  SODIUM  TARTRATE  IN  AQ.  ALCOHOL  SOLUTIONS  AT  25°. 

(Seidell,  1910.) 

Wt.  %  ,      .  Gms.  Wt.  %  .      .  Gms. 

QH6OH  s^'c*,       KNaC4HA.4H80  C2H5OH  J*«  2*          KNaC4H4O6.4H2O 

in  Solvent.  bat"  SoL  per  100  Gms.  Solvent  in  Solvent.          bat'  SoL     per  100  Gms.  Sat.  Sol. 

o  1.310  53.33  50  0.908  2.40 

10  .     1.216  41.60  60  0.878  0.90 

20  1.124  26.20  70  0-857  °-3° 

30  1.034  13.80  80  0.840  0.06 

40  0.961  6  100  0.789  trace 

POTASSIUM   DihydroxvTARTRATES  K2C4H4O8.H2O  and  KHC4H4O8.H2O. 

100  gms.  H2O  dissolve  2.66  gms.  K^I^Os.HoO  at  o°.  (Fenton,  jSgS.) 

100  gms.  H2O  dissolve  2.70  gms.  KHC4H4O8.H2O  at  o°. 

F.-pt.  data  for  mixtures  of  d  and  /  dimethyl  ester  of  potassium  bitartrate  and 
for  mixtures  of  d  and  /  diacetyl  dimethylester  of  potassium  bitartrate  are  given  by 
Adriani  (1900). 

POTASSIUM   TELLURATE  K2TeO4. 

100  gms.  H2O  dissolve  8.82  gms.  K2TeO4  at  o°,  27.53  gms.  at  20°  and  50.42  gms. 

at  30  .  (Rosenheim  and  Weinheber,  1910-11.) 

POTASSIUM  THIOCYANATE   KSCN. 

SOLUBILITY  IN  WATER. 


SStSSXL      SolidPhase'                  Auttefty. 

-  6.5 

16.7 

Ice                            (Rudorff,  1872.) 

-  9-55 

23.1 

«                                         « 

—31.2    Eutec. 

50.25 

"  +KSCN              (Wassilijew,  1910.) 

0 

63-9 

KSCN 

20 

68.5 

"                     (Rudorff,  1869.) 

25 

70.5 

"                    (Foote,  1903.) 

567 


POTASSIUM  THIOCYANATE 


SOLUBILITY  OF  MIXTURES  OF  POTASSIUM  THIOCYANATE  AND  SILVER 
THIOCYANATE  IN  WATER  AT  25°. 

(Foote,  1903.) 


Solid 
Phase. 

KSCN 
KSCN  4-  zKSCN.AgSCN 


Double  Salt. 
2KSCN.AgSCN  = 

53- 92%  KSCN 

2KSCN.AgSCN+ 

KSCNAgSCN 

Double  Salt. 

KSCN  .AgSCN  = 

36.9%  KSCN 

KSCN  AgSCN  +  AgSCN 


Gms.  per 

TOO  Gms.  Solution. 

Mols.  per 

ioo  Mols.  H^O. 

KSCN. 

AgSCN. 

KSCN. 

AgSCN." 

70-53 

44.36 

66-55 

9-32 

51  .13 

4.19 

64.47 

10.62 

47-98 

4-60] 

61  .25 

II  .76 

42.07 

4-7*1 

.58.34 

*3-55 

38.47 

5-23  1 

53-21 

17  .53 

33-71 

6.5oJ 

50.68 

20.43 

32.52 

7-67 

49-43 
32-51 

20.32 
18.34 

30.29 
12  .26 

7.28^1 
4-05  f 

24.68 

16.41 

7-77 

J 

23.86 

16.07 

7-36 

2.90 

SOLUBILITY  OF  POTASSIUM  THIOCYANATE  IN  ACETONE,  AMYL  ALCOHOL,  ETC. 

(von  Laszcynski,  1894.) 

In  Acetone.     In  Amyl  Alcohol.     In  Ethyl  Acetate.     In  Pyridine. 


Gms.  KSCN  per              Gms.  KSCN  per                  Gms.  KSCN  per                 Gms.  KSCN  per 
t°.         100  Gms.            t°.        100  Gms.               t°.           100  Gms.              t°.        100  Gms. 

(CH3)2CO. 

CsHnOH. 

CH3COOC2H6 

CsHfiN. 

22 

20-75 

13 

0.18 

o 

0.44 

0 

6-75 

58 

20-40 

65 

i-34 

14 

0.40 

20 

6.15 

100 

2.14 

79 

O.2O 

58 

4-97 

133-5 

3-i5 

97 

3-88 

"5 

3.21 

SOLUBILITY  OF  POTASSIUM  THIOCYANATE  IN  PYRIDINE,  DETERMINED  BY 
THE  SYNTHETIC  METHOD. 

(Wagner  and  Zerner,  1911.) 


-42 
-42.1 
-42.4 
-42.8 


Gms.  KSCN 

per  loo  Gms. 

Mixture. 

O 
0-5 

i-33 

2.4 


Solid 
Phase. 


Gms.  KSCN 

per  loo  Gms. 

Mixture. 


-43.3Eutec.    3.1 
about  +10  2.2 


+KSCN 
KSCN 


70-71 
II6-II7 
172.7 


173. 8m.  pt. 


Solid 
Phase. 

KSCN 


1.23 

0.89 

at  this  temperature  two  liquid 
layers  appear  and  do  not  be- 
come homogeneous  up  to  200°. 
100  KSCN 


ioo  gms.  anhydrous  acetonitrile  dissolve  11.31  gms.  KSCN  at  18°. 

(Naumann  and  Schier,  1914.) 

Fusion-point  data  for  mixtures  of  KSCN  +  NaSCN  and  KSCN  +  RbSCN 
are  given  by  Wrzesnewsky  (1912). 


POTASSIUM   THIOSULFATE 


568 


POTASSIUM   THIOSULFATE 

SOLUBILITY  IN  WATER. 


Solid  Phase. 


(Jo,  1911,1912.) 


O 

Gms.  K^Os 
per  ioo  Gms. 
H20. 

96.1 

17 

I50-5 

20 
25 

155-4 
165 

30 

175-7 

35 

2O2.4 

40 
45 

204.7 
208.6 

50 

215.2 

55 

227.7 

3K2S2O3.sH2O 


t°. 

Gms.  K2Sj03 
per  ioo  Gms. 

H20. 

56.1 

234-5 

60 

238.3 

65 

245-8 

70 

255-2 

75 

268 

78.3 

292 

80 

293.1 

85 

298.5 

90 

312 

Solid  Phase. 


2S2O3.H2O 
3K2SA.H20 


POTASSIUM   Sodium  THIOSULFATE  KNaS2O3.2H2O. 
100  gms.  H2O  dissolve  213.7  Sms-  KNaS2O3.2H2O  (a)  at  15°. 
100  gms.  H2O  dissolve  205.3  gms.  KNaS2O3.2H2O  (6)  at  15°. 


(Schwicker,  1889.) 


POTASSIUT3  FluoTITANATE  K2TiF6.H2O. 

SOLUBILITY  IN  WATER.     (Marignac,  1866.) 

t°.  o°.  3°.  6°.  10°.  14°.  20°. 

Gms.  K2TiF6  per  ioo  gms.  H20    0.55    0.67     0.77     0.91     1.04     1.28 

POTASSIUM  VANADATE  K3V5O14.5H2O. 

ioo  gms.  H2O  dissolve  19.2  gms.  at  17.5°.  (Radan.  1889.) 

POTASSIUM   ZINC  VANADATE  KZnV6O14.8H2O. 

ioo  gms.  H2O  dissolve  0.41  gm.  of  the  salt  (Radan). 

PRASEODYMIUM   CHLORIDE  PrCl3. 

SOLUBILITY  IN  WATER,  AQ.  HYDROCHLORIC  ACID  AND  IN  PYRIDINE. 

(Matignon,  1906,  1909.) 
Solvent.  t°.  Sp.  Gr.  Sat.  Sol.  Gms.  per  ioo  Gms.  Sat.  Sol. 

Water  13  1.687  5o.96PrCl3 

Aq.HCl  13  1.574  4i.o5PrCld-7.25HCl 

Pyridine         room  temp.  ...  2.1  PrCls 

PRASEODYMIUM   GLYCOLATE  Pr2(C2H3O3)3. 

One  liter  water  dissolves  3.578  gms.  Pr2(C2H3O3)3  at  20°.    Qantsch  &  Grunkraut,  '12-13.) 

PRASEODYMIUM  MOLYBDATE  Pr2(MoO4)8. 

One  liter  water  dissolves  0.0152  gm.  Pr2(MoO4)3  at  23°  and  0.0143  gms.  at  75°. 

(Hitchcock,  1895. 

PRASEODYMIUM   Double  NITRATES 

SOLUBILITY  AT  16°  IN  CONC.  HNO3  OF 

Salt. 


^=1.325.      (Jantsch,  1912.) 

Gms.   Hydrated 

Formula.  Salt  per  ioo  cc. 

Sat.  Solution. 


Praseodymium  Magnesium  Nitrate 
Nickel 
Cobalt 
Zinc 
Manganese       " 


Ni3 
Co3 
Zn3 
Mn3 


7.70 

9.28 

12.99 

14.69 

23.40 


569         PRASEODYMIUM   OXALATE 

PRASEODYMIUM   OXALATE  Pr2(C2O4)8.ioH2O. 

One  liter  H2O  dissolves  0.00074  Sm-  Pr2(C2O4)3  at  25°.  (Rimbach  and  Schubert,  1909.) 
ioo  gms.  aq.  19.4%  HNO3  (d  =  1.116)  dissolve  1.16  gms.  Pr2(C2O4)3  at  15°. 

(v.  Scheele,  1899.) 
ioo  gms.  aq.  10.2%  HNO3  (d  =  1.063)  dissolve  0.50  gm.  Pr2(C2O4)3  at  15°. 

Cv.  Scheele,  1899.) 

PRASEODYMIUM  Dimethyl  PHOSPHATE  Pr2[(CH3)2PO4]6. 

IOO  gms.  H2O  dissolve  64.1  gm.  Pr2[(CH3)2PO4]e  at  25°.      (Morgan  and  James,  1914.) 

PRASEODYMIUM   SULFATE  Pr2(SO4)3. 

SOLUBILITY  IN  WATER.      (Muthmann  and  Rolig,  1898.) 

Solid 
Phase. 

Pr2(S04)3.8H20 
Pr2(S04)3.8H20  + 
Pr2(S04)3.5H20 


PRASEODYMIUM  SULFONATES 

SOLUBILITY  IN  WATER. 


Gms.  Pr2(SO4)3 
t  "                  per  ioo  Gms. 

Solid          +  o 
Phase.             ' 

Gms.  Pr2(SO4)s 
per  loo^Gms. 

Solution. 

Water. 

Solution. 

Water. 

0 

I6.S 

19.8 

Pr2(S04)3.8H20  75 

4-0 

4-2 

18 

12-3 

I4.I 

8S 

J-5 

i-55 

35 

9-4 

10-4 

" 

55 

6,6 

7-1 

95 

I.O 

1.  01 

Praseodymium  Salt  of: 
Bromonitrobenzene  Sulfonic  Acid 

Benzene  Sulfonic  Acid 
m  Nitrobenzene  Sulfonic  Acid 
m  Chlorobenzene  Sulfonic  Acid 
Chloronitrobenzene  Sulfonic  Acid 

a  Naphthalene  Sulfonic  Acid 

1.5  Nitronaphthalene  Sulfonic  Acid 

1.6 

1.7 


Formula. 

Pr(C6H3.Br.N02.S03)i,4,2)s.- 

8H2O 

Pr(C6H6S03)3.9H20 
Pr[C6H4(N02)S03]3.6H2O 
PrICeH4Cl.S03j3.9H20 
Pr  (C6H3.SO3.NO2.Cl,i  ,3,6)3.- 

i4H2O 
Pr[C10H7S03]3.6H20 

,.  6B,O 
.  9H20 
.nH2O 


Gms.  Anhy- 
drous Salt 
per  ioo  Gms. 

H20. 

6 . 08  (Katz&  James,  '13.) 


Authority. 


55-6 
33-9 
12.6 

25-9 

6.1 

0.47 

0.18 


(Holmberg,  1907.) 


PRASEODYMIUM   TUNGSTATE  Pr2(WO4)3. 

One  liter  water  dissolves  0.0438  gm.  Pr2(WO4)3  at  75°. 

PROPIONIC  ACID   C2H5COOH. 


(Hitchcock,  1895.) 


SOLUBILITY  IN  WATER,  DETERMINED  BY  THE  FREEZING-POINT  METHOD. 

(Faucon,  1910.) 

t°of 
Solidif. 
-17.2 
—  21 


t°  of           Gms.  C2H5COOH       «  ,.  ,  p.. 
Solidif.         per  ioo  Gms.  Sol.        Sohd  Phase' 
-1.33               4.98                       Ice 

—2.60          10.  ii 

-    3.76 

—  6.  10 

-  7.70 

15 
25 
35. 

28 

—  9.20 
-10.80 
—  14.20 

45 
55 
65 

.20 

.88 

Gms.  C2H5COOH 
per  ioo  Gms.  Sol. 
73.48         Ice 

Sl-75 
86.85 
87.65 
89.12 
92.40 
97.22 
IOO 


Solid  Phase. 


+C2HJCOOH 
QHsCOOH 


—  29.10 

—  29.40 
-28.30 

—  26 . 90 
-  23 . 90 

—  19.30 

Additional  data  for  this  system  are  given  by  Tsakalatos  (1914),  Herz  (1917)  and 
Ballo  (1910).  The  last-named  investigator  also  determined  the  composition  of 
the  solid  phases  and  explains  the  abnormal  freezing-point  lowering  on  the  basis  of 
production  of  mix-crystals. 

The  ratio  of  distribution  of  propionic  acid  between  water  and  benzene  was 
found  by  King  and  Narracott  (1909)  to  be  1:0.129  at  room  temperature. 


PROPIONIC  ACID  570 

DISTRIBUTION  OF  PROPIONIC  ACID  BETWEEN  ETHER  AND  AQUEOUS  SALT 

SOLUTIONS  AT    l8°.      (de  Kolossovsky,  191 1.) 
Aq.  Salt  Solution  (2  Mols.  per  Liter).  QHsCOOH  per  100  cc.  of: 


Salt. 

Gms.  Salt  per  100  cc. 

Aq.  Layer  (q). 

Ether  Layer  (q1). 

q'' 

Water  alone 

I.I7O 

2.305 

0.50 

NaCl 

11.69 

0.762 

2-543 

0.30 

MgCl2 

19.05 

0.567 

3.I35 

0.18 

KNO3 

20.22 

0.972 

2.298 

0.42 

KC3H40 

1                                           22.43 

L324 

2.406 

o-55 

P  lodoPROPIONIC  ACID  CH2I.CH2.COOH. 

One  liter  sat.  solution  in  water  contains  80  gms.  CH2I CH2COOH  at  25°. 

(Sidgwick,  1910.) 

One  liter  sat.  solution  in  i  n  aq.  sodium  ft  iodopropionate  contains  126  gms.  at 
25°.  (Sidgwick,  1910.) 

0  PhenylPROPIONIC   ACID  (Hydrocinnamic  Acid)  CH2(C6H6).CH2COOH. 
SOLUBILITY  IN  WATER  AND  IN  AQ.  NORMAL  SODIUM  ft  PHENYLPROPIONATE. 

(Sidgwick,  1910.) 

Gms.  CH2(C6HS)CH2COOH  per  Liter  Solution  at: 

Solvent.  , * > 

11°.  25°. 

Water  4.80          7.5 

i  n  aq.  CH2(C6H6)CH2.COONa  7 . 65       172.5  (liquid  layers  formed) 

SOLUBILITY  OF  ft  PHENYLPROPIONIC  ACID  IN  WATER  AND  IN  ALCOHOLS. 

(Timofeiew,  1894.) 

Gms.  CH2(C,H6)-  Gms.  CH2(C,H5) 

Almhnl                      t°            CHjCOOH  per               Almhnl  t°             CH2COOH  per 

ioo  Gms.  Sat.  100  Gms.  Sat. 

Solution.  Solution. 

Water                        19  0.7  Ethyl  Alcohol  +19.6  77.2 

Methyl  Alcohol     -18.5  55.8  "           "                20  78.8 

-16  57.6  Propyl  Alcohol  -18.5  35 

"           "               o  66.9  "           "  -16  39 

+  19.6  82.8  "           "  +19.6  73.4 

20  83.8  "  "  20  73.9 

Ethyl          "          —18.5          46  Isobutyl  Alcohol       19.6          67.3 

-16  48 

SOLUBILITY  OF  ft  PHENYLPROPIONIC  ACID  IN  SEVERAL  SOLVENTS. 

(Herz  and  Rathmann,  1913.) 

CH2(C«H5)  CH2.COOH  CH2(C6H6)  CH2COOH 

Solvent.  Per  Liter.  Solyent  per  Liter. 

Mols.          Gms.  Mols.          Gms. 

Chloroform  5 . 444    817.2     Tetrachloro  Ethylene    4.725     709 . 2 

Carbon  Tetrachloride    4.604    691.1     Tetrachloro  Ethane        5.430    815.1 
Trichloro  Ethylene        5.140    771.6    Pentachloro  Ethane       5.019    753.4 

P  Phenyl  DibromoPROPIONIC   ACID    C2H2Br2(C6H6)COOH. 

ioo  cc.  sat.  sol.  in  carbon  tetrachloride  contain  o.  124  gm.  acid  at  26°.  (De  Jong,  1909.) 
ioo  cc.  sat.  sol.  in  petroleum  ether  contain  0.072  gm.  acid  at  26°. 

PhenylPROPIOLIC  ACID  C6H6C  :  C.COOH. 

SOLUBILITY  IN  SEVERAL  SOLVENTS.    (Herz  and  Rathmann,  1913.) 

C6H6C:C  COOH  C6HBC:C.COOH 

Solvent.  per  Liter.  Solvent.  per  Liter. 

Mols.         Gms.  Mols.        Gms. 

Chloroform  0.789115.30    Tetrachloro  Ethylene  0.324    47.34 

Carbon  Tetrachloride    0.227     33.16    Tetrachloro  Ethane      0.718104.90 
Trichloro  Ethylene         0.382     55.82     Pentachloro  Ethane     0.410     59.91 

PROPIONIC   ALDEHYDE  C2H5COH. 

ioo  gms.  H2O  dissolve  16  gms.  aldehyde  at  20°.  (Vaubel,  1899.) 


571  PROPIONITRILE 

PROPIONITRILE   C2H5CN. 

SOLUBILITY  IN  WATER. 
Synthetic  method  used.     See  Note,  p.  16.  (Rothmund,  1898.) 

Wt.  per  cent  C2H5CN  in:  Wt.  per  cent  C2H5CN  in: 

*°  '  Aq  C2H6CN  *"•  A^  C2HSCN 

Layer.  Layer.  Layer.  Layer. 

40  10.7  92.1  95                 19.6  78.0 

50  ii. 6  90.5  ioo                 22.4  75.5 

60  12.7  88.5  105                 26.0  72.1 

70  13.2  86.1  no                 32.0  66.5 

80  14-9  83.4  113 .1  (crit.  temp.)  48.3 

90  17.6  80.2 

PROPYL    ACETATE,    Butyrate   and   Propionate. 

SOLUBILITY  OF  EACH  IN  AQUEOUS  ALCOHOL  MIXTURES. 

(Bancroft  —  Phys.  Rev.  3,  205,  '95,  calc.  from  Pfeiffer.) 


cc.  Alco- 
hol in 

P.  Ace- 

P. Butyr 

P.  Propio- 

cc. Alco- 
hol in 

P.  Ace- 

P. Buty- 

P. Propio- 

Mixture. 

tate. 

rate. 

nate. 

Mixture. 

tate. 

rate. 

nate. 

3 

4-5° 

I.I9 

I.58 

21 

58-7I 

19.68 

27.83 

6 

10.48 

3-55 

4.70 

24 

00 

23.72 

33-75 

9 

17.80 

6.13 

8-35 

30 

32.10 

47-15 

12 

26.00 

9-o5 

12.54 

36 

41-55 

63.18 

15 

35-63 

12.31 

17-15 

42 

51  .60 

83-05 

18 

47-50 

15.90 

22.27 

48 

62  .40 

107.46 

54 

73  85 

*  cc.  H2O  added  to  cause  the  separation  of  a  second  phase  in  mixtures  of  the  given  amounts  of  alcohol 
and  3  cc.  portions  of  propyl  acetate,  butyrate  and  propionate 

SOLUBILITY  OF  PROPYL  ACETATE,  FORMATE,  AND  PROPIONATE  IN  WATER. 

100  cc.  H2O  dissolve  1.7  gms.  propyl  acetate  at  22°.  (Traube,  1884.) 

100  cc.  H2O  dissolve  2.1  gms.  propyl  formate  at  22°. 

100  cc.  H2O  dissolve  0.6  cc.  propyl  propionate  at  25°.  (Bancroft,  1895.) 

PROPYL   ALCOHOL  C3H7OH. 

Freezing-point  data  (solubilities,  see  footnote,  p.  i)  for  mixtures  of  propyl 
alcohol  and  water  are  given  by  Pickering  (1893).  Results  for  mixtures  of  iso- 
propyl  alcohol  and  water  are  given  by  Dreyer  (1913). 

100  gms.  sat.  solution  of  propyl  alcohol  in  liquid  carbon  dioxide  contain  36.5 
gms.  C3H7OH  at  —24°  and  57.5  gms.  at  —30°.  (Buchner,  1905-06.) 

MISCIBILITY  OF  PROPYL  ALCOHOL  WITH  MIXTURES  OF  CHLOROFORM  AND 

WATER  AT  o°. 

(Bonner,  1910.) 
See  Notes,  pp.  14  and  287. 

Composition  of  Homogeneous  Mixtures.  Composition  of  Homogeneous  Mixtures. 


Gms.  CHC13. 

Gms.  H2O. 

Gms. 
C3H7OH. 

Sp.  Gr.  of 
Mixture. 

Gms.  CHC13. 

Gms.  H2O. 

Gms. 
C3H7OH. 

Sp.  Gr.  of 
Mixture. 

0.977 

O.O23 

0.304 

1.28 

0.500 

0.50 

1-34 

0.97 

0.926 

0.074 

0.631 

I-I3 

0-394 

0.6o6 

1.32 

0.98 

0.90 

0.10 

0.76 

I  .11 

0.293 

0.707 

1-235 

0.96 

0.80 

0.20 

1.  06 

1.04 

0.194 

0.8o6 

0.996 

°-95 

0.70 

0.30 

I  .20 

1.  01 

0.097 

0.903 

0.672 

0.97 

0.60 

0.40 

1.30 

0.98 

0.030 

0.97 

0-39 

0.97 

PROPYL  ALCOHOL 


572 


MISCIBILITY  OF  PROPYL  ALCOHOL  AT  o°  WITH  MIXTURES  OF: 


Carbon  Tetrachloride  and  Water. 

(Bonner,  1910.) 
Composition  of  Homogeneous  Mixtures. 


Ethyl  Bromide  and  Water. 

(Bonner,  1910.) 
Composition  of  Homogeneous  Mixtures. 


Cms.  CC14. 

Cms.  H2O. 

Cms. 
C3H7OH. 

Sp.  Gr.  of 
Mixture. 

Cms. 
C2HBBr. 

Cms.  H2O. 

Cms. 
C3H7OH. 

Sp.  Gr.  of 
Mixture. 

o-975 

0.025 

0.317 

I-3I 

0.941 

0.039 

0.367 

I.  21 

0.931 

0.069 

0.536 

I.I7 

0.912 

0.088 

0.615 

I.  II 

0.90 

O.IO 

0.65 

I.I4 

0.90 

O.  IO 

0.64 

I.IO 

0.80 

0.2O 

0.949 

1.07 

0.80 

0.2O 

0.85 

1-05 

0.70 

0.30 

I.  12 

1  .02 

o.  70 

0.30 

I 

I.  O2 

0.60 

0.40 

I.  20 

0.99 

0.6o 

0.40 

1.09 

I 

0.499 

0.501 

1-234 

0.98 

0.491 

0.509 

I.I24 

0.98 

0.40 

O.60 

I-I95 

0-97 

0.40 

0.60 

I.  10 

0.97 

0.30 

0.70 

I.I3 

0.96 

,0.30 

0.70 

0.90 

0.96 

*0.25 

0-75 

I.  06 

0.20 

0.80 

0.81 

0.96 

0.194 

0.806 

0.912 

0.96 

o.  14 

0.86 

0.671 

0.96 

O.  IOO 

0.90 

0.68 

0.96 

O.IO 

0.90 

0.56 

0-97 

0.013 

0.987 

0-354 

0.96 

*0.023 

0.977 

0.227 

0.99 

See  Notes,  pp.  14  and  287. 

MISCIBILITY  OF  PROPYL  ALCOHOL  AT  o°  WITH  MIXTURES  OF: 
Bromobenzene  and  Water.    (Bonner,  1910.)      Bromotoluene  and  Water.  (Bonner,  1910.) 

Composition  of  Homogeneous  Mixtures.  Composition  of  Homogeneous  Mixtures. 


Gms.  C6H6Br. 

Gms.  H2O. 

Gms. 
C3H7OH. 

Sp.  Gr.  of 
Mixture. 

Gms. 
C6H4CH3Br. 

Gms.  H2O. 

Gms. 
C3H7OH. 

Sp.  Gr.  of 
Mixture. 

0.983 

O.OI7 

0.186 

1.29 

0.968 

0.032 

0.252 

1.23 

0.909 

0.091 

0.56 

I.  II 

0.90 

O.  IO 

0.52 

I.  II 

0.90 

O.IO 

0.58 

I.  II 

0.80 

0.20 

0.78 

1.03 

0.80 

0.20 

0.87 

1.05 

0.70 

0.30 

0.96 

I.  01 

0.70 

0.30 

1.05 

1  .02 

0.6o 

0.4O 

1.07 

0.99 

0.60 

O.40 

I-I5 

I 

0.50 

0.50 

I-I3 

0.97 

0.50 

0.50 

I.I9 

0.97 

0.40 

0.60 

I-I3 

0.96 

0.40 

0.60 

I.I9 

0-97 

0.30 

O.7O 

1.03 

0-95 

0.30 

0.70 

1.09 

0-95 

*0.25 

0-75 

0.97 

O.  20 

0.80 

0-93 

0-95 

0.  20 

0.80 

0.90 

0.94 

O.  IO 

0.90 

0.71 

0.96 

O.IO 

0.90 

0.72 

0-95 

0.021 

0.979 

o-457 

0.98 

0.013 

0.987 

0.424 

0.96 

See  Notes,  pp.  14  and  287. 

DISTRIBUTION  OF  PROPYL  ALCOHOL  BETWEEN  WATER  AND  COTTON-SEED 

OIL  AT  25°. 

(Wroth  and  Reid,  1916.) 


Oil  Layer. 
1.447 

1-475 
1-503 

H2O  Layer. 
8.  112 

8.897 
9.809 

5-60 

6.  10 
6-53 

Oil  Layer. 
I.5l6 
I-576 
1.694 

H2O  Layer. 
10.07 
10.49 
10.41 

6.64 
6.65 

6.  14 

Data  for  systems  composed  of  normal  propyl  alcohol,  water  and  various  in- 
organic salts  are  given  by  Timmermans,  1907. 

PROPYLAMINE  CH3.CH2.CH2.NH2. 

The  solubility  of  propylamine  in  water  at  60°,  determined  by  an  aspiration 
method  using  an  indifferent  gas,  is  191  when  expressed  in  terms  of  the  Bunsen 
absorption  coefficient  0  (see  p.  227)  and  /6o  =  233  when  expressed  in  terms  of  the 
Ostwald  solubility  expression.  (Doyer,  1890.) 


573 


PROPYL  AMINES 


Freezing-point  data  for  mixtures  of  propylamine  and  water,  isopropylamine 
and  water  and  for  dipropylamine  and  water  are  given  by  Pickering  (1893). 


DISTRIBUTION  OF  PROPYLAMINES  BETWEEN  WATER  AND  TOLUENE. 

(Moore  and  Winmill,  1912.) 


Results  at  18°. 


Amine. 


Gm.  Equiv. 

Amine  per 

Liter  of  Aq. 

Layer. 

Propylamine       o .  0973 

"  0.0928 

Dipropylamine  o .  0764 

0.0794 

Tripropylamine  0.0003 


Partition 
Coef. 


434 

439 


0.1185 
0.1188 
0.003 


Partition 
Coef. 


Results  at  25°. 

Gm.  Equiv. 

Amine  per 

Liter  of  Aq. 

Layer. 

0.03837 

o . 04300 

O.O722 

0.0681 


4.470 
4.470 
0.0769 
0.0771 


Results  at  32.35°. 

Gm.  Equiv. 

Amine  per 

Liter  of  Aq. 

Layer. 

o . 0602 

0.0578 


O. OIl68 
O.OII99 


Partition 
Coef. 


3-3I7 

0.05802 

0-05795 


PROPYLAMINE  HYDROCHLORIDE  a  NH2(C3H7).HC1. 

100  gms.  H2O  dissolve  278.2  gms.  NH2(C3H7).HC1  at  25°.      (Peddle  and  Turner,  1913.) 
100  gms.  CHC13  dissolve  5.26  gms.  NHi(C3H7).HCl  at  25°.    (Peddle  and  Turner,  1913.) 

DiPROPYL  AMINE   HYDROCHLORIDE  NH(C3H7)2.HC1. 

IOO  gms.  H2O  dissolve  165.3  Sms-  NH(C3H7)2.HC1  at  25°.        (Peddle'and  Turner,  1913.) 
100  gms.  CHC13  dissolve  47.24  gms.  NH(C3H7)2.HC1  at  25°.  (Peddle  and  Turner,  1913.) 


PROPYL   CHLORIDE,  Bromide,  etc. 

SOLUBILITY  IN  WATER. 

(Rex,  1906.) 


Propyl  Compound. 

CH3CH2CH2C1  (normal) 
CH3CH2CH2Br       " 
CH3CH2CH2I 
(CH3)2CHC1  (iso) 
(CH3)2CHBr    « 
(CH3)2CHI      « 


Grams  P.  Compound  per  100  Gms.  HjO  at: 


0°. 

10°. 

20°. 

30°. 

0.376 

0.323 

0.272 

0.277 

0.298 

0.263 

0.245 

0.247 

0.114 

0.103 

O.IO7 

0.103 

0.440 

0.363 

0.305 

0.304 

0.418 

o-365 

0.318 

0.3l8 

0.167 

0.143 

O.I4O 

0.134 

PROPYLENE  C8H6. 


SOLUBILITY  IN  WATER. 

(Than,  1862.) 


t".  ft.  q. 

o  0.4465  0.0834 

5  0.3493  0.06504 

10  0.2796  0.0519 

15  0.2366  0.0437 

20  0.2205  0.0405 

For  values  of  /3  and  q,  see  Ethane,  p.  285. 


PYRENE  C16H10 

SOLUBILITY  IN  TOLUENE  AND  IN  ABSOLUTE  ALCOHOL. 

100  gms.  toluene  dissolve  16.54  Sms-  pyrene  at  18°. 

100  gms.  absolute  alcohol  dissolve  1.37  gms.  pyrene  at  10°  and  3.08  gms.  at 
b.  pt. 


PYRIDINE 


574 


PYRIDINE  CH  <  (CH.CH)2  >  N. 

SOLUBILITY  IN  WATER,  DETERMINED  BY  THE  FREEZING-POINT  METHOD. 

(Average  curve  from  results  of  Pickering  (1893)  and  Baud  (1909.) 


t'.of 
Solidi- 
fication. 

Gms. 
C5H6N  per 
100  Gms. 
Mixture. 

Solid 
Phase. 

0 

0 

Ice 

—  I 

7-5 

" 

—  2 

i7 

" 

-3 

28 

u 

-4 

37-5 

" 

-5 

43-5 

" 

-6 

48 

« 

Q 

54 

" 

Gms. 
C6H6Nper  Solid 


J.G  nt 


Gms. 
C*H*N  Per 


Solid 

phase- 


— 10 

—  12. 

-15 

—  20 

-25 
-30 
-40 
-50 


58 
62 
64 

68 
7i 
73 
78 
81 


5       Ice 


-60 

-65  Eutec. 

-60 

-55 
-50 

-45 

-40 


84 
85 
87 
89 
92 

95 

97 


Ice 


+CtHjN 


—  38  m.  pt.  100 


Timmermans  (1912)  is  reported  to  have  made  determinations  on  the  above 
systems  but  the  original  paper  could  not  be  located. 

Baud  also  gives  data  for  the  densities  of  pyridine  +  water  mixtures. 

DISTRIBUTION  OF  PYRIDINE  BETWEEN  WATER  AND  BENZENE. 


At  Room  Temperature. 

(v.  Georgievics,  1915.) 
Gms.  CSH5N  per 


At  25°. 

(Hantzsch  and  Sebaldt,  1899.) 
Mols.  C8H5N  per  Liter. 


25  cc.  H2O  Layer. 
0.0617 
0.0958 
0.1549 
0.2432 
0.3297 
0.723 
1. 147 


75  cc.  CeH6  Layer. 

0.4733 
0.7631 
1.2249 
2.0096 
2.6553 
5-4I59 
9.878 


Aq.  Layer. 

C6H6  Layer. 

rs.ai.io. 

O.OOI48 

0.00436 

0-339 

0.00076 

0.00226 

0-339 

0.00038 

O.OOIIO 

0-345 

O.OOO2O8 

O.OOO546 

0.381 

O.OOOII2 

0.000274 

0.413 

(at 

5.5°)   0.000456 

O.OOO928 

0.491 

(at 

50°)    O.OOO3I4 

O.OOIO88 

0.289 

DISTRIBUTION  OF  PYRIDINE  BETWEEN  WATER  AND  TOLUENE. 

(Hantzsch  and  Vagt,  1901.) 

At  25°. 

er  Liter. 

Ratio. 

0.458 
0.466 
0.481 
0.496 

0.551 
0.629 
0.647 
0.696 

Data  for  systems  composed  of  py 
given  by  Timmermans,  1907. 

Methyl  PYRIDINES 

Data  for  the  reciprocal  solubility  of  3  methyl  pyridine  { =  0  picoline)  and 
water,  2.6  dimethyl  pyridine  (=  2.6  lutidine)  and  water,  methyl  pyridine  (=7 
picoline)  zinc  chloride  and  water,  methyl  pyridine  zinc  chloride  and  each  of  the 
following  alcohols;  methyl,  ethyl,  propyl,  isobutyl,  isoamyl,  cetyl  and  methyl 
hexylcarbinol,  determined  by  the  synthetic  method  (see  Note,  p.  16),  are  given  by 
'Flaschner  (1909).  See  also  p.  262,  for2.4.6trimethyl  pyridine  (collidine)  and  water. 


Mols.  C6HBN  per  Liter. 

Aq.  Layer. 

C«H&CH3  Layer. 

0.0517 
0.026l 

O.II29 
0.0559 

O.OI32 
0.0067 
0.0033 

0.0275 
0.0137 
0.0066 

O.OOI9 

O.OO34 

O.OOII 

0.0017 

0.0007 

0.0010 

At  Various  Temperatures. 
Mols.  C5H5N  per  Liter. 
t°                                 *                                 Ratio 

Aq.  Layer.  C6H5CH3  Layer. 

0 

0.0168 

O.O2OI 

0.840 

10 

0.0135 

0.0215 

0.627 

20 

O.OIII 

0.0228 

0.529 

30 

0.0108 

0.0234 

0.461 

40 

O.OIOI 

0.0245 

0.411 

50 

0.0096 

0.0252 

0.380 

70 

0.0085 

0.0263 

0-324 

90 

0.0082 

0.0266 

0.307 

e,  water  and  various  inorga: 

nic  salts  are 

575 


PYRIDINE 


PYRIDINAMINO   SUCCINIC  ACIDS. 

100  gms.  H2O  dissolve  1.67  gms.  of  the  d  compound,  1.64  gms  of  the  /  com- 
pound and  1.68  gms.  of  the  dl  compound  at  18°.  (Lutz,  1910.) 

PYROCATECHOL  o  C6H4(OH)2. 

100  gms.  H29  dissolve  45.1  gms.  C6H4(OH)2  at  20°.  (Vaubel,  1899.) 

100  gms.  pyridine  dissolve  an  unlimited  amount  of  CeH^OH^  at  20°.  (Dehn,  1917.) 
100  gms.  aq.  50%  pyridine  dissolve  101  +  gms.  of  CeH^OH^  at  20-25°.       " 
F.-pt.  data  for  pyrocatechol  +  resorcinol  are  given  by  Jaeger  (1907). 

PYROGALLOL  C6H3(OH)3  i,  2,  3. 

SOLUBILITY  IN  WATER,  ETC. 

(U.  S.  P.  VIII.) 


ioo  gms.  water  dissolve  62.5  gms.  C6H3(OH)3  at  25°^. 
100  gms.  alcohol  dissolve  ioo  gmi 
ioo  gms.  ether  dissolve  90.9  gms. 


ioo  gms.  alcohol  dissolve  ioo  gms.  C6H3(OH)3  at  25°. 

jms.  CeHa(OH),  at  25°. 


Dimethyl  PYRONE  C7H8O2. 

Freezing-point  data  for  mixtures  of  dimethyl  pyrone  and  each  of  the  following 
compounds:  salicylic  acid,  0,  m,  p  and  a  toluic  acids  and  trinitrotoluene  are  given 
by  Kendall  (i9i4a).  Results  for  mixtures  of  dimethyl  pyrone  and  sulfuric  acid 
are  given  by  Kendall  and  Carpenter  (1914). 


QUINHYDRONE 

Data  for  the  solubility  and  dissociation  of  quinhydrone  in  water  at  25°  are 
given  by  Luther  and  Leubner  (1912). 

QUINIDINE  C2oH24N202.  ?H2O. 

SOLUBILITY  IN  SEVERAL  SOLVENTS. 


Solvent.  t°. 

Water  18-22 

Water  25 

Ethyl  Alcohol  (95%)  20 

Ethyl  Alcohol 

Methyl  Alcohol 

Benzene 

Benzene 

Carbon  Tetrachloride 

Chloroform 

Chloroform 

Ether  (d  =  0.72) 

Ether  sat.  with  H2O 

H2O  sat.  with  Ether 

Ethyl  Acetate 

Pet.  Ether  (b.  pt.  59°-64°) 

i  vol.  C2H5OH+4  vols.  CHCU 

i  vol.  C2H5OH+4  vols.  C6H6 

i  vol.  CH3OH+4  vols.  CHCla 

i  vol.  CH3OH+4  vols. 

QUINIDINE    SALTS 


Gms. 


Gms.  Solvent. 
O.O2O 


I24  N2O2  per  ioo. 
cc.  Solvent. 


Authority. 


25 

25 

25 

1  8-2  2 

2-45 

1  8-2  2 

°-SS7 

18-22 

IOO+ 

25 

1  8-2  2 

0.78 

1  8-2  2 

1.63 

1  8-2  2 

0.031 

1  8-2  2 

1.76 

1  8-2  2 

0.024 

25 

25 

25 

25 

(Mullet,  1903.) 
0.0145    (Schaefer,  1910.) 

(Wherry  &  Yanovsky,  1918.) 
(Schaefer,  1913.) 


22 

66 


33-3 
12.5 

25 
6.6 


(Muller,  1903.) 


(Schaefer,  1913.) 
(Muller,  1903.) 


(Schaefer,  1913.) 


Quinidine  Salt. 
Q.  Hydrobromide 
Q.  Hydrochloride 
Q.  Hydroiodide 
Q.  Salicylate  0.060 


SOLUBILITY  IN  WATER  AT  25°. 

(Schaefer,  1910.) 

Gms.  Salt  per 
loo  Gms.  H2O. 

0.526 

1. 160 

0.082 


Quinidine  Salt. 

Q.  Sulfate 
Q.  Tannate 
Q.  Tartrate 
O.  Bitartrate 


Gms.  Salt  per 
100  Gms.  H2O. 

1.05 

0.0477 

2.86 

0.323 


QUINIDINE   SULFATE 


576 


SOLUBILITY  OF  QUINIDINE  SULFATE  IN  SEVERAL  SOLVENTS  AT  25°. 

(Schaefer,  1913.) 


Solvent. 

Ethyl  Alcohol 
Methyl  Alcohol 
Chloroform 
Benzene 


Cms.  Q.  Sulfate 

per  too  cc. 

Solvent. 

5 
40 

Insol. 


Solvent. 

i  vol.  C2H6OH+4  vols.  CHC13 
i  vol.  C2H5OH+4  vols.  C6H6 
i  vol.  CH3OH+4  vols.  CHCls 
i  vol.  CHaOH+4  vols.  CeH6 


Cms.  Q.  Sulfate 

per  too  cc. 

Solvent. 

33-3 

8-33 
33-3 
20 


QUININE  C2oH24N2O2.3H2O. 


Solvent. 


Water 


Ethyl  Alcohol 


Methyl  Alcohol 
Benzene 


Aniline 

Carbon  Tetrachloride 

Chloroform 

« 

Diethylamine 
Ether 


SOLUBILITY  IN  SEVERAL  SOLVENTS. 


sat.  with  H2O 
H2O  sat.  with  Ether 
Ethyl  Acetate 
Petroleum  Ether  (b. 

pt.  59°-64°) 
Oil  of  Sesame 
Glycerol 
Piperidine 
Pyridine 

Aq.  50%  Pyridine 
7.65gms.H3BO3perioo   room 

cc.  aq.  50%  Glycerol     temp. 
i5.3gms.H3BO3perioo   room 

cc.  aq.  50%  Glycerol    temp. 


Anhydrous  Quinine 
A0              Gms.  per  100. 

Hydrated 
oJU^oo                 Authority. 

Gms.  Solvent. 

Gms. 
Solvent. 

CC. 

Solvent. 

18-22 

0.051 

0.05  74  (Muller,  1903.) 

25 

0.057 

0. 

033 

0.065 

(U.  S.  P.;  Schaefer,  1910.) 

80 

0.123 

0.129 

(U.  S.  P.) 

20 

100 

.  . 

. 

(Wherry  and  Yanovsky,  1918.) 

25 

166.6 

. 

i6o\6 

(U.  S.  P.) 

25 

.  .  . 

1333 

(Schaefer,  1913.) 

2O 

66. 

6 

. 

•'                             .:• 

25 

o. 

55 

0.205 

(Schaefer;  Muller,  1903.) 

2O 

0-5 

. 

(Wherry  and  Yanovsky,  1918.) 

1  8-2  2 

. 

(Muller,  1903.) 

20 

14-5 

. 

(Scholtz,  1912.) 

20 

0-54 

. 

0.204 

(Gori,  1913;  Muller,  1903.) 

25 

50-52.6 

.  . 

. 

62.5 

(Schaefer,  1913;  U.  S.  P.) 

18-22 

100  -f- 

.  . 

. 

loo  + 

(Muller,  1903.) 

20 

57 

.  . 

. 

(Scholtz,  1912.) 

25 

22.2 

.  . 

. 

76.9 

(U.  S.  P.) 

1  8-2  2 

0.876 

.  . 

. 

1.62 

(Miiller,  1903.) 

1  8-2  2 

2.8 

» 

5-62 

" 

1  8-2  2 

0.085 

0.067 

" 

1  8-2  2 

24-7 

.    - 

4-65 

" 

18-28 

20 

25 

2O 

20 

20-25 


0.021 

0.633 
IIQ 
IOI 

59-4 

20 

40 


O.OIO 

0.053 

0.472 


(Zalai,  1910.) 

(U.  S.  P.;  Ossendowski,  1907.) 

(Scholtz,  1912.) 

(Dehn,  1917.) 

(Baroni  and  Barlinetto,  1911.) 


SOLUBILITY  OF  QUININE  IN  BENZENE,  DETERMINED  BY  THE  SYNTHETIC 
(SEALED  TUBE)  METHOD. 

(van  Iterson-Rotgans,  1914.) 

*"'        Qubint    Solid  Phase. 

53-5  4-8r 

63  6 . 09  Mixed  phase, 

91  30.01       probably  a 

I O2  43  •  4        colloid  or  sol- 

104 .5  45  . 9         ution  of  high 

109  51.8         viscosity. 

130  75.46 

*  Eutec. 


t". 

Wt.  % 
Quinine. 

Solid  Phase. 

5-4 

0 

QH, 

5-3* 

17 

0.72  c 

29 

1.48 

" 

38.5 

2-36 

« 

49 

5.22 

"  unstable 

±70 

28.9 

U               « 

t°. 

<SSL£""  .«— 

137 

80          CajH^NA 

142 

83.04 

146 

85.26 

152 

87.44 

158.5 

91.4 

166 

95-02 

174.7  loo 


577 


QUININE 


SOLUBILITY  OF  QUININE  IN  AQUEOUS  SOLUTIONS  OF  CAUSTIC  ALKALIES. 

(Doumer  and  Deraux,  1895.) 

METHOD.  —  A  one  per  cent  solution  of  quinine  sulfate,  containing  a  very 
small  amount  of  HC1,  was  gradually  added  to  200  cc.  portions  of  the  caustic 
alkali  solutions  of  the  various  concentrations  stated,  and  the  point  noted  at  which 
a  precipitate  of  the  appearance  corresponding  to  that  of  I  cc.  of  milk  in  100  cc. 
of  water,  remained  undissolved. 

In  Aq.  Ammonia.          In  Aq.  Sodium  Hydroxide.      In  Aq.  Pot.  Hydroxide. 


Gms.  NH3    Gms.  Anhydrous 

Gms.  NaOH 

Gms.  Anhydrous 

Gms.  KOH 

Gms.  Anhydrous 

per  200  cc. 
Solution. 

Quinine 
Dissolved. 

per  200  cc. 
Solution. 

Quinine 
Dissolved. 

per  200  cc. 
Solution. 

Quinine 
Dissolved. 

0.52 

0.084 

0.007 

0.092 

0.612 

0.088 

0.65 

0.084 

O.OI2 

0.091 

I.5I2 

0.082 

4-59 

0.096 

0.740 

0.090 

3-456 

0.068 

13.08 

0.122 

2.l6o 

0.079 

10.944 

0.039 

18.88 

0.144 

3-188 

0.056 

44.704 

0.006 

25.19 

0.174 

6.  172 

0.044 

35-79 

0.184 

8-537 

O.O2I 

17.074 

0.015 

SOLUBILITY  OF  QUININE  SALTS  IN  WATER. 

(Regnault  and  Willejean,  1887.) 


Salt. 

Brom  Hydrate  (basic) 
"  (neutral) 


Chlor  Hydrate  (basic) 


Lactate  (basic) 


AO       Gms.  Salt  per 
'     100  Gms.  H2O. 

14 

2.06 

12 

12.33 

14 

16 

13-19 
14-79 

15 

12 

14.20 
3-8o 

14 

4.14 

15 

4-25 

15 

37 

10.03 
16.18 

Salt. 

j-o          Gms.  Salt  per 
too  Gms.  H2O. 

Salicylate  (basic) 

15              0.114 

Sulfate           " 

14              0.139 

«               a 

16              0.153 

tt               « 

18             0.160 

"       (neutral) 

15             8.50 

«             « 

17             8.90 

«             « 

18            9.62 

Valerate  (basic) 

12-16       2.59 

SOLUBILITY  OF  QUININE  SALTS  IN  WATER  AT  25°. 

(Schaefer,  1910.) 


Salt. 

Gms.  Salt  per 
100  Gms.  H2O. 

Acetate 

2 

Anisol 

0.042 

Arsenate 

0.154 

Benzoate 

0.278 

Bihydrobromide 

20 

Bihydrochloride 

143  (133) 

Bihydrochloride  +  Urea 

100 

Bisulfate 

11.78 

Chlorhydrosulfate 

77  (So) 

Chromate 

0.032 

Citrate 

O.  121   (0.083) 

Glycerophosphate,  basic 

o.  1178  (insol.) 

Hydrobromide 

2-33 

Hydrochloride 

4.76 

Hydroferrocyanide 

0.05 

Hydroiodide 

0.49 
*  Insol. 

Salt. 

Gms.  Salt  per 
100  Gms.  H2O 

Hypophosphite 

2.85 

Lactate,  basic 

16.6 

Nitrate 

T-43 

Oxalate 

0.071 

Phosphate 

0.125 

Picrate 

0.029 

Quinate 

.    28.6 

Salicylate 

0.048 

Sulfate 

0.143 

Bisulfoguiacolate 

200 

Sulfophenate 

0.4 

Urate 

O.l82 

Phenylsulfate 

0.147 

Tartrate 

o.  105 

Tannate 

o.o5(*) 

Valerate 

1.25 

It  is  pointed  out  that  different  values  for  the  solubility  may  be  obtained  de- 
pending on  the  method  used  for  preparing  the  saturated  solution. 

Results  in  parentheses  are  by  Squire  and  Caines  (1905),  and  are  for  I5°-2O° 
instead  of  25°. 


QUININE   SALTS 


578 


SOLUBILITY  OF  QUININE  SALTS  IN  SEVERAL  SOLVENTS. 

(Phelps  and  Palmer,  1917-) 

Solubility,  Parts  per  100  Parts  Solvent  in: 


Salt. 

M.  pt. 

(uncorr.) 

ecu.      ( 

CHC13.         Ethyl  Acetate  (Alcohol  free)  . 

\lcoholfree).        Cold.                    Hot. 

Quinine  racemic  lactate    165  .  5 

0.00715 

28.6                 0.286               3.33 

d  lactate 

175 

O.OIII 

0.25 

/ 

171 

0.00476 

O.2O 

formate 

IIO-II3 

0.00625 

...                      ...                         ... 

acetate 

124-126 

0.05 

...                      ...                         ... 

propionate 

IIO-III 

0.238 

...                      ...                         ... 

butyrate 

77-5 

4 

...                      ...                         ... 

succinate 

192 

O.OOI 

0.4 

tartrate 

202.5 

0.0004 

...                      ...                     0.0333 

malate 

177-5 

0.0008 

0.5 

citrate 

i83-S 

0.00167 

0.0833 

sulfate 

214 

0.0025 

0.0333            0.00715            0.0133 

Quintoxime  lactate 

O.  II 

...                      ...                         ... 

Saturation  was  obtained  by  shaking  at  intervals  by  hand,  during  72  hours. 
In  case  of  the  determination  at  "hot,"  the  solutions  were  boiled  under  a  reflux 
condenser  for  18  hours. 


QUININE  HYDROCHLORIDE  C20H24N2O2.HC1.2H2O. 

SOLUBILITY  IN  AQUEOUS  SALT  SOLUTIONS  AT  16°. 

(Tarugi,  1914-) 

The  determinations  were  made  by  adding  an  aqueous  solution  of  quinine 
hydrochloride  to  the  aqueous  salt  solution  until  turbidity  occurred.  From  the 
volumes  involved,  the  solubility  per  100  cc.  was  calculated. 


In  Aq. 

NaCl. 

In  Aq. 

NaNO3. 

In  Aq 

.KC1. 

In  Aq 

.  CaCl2. 

Gms.  per  100  cc.  Sol.   - 

Gms.  per 

100  CC.  Sol. 

Gms.  per  100  cc.  Sol. 

Gms.  per 

TOO  cc.  Sol. 

'  NaCl. 

Q.HCl.' 

NaN03. 

Q.HCl.  ' 

'   KC1. 

Q.HCl. 

'CaClj. 

Q.HCl. 

2.02 

2.6 

0.677 

2-85 

2.63 

2-545 

6-37 

1.028 

2.49 

1.94 

0.970 

1.96 

3 

1.882 

7-03 

0.951 

3-40 

1.22 

2.008 

0.67 

5-57 

0.804 

7-75 

0.879 

8-34 

0-54 

3-65 

o-43 

8.26 

o.53i 

7.96 

0.765 

11.40 

0.205 

9-31 

o.  292 

10.42 

0.407 

34-42 

0.183 

I5-56 

o.  140 

19.  12 

0.168 

17.87 

0.205 

y 

19.83 

0.085 

3I-78 

0.0663 

25-74 

0.0997 

(Squire  and 
Caines, 
1905-) 


100  cc.  90%  alcohol  dissolve  20  gms.  Q.  bihydrochloride  at  I5°-2O°. 
chloroform         "        14.3    " 

90%  alcohol       "        14.3    "    Q.hydrochlorosulfateati5°-20°. 
0-5    "    Q-  glycerophosphate  at  I5°-2O°. 
100  gms.  H2O  dissolve  1.3  gms.  anhydrous  Q.  glycerophosphate  at  100°. 

(Rogier  and  Fiore,  1913.) 

QUININE   SALICYLATE  CMH24N2O2,C6H4(OH)COOH.2H2O. 
SOLUBILITY  IN  AQUEOUS  ALCOHOL  AT  25°. 

(Seidell,  1909,  1910.) 


Wt.  % 
C2HBOH 
in  Solvent. 

da  Of 

Sat.  Sol. 

Gms.  Q.  Sal. 
2H2O  per  100 
Gms.  Sat.  So) 

o 

0.999 

0.065 

IO 

0.982 

0.080 

20 

0.966 

0.  20O 

30 

0.952 

0.48 

40 

0.935 

i 

50 

0.916 

1.70 

Wt.  % 
C2H8OH 
in  Solvent. 

&*  of 
Sat.  Sol. 

Gms.  Q.  Sal. 
2H2O  per  loo 
Gms.  Sat.  Sol. 

60 

0.896 

2-45 

70 

0.876 

3-25 

80 

0.854 

4.20 

90 

0.832 

4.71 

92.3 

0.826 

4.62 

100 

0.797 

3-15 

579  QUININE   SULFATE 

SOLUBILITY  OF  QUININE  SULFATE  IN  SEVERAL  SOLVENTS  AT  25°. 

»(Schaefer,  1913.) 
s  .  Cms.  Q.  Sulfate  Solvent  Cms.  Q.  SuUate 

bolvent.  per  1QQ  cc  Solvent.  per  100  cc.  Solvent. 

Ethyl  Alcohol  0.4  i  vol.  C2H5OH+4  vols.  CHC13  12.5 

Methyl  Alcohol  3.12  i  vol.  C2H6OH+4  vols.  CeHe  o .  53 

Chloroform  0.27  i  vol.  CH3OH+4  vols.  CHC13  20 

Benzene  insol.  i  vol.  CH3OH+4  vols.  CeHe  4-76 

100  gms.  trichlorethylene  dissolve  0.07  gm.  Q.  sulfate  at  1 5°.    (Wester  and  Bruins,  1914-) 

QUININE   TANNATES  True  and  False 

SOLUBILITY  IN  WATER  AND  IN  AQUEOUS  HC1  AT  37°.    (Muraro,  1908.) 

Gms.  Q.  Tannate  per  100  Gms. 
Tannate.  Formula.  '  »_   rC7        A.,   .m 

H20.  ?Jci%         HCi 

True  Tannate  I        C2oH24N2O2.CioHi4O9.4H2O  o  0.984      3-656 

True  Tannate  II      (C2oH24N2O2)2.(CioHi4O9)3.8H2O  o  1.210      4.756 

False  Tannate          (C2oH24N2O2.H2SO4)2(C1oH14O9)5.i4H2O    0.313      0.847       1.560 

The  work  of  Muraro  is  criticized  by  Biginelli  (1908). 

IOO  cc.  90%  alcohol  dissolve  33.3  gms.  Q.  tannate  at  I5°-2O°.  (Squire and  Caines,  1905.) 

QUININE  PYROTARTRATES  /,  i,  d. 

SOLUBILITIES  IN  ALCOHOL  AT   18°.      (Ladenburg  and  Herz,  1898.) 

ioo  gms.  alcohol  dissolve  15  gms.  of  the  /  pyrotartrate,  3.2  gms.  of  the  i  and 
4.2  gms  of  the  d  compound.  The  results  show  that  the  i  acid  is  not  a  mixture  of  d 
and  /  acid,  and,  therefore,  that  the  i  quinine  compound  is  a  salt  of  the  racemic  acid. 

SOLUBILITY  OF  QUININE  AND  OF  QUININE  SALTS  IN  WATER  AND  OTHER 
SOLVENTS.     (U.  s.  P.  vm.) 

Gms.  Quinine  Compound  per  ioo  Gms.  Solvent  in: 


Compound.                                 Water.  Alcohol.          Ether.  Chloroform.  Glycerol. 

At  25°.  At  80°.  At  25°.  At  25°.  At  25°.          At  25°. 

C20H24N2O2  0.057  0.123  166.6  22.2  52.6  0.633 

C2oH24N2O2.3H2O  0.065  0.129  166.6  76.9  62.5  0.472 

C2oH24N2O2HC1.2H2O  5-55  250  166.6          0.417  122  12.2 
C20H24.N202.CeH4(OH).- 

COOH.|H2O  1.30  2.86  9.09        0.91  2.70        6.25 

(C20H24N2O2)2.H2SO4.7H2O  0.139  2-22  1-16          ...  0.25        2.78 

C20H24N2O2.H2SO4.7H2O  n-77  *47  5-55        0.056  0.109       5-55 

C20H24N2O2.HBr.H2O  2.5  33.3  149.2          6.2  12.5 

QUINOLINE   ETHIODIDE  C9H7N.C2H5l. 

IOO  gms.  H2O  dissolve  301.3  gms.  C9H7N.C2H5I  at  25°.       (Peddle  and  Turner,  1913.) 
ioo  gms.  CHC13  dissolve  1.78  gms.  C9H7N.C2H6I  at  25°. 

RADIUM   EMANATIONS 

SOLUBILITY  IN  WATER.    (Boyle,  1911;  Kofler,  1913.) 

Solubility.  Solubility. 

L-  , * v  t°.  , * X 

/(Boyle).  a  (Kofler).  /(Boyle).  a  (Kofler). 

o       0.508      0.54          30      0.195       0.205 
5       0.41       0.442          40      0.16        0.165 
10       0.34        0.37  50       ...         0.14 

15         0.29          0.31  60         ...  0.12 

20         0.245         0.265  70         ...  O.II 

25         0.215         0.232  90         ...  0.108 

The  results  of  Boyle  are  in  terms  of  /,  the  Ostwald  Solubility  Expression  (see 

V  —  v   E' 
p.  227).     Those  of  Kofler  are  in  terms  of  the  expression  a  = =,   where 

V  JtL 

V  and  v  are  the  volumes  involved  and  E'  and  E  the  total  amount  of  emanation 
contained  respectively  in  the  air  and  in  the  liquid. 


RADIUM   EMANATIONS 


58o 


SOLUBILITY  IN  SEVERAL  SOLVENTS. 

(Ramstedt,  1911;  Swinne,  1913.) 


Results  at  o". 

Results  at  18°. 

Results  at  14°. 

Solvent. 

(Boyle,  1911.) 

A). 

Sp.  Gr.  of  Sol. 

/18- 

Sp.  Gr.  of  Sol. 

IM 

Water 

0.52 

0.9999 

0.285 

0.9986 

0.30 

Sea  Water 

.  .  . 

.  .  . 

0-255 

Ethyl  Alcohol 

8.'  28 

0.8065 

6.17 

0.7911 

7-34 

Amyl  Alcohol 

9-31 

Acetone 

7-99 

0.8186 

6.30 

0.7972 

Aniline 

4-43 

1.0379 

3-80 

I.O2IO 

•  .  • 

Benzene 

12.82 

0.8811 

Carbon  Bisulfide 

33-4 

1.2921 

23.14 

i  .  2640 

Chloroform 

20.5 

1.5264 

15.08 

1.4907 

... 

Cyclohexane 

18.04 

0.7306 

. 

Ethyl  Acetate 

9.41 

0.9244 

7-34 

0.9029 

... 

Ethyl  Ether 

20.9 

0.7362 

15.08 

0.7158 

Glycerol 

.  .  . 

O.2I 

i.  262 

...   • 

Hexane 

23-4 

0.6769 

16.56 

0.6612 

.  .  . 

Toluene 

18.4 

0.8842 

13.24 

0.8666 

13-7 

The  above  results  are  in  terms  of  the  Ostwald  Solubility  Expression  (see  p.  227). 


RESORCINOL 

C6H4(OH)2 

!»  3- 

SOLUBILITY  IN: 

Water. 

Ethyl  Alcohol. 

(Speyers  —  Am.  J.  Sci.  [4] 

14,  294,  '02.) 

(Speyers.) 

to          Sp.Gr.of    Gms.C6H4(OH)2penooGms.         So.Gr.of 

Gms.  CeH4(OH)2  per  100  Gms. 

solutions 

•    *       Water. 

Solution.                    Solutions. 

Alcohol. 

Solution. 

0 

.101 

60 

37-5               1-033 

2IO 

67.8 

10 

.118 

81 

44-8 

•036 

223 

69.0 

20 

•134 

103 

5o-7 

.041 

236 

70-3 

25 

.142 

117 

53-9 

•045 

243 

70.8 

30 

.148 

56.7 

.048 

250 

71.4 

40 

•J57 

161 

.056 

266 

72.7 

50 

.165 

198 

66.5 

•065 

286 

74-1 

60 

.172 

246 

71.1 

•075 

311 

75-7 

70 

1.176 

320 

76.2 

.087 

34i 

77-3 

80 

I.I79 

487 

82.9 

.104 

375 

78-9 

NOTE.  —  The  original  results  of  Speyers  are  given  in  terms  of  mols.  per  100 
mols.  H2O. 

According  to  Vaubel  (1895),  100  gms.  H2O  dissolve  175.5  gms.  C6H4(OH)2, 
or  100  gms.  sat.  solution  contain  63.7  gms.  at  20°.  Sp.  Gr.  of  sol.  =  1.1335. 


SOLUBILITY  OF  RESORCINOL  IN  ALCOHOLS  AND  IN  ACIDS. 

(Timofeiew,  1894.) 

Solvent. 

t°. 

Gms.  C6H4(OH)2  m 
per  100  Gms. 

Solvent. 

t°. 

Gms.  C6H4(OH)2  m 
per  100  Gms. 

Sat.  Sol. 

Sat.  Sol. 

Methyl  Alcohol 

ii.  6 

69 

Formic       Acid 

15 

29.2 

Ethyl 

10.4 

59-2 

Acetic 

15 

32.5 

<<              ii 

ii.  6 

61.5  • 

Propionic      " 

15 

22.8 

Propyl        " 

10.4 

51-5 

Butyric 

i5 

14.7 

<<             « 

ii.  6 

51-6 

Isobutyric     " 

15 

9.6 

« 

Valeric 

15 

6-5 

581  RESORCINOL 

SOLUBILITY  OF  RESORCINOL  IN  BENZENE. 

(Rothmund,  1898.) 

to  Cms.  C6H4(OH)2  j.o  Cms.  CgH^OHJj 

per  100  Cms.  Sat.  Sol.  per  100  Cms.  Sat.  Sol. 

73  3-i8  95.5  61.7 

77  4-75  96.5                 77-64 

82  6.94  83.46  98.5 

95.5  37.44  90.23  100 

Between  the  concentrations  37.44  and  61.7  at  95.5°  two  liquid  layers  are 
formed.  The  reciprocal  solubilities  of  these  two  layers,  determined  by  the 
synthetic  method  (see  Note,  p.  16),  are  as  follows: 

Cms.  C6H4(OH)2  per  100  Cms.  Gms.  CjH4(OH)2  per  100  Cms. 


60 
70 
80 

C6Hg  Layer. 

4.8 
6.6 
9.2 

C6H4(OH)2  Layer. 

79-4 
77-5 
75 

90 

IOO 

105 

C6Hg  Layer. 
13 
19-5 
24.6 

C6H4(OH)2  Layer. 
71-3 
65.7 
60.7 

109.3  cnt-  temp.     42.4 

Resorcinol  mixes  with  pyridine  in  all  proportions.  (Dehn,  1917.) 

loo  gms.  aqueous  50%  pyridine  dissolve  901  gms.  C6H4(OH)2wat2O0-25°. 
IOO  cc.  olive  oil  dissolve  4.55  gms.  C6H4(OH)2  m  at  I5°-2O°.  (Squire  and  Caines,  1905.) 
The  coefficient  of  distribution  of  resorcinol  at  25°  between  olive  oil  and  water 

(cone,  in  oil  -5-  cone,  in  H2O)  is  given  as  0.04  by  Boeseken  and  Waterman  (1911, 

1912). 
Freezing-point  data  (solubility,  see  footnote,  p.  i),  for  mixtures  of  resorcinol 

and  p  toluidine  are  given  by  Philip  and  Smith  (1905)  and  by  Vignpn  (1891). 

Results  for  mixtures  of  resorcinol  and  m  xylene  are  given  by  Campetti  (1917). 

DISTRIBUTION  OF  RESORCINOL  BETWEEN  WATER  AND  ORGANIC 
SOLVENTS  AT  ORDINARY  TEMPERATURE. 

(Vaubel  —  J.  pr.  Ch.  [2]  67,  4?8,  '03.) 
Gms.  Gms.  CaH4(OH)  in: 


Solvents.  Organic 

Used.  H20  Layer,     g^^*  Layer 


1.191  60  cc.  H2O+  30  cc.  Ether  0.2014  0.9896 

1.191  60  cc.  H2O-f  60  cc.  Ether  0.2475  0.9525 

0.800  40  cc.  H2O  +  40  cc.  Benzene  °-5^73  0-2127 

0.800  40  cc.  H2O-f  80  cc.  Benzene  0.5773  0.2227 

0.500  50  cc.  H2O+   50  cc.  CC14  0.4885  0.0115 

0.500  50  cc.  H2O+ioo  cc.  CC14  0.4880  0.0120 

0.500  50  cc.  H2O+i5o  cc.  CC14  0.4880  0.0120 

RHODIUM    SALTS.     SOLUBILITY  IN  WATER. 

(Jorgensen  —  J.  pr.  Ch.  [2]  27,  433,  '83;  34,  394,  '86;  44,  SL  '91-) 
Salt.  Formula 

Chloro  Purpureo  Rhodium  Chloride  ClRh(NH3)5Cl2  17  0.56 

Luteo  Rhodium  Chloride                    Rh(NH3)6Cl3  8  13.3 

Luteo  Rhodium  Nitrate                       Rh(NH3)6(NO3)3  ord.  t  2.1 

Luteo  Rhodium  Sulphate                   [Rh(NH3)6]2(SO4)3.5H2O  20  2.3 

ROSANILINE  C20H21N3O. 

IOO  gms.  H2O  dissolve  0.03  gm.  CaoH^NaC^  at  2O°-25°.  (Dehn,  1917.) 

loo  gms.  pyridine  dissolve  41.5  gms.  C2oH2iN3O4  at  2O°-25°.  " 

100  gms.  aq.  50%  pyridine  dissolve  35.1  gms.  C2oH2iN3O4  at  2O°-25°.         " 


ROSANILINE  582 

Triphenyl  p  ROSANILINE  HYDROCHLORIDE 

SOLUBILITY  IN  SEVERAL  SOLVENTS  AT  23°. 

(v.  Szathmary  de  Szachmar,  1910.) 


Solvent. 


Methyl  Alcohol 

Ethyl 

Amyl 

Acetone 

Aniline 


Cms.  Triphenyl  p 
Rosaniline  HC1  per 
100  Cms.  Sat.  Sol. 

0.447 
0.285 
O.II 


O.SI8 


ROSOLIC  ACID  C20Hi603. 


100  gms.  H2O  dissolve  0.12  gm.  C2oHi6O3  at  2O°-25°. 

100  gms.  pyridine  dissolve  160  gm.  C^HieOa  at  2O°-25°. 

100  gms.  aq.  50%  pyridine  dissolve  80  gm.  C2oHi6O3  at  2O°-25°. 


(Dehn,  1917.) 


•UBIDIUM  ALUMS. 

See  also  Alums,  p. 

32. 

SOLUBILITY  IN 

WATER. 

(Locke,  1901.) 

Gms.  Alum  per  100  Gms.  H2O. 

Ali 

t  ° 

Alum. 

rormula. 

Anhydrous. 

Hydrated. 

G.  Mols. 

Rb.  Aluminum 

Alum 

RbAl(S04)2.i2H2O 

25 

I.8i 

3.15 

0.0059 

3° 

2.19 

0.0072 

35 

2.66 

.  .  . 

0.0087 

40 

3.22 

.  . 

0.0106 

Rb.Chr 

omium 

Alum 

RbCr(S 

04)2.i2H20 

25 

2-57 

4-34 

0.0079 

i 

30 

3-17 

o.  0096 

35 

4.11 

.  .  . 

0.0128 

tt 

40 

5-97 

0.0181 

Rb.  Vanadium 

Alum 

RbV(SO4)2.i2H2O 

25 

5-79 

9-93 

0.0177 

Rb.  Iron  Alum 

RbFe(SO4)2.i2H2O 

•25 

9-74 

16.98 

0.0294 

« 

« 

30 

20.24 

0.0617 

Biltz  and  Wilke,  1906,  find  for  the  solubility  of  rubidium  iron  alum  in  water, 
at  6.6°,  4.55  gms.  per  100  cc.  solution;   at  25°,  29  gms;   and  at  40°,  52.6  gms. 

RUBIDIUM  FLUOBORIDE   RbBF. 

100  gms.  H2O  dissolve  0.55  gm.  RbBF4  at  20°,  and  I  gm.  at  100°.      (Godeffroy,  1876.) 

RUBIDIUM  BROMIDE   RbBr. 


SOLUBILITY  IN  WATER. 

(Rimbach,  1905.) 


Gms.  RbBr  per  100  Gms. 


0-5 

5 
16 


Gms.  RbBr  per  100  Urns. 

Water. 
I3I-85 


Solution. 
56.87 
60.39 
67.24 


Water.  Solution. 

89.6  47.26  39.7 

98  49-5°  57-5  i52-47 

104.8        51.17  113.5  205.21 

Freezing-point  data  for  RbBr  -f  AgBr  are  given  by  Sandonnini  (i9!2a). 

RUBIDIUM   BiCARBONATE  RbHCO3. 

100  gms.  sat.  solution  in  H2O  contain  53.73  gms.  RbHCO3  at  about  20°. 

(de  Forcrand,  1909.) 

RUBIDIUM   CARBONATE  Rb2CO3. 

100  gms.  absolute  alcohol  dissolve  0.74  gm.  Rb2COs.  (Bunsen.) 


583 


RUBIDIUM  CHLORATE 


RUBIDIUM  CHLORATE  RbClO3. 

SOLUBILITY  IN  WATER. 

(Calzolari,  1912.) 

t  o  Cms.  RbClO3  per  f0  Gms.  RbClO3  per 

100  Cms.  H2O.  100  Cms.  H2O. 

o         2.138          42.2       12.48 
8         3.07          50         15.98 

19.8  5.36  76  34-12. 

30         8  99         62.8 

There  is  some  uncertainty  as  to  whether  the  results  of  Calzolari  refer  to  100 
gms.  of  H2O  or  100  gms.  of  saturated  solution. 

100  gms.  H2O  dissolve  3.  i  gms.  RbClO3at  15°  (d^  of  the  sat.  sol.  =  1.07).  (Carlson,  '10.) 
For  earlier  data  see  Reissig,  1863. 

RUBIDIUM  PerCHLORATE  RbC104. 

SOLUBILITY  IN  WATER. 

(Carlson,  1910;  Calzolari,  1912.) 


Gms.  RbClC-4  per  100  Gms.  H2O. 


Gms.  RbC104  per  100  Gms.  H2Q 


I  . 

(Calzolari.) 

(Carlson.) 

i  . 

(Calzolari.) 

(Carlson.) 

0 

°-5 

I.I  (l.007) 

SO 

3-5 

4.6 

10 

0.6 

1.2 

60 

4-85 

6.27  (1.028) 

20 

i 

1.56  (i.oio) 

70 

6.72 

8.2 

25 

1.2 

1.8 

80 

9.2 

11.04  (i  -°5°) 

30 
40 

i-5 

2-3 

2.2 
3.26  (I.OI7) 

90 
IOO 

12.7 
18 

iS-5 

22  (?)  (1.070) 

The  figures  in  parentheses  are  densities  of  sat.  solutions. 
IOO  gms.  H2O  dissolve  1.08  gm.  RbClO4  at  21.3°. 


(Longuimine,  1862.) 


RUBIDIUM   Potassium   PerCHLORATE  Rb2K(ClO4)3. 

100  gms.  sat.  solution  in  H2O  contain  1.55  gms.  Rb2K(ClO4)3  at  20°  (d20  of  the 


sat.  solution  =  I.OI3). 

RUBIDIUM   CHLORIDE   RBC1. 

SOLUBILITY  IN  WATER. 

(Rimbach,  1902;  Berkeley,  1904.) 


(Carlson,  1910.) 


A.  O 

Mols.  RbCl 

Gms.  RbCl 

:  rjer  100  Gms. 

to 

Mols.  RbCl 

Gms.  RbCl 

per  100  Gm 

fc       . 

per  Liter. 

Water. 

Solution. 

• 

per  Liter. 

'Water. 

Solution. 

O 

5.17 

77-o 

43-5 

60 

6.90 

115.5 

53-6 

10 

5-55 

84-4 

45-8 

70 

7-12 

121  .4 

54-8 

20 

5-83 

9I.I 

47-7 

80 

7-33 

127.2 

56.0 

30 

6.17 

97-6 

49-4 

90 

7-52 

I33-I 

57-i 

40 

6-43 

103-5 

5°-9 

IOO 

7.71 

138.9 

58-9 

50 

6.67 

109.3 

52  .2 

112.9 

7-95 

146.6 

59-5 

The  following  determinations  of  the  Sp.  Gr.  of  the  sat.  solutions  are  given  by 
Berkeley. 


t°. 
Sp.  Gr. 


0.55 
1.4409 


18.7 

1.4865 


60.25 
1.5558 


75-iS 
1.5746 


89.35 
1.5905 


"4 


1.6148 


31.5        44-7 
1.5118     1.5348 

*  Boiling-point. 

IOO  gms.  methyl  alcohol  dissolve  1.41     gms.  RbCl  at  25°.  (Turner  and  Bissett,  1913.) 
ethyl  0.078    gm. 

propyl  0.015      "  "  " 

"         amyl  0.0025    "        "       "  "  "  " 

loo  cc.  anhydrous  hydrazine  dissolve  5  gms  RbCl  at  room  temp. 

(Welsh  and  Broderson,  1915.) 

Freezing-point  data  (solubility,  see  footnote,  p.  i)  for  RbCl  +  AgCl  and 
RbCl  +  T1C1  are  given  by  Sandonnini  (1911,  1914).  Results  for  RbCl  +  NaCl 
are  given  by  Zemcznzny  and  Rambach  (1910). 


RUBIDIUM   CHLORIDE  584 

RUBIDIUM   TELLURIUM   CHLORIDE   Rb2TeCl6. 

loo  gms.  aq.  HC1  of  1.2  Sp.  Gr.  dissolve  0.34  gm.  Rb2TeCle  at  23°. 
100  gms.  aq.  HC1  of  1.05  Sp.  Gr.  dissolve  13.09  gms.  Rb2TeCl6  at  23°. 

(Wheeler,  1893.) 

RUBIDIUM   THALLIUM   CHLORIDE   3RbClTlCl3.2H2O. 

100  gms.  H2O  dissolve  13.3  gms.  at  18°,  and  62.5  gms.  at  100°.     (Godeffroy,  1886.) 

RUBIDIUM   CHROMATE  (Mono)  Rb2CrO4. 

SOLUBILITY  IN  WATER. 

(Schreinemakers  and  Filippo,  Jr.,  1906.) 

Gms.  RbCrO4 
t°.  per  loo  Gms. 

Solution. 

50  47-44 

60 . 4  48 . 90 

Solid  Phase,  Ice 
-0.6  0.95 

—  i.i  7.22 

-1.57  9.87 

EQUILIBRIUM  IN  THE  SYSTEM  RUBIDIUM  OXIDE,  CHROMIUM  TRIOXIDE  AND 

WATER  AT  30°. 

(Schreinemakers  and  Filippo,  Jr.,  1906.) 


Gms.  RbCrO4 

t°. 

per  100  Gms. 

Solution. 

-  7 

36.65 

o 

38.27 

10 

40.23 

20 

42.42 

30 

44.11 

40 

46.13 

Gms.  RbCrO4 
t°.             per  zoo  Gms. 
Solution. 

—  2.40 

I5-58 

-3-25 
-4.14 

20.03 
24.28 

-5-55 
-6.7I 

about  —7 

30.15 

34-3i 
36.65 

Gms.  per  100  Gms.  Sat.  Sol. 


Cr03. 

Rb2O. 

O 

60.56 

O 

56.82 

0.776 

37-88 

2.89 

34.89 

4.96 

30.20 

8-54 

28.17 

11.98 

27.99 

15-38 

28.73 

15-54 

28.55 

13.69 

23.87 

9.98 

17.56 

5-72 

8.47 

4.58 

7.98 

4.87 

4.60 

8.16 

3-57 

Solid  Phase. 
RbOH 


Gms.  per  100  Gms.  Sat.  Sol. 

Cr03.  Rb,0.  ' 

13.91  3.38 

15-05  3-45 

15-31  3-59 

15.19  3-I9 
18.96  2.37 

24.92  1.66 
37-34  i-6i 

48 . 20  i . 54 
53-87  1-67 
54.29  1.28 
58.69  1.07 
62.38  0.93 
62.74  0.93 
63.07  0.92 
62.28  o 


RUBIDIUM  DICHROMATE  Rb2Cr3O7. 

SOLUBILITY  OF  THE  POLYMORPHIC  FORMS  IN  WATER. 

(Stortenbecker,  1907;  see  also  Wyrouboff,  1901.) 


Solid  Phase. 


+Rb2Cr3010 


RbjCrAs 


"  +Rb2Cr207 
RfcCrA 


"  +Rb2CrA, 
Rb2Cr4Oi3 


+CrO, 
Cr03 


Gms.  Rb2Cr3O7  per  too  Gms.  Sat.  Sol. 


18 
24 
30 
40 
50 
65 


Monoclinic  Form. 

5-42 

6-94 

9.08 
13.22 
18.94 
28.10 


Triclinic  Form. 
4.96 

6-55 

8.70 
12.90 
18.77 
27.30 


+s  l        \j 

loo  gms.  sat.  aq.  solution  contain  9.47  gms.  Rb2O2O7,  at  30°. 

(Schreinemakers  and  Filippo,  Jr.,  1906.) 


RUBIDIUM  FLUORIDE  RbF.iiH2O. 

100  gms.  H2O  dissolve  130.6  gms.  RbF  at  18°. 


(de  Forcrand,  1911.) 


585  RUBIDIUM  HYDROXIDE 

RUBIDIUM   HYDROXIDE  RbOH. 

100  gms.  sat.  aqueous  solution  contain  63.39  £ms-  RbOH  at  30°. 

(Schreinemakers  and  Filippo.igoG.) 

100  gms.  sat.  aqueous  solution  contain  64.17  gms.  RbOH  at  15°.   (de  Forcrand,  igoga.) 
Fusion-point  data  for  mixtures  of  RbOH  +  NaOH  are  given  by  (v.  Hevesy, 
1900). 

RUBIDIUM   IODATE  RbIO3. 

100  gms.  H2O  dissolve  2.1  gms.  RbIO3  at  23°.  (Wheeler,  1892.) 

RUBIDIUM   PerlODATE  RbIO4. 

100  gms.  H2O  dissolve  0.65  gm.  RbIO4  at  13°,  dig.  of  sat.  solution  =  1.0052. 

(Barker,  1908.) 

RUBIDIUM   IODIDE  Rbl. 

100  gms.  H2O  dissolve  137.5  gms-  Rbl  at  6.9°,  and  152  gms  at  17.4°. 

(Reissig,  1863.) 

SOLUBILITY  OF  RUBIDIUM  IODIDE  IN  ORGANIC  SOLVENTS. 

(Walden,  1906.) 


Acetonitrile 
Propionitrile 
Nitromethane 
Acetone 
Furfurol 

CH3CN 
C2H5CN 
CH3N02 
(CH3)2CO 
C4H3O.COH 

1.478  at  o° 
0.274    " 
0.567    " 
0.960    " 

i.  350  at  25° 

0-305     " 
0.518     " 
0.674 
4-930 

Fusion-point  data  for  Rbl  +  Agl  are  given  by  Sandonnini  (i9i2a). 

RUBIDIUM   PerlODIDES 

SOLUBILITY  IN  WATER  AT  25°. 

(Foote  and  Chalker,  1908.) 

Gms.  per  100  Gms.  Sat.  Sol.  Gms.  per  100  Gms.  Sat.  Sol. 

'-RbL ' I—          Sohd  Phase.  ^^ —         Sohd  Phase. 

61.93  °  Rbl  28.01  64.85  RbI3+I 

59.94  5.90  "  +RbI3  27.85  65.12 

57.24  8.02  Rbi3  27.83  65.13 

33.89        38.08  27.99         64.98 

The  results  show  that  Rbly  and  Rblg  are  not  formed. 

RUBIDIUM   BROMIODIDE  RbBr2I. 

100  gms.  sat.  aq.  solution  contain  about  44  gms.  RbBr2I,  and  the  Sp.  Gr.  of 
the  solution  is  3.84.  (Wells  and  Wheeler,  1892.) 

RUBIDIUM   IRIDATE  and  IRIDITES 

SOLUBILITIES  IN  WATER. 

(Delepine,  1908.) 
Salt.  Formula.  t°.          i^Gms^lfo 

Rubidium  Chloroiridate  Rb2IrCle  19         0.0555 

Tri rubidium  Hexachloroiridite  RbalrCle.H^O       19         0.91 

Dirubidium  Aquopentachloroiridite   Rb2IrCl5(H2O)      19         1.05 

RUBIDIUM   ParaMOLYBDATE  5Rb2O.i2MoO3.H2O. 

100  cc.  sat.  aq.  solution  contain  1.941  gms.  of  the  salt  at  24°.         (Wempe,  1912.) 


RUBIDIUM  NITRATE  586 

RUBIDIUM  NITRATE  RbNO3. 

SOLUBILITY  IN  WATER. 

(Berkeley,  1904.) 

Mols.       Grams  RbNO3  per  100  Gms.  RbNO  Gms-  RbNO3-per  100  Cms. 

Per  Liter.         Water.       Solution.  Per  Liter.          Water.      Solution. 

O            I-27               19.5          16.3                  60  7.99               200         66.7 

10        2.04          33-o      24.8  70          9.02          251  71.5 

20        3.10          53.3       34-6  80          9.93          309  75.6 

30        4-34          81.3       44-8  90         10.77          375  7^-9 

40        5.68         116.7       53.9          100        n-54          452  81.9 

50        6.88        155-6      60.9          118.3    12.76         617  86.1 
The  following  Sp.  Gr.  determinations  are  also  given  by  Berkeley. 

t°.  0.6        15.85      31.55      45.85       63.4        75.60      90.95       118.3* 

Sp.  Gr.  Sat.  Sol.    0.1389     1.2665     1.4483     1.6216     1.8006     1.9055     2.0178       2.1867 

*  Boiling-point. 

THE  SOLUBILITY  AND  SUPERSOLUBILITY  ICE  CURVES  FOR  RUBIDIUM  NITRATE 

AND  WATER. 

(Jones,  1908.) 
Gms.  RbNO3  per  100  Gms.  H2O.  Gms.  RbNO3  per  100  Gms.  H2O. 

of  Ice.  Solubility      Supersolubility        of  ice>     '  Solubility       Supersolubility 

Curve.  Curve.  Curve.  Curve. 

-0.4  1.16  ...  -3-5  •••             9-94 

-1.8  ...  1.24  -2.3  13.97 

-2.1  5.39  -4.2  ...  13.97 

—  1.7  9.94  ...  —  2 . 7  Cryohydrate  17.11 

RUBIDIUM   Telluric  Acid  OXALATE  Rb2[H6TeO6.C2O4]. 
SOLUBILITY  IN  WATER. 

(Rosenheim  and  Weinheber,  1910-11.) 
t°.  0°          20°  30°  40°  50° 

Gms.  Rb2[H6Te06.C2O4]  per  zoo  gms.  H2O    3.85     7.26      9.40     12.76     16.90 

RUBIDIUM  PERMANGANATE   RbMnO4. 

One  liter  of  aqueous  solution  contains  6.03  gms.  RbMnO4  at  7°. 

(Muthmann  and  Kuntze,  1894.) 

100  cc.  sat.  aq.  solution  contain  0.46  gm.  RbMnO4  at  2°,  1.06  gms.  at  19°  and 
4.68  gms.  at  60°.  (Patterson,  1906.) 

RUBIDIUM   SELENATE  Rb2SeO4. 

100  gms.  H2O  dissolve  158.9  gms.  Rb2SeO4  at  12°.  (Tutton,  1897.) 

SOLUBILITY  OF  MIXED  CRYSTALS  OF  RUBIDIUM  ACID  SELENATE  AND  RUBIDIUM 
ACID  TELLURATE  AND  OF  RUBIDIUM  ACID  SULFATE  AND  RUBIDIUM  ACID  TEL- 

LURATE  IN  WATER  AT  25°.  (Pellini,  1909.) 

Results  for  RbHSeO4  +  RbHTeO4.  Results  for  RbHSO4  +  RbHTeSO4. 

Gms.  per  loop  cc.  Sat.  Sol.  Mol.  %  Selenate  Gms.  per  loop  cc.  Sat.  Sol.  Mol.  %  Sulfate 

RbHSe04.  RbHTe04.  in  Solid  Phase.  'RbHSO4.  RbHTeO4'.  in  Solid  Phase. 

76.46  39.51  51.55  26.675  38.403  47-91 

95-82  35.30  52.22  32.117  31.58  50.33 

171.70  22.98  53.95  42.917  26.764  50.74 

462.80      5       56.33       59.074'   20.182      50.99 

859-30       3.40      67. 46*       498.25        0.02887      52.52 

RUBIDIUM   FLUOSILICATE   Rb2SiF6. 

100  gms.  H2O  dissolve  0.16  gm.  Rb2SiF6  at  20°,  and  1.36  gms.  at  100°. 

(Stolba,  1867.) 

RUBIDIUM   SILICOTUNGSTATE  Rb8SiWi2O42. 

100  gms.  H2O  dissolve  0.65  gm.  RbsSiW^O^  at  20°,  and  5.1  gms.  at  100°. 

(Godeffroy,  1876.) 


587  RUBIDIUM   SULFATE 

RUBIDIUM  SULFATE  Rb2SO4.    SOLUBILITY  IN  WATER. 
SOLUBILITY  IN  WATER. 

(Etard,  1894;  Berkeley,  1904.) 

Gms. 


I   . 

per  Liter. 

Water. 

Solution. 

ii  . 

per  Liter. 

Water. 

Solution. 

0 

1.27 

36-4 

27-3 

60 

2.IS 

67.4 

40-3 

10 

I  .46 

42  .6 

29.9 

70 

2.25 

71.4 

41.7 

20 

I  .64 

48.2 

32-5 

80 

2-34 

75  -° 

42.9 

30 

1-79 

53-5 

34-9 

90 

2.42 

78.7 

44.0 

40 

1.92 

58-5 

36-9 

100 

2.49 

81.8 

45-o 

SO 

2.04 

63.1 

38-7 

IO2  .4 

2  .50 

82.6 

45-2 

The  following  Sp.  Gr.  determinations  are  also  given  by  Berkeley. 

t°.  0.5       15.80        31.6        44.2       57-90      74-75       89.45     102.4* 

Sp.Gr.Sat.Sol.  1.2740     1.3287     1.3704    1.3998     1.4232     1.4480    1.4649     1-4753 

*  b.  pt. 

100  cc.  sat.  solution  in  absolute  H2SO4  contain  58.81  gms.  Rb2SO4. 

(Bergius,  1910.) 

SOLUBILITY  OF  RUBIDIUM  DOUBLE  SULFATES  IN  WATER  AT  25° 

(Locke,  1902.) 

Per  IPO  cc.  H2O.  Per  100  cc.  H2O. 

Formula.  '   Gms.  Mols.  Formula.  '  Gms.      "     Mols. 

Anh.  Salt.       Salt.  Anh.  Salt.       Salt. 

Rb2Cd(SO4)2.6H2O  76.7  0.1615  Rb2Mn(SO4)2.6H2O  35.7  0.0857 

Rb2Co(SO4)2.6H2O  9.28  0.022  Rb2Mg(SO4)2.6H2O  20.2  0.0521 

Rb2Cu(SO4)2.6H2O  10.28  0.0241  Rb2Ni(SO4)2.6H2O         5.98  0.0142 

RblFefSO4)2.6H2O  24.28  0.0579  Rb2Zn(SO4)2.6H2O  10.10  0.0236 


RUBIDIUM  Dihydroxy  TARTARIC  ACID 

100  gms.  H2O  dissolve  6.51  gms.  Rb2C4H4O8.3H2O  at  o°.  (Fenton,  1898.) 

On  account  of  the  unstable  character  of  the  compound,  only  \  hour  was  allowed 
for  saturation  of  the  solution. 

RUTHENIUM   SALTS 

SOLUBILITIES  IN  WATER. 

(Howe,  1894.) 


Salt. 

Formula. 

t°. 

Gms.  Salt 
per  100  Gms. 

H20. 

Ruthenium  Potassium  Nitrosochloride 

K2RuCl5NO 

25 

12 

it 

tt                               it 

(i 

00 

80 

tt 

Ammonium  Nitrosochloride 

(NH4)2RuCl5NO 

25 

5 

n 

«                      n 

tt 

00 

22 

ti 

Rubidium  Nitrosochloride 

Rb2RuCl5NO 

25 

o-57 

(i 

a                    it 

u 

60 

2.13 

tt 

11  (hydrated) 

Rb2RuCl5NO.2H2O 

25 

114-3 

(i 

Caesium  Nitrosochloride 

Cs2RuCl5NO 

25 

O.2O 

n 

it                   tt 

tt 

60 

0.56 

n 

11                   "    (hydrated) 

Cs2RuCl5.NO.2H2O 

25 

105.8 

SACCHARIN    (i,  Benzosulfonazole,  2(1),  one)  C6H4<cQ2>NH. 

100  parts  H2O  dissolve  0.4  part  at  25°  and  4.17  parts  at  100°. 

100  parts  alcohol  dissolve  4  parts  at  25°.  (U.  S.  P.  VTH.) 

loo  gms.  trichlorethylene  dissolve  0.012  gm.  saccharin  at  15°. 

(Wester  and  Bruins,  1914.) 


SACCHARIN  588 

DISTRIBUTION  OF  SACCHARIN  AT  25°  BETWEEN: 

Water  *  and  Ether.  Water  f  and  Amyl  Acetate. 

(Marden,  1914.)  (Marden,  1914.) 

Gms.  Saccharin  per:  Gms.  Saccharin  per: 

'loocc.  H20            50  cc.  Ethe?        Dist>  CoeL  105  cc.  Aq.          50  cc.  AmyP       Dist>  Coef' 

Layer.                    Layer.  Layer.           Acetate  Layer. 


0.0290     0.0438    0.267       0-0045    0.0700    0.0306 

0.0458       0.0829      0.235          0.0065      0-0957      0.0322 

0.0719       0.1245      0.245          O.OII4      0.1724      0.0315 

*  Slightly  acidified  with  HC1.        f  Containing  5  cc.  cone.  HC1  per  100  cc. 

The  amount  of  saccharin  entering  the  ethereal  layer  is  increased  by  addition 
of  HC1  to  the  aqueous  layer.  With  5  cc.  cone.  HC1  per  100  cc.  H2O,  the  distribu- 
tion coefficient  is  reduced  to  0.0624. 

SALICIN  C6H4(CH2.OH)O.C6Hu05. 

SOLUBILITY  IN  SEVERAL  SOLVENTS. 

Solvent.  f.  GmS-SP0Tven?.GmS-  Authority. 

Water  15  3.52  (Greenish  and  Smith,  1903.) 

Water  25  4.16  (Dott,  1907.) 

90%  Alcohol  15  1.5  (Greenish  and  Smith,  1903.) 

90%  Alcohol  15  2  (Squire  and  Caines,  1905.) 

Trichlor  Ethylene  15  O.OI3  (Wester  and  Bruins,  1914.) 

SALICYLAMIDE   OH.C6H4CONH2. 

DISTRIBUTION  BETWEEN  WATER  AND  OLIVE  OIL. 

(Meyer,  1901.) 

Gms.  OHCeH^CONHz  per  100  cc. 

t°.  , •*• v  Dist.  Coef. 

H2O  Layer.  Oil  Layer. 

3  0.056  0.126  2.25 

36  0.075  0.107  i-40 

SALICYLIC  ACID   C6H4.OH.COOH'i:2. 

SOLUBILITY  IN  WATER. 


(Average  curve  from  the  closely  agreeing  determinations  of  Walker  and  Wood,  1898;  at  26.4°,  Philip, 
1905;  at  25°,  Paul,  1894;   at  20°,  Hoitsema,  i8g8a;   Hoffman  and  Langbeck,  1905.     For  determinations 
not  in  good  agreement  with  the  following,  see  Alexejew,  1886;  Bourgoin,  1878;  Ost.,  1878.) 

Gms. 

Gms. 

Gms. 

to            C6H4.OH.COOH 

t° 

C6H4.OH.COOH 

t° 

CsH^OH.COOH 

Liter  Solution. 

per 
Liter  Solution. 

Liter  Solution. 

0                     0.8 

25 

2.2 

60 

8.2 

IO                      1.2 

30 

2-7 

70 

13.2 

20                      1.8 

40 

3-7 

80 

20.5 

50 

5-4 

SOLUBILITY 

OF  SALICYLIC  ACID  IN 

WATER 

(Savorro,  1914.) 

Gms. 

Gms. 

Gms. 

t«,           C6H4.OH.COOH 

t° 

C6H4.OH.COOH 

t° 

C6H4.OH.COOH 

per  1000  Gms. 

*  . 

per  1000  Gms. 

i*  . 

per  1000  Gms. 

Sat.  Sol. 

Sat.  Sol. 

Sat.  Sol. 

o              1.24 

35 

3-51 

70 

13.70 

5             1-29 

40 

4.16 

75 

17-55 

10              1.35 

45 

4.89 

80 

22.O8 

15              1.84 

6-38 

85 

27.92 

20                    2 

55 

7-44 

90 

37-35 

25                    2.48 

60 

9 

95 

50-48 

30                   2  .  98 

65 

10.94 

100 

75-07 

589  SALICYLIC  ACID 

SOLUBILITY  OF  SALICYLIC  ACID  (LIQUID)  IN  WATER. 

Determinations  by  Synthetic  Method.     See  Note,  p.  16.     The  original  data 
in  each  case  were  plotted  and  the  following  figures  read  from  the  curves. 

(Flaschner  and  Rankin,  1910.) 


(Alexejew.) 

Cms.  C«H4OHCOOH  per 

100  Cms. 


Cms.  C|H«OHCOOH  per 
100  Cms. 


I  . 

Aqueous 

Salicylic  Acid 

i  . 

Aqueous 

Salicylic  Acid 

Layer. 

Layer. 

Layer. 

Layer. 

60 

7 

68 

60 

4-5 

68 

70 

8 

64 

70 

6-5 

62.5 

80 

12 

58 

80 

10 

54 

90 

19 

49 

8$ 

15 

46 

95  crit 

temp. 

•_i                  _r 

87  crit. 

temp.          30 

are  also  given  by  Flaschner  and  Rankin. 
SOLUBILITY  OF  SALICYLIC  ACID  IN  AQUEOUS  SALT  SOLUTIONS  AT  25°  AND 

AT  35°.       (Hoffman  and  Langbeck,  1905.) 

C6H4OH.COOH  Dissolved  at  25°.    C8H4OH.COOH  Dissolved  at  35°. 


Salt. 

iNormaiiiy 
of  Salt 
Solution. 

oms.       /- 
Salt  per 
Liter. 

Gms.  per 
1000  Gms. 
Sat.  Sol. 

Gm.  Mol. 
Per  cent. 

Gms.  per 
1000  Gms. 
Sat.  Sol. 

Gm.  Mol. 
Per  cent. 

KC1 

0.020 

I 

.49 

2.24 

2.92l6. 

io-4 

3 

•23 

4 

.2206. 

io-4 

u 

O.IOO 

7 

.46 

2.25 

2-9377 

tt 

3 

•23 

4 

.22O3 

11 

tt 

0.492 

36 

•73 

2.02 

2.6321 

tt 

3 

.01 

3 

.9268 

tl 

tl 

1.004 

74 

•.92 

1.89 

2.4759 

tt 

2 

.68 

3 

•5003 

It 

KN03 

0.020 

2 

.02 

2.25 

3-9351 

tt 

3 

•25 

4 

.2499 

tt 

« 

O.IOO 

10 

.12 

2.30 

3.0103 

tl 

3 

•32 

4 

•3334 

11 

tt 

0.504 

51 

.10 

2.38 

3  .  1061 

ft 

3 

.38 

4 

.4123 

It 

tt 

I  .OO4 

101 

.60 

2-39 

3.1249 

tl 

3 

•36 

4 

.3848 

It 

NaCl 

O.O2O 

I 

.19 

2.23 

2.9110 

tl 

3 

.22 

4 

.2062 

It 

tt 

O.IOO 

5 

•95 

2.22 

2.9027 

tt 

3 

.20 

4 

.1806 

tt 

it 

0.497 

29 

•  50 

2 

2.6128 

tl 

2 

-85 

3 

.7171 

tt 

tt 

0.988 

58 

.80 

1.72 

2.2487 

tt 

2 

•43 

3 

.1596 

tt 

SOLUBILITY  OF  SALICYLIC  ACID  IN  AQUEOUS  SALT  SOLUTIONS  AT  25°. 

(Philip,  1905;  Philip  and  Garner,  1909.) 


In  Aq.  Sodium 
Acetate. 

Gms.  per  Liter. 


CHjCOONa.    C«H4OHCOOH. 

i. oi  3.60 

2-48  5-93 

5-03         9-56 

10.07         16.81 

In  Aq.  Sodium 
Succinate. 

Gms.  per  Liter. 
C,H4(COONa)2.  C«H4OHCOOH. 

1.18  2.97 

2-93  4-34 

5-85  6.56 

11.73  10.82 


In  Aq.  Sodium 
Formate. 
Gms.  per  Liter. 
HCOONa.      C«H4OHCOOH. 

0.81  3.40 

1.63  4-42 

4.06  7.II 

8.14  IO.44 

In  Aq.  Potassium 
Formate. 

Gms.  per  Liter. 


HCOOK. 
0 

1.03 
2.56 


In  Aq.  Sodium  Monochlor 
Acetate. 

Gms.  per  Liter. 

CH2ClCOONa.     C^OHCOOH. 
1.38  2.83 

3-43  3-58 

6 . 84  4 . 64 

13.71  6.17 

In  Aq.  Sodium  Butyrate 
at  26.4°. 

Gms.  per  Liter. 
C,H4OHCOOH.     C,H7COONa.  CgH^OHCOOI?. 

2.265  i  3-3 

3-38  2  4.5 

4-93  4  6.85 

7-13  *  8.1 


One  liter  of  I  normal  aqueous  sodium  salicylate  solution  dissolves  4.97  gms. 
salicylic  acid  at  25°.  (Sidgwick,  1910.) 


SALICYLIC  ACID 


590 


SOLUBILITY  OF 


SALICYLIC  ACID  IN 
SALIC  YLATE 

(Hoitsema, 


Gm.  Mols.  per  Liter. 

^OOH1" 

QftOH- 
COONa. 

0.0132 

0 

O.OII2 

0.017 

0.0124 

0.113 

0.0143 

0.226 

0.0164 

0-344 

O.O2O3 

0.500 

O.O62 

1.70 

0.095 

2.  II 

0.091 

2.19 

0.086 

3-41 

O.oSl 

4-23 

0.048 

4.18 

O.O2I 

4.12 

O. 

4.15 

Sp.  Gr.  of 
Solutions. 


.OO2 
.003 
.009 
.016 
.024 

1-034 
I.  112 

1-137 

I.I44 
I.2I5 

1.263 


Cms.  per  Liter. 


259 
258 
257 


AQUEOUS  SOLUTIONS  OF  SODIUM 

AT  2O.I°. 


Solid  Phase. 
Cs^OHCOOH 


(  C6H4OHCOOH.C6H4OHCOONa 
(      +C6H4OHCOOH 
C6H4OHCOOH.C6H4OHCOONa 

(  C8H4OHCOOH.C8H4OHCOONa 
|      +C6H4OHCOONa 

QH4OHCOONa 


C6H4OH- 
COOH. 

QH4OH- 
COONa. 

1.823 

0 

1-55 
I.7I 

2.705 
17-98 

1.97 
2.26 
2.80 

54-74 

8.56 

270.5 

13.11 

335  •  7 

12.56 

11.88 

348.4 
542.6 

11.19 

673 

6.63 
2.90 
o 

665.1 

665.5 
660.3 

SOLUBILITY  OF  SALICYLIC  ACID  IN  AQUEOUS  SOLUTIONS  OF  ACIDS  AT  25°. 

(Kendall,  1911.) 


Gms.  per  Liter. 

Gms.  per  Liter. 

Acid. 

*»•       «- 

Acid. 

C.H.OH- 

Water  alone 

o 

2.257 

Formic  Acid 

230 

15 

HCOOH        2.370 

Acetic  Acid 

37.52CH3COOH 

2-335 

" 

46O 

30 

"             2.901 

" 

75-05 

" 

2.409 

Hydrochloric  Acid 

o 

653 

HC1           1  .  781 

" 

150.  10 

" 

2-549 

« 

I 

302 

1.710 

u 

300.20 

" 

2.850 

« 

A 

558 

" 

•677 

Formic  Acid 

2.38 

HCOOH 

2.114 

" 

9 

117 

"               3 

•649 

u 

4-59 

" 

2-035 

n 

18 

235 

" 

.551 

tt 

11.05 

" 

2.114 

Malonic  Acid 

•? 

253 

CH2(COOH)2 

.051 

ft 

21.17 

" 

2-035 

« 

10 

49 

" 

•944 

" 

28.76 

" 

2.049 

" 

20 

84 

« 

.880 

" 

57-53 

" 

2.066 

Methyl  Picric  Acid 

2 

28 

C7H607N,       2.115 

" 

115.07 

u 

2.  121 

SOLUBILITY  OF  SALICYLIC  ACID  IN  AQUEOUS  SOLUTIONS  OF  o  NITROBENZOIC 


Gms.  per  Liter. 


O 

2.615 

7-  202 
7.283 


o  C6H4- 
OHCOOH. 
2.257 
1-974 
1.887 
1.885 


ACID  AT  25°  AND  VICE  VERSA. 

(Kendall,  1911.) 

Gms.  per  Liter 
Solid  Phase.  '  ~  „  XT 


Salicylic  Acid 


+Nitrobenzoic 


7.188 
7.213 
7-233 


o  C«H4.OH.- 
COOH. 
2.243 

1.873 
1.294 


Solid  Phase. 


o  Nitrobenzoic  Acid 


da  of  Sat.  Sol. 


SOLUBILITY  OF  SALICYLIC  ACID  IN  AQUEOUS  ALCOHOL  AT  25°. 

(Seidell,  1908,  1909,  1910.) 

Wt.  Per  cent  Gms. 

C2H5OH  in  ^  Sat.  Sol.  C,H4OHCOOH 

Solvent.  per  100  Gms. 

Sat.  Sol. 

10  0.984  0.38 

2O  0.970  0.80 

3°  0.959  2.20 

40  0.951  5.90            90 

SO  0.945  12.20            100         0.919         33-20 


Wt.  Per  cent 
QHsOH  in 

Solvent. 

60 
70 
80 


0-943 
0.941 

0-937 
0.930 
0.919 


Gms. 

C6H4OHCOOH 

per  100  Gms. 

Sat.  Sol. 

18.30 

24 
28.30 


591 


SALICYLIC  ACID 


SOLUBILITY  OF  SALICYLIC  ACID  IN  AQUEOUS  SOLUTIONS  OF  ETHYL  ALCOHOL, 
ISOBUTYL   ALCOHOL,   DEXTROSE,   CANE  SUGAR,  AND  OF   LEVULOSE  AT  25° 

AND  AT  35°.  (Hoffmann  and  Langbeck,  1905.) 


Cone,  of  Solvent. 


C6H4OH.COOH  Dissolved 
at  25°. 


Aq.  Solvent. 

Normal- 
ity. 

Gms.  per 
Liter. 

Gm.  Mol. 
Per  cent. 

Gms.  per 
100  Gms. 
Sat.  Sol. 

Gm.  Mol. 
Per  cent. 

Gms.  per 
100  Gms 
Sat.  Sol. 

CjjHsOH 

0.0249 

I 

.146 

2 

.8966. 

io-4 

O.222 

4- 

2044. 

io-4 

0.322 

« 

0.0560 

2 

•578 

2 

.9150 

tt 

0.223 

4- 

2348 

11 

0.324 

cc 

0.1747 

8 

.04 

2 

.9901 

cc 

O.229 

. 

tt 

0.2399 

II 

•05 

.  .  . 

4- 

434i 

n 

0-339 

tt 

1.03 

47 

•4 

3 

•5279 

ct 

O.27O 

5- 

2816 

n 

0.404 

cc 

1.638 

75 

•44 

3 

•9253 

Cl 

0.300 

C^OH  (iso) 

0.020 

i 

.496 

2 

.909 

cc 

0.223 

4- 

229 

Cl 

0.324 

cc 

O.O5I 

3 

•74 

2 

•955 

cc 

O.226 

4- 

289 

n 

0.329 

It 

0.  100 

7 

.48 

3 

-033 

ct 

0.232 

4- 

435 

" 

0-339 

cc 

0.521 

38 

.60 

3 

.718 

Cl 

0.285 

5- 

624 

tt 

0.431 

C6H1206 

0.02 

3 

.6 

2 

.886 

Cl 

O.22I 

4- 

184 

n 

0.321 

tt 

O.IO 

18 

2 

.898 

Cl 

0.222 

4- 

202 

1C 

0.322 

tt 

0.50 

89 

.6 

2 

•954 

1C 

O.226 

4- 

263 

ct 

0.326 

tt 

I 

180 

3 

.015 

11 

0.231 

4- 

360 

11 

0-334 

Ci2H22On 

O.O2 

6 

.88 

2 

.902 

1C 

0.221 

4- 

206 

Cl 

0.322 

tt 

O.IO 

34 

•97 

2 

.964 

cc 

o.  227 

4- 

287 

11 

0.328 

tt 

0.50 

172 

3 

•239 

cc 

0.248 

4- 

697 

11 

0.360 

n 

I.IO 

376 

•3 

3 

-633 

1C 

0.278 

5- 

236 

11 

O.40I 

CeH1206 

O.02 

3 

.6 

2 

.888 

Cl 

O.22I 

. 

.  .  . 

cc 

0.06 

IO 

.8 

2 

•895 

1C 

O.22I 

.  . 

. 

tt 

0.25 

45 

2 

•944 

Cl 

0.225 

. 

SOLUBILITY  OF  SALICYLIC  ACID  IN  ALCOHOLS,  IN  ETHER  AND  IN  ACETONE. 

(Timofeiew,  1891;  at  15°,  Bourgoin,  1878;  at  23°,  Walker  and  Wood,  1898.)    . 


Solvent. 

CH3OH 
CH3OH 
C2H5OH 
C2H5OH 
C2H5OH 
C2H5OH  90% 

Gms.  C6H4OHCOOH 
t°f                 per  100  Gms. 

Solvent. 

C3H7OH(w) 
C3H7OH(n) 
(CH3)20 
(CH3)20 
(CH3)2CO 

Gms.  C6H4OHCOOH 
t°_                 per  loo  Gms. 

-  3 

+  21 

—  3 
+  15 

21 
15 

Solvent. 
40.67 
62.48 
36.12 

53-53 

42.09 

Solution. 
28.91 
38.46 
26.29 
33-17 
34.87 
29.62 

-  3 

+  21 
15 

23 

Solvent. 
26.  12 
37.69 
50-47 

Solution. 
2O.7I 
27.36' 

33-55 
23-4* 
31-3* 

Gms.  per  100  cc.  sat.  sol.  instead  of  per  100  gms.  sat.  sol. 

100  gms.  sat.  solution  in  methyl  alcohol  contain  39.87  gms.  salicylic  acid  at  15°. 

(Savorro,  1914.) 


SOLUBILITY  OF  SALICYLIC  ACID  IN  MIXTURES  OF  ACETONE  AND  BENZENE  AT  25°. 

(Marden  and  Dover,  1917.) 
Gms.  per  100  Gms.  Mixed  Solvent.     Gms.  per  100  Gms.  Mixed  Solvent.     Gms.  per  too  Gms.  Mixed  Solvent. 


Acetone. 

IOO 

00 

80 

70 


Salicylic  Acid. 

55 

4<U 

42.3 


Acetone. 

Salicylic  Acid. 

Acetone. 

Salicylic  Acid. 

60 

36.7 

20 

15 

50 

31 

10 

7-1 

40 

25-3 

0 

0.92 

3C 

20 

SALICYLIC  ACID  592 


SOLUBILITY  OF  SALICYLIC  ACID  IN  BENZENE. 

(Walker  and  Wood,  1898.)                                      (von  Euler  and  Lowenhamn,  1916.) 
Gms.  C«H4-                    Gms.  C6H4-                                                                              Gms.  C6H4- 
f0         OHCOOH        to          OHCOOH         «                          Solvent                            OHCOOH 
per  goo  Gms.                 per  100  Gms.                                                                             per  100  cc. 

c 

eHe. 

C6H6. 

Sat.  Sol. 

II 

•  7 

0. 

460 

34 

6 

I.26l 

18 

CeH6 

0.525 

18 

,2 

0. 

579 

36. 

6 

1-430 

25 

CeH6 

0.762 

25 

0. 

78 

49 

4 

2.380 

18 

o.5wCH2ClCqOHinC6H6 

1.698 

30 

•  5 

0. 

991 

64 

2 

4.40 

18 

o  .  5^  C-gilsOJii.  in  C-gldLs 

0.746 

SOLUBILITY  OF  SALICYLIC  ACID  IN  MIXTURES  OF  BENZENE  AND  ETHYL 
ACETATE  AT  25°. 

(Harden  and  Dover,  1917.) 

Cms,  per  100  Gms.  Mixed  Solvent.    Gms.  per  100  Gms.  Mixed  Solvent.     Gms.  per  100  Gms.  Mixed  Solvent. 
Ethyl  Acetate.      Salicylic  Acid.       Ethyl  Acetate.      Salicylic  Acid.        Ethyl  Acetate.     Salicylic  Acid. 

100  38  60  16.6  20  6.2 

90  24.2  50  14.5  10  3-42 

80  22.7  40  12.8  o  0.92 

70  19-5  30  9-6 

SOLUBILITY  OF  SALICYLIC  ACID  IN  SEVERAL  SOLVENTS  AT  25°. 

(Herz  and  Rathmann,  1913.) 

SolvPr  Gms.  Cel^OHCOOH  _,  Gms.  CeH4OHCOOH 

Solvent.  per  zoo  cc.  Sat.  Sol.  Solvent'  per  100  cc.  Sat.  Sol. 

Chloroform  2.168  Tetrachlor  Ethylene  1.105 

Carbon  Tetrachloride        0.4143  Tetrachlor  Ethane  2.085 

Trichlor  Ethylene  i-5*9  Pentachlor  Ethane  1.064 

100  gms.  dichlor  ethylene  dissolve  0.757  gm.  salicylic  acid  at  15°.  )     (Wester  and 
loo  gms.  trichlor  ethylene  dissolve  0.28  gm.  salicylic  acid  at  15°.   J  Bruins,  1914.) 

SOLUBILITY  OF  SALICYLIC  ACID  IN  OILS  (Temp,  not  stated). 

(Engfeldt,  1913.) 

Gms.  Gms. 

Oil  of-  C6H4OHCOOH  Oilof.  C6H4OHCOOH 

per  100  Gms.  per  100  Gms. 

Sat.  Sol.  Sat.  Sol. 

Phocae  (Dog  Fish  Oil)  i  .  70  Sesami  2.61 

Jecoris  Aselli  (Cod  Liver  Oil)  i  .-86  Cannabis  3 

Arachidis  (Peanut  Oil)  i  .  88  Lini  (Linseed  Oil)  3  .  04 

Amygdalarum  2.08  Juglandis  (Walnut  Oil)  3.15 

Olivae  (Olive  Oil)  2  .  14  Gossypii  (Cottonseed  Oil)  3  .  23 

Rapse  (Rape  Seed  Oil)  2.  17  Ricini  (Castor  Oil)  12.98 

Papaveris  (Poppy  Seed  Oil)  2.22  Paraffiniam  Liquid  o 

The  ratio  of  the  solubilities  of  salicylic  acid  in  olive  oil  and  in  water  (cone. 
in  oil  -5-  cone,  in  H^O)  at  25°  is  given  as  n.8  by  Boeseken  and  Waterman  (1911, 
1912).  This  corresponds  to  2.6  gms.  acid  per  100  gms.  olive  oil. 

DISTRIBUTION  OF  SALICYLIC  ACID  BETWEEN: 

Water  and  Benzene.    (Hendrixon,  1897.)       Water  and  Chloroform.    (Hendrixon,  1897.) 
Results  at  10°.          Results  at  40°.  Results  at  10°.  Results  at  40°. 

Gms.  Acid  100  cc.  Gms.  Acid  per  100  cc.          Gms.  Acid  per  100  cc.         Gms.  Acid^per  100  cc." 

H20  Layer.   QH,  Layer.    'H2O  Layer  '  C6H6  Layer.'    H2O  Layer.  CHC13  Layer!  H2O  Layer.   CHC13  Layer. 
0.0264       0.0391        O.O260       0.0400       0.0293        0.0442        0.0335        0.0475 


0.0377 

0.1200 
0.1292 

0.0655 
0.4159 
0.4713 

O.O7I9 
0.1220 
0.1563 
0.2014 

0.1649 

0-3539 
0.50l6 
0.7625 

0.0457 

o.  1172 

0.1229 
0.1236 

o  .  0946 
0.5640 
0.6196 
0.6269 

0.0819 

0.1589 
0.2687 
0.3053 

0.1775 
0.5297 

1.3887 
1.7570 

Similar  data  for  the  'distribution  between  water  and  benzene  at  18°  are  given 
by  Nernst  (1891). 


I/  . 

H20  Rich  Layer. 

Acid  Rich  Layer. 

25 

4-8 

50 

6 

74 

70 

10 

67 

80 

14 

00 

85 

17-5 

55 

87.5 

20 

50 

89  crit. 

temp.                    35 

593  SALICYLIC   ACID 

Acetyl  SALICYLIC  ACID  (Aspirin)  CH3COO.C6H4.COOH,  1.2. 
SOLUBILITY  AND  MELTING-POINT  CURVES  FOR  MIXTURES  OF  ACETYL  SALICYLIC 
ACID  AND  WATER,  DETERMINED  BY  THE  SYNTHETIC  METHOD. 

(Flaschner  and  Rankin,  1909.) 

Solubility  Curve  (Liquid  Acid+H2O).         M.-pt.  Curve  (Solid  Acid +H»O). 
Cms.  CH3COO.C6H4.COOH  per  100  Cms.  Cms.  CHjCOOQHr 

t°.  COOH  per  too  Cms. 

Mixture. 

82.4  4.8 

90.4  10 

92.4  20 

93 . 6  60 

99  80 

109.4  89.5 

131  100 

SALOL  (Phenylsalicylate)  CeH^OH.COOCeHs,  1.2. 

SOLUBILITY  OF  SALOL  IN  AQUEOUS  ALCOHOL  AT  25°.    (Seidell,  1909, 1910.) 

Wt.  Per  cent              .      *                Gins.  Salol  Wt.  Per  cent  .    ni  Gms.  Salol 

C,H6OHin  of?  ell            per  100  Gms.  C2H5OH  in  sit  Sol  per  100  Gms. 

Solvent.  Sat'  SoL  '          Sat.  Sol.  Solvent.  Sat.  Sol. 

O  0.999                 0.015  70  0.877  4.40 

20  0.967              0.020  80  0.863  7-7° 

40  0.934  0.22  90  0.865  *4 

50  0.914  0.76  92.3  0.868  17-70 

60  0.895  2-10  I0°  0.898  35 

SOLUBILITY  OF  SALOL  IN  SEVERAL  SOLVENTS.    (Seidell,  1907.) 

,  a.         Gms.  Salol  j  oaf     Gms.  Salol 

Solvent.             t°.            c,         per  100  Gms.                 Solvent.                  t°.  V>? t'  per  100  Gms. 

SoL           Sat.  Sol.  bo1'       Sat.  Sol. 

Acetone           30-31       ...           90 .99        Amyl  Alcohol            25  0.869     20.44 

Benzene          30-31     1.148        88.57        Acetic  Acid  (99. 5%)  21.5  1.143     63.24 

Amyl  Acetate  30-3 1     1.136        85.29        Xylene                      32.5  ...       87.14+ 

Aniline            30-31       ...     very  soluble   Toluene                      25  1.128    83.62 

100  gms.  pyridine  dissolve  381  gms.  salol  at  2O°-25°  (Dehn,  1917).     The  solu- 
tion in  aqueous  50  per  cent  pyridine  separates  into  two  layers. 

SOLIDIFICATION  TEMPERATURES  (Solubility,  see  footnote,  p.  i)  FOR  MIXTURES  OF: 


Salol  and  Thymol.    (Bellucci,  1912.) 

Salol  and  Urethan. 

(Bellucci, 

1912,  1913.) 

AO    t       Gms.  Salol 

c  r!rf    Per  I0°  Gms. 
Sohdif.  V  Mixture 

f  o    e       Gms.  Salol 
Snlirlif    per  too  Gms. 
Solldlf-       Mixture. 

+o    £         Gms.  Salol 

Solidif      per  \°°  Gms> 
Mixture. 

t°of 
Solidif. 

Gms.  Salol 
Mixture. 

42 

100 

23 

So 

42 

IOO 

36. 

5 

50 

34 

26 

90 
80 

29 
34-5 

40 
30 

36 
29 

Eutec. 

00 

86 

39 
41-5 

40 
30 

18 

70 

40 

20 

31 

80 

44 

2O 

J3 

Eutec. 

66 

46 

10 

30 

70 

47 

IO 

17 

•  5 

60 

Si 

o 

3*4 

60 

48. 

5 

0 

The  Eutec 

.  for  sa 

lol  +  cam 

phor  is  at 

-1-6°  and  contains  56% 

salol 

KBellucci, 

The  Eutec.  for  salol  4-monobromcamphorisat2i°and  contains  6o%salol.  (1912,  13.) 
Solidification   temperatures  for   Salol  +  Sulfonal  and  for  Salol  +  0  Naphthol 
are  given  by  Bianchini  (1914). 

SANTONIN  CiBHi8O3. 

SOLUBILITY  IN  SEVERAL  SOLVENTS. 


f.  rGmo^                   Authorit^ 

Water                                  20-25  0.02+        (Dehn,  1917.) 

Alcohol  (90%)                                15  about  2.  3        (Greenish  and  Smith,  1903.) 

Trichlor  Ethylene                      15  2.46             (Wester  and  Bruins,  1914.) 

Pyridine                                 20-25  12.72             (Dehn,  1917.) 

Aq.  50%  Pyridine                20-25  12.35 

F.-pt.  data  for  mixtures  of  stereoisomeric  santonin  salts  are  given  by  Malvino 
and  Manino  (1908). 


SAMARIUM   CHLORIDE  594 

SAMARIUM   CHLORIDE  SaCl3. 

100  gms.  pyridine  dissolve  6.38  gms.  SaCl3  at  15°.  (Matignon,  1906, 1909.) 

SAMARIUM   GLYCOLATE  Sa(C2H3O3)? 

100  gms.  H2O  dissolve  0.6373  Sm-  Sa(C2h3O3)3  at  20°. 

(Jantsch  and  Griinkraut,  1912-13.) 

SAMARIUM   Double  NITRATES. 

SOLUBILITY  IN  CONC.  HNO3  OF  dip  =  1.325  AT  16°. 

(Jantsch,  1912.) 


Samarium  Magnesium  Nitrate  [Sa(N03)e]Mg3 .  24  H2O  24 . 55 

Nickel  "  "        Ni3         "  29.11 

Cobalt  "  "        Co3       "  34.27 

Zinc  "  "        Zn3        "  36.47 

Manganese        "  Mn3      "  50.04 

SAMARIUM   OXALATE  Sa2(C2O4)3.ioH2O. 

One  liter  H2O  dissolves  0.00054  Sm-  Sa2(C2O4)3  at  25°,  determined  by  the 

electrolytic  Conductivity  method.  (Rimbach  and  Schubert,  1909-) 

SOLUBILITY  OF  SAMARIUM  OXALATE  IN  AQUEOUS  SOLUTIONS  OF  SULFURIC  ACID 

AT  25°. 

(Wirth,  1912.) 

^THSO^      ^i^Gmf.3        Solid  Phase.  NA°r^y of  °pTr  i^Gmf.3         Solid  Phase. 

Aq.H2S04.         *sat.  Sol.  Aq.  H2SO4.     »§•*.  fc^ 

I  O.IOI5         Sa2(C2O4)3.ioH20  2.8  0.3886         Sa2(C2O4)3.ioH2O 

1.445    0.1804       "        4- 32    0.7008 

1.93  0.2254  "  6.175         1.072 

SAMARIUM  Dimethyl  PHOSPHATE   Sa2[(CH3)2PO4]6. 

100  gms.  H2O  dissolve  35.2  gms.  Sa2[(CH3)2PO4]6  at  25°  and  about  10.8  gms. 
at  95°-  (Morgan  and  James,  1914.) 

SAMARIUM   SULFATE   Sa2(SO4)3. 

SOLUBILITY  IN  AQUEOUS  SOLUTIONS  OF  AMMONIUM  SULFATE  AT  25°.* 

(Keyes  and  James,  1914.) 

Clmc     rwvr   Tfv\   rime     TT-O  Cirrtc     r\**r   T/V\  Clmc     TT_O 

Solid  Phase. 


+(NH4)2SO4 


(NH4)2S04. 

Sa2(S04)3. 

ouiiu  .rjiase. 

(NH4)2S04. 

Sa2(S04)3. 

0.03 

2.1 

802(8003 

32.5 

0.9 

0.8 

2 

" 

46.3 

I 

i  .1 

2.8 

"  +1.1.7 

77-5 

i-3 

1.9 

i-5 

1.1.7 

77-3 

o-3 

7-4 

0.8 

« 

76.8 

0.6 

18.8 

0.8 

« 

1.1.7  =Sa2(S04)3.(NH4)2S04.7H20. 

SOLUBILITY  IN  AQUEOUS  SOLUTIONS  OF  SODIUM  SULFATE  AT  25°.* 

(Keyes  and  James,  1914.) 

Gms.  per  too  Gms.  H2O.  Gms.  per  100  Gms.  H2O. 

•N^SO..  •sa.CSO.)..'  SO"dPhaSe-  '  Na,SO..    '  Sa,(SO.).;  "• 

2 . 05  Sa2(SO4),  10.51         0.012       2Sa2(SO4)3.3Na2SO4.6H2O 

O.I  2  "  14.71         0.010 

0.5  O.I  I          2Sa2(S04),.3Na2SO4.6H2O          2O.O2        O.OI2 

1.9        0.03  "  23.68      0.018  " 

6.44      0.016  "  27.40      o.on  " 

*  The  mixtures  were  rotated  at  constant  temperature  for  5  months. 

loo  cc.  anhydrous  hydrazine  dissolve  I  gm.  Sa2(SO4)3  at  room  temp. 

(Welsh  and  Broderson,  1915.) 


595  SAMARIUM   SULFONATES 

SAMARIUM   SULFONATES 

SOLUBILITY  IN  WATER. 

Gm.  An- 
Salt.  Formula.  t°.  J^^G^1  Authority. 

H20. 

Samarium  m  Nitro- 
benzene Sulfonate        SatCjILXNO^SOskyHzO  15      50.9      (Holmberg,  1907.) 
Samarium  Bromonitro- 

benzene  Sulphonate    Sa[C6H3(i)Br(4)N02(2)SO3]3.ioH2O  25        7.84    (Katz  and  James,  1913.) 

SCANDIUM  OXALATE  Sc2(C2O4)3.5H2O. 

SOLUBILITY  IN  AQUEOUS  SOLUTIONS  OF  AMMONIUM  OXALATE  AND  OF  HYDRO- 
CHLORIC ACID. 

In  Aq.  Ammonia  Oxalate  at  25°.  In  Aq.  Hydrochloric  Acid  at  25° 

(Wirth,  1914.)  ,     and  at  50°.     (Meyer,  1914.) 

Gms.  per  100  Gms.  Gms.  Sc2(C2O4)3  per 

Sat.  Sol.                             Solid  Phase.  NoArmsi1& o£               100  Gms.  Sat.  Sol. 

-QOa"               Sc203.  'Atas0.                At  SoV 

1.624             0.3019           Sc2(C2O4)s  SH2O  O.I               0.0299             0.0420 

2.4                  O.40I2               "  0.5               0.0650             0.0870 

4.478              0.7108                "  +(NH4)2C2O4  I                     O.IO20             O.I435 

2  0.1716  0.2556 

5  0.4170          0.6533 

SOLUBILITY  IN  AQUEOUS  SOLUTIONS  OF  SULFURIC  ACID. 


Results  at  25°.     (Wirth,  1914.)               Results  at  25°  and  at  50°.     (Meyer,  1914.) 

Normality  of 
Aq.  H2SO4. 

per  zoo  Gms. 
Sat.  Sol. 

Solid  Phase.           N«ngjgjof 

Gms.  Sc2(C 

'2O4)3  per  100  Gms. 
Sat.  Sol. 

At  25°. 

At  50°. 

I 

0.1148 

Sc,(CA)a.5H*)               O.I 

0.0385 

0.0562 

2.1 

0.2573 

0-5 

0.0997 

0.1481 

2-43 

0.2904 

I 

0.1663 

0.2493 

3-57 

0.4204 

2 

0.3176 

0.4429 

4.86 

0.5834 

5 

0.7761 

I.I280 

100  gms.   sat.  solution  of  scandium  oxalate  in  2.43  n  H2SO4  +  0.5  n  oxalic 
acid  contain  0.0284  gm-  Sc2O3  at  25°.  (Wirth,  1914.) 

SCANDIUM   SULFATE   Sc2(SO4)3.5H2O. 

SOLUBILITY  IN  WATER  AND  IN  AQUEOUS  SULFURIC  ACID  AT  25°.      (Wirth,  1914.) 

Gms.  Sc2(SO4)3  Gms.  Sc2(SO4>3 

Solvent.        per  100  Gms.      Solid  Phase.  Solvent.  per  100  Gms.       Solid  Phase. 

Sat.  Sol.  Sat.  Sol. 

Water  28.52      Sc2(SO4)3.sH2o        4.86wH2S04        8.363        Sc2(SO4)3.sH2o 

o.5wH2S04      29.29  "  9.73ttH2SO4        1.315 

i     wH2SO4      19.87  22.35nH2SO4        0.484        Sc^SO^.sHzO 

Scandium  sulfuric  acid  double  sulfate,  Sc2(SO4)3.3H2SO4.     100  gms.  sat.  sol.  in 
cone.  H2SO4  of  d  =  1.6  contain  0.8616  gm.  of  the  double  salt.  (Wirth,  1914.) 

SEBACIC  ACID  (CH2)8(COOH)2. 

100  gms.  95%  formic  acid  dissolve  1.05  gm.  sebacic  acid  at  19°.      (Aschan,  1913.) 

DISTRIBUTION  OF  SEBACIC  ACID  BETWEEN  WATER  AND  ETHER  AT  25°. 

(Chandler,  1908.) 
Mol.  Concentration  of  Sebacic  Acid  in: 


Ratio. 

Aq.  Layer.  Ether  Layer. 

O.00062          O.O29I  O.O2I3 

O.OOO58          O.O272  O.O2I3 

0.00047          0.0213  0.0221 

0.00036          0.0155  0.0232 


SELENIUM  596 

SELENIUM   Se. 

SOLUBILITY  IN  CARBON  BISULFIDE. 

(Marc,  1906.) 

100  cc.  CSj  dissolve  0.065  gm.  amorphous  Se  at  room  temperature.  Se  which 
is  heated  to  180°  for  6-7  hours  is  insoluble  in  CSa.  Se  crystallized  from  the 
melt  at  200°  is  insoluble  in  CS-j.  Se  heated  once  quickly  to  140°  is  very  slightly 
soluble  in  CSa. 

100  cc.  CSz  dissolve  at  the  boiling-point  3-3.4  mgs.  Se  which  has  been  heated  to 
140°  for  i  hr. 

100  cc.  CSj  dissolve  at  the  boiling-point  2  mgs.  Se  which  has  been  heated  to 
195°  for  2  days.  (Marc,  1907.) 

,100  gms.  methylene  iodide  (CH2I2)  dissolve  1.3  gms.  Se  at  12°.       (Retgers,  1893.) 

SOLUBILITY  OF  Mix  CRYSTALS  OF  SELENIUM  AND  SULFUR  IN  CARBON  DISULFIDE 

AT  25°.      (Ringer,  1902.) 

Mols.  per  100  Mols.  Solution.           Mol.Per  Mols.  per  100  Mols.  Solution.  Mol.  Per 

,—  -  —  -  *-  -  —  -         Cent  Se  in  /-—  -  -*  -  -  -  .  Cent  Se  in 

CSj.                   Se.               S.             Crystals.  CS2-               Se-                S.  Crystals. 

43-i             o    .          56.9            o  58.24        2.35        39.41          55.67 

45-i             o-93         53-97           3-54  64.66         1.58        33.76          68.38 

44.98           1.03         53.99           3.81  8r.ii         2.4           16.49           58.7 

47.84           2.07         50.59           8.69  88.41         2.17          9.42           61.5 

49.54           2.19        48.27         16.4*  91-38        1.68          6.94          65 

47.62           2.16         50.22         14.2*  99-51         °-49           o  ioof 

46.12           1.485      52.39        29-35*  99-14        0.86          o  iooj 
*  Mix  crystals  homogeneous  in  all  except  these  solutions. 

t  =  Solubility  of  hexagonal  selenium.  t   =  Solubility  of  amorphous  selenium. 

Fusion-point  curves  for  mixtures  of  selenium  and  other  metals  are  given  by 
Pelabon  (1909).  Results  for  Se  +  Te  are  given  by  Pellini  and  Vio  (1906). 

Diohenyl   SELENIUM   BROMIDE  (C6H6)2SeBr2. 

"RECIPROCAL  SOLUBILITY  OF  DIPHENYL  SELENIUM  BROMIDE  AND  DIPHENYL 
TELLURIUM  BROMIDE  IN  WATER  AT  25°. 

(Pellini,  igo6a.) 

Gms.  per  1000  cc.  Sat.  SoL         Mo1-  %  (C6H6)r  Qms.  per  1000  cc.  Sat.  Sol.       Mol. 

'(C,H6)2TeBr2.  *    (C6H5)2SeBr2.'      bC  Mixture^'          (QH^TeBr,.  "    (C6H5)2SeBr2.  * 


18.614      °         o  10.224     14.608      44-89 

17.400        1.448         4.91  7.544       19.876        51.18 

16.152      4-172      10.51  6.780     18.984      94-25 

15.030      6.210      18.21  3-184     17.392      95-82 

13.320      8.148      24.98  o        18.984     100 
11.940     11.420      34-94 

SELENIC  ACID   H2SeO4 

SOLUBILITY  IN  WATER,  DETERMINED  BY  FREEZING-POINT  METHOD. 

(Kremann  and  Hofmeier,  1908.) 

Gms.  H2SeO4  Gms.  H2SeO4 

t°.            per  100  Gms.         Solid  Phase.  t°.           per  100  Gms.        Solid  Phase. 

Sat.  Sol.  Sat.  Sol. 

o                         o            Ice  —  55                      71.5      H2SeO4.4H2O 


—  10  21 

—  20  •.  30 
-30  36 
—40                     40 
-50  42.5 


—65  Eutec.  74  "  +H2SeO4.H,0 

—  50  75.5 

-20  79 

o  81 

+20  85 


—60  45  26  m.  pt.  88 

—80  48      '      "  20  91  " 

-95  Eutec.  50  «  +HzSe04.4H20  16  Eutec.  91.5  "  +HfSeO4 

-80  52  H2Se04.4H20  30  93  H2Se04 

-70  54  "  40  94.5 

-60  58  "  50  96.5 

—  51  m.  pt.  67  "  60  loo  " 


597 


SELENIOUS    ACID 


SELENIOUS   ACID 


H2SeO3. 

SOLUBILITY  IN  WATER. 

(Etard,  1894.) 


—  IO 
O 

+  10 
20 


Cms.  H2SeO3  per 
100  Cms.  Solution. 

42.2 

47-4 

55 
62.5 


25 
30 
40 

50 


Cms.  H2SeO3  per 
100  Cms.  Solution. 

67 

70.2 

77-5 
79.2 


60 
70 
80 
90 


Cms.  H2SeO3  per 
100  Cms.  Solution. 

79-3 
79-3 
79-3 
79-4 


SELENIOUS   ANHYDRIDE    (Selenium  Dioxide)  SeO2. 
SOLUBILITY  IN  SEVERAL  SOLVENTS. 

(de  Coninck,  1906.) 
Solvent. 

Water 

Ethyl  Alcohol  (93%) 

Methyl  Alcohol 

Acetone 

Acetic  Acid  (Glacial) 

SILICA  Si02. 

SOLUBILITY  IN  WATER  AND  IN  AQUEOUS  SOLUTIONS  OF  ACIDS. 

(Lenher  and  Merrill,  1917.)    . 

A  platinum  bottle  and  stirrer  were  used.  The  silica  was  prepared  by  adding 
silicon  tetrachloride  to  water.  The  gel  thus  formed  was  washed  until  free  of 
HC1  and  dried  between  filter  papers.  Conductivity  water  was  used  and  equi- 
librium was  reached  within  24  hours.  The  saturated  solution  was  evaporated 
to  dryness  in  a  platinum  dish.  The  residue  was  weighed  and  the  silica  volatil- 
ized with  HF1  +  H2SO4.  The  difference  was  considered  to  show  "the  amount 
of  silica  which  had  changed  from  an  unfiiterable  to  a  filterable  state  of  division." 


t°. 

11-3-15 

Cms.  SeO2  per 
100  cc.  Solvent. 

38.5 

14.1 

ii.  8 

10.2 

6.66 

15-3 

4-35 

12.9 

i.  ii 

At 

25°. 

Per  cent 
HC1. 

0 

Gm.  SiO2  per 
50  cc.  Sol. 

O.OOSo 

3 
6-3 

0.00665 

o  .  00465 

II.  I 
18.9 
25.1 

34-6 

0.00245 
0.0008 
O.OOO6 
0.0003 

Results  for  Aq.  HC1: 


At  90°. 


Results  for  Aq.  H2SO4: 
At  90°. 


Per  cent 
HC1. 

O 
2 
3 

5-4 

7.6 
10 

13.6 

18.6 


Gm.  SiO2  per 
50  cc.  Sol. 

0.0213 
0.0198 

0.0186 
0.0152 
0.0115 
0.0091 
0.0056 
0.0029 


Per  cent 
H2S04. 

Gm.  SiO2  per 
50  cc.  Sol. 

3-9 

0.02II 

7-3 

0.0186 

15.6 

O.OII2 

25.4 

0.0058 

36 

0.0034 

46.9 

0.0013 

55.6 

O.OOO5 

71 

0.0004 

At  90°,  a  slow  current  of  CO2  through  the  solutions  did  not  affect  the  results. 
Ignited  silica  reaches  equilibrium  very  slowly  as  compared  with  silica  gel.  The 
true  solubility  of  ignited  silica  is  probably  the  same  as  that  of  gelatinous  silica. 

SOLUBILITY  OF  SILICA  IN  MELTED  CALCIUM  CHLORIDE. 

(Arndt  and  Lowenstein,  1909.) 


800 
850 
900 
950 


Cms.  SiO2 
per  100  Gms. 
Sat.  Solution. 

2-5 
3-8 

5-4 
7.6 


SILICON   Si  598 

SOLUBILITY  IN  LEAD,  IN  ZINC  AND  IN  SILVER. 

(Moissan  and  Siemens,  1904.) 

In  Lead.  In  Zinc.  In  Silver. 

j.o  Gm.  Si  per  ^ 0  Gm.  Si  per  ^ 0  Gm.  Si  per  ioo  Gms. 

ioo  Gms  Lead.  ioo  Gms.  Zinc.  Silver. 

1250  0.024  600  0.06  970  9.22(58.02) 

1330  O.O7O  650  O.I5  H5O  14.89(27.66) 

1400  0.150  730  0.57  1250  19.26  (19) 

1450  0.210  800  0.92  1470  41.46(16) 

1550  0.780  850  1.62 

The  silicon  which  crystallized  from  the  saturated  solution  in  silver  was  found 
to  be  incompletely  soluble  in  HF.  The  figures  in  parentheses  show  the  per- 
centage soluble  in  HF  in  each  case. 

Freezing-point  data  for  mixtures  of  silicon  tetraphenyl  and  tin  tetraphenyl 
are  given  by  Pascal  (1912). 

SILICON  IODIDES   Si2I6,  SiI4. 

SOLUBILITY  IN  CARBON  DISULFIDE. 

(Friedel  and  Lachburg,  1869;  Friedel,  1869.) 

IOO  gms.  CSa  dissolve  19  gms.  Si2Ie  at  19°. 
IOO  gms.  CSa  dissolve  26  gms.  Si2I6  at  27°. 
ioo  gms.  CSa  dissolve  2.2  gms.  SiI4  at  27°. 

SILICO  TUNGSTIC  ACID   H8SiWi2O42. 

ioo  gms.  H2O  dissolve  961.5  crystallized  silico  tungstic  acid  at  18°,  and  the 
solution  has  Sp.  Gr.  2.843. 

SILVER  Ag. 

For  equilibrium  between  metallic  Silver  and  mercury  (Silver  amalgam)  and 
mixed  aqueous  solutions  of  their  nitrates,  determined  for  mixtures  of  the  two 
metals  in  all  proportions,  see  Reinders,  1906. 

SILVER  ACETATE  CH3COOAg. 

SOLUBILITY  IN  WATER. 

(Nernst,  1889;    Arrhenius,  1893;    Goldschmidt,  1898;    Nauman  and  Rucker,  1905;   Raupenstrauch, 
1885;  Wright  and  Thompson,  1884,  1885.) 

to       Gms.Ag(C2H3O2)  to       Gms.  Ag(C2H3O2)  te      Gms.  Ag(C2H3O2) 

per  Liter.  per  Liter.  per  Liter. 

O  7-22  25  II. 2  50  16.4 

IO  8.75  30  12. I  00  18.9 

15  9.4  40          14- r  7°          2I-8 

20  10.4  80  25.2 

SOLUBILITY  OF  SILVER  ACETATE  IN  AQUEOUS  SOLUTIONS  OF: 
Silver  Nitrate.  Sodium  Acetate. 


Gms.  CH3COOAg  per  Liter  at:  rnJrOON  Gms-  CH3COOHg  per  Liter  at: 

pergLiter.  16°  (Nernst).  'i9.8°(Arrhenius).  per  Liter  *  '16°  (N.,N.andR.).  i8.6°(A.).  ' 

o  10.05  9-^5  o            10.05            9-9 

5  8.2  7.9  5              6.3              6.6 

10  7  .o  6.6  10             4.6             4.9 

15  6-4  5-5  J5              3-8              4-i 

20  5.7  4-5  20             3-3              3-5 

30  4.4  ...  30              ...              2.8 

40  3.2  ...  40              ...              2.4 


599  SILVER  ACETATE 

SOLUBILITY  OF  SILVER  ACETATE  IN  AQUEOUS  SALT  SOLUTIONS  AT  25°.  (jaques,  1910.) 

Aq.  Solution  of; 


Water  alone 

Cadmium  Acetate 

ii  ii 


Lead  Acetate 


o 

ii.  08 

i-i5 

10.39 

5.76 

8.10 

11.52 

6.71 

57-6 

4-33 

115.2 

3-95 

1.63 

10.69 

8.13 

9-45 

16.26 

8-34 

81.3 

7.26 

162.6 

5-99 

Aq.  Solution  of: 

Potassium  Acetate 


Silver  Nitrate 


Sodium  Acetate 


Gms.  Salt 
per  Liter. 

2.22 

Gms. 
AgCjHA 
per  Liter. 

9.60 

22.2 

4-43 

III 
222 

2.41 
2.18 

2.77 

9-93 

5-55 

9 

II.  10 
22.21 

7.41 
5-8i 

1.97 

9.27 

19.7 
98.5 

4.21 
2-33 

197 

2.07 

SOLUBILITY  OF  SILVER  ACETATE  IN  AQUEOUS  SOLUTIONS  OF  NITRIC  ACID  AT  25°. 

(Hill  and  Simmons,  1909.) 


Normality  of 
Aq.  HNO3. 

Per  cent  HNO3  in 
Solvent.                         S 

4*  of 
at.  Sol. 

Gms.  AgQHsOj 
per  Liter  Sat.  Sol. 

0 

0                                   ] 

[.005 

11.13 

0.50 

3.096                         ] 

[.072 

85-3I 

I 

6.128                         ] 

.I4O 

161.9 

2 

11.757                -a 

.267 

307-4 

4.02 

22.386                3 

.470 

549-3 

5-03 

27.328 

.561 

656 

6.44 

r    _  -u_  _-i-.t-Mr.i-  t  A  _./• 

.670 

792.2 

Results  are  also  given  for  the  solubility  of  AgC2H3O2+AgNO3  in  Aq.  HNO3at  25°. 
SOLUBILITY  OF  SILVER  ACETATE  IN  AQUEOUS  SOLUTIONS  OF  SEVERAL 

COMPOUNDS  AT  25°.      (Armstrong  and  Eyre,  1913.) 


Gms. 


Gms. 


Aqueous 
Solution  of: 


wuiiipouuu 
per 
1000  Gms. 

rtg^2n3^f2 

per  1000 
Gms. 

Aqueous 
Solution  of: 

H20. 

Sat.  Sol. 

0 

II.  08 

Propyl  Alcohol 

II 

10.13 

II 

8.92 

Glycerol 

33 

9.16 

Glycol 

66.4 

7-55 

u 

Water 
Acetaldehyde 

Paraldehyde 
ii 

Isobutyl  Alcohol 

SILVER  MonochlorACETATE  CH2ClCOOAg. 

One  liter  aqueous  solution  contains  12.97  gms.  CHjClCOOAgat  16.9°.  (Arrhenius/93.) 


Gms. 

Gms. 

Compound 

per 
looo  Gms. 

per  1000 
Gms. 

H20. 

Sat.  Sol. 

15 

9.88 

60 

8.03 

9.21 

8.66 

15-5 

10.86 

62.1 

8.44 

SOLUBILITY  OF  SILVER  MONO  CHLOR  ACETATE  AT   16.9 
AQUEOUS    SOLUTIONS    OF: 


IN 


Silver  Nitrate. 


Sodium  Chlor  Acetate. 


Gms. 
AgNOa 
per  Liter. 

Gms. 
CH2ClCOOAg 
per  Liter. 

Gms. 
CH2ClCOONa 
per  Liter. 

Gms. 
CH2ClCOOAg 
per  Liter. 

0-0 

9.6 
17.0 

12-97 
10.05 

7-55 

O-O 
3.88 

7-77 
15-53 

12.97 
10.05 
8.16 

6.  02 

31.07 
58.26 

4.19 
3.26 

SILVER  ACETATE 


600 


SOLUBILITY  OF  SILVER  MONOCHLORO  ACETATE  IN  NITRIC  ACID  AT  25°. 

(Hill  and  Simmons,  1909.) 


Normality 

Gms.  HN03 

Gms. 

of  Aq. 
HN03. 

per  100  Gms. 
Solvent. 

Sa*  Sol. 

AgC2H2C102 
per  Liter. 

0 

0 

.0095 

I5.I8 

0.25 

1.564 

.0426 

50.33 

0.50 

3.096 

.0791 

91.83 

I 

6.128 

•1473 

167.3 

2 

n-757 

.2716 

310.8 

4 

22.277 

•4749 

549-1 

5 

27.185 

•5673 

659.2 

SILVER  Dipropyl  ACETATE  AgC8H15O2. 

100  gms.  H2O  dissolve  0.123  gm.  AgC8Hi502  at  11.7°,  and  0.190  gm.  at  72°. 


(Fiirth,  1888.) 


SILVER  Methyl  Ethyl  ACETATE  Ag.CH3.CH2CH(CH3)COO. 
SILVER  Diethyl  ACETATE  Ag[(C2H5)2CH.COO]. 
SILVER  Trimethyl  ACETATE  Ag(CH3)3CCOO.* 


SOLUBILITY  OF  EACH  IN  WATER. 

(Sedlitzky,  1887;  Keppish,  1888;  Stiassny,  1891.) 


Gms.  per  100  Gms.  H2O. 


Gms.  per  100  Gms.  H2O. 


I  . 

Ag.C5H902. 

AgC.HuOj. 

AgC5H902.* 

i  . 

AgCBH902. 

AgC.HuO,. 

AgC5H902.* 

0 

I  .112 

0.402 

1.  10 

50 

I.  602 

0-536 

i-47 

10 

I  .126 

0.413 

I-I5 

60 

1.827 

0.585 

i-57 

20 

I.I82 

0.432 

1.22 

70 

2.093 

0.643 

1.68 

30 

1.280 

0.458 

1.22 

80 

2.402 

i.  80 

40 

I  .420 

0.494 

1-37 

SILVER  ARSENATE  Ag3AsO4. 

One  liter  H2O  dissolves  0.0085  gm.Ag3AsO4  at  20°.    See  Note,  p.  608.   (Whitby,  1910.) 

SILVER  ARSENITE   Ag3AsO3. 

One  liter  H2O  dissolves o.oi  15  gm.  Ag3AsO3at  20°.    See  Note,  p.  608.   (Whitby,  1910.) 

SILVER  BENZOATE  C6H6COOAg. 

One  liter  of  aqueous  solution  contains  1.763  gms.  C6H5COOAg  at  14.5°,  and  2.607 
gms.  at  25°.  (Holleman,  1893;  Noyes  and  Schwartz,  1898.) 

SOLUBILITY  OF  SILVER  BENZOATE  AT  25°  IN  AQUEOUS  SOLUTIONS  OF: 


Gms.  per  Liter. 


Nitric  Acid  (N.  and  S.). 
Gms.  Mols.  per  Liter.              Gms.  per  Liter. 

Chloracetic  Aci< 
Gms.  Mols.  per  Liter. 

HNO3. 

COOAg. 

HNO3. 

C«H6 
COOAg. 

C1COOH. 

C6H5 
COOAg. 

0 

0 

.01144 

O 

2  .607 

O 

0 

.01144 

0 

-004435 

0 

•01395 

O 

.280 

3-195 

o 

.00394 

0 

.01385 

0 

.00887 

O 

.01698 

O 

•559 

3.889 

0 

,00787 

O 

.Ol6l2 

O 

.00892 

0 

.01715 

O 

.562 

3.926 

o, 

01574 

0 

.02093 

O 

.01774 

0 

.02324 

X 

.118 

5-321 

O 

.02674 

0 

.03071 

I 

.686 

7.031 

CH2 


C6H6 


C1COOH.  COOA5g. 

o  2.607 

0.371  3.172 

0.744  3.691 

1.487  4.792 


One  liter  of  cold  alcohol  dissolves  0.169  gm.  C6H6COOAg;  one  liter  of  boiling 
alcohol  dissolves  0.465  gm.  (Liebermann,  1902.) 

SILVER  BORATE  AgBO2. 
One  liter  of  aqueous  solution  contains  about  9.05  gms.  AgBO2  at  25°. 

(Abegg  and  Cox,  1903.) 


Normality  of  Aq. 
Acetic  Acid. 

o  .  0498 

0.0997 
0.1995 

Gms.  AgBrO3  per 
Liter. 

1.9429 

1-9379 
1.9206 

Normality  of  Aq. 
Acetic  Acid. 

0.4988 

0-9975 
1.8721 

6oi  SILVER   BROMATE 

SILVER  BROMATE  AgBrO3. 

SOLUBILITY  IN  WATER. 

t°.  Cms.  AgBrO3  per  Liter.  Authority. 

20  I  .  586  (BSttger,  1903.) 

24.5  I.gil  (Noyes,  1900.) 

25  1.68  (Longi,  1883.) 

27  I  .  71  (Whitby,  1910,  see  note,  p.  608.) 

25  1-949  (Hill,  1917.) 

SOLUBILITY  OF  SILVER  BROMATE  IN  AQUEOUS  ACETIC  ACID  AT  25°. 

(Hill,  1917-) 

Cms.  AgBrO3  per 
Liter. 

1.863 

I.80I3 

1.6178 

SOLUBILITY  OF  SILVER  BROMATE  IN  AQUEOUS  AMMONIA  AND  NITRIC 
ACID  SOLUTIONS  AT  25°. 

(Longi,  1883.) 

Gms.  AgBrO3  per 

Solvent.  , -T-5 i±I _, 

1000  cc.  Sol.      1000  Gms.  Sol. 

Ammonia         Sp.  Gr.  0.998  =  5%  35.10          35.54 

Ammonia         Sp.  Gr.  0.96    =  10%         443.6          462.5 
Nitric  Acid      Sp.  Gr.  1.21    =35%  3.81  3.12 

SOLUBILITY  OF  SILVER  BROMATE  AT  24.5°  IN  AQUEOUS 
SOLUTIONS  OF: 

Silver  Nitrate  (Noyes).  Potassium  Bromate  (N.). 

Normal  ^Content.  Gms.  per  Liter.  Normal  Content.  Gms.  per  Liter. 

AgN03.        AgBr03."  'AgNOs-        AgBrO3.          KBrO3.          AgBrO3".  KBrO3.    AgBrOi 

o.o    0-0081    o.o    1.911    o.o    0.0081    o.o   1.911 
0.0085  0.0051    1-445  I-203    0.0085  0.00519    1-42  1-225 

0.0346   0.0022      5.882   0.510     0.0346   0.00227     5.78   0.536 

SILVER    BROMIDE   AgBr. 

SOLUBILITY  IN  WATER. 

t  °.  Gms.  AgBr  per  Liter.  Authority. 

2O  O  -000084  (Bottger  — Z.  physik.  Ch.  46,  602,  '03.) 

25  O  .OOOI37  (Abegg  and  Cox  —  Z.  physik.  Ch.  46,  u,  '03.* 

IOO  O  •  OO3 70  (Bottger  —  Z.  physik.  Ch.  56,  93,  '06.) 

(See  alsoHolleman  —  Z.  physik.  Ch.  12,  129,  '93;  Kohlrausch  —  Ibid.  50,  365,  '05.) 

SOLUBILITY  OF  SILVER  BROMIDE  IN  AQUEOUS  AMMONIA  SOLUTIONS. 

(Longi  —  Gazz.  chim.  ital.  13,  87,  '83;  at  80°,  Pohl  —  Sitzber.  Akad.  Wiss.  Wien,  41,  267,  '60.) 

Gms.  AgBr  at  12°  per  Gms.  AgBr  at  80°  pet 

Solvent.  1000  cc.  1000  Gms.  IO°°1 Gms- 

Solvent.  Solvent.  Solvent. 

Ammonia  Sp.  Gr.  0.998=5%      0.114          0.114  ... 

Ammonia  Sp.  Gr.  0.96  =10%    3-33-4-0    3.47 

Ammonia  Sp.  Gr.  0.986  ...  0.51*1.0! 

*  Dried  AgBr.  t  Freshly  pptd. 


SILVER  BROMIDE 


602 


SOLUBILITY  OF  SILVER 

Results  at  15°. 
(Bodlander,  1892.) 


BROMIDE  IN  AQUEOUS  AMMONIA  SOLUTIONS. 

Results  at  25°.  Results  at  25°. 

(Bodlander  and  Fittig,  1901-02.)      (Whitney  and  Melcher,  1903.) 


<*lfi.5  Of 

Sat.  Sol. 

Cms.  Mols.  per  Liter.        Gms.  Mols.  per  roc 

o  Gms.  H2O. 

G 

oncentrat 

ion 

per  Liter. 

'NH3. 

Ag2Br2. 

NH3. 

AgBr. 

G.  Mols.  NH3. 

G 

.  Atoms  Ag. 

0.9932 

1.085 

0 

.0011 

0 

.1932 

0 

.OOO6O 

0 

.0764 

0 

.000276 

0-9853 

2.365 

o 

.0031 

o 

.3849 

o 

.00120 

0 

•115 

O 

.000391 

0.9793 

3.410 

0 

.0050 

0 

•7573 

0 

.00223 

0 

.268 

O 

.000941 

O.972O 

4-590 

0 

.0074 

I 

•965 

0 

.00692 

o 

•273 

0 

.00107 

O-Q^SS 

5-725 

0 

.OIOI 

3 

.024 

o 

.01163 

o 

•450 

0 

.00170 

5.244   0.02443   0.497  0.00159 


SOLUBILITY  OF  SILVER  BROMIDE  IN 
Ammonia  at  o°. 

(Jarry,  1899.) 
Grams  per  TOO  cc.  Solution. 


AQUEOUS  SOLUTIONS  OF: 

Monomethyl  Amine  at  11.5°. 

(Jarry.) 
Gms.  per  100  cc.  Solution. 


NHsGas. 

AgBr. 

NH3  Gas. 

AgBr. 

3-07 

O.oSo 

26.27 

1.067 

4.88 

0-096 

31.26 

1.568 

6.69 

O.I72 

33-89 

I.987 

8.29 

0.212 

36-52 

2  .669 

11.51 

c-349 

37-22 

2.888 

I5-32 

o-557 

37-70 

2.930 

18.09 

0.722 

39.26 

2.892 

19-53 

0.741 

39-95 

2.852 

NH2CH3. 

AgBr. 

II  .01 

O.O7 

13  .  17 

O.I2 

J5  •I3 

0.16 

17.97 
32-58 
35-62 

0.28 

o-55 
o-73 

43  •" 

48.44 

1.27 
2.89 

SOLUBILITY  OF  SILVER  BROMIDE  IN  AQUEOUS  SOLUTIONS  OF  METHYL 
AMINE  AND  OF  ETHYL  AMINE  AT  25°. 

(Bodlander  and  Eberlein,  1903;  Wuth,  1902.) 

In  Methyl  Amine.  In  Ethyl  Amine. 

Mols.  per  Liter.  Mols.  per  Liter. 


Total  Base.       AgBr.       Free  Base.* 

1.017  0.0025  i. 012  (B.&E.) 

0.508  0.0013  0.505  (B.&E.)    0.200 

0.203  0.00049  0.202  (B.&E.,  W.)  o.ioo 

0.102  0.00026  o.io2(B.&E.)    0.103 


0.00026  o.io2(B.&E.) 

0.0947  0.00041  ...  (W.) 

0.051  0.00012  0.051  (B.&E.) 

0.04   0.00034  ...  (W.) 

O.O2         O.OOO26  ...      (W.) 


Total  Base.          AgBr.      Free  Base.* 

0.483   0.00231  0.478  (B.&E.) 
0.00097  0.198   " 
0.000475  0.099   " 
0.000711  . . .  (W.) 
0.06572  0.000258   ...   " 
0.05512  0.000193  •  •  •  " 
0.03942  0.000137  •  •  •  " 
0.01272  0.0000867 


*  The  free  base  is  found  by  subtracting  from  the  total  base  two  mols.  of  base  for  each  atom  of  dissolved  Ag. 

SOLUBILITY  OF  SILVER  BROMIDE  IN  AQUEOUS  SOLUTIONS  OF  MERCURIC 
NITRATE  AT  25°. 

(Morse,  1902.) 

Mols.  HgNOr        Mols.  AgBr        Gms.  AgBr 
(HNOs)  per  Liter.       per  Liter.  per  Liter. 

I  0.03660  6.878 

o.io          0.00873        1.640 

o .  05  o .  0063.9        T  •  2O° 

Since  HNO3  was  present  in  all  cases,  its  influence  on  the  solubility  was  ex- 
amined. It  was  found  that  no  appreciable  differences  were  obtained  with  con- 
centrations varying  between  o.i  and  2  normal  HNOa.  Both  crystallized  and 
amorphous  silver  bromide  gave  identical  results. 


Mols.  HgNOr 
(HN03)  per  Liter. 
0.025 
O.OI25 
O.OIOO 

Mols.  AgBr 
per  Liter. 

0.00459 
0.00329 

o  .  00306 

Gms.  AgBr 
per  Liter. 

0.863 

0.618 
0-575 

603  SILVER  BROMIDE 

SOLUBILITY  OF  SILVER  BROMIDE  IN  AQUEOUS  SALT  SOLUTIONS. 

(Mees  and  Piper,  1912.) 

Aqueous  Solution.  t°.         Gms.  AgBr 

per  Liter. 

Aq.  i  per  cent  Sodium  Thiosulf ate  ?  2 . 06 

"       Ammonium  Thiocyanate  0.03 

"            "       Ammonium  Carbonate  "  0.004 

"            "       Sodium  Sulfate  "  0.055 

"            "       Thiocarbamide  "  1.49 


SOLUBILITY  OF  SILVER  BROMIDE  IN  AQUEOUS  SALT  SOLUTIONS. 

(Valenta,  1894;  see  also  Cohn,  1895.) 

Gms.AgBr  per  100  Gms.Aq.  Solution  of  Concentration: 

Salt  Solution.  t°.      / * > 

1:100.         5:100.         10:  100.       15:100.       20:100. 

Sodium  Thio  Sulphate  20  0.35       1.90  3.50  4.20      5.80 

"               "  Calc.  by  Cohn  20  0.50       2.40  4.59  6.58      8.40 

Sodium  Sulphite  25  ...          ...  0.04        ...        0.08 

Potassium  Cyanide  25  ...        6.55 

"  Calc.  by  Cohn  25  ...        6.85  

Potassium  Sulphocyanide  25        0.73        

Ammonium  Sulphocyanide  20  ...        0.21  2.04  5-30 

Calcium  Sulphocyanide  25        0.53        

Barium  Sulphocyanide  25        0.35        

Aluminum  Sulphocyanide  25  ...          ...  4.50        

Thio  Carbamide  25        1.87        

Thio  Cyanime  25  0.08      0.35  0.72        

NOTE.  —  Cohn  shows  that  the  lower  results  obtained  by  Valenta  are  due  to  the 
excess  of  solid  AgBr  used  and  the  consequent  formation  of  the  less  soluble  di  salt, 
3(AgS2O3Na)2,  instead  of  the  more  soluble  tri  salt,  (AgS^OsNa^NazSzOs. 

100  cc.  H2O  containing  10  per  cent  of  normal  mercuric  acetate,  Hg(C2H3O2)2-h 
Aq.f  dissolve  0.0122  gm.  AgBr  at  20°. 

100  gms.  NaCl  in  cone.  aq.  solution  dissolve  0.474  g™-  AgBr  at  15°. 

100  gms.  NaCl  in  21  per  cent  solution  dissolve  0.182  gm.  AgBr  at  15°. 

100  gms.  KBr  in  cone,  solution  dissolve  3.019  gms.  AgBr  at  15°. 

95  gms.  NaCl  +  10  gms.  KBr  in  cone.  aq.  solution  dissolve  0.075  gm.  AgBr 
at  15°.  (Schierholz,  1890.) 

SOLUBILITY  OF  SILVER  BROMIDE  IN  AQUEOUS  POTASSIUM  BROMIDE  AT  25°. 

(Hellwig,  1900.) 

Mols.  KBr  per  Liter       2.76        3.68          4.18          4.44          4.864 
Gms.  KBr  per  Liter        2.20        7.50        13.50        17 .95        26.44 

SOLUBILITY  OF  SILVER  BROMIDE  IN  AQUEOUS  SOLUTIONS  OF  SODIUM  SULFITE. 

Results  at  Room  Temperature  (?).  Results  at  25°. 

(Mees  and  Piper,  1912.)  (Luther  and  Leubner,  i9i2a.) 


Gms. 

per  Liter. 

Gms.  per  Liter. 

Gms.  Formula  Weights 
per  Liter. 

Na2SO3. 
0.08 
0.17 
0.30 

o-59 
1-13 

2.08 

AgBr. 

o  .  000746 

O  .  OO2  19 
0.00393 

o  .  00448 

O.OO865 
0.01585 

Na^Oa. 
4.85 

9-47 

I7-65 

3^.2 

70.75 
83.75 

AgBr. 
0.0329 
0.05264 

0.116 
0.265 

0-57 
0.79 

S03". 
0.232 
0.406 
0.448 
0.466 

0-474 
0.675 

Ag'. 
O.OO25 
0.0023 
0.0023 
0.0053 
0.0055 
0.0084 

SILVER  BROMIDE 


604 


SOLUBILITY  OF  SILVER  BROMIDE  IN  AQUEOUS  SOLUTIONS  OF  SODIUM 
THIOSULFATE  AT  35°. 

(Richards  and  Faber,  1899.) 


Cms.  Cryst.  Na 
Thiosulfate 
per  Liter. 

Cms.  AgBr 
Dissolved  per  Gm. 
of  Thiosulphate. 

Mols.  AgBr 
Dissolved  per 
Mol.  of  Na«SA. 

100 

0.376 

0.496 

2OO 

0.390 

0-SI5 

300 
400 

o-397 
0.427 

,        0.524 
0.564 

100  cc.  of  3  n  AgNO3  solution  dissolve  0.04  gm.  AgBr  at  25°.          (Hellwig,  1900.) 

Fusion-point  data  for  mixtures  of  AgBr  +  AgCl  and  AgBr  +  Agl  are  given  by 
Monkemeyer  -(1906).  Results  for  AgBr  +  NaBr  are  given  by  Sandonnini  and 
Scarpa  (1913)- 

SILVER  BUTYRATE  C3H7COOAg. 

SILVER   (Iso)BUTYRATE  (CH3)2CHCOOAg. 

SOLUBILITY  OF  EACH  SEPARATELY  IN  WATER. 

(Goldschmidt,  1898;  Arrhenius,  1893;  Raupenstrauch,  1885.) 


Cms.  per  too  Gms.  H2O. 


Cms.  per  100  Gms.  H2O. 


I  .         f—  — 

Butyrate. 

—  —  >        I/  . 
Iso  Butyrate. 

Butyrate. 

Iso  Butyrate. 

O 

O 

.363 

0.796 

30 

0. 

561 

I 

.060 

(l.I022) 

10 

O 

.419 

0.874 

40 

O. 

647 

I 

.176 

(R.) 

I7.8 

0 

.432 

(A.) 

50 

O. 

742 

I 

.313 

18.8 

0 

-445 

(A.) 

60 

O. 

848 

20 

O 

.484 

0.961 

(0.9986) 

70 

0. 

964 

I 

.670 

25 

. 

(1.0442) 

80 

I  . 

14 

I 

.898 

SOLUBILITY  OF  SILVER  BUTYRATE  IN  AQ.  SOLUTIONS  OF  SILVER  ACETATE, 
SILVER  NITRATE  AND  OF  SODIUM  BUTYRATE. 

(Arrhenius,  1893.) 

In  Silver  Acetate  at  17.8°.  In  Silver  Nitrate  at  18.8°. 


G.  Mols, 

,  per  Liter. 

Grams  per  Liter. 

G.  Mols^per  Liter. 

Grams  per  Liter. 

COOAg. 

C3H7 
COOAg. 

'   CH3 
COOAg. 

C3H7 
COOAg. 

AgNO3. 

C3H/ 
COOAg. 

AgNOa- 

COOAg. 

0.0 

O-O22I 

o.o 

4-32 

o.o 

O.O228 

o.o 

4-445 

0.0270 

0.0139 

4-51 

2.71 

0.0667 

0.0078 

n-33 

1.521 

0.0506 

O.OIO3 

8-45 

2  -OI 

O.IOO 

O.OO62 

17.00 

1.209 

G.  Mols.  per  Liter. 
COONa.       COOAg. 

o.o          0.0224 

O.OO66  O.OI99 
0.0164  0.0169 
0-0329  O.OI3I 


In  Sodium  Butyrate  at  18.2°. 


Grams  per  Liter. 

COONa.    COOAg 

0-0         4-363 
0.73      3-881 

1.81     3.296 
3-62     2.555 


G.  Mols.  per  Liter. 

'    C3H7  C3H7  ' 

COONa.  COOAg. 

0-0658  O.OO9I 

0.1315  0-0060 

0.263  O.OO4O 

0.493  O-OO27 


Grams  per  Liter. 


C3Hr 
COONa. 

7-24 
14-47 


COOAg. 

1-774 

.170 


28.96     0.780 

54.28    0.526 


605  SILVER   CAPROATES 

SILVER   CAPROATES  Ag(C6HnO2). 

SOLUBILITY  OF  EACH  SEPARATELY  IN  WATER. 

(Keppish,  1888;  Stiassny,  1891;  Kulisch,  1893;  Konig,  1894;  Altschul,  1896.) 
Results  in  terms  of  gms.  salt  per  100  gms.  H2O. 


a  Methyl  Pentan 

Methyl  3  Pentan      4  Methyl  Pentan 

Normal  Caproate                         4  Acid 

Acid  4                     4  Acid 

»«. 

CH3(CH2)4COOAg.                   CH3.CH.CHa 

CH3.CH2            CH3(CH2)2CH(CH3) 
.CHCH3CH2COOAg.      .COOAg. 

.(CH2)2COOAg. 

o 

0.076  (A.)     0-078(Keppish)     O.l68  (Konig)     o  .880  (Kulish)   o  .510  (Stiassny) 

10 

0-085              0.089                     O.l62 

0.858                   0.528 

20 

o.ioo          0.107                 0.163 

0.849             °-55° 

3° 

O..I23          0.131                0.170, 

0.854             0.574 

40 

0.154          0.161                 0.183 

0.871             0.602 

5° 

0.193              0.198                      0.203 

0.902             0.632 

60 

0.240              0.243                      0.229 

o  .  946              o  .  666 

7o 

0.295              0-288                      0.263 

i  .  003              o  .  702 

80 

0-354                                                 0.300 

1.073              °-742 

90 

0-347 

1.157 

SILVER  CARBONATE  Ag2CO3. 

SOLUBILITY  IN  WATER. 

t°.      Gms.  Ag2CO3  per  Liter. 

Authority. 

15                 0.031 

(Kremers,  1852.) 

25                 0  .  033    (0.00012  gm.  atoms  Ag.) 

(Abegg  and  Cox,  1903.) 

25                 0.032    (by  potential  measurement)          (Spencer  and  Le  Pla,  1909.) 

loo            0.50 

(Joulin,  1873.) 

15                 0.85      (in  H2O  sat.  with  COz) 

(Johnson,  1886.) 

SILVER   CHLORATE  AgClO3. 

100  gms.  cold  water  dissolve  10  gms.  AgClO3  (Vauquelin);  20  gms.  AgC103 
(Wachter). 

SILVER   CHLORIDE  AgCl. 

SOLUBILITY  IN  WATER. 

(A  large  number  of  determinations  are  quoted  by  Abegg  and  Cox,  1903;  see  also  Kohlrausch,  1904-  05; 
Bottger,  1903,  1906.) 

t°.  14°.  20°.  25°.  42°.  100°. 

Gms.  AgCl  per  Liter          0.0014    0.0016    0.0020    0.0040    0.0218 
More  recent  determinations  are  as  follows: 

**•  Gw'uf£l                      Method'  Authority. 

10  0  .  00089  Conductivity  (Kohlrausch,  1908.) 

l8  O.OOI5O  Conductivity  (Melcher,  1910.) 

21  O  .  OOI  54  Colorimetric  (See  Note,  p.  608)         (Whitby,  1910.) 

25  0.00172  Analytical  (Glowczynski,  1914.) 

5O  0.00523  Conductivity  (Melcher,  1910.) 

IOO  O.O2IO7  (Melcher,  1910.) 

loo          0.0217          Colorimetric  (Whitby,  1910.) 

Note  in  the  case  of  determination  by  Glowczynski,  one  liter  of  sat.  solution  was  treated  with  freshly  dis- 
tilled ammonia  and  evaporated  to  dryness  in  a  platinum  dish.  The  residue  was  dissolved  in  strong  am- 
monia and  again  evaporated.  The  residue  then  dissolved  in  5-6  cc.  of  0.05  n  KCN  and  the  silver  separated 
electrolytically,  dissolved  in  HNO3  and  titrated  with  o.oi  n  NH<SCN. 

Comparative  determinations  of  the  solubilities  of  AgCl,  AgSCN,  AgBr  and  Agl 
in  water  at  25°,  showed  that  if  the  solubility  of  AgCl  be  taken  as  I,  that  of  AgSCN 
is  0.0748,  that  of  AgBr  is  0.0550  and  that  of  Agl  is  0.00077.  (Hill,  1908.) 


SILVER   CHLORIDE 


606 


SOLUBILITY  OF  SILVER  CHLORIDE  IN  AQUEOUS  AMMONIA  SOLUTIONS  AT  25°. 


(Whitney  and  Melcher,  1903.) 


Gm.  Mols. 

Gm.  Atoms 

NH,  (total) 
per  Liter. 

Ag 
per  Liter. 

0.0282 

O.OCI4I 

0.0288 

O.OOI49 

0.0590 

o  .  00304 

O.II8 

0.00621 

0-253 

O.OI4O 

o-397 

0.0227 

0.428 

O.O249 

0.818 

0.0514 

0.863 

0.0541 

0.896 

0.0569 

0.909 

0.0584 

0.961 

0.0616 

1.991 

0.147 

2.042 

0.151 

(Straub,  1911.) 


Gm.  Mols. 

Gm.  Atoms 

NH,  (total)  per 
looo  Cms.  H2O. 

Ag  per 
looo  Gins.  H2O. 

Solid  Phase. 

0.0428 

O.O25 

AgCl 

1.688 

0.1308 

" 

3.782 

0.372 

" 

3-945 

0.378 

" 

5-io 

0-574 

" 

5-33 

0.609 

" 

5-545 

0-633 

" 

6.26 

0-754 

"    +2AgCl.3NH, 

6.52 

0-775 

2AgC1.3NH, 

8.28 

0.848 

" 

11.78 

0.980 

" 

12.68 

1.030 

" 

12.96 

I  .090 

K 

14.47 

1.039 

« 

Additional  data  for  the  above  system  at  25°  are  given  by  Bodlander  and  Fittig 
(1901-02).  These  authors  also  give  results  showing  the  effect  of  KC1  and  of 
AgNOs  on  the  solubility  of  AgCl  in  aqueous  ammonia.  Determinations  at  15° 
are  given  by  Bodlander  (1892), 


SOLUBILITY  OF  SILVER  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF: 

Monomethyl  Amine  at  11.5°. 
(Jarry.) 

Gms.  per  100  Gms.  Solution. 


Ammonia  at  o°. 
(Jarry,  1899.) 

Gms.  per  100  Gms.  Solution. 

NH3  Gas. 

i-45 

2.94 
5-6o 
6.24 
11.77 
16.36 

AgCl. 
0.49 
1.36 

3-44 
4 
4.68 

5-i8 

NH3  Gas. 
28.16 
29.80 
30.19 

32.43 
34.56 
37-48 

AgCl. 
6.50 
7.09 
7-25 
5-87 

4-77 
3-90 

NH2CH3. 

AgCl. 

I.78 

0.16 

4.44 

0.62 

5-51 

0.83 

7.66 

1.32 

13.70 

3-29 

18.69 

5-43 

36.69 

9-93 

SOLUBILITY  OF  SILVER  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  AMMONIA. 


(Longi,  1883;  at  25°,  Valenta,  1894;  at  80°,  Pohl,  1860.) 
Solvent.  t°. 


Aq.  Ammonia  of  o .  998  Sp.  Gr.  =  5% 
0.96    Sp.  Gr.  =  10% 
"  o.986Sp.  Gr. 

=  3% 


12 
18 
80 
25 
25 


Gms.  AgCl  per 
too  Gms.  Solvent. 

0.233 
7.84 
1.49 
1.40 

7-58 


607  SILVER   CHLORIDE 

SOLUBILITY  OF  SILVER  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  METHYL 
AMINE  AND  OF  ETHYL  AMINE  AT  25°. 

(Bodlander  and  Eberlein,  1903;  Wuth,  1902;  Euler,  1903.) 

Results  for  Methyl  Amine.  Results  for  Ethyl  Amine. 

Mols.  per  Liter.  Mols.  per  Liter. 


Total  Base. 
I.OI7 

0 

AgCl. 
.0387 

Free  Base. 

0.940  (B.  &E.) 

Total  Base. 
0.483 

0 

AgCl. 

.0314 

Free  Base. 

0.420  (B.  & 

\ 

E.) 

0-93 

O 

•0335 

.  .  . 

(E.) 

0.200 

0 

.0115 

0.177 

" 

0.508 

0 

.0178 

0 

.472 

(B.  &  E.) 

O.  IOO 

0 

,0062 

0.088 

u 

0.203 

0 

.0068 

0 

.189 

lt 

0.094 

0, 

,0048 

.  .  . 

(E.) 

0.102 

o 

,0036 

o 

.0050 

11 

0.050 

0 

0029 

0.044 

(B.  & 

E.) 

0.195 

0. 

00048 

(W.) 

0.103 

0. 

00824 

(W.) 

0.074 

0, 

00042 

tt 

0.0551 

0. 

000235 

.  .  . 

M 

O.O2O 

0. 

00030 

</f 

O.OI27 

0. 

000114 

11 

SOLUBILITY  OF  SILVER  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  AMMONIUM 

CHLORIDE. 

(Schierholz,  1890;  see  also  Vogel,  1874;  Hahn,  1877.) 

Solubility  at  15°.  Solubility  at  Different  Temperatures. 

Gms.  per  100  Gms.  Solution.  Gms.  per  100  Cms.  Solution. 


NH4C1. 

AgCl. 

I/  . 

NH4C1. 

AgCl. 

IO 

0.0050 

15 

26.31 

0.276 

14.29 

0.0143 

40 

tt 

0.329 

17.70 

0-0354 

60 

tt 

0.421 

19.23 

0.0577 

80 

tt 

0.592 

21.91 

O.IIO 

90 

tt 

0.711 

25-3I 

0.228 

IOO 

U 

0.856 

28.45 

0.340  (24.5) 

no 

tt 

1-053 

Sat.  at  ord.  temp.     p.  157  Sp.  Gr.  of  26.31%  NH^Cl  solution 

at  15°  =  i. 08. 

One  liter  aq.  sol.  containing  0.00053  gm.  NH4C1  dissolves  0.001604  Sm- 
at  25°. 

One  liter  aq.  sol.  containing  0.00530  gm.  NH4C1  dissolves  0.002379  gm.  AgCl 

at  25°.  (Glowczynski,  1914.) 

SOLUBILITY  OF  SILVER  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  AMMONIUM 
CHLORIDE  AT  25°.       (Forbes,  1911.) 

Gms.  Equiv.  per  Liter.  Gms.  Equiv.  per  Liter.  Gms.  Equiv.  per  Liter. 

'NH4C1.  A^  'NH4C1.  A^  '  NH4C1.  Ag^ 

0.513    0.000042       2.566    0.001425       4-777   0.0135 

0.926    O.OOOII3         2.918     O.OO2IOO          4.902    0.01492 

1.141        0.000172  3.162         0.002795  5-503      0.02404 

1.574        0.000365  3-510        0.004029  5-764      0.03017 

2.143        0.000842  4.363         0.009353 

These  determinations  were  made  by  gradually  adding  0.25  n  and  o.oi  n  AgNOj 
to  the  chloride  solution  and  observing  the  point  of  initial  opalescence 

SOLUBILITY  OF  SILVER  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  ALUMINIUM 

AND  AMMONIUM  SALTS.      (Valenta;  see  also  Cohn,  1895.) 

Gms.  AgCl  per  100  Gms.  Solvent 
Aq.  Salt  Solution.  t°.  of  Concentration: 

i  :  loo.          5  :  loo.        10  :  100. 

Aluminium  Thiocyanate                                   25  ...  ...  2.02 

Ammonium  Carbonate                                      25  ...  ...  0.05 

Thiocyanate                                  20  ...  o .  08  o .  54 

Thiosulfate                                    20  0.57  1.32  3.92 

Calc.  byCohn*  0.64  3.07  5.86 

*  See  Note,  p.  603. 


SILVER   CHLORIDE 


608 


SOLUBILITY  OF  SILVER  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  BARIUM 
CHLORIDE  AND  OF  CALCIUM  CHLORIDE. 

(Forbes,  1911.) 


Gms.  Equiv. 

per  Liter. 

Gms.  Equiv. 

per  Liter. 

Aq.  Solution  of: 
Barium  Chloride 

t°.     BaClj 

Aq.  Solution  of:         t°. 
000186     Calcium  Chloride    25 

CaCl2  ^ 

2 
3.264 

O. 

Ag. 
001463 

25 

i. 

2 
248 

O. 

" 

25 

I, 

,  610 

0. 

000339 

25 

3 

•737 

O.OO2I82 

H 

25 

2 

.676 

0. 

001274 

2S 

4 

•033 

O. 

002802 

tt 

25 

3 

.  260 

0. 

002366 

2S 

4 

0. 

004175 

CaCU 

2 

25 

5 

.005 

0. 

005823 

Calcium  Chloride 

25 

i 

.748 

0. 

000289 

I 

3 

•512 

o  .  000964 

u 

25 

2 

.2OI 

0. 

000501 

25 

3 

.320 

0. 

001514 

u 

25 

2 

.741 

0. 

000900 

35 

3 

.  221 

0. 

001806 

SOLUBILITY  OF  SILVER  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  HYDRO- 
CHLORIC ACID  AT  25°. 

(Forbes,  1911.) 


Gms.  Equiv.  per  Liter, 
licl Ag! 
0.649          O.OO0032 
1.300          O.OOOI26 
I.QII  O.000266 


Gms.  Equiv.  per  Liter. 


Gms.  Equiv.  per  Liter. 


HC1. 
2.149 

2-975 


Ag. 

0.000374 
0.000814 
0.001358 


HC1. 
4.182 

4-735 
5.508 


Ag. 

0.002147 
0.003168 
0.005126 


O.OIW 


The  determinations  of  Forbes  were  made  by  gradually  adding  0.25  n  and  o.c 
AgNOs  to  the  chloride  solution  and  observing  the  point  of  initial  opalescence. 

Oneliterof   I  per  cent  aq.HCl  dissolve  0.0002  gm.AgCl  at  21°.    (Whitby,  '10.) 

1    5  0.0033  " 

"  10    .  "  (0.0555)0.0740  " 

NOTE.  —  The  determinations  of  Whitby  were  made  by  a  colorimetric  method 
which  was  based  upon  the  observation  that  the  color  produced  by  heating  a  solution 
of  a  silver  salt  with  sodium  hydroxide  and  certain  organic  compounds  such  as  dex- 
trin, glycerol,  starch,  sugar,  etc.,  is  proportional  to  the  amount  of  silver  present. 


SOLUBILITY  OF  SILVER  CHLORIDE  IN  AQUEOUS  HYDROCHLORIC  ACID  SOLU- 
TIONS AT  ORDINARY  TEMPERATURE. 

(Pierre,  1847;  Vogel.) 


Solvent. 

Cone.  HC1  +  Aq. 
i  vol.  Cone.  HC1  +  i  vol.  H2O 
Sat.  HC1  Sp.  Gr.  1.165 


Gms.  AgCl 
per  Liter. 

1.6 
2.98 


(at  b.  pt.)     5 . 60 


Solvent. 


Gms.  AgCl 
per  Liter. 

ioo  vol.  sat.  HC1  +  10  vol.  H2O     o.  56 

+  20  "  0.18 

+  30     "       0.09 
+  50     "       0.035 


SOLUBILITY  OF  SILVER  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  MERCURIC 
NITRATE  AT  25°, 

(Morse,  1902.) 


A101S. 

HgN03(HNO3) 
per  Liter. 

Mols.  AgCl 
per  Liter. 

Gms.  AgCl 
per  Liter. 

MOIS. 

HgNOaCHNOa) 
per  Liter. 

Mols.  AgCl 
per  Liter, 

Gms.  AgCl 
per  Liter. 

O.OIOO 

0  .  0043  2 

0.620 

0.050 

0.00914 

I.3IO 

0.0125 

0.00499 

0-7I5 

O.  IOO 

0.01395 

2 

0.025 

o  .  00690 

0.990 

I 

0.04810 

6.896 

Since  HNO3  was  present  in  all  cases,  its  influence  on  the  solubility  was  examined. 
It  was  found  that  no  appreciable  differences  were  obtained  with  concentrations 
varying  between  o.i  and  2  normal  HNO3.  Both  crystallized  and  amorphous 
silver  chloride  gave  identical  results. 


669 


SILVER  CHLORIDE 


SOLUBILITY  OF  SILVER  CHLORIDE  IN  AQUEOUS  SALT  SOLUTIONS. 

(Vogel;  Hahn;  Valenta  ) 
Salt  Solution. 

Barium  Chloride 
Barium  Chloride 
Barium  Sulphocyanide 
Calcium  Sulphocyanide 
Calcium  Chloride 
Calcium  Chloride 
Copper  Chloride 
Ferrous  Chloride 
Ferric  Chloride 
Manganese  Chloride 
Magnesium  Chloride 
Magnesium  Chloride 
Magnesium  Chloride 
Strontium  Chloride 
Zinc  Chloride 
Potassium  Chloride 
Potassium  Chloride 
Potassium  Cyanide 
Potassium  Cyanide 
Potassium  Sulphocyanide 
Sodium  Chloride 
Sodium  Chloride 


SOLUBILITY  OF  SILVER  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  NITRIC 
ACID  AT  25°. 

(Glowczynski,  1914-) 
Mols.  per  Liter.  Cms.  per  Liter. 


Cone,  of  Salt. 

t  o                           Gms.  AgCl  per 
loo  Gms.  Solution. 

27.32% 

24-5 

0.057 

(H.) 

saturated 

ord.  temp. 

0.014 

(Vg.) 

io  :  100 

25 

0-20 

(VI.) 

io  :  100 

25 

0.15 

(VI.) 

41.26% 

24-5 

0-571 

(H.) 

saturated 

ord.  temp. 

0-093 

(Vg.) 

" 

24-5 

0-053 

(H.) 

n 

it 

0.169 

(H.) 

" 

" 

O-OO6 

(H.) 

<( 

it 

0.013 

(H.) 

50  :  100 

25 

0.50 

(VI.) 

36.35% 

24  5 

0-531 

(H.) 

saturated 

ord.  temp. 

O.I7I 

(Vg.) 

" 

it 

0.088 

(Vg.) 

" 

24-5 

0.0134 

(H.) 

it 

ord.  temp. 

0-0475 

(Vg.) 

24-95% 

19.6 

0.0776 

(H.) 

5  *•  100 

25 

2-75 

(VI.) 

5:100 

25 

5-24 

(Cohn*) 

io:  100 

25 

O.II 

(VI.) 

saturated 

ord.  temp. 

0.095 

(Vg.) 

25-95% 

19-6 

0-105 

(H.) 

*  See  Note,  p. 

603. 

HNO3. 

AgCl. 

0.0005 

I.I5.IO-5 

O.OOI 

i.ig.io"5 

0.01 

i  .  24  .  io~5 

0.30 

I.57.IO-5 

'  HN03. 

AgCl. 

0.0315 

0.001647 

0.063 

O.OOI7O5 

0.630 

0.00176 

18.9 

0.00225 

94-5 

0.00245 

1.71.10-° 

SOLUBILITY  OF  SILVER  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  POTASSIUM 
CHLORIDE  AT  25°. 

(Forbes,  1911.) 
Gms.  Equiv.  per  Liter.   Gms.  Equiv.  per  Liter. 


(Glowczynski,  1914.) 
Mols.  per  Liter.  Gms.  per  Liter. 


KC1. 
I. Ill 


Ag. 
0.000141 


KC1.     Ag. 
2.850  0.001845 


KC1. 


AgCl. 


KC1. 


AgCl. 


1.425  0.000235  3.081  0.002435 
0.000391  3.424  0.003602 


2.022  0.00o6l6   3.843  0.005725 


3.I6.IO"5  I.28.IO""6  0.00236  0.001836 

6.32.IQ-6  I.52.IQ-6 

2.O.  IO  ~*  2.  13.  IO"5 

4.0.  io  ~*  2.24.  lo"5 


0.00471  0.002178 
O.OI49I  0.003052 
0.02984  0.003209 

2.396    0.001050     3.325    o.ooi734(at  i°) 
2.628    0.001390     2.955    0.002 786 (at 35°) 

The  determinations  of  Glowczynski  were  made  by  the  method  described  in 
Note,  on  p.  605.  The  determinations  of  Forbes  were  made  by  gradually  adding 
0.25  n  and  o.oi  n  AgNO3  to  the  chloride  solution  and  observing  the  point  of 
initial  opalescence. 

One  liter  4  n  aq.  KC1  dissolves  0.00637  Sm-  mol.  =  0.915  gm.  AgCl  at  25°. 

(Hellwig,  1900.) 


SILVER  CHLORIDE  610 

SOLUBILITY  OP  SILVER  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OP 
POTASSIUM  CHLORIDE  AT  15°. 

(Schierholz  —  Sitzber.  K.  Akad.  Wiss.  (Vienna)  101,  ab,  8,  '90.) 

Grams  per  too  Grams  Grams  per  100  Grams 

Solution.  Solution. 


KC1.  AgCl.  KC1.  AgCl. 

lo.o  o.ooo  22.47  0-045 

14.29  O-OO4  24.0  O.O72 

16.66  0.008  25.0  0.084 

20.00  0.020        Sp.  Gr.  of  25%  KC1  sol,=  1.179 

MIXTURES  OF  SILVER  CHLORIDE   AND   SILVER  HYDROXIDE   IN    EQUI- 
LIBRIUM WITH  AQ.  POTASSIUM  HYDROXIDE  SOLUTIONS  AT  25°. 

(Noyes  and  Kohr  —  J.  Am.  Ch.  Soc.  24,  1144,  '02.) 

Normality  Millimols  per  Liter.  Grams  per  Liter. 

ofKOH.  KC1.  KOH.'  KC1.  KOH.  AgCl. 

0-333        3-4I4        347-8  0.255        IO-°5        0.4896 

0-065     0-598      65.0       0-0446     2.OO     0-0828 

SOLUBILITY  OF  SILVER  CHLORIDE  IN  AQ.  SODIUM  CHLORIDE  SOLUTIONS. 

(Schierholz;  Vogel;  Hahn.) 

Solubility  at  15°.  Solubility  at  Different  Temperatures 

Gms.  per  100  Gms,  +  0  Gms.  AgCl  per  100  Gms. 

Solution.  Solution  in: 


NaCl.                    AgCl.  14%  NaCl                  26.3%  NaCl. 

io.o            0.0025                  15  0.007                0.128 

14.29          0.0071                   30  O.OIT                 0.132 

18.18          0.0182                   40  0-014                0.158 

21.98          0.0439                  50  0.023                 0.184 

23-53          0.0706                  70  0.042                0.263 

25.64          0.103                    80  0.054                0.315 

26.31          0.127                    90  0.069                0.368 

100  0.090                o  460 

Sp.Gr.  of  26.31%  NaCl  sol.  =  1.207.  109  0.107(104°)     0.571 

SOLUBILITY  AT  20°,  50°,  AND  90°  (CALC.  FROM  ORIGINAL). 

(Barlow  —  J.  Am.  Chem.  Soc  28,  1446,  '06.) 


Gms.  NaCl      Gms.  AgCl  dissolved  per  100  cc.          Gms.  NaCl 
per  loo  cc.                       Solution  at:                               per  I00  cc. 

Gms.  AgCl  dissolved  per  100  cc. 
Solution  at: 

Solution. 

20°. 

50°. 

90° 

Solution. 

'20°. 

50°. 

00°. 

3-43 

0 

.OOOlS 

0.0016 

0 

.0067 

"•5 

0 

.0031 

0 

.0124 

0.0436 

4.60 

0 

OO025 

0.0025 

0 

•  OIOO 

i5-3 

0 

.009O 

0 

.0191 

0.0732 

5-75 

0 

.00047 

0.0034 

0 

•0135 

23.0 

0 

•0313 

0 

.0889 

0.1706 

7.67 

0 

OOI25 

0.0058 

0 

.0236 

Results  are  also  given  for  the  solubility  of  silver  chloride  in  aqueous  sodium 
chloride  solutions  containing  hydrochloric  acid. 

SOLUBILITY  OF  SILVER  CHLORIDE  IN  AQUEOUS  SODIUM  CHLORIDE  AT  25°. 

(Forbes,  1911.) 

Gms.  Equiv.  per  Liter.  Gms.  Equiv.  per  Liter.  Gms.  Equiv.  per  Liter. 

[NaCl].  [Ag]Xio».  '  [NaCl].  [AglXioS.'  '  [NaCl].          [Ag]Xio3.' 

0.933  0.086  2.272  0.570  3-747  2.462 

1.190  0.130  2.658  0.851  3-977  2.879 

1.433  0.184  2.841  1.040  4-363  3-810 

1.617  0-245  3-270  1-583  4-535  4-298 

1.871  0.348  3.471  1.897  5.039  6.039 


6n  SILVER  CHLORIDE 

SOLUBILITY  OF  SILVER  CHLORIDE  IN  AQ.  SODIUM  NITRATE  SOLUTIONS. 

Cms,  per  100  Cms.  HtO.  Cms.  per  100  Cms.  H2O. 

NaN03. AgCl.    '  NaN03. AgCl.    ' 

5      0.787    0.00086      15-20   0.393    0.00096 
18      0.787    0.00146  0.787    0.00133 

30        0.787      0.00233  2.787      0.00253 

45-55    0-787     0.00399  (Mulder.) 

One  liter  aq.  3  n  AgNO3  dissolves  0.0056  gm.  mols.  =  0.8  gm.  AgCl  at  25°. 

(Hellwig,  1900.) 

SOLUBILITY  OF  SILVER  CHLORIDE  IN  AQUEOUS  SODIUM  SULFITE  SOLUTIONS 

AT  25°. 
(Luther  and  Leubner,  1912.) 

Gms.  Formula  Weight  per  Liter.  Gms.  Formula  Weight  per  Liter. 

S03".  Ap!  S03".  Ap! 

0.080  o.on  0.483  0.059 

0.106  0.017  0.470  0.070 

0.220  0.033  0.652  0.103 

0.234  0.036  0.890  O.I4O 

0.478  0.057  0.937  0.142 

The  AgCl  was  prepared  by  precipitating  dilute  AgNO3  with  alkali  chloride  at 
the  b.  pt.  The  resulting  solid  corresponded  to  the  granular  modification  of  Stas. 
About  one  hour  constant  agitation  was  allowed  for  attainment  of  equilibrium. 

SOLUBILITY  OF  SILVER  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  SODIUM 
THIOSULFATE,  ETC. 

(Valenta;  Cohn;  Richards  and  Faber,  1899.) 

Gms.  AgCl  per  100  Gms.  Aq.  Solutions  of  Concentration: 

Salt  Solution.  t°.  , » N 

i  :  zoo.       5  : 100.       10  : 100.     15  : 100.      20  : 100. 

Sodium  Sulfite  25        ...         ...       0.44        ...       0.95 

Sodium  Thiosulfate  20      0.40      2  4.10      5.50      6.10 

"  Calc.  by  Cohn.*        0.38        1.83        3.50        5.02        6.41 

Sodium  Thiosulfate  35        9.o8f 

Thiocarbamide  25        ...          ...        0.83 

Thiocyanimine  25      0.40      1.90      3.90 

*  See  Note,  p.  603.  t  Gms.  per  100  cc.  solution  (R.  and  F.). 

SOLUBILITY  OF  SILVER  CHLORIDE  IN  AQUEOUS  STRONTIUM  CHLORIDE  AT  25°. 

(Forbes,  1911.) 


Gms.  Equiv.  per  Liter. 

Gms.  Equiv.  per  Liter. 

Gms.  Equiv.  per  Liter. 

SrCl2 

2 

AgXio». 

'  SrCl2- 

2 

AgXioS. 

SrCl2- 

2 

AgXio*. 

0.550 

0-033 

1.818 

0.348 

3-494 

2.018 

0.989 

0.092 

2.140 

0.510 

4-I52 

3-594 

1-359 

0.173 

2.476 

0-747 

5.216 

8.174 

1-572 

0.236 

2.992 

1.252 

5-775 

12.040 

The  determinations  were  made  by  gradually  adding  0.25  n  and  o.oi  n  AgNOs  to 
the  chloride  solution  and  observing  the  point  of  initial  opalescence. 
One  liter  of  4.777  n  ZnCl2  solution  dissolves  0.000364  mol.  AgCl  at  25°. 

(Forbes,  1911.) 

Fusion-point  data  are  given  for  the  following  mixtures. 

AgCl  +  Agl.  (Monkemeyer,  1906.) 

AgCl  +  Ag2S.  (Truthe,  1912;  Sandonnini,  1912.) 

AgCl  +  NaCl.  (Sackur,  1913;  Botta,  1911;  Sandonnini,  1911,  1914.) 

AgCl  +  T1C1.  (Sandonnini,  1911,  1914.) 


SILVER   CHLORIDE  612 

SOLUBILITY  OF  SILVER  CHLORIDE  IN  PYRIDINE. 

(Kahlenberg  and  Wittich,  1909.) 

Cms.  AgCl  Cms.  AgCl      c  ..  . 

t°.  per  100  Cms.  Solid  Phase.  t°.  per  100  Gms.  p.? 

Pyridine.  Pyridine.  Phase" 

—  57  EutCC.  ...  AgC1.2C6H6N+C6H6N  O  5.35          AgCl 

—  49  0.77  AgCl.2C6H6N  10  3.17 

—  35  0.99  20  I.QI 
-30  1.36  "  30  1.20 

—  25  1.  80  40  0.80 

—  22  2.20  ".  50  0-53 

—  tr.pt.     2.75        "  +Agd.c6H5N  60          0.403 

—  20  3.75  AgCLCsHsN  70  0.32 

-18  3.85  "  80          0.25 

-10  4.35  "  90  0.22 

—  5  5.05  ioo          0.18 

—  I  5.60  "  110  0.12 

SILVER  CHROMATE  Ag2CrO4. 

One  liter  of  water  dissolves  0.026  gm.  Ag2CrO4  at  18°,  and  0.020  gm.  at  25°. 

(Abegg  and  Cox,  1903;  Kohlrausch,  1904-05.) 

One  liter  H2O  dissolves  0.029  gm.  AgiCrO4  at  25°.  (Schafer,  1905.) 

One  liter  of  H2O  dissolves  0.0142  gm.  Ag2CrO4  at  0.26°;  0.0225  gm.  at  14.8°, 

0.036  gm.  at  30.7°  and  0.084  gms-  at  75°-  (Kohlrausch,  1908.) 

One  liter  H2O  dissolves  0.0256  gm.  at  18°,  0.0341  gm.  at  27°  and  0.0534  Sm-  at 

50°,  determined  by  a  colorimetric  method  (see  Note,  p.  608).  (Whitby,  1910.) 

SOLUBILITY  OF  SILVER  CHROMATE  IN  AQUEOUS  AMMONIA  AT  25°. 

(Sherrill  and  Eaton,  1907.) 

Mols.  NHiOH  per  Liter  o.oi        0.02        0.04          0.08 

Mols.  X  io3  Ag2CrO4  per  Liter      2.004      4.169      8.595       17.58 

SOLUBILITY  OF  SILVER  CHROMATE  IN  AQUEOUS  NITRIC  ACID  AT  25°. 

(Sherrill  and  Russ,  1907.) 


Mols.  HNO3  Milliatoms  per  Liter.       Solid 
per  Liter.          Cr.             Ag.            Phase. 

Mols.  HNO3  Milliatoms^  per  Liter. 
per  Liter.           Cr.              Ag. 

O 

.OI 

3 

•157 

6.315      Ag2CrO4 

O.O6 

6 

•833 

. 

O 

.015 

3 

•730 

" 

O, 

.07 

7 

•333 

. 

0.02 

4 

.177 

8.356 

O. 

•075 

7 

•477 

14 

•85 

0 

.025 

4 

.567 

.  .  . 

0, 

,08 

7 

.260 

i5 

•45 

0 

•03 

5 

.200 

...                " 

0, 

,1(7 

5 

•647 

19 

.01 

/   O 

.04 

5 

•803 

11.62 

O. 

13 

4 

•293 

23 

.89 

0 

•93 

6 

.380 

...                " 

O, 

,14 

3 

.948 

25 

•63 

Solid 
Phase. 


Ag,CrO4 


One  liter  65%  aqueous  alcohol  dissolves  0.78  X  io~4  gms.  equivalents  =  0.0129 
gm.  Ag2CrO4  at  room  temp.  (?).  (Guerini,  1912.) 

SOLUBILITY  OF  SILVER  CHROMATE  IN  AQUEOUS  SOLUTIONS  OF  NITRATES  AT  100°. 

(Carpenter,  1886.) 

Gms.  Salt  Gms.  Ag2CrO4 

Solvent.  per  too  cc.  per  ioo  cc. 

H2O.  Solution. 

Water  o  o .  064 

Sodium  Nitrate  50  o .  064 

Potassium  Nitrate  50  0.192 

Ammonium  Nitrate  50  0.320 

Magnesium  Nitrate  50  0.256 


6i3  SILVER  CHROMATE 

SILVER   (Di)   CHROMATE  Ag2Cr2O7. 

One  liter  of  aqueous  solution  contains  0.00019  gni.  mol.  or  0.083  gm-  Ag2Cr2O7 
at  15°.  (Mayer,  1903.) 

SOLUBILITY  OF  SILVER  DICHROMATE  IN  AQUEOUS  NITRIC  ACID  AT  25°. 

(Sherrill  and  Russ,  1907.) 

Milliatoms  per  Liter. 

Solid  Phase. 


>er  Liter. 

Cr. 

Ag. 

0 
0.01 
O.O2 

32.20 
25.06 
2O.  21 

5-390 
6.131 
7.148 

0.04 
0.06 

13-59 
II.  10 

9-529 
II.  I 

0.08 

II  .1 

II.  I 

0.08+0.1  AgNO3 

6.625 

.  .  ... 

At  the  lower  concentrations  some  of  the  dichromate  is  converted  into  solid 
chromate. 

SILVER  CITRATE   C6H5O7Ag3. 

loo  gms.  H2O  dissolve  0.0277  gm.  CeHsO/Ags  at  18°,  and  0.0284  Sm-  at  25°- 

(Partheil  and  Hubner,  1903.) 

SILVER  CYANIDE  AgCN. 

One  liter  of  aqueous  solution  contains  0.000043  gm.  AgCN  at  17.5°  and  0.00022 
gm.  at  20°  (by  Conductivity  Method).  (Abegg  and  Cox;  Bottger,  1903.) 

SOLUBILITY  OF  SILVER  CYANIDE  IN  AQUEOUS  AMMONIA  SOLUTIONS. 

(Longi,  1883.) 

100  gms.  aq.  ammonia  of  0.998  Sp.  Gr.  =  5%,  dissolve  0.232  gm.  AgCN  at  12°. 
100  gms.  aq.  ammortia  of  0.96  Sp.  Gr.  =  10%^  dissolve  0.542  gm.  AgCN  at  18°. 

One  liter  aq.  3  n  AgNO3  dissolves  0.0091  gm.  mol.  =  1.216  gm.  AgCN  at  25°. 

(Hellwig,  1900.) 

Fusion-point  data  for  mixtures  of  AgCN  +  NaCN  are  given  by  Truthe  (1912). 

SILVER  FERRICYANIDE  Ag3FeCN6. 

3FeCN6  at  20°.     See  Note,  p 

fhitby,  1910.) 


One  liter  H2O  dissolves  0.00066  gm.  Ag3FeCN6  at  20°.     bee  JNote,  p. 

(Wl 


SILVER   SODIUM   CYANIDE  AgCN.NaCN. 

100  gms.  H2O  dissolve  20  gms.  at  20°,  and  more  at  a  higher  temperature.     100 
gms.  85%  alcohol  dissolve  4.1  gms.  at  20°.  (Baup,  1858.) 

SILVER  THALLOUS   CYANIDE  AgCN.TICN. 

100  gms.  H2O  dissolve  4.7  gms.  at  o°,  and  7.4  gms.  at  16°.  (Fronmuller,  1878.) 

SILVER  FLUORIDE  AgF.2H2O. 

SOLUBILITY  IN  WATER. 

(Guntz  and  Guntz,  Jr.,  1914.) 


—  14.2  EutCC.           60  Ice+AgF.4H2O  25  1  79  -5         AgF.2H2O 

+  18.5  165  AgF.4H20  28.5  215 

18.65  z^9-5  "  +AgF.2H2O  32  193 

2O  172  AgF.2H2O  39-5  222                     "  +AgF 

24  178  "  I08  205                     AgF 

Two  unstable  hydrates,  AgF.H2O  and  3AgF-5H2O  were  also  obtained. 

100  gms.  H2O  dissolve  181.8  gms.  AgF  at  15.8°,  di$.&  of  Sat.  Sol.  =  2.61.  (Gore,  1870.) 


SILVER  FLUORIDE 


614 


SOLUBILITY  OF  SILVER  FLUORIDE  IN  AQUEOUS  SOLUTIONS  OF  HYDRO- 
FLUORIC ACID  AT  O°  AND  AT  24°. 
(Guntz  and  Guntz,  Jr.,  1914-) 

Results  at  24°. 


Results 

Gms.  per  ioo  Gms.  H2O.' 

Solid  Phase. 

AgF. 

HF. 

87-5 

0.40 

AgF.4H2O 

89.4 

2.0O 

" 

93-8 

3-97 

ii 

Il8.5 

9.60 

" 

156 

14 

"        +AgF. 

159 

17.2 

AgF.aH.O 

185 

24 

" 

I89 

25-7 

AgF 

188 

29-5 

" 

196 

39-8 

" 

142.1 

52 

AgF.2H2O 

121.75 

57-2 

M 

94-93 

66.57 

" 

173-75 

0.4 

3AgF.sH2O 

174 

3-6 

" 

AgF. 

HF. 

•»           ouiiu  iruasc. 

I78 

O 

AgF.2H2O 

178.5 

i-73 

" 

I77-65 

5-42 

*! 

179-5 

IO 

" 

189.5 

13-4 

ii 

I9I-5 

14-3 

"        +AgF(?) 

207 

0-15 

3  AgF.5H20 

2O6.2 

1-25 

" 

202.5 

7-9 

ii 

198.6 

12.65 

" 

195-5 

11.7 

AgF.H,O 

194-5 

13 

" 

189.5 

18.8 

3AgF.SH20+AgF(?) 

193 

36.6 

AgF 

193-5 

16 

Additional  determinations  at  other  temperatures  are  given. 

SILVER  FULMINATE   CAg^NO^CN. 

One  liter  of  aqueous  solution  contains  0.075  gm.  C2Ag2N2O2  at  13°,  and  0.180 

gm.  at  3Or  (Holleman,  1896.) 

SILVER  HEPTOATE  (Onanthylate)  AgC7H13O2. 


SOLUBILITY  IN  WATER. 

(Landau,  1893;  Altschul,  1896.) 


^o  Gms.  AgCyHisOj  per  ioo  Gms.  H2O.  ^.o 

O  O  .  0635  (Landau)    O  .  0436  (Altschul)  50 

10  0.0817      0.0494  60 

20  0.1007      °-°555  7° 

30  o.i 206      0.0617  80 

40  0.1420  0.0714 


Gms. 


ioo  Gms. 


0.1652  (Landau)  O  .  08  5  8  (Altschul) 

0.1906  0.1036 

0.2185  °-I35I 

0.2495  0.1688 


SILVER  IODATE  AgIO3. 

One  liter  of  aqueous  solution  contains  0.04  gm.  or  0.00014  &m-  mol.  at  i8°-2O°, 
and  0.05334  gm.  or  0.000189  gm-  mol.  at  25°. 

(Longi;  Bottger;  Kohlrausch;  Noyes  and  Kohr,  1902.) 

The  solubility  of. silver  iodate  in  water,  determined  by  a  colorimetric  method 
(see  Note,  p.  608),  was  found  by  Whitby  (1910)  to  be  0.039  gm-  AgIO3  per 
liter  at  20°.  Determinations  reported  by  Sammet  (1905)  made  by  a  chain  cell 
method,  gave  0.0611  gm.  AgIO3  per  liter  at  25°  and  0.1849  Sm-  at  6o°- 

One  liter  of  H2O  dissolves  0.0275  gm-  AgIO3  at  9.43°,  0.039  gm.  at  18.4°  and 
°-°539  gm-  at  26.6°.  (Kohlrausch,  1908.) 

SOLUBILITY  OF  SILVER  IODATE  IN  AQUEOUS  SOLUTIONS  OF  AMMONIA  AND 
OF  NITRIC  ACID  AT  25°. 

(Longi,  1883.) 

ioo  gms.  aq.  ammonia  of  0.998  Sp.  Gr.  =  5%  dissolve  2.36  gms.  AgIO3. 
ioo  gms.  aq.  ammonia  of  0.96  Sp.  Gr.  =  10%  dissolve  45.41  gms.  AgIO3. 
ioo  gms.  aq.  nitric  acid  of  1.21  Sp.  Gr.  =35%  dissolve  0.096  gm.  AgIO3. 


6i5 


SILVER  IODATE 


SOLUBILITY  OF  SILVER  IODATE  IN  AQUEOUS  SOLUTIONS  OF  NITRIC  ACID  AT  25°, 

(Hill  and  Simmons,  1909.) 


Normality  of 
Aq.  HNO,. 
O 

0.125 
0.250 
0.500 


Cms.  AglOj 
per  Liter. 
0.0503 

o . 0864 

0.1075 
O.I4I4 


Normality  of 
Aq.  HNO3. 

I 

2 

4 

8 


Cms.  AglOj 
per  Liter. 
0.2067 

0.3319 
0.6085 
1.587 


The  solubility  of  the  amorphous  modification  of  AglOs  is  considerably  higher 
than  that  of  the  crystalline,  but  the  amorphous  product  rapidly  becomes  crystalline 
and  correct  results  are  soon  obtained. 


SILVER  IODIDE  Agl. 

One  liter  of  aqueous  solution  contains  0.0000028  gm.  Agl  at  2O0-2§°. 

(Average  of  several  determinations  by  Kohlrausch,  Abegg  and  Cox,  etc.,  Holleman  gives  higher  figures.) 

One  liter  of  water  dissolves  0.0000253  Sm-  Agl  at  60°,  determined  by  a  chain 
cell  method  (Sammet,  1905).  This  author  also  gives  data  for  the  solubility  of 
Agl  in  i  n  and  o.i  n  KI  solutions  at  60°. 


Per  cent  Con- 
centration of  Aq. 
Ammonia. 

7 
10 


SOLUBILITY  OF  SILVER  IODIDE  IN  AQUEOUS  AMMONIA. 

Authority. 


d  of  Aq. 
Ammonia. 


Gms.  Agl 
per  Liter. 


0.971  1 6  0.045  (Ladenburg,  1902.) 

0.960  12  0.035  (Longi,  1883.) 

2O  0.926  l6  O.l66  (Baubigny,  1908.) 

Baubigny  used  a  sealed  tube  and  noted  the  first  appearance  of  crystallization 
of  Agl  in  mixtures  of  known  compositions. 

SOLUBILITY  OF  SILVER  IODIDE  IN  AQUEOUS  MERCURIC  NITRATE  AT  25°. 

(Morse,  1902.) 


Mols.  Hg(NOs), 
per  Liter. 

Mols.  Agl 
per  Liter. 

Gms.  Agl     Mols.  Hg(NO3), 
per  Liter.          per  Liter. 

Mols.  Agl  per 
Liter,  j 

Gms.  Agl 
per  Liter. 

O.OIO 

o  .  00340 

0.800 

0.050 

O.0074O 

1-737 

0.0125 

0.00358 

0.841 

0.  IOO 

o.  01161 

2.730 

0.025 

0.00476 

i.zxS 

I 

O.I070O 

25.  160 

Since  HNOs  was  present  in  all  cases  its  influence  on  the  solubility  was  examined. 
It  was  found  that  no  appreciable  differences  were  obtained  with  concentrations 
varying  between  o.i  and  2  n  HNO3.  Both  crystallized  and  amorphous  silver 
iodide  gave  identical  results. 

SOLUBILITY  OF  SILVER  IODIDE  IN  AQUEOUS  SOLUTIONS  OF  POTASSIUM 
IODIDE  AND  OF  SILVER  NITRATE  AT  25°. 

(Hellwig,  1900.) 


In  Aq.  KI  Solutions. 


In  Aq.  AgNO3  Solutions. 


fols.  KI 

Mols.  Agl 

Gms.  Agl 

Mols. 

AgN03 

Mols.  Agl 

Gms.  Agl 

Solid 

er  Liter. 

per  Liter. 

per  Liter. 

per 

Liter. 

per  Liter. 

per  Liter. 

Phase. 

0. 

335 

0.000363 

o 

0853 

O. 

20 

O 

OO0289 

O 

.068 

Agl 

0. 

586 

O.O02I8 

0 

5" 

0. 

35 

0 

000532 

0 

.121 

0. 

734 

0.0044 

I 

032 

0. 

50 

O 

OOI27 

O 

.299 

" 

008 

O.OI4I 

3 

32 

0. 

70 

O 

00362 

0 

.850 

" 

018 

0.0148 

O 

47 

I. 

215 

0 

0131 

3 

.08 

AgjINO, 

406 

0.0535 

12 

55 

I. 

63 

0 

0267 

6 

.26 

" 

486 

0.0658 

15 

46 

2. 

04 

O 

0458 

IO 

•9 

« 

6304 

0.102 

24 

01 

2. 

54 

0 

0678 

16 

.  i 

AftKNO,), 

. 

937 

0.198 

46 

42 

3- 

75 

0 

141 

33 

.2 

4- 

69 

0 

227 

53 

.2 

« 

5- 

90 

O 

362 

85 

u 

SILVER  IODIDE 


616 


SOLUBILITY  OF  SILVER  IODIDE  IN  AQUEOUS  SALT  SOLUTIONS. 

(Valenta,  1894;  Cohn,  1895.) 


Aq.  Salt.  Solution.  t°. 

Sodium  Thiosulfate  20 

"  Calc.  by  Cohn.* 

Potassium  Cyanide  25 

"  Calc.  by  Cohn.* 

Sodium  Sulfite  25 

Ammonium  Thiocyanate      20 

Calcium 

Barium 

Aluminium  " 

Thiocarbamide 

Thiocyanime 


Gms.  Agl  per  100  Cms.  Aq.  Sol.  of  Concentration: 


i  :  ioo. 

5  :  ioo. 

10  :  ioo. 

15  :  ioo. 

20  :  ioo. 

0.03 

0-15 

0.30 

0.40 

0.60 

0.623 

2.996 

5.726 

8.218 

10.493 

8.28 

.  .  . 

8.568 

.  .  . 

.  .  . 

.  .  . 

.  .  . 

O.OI 

.  .  . 

0.02 

O.O2 

0.08 

0.13 

... 

0.03 

O.O2 

.  .  . 

.  .  . 

.  .  . 

O.O2 

... 

... 

0.79 

.  .  . 

.  .  . 

0.008 

0.05 

O.O9 

25 
25 
25 
25 
25 

*  See  Note,  p.  603. 


SOLUBILITY  OF  SILVER  IODIDE  IN  AQUEOUS  SOLUTIONS  OF  SODIUM  CHLORIDE, 
POTASSIUM  BROMIDE  AND  OF  POTASSIUM  IODIDE  AT  15°. 

(Schierholz,  1890.) 


In  Sodium  Chloride. 

Gms.  per  100  Gms.  Solution. 


In  Potassium  Iodide. 

Gms.  per  100  Gms.  Solution. 


NaCl. 

26.31 

25.00 


Agl. 

O.O244 
O.OOO72 


KI. 
59.16 

Agl. 
53-^3 

57-15 

40-0 

50.0 

25.0 

4O.O 

13.0 

33-3 

7-33 

25.0 
21.74 

20-0 

2-75 
1.576 
0.80 

In  Potassium  Bromide. 

Gms.  per  IPO  Gms.  Solution. 

KBr  Agl 

30.77  0.132 

ioo  gms.  sat.  silver  nitrate  solution  dissolve  2.3  gms.  Agl  at  11°,  and  12.3  gms. 
at  b.  pt. 

ioo  gms.  pyridine  dissolve  o.io  gm.  Agl  at  10°,  and  8.60  gms.  at  121°. 

»  (von  Laszcynski,  1894.) 

SOLUBILITY  OF  SILVER  IODIDE  IN  AQUEOUS  SODIUM  IODIDE  AT  25°. 

(Krym,  1909.) 


Gms.  per  ioo  Gms.  H2O. 


Nal. 

59-29 
67.47 

Agl. 
31.21 

28.52 

I34-I 
156.9 

99-54 
124.6 

179.8 
196.3 

150 
134.8 

223.7 

122 

Solid  Phase. 


Gms.  per  ioo  Gms.  H2O. 


Agl 


"  +AgI.NaI.3*H2O 
AgI.NaI.3*H2O 


Nal.               Agl. 

ouuu  jriiasc. 

226            120-9 

AgI.NaI.3§HjO+NaI 

222-7       H2.  1 

Nal 

214.7         90.84 

" 

203.9         59.48 

" 

194.5         31.10 

" 

185.52      o 

" 

The  above  table  was  calculated  from  the  original  results  which  are  expressed  in 
mols.  per  1000  mols.  H2O. 

Fusion-point  data  for  mixtures  of  Agl  +  HgI2  are  given  by  Steger  (1903). 
Results  for  Agl  +  Nal  are  given  by  Sandonnini  and  Scarpa  (1913). 


Laurate. 

Myristate. 

Palmitate. 

Stearate. 

35 

0.007 

O.OO4 

O.O04 

50 

.  .  . 

O.OO7 

O.OO6 

O.OO4 

25 

0.009 

0.008 

O.007 

O.OO7 

So 

0.009 

0.008 

O.OO7 

O.007 

15 

0.074 

0.063 

0.060 

0.051 

25 

0.072 

0.067 

0.059 

0.052 

35 

0.078 

0.071 

O.062 

0.055 

50 

0.083 

0.073 

0.066 

0.000 

15 

O.OIO 

0.009 

O.OO9 

0.007 

617  SILVER  LAURATE 

SILVER  LAURATE,  MYRISTATE,  PALMITATE  and  STEARATE 

SOLUBILITY  OF  EACH,  DETERMINED  SEPARATELY,  IN  WATER  AND  OTHER 
SOLVENTS  AT  SEVERAL  TEMPERATURES. 

(Jacobson  and  Holmes,  1916.) 

Cms.  each  Salt  per  too  Gms.  Solvent. 
Solvent. 

Water 
u 

Abs.  Ethyl  Alcohol     25 

a  ii 

Methyl  Alcohol 


Ether 

SILVER  LEVULINATE  (Acetyl  propionate)  CH3.COCH2CH2COOAg. 
SOLUBILITY  IN  WATER. 

(Furcht  and  Lieben,  1909.) 
jo  Gms.  per  loo  Gms.  Sat.  Solution. 

8  o.  5363  (white  salt)  o.  5195  (yellow  salt) 

9  0.5166  0.5372 
14-15  0.6078  0.6448 
99-6  3-49  3-70 

SILVER  MALATE   C4H4O5Ag2. 

100  gms.  H2O  dissolve  0.0119  Sms.  at  18°,  and  0.1216  gm.  at  25°. 

(Partheil  and  Hiibner,  1903.) 

SILVER  NITRATE  AgNO3. 

SOLUBILITY  IN  WATER. 

(Etard,  1894;  Kremers,  1854;  Tilden  and  Shenstone,  1884.) 
Gms.  AgNO3  per  100  Gms.  Gms.  AgNO3  per  100  Gms. 


Solution. 

Water. 

Solution. 

Water. 

~  5 

48  (Etard)     

50 

79  (Etard) 

82 

455 

0 

53 

55 

122 

60 

8x. 

5 

84 

525 

IO 

62 

63 

170 

80 

85. 

5 

87 

669 

20 

68 

69 

222 

IOO 

88. 

5 

90* 

952 

25 

70. 

5 

72 

257 

120 

9i 

95 

1900 

30 

72. 

5 

75 

300 

140 

93- 

5 

.  .  . 

.  .  . 

40 

76. 

5 

79 

376 

160 

95 

ioo  gms.  sat.  aq.  solution  contain  47.1  gms.  AgNO3  at  —7.3°  (=  Eutectic). 

(Middleberg,  1903.) 

IOO  gms.  sat.  aq.  sol.  contain  65.5  gms.  AgNOs  at  15.5°.          (Greenish  and  Smith,  1903.) 
IOO  gms.  sat.  aq.  sol.  contain  73  gms.  AgNOs  at  30°.    (Schreinemakers  and  de  Baat,  igioa.) 

SOLUBILITY  OF  SILVER  NITRATE  IN  AQUEOUS  NITRIC  ACID  AT  25°. 

(Masson,  1911.) 


4.  of  Sat. 

Gm.  Mols 

.  per  Liter. 

Gms.  AgNO3 

4;  of  Sat. 

Gm.  Mols. 

per  Liter.    Gms.  AgNO, 

Sol. 

'  HN03. 

AgNOj. 

per  Liter. 

Sol. 

'  HNOS. 

AgN03. 

per  Liter. 

2.3921 

0 

10.31 

1752 

I  .  4980 

4-497 

2.590 

440.1 

2.2754 

0.4042 

9-36 

1591 

I.4I95 

5-992 

1.698 

288.6 

2.1243 

0.962 

8.08 

1373 

1.3818 

8.84 

0.843 

143-2 

1.9402 

1.698 

6-54 

IIII 

1.3976 

12.53 

0-347 

58.96 

T.7052 

2.834 

4.526 

769.1 

ioo  gms.  2HNOS.3H2O  dissolve  3.33  gms.  AgNO3  at  20°,  and  16.6  gms.  at  100°. 
ioo  gms.  cone.  HNOi  dissolve  0.2  gm.  AgNOj.  (Schultz,  1860.) 


SILVER  NITRATE  618 

SOLUBILITY  OF  MIXED  CRYSTALS  OF  SILVER  NITRATE  AND  SODIUM  NITRATE 
IN  AQUEOUS  ETHYL  ALCOHOL. 

(Hissink,  igoo.) 

Results  at  25°  in  Results  at  50°  in 

Aq.  C2H6OH  of  fa  =  0.945  (37  wt.  %).     Aq.  C2H6OH  of  d17  =  0.859  (75  wt.  %). 


Gms.  per  100 
Gms.  Sol. 

Wt.  per  cent  in 
Mix  Crystals. 

Gms.  per  100 
Gms.  Sol. 

Wt.  per  cent  in 
Mix  Crystals. 

'  AgNO3. 

NaN03. 

AgN03. 

NaNO3 

AgN03. 

NaN03. 

AgNO3. 

NaNOs 

47-32 

o 

•  O 

100 

O 

.0 

29 

.78 

o.o 

100 

o.o 

44-01 

8 

,78 

99-1 

O 

•9 

27 

•9 

2-5 

99 

5 

°-5 

36.78 

20 

.42 

42.9 

57 

.1 

26 

•4 

4.2 

99 

•3 

0.7 

29.97 

23 

.2 

33-6 

66 

•4 

23 

.0 

6.3 

42 

9 

57-i 

24.56 

24 

.82 

27.6 

72 

•4 

18 

•3 

7.1 

3* 

.0 

69.0 

8.02 

26 

.41 

9-9 

90 

.1 

9 

•5 

8.3 

17 

•5 

82.5 

o.o 

26 

•77 

o.o 

100 

.0 

0 

.0 

8.54 

o 

.0 

100.  0 

Very  extensive  data  for  equilibrium  in  the  system  silver  nitrate,  succinic  acid 
nitrile  and  water  are  given  by  Middelberg  (1903).  This  author  first  gives  data 
for  the  ternary  systems  and  then  results  for  isotherms  of  the  ternary  system  at 
o°,  12°,  20°,  25°  and  26.5°.  A  number  of  determinations  for  higher  temperatures 
are  also  given.  The  following  compounds  of  succinic  nitrile  and  silver  nitrate 
were  identified;  C2H4(CN)2.4AgNO3,  C2H4(CN)2.2AgNO3,  C2H4(CN)2.AgNO3, 
2C2H4(CN)2.AgN03.H20,  and  4[2C2H4(CN)2.AgNO3]H2O.  Additional  data  for 
this  system  are  also  given  by  Timmermans  (1907). 


SOLUBILITY  OF  SILVER  NITRATE  IN  ALCOHOLS. 

(de  Bruyn,  1892.) 

100  gms.  abs.  methyl  alcohol  dissolve  3.72  gms.  AgNO3  at  19°. 
100  gms.  abs.  ethyl  alcohol  dissolve  3.10  gms.  AgNO3  at  19°. 


SOLUBILITY  OF  SILVER  NITRATE  IN  AQUEOUS  ETHYL  ALCOHOL, 

(Eder,  1878.) 

Sp.  Gr.of  Aq.        Volume  Gms.  AgNO3  per  100  Gms.  Aq.  Alcohol  at: 

Alcoholic  per  cent  / * s 

Mixture-  Alcohol.  15°.  50°.  75°. 

0.815     95      3.8     7.3     18.3 
0.863     80     10.3     ...      42.0 

0.889        70         22.1 

0.912        60         30.5        58.1         89.0 

0.933        50         35.8 

0.951     40      56.4     98-3     160.0 
0.964     30      73.7 

0-975        2°        107.0      214.0        340-0 

0.986  10  158-0 

ioo  gms.  of  a  mixture  of  I  vol.  (95%)  alcohol  +  I  vol.  ether  dissolve  1.6  gms. 
AgNO3  at  15°. 

ioo  gms.  of  a  mixture  of  2  vols.  (95%)  alcohol  +  I  vol.  ether  dissolve  2.3  gms. 
AgNO3  at  15°. 

ioo  gms.  H2O  sat.  with  ether  dissolve  88.4  gms.  AgNO3  at  15°.          (Eder,  1878.) 

ioo  gms.  acetone  dissolve  0.35  gm.  AgNO3  at  14°,  and  0.44  gm.  at  18°. 

(von  Lasczynski,  1894;  Naumann,  1904.^ 


6 19  SILVER  NITRATE 

SOLUBILITY  OF  SILVER  NITRATE  IN  SEVERAL  SOLVENTS. 


Solvent. 

Acetonitrile  (anhydrous) 

a 

1  8                       290 
ord.  temp,     about  150 

Authority. 
(Naumann  and  Schier,  1914.) 
(Scholl  and  Steinkopf,  1906.) 

Benzonitrile 

18           about  105 

(Naumann, 

1914.) 

Benzene 

35 

O.022 

(Linebarger 

,  1895.) 

{( 

40.5 

0.044 

Hydrazine 

(anhydrous) 

ord.  temp. 

I  (with  decomp.)         (Welsh  and  Broderson,  1915.) 

SOLUBILITY  OF  SILVER  NITRATE  IN 

PYRIDINE. 

(Kahlenberg  and  Brewer,  1908.) 

t°. 

Gms.  AgNOj 
per  100  Gms. 

Solid  Phase. 

t°. 

Gms.  AgNO, 
per  too  Gms. 

Solid  Phase. 

CjHjN. 

C^N. 

-48.501. 

pt.     o 

C5H6N 

45 

62  .  26     AgNOj.sQHjN 

-50-5 

3 

" 

46 

63  .  09 

-53 

6 

" 

47 

66.35         ' 

| 

-59 

9 

« 

48 

70.85         ' 

—65  Eutec. 

"+AgNO3.6C5H8N 

48.5tr. 

pt.    ... 

[+AgNO,.2CsHbN 

-51-25 

II.  I 

AgNO,.6CsHsN 

45 

69.85 

AgNOa.jQHiN 

-44 

ix.  7 

" 

50 

72.25 

" 

-40 

12.2 

" 

60 

78.60 

« 

-35 

12.6 

" 

70 

89.10 

" 

-30 

13-9 

<( 

80 

121.  21 

« 

-25 

I7.6 

" 

87 

215.02 

" 

—  24  tr.  pt 

.            ... 

"+AgN03.3C5H6N 

80 

228.5 

« 

—  22 

18.8 

AgNOs.aCsHsN 

74 

230.6 

« 

—  10 

20.03 

" 

74 

225.4 

H 

0 

22.34 

« 

80 

230.4 

« 

+  10 

27.21 

<( 

87 

237.1 

H 

20 

33.64 

" 

90 

241.9 

" 

30 

40.86 

" 

100 

253-8 

M 

40 

53.52 

« 

no 

271.4 

* 

Fusion-point  data  for  mixtures  of  AgNOa  +  T1NO3  are  given  by  van  Eyk  (1905). 

SILVER  NITRITE  AgNO2. 

SOLUBILITY  IN  WATER. 

(Creighton  and  Ward,  1915.) 


O 
10 

15 


Cms.  AgN02 
per  Liter. 

1-55 
2.  2O 

2-75 


2O 

25 
30 


Cms.  AgNOj 
per  Liter. 

3-40 
4.14 
5 


40 
50 
60 


Gms.  AgNOj 
per  Liter. 

7-15 

9-95 
13-63 


The  determinations  by  Abegg  and  Pick  (1906)  are  slightly  higher  than  the 
above  at  temperatures  below  20°.  Single  determinations  agreeing  well  with 
the  above  are  given  by  Ley  and  Schaefer  (1906),  and  by  von  Niementowski  and 
von  Roszkowski  (1897). 


SOLUBILITY  IN 

Mols,  per  Liter. 

AQUEOUS  SOLUTIONS  OF  SILVER  NITRATE  AT  18°. 

(Naumann  and  Rucker,  1905.) 
Grams  per  Liter.              Mols.  per^  Liter                     Grams  per  Liter. 

AgNO3. 

o.oooo 

0-00258 
0-00517 
0.01033 

AgNO2. 
0.02067 
0.01975 
0.01900 
0.01689 

AgN03. 

o.ooo 

0-439 
0.878 

I-756 

AgN02. 
3.184 
3.042 
2  .926 
2  .6ol 

AgN03. 
0.02067 

0.04134 
0.08268 

AgN02. 
0-01435 

o.  01168 

0-00961 

AgN03- 

3-512 

7.024 
14.048 

AgN02. 
2.201 
1-799 
1.480 

SILVER  NITRITE  620 

SOLUBILITY  OF  SILVER  NITRITE  IN  AQUEOUS  SOLUTIONS  OF  SILVER  NITRATE 
AND  OF  POTASSIUM  NITRITE  AT  25°. 

(Creighton  and  Ward,  1915.) 
In  Aqueous  AgNO3.  In  Aqueous  KNO2. 

Mols.  AgNOj,          Dissolved  AgNO2  per  Liter.  Mols.  KNO2.        Dissolved  AgNO2  per  Liter. 

per  Liter.  Mols.         =        Cms.  per  Liter.  Mols.  Cms. 

o  0.0269  4-135  o  0.0269  4-135 

0.00258  0.0260  3-991  0.00258  0.0259  3-974 

0.00588  0.0244  3-735  0.00588  0.0249  3.820 

0.01177  0.0224  3.432  0.01177  0.0232  3-56o 

0.02355  0.0192  2.943  0.02355  0.0203  3-ii9 

0.04710  0.0164  2.498  0.04710  0.0181  2.765 

Additional  determinations  of  the  solubility  of  silver  nitrite  in  aqueous  silver 
nitrate  solutions  at  25°  are  given  by  Abegg  and  Pick  (1905). 

One  liter  aqueous  0.02  n  NaNO2  dissolves  3.185  gms.  AgNO2  at  25°., 
"       "          "        0.20  n       "  "        3.016     " 

"       "          "        o.2onNaNO3        "        4.956     " 

(Ley  and  Schaefer,  1906;  see  also  p.  660.) 

ioo  gms.  H2O  sat.  with  both  salts  contain  10.9  gms.  AgNO2  +  78.3  gms. 
Sr(NO2)i  at  14°.  (Oswald,  1912, 1914.) 

ioo  gms.  acetonitrile  dissolve  about  23  gms.  AgNO2  at  ord.  temp,  and  about 
40  gms.  at  the  boiling-point  (8l.6°).  (Scholl  and  Steinkopf,  1906.) 

SILVER  OXALATE  Ag2C2O4. 

One  liter  H2O  dissolves  0.0378  gm.  Ag2C2O4  at  21°,  see  Note,  p.  608. 

(Whitby,  1910.) 
One  liter  H2O  dissolves  0.0416  gm.  Ag2C2O4  at  25°.     Conductivity  method. 

(Schafer,  1905.) 

One  liter  H2O  dissolves  0.0265  gm.  Ag2C2O4  at  9.72°,  0.034  Sm-  at  18.5°  and 
0.043  gm.  at  26.9°.  (Kohlrausch,  1908.) 

SOLUBILITY  OF  SILVER  OXALATE  IN  AQUEOUS  NITRIC  ACID  AT  25°. 

(Hill  and  Simmons,  1909.) 


Normal- 

Per cent 

3      t 

Gms. 

Normal- 

Per cent 

J        -.£ 

Gms. 

ity  of 
Aq.  HNO3. 

Cone, 
of  HNO3. 

«25  OI 

Sat.  Sol. 

Ag2C204. 
per  Liter. 

ity  of 
Aq.  HN03. 

Cone, 
of  HNO3. 

026  O* 

Sat.  Sol. 

Ag,CA 
per  Liter  . 

0.2517 

1-574 

1.0080 

1-345 

4.017 

22.37 

I.I4I5 

17.11 

0.5025 

3-II7 

I.OI86 

2.189 

5-564 

29.84 

1.1996 

29.96 

0.9806 

6.017 

1-0339 

3-720 

5.83 

31.085 

I.2I62 

33-88 

1.040 

11.476 

I  .  0647 

7.170 

SILVER   OXIDE  Ag2O. 
One  liter  of  H2O  dissolves  0.021  gm.  at  20°,  and  0.025  gm«  at  25°. 

(Noyes  and  Kohr;  Bottger;  Abegg  and  Cox.) 

One  liter  H2O'dissolves  0.0215  gm.  Ag2O  at  20°.     (See  Note,  p.  608.)  (Whitby,  1910.) 
SOLUBILITY  OF  SILVER  OXIDE  IN  WATER. 

(Rebiere,  1915.) 

Gm.  Mols.  Ag2O  per  Liter.         Gms.  Ag2O  per  Liter. 

Method  of  Preparation  of  the  Sample. S_±I . — .        ,_ ~i£r — > 

At  25  .  At  50  .  At  25°.         At  50  . 

By  action  of  NaOH  on  AgNO3      2.I6.IQ-4  2.97.IQ-4  0.050  0.0691 

By  action  of  Ba(OH)2  on  AgNOs  2.23.IO"4  s.OQ.icr4  0.0519  0.0719 

By  action  of  KOH  on  AgCl           2.32.10-*  3.55.IQ-4  0.0538  0.0825 

By  action  of  KOH  on  Ag2COj        2 . 95 .  lo"4  3 . 89 .  lo"4  o .  0680  o .  0904 

SOLUBILITY  OF  SILVER  OXIDE  IN  AQUEOUS  AMMONIA  AT  25°. 

(Whitney  and  Melcher,  1903.) 

Mols.  NH3        Gm.  Atoms  Ag  Mols.  NH3         Gm.  Atoms  Ag  Mols.  NH3        Gm.  Atoms  Ag 

(Total)  per  Liter.        per  Liter.          (Total)  per  Liter.        per  Liter.  (Total)  per  Liter.       per  Liter. 

0.220  0.0658  0.733  0.224  I-I47  0.343 

0.469  0.134  0.876  0.257  1.498  0.454 

©•.684  O.2O5  0.915  0.276  1.522  0.470 


621 


SILVER  OXIDE 


SOLUBILITY  OF  SILVER  OXIDE  IN  AQUEOUS  SOLUTIONS  OF  ETHYL  AMINE  AND 
OF  METHYL  AMINE  AT  18°. 

(Euler,  1903.) 
In  Aqueous  Ethyl  Amine.  In  Aqueous  Methyl  Amine. 

Normality  of  Normality  of  Normality  of  Normality  of 

Aq.  Amine.  Dissolved  Ag.  Aq.  Amine.  Dissolved  Ag. 

O.IOO  0.0322  O.IOO         O.O22I 

0.50  0.160  0.500  0.118 

I  O-3I4  I  O.228 

SILVER  PERMANGANATE  AgMnO,. 

100  gms.  cold  water  dissolve  0.92  gm.:  hot  water  dissolves  more. 

(Mitscherlich,  1832.) 

SILVER  PHOSPHATE  Ag3PO4. 

One  liter  of  water  dissolves  0.00644  gm.  at  20°. 


SILVER  PROPIONATE  C2H5COOAg. 

SOLUBILITY  IN  WATER. 

(Raupenstrauch,  1885;  Arrhenius,  1893;  Goldschmidt,  1898.) 

t o '  Gms.  C3H5O2Ag  to  Gms.  C3H5O2Ag  t<, 

per  Liter.  per  Liter. 

O  5.12  20  8.36(8.48)  50 

10  6.78  25          9.06  70 

18.2  8. 36  (A)  30          9.93(9.70)  80 


(Bottger,  1903.) 


Gms.  C3HBO2Ag 
per  Liter. 

13-35 
17.64 
20.30 


SOLUBILITY  OF  SILVER  PROPIONATE  IN  AQUEOUS  SOLUTIONS  OF: 

(Arrhenius.) 


Silver  Nitrate  at  19.7°. 

Mols.  per  Liter.  Gms.  per  Liter. 


Sodium  Propionate  at  18.2°. 

Mols.  per  Liter.  Gms.  per  Liter. 


AgNO3. 

C3H502Ag. 

AgN03.      C3H502Ag. 

C3H5O2Na. 

C3H6O2Ag. 

C3H502Na. 

C3H502Ag. 

O 

0 

,0471 

O 

8.519 

O 

O, 

,0462 

0 

8.362 

0.0133 

0. 

0415 

2 

,289    7.511 

0. 

0167 

0 

0393 

I. 

607 

7.II4 

0.0267 

0. 

0379 

4 

,577     6.86 

0. 

0333 

0, 

0345 

3- 

215 

6.244 

0.0533 

0. 

0307 

9 

059     5-556 

O. 

0667 

0. 

0258 

6. 

429 

4.670 

O.IOO 

0. 

0222 

16, 

997     4-019 

0. 

1333 

0. 

0191 

12. 

859 

3.456 

0. 

2667 

0. 

0131 

25. 

7l8 

2.371 

O. 

5000 

0. 

OIOI 

48. 

77 

1.828 

SILVER  SALICYLATE  C6H4.OH.COOAg  1,2. 

One  liter  of  aqueous  solution  contains  0.95  gm.  at  23°. 


(Holleman,5i893.) 


SILVER  SUCCINATE  C4H4O4Ag2. 

100  gms.  H2O  dissolve  0.0176  gm.  at  18°,  and  0.0199  Sm-  at  25°- 

(Partheil  and  HUbner,  1903.) 

SILVER  SULFATE  Ag2SO4. 


O 
IO 
20 
25 


Gms.  Ag2SO4  per 
100  Gms.  Sat.  Sol. 

0-57 
0.69 
0.79 
0.834 


SOLUBILITY  IN  WATER. 

(Barre,  1911.) 

.  „  Gms.  Ag2SO4  per 

1  *         100  Gms.  Sat.  Sol. 

0.88 


30 
40 

50 
60 


0.97 
1.05 
I.I4 


70 

80 

00 

100 


Gms.  Ag2SO4  per 
100  Gms.  Sat.  Sol. 

I. 21 

1.28 

1-34 

1-39 


The  result  at  25°  is  the  average  of  the  very  accurate  and  closely  agreeing 
determinations  of  Hill  and  Simmons  (1909),  Rothmund  (1910)  and  Harkins 
(191 1 ).  Earlier  determinations,  differing  somewhat  from  the  above,  are  given  by 
Euler  (1904),  Wright  and  Thompson  (1884),  Wentzel  (  )  and  Drucker  (1901). 


SILVER  SULFATE 


622 


SOLUBILITY  OF  SILVER  SULFATE  IN  AQUEOUS  SOLUTIONS  OF  AMMONIUM 

SULFATE. 

(Barre,  1911.) 


Results  at  33°. 

Gms.  per  100  Gms. 
Sat.  Sol. 

Results  at  51°. 

Gms.  per  100  Gms. 
Sat.  Sol. 

Results  at  75°. 

Gms.  per  100  Gms, 
Sat.  Sol. 

Results  at  100°. 

Gms.  per  100  Gms. 
Sat.  Sol. 

(NH4)2S04.    I 
8.85 
15.90 
22.22 
27.25 
30.80 

35-88 
43.22 

^g2SO4. 
.101 

•331 

.500 

.585 

.619 

.627 

.600 

•557 

8.90* 
16.27 
22.43 
32.10 
35-38 
39-03 
42.37 
45-05 

Ag2S04." 
1.362 
1.680 
1.887 
2.o6l 
2.095 
2  .082 
2-055 
2.026 

(NH4)2S04. 
8.80 

I5-23 
22.30 
28.25 
32 
35-82 
4I.l6 
46.46 

Ag2so;. 

1.758 

2.155 
2.490 

2.734 

2.823 
2.889 
2.929 
2.902 

(NH4)2S04. 
9.23 
15 
22.01 

27 
34.90 
38.70 

44-15 
47.63 

Ag2so4: 

2.221 
2.626 
3-075 
3-325 
3-663 
3-772 

^867 

A  series  of  determinations  at  16.5°  is  also  given. 


SOLUBILITY  OF  SILVER  SULFATE  IN  AQUEOUS  NITRIC  ACID  AT  25°. 


(Hill  and  Simmons,  1909.) 


Normality 


01  Aq. 
HNO3. 

L-onc.  01  Aq. 
HN03. 

Sat.  Sol. 

per  Liter. 

OI  Aq. 

HNO3. 

^onc.  01  Aq 
HN03. 

'    Sat.  Sol. 

per  Liter. 

0 

0 

I 

.0054 

8-35 

4 

.209 

23-33 

I 

.1956 

73.212 

1.0046 

6 

•154 

I 

.O6l 

34.086 

5 

•564 

29.84 

I 

.2456 

84  .  609 

2.0452 

12 

.005 

I 

.1069 

49-OIO 

8 

.487 

42.37 

I 

.3326 

94.671 

4.017       22.37      1.1871     71.166    10.034    48.77     1.3676    90.806 

SOLUBILITY  OF  SILVER  SULFATE  IN  AQUEOUS  SOLUTIONS  OF  ACIDS  AND 

SALTS  AT  25°. 

(Swan,  1899.) 


Acid  or 
Salt. 

Gm.  Equiv.    Gms.  Dissolved 
per  Liter.     Ag2SO4  per  Liter. 

HNO3 

0 

8.41 

" 

0.01589 

9-33 

tt 

0.03178 

10.18 

(( 

0.06357 

11.83 

KHS04 

0.05264 

8.13 

tt 

0.10526 

8.07 

Acid  or 
Salt. 

Gm.  Equiv.        Gms.  Dissolved 
per  Liter.          Ag2SO4  per  Liter. 

H2SO, 

O 

8.41 

u 

0.02902 

8-55 

u 

0.05802 

8.68 

K 

O.IO526 

8.86 

K2SO4 

O.O27I8 

7-93 

tt 

0.05434 

7.68 

SOLUBILITY  OF  SILVER  SULFATE  IN  AQUEOUS  SOLUTIONS  OF  SALTS  AT  25°. 

(Harkins,  1911.) 


Gm.  Eauiv.             j 

Gms. 

Gm.  Eauiv. 

j     *r 

Gms. 

Salt. 

A.    **»• 

Ag2SO4  per 
Liter. 

Salt. 

Salt 
per  Liter. 

"25  ul 

Sat.  Sol.  * 

Ag2S04 
per  Liter. 

KNO3 

o 

.  .  . 

8-344 

AgN03 

0. 

09961 

I 

0137 

2 

.644 

u 

0 

024914 

.0072 

8.996 

K2SO4 

O. 

025024 

i 

0064 

7 

.899 

u 

0 

049774 

.0092 

9.531 

tt 

0. 

050044 

i 

0079 

7 

.694 

tt 

o 

09987 

.0034 

10.435 

tt 

0. 

IOO 

x 

0112 

7 

•49 

Mg(N03)2 

0 

024764 

.0073 

9.267 

" 

0. 

20003 

I 

Ol8o 

7 

.531 

" 

0 

049595 

.0094 

10.029 

MgS04 

o. 

020022 

X 

.0061 

8 

.140 

lf 

0 

09946 

•0133 

".334 

" 

o. 

050069 

X 

.0079 

7 

.941 

AgN03 

0 

024961 

.0065 

6.095 

tt 

0. 

IOOO4 

X 

.0105 

7 

.740 

" 

0. 

04986 

.0084 

4.487 

tt 

0. 

20005 

X 

0164 

7 

•  733 

One  liter  of  aqueous  solution  in  contact  with  a  mixture  of  silver  sulfate  and 
silver  acetate  contains  3.95  gms.  Ag2SO4  +  8.30  gms.  CH3COOAg  at  17°.  Sp.  Gr. 

of  solution  =  1.0094.  (Euler,  1904.) 


623 


SILVER  SULFATE 


SOLUBILITY  OF  SILVER  SULFATE  AT  25°  IN  AQUEOUS  SOLUTIONS  OF: 

(Drucker,  1901.) 


Sulfuric  Acid. 

Mols.  per  Liter.  Cms.  per  Liter. 


Potassium  Sulfate. 

Mols.  per  Liter.  Cms,  per  Liter. 


Ag2S04. 

H2SO4. 

Ag2S04. 

H2so4: 

'Ag2S04. 

K2S<V 

Ag2S04. 

K2so4: 

O.O26O 

O.O2 

8.  ii 

0.98 

0.0246 

O.O2 

7.67 

1.74 

0.0264 

0.04 

8.23 

1.96 

0.0236 

O.O4 

7.36 

3-49 

0.0271 

O.IO 

8-45 

4.90 

0.0231 

O.IO 

7.20 

8.72 

0.0275 

O.2O 

8.58 

9.81 

0.0232 

O.2O 

7.24 

17.44 

SOLUBILITY  OF  SILVER  SULFATE  IN  AQUEOUS  POTASSIUM  SULFATE  SOLUTIONS. 

(Barre,  1911.) 


Results  at  33°.          Results  at  51°.  Results  at  75°. 


Results  at  100°. 


Gms.  per  100  Gms. 
Sat.  Sol. 

Gms.  per  100  Gms. 
Sat.  Sol. 

Gms.  per  100  Gins. 
Sat.  Sol. 

Gms.  per  100  Gms. 
Sat.  Sol. 

K2S04. 
3.22 
5-62 

8-37 
10.41 
11.80 

Ag2S04. 
0.863 
0.940 
1.046 
I.II7 
I.I77 

'K2S04. 
3-20 
5-6l 
8.40 

10.55 
I3.l6 

14-37 

Ag2S04. 
1.023 
I.I27 
1.247 
1.340 
1.450 
1.524 

'K2S04. 
3-12 

5-73 
8-43 
10-55 
13-17 
17.06 

Ag2SO4. 

1.273 
1.406 

1-554 
1.665 
i.  806 

2.021 

K2S04. 
3-23 
5.60 

8-45 
11.30 

I5.07 
18.58 

Ag2S04. 
1.488 

I.675 
1.890 

2.H5 
2.410 
2.677 

Results  at  14.5°  are  also  given. 
SOLUBILITY  OF  SILVER  SULFATE  IN  AQUEOUS  SODIUM  SULFATE  SOLUTIONS. 

(Barre,  1910,  1911.) 


Results  at  33°. 

Gms.  per  100  Gms. 
Sat.  Sol. 

Results  at  51°. 

Gms.  per  100  Gms. 
Sat.  Sol. 

Results  at  75°. 

Gms.  per  100  Gms. 
Sat.  Sol. 

Results  at  iood. 

Gms.  per  too  Gms. 
Sat.  Sol. 

Na2S04. 

Ag2S04. 

Na2SO4. 

Ag2SO4. 

Na2S04. 

Ag2SO4. 

Na2S04.        Ag2S04. 

0.25 

0.861 

0.25 

1.032 

O.20 

I.2I5 

0.50 

•341 

0.98 

0.816 

1.02 

0-995 

0.98 

I.  210 

1.  01 

.363 

2.OI 

0.832 

1.90 

I.OI7 

1.96 

1.238 

1.94 

.418 

3 

0.867 

2.92 

1-053 

2.98 

1.296 

3-02 

•494 

5-34 

0.972 

5-40 

I-I73 

5-37 

1.458 

5-33 

.651 

10.05 

1.150 

IO.  II 

1-379 

9.81 

1.697 

IO.I5         2.OI2 

20.09 

1.448 

20.25 

1-705 

19.98 

2.075 

25-45         2.351 

29-55 

1-570 

29.23 

1.802 

29.66 

2.138 

34.72         2.012 

39-44 

1.462 

39-30 

1.540 

38.94 

1.603 

38.63         1.687 

46.976 

0.932 

44.46 

0.882 

41.36 

I.I56 

40.16         I.I58 

Results  at  14.5°  and  at  18°  are  also  given. 

SOLUBILITY  IN  SILVER  SULFATE  IN  AQUEOUS  0.5  n  SOLUTIONS   OF   VARIOUS 

COMPOUNDS  AT  25°. 

(Rothmund,  1910.) 


Aq.  0.5  n 

Gms. 
Dissolved 

Aq.  0.5  » 

Gms. 
Dissolved 

Aq.  0.5  n 

Gms. 
Dissolved 

Solution  of: 

Ag2SO< 
per  Liter. 

Solution  of: 

Ag2S04 
per  Liter. 

Solution  of: 

Ag2S04 
per  Liter. 

Methyl  Alcohol 

7- 

764 

Glycerol 

8 

.202 

Acetonitrile 

16. 

37 

Ethyl  Alcohol 

7- 

109 

Mannitol 

9 

.262 

Glycocol 

13 

50 

Propyl  Alcohol 

6 

798 

Grape  Sugar 

8 

.418 

Acetic  Acid 

7 

857 

AmyPAlc.  (tert.) 

6 

36 

Urea 

9 

.448 

Phenol 

ii 

,81 

Acetone 

6 

.86 

Dimethylpyrone 

6 

.736 

Chloral 

7, 

,266 

Ether 

6 

424 

Urethan 

7 

.078 

Methylal 

6 

393 

Formaldehyde 

7 

078 

Formamide 

8 

.42 

Methyl  Acetate 

6 

61 

Glycol 

8. 

076 

Acetamide 

7 

•794 

Fusion-point  data  for  Ag2SO4  +  Na2SO4  are  given  by  Nacken  (1907). 


SILVER   SULFIDE  624 

SILVER  SULFIDE  Ag2S. 
One  liter  H2O  dissolves  about  4.10-"  gm.  atoms  Ag  as  sulfide  at  about  18°. 

(Bernfeld,  1898.) 

One  liter  H2O  dissolves  0.55. lO"6  gm.  mols.  =  0.0001363  gm.  Ag2S  at  18°. 

(Weigel,  1907.) 
Fusion-point  data  for  AgaS  -f-  ZnS  are  given  by  Friedrich  (1908). 

SILVER   SULFONATES 

SOLUBILITY  IN  WATER  AT  20°. 

(Sandquist,  1912.) 

<?iilfnnati»  Cms.  Sulfonate"' 

per  100  Gms.  H2O. 

Silver  .2  Phenanthrene  Monosulfonate]  o.ooo 

"        -3  "  0.20 

"        .10  0.52 

SILVER  TARTRATE  C4H4O6Ag2. 

100  gms.  H2O  dissolve  0.2012  gm.  C^OeAgjj  at  18°,  and  0.2031  gm.  at  25°. 

(Partheil  and  Hiibner,  1903.) 

SILVER  THIOCYANATE  AgSCN. 

SOLUBILITY  IN  WATER. 

t°.  Gm.  AgSCN  per  Liter.  Authority. 

20  O.OOOI4  (Bottger,  1903.) 

21  0.00025  (Whitby,  1910.    See'Note,  p.  608.) 
25                      O  .  OOOI 7  (Kuster  and  Thiel,  1903.) 

25  O  .  OOO2  (Abegg  and  Cox,  1903.) 

100  0.0064  (Bottger,  1906.) 

Additional  data  for  the  solubility  of  AgSCN  in  water  are  given  by  Kirschner 
(1912.) 

SOLUBILITY  OF  SILVER  THIOCYANATE  IN  AQUEOUS  POTASSIUM  THIOCYANATE 

AT  25°.      (Hellwig,  1900.) 

Mols.  KSCN       Mols.  AgSCN    Gms.  AgSCN  Mols.  KSCN      Mols.  AgSCN      Gms.  AgSCN 

per  Liter.  per  Liter.  per  Liter.  per  Liter.  per  Liter.  per  Liter. 

0.573     0.0124    2.06       1. 12    0.0975    16.18 
0.626     0.0168    2.08       1.20    0.120     iQ-93 

1. 066      0.0850     14.01          1.25      0.134       22.34 

One  liter  of  aqueous  3  n  AgNO3  dissolves  0.0432  gm.  AgSCN  at  25.2°.  (Hellwig,  1900.) 

SILVER  VALERATES  AgC6H9O2. 

Normal  Valerate,  CH3(CH2)3.COOAg.     Iso  Valerate,  CH3.CH(CH3)2CH2COOAg. 
SOLUBILITY  OF  EACH  SEPARATELY  IN  WATER. 

(Fiirth,  1888;  Sedlitzky,  1887.) 

Gms.  per  100  Gms.  H2O.  Gms.  per  100  Gms.  HaO.  • 

t0'  Normal  V.  Is^T.  t0'  Normal  V.  Iso  V.  " 

o  0.229  °-I77  50  Q-474  0.360 

10  0.259  0.211  60  0.552  0.401 

20  0.300  0-246  70  0.636  0.443 

30  0.349  0.283  80  ...  0.486 

40  0.408  0.321 

loo  gms.  H2O  dissolve  0.73  gm.  silver  valerate  at  20°.  (Markwald,  1899.) 

loo  cc.  sat.  aq.  solution  contains  0.71  gm.  dextro  silver  valerate  at  15°. 

(Taverne,  1900.) 


625 


SILVER  VALERATE 


SOLUBILITY  OF  SILVER  VALERATE  IN  AQUEOUS  SOLUTIONS  OF  SILVER 
ACETATE,  SILVER  NITRATE  AND  OF  SODIUM  VALERATE. 

(Arrhenius,  1893.) 


In 

Silver  Acetate  at  17.8°. 

In  Silver  Nitrate  at  16.5°. 

IMols. 

per  Liter. 

Gms.  per  Liter. 

Mols.  per  Liter. 

Gms. 

per  Liter. 

C2H302Ag. 
0 
0.0067 

C6H902Ag. 
0.0094 
O.0070 

C^HiAAg.   CBH9O2Ag. 

o              1.96 

I  .  13           I  .  46 

AgN03.      C5H902Ag. 

o              0.0094 

0.0067      0.0068 

AgNO3. 
0 
I.I4 

C6H902Ag. 
1.96 
1.42 

0.0135 
O.027O 
0.0505 

0.0057 
0.0037 
0.00265 

2.27           I.I9 
4.54           0.77 
8.48           0.55 

0.0133      0.0051 
0.0267      O.003I 
O.IOOO      O.OOI2 

2.29 
4.58 
17. 

1.07 
0.65 
0.25 

In  Sodium  Valerate  at  18.6°. 

Mols. 

per  Liter. 

Gms.  per  Liter. 

C2H302Na. 
O 
0.0175 
0.0349 
0.0698 

CBH902Ag. 
0.0095 
0.0047 
0.0030 
O.OOlS 

C2H,02Na. 
0 
2.17 
4-32 
8.65 

CBH902Ag. 
1.986 
0.982 
0.627 
0.376 

0.1395 

0.0015 

17.  31 

0.313 

SILVER  VANADATE  Ag,V4Qii. 

One  liter  of  aqueous  solution  contains  0.047  gm.  at  14°,  and  0.073  gm.  at  iOo° 

(Carnelly,  1873. 

SODIUM  Na. 

SOLUBILITY  IN  LIQUID  AMMONIA. 

(Ruff  and  Geisel,  1906.) 


t". 

105 

70 
50 

Mols.  NH3  Required 
to  Dissolve  i  Gm. 
Atom  Na. 

4.98 
5.20 

5-39 

t°. 
-30 

0 
+  22 

Mols.  NH3  Required 

to  Dissolve  i  Gm. 

Atom  Na. 

5-52 
5-87 
6.14 


SOLUBILITY  OF  SODIUM  IN  MELTED  SODIUM  HYDROXIDE. 

(von  Hevesy,  1909.) 

t°.  480°       600°       610°       670°       760° 

Gms.  Na  per  zoo  Gms.  NaOH       25.3       10.1        9.9        9.5        7.9 


800° 
6.9 


Saturation  could  not  be  reached  at  temperatures  below  480°.  The  saturated 
mixtures  were  cooled  by  plunging  the  container  in  water  and  the  solidified  con- 
tents analyzed. 

SOLUBILITY  OF  SODIUM  IN  MELTED  SODIUM  HYDROXIDE  CONTAINING  OTHER 

METALS  AT  480°. 

(von  Hevesy,  1909.) 


'Added 

Metal. 

Gms.  Added 
Metal  per  100 
Gms.  NaOH. 

Gms.  Dissolved 
Na  per  100 
Gms.  Solvent. 

Added 
Metal. 

Gms. 
Metal 
Gms. 

Added 
per  too 
NaOH. 

Gms.  Dissolved 
Na  per  100 
Gms.  Solvent. 

Thallium 

5 

.40 

23.13 

Cadmium 

2 

.87 

24-34 

M 

8 

•30 

23.54 

u 

3 

.l6 

24.29 

M 

12 

.42 

21.29 

Gold 

6 

•03 

23.92 

It 

31 

•37 

20.91 

" 

8 

.22 

23.39 

Zinc 

30 

•37 

25.38 

SODAMMONIUM  Na2(NH3)2. 

100  gms.  liquid  ammonia  dissolve  60.5  gms.  Na2(NH3)a  at  —23°,  56.4  gms.  at 
0°,  56  gms.  at  +5°  and  55  gms.  at  9°.  (Joannis,  1906.) 


SODIUM  ACETATE  626 

SODIUM  ACETATE  CH3COONa.3H2O. 


Cms. 

t°. 

CH3COONa 

per  100 

Cms.  H2O. 

—  10 

19 

-18 

30-4 

—  10 

33 

o 

36.3 

+10 

40.8 

20 

46.5 

30 

54-5 

40 

65.5 

50 

83 

58 

138 

0 

119 

IO 

121 

SOLUBILITY  IN  WATER. 


(Green,  1968.) 


Solid  Phase. 


Ice 


CH3COONa.3H2O 


Cms. 

t°. 

CH3COONa 

per  100 

Cms.  H2O. 

20 

123.5 

30 

126 

40 

129.5 

50 

134 

60 

139-5 

70 

146 

80 

153 

90 

161 

100 

170 

no 

180 

120 

191 

123  b.  pt. 

193 

Solid  Phase. 


CH3COONa  (unstable) 


CH3COONa  (unstable) 


"  Results  differing  somewhat  from  the  above  are  given  by  Kohler  (1897) ;  Enklaar 
(1901)  and  Schiavor  (1902). 


SOLUBILITY  OF  SODIUM  ACETATE  IN  AQUEOUS  SOLUTIONS  OF  ACETIC  ACID  AT 
VARIOUS  TEMPERATURES. 

(Dunningham,  1912.) 

Results  at  o°.      Results  at  15°.    Results  at  30°.     Results  at  75°. 


Gms.  per  100  Gms. 
Sat.  Solution. 

Gms.  per  too  Gms. 
Sat.  Solution. 

Gms.  per  roo  Gms. 
Sat.  Solution. 

Gms.  per  100  Gms. 
Sat.  Solution. 

Solid  Phase 
in 

.NazO.  (CH3CQ)2O. 

29-34 

(CH3CO)20 
0-15 

.    Na2O. 

35-31 
26.25 

(CH3CO)2C 

0.77 
8.92 

>.    Na-,0. 

44-45 
32.47 
22.30 

17.85 
11.05 

7.63 

0.44 

(CH3CO)20.    Each  Case. 
0.76       CHjCOONa 
5.03 
36.69 
.  .  .      CH3COONa.3H20 

"  +1.1 
43  •  06              i.i 
65.71 
8i.49 
98.35 

"   +1.2 
...                        1.2 
« 
«« 
« 
el 
« 

24.12 
14.46 
9-72 

9-77 
9.04 

2.04 

8.55 

41.23 
43-94 

25-94 
15-49 

n-45 
11.25 
10.33 

10.22 
9.l6 

4 

12 
23 

34 
39 
39 
49 

.19 

.01 

•54 
-56 
.08 

•73 
-32 

25- 

18. 
13- 
13- 
13- 

7- 

98 
09 

53 
24 
14 
64 

9 
13 
21 

33 
32 
65 

.06 
.62 
.88 

.05 
.90 
.07 

8.96 
8.72 

7-83 
6.19 
4.02 
1.05 
0.42 

44.80 
45.10 
50.03 
62.44 
79.29 
92.29 
97-51 

8.56 
7.06 

5-95 
4.84 
2.87 
i.  02 
0.79 

.54 
61 
70 
77 
86 

95 
98 

•34 
•63 
-55 
.60 
.61 

-87 
.09 

7- 

6. 

5- 
3. 

2. 
I. 

67 
33 
61 

52 

78 
94 
27 

66 

69 

72 
77 
83 
86 

94 

-42 
.68 

-85 
.76 

•92 
-73 
.78 

i.i  =  CH3COONa.CH3COOH.     1.2  =  CH3COONa.2CH3COOH. 

Additional  data  for  5°,  20°,  45°  and  60°  are  also  given. 

Similar  data  for  30°  are  given  by  Dukelski  (1909),  and  for  20°  by  Abe  (191 1-12). 
One  determination  at  25°,  expressed  in  terms  of  volume  of  solution,  is  given  by 
Herz  (1911-12).  Two  determinations  at  10°  similarly  expressed,  are  given  by 
Enklaar  (1901). 

Data  for  the  freezing-point  of  mixtures  of  sodium  acetate  and  acetic  acid  are 
given  by  Vasilev  (1909). 


627 


SODIUM  ACETATE 


SOLUBILITY  OF  SODIUM  ACETATE  IN  AQUEOUS  ETHYL  ALCOHOL  AT  25°. 

(Seidell,  1910.) 

Gms.  CHjjCOO- 


Wt.  Per  cent 
QHsOH  in 
Solvent. 

•,    n(        Gms.  CH3COO- 
SfttSoL     NGm?2srri°° 

0 

1.209 

55-7 

IO 

1.  160 

53 

20 

i.i35 

49-8 

30 

1.108 

46.5 

40 

1.072 

42 

50 

1.038 

37 

Wt.  Per  cent 

,    * 

QHsOH  in 
Solvent. 

Sat5  Sol. 

60 

0.990 

70 

0.942 

80 

0.882 

90 

0.838 

95 

0.828 

IOO 

0.823 

30.4 

22.8 
13 
6.7 

6.1 

7-3 

The  solid  phase  in  contact  with  the  solution  was  CH3COONa.3H2O  in  all 
cases. 

ioo  gms.  absolute  alcohol  dissolve  7.49  gms.  CH3COONa.3H2O  at  room  temp. 

(Bodtker,  1897.) 

SOLUBILITY  OF  SODIUM  ACETATE  IN  AQUEOUS  ALCOHOL: 

At  Different  Temperatures. 

(Schiavor,  1902.) 


At  1  8°. 

(Gerardin,  1865.) 

Wt. 

Per  cent 
Alcohol. 

Gms.  CH3COONa 
per  ioo  Gms. 
Aq.  Alcohol. 

5-2 

38 

9.8 

35-9 

23 

29.8 

29 

27-5 

38 

23-5 

45 

20.4 

59 

14.6 

86 

3-9 

91 

2.1 

t°. 

Degree 
of 
Alcohol. 

Gms.  per  too  Gms.  Alcohol. 

CH3COONa. 

CH3COONa.3H2O. 

8 

98.4 

2.08 

3-45 

12 

98.4 

2.12 

3-51 

19 

98.4 

2-33 

3-86 

II 

90 

2.O7 

3-42 

13 

90 

2.13 

3-52 

15 

63 

I3-46 

22.32 

18 

63 

13.88 

23.03 

21 

63 

14.65 

24.30 

23 

40 

28.50 

47.27 

ioo  gms.  H2O  dissolve  237.6  gms.  sugar  +  57.3  gms.  CH3COONa,  or  100 
gms.  of  the  saturated  solution  contain  58.93  gms.  sugar  +  14.44  gms.  CH3COONa 
at  3 1. 25°.  (Kohler,  1897.) 

ioo  cc.  anhydrous  hydrazine  dissolve  6  gms.  sodium  acetate  at  room  temp. 

(Welsh  and  Broderson,  1915.) 

ioo  gms.  propyl  alcohol  dissolve  0.97  gm.  sodium  acetate.  (Schlamp,  1894.) 


SODIUM  SulfoANTIMONATE  Na3SbS4.9H2O. 


•o.i 

•0.65 

•0.9 

•1.26 

•1-45 


Gms. 

NajSbS4per 
too  Gms. 
Sat.  Sol. 

0-5 

4 

5-7 
7.8 
9.2 


Solid 
Phase. 

Ice 


SOLUBILITY 

IN  WATER 

(Donk, 

1908.) 

Gms. 
to       Na3SbS4  per        Solid 
ioo  Gms.          Phase. 
Sat.  Sol. 

—  I 
0 

.75       II.  2 
II.  8 

Ice 
Na3SbS4.9H2O 

15 
30 
38 

19-3 
27.1 

32 

it 

r. 

49.6 

59-6 
69.6 
79-5 


Gms. 

Na3SbS4  per      Solid 
ioo  Gms.        Phase. 
Sat.  Sol. 
38.9    Na3SbS4.9H20 

45 
50.7 

57-1 


SOLUBILITY  OF  SODIUM  SULFOANTIMONATE  IN  AQUEOUS  SOLUTIONS  OF  SODIUM 

HYDROXIDE  AT  30°. 

(Donk,  1908.) 

Gms.  per  ioo  Gms.  Sat.  Sol. 


Na3SbS4. 
27.1 

NaOH. 
0 

ooua  rnase. 
Na3SbS4.9H2O 

13 
5-9 

9.9 
24.8 

« 

10.5 

32.9 

• 

Na3SbS4. 

NaOH. 

*            ooua  rnase. 

16.4 

42.6 

Na2SbS4.9H,O 

17.7 

47.2 

"+NaOH.H2O 

9.1 

49-5 

NaOH.H2O 

0 

54.3 

SODIUM  SulfoANTIMONATE 


628 


SOLUBILITY  OF  SODIUM  SULFOANTIMONATE  IN  AQUEOUS  SOLUTIONS  OF  SODIUM 

THIOSULFATE. 

(Donk,  1908.) 


Results  at  o°. 

Gms.  per  100  Gms.  Sat.  Sol. 
'  Na3SbS4. 


Solid  Phase. 


ii. 8 
4.4 
0.8 

O.I 

o 
o 


o 

4-9 

14.6 

27-3 
33-6 
33-6 


Na3SbS4.9H20 


Na8S20J.SHiO 


Results  at  30°. 


Na3SbS*. 
19.9 
12-5 

Na2S203.   ' 

7-7 
16.4 

ooiia  rnase. 
Na3SbS4.9H20 

4-2 

37-7 

" 

I 

43-8 

" 

I 

47 

" 

I 

47.8 

"  +Na2S203.5H20 

0 

45-8 

Na2S203.SH20 

SOLUBILITY  OF  SODIUM  SULFOANTIMONATE  IN  AQUEOUS  ETHYL  ALCOHOL. 

(Donk,  1908.) 


Results  at  30°. 

Cms.  per  100  Gms.  Sat.  Sol. 


Results  at  65°. 

Gms.  per  100  Gms.  Sat.  Sol. 


Results  at  o°. 

Gms.  per  100  Gms.  Sat.  Sol. 
N&sSbS^  CjHsOri. 

ii. 8  o 

8.2  3.7 

3.2  12.7 

0.9  29 

o  60.8 

*  Two  liquid  layers  separate  between  these  concentrations  of  alcohol.    The  composition  of  several 
of  these  conjoined  layers  is  as  follows: 


Na3SbS4. 

C2H5OH. 

Na3SbS4. 

C2HBOH.  ' 

19-3 

5 

47-9 

0 

14.6 

10.3 

39-3 

4-7 

6.4 

24.8 

36.5 

8* 

1.2 

46 

4.1 

54.i* 

0 

76.2 

o 

81 

Gms.  per  100  Gms.  Alcoholic  Layer. 

Na3SbS4. 

4.1 
10.2 
I4.I 


Gms.  per  100  Gms.  Aqueous  Layer. 


54-1 
40.4 

33-5 
o 


Na3SbS4. 

36.5 
27.8 
24.1 

18 


C2HBOH. 

8 

14.3 

18.8 
27.2 


The  solid  phase  in  contact  with  each  of  the  above  solutions  is  Na3SbS4.9H2O. 


SOLUBILITY  OF  SODIUM  SULFOANTIMONATE  IN  AQUEOUS  METHYL  ALCOHOL. 

(Donk,  1908.) 


Results  at  oc 


'  Na3SbS4. 

CH3OH." 

OUilU   JTllitSC. 

8.6 

3-4 

Na3SbS4.9H26 

2.8 

15-5 

" 

2.1 

23.1 

« 

0-3 

50.3 

" 

O.I 

57 

« 

0.05 

81.7 

" 

O.2 

92 

« 

2 

95-9 

M 

Results  at  30°. 

Gms.  per  100  Gms.  Sat.  Sol. 


Na3SbS4. 

CH3OH. 

27.1 
12.8 

O 

18.1 

5.8 

O.I 
O.I 

33-i 
65.7 
84.2 

1.2 

91.2 

3-9 

94 

Solid  Phase. 
Na3SbS4.9H2O 


SODIUM  ARSENATE  Na3AsO4.i2H2O. 

100  gms.  aqueous  solution  contain  21.1  gms.  Na3AsO4.i2H2O  (=  10.4  gms. 

Na8AsO4)  at  17°.     Sp.  Gr.  of  solution  =  1.1186.  (Schiff,  1860.) 

100  gms.  glycerol  dissolve  50  gms.  sodium  arsenate  at  15.5°.    (Ossendowski,  1907.) 


629 


SODIUM   ARSENATES 


EQUILIBRIUM  IN  THE  SYSTEM  SODIUM  OXIDE,  ARSENIC  TRIOXIDE,  WATER  AT  25°. 

(Schreinemakers  and  de  Boat,  1917.) 

Solid  Phase. 


AS20V 

N&£>. 

ouiiu  niiibc. 

As-A. 

Na2O. 

2.019 

0 

AsA 

3I-05 

21.82     ] 

14.45 

2-45 

" 

±29 

±22.7 

24.42 

4-23 

" 

21.92 

24.04 

37-73 

6.46 

" 

17-50 

25.64 

58.54 

9.60 

" 

14.26 

29.16 

±73 

±12 

"  +NaAs02 

14-63 

30.24 

63.01 

12.73 

NaAs02 

19.32 

32.04 

57-90 

13.24 

" 

15-53 

33-57 

48.05 

14.27 

M 

10.49 

36.21 

36.32 

18.74 

" 

6-59 

39-39 

±34 

±21.1 

"  +Na4As205.9H20 

5-ii 

39-69 

32.24 

21.6 

Na4As2O6.9H2O 

o 

41.2 

+NaioAs4On.26H,O 
Na10As4O11.26H2O 


+NaOH.H2O 
NaOH.H2O 


SODIUM   Hydrogen  ARSENATE  Na2HAsO4.i2H2O. 
SOLUBILITY  IN  WATER. 

(Average  curve  from  results  of  Schiff,  1860;  Tilden,  1884;  Greenish  and  Smith,  1901.) 


Cms.  Na2HAsO4 
per  100  Gms.  H2O. 


O 
10 
IS 


7-3 
15-5 

20.50*  = 


=  1.1765) 


20 
25 
30 


Gms.  Na2HAsO4 
per  100  Gms.  H2O. 
26.5 
33 
37 


40 
60 
80 


Gms. 
per  loo  Gms. 

47 
65 
85 


SODIUM   Diethyl  BARBITURATE   Na(C8HnO8N2). 
SOLUBILITY  IN  WATER. 

(Puckner  and  Hilpert,  1909.) 

16.87 


Gms.  Salt  per  100  Gms.  Sat.  Sol. 
SODIUM  BENZOATE  C6H5COONa. 


5° 
6.08 


25° 

17.18 


32-50 


SOLUBILITY  IN  AQUEOUS  ETHYL  ALCOHOL  AT  25°. 

(Seidell,  1910.) 


Wt.  Per  cent 

C2H5OH  in 

Solvent. 

O 
IO 
20 
30 
40 
50 


SODIUM  (Tetra)  BORATE  Na2B4O7.ioH2O  (Borax). 
SOLUBILITY  IN  WATER. 

(Horn  and  Van  Wagener,  1903.) 


1 
#25  OI 

3ms.  C6H5COONa 
per  100  Gms. 
Sat.  Sol. 

Wt.  Per  cent 
C2H5OH  in 
Solvent. 

&c  of        G 

Sat.  Sol. 

ms.  C6H5COONa 
per  loo  Gms. 
E  Sat.  Sol. 

-155 

36 

60 

0-975 

21.3 

.132 

35-3 

70 

0.927 

15-4 

.110 

33-7 

80 

0.877 

8.8 

.086 

90 

0.831 

2.8 

•055 

28.9 

95 

0.812 

1.3 

.020 

25-6 

100 

0-795 

0.6 

t°. 

0-5 
IO 

21.5 
30 

37-5 
45 


Gms. 
per  roo  Gms. 
H20. 

i!6 
2.8 
3-9 
5-6 
8.1 


5o 
54 

II 

57 


Gms.  Na2B4O/7 
per  too  Gms. 

H20. 

10.5 

13-3 
14.2 

II 


60 
62 

65 
70 
80 
oo 

IOO 


Gms.  NajB4O7 

per  100  Gms. 

H20. 

19.4 

20.3 

22 

20.7 

22 

21.9 

24-4 

31-5 

41 

52-5 

Tr.  temp.,  Na2B4O7.ioH2O->Na2B4O7.5H2O,  approximately  62°. 

^16.5°  of  sat.  sol.  =  I.O2O.  (Greenish  and  Smith,  1901.) 

ioo  gms.  H2O  dissolve  3.33  gms.  Na2B4O7  at  25°,  determined  by  refractometer. 

(Osaka,  1903-08.) 


SODIUM  BORATES 


630 


SOLUBILITY  OF  SODIUM  BORAXES  IN  WATER  AT  30°. 

(Dukelski,  1906,  complete  references  given.) 
Cms,  per  100  Gms.  Solution.       Gms.  per  100  Gms.  Residue. 


'     NaA 

B203. 

Na20.               B203.     ' 

42.0 

NaOH.H2O 

41-37 

5.10 

43.54             4.19 

38.85 

5-55 

37-20           II.  1  8         Na2O  .B2O3.4H2O 

34-44 

3-73 

33.52           I0.8o 

29-39 

2.51 

29.63         io.ii                " 

26.13 

2-75 

27.85           15.21 

23.00 

3.82 

24.91            II.  60 

16.61 

13.69 

21.29           20.64 

21.58 

4-63 

24.52           1  9  .  04        Na2O  .B2O3.4H2O  +|Na2O.B2O3.8H2O 

20.58 

4.69 

21.  6  1            16.59         NajsO  .B2O3.8H2O 

I5-32 

6.21 

19.70           17.84 

12.39 

9.12 

18.05           18.17 

8.85 

10.49 

11.72           2O.62         Na20  .2B2O3.ioH2O 

5.81 

6.94 

IO.82           21.31 

1.88 

2.41 

7-31        J5-5o 

1-38 

5-i6 

7.16           17.44 

2.02 

7-79 

6.24           16.38 

4.08 

17.20 

8  .  96            29  .  20         Na2O.2B2O3.ioH2O  +  Na2O.5B2O8.ioH2G 

3-79 

15.84 

5  .  68            28.19         Na20.sB203.ioH20 

2.26 

12.14 

5-21            29.19 

1.99 

11.84 

5  .  74           39  .  66         Na2O.2B2O3.ioH2O  +  B(OH)3 

1.86 

ii.  18 

1.  06            28.78         B(OH)3 

0.64 

6.  ii 

0.31            31.19 

3-54 

...                  " 

EQUILIBRIUM  IN  THE  SYSTEM  SODIUM  OXIDE,  BORIC  OXIDE,  WATER  AT 

60°. 

(Sborgi  and  Mecacci,  1915,  1916.) 

Gms.  per  100  Gms. 

Gms.  per  100  Gms. 

Sat. 

Sol. 

Solid  Phase.                           Sat.  Sol.                          Solid  Phase. 

NajO. 

B203. 

NaaO.            B2O3. 

49-25 

O 

NaOH.H2O                            19.29         22.78    Na20.B2O3.4H2O 

48.44 

0.81 

20.30         25.50 

49.28 

i-53 

"  +2Na2O.B2O3.H2O          22.21          32.17        "  +Na2O.2B2O3.s 

H2C 

47.38 

2.  24 

2Na2O.B2O3.H2O                     19-43          27.09    Na20.2B2O3.sH2O 

44-74 

3.78 

16.13          23.05        « 

42-94* 

5.67 

"  +Na2O.B2O3.H2O            13-51          IQ.IO 

40.14 

5-41 

Na2O.B2O3.H2O                       1  1-  58         16.62        " 

38.70 

5.56 

6.95          11.50        " 

35.76 

6.29 

5.65         14.89        « 

34-93 

6.80 

"                                           6.84         20.40        " 

31-88 

9.85 

"  (unstable)                          8.42         28.05        " 

29-56 

11.83 

"                                         11.29         41.47        "  +Na20.5B203.ioH20 

28.07 

14.65 

8.29         33.57           Na20.SB203.ioH20 

33-12 

7-47 

"  +NajO.B2O3.4H2O            6.29         28.77 

28.64 

6.51 

Na20.B2O3.4H2O                3-22         21.94 

22.06 

10.29 

3-40         22.59                         "  +H3BO, 

18.72 

J7-33 

1.39         13.92                     H3B03 

18.32 

19.17 

o              7.39 

SODIUM   BORAXES  631 

SOLUBILITY  OF  SODIUM  BORAXES  IN  SEVERAL  SOLVENTS. 


Borate. 

Sodium  borate 


Sodium  Biborate 


Solvent.  f. 

Alcohol  (d=  0.941)  15.5 
Glycerol  15.5 

80 
Trichlorethylene      15 


gS*.         Authori*- 

2  .  48  (u.  s.  P.  vm.) 

60.3  <u.  s.  p.  vm.) 

100  (u.  s.  P.  vni.) 

o.  on  (Wester  and  Bruins,  1914.) 


Gms.  NaBrO3  per  100  Gms.  H20 


Fusion-point  data  for  mixtures  of  NaBO2+NaPO3  and  NaBO2+Na2SiO3  are 

C"  ren  by  Van  Klooster  (1910-11).     Results  for  Na2B4O7+Na4P2C)7  are  given  by 
Chatelier  (1894). 

SODIUM  BROMATE   NaBrO3. 

SOLUBILITY  IN  WATER. 

(Kremers,  i8ss-s6a.) 

0°          20°         40°         60°         80°          100° 

27.5    34-5     50-2    62.5     75.7      90.9 

Sp.  Gr.  of  saturated  solution  at  19.5°  =  1.231.  (Gerlach.) 

100  cc.  anhydrous  hydrazine  dissolve  I  gm.  NaBrO3  with  decomposition. 

(Welsh  and  Broderson,  1915.) 

SODIUM   BROMIDE   NaBr.2H2O. 

SOLUBILITY  IN  WATER. 

So!id  Phase.  V.      £%*&&  Solid  Pb**. 

Ice  50  53.7  (4)        NaBr.2H2O 

"  +NaBr.SH2C,  50.7        53-9(5 

NaBr.sH2O+NaBr.2H2O  80  54-2(4 

NaBr.2H2O 


to 

Gms.  NaBr  per 

. 

100  Gms.  Sat.  Sol. 

—  IO.I 

20.8  (i) 

-28 

40.3  (2) 

-23.5 

41.2  (3) 

—  20 

41.8(4) 

—  10 

42.9  (4) 

0 

44.3  (4) 

+16.4° 

47      (8)* 

20 

47  -5  (4) 

30 

49-4(7) 

40 

5i-4(4) 

50 
50. 
80 

100 

no 

140 
180 

210 

230 


+NaBr 
NaBr 


54-8  (4) 
55-1  (4) 
56.5(6) 
59-5(6) 
60.9  (6) 
62  (6) 


1-523). 


(i)  Rudorff  (1862);   (2)  Guthrie  (1875);   (3)  Panfiloff  (1893);   (4)  de  Coppet  (1883);   (5)  Richards 
and  Churchill  (1899);  (6)  Etard  (1894);  (7)  Cocheret  (1911);   (8)  Greenish  (1900). 

SOLUBILITY  OF  SODIUM  BROMIDE  IN  AQUEOUS  SOLUTIONS  OF  SODIUM 
HYDROXIDE  AT  17°. 

(Ditte,  1897.) 


Gms.  per  100  Gms. 


Gms.  per  too  Gms.  H2O. 


Gms.  per  100  Gms.  H2O. 


NaOH. 

NaBr. 

NaOH. 

NaBr. 

NaOH. 

NaBr. 

0-0 

9I.38 

17.17 

63.06 

28.43 

48.00 

3.26 

79.86 

19.12 

62  .51 

36.61 

38.4I 

9.24 

68.85 

22-35 

59.60 

46.96 

29-37 

13-43 

64.90 

24.74 

55-03 

54-52 

24.76 

SOLUBILITY  OF  SODIUM  BROMIDE  IN  AQUEOUS  ETHYL  ALCOHOL  AT  30°. 

(Cocheret,  1911.) 


CjHjOH. 

NaBr. 

ouuu  riiiise. 

O 

49-4 

NaBr.2H2O 

11.79 
31.78 
43-22 

54.59 

42.9 
32.12 
26.79 
20.83 

" 

Gms.  per  too  Gms.  Sat.  Sol. 
'C2H6OH. NaBr. ' 

65.51  16.08 

72.36  13.41 

76.92  I2.O3 

87.35  7-44 

97 . 08  3 . 01 


Solid  Phase. 
NaBr.2H2O 

"  +NaBr 
NaBr 


SODIUM  BROMIDE 


632 


SOLUBILITY  OF  SODIUM  BROMIDE  IN  ALCOHOLIC  SOLUTIONS. 

(Rohland,  1898-05;  de  Bruyn,  1892;  Eder,  1876.) 


Alcohol. 

Concentration 
of  Aq.  Alcohol. 

t°. 

Cms.  NaBr 
per  100  Gms. 
Alcohol. 

Methyl  Alcohol 

^i5=o-799 

room  temp. 

21-7                   (R.) 

Ethyl 

d15=o.8io 

tt 

7.14 

Propyl 

d15=o.8i6 

« 

2.01 

Ethyl 

90%  by  vol. 

? 

4.0   (hydrated  NaBr) 

Methyl       " 

Absolute 

19-5 

17.35        (de  Bruyn.) 

Ethyl 

it 

15 

6.3    (NaBr2H20)  (Eder.) 

Ethyl  Ether 

:c 

15 

0.08 

^  A  sat.  solution  of  NaBr  in  CH3OH  contains  0.9  gin.  NaBr  per  100  gms.  solu- 
tion at  the  critical  temperature.  (Centnerszwer,  1910.) 
loo  cc.  of  ethyl  alcohol  of  d  =  0.8327  dissolve  7.37  gms.  NaBr  at  16.4°,  du  of 

Sat.  sol.   =  0.889.  (Greenish,  1900.) 

ioo  gms.  propyl  alcohol  dissolve  2.05  gms.  NaBr  at  ord.  temp.      (Schlamp,  1894.) 
SOLUBILITY  OF  SODIUM  BROMIDE  IN  MIXTURES  OF  ALCOHOLS  AT  25°. 

(Herz  and  Kuhn,  1908). 


In  CH3OH  +  C2H6OH. 

Per  cent                            Gms. 
CH3OH         A*  of        NaBr  per 
in            Sat.  Sol.       ioo  cc. 

In  CH3OH  +  C8HrOH. 

Per  cent                           Gms. 
CjH7OH         <*25  of       NaBr  per 
in           Sat.  Sol.       too  cc. 

In  C2H6OH  +  C3H7OH. 

Per  cent                               Gms. 
CSH7OH           ^25  of         NaBr  pei 
e  in             Sat.  Sol.         ioo  cc. 

Mixture. 

Sat.  Sol. 

Mixture. 

Sat.  Sol. 

Mixture. 

Sat.  Sol. 

O 

0. 

8189 

2-93 

0 

0.9238 

14.40 

0 

0.8189 

2-93 

4-37 

0. 

8265 

3.65 

II. 

n 

0.9048 

12-43 

8. 

i 

0.8147 

2.49 

10.4 

0. 

8273 

4.04 

23- 

8 

0.8887 

10.53 

17- 

85 

O.8l45 

2.47 

41.02 

0. 

8593 

7,24 

65- 

2 

0.8390 

4.42 

56. 

6 

0.8107 

1.90 

80.69 

0. 

9079 

12.51 

91. 

8 

0.8153 

1.47 

88. 

6 

0.8116 

I.  II 

84.77 

0. 

9104 

12.86 

93- 

75 

0.8144 

1.26 

91. 

2 

0.8083 

0.83 

91.25 

0. 

9235 

14.32 

IOO 

0.8093 

0.74 

95- 

2 

o  .  8090 

0.82 

roo 

0. 

9238 

14.40 

IOO 

0.8093 

0.74 

SOLUBILITY  OF  SODIUM  BROMIDE  IN  ACETAMIDE  AT  VARIOUS  TEMPERATURES. 

(Menschutkin,  1908.) 


Gms.  per  ioo  Gms. 
Sat.  Sol. 


N  - 


Solid  Phase. 


82* 

8o 
78 
76 

74 
72 

80 


CONHj 

6 

II-  5 

16.3 

2O.  2 

23 

25 

27 


...      CHjCONH, 

2.8        « 

5-36      " 

7.6        « 

9.4         " 
10.7         « 

1  1.  6         "+NaBr.2CH3CONH2 
12.6      NaBr.aCHjCONHj 

*  M.  pt.  f  Tr.  pt. 


•\ 

*"•  s 

3ms.  per  ioo  Gms. 
Sat.  Sol. 

Solid  Phase. 

aBr.2CHr 
CONH2     = 

NaBr. 

90 

29.4 

13-7 

NaBr.2CH3CONH, 

IOO 

32.2 

IS 

" 

no 

35-3 

16.4 

« 

120 

38-7 

18 

" 

130 

42.6 

19.8 

« 

i3St 

45-3 

21.  I 

"  +NaBr 

155 

46.4 

21.6 

NaBr 

175 

47-5 

22.  I 

" 

t  Eutec 

ioo  gms.  95%  formic  acid  dissolve  22.3  gms.  NaBr  at  18.5°. 


(Aschan,  1913.) 


ioo  cc.  anhydrous  hydrazine  dissolve  37  gms.  NaBr  at  room  temp. 

(Welsh  and  Broderson,  1915.) 

FUSION-POINT  DATA  (Solubilities,  see  footnote,  p.  i)  ARE  GIVEN  FOR  THE 
FOLLOWING  MIXTURES. 


NaBr  +  NaCl 
NaBr  +  Nal 
NaBr  +  NaF. 
NaBr  +  NaOH 
NaBr  +  NaNO2. 
NaBr  +  Na2SO, 


(Amadori, 

(Amadori, 

(Ruff  and  Plato,  1903.) 

(Scarpa,  1915-) 

(Meneghini,  1912.) 

(Ruff  and  Plato,  1903.) 


;  Ruff  and  Plato,  1903.) 


633 
SODIUM  CACODTLATE  (CH3)2AsO.ONa. 


SODIUM  CACODYLATE 


100  gms.  H2O  dissolve  about  200  gms.  of  the  salt  at  I5°-2O°.     (Squire  and  Caines,  1905.) 
loo  cc.  90%  alcohol  dissolve  about  100  gms.  of  the  salt  at  I5°-2O°.      " 


SODIUM   CAMPHORATIS 

SOLUBILITY  IN  AQUEOUS  d  CAMPHORIC  ACID  SOLUTIONS  AT  i3.5°-i6°. 

(Jungfleisch  and  Landrieu,  1914.) 


Gms.  per  100  Gms. 

Sat.  Sol.  Solid  Phase. 

C10H1(A.  C10HM04Na2. 
O.62I         O        Ci0H16O4 
2.03  4.19      " 

2.87  8.32 

3.03         10.05      " 
2.97  7.80 

2.87  9.06 

2.94  10.46 
2.68  14.99 
2-64  17.53 


Gms.  per  100  Gms. 
Sat.  Sol. 


Solid  Phase. 


2-74 
2.63 

1    +C10H16O4Na.2Ci0H16O4.2H2O  2.29 
C10H1604Na.2C10H1604-2H20        2.17 
1. 06 
0.88 
O 


CioH1804.  CwH1404Na2. 

2 . 87         25 . 62  C10H1604Na.2C10H1804.2H^) 
2.89         27.41 
30.69 

32.75 

40. 10  CMH16O4Na.H2O  (or  iH20) 

40-54 

47.04 

49 . 60         C10H14O4Na2.3H20 

50.2 


CioHi6O4  =  Camphoric  acid.  CioHi6O4Na.2CioHi6O4.2H2O  =  Monosodium  d  tri- 
camphorate.  Ci0Hi5O4Na.H2O  =  Monosodium  d  camphorate.  CioHuC^Na-^HjO 
=  Disodium  d  camphorate  (neutral). 

(The  mixtures  were  kept  in  a  cellar  at  a  nearly  constant  temperature  and 
shaken  from  time  to  time.  Additional  determinations  at  i7°-23°  are  also  given.) 


SODIUM  CARBONATE  Na2CO3.ioH2o. 


SOLUBILITY  IN  WATER. 

(Wells  and  McAdam,  Jr.,  1907;  Mulder,  below  27°  and  above  44°.) 


r. 

Gms. 
NajCOa  per 
loo  Gms.  H2O. 

O 

7 

5 

9.5 

10 
15 

12-5 
16.4 

20 
27.84 

21-5 

34-20 

29-33 

37-40 

30.35 

40.12 

3L45 
32.06 

43-25 

32.15 

33-10 

30.35 
32.86 

43.50     - 
46.28 

Solid  Phase. 


Gms. 


+Na2C03.7H20 
+Na2C03.H20 


t°. 

Na.COa  p 

100  Gms.  I 

34-76 

48.98 

35-62 

50.08 

35.50 

.  .  . 

29.86 

50.53 

31.80 

50.31 

35.17 

49-63 

36.45 

49-36 

37-91 

49.11 

41.94 

48.51 

43-94 

47.98 

60 

46.4 

80 

45.8 

TOO 

45-5 

105 

45-2 

Solid  Phase. 


NajCO,.7H2O 


NajCOj-HjO 


The  determinations  of  Wells  and  McAdam,  Jr.,  were  made  with  extreme  care. 
They  correct  the  discrepancies  which  have  so  far  existed  between  the  solubility 
and  transition  points  of  the  hydrates.  Earlier  data,  which  differ  more  or 
less  from  the  above,  are  given  by  Lowel,  1851;  Reich,  1891;  Eppel,  1899  and 
Ketner,  1901-02.  Single  determinations  at  15°,  25°,  and  30°  are  given  by 
Greenish  and  Smith  (1901);  Osaka  (1910-1911);  de  Paepe  (1911)  and  Cocheret 
(1911). 

Sp.  Gr.  of  solution  saturated  at  17.5°,  1.165  (Hager);  at  18°,  1.172  (Kphl- 
rausch);  at  23°,  1.22  (Schiff);  at  30°,  1.342  (Lunge).  See  also  Wegscheider 
and  Walter,  1905,  for  Sp.  Gr.  determinations  at  other  temperatures. 


SODIUM  CARBONATE 


634 


EQUILIBRIUM  IN  THE  SYSTEM  SODIUM  CARBONATE,  SODIUM  BICARBONATE, 
AND  WATER  AT  25°. 

(McCoy  and  Test,  1911.) 

'(Forty  grams  of  NaHCO3  and  about  200  cc.  of  H2O  were  rotated  at  25°  until 
equilibrium  was  reached.  Small  portions  of  the  clear  solution  were  then  ana- 
lyzed by  the  Winkler  method  for  carbonate  content,  and  by  titration  in  presence 
of  methyl  orange,  for  sodium.  About  15  gms.  of  Na2CO3.ioH2O  were  then  added, 
and  the  mixture  again  rotated  until  equilibrium  was  reached,  and  again  analyzed. 
This  was  continued  and  the  following  results  were  obtained.) 


Solid  Phase. 

Na2C03.ioH2O 

"  +Na2CO3.NaHC03.2H2O 
Na2CO3.NaHC03.2H2O 

*  "  +NaHCO3 

NaHCO, 


Per  cent  of 
Total  Na 
Present  as 
Bicarbonate. 

Gms.  Na 
per  Liter. 

Gms. 
Bicarbonate 
per  Liter. 

Gms.  Carbonate 
per  Liter. 

O 

II9.9 

O 

276.4 

5-92 

127.6 

27.6 

276.3 

7-5 

120 

10 

107 

12.89 

108 

50.8 

216.6 

15 

100 

20 

80 

.  .  . 

... 

32 

60 

.  .  . 

.  .  . 

56 

40 

.  .  . 

.  .  . 

80 

30 

100 

27.02 

98.7 

O 

The  following  data  for  this  system  also  at  25°,  but  given  in  terms  of  weight 
instead  of  volume  of  solution,  are  reported  by  de  Paepe  (1911). 


Gms.  per  100  Gms.  H2O. 
NaHCOs'. 
O 

2.1 
4.2 

5-7 


28.3 

27-3 
26.5 
19.2 


Solid  Phase. 
NaaCCvioHjO 

"  +NaHC03 
NaHCO8 


Gms.  per  100  Gms.  H2O. 
NaaCOs.  NaHCO3. 

12.4  7-3 

6.2  9 

I  10. 1 


Solid  Phase. 
NaHCO, 


SOLUBILITY  OF  SODIUM  CARBONATE  IN  AQUEOUS  SOLUTIONS  OF  SODIUM 
BROMIDE  AND  OF  SODIUM  IODIDE  AT  30°. 

(Cocheret,  1911.) 


In  Aq.  NaBr  Solutions. 


Na2C03. 

NaBr.    " 

27.98 

O 

NajCO3.ioH2O 

27-54 

2.41 

« 

26.72 

4.06 

«« 

26.23 

6.26 

"  +Na2C03.7H20 

23.40 

II 

Na2C03.7H2O 

22.68 

12.22 

" 

19.86 

16.88 

" 

19-57 

16.95 

"  +Na2C03.H20 

i8.ii 

19.32 

NazCOj.HzO 

8-45 

33-39 

" 

6.90 

36-13 

" 

3-04 

44-75 

" 

2.99 

45-31 

"  +NaBr.2H2O 

2.60 

45-68 

NaBr.aH2O 

0 

49.40 

" 

In  Aq.  Nal  Solutions. 


Na2CO3. 

Nal. 

26.5 

2.4 

Na2C03.ioH2O 

25-5 

4-7 

" 

24.4 

8.6 

" 

24-3 

9-5 

"  +Na2C03.7H20 

23 

II  .2 

Na2C03.7H2O 

20.8 

14 

" 

18.7 

18.4 

" 

15-3 

25-4 

"  +Na2CO3.H2O 

13-1 

29.1 

Na2CO3.H2O 

10.4 

33-3 

" 

4.2 

46 

" 

2-7 

.51 

" 

0.9 

57-6 

" 

o-3 

65.6 

"  +NaI.2H20 

0 

65-5 

NaI.2H2O 

635 


SODIUM  CARBONATE 


SOLUBILITY  OF  SODIUM  CARBONATE  IN  AQUEOUS  SOLUTIONS  OF  SODIUM 

CHLORIDE  AT  15°. 

(Reich,  1891.) 


Gms.  per  100  Gms. 
H2O. 

Gms.  NaCl 
per 

Gms.  NajCOj 
per  100  Gms. 

Gms.  per  too  Gms. 
H20. 

NaCl. 

Na2CO3.io- 
H20. 

looGms. 
Solution. 

NaCl 
Solution. 

NaCl.       I 

^COfio- 

0 

61.42 

o 

16.42 

23.70 

39-06 

4.03 

53-86 

2.92 

14-47 

27-93 

39-73 

8.02 

48 

5-8o 

12.87 

31.65 

41.44 

12.  O2 

43.78 

8.61 

11.62 

35-46 

43-77 

16.05 

40.96 

11-31 

10.70 

37-23 

45-27* 

19.82 

39.46 

I3-7I 

10.  II 

*  Both  salts  in  solid  phase. 

Gms.  NaCl  Gms.  Na-jCOa 

per 

100  Gms. 
Solution. 


per  100  Gms. 

NaCl 
Solution. 


15.96 
18.26 
20.06 

21-75 
22.46 


9.76 
9.62 
9-73 
7-95 
10.13 


SOLUBILITY  OF  SODIUM  CARBONATE  IN  AQUEOUS  SODIUM  CHLORIDE  AT  30° 

(Cocheret,  19  n.) 


Gms.  per  100  Gms.  Sat.  Sol. 


Na2C03. 
27.98 
27.48 
27.12 
26.82 

25-59 
24.  26 

22.75 


NaCl. 

o 

0.90 

3-33 

4-iS 

5-17 

5-93 

10.24 


Solid  Phase. 


Gms.  per  100  Gms.  Sat.  Sol. 


+Na2C03.7H20 


+Na2CO,.H20 


Na2C03. 

NaCl. 

>     ouiiu  runsc. 

20.72 

11.49 

NajCOs.HjO 

18 

14.  12 

"  +NaCJ 

14.81 

16.26 

NaCl 

9.71 

18.76 

" 

5.65 

21-94 

« 

o 

26.47 

<« 

SOLUBILITY  OF  SODIUM  CARBONATE  IN  AQUEOUS  SOLUTIONS  OF  SODIUM  NITRATE. 

(Kremarm  and  Zitek,  1909.) 

,     Gms.  per  TOO  Gms.  H2O.  ^ 


t°.  c 

10 
10 
IO 

24.2 
24.2 

Ims.  per  100  Gms.  H2O.         ^  __ 

u.  98* 

8-75 
o 

28.55 
26.33 

NaNO3. 
O 

70.48 
80.5 

0 

45.96 

"  +NaNO3 
NaNO3 
Na-sCOj.ioHzO 

24.2 
24.2 
24.2 
24.2 

24.63 
21.8 

5.96 

0 

NaNO3. 

54-43 
62.7 

84.45 
91-3 

Na2C03.7H20 
"  +NaNO, 
NaNO, 

SOLUBILITY  OF  SODIUM  CARBONATE  IN  AQUEOUS  ETHYL  ALCOHOL  AT  30°. 

(Cocheret,  1911.) 


Solid  Phase. 


Gms.  per  100  Gms.  Sat.  Sol. 
'  NajCOs.  QHfiOH.  " 

26.61  2.64        NajCOj.ioHjO 

26.14  3-41* 


Gms.  per  100  Gms.  Sat.  Sol. 


Solid  Phase. 


1.38 
0.62 

0-53 
0.51 


44-81* 
52.99 
55-70 
56.56 


+Na2C03.7H20 


NajCO,. 

C;,H6OH. 

—  »             OU11U  JTllttSC. 

0.40 

63.20 

Na2CO3.7H2O 

O.  II 

73.06 

"  +Na2COs.H,0 

O.O7 

78.19 

NajCOj.HjO 

0.06 

90.95 

" 

0.03 

95.06 

"  +Na2C03 

98.46 

NajCO, 

*  Between  these  two  concentrations,  the  mixtures  separate  into  two  liquid  layers. 

Results  are  also  given  for  the  solubility  of  Na2CO3  +  NaBr  and  of  Na2CO3 
+  NaCl  in  Aq.  C2H6OH  at  30°. 

SOLUBILITY  OF  SODIUM  CARBONATE  IN  AQUEOUS  SOLUTIONS  OF  ETHYL  AND  OF 
PROPYL  ALCOHOL  AT  20°. 

(Linebarger,  1892.) 

Wt.  Per  cent  Gms.  Na^COa  per  100  Gms.  Sol. 

Alcohol.  '   In  Ethyl  In  Propyl.  ' 

28  ...  4-4 

38  ...  2.7 

44  1-7  1-7 

46  1.13  i-S 


Wt.  Per  cent 
Alcohol. 

48 
50 
54 
62 

Gms.  NajCOj  per  100  Gms.  Sol. 

In  Ethyl. 
0.9 
0.84 
0.80 

In  Propyl. 
i-3 

1.2 
0.9 
0.4 

SODIUM   CARBONATE  636 

SOLUBILITY  OF  SODIUM  CARBONATE  IN  AQUEOUS  SOLUTIONS  OF  ETHYL  ALCOHOL. 

(Ketner,  1901-02.) 

NOTE.  —  The  mixtures  were  so  made  that  alcoholic  and  aqueous  layers  were 
formed,  and  these  were  brought  into  equilibrium  with  the  solid  phase. 

Gms.  per  100  Gms.  Alcoholic  Layer.         Gms.  per  100  Gms.  Aq.  Layer. 

t°.        , * s         / * >         Solid  Phase. 

C2H5OH.        Na2CO,.         H2O.  C2HbOH.      Na2CO3.          H2O. 

35  62.9  0.3  36.8  i  32.4  66.6       Na2co3.H2o 

40  61  0.4  38.6  1.2  31.9  66.9              " 

49  61  0.4  38.6  1.2  31.5  67.3 

68  55.8  0.9  43.3  2.3  28.8  68.9 

31.2  52.4  0.8          46.8  ...  29.3  ...      Na2CO3.7H2O(0) 
31.9          54.8             0.7          44.5                  1.7           29.8          68.5 

32.3  56.1          0.6        43.3  1.5        30.2        68.3 

33.2          58.1  0.5          42.4  1.4    '       31  67.6 

27. 7  Crit.  sol.  ±  14%  C2H2OH  ±  13%  Na2CO.,  ±  73%  H2O 

28.2          23.5  7.3  69.2  7.9  18.6  73.5       NajCOj.ioHjO 

29        32.7       3.8      63.5          4.3      22.7      73.0 

29.7          40  2.1  57.9  2.9  25.5  71.6 

30.6          47.8  1.2  51  2.3  27.8          69.9  " 

SOLUBILITY  OF  Na2CO3.ioH2O  IN  DILUTE  ALCOHOL  AT  21°. 

(Ketner.) 
Gms.  per  100  Gms.  Solution.  Gms.  per  100  Gms.  Solution. 


Na,COj.  QHSOH.  H2O.  N^COj.  QH5OH.  H2O. 

18.5  O  81.5  1.2  39.2  59.6 

12.7  6.2  81.1  0.2  58.2  41.6 

6.9  15.3  77.8  o.i  67.1  32.8 

3.2  26.1  70.7  0.06  73.3  26.64 

Isotherms  showing  the  compositions  of  the  conjugated  liquids  at  28.2°,  29.7° 
and  40°  are  also  given. 

EQUILIBRIUM  IN  THE  SYSTEM  SODIUM  CARBONATE,  NORMAL  PROPYL  ALCOHOL 

AND  WATER  AT  20°. 

(Frankforter  and  Temple,  1915.) 

(Note.  In  this  paper  the  results  for  the  binodal  curve  are  reported  in  terms  of 
gms.  per  100  gms.  solvent  (water  -f-  alcohol),  instead  of  gms.  per  100  gms.  of  the 
homogeneous  liquid  (sodium  carbonate  +  water  +  alcohol.) 

Gms.  per  100  Gms.  Alcohol  +  Water.  Gms.  per  100  Gms.  Alcohol  +  Water. 


Na^CO,.  Alcohol.  Water.  Na^COj.  Alcohol.  Water. 

16.568      3.409    96.591       J-99o     31-537    68.463 

15.363        4.472      95-528         1.338       40.796      59-204 
11.696        6.595      93-405         0.930       46.933      53-067 

8.415  9-176  90.824  0.567  53-875  46.125 

6.669  n. 221  88.779  0.298  59-507  40.493 

4.138  15.785  84.215  0.160  63.568  36.432 

2.878  21.099  78.901  0.109  75-159  24.841 

For  results  on  the  system  sodium  carbonate,  allyl  alcohol,  water  at  20°  see 
last  table,  p.  647. 

100  gms.  glycerol  (du  =  1.256)  dissolve  98.3  gms.  Na2CO3  at  i5°-i6°. 

(Ossendowski,  1907.) 

loo  gms.  saturated  solution  in  glycol  contain  3.28-3.4  gms.  sodium  carbonate. 

(de  Coninck,  1905.) 

100  gms.  H2O  dissolve  229.2  gms.  sugar  +  24.4  gms.  Na2CO3,  or  100  gms.  sat. 
aq.  solution  contain  64.73  gms.  sugar  -f-  6. 89  gms.  Na2CO3  at  31.25°.    (Kohler,  1897.) 


637 


SODIUM  CARBONATE 


EQUILIBRIUM  IN  THE  SYSTEM  SODIUM  CARBONATE,  PYRIDINE,  WATER. 

(Limbosch,  1909.) 

Very  pure  materials  were  used.  The  boiling-point  (cor.)  of  the  pyridine  was 
115°-!  15.07°.  Increasing  amounts  of  this  pyridine  were  added  to  aqueous 
solutions  of  sodium  carbonate  contained  in  glass  tubes.  After  the  tubes  were 
sealed  they  were  placed  in  a  bath  and  the  temperature  noted  at  which  the  liquid 
mixture  passed  from  a  homogeneous  to  an  opalescent  condition.  During  the 
observation,  the  contents  of  the  tubes  were  stirred  by  means  of  pieces  of  iron, 
moved  with  the  aid  of  a  magnet  on  the  outside  of  the  tube. 


Per  cent 
of 

Per  cent 
of 

t°  of  Sat. 

Per  cent 
of 

Per  cent 
of 

Per  cent 
t°  of  Sat.         of 

Per  cent 
of 

t°  oi  bat. 

Pyridine. 

NajCOs. 

Pyridine. 

Na,CO3. 

Pyridine. 

O.I29 

66.2 

12 

2. 

5o 

50 

199 

6.12 

23- 

5 

1  2O 

0.129 

66.4 

25 

2. 

5o 

53-3 

197 

6.12 

25. 

5 

132 

O.I29 

67.7 

36 

2. 

5o 

59-4 

173 

6.12 

28. 

4 

152 

0.129 

69.2 

44 

2. 

50 

69.2 

123 

6.99 

13- 

8 

54.2(40.5) 

0.129 

73-5 

53 

2. 

5o 

73-8 

1  10 

6.99 

15- 

4 

81 

d7) 

o.  129 

74.8 

2. 

5o 

74-8 

* 

6.99 

19. 

5 

117 

0.129 

76.1 

25.  s(—  64) 

3- 

49 

30-3 

-0-5 

6.99 

22. 

7 

142 

o.  129 

77-8 

ii     (-59) 

3- 

49 

32.6 

39 

6.99 

25- 

i 

158 

I.OI 

47.6 

17 

3- 

49 

34-3 

86.5 

6.99 

27. 

6 

169 

I  .OI 

49-9 

36 

3- 

49 

36.7 

107 

6.99 

32. 

6 

180+ 

I.OI 

51-2 

55 

3- 

49 

37-4 

123 

9.36 

8. 

50 

64 

(26) 

I.OI 

52.2 

72 

3- 

49 

42.5 

194 

9.36 

9 

78 

(18) 

I.OI 

56-1 

107 

3- 

49 

69.6 

167 

9.36 

ii. 

4 

106.5 

I.OI 

60.6 

in 

3- 

49 

71.2 

* 

9.36 

13- 

8 

127 

I.OI 

66.8 

no 

5- 

23 

23-3 

63(27 

.5)  9.36 

16. 

3 

148 

I.OI 

75-i 

86.5 

S- 

23 

23-7 

70(20 

.5)  9.36 

20. 

i 

169 

I.OI 

76.9 

71 

5- 

23 

24.6 

79 

9.36 

25 

180+ 

I.OI 

78.1 

* 

5- 

23 

26.2 

96 

9-36 

50 

180+ 

2.50 

36.3 

22 

5- 

23 

28.7 

in 

18.1 

2. 

12 

48 

(18) 

2.50 

37-9 

53-25 

§• 

23 

32.5 

155 

18.1 

2. 

25 

66 

2.50 

39-2 

74-5 

5- 

23 

36.6 

196 

18.1 

2, 

70 

79 

2.50 

40 

94 

5- 

23 

37-2 

200+ 

I*,  i 

4 

20 

108 

2.50 

43-6 

147 

5- 

23 

55-4 

* 

18.1 

5 

,40 

126 

2.50 

47.6 

185 

18.1 

6 

80 

155 

*  Precipitate  of  NajCOs.     Results  in  parentheses  show  lower  temperatures  of  saturation. 

Fusion-point  data  for  Na2CO3  +  NaCl  are  given  by  Le  Chatelie  0*1894)  and 
Sackur  (1911-12).  Results  for  Na2CO3  +  NazSO*  are  given  by  Le  Chatelier 
(1894),  Sackur  (1911-12)  and  by  Amadori  (1912).  Results  for  Na2CO3  +  KC1 
are  given  by  Sackur  (1911-12). 


SODIUM  (Bi)  CARBONATE  NaHCO3. 

SOLUBILITY  IN  WATER. 

(Dibbits,  1874;   Fedotieff,  1904.) 


o 
10 

20 
25 


Cms.  NaHCOs  per  100  Cms. 


Water. 

6.9 

8.15 

9.6 

10.35 


Solution. 

6.5 

7.5 
8.8 
9-4 


30 
40 
50 
60 


Cms.  NaHCO  per  100  Cms. 
Water.  Solution. 

ii.  i  10 

12.7  11.3 

14.45  I2-6 

16.4  13.8 


100  gms.  H2O  dissolve  9.03  gm.  NaHCO3  at  15°,  di6  =  1.061. 

(Greenish  and  Smith,  1901.) 

100  gms.  alcohol  of  0.941  Sp.  Gr.  dissolve  1.2  gms.  NaHCO3  at  15.5° 

100  gms.  glycerol  dissolve  8  gms.  NaHCO3  at  15.5°.  (Ossendowski,  1907.) 


SODIUM  (Bi)  CARBONATE 


638 


SOLUBILITY  OF  SODIUM  BICARBONATE  IN  AQUEOUS  AMMONIUM  BICARBONATE 
SOLUTIONS  SATURATED  WITH  CO2. 

(Fedotieff,  1904.) 


.0         Wt.  of  i  cc.    ! 
*  -          Solution. 

Ylols.per  IDC 

>o  Gms.H20 

NHtHCOs. 

NaHCO3". 

o        1.072 

i-39 

0.58 

tt 

o.o 

0.82 

g 

.056 

O-O 

1.05 

it 

.061 

0.29 

o-95 

tt 

.065 

0.56 

0.89 

It 

•073 

1.  08 

0.79 

It 

.090 

2.16 

0.71 

30 

o.o 

1.65 

tt 

2.91 

0.83 

Grams  per  1000  Gms.  H2O- 
'NH4HCO3.    NaHCO3. ' 
109.4 
O.O 
0-0 

23.0 
44.0 

85-7 


170.6 

o.o 

230 


48.2 

69.0 
88.0 
80.0 
74.6 
66.7 

59-2 

138.6 

70.0 


SOLUBILITY  OF  SODIUM  BICARBONATE  IN  AQUEOUS  SOLUTIONS  OF  SODIUM 
CHLORIDE  SATURATED  WITH  CO2. 

(Fedotieff;  see  also  Reich,  1891.) 


0 

Wt.  of  i  cc. 

Mols.  per  icx 

DO  Gms.H2O. 

Grams  per  i< 

XXD  Gms.  H2< 

Solution. 

NaCl. 

NaHCO3. 

NaCl. 

NaHCO3. 

o 

0-0 

0.82 

0-0 

69.0 

u 

1.  208 

6.0 

O.O9 

35°  -1 

7-7 

15 

I  .056 

o.o 

1.05 

O-O 

88.0 

1.063 

0.52 

0.82 

30.2 

68.6 

t( 

1.073 

1.03 

0.64 

60.  1 

53-6 

It 

1.096 

2.  II 

0.41 

123  .1 

34-8 

It 

I.I27 

3-20 

0.28 

187.2 

23.0 

u 

1.158 

4-39 

O.I9 

256.9 

16.1 

tt 

1.203 

6.06 

O.I2 

354-6 

IO.Q 

30 

1.066 

o.o 

I  .31 

o.o 

no.  2 

tt 

1.079 

1.02 

0.87 

59-9 

72.8 

tt 

i  .100 

2.08 

0.56 

121.9 

47-3 

tt 

i  .127 

3.18 

0.38 

186.3 

32-0 

tl 

1.156 

4-38 

0.27 

256.0 

22.3 

tt 

1.199 

6.12 

0.17 

358-1 

13-9 

45 

1.077 

o.o 

I.6S 

o.o 

138.6 

tt 

i.  086 

1.04 

1.  12 

60.7 

94.0 

" 

1.115 

2.65 

O.62 

155-2 

52.0 

" 

i  -127 

3-24 

0.52 

189.4 

43-4 

u 

i  .155 

4-38 

o-37 

256.1 

30-7 

tt 

1.198 

6.18 

0.23 

361-5 

19-5 

100  gms.  alcohol  of  0.941  Sp.  Gr.  dissolve  5.55  gms.  sodium  sulfocarbonate  at 
15-5°. 

SOLUBILITY  OF  SODIUM  BICARBONATE  IN  AQUEOUS  SODIUM  NITRATE 

SOLUTIONS. 

(Fedotieff  and  Koltunoff,  1914.) 


o 

15 
15 
15 


Sp.  Gr.  of 
Sat.  Sol. 

I-356 
1.183 
1.285 

1-377 


Gms.  per  100  Gms.  H2O. 

'NaNO3.  NaHCO3.' 
72.74  1.41 

29.06  3.40 
54.56  2.l6 

83.20  1.57 

95.14  I. 80 


639  SODIUM  CHLORATE 

SODIUM   CHLORATE  NaC103. 

SOLUBILITY  IN  WATER. 

(Carlson,  1910;  Le  Blanc  and  Schmandt,  1911;  Osaka,  1903-08.) 


,„                   dof 

*  •               Sat.  Sol. 

Gms.  NaClOs  per              to 
zoo  Gms.  EkO. 

dof 
Sat.  Sol. 

Gms.  NaClO3  per 
loo  Gms.  H2O. 

-15 

I 

.380 

72- 

40 

I 

.472 

126 

(i  15  LeB.&S.) 

0 

I 

.389 

79 

(80    LeB.&S.) 

50 

140 

(126 

10 

89 

(87 

60 

I 

.514 

155 

15 

I 

.419 

95 

(91            " 

70 

172 

20 

I 

.430 

IOI 

(95-7         " 

80 

I 

•559 

I89 

25 

I 

•44 

1  06 

(101  O.) 

IOO 

I 

.604 

230 

30 

JI3 

(105  Le  B.  &  S.) 

122  (b.  pt.) 

I 

.654 

286 

The  earlier  data  of  Kremers  (1856)  lie  between  the  values  of  Carlson  and  of 
Le  Blanc  and  Schmandt. 


SOLUBILITY  OF  SODIUM  CHLORATE  IN  AQUEOUS  SODIUM  CHLORIDE  SOLUTIONS 

AT  20°. 

(Winteler,  1900.) 


Sp.  Gr.  of 

Gms.  per  Liter. 

Sp.  Gr.  of 

Gms.  per  Liter. 

Solutions. 

Nad. 

NaClO3. 

Solutions. 

NaCl. 

NaClO,. 

1.426 

5 

668 

I 

.365 

175 

393 

I.4I9 

25 

638 

I 

•345 

2OO 

338 

I.4I2 

5o 

599 

j 

319 

225 

271 

1.405 

75 

559 

I 

,289 

250 

197 

1.398 

IOO 

522 

I, 

,256 

275 

1  20 

1.389 

125 

484 

j 

•235 

290 

78 

1-379 

150 

442 

I 

.217 

300 

55 

100  gms.  H2O  dissolve  24.4  gms.  NaCl  +  50.75  gms.  NaClO3  at  12°. 
loogms.  H2O  dissolve  1 1 .5  gms.  NaCl  +  249.6  gms.  NaClO3at  122°.  (Schlosing,  1871.) 

SOLUBILITY  OF  SODIUM  CHLORATE  IN  AQUEOUS  ETHYL  ALCOHOL. 

(Carlson,  1910.) 
Gms.  NaClO3  per  Liter  of  Sat.  Sol.  in  Aqueous  Alcohol  of: 


If  . 

50  Per  cent. 

75  Per  cent 

90  Per  cent. 

20 

3I3-3 

II0.8 

16.1 

40 
60 

70 

321.8 
326.8 

133-5 
155-8 
161.3 

22.9 
29 

gms.  alcohol  of  77  Wt.  per  cent  dissolve  2.9  gms.  NaClO3  at  16°.  (Wittstein.) 
gms.  alcohol  dissolve  i  gm.  NaClO3  at  25°,  and  2.5  gms.  at  b.  pt. 


IOO 
IOO 

100  gms.  glycerol  dissolve  20  gms.  NaClOs  at  15.5°.  (Ossendowski,  1907.) 

100  cc,  anhydrous  hydrazine  dissolve  66  gms.  NaClOs  at  room  temperature. 

(Welsh  and  Broderson,  1915.) 


SODIUM   PerCHLORATE  NaClO4.H2O. 


SOLUBILITY  IN  WATER. 

(Carlson,  1910) 


is 

50 

143 


dot 
Sat.  Solution 

Gms.  NaClO4 
per  TOO  cc. 
Sat.  Solution. 

Solid  Phase. 

1.666 

107.6 

NaClCvHjO 

I-73I 
1.789 

123.4 
141.4 

NaCIO. 

SODIUM  CHLORIDE  640 

SODIUM   CHLORIDE  NaCl. 

SOLUBILITY  IN  WATER. 

(Mulder;    de  Coppet,  r883,'Andrae,  1884;    Raupenstrauch,  1885;    above  100°,  Tilden  and  Shenstone, 
1884;    Berkeley,  1904;   Etard,  1894,  gives  irregular  results.) 


to        Cms.  NaCl  per              Gms^NaCl 

AO           Gms.  NaCl  per 

Gms.  NaCl 

looGms-HaO.                jooTsoL 

100  Gms.  H2O. 

per 
ioo  g.  Sol. 

o    35-7*    35-63t        26.28! 

70    37.8*    37-5if 

27-27t 

10     35-8       35.69           26.29 

80      38.4         38.00 

27-54 

20      36.0         35.82              26.37 

90    39-o      38-52t 

27.80 

25     36-12     35-92          26-43 

ioo    39.8      39-I2J 

28.12 

30    36-3      36-°3          26.49 

118                 39.8 

28.46 

40    36.6      36.32          26.65 

140                42  .  1 

29.63 

50    37.0      36.67          26.83 

160                  43-6 

30-37 

60    37.3      37-06          27.04 

180                  44-9 

30.98 

*  M.;  de  C.                           t 

A.                           *  B. 

The  original,  very  carefully  determined 

figures  of  Berkeley,  are  as 

follows. 

f0                      d  of            Gms.  NaCl  per 
Sat.  Sol.        loo  Gms.  H2O. 

+o                                doi 
Sat.  Sol. 

Gms.  NaCl  per 
ioo  Gms.  H2O. 

0.35             1.2090            35.75 

6l.70                    1.1823 

37-28 

t5.20              1.2020            35.84 

75.65                     1.1764 

37-82 

30.05              1.1956            36.20 

90.50                    I.I7OI 

38.53 

45.40              1.1891             36.60 

107  b.  pt.         1.1631 

39.65 

ioo  gms.  H2O  dissolve  35.99  gms.  NaCl  at  30°.  (Cocheret,  1911.) 

SOLUBILITY  OF  SODIUM  CHLORIDE  IN  WATER,  DETERMINED  BY  THE  FREEZING- 
POINT  METHOD. 

(Matignon, 


Gms.  NaCl 
t°.             per  ioo  Gms.       Solid  Phase. 

t°. 

Gms.  NaCl 
per  ioo  Gms.         Solid  Phase. 

H2O. 

H20. 

0.4 

0.69 

Ice  (Raoult) 

-12.7 

20 

Ice 

0.8 

1-37 

"   (Biltz) 

-16.66 

25 

" 

2.86 

4.9 

"   (Kahlenberg) 

-21.3 

30.7 

"  +NaCl.2H2O 

3-42 

5.85 

"    (Raoult) 

-14 

32.5 

NaCl.2H2O  (de  Coppet) 

6.6 

II 

" 

—  12.25 

32.9 

"  (Matignon) 

9.25 

15 

" 

—  6.25 

34-22 

"  (de  Coppet) 

Data  for  the  influence  of  pressure  on  the  solubility  of  sodium  chloride  in  water 
are  given  by  v.  Stackelberg  (1896);  Cohen,  Inouye,  and  Euwen  (1910)  and  by 
Sill  (1916). 

SOLUBILITY  OF  SODIUM  CHLORIDE  IN  AQUEOUS  SOLUTIONS  SIMULTANEOUSLY 
SATURATED  WITH  OTHER  SALTS. 

The  various  papers  of  J.  H.  van't  Hoff  and  collaborators,  on  this  subject,  have 
been  collected  by  H.  Precht  and  E.  Cohn  in  a  volume  entitled  "  Untersuchungen 
iiber  die  Bildungsverhaltnisse  die  Ozeanischen  Salzablagerungen,"  Leipzig,  1912, 
p.  374-  By  far  the  larger  part  of  the  new  data  in  these  papers  are  for  solutions 
simultaneously  saturated  with  three  or  more  salts  and  are,  therefore,  beyond  the 
limits  of  complexity  of  mixture,  set  for  the  present  volume.  The  various  systems 
are  described  in  detail  and  diagrams  are  given.  A  table  summarizing  much  of 
the  data  (van't  Hoff  (1905))  is  given  on  the  following  page. 


641  SODIUM  CHLORIDE 

SOLUBILITY  OF  SODIUM  CHLORIDE  IN  AQUEOUS  SOLUTIONS  SIMULTANEOUSLY 
SATURATED  WITH  OTHER  SALTS  AT  25°. 

(van't  Hoff,  1905.) 

Mols.  per  1000  Mols.  HjO. 

Solution  Saturated  with  Respect  to  NaCl  and: 


K2C12.        MgCl2.        MgSO4.  . 

1  0.5      105           ......  MgCl2.6H2O  -f  Carnallite 

2  5.5        70.  5        ......  KC1  +  Carnallite 

44         20            ...           ...         4.5  "    -|-  Glaserite 

44         10.5        ......       14-5  Na2SO4+    " 

46          ...         ...          16.5      3.0  "      +  Astrakanite 

26          ...           7           34         ...  MgSO4.7H20  +  Astrakanite 

4       «...         67.5        12          ...  "           +MgS04.6H20 

2.5       ...         79             9.5      ...  Kieserite  + 

i          ...       101           5           ...  "        +  MgCl2.6H2O 

23          14           21.5        14         ...  KC1  +  Glaserite  +  Schonite 

19.5      14.5        25.5        14.5      ...  "    +  Leonite    -f- 

9.5       9.5       47           14.5      ...  "    +       "       -f  Kainite 

2.5       6           68             5          ...  "    +  CarnaUite  +    " 

i            i           85.5         8          ...  Kieserite  +  Carnallite  +  Kainite 

42           8            ...          16          6  Na2SO4  +  Glaserite  -f  Astrakanite 

27.  5      10.  5        16.5        18.5      ...  Schonite  +  Glaserite  +  Astrakanite 

22          10.  5        23            19          ...  Leonite  +  Glaserite  +  Astrakanite 

10.5       7.5       42           19         ...  +  MgSO4.7H2O  4-  Astrakanite 

9           7-5        45            19.5      ...  "4-            "           4-  Kainite 

3-5       4           65.5        i3         ...  MgS04.6H20+"          4-      " 

1.5        2           77            10         ...  MgSO4.6H2O  +  Kieserite  +    " 

i           0.5      100             5          ...  CarnaUite  +  MgCl2.6H20  +    " 

1  0.5      105            ......  MgCl2.6H2O  +  Carnallite 

2  5-5      70.5         ......  KC1              + 

CaCl2. 

i           ...        51.5         90.  5      ...  MgCl2.6H2O  +  Tachhydrite 

i         ii          ...         146         ...  KC1+  CaCl2.6H2O 

i           ...        35.5       121.5      ...  Tachhydrite  +  CaCl2.6H2O 

i           1.5      50.5         90.5      ...  MgCl2.6H2O+Tachhydrite+Carnallite 

i           9.5        5           141  .  5      ...  CaCl2.6H2O  +  KC1  +  CarnaUite 

i           2          34.5       121.5      ...  CaCl2.6H2O+Tachhydrite+  Carnallite 

Carnallite  =  KMgCl3.6H2O,  Glaserite  =  K3Na(SO4)2,  Astrakanite  =  Na2Mg- 
(SO4)2.4H2O,  Kieserite  =  MgSO4.H2O,  Leonite  =  MgK2(SO4)2.4H2O,  Schonite  = 
MgK2(SO4)2.6H2O,  Kainite  =  MgSO4.KC1.3H2O. 

SOLUBILITY  OF  SODIUM  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  AMMONIUM 

CHLORIDE. 

(Fedotieff,  1904.) 

f  o           Wt.  of  i  cc.             Mols.  per  1000  Gms.  H2O.  Gms.  per  1000  Gms.  H2O. 

Solution.                '  NH4C1.  NaCl.  '                'NI^Cl.                 N^O? 

o     ...       o  6.09        o      356.3 

.185         2.73  4.89         146.1       286.4 

15     .200      o  6.12        o      357-6 

191       1.07  5-58       57-3     326.4 

183          2.22  5.13          II8.9       300 

176         3-48  4.64         186.4       271.6 

175         3.72  4.55          198.8       266.8 

30     ...       o  6.16        o      360.3 

1.166      4.77  4.26      255.4     249 

45     •••       o  6.24        o      365 

6.02  4                     322.1            233.9 


SODIUM  CHLORIDE 


642 


SOLUBILITY  OF  SODIUM  CHLORIDE  IN  AQUEOUS  AMMONIA  AT  30°, 

(Hempel  and  Tedesco,  1911.) 
Gms.  per  1000  cc.  Sat.  Sol. 
Sat"  Sol.  '    NH3.  NaCl. " 

I.I735  29.535  293.38 

1.1656  40-655  292.5 

1.160  47.26  289.7 

I.I494  60.78  286.5 

Data  for  equilibrium  in  the  system  sodium  chloride,  arsenic  trioxide,  water,  at 
30°,  are  given  by  Schreinemakers  and  deBaat  (1915). 


dsoof 

Gms.  per  1000  cc.  Sat.  Sol. 

Sat.  Sol. 

NH3.                    NaCl.  ' 

I  .  1406 

72.07                283.38 

I-I395 

72.715              283.06 

I.I30I 

81.855              277.49 

I.I205 

97.49                270.57 

SOLUBILITY  OF  SODIUM  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  HYDRO- 
CHLORIC ACID. 

(Engel,  1888;  Enklaar,  1901.) 
AtO°.    (Engel.) 

Gms.  per  Liter. 


Mg.  Mols.  per  10  cc. 
HCl.        NaCl. 


Sp.  Gr.  of 

Solution. 


0.0 
1.0 

1.85 

9.28 
30.75 


54-7 
53  •$ 
52.2 

48-5 
44-0 

37-9 

23-5 

6.1 


207 

204 

202 

196 

185 

173 

i  .141 

i  .119 


HCl. 

NaCl". 

o.o 

32.0 

0.365 

0.674 

30-5 

1.859 

28.4 

3-38 

25-7 

5-49 

22.2 

ii  .20 

13-7 

20.54 

3-6 

At  I0°-I0.5°.    (Enklaar.) 
Mols.  per  Liter.          Grams  per  Liter. 


HCl. 

NaCl." 

o.o 

6.  ii 

0.27 

5-77 

o-35 

5-67 

0-43 

5-59 

o-57 

5-43 

0.72 

5-28 

2.60 

3-42 

2.80 

3-i8 

3.31 

2-74 

Results  at  o°  and  at  25°. 

(Armstrong  and  Eyre,  1910-11.) 


Gms.  HCl 
per  Liter 
of  Solvent. 

O 

9.II 
18.22 

36.45 
182.25 


Gms.  NaCl  per  100  Gms.  Sat.  Sol. 

At  o°.  At  25°. 

26.35  26.52(^25=1.2018) 
25.30  25.45(^25=1.1970) 
24.15  25.42(^25=1.1915) 
21.93  22.34(^25=1.1822) 
7.04(^25=1-1238) 


NaCl. 

35-77 
33-76 

33-19 
32.71 

3i-77 
30.89 

20.01 
19.04 
16.03 

Results  at  25°.       Results  at  30°. 

(Herz,  1911-12.)    (Schreinemakers,  1909-10.) 
Gms.  per  100  Gms.jSat.  Sol. 


HCl. 

0.0 

9.84 

12.76 

15.68 

20.78 

26.06 

94-77 

102. 1 
I2O.6 


Mols.  per  Liter. 


HCl. 
0.607 
1.032 
1.590 
2.II7 
3.283 


NaCl. 
4.850 
4.467 
3.782 
3-297 
2-343 


HCl. 

o 

6.93 
12.50 

17-35 
35-60 


NaCl. 
26.47 

16.16 

9.35 
4.52 

O.II 


Results  at  30°.    (Masson,  1911.) 

Gm.  Mols.  per  Liter.                              ^  of  Gms.  Mols.  per  Liter. 

Sat.  Sol.  '~HCL  NaCl.  * 

1.1427  3.052  2.463 

1.1289  4.152  1.628 

1.1188  5-950  0.630 

1.1258  7.205  0.268 


In  the  case  of  the  results  of  Masson  equilibrium  was  approached  from  above  and 
the  solutions  were  kept  in  a  thermostat  and  shaken  occasionally  during  2-6  days. 

SOLUBILITY  OF  SODIUM  CHLORIDE  IN  AQUEOUS  CALCIUM  CHLORIDE  SOLUTIONS 

AT  25°. 

(Mills  and  Wells,  1918.) 


Sat.  Sol. 

HCl. 

NaCl. 

I.  20l8 

O 

5.400 

I  .  1906 

0-4575 

4-932 

I  .  l8oi 

0.969 

I.I633 

1.786 

3.589 

I.I5I2 

2.412 

2.978 

Gms.  per  100  Gms.  Sat.  Sol. 


Sat.  Sol. 

CaCl2. 

NaCl.  ' 

I.2O7 

I.  103 

25.30 

I.  210 

2.l6o 

24.32 

1.209 

3.220 

23-37 

1.216 

5-451 

20.43 

I.22O 

7.398 

19.17 

^  Of  Gms.  per  100  Gms.  Sat.  Sol. 

Sat.  Sol,  '    CaCl2.  NaCl. 

1.225  9-50  17-55 

1.233  "-48  I5-9I 

1.241  17.77  IO-54 

1.257  21  8.05 

1.276  24.58  5.63 


643 


SODIUM  CHLORIDE 


SOLUBILITY  OF  SODIUM  CHLORIDE  IN  AQUEOUS  POTASSIUM  NITRATE  AT  25. 

(Ritzel,  1911.) 

Cms,  per  100  cc.  Sat.  Sol.  Cms,  per  100  cc.  Sat.  Sol. 

KNO3.               NaCl.  KNO3.               NaCl.    " 

O                 31.80  12                  30.86 

4     32-26  16     30.45 

8      1-8  20     30.10 


NaCl. 
31.80 

32-26 
31-85 

Data  for  the  solubility  of  NaCl  in  aqueous  MgCl2  solutions  are  given  by  Feit 
and  Przibylla  (1909.) 


Solvent. 

Water 


SOLUBILITY  OF  MIXTURES  OF  SODIUM  CHLORIDE  AND  OTHER 
SALTS  IN  WATER,  ETC. 

to  Gms.  per  100  Gms.  Solvent.  Authority. 


17 


25 

80 

Alcohol  (40%)   25 

Water  20 

25 


26.4  NaCl+22.iNH4Cl* 
34-5  "    +  4-iBaCl2 
38.3  «    +29-5KN03 

38.5  "    +41-14     " 
39.81  "    +168.8     " 
I5-78  +13-74     " 
30.54  +I3-95 
28.90  "    +16.12 

*  Sp.  Gr.  of  solution  at  17°  =  1.179. 


(Karsten.) 


(Soch  — J.  Physic.  Ch.  2,  46,  '08.) 


(Quoted  by  Euler  — Z.  physik.  Ch. 
49,  315.  '04-) 


SOLUBILITY  OF  MIXTURES  OF  SODIUM  CHLORIDE  AND  POTASSIUM  SULFATE 
IN  WATER  AT  VARIOUS  TEMPERATURES. 

(Precht  and  Wittgen,  1882.) 


to         Grams  per  100 

Grams  H2O.         f  0 

Grams  per  100  Grams 

H2O. 

NaCl 

K2S04 

KCl 

NaCl 

K2S04 

KCl 

10 

33-4 

8 

.1 

3 

.2 

60 

36-4 

II 

•9 

2 

•7 

20 

34-o 

8 

-9 

3 

.1 

7o 

36.6 

12 

.8 

3 

.2 

30 

34-6 

9 

.6 

2 

•9 

80 

36.0 

12 

•3 

5 

.1 

40 

35-2 

10 

•4 

2 

.8 

9o 

35-9 

12 

4 

7 

•  O 

50 

35-8 

ii 

.1 

2 

.8 

100 

35-6 

12  , 

6 

8 

.8 

SOLUBILITY  OF  SODIUM  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  SODIUM 
BICARBONATE  SATURATED  WITH  CO2.      (Fedotieff  1904.) 


3° 

« 

1? 


Wt.  of  i  cc. 
Solution. 


I.  208 
1.203 
1.203 
I  .196 
I.I99 
1.189 
I.I98 


Mols.  per  1000  Gms.  H2O. 


Gms.  per  1000    Gms.  H2O. 


NaHCO3. 

NaCl. 

0 

6.09 

0.09 

6 

O 

6.12 

O.I2 

6.06 

0 

6.16 

0.17 

6.12 

0 

6.24 

0.23 

6.18 

'NaHC03. 

NaCl.  ' 

O 

356.3 

7-7 

350-1 

0 

357-6 

IO 

354-6 

0 

360.3 

13-9 

358.1 

0 

365 

19-5 

361.5 

SOLUBILITY  OF  SODIUM  CHLORIDE  IN  AQUEOUS  SODIUM  HYDROXIDE  AT  30° 


Gms.  per  100  Gms.  Sat.  Sol. 
'    Na20.  NaCl. 

o  26.47 

4.47  21.49 

12.22  13.62 

24.48  4-36 


(Schreinemakers,  1909-10,  1910.) 

Solid 
Phase. 

NaCl 


NasO. 

NaCl.  ' 

OUUU   i  11<UC. 

29.31 

2.40 

NaCl 

37.85 

1.  12 

" 

41.42 

0.97 

"  +NaOH.H2O 

±42 

0 

NaOH.H2O 

SODIUM   CHLORIDE 


644 


SOLUBILITY  OF  SODIUM  CHLORIDE  IN  AQUEOUS  SODIUM  HYDROXIDE 

SOLUTIONS. 


At  o°  (Engel). 


Mg.  Mols.  per  10  cc. 


NajO. 
O 

4-8 

6-73 
10.41 

14.78 
30.50- 
37.88 

53-25 


NaCl. 

54-7 
49-38 
47-21 
42.38 

39-55 

24.95 

19.30 

9.41 


Sp.  Gr.  of 
Solutions. 


207 
221 
225 
236 
249 
295 
314 


1.362 


(Engel;  Winteler,  1900.) 


Gms.  per  Liter. 


NaOH. 

O 
38.4 

53-8 
183.2 
118.2 

244 
303 

426 


NaCl. 
320 
288.9 
276.2 
247.9 

23I-4 
146 
112  .9 

55 


At  20°  (Wintelei 

Gms.  per  Liter.          gt 

). 

>.  Gr.  of 

jluiions. 

[.200 

NaOH. 
10 

NaCl.     '     S 
308            ] 

SO 

297            1.230 

100 

253 

.250 

150 

2I3            ] 

.270 

200 

173          3 

.290 

300 
100 

112           3 
6l 

•330 

•375 

500 
640 

30              -425 

18        1.490 

SOLUBILITY  OF  SODIUM  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  SODIUM 
NITRATE  AND  VICE  VERSA. 

(Bodlander,  1891;  Nicol,  1891;  results  at  25°  by  Soch,  1898.) 


NaCl  in  Aqueous  NaNOa. 
Results  at  15.5°  (B.). 


NaNO3  in  Aqueous  NaCl. 
Results  at  15°  (B.). 


Sp.  Gr.  of 

Gms.  per 

ioo  cc.  Sat. 

Solution. 

Sp.  Gr.  of 

Gms.  per 

ioo  cc.  Sat 

.  Solution. 

Solutions. 

NaN03. 

H20. 

NaCl. 

Solutions. 

NaCl. 

H20. 

NaN03. 

1.2025 

O 

88.47 

31 

.78 

I 

•3720 

0 

74.82 

62 

•38 

I-2305 

7 

•53 

87.63 

27 

.89 

I 

•3645 

4-0 

75-69 

56 

.76 

1.2580 

13 

.24 

86.25 

26 

•31 

I 

•3585 

7-24 

75-71 

S2 

.09 

I  .2810 

21 

•58 

82.66 

23 

.98 

I 

•3530 

11.36 

76.86 

47 

.08 

1.3090 

28 

.18 

80.42 

22 

•30 

I 

•3495 

15-33 

76.96 

42 

.66 

i  -3345 

33 

.80 

79-25 

20 

•  40 

I 

•3485 

I7.8l 

77-14 

39 

.90 

1-3465 

37 

.88* 

77-37 

19 

.40* 

I 

•3485 

I8.97* 

77-15 

38 

•73* 

I-3465 

37 

.64* 

77-34 

J9 

.67* 

I 

•3485 

19.34* 

77-49 

38. 

,02* 

)  Results  at  20°  (N.). 

Grams  per  ioo  Grams  H2O.  Grams  per  ioo  Grams  H2O. 


NaNO, 


14.17 

28-33 
42.50 

54-63* 


35.91  NaCl 

32.82  " 
29.78  « 
26.91  " 
24.92*  " 


o      NaCl 

87.65  NaNO3 

6-5 

11 

77-34 

si 

13.0 

it 

68.50 

M 

19-5 

It 

60.49 

14 

ioo  gms.  H2O  dissolve  43.66*  gms.  NaNO3  +  26.58*  gms.  NaCl  at  25°. 
ioo  gms.  H2O  dissolve  121.6*  gms.  NaNO3  +  17.62*  gms.  NaCl  at  80°. 
ioo  gms.  aq.  alcohol  of  40  wt.  per  cent  dissolve  22.78  gms.  NaNO3  +  10.17 
NaCl  at  25°. 

*  Indicates  solutions  saturated  with  both  salts. 


645 


SODIUM  CHLORIDE 


SOLUBILITY  OF  SODIUM  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  SODIUM  NITRATE 

AND  VICE  VERSA. 

(Leather  and  Mukerji,  1913.) 


Results  at  30°. 

,     Gms.  per  100  Gms. 
atsol    -    -^2_      ,    S 

Results  at  40°. 
Gms.  per  100  Gms. 
at  Sol                H?°-              S 

Results  at  91°. 

Gms.  per  100  Gms. 
£of                  H?0. 

Solid  Phase 
in  Each  Case 

>L  NaN03.      NaCl. 
.202        0              36.3 

.2j6    24.21     31.16 

.343  48.15    26.35 
.379  63.08   23.50 
.  388   63  .40    23  .  40 
.381   67.91    19.69 
.394   81.46     9.76 

.  406    95  .  90      o 

"NaN03.      NaCl.-- 
•197         o          36.53 

.284     27.31    30.53 
.323     54.82    26.50 
.409     73.96    21.87 
.397     74.01    21.71 

.396       75.29     21.  61 
.410       89.90     10.80 
.421     105.2        o 

NaN03.       NaCl/ 
[.189          0            38.72 
•296        37.43      30.21 
.381        79.65      23.17 
.487      127.2        17.05 
.519      141.4        15.93 
.518      141.3        15.83 
.504      149.5          9-03 
.521     160.8        o 

NaCl 

« 
« 

"  f  NaN03 
"  NaNO3 

Results  are  also  given  at  20°  which  agree  satisfactorily  with  those  of  Nicol. 
Additional  results  at  30°,  agreeing  fairly  well  with  the  above,  are  given  by  Coppa- 
doro  (1913).  Data  for  the  solubility  of  sodium  chloride  in  dilute  solutions  of 
sodium  nitrate  at  o°  and  at  25°  are  given  by  Armstrong  and  Eyre  (1910-11). 

SOLUBILITY  OF  SODIUM  CHLORIDE  IN  AQUEOUS  7.45  PER  CENT  SODIUM 
SULFATE  SOLUTIONS. 

(Marie  and  Marquis,  1903.) 


14.8 
17.9 
25.6 


Gms.  NaCl  per 
100  Gms.  Sat.  Sol. 

23-30 
23-33 
23.485 


27-75 
32.18 
34-28 


Gms.  NaCl  per 
100  Gms.  Sat.  Sol. 


23.55 
23.68 


For  additional  data  on  this  system  see  sodium  sulfate,  pp.  669  and  670. 


SOLUBILITY  OF  SODIUM  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  ETHYL 

ALCOHOL. 

(Armstrong  and  Eyre,  1910-11.) 


Results  at  o°. 


Results  at  25°. 


Solvent  Gms. 
C2H5OH  per 
1000  Gms.  H2O. 

0 

Gms.  NaCl 
per  loo  Gms. 
Sat.  Sol. 

26.46 

11.51 

25-97 

23-03 
46.06 
138.18 

24.41 
20.95 

<*25  Of 

Sat.  Sol. 

Solvent  Gms. 
C2H6OH  per 
1000  Gms.  H2O. 

Gms.  NaCl 
per  100  Gms. 
Sat.  Sol. 

I  .202 

O 

26.55 

.196 

11.51 

26.06 

.190 

23-03 

25.63 

.179 

46.06 

24-75 

.159 

92.12 

23.29 

.1115 

230.3 

19.35 

SOLUBILITY  OF  SODIUM  CHLORIDE  IN  AQUEOUS  ALCOHOL  AT  28°. 

(Fontein,  1910.) 


Gms.  per  100  Gms.  Sat.  Sol. 


Gms.  per  100  Gms.  Sat.  Sol. 


QH6OH. 

H20. 

NaCl. 

O 

73-53 

26.47 

3-8 

71.6 

24.6 

7-7 

69.7 

22.6 

16.1 

64.6 

19-3 

25-3 

58-9 

15-8 

35 

52-5 

12-5 

C2HBOH. 

H20. 

NaCl. 

45-35 

45-35 

9-3 

56.2 

37-5 

6.3 

67.4 

28.9 

3.7 

78.8 

19.7 

1.5 

89.6 

10 

0.4 

Results  are  also  given  by  Fontein  showing  the  solubility  of  sodium  chloride  in 
mixtures  of  ethyl  alcohol,  amyl  alcohol  and  water  at  28°,  both  when  one  liquid 
phase  is  present  and  when  conjugated  liquid  layers  are  formed. 


SODIUM  CHLORIDE  646 

SOLUBILITY  OP  SODIUM  CHLORIDE  IN  ALCOHOLS. 

(At  18.5°,  de  Bruyn  —  Z.  physik.  Ch.  10,  782,  '92;  Rohland  —  Z.  anorg.  Ch.  i89  327,  '98.) 

Gms.  NaCl  Gms.  NaCl 

t°.  Alcohol.  per  too  t°.  Alcohol  per  100 

Gms .  Alcohol .  Gms .  Alcohol , 

18.5      Abs.  Methyl      1.41        room  temp.     Methyl  ^15= 0.799      I-33 
"     Ethyl        0.065  Ethyl  <Z15    =0.81        0.176 

"  Propyl<£15  =0.816      0.033 


SOLUBILITY  OF  SODIUM  CHLORIDE  IN  AQUEOUS  ETHYL  ALCOHOL 

SOLUTIONS. 

(Bodlander  —  Z.  physik.  Ch.  7,  317,  '91;  Taylor  —  J.  Phys.  Ch.  i,  723,  '97;  also  Bathrick  —  Ibid,  i, 

159,  '96.) 

Results  at  11.5°  (B.).  Results  at  13°  (B.). 


Sp.  Gr.  of 

Gms.  per  loo^cc.  Solution. 

Sp.  Gr.  of 

Gms.  per  TOO  cc.  Solution. 

Solutions.        CgHeOH. 

H2O. 

Na 

,C1. 

Solutions. 

C2H5OH. 

H20. 

NaCl. 

I 

•2035 

O 

86.62 

31 

•73 

I 

.2030 

O 

88.70 

31.60 

I 

.1865 

2 

.86 

86.14 

29 

.66 

I 

.1348 

II.  8l 

78.41 

23.26 

I 

.1710 

5 

.41 

83  -93 

27 

•77 

I 

.1144 

J5-99 

74.64 

20.  8l 

I 

•1548 

7 

•93 

81.50 

26 

•05 

I 

.0970 

19-39 

71-45 

18.86 

I 

•1350 

10 

.84 

78.78 

24 

.28 

I 

.0698 

24-95 

65.80 

16.23 

I 

.1390 

ii 

.22 

78.62 

23 

-65 

I 

.0295 

32-33 

57.96 

12.66 

I 

.1088 

16 

•85 

73-40 

20 

•63 

O 

.9880 

40.33 

49-34 

9.13 

O 

•9445 

49.28 

38.54 

5-93 

0 

•9075 

57-91 

29-37 

3-47 

o 

.8700 

63.86 

21  .62 

1.52 

o 

.8400 

72  .26 

11.24 

0.50 

Results  at  30°  and  at  40°  (T.). 

Wt.  per  cent        At  30°,  Gms.  NaCl  per  100  Gms.  At  40°,  Gms.  NaCl  per  TOO  Gms. 

Alcohol  in  Solvent.  '   Solution.  Water.  Solution.  Water. 

o  26.50  36-05  26.68  36-38 

5  24.59  34.29  24.79  34-69 

10  32.66  32-57  22.90  33 .00 

20  I9-o5  29.40  19.46  30.20 

30  15.67  26.53  16.02  27.25 

40  12.45  23.70  12.75  24.37 

50  9  34  20.60  9.67  21.42 

60  6.36  16.96  6.65  17.82 

70  3.36  12.75  3-87  13 -^ 

80  1.56  7.95  1.69  8.68 

90  0.43  4-30  0-50  5.10 

100  gms.  alcohol  of  0.9282  Sp.  Gr.  =  45.0%  by  wt.  dissolve  at: 

4°       10°       13°         23°       32°       33°       44°       5i°       6°° 
10.9     ii. i     11.43     Il-9     I2-3     I2-5     I3-1     J3-8     14- 1  gms.  NaCl 

(Gerardin  —  Ann.  chim.  phys.  [4]  5,  146,  '56.) 

ioo  gms.  of  a  mixture  of  equal  parts  of  96%  alcohol  and  98%  ether 
dissolve  o.n  gm.  NaCl. 

(Mayer  —  Liebig's  Ann.  98,  205,  '56.) 


647  SODIUM  CHLORIDE 

SOLUBILITY  OF  SODIUM  CHLORIDE  IN  AQUEOUS  METHYL  ALCOHOL. 

(Armstrong  and  Eyre,  1910-11.) 

Results  at  o°.  Results  at  25°. 

Solvent,  Gms.  Gms.  NaCl  Solvent,  Gnu.  Gms.  NaCl 

CH,OH  per  per  100  Gms.  CH,OH  per  per  100  Gms. 

1000  Gms.  HaO.  Sat.  Sol.  1000  Gms.  H20.  Sat.  Sol. 

o  26.35  8.01  26.29 

8.01  26.05  16.02  26.02 

16.02  25.79  32.04  25.50 

32.04  29.19  96.12  23.50 

A  sat.  solution  of  NaCl  in  CH3OH  contains  o.i  gm.  NaCl  per  100  gms.  solution 
at  the  critical  temperature.  (Centnerszwer,  1910.) 

SOLUBILITY  OF  SODIUM  CHLORIDE  IN  AQUEOUS  PROPYL  ALCOHOL. 

(Armstrong  and  Eyre,  1910-11.) 

Aqueous  propyl  alcohol  containing  15.01  gms.  C3H7OH  per  1000  cc.  H2O  dis- 
solves 25.71  gms.  NaCl  per  100  gms.  sat.  solution  at  o°  and  25.95  gms.  at  25°. 

Aqueous  propyl  alcohol  containing  30.02  gms.  C3H7OH  per  1000  cc.  H2O  dis- 
solves 25.12  gms.  NaCl  per  100  gms.  sat.  solution  at  o°  and  25.37  gms.  at  25°. 


EQUILIBRIUM  IN  THE  SYSTEM  SODIUM  CHLORIDE,  NORMAL  PROPYL  ALCOHOL 
AND  WATER  AT  23-25°. 

(Frankforter  and  Frary,  1913.) 

The  authors  determined  the  binodal  curve  and  quadruple  points  of  the  system 
but  did  not  locate  tie  lines. 

Gms.  per  100  Gms.  Homogeneous  Liquid.  Gms.  per  100  Gms.  {Homogeneous  Liquid. 

NaCl.  C3H7OH.  H2O.A  NaCl.  C3H7OH.  H2O.' 

0.55  87.7  11-75*  14-38  5-39  80.23 

2.23  51.57  46.20  15.42  5.11  79.47 

3-55  18.99  77-46  16.38  4.47  79.14 

3.90  14.78  81.32  18.08  3.83  78.09 

5.27  12.77  81.96  20.  12  3.27  76.61 

8.04  9.49  82.47  22.35  2.64  7S-01 

10.49  7-79  81.72  24.50  2.13  73.37 

12.20  6.57  8l.23  24.9  2.3  72.8* 

*  Quad.  pt. 

The  effect  of  temperature  upon  the  equilibrium  in  the  above  system  was  greater 
than  observed  in  any  of  the  other  systems  investigated  and  additional  data,  illus- 
trating the  extent  of  the  temperature  influence,  are  given. 

100  gms.  sat.  sol.  of  NaCl  in  99.6  per  cent  C3H7OH  contain  0.04  gm.  NaCl 
at  25°.  (Frankforter  and  Frary,  1913.) 

EQUILIBRIUM  IN  THE  SYSTEMS  SODIUM  CHLORIDE,  ALLYL  ALCOHOL,  WATER,  AT 
20°  AND  SODIUM  CARBONATE,  ALLYL  ALCOHOL,  WATER,  AT  20°. 

(Frankforter  and  Temple,  1915.) 

Results  for  Results  for 

NaCl  +  CH2  :  CHCH2OH  +  H2O.  Na2CO3  +  CH2  :  CH.CH2OH  +  H2O. 

Gms.  per  100  Gms.  Alcohol  +  Water.  Gms.  per  100  Gms.  Alcohol  +  Water. 


rNaCl.  Alcohol.  Water.  Na^CO,.  Alcohol.  Water. 

3.509  69.867  30.133  0.456  61.112  38.888 

4.452  64.858  33-142  0.708  56.334  43-666 

5.079  60.821  39-179  i.  on  51.930  48-070 

6.712  54-683  45-3*7  1.468  48.109  5I-89i 

8.776  47-132  52.868  2.580  41-052  58.948 

10.650  40.392  59.608  3.414  37-I26  62.874 

12.535  33-224  66.776  4.739  ,32.166  67.834 

14.925  27.261  72.739  7-774  '23-753  76.247 

18.557  I9-705  80.295  10.079  18.407  81.593 


SODIUM  CHLORIDE 


648 


SOLUBILITY  OF  SODIUM  CHLORIDE  IN.  SEVERAL  ALCOHOLS  AT  25°. 

(Turner  and  Bissett,  1913.) 

Cms.  Nad  per 
100  Cms.  Alcohol. 

1.31 
o  .  065 


A,    ,    , 
AlcohoL 

Methyl  Alcohol,    CH3OH 
Ethyl  Alcohol, 


C2H5OH 


Propyl  Alcohol, 
Amyl  Alcohol, 


C3H7OH 
C5HnOH 


0.012 
0.002 


SOLUBILITY  OF  SODIUM  CHLORIDE  IN  AQUEOUS  ACETONE  SOLUTIONS  AT  20° 

(Frankforter  and  Cohen,  1914.) 
Cms.  per  100  Cms.  Sat.  Sol.  Cms.  per  100  Cms.  Sat.  Sol. 


NaCl. 

H20. 

(CH3)2CO. 

25-9 

73-06 

I.O4 

24.19 

71.18 

4-03 

20.85 

66.78 

12.37 

18.32 

63.16 

18.52 

17.89 

62.21 

19.90 

NaCl. 

H20. 

(CH3)2CO. 

16.55 

61.59 

21.86* 

0-45 

13-75 

85.8* 

0.32 

13.92 

85.76 

o.  19 

10.82 

88.99 

O.I2 

8.94 

90.94 

*  Quad  pt. 

Between  the  concentration  21.86  and  85.8  per  cent  acetone,  two  layers  are 
formed.  The  binodal  curve  corresponding  to  this  range  of  concentration  was 
determined  and  it  is  stated  by  the  authors  that  tie  lines  were  located  but  the 
analytical  data  for  them  are  not  given.  The  results  for  the  binodal  curve  are  as 
follows: 


Cms.  per  100  Cms.  Homogeneous  Liquid. 


Gms.  per  100  Cms.  Homogeneous  Liquid. 


NaCl. 

H20. 

(CH3)2CO. 

0-59 

15.46 

83.95 

0.79 

17-58 

81.63 

0-93 

18.83 

80.24 

1.27 

22.19 

76.54 

i-57 

23.89 

74-54 

2.31 

27.27 

70.42 

4.87 

36.79 

58-34 

'NaCl. 

H20. 

(CH3)2CO. 

5-87 

40.19 

53-94 

6-45 

42.  12 

51-43 

7-53 

46.  12 

46.35 

8.87 

49-39 

41.74 

9-47 

50.92 

39.61 

to.  35 

53-o6 

36.59 

15-87 

59-71 

24.42 

Additional  data,  showiner  the  effect  of  temperature  on  the  above  system,  are 
also  given 


SOLUBILITY  OF  SODIUM  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF: 


Acetone  at  20°. 
(Herz  and  Knoch,  1904.) 


cc.  Acetone                          NaCl  per.ioo  cc. 
per  100  cc.                                   Solution. 

Solvent.                         Millimols. 

o                         537-9 
10                         464.6 

20                                  394.8 
30                                  330.1 

32  )  Lower  layer  308  .  5 
87  j  Upper  layer      7  .  7 
88                            7.3 
90                            4-3 

Gms. 

31-47 
27.18 
23.10 
19.32 
18.05 
0-45 
0-43 
0.25 

Glycerol  at  25°. 
(Herz  and  Knoch,  1905.) 


Wt.  Per  cent       NaCl  per  100  cc. 
Glycerol  in               Solution.                 Sp.  Gr.  of 

Solvent. 

Millimols. 

Gms. 

O 

545-6 

31-93 

.  1960 

13.28 

501.1 

29.31 

.2048 

25.98 

448.4 

26.23 

•2133 

45-36 

370.2 

21.66 

.2283 

54-23 

333-9 

19-54 

•  2381 

83.84 

220.8 

12.91 

.2666 

100* 

167.1 

9-78 

.2964 

*  Sp.  Gr.  of  Glycerol,  1.2592.     Impurities  about  1.5%. 

100  gms.  sat.  solution  in  glycol  contain  31.7  gms.  NaCl  at  14.8°. 

(de  Coninck,  1905.) 

100  gms.  H2O  dissolve  236.3  gms.  sugar  -f-  42.3  gms.  NaCl  at  31.25°,  or  100 
gms.  sat.  aq.  solution  contain  62.17  gms.  sugar  +  11.13  gms.  NaCl.    (Kahler,  1897.) 


649  SODIUM   CHLORIDE 

EQUILIBRIUM  IN  THE  SYSTEM  SODIUM  CHLORIDE,  METHYL  ETHYL  KETONE 
AND  WATER  AT  25°  (BINODAL  CURVE). 

(Frankforter  and  Cohen,  1916.) 
Cms.  per  100  Cms.  Homogeneous  Liquid.  Cms.  per  100  Cms.  Homogeneous  Liquid. 

'NaCl.  CH3.CO.QH6.            H20.  NaCl.  CH3.CO.C2H5.            HA 

0.35                  20.13  79.52                         6.75  10.80  82.45 

0-55                  19-75  79-70  10.07  7-65  82.28 

1.42                  16.52  82.06  I4-32  5-36  80.32 

1. 80                  17.70  80.50  14.65  3.83  81.52 

2.47  16.24          81.29  23-i5  2.08          74-77 

4.11  13.34          82.55  24.14  0.94          74.92 


SOLUBILITY  OF  SODIUM  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  CARBAMIDE 
(UREA)  AND  OF  FORMAMIDE  AT  25°. 

(Ritzel,  1911.) 

In  Aqueous  Carbamide.  In  Aqueous  Formamide. 

Cms.  CO(NH2)2  Cms.  NaCl  Cms.  HCO.NH2  Cms.  NaCl 

per  100  cc.  per  100  cc.  per  100  cc.  per  100  cc. 

Solution.  Solution.  Solution.  Solution. 

o  31-80          o  31-80 

5  30-63          2.3  30.98 

9-6  29.05          5.3  30.86 

13  28.46          8  30.40 

18  27.65  ii  29.11 

23  27.24  15  28.52 

28  26.56  18.8  27.76 

According  to  results  by  Fastert  (1912),  the  solubility  of  sodium  chloride  in 
aqueous  solutions  of  urea  increases  slightly  with  increase  of  urea  in  solution,  thus: 

Cms.  CO(NH2)2  per  100  cc.  Sol.    10          20          30          40          50 
Cms.  NaCl  per  100  cc.  Sol.  31.92    32.17    32.51     32.93     33.40 

Data  for  equilibrium  in  the  system  sodium  chloride,  succinic  acid  nitrile,  water 
are  given  by  Timmermans  (1907). 

loo  gms.  95%  formic  acid  dissolve  5.8  gms.  NaCl  at  19.7°.  (Aschan,  1913.) 

IOO  gms.  hydroxylamine  dissolve  14.7  gms.  NaCl  at  17.5°.  (deBruyn,  1892.) 

100  cc.  anhydrous  hydrazine  dissolve  8  gms.  NaCl  at  room  temp. 

(Welsh  and  Broderson,  1915-) 


FUSION-POINT  DATA  (Solubilities,  see  footnote,  p.  i)  ARE  GIVEN  FOR  THE 
FOLLOWING  MIXTURES. 

NaCl  +  HC!.  (Dernby,  1918.) 

+  Na2CrC>4.  (Sackur,  1911-12.) 

+  NaCN.  (Truthe,  1912.) 

-j-  NaF.  (Ruff  and  Plato,  1903;  Wolters,  1910;  Plato,  1907.) 

+  NaOH.  (Scarpa,  1915.) 

-j-  Nal.  (Ruff  and  Plato,  1903;  Amadori,  19123.) 

-j-  NaNC>2.  (Meneghini,  1912.) 

+  Na4P2O7.  (LeChatelier,  1894.) 

-{-  Na2SO4.  (Ruff  and  Plato,  1903;   janecke,  1908;   Wolters,  1910;  Sackur,  1911-12.) 

-j-  SrCU.  (Vortisch,  1914;  Sackur,  1911-12.) 

-j-  SrCO3.  (Sackur,  1911-12.) 

-j-  T1C1.  (Sandonnini,  1911,  1914.) 


SODIUM   CHROMATES  650 

SODIUM   CHROMATES  (Mono,  Di,  etc.) 


SOLUBILITY  IN  WATER. 

(Mylius  and  Funk,  1900;  see  also  Salkowski,  1901.) 

Sodium  Monochromate.                              Sodium  Bichromate. 

Gms.  Na2      Mols.  Na2                                           Gms.  Na2    Mols.  Na2 
«.  o           CrO4  per    CrO4  per        Solid                t  o       Cr2O7  per     Cr2O7    per               Solid 
"    *          TOO  Gms.     100  Mols       Phase.                         100  Gms.       100  Mols.                Phase. 

Solution. 

H20. 

Solution. 

H2O. 

0 

24 

.07 

3 

a^rC^.ioH^    O 

6z. 

98 

II 

.2 

Na2Cr2O7.2H2O 

10 

33 

.41 

5 

•55 

17 

63- 

82 

12 

.1 

41 

18* 

40 

.10 

7 

•43 

i8| 

63- 

92 

12 

.l6 

" 

18. 

5 

41 

•65 

7 

•94 

34-5 

67.36 

14 

.2 

" 

19. 

5 

44 

.78 

9 

.01 

"          52 

71  . 

76 

17 

•4 

M 

21 

47 

.40 

10 

.00 

72 

76. 

9 

22 

.8 

M 

25. 

6 

46 

.08 

9 

a2CrO4.4H2O   8  1 

79- 

8 

27 

.1 

" 

31- 

5 

47 

•05 

9 

.90 

93 

81. 

19 

29 

.6 

Na2Cr207 

36 

47 

.98 

10 

•  2 

98 

8z. 

25 

29 

.8 

" 

40 

48 

•97 

10 

.6 

M 

Sodium  Tri  Chromate. 

A  £ 

^\O 

.20 

II 

•• 

T"0 

V 

Gms.  I 

sTa2 

Mols. 

Na2 

49  • 

5 

50 

•93 

II 

•5 

to 

Cr30,0 

per 

Cr3Ojo  per 

Solid 

54- 

5 

52 

.28 

12 

.2 

• 

11 

100  Gms. 
Solution. 

100  Mols. 
H20 

Phase. 

59- 

5 

53 

•39 

12 

•7 

o 

80. 

03 

19 

•9 

Na2Cr3010.H20. 

65 

55 

•23 

13 

•7 

Na2Cr04       15^ 

80.44 

2O 

•4 

" 

70 

55 

•15 

13 

.6 

IS 

80.60 

2O 

•56 

«• 

80 

55 

•53 

13 

.8 

55 

82.68 

23 

•7 

« 

100 

55 

•74 

14 

.0 

99 

85.78 

29 

•9 

" 

*  Sp.  Gr.  of  sat.  sol.  at  18°  =  1.432.  f  Sp.  Gr.  of  sat.  sol.  at  18° 

t  Sp.  Gr.  of  sat.  solution  at  18°  =  1.745. 


2.059 


Sodium  Tetrachromate. 


Tetrasodium.  Chromate. 


Gms. 

Mols. 

Gms. 

Mols. 

1°  ~ 

Na2Cr4Ol3 

Na2Cr4Ol3 

Solid 

t°. 

Na4Cr05 

Na4CrO8 

per  zoo  Gms. 
Solution. 

per  100 
Mols.H2O. 

Phase. 

per  100  Gms.    per  100 
Solution.      Mols.H2O. 

O 

72.96 

10.5 

Na2Cr4O,3.4H2O 

O 

33-87 

4.II 

16 

74.19 

II  .2 

it 

10 

35-58 

4.42 

18* 

74.60 

II  .27 

" 

i8t 

37-50 

4.81 

22 

76.01 

12-3 

" 

27. 

7  40-09 

5-38 

37 

45-13 

6.62 

Solid 
Phase. 


*  Sp.  Gr.  of  sat.  solution  at  i8°=«  1.926. 


t  Sp.  Gr.  of  sat.  solution  at  18°  =  1.446. 


A  new  hydrate  of  sodium  chromate,  Na2CrO4.6H2O,  was  found  by  Salkowski, 
(1901)  and  the  following  data  for  its  range  of  existence  were  determined. 


f. 

17.7 

19.2 

19.525 

21.2 
24.7 


Gms. 

NajCrO4 
per  100 
Gms. 

Solution. 

43.65 
44.12 

44-2* 
44.64 
45-75 


Mols. 


per  100        Solid  Phase. 
Mols. 
H20. 

8 . 62  Na2CrO4.ioH2O 
8.77    " 

...      "  +Na2CrO4.6H2O 
8.96   Na2CrO4.6H2O 
9-37 


Gms. 
Na2CrO4 

per 
100  Gms. 

Sol. 


25.9        46.3^ 


28.9 
29.7 
31.2 


46.47 

46.54 
47.08 


Mols. 
Na,CrO« 

per          Solid  Phase. 
100  Mols. 
H20. 

9.57  Na2CrO4.6H2O 

+Na2CrO4.4HzO 

9.64 
9.67 
9.88 


*  This  determination  by  Richards  and  Kelley  (1911). 


651 


SODIUM   CHROMATES 


SOLUBILITY  OF  SODIUM  CHROMATES  IN  WATER  AT  30°. 

(Schreinemakers,  1906.) 

• 

Composition  in  weight  per  cent: 

Of  Solution.  Of  Residue. 


%Cr03. 

%Na20. 

o 

±42 

2.00 

41.44 

2.04 

40.89 

4-23 

35  -51 

6.64 

32-34 

15.19 

27.06 

10-22 

29-39 

8-93 

28.49 

8.62 

26.91 

13  .12 

23.91 

18.44 

22.86 

19.26 

22.98 

17.84 

24.21 

28.82 

17.88 

38.93 

16.30 

48.70 

16.49 

50.68 

15-72 

58.08 

13-89 

66.13 

13.70 

65.98 

14-15 

68.46 

10.95 

66.88 

9-85 

70.06 

11.85 

69.04 

11.04 

67.84 

9.81 

64.48 

4-51 

62.28 

0-0 

%Cr08. 


27.52 
27.72 

37-07 
I5-48 
18.09 


%Na20. 


5.83         42.64 


36.57 
34-60 
32.20 
28.41 
26.89 


18.57         25.92 


21.54 

25-31 

26.24 

24-98 

31-97 

23-47 

40.70 

20.83 

47-49 

19-75 

62.76 

I7-38 

69.48 

16.06 

69.46 

15.15 

73.88 

I3-38 

71.27 

10.67 

83  -95 

9-57 

81.80 

6-43 

82.85 

5-42 

79-49 

2.71 

Solid  Phase. 
NaOH.H2O 

NaOH.H20  +  Na2Cr04 
Na2Cr04 


Na2Cr04.4H20 


Na2CrO4. 


Na2Cr30,0.H20 

Na2Cr3Oio.H20  +  Na2Cr4Ql3^HaO 

Na2Cr30l3.4HaO 

Cr08 


100  gms.  of  a  saturated  aqueous  solution  contain  at  30°: 
46.627  gms.  Na2CrO4,  or  100  gms.  H2O  dissolve  87.36  gms.  Na2CrO4. 
66.4  gms.  Na2Cr2O7,  or  100  gms.  H2O  dissolve  197.6  gms.  Na2Cr2O7. 
100  gms.  absolute  methyl  alcohol  dissolve  0.345  Sms.  Na2CrO4  at  25°. 

(de  Bruyn,  1892.) 

Data  for  equilibrium  in  the  system  sodium  chromate,  sodium  sulfate  and  water 
at  15°  and  at  25°  are  given  by  Takenchi  (1915).  The  mixtures  were  rotated  at 
constant  temperature  until  attainment  of  equilibrium  and  both  the  saturated 
solutions  and  the  undissolved  residues  were  analyzed.  Very  extensive  tables  of 
results  are  given.  The  decahydrates  of  sodium  and  chromium  are  isomorphous 
and  the  results  show  that  these  two  salts  are  mutually  miscible  in  all  proportions 
at  15°.  At  25°  the  solubility  curve  consists  of  three  branches.  The  solutions  of 
the  first  branch  are  in  equilibrium  with  decahydrated  mixed  crystals,  those  of  the 
second  branch  with  anhydrous  sulfate  and  those  of  the  third  with  both  anhydrous 
sodium  sulfate  and  hexahydrated  sodium  chromate. 


SODIUM   CHROMATES  652 

SOLUBILITY  OF  SODIUM  DICHROMATE  IN  ALCOHOL  AT  19.4°. 

(Reinitzer,  1913.) 

An  excess  of  Na2Cr2O7.2H2O  was  shaken  with  absolute  alcohol  for  10  minutes 
and  the  mixture  filtered.  The  filtrate  contained  5.132  gms.  NaaC^Oy^I^O  per 
100  cc.  and  its  d\$.i  was  0.8374.  The  solution  decomposed  within  a  few  minutes 
with  production  of  a  brown  precipitate  and  evolution  of  an  aldehyde  odor.  The 
results  are,  therefore,  only  approximately  correct. 

SODIUM   CINNAMATE     C6H5CH:CHCOONa. 

100  gms.  H2O  dissolve  9.1  gms.  sodium  cinnamate  at  15.20°. 

100  cc.  90%  alcohol  dissolve  0.625  Sm-  at  15-20°.  (Squire  and  Caines,  1905.) 

SODIUM   CITRATE  (CH2)2COH(COONa)8.5iH2O. 

SOLUBILITY  IN  AQUEOUS  ETHYL  ALCOHOL  AT  25°. 

(Seidell,  1910.) 


Wt.  Per  cent               •,    nf          Gms.  C6H5O7Na3.-     Wt.  Per  cent 
QH5OH  in              c  *  c  i       S5H2O  per  100  Gms.      QHsOH  in 
Solvent.                                           Sat.  Sol.                 Solvent. 

d2Bo{         Gms.C6H5C 

0 

1.276 

48.1 

40 

o-953 

4-5 

10 

I  .190 

37-4 

50 

0.918 

1-4 

20 

1.  100 

25 

60 

0.892 

0.3 

30 

1.  006 

ii.  8 

100 

0.789 

0 

Data  for  equilibrium  in  the  system  sodium  hydroxide,  citric  acid,  phosphoric 
acid  and  water  at  20°  are  given  by  Pratolongo  (1913). 

The  author  fails  to  describe  clearly  the  terms  in  which  the  results  are  expressed, 
consequently  their  exact  meaning  is  not  clear. 

SODIUM  (Ferro)  CYANIDE  Na4Fe(CN)6. 

SOLUBILITY  IN  WATER. 

(Conroy,  1898.) 

t°.  20°.  42°.  80°.  98-5°. 

Gms.  Na4Fe(CN)e  per  100  gms.  H^O       17.9      30  .  2      59  .  2      63 

SODIUM  FLUORIDE  NaF. 

100  gms.  sat.  aq.  solution  contain  4.3  gms.  NaF  at  18°.  Sp.  Gr.  of  solution  = 
1.044.  (Mylius  and  Funk,  1897.) 

SOLUBILITY  OF  SODIUM  FLUORIDE  IN  AQUEOUS  SOLUTIONS  OF  HYDRO- 
FLUORIC ACID  AT  21°. 

(Ditte,  1896.) 
Gms.  per  1000  Gms.  H2O.  Gms.  per  1000  Gms.  H20. 


o     HF 

4i 

.7  NaF 

83.8 

HF 

22.9  NaF 

10 

(i 

4i 

-4 

1C 

129.7 

tt 

23.8 

(( 

45-8 

tt 

22 

•5 

(I 

596.4 

tt 

48.8 

(( 

56.5 

a 

22 

-7 

ft 

777-4 

it 

81.7 

It 

FUSION-POINT  DATA  (Solubility,  see  footnote,  p.  i)  ARE  GIVEN  FOR  THE 
FOLLOWING  MIXTURES. 

NaF  +  FeF3.  (Puschin  and  Baskov,  1913-) 

"     +ZnF3. 

+  Nal.  (Ruff  and  Plato,  1903.) 

+  NaOH.  (Scarpa,  1915.) 

+  Na2SO4.  (Wolters,  1910.) 

SODIUM  FLUOSILICATE  Na2SiF6. 

100  gms.  H2O  dissolve  0.65  gm.  at  17.5°,  and  2.45  gms.  at  100°.       (Stolba,  1872.) 


653 


SODIUM  FORMATE 


SODIUM  FORMATE  HCOONa. 


SOLUBILITY  IN  WATER. 


(Groschuff,  1903.) 


—  20 

O 

+  15 

18 

18 

21 
23 


Gms.  Mols. 

HCOONa  HCOONa 

per  ioo  Gms  per  ioo  Mols. 
Solution. 

22.80 


30-47 
41.88 
44.92 

44-73 
46.86 
48.22 


H20. 

7.82 

ii. 6 
19.1 

21.6 

21.4 

23-3 
24.65 


Solid 
Phase. 


HCOONa.3H2O 


HCOONa.2H2O 


Gms. 
HCOONa 

Mols. 
HCOONa 

Solid 

"      per  ioo  Gms.  per  ioo  Mols 

Phase. 

Solution. 

H20. 

25- 

5    50-53 

27.0 

HCOONa.2H30 

18 

49.22 

25-65 

HCOONa 

29 

50-44 

26.9 

" 

54 

53-8o 

30.8 

M 

74- 

5    56-82 

34-8 

44 

ioo. 

5    6l-54 

42-35 

44 

123 

66.20 

44 

Sp.  Gr.  of  the  saturated  solution  of  the  dihydrate  at  18°  =  1.317. 

SOLUBILITY  OF  SODIUM  ACID  FORMATE  (EXPRESSED  AS  NEUTRAL 
SALT)  IN  AQUEOUS  SOLUTIONS  OF  FORMIC  ACID. 

(Groschuff.) 


Gms.  Mols. 

to         HCOONa  HCOONa 

'    per  ioo  Gms.  per  ioo  Mols- 
Solution.          H2O. 

o        22.35      T9-5 

25.5       29.62         28.45 
66.5      41.08         47-1 


Solid 
Phase. 

HCOONa.HCOOH 


Gms.  Mols. 

to       HCOONa    HCOONa         Solid 
'    per  ioo  Gms.  per  ioo  Mols.    Phase. 
Solution.        'H2O. 


45-5 

70 
85 


38.8S 
41.27 

43-09 


HCOONa 


47-5 
51-2 


SODIUM   GLYCEROPHOSPHATE  (Disodium)  OP(OC3H7O2)(ONa)2.5H2O. 

ioo  gms.  sat.  solution  in  H2O  contain  27.38  gms.  of  the  anhydrous  salt  at  18°. 

(Rogier  and  Fiore,  1913.) 

SODIUM  HYDROXIDE  NaOH. 

SOLUBILITY  IN  WATER. 

(Pickering,  1893;  Mylius  and  Funk  (Dietz) 


Gms.  NaOH 
t°.           per  ioo  Gms. 

Solution 

,    Water. 

-  7-8 

8.0 

8-7 

—  20 

16.0 

19.1 

-28 

19.0 

23-5 

-24 

22.2 

28.5 

-17.7 

24-5 

.32-5 

0 

29.6 

42  .0 

+  5 

32.2 

47-5 

10 

34-o 

51  .5 

15.5 

38-9 

63-53 

5 

45-5 

83-5 

12 

50-7 

103.0 

Ice 


Solid 

Phase. 


aOH.7H2O 
NaOH.7H2O  +  NaOH-sH2O 
NaOH.5H2O  +  NaOH4H2O  a 
NaOH.4H2O  a 

NaOH.4H2O  a  +  NaOH3iH2O 
NaOH.3iH2O 

f.  pt. 
NaOH.s  JHjsO  -f  NaOH-zH^ 


Dietz) 

,  1900.) 

Gms. 

NaOH 

^o.         per  ioo  Gms. 

Solid 
Phase. 

Solution, 

.  Water.  " 

20 

52.2 

IOO 

NaOH-HaO 

30 

54-3 

1  19 

44 

40 

56.3 

129 

M 

50 

59-2 

145 

M 

60 

63-5 

174 

M 

64. 

369.0 

222-3 

"  f  .  Pt. 

6l. 

874.2 

288 

NaOH.H2O 
H-NaOH 

80 

75-8 

3r3 

NaOH  (?) 

no 

78.5 

365 

" 

192 

83-9 

52i 

M 

Sp.  Gr.  of  sat.  solution  at  18°  =  1.539. 

For  determinations  of  the  Sp.  Gr.  of  sodium  hydroxide  solution,  see  Kohlrausch, 
1879;  Wegscheider  and  Walter,  1905. 

ioo  gms.  of  the  sat.  solution  in  water  contain  46.36  gms.  NaOH  at  15°. 

(de  Forcrand, 


SODIUM  HYDROXIDE 


654 


1000  gms.  liquid  ammonia  dissolve  0.0025  Sm-  NaOH  at  —40°. 

(Skossareswky  and  Tchitchinadze,  1916.) 

Data  for  equilibrium  in  the  system  sodium  hydroxide,  resorcinol  and  water  at 
30°  are  given  by  van  Meurs  (1916). 

Fusion-point  data  for  NaOH  +  Nal  are  given  by  Scarpa  (1915). 


SODIUM  IODATE  NaIO3. 

SOLUBILITY  IN  WATER. 
t°. 
Gms.  NalOs  per  100  gms. 


(Gay-Lussac;  Kremers,  i8s6a.) 


o  . 
2-5 


20°. 

9 


40 . 
15 


60°. 

21 


80°. 
27 


100  , 

34 


EQUILIBRIUM  IN  THE  SYSTEM  SODIUM  IODATE,  IODIC  ACID  AND  WATER  AT  30°. 


(Meerburg,  1905.) 


ioo  Gms.  Sat.  Sol 


HIO,. 

NaI03. 

•»        ouiiu  .rnase. 

O 

9.36 

NalOj.iiHjO 

1.98 

9-52 

" 

4-86 

10.22 

" 

5.86 

11.04 

« 

7.40 

II.  60 

"  unstable 

9-73 

14.73 

«        « 

6.70 

II.  21 

"  +Na2O.2l2< 

7.80 

10.30 

NaA2l»C 

9.15 

9 

" 

9-93 

8.71 

" 

Gms.  per  TOO  Gms.  Sat.  Sol. 


Solid  Phase. 


HIO3. 

NaI03. 

11.20 

7-54 

Na2O.2lA 

11.82 

7.20 

"  +NaIO3.2HIO3 

11.62 

5.65 

NaI03.2HIO, 

23.23 

3-69 

" 

32.68 

2.91 

" 

46.62 

2.67 

" 

55.48 

2.12 

« 

65.47 

1.83 

" 

76.19 

1.42 

+HIO, 

76.7Q 

0 

HIO, 

SODIUM   IODIDE  NaI.2H2O. 


SOLUBILITY  IN  WATER. 

(de  Coppet,  1883;  see  also  Etard,  1884;  and  Kremers,  i8.<;6a.) 


t° 

Grams  Nal 

per  ioo  Gm; 

5-       Solid 

Water. 

Solution. 

Phase. 

—  2O 

148.0 

59-7 

NaI.2H2O 

O 

I58-7 

61  .4 

it 

10 

168.6 

62.8 

* 

20 

178.7 

64.1 

M 

25 

184.2 

64.8 

H 

30 

190.3 

65.6 

" 

40 

205.0 

67.2 

" 

50 

227.8 

." 

t°. 

Grams  Nal 

per  ioo  Gms. 

Solid 
Phase. 

'  Water. 

Solution. 

60 

256.8 

72.0 

NaLaHaO 

65 

278.4 

73-6 

" 

67 

'     293 

74.6 

Nal 

70 

294 

74-6 

" 

80 

296 

74-7 

M 

IOO 

302 

75.1 

It 

120 

310 

75-6 

• 

140 

32I 

76.3 

« 

The  eutectic  mixture  of  Ice  +  NaI.sH2O  is  at  —31.5°  and  contains  about  39 

per  cent  Nal.  (Meyerhoffer,  1904.) 

The  tr.  pt.  for  NaI.sH2O  +  NaI.2H2O  is  at  —13.5  and  the  saturated  solution 
contains  60.2  gms.  Nal  per  100  gms.  (Panfiloff,  iSgaa.) 

The  tr.  pt.  for  NaI.2H2O  +  Nal  is  at  64.3°  and  the  saturated  solution  contains 
74.4  gms.  Nal  per  100  gms.  (Panfiloff,  1893.) 

100  gms.  HaO  dissolve  172.4  gms.  Nal  at  15°  and  the  d\6  of  the  sol.  is  1.8937. 

(Greenish,  1900.) 

100  gms.  sat.  solution  in  H2O  contain  65.5  gms.  Nal  at  30°.          (Cocheret,  1911.) 
SOLUBILITY  OF  SODIUM  IODIDE  IN  ALCOHOLS  AT  25°. 

(Turner  and  Bissett,  1913.) 

loo  gms.  Methyl  alcohol,  CH3  OH  dissolve  90.35  gms.  Nal. 
Ethyl  "       C2HBOH         "       46.02 

Propyl         "       C3H7OH        "       28.22 
Amyl  "       C6HUOH        "       16.30 


655 


SODIUM  IODIDE 


SOLUBILITY  OF  SODIUM  IODIDE  IN  AQUEOUS  ETHYL  ALCOHOL  AT  30°. 

(Cocheret,  1911.) 


Nal. 

C2H6OH.' 

ounu  jriioac. 

65.52 

O 

NaI.2H2O 

64 

3-42 

" 

54-2 

18.S 

ii 

48.8 

28.5 

« 

42.35 

41.7 

" 

Gms.  per  100  Cms.  Sat.  Sol. 

'~NaL CzH6OH". 

38.5  53-2 

37-49  55-37 

35.65  59.24 

33-24  61.78 

30.90  68.70 


Solid  Phase. 

NaI.2H20 

"  +  Nal 
Nal 


Data  are  also  given  for  the  solubility  of  mixtures  of  Nal  +  Na2CO3  in  aqueous 
ethyl  alcohol  at  30°. 

SOLUBILITY  OF  SODIUM  IODIDE  IN  ABSOLUTE  ETHYL  ALCOHOL  AT  TEMP- 
ERATURES UP  TO  THE  CRITICAL  POINT. 

(Tyrer,  igioa.) 


IO 

30 


IOO 


Gms.  Nal  per 
loo  Gms.  C2H6OH 

43-77 
44-25 
44-50 
45 

45-i 


f  o               Gms.  Nal  per 
loo  Gms.  QjHsOH. 

1  2O 

160 
180 

45-2 

45 
44-3 

2OO 
22O 
230 

42-3 
38.5 
36.2 

240 
250 

255 
260 

261.5* 


Gms.  Nal  per 
loo  Gms. 


32-7 
26.2 
21 

10.8 
8.6 


'  crit.  t.  of  solution. 


The  mixtures  were  placed  in  sealed  glass  tubes  which  were  heated  in  a  specially 
constructed,  electrically  heated  air  bath.  The  temperature  at  which  the  last 
trace  of  salt  just  dissolved  was  determined  in  each  case.  The  experiments  were 
made  with  very  great  care.  Results  are  also  given  for  the  solubility  of  sodium 
iodide  in  the  vapor  of  ethyl  alcohol  above  the  critical  point. 

SOLUBILITY  OF  SODIUM  IODIDE  IN  MIXTURES  OF  ALCOHOLS  AT  25°. 

(Herz  and  Kuhn,  1908.) 

In  CHsOH  +  C2H6OH.      In  CH3OH  +  C3H7OH.      In  C2H6OH  + 


Per  cent 

d     of 

Gms.  Nal 

Per  cent 

A  -  of 

Gms 

Nal 

Per  cent 

dapoi 

Gms.  Nal 

CH3OH  in 
Mixture. 

.3.5  Ui> 

Sat.  Sol. 

per  100  cc. 
Sat.  Sol. 

C3H7OHin    ( 

Mixture.       • 

U2A  Wi 

sat.  Sol. 

peri 
Sat. 

30  CC. 

Sol. 

C3H7OHin     ( 

Mixture. 

>at.  Sol. 

per  loo  cc. 
Sat.  Sol. 

0 

.0806 

35-15 

O 

•3250 

63 

22 

O 

.0806 

35-15 

4.37 

.1029 

37-68 

II.  II 

-2853 

58 

45 

8.1 

.0732 

34.60 

10.4 

.1123 

38.71 

23.8 

.2528 

54 

64 

17-85 

.0720 

34.05 

41.02 

.1742 

45.98 

65-2 

.1387 

40 

71 

56.6 

.0276 

28.41 

80.69 

.2741 

57-44 

91.8 

.0420 

29 

14 

88.6 

.0130 

26.13 

84.77 

.2886 

58.92 

93-75 

.0178 

26 

49 

91.  2 

.0104 

25.88 

91.25 

-3056 

61.10 

IOO                 « 

>.9968 

24 

ii 

95-2       i 

[.OO2O 

24.74 

IOO 

.3250 

63.22 

IOO              < 

>.9968 

24.11 

SOLUBILITY  OF  SODIUM  IODIDE  IN  SEVERAL  SOLVENTS. 

(At  22.5°,  de  Bruyn,  1892;  at  ord.  temp.  Rohland,  1898;  Walden,  1906.) 


Solvent. 


Gms.  Nal 

per  loo  Gms. 

Solvent. 


Solvent. 


Gms.  Nal  per  100  cc. 
Sat.  Solution. 


Absolute  Ethyl  Alcohol       22.5  43 .  i 

Ethyl  Alcohol,  d\5  =  0.810  ord.  temp.  58. 8 

Absolute  Methyl  Alcohol    22.5  77 . 7 

Methyl  Alcohol,  d\$  =  0.799  ord.  temp.  83 . 3 

Propyl  Alcohol,  d^=  0.816  ord.  temp.  26.3 


at  o°.        at  25°. 

Acetonitrile  2  2 . 09  1 8 . 43 
Propionitrile  9.09  6.23 
Nitro  Methane  0.34  0.48 
Acetone  very  soluble 

Furfural  ...       25.10 


SODIUM  IODIDE 


656 


SOLUBILITY  OF  SODIUM  IODIDE  IN  ACETAMIDE. 

.  (Menschutkin,  1908.) 


Gms.  per  100  Gms. 
Sat.  Sol. 


Solid  Phase; 


NaI.2CHr  _  NaT 
CONH2     -  NaL 
82     m.pt.ofpureacetamide  CHsCONHj 


78 

9-5 

5-32 

74 

18 

10.08 

70 

25-5 

14 

66 

3i-9 

17.86 

62 

37-3 

20.9 

58 

41.9 

23-44 

54 

46.1 

25-8 

50 

50 

28 

46 

53-7 

30.1 

41-5 

57-7 

32-3 

+NaI.2CH3CONH2 


Gms.  per  100  Gms. 
t°.                Sat.  Sol. 

Solid  Phase. 

NaI.2CHr 
CONH2 

=  NaI. 

50 

59 

33 

NaI.2CH3CONH, 

60 

60.S 

33-9 

" 

70 

62.2 

34-8 

" 

80 

64.2 

35-9 

« 

90 

66.5 

37-2 

« 

IOO 

69.2 

38.7 

" 

no 

72.6 

40.6 

« 

1  20 

78.7 

44 

« 

125 

84.7 

47-4 

"  +NaI 

150 

85.1 

47-7 

Nal 

175 

85.5 

47-9 

" 

loo  cc.  anhydrous  hydrazine  dissolve  64  gms.  Nal  at  room  temp. 

(Welsh  and  Broderson,  1915.) 

SODIUM  IODOMERCURATE 

A  saturated  solution  at  24.75°,  prepared  by  adding  Nal  and  HgI2  in  excess  to 
water,  contained  4.59%  Na,  25%  Hg,  58.25%  I  and  12.2%  H2O,  corresponding 
to  0.20  mol.  alkali,  0.12  mol.  Hg  and  0.45  mol.  I.  (Duboin,  1905.) 


SODIUM  MOLYBDATE  Na2MoO4. 

SOLUBILITY  IN  WATER. 

(Funk,  igooa.) 

Gms. 

Mols. 

Gms. 

t°. 

Na2MoO4 
per  loo  Gms. 
Solution. 

Na2MoO4 
per  loo 
Mols.  H2O. 

Solid  Phase.              t°. 

Na2MoO4 
per  loo  Gm 
Solution. 

o 

30-63 

3-86 

Na2MoO4.ioH2O        15-5 

39.27 

4 

33.83 

4-47 

18 

39-40 

6 

35.58 

4-83 

32 

39.82 

9 

38.16 

5-39 

"               5z-5 

41.27 

10 

39-28 

5-65 

Na2MoO4.2H2O        IOO 

45-57 

Mols. 


&»»»-"• 


lols.  H2O. 
5.65 
5.70 
5.78 
6.14 
7-32 


d  of  the  sat.  sol.  at  18°  is  1.437. 


100  gms.  H2O  dissolve  3.878  gms.  sodium  trimolybdate,  Na2Mo3Oi0,  at  20°,  and 
13-7  gms.  at  100°.  lUffik,  1867.) 

i  oo  cc.H2O  dissolve  28.39  gms.  Na2O.4MoO3.6H2Oat2i°,(fj5  =  1.47.  (Wempe,  1912.) 
Fusion-point  data  for  Na2MoO4  +  Na2WO4  and  Na2MoO4  +  NazSO4  are  given 
by  Boeke  (1907). 

SODIUM  NITRATE  NaNO3. 

SOLUBILITY  IN  WATER. 

(Mulder;  Berkeley,  1904;  see  also  Ditte,  1875;  Maumee,  1864;  Etard,  1894.) 


Gms. 

NaNO3per  looGms.     Mols.  per 

t° 

Gms.  NaNOj  per  100  Gms. 

Mols.  per 

Solution. 

Water. 

Liter. 

I      . 

Solution. 

Water. 

Liter. 

O 

42 

.2 

72. 

9-  73     * 

6.7I* 

80 

59- 

7 

148 

-I48.    * 

10-35* 

IO 

44 

•7 

80. 

8-  80.5 

7.l6 

IOO 

64- 

3 

180 

-175.8 

II-30 

20 

46 

•7 

87. 

5-88 

7.60 

1  2O 

68. 

6 

218 

-208.  8f 

I2.22f 

25 

47 

.6 

91 

-  92 

7.8o 

180 

78. 

I 

356. 

7 

30 

48 

-7 

94- 

9-  96.2 

8.06 

220 

83. 

5 

506 

40 

50 

•5 

IO2 

-104.9 

8.51 

225 

91. 

5 

1076 

50 

52 

.8 

112 

-114 

8-97 

3!3t 

IOO 

oo 

00 

54 

•9 

122 

-124 

9.42 

* 

Berkeley. 

T  at  119°. 

J  m.pt. 

657 


SODIUM  NITRATE 


SOLUBILITY  OF  SODIUM  NITRATE  IN  AQUEOUS  AMMONIA  SOLUTIONS  AT  15°. 

(Fedotieff  and  Koltunoff,  1914.) 


In  Aqueous  NH3. 


In  Aqueous  NH3  +  NH4NO3. 


duoi 
Sat  Sol. 

I.2S3 

1-233 
I. 212 


Cms.  per  100  Gms.  H2O. 


NH3. 

13.87 
17.28 
20.38 


NaNO3. 
75.03 
73-99 
73.18 


d15of 
Sat.  Sol. 

Gms 

.  per  100  Gms. 

H20. 

NH3. 

NHUNO-,. 

NaNO,. 

1.324 
1-330 

12.91 
16.97 

83.51 
128.9 

74.10 
69.40 

SOLUBILITY  OF  SODIUM  NITRATE  IN  AQUEOUS  SOLUTIONS  OF  NITRIC  ACID  AT  o°. 

(Engel,  1887;  see  also  Schultz,  1860.) 


valents  per  10  cc.  Solution.            SD.  Gr.  of 

Grams  per  TOO  cc.  Solut 

NaNO3. 

HNO3. 

NaNO3. 

HNO3. 

66.4 

0 

-341 

56.5 

O-OO 

63-7 

2-65 

•338 

54-2 

1.67 

60.5 

5-7 

•331 

51.48 

3-59 

56-9 

8.8 

.324 

48.42 

5-55 

52-75 

12-57 

.312 

44.88 

7.92 

48.7 

16.9 

•308 

41.44 

10.65 

39-5 

27.0 

.291 

33  -61 

17.02 

35-1 

32-25 

.285 

29.86 

20.33 

3i-i 

37-25 

.282 

26.46 

23.48 

23-5 

48.0 

.276 

20.  o 

30.26 

18.0 

57-25 

.276 

*5-32 

36.09 

12.9 

71.0 

.291 

10.97 

44.76 

SOLUBILITY  OF  MIXTURES  OF  SODIUM  NITRATE  AND  POTASSIUM  NITRATE 
IN  WATER  AT  20°. 

(Carnelly  and  Thomson,  1888.) 


Per  cent 
NaNO3  in 
Mixtures 

Gms.  per  100  Gms. 
H20. 

Used. 

NaN03. 

KN03. 

100 

86.8 

0 

90 

96.4 

13.2 

80 

98.0 

38.5 

60 

90.0 

47-6 

50 

66.0 

40.0 

Per  cent 
NaNO3  in 
Mixtures 

Gms.  per  100 
H20. 

Gms. 

Used. 

NaN03. 

KNO3. 

45-7 

53-3 

34.7 

40 

45  -6 

35-5 

20 

20.8 

33-3 

10 

9-4 

31-5 

O 

o.o 

33-6 

100  gms.  H2O  dissolve  24.9  gms.  NaCl  +  53-6  gms.  NaNO3  at  20°. 

(Rudorff,  1873;  Karsten;  Nicol,  1891.) 


-UBILITY 

OF  SODIUM 

NITRATE  IN  AQUEOUS 

SOLUTIONS  OF  SODIUM 

HYDROXIDE  AT  o°. 

(Engel,  1891.) 

Milligram  Mols.  per  10 
cc.  Solution. 

Sp.  Gr. 
of 

Grams  per  100  cc. 

Solution. 

Na20. 

NaN03. 

Solutions. 

NaOH. 

NaNO3. 

O-O 

66.4 

I-34I 

o.o 

56-50 

2.875 

62-5 

I-338 

2.30 

53-19 

6.1 

57-15 

1-333 

4.89 

48.63 

12-75 

47-5 

•327 

IO.2I 

40.42 

26.0 

29-5 

-326 

20.83 

25.10 

39-o 

17-5 

•332 

3I-25 

14-89 

45-88 

I3-I9 

•356 

36.76 

II  .22 

60.88 

6.05 

.401 

48-75 

5-15 

SODIUM  NITRATE 


658 


Data  for  equilibrium  in  the  system  sodium  nitrate,  sodium  sulfate  and  water  at 
10°,  20°,  25°,  30°,  34°  and  35°  are  given  by  Massink  (1916,  1917). 


SOLUBILITY  OF  SODIUM  NITRATE  IN  AQUEOUS  SOLUTIONS  OF  SODIUM 
THIOSULFATE. 

(Kremann  and  Rodemund,  1914.) 

Results  at  9°. 


Cms.  per  100  Gms. 
Sat.  Sol. 


NaNO3. 

33-31 

22.57 
4.22 


Na2S203. 
12.26 
23-4I 

34-77 


Solid  Phase. 

NaN03 

"      +Na2S203.SH20 
NaaSA.53 


Results  at  25°. 

Gms.  per  100  Gms. 
Sat.  Sol. 

Solid  Phase. 

NaNO3. 

Na2S2O3. 

35-42 

12.72 

NaN03 

25.40 
19.90 

18.02 

24.25 
3I.8I 
32.83 

"      +Na2S203.SHzO 
Na2S203.sH20 

4-33 

40.50 

" 

SOLUBILITY  OF  SODIUM  NITRATE  IN  ALCOHOLS. 

100  gins.  abs.  methyl  alcohol  dissolve  0.41  gm.  NaNO3  at  25°. 
100  gms.  abs.  ethyl  alcohol  dissolve  0.036  gm.  NaNO3  at  25°. 


(de  Bruyn,  1892.) 


SOLUBILITY  OF  SODIUM  NITRATE  IN  AQUEOUS  ETHYL  ALCOHOL  AT 
DIFFERENT  TEMPERATURES. 

(Bodlander,  1891;  Taylor,  1897;  Bathrick,  1896.) 


Results  at  13°  (B.). 

Sn  Or  of           Gms.  per  100  cc.  Solution. 

Results  at  16.5°  (B.). 

So.Gr.of       Gms.  per  100  cc.  Solution. 

Solutions. 

QsH6OH. 

H20. 

NaNO3. 

Solutions. 

C6H5OH. 

H2O. 

NaNO3. 

1.3700 

O-O 

75 

•34 

6l 

.66 

I 

3745 

o.o 

75 

•25 

62  -2O 

*-3395 

3-08 

73 

•53 

57 

•34 

j 

,3162 

6.16 

70 

.82 

54-64 

1.3120 

6.01 

7i 

.81 

53 

•39 

j 

.2576 

II  .60 

68 

.10 

46.06 

1.2845 

8.30 

70 

•85 

49 

•3o 

I 

.2140 

16.49 

65 

.04 

39-87 

1.2580 

10.91 

69 

•47 

45 

.42 

j 

.1615 

22.17 

61 

-67 

32-3I 

1-2325 

13-77 

67 

.12 

42 

•36 

j 

•0855 

32.22 

S2 

.92 

23-4I 

I.2OIO 

16.46 

66 

.16 

37 

.48 

I 

•0558 

37-23 

48 

•50 

19.85 

I 

.0050 

43-98 

42 

.78 

13-74 

0 

.9420 

52.60 

32 

•13 

9-47 

0 

.9030 

6o.OO 

25 

•65 

4-65 

0 

.8610 

63.16 

21 

•31 

1.63 

Results  at  30°  (T.). 


Wt.  per  cent 
Alcohol  in 

Gms.  NaNO3 
per  100  Gms. 

Solvent. 

Solution. 

Water- 

0 

49-10 

96.45 

5 

46.41 

9I-I5 

10 

43-50 

85-55 

20 

37-42 

74-75 

30 

3i-3i 

65.10 

40 

25.14 

55-95 

50 

18.94 

46.75 

60 

12.97 

37-25 

70 

7.81 

28.25 

90 

1.  21 

12.25 

Results  at  40°  (Bathrick). 

Gms.  NaNOs 
per  100  Gms. 
Aq.  Alcohol. 


Wt. 

"per  cent 
AlcohoL 

O 

8.22 
17.4 
26.O 
36.0 
42.8 

55-3 
65-1 
77-o 
87.2 


104-5 
90.8 

73-3 
61 

48 
40.6 

27 
18 

9-4 
4.2 


659 


SODIUM  NITRATE 


SOLUBILITY  OF  SODIUM  NITRATE  IN  AQUEOUS  ALCOHOL  AT  25°. 

(Armstrong  and  Eyre,  1910-11.) 


Solvent. 


Mols.  C2H5OH 
per  1000  Gms.  HjO. 

O 

0.25 

0.50 

I 
2 


Gms.  C2H6OH 
per  1000  Gms.  H2O. 

O 


23.03 
46.06 
Q2.I2 


Gms.  NaNO, 

per  loo  Gms. 

Sat.  Sol. 

47-93 
47.32 
46.73 

45-43 
43-04 


SOLUBILITY  OF  SODIUM  NITRATE  IN  AQUEOUS  SOLUTIONS  OF  ACETONE. 


Results  at  30°. 
(Taylor,  1897.) 

Wt.  per  cent 
Acetone  in 
Solvent. 

0 

5 

Gms.  NaNO3 
per  ioo  Gms» 

Solution. 

49-10 
46.96 

Water. 

96.45 
93.20 

9.09 

20 

45-11 
40.10 

90.40 
83.70 

3° 
40 

60 

29.80 

24-34 

77-20 

70-75 
64.40 

59-95 

70 
80 

00 

7.10 

I.Q8 

50-50 
38.20 
20.20 

Results  at  40°. 

(Bathrick, 

1896.) 

Wt.               Gms.  NaNOs 

per  cent             p 

er  ioo  Gms. 

Acetone.             A 

LQ.  Acetone. 

o.o 

105 

8.47 

91.2 

16.8 

78-3 

25.2 

66.4 

34-3 

57-9 

44.1 

46.2 

53-9 

32-8 

64.8 

23.0 

76.0 

10.8 

87.6 

3-2 

IOO  gms.  hydroxylamine  dissolve  13.1  gms.  NaNO3  at  17-18°.      (de  Bruyn,  1892.) 
100  cc.  anhydrous  hydrazine  dissolve  100  gms.  NaNO3  at  room  temp. 

(Welsh  and  Broderson,  1915.) 

Fusion-point  data  for  NaNO3  +  NaNOa  are  given  by  Bruni  and  Meneghini 
(1909,  1910). 

Results  for  NaNO3  +  SrNO3  +  KNO3  are  given  by  Harkins  and  Clark  (1915) 
and  results  for  NaNO3  +  T1NO3  by  van  Eyk  (1905). 


SODIUM  NITRITE 


NaN02. 

SOLUBILITY  IN  WATER. 

(Oswald,  1912,  1914.) 


Gms.  NaNO2 
loo  Gms.  Sat. 


4-5 
9 
12 


-12.5 


9.1 

23.8 

29.6 

i5.5Eutec.  39.7 
8  40.8 

o  41-9 

43-8 


Solid  Phase. 
Ice 


+NaNO, 
NaNOj 


10 

20 


45.8  (d=  1.3585)  " 


30 
40 

52 
65 

81 

92 

103 

128 


Gms.  NaNO2  per  c  ,• ,  p«  aci 
loo  Gms.  Sat!  Sol.  Solld  Phase' 


47-8 

49-6 

51.4 
54.6 

57.9 

59-7 
62.6 
68.7 


NaNOj 


(Divers,  1899.) 


ioo  gms.  H2O  dissolve  83.3  gms.  NaNO2  at  15°. 
100  gms.  H2O  dissolve  83.25  gms.  NaNO2  at  15°. 

(v.  Niementowski  and  v.  Roszkowski,  1897.) 
ioo  gms.  H2O  dissolve  73.5  gms.  NaNO2  at  15°,  di6  =  1.3476. 

(Greenish  and  Smith,  1901.) 


SODIUM  NITRITE  660 

SOLUBILITY  OF  SODIUM  NITRITE  IN  AQUEOUS  SOLUTIONS  OF  SODIUM 
NITRATE  AND  VICE  VERSA  AT  SEVERAL  TEMPERATURES. 

(Oswald,  1912,  1914.) 


Results  at  o°. 

Results  at  21°. 

Results  at  52°. 

Results  at  103°. 

jms.  per  100  Gms.  H2O. 

Gms.  per  100  Gms.  H2O. 

Gms.  per  100  Gms.  H2O. 

Gms.  per  100  Gms.  H2O. 

'NaN02. 

NaN03.  ' 

'  NaNO2. 

NaNOj. 

NaNO2. 

NaNOj. 

NaNO2. 

NaNOa.  ' 

73 

0 

84.75 

0 

108.8 

0 

166 

O 

68 

19 

81.1 

9.6 

104.3 

20.6 

153-3 

33-2 

67 

36.3 

79-7 

23-5 

99-5 

43-2 

148.8 

58.8 

64.9 

41.7* 

73-8 

50.8 

98.8 

82      * 

142.4 

116    * 

50-3 

46.8 

54.5* 

65.2 

88 

100 

126.8 

30.2 

55-4 

64.2 

56.7 

44.2 

92.9 

60.  i 

142.9 

0 

74.2 

46.8 

62.8 

27.2 

101.4 

0 

181.2 

21.6 

74-7 

14.7 

109 

o 

89.3 

0 

118 

*  Both  salts  in  solid  phase. 

Similar  results  are  also  given  for  18°,  65°,  81°  and  92°. 

100  gms.  H2O,  simultaneously  saturated  with  both  salts,  contain  53.9  gms. 
NaNO2  +  1 1. 8  gms.  Na2SO4  at  16°.  (Oswald,  1914.) 

SOLUBILITY  OF  MIXTURES  OF  SODIUM  NITRITE  AND  SILVER  NITRITE  IN  WATER 
AT  14°  AND  AT  22°.     (See  also  p.  620.) 

(Oswald,  1912,  1914.) 

Results  at  14°.  Results  at  22°. 

Gms.  per  100  Gms.  H2O.  Gms.  per  100  Gms.  H2O. 

tfaNOT AiNO;.  tfaNOT AiN02.  SoMPhaaem  Each  Case. 

55  15.2  58.3  21.5  AgN02+Na2Ag2(N02)4.H20 

74-7  II- 3  78.3  13.4  NaNQ,+NagAg8(NOj)4.H,0 

100  gms.  abs.  methyl  alcohol  dissolve  4.43  gms.  NaNO2  at  19.5°. 

100  gms.  abs.  ethyl  alcohol  dissolve  0.31  gm.  NaNO2  at  19.5°.      (de  Bruyn,  1892.) 

SODIUM  RHODONITRITE  Na6Rh2(NO2)i2. 

100  gms.  H2O  dissolve  40  gms.  at  17°,  and  100  gms.  at  100°.  (Leidie,  1890.) 

SODIUM  OLEATE  C8Hi7CH:CH(CH2)7COONa. 

SOLUBILITY  IN  WATER  AND  AQUEOUS  BILE  SALTS. 

(Moore,  Wilson  and  Hutchinson,  1909.) 

c  i       i.  Gms.  Oleate  per 

Solvent-  100  Gms.  Sat.  Sol. 

Water  5 

Aq.  5%  Bile  Salts  7.6 

Aq.  5%  Bile  Salts  +  i%  Lecithin  n  .6 

SODIUM   OXALATE   Na2C2O4. 

SOLUBILITY  IN  WATER. 

(Souchay  and  Leussen,  1856;  Pohl,  1852.) 
t°.  15.5°.  21.8°.         f     100°. 

Gms.  Na2C2O4  per  100  gms.  H2O  3.22          3 . 74          6 .33 

100  gms.  sat.  solution  of  sodium  oxalate  in  water  contain  3.09  gms.  NajC2O4  at 

15°  and  4.28  gms.  at  50°.  (Colani,  1916.) 

loo  gms.  95%  formic  acid  dissolve  8.8  gms.  Na2C2C>4  at  19.3°.       (Aschan,  1913.) 


66i 


SODIUM   OXALATE 


SODIUM   OXALATE 

SOLUBILITY  OF  MIXTURES  OF  SODIUM  OXALATE  AND  OXALIC  ACID  IN 

WATER  AT  25°.     (Foote  and  Andrew,  1905.) 

Solid 
Phase. 


Gms.  per  100  Cms. 
Solution. 

Mols.  per  100  Mols. 
H2O. 

H2C204.         Na2C204". 

H2C204. 

Na2C204. 

10.20 

2.274 

10.50           0.83 

2.370 

0.130 

9.15            0.71 

2.032 

0.106 

6.88        0.86 

1-493 

0.125 

1.14        1.25 

0.234 

0.172 

0.47        3.20 

0.098 

o  .  446 

0.42        3.85 

0.090 

0.541 

3.60 

0.502 

HaC204.2H20  +  HNaC204.H20 


Double  Salt,  HNaC2O4.H2O 

HNaC2O4.H2O  +  Na^^ 
Na2C204 

SOLUBILITY  OF  MIXTURES  OF  SODIUM  OXALATE  AND  OTHER  SODIUM  SALTS 
IN  WATER  AT  15°  AND  AT  50°.     (Colani,  1916.) 


Gms.  per  100  Gms.  Sat.  Solution. 


i5 

0. 

027 

Na2C204 

+ 

26.28 

NaCl 

o. 

063 

H 

+ 

26.64 

H 

i5 

0. 

86 

" 

+ 

IO.26 

Na2S04 

0. 

22 

(( 

+ 

31-95 

tt 

15 

0. 

051 

" 

+ 

45.86 

NaN03 

5o 

o. 

047 

tt 

+ 

53-06 

u 

Solid  Phase. 


NajCA  +Na2SO4.ioH2O 

"       +Na2S04 


EQUILIBRIUM  IN  THE  SYSTEM  SODIUM  OXALATE,  URANYL  OXALATE  AND 
WATER  AT  15°  AND  50°.     (Colani,  1917.) 

Results  at  50°. 

Gms.  per  100  Gms. 

Sat.  Sol.  Solid  Phase. 


Gms.  per  100  Gms 
Sat.  Sol. 


Results  at  15°. 

Solid  Phase. 


Na2C2O4. 
3-09 
4-93 
I.  80' 
0.80 
O 


U02C204. 

o 

3.14 
5.01 

2.65 

0.47 


Na2C204 
"  +2.1.2.5 
2.1.2.5+2.4.5.11 
2.4.5-11  +U02C204.3H20 
U02C204.3H20 


Na2C204. 
4.28 

9-03 
4.62 
3-60 
I.OI 

o 


U02C204. 

o 

13.09 

12.33 

9.84 
3.58 

I 


"  +2.1.2.5 

2.1.2.5+2.2.3.5 

2.2.3.5+2.4.5.11 

2.4.5-1 1  +UO2C2O4.3H2O 
U02.C204.3H20 


2.1.2.5  =  Na2(U02)(C204)2.5H20,    2.2.3.5 
Na2(U02)4.(C204)5.iiH20. 


Na2(U02)2(C204)3.5H20,    2.4.5.11  = 


SODIUM  PALMITATE   CH3(CH2)14COONa. 

100  gms.  sat.  solution  in  H2O  contain  0.2  gm.  sodium  palmitate. 

100  gms.  sat.  solution  in  5%  aq.  bile  salts  contain  I  gm.  sodium  palmitate. 

ipo  gms.  sat.  solution  in  5%  aq.  bile  salts  +  i%  lecithin  contain  2.4  gms. 
sodium  palmitate.  (Moore,  Wilson  and  Hutchinson,  1909.) 


SOLUBILITY  OF  SODIUM  PALMITATE  IN  PALMITIC  ACID. 

Gms.  Na  Palmitate 

per  100  Gms. 

Solid  Phase  (Na  t°. 

Palmitate + 
Palmitic  Acid). 

0.7  71 

II. 12  72.9 

13-78  73-5 

16.36  76 

18.70  79.2 

26.55  82 


(Donnan  and  White,  1911.) 


60.2 
62 

64.4 
66.65 

67-75 
68.95 


Gms. 

Na  Palmitate 
per  zoo  Gms. 
Liquid  Phase, 

2-3 

4.96 

7.98 

12.28 

13.72 

15.56 


Gms. 

Na  Palmitate 
per  loo  Gms. 
Liquid  Phase. 

22.60 

28.65 

29.07 

30-7 

33.36 

36.02 


Gms.  Na  Palmitate 

per  100  Gms. 
Solid  Phase  (Na 

Palmitate + 
Palmitic  Acid). 

25.38 
35.05 
35-23 
35-9 

35-66 
39.64 


The  solid  phases  form  three  series  of  solid  solutions. 

A  special  apparatus  was  devised  for  preparing  the  saturated  solutions  and  filter- 
ing from  the  solid  phases. 


SODIUM   PHENOLATE 


662 


SODIUM  p  NITROPHENOL  C6H4.ONa(i).NO2(4). 

SOLUBILITY  IN  WATER  AND  IN  AQUEOUS  NORMAL  SOLUTIONS  OF  NON- 
ELECTROLYTES. 

(Goldschmidt,  1895.) 
Cms.  C6H4.ONa(i).NO2(4)  per  100  Cms.  Solution  in: 


*  . 

Water. 

Alcohol. 

Urea. 

Glycerine. 

Acetone. 

Propionitril. 

Acetonitril.   Urethane. 

23-7 

5-597 

5.6I5 

6.244 

6.188 

6. 

225 

6.257 

6 

.065 

6. 

520 

28.6 

6.721 

6.874 

7.489 

7.440 

7- 

498 

7-571 

7 

.328 

7- 

889 

30.6 

7.256 

. 

» 

33-6 

8.125 

8.318 

9-000 

9.025 

9- 

025 

9.066 

8 

.886 

9- 

507 

35-9 

8.851 

. 

•  . 

36.i 

8.883 

9.683 

9.688 

9- 

665 

9.911 

9 

.667 

10. 

248 

40.2 

9.881 

10.147 

10.666 

10.777 

10. 

695 

10.905 

10 

.667 

ii. 

379 

45-2 

".235 

11.513 

12.068 

12.229 

12. 

869 

So.  i 

12.730 

13.133 

13.555 

13.785 

. 

, 

The 

solid  phase  is  C6H4ONa.NO2.4H20 

below  36°,  and  C6H4ONa. 

NOt. 

2H2O 

above 

36°  in  each 

case. 

• 

SODIUM  PHOSPHATE  (Ortho)  Na3PO4.i2H2O. 

SOLUBILITY  IN  WATER. 

(Mulder). 

«               Gms.  per  100 
1  •               Gms.  H20. 

t°. 

Gms.  per  100 
Gms.  H2O. 

o               1.5 

25 

15.5 

10               4.1 

30 

2O 

20                   II 

40 

31 

50 

43 

60 

80 

IOO 


Gms.  per  100 
Gms.  H2O. 

55 
8l 

108 


SODIUM   Hydrogen  PHOSPHATE  Na2HPO4.i2H2O. 
SOLUBILITY  IN  WATER. 

(Shiomi,  1908;  Menzies  and  Humphrey,  1912.) 


Gms.  NajHPC 

)4 

t°. 

per  loo  Gms. 

Solid  Phase. 

H20. 

-0.43 

1.42 

Ice 

—  0.24 

0.70 

" 

—    O.5Eutec. 

.  .  . 

"+Na2HP04.i2H20 

+0.05' 

1.67 

Na2HPO4.i2H2O 

IO.26 

3-55(S) 

" 

IS-" 

5-23(8) 

" 

2O 

7.66 

" 

25 

12 

" 

30.21 

20.81(8) 

" 

30.76 

23.41(8) 

" 

32 

25.7 

" 

33.04 

30.88(8) 

M 

34 

33.8 

" 

35.2  tr.pt. 

'  "  +Na2HPO4.7H2O 

36.45     ' 

...  (S) 

«i 

37-27 

47.5i(S) 

NajHPO4.7H2O 

39.2 

51-8 

" 

45 

67.3 

47-23 

76.58(8) 

48.3tr.pt. 

48   " 

:::  (s)i 

50 

80.2  N 

55.17 

81.4  (S) 

60 

82.9 

70.26 

88.n(S) 

80 

92-4 

89.74 

102.87(8) 

90.2 

IOI.I 

95   tr.pt. 

.  .  . 

95.2  " 

...  (S) 

96.2 

104.6 

99.77 

102.15(8) 

105 

103.3 

1  20 

00.2 

per  loo  Gms.        Solid  Phase. 


NaaHPO4.7H2O 


NajHPO* 


Results  marked  (S)  by  Shiomi,  all  others  by  Menzies  and  Humphrey. 

100  gms.  H2O  dissolve  12.2  gms.  Na2HPO4  at  25°,  determined  by  refractometer. 

(Osaka,  1903-8.) 

IOO  gms.  H2O  dissolve  5.23  gms.  Na2HPO4at  15°,  6?i6=  1.049.  (Greenish  and  Smith,  1901.) 
loo  gms.  alcohol  of  </i6  =  0.941  dissolve  0.33  gm.  Na2HPO4  at  15.5°. 


663 

SODIUM   Dihydrogen  PHOSPHATE  NaH2PO4. 
SOLUBILITY  IN  WATER. 

(Imadsu,  1911-12.) 
Cms.  NaH2PO4 

Solid  Phase. 


NaH2P04.2H20 


SODIUM  PHOSPHATES 


t°.               per  100  Gms. 
H20. 

O.I 

57-86 

5 

63.82 

10 

69.87 

IS 

76.72 

20 

85.21 

25 

94.63 

30 

106.45 

35 

120-44 

40 

138.16 

40  .  8  tr.  pt. 

142.55 


+NaH2P04.H20 
NaH2PO4.H2O 


Gms.  NaH2PO4 
t°.             per  loo  Gms.        Solid  Phase. 

H20. 

45 

148  .  20 

NaH2P04.H,0 

50 

I58.6I 

" 

55 

170.85 

" 

57 

I75.8I 

.«• 

57-4tr. 

pt.      ... 

"  +NaH2Pl 

60 

179-33 

NaH2PO4 

65 

184.99 

" 

69 

190.24 

" 

80 

207  .  29 

" 

90 

225.31 

if 

99.1 

246.56 

" 

SODIUM  Acid  PHOSPHATE  NaH2PO4.H3PO4. 

SOLUBILITY  IN  WATER  AND  IN  ANHYDROUS  PHOSPHORIC  ACID,  DETERMINED 
BY  THE  SYNTHETIC  METHOD. 

(Parravano  and  Mieli,  1908.) 

Solubility  in  Water.  Solubility  in  H8PO8. 

'Gms.  Gms. 

NaH2PO4.- 

H3P04per 

100  Gms. 

Sat.  Sol. 

87.48    NaH2P04 
88.65        " 

91.47 

92.67 

95-79 
97-99 
100 


t°. 

Gms. 
NaH2P04.- 
H3PO4per 
100  Gms. 

Solid  Phase.      t°. 

Sat.  Sol. 

-  5-7 

20.77 

Ice           79.7 

-  7.9 

26.92 

85 

-11.4 

34-15 

IOI.7 

-38 

56.66 

104.5 

-34 

80.46 

NaH2P04    1  10 

81.82 

119 

51.7 

83.68 

126.5 

Solid  Phase.  t°. 

98.5 

III 

"+NaH2P04.H3P04  119 

NaH2PO4.H3PO4     122 

123 


NaH2P04.- 
H3PO4per 
loo  Gms. 
Sat.  Sol. 

52.72 


77-55 
81.71 
87.20 


m.  pt.  of  the  HaP04  =  40.6" 


Data  are  also  given  for  the  fusion  points  of  NaH2PO4  +  H3PO4. 
Fusion-point  data  for  mixtures  of  NaPOa  +  Na4P2O4  are  given  by  Parravano 
and  Calcagni  (1908,  1910.) 

EQUILIBRIUM  IN  THE  SYSTEM  SODIUM  HYDROXIDE,  PHOSPHORIC  ACID  AND 

WATER  AT  25°. 

(D'Ans  and  Schreiner,  igioa.) 


Mols.  per  1000  Gms.  Sol. 


Na. 

P04. 

13-32 

4.28 

0.040 

3-24 

0.183 

2.24 

0.752 

2-73 

1.  08 

3-48 

1.33 

2.62 

1.09 

1.56 

0.78 

2.38 

1.  60 

3.18 

2.24 

4-65 

3-55 

S-63 

3.87 

6.31 

4.63 

Solid  Phase. 

NaOH.H20 
NasPO4.i2H2O 


NasPO4.i2H2O+Na2HPO4.i2H2O 
Na2HP04.i2H20 


Na2HP04.7H20 


Na. 

P04. 

—  >       ouiiu  JT  uase. 

6.76 

4.88 

Na2HPO4.7H2O 

7-31 

5.55 

"  unstable 

6.76 

4.88 

"  +NatHPO4.2H2O 

6.19 

4.68 

NajHPO^HjO 

6.01 

4.67 

n 

5-i2 

4.36 

« 

4.81 

4.22 

a 

4.36 

4.08 

a 

4.06 

4-03 

« 

4.19 

4.38 

" 

4.32 

4.96 

u 

4.65 

5.89 

tt 

4.88 

6.40 

M 

SODIUM  PHOSPHATES 


664 


SODIUM   PyroPHOSPHATE   Na4P2O7.ioH2O. 

SOLUBILITY  IN  WATER, 

(Mulder;  Poggiale.) 


O 
10 

20 


Cms.  per 
100  Cms.  H2O. 

3-16 

3-95 
6.23 


25 
30 
40 

So 


Gins,  per 

loo  Cms.  H2O. 

8.14 

9-95 

13.50 
17.45 


60 
80 

IOO 


Cms.  per 
zoo  Cms.  H2O. 
21.83 
30.04 
40.26 


SODIUM   PyroPHOSPHATES. 

SOLUBILITY  IN  WATER. 

(Giran, 
Salt. 

Monosodium  Pyrophosphate 
Disodium  Pyrophosphate 
Trisodium  Pyrophosphate 


Formula. 

NaH3P207 

Na2H2P207.6H2O 

Na3HP207.6H2O 


'AO       Gms.  Anhydrous  Salt 
per  loo  cc.  Sat,  Sol. 

18  62.7 

18  14.95 

18  28.17 


SODIUM  PHOSPHITES 

SOLUBILITY  OF  SODIUM  PHOSPHITES,  ETC.,  IN  WATER. 


Salt. 

Formula. 

Gms.  Salt 
t°.     per  loo  Gms.           Authority. 
H,0. 

Hydrogen  Phosphite 

(NaH)HPO3.2iH2O  o 

56 

!(Amat.  —  Compt. 

tt 

tt 

10 

66 

rend.  106,  1351,  '88.) 

u 

" 

42 

*93 

Hypophosphate 

Na4P2O6.ioH20 

cold 

3- 

3  j 

Hydrogen  Hypophosphate 

Na3HP206.9H20 

? 

4 

5 

(Salzer  —  Liebig's 

Tri  Hydrogen 

u 

NaH3P2063H20 

cold 

6. 

7 

-/Vim*  2  1  if  Xf  o2./ 

Di  Hydrogen 
Di  Hydrogen 

u 
tt 

Na2H2P2O6.6H20 
Na2H2P2O6.6H2O 

cold 
b.  pt. 

2. 
20. 

«; 

0 

(Salzer  —  Liebig's 
Ann.  187,  331,  '77.) 

Hypophosphite 

(NaH)HP02.H2O 

25 

IOO. 

0 

(U.  S.  P.) 

Hypophosphite 

(NaH)HPO2.H2O 

b.  pt. 

830 

100  gms.  H2O  dissolve  108.7  gms.  anhydrous  sodium  hypophosphite  (NaH2PO2) 
at  15°,  dis  of  sat.  sol.  =  1.388.  (Greenish  and  Smith,  1901.) 

SODIUM   (Double)   PHOSPHATE,   FLUORIDE  Na3P04.NaF.i2H2O. 

IOO  gms.  water  dissolve  12  gms.  of  the  double  sodium  salt  at  25°,  and  57.5  gms. 
at  70°.    Sp.  Gr.  of  solution  at  25°  =  1.0329;  at  70°  =  1.1091.  (Briegleb,  1856.) 

SODIUM  PICRATE  C6H2(NO2)3.ONa.H2O. 

SOLUBILITY  IN  WATER  AND  IN  AQUEOUS  SOLUTIONS  AT  25°. 

(Fisher  and  Miloszewski,  1910.) 

IOO  cc.  H2O  dissolve  4.247  gms.  C6H2(NO2)3.ONa.H2O  at  25°. 

Solubility  in  Aq.  Gms>  C6H2(NO2)3.ONa.H2O  per  100  cc.  Aq.  Solution  of  Normality: 


Solution  of: 

O.OI. 

O.O2. 

0.04. 

0.066. 

O.IO. 

0.25. 

0.5. 

I. 

Na2C03 

4.159 

4.044 

3 

.807 

3- 

434 

3.187 

2 

.017 

I.I2O 

0.611 

NaCl 

4.189 

3.956 

•677 

3. 

335 

3.021 

I 

.678 

0.846 

0.410 

Na2S04 

4.246 

4.102 

3 

.879 

3- 

651 

3.195 

2 

.053 

I.I56 

0-552 

Na3PO4 

4.235 

4.051 

3 

.814 

3- 

562 

3.225 

2 

.219 

1.329 

0.705 

NaOH 

4.192 

4.048 

3 

.715 

3- 

339 

2.941 

X 

.781 

0.921 

0.371 

NaNO3 

4.154 

4.029 

3 

.710 

3- 

363 

3.041 

I 

-932 

0-943 

0.684 

NaBr 

4.190 

4.II7 

3 

.770 

3- 

384 

3.024 

I 

•777 

0.912 

0.499 

Data  for  the  solubility  of  sodium  picrate  and  the  sodium  salts  of  other  nitro- 
phenols  in  aqueous  alcohol  and  acetone  solutions  at  25°  are  given  by  Fisher  (1914). 


Wt.  Per  cent 
CzHjOH  in 
Solvent. 

dx  of 
Sat.  Sol. 

Gms.  CeB^OH- 
COONa  per  100 
Gms.  Sat.  Sol. 

Wt.  Per  cent 
QH6OH  in 
Solvent. 

da,  of 
Sat.  Sol. 

O 

1.256 

53-56 

60 

1.  066 

10 

1-235 

52.10 

70 

1.016 

20 

1.205 

50.20 

80 

0-957 

30 

1.176 

48 

90 

0.885 

40 

1.142 

45-50 

92.3 

0.864 

50 

1.106 

42.20 

IOO 

0.805 

66s  SODIUM   SALICYLATE 

SODIUM  SALICYLATE  C6H4.OH. COONa. 

SOLUBILITY  IN  AQUEOUS  ETHYL  ALCOHOL  AT  25°.    (Seideii,  1909, 1910.) 

Gms.  CgEUOH- 
COONa  per  100 
Gms.  Sat.  Sol. 

38.40 

33 
25 
15 

12 
3-82 

100  gms.  sat.  solution  in  water  contain  51.8  gms.  C6H4OHCOONa  at  15°  and 
du  of  the  sat.  sol.  is  1.249.  (Greenish  and  Smith,  1901.)  See  also  last  line  of  first  table 
on  p.  590. 

100  gms.  propyl  alcohol  dissolve  1.16  gms.  C6H4OHCOONa  at  ord.  temp. 

(Schlamp,  1894.) 

Sodium  salicylate  distributes  itself  between  olive  oil  and  water  at  15°  in  the 
ratio  of  0.156  gm.  C6H4OHCOONa  per  100  cc.  oil  layer  and  1.444  gms.  per  100  cc. 
aqueous  layer.  (Harrass,  1903.) 

SODIUM  SELENATE  Na2SeO4.ioH2O. 

SOLUBILITY  IN  WATER.    (Funk,  igooa.) 

Gms.  Mols.  Gms.  Mols. 

to    Na2Se04per  Na2SeO4per  Solid  to  Na2SeO4  per  Na2SeO4  per       Solid 

100  Gms.  loo  Mols.  Phase.  100  Gms.       100  Mols.         Phase. 

Solution.  H2O.  Solution.  H^. 

O  11-74  I-26       NaaSeOi-ioHaO  35.2  45-47  7-94       NaaSeO* 

15  25.01  3.18  39.5  45.26  7.87 

18        29.00        3.90  50  44.49        7-63 

25-2    36-91        5-57  75  42-83        7.14 

27        39.18       6.13  100  42.14       6.93 

30       44.05        7.50 
Sp.  Gr.  of  saturated  solution  at  1 8°  =  1.315. 

SODIUM  [SILICATE   Na2SiO3.9H2O. 

SOLUBILITY  IN  AQUEOUS  SODIUM  HYDROXIDE  AND  SODIUM  CHLORIDE 

SOLUTIONS.       (Vesterberg,  1912.) 

Gms.  per  100  cc.  Sat.  Solution. 
Solvent.  t°.  dtt  of 


Sat.  Sol.         NaaO.          SiO2   =  NajSiOs.gHzO.     NaCl. 

Approx.  0.5  n  NaOH         17.5      1.129      6.942    5.419  =25.56 

NaCl  17.5      1.150      7.347    7.172        33.83        2.297 

^Saturated  NaCl  Solution  19          1.258      4.563    4.376        20.64      27.91 

~  Solid  phase  Na2SiO3.9H2O  in  each  case. 

Fusion-point  data  for  Na2SiO3  +  SrSiO3  are  given  by  Wallace  (1909).     Results 
for  Na2SiO3  +  Na2WO4  are  given  by  van  Klooster  (1910-11). 

SODIUM   STANNATE  Na2SnO3.3H2O. 

100  gms.  H2O  dissolve  67.4  gms.  at  o°,  and  61.3  gms.  at  20°.     Sp.  Gr.  of  solution 
at  0°  =  1.472;  at  20°  =  1.438.  COrdway,  1865.) 

SODIUM  SUCCINATE  (CH2)2(COONa)2.6H2O. 

SOLUBILITY  IN  WATER.      (Marshall  and  Bain,  1910.) 
Gms.  (CH2)r  Gms. 

• 


«••     per,  S°M  Phase. 

H20.  H20. 

O          21.45  (CH2)2(COONa)2.6H20  50  56.3         (CH2)2(COONa)2.6H2O 

I2.S      27.38  62.5        78.49 

2$          34.90  64.9        83.38  "  +(CH2)2(COONa), 

37-5     43.64  75  86.63      (CHMCOONa), 


SODIUM  SUCCINATES 


666 


o 

2-5 

25 

37-5 


SOLUBILITY  OF  SODIUM  HYDROGEN  SUCCINATE  IN  WATER. 

(Marshall  and  Bain,  1910.) 

Cms.  (CH^y 

(COOH)(COONa)    Solid  Phase, 
per  100  Cms.  H2O. 

NaHSu*.3H2O 


Cms.  (CH2)2- 
(COOH)(COONa) 


17-55 
27-93 
39.82 

60. 01 


Solid  Phase, 
per  loo  Cms.  H2O. 

38.7  63 . 99          NaHSu.3H2O  +NaHSu 

50  67.37  NaHSu 

62-5  76.15 

75  86 


EQUILIBRIUM  IN  THE  SYSTEM  SODIUM  SUCCINATE,  SUCCINIC  ACID  AND  WATER. 

(Marshall  and  Bain,  1910.) 


Results  at  o°. 


Gms.  per  too  Gms. 
Sat.  Sol. 


NaaSu. 

H2Su.' 

O 

2.68 

H2Su' 

3-23 

4-76 

" 

5.38 

5-83 

" 

8.27 

7.12 

"  4 

8.67 

6.27       Na] 

asu.3i 

9.68 

4-74 

« 

11.74 

3-49 

" 

15.62 

2-34 

« 

18.36 

1.90 

"  4 

18.07 

1.67 

Na, 

17.87 

0.94 

17.64 

Results  at 

50°. 

0 

19.27 

H2Su' 

5-95 

22.90 

" 

10*25 

25-33 

ii 

15.49 

28.73 

" 

19.65 

31-73 

" 

20.72 

26.51         NaHSu 

22.53 

18.44 

« 

25-53 

13.09 

* 

28.28 

9.46 

" 

30.48 

7.38 

ii 

37-33 

4.20 

36.85 

3-88 

Na, 

36.67 

2.66 

36.43 

0 

Solid  Phase. 


+NaHSu.3H2O 


+Na2Su.6H20 


+NaHSu 


+Na2Su.6H20 


'  The  following  double  and  triple  points  were  located : 


Results  at 

25°. 

Gms.  per  100  Gms. 

Sat.  Sol. 

Solid  Phase. 

NajSu. 

H2Su. 

0 

7.71 

H2Su 

3-68 

10.26 

" 

8.99 

13-35 

* 

12.64 

15-53 

" 

15.26 

16.90 

"    +NaHSu.3H,O 

15.97 

13  .  83       NaHSu.3H2O 

18.89 

8.41 

" 

22.71 

5-65 

" 

26.88 

4.08 

"  +Na2Su.6HaO 

26.50 

2.38 

Na2Su.6H2O 

26.11 

0.85 

" 

25.87 

O 

" 

Results  at 

75°. 

0 

37-64 

H2Su 

8.22 

40.38 

" 

13.14 

42.50 

" 

16.93 

44.38 

« 

19.56 

45-98 

"    4-NaHSu 

21.88 

35-6o 

NaHSu 

24.30 

26.82 

" 

29-45 

15.28 

" 

36.11 

7-79 

" 

41.26 

4-93 

" 

45-27 

4 

"   +Na2Su.H20 

45-36 

3-17 

NazSu.HaO 

45-93 

1.23 

" 

46.42 

0 

' 

34.9 
37-8 
38.7 
63.4 
64.9 


Gms.  per  100  Gms.  Sat.  Sol. 


5.6 

25.46 

16.44 
3.64 


30.8 
19.6 
22.47 
42.92 

45-43 


Solid  Phase. 

NaHSu.3H2O  +NaHSu  H-N^Sn. 
NaHSu.3H20  +NaHSu+H2Su 
NaHSu.3H2O+NaHSu 
Na,Su.6H2O+Na2Su.H2O4-NaHSu 


*In  the  above  tables  the  abbreviation  Su  is  used  for  (CH2)2(COO)2. 


667 


SODIUM   SULFATE 


SODIUM   SULFATE  Na2SO4. 


SOLUBILITY  IN  WATER. 

(Mulder;  Lowel,  1851;  Tilden  and  Shenstone,  1883;  Etard,  1894;  Funk,  igooa;  Berkeley,  1904.) 


Gms.  Na2SO4  per 
t°.                100  Gms.        j; 

Mols. 
fa2SO4pe: 

Solution. 

Water/ 

Liter  (B.; 

0 

4.76 

5-o 

0.31  : 

5 

6.0 

6.4 

10 

8-3 

9-0 

0.631 

15 

n.  8 

13-4 

20 

16.3 

19.4 

1.32 

25 

21.9 

28.0 

27 

•5     25.6 

34-o 

.  .  . 

30 

29.0 

40.8 

2.63 

31 

30.6 

44.0 

32 

32-3 

47-8 

32 

•75  33-6 

50.65 

3.II 

33 

33-6 

50.6 

35 

33-4 

50.2 

40 

32.8 

48.8 

3.01 

Na2SO4 


Gms.  Na2SO4 
t°.          too  Gms. 

per 
] 

Mols. 
*a2S04p 

Solution. 

Water.      Liter  (I 

50 

3i 

.8 

46 

•7 

2  .92 

60 

31 

.2 

45 

•3 

2.83 

80 

3o 

•4 

43 

•7 

2.69 

100 

29 

.8 

42 

•5 

2.6o 

120 

29 

•5 

41 

•95 

I4O 

29 

.6 

42 

160 

30-7 

44 

•25 

230 

3i 

•7 

46 

•4 

o 

16 

.3 

19 

•5 

5 

19 

•4 

24 

10 

.23 

.1 

30 

15 

27 

•o 

37 

20 

30 

.6 

44 

25 

34 

.6 

53 

... 

Na»SO« 


Na2S04.7HjO 


The  very  carefully  determined  values  of  Berkeley  are  as  follows: 


Gms. 


dtoi 
Sat.  Sol. 

Na2SO4  pe 
100  Gms. 

H20. 

0.70 

[.0432 

4.71 

10.25 

.0802 

9.21 

15.65 

.1150 

14.07 

20.35 

.1546 

.  .  . 

24.90 

.2067 

27.67 

27.65 

•2459 

34-05 

30.20    ] 

[.2894 

41.78 

31.95   ] 

[.3230 

47.98 

Gms. 

dt  of      Na,jSO4  per 
Sat.  Sol.     100  Gms. 
H20. 


Solid  Phase. 


32.5tr.pt. 
33-5 
38.15 
44.85 

60. 10 

75.05 
89-85 

[oi .  9* 

*  B.  pt. 


3307 
3229 
3136 
2918 
2728 

2571 
2450 


49.39 
48.47 

47-49 
45-22 

43-59 
42.67 
42.18 


Na2SO4.ioH2O+NajSO4 
NasSO, 


The  following  additional  data  at  high  temperatures,  determined  by  the  sealed 
tube  method,  are  given  by  Wuite  (1913-14). 


t° 

Mol. 
Per  cent 

Gms. 
Na2SO4  per 

Na2SO4. 

IOH2OmS 

62 

5.39 

44-92 

70 

5-27 

43.87 

80 

5.18 

43-07 

1  2O 

5.04 

41.84 

190 

5-255 

43.74 

192 

5-27 

43.87 

Solid  Phase. 


NazSO,  (rhombic) 


Mol. 
t°.       Per  cent 
Na^SO,. 

Gms. 
NajSO,  per 
100  Gms. 
H20. 

208        5.39 

44.92     ] 

235tr.pt. 

241      5-39 

250        5.04 

279      4.12 

319        2.56 

44.92 
41.84 

33.84 
20.71 

Solid  Phase. 

(rhombic) 
"  +monoclinio 
monoclinic) 


Supersolubility  curves  for  the  ice  phase,  Na2SO4.7H2O  phase  and  Na2SO4  phase 
were  determined  by  Hartley,  Jones  and  Hutchinson  (1908)  by  agitating  mixtures 
of  sodium  sulfate  and  water  contained  in  sealed  tubes,  and  noting  the  points  at 
which  spontaneous  crystallization  occurred  while  the  tubes  were  gradually  cooled. 
The  effect  of  mechanical  friction,  produced  by  bits  of  glass,  garnet,  etc.,  was  also 
studied. 


SODIUM  SULPATE  668 

SODIUM  SULFATE 

SOLUBILITY   OF   MIXTURES  OF  SODIUM  SULFATE  AND  MAGNESIUM  SULFATE 
IN  WATER  (ASTRAKANITE)  Na2Mg(SO4)24H2O. 

(Roozeboom,  1887, 1888.) 


Solid 
Phase. 

Astrakanite 


Astrakanite  +  NajSO4 


Astrakanite  +  MgSO4 


Mols. 

per  100 

Grams  per  100 

«;». 

Mols. 

H20. 

Grams 

HaO. 

fra2SO4.          MgSO4. 

Na2S04. 

Mgso4: 

22 

2 

•95 

4 

.70 

23 

•3 

31 

•4 

24 

•5 

3 

•45 

3 

.68 

27 

.2 

24 

.6 

30 

3 

•59 

3 

•59 

28 

•4 

24 

.1 

35 

3 

.71 

3 

.71 

29 

•4 

24 

.8 

47 

3 

.6 

3 

.6 

28 

•4 

24 

.1 

22 

2 

•95 

4 

.70 

23 

•3 

31 

•4 

24 

•5 

3 

•45 

3 

.62 

27 

.2 

24 

.2 

30 

4 

•58 

2 

.91 

36 

.1 

19 

.1 

35 

4 

•3 

2 

.76 

33 

•9 

18 

•44 

18 

•5 

3 

.41 

4 

.27 

45 

•5 

22 

2 

•85 

4 

•63 

35 

.2 

48 

•9 

24 

•5 

2 

.68 

4 

.76 

32 

•5 

5° 

.3 

30 

2 

•3 

5 

.31 

25 

•9 

55 

•  o 

35 

I 

•73 

5 

.88 

23 

•5 

59 

•4 

SOLUBILITY  OF  MIXTURES  OF  SODIUM  SULFATE,  POTASSIUM  CHLORIDE, 
POTASSIUM  SULFATE,  ETC.,  IN  WATER. 

(Meyerhoffer  and  Saunders,  1899.) 


*-  o 

Sp.  Gr.  of 

Mols.  per  1000  Mols.  H2U. 

* 

Solutions. 

SO,            K9 

Na2 

C12 

*4- 

4 

5- 

42 

14. 

39 

5I-83 

60. 

8 

K3Na(SO4)2+Na2SO4.ioH2O-r- 

0. 

2 

3- 

35 

12. 

78 

50- 

93 

60.36 

Na2S04.ioH2O+KCl+NaCl 

—    0. 

4 

3- 

59 

16. 

38 

40-75 

53- 

54 

Na2S04.ioH20+KCl+K3Na(SO4)2 

16. 

3 

4- 

72 

17- 

58 

50. 

56 

63.42 

K3Na(S04)2+KCl+NaCl 

24- 

8 

1.2484 

4- 

37 

20. 

oo 

48. 

36 

64. 

01 

K3Na(SO4)2+KCl+NaCl 

*i6. 

3 

16.29 

9- 

16 

61. 

06 

53- 

93 

K3Na(S04)2+NaCl-i-Na2SO4.ioH2O+ 
Na2SO4 

24. 

5 

1.2625 

14. 

45 

9- 

90 

58. 

46 

53- 

91 

K3Na(S04)2+NaCH-Na2SO4 

0. 

3 

2. 

75 

25- 

77 

17- 

93 

40. 

95 

K3Na(SO4)2+KCl+K2SO4 

25- 

o 

1.2034 

2. 

94 

36. 

20 

14. 

80 

48. 

06 

K3Na(SO4)2+KCl+K2SO4 

*i7- 

9 

1.2474 

13- 

84 

0. 

0 

62. 

57 

48. 

70 

Na2SO4.ioH20+Na2SO4+NaCl 

i 

1  .  2890 

IO. 

08 

40. 

33 

0. 

0 

K3Na(SO4)2+Na2SO4.ioH2O+Na2SO4 

—  21. 

4 

... 

.. 

. 

.. 

. 

46. 

61 

46. 

36 

NaCl.2H2O+Na2SO4.ioH2O 

-23. 

7 

. 

10. 

51 

39- 

58 

09 

NaCl.2H2O+KCl 

—  10. 

9 

I. 

45 

30. 

68 

29. 

23 

KC1+K2SO4 

-  3 

16. 

25 

IO. 

03 

6. 

21 

K3Na(SO4):r|-Na2SO4.ioH2O 

-  3 

16. 

24 

10. 

03 

6. 

21 

. 

K3Na(S04)2+K2S04 

-14 

i. 

39 

25- 

59 

8. 

78 

32- 

94 

KsNa(SO4)iH-Na2SO4.ioH2O-|-KCl 

-14 

i. 

39 

25. 

59 

8. 

78 

32- 

94 

K3Na(SO4)2+K2SO4+KCl 

-23. 

3 

... 

o. 

4i 

15. 

15 

44. 

20 

58. 

97 

Na2SO4.ioH2O+KCl+NaCl.aH2O 

*  Indicates  transition  points. 


669 


SODIUM   SULFATE 


SOLUBILITY  OF  SODIUM  SULFATE  IN  AQUEOUS  SOLUTIONS  OF  SODIUM 
ACETATE  AT  25°. 

(Fox,  1909.) 


Gms.  per  100  Gms.  Sat.Sol. 

Solid  Phase. 

Gms.  per  too  Gms.  Sat.  Sol. 

Solid  Phase. 

'  CHjCOONa. 

Na2SO4. 

CH3COONa. 

j^ajSO4. 

0 

21-9 

NasS04.ioH20 

12.58 

I3-50 

Na,SO4.ioH,O 

4.10 

17.72 

" 

16.26 

II  .50 

" 

7.71 

16.48 

H 

20.68 

8.10 

it 

SOLUBILITY  OF  SODIUM  SULFATE  IN  AQUEOUS  SODIUM  CHLORIDE  AT  15°. 

((Schreinemakers  and  de  Baat,  1909.) 

Gms.  per  100  Gms.  Sat.  Sol. 
NaCl. 


Solid  Phase. 


Gms*  per  100  Gms.  Sat.  Sol. 


5-42 
11-51 
15-97 


7.86 
5-87 
5-23 


NajS04.ioH20 


NaCl. 
21.03 

23-39 
25.21 


NajSO,. 
5.26 


Solid  Phase. 


Na2S04.ioH,0 
5.64        "  +NaCl 
2  . 26      NaCl 


SOLUBILITY  OF  SODIUM  SULFATE  IN  AQUEOUS  SOLUTIONS  OF  SODIUM 
CHLORIDE  AT  DIFFERENT  TEMPERATURES. 

(Seidell,  1902.) 


Results  at  10°. 


Results  at  21.5°. 


Results  at  27* 


Sp.  Gr. 
of 

Gms.  per  too  Gms. 
H20. 

Sp.  Gr. 

of 

Gms.  per  100  Gms. 
H20. 

Sp.  Gr. 
of 

Gms.  per  100  Gms. 
HzO. 

Solutions.    NaCl. 

Na2SO4. 

Solutions. 

Nad. 

Na2SO4.' 

Solutions. 

NaCl. 

Naa 

S04. 

1.  080 

o.o 

9- 

14 

I 

164 

O-O 

21-33 

1.228 

o.o 

31- 

10 

1.083 

4.28 

6. 

42 

I 

169 

9-05 

15.48 

1.230 

2.66 

28. 

73 

I  .IO2 

9.60 

4- 

76 

I 

199 

17.48 

13-73 

1.230 

5-29 

27. 

17 

I.I50 

I5-65 

3- 

99 

I 

.214 

20.41 

13.62 

1-235 

7.90 

26. 

02 

1.164 

21.82 

3 

97 

I 

•243 

26.01 

15-05 

1.259 

16.13 

24. 

83 

I  .192 

28.13 

4 

I 

.244 

26.53 

14.44 

1-253 

18.91 

21. 

39 

I  .207 

30.11 

4 

34 

I 

•244 

27-74 

13-39 

1.249 

19.64 

2O. 

ii 

I  .217 

32.27 

4 

59 

I 

.244 

31-25 

10.64 

1.245 

20.77 

19. 

29 

1.223 

4 

75 

I 

•243 

31.80 

10.28' 

1.238 

32-33 

9- 

53 

I 

•245 

32.10 

8.43 

I 

.219 

33-69 

4-73 

I 

.212 

34.08 

2-77 

I 

.197 

35-46 

o.oo 

Results  at  30°. 

Results  at 

33°. 

Results  at 

35°. 

Sp.  Gr. 

of 

Gms.  per  100  Gms. 
HizO. 

Sp.  Gr. 

of 

Gms.  per  100  Gms. 
H?0. 

Sp.  Gr. 
of 

Gms.  per  100  Gms. 

Solutions. 

NaCl. 

Na2S04. 

Solutions. 

NaCl. 

Na2SO4. 

Solutions. 

NaCl. 

Na2SO  . 

I.28l 

o.o 

39 

.70 

I 

•329 

o.o 

48.48 

1.324 

o.o 

47 

94 

1.282 

2.45 

38 

•25 

I 

•323 

1.22 

46.49 

«-3«4 

2.14 

43 

•75 

1.284 

5-6i 

36 

I 

.318 

1-99 

45.16 

1.256 

13-57 

26 

.26 

I  .290 

7.91 

35 

:96 

I 

•3r5 

2.64 

44.09 

1.238 

18.78 

19 

74 

1.276 

10.  61 

31 

.64 

•309 

3-47 

42.61 

1.231 

71  .  OI 

8 

.28 

1.270 

12.36 

29 

-87 

•265 

12.14 

29.32 

i-i93 

3  ?  -  63 

o 

.00 

1.258 

15-65 

25 

.02 

•237 

21.87 

16-83 

1.249 

18.44 

21 

•30 

•234 

32.84 

8.76 

1.244 

20.66 

19 

.06 

.217 

33-99 

4.63 

1.236 

32-43 

9 

.06 

I 

.208 

34-77 

2-75 

SODIUM   SULFATE 


670 


SOLUBILITY  OF  SODIUM  SULFATE  IN  AQUEOUS  SOLUTIONS  OF  SODIUM 
CHLORIDE  AT  25°. 

(Cameron,  Bell  and  Robinson,  1907.) 
^  Of     Gms.  per  100  Gms.  H2O. 


Sat.  Sol.  .' 

I.2I73 

I.2l62 

I.2I50 

1.2275 

1.2385 

1.2571 

1.2476 


NaCl. 
2.96 

5-79 
9.90 

13-43 
15-82 

19-13 
23.22 


NazSO,. 
26.60 
24.32 
21.41 
19.62 
19.64 
20.73 
16.28 


Solid  Phase. 
Na2SO4.ioH2O 


Sat.  Sol. 

NaCl. 

Na,S04. 

ouiiu  i  nase. 

.2429 

26.54 

12.64 

Na2S04 

.2438 

31.06 

9.98 

" 

•2451 

32.41 

9-93 

" 

•2453 

33 

9-84 

"  +NaCl 

.2309 

33-81 

6.66 

NaCl 

.2162 

34.60 

3.38 

" 

.2002 

35.8o 

0 

" 

Data  are  also  given  for  the  ^ystem  sodium  sulfate,  sodium  chloride,  calcium 
sulfate  and  water  at  25°. 

SOLUBILITY  OF  SODIUM  SULFATE  IN  AQUEOUS  SOLUTIONS  OF  SODIUM 
HYDROXIDE  AT  25°. 

(D'Ans  and  Schreiner,  1910.) 

Mols.  per  1000  Gms.  Sat.  Sol. 


Mols.  per  looq  Gms.  Sat.  Sol. 
(NaOH)2.          NajSCv 
0.074  1.41 

0.70  1. 08 

1-47  0.90 

2.02  0.59 


Solid  Phase. 


NasSO, 


(NaOH)2. 
2.82 
3-52 
5.83 
6.62 


Na,S04. 

0.24 

0.126 

0.013 

O 


Solid  Phase. 
Na,SO« 

NaOH.H20 


SOLUBILITY  OF  SODIUM  SULFATE  IN  AQUEOUS  SOLUTIONS  OF  SULFURIC 

ACID  AT  25°. 

(D'Ans,  1906;  19090;  1913.) 


Mols.  per 

looo  Gms. 

Sat. 

Sol. 

Solid  Phase. 

H2S04. 

Na2S04. 

0 

I.54I 

Na2S04.ioH20 

0.286 

1.671 

" 

0.338 

1.742 

i< 

O.6o 

1.85 

" 

0.763 

2 

" 

0.884 

2.256 

4-NajJ 

0.423 

0.77 

NaHSO4.H2O 

0.496 

0.47 

" 

1.666 

2-437 

Na2SO4+Na3H(SO4)2 

1.576 

2.363 

"  +Na3H(SO4)2.H2O 

2.611 

2.091 

Na3H(S04)2+       " 

5-91* 

0.409 

NaHSO4 

6.30 

0.332 

« 

6.64 

0.297 

"  +NaH3(S04)2.H20 

6.90 

0.173 

NaH3(S04)2.H20 

7.36 

O.07I 

" 

7-74 

0.047 

« 

8.12 

0.037 

« 

8.40 

0.046 

" 

Mols.  per  1000  Gms. 

Sat. 

Sol. 

Solid  Phase. 

S03. 

Na2SO4. 

8.70 

0.076 

NaH3(SO4)2.H2O 

8.86 

0.156 

" 

8.93 

0.273 

" 

8.84 

0.527 

"    (unstable) 

8.70 

0.8o8 

"          " 

8.62 

0.844 

"          " 

8.61 

0.899 

" 

8.87 

0-445 

•  "  +Na,S04.4*H2S04 

8-93 

0-437 

Na2S04.4|H2S04 

9.08 

0-394 

" 

9-36 

0.425 

"  +NaHS20, 

9.18 

0.567 

NaHSjiO, 

9.42 

0.728 

" 

9.48 

0.76 

" 

9.48 

0-953 

"    +? 

9-85 

0.787 

? 

9.98 

0.908 

? 

9.77 

1.03 

unstable 

10.  16 

0.797 

10.78 

0.302 

'  From  this  point  on  the  figures  in  this  column  are  Mols.SO3  =  H2SO4  +  S03. 

loo  cc.  sat.  solution  of  Na2SO4  in  absolute  H2SO4  contain  29.99  gms.  Na2SO4 
and  the  molecular  compound  which  is  formed  contains  8  mols.  H2SO4  per  I  mol. 
Na2SO4  and  melts  at  about  40°.  (Bergius,  1910.) 

Aqueous  H2SO4  containing  0.51  mol.  per  liter  dissolve  2.238  mols.  Na2SC>4  per 
liter  at  25°;  Aq.  H2SO4  of  0.779  mol-  per  liter  dissolves  2.465  mols.  Na2SO4  at  the 
same  temperature.  (Here,  1911-12.) 


671 


SODIUM   SULFATE 


SOLUBILITY  OF  SODIUM 


SULFATE  IN  AQUEOUS  ETHYL  ALCOHOL. 

(de  Bruyn,  1900.) 


r. 

Concentra- 
tion of 
Alcohol  in 
Wt.  %. 

Gms.  NajSO4 
per  too  Gms. 
Aq.  Alcohol. 

IS 

0 

12.7 

9.2 

6-7 

" 

19.4 

2.6 

II 

39-7 

o-5 

" 

58.9 

O.I 

(I 

72 

0 

M 

0 

37-4 

" 

II.  2 

16.3 

" 

20.6 

7 

II 

30.2 

2 

25 

0 

28.2 

ti 

10.6 

13-9 

tt 

24 

4-5 

ft 

54 

0.4 

36 

0 

49-3 

8.8 

29.2 

" 

12.8 

22.4 

II 

17.9 

15-4 

II 

18.1 

15-3 

II 

28.9 

5-4 

II 

48.7 

0.8 

45 

o 

47-9 

*' 

9 

27-5 

ii 

14-5 

19.2 

" 

20.  6 

12.3 

Gms. 

per  100  Gms. 

Solution. 

bond  Phase. 

HA 

CiH6OH. 

Na2S04. 

88.7 

0 

11.3 

NajSO4.ioH,O 

85.1 

8.6 

6-3 

•     « 

78.6 

18.9 

2.5 

« 

60 

39-5 

0-5 

« 

4I.I 

58.8 

O.I 

» 

28 

72 

0 

« 

72.8 

o 

27.2 

Na.S04.7HA 

76.5 

9-5 

14 

74-3 

19.2 

6.5 

M 

68.4 

29.6 

2 

« 

78.I 

o 

21.9 

Na,SO4.ioH,O 

78-5 

9-3 

12.2 

" 

72.8 

22.9 

4-3 

" 

45-6 

54 

0.4 

"  +Na2S04 

67 

0 

33 

NaaSO, 

70.6 

6.8 

22.6 

" 

71.2 

10.5 

I8.3 

" 

71.1 

15-5 

13-4 

" 

71 

15-7 

13-3 

" 

66.5 

28.4 

" 

50-9 

48.3 

o.S 

ti 

67.6 

0 

32.4 

" 

71  3 

7-  I 

21.6 

« 

71.8 

12.  I 

16.1 

« 

70.6 

18.4 

IO 

" 

65-6 

29.5 

4.9 

" 

The 
and  de 

25 


following  additional  determinations  at  25°  are  given  by  Schreinemakers 
Baat  (1909): 

63.41  34.84  1.75       Na2S04.ioHI0 

...  49  50-5 


46.6 
34*9 


53 
64-95 


1-75 
0.5 
0.4 
0.15 


+Na,S04 
NajSO, 


Between  certain  concentrations  of  the  aqueous  alcohol  the  liquid  separates  into 
two  layers.     The  following  results  were  obtained  at  25°,  36°  and  45°: 


Upper  Layer. 


Lower  Layer. 


Gms.H20.  Gms.C2H5OH 

.  Gms.Na2SO4. 

Gms.H2O.    Gms.C2H6OH 

.  Gms.Na2SO4. 

25 

66.5 

27-3 

6.2 

67.4 

5-1 

27-5 

n 

68.1 

23-9 

8.0 

68.5 

6.0 

25-5 

tt 

68.3 

23.1 

8.6 

68.3 

6.7 

25.0 

36 

.  .  . 

.  .  . 

66.6 

4.1 

29-3 

« 

57-7 

38-4 

3-9 

M 

65.0 

28.3 

6.7 

68.8 

5-9 

25-3 

II 

68.1 

21  .2 

10.7 

68.9 

9-4 

21.7 

45 

61.8 

32-9 

5-3 

ii 

65.8 

25-3 

8.9 

68.4 

8.8 

22.8 

tt 

66.0 

24.  Q 

10.  0 

68.6 

10.  1 

21-3 

Data  for  equilibrium  in  the  system  Na2SO4  +  NaCl  +  C2H5OH  +  H2O  at  15°, 
25°  and  35°  are  given  by  Schreinemakers  and  de  Baat  (1909),  and  Schreinemakers 
(1910). 


SODIUM   SULFATE 


672 


SOLUBILITY  OF  SODIUM  SULFATE  IN  AQUEOUS  PROPYL  ALCOHOL  AT  20°. 

(Linebarger,  1892.) 


Gms. 
per  ioo  Gms. 
Alcohol-Water 
Mixture. 


Gms.  Na2SC>4 
per  ioo 
Gms.  Sat. 
Solution. 

1-99 


Gms.  C3H7OH 

per  100  Gms. 

Alcohol-Water 

Mixture. 


Gms.  Na2SO4 
per  ioo 
Gms.  Sat. 
Solution. 


42.20  1-99  50.57  0.55 

49-77  I-I5  60.64  0-44 

55.65  0.72  62.8l  0.38 

ioo  gms.  H2O  dissolve  183.7  gms-  sugar  +  30.5  gms.  Na2SO4  at  31.25°,  or  ioo 

gms.  sat.  solution  contain  52.2  gms.  sugar  +  9.6  gms.  Na2SO4.  (Kohler,  1897.) 

ioo  gms.  95%  formic  acid  dissolve  16.5  gms.  Na2SO4  at  19°.  (Aschan,  1913.) 

SOLUBILITY  OF  SODIUM  SULFATE  IN  AN  AQUEOUS  SOLUTION  OF  UREA. 

(Lowenherz,  1895.) 


Solvent. 

ioo  gms.  H2O+i2  gms.  urea 


Gms. 
Na2SO4  per 

The  Corresponding  Fig- 
ure for  the  Solubility 

t. 

ioo  Gms. 
Sat.  Sol. 

of  Na2SO4  in  Pure  Water 
Was  Found  to  be: 

20.86 

22.36 

.  .  . 

24-83 

21.21 

21.62 

28.32 

26.50 

26.48 

29.83 

28.23 

31.90 

32.34 

34.85 

27-73 

33.09 

39-92 

27.19 

32.58 

Fusion-point  data  for  Na2SO4  +  KC1  are  given  by  Sackur  (1911-12).  Results 
for  Na2SO4  +  SrSO4  are  given  by  Calcagni  (191  2-  1912  a).  Results  for  Na2SO4 
+  Na2WO4  are  given  by  Boeke  (1907). 

SODIUM   BiSULFATE  NaHSO4.     (See  also  last  table,  p.  670.) 

ioo  gms.  H2O  dissolve  30  gms.  NaHSO4  at  16°.  (Aschan,  1913.) 

ioo  gms.  H2O  dissolve  28.  6  gms.  NaHSO4at  25°  and  50  gms.  at  100°.  (U.S.P.VIII.) 
ioo  gms.  95  per  cent  alcohol  dissolve  about  1.4  gms.  NaHSO4at  25°.  (U.S.P.VIII.) 
ioo  gms.  95%  formic  acid  dissolve  30  gms.  NaHSO4  at  19.3°.  (Aschan,  1913.) 

SODIUM   SULFIDE  Na2S.9H2O. 


SOLUBILITY  IN  WATER. 

(Parravano  and  Fornaini,  1907.) 


Gms.  NajS 

per  ioo  Gms. 

Sat.  Sol. 

—  lOEutec.     9.34 


Solid  Phase. 


+  10 

15 
18 
22 
28 
32 

37 
45 


50 


pt. 


13-36 
14.36 
15-30 
16.20 

17-73 
19.09 
20.98 
24.19 

28.48 


Gms.  NasS 

t°. 

per  ioo  Gms. 
Sat.  Sol. 

60 

29.92 

70 

3I-38 

80 

33-95 

90 

37-20 

48 

tr.  pt. 

50 

26.7 

60 

28.1 

70 

30.22 

80 

32.95 

90 

36.42 

91 

.5tr.pt.     ... 

Solid  Phase. 


+Na2S.sJH20 


JO  28.48  NajS.siHzO  9I.5tr.pt.     ...  "  +NajS.si 

Fusion-point  data  for  Na2S  +  S  are  given  by  Thomas  and  Rule  (1917). 

SODIUM  Antimony  SULFIDE.    See  Sodium  Sulfoantimonate,  p.  627. 


673 


SODIUM  SULFITE 


SODIUM  SULFITE  Na2SO3. 


t°. 

0.76 

Cms.  NajSOs 
per  ioo  Gms. 
H20. 

2.15 

1-37 
1.96 

4-21 
6.24 

2.77 
3-5* 

9.44 
12.48 

4-5 

17.91 

1.9 

2 

5-9 
10.6 

13.09 
14.82 
17.61 
2O.  OI 

SOLUBILITY  IN  WATER. 

(Hartley  and  Barrett,  1909.) 


Solid  Phase. 


Ice 


1    +Na2S03.7H20 
Ice  (unstable) 


Gms.  N^SOs 

t°. 

per  100  Gms. 

Solid  Phase. 

H20. 

18.2 

25-3I 

Na2S03.7H20 

23.5 

29.92 

"     (unstable) 

29 

34-99 

«           « 

37-2 

44.08 

«           « 

21.  6f 

"     +Na,SO, 

37 

28.04 

Na,SO, 

47 

28.13 

H 

55-6 

28.21 

« 

59-8 

28.76 

« 

84 

28.26 

" 

t  tr.  pt. 

*  Eutec. 

Oxidation  was  prevented  by  preparing  the  material  and  making  the  solubility 
determinations  in  an  atmosphere  of  hydrogen. 
Supersolubility  curves  for  the  salt  are  also  given. 
The  Sp.  Gr.  of  the  sat.  solution  at  15°  is  I.2I.  (Greenish  and  Smith,  1901.) 

SODIUM   HydroSULFITE  Na2S2O4. 


SOLUBILITY  IN  WATER,    (jeliinck,  1911.) 


Solid  Phase. 


Gms.  NajSA 
per  100  Gms. 

H20. 
19  Ice+Na2S204.2H20 

22  (±5%  error)   Na2s2o4.2H2o 

27.8  "  +Na2S204 

24.1  Na2S2O4  (unstable) 


The  pure  sample  was  prepared  by  salting  out  the  commercial  product  with 
NaCl.  It  is  very  easily  oxidized  to  Na2S2O5  and  must  be  kept  in  an  indifferent 
atmosphere  or  a  vacuum.  A  special  apparatus  was  required  for  the  freezing-point 
determinations  (ice  curve)  and  for  the  solubility  determinations.  Great  difficulty 
was  experienced  in  obtaining  concordant  results  with  a  given  sample  of 


Gms.  NajSA     <.,., 

*°        periS$;n8'    Phase. 

t°. 

—  O.IO7 

0.394         Ice 

—    4.58  Eutec. 

—  I.IO 

4 

+  20 

—  2.21 

9 

52  tr.  pt. 

-3-15 

13 

20 

-4.17 

17 

SODIUM  SULFONATES 


SOLUBILITY  IN  WATER. 


Salt. 

Sodium: 
2.5  Diiodobenzene  Sulfonate 


Formula. 


Gms. 

O     Anhydrous 

'  Salt  per  ioo 

Gms.  H2O. 


Authority. 


3-4 

0  Naphthalene  Sulfonate 
<(  <( 

2  Phenathrene  Sulfonate 
~  «  it 

10  " 

Phenol  Sulfonate 


1.019. 


C6H3I2S03Na.H2O 

Ci0H7.SO3Na 
u 

Ci4H9S03Na.|H20 

Ci4H9SO3Na.H2O 

Ci4H9.SO3Na.2H2O 


22.5 
22.5 
23-9 
25 

20 
20 
20 


(Boyle,  1909.) 


6.82 

3-47 
6.04 

5.87* 
0.42 
i.i 
1.63 
14- 7t 

IQ.  2% 

K  =  I.067.  t  <*25  = 

SOLUBILITY  OF  SODIUM  /3  NAPHTHALENE  SULFONATE  IN  AQUEOUS  HYDRO- 
CHLORIC ACID  AT  23.9°.      (Fischer  1906.) 

Normality  of  Aq.  HC1.  i.o».  2  n.  3  n.  5  n. 

Gms.CioHT.SOsNaperioogms.  Aq.HCl  6.47        5.35        4.13        2.42 


25 


(Fischer,  1906.) 
(Witt,  1915.) 
(Sandquist,  1912.) 


(Greenish  &  Smith,'oi.) 
(Seidell,  1910.) 
1.079 


SODIUM  SULFONATES 


674 


SOLUBILITY  OF  SODIUM  PHENOL  SULFONATE  IN  AQUEOUS  ALCOHOL  AT  25°. 

(Seidell,  1910.) 

Wt.  Per  cent  j      r          Gms.  CsILXOH).    Wt.  Per  cent 

CjHiOH  in 
Solvent. 


o(=H20) 
10 

20 
30 
40 

50 


ms.  Sat.  Sol. 

19.38 

17.4 

15-5 
13-6 

ii. 7 

9-7 


rtveat. 
60 


70 
80 
90 

95 

100 


d    nf         Gms.  CjEUCOH) 
Sa?  Sol        SO3Na.2H20  per 
loo  Gms.  Sat.  Sol. 

0.919 

0.886 

7-5 

0.852 
0.820 

2.9 
i.i 

0.810 

0.8 

0.800 

i.S 

1.079 
1.054 
1.030 
1.004 
0.977 

In  "the  ioo  per  cent  C2H6OH  solution,  the  solid  phase,  C6H4(OH)  S03Na.2H2O, 
became  opaque. 

ioo  gms.  H2O  dissolve  18.25  gms.  C6H4(OH)SO3Na.2H2O  at  14.8°,  du.&  of  sat. 

sol.  =  1.0675.  (Greenish  and  Smith,   1901.) 

SODIUM   TARTRATES 

SOLUBILITY  IN  WATER. 

Gms.  Salt 
Salt.  Formula.  t°.     per  ioo 

Gms.  H2O. 

Sodium  Neutral  Inactive  Pyrotartrate  C6H6O6.Na2.6H2O    20 

Dextro  20 

Sodium  Dihydroxy  Tartrate  C4H4O8Na2.3H2O       o 

SODIUM  TELLURATE  Na2TeO4.2H2O. 

ioo  gms.  H2O  dissolve  o.f  7  gm.  Na2TeO4  at  18°,  and  2  gms.  at  100°. 
phase  Na2TeO4.2H2O. 

ioo  gms.  H2O  dissolve  1.43  gms.  Na2TeO4  at  18°,  and  2.5  gms.  at  50°.     Solid 
phase  Na2TeO4.4H2O.  (Mylius,  1901.) 

SODIUM  THIOSULFATE  Na2S2O3.5H2O(I). 

SOLUBILITY  IN  WATER.      (Young  and  Burke,  1904, 1906.) 


Authority. 

39.73    (Schlossberg,  1900.) 
41.10  " 

0.039  (Fenton,  1898.) 

Solid 


Gms.  NazS-A  per 
i°Jf.            ioo  Gms.                  gelid  Phase.              t°. 

Gms.  NajSA  per 
ioo  Gms. 

Solid  Phase. 

Sat.  Sol. 

Water. 

Sat. 

Sol. 

Water. 

O 

33- 

40 

50 

.  l5NaaS2O3.sH2O(I) 

0 

60. 

47 

153 

Na 

iSA-HjOdD 

10 

37- 

37 

59 

.66  " 

IO 

61. 

04 

156. 

7 

" 

20 

41. 

20 

70 

.07  " 

2O 

62. 

ii 

163. 

9 

** 

25 

I43> 

15 

75 

.90  " 

25 

62. 

73 

168. 

3 

a 

35 

47- 

71 

91 

.24  " 

30 

63- 

56 

174. 

4 

** 

45 

55-33 

123 

.87  " 

40 

65.22 

187. 

6 

** 

48. 

17*  -. 

. 

.  . 

.        "+Na2S203.2H20(I) 

50 

66. 

82 

201. 

4 

it 

. 

o 

52. 

73 

in 

.6oNa2S203.2H20(I) 

56.5* 

. 

.  .  . 

«* 

+Na,SA 

10 

53- 

94 

117 

.  10    " 

0 

46. 

14 

85  .  67  NajSjOa-GHjOdllandlV) 

20 

55- 

IS 

122 

.68  " 

IO 

66 

106. 

8 

** 

25 

56. 

03 

127 

•43  " 

13 

54- 

96 

122 

« 

30 

57- 

13 

138 

.84  " 

14.35* 

« 

+Na2S2O3.fH2O.(IV) 

40 

59- 

38 

146 

.20    " 

14.3* 

.  . 

.  .  . 

u 

+Na2S203.7H20(III) 

50 

62. 

28 

165 

.11 

o 

57- 

42 

134- 

8  Na,SA.7H20(III) 

60 

65- 

68 

191 

•30  .  " 

IO 

58. 

28 

139- 

7 

" 

66. 

5*     .- 

. 

.  .       "+Na,SA 

20 

59.28 

145.6    •• 

o 

41. 

96 

72 

.3oNa2S203.SH20(ID 

25 

60. 

18 

I 

« 

10 

45- 

25 

82 

•65    " 

30 

60. 

78 

155 

* 

20 

49. 

38 

97 

•55  " 

40 

62. 

60 

I67. 

4 

*• 

25 

52- 

15 

108 

.98  '« 

47-5 

64. 

68 

i 

« 

30 

56.57 

130 

.26  " 

48.5* 

.  .  . 

r- 

+Na2S203.H20(IID 

30.22*    ... 

,  .        "+Na2St03.4H20(ID 

47-5 

64.' 

78 

l83.9Na2S203.H20(IID 

33- 

5    58. 

59 

141 

.48Na2S203.4H20(II) 

65. 

3 

188. 

2 

« 

36. 

2      60. 

5* 

153 

•23    " 

55 

66. 

45 

198. 

I 

* 

36. 

6    62. 

80 

168 

.82    " 

60 

68. 

07 

213. 

I 

* 

40. 

65*.. 

.    . 

. 

"+Na2SJOa.H20(II) 

61* 

M, 

-f-^SA 

*  tr.pt. 

675 


SODIUM  THIOSULFATE 


SOLUBILITY  IN  WATER  (Continued). 


Cms.  Na 

2SA  per 

Gms.  NajSjOs 

per 

t". 

100  ( 

jins. 

Solid  Phase.            t°. 

100  1 

Lrms. 

,  Solid  Phase. 

Sat. 

Sol. 

Water. 

Sat. 

Sol. 

Water. 

O 

57 

•63 

136 

Na2S203.iH,0(IV)      30 

63- 

34 

172 

.80 

Na2S20,.H10(V) 

10 

58 

.49 

I4O. 

9 

40 

64. 

75 

183.70       « 

2O 

59 

•57 

147- 

3 

50 

66. 

58 

199 

.2 

« 

25 

60 

•35 

152. 

2 

55 

67. 

59 

208 

•5 

" 

30 

61 

•03 

156. 

6 

43* 

"+NasS203.*H20'(V) 

40 

62 

•95 

I69. 

9 

"        .                25 

64*. 

21 

179 

•4 

Na1S203.JHJ0(V) 

50 

65 

•45 

I89. 

5 

40 

64. 

99 

185 

.6 

" 

55 

67.07 

203. 

7 

50 

66. 

02 

194 

•3 

" 

58* 

.  . 

"  +Na2S203           60 

67. 

4 

2O6 

•7 

« 

O 

57 

•63 

136 

Na2S203.2H20(V)           70 

69. 

06 

223 

.2 

<« 

10 

59 

•05 

144. 

2 

70* 

"  +Na2S20, 

20 

61 

.02 

156. 

5 

40 

67^4 

206 

•7 

Na2S20, 

25 

62 

•30 

165- 

3 

50 

67. 

76 

210 

.2 

" 

30 

63 

•56 

174. 

4 

60 

68. 

48 

217 

•3 

« 

35 

65 

.27 

188 

70 

69. 

05 

223 

.1 

(i 

27-5* 

"  +N02S203.H20  (V)   80 

69- 

86 

231 

.8 

« 

*  tr.  pt. 

The  authors  adopted  a  new  system  of  naming  the  hydrates,  based  upon  their 
mutual  transition  relations.  These  transitions  occur  in  such  a  way  that  the 
members  of  one  group  undergo  transition  into  members  of  the  same  group  and 
not  into  members  of  another  group.  Those  hydrates  belonging  to  group  (I)  are 
called  primary  hydrates,  those  belonging  to  group  (II)  are  called  secondary  and 
those  belonging  to  the  (III),  (IV)  and  (V)  groups  are  called  tertiary,  quaternary 
and  quintary  respectively. 

Commercial  sodium  thiosulfate  is  the  primary  pentahydrate,  Na2S2O3.5H2O  (I). 

100  gms.  alcohol  dissolve  0.0025  gm.  Na2S<jO3  and  0.0034  Sm-  Na2S2O3.5H2O  at 
room  temperature.  (Bodtker,  1897.) 

100  gms.  alcohol  of  0.941  Sp.  Gr.  dissolve  33.3  gms.  sodium  thiosulfate  at  15.5°. 

Data  for  the  lowering  of  the  freezing-point  of  Na2S2O3-5H2O  by  each  of  the  fol- 
lowing compounds:  urea,  glucose,  cane  sugar,  NaCl,  NaClO3,  NaNO3  and  Na2SO4 
are  given  by  Bautaric  (1911). 


SODIUM  TUNGSTATE  Na2WO4.2H2O. 


SOLUBILITY  IN  WATER. 

(Funk,  igooa.) 


- 

Gms. 
Na2W04  per 
100  Gms. 
Solution. 

Mols. 
Na2WO4 
per 
100  Mols. 
H20. 

Solid                 t  o 
Phase. 

Gms. 
Na2W04  per 
100  Gms. 
Solution. 

Mols. 
Na2WO4 

100  Mols. 
H20. 

Solid 
Phase. 

-5 

30.60 

2.70 

Na2WO4.ioH2O   —3. 

1  ») 

41.67 

4-37 

Na3W04.2HjO 

-4 

3I-87 

2.86 

+  0. 

5 

41-73 

4-39 

" 

~~  3 

5  32-98 

3-01 

18 

42  .O 

4.40 

M 

—  2 

34-52 

3-23 

21 

42.27 

4.48 

" 

0 

3-52 

43 

.5 

43  -98 

4.81 

" 

+  3 

39-20 

3-95 

80 

•5 

47-65 

5-57 

II 

5 

41  .02 

4.26 

100 

49-31 

5-95 

H 

Sp.  Gr.  of  sat.  solution  at  18°  =  1-573- 
solutions  at  20°,  see  Pawlewski,  1900. 


For  Sp.  Gr.  determinations  of  aqueous 


Fusion-point  data  for  Na2WO4  +  WO3  are  given  by  Parravano  (1909). 


SODIUM  URATE  676 

SODIUM   URATE  C5H3N4O3.Na. 

SOLUBILITY  IN  AQUEOUS  SODIUM  CHLORIDE  AT  37°. 

(d'Agostino,  1910.) 

Gms.  Mols;  per  Liter.  Cms.  Mols.  per  Liter.  Gms.  Mols.  per  Liter. 

NaCl.         'c6H3N403.Na.  '  NaCl.          "  C6H3N4O3Na.  '  NaCl.  "  CsH3N4O3.Na. 

O                           O.OO536  O.OIO84           O.002II  O.O5II6  O.OOO5O 

O.OO486           0.00340  0.01398           O.OOI72  0.06667  O.OOO34 

0.00532           0.00321  0.02564           0.00102  0.07363  0.00032 

O.O0865           O.OO256  O.040I2           0.00054  0.08595  O.00026 

One  liter  of  H2O  dissolves  1  .5  gms.  sodium  urate  at  37°.       (Bechhold  and  Ziegler,  1910.) 
One  liter  of  serum  dissolves  0.025  Sm-  sodium  urate  at  37°. 

SODIUM   MetaVANADATE  NaVO3. 

SOLUBILITY  IN  WATER. 

(MacAdam  and  Pierle,  1912.) 
Solid  Phase.  f.  *™  Solid  Phase. 


25  21.10  NaV03  2$  15.3  NaVO3.2H2O 

40  26.23  "  40  30.2 

60  32.97  "  00  68.4 

75  38.83  "  75  38.8  Navo, 

Considerable  time  was  required  for  attainment  of  equilibrium.  The  two  solid 
phases  appear  to  exist  for  the  whole  rage  of  temperature  and  the  conditions  for 
the  transformation  of  one  into  the  other  were  not  ascertained. 

SODIUM   FluoZIRCONATE  5NaF.ZrF4. 

IOO  gms.  H2O  dissolve  0.387  gm.  at  18°,  and  1.67  gms.  at  IOO°.      (Marignac,  1861.) 

SPARTEINE  C15H26N2. 

SOLUBILITY  IN  WATER  AND  IN  AQUEOUS  SODIUM  CARBONATE  SOLUTIONS. 

(Valeur,  1917.) 

The  author  prepared  solutions  of  recently  distilled  colorless  sparteine  (a  = 
—  2°46'  in  5  cm.  tube)  in  aqueous  5  per  cent  Na2CO3  and  determined  the  tem- 
perature at  which  clouding  occurred  in  each. 


t°  of  Gms.  QsHasNu  t°  of          Gms.  Ci5H26N2  t°  of          Gms.  CiBH26N, 

Clouding.  per  100  cc.  Clouding.         per  100  cc.  Clouding.         per  100  cc. 

23-4  2.1  33.5  1.5  47  0.9 

24  1-95  36.5  1-35  53  0.75 

25  1.8  39.8  1.2  60.2  0.60 

28.6          1.65  43.5         1.05  72.5         0.45 

A  saturated  solution  of  sparteine  in  water  was  prepared,  and  after  removing  the 
solid  phase  by  centrif  ugation,  the  amount  of  sparteine  in  the  saturated  solution  was 
determined  with  the  aid  of  the  data  in  the  above  table.  Enough  Na2CO3  and 
H2O  to  yield  5  per  cent  Na2CO3  were  added  and  the  temperature  of  clouding  ob- 
served and  compared  with  the  above  results.  The  average  of  these  determina- 
tions was  0.556  gm.  sparteine  per  100  cc.  sat.  solution  in  water  at  10.8°. 

SPARTEINE   SULFATE   Ci5H26N2.H2SO4.5H2O. 

100  gms.  H2O  dissolve  about  200  gms.  sparteine  sulfate  at  15-20°. 

100  cc.  90%  alcohol  dissolve  about  20  gms.  sparteine  sulfate  at  15-20°. 

(Squire  and  Caines,  1905-)' 

STEARIC  ACID   CH3(CH2)16COOH. 

100  gms.  H2O  dissolve  o.i  gm.  stearic  acid  at  37°. 

100  gms.  5%  aqueous  solution  of  bile  salts  dissolve  less  than  o.i  gm.  stearic  acid. 
100  gms.  5%  aq.  sol.  of  bile  salt  +  i%  lecithin  dissolve  0.2  gm.  stearic  acid. 
In  the  same  solvents  there  is  dissolved  of  sodium  stearate,  o.i,  0.2-  and  0.7  gm. 
respectively.  (Moore,  Wilson  and  Hutchinson,  1909.) 


677  STEARIC  ACID 

SOLUBILITY  OF  STEARIC  ACID  IN  AQUEOUS  ETHYL  ALCOHOL  AT  25°. 

(Seidell,  1910.) 

Wt.%  ,      f        Cms.  CnHjjCOOH  Wt.  %  ,      .       Cms.  CnR^COOn 

CzHjOH  JPfa  per  100  Cms.  C2H6OH  sS'Sl  per  100  Cms. 

in  Solvent.  Sat.  Sol.  in  Solvent.  Sat.  Sol. 

o  0.999  0.034  7°  0.865  0.80 

20  0.967  0.04  80  0.841  1.63 

40  0.932  o.io  90  0.818  3-3Q 

50  0.911  0.18  95  0.807  5.55 

60  0.888  0.40  loo  0.795  8.30 

100  cc.  f  94.3  Vol.  %  C2H6OH  contain  0.0996  gm.  CnHasCOOH  at  o°  (do  =  0.83 1 8) . 

sat.  sol.<  95.1      "  "       0.1139  "  "  (^0  =  0.8287). 

in       [95.7      "  "       0.1246  "  "  (do  =  0.8265). 

Saturation  was  approached  from  above  without  constant  agitation.  (Emerson,  1907.) 

SOLUBILITY  OF  STEARIC  ACID  IN  ETHYL  ALCOHOL  AT  SEVERAL  TEMPERATURES. 

(Falciola,  1910.) 
Cms.  CnHjjjCOOH  per  100  cc.  of: 


Absolute  Alcohol.      75%  Alcohol.  50%  Alcohol. 

10  0.9  0.15 

20  2  ...  0.08(23°) 

30  4-5  0.39  o.io 

40  13.8  0-77  0.12 

loo  cc.  sat;  solution  in  94.4  Vol.  %  CH3OH  ("methylated  alcohol"  of  d  = 
0.8183)  contain  0.15  gm.  CiyHasCOOH  at  +0.2°.  Saturation  was  approached 
from  above  without  constant  agitation.  (Hehner  and  Mitchell,  1897.) 

SOLUBILITY  OF  STEARIC  ACID  IN  SEVERAL  SOLVENTS  AT  25°. 

(Seidell,  1910.) 

,     f  Cms.  C17H35COOH 

Solvent.  d  of  Solvent.  c^5  cli  per  100  Cms. 

Sat.  Sol.  Sat  Sol 

Acetone                            ^15= 0.797            0.815  4-73 

Amyl  Alcohol  (iso)           ^20=0.817            0.815  9.43 

Amyl  Acetate                   ^20=0. 875            0.867  11.19 

Carbon  Bisulfide              ^25=  1.259             -1.163  19.20 

Carbon  Tetrachloride      d25=  1.587             1-465  10.25 

Chloroform                       d^=  1.476             1.332  15.54 

Ether  (abs.)                       ^22=0.711             0.744  20.04 

Ethyl  Acetate                  ^25=0.892             0.895  7-36 

Nitrobenzene                    ^25=1.205             1.199  1.24 

Toluene                             ^15=0.872             0.865  13.61 

Fusion-point   data  for  stearic   acid  +  tristearin   and   for  stearic  acid  -f-  tri- 

stearin  +  palmitic  acid  are  given  by  Kremann  and  Kropsch  (1914). 

STILBENE  C6H5CH:CH.C6H5. 

Freezing-point  data  for  mixtures  of  stilbene  and  p  dimethoxystilbene  are  given 
by  Pascal  and  Normand  (1913). 

STRONTIUM   ACETATE  Sr(CH3COO)2.iH2O. 

SOLUBILITY  IN  WATER. 

(Osaka  and  Abe,  1911.) 


t»        Cms.  Sr(CH3COO)2          s  ,}d  p, 
*  '        per  100  Cms.  H2O. 

0.05            36.93        Sr(CH3COO)2.4H20 

25 

40.19 

5                    39-91 

35-03 

38-82 

10                43  .61 

50 

37-35 

8  .  4  tr.  pt.  43  .  1              "  +Sr(CH3COO)2.*H20 

70 

36-24 

8                    43  .  5               Sr(CH3COO)2.*H20 

80 

36.10 

10               42.95 

90 

36.24 

15                    41.00 

97 

36.36 

Sr(CH3COO)2.JH20 


STRONTIUM  BENZOATE       678 

STRONTIUM  BENZOATE  Sr(C7H6O2)2.H2O. 

SOLUBILITY  IN  WATER. 

(Pajetta,  1906.) 
t°.  15-7°.          24.7°.          31.4°.  40.9°. 

Gms.  Sr(C7H602)2  per  loo  Gms.  Solution     5.31        5.4        5.56        5.77 

STRONTIUM   BROMATE  Sr(BrO3)2. 

One  liter  of  aqueous  solution  contains  0.9  gm.  molecules  or  309  gms.  Sr(BrOj)j 
at  1 8°.  (Kohlrausch,  1897.) 

STRONTIUM   BROMIDE   SrBr2.6H2O. 

SOLUBILITY  »  IN  WATER. 

(Average  curve  from  results  of  Kremers,  1858;  and  Etard,  1894.) 

Gms.  SrBr2  per  100  Gms.  Gms.  SrBr2  per  100  Gms. 

Solution.  Water.  '  Solution.  Water.  ' 

o  46                 85.2  40  55.2  123.2 

10  48.3              93  50  57.6  135.8 

20  50.6  102.4  60  60  150 

25  51.7  107  80  64.5  181.8 

30  52.8  111.9  I0°  69  222.5 

Sp.  Gr.  of  sat.  solution  at  20°  approximately  1.70. 

100  gms.  abs.  alcohol  dissolve  64.5  gms.  SrBr2  at  o°.     Sp.  Gr.  of  solution  =  1.21. 

(Fonzes-Diacon,  1895.) 

SOLUBILITY  OF  STRONTIUM  BROMIDE  IN  AQUEOUS  SOLUTIONS  OF  STRONTIUM 

NITRATE  AT  25°. 

(Harkins  and  Pearce,  1916.) 


Mols.  per  1000  Gms.  H2O. 
"  Sr(NO3)2.  '       SrBr2.;  '_] 

o               4.3080 

0.036          4-3I05 
0.07216     4.3125 
0.14568     4.3170 

Gms.  SrBr2 
per  1000  Gms 

I066.  I 
1066.95 
1067.42. 
1068.54 

«¥cf 

•    Sat  Sol. 
1.7002 

1.70325 
1.72844 

Mols.  per  1000  Gms.  H2O. 

Gms.  SrBr2 

1068.8 
1069.  17 
1073-97 

d^ot 
Sat.  Sol. 
1.73766 
I  .  74866 
1.77368 

0 
0, 
I  , 

30663 
61124 
,86lO 

SrBr2. 
4.3180 

4.3190 
4-3390 

Data  for  equilibrium  in  the  system  strontium  bromide,  strontium  oxide  and 
water  at  25°  are  given  by  Milikau  (1916). 

STRONTIUM   CAMPHORATE  d  C10H14O4Sr.4H2O. 

SOLUBILITY  IN  AQUEOUS  SOLUTIONS  OF  CAMPHORIC  ACID  AT  16-17°. 

(Jungfleisch  and  Landrieu,  1914.) 

Gms.  per  100  Gms.  Sat.  Sol.  Gms.  per  100  Gms.  Sat.  Sol. 

C8H14(COOH)",   C10H1404Sr.  Sohd  Phase.       ^(COOH)",   C10H14O4Sr.  S«^  Phase. 


1.25  I.4I3  C8H14(COOH)2  1.20  17.99 

1.03  1.7705    (C10H1604)2Sr(C10H1,04)J       O  16.95  CwH14O4Sr.4H2O 

1.13          6.525  o  16.56 

i.  20         12.452  o  I2.86(atg8c)  " 

STRONTIUM   CARBONATE   SrCCX. 

One  liter  of  water  dissolves  0.00082  gm.  at  8.8°  and  0.0109  Sm-  at  24°  by  con- 
ductivity method.  (Holleman,  1893;  Kohlrausch  and  Rose,  1893.) 

One  liter  of  water  saturated  with  CO2  dissolves  1.19  gms.  Sr(HCO3)2. 

Data  for  the  solubility  of  strontium  carbonate  in  water  containing  CO2  at 
pressures  between  0.05  and  i.i  atmospheres  are  given  by  McCoy  and  Smith 
(1911).  The  equilibrium  constant  is  k  =  1.29  X  IO"2  with  an  average  deviation 
from  the  mean  of  1.2  per  cent.  From  this  value,  the  solubility  product  is  calcu- 
lated to  be  Sr  X  CO8  =  k3  =  1.567  X  IQ-9. 


679 


STRONTIUM   CARBONATE 


SOLUBILITY  OF  STRONTIUM  CARBONATE  IN  AQUEOUS  AMMONIUM  CHLORIDE. 

(Cantoni  and  Goguelia,  1905.) 


Cms.  NH4C1  per 
100  Cms.  Solution. 


Cms.  SrCO3  per 
1000  cc.  Sat.  Solution. 


5-35  0.179 

10  0.259 

20  0.358 

The  mixtures  were  allowed  to  stand  at  12-18°  for  98  days. 
Fusion-point  data  for  SrCO3  +  SrCl2  are  given  by  Sackur  (1911-12). 

STRONTIUM   CHLORATE   Sr(ClO3)2. 

100  gms.  H2O  dissolve  174.9  gms.  Sr(ClO)2,  or  100  gms.  sat.  solution  contain 
63.6  gms.  at  18  .     Sp.  Gr.  of  solution  is  1.839.  (Mylius  and  Funk,  1897.) 

STRONTIUM   CHLORIDE   SrCl2.6H2O. 


SOLUBILITY  IN  WATER. 

(Average  curve  from  the  results  of  Mulder;  Etard;  see  also  Tilden,  1884.) 


Gms.  SrCl2  per  100  Gms.        Solid 

to 

Gms.  SrCl2  per  100  Gms. 

Solid 

* 

Solution. 

Water. 

Phase. 

• 

Solution.           Water* 

Phase. 

—  20 

26.O 

35-1 

SrCl2.6H2O 

60 

45-o 

81.8 

SrCl2.6H2O 

O 

30-3 

43-5 

M 

70 

46.2 

85-9 

SrCl2.2H20 

10 

32.3 

47-7 

" 

80 

47-5 

90-5 

M 

2O 

34-6 

52-9 

(I 

100 

50.2 

100.8 

M 

25 

35-8 

55-8 

" 

I2O  . 

112.  8 

M 

30 

37-o 

58-7 

" 

140 

55-6 

125.2 

M 

40 

39-5 

65-3 

" 

160 

58-5 

141.0 

u 

50 

42  .0 

72.4 

41 

180 

62.0 

163.1 

M 

Transition  temperature 

about  62.5°. 

Sp.  Gr. 

of  sat. 

solution  at  o° 

=  I-334J  at 

15°  =  1.36. 


SOLUBILITY  OF  STRONTIUM  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF 
HYDROCHLORIC  ACID  AT  o°.    (Engei,  1888.) 


Mg.  Mols.  per  TO  cc.  Solution. 


*SrCl2. 
S1.6 

44-8 

37-85 
27.2 

22. 0 
14.0 
4.25 


HC1. 
O 

6.1 

12.75 
23-3 

28.38 
37-25 
52-75 


Sp.  Gr.  of 
Solution. 


•334 
•304 
.269 
.220 

.201 

.167 
i-'33 


Grams  per  100  cc.  Solution. 


SrCl2. 

HCl. 

40.9 

0-0 

35-5 

2  .22 

30.0 

4-65 

21  .56 

8-49 

17.44 

10.35 

II  .09 

I3-58 

3-37 

19.23 

SOLUBILITY  OF  STRONTIUM  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  HYDRO- 
BROMIC  AND  OF  HYDROCHLORIC  ACIDS  AT  25°. 

(Harkins  and  Paine,  1916.) 

In  Aqueous  HBr.  In  Aqueous  HCl. 


Gms.  Equiv.  HBr      j     of 

Gms.  SrCl2 

Gms.  Equiv.  HCl        4     of 

Gms.  SrClj 

per  looo  Gms.            T 
H20.                Sat.  Sol. 

per  100  Gms. 
Sat.  Sol. 

per  looo  Gms.              « 
H2O.                 Sat.  Sol. 

per  too  Gms. 
Sat.  Sol. 

o                   1.4015 

35-80 

O.I55I            1.3953 

35-17 

0.06817          1.4020 

35-47 

0.5162            L3788 

33-60 

0.4191             I.4OIO 

33-92 

I.OI7              I-3563 

31.42 

0.9716             I-3992 

3I-52 

2.165              I-3065 

26.33 

I.I54               1-3995 

20.78 

9  .  205          i  .  1498 

3-055 

STRONTIUM  CHLORIDE 


680 


SOLUBILITY  OF  STRONTIUM  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  ACIDS 
AND  OF  SALTS  AT  25°. 

(Harkins  and  Paine,  1916.) 


Aqueous     g^ded  gait        ^%B  °^ 
ution  per  1000  Gms.     Sat.  Sol. 

Gms.  SrCl2 
per  loo  Gms. 
Sat.  Sol. 

Aqueous 
Solution 
of: 

Gms.  Equiv.       ,       , 
added  Salt       *tt  of 
per  looo  Gms.   Sat.  Sol. 

XlgvJ. 

Gms. 
er  icx 

SrCl, 
3  Gms 

CuCl2 

o 

7U4 

i 

.4200 

34 

•005 

KNO3 

0.09796 

.4107 

35 

.86 

" 

a 

276 

i 

•4595 

30.40 

0-4755 

•4349 

35 

.90 

HI 

0 

1641 

z 

.4058 

34 

.850 

HNO3 

0.1771 

.4038 

35 

•52 

tt 

0 

.4462 

i 

.4121 

33 

.28 

" 

0.3521 

•4059 

35 

.40 

ti 

0 

•7539 

i 

.4196 

•52 

tt 

1.277 

•4175 

34 

.04 

KI 

0.09199 

i 

•4093 

35 

•45 

NaN03 

0.3621 

.4216 

35 

-63 

" 

o 

5401 

i 

.4466 

33 

•79 

" 

0.5010 

.4588 

35 

.60 

" 

o 

6015 

i 

.4513 

33 

.60 

" 

3-553      1-5214 

30 

.88 

" 

I 

445 

i 

.5154 

30 

.90 

" 

6.856      1-5581 

25 

•53 

KC1 

0 

0719 

i 

•4032 

35 

.62 

Sr(N03)2 

0.1372     1.4113 

35-42 

" 

o 

433 

i 

.4085 

34 

.80 

n 

0.5766     1.4336 

34 

•47 

a 

0 

8576 

i 

.4152 

33 

.89 

tt 

1.0988     1.4636 

33 

•30 

tt 

I 

594 

i 

.4266 

32 

.40 

" 

3.318      1.6664 

28 

•97 

Data  for  equilibrium  in  the  system  strontium  chloride,  strontium  oxide  and 
water  at  o°,  25°  and  40°  are  given  by  Milikau  (1916). 

100  gms.  abs.  methyl  alcohol  dissolve  63.3  gms.  SrCl2.6H2O  at  6°. 

loo  gms.  abs.  ethyl  alcohol  dissolve  3.8  gms.  SrCl2.6H2O  at  6°.    (de  Bruyn,  1892.) 


SOLUBILITY  OF  STRONTIUM  CHLORIDE  IN  AQUEOUS  ETHYL  ALCOHOL 
SOLUTIONS  AT  18°. 

(Gerardin,  1865.) 


Sp.  Gr.  of 
Aq.  Alcohol 
ato°. 

Wt. 
per  cent 
Alcohol. 

Gms.  SrCl2 
per  100  Gms. 
Alcohol. 

Sp.  Gr.  of 
Aq.  Alcohol 
ato°. 

Wt. 
per  cent 
Alcohol. 

Gms.  SrClj 
per  100  Gm 
Alcohol. 

0.990 

6 

49.8l 

0-939 

45 

26.8 

0.985 

10 

47-0 

0.909 

59 

19.2 

o-973 

23 

39-6 

0-846 

86 

4-9 

0.966 

30 

35-9 

0.832 

91 

3-2 

o-953 

38 

30-4 

100  gms.  95%  formic  acid  dissolve  23.8  gms.  SrCl2  at  19°.  (Aschan,  1913.) 

100  cc.  anhydrous  hydrazine  dissolve  8  gms.  SrCl2  at  room  temp. 

(Welsh  and  Broderson,  1915.) 

Fusion-point  data  for  SrCl2  +  SrF2  are  given  by  Plato  (1907).  Results  for 
SrCl2  +  SrO  and  SrCl2  +  SrSO4  by  Sackur  (1911-12).  Results  for  SrCl2  +  T1C1 
by  Korreng  (1914)  and  results  for  SrCl2  +  ZnCl2  by  Sandonnini  (i9i2a,  1914). 


STRONTIUM   CHROMATE  SrCrO4. 


SOLUBILITY  IN  WATER,  ETC.,  AT  15°. 

(Fresenius,  1891.) 


Solvent. 


Water 

Aq.  NH4C1  (5%) 

Aq.  CHaCOOH  (i%) 


Gms.  SrCrO4 

per  loo 
Gms.  Solvent. 

0.12 
0.195 


Gms.  SrCrO4 
Solvent.  per  100 

Gms.  Solvent. 

Aq.  Ethyl  Alcohol  (29%)     0.0132 
Aq.  Ethyl  Alcohol  (53%)     0.002 


68i 


STRONTIUM   CINNAMATE 


STRONTIUM   CINNAMATE  (C6H6CH:CH.COO)2Sr.2H2O. 
100  gms.  H2O  dissolve  i  gm.  (C6H5CH:CH.COO)2Sr  at  I5°-2O°. 

(Squire  and  Caines,  1905-) 

100  gms.  sat.  aqueous  solution  contain  1.18  gm.  (C«H6CH  :CH.COO)2Sr  at  15° 
and  3.11  gms.  at  IOO°.  (Tarugiand  Checchi,  1901.) 


STRONTIUM   FORMATE  Sr(HCOO)2.2H2O. 

SOLUBILITY  IN  WATER.    (Stanley,  1904.) 


F. 

0 

ii 
28.6 
37-4 
Si-4 

Gms.  Sr(HCOO)2 
loo  Gms.  H2O. 
7-02  (8.35) 

8.08(9.54), 
11.62  (13.25 
13.01  (14.68 

16.31  (17.83 

per        Solid  Phase. 
Sr(HCOO)2.2HiO 

it 

F. 
67.5 

86' 
91.7 

IOO 

20.62  (21.76) 
26.14  (26.36) 
27-58  (27-57) 
27.01  (27.07) 
26.57  (26.72) 

Sr(HCOO)2.2H2O 
Sr(HCOO)2.H2O 


There  appears  to  be  an  error  in  the  calculation  of  the  results  as  given  by  the 
author  in  his  table.  The  figures  given  above  in  parentheses  have,  therefore, 
been  calculated  from  the  weights  of  SrSC>4  recorded  in  the  original  table  and 
show  the  weight  of  Sr(HCOO)2  per  100  gms.  of  saturated  solution. 

STRONTIUM   FLUORIDE   SrF2. 

One  liter  of  water  dissolves  0.1135  Sm-  SrF2  at  0.26°,  0.1173  gm-  at  I7-4°  an<3 
0.1193  gm.  at  27.4°,  determined  by  the  conductivity  method.  (Kohlrausch,  1908.) 

STRONTIUM   GLYCEROPHOSPHATE  C3H7O2PO4Sr.2H2O. 

100  gms.  sat.  solution  in  water  contain  2.09  gms.  anhydrous  salt  at  18°  and  0.8 

gm.  at  60°.  (Rogier  and  Fiore,  1913.) 

STRONTIUM  HYDROXIDE   Sr(OH)2.8H2O. 

SOLUBILITY  IN  WATER.    (Scheibler,  1883.) 

Grams  per  100  Grams  Solution.  Grams  per  TOO  cc.  Solution. 


V   . 

SrO. 

Sr(OH)2.8H20.' 

o 

o-35 

0.90 

10 

0.48 

1.23 

20 

0.68 

i-74 

30 

I  .00 

2-57 

40 

1.48 

3.80 

50 

2.13 

5  -46 

60 

3-03 

7-77 

70 

4-35 

ii  .  16 

80 

6.56 

16.83 

90 

12  .O 

30.78 

IOO 

18.6 

47  .71 

SrO. 

Sr(OH)2.8H2O. 

o-35 

0.90 

0.48 

1.23 

0.68 

1.74 

1.  01 

2-59 

i-S1 

3-87 

2.18 

5-59 

3.12 

8.00 

4-55 

11.67 

7.02 

18.01 

13.64 

34-99 

22.85 

58.61 

MUTUAL  SOLUBILITY  OF  STRONTIUM  HYDROXIDE  AND  STRONTIUM  NITRATE 

IN  WATER  AT  25°.      (Parsons  and  Perkins,  1910.) 


j              Gms.  per  100  Gms.  H2O. 

,5}*°*,      '    SrO  as 
Sat.  Sol.       Sr(OH)2. 

Sr(NO.,)2. 

1.481         o 

79.27 

1.492            0.38 

79-47 

1.494           0.78 

80.83 

1.506 

.76 

81.06 

1.490 

•71 

74.27 

1.419 

.51 

63-71 

1.381 

.41 

56.30 

1.327 

.27 

46.97 

Gms.  per  100  Gms.  H2O. 


Solid  Phase. 


Sr(OH)2.8H2O 


ffcot    ' 
at.  Sol. 

SrO  as 
Sr(OH)2. 

sr(NOl>,.' 

.267 

I.  II 

37.81         Sr(OH)2.8H2O 

.217 

I.OI 

28.80 

.178 

0.95 

23-83 

.148 

0.91 

17.96 

.108 

0.84 

12.78 

.079 

0.81 

8.96 

•059 

0-79 

6.  29 

1.033 

0.78 

4-45 

STRONTIUM  HYDROXIDE 


682 


SOLUBILITY  OF  STRONTIUM  HYDROXIDE  IN  AQUEOUS  SOLUTIONS  AT  25°. 

(Rothmund,  1910.) 


Aqueous  Solution  of: 

Mols. 
Sr(OH)2.- 
8H20 

Cms. 

Sr(OH)2 
per 

per  Liter. 

Liter. 

Water  alone 

0.0835 

10.16 

0.5  n  Methyl  Alcohol 

0.0820 

9-97 

"     Ethyl  Alcohol 

0.0744 

9-05 

"     Propyl  Alcohol 
"     Amyl  Alcohol 

0.0708 

8.61 

(tertiary) 

0.0630 

7.66 

"     Acetone 

0.0692 

8.42 

"     Ether 

0.0645 

7-85 

Aqueous  Solution  of: 

0.5  n  Glycol 
"     Glycerol 
"     Mannitol 
Urea 
"     Ammonia 
"     Dimethylamine 
"     Pyridine 

Mols. 
Sr(OH)2. 
8H20 
per  Liter. 
O.O922 

o.  1094 
o.  1996 

0.0820 
0.0785 
0.0586 

o  .  0694 

Gms. 
Sr(OH)2 

tSu. 

II.  21 
24.29 

9-97 
9-55 

8^44 

Data  for  equilibrium  in  the  system  strontium  hydroxide,  phenol  and  water  at 
25°  are  given  by  van  Meurs  (1916). 


STRONTIUM  IODATE   Sr(IO3)2. 

100  gms.  H2O  dissolve  0.026  gm.  at*i5°,  and  0.72-0.91  gm.  at  100°. 

~    -Li 


(Gay-Lussac;  Rammelsberg,  1838.) 


STRONTIUM   IODIDE   SrI2.6H2O. 


SOLUBILITY  IN  WATER. 

(Average  curve  from  the  results  of  Kremers,  1858;  and  Etard,  1874.) 


Gms.  SrI2  per 

TOO  Gms. 

Solid 

Solution. 

Water. 

'      Phase. 

0 

62.3 

I65-3 

SrI2.6H20 

20 

64.0 

177.8 

" 

40 

65-7 

I9I.5 

«« 

60 

68.5 

217-5 

" 

80 

73-o 

270.4 

• 

t°. 

Gms.  Srls  per 

ioo  Gms. 

Solid 

Solution. 

Water.    " 

Phase. 

90 

78-5 

365-2 

SrI2.2H2O 

100 

79-3 

383-I 

" 

120 

80.7 

4I8.I 

it 

I4O 

82.5 

47I-S 

" 

J75 

85.6 

594-4 

<• 

Transition  temperature  about  90°.     Sp.  Gr.  of  sat.  solution  at  20°  =  2.15 
ioo  gms.  sat.  solution  of  strontium  iodide  in  absolute  alcohol  contain  2.6  gms. 

SrI2  at  —20°,  3.1  gms.  at  +4°,  4-3  gms.  at  39°,  and  4.7  gms.  at  82°.    (Etard,  1874.) 
Data  for  equilibrium  in  the  system  strontium  iodide,  strontium  oxide  and 

water  at  25°  are  given  by  Milikau  (1916). 


STRONTIUM   PerlODIDE   SrI4. 

Data  for  the  formation  of  strontium  periodide  in  aqueous  solution  at  25° 
are  given  by  Herz  and  Bulla  (1911).  The  experiments  were  made  by  adding 
iodine  to  aqueous  solutions  of  SrI2  and  agitating  with  carbon  tetrachloride. 
From  the  iodine  content  of  the  CC14  layer  the  amount  of  iodine  in  the  aqueous 
layer  can  be  calculated  on  the  basis  of  the  distribution  ratio  of  iodine  between 
water  and  CCU.  This  furnishes  the  necessary  data  for  calculating  the  amount 
of  the  strontium  periodide  existing  in  the  aqueous  layer. 


STRONTIUM   IODOMERCURATE  SrI2.HgI2.8H2O. 

A  saturated  aqueous  solution  prepared  by  adding  SrI2  and  HgI2  in  excess  to 
warm  water  and  filtering  when  the  temperature  had  fallen  to  16.5°  was  found 
to  have  the  composition  i.o  SrI2.i.24  HgI2.i8.O9  H2O.  The  die. 5  was  2.5 

(Duboin,  1906.) 


683 


STRONTIUM  MALATE 


STRONTIUM   MALATE  SrC4H4O5. 

SOLUBILITY  IN  WATER. 

(Cantoni  and  Basadonna,  1906.) 


20 
25 

30 

35 


Gms.  per  100 
cc.  Solution. 

0.448 

0-550 
0.752 
1.036 


40 

45 
50 


Gms.  per  100 
cc.  Solution. 

I-385 

1-743 
2.098 


55 
60 

65 

70 


Gms.  per  100 
cc.  Solution. 

2.460 
2.821 
3.148 


STRONTIUM  MALONATE  CH2(COO)2Sr. 

SOLUBILITY  IN  WATER. 

(Cantoni  and  Diotalevi,  1905.) 


O 
IO 

20 


Gms.  per  100  cc. 
Sat.  Sol. 

0-541 
0.540 
0.532 


25 
30 

35 


Gms.  per  100  cc. 
Sat.  Sol. 
O.52I 
0.499 
0.478 


40 

45 
50 


Gms.  per  too  cc. 
Sat.  Sol. 
0.464 
0-453 
0-443 


STRONTIUM  MOLYBDATE  SrMoO4. 

100  gms.  H2O  dissolve  0.0104  gm.  SrMoO4  at  17°. 

STRONTIUM  NITRATE  Sr(NO3)2. 

SOLUBILITY  IN  WATER. 

(Berkeley  and  Appleby,  1911.) 


(Smith  and  Bradbury,  1891.) 


t°. 

dtoi 

Sat.  Sol. 

G 

Sr(N( 
loo  Gr 

53)2  pe 
ns.  H2 

3. 

t°. 

dtoi 
Sat.  Sol. 

Gms.           c  i'j 
Sr(N03)2per    pSh°^ 
100  Gms.  H2O.  Phase- 

0.58 

.28561 

40. 

124 

Sr(NO3)2.4H2O 

30-74 

.51282 

90.086    Sr(NO,)1 

14.71 

.39380 

00. 

867 

" 

47-73 

•5II50 

91.446 

26.40 

.48831 

82. 

052 

« 

61.34 

.  51048 

93.856          " 

29.06 

.51098 

87. 

648 

« 

68.96 

•51057 

95.576 

29.3* 

"  +Sr(N03)2 

78.98 

.51091 

97.865           «« 

30.28 

.51441 

88  ! 

577 

Sr(NOj)2 

88.94 

•5II74 

100.  136        " 

32.58 

.51408 

88. 

943 

" 

The  determinations  were  made  with  very  great  accuracy. 

SOLUBILITY  OF  STRONTIUM  NITRATE  IN  AQUEOUS  ALCOHOL  AT  25°. 

(D'Ans  and  Siegler,  1913.) 


Wt.  % 
CAOH 

Solvent 

Gms.  per  100  Gms. 
m         Sat.  Sol. 

Solid  Phase. 

Wt.  % 
C2HBOHiE 
Solvent. 

Gms 

i 

.  per  100  Gms. 
Sat.  Sol.       • 

Solid  Phase. 

•  QzHsOH. 

Sr(N03)2. 

C2H5OH. 

Sr(NO3)2. 

0 

0 

44 

•25 

Sr(NO3)2.4H2O 

IO 

6 

40. 

05 

Sr(NOj)2  (unstable) 

4 

i-7 

42 

.8 

" 

15 

05 

9 

5 

36, 

>j 

"          (unstable) 

6 

2.6 

42 

.1 

« 

18 

.8* 

12 

35 

34 

3 

"  +Sr(N03)2.4H20 

10.8 

4-95 

40 

•4 

" 

20 

6 

13 

.8 

33 

2 

SrCNOdi 

16 

7-95 

37 

.6 

" 

40 

65 

32 

35 

20. 

5 

" 

20* 

12.35 

34 

•3 

"  +Sr(N03)J 

59 

9 

53 

6 

IO, 

5 

« 

O 

o 

46 

.6 

Sr(NOa)2  (unstable) 

79 

,2 

77 

15 

2, 

6 

« 

6 

3-45 

42 

•  7 

"                " 

99 

4 

99 

38 

0, 

02 

« 

*  Tr.  pt. 

100  cc.  anhydrous  hydrazine  dissolve  5  gms.  Sr(NOa)2  at  room  temp. 

(Welsh  and  Broderson,  1915.) 

STRONTIUM   NITRITE  Sr(NO2)2.H2O. 

100  cc.  sat.  solution  in  water  contain  62.83  gms.  Sr(NO2)2.H2O  at  19.5°. 

41  90%  alcohol       "         0.42     "  "  "  20°. 

"  abs.  alcohol        "         0.04     "  "  "  20°. 

(Vogel,  1903.) 


STRONTIUM  NITRITE  684 


SOLUBILITY  OF  STRONTIUM  NITRITE  IN  WATER. 

(Oswald,  1912,  1914.) 


Gms.  Sr(NO2)s  Gms. 

t°                   per  100  Gms.          Solid  Phase.                        t°.  per  100  Gins?     Solid  Phase. 

Sat.  Sol.  Sat.  Sol. 

—    1.3                 II-3         Ice                                      35  43-1          Sr(NQd,.HiO 

-  3-1                 J9-6          "                                        52.5  46.5 

-  7-7              35-5                                           60.5  49.3 

-6.8                 32.8           "  +Sr(N02)2.H20               65.5  50.7 

-  2.3                 33.4             SrCNO^.HjO                   82.5  54 

-  0.3                 34-5                                                      92  56.6 

+  19                 39-3*                                         98  58.1 

*  d  =  1.4461. 

STRONTIUM   OXALATE  SrC2O4.H2O. 

One  liter  of  water  dissolves  0.0328  gm.  SrC2O4  at  1.35°,  0.0444  gm.  at  15.9°, 
0.0461  gm.  at  18°,  0.0575  gm-  at  3l-7°  and  0.0617  Sm-  at  37.3°,  determined  by 

the  conductivity  method.  (Kohkausch,  1908.) 

One  liter  of  sat.  aqueous  solution  contains  0.057  gm-  SrC2O4  at  o°,  0.077  gm. 

at  20°  and  0.093  Sm-  at  4°°-  (Cantoni  and  Diotalevi,  1905.) 

SOLUBILITY  OF  STRONTIUM  OXALATE  IN  AQUEOUS  ACETIC  ACID  SOLUTIONS 

AT   26°-27°. 
(Herz  and  Muhs,  1903.) 


Normality  of 
Acetic  Acid. 

Gms.  per  100  cc.  Solution. 

Normality  ol 
Acetic  Acid. 

Gms.  per  100  cc.  Solution. 

CH3COOH. 

SrC204.H2O.     ' 

CH3COOH. 

SrCA.H20 

O 

0 

O.OO9 

3.86 

23.16 

0.0598 

0.58 

3.48 

0.0526 

5-79 

34-74 

o  .  0496 

1-45 

8.70 

0.0622 

16.26 

O.OO6O 

2.89 

17-34 

0.0642 

STRONTIUM   OXIDE  SrO. 

Fused  SrCl2  dissolves  18.3  gms.  SrO  per  100  gms.  of  the  fused  melt  at  910°. 

(Arndt.,  1907.) 

STRONTIUM  PERMANGANATE  Sr(MnO4)2. 

100  gms.  of  the  sat.  solution  in  water  contain  about  2.5  gms.  Sr(MnO4)2  at  o°. 

(Patterson,  1906.) 

STRONTIUM   SALICYLATE  (C6H4OH.COO)2Sr.2H2O. 

100  gms.  sat.  solution  in  water  contain  3.04  gms.  (C6H4OHCOO)2Sr  at  15°  and 

20.44  gmS.  at  IOO°.  (Tarugi  and  Checchi,  1901.) 

SOLUBILITY  OF  STRONTIUM  SALICYLATE  IN  AQUEOUS  ALCOHOL  AT  25°. 

(Seidell,  1909,  1910.) 


Wt.  % 
2H,OH  in 
Solvent. 

d^ol 
Sat!  Sol 

Gms.  (C6H4.OH.- 
COO)2Sr.2H2O 
per  100  Gms. 
Sat.  Sol. 

Wt.  %f 
CaHsOH  in 
Solvent. 

Sat.  Sol. 

Gms.  (C6ILOH- 
COO)2Sr.2H20 
per  100  Gms. 
Sat.  Sol. 

0 

I.O22 

5-04 

60 

0.923 

7-15 

10 

1.  006 

4.88 

70 

0.893 

5-90 

20 

0-993 

5-22 

80 

0.859 

4.40 

30 

0.982 

6.20 

90 

0.824 

2.56 

40 

0.966 

7.70 

92.3 

0.815 

2.02 

50 

0.948 

8.08 

100 

0.790 

0.44 

The  solid  phase  was  (C6H4OH.COO)2Sr.2H2O  in  all  cases  except  the  solution 
m  100  per  cent  alcohol,  in  which  partial  dehydration  and  conversion  of  the 
crystalline  salt  to  an  amorphous  bulky  white  powder  occurred. 


Gms.  QHASr 

Gms.  C.H.O 

t°. 

per  100  cc. 

t°. 

per  zoo  cc, 

Sat.  Sol. 

Sat.  Sol. 

0 

0.052 

2O 

0.270 

5 

0.076 

25 

0.382 

10 

O.III 

30 

0.451 

15 

0.177 

35 

0.413 

685  STRONTIUM   SUCCINATE 

STRONTIUM   SUCCINATE  C4H4O4Sr. 

100  gms.  sat.  solution  in  water  contain  0.439  gm.  C4H4O4Sr  at  15°  and  0.215 
gm.  at  IOO°.  (Tarugi  and  Checchi,  1901.) 

SOLUBILITY  OF  STRONTIUM    SUCCINATE  IN  WATER. 

(Cantoni  and  Diotalevi,  1905.) 

Gms.  C^x^OjSr 
t°.  per  100  cc. 

Sat.  Sol. 
40  0.375 

45  0.389 

50  0.424 


STRONTIUM   SULFATE  SrSO4. 

One  liter  of  water  dissolves  0.1133  gm.  SrSO4  at  2.85°,  0.1143  gm.  at  17.4° 
and  o. 1 143  gm.  at  32.3°,  determined  by  the  conductivity  method.  (Kohlrausch,  1908.) 

SOLUBILITY  OF  STRONTIUM  SULFATE  IN  AQUEOUS  SOLUTIONS  OF  AMMONIUM 

ACETATE  AT  25°. 

(Marden,  1916.) 

Gms.  per  too  Gms.  Sat.  Sol.  Gms.  per  too  Gms.  Sat.  Sol. 

CHsCOONH*.  SrS04.  CHaCOONH,.  SrSO4.  " 

0  0.0151  10.68  0.0942 

2.13  0.0451  21.37  O.II5 

5.34  0.0732 

SOLUBILITY  OF  STRONTIUM  SULFATE  IN  AQUEOUS  CALCIUM  NITRATE  AT 
ROOM  TEMPERATURE 

(Raffo  and  Rossi,  1915.) 

Analyzed  solutions  of  Sr(NO3)2,  Ca(NO3)2  and  CaSO4  were  mixed  at  60°  and 
allowed  to  stand  at  room  temperature  I  to  2  days.  The  resulting  SrSO4  was 
determined  and  the  difference  between  the  amount  found  and  the  amount 
which  would  have  resulted  if  all  the  Sr(NO3)2  had  been  converted  to  SrSO4f 
was  taken  as  the  amount  of  SrSO4  dissolved.  Gradually  increasing  concentra- 
tions of  Ca(NO3)2  were  used. 

Gms.  per  100  cc.  Sat.  Sol.  Gms.  per  100  cc.  Sat.  Sol. 

"Ca(NOdj.  SrS04.  '  'Ca(NOa)2.  SrSO4.  " 

0.5  0.0483  4  0.1489 

1  0.0619  5  0.1698 

2  0.1081  6  0.1955 

3  0.1275 

SOLUBILITY  OF  STRONTIUM  SULFATE  IN  AQUEOUS  SOLUTIONS  OF 
HYDROCHLORIC,  NITRIC,  CHLORACETIC  AND  FORMIC  ACIDS. 

(Banthisch,  1884.) 


ec.  of  Aq. 
Acid    con- 
taining   i 
Mg.  Equr 
ineachcasi 

In  Aq.  HC1 
Gms.  per  zoo  cc. 

In  Aq.  HNOs 
Gms.  per  100  cc. 

Sol. 

In  Aq.CH2ClCOOH 
Gms.  per  100  cc.  Sol. 

In  Aq.  HCOOH 
Gms.  per  100  cc. 
^ol. 

CH2C1 
COOH. 

SrS04. 

I'.  '  HC1. 

SrSO4. 

HN03. 

SrSO4. 

HCOOH, 

.    SrSO4. 

0.2 

18.23 

0 

.161 

31 

•52 

0 

.381 

.  .  . 

o-5 

7.29 

0 

.207 

12 

.61 

0 

•307 

.  .  . 

... 

x.o 

3-65 

0 

.188 

6 

•3o 

0 

.217 

94-47 

O.O26 

46.02 

0.024 

2  -O 

1.82 

0 

.126 

3 

•!5 

0 

.138 

47-23 

O.O22 

.  .  . 

... 

IO.O 

0.36 

0 

.048 

0 

•63 

0 

.049 

ioo  gms.  95  per  cent  formic  acid  dissolve  0.02  gm.  SrSO4  at  18.5°.      (Aschan,  1913)- 


STRONTIUM   SULFATE  686 

SOLUBILITY  OF  STRONTIUM  SULFATE  IN  AQUEOUS  SODIUM  CARBONATE  AT  25°. 

(Herz,  rgio.) 

Freshly  prepared  and  dried  SrSO4  was  shaken  5  days  with  aqueous  sodium 
carbonate  solutions  and  the  supernatant  clear  solutions  analyzed. 

Normality  of  Aqueous  Gm.  Mols.  per  Liter  Sat.  Sol. 

M,  CQ   /Na*COA  t  NaaCO,.  Na2SO4' 

V    2  /  2  2 

0.6025  0.0382  0.5643 

I.2O5  0.076  I.I29 

2-41  0-153  2.257 

SOLUBILITY  OF  STRONTIUM  SULFATE  IN  SULFURIC  ACID  SOLUTIONS. 

f.  Conc.ofH2SO,  GmSGS^0ASd.100  Authority. 

ord.  concentrated  5 . 68    .         (Sturve,  1870.) 

fuming  9.77  " 

"  91%  O.o8  (Varenne  and  Paulean,  1881.) 

70  Sp.  Gr.  1.843  =  99%  14  (Garside,  1875-) 

ord.          Absolute  H2S04  21.7*  (Bergius,  1910.) 

*  per  100  cc.  Sat.  Sol. 

SOLUBILITY  OF  STRONTIUM  SULFATE  IN  AQUEOUS  SALT  SOLUTIONS. 

(Virck,  1862.) 

In  Aq.  NaCl.  In  Aq.  KC1.  In  Aq.  MgCl2.  In  Aq.  CaCl2. 

'     (a.)  (6.)  (a.)  (6.)  (a.)  (6.)  '     (a.)  (ft.)  " ' 

8.44      0.165  8.22      0.193  1.59      0.199  8-67      0.176 

15.54     0.219         12.54     0.193  4.03      0.206         16.51      0.185 

22.17      0.181          18.08      0.251          13.63      0.242          33.70      0.171 

(a)  =  Cms.  salt  per  100  gms.  aq.  solution.     (6)  =  Cms.  SrSO4  per  100  gms. 
solvent. 

STRONTIUM  TARTRATE  SrC4H4O6.3H2O. 

SOLUBILITY  IN  WATER. 

,  (Cantoni  and  Zachoder,  1905.) 

Gms.  Gms.  Gms. 

t°.         SrC4H4O6.3H2p  per  t°.         SrC^O^H-sO  per  t°          SrC.HA^HaO  per 

100  cc.  Solution.  too  cc.  Solution.  100  cc.  Solution. 

O       O.II2  25        0.224  60       0.486 

10      0.149        3°      0.252        70      0.580 
15      0.174        40      0.328        80      0.688 

20        0.200  50         0.407  85         0.755 

SOLUBILITY  OF  STRONTIUM  TARTRATE  IN  AQUEOUS  SOLUTIONS  OF  ACETIC  ACID 

AT  26°-27°. 

(Herz  and  Muhs,  1903.) 

Normality  of  Gms.  per  ico  cc.  Solution.  Normality  of         Gms.  per  too  cc.  Solution. 

Acetic  Acid.          CH3COOH.      SrC4H4O6.3H20.  Acetic  Acid.       CH3COOH. '  SrC4H4O6.3H2O. 

o  o  0.227  3-77  21.85  1.051 

o-5<55  3-39  0.678  5.65  33.90  0.982 

1.425  8.15  0.864  16.89  101.34  0.184 

2.85  17.10  0.996 

STRONTIUM   (Di)   TUNGSTATE   SrW2O7.3H2O. 

100  cc.  H2O  dissolve  0.35  gm.  at  15°.  (Lefort,  1878.) 


687 


STRYCHNINE 


STRYCHNINE 


SOLUBILITY  IN  SEVERAL  SOLVENTS. 


Gms.  CnH-aNjOj 

Gms.  QiH^N 

Solvent. 

t°. 

per  100  Gms.                       Solvent. 

t-. 

per  zoo  Gms 

Solvent. 

Solvent. 

Water 

ord.t. 

0.014    C1 

Carbon  Tetrachloride 

20 

0.158    (5) 

u 

20 

0.0125(2 

«                                      Cf 

20 

0.22         9) 

" 

20 

0.0143(3 

(t                     11 

T7 

0.645       IC 

(C 

25 

0.016  (4)       Chloroform 

25 

10.25       6] 

(f 

20 

0.021   (5) 

25 

16.6         i/ 

Aq.  io%NHs 

2O 

°-°33   (3)       Diethylamine 

20 

1-7       (3) 

Aq.  3%  H3BO3  in  50% 
Glycerol                     ord.  t. 

3-5         i 

Ethyl  Acetate 
Ether 

20 
20 

0.197  (s 

0.043    (5 

C2H6OH  (^=0.83) 

15-20 

0.71       7 

M 

25 

0.018   (4 

"        (^=0.83) 

2O 

0-833     3 

"     sat.  with  H2O 

2O 

0-051    (5 

"        (<*=o.83) 

25 

v             *f 

0.91     (4 

Glycerol 

15 

0.25 

"     +10% 

NHs  20 

0.256   (3)       Petroleum  Ether 

2O 

0.0093(5] 

"        (^=0.785) 

25 

0.70     (6 

Piperidine 

20 

0.7       (3) 

CH3OH  (^=0.796) 

25 

0.49     (6 

Pyridine 

20 

i.S       (3) 

Aniline 

20 

20           (3 

« 

26 

1.24     (i: 

Amyl  Alcohol 

25 

/ 

0-55     (4 

Aq.  50  %  Pyridine 

20-25  2.43     (8) 

Benzene 

2O 

0.77    (s 

Water  sat.  with  Ether 

20 

0.017   (S> 

M 

25 

0.76     (6 

Oil  of  Sesame 

20 

0.061    (2] 

(i)  Baroni  and  Barlinetto  (1911);  (2)  Zalai  (1910);  (3)  Scholtz  (1912);  (4)  U.  S.  P.  8th  ed.;  (5)  Mullet 
[1903);    (6)  Schaefer  (1913);  (7)  Squire  and  Caines  (1905);    (8)  Dehn  (1917);    (9)  Gori  (1913);    (10) 
Holty  (1905). 


lindelmeiser  (1901);  (u) 


SOLUBILITY  OF  STRYCHNINE  IN  AQUEOUS  ALCOHOL  AT  i5°-2oa. 

(Squire  and  Caines,  1905.) 

Per  cent  Alcohol  in  Solvent  20          45          60          70 

Cms.  C2iH22N2O2  per  100  cc.  solvent      0.024    0.125    0.25      0.40 


90 
0-59 


SOLUBILITY  OF  STRYCHNINE  IN  MIXTURES  OF  ETHER  AND  CHLOROFORM  AT  25°. 


(Harden  and  Dover,  1916.) 


Per  cent 

CHC13  in 

Mixed  Solvent. 

100 

90 

80 

70 

60 


Cms.  CziH-sNzOz 
per  100  Gms. 
Mixed  Solvent. 

15-3 


2.77 

i-5 
0.65 


Per  cent 
CHC13  in 
Mixed  Solvent. 

Gms.  QiHaNjOj 
per  100  Gms. 
Mixed  Solvent. 

50 

0-35 

30 

0.21 

20 

0-15 

10 

0.09 

O 

O.O2 

SOLUBILITY  OF  STRYCHNINE  IN  MIXED  SOLVENTS  AT  25°. 

(Schaefer,  1913.) 

Gm- 


One  volume  of  C2H5OH+4  vols.  CHCla 
One  volume  of  C2H5OH+4  vols.  CeH6 
One  volume  of  CH3OH  +4  vols.  CHCla 
One  volume  of  CH3OH  +4  vols.  C6H6 


per 


25 

5 
25 

6.  7 


DISTRIBUTION  OF  STRYCHNINE  BETWEEN  WATER  AND  CHLOROFORM  AT  25°. 

(Seidell,  igioa.) 


Gm.  CK 
per  15  cc 


Added 
4-iS  cc. 


Gms.  C21H22N2O2  Recovered  per  15  cc: 


0.00$ 
0.025 
0.12$ 
O.62C 


H2O  Layer  (a). 
O.0006 
O.OOIO 
O.OO2I 
0.0099 


CHC13  Layer  (b). 
O.OI03(?) 
0.0253 
0.1299 
0.6225 


(6) 


25.2 

61 
64 


STRYCHNINE  688 

STRYCHNINE  ARSENATE  C21H22N2O2.H3AsO44H2O(.iiH2O). 

loo  gms.  sat.  solution  in  water  contain  4.53  gms.  C2iH22N2O2.H3AsO4  at  25°. 

(Puckner  and  Warren,  1910.) 

IOO  gms.  CHCU  dissolve  0.085  gm.  C2iH22N2O2.H3AsO4  at  15°.  (Hill,  1910.) 

STRYCHNINE  FORMATE  C2iH22N2O2.HCOOH.2H2O. 

SOLUBILITY  IN  WATER  AND  IN  ALCOHOL. 

(Hampshire  and  Pratt,  1913.) 

Solubility  in  Water.  Solubility  in  Abs.  Alcohol. 

t«,  Gms.  Salt  per  ^.o  Gms.  Salt  per 

loo  Gms.  H2O.  loo  Gms.  C2H6OH. 

19-5  30-59  18.5  10 

24  39-68  20  10.3 

27  44-25  22  10.64 

STRYCHNINE  HYDROBROMIDE  CnHEN-A.HBr. 

IOO  CC.  H2O  dissolve  1.54  gms.  of  the  salt  at  I5°-2O°.          (Squire  and  Caines,  1905.) 

loo  cc.  90%  alcohol  dissolve  1.04  gm.  of  the  salt  at  I5°-2O°. 


STRYCHNINE  HYDROCHLORIDE 

IOO  cc.  H2O  dissolve  2.86  gms.  of  the  salt  at  I5°-2O°.         (Squire  and  Caines,  1905.) 

loo  cc.  90%  alcohol  dissolve  1.37  gms.  of  the  salt  at  I5°-2O°. 

100  gms.  CHCls  dissolve  0.592  gm.  of  the  salt  at  15°.  (Hill,  1910. 


STRYCHNINE  NITRATE 

SOLUBILITY  IN  SEVERAL  SOLVENTS. 

Gms.  Salt  Solvent.                                         Gms.  Salt 

Solvent.               t°.         per  100  cc.  t°.        per  100  cc. 

Solvent.  Solvent. 

Water                    15        1.4    (i)  CHaOH                                         25      0.345  (3 

15-20      1.6    (2)  CHCU                                           25      1.25    (3 

25         2.38(4)  i  vol.  CJfcOH+4  vols.  CHO.     25       5          (3 

80      12.5    (4)  i  vol.  C2HfiOH+4  vols.  C6H6        25      0.66    (3 


9o%C2H6OH     15-20      0.83 

i5        0.77 
b.  pt.      3.45 


2)       i  vol.  CHaOH+4  vols.  CHCU      25       4          (3 
i)      i  vol.  CHaOH+4  vols.  C6H6         25       i          (3 


i)      Glycerol  25      1.66   (4) 

100%  CzHfiOH       2*5        0.37  (3) 

(i)  Dottdgio);  (2)  Squire  and  Caines  (1905);  (3)  Schaefer  (1913);   (4)  U.  S.  P.  VIII  ed. 


DISTRIBUTION  OF  STRYCHNINE  NITRATE  BETWEEN  WATER  AND  CHLOROFORM 

AT  25°. 

(Seidell,  igioa.) 

Gms.  CzjH-aNzOis.HNOa        Gms.  Q^zjNzOz.HNOs  per  15  cc.:  a 

Added  per  15  cc.  t • *• \  -• 

HjO  +  15  cc-CHCla.        H2O  Layer  (a).  CHC13  Layer  (b). 

0.005  0.0051  o.oo3o(?) 

0.025  0.0222  0.0042  5.3 
0.125  O.IOI7  0.0243  4-2 
0.625  0.3250  0.1698  2 

STRYCHNINE  OXALATE 

loo  gms.  H2O  dissolve  1.13  gms.  of  the  anhydrous  salt  at  about  15°. 

(Dott,  1910.) 

STRYCHNINE  PERCHLORATE  C21H22N2O2.HC1O4. 

100  gms.  HaO  dissolve  0.022  gm.  perchlorate  at  15°. 

(Hofmann,  Roth,  Hobold  and  Metzler,  1910.) 


689 


STRYCHNINE   SULFATE 


STRYCHNINE   SULFATE 


SOLUBILITY  IN  SEVERAL  SOLVENTS. 


Solvent. 
Water 
« 
90%  C2H6OH 

94%        " 
94%        " 
100%        " 
CHaOH 

t°. 

15-20 

25 
80 
15-20 

25 
60 

25 
25 

Gms.  Salt 
per  ioo  cc. 
Solvent. 
2.08  (i) 
3-23  (2) 

16.6    (2] 
0.74  (i) 
1.9    (') 

6.2        2 

0.8     3 
8-33    3 

Solvent. 


CHCU 


i  vol.  C2H50H+4vols.  CHCU 
i  vol.  C2H50H+4  vols.  CeHe 
i  vol.  CHsOH+4  vols.  CHCls 
i  vol.  CHaOH+4  vols. 
Glycerol 


15 

25 
25 
25 
25 
25 
25 
15 


Gms.  Salt 
per  ioo  cc. 
Solvent. 
0.05 
0.31 

0-43 
12.8 

0.725  (3) 
25  (3) 
12.5 

18 


(4) 

8 
8 

(3) 

I 


(i)  Squire  and  Caines  (1905);  (2)  U.  S.  P.  VIII;  (3)  Schaefer  (1913);  (4)  Hill  (1910). 


d  Tartrate. 

/  Tartrate. 

Racemic  Tartrate, 

14.14 

9.48 

14.02 

17.72 

11.50 

19.12 

22.9 

I4-52 

24.70 

15.60 

17.02 

35-18 

22.90 

38.42 

STRYCHNINE  TARTRATE 

SOLUBILITY  OF  d,  I  AND  OF  RACEMIC  STRYCHNINE  TARTRATE  IN  WATER. 

(Dutilh,  1912.) 

Gms.  of  Each  Separately  per  1000  gms.  H2O.     ,. 
t°.  d  Tarti 

7-35 
16 

25 
27 
30 
40 

SOLUBILITY  OF  MIXTURES  OF  d  AND  /  TARTRATES  AND  OF  RACEMIC  STRYCHNINE 
TARTRATE  IN  WATER. 

(Ladenburg  and  Doctor,  1899.) 

Results  for  d  +  /  Tartrate.  Results  for  Racemic  Tartrate. 

Gms.  Anhydrous  Gms.  Anhydrous. 

t°.            Salt  per  ioo  Gms.  Solid  Phase.                   t°.          Salt  per  ioo  Gms.        Solid  Phase. 

H20.  H20. 

7                      1.48  S°%d+S%l                   7                     1-39             Racemic  Tartrate 

19  i-95  *9  i-90 

27  2.38  27  2.33 

35  3-02  35  3-i7 

42  3-75  42  3-92 

ioo  gms.  sat.  solution  in  water  contain  0.45  gm.  anhydrous  strychnine  acid 
tartrate  at  about  15°.  (Dott,  1910.) 

SUBERIC   ACID  C6H12(COOH)2. 

SOLUBILITY  IN  WATER. 

(Lamouroux,  1899.) 
t°.  o°.  15°.          20°.         35°. 

Gms.  CeHi2(COOH)2  per  ioo  cc.  sol.      0.08    0.13    0.16    0.45 


50°. 

0.98 


65°. 

2.22 


SOLUBILITY  OF  SUBERIC  ACID  IN  ALCOHOLS  AT  4°. 

(Timofeiew,  1894.) 

Gms.  C6Hi2(COOH)2  per  ioo  Gms. 


Alcohol. 


Sat.  Sol.  Alcohol. 

Methyl  Alcohol  20.32  3  2  .  04 

Ethyl  Alcohol  15.5  1  8  .  44 

Propyl  Alcohol  12.2  13.9 

ioo  gms.  95  per  cent  formic  acid  dissolve  2.13  gms.  C6Hi2(COOH)2  at  19.5°. 

(Aschan,  1913.) 

Data  for  the  distribution  of  suberic  acid  between  water  and  ether  at  25°  are 
given  by  Chandler,  1908. 


SUCCINIC  ACID 

SUCCINIC  ACID  (CH2)2(COOH)2. 


690 


SOLUBILITY  IN  WATER. 

(Miczynski,  1886;   van  der  Stadt,  1902;   Lamouroux,  1899;    for  other  concordant  results,  see  Bourgoin, 

1874;  Henry,  1884.) 


*°-                  Gms.  (CH2)2(COOH)2  per  too 

Gms.  Succinic 
Anhydride 
(CH2)2COCOO 
per  too  Gms. 

Mol. 

Per  cent. 

Gms.  H2O. 

cc.  Solution. 

H20. 

(CH2)2COCOO: 

H2O. 

0 

2.80 

2.78(L.) 

2-34 

99.58 

0.42 

IO 

4.51 

4 

3-80 

99-32 

0.68 

20 

6.89 

5-8 

5-77 

98.97 

1.03 

25 

8.06 

7 

6.74 

98.80 

1.20 

30 

10.58 

8-5 

8.79 

98.44 

1.56 

40 

16.21 

12.5 

13-42 

97.64 

2.36 

50 

24.42 

18 

19-95 

96.53 

3-47 

60 

35.83 

24-5 

28.77 

95-07 

4-93 

70 

51.07 

40.  ii 

93.26 

6.74 

80 

70.79 

54.08 

91.12 

8.88 

89.4 

95-4.' 

70.62 

88.71 

ii.  29 

104.8 

146.3 

IOI.2 

84.57 

15-43 

II5.I 

188.5 

126.8 

81.4 

18.6 

134-2 

335-4 

187.8 

74-72 

'  25.28 

159-5 

748.2 

295.2 

65.27 

34-73 

180.6 

1839 

.  .  . 

408.5 

57-6 

42.4 

182.8 

00 

542-3 

5° 

50 

174.4 

.  .  . 

.  .  . 

808.5 

40.7 

59-3 

153.3 

.  .  . 

2239 

19.86 

80.14 

128 

.  .  . 

8865. 

5-89 

94.11 

II8.8-II9 

00 

0 

100 

The  following  very  careful  determinations  of  the  solubility  of  succinic  acid 
in  water  are  given  by  Marshall  and  Bain  (1910). 

t°.  o°.  12.5°.  25°.         37.  S°-          50°-  62.5°.  75°. 

Gms.  (CH2)2  (COOH)2 

per  100  gms.  H2O       2.75       4.92       8.35       14       23.83       39.35       60.37 

SOLUBILITY  OF  SUCCINIC  ACID  IN  AQUEOUS  SOLUTIONS  OF  SALTS  AND  OF 

ACIDS  AT  25°. 

(Herz,  igiob,  1911.) 


In  Aq.  HBr. 

Gms.  per  Liter. 

In  Aq.  HC1, 

Gms.  per  Liter. 

In  Aq.  KBr. 

Gms.  per  Liter. 

In  Aq.  KC1. 

Gms.  per  Liter. 

HBr. 

C4H604. 

HC1.              C4H6O4. 

KBr.            C4H6O4. 

KC1. 

C4H604. 

0 

8l.2I 

18.45        66. 

25 

0 

81. 

21 

28.34 

75.58 

79- 

3 

57-38 

45-6          50, 

,78 

65- 

45       75- 

58 

77.56 

74-39 

274- 

4 

32.83 

87-9          35 

,42 

260. 

5        69. 

68 

150.7 

69.68 

166.6          27 

•75 

502. 

i        62. 

59 

267 

61.41 

In  Aq. 

KI. 

In  Aq.  LiCl. 

In 

Aq.  NaCl. 

Gms.  per  Liter. 

Gms.  per  Liter. 

Gms 

.  per  Liter. 

Solid 

KI. 

C4HeO4. 

LiCl. 

C4He04- 

'  NaCl. 

C4H604. 

Phase. 

0 

8l.2I 

0 

81. 

21 

l8.7 

74-39 

C4Hfl04 

46, 

,48 

79-12 

7.63 

70. 

86 

32.73 

69.68 

" 

102 

9 

77-93 

23.32 

62. 

59 

64.3 

61.41 

H 

,  '  , 

57-66 

47- 

24 

I32.I 

49-55 

" 

ny 

29. 

Si 

289.4 

27.16 

" 

176.4 

20. 

07 

3I5-I 

22.44 

NaCl 

231-5 

14. 

318 

4-72 

" 

691 


SUCCINIC   ACID 


SOLUBILITY  OF  SUCCINIC  ACID  IN  AQUEOUS  SOLUTIONS  OF  POTASSIUM 

SUCCINATE  AND   VlCE   VERSA  AT   SEVERAL   TEMPERATURES. 

(Marshall  and  Cameron.  1907.) 


Gms.  per  100  Gms 
4o.             Sat.  Sol. 

Solid  Phase. 

Gms.  per  100  Gms. 
t°.             Sat.  Sol. 

Solid  Phase. 

H2C4H404. 

K2C4H4O4.                                                     H2C4H4O4. 

K2C4H404. 

0 

2 

•71 

o 

H2C4HA     • 

25 

7-88 

0 

H2C4H404 

0 

7 

,26 

8. 

09 

"  +KH3(C4HA)2 

25 

9- 

965 

3- 

17 

" 

o 

7 

.86 

7- 

66 

"              " 

25 

12. 

77 

8. 

4 

" 

0 

8 

.24 

9- 

95 

KH3(C4HA)2 

25 

17- 

6 

14- 

15 

cc 

0 

8, 

.  ii 

12. 

77 

" 

25 

18. 

i 

14- 

3 

"  +KH,(CJH,04), 

0 

7-87 

15- 

47 

"  +KHC4H4O4.2H2O 

25 

15- 

36 

18. 

48 

KH3(C4H404)2 

0 

0 

40. 

2 

K2C4H404.3H20 

25 

7 

23- 

6 

"  H-KHC^O* 

14 

i 

.468 

41. 

3 

K2C4H404+KHC4H4O4 

25 

13- 

06 

23- 

81 

KHC4H4O4 

+KHC4H4O4.2H20 

25 

ii. 

98 

24. 

43 

" 

15. 

9  i 

-7 

34- 

36 

KHC4H404.2H2O+KHC4H4O4 

25 

9-97 

25 

" 

20 

6 

•39 

o 

H2C4H4O4 

25 

6. 

61 

28. 

6 

" 

20 

7 

.48 

i. 

85 

" 

25 

2. 

6 

38. 

2 

" 

20 

14 

•63 

ii. 

64 

" 

25 

2. 

ii 

40. 

6 

CC 

20 

15 

•03 

13- 

32 

"  +KH3(C4H404)2 

25 

I, 

<>3 

48. 

7 

"  +K2C4H404.3H20 

20 

13 

•32 

18. 

46 

KHsCC^O^z 

25 

0. 

13 

56. 

IS 

K2C4H404.3H20 

20 

12 

-74 

22. 

45 

"  +KHC4H404 

25 

O 

58. 

05 

" 

20 

II 

-7 

22. 

91 

KHC4H4O4 

40 

12, 

9 

0 

H2C4H404 

20 

I 

42. 

I  ' 

" 

40 

25 

•  5 

16. 

83 

"  +KH3(C4H4O4)2 

20 

I 

•05 

47- 

3 

"  +K2C4H404.3H20 

40 

19 

25- 

481 

^-  H-3^  04^X404)  2"i    K.  XI  (^4X14^ 

20 

O 

•985 

48. 

i 

K2C4H404.3H20 

40 

*5 

•83 

26.56 

KHC4H4O4 

20 

0 

.909 

48. 

75 

" 

40 

o 

62. 

10 

KjC^C^HjO 

20 

o 

-159 

54- 

3 

" 

20 

0 

56.6 

SOLUBILITY  OF  SUCCINIC  ACID  IN  ALCOHOLS  AND  IN  ETHER. 

(Timofeiew,  1891,  1894;  at  15°,  Bourgoin,  1878.) 


Solvent. 

Abs.  Methyl  Alcohol 
Abs.  Ethyl 
90%      " 
Abs.  Propyl 
Abs.  Ether 
Isobutyl  Alcohol 


Gms.  (CH2)2(COOH)2  per  100  Gms.     Solvent  at: 


10.51 
5.06 

2. II 


+15°. 

12.59 
7-51 

1.265 


+21-5°. 

19.40 

9-49 
4-79 
2-73 


+39°- 
28.7 
15 

7-53 


loo  gms.  95  per  cent  formic  acid  dissolve  2.06  gms.  (CH2)2(COOH)2  at  18.5°. 

(Aschan,  1915.) 


DISTRIBUTION  OF  SUCCINIC  ACID  BETWEEN  WATER  AND  AMYL  ALCOHOL 

AT  20°. 

(Herz  and  Fischer,  1904.) 


Millimols  JC4H«O4 
per  10  cc. 

Gms.  C4H«O4 
per  100  cc. 

Millimols  iC4H«O4 
per  10  cc. 

Gms.  C4HgO4 
per  100  cc. 

Alcohol 
Layer. 

0.1888 

0.3643 
0.7077 
1.440 
2.715 

Aq. 
Layer. 

0.2684 

0.5252 

1-0373 
2.1266 
4.0495 

Alcohol 
Layer. 

o.  1114 

0.215 
0.418 
0.850 
1.603 

Aq. 
Layer. 

0.1584 
0.310 

0.612 

1.255 
2.391 

Alcohol 
Layer. 

3.899 
5-199 

6-334 
7.119 

Aq. 
Layer. 

6.0795 
8.099 

10.  170 

11.555 

Alcohol 
Layer. 

2.302 
3.069 

3-739 
4.202 

Aq. 
Layer. 

3-588 

4-779 
6 
6.821 

SUCCINIC  ACID 


692 


SOLUBILITY  OF  SUCCINIC  ACID  IN  AQUEOUS  ACETONE  AT  20°. 

(Herz  and  Knoch,  1904.) 


cc.  Acetone  per 
zooicc.  Solution. 

O 
10 

20 

30 
40 
50 


C4HgO4  per  100  cc.  Solution. 


Millimols. 
107.8 
127.4 
155-8 
186.7 
225-4 
254-3 


Gms. 
6.363 
7.5I9 
9.194 
II. O2 
I3.30 
15.01 


cc.  Acetone  per 
100  cc.  Solution. 

C4H6O4  per  zoo  cc.  Solution 

Millimols.                Gms. 

60 

275.7                16.27 

70 

278.5                16.44 

80 

265.3                15-66 

90 

201.9                11.91 

iOO 

5L5                  3-04 

SOLUBILITY  OF  SUCCINIC  ACID  IN  AQUEOUS  GLYCEROL  SOLUTIONS  AT  25°. 

(Herz  and  Knoch,  1905.) 


Wt.  % 
Glycerol  in 
Solvent. 

C4H6O4  per  100  cc. 
Solution. 

Sp.  Gr.  of 
Solutions. 

Wt.  % 
Glycerol  in 
Solvent. 

C4H« 

iO4  per  zoo  cc. 

solution. 

Sp.  Gr.  of 

Solutions. 

Millimols. 

Gms. 

Millimols. 

Gms. 

0 

133 

•4 

7.874 

I 

.0213 

40.95 

105. 

8 

6.244 

I.  I  I  20 

7- 

15 

128 

.2 

7.566 

I 

.0407 

48.70 

99. 

9 

5.896 

1.1298 

20. 

44 

118 

•3 

6.982 

I 

.0644 

69.20 

88. 

5 

5.223 

I  .  1804 

31- 

55 

109 

•7 

6.476 

I 

.0897 

IOO* 

74- 

6 

4.440 

1.2530 

*  Sp.  Gr.  of  Glycerol  =  1.2555.    Impurity  about  1.5  per  cent. 

DISTRIBUTION  OF  SUCCINIC  ACID  BETWEEN  WATER  AND  ETHER  AT 

AND  25.5°. 

(Pinnow,  1915.) 


Results  at  15 

Gm.  Mok.  per  Liter. 

0 

c 
c 

6. 
6. 
6. 

Results  at  20 

Gm.  Mols.  per  Liter. 

0 

c 
c' 

6. 
6. 
6. 
6. 

Results  at  25. 

Gm.  Mols.  per  Liter. 

c 

7- 
7- 
7- 

52 
52 
7i 

Aqueous 
Layer  (c). 

0.474 
0.2585 
O.II75 

Ether 
Layer  (c*). 
0.0783 
0.0415 
0.0187 

05 
23 

28 

Aqueous 
Layer  (c). 
0.644 
0.312 
O.I5I 
0.0405 

Ether 
Layer  (c')- 
0.096 
0.046 

0.0218 

O.OO6 

71 
87 

93 
75 

Aqueous 
Layer  (c). 
0.3293 
0.1768 
0.0894 

Ether     " 
Layer  (c'). 
0.0438 
0.0235 

0.0116 

Very  careful  determinations  of  this  distribution  at  o°  and  at  25°,  in  which  the 
ionization  of  the  succinic  acid  in  the  two  solvents  is  taken  into  consideration,  are 
given  by  Chandler,  1908.  Two  determinations  at  o°  and  two  at  15°  are  quoted 
by  Kolossovsky,  1911.  Earlier  data  for  this  system  are  given  by  Nernst,  "  Theo- 
retical Chemistry,"  3rd  English  edition,  p.  496. 

BromSUCCINIC  ACID  CHBr(CH2)(COOH)2  (m.  pt.  159°). 
SOLUBILITY  IN  ALCOHOLS  AT  22°. 

(Timofeiew,  1894.) 

Gms.  CHBr(CH2)(COOH)2  per  100  Gms. 


Methyl  Alcohol 
Ethyl  Alcohol 
Propyl  Alcohol 

Sat.  Solution. 
56-5 

45-5 
33-1 

Alcohol. 
129.7 
83.6 
49.4 

Data  for  the  distribution  of  monobromsuccinic  acid  between  water  and  ether 
at  25°  and  for  dibromsuccinic  acid  between  water  and  ether  at  25°  are  given  by 
Chandler  (1908). 

Data  for  the  melting-points  of  mixtures  of  the  following  pairs  of  optical  anti- 
podes are  given  by  Centnerszwer  (1899). 

d  +  /  Chlorsuccinic  Acid. 

d  4-  i  Chlorsuccinic  Acid. 

d  Chlorsuccinic  Acid  +  I  Bromsuccinic  Acid. 

i  Chlorsuccinic  Acid  + 1  Bromsuccinic  Acid. 

d  +  /  Benzylaminosuccinic  Acid. 

d  -f-  /  Aminosuccinic  Acid. 


693 


SUCCINIMIDE 


SUCCINIMIDE 


CO 


SOLUBILITY  IN  WATER  AND  IN  ETHYL  ALCOHOL. 


Interpolated  from  original  results. 
In  Water. 


(Speyers,  1902.) 


In  Ethyl  Alcohol. 


Wt.of 

Mols.  per 

Cms.  per 

Wt.of 

Mols.  per 

Gms.  per 

t°.                        I  CC. 

100  Mols. 

100  Gms. 

I  CC. 

ioo  Mols. 

ioo  Gms 

Solution. 

H20. 

H20. 

Solution. 

QHfiOH. 

QH6OH 

o            1.025 

1.58 

8.69 

0.815 

0.88 

1.89 

10            1.035 

2.4 

14 

0.809 

i-35 

2.7 

20 

.052 

4 

23 

0.8o6 

2 

4.1 

25 

.067 

5-9 

33 

0.805 

2-5 

5-3 

30 

.086 

8 

45 

0.804 

3-i 

6.8 

4P 

.I2O 

12.8 

70 

0.809 

4.9 

10.5 

50 

•145 

17.8 

96 

0.816 

7.8 

16 

60 

.167 

22.6 

124 

0.835 

12.3 

26.5 

70 

.189 

27.5 

152 

0.873 

80 

.204 

32-8 

0-954 

Freezing-point  data  (solubilities,  see  footnote,  p.  i),  are  given  for  ethylsuc- 
cinimide  +  bromotoluene  and  for  ethylsuccinimide  +  p  xylene  by  Paterno  and 
Ampola  (1897). 

SUCCINIC  NITRILE  (Ethylene  Cyanide)  CNCH2CH2CN. 

The  solubility  of  succinic  nitrile  in  water  and  also  in  aqueous  sodium  chloride 
solutions  at  various  temperatures  has  been  determined  by  Schreinemakers  (1897), 
and  the  results  presented  in  terms  of  mols.  of  nitrile  per  ioo  mols.  of  nitrile  -j-  H2O. 
The  following  calculations  of  these  results  to  gram  quantities  was  made  by 
Rothmund.  (Landolt  and  Bernstein's,  "  Tabellen  "  1906.) 


t°. 

18.5 

20 

39 
45 


Gms.  CNCH2CH2CN  per  ioo  Gms. 


Gms.  CNCH2CH2CN  per  ioo  Gms. 


Aq.  Layer. 
IO.2 
II 

22 


Nitrile  Layer. 
92 

91-5 
85.2 


Aq.  Layer. 
53-5  33-2 

55  40-3 

55.4  crit.  temp. 


Nitrile  Layer. 
66.4 
62.8 


Very  complete  data  for  the  system  succinic  acid  nitrile,  ethyl  alcohol  and 
water,  determined  by  the  synthetic  sealed-tube  method,  are  given  by  Schreine- 
makers  (i8o.8c).  Results  for  the  system  succinic  acid  nitrile,  cane  sugar  and 
water  are  given  by  Timmermans  (1907). 

SUGAR  Ci2H22Ou  (Cane  Sugar.) 

SOLUBILITY  IN  WATER. 

(Herzfeld,  1892;  see  also  Courtonne,  1877.) 
per 


ioo  Gms. 


O 

5 
10 

15 

20 
25 
30 

35 


Solution. 

Water. 

64.18 

179.2 

64-87 

184.7 

65.58 

190.5 

66.33 

197 

67.09 

203.9 

67.89 

2II.4 

68.70 

219.5 

69.55 

228.4 

40 

45 


70 

80 

90 

ioo 


Gms.  CigHaOu  per 
ioo  Gms. 

Solution. 

Water. 

70.42 

238.1 

71.32 

248.7 

72.25 

260.4 

74.18 

287.3 

76.22 

320.4 

78.36 

362.1 

80.  61 

415.7 

82.97 

487.2 

Sp.  Gr.  of  sat.  solution  at  15°  =  1.329;  at  25°  =  1.340. 

ioo  gms.  H2O  dissolve  212  gms.  cane  sugar  at  25°,  determined  by  means  of 
Pulf rich's  refractometer.  (Osaka,  1903-08.) 


SUGAR 


694 


SOLUBILITY  OF  SUGAR  IN  AQUEOUS  SALT  SOLUTIONS  AT  30°,  50°,  AND  70°. 


Interpolated  from  original  results. 


(Schukow,  1900.) 


Gms. 


per  100  grams  EfeO  in  Aq.  Solution  of: 


loo  Gms.  H2O.   KC1. 

KBr. 

KN03. 

Nad. 

CaCl2. 

3? 

0 

219.5 

219.5 

219.5 

219.5 

219.5 

10 

216 

218 

217 

2IO 

197 

tt 

20 

221 

22O 

216 

211 

189 

" 

30 

228 

224 

216 

219 

I92 

M 

40 

237 

228 

217 

233 

20O 

K 

50 

218 

25O 

218 

M 

60 

269 

243 

50 

0 

260.4 

260.4 

260.4 

260.4 

260.4 

(i 

10 

26l 

262 

260 

255 

239 

(I 

20 

266 

266 

261 

260 

228 

« 

30 

274 

272 

262 

269 

228 

U 

40 

284 

276 

262 

284 

236 

" 

50 

296 

280 

263 

302 

253 

(< 

60 

276 

70 

0 

320.5 

320.5 

320.5 

320.5 

320. 

(C 

10 

326 

324 

321 

323 

295 

u 

20 

334 

328 

324 

330 

286 

u 

30 

345 

334 

327 

344 

286 

n 

40 

357 

34i 

33i 

361 

295 

u 

50 

37° 

349 

•  334 

384 

308 

u 

00 

384 

357 

337 

406 

327 

SOLUBILITY  OF  CANE  SUGAR  IN  SATURATED  AQUEOUS  SALT  SOLUTIONS  AT 

31.25°.    (Kohler,  1897.) 


Salt. 

CH3COOK 
C3H7COOK 
C3H4.OH.(COOK)3 
.K2C08 
KC1 

CH3COONa 
NaCl 


Gms.  Sugar  per  100  Gms. 
Solution. 

49.19 

56.0 
62.28 

59-93 
62.17 


Water. 
324.8 
306.1 

265.4 
246.5 
237.6 
236.3 


Gms.  Sugar  per  100  Cms- 


Solution. 

Na2C03          64-73 
KNO3            61.36 
K2S04            66.74 
CH3COOCa  60.12 

Na2SO4           52.20 
CaCl2              42-84 
MgS04           46-52 

Water. 
229.2 
224.7 
219.0 
190.0 
I83-7 
I35-I 
119.6 

SOLUBILITY  OF  CANE  SUGAR  IN  AQUEOUS  ALCOHOL  SOLUTIONS  AT  14°. 

(Schrefeld,  1894.) 


Wt. 

per  cent 
AlcohoL 

Wt. 
per  cent 
Sugar. 

Gms.  Sugar  per  100 
CC.  Alcohol-H2O 
Mixture. 

Wt. 

per  cent 
Alcohol. 

Wt. 
per  cent 
Sugar. 

Gms.  Sugar  per  100 
cc.  Alcohol-HsO 
Mixture. 

0 

66.2 

I95.8 

50 

38.55 

62.7 

5 

64.25 

179.7 

60 

26.70 

36.4 

10 

62.20 

164.5 

70 

12.25 

13-9 

20 

58.55 

141  .2 

80 

4.05 

4-2 

30 

54-05 

II7.8 

90 

o-95 

0-9 

40 

47-75 

91  . 

IOO 

c-oo 

O-O 

695 


SUGAR 


SOLUBILITY  OF  CANE  SUGAR  IN  AQUEOUS  ALCOHOL  SOLUTIONS. 

(Scheibler,  1872;  correction,  1891.) 


Results  at  o°. 

Results  at  14°. 

Results 
at  40°. 

Per  cent 

Sp.  Gr.  of 

Cms.  Sugar        Sp.  Gr.  of 

Cms. 

per  100  cc.  Solution. 

Gms.  Sugar 

Alcohol 

Solution  a,t 

per  100  cc.        Solution  at 

A 

per  100  cc. 

by  Vol. 

17.5°. 

Solution.              17-5°. 

Sugar. 

C2H5OH. 

H20. 

Solution. 

O 

1-325 

85.8       1.326 

87.5 

0 

45-iQ 

IO 

1.299 

80.7 

•  300 

8l-5 

3-91 

44.82 

95-4 

20 

1.236 

74.2 

.266 

74-5 

8.52 

43-83 

90 

30 

1.229 

65-5 

•233 

67.9 

13-74 

41.87 

82.2 

40 

1.182 

56.7 

.185 

58 

20.  24 

40.38 

74-9 

50 

1.  129 

45-9 

•131 

47-1 

28.13 

38.02 

63-4 

60 

1.050 

32.9 

.058 

33-9 

37-64 

34-47 

49-9 

70 

0.972 

18.2          0.975 

18.8 

46.28 

29-57 

3i-4 

80 

0.893 

6.4          0.895 

6.6 

6I.I5 

21.95 

13-3 

90 

0.837 

0.7          0.838 

0.9 

7I.I8 

12.83 

2-3 

97-4 

0.806 

0.08        0.808 

0.36 

77-39 

3-28 

0-5 

100  gms.  absolute  methyl  alcohol  dissolve  1.18  gms.  cane  sugar  at  19°. 

(de  Bruyn,  1892.) 


SOLUBILITY  OF  CANE  SUGAR  IN 

AQUEOUS  ACETONE  AT  25°. 

(Herz  and  Knoch,  1904.) 

Sp.  Gr.  of 

cc.  Acetone 

Gms.  Sugar 

Gms.  per  100  cc. 

Solution. 

Solutions. 

Solvent. 

Solution. 

H20. 

(CH3)2CO 

CiuHaOn 

1.3306 

0 

89.8 

43-3 

0 

89.8 

1.2796 

20 

76.7 

42.9 

8.4 

76.7 

1.2491 

30 

72.1 

39-5 

13-4 

72.1 

1.2002 

40 

59-3 

39-8 

20.9 

59-3 

I.  1613 

45 

52.5 

39 

24.6 

52-5 

Above  45  cc.  acetone  per  100  cc.  solvent  the  solution  begins  to  separate  into 
two  layers.  The  lower  of  these  contains  51  gms.  sugar  per  100  cc.  and  has  Sp. 
Gr.  1.1522.  The  upper  layer  contains  so  little  sugar  that  the  amount  could  not 
be  determined  by  the  method  employed.  100  cc.  evaporated  in  a  vacuum  desic- 
cator left  a  residue  of  3.68  gms.  Above  the  concentration  of  80  cc.  acetone  per 
100  cc.  solvent  the  two  layers  unite.  In  pure  acetone  100  cc.  solution  gave  a 
residue  of  0.18  gm.  sugar. 


Sugar. 

Cane  Sugar  (Sucrose) 

Milk  Sugar  (Lactose) 

Grape  Sugar  (Glucose) 

Fruit  Sugar  (Fructose) 

Galactose 

Maltose 

Mannose 

Raffinose 


SOLUBILITY  OF  SEVERAL  SUGARS  IN  PYRIDINE  AT  26°. 

(Holty,  1905.) 

Gms.  Sugar 


Formula. 


d  C6H12O6.H20 


CeHxA 
C18H32016.5H20 


J26  of  Sat.  Sol. 

per  100  Gms. 

Sat.  Sol. 

6-45 

0.981 

2.18 

1.005 

7.62 

1.052 

18.49+ 

1.0065 

5-45(?) 

98.10* 

.  .  . 

29.9* 

75* 

(Dehn,  1917.) 


*  It  is  uncertain  whether  these  figures  refer  to  gms.  per  100  gms.  sat.  solution  or  gms.  per  100  gms. 
pyridine  at  2o°-2S°. 

100  gms.  aq.  50  per  cent  pyridine  dissolve  the  following  gms.  of  sugars  at  20°- 

25°;    sucrose,  38.5;    maltose,  43.07;    mannose,  78.70;    lactose,   1.98;    fructose, 

85.42;   galactose,  68.3;   glucose,  49.17;  raffinose,  8.76.  (Dehn,  1917.) 

100  gms.  trichlorethylene  dissolve  0.004  gm.  cane  sugar  at  I5°-  (Wester  &  Bruins,  1914.) 

For  additional  data  on  Galactose,  see  p.  305  and  on  Glucose,  see  p.  306. 


SUGARS 


696 


SOLUBILITY  OF  MILK  SUGAR  (LACTOSE)  HYDRATE  AND  ft  ANHYDRIDE  IN 

WATER. 

(Hudson,  1904,  1908.) 

It  was  found  that  the  saturation  point  was  reached  very  slowly  with  this 
compound.  From  the  results,  it  was  concluded  that  "aqueous  solutions  of 
milk-sugar  contain  two  substances  in  equilibrium  and  that  the  mutarotation  of 
milk-sugar  results  from  the  slow  establishment,  in  cold  solutions,  of  the  equi- 
librium of  the  balanced  reaction,  Ci2H24Oi2  (Hydrate)  <=±  H2O  +  Ci2H22Ou  (ft-an- 
hydride). 

The  final  solubility  of  hydrated  milk  sugar  was  determined  by  approaching 
saturation  from  below  and  from  above  with  mixtures  of  water  and  excess  of  once 
recrystallized  hydrated  milk  sugar.  These  were  constantly  rotated  until  equilib- 
rium was  reached  (one  week  was  allowed  in  all  cases).  The  filtered  saturated 
solutions  were  evaporated  to  dryness  and  the  crystalline  residues,  consisting  of 
the  a  and  ft  anhydrides,  weighed. 


o 

15 
25 

39 


Cms.  CuHsAi 

per  100  Gms. 

Sat.  Sol. 

10.6 

14-5 
17.8 

24 


t-. 

49 
64 
74 
89 


Gms. 
per  100  Gms. 
Sat.  Sol. 

29.8 

39-7 
46.3 
58.2 


The  initial  solubility,  obtained  by  agitating  an  excess  of  milk  sugar  hydrate 
with  water  for  a  few  minutes,  was  somewhat  less  than  one-half  the  above  figures, 
at  temperatures  up  to  25°. 

The  final  solubility  of  ft  anhydrous  milk  sugar  was  difficult  of  determination 
on  account  of  the  high  concentration  and  instability  of  the  saturated  solution 
below  92°.  At  o°  the  final  saturation  was  hastened  by  addition  of  o.i  n  NHaOH 
solution.  At  o°,  42.9  gms.  Ci2H22On  per  100  gms.  sat.  solution  were  found  and 
at  1 00°,  61.2  gms. 


SOLUBILITY  OF  SEVERAL  SUGARS  IN  AQUEOUS  ALCOHOL  AT  20°. 


(Hudson  and  Yanovsky,  1917.) 


Sugar. 

a.  Arabinose 
ft  Cellose 
ft  Fructose 

ft        « 

ft        " 

a  Galactose 

a         " 

ft,  a  Glucoheptose 

a  Glucose 

a. 

a       "       hydrate 

ft  Glucose 

a  Lactose  hydrate 

a  Lyxose 

ft  Maltose  hydrate 

ft  Mannose 

ft 

ft  Mellibose  Dihydrate 

a  Rhamnose  Hydrate 

a.          " 

a  Xylose 

Sucrose 

Trehalose  Dihydrate 

Raffinose  Pentahydrate 


Gms.  Anhydrous  Sugar 

Formula. 

Solvent. 

per  100  cc. 

Solution. 

Initial 

Final 

Solubility. 

Solubility. 

CSHM05 

80%  C2H5OH 

0.74 

1.94 

CpHaOu 

20%            « 

3-2 

4-7 

C.H^O, 

80%            " 

13-4 

27.4 

it 

95%        " 

1.8 

4-2 

" 

Methyl  Alcohol 

5-2 

ii.  i 

QHtfOg 

60%  C2H6OH 

i.i 

3-  r 

" 

80%        " 

0.27 

0.65 

C7Hi4O7 

20%            " 

4 

4-5 

C,H1204 

80%            " 

2 

4-5 

Methyl  Alcohol 

0.85 

1.6 

C6H1206.H20 

80%  C2H6OH 

I-3 

3 

C,H1206. 

80%        " 

4-9 

9.1 

CaByOuJB^O 

4o% 

i.i 

2.4 

C5HU05 

QO%               " 

5-4 

7-9 

CaHaOu.HiO 

60%               " 

3 

4-75 

80%               " 

2.4 

13 

" 

Methyl  Alcohol 

0.78 

4-4 

Ci2H22O4.2H2O 

80%  C2H5OH 

0.76 

j.j 

C6HU06.H20 

100%        « 

8.6 

9-5 

" 

70%        " 

8.2 

9.6 

CBH1005 

80%        " 

2.7 

6.2 

CaHaOu 

80%        " 

3-7 

3-7 

CuHaOu.aHtO 

70%        " 

1.8 

1.8 

CigHszOjg.sHzO 

50%        " 

1.4 

1-4 

697  SUGARS 

SOLUBILITY  OF  SORBOSE  AND  GULOSE  IN  WATER  AND  ALCOHOLS. 

(de  Bruyn  and  van  Ekenstcin,  1900.) 

Gms.  Sugar  per  100  cc.  Sat.  Sol.  in: 
Sugar.  M.-pt. 


H,O  at  100°.  CH3OH  at  17°.  QHBOH  at  17°. 

d  Sorbose  151  0.22  1.70  1.02 

/  Sorbose  150  0.23  1.68  i 

/  Gulose  150  0.24  1.72  1.04 

100  gms.  H2O  dissolve  108  gms.  maltose  at  2O°-25°.  (Dehn,  1917.) 

100  gms.  H2O  dissolve  14.3  gms.  raffinose  at  2O°-25°.  " 


SOLUBILITY  OF  PHENYLHYDRAZONES  AND  /3  NAPHTHYLHYDRAZONES  OF  THE 
SUGARS  IN  WATER  AND  IN  ALCOHOLS  AT  i6°-i8°. 

(van  Ekenstein  and  de  Bruyn,  1896.) 

The  hydrazones  were  prepared  by  adding  to  a  concentrated  and  warm  solution 
of  the  sugar  the  equivalent  quantity  of  the  hydrazine  dissolved  in  the  molecular 
quantity  of  glacial  acetic  acid.  The  precipitated  hydrazones  were  recrystallized 
from  30  to  50  per  cent  alcohol.  No  details  in  regard  to  the  method  of  obtaining 
saturation  or  of  analysis  of  the  solutions  are  given. 

Gms.  Compound  per  too  cc.  Sat.  Sol.  in: 
Phenylhydrazone  of:  M.-pt. 


Water.  CH3OH.  QH5OH. 

Methyl  Mannose  178  0.2-0.06  0.59  0.05-0.02 

Arabinose  161 

"       Rhamnose  124  "              very  si.  sol.  " 

"       Galactose  180 

Ethyl  Galactose  169  ...  ...  o.  i 

Mannose  159  ...  ...  0.2 

"     Arabinose  153  ...  ...  0.4 

"     Rhamnose  123  ...              very  si.  sol. 

Amyl  Galactose  116  ...  ...  0.6 

'     Mannose  134                ...  3.5 

'     Arabinose  120                ...  3.6 

Rhamnose  99  ...              very  si.  sol.  6.5 

Glucose  128  ...  ...  1.2 

'     Lactose  123  ...  ...  0.4 

Allyl  Galactose  157  ...  ...  0.3 

"     Mannose  142  ...  0.7 

"     Arabinose  145  ...  0.5 

Rhamnose  135  ...  ...  ... 

Glucose  155 

Lactose  132  ...  ...  0.2 

"     Melibose  192  ...  ...  0.3 

Benzyl  Galactose  154  ...  0.9  0.08 

"       Mannose  165  ...  °-5S  0-2 

Arabinose  170  ...  0.4  0.06 

Rhamnose  121  ...  15.4  6.7 

Glucose  150  ...  0.5  o.io 

"       Lactose  128  ...  0.9  0.06 

/3  Naphthyl  Galactose  167  0.14  ...  0.24* 

Mannose  157  0.18  ...  0.25* 

Arabinose  141  0.22  ...  0.62* 

Rhamnose  170  0.20  ...  0.44* 

Glucose  95  0.25  ...  5* 

Xylose  70  0.32  ...  6.62* 

Lactose  203  0.07  ...  0.2* 

Maltose  176  ...  ...  0.4* 

Melibose  135  ...  ...  1.3* 

*  Solvent  96  per  cent  CjHjOH. 


SUGARS 


698 


SOLUBILITY  OF  THE  BENZALIC  COMPOUNDS  OF  SOME  POLYATOMIC  ALCOHOLS 

AT    I6°-I8°. 
(de  Bruyn  and  van  Ekenstein,  1899.) 


No  details  of  the  determinations  are  given, 
sufficiently  exact  for  use  in  identifying  hexites. 


Name  of  Compound. 

Dibenzalerythritol 

Monobenzalarabitol 

Dibenzaladonitol 

Dibenzalxylitol 

Dibenzalrhamnitol 

Monobenzal-d-Sorbitol 

Dibenzal-d-Sorbitol 

Tribenzalmanni  tol 

Tribenzal-Mditol* 

Tribenzal-d-talitolt 

Dibenzaldulcitol 

Dibenzalperseitol 


M.-pt. 


2OI   (Fischer) 
152 


175 
203 

175 

I63 

213-8 

215-8 

2IO 

215-20 
230-5 


(Meunier) 


(Fischer) 


It  is  stated  that  the  results  are 


Gms.  Compd.  Dissolved  per  100  cc. 
Sat.  Sol.  in: 


Acetone. 

Chloroform. 

Alcohol. 

0-34 

3.64 

0.02 

0.64 

1*36 

O.I4 

I.  10 

0.85 

0.70 

.2-55 

I.  10 

very 

easily  soluble 

5-44 

o.  16 

O.IO 

0.42 

8-75 

0.10 

0.47 

0.17 

O.O5 

0.30 

4.42 

trace 

0.42 

0.83 

trace 

0.04 

trace 

O.02 

*  Prepared  from  /  idonic  acid.        t  Prepared  from  d  talonic  acid. 

ioo  gms.  sat.  solution  in  pyridine  contain  0.47  gm.  mannitol  at  26°.    (Holty,  1905.) 
100  gms.  sat.  solution  in  pyridine_contain  2.5(?)  gms.  erythritol  at  26°. 


SULFANILIC   ACID   NH2.C6H4.S03H.H2O. 

SOLUBILITY  IN  WATER. 

(Philip,  1913;  results  for  60°  and  over  by  Dolinski,  1905.) 


Solid  Phase. 


NH2.C6H4.SO3H.2H2O 


NH2.C6H4.S03H.H2O 


Gms.  NH2.- 

C6H4.S03H 

t  . 

per  ioo  Gms. 

Sat.  Sol. 

0 

0.444 

7.2 

0.622 

13-3 

0.841 

18.9 

1.093 

18.9 

I.I37 

25-1 

1.384 

31-1 

1.662 

37-2 

2.0O4 

Gms.  NH2.- 

4°. 

C6H4.S03H 

per  ioo  Gms, 

Solid  Phase. 

Sat.  Sol. 

44 

2.44 

NH2.C6H4.S03H.H20 

44 

2.36 

NH2.C6H4.SO3H 

47-5 

2.52 

" 

54-5 

2.85 

u 

60 

3.01 

" 

70 

3.65 

" 

80 

4-32 

" 

IOO 

6.26 

" 

SULFONIUM   PERCHLORATES 

SOLUBILITY  IN  WATER. 

(Hofmann,  Hobold  and  Quoos,  1911-12.) 


Name. 


Formula. 


Trimethyl 
Ethyl   dimethyl 
Propyl        " 
n  Butyl      " 
Ethylene  dismeihyl 
Vinyl  dimethyl 
Trimethylene  dismethyl 


Sulfine  Perchlorate  (CH3)3sciO4 

C2H5(CH3)2SC104 
C3H7(CH3)2SC104 
C4H9(CH3)2SC1O4 
C2H4(C2H6SC104)2 
C2H3.S(CH3)2.C104 


Per  ioo  Gms.  H2O. 

' 

Gm.  Mols. 

=  Gms. 

16.5 

0.0784 

13.84 

15-9 

o.  1191 

22.31 

15 

0.0590 

12.04 

15 

0.0607 

13.24 

18 

0.0423 

14.86 

18 

0.0731 

13.75 

18 

0.0402 

14.68 

699  SULFONIUM   IODIDE 

TriethylSULFONIUM  IODIDE  S(C8H6),I. 

IOO  gms.  H2O  dissolve  431  gms.  S(C2H5)3l  at  25°.  (Peddle  and  Turner,  1913.) 

IOO  gms.  CHC13  dissolve  47.7  gms.  S(C2H6)3l  at  25°.  (Peddle  and  Turner,  1913.) 


SULFUR  S. 

In  a  series  of  papers  by  Aten  (1905-06,  1912,  1912-13,  1913,  1914  and  I9i4a), 
the  preparation  and  properties  of  the  four  known  modifications  of  sulfur  are  de- 
scribed. These  are  designated  by  the  symbols,  S\,  S^,  ST  and  Sp. 

S\  is  ordinary  rhombic  sulfur  and  its  molecule  is  considered  to  be  composed  of 
eight  atoms  of  sulfur,  Ss. 

SM  is  the  insoluble,  so-called  amorphous  sulfur. 

S^  is  obtained  when  ordinary  sulfur  is  heated  above  its  melting-point  and 
quickly  cooled;  it  is  especially  easily  prepared  by  warming  S\  in  sulfur  chloride. 
Its  molecule  is  probably  represented  by  84. 

Sp  was  discovered  by  Engel  and  is  prepared  by  mixing  concentrated  HC1, 
cooled  to  o°,  with  saturated  sodium  thiosulfate  solution.  The  precipitated 
NaCl  is  removed  by  filtration  and  the  solution  extracted  with  toluene.  The 
aqueous  layer  soon  yields  a  cloudy  precipitate  of  Sp.  The  molecule  of  this 
sulfur  is  considered  to  have  the  composition  S6. 


SOLUBILITY  OF  SULFUR  (S\)  IN  SULFUR   MONOCHLORIDE   (SaCk)   DETERMINED 
BY  THE  MELTING-POINT  METHOD. 

(Aten,  1905-06.) 
t°  of  Melting.       M  "*       Solid  Phase.  t°  of  Melting.  '  ™        Solid  Phase. 


Mixure 

—  1  6  4.3  Rhombic  S  83.5  67  Rhombic  S 

06"  95.6  8l.8 

+  17.9  9-9  "  86  8l.8  MonoclinicS 

36.8  I7.I  103.2  88.4 

55.2      28.5  110.4      95 

65.6      40.3  118.8     loo 

77-7      55-4 

SOLUBILITY  OF  SULFUR  (S,-)  IN  SULFUR  MONOCHLORIDE  (S2C12) 

(Aten,  1912-13.) 

A  preliminary  experiment  showed  that  if  a  solution  of  Sx  in  sulfur  monochlo- 
ride,  saturated  at  20°,  is  heated  to  170°  and  cooled,  it  will  then  dissolve  as  much 
Sx  as  already  required  to  saturate  it.  The  following  determinations  were  made 
by  sealing  known  amounts  of  Sx  and  S2C12  in  tubes,  heating  them  to  100°  for 
several  hours  and  then  cooling  quickly  to  the  indicated  temperatures  and  shak- 
ing for  \  hour  in  the  case  of  the  o°  and  25°  results  and  2  hours  in  the  case  of  the 
—  60°  results.  The  saturated  solutions  were  analyzed  by  oxidizing  with  HC1 
+  HNO3  +  Br  and  titrating  the  H2SC>4,  after  removing  the  volatile  acids. 

Atoms  S  per  100  Atoms  S+S2C12  in:  Atoms  S  per  100  Atoms  S+SjClj  in: 


Original                  Saturated  Solution  at:  Original  Saturated  Solution  at; 

Mixture.           ^60°.              o°.              +25°.  '  Mixture.  -60°.              o°.               +25°. 

o              ii. 6        36.1         53.5  79-4  65.2         72 

10              18.1        40.1         57.6  80. i  66.1        71.6 

28.7          31.9        47.4        62  89.9  ...           ...         82.1 

49.9          42.9        56            66.4  90.1  80.5 

60. i          47.7        59.9        69.4  94.6          87.7 

69-1                           ...         72.8  98              93.4 

Results  similar  to  the  above  are  also  given  (Aten,  1912),  for  mixtures  previ- 
ously heated  to  50°,  75°  and  125°.  All  the  data  confirm  the  formation  of  the 
the  new  modification  S*-. 


SULFUR  700 

SOLUBILITY  OF  SULFUR  (S*-)  IN  SULFUR  MONOCHLORIDE  (S2C12)  AT  25°. 

(Aten,  1912,  1913.) 

The  samples  were  heated  to  the  temperatures  indicated  and  rapidly  cooled 
and  powdered.  The  method  of  determining  the  solubilities  is  not  described. 

Atoms  S  Dis- 

Previous  Treatment  of  Sample.  solved  per  100 

Atoms  S+S2C12. 

Unheated  Sulfur  53 . 5 

Mixture  of  Rhombic  and  Amorphous 
Sulfur  54-5 

Rhombic  Sulfur  heated  tO  125°  56-58 .  5  (depending  on  excess  of  S  present.) 

"  "  "          "    165°  60  (determined  immediately.) 

"  "  "         "    165°  59.5  "          after    i  hr.) 

"    165°  57.5  "  "     24hrs.) 

"    165°  53.2  "       8  days.) 

SOLUBILITY  OF  SULFUR  (ST)  IN  TOLUENE  AT  o°  AND  AT  25°. 

(Aten,  1913.) 

Comp.  of  Mix-  Solubility  in  Atom  %  S.  Comp.  of  Mix-  Solubility  in  Atom  %  S. 

ture  in  Atom » .  ture  in  Atom  / • * 

Per  cent  S.  At  o  .  At  25  .  per  cent  S.  At  o  .  At  25  . 

35  2.88  5.94  74  4.05          7.52 

47  6.65  77  3.90 

54  3.26  6.76  80  4.22 

57  3-30  6.88  83  ...  7.93 

73  7-45  85  8.08 

These  results  show  that  the  greater  the  excess  of  Sv,  the  greater  the  solubility. 
It  was  found  that  under  the  same  conditions,  unchanged  rhombic  sulfur  gives 
constant  figures  irrespective  of  the  excess  of  S  present.  At  o°,  2.59  atom  per  cent 
S\  was  found  and  at  25°,  5.65  atom  per  cent. 

SOLUBILITY  OF  SULFUR  (SM)  IN  CARBON  DISULFIDE  AND  CARBON 
TETRACHLORIDE. 

(Wigand,  1910.) 

When  "insoluble"  sulfur  (SM)  is  treated  with  CS2  or  CCU,  a  small  amount 
dissolves,  depending  upon  the  length  of  time  of  contact,  temperature  and  nature 
of  the  solvent  but  not  on  the  relative  amount  of  solvent.  This  action  is  ex- 
plained on  the  assumption  that  a  partial  transformation  of  SM  to  soluble  sulfur 
S\,  takes  place. 

Data  for  the  fusion  points  of  mixtures  of  rhombic  sulfur  and  "insoluble" 
sulfur  (Sj,)  and  for  monoclinic  sulfur  and  "insoluble"  sulfur  (S/J  are  given  by 
Kruyt  (1908). 

SOLUBILITY  OF  SULFUR  IN  LIQUID  AMMONIA. 

(Ruff  and  Hecht,  1911.) 

At  the  temperatures  o°  to  40°,  the  solutions  were  constantly  shaken  for  3  to  4 
days.  For  the  results  at  the  lower  temperatures  the  solutions  were  saturated 
at  room  temperature  then  cooled,  partially  evaporated  and  shaken  4  to  6  hours. 
The  saturated  solutions  were  analyzed  by  evaporation  of  the  ammonia  by  means 
of  a  current  of  hydrogen,  absorbing  in  HCl  and  converting  to  the  platinic  chloride 
for  weighing.  The  S  residues  were  dried  at  100°,  with  proper  precautions,  and 
weighed. 

*o  Gms.  S  per  100  Gms.  f0  Gms.  S  per  100  Cms. 

Sat.  Solution.  Sat.  Solution. 

-78  38.6*  +I6.4  25.65 

-20.5  38.1*  30  21 

o  32.34  40  18.5 

*  This  figure  corresponds  to  the  compound  S(NH3)3  =  38.5%  S. 


yoi  SULFUR 

SOLUBILITY  OF  SULFUR  IN  AQUEOUS  SODIUM  SULFIDE  SOLUTIONS. 

(Kuster  and  Heberlein,  1905.) 

The  results  are  expressed  in  terms  of  x  which  represents  the  number  of  S 
atoms  dissolved  for  each  Na2  in  the  solution.  The  figures,  therefore,  show  the 
atomic  ratio  of  S  to  Naa  in  the  saturated  solution  and  at  the  same  time,  the  sulfur 
content  of  the  compound  NaaSx  which  is  formed.  In  order  to  find  the  actual 
amount  of  sulfur  dissolved  per  liter,  it  is  only  necessary  to  multiply  the  x  value 
by  the  normality  of  the  aqueous  sodium  sulfide  solution  used  as  solvent  in  the 
particular  case. 

A  series  of  determinations  made  at  25°,  by  agitating  aqueous  sodium  sulfide 
solutions  with  crystalline  sulfur  until  equilibrium  was  reached,  and  then  diluting 
each  solution  with  an  equal  volume  of  water  and  shaking  with  excess  of  sulfur 
until  equilibrium  was  again  reached,  gave  the  following  results: 

Normality  of  the  Aq.        *  in  the  Result-  Normality  of  the  Aq.  x  in  the  Result- 

NazS  Solution.  ing  NaaS».  NauS  Solution.  ing  NajS-j. 

4  4-475  0.125  (32hrs.)  5.225 

2  (2  hrs.)  4.666  0.0625  5. 239 

i  4.845  0-03125  5.198 

0.5  4.984  0.015625  5.034 

0.25  5.115  0.007812  (128  hrs.)  4-456 

The  figures  in  parentheses  in  the  above  table  show  the  number  of  hours  re- 
quired for  attainment  of  equilibrium  in  these  three  cases.  The  authors  also 
made  determinations  of  the  influence  of  temperature  on  the  amount  of  sulfur 
dissolved,  and  found  that  for  a  normal  Na2S  solution,  the  x  value  did  not  vary 
appreciably  from  the  figure  given  above,  over  the  range  o°  to  50°. 

Results  are  also  given  showing  the  influence  of  the  presence  of  NaCl  and  of 
KOH  on  the  amount  of  sulfur  dissolved  by  aqueous  Na2S  solutions.  In  the 
former  case  the  solubility  was  distinctly  lowered,  while  in  the  latter  it  was  notably 
increased. 


SOLUBILITY  OF  SULFUR  IN: 

Tin  Tetrachloride.  Amyl  Alcohol. 
(Gerardin,  1865.)  (Gerardin.) 

•••   ~SJ-    as.          -•  -Xar 

99          5.8  SolidS  95  1.5  Solid  S 

101  6.2  "  IIO  2.1-2.2  " 

no          8.7-9.1  "  112  2.6-2.7        Liquids 

112          9.4-9.9        Liquids  120  3.0 

121         17.0  "  131  5.3  " 


SOLUBILITY  OF  SULFUR  IN  AQUEOUS  ACETONE  AT  25°. 

(Herz  and  Knoch,  1905.) 

Wt.  Per  cent  Sulfur  per  100  cc.  Solution.  Sp.  Gr.  of 

in  SoKent.  Millimols.                         Cms. '  Solution. 

ioo  65         2.084  0.7854 

95.36  45         1.442  0.7911 

90.62  33         1.058  0.8165 

85.38  25.3       o.8n  0.8295 


SULFUR  702 

SOLUBILITY  OF  SULFUR  IN  ETHYL  AND  METHYL  ALCOHOLS. 

Cms. 

t*.  Alcohol.  per  100  Gms.  Authority. 

Alcohol. 

15  Abs.  Ethyl  0.051  (Pohi.) 

18.5  O  . 053       (de  Bruyn  —  Z.  physik.  Chem.  10,  781,  'pa.) 

b.  pt.  O  .42         (Payen  —  Compt.  rend.  34,  356,  '52.) 

18.5  Abs.  Methyl  O.O28  (de  Bruyn.) 

SOLUBILITY  OF  SULFUR  IN  BENZENE  AND  IN  ETHYLENE  DIBROMIDE. 

(Etard,  1894;  see  also  Cossa,  1868.) 

In  C6He.  In  C2H4Br2. 


Gms.  S  Gms.  S  Gms.  S  Gms.  S 

t°.  per  loo  Gms.        t°.    per  100  Gms.  t°.     per  100  Gms.      t°.        per  100  Gms. 

Solution.  Solution.  Solution.  Solution. 

o         i -o          70          8.0  o         1.2          50          6.4 

10         1.3  80         10.5  10         1.7  60          8.4 

20  1-7  QO  13.8  20  2.3  70  II.4 

25  2.1  100  17.5  25  2.8  80  16.5 

30         2,4         no         23.0  30        3.3  90         24.0 

40  3.2  120  29.0  40  4.4  100  36.5 

50        4-3         130        36-o 
60        6.0 

RECIPROCAL  SOLUBILITY  OF  SULFUR  AND  BENZENE,  DETERMINED  BY  THE 
SYNTHETIC  METHOD. 

(Kruyt,  1908-09.) 

Wt.  %  S  in     Limiting  t°  of  ^Homogeneity.  \yt.  %  S  in         Limiting  t°  of  ^Homogeneity. 

Mixture.  Lower.  Upper.  Mixture.  '  Lower.  Upper.    " 

41.5  146  247  79.8  141  230 

55.2  158  230  81.4  138      above  246 

74.5  157  226  83.4  131  272 

loo  gms.  sat.  solution  of  S  in  benzoyl  chloride,  C6H6.COC1,  contain  i  gm.  S  at 
o°  and  55.8  gms.  at  134°.  (Bogousky,  1905.) 

SOLUBILITY  OF  OCTOHEDRAL  AND  OF  PRISMATIC  SULFUR  IN  SEVERAL  SOLVENTS. 

(Brdnsted,  1906.) 

The  solubility  of  prismatic  sulfur  could  not  be  determined  in  the  ordinary  way 
on  account  of  its  rapid  transition  to  octohedral  sulfur.  A  special  apparatus  was 
used  which  permitted  the  solvent  to  remain  in  contact  with  the  solid  for  only  a 
short  time.  Since  sulfur  dissolves  very  rapidly,  this  procedure  was  found  to  give 
satisfactory  results.  . 

Gms.  each  Variety  Separately  per 
100  cc.  Saturated  Solution. 

Solvent.  t°.  . • TN 

Prismatic  Octohedral 

Sulfur.  Sulfur. 

Benzene  18.6  2.004  1.512 

25.3  2.335  I-835 

Chloroform  o  i.ioi  0.788 

15-5  1-658  1.253 

40  2.9  2.4 

Ethyl  Ether  o  0.113  0.080 

25-3  0.253  0.200 

Ethyl  Bromide  o  0.852  0.611 

25.3  1.676  1.307 

Ethyl  Formate  o  0.028  0.019 

Ethyl  Alcohol  25.3  o .  066  o .  05  2 


703  SULFUR 

SOLUBILITY  OF  SULFUR  IN  SEVERAL  SOLVENTS. 

Cms.  S  Cms.  S 

Solvent.  t°.     per  100  Gms.  Solvent.  t°.  per  100  Gms. 

Solvent.  Solvent. 

Aniline  130     85.3   (i)     Glycerol  15.5  0.14(4) 

Benzene  15.2    1.5   (2)     Hydrazine  (anhy.)  room  temp.  54(decomP.)(5) 

19.3    1.7   (2)     Lanoline  (anhy.)  45  0.38(6) 

26       0.97(1)     Methylene  Iodide       10  10       (7) 

"  7i       4.38(1)     Nicotine  100  10.6   (8) 

Carbon Tetrachloride  25       0.86(3)     Phenol  174  16.4  (i) 

Chloroform  12.2   0.75(2)     Pentachlor  Ethane      25  1.2   (3) 

19.3   0.92(2)     Toluene  23  1.48(1) 

22       1.21(1)     Tetrachlor  Ethane      25  1.23(3) 

Dichlor  Ethylene        25       1.28(3)     Tetrachlor  Ethylene  25  1.53(3) 

Ethylene  Chloride      25       0.84(3)     Trichlor  Ethylene       25  1.63(3) 

Ethyl  Ether  23.5   0.97(1)  15  1.16(9) 

(i)  Cossa,  1868;  (2)  Bronsted,  1906;  (3)  Hoffman,  Kirmreuther  and  Thai,  1910;  (4)  Ossendowski,  1907; 
(5)  Welsh  and  Broderson,  1915;  (6)  Klose,  1907;  (7)  Retgers,  1893;  (8)  Kleven,  1872;  (9)  Wester  and 
Bruins,  1914. 

SOLUBILITY  OF  SULFUR  IN  CARBON  DISULFIDE. 

(Etard,  1894;  Cossa,  1865;  at  10°,  Retgers,  1893;  below  77°,  Arctowski,  1895-96.) 


0     Gms.  S  per  joo  Gms.          A0 

Gms.  S  per  100  Gms.           ^0 

Gms.  S  per  100  Gms. 

Solution. 

CS2 

Solution. 

CS2. 

Solution. 

CS2.   " 

—  no 

3.0 

3.1 

—  10 

*3-5 

15-6 

50 

59-o 

143.9 

—  100 

3-5 

3-6 

o 

18.0 

22  -O 

60 

66.0 

194.1 

-  80 

4.0 

4.2 

10 

23.0* 

29.9 

70 

72.0 

-  60 

3-5 

3-6 

20 

29-5 

41.8 

80 

79.0 

376.1 

-   40 

6.0 

6.4 

25 

33-5 

50-4 

90 

86.0 

614.1 

—   20 

10.5 

11.7 

30 

38.0 

100 

92  .0 

1150.0 

40 

50.0 

100  .0 

*  26.4  R. 

Sp.  Gr.  of  solution  saturated  at  15°  containing  26  gms.  S  per  100  gms.  solution 
=  1.372. 

SOLUBILITY  OF  SULFUR  IN  HEXANE  (C6Hi4). 

(Etard.) 

to  Gms.  S  per  to  Gms.  S  per  t<>  Gms.  S  per 

100  Gms.  Solution.  100  Gms.  Solution.  100  Gms.  Solution. 

—  20  0.07  60  i.o  130  5.2 

o  0.16  80  1.7  140  6.0 

20  0.25  100  2.8  160  7.2 

40  0.55  120  4.4  180  8.2 

SOLUBILITY  OF  SULFUR-  (Sx)  IN  /3  NAPHTHOL,  DETERMINED  BY  THE 
SYNTHETIC  METHOD. 

(Smith,  Holmes  and  Hall,  1905.) 

The  mixtures  of  sulfur  and  ft  naphthol  were  heated  until  they  were  homo- 
geneous and  then  cooled  to  the  temperature  at  which  clouding  appeared. 


t°of 
Clouding. 

Gms.  S 
per  loo  Gms. 
0  Naphthol. 

t°of 
Clouding. 

Gms.  S 
per  100  Gms. 
0  Naphthol. 

fof 

Clouding. 

Gms.  S 
per  100  Gms. 
/3  Naphthol. 

118 

34 

154 

84.1 

164 

209.7 

132.5 

46.6 

157 

97-4 

163-8 

238.1 

134-5 

48.8 

160.5 

119.3 

163-8 

264.8* 

143-5 

59-3 

162.5 

145.1 

I63 

300* 

149-5 

70 

163.5 

177.6 

*  Solid  phase,  /3  naphthol. 


SULFUR  704 

CJLFUR  IN  COAL  TAR  Oi 

(Pelouze,  1 86s 
Grams  S  per  100  Grams  Coal  Tar  Oil  of:  G   S      r  10 


SOLUBILITY  OF  SULFUR  IN  COAL  TAR  OIL,  LINSEED  OIL  AND  IN  OLIVE  OIL. 

(Pelouze,  1869;  Pohl.) 


4o   Sp.Gr.:     0.87 
*  •  b.  pt.:  8o°-ioo°. 

0.88 
85°-i2o«. 

0.882 

I20°-220° 

0.885 

.    I50°-200° 

.    2IO°-300° 

1.02 
.    220°-300°. 

OU'    0.885  Sp.Gr 

15 

2 

.1 

2. 

3 

2-5 

2 

.6 

6.0 

7.0 

0-4 

2-3 

30 

3 

.0 

4- 

0 

5-3 

5 

.8 

8-5 

8-S 

0.6 

4-3 

SO 

5 

.2 

6. 

i 

8-3 

8 

•7 

IO.O 

12  .O 

I  .2 

9.0 

80 

ii 

.8 

13- 

7 

15-2 

21 

.0 

37-o 

41  -O 

2  .2 

18.0 

100 

15 

.2 

18. 

7 

23.0 

26 

•4 

52-5 

54-o 

3'° 

25.0 

110 

. 

23- 

o 

26.2 

31 

.0 

105.0 

115.0 

3-5 

30.0 

120 

.  . 

. 

27. 

o 

32-0 

38 

.0 

00 

00 

4.2 

37-o 

130 

. 

. 

38.7 

43 

.8 

00 

00 

5-o 

43-o 

(160°) 

10-0 

100  gms.  oil  of  turpentine  dissolve  1.35  gms.  S  at  16°,  and  16.2  gms.  at  b.  pt. 

(Payen,  1852.) 

SOLUBILITY  OF  SULFUR  IN  TRIPHENYL  METHANE,  DETERMINED  BY  THE 
SYNTHETIC  METHOD. 


Results  of  Smith,  Holmes  &  Hall,  1905. 

Results  of  Kruyt,  1908-09. 

%  Triphenyl 
Methane  in 

t°  of  First 
Limit  of 

%  Triphenyl  t°  of  Second 
Methane  in      Limit  of 

%  Triphenyl  t°  of  First  %  Triphenyl 
Methane  in    Limit  of     Methane  in 

t°  of  Second 
Limit  of 

Mixture. 

Mixing. 

Mixture. 

Mixing. 

Mixture. 

Mixing. 

Mixture. 

Mixing. 

69.1 

108.5 

35-5 

214.5 

66.7 

113 

7 

2II-5 

58.8 

127 

32.5 

211 

60.2 

125.3 

9-3 

201.5 

50.8 

136.5 

28.4 

506 

5O.  2 

136.8 

12 

198.8 

46.6 

141 

24.5 

203 

41 

144-2 

13.7 

199-5 

42.8 

144 

21.6 

200 

30.8 

I46 

16.4 

20O.4 

37-8 

146 

19.2 

199 

2O 

145-2 

19.8 

2O2.  I 

33-7 

146.5 

15.4 

I98 

13-2 

137.6 

23-5 

203.7 

30-3 

147 

8.1 

II8.6 

28.7 

208 

25.4 

146 

7 

crystals 

34-5 

215.2 

SOLUBILITY  OF  SULFUR  IN  PHENOL,  DETERMINED  BY  THE  SYNTHETIC  METHOD. 

(Smith,  Holmes  and  Hall,  1905.) 

f he  mixtures  of  sulfur  and  phenol  were  heated  until  they  were  homogeneous 
and  then  cooled  to  the  temperature  at  which  clouding  appeared. 

+0    £              Gms.  S  per                      t<>    f               Gms.  S  per  to    e            Gms.  S  per 

Clouding.            'ojGg-.                   Clouding.             '~£f  Clouding.          '~£f 

89.5              9.1                  155                26.3  166             31.6 

96.5            10.4                 157.5            27.1  167.5          32.4 

122.5            15.3                 160.5            28.6  170             33.5 

138                19.9                 162                29.6  172              34.9 

148.5            23.6                  164.5            30-7  J75              36.5 

RECIPROCAL  SOLUBILITY  OF  SULFUR  AND  TOLUENE,  DETERMINED  BY  THE 
SYNTHETIC  METHOD. 

(Kruyt,  1908-09.) 

Wt.  %  S  in           Limiting  t"  of  Homogeneity.                 \yt.  %  S  in  Limiting  t°  of  Homogeneity. 

Mixture.                   Lower.               Upper.     "                    Mixture.  '  Lower.               Upper. 

50.5  167         250             75.7  178         221 
62             179         223             77.9  174 

69.6  l8o         222             83.3  l6o         223 

73         180      222         90.5  124   above  250 


70S 


SULFUR 


RECIPROCAL  SOLUBILITY  OF  SULFUR  AND  META  XYLENE,  DETERMINED 
BY  THE  SYNTHETIC  METHOD. 

(Kruyt,  1908-09.) 


Wt.  %  S  in 
Mixture. 

50-9 
49.1 

47-7 

44.2 
40.4 

Limiting  t°  i 

af  Homogeneity. 

Lower. 

181 

177 

172.5 
161.5 

153-5 

Upper. 
213 
228 

none  (?) 
"     (255) 
"     (215) 

Wt.  %  S  in 
Mixture. 

39-9 
84.2 

86.1 

87 
90 


Limiting  t°  of  Homogeneity. 


Lower. 
152 

none 
164.5 
159 
139 


Upper. 

none  (230) 

« 

199 

202.5 
none  (220) 


Fusion-point  data  for  the  system  sulfur-tellurium  are  given  by  Pelabon  (1909); 
Pellini  (1909);  Chikashige  (1911,  1911-12);  Jaeger  and  Menke  (1912). 

Data  for  mixtures  of  sulfur  and  each  of  the  following  metals  are  given  by  Pela- 
bon (1909);  antimony,  tin,  lead,  silver,  gold  and  arsenic. 

SULFUR  DIOXIDE  SO2 


SOLUBILITY  IN  WATER. 

(Schonfeld,  1855;  Sims,  1861;  Roozeboom,  1884.) 

Schonfeld.                                     Sims. 

Vols.  SO2  (at  o°  and        Cms.  SO2  per                                       „  ~ 
760  mm.)  per  i  Vol.        I00  Cms?  HaO             SO2  per  i  Gm.  H2O. 

Roozeboom. 

S02  Dissolved 
peript.HaO 

*•.        Sat.  SO, 
+  Aq. 

H20. 

at  total  pressure    t  ». 
760  mm. 

Cms. 

Vols.' 

t   . 

Ul     /LKJ    Ullll. 

pressure. 

O 

68 

.86 

79 

•79 

22 

.83 

8 

0.168 

58.7 

O 

0.236 

5 

59 

.82 

67 

.48 

19 

10 

0.154 

53-9 

2 

0.218 

10 

51 

•38 

56 

•65 

16 

.21 

14 

0.130 

45-6 

4 

0.201 

15 

43 

•56 

47 

.28 

!3 

•54 

20 

O.IO4 

36-4 

6 

0.184 

2O 

36 

.21 

39 

•37 

II 

•29 

26 

0.087 

30-5 

7 

0.176 

25 

30 

•77 

32 

•79 

9 

.41 

30 

0-078 

27-3 

8 

0.168 

30 

25 

.82 

27 

.16 

7 

.81 

36 

0.065 

22.8 

10 

0.154 

35 

21 

•23 

22 

•49 

40 

0.058 

20.4 

40 

17 

.01 

18 

•77 

5 

.41 

46 

0.050 

17.4 

12 

0.142 

50 

0.045 

15.6 

Sp.  Gr.  of  sat.  solution  at  o°  =  1.061;  at  10°,  1.055;  at  20°  =  1.024. 
The  results  of  Sims  are  discussed  and  recalculated  by  Fulda,  1909. 
I  gm.  H2O  dissolves  0.0909  gm.  SO2  =  34.73  cc.  (measured  at  25°)  at  25°  and 
760  mm.  pressure.  (Walden  and  Centnerszwer,  1902-03.) 


FREEZING-POINT  DATA  FOR  THE  SYSTEM  SULFUR  DIOXIDE  —  WATER. 


Mols.  SO, 

VrLSLm             I*51  I0°  M°ls'        Solid  Phase- 
Freezing.             SO2+H2O. 

O 

O 

Ice 

—  0.2 

0.8 

" 

-3  Eutec. 

.  .  . 

"  +S02  Hydrate 

—  O.2 

2.8 

SO2  Hydrate 

+3.5 

3-3 

" 

6.8 

5-5 

" 

(Baume  and  Tykociner,  1914.) 

t°of 
Freezing. 

7-7 
8-3 

9-3 

12. I 
12.2 


Mols.  SOj 
per  loo  Mols. 


Solid  Phase. 
SO,  Hydrate 


5-9 


ii 


95-1 


At  the  temperature  +12.1°  and  extending  over  the  range  of  concentration  n 
to  95.1  mols.  per  cent  SO2  a  second  phase  rich  in  SO2  separates.  This  crystal- 
lizes at  —74°  and  the  diagram  is  consequently  composed  of  two  lines  parallel  to 
the  axis  of  concentration,  the  one  at  the  +12.1°  level  corresponding  to  the  SO2 
hydrate,  and  the  other  at  the  —74°  level,  to  the  SO2  rich  phase.  The  diagram  is 
terminated  by  a  very  short  branch  rising  from  —74°  to  the  temperature  of  solidi- 
fication of  pure  SO2  (—72.3°). 


SULFUR  DIOXIDE  706 

SOLUBILITY  OF  SULFUR  DIOXIDE  IN  WATER  AT  DIFFERENT  PRESSURES. 

(Lindner,  1912.) 

Results  at  o°.  Results  at  25°.  Results  at  50°. 

mm-Hg-  ^ItVsoL0'  mm.  Hg.  ^af.^oT  nxm.  Hg.  'sLufe?' 

0.4  0.0537  i-4  0.0534  4.9  0.0525 

3-5  0.237  n-75          0.234  30.5  0.2276 

29.4       1.227          87.9        I. 212         204.5        I.lSl 

109.4    3.804     313     3.750     696     3.628 

SOLUBILITY  OF  SULFUR  DIOXIDE  IN  AQUEOUS  SALT  SOLUTIONS. 

(Fox,  1902.) 

Results  in  terms  of  the  Ostwald  Solubility  Expression.     See  p.  227. 

A  SoJubility  Coefficient  /  of  SO2  in  aq.  Solutions  of  Concentrations: 

Aqueous  A 

Salt  Solution.  r0.s  Normal  1.0  N.         i.±V.          2.0  N.          2.5  N.        3-0  N? 

NH4C1           £35=34-58  36-37  38-06  39.76  41.37  42.78 

NH4Br           £35=36-25  39.46  42.78  46.06  49.17  52.25 

NH4CNS        £35=37-78  42.74  47.26  52.26  57.01  61.46 

NH4NO3        £35=33-96  35-o7  36-28  37.27  38.01  39.14 

NH4NO3        £35=23-35  24-23  24.78  25.57  26.66  27.43 

(NH4)2SO4     £35=33-35  33 -82  34-33  34-95  35-47  35-96 

(NH4)2SO4      /35=22.9i  23.14  23.49  23.93  24.23  24.60 

/25=3i.66  30.55  29.46  28.16  27.09  26.06 

£35=2! -73  21.23  20.55  20.02  19.23  18.68 

CdBr2             /25=3i.9i  31.01  30.17  29.27  28.15  27.46 

CdBr2             /35=2i.88  21.46  20.81  20.60  19-70  19-17 

CdI2               £25=33-27  33-76  34.16  34.74  34.98  35.77 

CdI2               /35=22.75  23.06  23.36  23.71  23.99  24.30 

CdSO4            /25=3i.ii  29.71  28.24  26.58  25.14  23.76 

CdSO4            /35=2i.45  20.43  19-42  18-31  17-41  16.25 

£25=34-42  36-05  37-76  39.32  40.96  42.27 

£35=23-74  25.15  26.54  27.94  28.93  30.02 

KBr               £25=35-94  39 -11  42-41  44-96  48-87  52.26 

KBr                /35=24.83  27.49  29.64  31.93  34.12  36.14 

KCNS            £25=37-57  42-38  47 -02  51.81  55.87  61.26 

KCNS            £35=25-63  28.79  32-03  35-05  38.13  42.94 

/25=38.66  44-76  50-58  56-75  62.63  68.36 

£35=26.30  30.25  34-64  38.04  41-87  45-43 

KNO,            £35=33-80  34-79  35-77  36-66  37.57  38.52 

KNO3             £35=23.27  24.03  24.79  25.72  26.54  27.33 

K2SO4            £35=33-20  33.61 

NaBr              £25=33-76  34-54  35-27  36-26  36.84  37.74 

NaCl              735=32.46  32.25  31.96  31.76  31.51  31.36 

NaCNS          £35=35-44  38-24  40-78  43-37  45-86  48-34 

Na2SO4          /25=3i. 96  31.14  30.45  29.51  28.66  28.44 

Na^C^           /35=2i.88  21.35  20.81  20.21  19.75  19-27 

The  author  also  gives  a  series  of  determinations  in  which  a  mixture  of  SO2  +  CO2 
is  used  for  saturating  the  solutions,  thus  changing  the  concentration  of  the  SO2 
and  yielding  results  for  certain  partial  pressures  of  this  gas. 

m  Additional  data  for  the  solubility  of  sulfur  dioxide  in  aqueous  salt  solutions  are 
given  by  Walden  and  Centnerszwer  (1902-03)  but  these  authors  present  their 
results  in  terms  of  the  difference  between  the  amount  of  SO2  dissolved  in  water 
and  in  the  aqueous  solution.  The  exact  manner  in  which  these  calculations  were 
made  is  not  clearly  explained. 


707 


SULFUR  DIOXIDE 


SOLUBILITY  OF  SULFUR  DIOXIDE  IN  SULFURIC  ACID  OF  1.84  SP.  GR. 


Interpolated  from  original  results. 


o 
10 
20 
25 
30 
40 


Sp.  Gr. 

Coefficient 

of  Sat. 

of  Absorp- 

t °  . 

Solution. 

tion  (760  mm.). 

53-o 

50 

1.8232 

35-o 

60 

1.8225 

25  .0 

70 

I  .8221 

21  -O 

80 

I.82I6 

18.0 

90 

1.8205 

13.0 

(Dunn,  1882.) 


Sp.  Gr. 

Coefficient 

of  Sat. 

of  Absorp- 

Solution. 

tion  (760  mm.) 

I.  8l86 

9-5 

1.8165 

7.0 

I.8l40 

5-5 

1.8112 

4-5 

I.  8080 

4-0 

SOLUBILITY  OF  SULFUR  DIOXIDE  IN  AQUEOUS  SULFURIC  ACID  SOLUTIONS. 

(Dunn;  see  also  Kolb,  1872.) 


Sp.  Gr.  of 

Approximate 

Coefficient 

< 

>p.  Gr.  of 

Approximate 

Coefficient 

t  ° 

H2SO4 

Per  cent 

of 

t  °« 

H2SO4 

per  cent 

of 

Solution. 

H2S04. 

Absorption. 

Solution. 

H2S04. 

Absorptior 

6 

9 

•139 

20 

48.67 

15 

2 

i 

•173 

25 

31.82 

6 

9 

•  300 

40 

4S-38 

16 

8 

X 

•I5I 

21 

3I-56 

8 

.6 

.482 

58 

39  -91 

14 

8 

z 

.277 

36 

30.41 

9 

.8 

•703 

78 

29.03 

15 

.1 

I 

•458 

S^ 

29.87 

5 

•5 

.067 

10 

36.78 

15 

.6 

I 

.609 

70 

25-I7 

6 

.0 

.102 

15 

3.408 

15 

0 

I 

•739 

81 

20.83 

For  definition  of  Coefficient  of  Absorption,  see  Ethane  p.  285. 


SOLUBILITY  OF  SULFUR  DIOXIDE  IN  ALCOHOLS  AND  IN  OTHER  SOLVENTS. 

(de  Bruyn,  1892;  Schulze,  1881.) 


In  Ethyl  Alcohol 
at  760  mm. 

o        Gms.  SO2  per  100  Gms. 


In  Methyl  Alcohol 
at  760  mm. 

Gms.  SO2  per  100  Gms. 


Solution. 

C2HsOH.                  Solution. 

CH3OH. 

0 

53 

•5 

115 

.0 

71.1 

246 

.0 

7 

45 

•o 

8l 

.0 

59-9 

149 

•4 

12 

•3 

39 

•9 

66 

•4 

52.2 

109 

.2 

18 

.2 

32 

.8 

48 

.8 

(17.  8°)  44-0 

78 

,6 

26 

•  O 

24 

4 

32 

•3 

3I-7 

46 

•4 

In  Several  Solvents 
at  o°  and  725  mm.  (S.) 

S  lve~t          SO2  per  i  Gm. Solvent 
Grams.       Vols. 

Camphor      o .  880  308 

CH3COOH  0.961  318 

HCOOH      0.821  351 

(CH3)2CO     2.07  589 

SO2C12          0.323  189 


SOLUBILITY  OF  SULFUR  DIOXIDE  IN  CHLOROFORM. 

(Lindner,  1912.) 

Results  at  o^  Results  at  25°. 


Pressure  in 
mm.  Hg. 

Gms.  SO; 
per  100  cc 
Sat.  Sol. 

2.7 

5-6 

22 

O.O7OI 
0.1790 
0.6982 

90.2 
219.6 

3-097 
8.217 

Pressure  in 
mm.  Hg. 

5-7 
12.9 
48 

200.2 
488.8 


Gms.  SOz 

per  100  cc. 

Sat.  Sol. 

0.0669 
O.I7I2 
0.6728 
2-954 


SULFUR  DIOXIDE 


708 


SOLUBILITY  OF  SULFUR  DIOXIDE  IN  SEVERAL  SOLVENTS. 

(Lloyd,  1918.) 

The  dry,  air  free,  SO2  was  passed  through  the  solvent  until  saturation  was 
reached  and  5  cc.  (usually)  of  the  saturated  solution  were  mixed  with  a  large  volume 
of  water  and  titrated  with  standardized  iodine  solution. 

Gms.  SO2  per  Liter  of  Saturated  Solution  in: 


-  5 
o 

+  5 

10 

15 

20 
25 
3° 
40 

50 
00 


Benzene. 

Nitro- 
benzene. 

Toluene. 

o  Nitro- 
toluene. 

Acetic 
Anhydride. 

.  .  . 

196 

148(^=1.22) 

136 

.  .  . 

.  .  . 

.  .  . 

122 

3II-4 

.  .  . 

290.8 

114 

267.4 

217-5 

236 

106 

227.9 

170.4 

192.2 

99 

127.5 

190 

124.4 

160.7 

90 

82.9 

I32 

93-6 

II8.5 

.  .  . 

60.3 

98.7 

77.2 

87.2 

.  .  . 

34 

78.6 

54-7 

68.8 

DISTRIBUTION  OF  SULPHUR  DIOXIDE  AT  20°  BETWEEN: 

(McCrae  and  Wilson,  1903.) 


Water  and  Chloroform. 


Aq.  HC1  and  Chloroform. 


Cms.  SOa  per 
Liter  in: 

Gm.  Equiv.  iSO2 
per  Liter  in: 

Cone. 

Gms.  SOa  per 
Liter  in: 

Gm.  Equiv.    iSO2 
per  Liter  in: 

Aq. 
Layer. 

CHC13 
Layer. 

Aq. 
Layer. 

CHC13 

Layer. 

of 
HC1. 

Aq. 
Layer. 

CHC13 
Layer. 

Aq. 

Layer. 

CHC13 
Layer. 

I-738 

I 

.123 

0 

•0543 

0 

•0351 

0.05 

1.86 

I  .46 

0-0581 

0.0456 

i-753 

J. 

.122 

0 

•0547 

O 

•0350 

it 

3-07 

2.83 

0-0960 

0.0884 

2.346 

I 

•703 

0 

.0732 

0 

•0532 

ti 

4.28 

4.07 

0.1336 

O.I27I 

2.628 

I 

.897 

0 

.082I 

0 

.0592 

tt 

5-34 

,5.42 

0-1667 

0.1692 

3-058 

2 

.385 

0 

•0955 

0 

•0745 

0.10 

1-25 

I.4I 

0-039 

O.O44 

3-735 

3 

.062 

0 

.1166 

0 

.0956 

« 

2.78 

3.08 

0.0868 

0.0962 

4.226 

3 

.626 

0 

'W9 

0 

.1132 

« 

3.86 

4.08 

0.1199 

0-1275 

5.269 

4 

.798 

0 

.1645 

0 

.1498 

a 

5.161 

5-72 

0.1612 

0.1784 

6.588 

6 

.I83 

0 

.2057 

0 

.1930 

0.2 

1.268 

I-5I 

0.0396 

0.0471 

31.92 

33 

.84 

0 

.9968 

I 

.056 

if 

1.914 

2  .27 

0.0597 

O.O7lo 

33-26 

37 

•25 

I 

.038 

I 

.163 

(I 

2.464 

3-°4 

0.0769 

0-0949 

a 

3-967 

4.90 

0.1239 

0-I530 

0-4 

i  .202 

1.61 

0.038 

0.0504 

it 

1.894 

2  .26 

0.059 

0-0706 

Freezing-point  data  for  mixtures  of  sulfur  dioxide  and  sulf uryl  chloride  (SO2C12) 
are  given  by  van  der  Goot  (1913). 


SULFURIC  ACID   H2SO4  (Sulfur  Trioxide,  SO3). 
SOLUBILITY  IN  WATER. 

(Landoldt  and  Bornstein,  "Tabellen,"  4th  Ed.,  pp.  472-3,  1912.) 

The  available  data  for  the  freezing-points  of  mixtures  of  sulfuric  acid  and  water 
have  been  plotted  and  the  most  probable  values  read  from  the  curves.  The  data 
are  also  calculated  to  SO8.  The  complete  results  are  given  on  the  following  page. 


709 


SULFURIC  ACID 


SOLUBILITY  OF  SULFURIC  ACID  IN  WATER,  DETERMINED  BY  THE 
FREEZING-POINT  METHOD. 


Gms. 

Gms. 

H2S04 

Gms.  SO4 

H2S04         Gms.  S( 

\ 

t°. 

per  100 

per  100  Gms.         Solid  Phase.             t°. 

per  100      per  100  Gms.        Solid  Phase. 

Gms. 

Sat.  Sol. 

Gms.           Sat.  So 

1. 

Sat.  Sol. 

Sat.  Sol. 

IO 

16.25 

l3-25(i)  (S)  .    Ice 

—  IO 

77-75      63.5    (3)        SO,.2H20 

20 

24 

i9-5(i)( 

2)  (3)        " 

0 

80.25      65.5    (2) 

30 

28.5 

23-25  (2) 

+  8.35 

*  84-5        68.98  (2) 

40 

3I-25 

25-5     (2)    .            " 

8.81 

84.5        68.98 

i 

50 

33-5 

27.25(l) 

(2) 

o 

88.25      72 

2 

60 

35-25 

28.75  « 

" 

—  20 

91-5        74-75 

« 

70 

36.75 

30         (2) 

-30 

92-5       75-5    ( 

75 

38 

31        (2)             "  +S03.SH20 

-38 

93           76       (2)          "+S03.H20 

70 

39 

31.75(2)    S03.SH20 

-30 

93-75      76.5    (4)        S03.H20 

60 

4i.5        33-75(2)     ' 

—  20 

95-25      77.75  (4) 

50 

44 

36        (2)     • 

—  IO 

96.25      78.5    (i)(4)     " 

40 

47-75 

39       (2)     " 

o 

97-75      79-75  (4) 

30 

53-25 

43-25  (2)     " 

+  10 

99.75     81       (4) 

25* 

57.65 

47.06  (2)     "                                10.35 

100          81.62  (i)(3)  (7X4) 

30 

61 

49-75  (2)     " 

10 

...        82       (4)        «' 

40 

65-25 

53-25  (2)     " 

0 

•  •  •        83.25  (4)        " 

60 

70.75 

57-75  (3)      "  (unstable) 

—  IO 

...        84.5    (4)         " 

70 

73-25 

59-75(3)     "      "     +S03.2H20 

—  12 

85       (4)         "+S03.*H20 

60 

73-50 

60       (3 

SO3.2H2O  (unstable) 

—  IO 

85.25  (4)           S03.*H20 

50 

74-25 

60.5    (3 

Cl 

O 

...        86       (4) 

50 

68 

55-5    (2 

SO3.sH2O+SO3.3H2O 

+  10 

.  .  .        86.75  (4) 

45 

68.5 

56      (6 

SO3.3H2O 

20 

...        87.5    (4) 

40 

58       (6)    '• 

3° 

...        88.5    (4) 

38.9* 

73.M 

59-69  (6)    " 

36* 

.  .  .        89.89  (4) 

40 

74-25 

60.5    (6)    « 

30 

...        90-5    (4) 

41 

74-75 

6  1       (6)     "  +SO3.2H2O 

20 

91.5    (4) 

40 

74-75 

6  1        (4)  SO3.2H2O 

10 

.  .  .        92.25  (4) 

3° 

75-25 

6i-5    (4) 

6.5 

...        93       (4)                "    +(?) 

20 

76.5 

62.5    (3). 

*  m.  pt. 

(i)  =Pfaundler  and  Schnegg  (1875);  (2)  =  Pickering  (1890);  (3)  =  Thilo  (1892);  Pictet  (1894);  (4) 
=  Knietsch  (1901);  (5)  =  Rudorff  (1862);  (6)  =  Biron  (1899);  (7)  =  Marignac  (1853).  See  also  Pickering 
(1890-91);  Lespieau  (1894)  and  Giran  (1913). 


SOLUBILITY  OF  SULFURIC  ACID  IN  BENZENE  SOLUTIONS  OF  VALERIC 
ACID  AT  1 8°. 

(Gurwitsch,  1914.) 

The  mixtures  were  shaken  with  excess  of  95.8%  H2SC>4  at  o°  and  then  brought 
to  equilibrium  at  1 8°. 


Gms.  Valeric 

Acid  per  100 

Gms.  Valeric 

Acid+Benzene. 

o=Pure  benzene 

0.584 

1.62 

3-64 
7.60 

17-5 


Gms.  H2S04 
per  100  Gms. 

of  the 
Sat.  Solution. 

O 

0.052 

O.IO4 

0.226 

0.378 

0.454 


TANNIC  ACID  710 

TANNIC  ACID 

When  a  sample  of  tannic  acid  of  apparently  very  good  quality  was  added  to 
water  at  room  temperature,  the  solution  increased  so  greatly  in  viscosity,  that 
even  before  the  saturation  point  was  reached,  it  became  evident  that  a  satisfac- 
tory separation  of  liquid  and  solid  could  not  be  made.  The  solubility  in  water  is 
variously  given  in  the  pharmaceutical  literature  from  about  20  to  300  gms.  tannic 
acid  per  100  gms.  of  water.  Similarly,  the  quoted  results  for  the  solubility  in 
alcohol  vary  from  about  50  to  400  gms.  acid  per  100  gms.  of  alcohol.  (Seidell,  1910.) 
100  gms.  glycerol  dissolve  48.8  gms.  tannin  at  15-16°.  (Ossendowski,  1907.) 

100  gms.  trichlorethylene  dissolve  0.012  gm.  tannin  at  15°.    (Wester  and  Bruins,  1914.) 

TANTALUM   Potassium  FLUORIDE  TaK2F7. 

SOLUBILITY  IN  AQUEOUS  HYDROFLUORIC  AND  POTASSIUM  FLUORIDE  SOLUTIONS. 

(Ruff  and  Schiller,  1911.) 

The  tantalum  salt  was  purified  by  repeated  crystallizations  from  pure  anhydrous 
HF1.  After  drying  at  120°,  it  was  shaken  in  platinum  flasks  for  3  hour  periods  at 
constant  temperature  with  HF1  or  KF1  solutions  or  both  together.  The  saturated 
solutions  were  filtered  by  means  of  a  platinum  funnel  and  subjected  to  analysis. 

Mixture  Shaken 
in  Pt.  Flask. 

K2TaF7+H2O 

"  +aq.4.77%KF 

"  +aq.  7-35%  KF 

"  +aq.4.47%HF 

"  +aq.    4-2  %HF 

"  +aq.  24.3 %HF 

"  +aq.  10.44%  HF+  ? 

2I.92%KF  $ 

"  +H20 

'  +aq.  4-77%  KF 
'  +aq.4.47%HF 
'  +aq.  4-2 %HF 
'  +aq.  23.3 %HF 
'  +aq.  21.92%  KF-f 

10.44%  HF 

The  solid  phases  were  identified  only  by  their  crystal  forms  and  it  is  possible 
that  still  others  may  be  present. 


TaH5. 

KF. 

HF. 

OU11U  JTilclbC. 

i8 

0.25 

O.I2 

O.O29 

KzTayOzF«+K2TaF 

18 

0.  10 

4-79 

0.074 

" 

16 

0.09 

6-73 

0.015 

" 

18 

1.33 

0.56 

4-47 

K2TaF7 

18.5 

1.24 

0.52 

4-2 

" 

18 

5-35 

2.25 

24-3 

" 

18 

0.036 

21.93 

10.44 

" 

85 

2.18 

1.69 

0.85 

K*Ta,AFM+K2TaF7 

85 

0.96 

5-27 

1.17 

" 

90 

5-73 

2.41 

4-47 

K2TaF7 

90 

6 

2.52 

4.2 

" 

90 

10.9 

4-59 

24-3 

" 

90 

1.18 

22.42 

10.44 

" 

TARTARIC   ACIDS   C2H2(OH)2(COOH)2.     d,  I,  and  racemic 
SOLUBILITY  OF  EACH  SEPARATELY  IN  WATER. 

(Leidie,i882.) 
t°.        Grams  Tartaric  Acid  per  iooGms.'H2O.  t°.      Gms.  Tartaric  Acid  per  100  Gms.  H2O. 


Dextro 

Racemic 

Racemic 

Dextro 

Racemic 

Racemic 

and  Laevo 

Ac. 

Ac. 

and  Laevo 

Ac. 

Ac. 

Acids. 

Anhydrous. 

Hydrated. 

Acids. 

Anhydrous. 

Hydrated 

o 

115.04 

8.l6 

9-23 

50 

195.0 

5O.O 

59-54 

10 

125.72 

12.32 

I4.OO 

60 

217-55 

64.52 

78.33 

20 

139-44 

18.0 

20.6o 

70 

243  .66 

80.56 

99.88 

25 

147.44 

21.4 

24.61 

80 

273-33 

98.12 

124.56 

30 

156.2 

25.2 

29.10 

•90 

306.56 

117  .20 

I52-74 

40 

176.0 

37-o 

43-32 

100 

343-35 

137.80 

184.91 

loo  gms.  H2O  dissolve  140.8  gms.  tartaric  acid  at  15 
solution  is  1.31. 


0     The  Sp.  Gr.  of  the  sat. 

(Greenish  and  Smith,  1902.) 


TARTARIC  ACID 


SOLUBILITY  OF  TARTARIC  ACID  IN  ALCOHOLS. 

(Timofeiew,  1894.) 


Alcohol. 


Methyl  Alcohol 


Ethyl  Alcohol 


r. 

Gms.  C2H2(OH)r 
(COOH)2                 M    .   , 
per  100  Gms. 

t°. 

per  100  Gms. 

Solvent. 

Solvent. 

-  3 

67.5        Ethyl  Alcohol 

+  23 

28.9 

+  19.2 

70.1 

39 

31.8 

23 

73  .  2        Propyl  Alcohol 

-  3 

8.74 

39 

77-3 

+  19 

,2         10.85 

-  3 

22.4                    " 

23 

11.85 

+  19.2 

27.6 

39 

14.4 

SOLUBILITY  OF  TARTARIC  ACID  IN  AQUEOUS  ETHYL  ALCOHOL  SOLUTIONS  AT  25°. 

(Seidell,  1910.) 


Wt.  Percent      j      , 
C2HBOH      cTsol 

Gms.  C2H2(OH)2(COOH)2 
per  loo  Gms. 

in  Solvent. 

Sat.  Sol. 

Solvent. 

0 

I.32I 

57-9 

137.5 

IO 

1.300 

56 

127.3 

20 

1.276 

54-1 

II7.9 

30 

I.25I 

52 

108.3 

40 

I.22O 

49.6 

98.4 

50 

I.I84 

47 

88.6 

Wt.  Per  cent 


Gms.  C2H2(OH)2(COOH)2 
per  100  Gms. 


Solvent 

Sat.  Sol. 

Solvent. 

60 

1.142 

43.9 

78-3 

70 

1.095 

4O.2 

66.9 

80 

1.040 

35-3 

54-6 

90 

0-973 

29 

40.8 

95 

0-937 

25-4 

34-1 

IOO 

0.905 

21.6 

27.6 

SOLUBILITY  OF  TARTARIC  ACID  IN  SEVERAL  SOLVENTS. 


Solvent. 


Amyl  Alcohol 

Benzene 

Carbon  Tetrachloride 

Ether 

u 

Dichlorethylene 
Trichlorethylene 


Sp.  Gr.  of 
Solvent. 

<*25  Of 

Sat.  Sol. 

Gms.  C2H2(OH)2- 
t°.    (COOH)2  per  100      Authority. 
Gms.  Solvent. 

^20  =  0.817 
f/25  =  0.873 

dz^  —  1.587 
dzz  =  0.711 

0.824 

0.875 
1.589 
0.715 

25 
25 
25 
25 

3  .  50          (Seidell,  1910.) 
0.0086 
0.0189 
O.6l                     " 

15 

0  .  40          (Bourgoin,  1878.) 

IS 

0  .  005     (Wester  &  Bruins,  '14.) 

15 

O.O05 

DISTRIBUTION  OF  TARTARIC  ACID  BETWEEN  WATER  AND  ETHER. 


Results  at  15°. 

Gms.  Mols.  per  Liter. 


(Pinnow,  1915.) 


H2O  Layer,  c. 
I.4O2 
0.790 
0.446 


Ether  Layer,  c' 
O.OO72 
0.0037 
O.OO22 


Results  at  27°. 

Gms.  Mols.  per  Liter. 


197 
2l6 
2IO 


H2O  Layer,  c. 
1.625 

0.857 
0.427 


Ether  Layer,  c'. 
0.0070 
0.0033 

0.0016 


233 
259 
268 


F.-pt.  data  are  given  for  mixtures  of  the  d  and  racemic  modifications  of  dimethyl 
ether  of  tartaric  acid,  and  for  mixtures  of  the  d  and  racemic  modifications  of  di- 
methyl ether  of  diacetyl  tartaric  acid  by  Roozeboom  (1899).  Results  for  mixtures 
of  the  d  and  *  forms  of  the  diformalic  derivative  of  racemic  tartaric  acid  by  Ringer 
(1902).  Results  for  mixtures  of  d  tartaric  acid  and  racemic  acid  ester  and  for  d 
diacetyl  tartrate  and  racemic  acid  ester  are  given  by  Beck  (1904).  Data  for 
mixtures  of  d  and  /  tartaric  acid  and  for  mixtures  of  d  and  i  dimethyl  ester  of  tar- 
taric acid  are  given  by  Centnerszwer  (1899). 


PyroTARTARIC  ACID  (Methyl  Succinic  Acid)  CH3.CH(COOH).CH2(COOH). 


loo  gms.  H2O  dissolve  51  gms.  CH3CH(COOH).CH2COOH  at  19.5°. 

(Timofei 


imofeiew,  1894.) 


PyroTARTARIC  ACID 


712 


Alcohol. 

t°. 

Gms.  Acid 
per  loo  Gms 

Solvent. 

Methyl  Alcohol 

—  18.5 

53 

tt 

+19 

109.8 

ii 

+  I9-S 

II2.5 

Ethyl  Alcohol 

+  19 

70.8 

SOLUBILITY  IN  ALCOHOLS. 

(Timofeiew,  1894.) 


Alcohol. 


Ethyl  Alcohol      19 
Propyl  Alcohol    19 


5 
iQ-5 


Gms.  Acia 

per  100  Gms. 

Solvent. 

72.4 

44-9 
47.1 


100  gms.  95%  formic  acid  dissolve  17.8  gms.  pyrotartaric  acid  at  18.5°. 

(Aschan,  1913.) 

TERPIN  HYDRATE  Ci0H18(OH)2.HsO. 

100  cc.  H2O  dissolve  0.36  gm.  terpin  hydrate  at  15-20°.  . 

100  cc.  90%  alcohol  dissolve  7.1  gms.  terpin  hydrate  at  15-20°. 

(Squire  and  Caines,  1905.) 

TELLURIUM  Te. 

100  gms.  methylene  iodide,  CH2l2,  dissolve  o.i  gm.  Te  at  12°.        (Retgers,  1893.) 

DISTRIBUTION  OF  TELLURIUM  BETWEEN  AQUEOUS  HYDROCHLORIC  ACID  AND 
ETHER  AT  ROOM  TEMPERATURE. 

(Mylius,  1911.) 

When  i  gm.  of  tellurium  as  the  chloride,  TeCU,  is  dissolved  in  100  cc.  of  aqueous 
HC1  and  shaken  with  100  cc.  of  ether,  the  following  per  cents  of  the  metal  enter 
the  ethereal  layers.  With  20%  HC1,  34  per  cent;  15%  HC1,  12  per  cent;  10% 
HC1,  3  per  cent;  5%  HC1,  0.2  per  cent  and  with  i%  HC1,  only  a  trace  of  the 
tellurium. 

Fusion-point  curves  for  mixtures  of  tellurium  and  each  of  the  following  metals 
are  given  by  Pelabon  (1909) :  Sb,  Sn,  Pb,  Ag,  Au  and  As.  Results  for  mixtures  of 
Te  and  Zn  are  given  by  Kobayashi  (1911-12). 


Mols. 

"ss^r 

H20. 
4.67       H2Te04.2H20 

5-33 
7.04 

9-93 
14.52 
19 

TELLURIUM  DOUBLE  SALTS 

SOLUBILITY  OF  TELLURIUM  DOUBLE  BROMIDES  AND  CHLORIDES  IN  AQUEOUS 
HYDROCHLORIC  AND  HYDROBROMIC  ACIDS  AT  22°. 

(Wheeler, 


TELLURIC  ACID  H2TeO4.2H2O. 
SOLUBILITY  IN  WATER. 

(Mylius,  1901.) 

Gms.            Mols. 

Gms. 

t°. 

H2TeO4  per  H2TeO4  pe 
100  Gms.      100  Mols. 

r   Solid  Phase. 

t°. 

H2TeO4  per 
100  Gms. 

Sol.              H2O. 

Sol. 

0 

13.92         1.51 

H2TeO4.6H2O 

30 

33.36 

5 

17.84         2.03 

" 

40 

36.38 

10 

26.21         3.31 

« 

60 

15 

32.79      4-55 

« 

80 

S'-SS 

10 

25-29        3-15 

H2TeO4.2H2O 

100 

60.84 

18 

28.90        3.82 

" 

no 

67 

Tellurium  Double  Salt. 


Formula. 


Solvent. 


Gms.  Double  Salt  per  too 
Gms.  Solvent 


Te  Caesium  Bromide      TeBr4.2CsBr    Aq.  HBr 
Te  Potassium  Bromide      TeBr4.2KBr 
Te  Rubidium  Bromide 
Te  Caesium  Chloride 
Te  Rubidium  Chloride 


TeBr4.2RbBr          " 
TeCl4.2CsCl    Aq.  HC1* 
TeCl4.2RbCl 


of  i  .49  Sp.  Gr. 

of  i  .08  Sp.  Gr. 

O-O2 

0.13 

6-57 

62.90 

0.25 

3-88 

0.05 

0.78 

o-34 

13.09 

•  Sp.  Gr.  of  Aq.  HC1  solutions  1.2  and  1.05  respectively. 


TELLURIUM  IODIDE 


TELLURIUM  TetralODIDE  TeI4. 

SOLUBILITY  IN  MIXTURES  OF  AQUEOUS  HYDRIODIC  ACID  AND  IODINE  AT  25°. 

(Menke,  1912.) 

Weighed  amounts  of  TeL  +  1+65  wt.  %  HI  solution  were  shaken  in  sealed 
glass  tubes  for  10  days.  Both  the  clear  saturated  solution  and  the  solid  phase 
were  analyzed. 


Solid  Phase. 

Small  amt.  TeL..HI.8HaO 
tiuch 
t<  «< 

small  amt.          " 
TeI<.HI.8H,0 
Iodine 


SOLUBILITY  IN  WATER  AT  25°. 

(Locke,  1901.) 

Salt  per  100  Grams  HjO. 


Composition  of  Original  Mixture 
in  Gms. 

Gms.  per  100  Gms. 
Solution. 

TeL.. 

i. 

64%  HI. 

•  Tel*. 

i. 

3 

i-5 

I9-25 

12 

11.7 

2 

o-5 

9.61 

13 

o 

2 

o-S 

9.61 

13-5 

8.2 

3 

3 

8.99 

20 

21.8 

Excess 

None 

5  (cc-) 

9 

0.19 

2 

9 

9.10 

IO 

52.4 

4 

10 

9.27 

15 

47-7 

3 

7 

9.02 

J7-5 

47-9 

None 

Excess 

5  (cc.) 

None 

61.1 

THALLIUM  ALUMS 


Alum. 


Formula. 


Tl  Aluminum  Alum 
Tl  Vanadium  Alum 
Tl  Chromium  Alum 
Tl  Iron  Alum 
See  also  pp.  31  and  32. 


TlAl(S04)2.i2H20 
TlV(S04)2.i2H00 
TlCr(S04)2.i2H20 
TlFe(S04)2.i2H20 


Gms. 

Gms. 

Gm. 

Anhydrous. 

Hydrated. 

Mols. 

7-5 

11.78 

0.0177 

25.6 

43-31 

0-0573 

10.48 

16.38 

0.0212 

36-I5 

64.6 

0.0799 

THALLIUM   BROMATE  TlBrO3. 

One  liter  saturated  aqueous  solution  contains  3.463  gms.  TIBrOs  at  19.9°  (B6tt- 
ger,  1903)  and  7.355  gms.  at  39.75°.  (Noyes  and  Abbot,  1895.) 

THALLIUM   BROMIDE  TIBr. 

One  liter  sat.  aqueous  solution  contains  0.238  gm.  TIBr  at  0.13°,  0.289  gm-  a* 
9.37°,  0.4233  gm.  at  1 8°  and  0.579  gm.  at  25.68°.  (Kohlrausch,  1908.) 

SOLUBILITY  OF  THALLIUM  BROMIDE  IN  AQUEOUS  SOLUTIONS  OF  THALLIUM 

NITRATE  AT  68.5°. 

(Noyes,  1890.) 
Gms.  Mols.  per  Liter.  Gms.  per  Liter. 


T1NO3. 
O 

0.0163 
0.0294 

0-0955 


TIBr. 

0.00869 
O.OO4IO 
0.00289 
O.OOI48 


T1NO3. 
O 

4.336 

7.820 

25.400 


TIBr. 
2.469 
I.l64 
0.821 
0.420 


F.-pt.  data  for  mixtures  of  TIBr  +  T1C1,  TIBr  +  Til  and  T1C1  +  Til  are  given 
by  Monkemeyer  (1906).  Results  for  T1C1  +  SnCl2  and  T1C1  +  ZnCl2  are  given 
by  Korreng  (1914). 

THALLIUM, CARBONATE  T12C03. 

SOLUBILITY  IN  WATER. 

(Crookes,  1864;  Lamy,  1863.) 
t°.  15.5°-  18°.         62°.  100°.          100.8°. 

Gms.  T12CO3  per  100  gms*  H20    4.2  (C.)  5.23  12.85  27-2  (C.)  22.4 


THALLIUM   CHLORATE  714 

THALLIUM  CHLORATE  T1C1O3. 

SOLUBILITY  IN  WATER. 

(Muir,  1876.) 

t°.  0°.  20°.  50°.  80°.  100°. 

Gms.  TIClOs  per  ioo  gms.  H2O   2    3.92  12.67  36-65  57.31 

One  liter  sat.  aq.  solution  contains  38.51  gms.  T1C1O3  at  20°.      (Noyes  and  Parrel,  1911.) 

One  liter  of  aqueous  solution,  saturated  with  both  salts,  contains  30.4  gms. 

TIClOa  +  3443  gms.  T12SO4  at  2O°.  (Noyes  and  Farrel,  1911.) 

SOLUBILITY  OF  MIXED  CRYSTALS  OF  THALLIUM  CHLORATE  AND  POTASSIUM 
CHLORATE  IN  WATER  AT  10°. 

(Roozeboom,  1891.) 

NOTE.  —  Solutions  of  the  two  salts  were  mixed  in  different  proportions  and 
allowed  to  crystallize,  such  amounts  being  taken  that  not  more  than  one  or  two 
grams  would  separate  from  one  liter. 

Gms.  per  1000  cc.  Mg.  Mols.  per  1000  cc.  Sp.  Gr.  Mols.  per  cent 

Solution. ^ Solution. of  KC1O3  in  Mixed 

'T1C1O3.  KC1O3.  T1C1O3.  KC1O3.  Solutions.  Crystals. 

25-637  •••  89.14  ...  I.O2IO  O 
19.637  6.884  68.27  56.15  I.O222  2 
12.001  26.100  41.73  212.89  1.0278  12. 6l 

9.036  40.064  3I-42  326.79  i -0338  25.01 

7.885  46.497  27.42  379.26  1.0359  >  36.30_97 

7.935  46.535  27.60  379-57  1.0360  )  * 

6.706  46.410  23.32  378.55  1-0357  99-28 

6.723  47-109  23.37  384-25  1-0363  99.60 

4.858  47-312  16.89  385-91  1-0345  99-62 

2.769  47-134  9-63  384.46  1.0330  99.67 

49.925  ...  407.22  1.0330  ioo 


SOLUBILITY  OF  MIXED  CRYSTALS  OF  THALLIUM  CHLORATE  AND  POTASSIUM 
CHLORATE  IN  WATER  AT  -DIFFERENT  TEMPERATURES. 

(Quoted  by  Rabe,  1902.) 

ioo  gms.  H2O  dissolve  2.8  gms.  T1C1O3  +  3.3  gms.  KC1O3  at  o°. 
H2O  dissolve  10  gms.  T1C1O3  +  1.5  gms.  KC1O3  at  15°. 
H2O  dissolve  12.67  gms.  T1C1O3  +  16.2  gms.  KC1O3  at  50°. 
H2O  dissolve  57.3  gms.  T1C1O3  +  48.2  gms.  KC1O3  at  100°. 


THALLIUM   PerCHLORATE  T1C1O4. 

SOLUBILITY  IN  WATER. 

(Carlson,  1910.) 

c     n  Gms.  T1C1O4  c     r  Gms.  T1C1O4  per 

t°.  IP-^J  per  ioo  Gms.  t°.  Jg-gS  ioo  Gms. 

H20.  Sat' SoL  H20. 

o     i. 060      6          50     1.251     39-62 
10     1.075      8.04       70     1.430     65.32 

30  1.146  I9.72  80  L520  81.49 

ioo  gms.  H2O  dissolve  10  gms.  T1C104  at  15°  and  166.6  gms.  at  100°. 

(Roscoe,  1866.) 


715 


THALLIUM  CHLORIDE 


THALLIUM   CHLORIDE  T1C1. 

SOLUBILITY  IN  WATER. 

(Average  curve  from  results  of  Noyes,  1892;  Bottger,  1903;  Kohlrausch,  1904;  Hebberling;  Crookes; 
Lamy.    The  results  of  Berkeley,  1904  are  also  given.) 


jo^  Cms.  T1C1  per  Liter. 

o  2.1  (av.)  1.7  (B.) 

10  2.5  2.4 

20  3.3  3-4 


t°. 

25 
30 
40 
50 


Gms.  T1C1  per  Liter 

.     t°.    Gms-  T1C1  per  Liter. 

3-86 
4.2 
5-2 
6-3 

4 
4.6 
6 
8 

60 
80 
IOO 

8 

12 

18 

IO.2 

16 

24.1 

(99.3°) 

The  results  of  Berkeley  are  in  terms  of  gms.  of  T1C1  per  1000  gms.  H2O  but 
since  the  densities  of  the  solutions  are  approximately  I  in  all  cases,  except  for 
temperatures  above  60°,  the  differences  are  negligible.  The  Sp.  Gr.  of  the  sat. 
sol.  at  99.3°  is  0.9787  and  the  figure  24.1,  therefore,  becomes  23.58  gms.  per  liter. 

One  liter  sat.  solution  in  water  contains  2.27  gms.  T1C1  at  9.54°,  3.05  gms.  at 
17.7°,  and  3.97  gms.  at  25.76°.  (Kohlrausch,  1908.) 


SOLUBILITY  OF  THALLIUM  CHLORIDE  AT  25°  IN  AQUEOUS  SOLUTIONS  OF: 

Nitric  Acid. 
(Hill  and  Simmons,  1909.) 


Normality  of 
Aq.  CHsCOOH 

0 
0.0501 
0.0958 
0.263 
0.524 

Acetic  Acid. 
(Hill,  1917.) 
T1C1  per  Liter. 

••      Gms. 
3.8515 
3.8375 
3.8326 

3.7503 
3.6539 

Gm.  Equiv. 
O.Ol6o85 
O.OI6027 
O.Ol6oo6 
0.015662 
0.015258 

Normality  of         d^  of 
Aq.  HN03.        Sat.  Sol. 

o                0.996 
0.4977        1.0184 
1.0046        1.0359 

T1C1  per  Liter. 

'Gms.         Gm.  Equiv." 
3.951         0.0165 

5-937       2.475 
6.882       2.875 

2.0452        1.0705 
4.0170        1.1362 

8.143       3-401 
9.925       4.145 

SOLUBILITY  OF  THALLIUM  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  SALTS 

WITH  A  COMMON  ION  AT  25°. 

(Noyes,  1892.) 


Aqueous 
Solution  of: 

Gms.  Equiv. 
Added  Salt 
per  Liter. 

Gms.  Equiv. 
Dissolved  T1C1 
per  Liter.     . 

Water  alone 

O 

o.  01612 

NH4C1 

0.025 

0.00877 

" 

0.05 

0.00593 

" 

0.20 

O.0027I 

BaCl2 

0.05 

O.OO62O 

" 

O.IO 

0.00425 

CdCl2 

0.025 

O.OI040 

" 

0.05 

0.00780 

" 

O.IO 

0.00578 

tt 

O.2O 

0.00427 

CaCl2 

0.025 

0.00899 

" 

0.05 

0.00624 

u 

O.  IO 

0.00417 

" 

O.  2O 

0.00284 

CuCl2 

0.025 

0.00905 

" 

0.05 

0.00614 

tt 

O.IO 

O.OO422 

tt 

O.2O 

O.OO29I 

HC1 

0.025 

0.00869 

" 

0.05 

0.00585 

" 

O.IO 

0.00384 

tt 

O.2O 

0.00254 

Aqueous 
Solution  of: 

Gms.  Equiv. 
Added  Salt 
per  Liter. 

Gms.  Equiv. 
Dissolved  T1C1 
per  Liter. 

MgCl2 

0.025 

o  .  00904 

u 

0.050 

0.0o6l8 

" 

O.  10 

0.00413 

tt 

O.20 

0.00275 

MnCl2 

0.025 

0.00898 

tt 

0.05 

0.00617 

u 

O.IO 

O.OO4I2 

u 

O.2O 

O.O0286 

KC1 

0.025 

0.00872 

u 

0.05 

0.00593 

K 

O.IO 

0.00399 

" 

O.2O 

O.O0265 

tt 

0.80 

O.OOI70 

NaCl 

0.025 

0.00869 

tt 

0.05 

0.00592 

tt 

O.IO 

0.00395 

(l 

O.2O 

O.OO27I 

TIClOs 

0.025 

0.00897 

tt 

0.025 

0.00894 

T1N03 

0.025 

0.00883 

tt 

0.05 

O.OO626 

tt 

O.IO 

0.00423 

THALLIUM  CHLORIDE 


716 


SOLUBILITY  OF  THALLIUM  CHLORIDE  IN  AQUEOUS  SALT  SOLUTIONS  AT  25°. 

(Noyes,  1890;  Noyes  and  Abbott,  1895;  Geffcken,  1904.) 


Aq.  Salt  Solution. 
Ammonium  Nitrate  NT^NOa 


Barium  Chloride  BaCl2 
u 

Cadmium  Sulfate  CdSO4 
u 

II 

Hydrochloric  Acid  HC1 
Lithium  Nitrate  LiNO3 


Potassium  Chlorate  KC103 
Potassium  Nitrate  KNO8 


Sodium  Acetate  CHsCOONa 


Sodium  Nitrate  NaNOs 


Sodium  Chlorate  NaClO« 


Thallium  BromateTlBrOs  (at  39.75°) 
ThaUium  Nitrate  T1NO3 


ThaUium  Sulfate  T12SO4 

ThaUium  Thiocyanate  T1SCN 

(at  39.75°) 

NOTE.  —  In  the  case  of  'the  results  for  thallium  bromate  and  thallium  thio- 
cyanate  at  39.75°,  the  solutions  were  saturated  with  respect  to  these  salts  as  well 
as  with  respect  to  thallium  chloride. 


G.  Mols^per  Liter. 

Cms.  per  Liter. 

'    Salt. 

T1C1.   " 

Salt. 

T1C1.  ' 

o 

0.01612 

0 

3-86i(G.) 

o-S 

0.02587 

40.02 

6.209 

i 

0.03121 

80.05 

7-473 

2 

0.03966 

160.  10 

9-497 

0.0283 

0.00857 

5-895 

2.052  (N.) 

0.1468 

0.00323 

30.59 

0-773 

0.030 

0.0206 

6.255 

4-933(N.) 

0.0787 

0.0254 

16.41 

6.081 

0.1574 

0.0309 

32.82 

7-399 

0.0283 

0.00836 

1.032 

2.002  (N.) 

0.0560 

0.00565 

2.043 

1-353 

0.1468 

0.00316 

5-357 

0-757 

o-5 

0.02542 

34-53 

6.085  (G.) 

i 

0.03035 

69.07 

7.266 

2 

0.03785 

138-14 

9.063 

3 

0.04438 

207.21 

10.630 

0-5 

0.0237 

61.28 

5-674(0.) 

0.015 

0.0170 

i.5i7 

4.070  (N.) 

0.030 

0.0179 

3-033 

4.286 

0.0787 

0.0192 

7.775 

4-597 

0.1574 

0.0212 

15-920 

5.076 

o-S 

0.0257 

50.55 

6.i53(G.) 

i 

0.0308 

IOI.  II 

7-375 

2 

0.0390 

202.22 

9-340 

0.015 

0.0168 

I.23I 

4.023  (N.) 

0.030 

0.0172 

2.462 

4.118 

0.0787 

0.0185 

6.46 

4-430 

0.1574 

0.0196 

12.92 

4-693 

0-5 

0.02564 

42.50 

6.i39(G.) 

I 

0.03054 

85.01 

7.313 

2 

0.03851 

I7O.O2 

9.  221 

3 

0.04544 

255-03 

10.88 

4 

0.05128 

340.12 

12.28 

o.S 

0.02320 

53-25 

5-555(G.) 

i 

0.02687 

106.5 

6-433 

2 

0.03060 

213 

7-326 

3 

0.03303 

3I9-S 

7.909 

4 

0.03850 

426 

9-215 

0.01567 

0.01959 

5-201 

4.690(N.&A.) 

0.0283 

0.0083 

7.518 

1.987  (N.) 

0.0560 

0.00571 

14.89 

1.368 

0.1468 

0.00332 

39-05 

0-795 

0.0283 

0.00886 

14.27 

2.  121  (N.) 

0.0560 

0.00624 

28.23 

1.494 

0.0107 

0.0119 

2.802 

2.849  (N.) 

0.02149 

0.01807 

5.632 

*.326(N.&A.) 

717 


THALLIUM   CHLORIDE 


SOLUBILITY  OF  THALLIUM  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  SALTS  AT  25° 

(Bray  and  Winninghoff,  1911.) 


Solvent. 


Saturated  Solution. 


Salt 

Gms.  Equiv. 

dj>*  of  Aq. 

Gms.  Equiv. 

dy.  of  Sat. 

Gms.  Equiv. 

Present. 

Salt,  per  Liter. 

Solvent. 

Salt  per  Liter. 

Sol. 

T1C1  per  Liter. 

None 

.  .  . 

0-9994 

0.01607 

KNO3 

O.O200I 

0.9973 

O.020 

I.OO09 

0.01716 

" 

O.05000 

0.9992 

0.04997 

1.0028 

0.01826 

" 

0.10005 

1.0023 

0.09998 

1.0063 

0.01961 

" 

0.3002 

I.OI45 

0.3000 

1.0194 

0.02313 

M 

1.0005 

1.0568 

0.9996 

1.0632 

0.03072 

K2SO4 

0.01997 

0.9975 

0.01996 

I.  0012 

0.01779 

(i 

O.O5000 

0.9995 

0.04996 

1.0037 

0.01942 

" 

0.  IOOO 

1.0030 

0.09989 

1.0074 

0.02137 

" 

0.3000 

1.0167 

0.29966 

I.O22I 

0.026OO 

M 

I 

1.0628 

0.9986 

1.0698 

0.03416 

T12S04 

0.02OO 

I.OOO7 

O.OI999 

1.0028 

0.01034 

" 

O.05OO 

1.0076 

0.04999 

I  .  0090 

0.006772 

" 

O.  IOOO 

I.OI9I 

0.09997 

I.O200 

o  .  004679 

One  liter  of  water  dissolves  2.7  gms.  thallo  thallic  chloride  3T1C1.T1C13  at  I5°-I7°, 
and  35  gms.  at  IOO°.  (Crookes,  1864;  Lamy;  Hebberling.) 


THALLIUM   CHROMATE  Tl2CrO4. 

100  gms.  H2O  dissolve  0.03  gm.  Tl2CrO4  at  60°,  and  0.2  gm.  at  100°. 

(Browning  and  Hutchins,  1900.) 

One  liter  of  aq.  31  per  cent  KOH  solution  dissolves  18  gms.  Tl2CrO4. 

(Lepierre  and  Lachand,  1891.) 

One  liter  of  H2O  dissolves  0.35  gm.  thallium  trichromate,  T^CrsOio,  at  15°, 
and  2.27  gms.  at  IOO°.  (Crookes,  1864.) 


THALLIUM   CYANIDE   T1CN  and  Double  Cyanides. 
SOLUBILITY  IN  WATER. 

(Fronmtiller,  1878.) 


Formula. 


Cyanide. 

Tl  Cyanide  T1CN 

Tl  Cobalti  Cyanide  Tl3Co(CN)6  3.6 

Tl  Zinc  Cyanide        2TlCN.Zn(CN)2    8.7 
Tl  Ferro  Cyanide     Tl4Fe(CN)6.2H20 


Gms.  Salt  per  100  Gms.  H2O. 

16.8    at  28.5°. 
at  oc 
at  o°;  15.2    at  14°;    29.6   at  31°. 

0.37  at  l8°;  3.93  at  IOI°.     (Lamy.) 


5.86  at  9.5°;   10.04  at  19.5° 


THALLIUM  FLUORIDE  TIP. 

100  gms.  H2O  dissolve  80  gms.  T1F  at  15°. 

THALLIUM  HYDROXIDE  T1OH. 


(Bttchner,  1865.) 


SOLUBILITY  IN  WATER. 

(Bahr,  1911.) 

to                          4lB  °f 

Mols.  T1OH 

Gms.  T10H 

t° 

Mols.  T1OH 

Gms.  T1OH 

Sat.  Sol. 

per  Liter. 

per  Liter. 

v  * 

per  Liter. 

per  Liter. 

O 

.231 

I.I5I 

254-4 

44-5 

2.442 

539-8 

I8.5 

.317 

1.554 

343-4 

54-1 

2.940 

649.7 

29 

•342 

1.803 

398.5 

64.6 

3.601 

795-8 

32.1 

•377 

1.861 

4II.2 

78.5 

4.673 

1033 

36 

.417 

2.075 

458.6 

90 

5.705 

1261 

40 

.446 

2.240 

495 

99.2 

6.708 

1483 

The  solutions  were  stirred  by  means  of  a  current  of  hydrogen.     The  solid  phase 
is  the  same  at  all  temperatures. 


THALLIUM  IODATE  718 

THALLIUM   IODATE  T1IO3. 

One  liter  aq.  solution  contains  0.578  gm.  T1IO3  at  20°.  (Bottger,  1903.) 

One  liter  aqueous  solution  contains  1.76.10^  mols.  TlIOs  at  25°  =  0.667  gm-» 

determined  by  means  of  electrodes  of  the  third  kind.  (Spencer,  1912.) 

THALLIUM   IODIDE  Til 

One  liter  sat.  solution  in  water  contains  0.0362  gm.  at  9.9°,  0.056  gm.  at  18.1° 
and  0.0847  Sm-  at  26°.  (Kohlrausch,  1908.) 

SOLUBILITY  OF  THALLIUM  IODIDE  IN  WATER. 

(Average  results  from  Bottger,  1903;  Kohlrausch,  1904-05;  Werther;  Crookes,  1864;  Lamy;  Hebberling.) 
t°.  o°.  20°.  40°.  60°.  .  80°.  100°. 

Cms.  Til  per  liter          0.02       0.06      0.15      0.35      0.70      1.20 

One  liter  of  2^  per  cent  aq.  ammonia  dissolves  0.761  gm.  T1C1. 
One  liter  of  6^  per  cent  aq.  ammonia  dissolves  0.758  gm.  T1C1. 
One  liter  of  90  per  cent  alcohol  dissolves  0.0038  gm.  T1C1. 
One  liter  of  50  per  cent  alcohol  dissolves  0.027  gm>  T1C1.  (Long,  1888.) 

Data  for  the  temperatures  of  solidification  of  mixtures  of  Til  and  TINOs  are 
given  by  Van  Eyk  (1901). 

THALLIUM  NITRATE  T1NO3. 

SOLUBILITY  IN  WATER. 

(Berkeley,  1904;  see  also  Etard,  1894;  Crookes;  Lamy.) 

e     Gms.  TINOa  per  100  Cms.  0        Gms.  TINOa  per  TOO  Gms. 

Solution.  Water.  Solution.  Water. 

o    3.76    3.91       60    31.55    46.2 

10      5-86      6.22  70     41.01       69.5 

10  8.72  9.55  80  52.6  in.o 

30  12.51  14.3  90  66.66  200. o 

40  17.33  20-9  I0°  8o-54  4i4-o 

50  23.33  3o-4  105  85.59  594.0 

Solid  phase.     TINOs  rhombic. 

loo  gms.  H2O  dissolve  43.5  gms.  T1NO3  +  104.2  gms.  KNO8  at  58°.  (Rabe,  1902.) 

THALLIUM   OXALATE  T12C2O4. 

One  liter  of  saturated  aqueous  solution  contains  15.77  gms.  T12C2O4  at  20°,  and 
18.69  gins,  at  25°.  (Bottger,  1903;  Abegg  and  Spencer,  1905.) 

SOLUBILITY  OF  THALLIUM  OXALATE  AT  25°  IN  AQ.  SOLUTIONS  OF: 


Thallium  Nitrate. 
(Abegg  and  Spencer.) 
Mol.  Concentration.            Grams  per  Liter. 

Potassium  Oxalate. 
(Abegg  and  Spencer.) 
Mol.  Concentration.            Grams  per  Liter. 

T1NO3. 
0.0 
O.O4II4 
0.0799 

o-i597 

T12C204. 

0.03768 
0.0264 
0.0195 
0.01235 

T1N03. 

o.oo 

10-95 
21  .26 
42.51 

T12C204. 
18.69 
13.10 
9.68 
6.128 

K2C204. 
0-0498 
0-0996 
0.2467 
0.4886 
0.9785 

T12C2O4. 
0.0351 
0-03565 
0.0390 
0-04506 
0-05536 

K2C204. 
8.281 

16.57 
41  .02 
81.25 
162.6 

T12C204. 
17.42 
17.69 
19.36 
22.37 
27.48 

THALLIUM   PHOSPHATE  (ortho)  T13PO4. 

One  liter  of  sat.  aqueous  solution  contains  4.97  gms.  T13PO4  at  15°  and  6.71 

(Crookes,  1864.) 


719 


THALLIUM  PICRATE 


THALLIUM  PICRATE  T10C6H2(NO2)3. 

SOLUBILITY  IN  WATER. 

(Rabe,  1901.) 
Cms. 

T10C,H2(N02), 

per  100  Gms. 

H20. 

0.135 

0.36 

o-575 


Gms. 


t, 


Solid  Phase. 


Solid  Phase. 


o 
18 

30 
40 

47 


Monoclinic  Red 


per  ioo  Gms. 
H20. 

1.04  Triclinic  Yellow 

1 . 10  " 

1.205 

0.825  "  60  1.73 

2-43 

ioo  gms.  H2O  simultaneously  sat.  with  both  salts  dissolve: 
0.132  gm.  C6H2(N02)3OT1   +  0.36  gm.  C6H2(NO2)8OK   at    o°. 
0.352     "  +  0.44  "  15°. 

0.38  +0.23  "20°.  (Rabe,  1901.) 

SOLUBILITY  OF  THALLIUM  PICRATE  IN  METHYL  ALCOHOL. 


45 

47 
50 
60 
70 


Gms. 

t°. 

TlOC,H2(NO2)s 
per  loo  Gms. 
CHjOH. 

o 

0.39        I 

18 

0-S9 

25 

0.70 

30 

o-795 

35 

0.90 

40 

i.  02 

45 

1.17 

47 

1.265 

(Rabe,  1901.) 


Solid  Phase. 


Red  Form  (monoclinic) 


Gms. 
to          T10C,H2(NO2)8 

per  ioo  Gms. 

CH3OH. 

45 

-195 

48 

.265 

50 

•325 

53 

.41 

57 

•54 

00 

•65 

65 

.84 

Solid  Phase. 


Yellow  Form  (triclinic) 


THALLIUM  SEI,ENATE  Tl2SeO4. 

SOLUBILITY  IN  WATER. 


9-3 

12 

20 

80 

100 


Gms.  Tl2SeO4 
per  100  Gms.  H2O. 

2.13 

2.4 

2.8 

8-5 
10.86 


Authority. 
(Tutton,  1907.) 

(Glauser,  1910.) 
« 

(Tutton,  1907.) 


THALLIUM  SULFATE  T12SO4. 

SOLUBILITY  IN  WATER. 

(Berkeley,  1904;  see  also  Crookes;  Lamy.) 
Gms.  TljiSC^  per  100  Gms. 


i  . 

Solution. 

Water. 

0 

2.63 

2.70 

IO 

3-57 

3-70 

20 

4.64 

4.87 

30 

5.8o 

6.16 

50 

8-44 

9.21 

I  . 

Solution. 

Water. 

60 

9.89 

10.92 

70 

II-3I 

12.74 

80 

12.77 

14.61 

00 

14.19 

16.53 

99-7 

15-57 

18.45 

ioo  gms.  H2O  dissolve  3.36  gms.  T12SO4  at  6.5°,  4.3  gms.  at  12°  and  19.14  gms. 

at  100°.  (Tutton,  1907.) 

One  liter  sat.  solution  in  water  contains  48.59  gms.  T12SO4  at  20°  (Noyes  and 
Farrel,  1911)  and  54.59  gms.  at  25°  (Noyes  and  Stewart,  1911). 

ioo  gms.  H2O  simultaneously  sat.  with  both  salts  dissolve: 
4.74  gms.  T12SO4  +  10.3  gms.  K2SO4  at  15°. 
11.5       "          "       +  16.4  62°. 

18.52      "  "        +26.2       "  100°.  (Rabe,  1902.) 


THALLIUM  SULFATE 


720 


SOLUBILITY  OF  THALLIUM  SULFATE  IN  AQUEOUS  SOLUTIONS  AT  25°. 

(Noyes  and  Stewart,  1911.) 

Saturated  Solution. 


Solvent. 

Salt  Present. 

T1NO3 

Formula  Wts. 
Salt 
per  Liter. 

tt 

0.04995 
O.2O 

NaHSO4 
H2SO4 

O.IOI5 
0.04967 

" 

0.09933 

Formula  Wts. 

Formula  Wts. 

j      _r 

Gms. 

Gms. 

Salt 
per  Liter. 

T12S04 
per  Liter. 

Sat  Sol. 

Salt 
per  Liter. 

T12S04 
per  Liter. 

o  .  0996 

0.08365 

.  .  . 

26.51 

42.17 

0.0497 

o  .  1080 

I-053I 

7.062 

54-44 

0.1988 

O.II73 

1-0754 

28.25 

59-13 

O.IOIO 

0.1161 

1.0596 

12  .12 

58.53 

o  .  0494 

0.1172 

I  .  0540 

4.878 

59-09 

0.0987 

0.1249 

I  .  0604 

9-747 

62.95 

SOLUBILITY  OF  THALLIUM  SULFATE  IN  AQUEOUS  SOLUTIONS  OF  SULFURIC 

ACID  AT  25°. 

(D'Ans  and  Fritsche,  1909.)  • 


'     H2S04. 

T12SO4.    ' 

H2S04. 

T12S04. 

.     ouiiu  jriiasc. 

0 

0.103 

T12S04 

4.89 

o-59 

T1HS04 

2.99 

0.46 

"     +T13H(S04)2 

4.92 

0.66 

" 

4-25 

0.61 

T13H(S04)2+T1HS04 

4.78 

0-75 

it 

4-55 

0.56 

T1HSO, 

4.26 

1.  01 

* 

4-79 

o-55 

" 

4-03 

i.  08 

•i 

THALLIUM  DOUBLE   SULFATES 


SOLUBILITY  IN  WATER  AT  25°. 

(Locke,  1901.) 


Double  Sulfate. 

Tl  Copper  Sulfate 
Tl  Nickel  Sulfate 
Tl  Zinc  Sulfate 


Formula. 


Tl2Cu(SO4)2.6H2O 
Tl2Ni(S04)2.6H20 
Tl2Zn(SO4)2.6H2O 


Salt  per  100  cc.  H2O. 
Gms.  Anhydrous.       Gms.  Mols. 
8.1  O.OI22 

4.6l  O.OO7 

8.6  0.0129 


THALLIUM  SULFIDE  T12S. 

One  liter  of  sat.  aqueous  solution  contains  0.215  gm-  T12S  at  20°.  (Bottger,  1903.) 

A  diagram  and  discussion  of  the  fusion  points  of  T12S  +  S,  T12S  +  Se  and 
T12S  +  Te  are  given  by  Pelabon,  1907. 


(Seubert  and  Elten,  1892.) 


THALLIUM  SULFITE  T12SO8. 

100  gms.  H2O  dissolve  3.34  gms.  T12SO3  at  15.5°. 

THALLIUM  THIOCYANATE  T1SCN. 

SOLUBILITY  IN  WATER  AND  IN  AQUEOUS  SALT  SOLUTIONS. 

(Bottger,  1903;  Noyes,  1890;  Noyes  and  Abbott,  1895.) 

One  liter  sat.  aq.  solution  contains  3.154  gms.  T1SCN  at  20°,  3.905  gms.  at  25* 
and  7.269  gms.  at  39.75°. 


Aq.  Salt  Solution. 


Gms.  Mols.  per  Liter. 
SalT  T1SCN. 

Thallium BromateTlBrOa (excess)  39-75     0.01496     O.O22I 


Gms.  per  Liter. 


Thallium  Nitrate  T1NO3 
« 

Potassium  Thiocyanate,  KSCN 


25 
25 
25 


0.0227 
0.0822 


Salt.  T1SCN. 

4.966  5.793(N.&A.) 

0.00852   6.04.  2.233(N.) 

0.00406  21.88  .  1.064 

0.0083    2.208  2.i76(N.) 


721 


THALLIUM  VANADATES 


THALLIUM  VANADATES. 

SOLUBILITY  IN  WATER. 


Vanadate. 

Tl.  meta  vanadate 
"  ortho  vanadate 
"  pyro  vanadate 
"  vanadate 


Formula. 

T1V03 


(Carnelly,  1873;  Liebig,  1860.) 

Gms.  Vanadate  per  100  Gms.  H2O. 


At  15°. 

0.087  C1*0 
I 
O.20  (14°) 

0.107 


THEBAINE  (Para  Morphine)  Ci9H2iNO3. 

SOLUBILITY  IN  SEVERAL  SOLVENTS. 

Solvent. 

92  Wt.  %  Alcohol 

Ether 

Aniline 

Pyridine 

Piperidine 

Diethylamine 

THEOBROMINE  (Dimethyl  Xanthine)  C6H2(CH3)2N402. 
SOLUBILITY  IN  SEVERAL  SOLVENTS. 


t°. 

Gms.  Thebaine  per 
100  Gms.  Solvent. 

25 

O.I 

10 

0.71 

20 

30 

20 

9 

20 

2 

2O 

0.7 

At  i  oo6. 
0-21 
1.74 
0.26 

°-29 


Authority. 


(Scholtz,  1912.) 


Solvent. 


Water 


t°. 

N4O2  per  zoo  Gms. 
Solvent. 

Authority. 

18 

0.0305 

(Paul,  1901.) 

15-20 

0.059 

(Squire  &  Caines,  1905.) 

18 

0.047 

(Paul,  1901.) 

18 

0.083 

" 

18 

I.78 

it 

18 

4.56 

" 

15 

3.69 

(Brissemoret,  1898.) 

21 

0.045 

(Squire  &  Caines,  1905.) 

15-20 

O.O2 

" 

15 

0.005 

(Wester  &  Bruins,  1914.) 

15 

O.OOS 

" 

b.  pt. 

0.021; 

(Gockel,  1897.) 

b..pt. 

0.032 

" 

Aq.  0.25  n  HC1 

"   i       wHCl 

"  o.i    wNaOH 

"  0.25  n       " 

"   i5.6percentNa3(PO4)2.Sol. 
92.3  Wt.  %  Alcohol 
90  Wt.  %  Alcohol 
Dichlorethylene 
Trichlorethylene 
Carbon  Tetrachloride 
Ether 

THIOPHENE  MonoCARBONIC  ACIDS  a,  ft  and  a  C4H3SCOOH. 

The  solubility  of  the  three  isomers  is  given  by  Voerman  (1907)  as  0.57  gm.  of 
the  a  acid  per  100  cc.  sat.  solution  at  21°;  0.445  gm-  of  the  0  acid  at  18°,  and  0.75 
gm.  of  the  a  acid  at  17°.  The  solvent  is  not  stated.  Data  for  the  solidification 
points  of  mixtures  of  the  a  and  /3  acid  are  also  given.  • 

THEOPHYLLINE  (Theocin)  C6H2(CH3)2N4O2.H2O. 

100  gms.  H2O  dissolve  0.52  gm.  theophylline  at  15-20°.         (Squire  &  Caines,  1905.) 
100  cc.  90  vol.  %  alcohol  dissolve  1.25  gms.  theophylline  at  15-20°. 

THORIUM  EMANATIONS. 

Data  for  the  solubility  of  thorium  emanations  are  given  by  Klaus  (1905). 

THORIUM    ChloroACETATES. 

SOLUBILITY  IN  WATER  AT  25°.    (Karl.  1310.) 

Name  of  Salt.  Formula.  SS^SfjR 

Basic  Thorium  Monochloroacetate     (ClCH2COO)2Th(OH)2.H2O       0.0663 
Basic  Thorium  Dichloroacetate  (Cl2CHCOO)2Th(OH)2  0.0887 

Basic  Thorium  Trichloroacetate          (Cl3C.COO)2Th(OH)2  0.0091 


THORIUM  BORATE 


722 


THORIUM  BORATE. 

The  precipitate  which  results  when  thorium  nitrate  is  added  to  a  solution  of 
borax  is  not  a  stable  compound.  Solubility  determinations  made  by  four  suc- 
cessive extractions  of  it  at  18°  with  water,  gave  the  following  gms.  of  material 
per  100  gms.  H2O;  0.5366,  0.1250,  0.0611  and  0.0560.  After  the  fourth  ex- 
traction, the  residue  then  contained  10.14%  B2O3  and  after  boiling  10  gms. 
with  100  cc.  of  H2O  for  6  hrs.  and  repeating  this  four  times,  it  contained  9.63- 
9.81%  B2O3.  (Karl,  1910.) 


THORIUM  HIPPURATE  Th(C6H6.CO.CH2.NH.COO)4. 
100  gms.  H2O  dissolve  0.0318  gm.  of  the  salt  at  25°. 


(Karl,  1910.) 


THORIUM   OXALATE  Th(C2O4)2.6H2O. 

SOLUBILITY  IN  AQUEOUS  SOLUTIONS  OF  AMMONIUM  OXALATE  AT  25°. 

(Hauser  and  Wirth,  igoga,  1912.) 


Gm.  Mols.  per  1000  Gms. 
Sat.  Sol. 


(NHOzCA. 

Th(CA),. 

0.00033 

0.00005 

0.00072 

O.OOOI2 

0.00120 

O.OOO2O8 

O.OOI53 

0.00026 

o.6oif 

0.195 

i.iSif 

0.427 

1.420} 

0.540 

i.48ot 

0.563 

Solid  Phase. 


Th(CA)2.6H20 


[Th(C204]3(NH4)2.3H20 


Normality 

Vjms.  J.n\j2 
per 
1000  Gms. 
Sat.  Sol. 

0.01 

0.040 

O.IO 

0.5* 

2.203 
7.660 
10.63 

0.5* 

0.5* 
0.5* 

15.90 
17.60 
17-75 

Solid  Phase. 


[Th,(CA>iKNHl)fr7HlO 


*  In  these  cases  the  greater  part  of  the  ammonium  salt  entered  the  solid  phase  complex  and  it  was, 
therefore,  necessary  to  add  additional  ammonium  oxalate  until  constant  results  were  obtained. 

t  In  these  cases  the  solvent  was  saturated  ammonium  oxalate  solutions  containing  an  excess  of  the 
crystals. 

A  thorium  ammonium  oxalate  of  the  composition  Th(C2O4.NH4)4.4H2O  is 
described  by  Brauner  (1898).  It  is  partially  hydrolytically  decomposed  in 
aqueous  solution  and  a  solubility  determination  made  by  analyzing  the  solution 
from  which  the  nearly  pure  salt  began  to  crystallize,  showed  that  100  gms.  H2O 
contain  90.3  gms.  Th(C2O4.NH4)4.4H2O  and  9.3  gms.  of  (NH4)2C2O4  (=  an  addi- 
tional \  mol.  wt.) 


SOLUBILITY  OF  THORIUM  OXALATE  IN  AQUEOUS  SOLUTIONS  OF 
HYDROCHLORIC  ACID. 


Solid  Phase. 


Results  at  17°. 

Results  at  25°. 

(Colani,  1913.) 

(Hauser  and  Wirth,  1912.) 

Gms.  per  100  Gms. 
Sat.  Sol. 

Cone,  of 
Aq.  HC1  in 

Gm.  ThO2  per 
1000  Gms.             Sc 

HC1.              ThtCjOOj. 

Per  cent. 

Sat.  Sol. 

o            0.0017 

24.8 

0  .  100      3Th(C 

1.2           0.0035 

37 

3-450 

3.6         0.0061 

37-6 

3-492 

4.6         0.0094 

8.4         0.017 

13.1         0.028 

16.2         0.038 

19.8         0.064 

Results  at  50°. 

(Colani,  1913.) 

Gms.  per  100  Gms. 
Sat.  Sol. 

HC1. 
0 

Th(C204)2. 
0.0017 

4.1 

8-4 

0.010 

0.028 

12.4 
16.1 
18 
19.9 

21.6 

0.057 

0.103 
0.134 
0.169 
0.232 

Data  are  also  given  for  the  solubility  of  thorium  oxalate  in  aqueous  solutions 
of  mixtures  of  hydrochloric  and  oxalic  acids  at  the  above  temperatures. 


723 


THORIUM   OXALATE 


SOLUBILITY  OF  THORIUM  CHLOROOXALATE,  3Th(C2O4)2ThCl4.2H2O,  IN  AQUEOUS 

HYDROCHLORIC  ACID. 

(Colani,  1913.) 
Cms,  per  100  Gms.  Sat.  Sol. 


12 
15 
12 
15 

12 
IS 


'     HC1. 

Th4(c2o4)ci4: 

23 
26.3 

O.I2 
0.17 

29.9 
32.5 

0.27 
0.48 

33-1 

0-53 

35 

1.03 

50 
50 
50 
50 

50 
50 


Cms,  per  100  Gms.  Sat.  Sol. 
HCL    ' 
21.2 
23 

26.8 
29.8 

32.3 
34-6 


0.29 
0.34 
0.46 
0.75 

1.51 
2.59 


Results  are  also  given  showing  the  effect  of  oxalic  acid  upon  the  solubility  of 
the  above  salt  in  aqueous  hydrochloric  acid. 

SOLUBILITY  OF  THORIUM  OXALATE  IN  AQUEOUS  OXALIC  ACID  SOLUTIONS. 


Results  at  25°. 
(Hauser  and  Wirth,  1912.) 


Normality  of 
Aq.H2CA. 


Gm.  ThO2  per 
1000  Gms.  Sat.Sol. 


<,  ,.  ,  p, 
Sohd  Phase. 


Results  at  50°. 

(Colani,  1913.) 
Gms.  per  100  Gms.  Sat.  Sol. 


H2C2Q4. 
I  0.0015          Th(C2O4)2.6H2O  1.7 

Sat.  Solution  0.0030          "  +H2c2o4.2H2o  9.3 

03 

SOLUBILITY  OF  THORIUM  OXALATE  IN  AQUEOUS  SOLUTIONS  OF  SULFURIC 

ACID  AT  25°. 
(Hauser  and  Wirth,  igoga,  1912;  Wirth, 


Th. 
0.0002 

o.ooi 
0.003 


Nonnalityof 
Aq.H2S04. 

0.25 
0.5 

i 

2.1 
3.2 


Sat.  Sol. 
0.07 
0.14 

0.26 

0.418 
0.71 


Solid  Phase. 


Th(C2O4)2.6H2O 


4.32 
4-9 

6.175 

6.885 
8.45 


Sat.  Sol. 
1.  10 
1.32 

1.513 

1.794 
2.473 


Solid  Phase. 


Th(CjO4)2.6H2O 


THORIUM  PICRATE  Th(C6H2N3O7)4.ioH2O. 
100  gms.  H2O  dissolve  0.3052  gm.  of  the  salt  at  25°. 

THORIUM   SELENATE  Th(SeO4)2.9H2O. 

100  gms.  H2O  dissolve  0.498  gm.  Th(SeO4)4  at  o°  and  1.972  gms.  at  100°. 

THORIUM   SULFATE  Th(SO4)2. 

SOLUBILITY  IN  WATER. 

(Roozeboom,  1890;  Demarcay,  1883.) 


(Karl,  1910.) 


(Cleve,  1885.) 


Gms.  Th(SO4)2 

Per                 Solid 

-o       Gms.  Th(SO4)2  per 
100  Gms.  H2O. 

Solid 
Phase. 

' 

100  Gms. 

H20.    '               Phase. 

O 

0 

•74<R) 

0 

.88(D)  Th(S04)2.9H20 

O 

i 

•5o(R) 

Th(SO4)2.6H2O 

10 

0 

.98 

I 

.02 

15 

i 

•63 

" 

20 

X 

•38 

I 

•25 

30 

2 

•45 

44 

30 

I 

•995 

I 

.85 

45 

3 

•85 

44 

40 

2 

.998 

2 

.83 

60 

6 

.64 

" 

5° 

5 

•22(51°) 

4 

.86 

17 

9 

.41  (D) 

ThCSOJj^HjO 

55 

6 

.76 

6 

•5± 

40 

4.  04  (R)  4  -5  (35°  E>) 

o 

i 

.0 

Th(SC>4)2.8Ha 

50 

2-54 

1.94 

(55") 

44 

15 

i 

•38 

60 

1-63 

" 

25 

X 

•85 

44 

70 

1.09 

1.32 

(75°) 

• 

44 

3 

•71 

• 

95 

0.71 

n 

Additional  results  for  the  .8H2O  and  the  .9H2O  salt,  in  fair  agreement  with  the 
above,  are  given  by  Wyrouboff  (1901). 


THORIUM   SULFATE 


724 


SOLUBILITY  OF  THORIUM  SULFATE  IN 

AQUEOUS  SOLUTIONS  OF: 

Ammonium  Sulfate  at  16°. 

Lithium  Sulfate  at  25°. 

(Barre,  igii.) 

(Barre,  1912.) 

Gms.  per  100  Gms.  H2O. 

Solid  Phase. 

Gms.  per  100  Gms.  H2O. 

(NH4)2SO4.                    Th(SO4)2. 

Li2S04.                        Th(S04)2: 

2.13                        3.361 

TKSO^.gl^O 

o                        1.722 

4.80                        5.269 

" 

2-57                 4-13 

10.02                        8.947 

" 

4-93                   6.20 

•16.56                      I3-330 

"  +1.1.4 

6.98                  7-95 

28                              10.359 

1.1.4 

9.23                  9.68 

35.20                        9.821 

"    +1.2.2 

11.13                11.05 

45.14                        6.592 

1.2.2- 

13.18                12.54 

49-05                        5-750 

'' 

16.12                14-52 

52.88                        4.583 

1-3-3 

2O.49                        l6.Q2 

69.74                        1.653 

" 

25.18                        18.87 

1.1.4  =  Th(S04)2.(NH4)2S04.4H20;    1.2.2  = 

Th(S04)2.2(NH4)2S04.2H20;    1.3.3 

Th(S04)2.3(NH4)2S04.3H20. 

SOLUBILITY  OF  THORIUM 


Results  at  16°. 

Gms.  per  100  Gms.  H2O. 

K2S04. 

Th(SOJ2. 

0 

i-39 

0.424 

1.667 

.004 

2.193 

•152 

3-i9i 

.224 

2.514 

.283 

2.222 

.348 

1.706 

-378 

I-637 

.487 

0.870 

.844 

0.370 

3.092 

0.070 

4-  050 

O.O27 

4.825 

0.003 

SULFATE  IN  AQUEOUS  SOLUTIONS  OF  POTASSIUM 
SULFATE. 

(Barre,  1911.) 

Results  at  75°. 


Solid  Phase. 


Gms.  per  100  Gms.  H2O. 


Th(S04)2.K2S04.4H20 


K2SO4. 
O 

0.865 
1.167 

0.9248 
i-i37 
I-I73 

1  .172 

I  .121 

1  .270 
1.296 

1.852 

0.907 

0-495 
0.297 

3-«7 

4-659 
5-348 

O.2OI 
0.256 
0.170 

5-932 

0.123 

7.177 
9.706 

0.031 
O.O22 

Th(S04)2.3^K2S04 


SOLUBILITY  OF  THORIUM  SULFATE  IN  AQUEOUS  SOLUTIONS  OF  HYDROCHLORIC 
ACID  AND  OF  NITRIC  ACID  AT  30°. 

(Koppel  and  Holtkamp,  1910.) 


In  Aq.  Hydrochloric  Acid. 


Wt.  %  HC1 
in  Solvent. 

Gms.  Th(SO4)' 
per  too  Gms. 
Sat.  Sol. 

0 

2.15 

4-55 

3-541 

6-95 

3-431 

12.14 

2.811 

15.71 

2.360 

18.33 

2.199 

20 

2.IIO 

20 

2.I4I 

23-9 

1.277 

Solid  Phase. 


In  Aq.  Nitric  Acid. 

Solid  Phase. 


Wt.  %  HN03 
in  Solvent. 

oms.  iiivov. 
per  zoo  Gn 
Sat.  Sol. 

0 
5-17 

2-15 

3-68 

IO.O4 

16.68 

4.20 

4.84 

21.99 

28.33 
28.51 

4-47 
3-88 

33-17 
38.82 

3-34 
2.51 

725 


THORIUM   SULFATE 


SOLUBILITY  OF  THORIUM  SULFATE  IN  AQUEOUS  SOLUTIONS  OF: 


Sodium  Sulfate  at  16°. 
(Barre,  1910,  1911.) 
Gms.  per  100  Gms.  H20. 

Sulfuric  Acid  at  25°. 

(Barre,  1912.) 
Gms.  per  100  Gms.  H2O. 

Na2S04. 
1.094 
1.960 
2.98 
4.II 

5-79 
9-35 
12.24 

15-36 

1  .  7432           ThtSO^.NajSCVGHjO 
2.387 
3-962 

3-375 
2.136 

1-379 
1.169 
i  .  048 

H2S04. 
O 
1.072 
I.94I 
2.821 

3.843 
5.212 

8.055 
10.105 

1.722 
I.9I9 
2.OI7 
2.060 
2.o6l 
2.035 
1.863 
I.7O2 

SOLUBILITY  OF  THORIUM  SULFATE  IN  AQUEOUS  SOLUTIONS  OF  SULFURIC  ACID 


Results  at  25°. 

(Wirth,  1912.) 

Results  at  20°  and  at  the  b.-pt. 

(Koppel  and  Holtkamp  1910.) 

Normality     Gms.  Th(SO4)2 

Wt.  % 

Gms.  Th(SO4)2 

of 

per  100  Gms.        Solid  Phase. 

t°.            H2SO4  in 

per  loo  Gms. 

Solid  Phase. 

Aq.  H2S04. 

Sat.  Sol. 

Solvent. 

Sat.  Sol. 

O 

1  .  593           Th(S04)2.9H20 

20            5 

1.722 

Th(SO4)2.8HJO 

I.I 

1.831 

20              15 

0.9752 

" 

2.l6 

1.488 

20              25 

0.3838 

" 

4-32 

0.8751 

2O             40 

O.OIO3 

ThtSO^^HjO 

6.68 

0.4312 

b.  pt.          5 

0.7407 

TMSOJj.SHjO 

9.68 

0.1045         Th(SO4)».8HaO 

IO 

0.4808 

" 

10.89 

0.0636 

IS 

0.3882 

" 

15.15 

0.0308         Th(SO4)i.4HjO 

Results  at  30°. 

(Koppel  and  Holtkamp,  1910.) 

Wt.  %  H2SO4 
in  Solvent. 

Gms.  ThCSOt),  per       Solid  Phase           Wt.  %  H2SO4    Gms.  ThCSO^j  p 
100  Gms.  Sat.  Sol.                                       in  Solvent.      looGms.  Sat.  So 

fr  Solid  Phase. 

0 

2.152             Th(SO4)t.8 

H2O             15.03 

1.484 

TMSO^.SHjO 

0.466 

2.055 

23.64 

0.7196 

" 

0.72 

2.085 

32.68 

0.3364 

" 

1.468 

2.267 

37-80 

0.077 

Th(S04)*.4HtO 

2.983 

2.3H 

43.28 

0.0213 

" 

4.38 

2.367 

45.69 

0.0047 

" 

4-97 

2.323 

74 

o.i  208 

« 

9-95 

1  .  961 

80.5 

0 

" 

THORIUM  m  Nitrobenzene  SULFONATE  Th(C6H4.NO2.SO3)4.7H2O. 

100  gms.  H2O  dissolve  61  gms.  of  the  anhydrous  salt  at  15°.          (Holmberg,  1907.) 

THULIUM  OXALATE  Tma(C2O4)3.9H2O(?.ioH2O). 

100  cc.  aq.  20%  methyl  amine  oxalate  dissolve  approx.  4.082  gms.  thulium  oxalate. 
100  cc.  aq.  20%  ethylamine  oxalate  dissolve  approx.  5.728  gms.  thulium  oxalate. 
loo  cc.  aq.  20%  triethylamine  oxalate  dissolve  approx.  1 .340  gms.  thulium  oxalate. 

(Grant  and  James,  1917.) 

THULIUM    Bromonitrobenzene    SULFONATE    Tm(C6H3Br.NO2.SO3, 1.4.2)3.- 
I2H2O. 

100  gms.  sat.  solution  in  water  contain  6.379  Sms.  of  the  anhydrous  salt  at  25°. 

(Katz  and  James,  1913.) 

THYMOL  (3  Methyl  6  Isopropyl  Phenol)  C3H7.C6H3.OH.CH3. 
SOLUBILITY  IN  WATER.     (Seidell,  1912.) 

f  o          Gms.  Thymol  per  f  0          Gms.  Thymol  per 

zoo  Gms.  Sat.  Sol.  100  Gms.  Sat.  Sol. 

10  0.067  25  0.0995  37  0.132 
15  0.077  3°  0.112  40  0.141 
20  0.088  35 


O.II2 
O.I26 


Gms.  Thymol  per 
100  Gms.  Sat.  Sol. 


THYMOL  726 

SOLUBILITY  OF  THYMOL  IN  AQUEOUS  HYDROCHLORIC  ACID.   (Seideii,  1912.) 

Normality  of  Gm.  Thymol  per  100  cc.  Sat.  Sol,  at: 

Aq.HCl. 

o 

O.I 

O.5 

I 

2.5 

5 

100  cc.  90  vol.  per  cent  alcohol  dissolve  about  300  gms.  of  thymol  at  I5°-2O°. 

(Squire  and  Caines,  1905.) 

SOLUBILITY  OF  THYMOL  IN  SEVERAL  OILS.     (Seideii,  1912.) 

Gms.  Thymol  per  100  Gms.  of: 


25°. 

37.2°. 

0.0995 

O.O968   (^26  =  I.OO2) 
O  .  0884   (^25  =  I  «OOg) 
O.O8O2   (<*2S  =  I.Ol8) 

0.132 

0.129 

O.I2I 
O.II2 

0.0612  (1*25  =  1.043) 

0.0935 

0.0445 

O.O772 

t°. 

Olive 

Peanut 

Cod  Liver 

Liquid 

Castor 

Cottonseed 

Linseed 

Oil. 

Oil. 

Oil. 

Petrolatum. 

Oil. 

Oil. 

Oil. 

10 

46.2 

73 

50 

3-i 

8l.2 

56.2 

62.3 

IS 

50-1 

73-8 

52 

3-95 

Q0.2 

64 

63-1 

20 

56.2 

74.6 

55-5 

5-6 

101  .5 

74.2 

65.1 

25 

66.9 

76.4 

63.1 

9.78 

Il6.5 

89.4 

69 

30 

84.5 

83.2 

77 

16.3 

137    ' 

II3-7 

78.3 

35 

III 

106.7 

102 

25-5 

165 

146.5 

100 

37 

124-3 

130.5 

II6.5 

29.9 

180 

166.5 

II6.5 

40 

I5I-9 

212.5 

150 

38-9 

213 

217-5 

152 

The  specific  gravities  of  the  above  saturated  solutions  and  of  solutions  of 
lower  concentrations  of  thymol  in  the  several  oils  are  also  given. 

DISTRIBUTION  OF  THYMOL  BETWEEN  WATER  AND  OILS  AT  25°  AND  AT  37°. 

(Seideii,  1912.) 
Water  +  Olive  Oil.          Water  +  Cod  Liver  Oil.        Water  +  Peanut  Oil. 

Gms.  Thymol  per  TOO  cc.  Gms.  Thymol  per  100  cc.  Gms.  Thymol  per  TOO  cc. 

*"•  '     OH  i£o '   —  •  ' oii  5^5     '  — •     '      oii  H^T"    -r- 

Layer  (c0).    Layer  (cj.     Cw        Layer  (c0)    Layer  (cw).      Cv>  Layer  (c0).     Layer  (c«,). 

25     0.1014    44-95     443     0.1079     49          454    0.1077       46.48     431 
25     0.0848    36.. 34    428    0.0816    32.58    400    0.0786       32.45     413 
25    0.0349     16.26    465     0.0371     16.18    436    0.0395       16.16     409 
25    0.0106      4.54    430    0.0127      4-57    359    o.oo88(?)     4.63     523 
37    0.1087    46.35    427    0.1099    43-8i     399 
37    0.0807    33-48    415    0.0862    32.90    380 
37    0.0381     16.24    426    0.0574     22.51     392 
37    0.0122      4.61     378    0.0250      8.86    357 

Freezing-point  data  for  mixtures  of  thymol  and  sulfuric  acid  are  given  by 
Kendall  and  Carpenter  (1914). 

Results  for  thymol  +  bromotoluene  are  given  by  Paterno  and  Ampola  (1897). 

TIN  Sn. 

DISTRIBUTION  OF  TIN  BETWEEN  AQUEOUS  HYDROCHLORIC  ACID  AND  ETHER  AT 
ROOM  TEMPERATURE.    (Mylius,  1911.) 

When  i  gm.  of  tin  as  the  chloride,  SnCl4,  is  dissolved  in  100  cc.  of  aqueous 
hydrochloric  acid  and  shaken  with  100  cc.  of  ether,  the  following  per  cents  of  the 
metal  enter  the  ethereal  layers.  With  20%  HC1,  17  per  cent;  with  15%  HC1, 
28  per  cent;  with  10%  HC1,  23  per  cent;  with  5%  HC1,  10  per  cent  and  with 
i%  HC1,  0.8  per  cent  of  the  tin. 


727  TIN  CHLORIDE 

TIN   CHLORIDE  (Stannous)  SnCl*. 

100  gms.  H2O  dissolve  83.9  gms.  SnCl2  at  o°  and  269.8  gms.  at  15°.     Sp.  Gr. 
of  Solutions  1.532  and  1.827  respectively.  (Engel,  1889;  Michel  and  Krafft,  1851.) 

SOLUBILITY  OF  STANNOUS  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF 
HYDROCHLORIDE  ACID  AT  o°. 

(Engel.) 


Milligram 

Mols.  per  10  cc. 

Sp.  Gr. 

Grams  per  100  cc. 

Solution. 

of 

Solution. 

HC1. 

iSnCl*. 

Solution. 

HC1. 

SnClj. 

0 

74-0 

•  1-532 

o.o 

70.26 

6.6 

66.7 

1.489 

2.405 

63-33 

13-54 

63-7S 

1.472 

4-935 

60.52 

24.8 

68.4 

1.524 

9.04 

64.95 

34-9 

8l.2 

I  .625 

12.72 

77.11 

40-0 

94.2 

1.724 

14.58 

89.45 

44-o 

117.6 

1.883 

16.04 

111-7 

49-4 

147.6 

2.II4 

18.01 

I38.6 

66.0 

156.4 

2.190 

24.05 

148.5 

78.0 

157-0 

2.199 

28.43 

149.0 

100  gms.  acetone  dissolve  55.6  gms.  SnCl2  at  18°.     (dip  = 

1.6.)      (Naumann, 

1904.) 

100  gms.  ether 
100  gms.  ethyl 

dissolve  11.4  gms.  SnCl2.2H 
acetate  dissolve  31.2  gms. 

2O  at  o°-35.5°. 
SnCl2.2H2O  at 

-2°,  35-53  gms.  at 

+22°  and  73-44  gms.  at  82°.  (von  Laszynski,  1894.) 

100  gms.  ethyl  acetate  dissolve  4.46  gms.  SnCl2  at  18°.     dip  of  the  sat.  solution 

=  0.9215.  (Naumann,  1910.) 

ioo  gms.  95  per  cent  formic  acid  dissolve  4.1  gms.  SnCl2  at  19°.     (Aschan,  1913.) 
Freezing-point  data  for  mixtures  of  SnCl2  +  ZnCl2  are  given  by  Herrmann 
(1911). 

TIN   CHLORIDE   (Stannic)   SnCl4. 

DISTRIBUTION  OF  STANNIC  CHLORIDE  BETWEEN  WATER  AND  XYLENE. 

(Smirnoff,  1907.) 

Very  concentrated  aqueous  stannic  chloride  solutions  were  agitated  with 
xylene  at  various  temperatures  and  the  amount  of  SnCl4f  in  terms  of  Cl,  which 
entered  the  xylene  layer  was  determined.  The  amount  of  Sn  and  Cl  in  the 
xylene  was  found  to  correspond  to  SnCl4. 

Results  for  Xylene  +  SnCl4.5H20.  Results  for  Xylene  +  SnCl4.4H2O. 


Gms.  Cl  per  ioo  Gms. 

^ 

Gms.  Cl  per  ioo  Gms. 

c 

t°. 

Aq. 
Layer,  c. 

Xylene 
Layer,  c'. 

c' 

r. 

Aq. 
Layer,  c. 

Xylene 
Layer,  c'. 

66 

40.35 

0.08 

504.4 

66 

41.9 

0.92 

45-3 

80 

39-95 

0.18 

228.5 

80 

41.91 

1.56 

27 

97-5 

40.24 

0-33 

122.  I 

IOO 

41.85 

2.52 

!6.7 

in 

40.27 

0.68 

59-3 

III 

41.68 

3-23 

12.9 

Per  cent  Cl  in  SnCl4.sH2O  =  40.38.  Per  cent  Cl  in  SnCl4.4H2O  =  42.37. 

Results  for  Xylene  +  SnCl4.3H2O. 

Gms.  Cl  per  too  Gms. 

t°«  Aq.  Xylene  ~i' 

Layer,  c.  Layer,  c'. 

80  43.2  .    9.93  4.4 

94                    42.54  9.32  4.6 

ioo                    42.64  10.56  4.1 

in                    42.31  10.03  4-2 
Per  cent  Cl  in  SnCl4.3H2O  =  45.12. 


TIN  HYDROXIDE  728 

TIN  HYDROXIDE  (Stannous)  Sn(OH)2. 
One  liter  of  the  saturated  solution  in  water  contains  0.0000135  gm.  mols. 

Sn(QH)2  at  25°.  (Goldschmidt  and  Eckhardt,  1906.) 

SOLUBILITY  OF  STANNOUS  HYDROXIDE  IN  AQUEOUS  SODIUM  HYDROXIDE 
SOLUTIONS  AT  25°. 

(Goldschmidt  and  Eckhardt,  1906.) 

The  authors  desired  to  ascertain  whether  the  mono,  NaHSnO2,  or  the  disodium 
salt,  Na2SnC>2,  predominates  in  alkaline  tin  hydroxide  solutions.  Given  amounts 
of  carefully  prepared  tin  chloride,  made  from  tin  and  HC1,  and  sodium  hydroxide 
solutions  were  mixed  in  vessels  containing  hydrogen.  The  mixtures  were  shaken 
at  25°  and  the  clear  supernatant  solutions  in  contact  with  the  precipitated 
Sn(OH)2,  analyzed. 

Gm.  Mols.  per  Liter.  Gm.  Mols.  per  Liter. 


Total  Na. 

NaHSn02. 

NaOH. 

Total  Na. 

NaHSnO2. 

NaOH. 

0.00451 

0.0009845 

0.003525 

0.02250 

0.00838 

O.OI4I2 

0.00(58o 

0.002l8 

0.00462 

0.02788 

0.01038 

0.01755 

0.01149 

0.003495 

0.007995 

0.02940 

0.00874 

O.O2066 

0.02143 

0.006935 

0.014495 

O.03OI2 

0.00865 

0.02147 

0.02143 

O.00660 

0.01483 

0.03036 

O.OIO82 

0.01954 

0.02186 

0.00628 

0-015575 

0.03044 

0.009405 

0.021035 

SOLUBILITY  IN  AQUEOUS  SODIUM  HYDROXIDE  SOLUTIONS.     MOIST  TIN 
HYDROXIDE  USED.  ORDINARY  TEMPERATURE. 

(Rubenbauer,  1902.) 


Gms.  per  20  cc.                     Mol. 
Solution.                 Dilution  of  the 

Gms.  per  20  cc.                       Mol. 
Solution.                     Dilution  of  the 

Na. 

o  .  2480 

0.3680 
0.6394 

Sn. 
0.1904 
0.2614' 
0.4304 

NaOH. 

1.86 

i-*5 

0.72 

Na. 
0.8326 
0.9661 
2.1234 

Sn/ 
0.5560 
0.7849 
1.8934 

NaOH. 

o-55 

'0.48 
0.23 

TIN  IODIDE    (Stannous)  SnI2. 

SOLUBILITY  IN  WATER  AND  IN  AQUEOUS  HYDRIODIC  ACID. 

(Young,  1897.) 
t*.  Gms.  Snla  per  100  Gms.  Aqueous  HI  Solutions  of: 


' 

o^=H20. 

5-83%. 

9-60%. 

15-2%. 

20.44%. 

24-8%. 

30.4%. 

36.82%. 

2O 

0.98  ' 

O-2O 

0.23 

0.6O 

1.81 

4-20 

10.86 

25  -31 

30 

1.16 

0.23 

0.23 

0.64 

1.81 

4.06 

10.28 

23.46 

40 

i  .40 

o-33 

0.28 

0.71 

1.90 

4-12 

10.  06 

23-15 

5° 

i  .69 

0.46 

0.38 

0.82 

2  .12 

4-34 

10.35 

23.76 

6o 

2.07 

0.66 

o-55 

I  .11 

2.51 

4.78 

11.03 

24.64 

70 

2.48 

0.91 

0.80 

I  .37 

2.92 

5-43 

11.97 

25.72 

80 

2-95 

1.23 

1.13 

1.83 

3-70 

6.38 

I3-30 

27.23 

9o 

1.65 

1.52 

2.4O 

4.58 

7.82 

I5-52 

29.84 

100 

4-03 

2.23 

2.04 

3-63 

5-82 

9.60 

34-os 

TIN;  IODIDE  (Stannic)  SnI4. 

SOLUBILITY  IN  ORGANIC  SOLVENTS. 

(McDermott,  1911.) 


+°                       Sp.  Gr.  Gms.  SnL,  per 

Sat.  Sol.  100  Gms.  Sat.  Sol. 

Carbon  Tetrachloride          22.4                1.59  5.25 

50                   1.63  12.50 

Chloroform                          28                   1.50  8.21 

Benzene                               20.2               0.95  12.65 


729  TIN  IODIDE 

SOLUBILITY  OF  STANNIC  IODIDE  IN  CARBON  DISULFIDE. 

(Sneider,  1866;  Arctowski,  iSgs-'gG.) 

—  ii4°.S.       —94°.         ^-89°.         —84°.          —58°.         Ord.  temp. 

Cms.  Snl4  per  100  Gms. 
Solution  9.41     10.65    9-68     10.22     16.27     59.2(8) 

100  gms.  methylene  iodide,  CH2I2,  dissolve  22.9  gms.  SnI4  at  10°.     Sp.  Gr.  of 
solution  =  3.481.  (Retgers,  1893-) 

TIN   OXALATE  (Stannous)  Sn(COO)2. 

100  gms.  95  per  cent  formic  acid  dissolve  0.16  gm.  Sn(COO)2  at  19°.   (Aschan,  1913.) 

TIN  TetraPHENYL  (Stannic)  Sn(C6H6)4. 

Freezing-point  data  for  Sn(C6H6)4  +  Si(C6H6)4  are  given  by  Pascal  (1912). 

TIN  SULFATE  (Stannous)  SnSO4. 

100  gms.  H2O  dissolve  18.8  gms.  SnSO4  at  19°  and  18.1  gms.  at  100°.  (Marignac.) 

TOLUENE  C6H6CH3. 

SOLUBILITY  IN  SULFUR. 
Figures  read  from  curve,  synthetic  method  used,  see  Note,  page  16.  (Alexejew,  1886.) 

Gms.  CeHsCHg  per  100  Gms.  Gms.  CpHsCHa  per  100  Gms 

*  °-  '~S  Toluene  *  °*  /~S  Toluene 

Layer.  Layer.  Layer.  Layer. 

ioo  3  73  150              12.5  59 

no  4  71  160              16  53 

120  5  68  170              22  47 

130  7  66  175              25  43 

140  9.5  63  178  crit.  temp.  34 

NitroTOLUENE  o  C6H4.CH3.NO2. 

RECIPROCAL  SOLUBILITY  OF  o  NITROTOLUENE  AND  WATER. 

(Campetti  and  Delgrosso,  1913.) 

The  original  results  were  plotted  and    the  following  figures  read  from  the 
curve. 

Gms.  o  Nitrotoluene  per  ioo  Gms.  Gms.  o  Nitrotoluene  per  ioo  Gms. 

t°.  H2O  Rich  Nitrotoluene  *"•  H2O  Rich          Nitrotoluene' 

Layer.  Rich  Layer.  Layer.  Rich  Layer. 

150              i  98  245  13  81 

175               1.5  96  250  16  78 

200  3  93  255  20  72 

225  6.5  89  260  29  63 

240  10.5  84  263. 5  crit.  t.  43 

ioo  gms.  95  per  cent  formic  acid  dissolve  13.25  gms.  p  CeH4.CH3.NO2  at  20.8°. 

(Aschan,  1913.) 

TrinitroTOLUENE  2,4,6  C6H2.CH3(NO2)3. 

ioo  gms.  H2O  dissolve  0.021  gm.  C6H2.CH3(NO2)3  at  15°  and  0.164  Sm-  at  IOO°' 
ioo  gms.  alcohol  dissolve  1.6  gms.  C6H2CH3(NO2)3  at  22°  and  10  gms.  at  58°. 

(Capisarow,  1915-) 

TOLUENE   SULFONAMINES  o,  m  and  p. 

SOLUBILITY  OF  EACH  IN  WATER  AT  25°.     (Holleman  and  Caland  (1911-) 

Compound.  Gins.  Cgmp'djjer  Liter 

Amine  of  o  Toluene  Sulfonic  Acid  i  .624 

"       "  m  "          "  7.812 

"       "  p        "  "          "  3-156 


TOLUENE  730 

FREEZING-POINT  DATA  (Solubility,  see  footnote,  p.  i),  FOR  MIXTURES  OF  SUB- 
STITUTED TOLUENES  AND  OTHER  COMPOUNDS. 

Mixture.  Authority. 

o  Bromotoluene  +  p  Bromotoluene  (van  der  Laan,  1907.) 

Bromotoluene      +  p  Xylene  fPaterno  and  Ampola,  1897.) 

+  Veratrol 

-f-  Tribenzylamine  "  " 

p  Nitrotoluene    +  «  Ortho  Nitrotoluene  (Holleman,  1914.) 

+  2,  4  Dinitrotoluene  (Giua,  1914, 1915.) 

+  2,  6  (Giua,  1915.) 

+  2,4,6 

+  m  Nitrotoluene  (Holleman  and  van  den  Arend,  1909.) 

+  Urethan  (Mascarelli,  1908,  1909.) 

2,  4  Dinitrotoluene  +  2,  6  Dinitrotoluene  (Giua,  1914, 1915.) 

+  2,  4,  6  Trinitrotoluene  (Giua,  1915.) 

2,  6  +  (Giua,  1914,  1915.) 

a  Trinitrotoluene  -f-  p  Amino  Acetophenone  (Giua,  1916.) 

+  7  Trinitrotoluene  (Giua,  1915.) 

o  Toluene  Sulfochloride  +  p  Toluene  Sulfochloride  (Holleman  and  Caland,  1911.) 
Binary   Mixtures  of  Isomeric  Tribromotoluenes      (Jaeger,  1904.) 

"         Chloronitrotoluenes  (Wjbaut,  I9i3;  Holleman  and  van  den 
Arend,  1909.) 

TOLUIC  ACIDS  (Monomethyl  Benzole  Acids)  CH3.C6H4COOH. 
SOLUBILITY  IN  WATER  AT  25°. 
(Paul,  1894.) 

Add  CH3.C6H4.COOH  per  Liter  Solution. 

Grams.  Millimols. 

Meta  Toluic  Acid  0.9801  7.207 

Ortho  Toluic  Acid  i .  1816  8 . 683 

Para  Toluic  Acid  0.3454  2.540 

One  liter  sat.  solution  in  water  contains  0.42  gram  p  toluic  acid  at  25°.  One  liter 
sat.  solution  in  i  n  aq.  sodium  p  toluate  contains  0.735  gm-  P  toluic  acid  at  25°. 

(Sidgwick,  1910.) 

SOLUBILITY  OF  TOLUIC  ACIDS  (EACH  SEPARATELY)  IN  WATER  AT  VARIOUS 

TEMPERATURES. 

(Sidgwick,  Spurrell  and  Davies,  1915.) 

The  determinations  were  made  by  the  synthetic  method,  see  p.  16;  melting- 
point  of  o  toluic  acid  =  102.4°,  of  m  acid  =  110.5°  and  of  p  acid  =  176.8°.  The 
triple  point  (solid  phase  present)  for  the  o  acid,  is  at  93.5°  and  the  concentration 
of  acid  in  the  two  layers  is  2.5  and  91.2  gms.  respectively  per  100  gms.  sat.  solu- 
tion. The  tr.  pt.  for  the  m  acid  is  at  91.8°  and  concentrations  are  1.6  and  90.5; 
the  tr.-pt.  for  the  p  acid  is  at  142°  and  concentrations,  5  and  74. 


Gms.  per  100  Gms.  Sat.  Sol. 

Gms.  per  100  Gms.  Sat.  Sol. 

*°-            o  Toluic 

m  Toluic 

P  Toluic                   *  • 

o  Toluic 

m  Toluic 

*  Toluic 

Acid. 

Acid. 

Acid. 

Acid. 

Acid. 

Acid. 

80 

2 

•03* 

1.16* 

140 

9- 

25 

5-77 

4.30* 

90 

2 

•42* 

i-54 

.  .  . 

ISO 

13- 

7 

8.40 

9-33 

100 

2 

•97 

1.98 

I 

.16* 

159 

.  i  crit  t. 

.  . 

. 

.  .  . 

00 

no 

3 

•7i 

2.52 

I 

.36* 

1  60 

30 

19.4 

120 

5 

.10 

3-24 

1 

•75* 

161 

.  i  crit.  t. 

00 

130 

6 

•93 

4-30 

2 

.50* 

162 

.  2  crit.  t. 

00 

*  Indicates  that  a  solid  phase  is  present. 

Additional  data  for  the  solubility  of  the  above  compounds  in  water,  determined 
by  the  synthetic  method,  are  given  by  Flaschner  and  Rankin  (1910). 


731  TOLUIC  ACIDS 

RATIO  OF  THE   SOLUBILITIES  OF  TOLUIC  ACIDS   (SEPARATELY   DETERMINED) 
IN  WATER  AND  IN  OLIVE  OIL  AT  25°. 

(Boeseken  and  Waterman,  1911,  1912.) 

The  solubilities  of  each  acid  in  water  and  in  olive  oil  was  separately  determined 
and  the  ratio  considered  to  correspond  to  the  distribution  coefficients  in  each 
case.  The  concentrations  of  the  dissolved  acids  are  not  given. 


n  t.      ,  Solubility  m  Olive  Oil 

Acid.  Ratio  of    0  .  .... — 1—7= • 

Solubility  m  Water 

o  Toluic  Acid  40 . 5 

m      "         "  21  * 


p  39.5 

100  gms.  95%  formic  acid  dissolve  2.99  gms.  o  toluic  acid  at  20.8°.   (Aschan,  1913.) 
Freezing-point  data  for  mixtures  of  o,  m,  p  and  a  toluic  acids  (each  separ- 
ately) and  sulfuric  acid  are  given  by  Kendall  and  Carpenter  (1914).     Results  for 
mixtures  of  o,  m  and  a  acids  and  picric  acid  are  given  by  Kendall  (1916). 

TOLUIDINE  C6H4CH3.NH2. 

SOLUBILITY  IN  WATER. 

(Vaubel,  1895;  Lowenherz,  1898.) 

Gms.  Gms. 

to  CeHiCHa-NHa  Solid  to  CeRkCHjjNHa  Solid 

per  1000  Phase.  per  1000  Phase. 

Gms.  H2O.  Gms.  H2O. 

2O  l6.26  Liquid  ortho  T.  2O-8  7.39  Para  T. 

20  0.15  Ortho  T.  26.7  9.50  " 

20  6.54  ParaTc  31.7  11.42  " 

One  liter  sat.  solution  in  water  contains  15  gms.  o  toluidine  at  25°. 

One  liter  sat.  solution  in  i  n  aq.  o  toluidine  hydrochloride,  contains  30  gms. 
o  toluidine  at  25°.  (Sidgwick,  1910.) 

The  following  results  for  p  toluidine,  differing  considerably  from  the  above, 
are  given  by  Walker  (1890). 

t°.  22°      30°      36.7°   44°      57-5°  69° 

Gms.  p  Toluidine  per  100  Gms. 
Sat.  Sol.  in  Water  19.6     26.9    35.4    44.5     51.4    58.9 

SOLUBILITY  OF  PARA  TOLUIDINE  IN  ETHYL  ALCOHOL. 

(Interpolated  from  original  results  of  Speyers,  1902.) 

Wt.  Mols.  per    Gms.  per  Wt.          Mols.  per      Gms.  per 

t*.         of  i  cc.         100  Mols.     too  Gms.  t°.  of  i  cc.        100  Mols.      100  Gms. 

Solution.        C2H5OH.     C2H6OH.  Solution.      C2H6OH. 


O    0.8885    20.72    48.1         20    0.9265    47-0    IIO.O 

5  0.8982  26.0  60.0  25  0.9360  56.0  132.0 
10  0.9080  32.0  74  -o  30  0.9460  66. o  156.0 
15  0.9180  38.6  90.0 

ioo  gms.  pyridine  dissolve  126  gms,  p  toluidine  at  2O°-25°.  (Dehn,  1917.) 

100  gms.  aq.  50%  pyridine  dissolve  96.1  gms.  p  toluidine  at  2O°-25°.  " 

DISTRIBUTION  OF  PARA  TOLUIDINE  BETWEEN  WATER  AND  CARBON 
TETRACHLORIDE. 

(Vaubel,  1903.) 

Gm^Toluidim  Votaes  of  Solvent,  Cms.  C.H/CH.)NH. » in: 

Used-  H2O  Layer.  CCU  Layer. 

i  200  cc.  H2O+ioo  cc.  CCU  0.1406  0.8594 

i  200  cc.  H20-J-200  cc.  CCU  0.0666  0.9334 


TOLUIDINE  732 

DISTRIBUTION  OF  o,  m  AND  p  TOLUIDINE  BETWEEN  WATER  AND 
BENZENE  AT  25°. 

(Farmer  and  Warth,  1904.) 

Base.  Dist.-Coef.^°nc-in^. 

Cone,  in  H2O 

o  Toluidine  13.4 

m       "  19.1 

P  '4-1 

Aceto  TOLUIDINE  p  CH3C6H4NH.C2H3O. 

SOLUBILITY  IN  MIXTURES  OF  ALCOHOL  AND  WATER  AT  25°. 

(Holleman  and  Antusch,  1894.) 

Vol  ^         Gms'  P61"  SP'  Gr'  Vol  %      Gms-  Per          SP-  Gr° 

AI  YS        ioo  Gms.  of  Ai     u  i       ioo  Gms.  of 

Alcohol.        Solvent>  Solutions.  AlcohoL       Solvent.         Solutions. 

ioo  10.18  0.8074  50  1.92  0.9306 

95  10.79  0.8276  45  1.41  0.9380 

90  10.62  0.8440  40  0.96  0.9460 

85  9.62  0.8576  35  0.66  0.9544 

80  8.43  0.8685  25  0.31  0.9668 

75  7.04  0.8803  20  0.23  0.9725 

70  5-8i  0.8904  15  0.16  0.9780 

65  4.39  0.9021  5  0.13  0.9903 

60  3.59  0.9115  o  0.12  0.9979 

55  2.69  0.9207 

See  remarks  under  a  acetnaphthalide,  p.  13. 

TRIPHENYLAMINE,   TRIPHENYLPHOSPHINE,  etc. 
F.-pt.  data  are  given  by  Pascal  (1912)  for  the  following  mixtures: 

Triphenylamine  +  Triphenylarsine  Triphenylarsine  +  Triphenyl  Stibene 

Triphenylamine  +  Triphenylphosphine   Triphenylarsine  +  Triphenylbismuthine 
Triphenylarsine  -j-  Triphenylphosphine    Triphenylphosphine  -f- 

aand/S  TRITHIOACET ALDEHYDE,  (CH3CHS)3. 

a.  and  0  TRITHIOBENZALDEHYDE,    (C6H6CHS)3. 

SOLUBILITY  OF  EACH  (DETERMINED  SEPARATELY)  IN  SEVERAL  SOLVENTS 

AT  25°. 

(Suyver,  1905.) 

Gms.  per  ioo  Gms.  Solvent. 

Solvent.  , * v 

«(CH3CHS)3.  /3(CH3CHS)3.        « (C6HBCHS)3.       ft  (C6H5CHS)3. 

Ether  15-58  13-67  1.09  0.37 

Ethyl  Alcohol  3 . 86  3.97  o .  20  o .  04 

Methyl  Alcohol  4 . 04  3 . 89  0.17  o .  04 

Acetone  20.96  18.31  2.45  1.12 

Chloroform  57-59  51-22  ii.n  0.20 

Carbon  Bisulfide  25.50  20.75  5-8i  0-22 

Benzene  36.40  26.98  6.08  0.014 

Ethyl  acetate  *7-52  15-48  2.05  0.93 

Data  for  the  solidification  points  of  mixtures  of  a  and  £  trithioacetaldehyde 
are  also  given.  Similar  data  for  mixtures  of  a  and  /?  trithiobenzaldehyde  could 
not  be  determined  on  account  of  decomposition  with  production  of  resins. 

TROPIC  ACID  («  Phenylhydracrylic  Acid)  i  and  /,  C6H6.CH(CH2OH)COOH. 
ioo  gms.  sat.  solution  in  H2O  contain  1.975  Sms-  °l tne  *  acjd  at  20°.  )  (Schlossberg. 
ioo  gms.  sat.  solution  in  HaO  contain  2.408  gms.  of  the  I  acid  at  20°.  f  1900.) 


733  TURPENTINE 

TURPENTINE   OIL 

SOLUBILITY  IN  ETHYL  ALCOHOL. 

(Vezes  and  Mouline,  1904,  1905-06.) 

Spirit  of  turpentine  and  absolute  alcohol  are  miscible  in  all  proportions  and  the 
mixture  may  be  cooled  to  a  very  low  temperature  without  ceasing  to  be  homo- 
geneous. In  the  case  of  alcohol  containing  a  small  amount  of  water,  the  mixture, 
which  is  uniform  at  ordinary  temperature,  separates  into  two  layers  when  cooled. 
The  following  data  were  obtained  for  mixtures  of  98  vol.  %  alcohol  ( =  0.968  gm. 
C2HsOH  per  I  gm.  aq.  alcohol)  and  spirits  of  turpentine  and  for  mixtures  of  95 
vol.  %  alcohol  ( =  0.924  gm.  C2H5OH  per  I  gm.  aq.  alcohol)  and  spirits  of  tur- 
pentine. 

Results  for  98  Vol.  %  Alcohol.  Results  for  95  Vol.  %  Alcohol. 


Cms.'  98  Vol.       ,o    .         Cms.  98  Vol.        ,  0    .    *  Cms.  95  Vol.        f  „  _f        Cms. 


.  95 

» 


Mixture. 

Mixture. 

Mixture. 

uon. 

Mixture. 

-35-6 

2.7 

—  20.9 

32-9 

+  20.7 

2.4 

29.6 

48.3 

-23 

4.8 

—  26.1 

42.6 

42.2 

3-4 

23-9 

52.8 

—  2O-9 

9-5 

-30 

48.2 

"  53 

7.2 

16-3 

61.4 

-i8.i 

13.2 

-45-3 

58 

IO.2 

-15-5 

76.6 

-17.8 

16 

-79.2 

71.9 

44 

20.3 

-24 

81.1 

-18.8 

24.4 

37-2 

30.6 

-63 

87.1 

Data  in  regard  to  the  sample  of  spirits  of  turpentine  which  was  used,  are  not 
given. 


URANYL   Potassium  BUTYRATE 

The  double  salt  is  decomposed  by  water  at  ordinary  temperatures  and  the  solu- 
tion gets  richer  in  uranyl  butyrate.  The  solubility  at  29.4°  in  water  containing 
KC4H7O2  is  2.10  gms.  UCMC^C^)  +  0.38  gm.  KC^H-jOz  per  100  gms.  solution. 
The  atomic  relation  being  1  :  0.64.  (Rimbach,  1904.) 


URANYL  Ammonium  CARBONATE 

SOLUBILITY  IN  WATER. 

(Giolitti  and  Vecchiarelli,  1905.) 

A  large  excess  of  the  double  carbonate  was  agitated  with  water  at  constant 
temperature  and  the  clear  saturated  solutions  analyzed. 

Gms.  per  100  Gms.  Sat.  Sol.  Mol.  Ratio. 

U!  CO2.  NH3.  /U       I COT      :       NH3.  " 

18.6  2.71  1.54  0.795  I  3-o8  4.10 

36.5  3.09  2.29  1.188  i  4.01  5.35 

48.3  3.03  2.71  1.35  i  4-95  6.35 

62  ...  3-*7  i -62  ...        ... 

87-3  3-95  3-96  2.027  i  5.42  7.15 

Theoretical  molecular  ratio  for  UO2CO3.2(NH4)2CO3  =  1:3:4. 

Thus  at  the  lower  temperature,  the  composition  of  the  dissolved  salt  is  very 
near  the  ratio  corresponding  to  the  formula. 

The  author  calculates  that  6.04  gms.  of  UO-jCOs^CNH^COs  are  contained  in 
loo  gms.  of  the  sat.  solution  at  18.6°  (a  recalculation  from  the  U  value,  2.71,  in- 
dicates that  this  figure  should  be  5.26  gms.). 

URANYL   CHLORIDE  UO2C12.3H2O. 

IOO  gms.  H2O  dissolve  320  gms.  UO2C12  at  18°.  (Mylius  and  Dietz,  1901.) 


URANYL   CHLORIDES 


734 


SOLUBILITY  OF  URANYL  AMMONIUM  CHLORIDE,  U.  TETRA  METHYL  AMMONIUM 
CHLORIDE,  U.  TETRA  ETHYL  AMMONIUM  CHLORIDE,  U.  CAESIUM  CHLORIDE,  U. 
RUBIDIUM  CHLORIDE,  AND  U.  POTASSIUM  CHLORIDE  IN  WATER. 

(Rimbach,  1904.) 


Formula^  of  Double      ^.o         Gms.  per  100  Gms.  Sat.  Sol. 

Atomic  Relation  in  Sol. 

Solid  Phase. 

U02C12.2NH4C1.2H2O  15        40.67UO2+3.5iNH4+i9.i5Cl 

IU02:z.59NH4:3.590  ^^Sgg 

UO2Clj.2N(CH3)4O      29.8     19.85   "   +io.44O2    =41.24* 

iUO2:  4-020 

Double  salt 

80.7     20.23    "    +io.52O2    =41.91* 

iU02:  3.980 

* 

UO2O2.2N(C2H5)4O     27.1     15-02 

+  7-8iO2    =37-i5t 

iU02:  3-97C1 

" 

80.7     15.12 

+  7.78O2    =37-23t 

iU02:  3-940 

.  (i 

UO2O2.2CsO               29.75  22.11 
UO2O2.2RbC1.2H2O     24.8    27.18 

+22.5  Cs    =56.04$ 
+16.6  Rb    +i3.8O§ 

iUO2:  2.o7Cs 
iU02:i.96Rb:3.9od 

« 

80.3    30.66 

+ig.iRb      +I5.8OH 

iU02:i.98Rb:  3-95C1 

u 

U0202.2KC1.2H20        0.8    38.57 
14-9    33-71 

+13-590     +  3-86K 

iUO2:  2.690  :  o.69K 
iUO2:  3.o6O  :i.o6K 

The  double  salt 

I7-S    37-36 

+i4.'soCl     +  5-27K 

iU02:  2.960  :  o.96K 

is  decomposed 

25        35.01 

+15.260     +  ...  K 

lUCy.  3-330  :  I.33K   • 

by     water     at 

4I-S    35-27 

+15.920     +  7-39K 

iU02:  3-440  :  I.44K 

temperatures 

So        34-18 

+16.560     +  .  .  .  K 

iUO2:3.7id  :i.7iK 

below  60°. 

60        34-19 

+17.250     +  9.I4K 

iU02:  3-850  :  i.8sK 

71.5     33.55 

+I7.44C1     +  Q.28K 

iU02:  3-96C1  :  I.96K 

Double  salt 

78.5     35-26        +18.240     +  9-95K 

iU02:  3-950  :  I.95K 

UO2C12.2N(CH3)4C1.               f  UO2C12.N(C2H6)4O.               *  UO2O2.2CsCl. 
§  =57-9  gms.  UO2O2.2RbO2.                      ||   =65.8  gms.  UO2O2.2RbO2. 

URANYL   Sodium   CHROMATE  2(UO2)CrO4.Na2CrC>4.ioH2O. 

100  gms.  sat.  aqueous  solution  contain  52.52  gms.  2(UO2)CrO4Na2CrC>4  at  20°. 

(Rimbach,  1904.) 


URANYL  IODATE   UO2(IO3)2. 


SOLUBILITY  OF  THE  DIFFERENT  CRYSTALLINE  FORMS  IN  WATER  AT  18°. 

(Artmann,  1912-13.) 

Gms.  UO2(IO3)2 
per  loo  Gms.  H2O. 

o . 1049 


U02(I03)2.H20 

« 

UO2(IO3)2.2H2O 


Appearance  of  Crystals. 

Type  I   warty,  later  prismatic  needles 


Type  II  pyramids,  sphenoids 


0.1214 
o . 2044 


URANYL  NITRATE   UO2(NO3)2.6H2O. 


SOLUBILITY  IN  WATER. 

(Wasilieff,  1910.) 


Gms.  UO2(NO3)i 
t°.           per  100  Gms.                  Solid  Phase. 

Gms.  UO2(NO3)2 
t°.         per  100  Gms. 

Sat.  Sol. 

Sat.  Sol. 

-   1.6 

IO  .  83       Ice 

—    2.2 

48.77   . 

—    2.1 

12.24         " 

0 

49.46 

~    2.9 

17.19         " 

5-5 

50-55 

-    4.4 

23.52 

12.3 

52.88 

-  6 

26  .  20 

21.  1 

55.98 

-  7.9 

32.53         " 

25.6 

57.17 

—  II  .2 

37.09         « 

36.7 

6l.27 

-18.1 

43.12         "  +U01(N03)2.6H20 

45-2 

65.12 

—  12.  1 

45-53              U02(N03)2.6H20 

51-8 

67.76 

Solid  Phase. 
UO2(NOS)2.6H20 


loo  gms.  abs.  acetone  dissolve  1 .5  gms.  UO2(NO3)2.6H2O  at  12°.    (de  Coninck,  1900.) 
100  gms.  85%  alcohol  dissolve  3.3  gms.  UO2(NO3)2.6H2O  at  12°. 
Data  for  the  densities  of  uranyl  nitrate  solutions  in  water  and  other  solvents 
are  given  byde  Coninck  (1900). 


735 


URANYL  NITRATE 


SOLUBILITY  OF  URANYL  NITRATE  IN  ETHER. 

(Lebeau,  1911.) 

When  a  large  excess  of  uranyl  nitrate  is  shaken  with  ether  at  7°,  two  liquid 
layers  are  formed.  The  ethereal  layer  contains  59  gms.  UO2(NO3)2  per  100  gms. 
of  solution  and  the  aqueous  layer  contains  62.5  gms.  per  100  gms.  of  solution.  An 
elevation  of  temperature  was  noted  when  ether  and  UO2(NO3)2.6H2O  were  mixed 
at  room  temperature,  therefore,  indicating  that  solution  is  accompanied  by  com- 
bination and  elimination  of  the  water  of  the  salt. 

URANYL  DOUBLE  NITRATES. 

SOLUBILITY  OF  URANYL  AMMONIUM  NITRATE  +  URANYL  NITRATE;  U.  CAESIUM 
NITRATE  +  CAESIUM  NITRATE;  U.  POTASSIUM  NITRATE  +  POTASSIUM  NITRATE 
AND  U.  RUBIDIUM  NITRATE  +  RUBIDIUM  NITRATE  IN  WATER. 

(Rimbach,  1904.) 


Formulci  of  Stilt 

Gms.  per  100  Gms.  Sat 

.  Solution. 

Atomic  Relation 

' 

'U02. 

Total  Salt. 

in  Solution. 

UO2(N03)2.NH4NO3 

0.5 

29.71  +  2.92  NH4 

=    .  ..     i  U 

?2 

i.47NH4:3.47NO3 

« 

24.9 

36.46  +  3.54    " 

=  68.95 

1.46    "    13.46  " 

(i 

59 

44.37  +  2.90    ' 

0.98     "    :  2.98  " 

U 

80.7 

44.95  +  2.98    ' 

=  78.95 

i         w  :  t 

UO2(NO3)2.CsNO3 

16 

31.  39  +  6.  59  Cs 

=  55-4 

0.44  Cs 

UO2(NO3)2.KNO3 

o-5 

2.37  NO3:o.37K 

13 

33.40  +  2.72    ' 

=    .  .  . 

2-57  '   '    :o.57' 

25 

37.07+4.01    ' 

=  64.82 

i.  60    "    =0.76' 

45 

42.18  +  5.16    ' 

=    ... 

2.84    "    :o.84' 

59 

41.65  +  6.03    ' 

= 

3           "    :i       ' 

80.6 

43.71  +  6.38    ' 

=  80.  i 

3.01      '    n.oi1 

U02.(N03)2.RbN03 

25 

35.41+4.65  Rbf 

=  59.60 

i.  40    "    :o.45Rb 

«« 

80 

34.66  +  11.01  " 

=  69.49 

3          "    n.oi    " 

*  +  23-SN03.  t  +  I9-74NO,. 

URANYL   OXALATE  UO2.C2O4.3H2O. 

100  gms.  H2O  dissolve  0.7401  gm.  UO2C2O4.3H2O  at  25°. 


(Dittrich,  1899.) 


EQUILIBRIUM  IN  THE  SYSTEM  URANYL  OXALATE,  AMMONIUM  OXALATE 

AND  WATER. 

(Colani,  1917.) 

Results  at  15°.  Results  at  50°. 


Gms.  per  100  Gms. 
Sat.  Solution. 


Solid  Phase. 


Gms.  per  100  Gms. 
Sat.  Solution. 


Solid  Phase. 


0.47        o          U02C204.3H20  i 

7.19  2.14  "  +(NH4)2(U02)2(Q!04)3.3H20     5-II 

8.78  2.99  (NH4)2(U02)(C2O4)2.2H2O  +  "       19.89 

Q.66  6.43  "  +(NH4)2C204.H20                   23.82 

O  3-^9  (NH4)2C2O4.H2O                     O 

Two  determinations  at  75°  are  also  given. 

EQUILIBRIUM  IN  THE  SYSTEM  URANYL  OXALATE,  POTASSIUM  OXALATE 

AND  WATER. 

(Colani, 


O  U02.C204.3H20 

1-36  "  +(NH4)2(U02)2(C204), 

8.52  (NH4)2(U02)(C204)2+  " 

15.90  "  +(NH4)2C204.H20 
9-36 


Results  at  15°. 


Results  at  50°. 


Gms.  per  100  Gms. 
Sat.  Solution. 

Solid  Phase. 

U02C204.3H20 

"  +K2(U02)2(C204)3.4H20 

"  +Ke(U02)2(C204)B.ioH20 
K2C2O4.H2O+ 
K2C20«.H20 

Gms.  per  100  Gms. 
Sat.  Solution. 

Solid  Phase. 

"  +K,(U02)2(C204)8.4H20 
K2(U02)(C204)2+       " 
"  +K,(U02)2(C204)6.ioH2O 
K2C204.H20+ 

U02C204. 
0.47 
1-34 
3.89 
3.76 
0.10 
0 

K2c2o4: 

0 

0.42 

1.83 
1.85 

24.30 
24.09 

U02P204. 

I 

3-45 
9.82 

9-59 

I.  22 
0 

K2Q04. 
0 
I.  II 
4.83 
5-6l 
32.65 
32.75 

URANYL   OXALATE 


736 


SOLUBILITY  OF  URANYL  OXALATE  IN  AQUEOUS  SODIUM  OXALATE  AT  25°. 

(Dittrich,  1899.) 


Cms.  UO2.C2O4.3H2O 
per  100  cc.  Sat. 
Solution. 
2.0125 
0.9867 
0.6059 


Gms.  Na2C2O4 

per  lop  cc. 

Solution. 

0.6706 

0-3353 
0.2235 

URANYL  Ammonium  PROPIONATE 

URANYL  Potassium  PROPIONATE  UO2(C3H5O2)2.KC3H6O2. 

100  gms.  aq.  solution  contain  16.48  gms.  2UO2(C3H5O2)2.NH4C3H6O2  at  29.8°. 
100  gms.  aq.  solution  contain  2.362  gms.  UO^CsHsO^  +  0.82  grn.  KCsH5O2 
at  29.4°,  atomic  relation,  i:  1.29.  (Rimbach,  1904.) 

URANYL  SULFATE  UO2SO4.3H2O. 

SOLUBILITY  IN  SEVERAL  SOLVENTS. 

(de  Coninck,  1901,  1903.) 

Gms.  UO2SO4.- 
t°.         sH2O  per  zoo 
Gms.  Solvent. 
13.2  18.9 

15-5  20.5 

12.3 
2.6 
30 


Solvent 


Water 

Water 

16.2%  Alcohol     10 

85%  Alcohol        1 6 

Cone.  HC1  13 


Solvent. 


Cone.  HBr  (J=i.2i) 
Cone.  HN03 
Cone.  H2SO4  (d=  1.138) 
i  Vol.  HCl+i  Vol.  HNO3 
Selenic  Acid  (d=  1.4) 


Gms.  UO2S04.- 

t°.      3H2O  per  100 

Gms.  Solvent. 

16.8 


12 
12 
13 

16 
IS 


9.1 

24-3 
18 

27 


URANYL   Potassium   SULFATE  U02SO4.K2SO4.2H2O. 

100  gms.  sat.  aq.  solution  contain  10.41  gms.  UO2SO4.K2SO4  at  25°  and  23.13 
gms.  at  70.5°.  (Rimbach,  1904.) 

SOLUBILITY  OF  UO2SO4.2K2SO4.2H2O  +  UO2SO4.K2SO.2H2O  IN  WATER. 

Gms.  per  100  Gms.  Solution.  Atomic  Relation  in  Sol.         Mol.  %  in  Solid  Phase. 


UO, 
14  0.85 

50          6 . 70 
80        14. 29 


K. 

4.19 
8.15 
8-54 


S04. 

5-71 
12.37 

15-53 


U02 

.        K. 

S04. 

I 

35-75 

18.88 

I 

5.20 

8.40 

I 

4-i3 

3.06 

Mono  Salt.  Di  Salt. 

29  71 

76  24 

12  88 


URANIUM   SULFATE  (ous)  U(S04)2. 

i  SOLUBILITY  IN  WATER. 

(Giolitti  and  Bucci,  1905.) 

Gms.  U(SO4)2 
Solid  Phase.  t°.  per  100  Gms. 

Sat.  Sol. 

93  63 . 2 

24  9.8 

37  8.3 

48.2       8.1(7.8) 

63  7.3 


18 

25.6 

37 

48.2 

62 


Gms.  U(SO4)2 

per  loo  Gms. 

Sat.  Sol. 

10. 17 

I3-32 
19.98 
28.72 
36.8 


Solid  Phase. 
U(SO4)2.8H2O 


The  determinations  were  made  with  difficulty  on  account  of  the  considerable  tend- 
ency towards  formation  of  basic  sulfate  and  simultaneous  clouding  of  the  solution. 

APPROXIMATE  SOLUBILITY  OF  URANIUM  SULFATE,  IN  AQUEOUS  SOLUTIONS. 

(de  Coninck,  1903.) 


Solvent. 

Water  n 
Dilute  HC1  (1:4)          9 

Dilute  HN03  (1:4)  10.5 


Gms. 

U(S04)2.4H2O 

per  100  Gms. 

Solvent. 

23.2 

17.2 

18.2 


Solvent. 


Gms. 

U(S04)2.4H20 

per  100  Gms. 

Solvent. 


Dilute  Selenic  Acid  (1:4)    11.4      21.7 
Dilute  H2SO4  (1:4)  10         15.6 

Dilute  Alcohol  (i:  4)          11.3      12.3 


737 


UREA 


UREA  CO(NH2)2. 

SOLUBILITY  IN  WATER  AND  IN  ALCOHOLS. 

(Campetti,  1902;  Speyers,  1902.) 

NOTE.  —  Speyer's  original  results  are  in  terms  of  Mols.  CO(NH2)2  per  100  mols. 
H2O  at  irregular  temperatures. 

In  Water.  In  Methyl  Alcohol.  In  Ethyl  Alcohol. 


t°. 

Wt.  of  i  cc. 
Solution. 

Cms.  CO(NH2)2  per         Wt.  of  i  cc. 
100  Cms.  H2O.                   Solution. 

Gms. 
CO(NH2)2 
per  100  Gms. 

Gms. 
Wt.  of  ice.    CO(NH2)a 
Solution,    per  100  Gms 

CH3OH. 

(J2H5OH. 

o 

I  .121 

55-9 

0.861 

13.8 

0.8213 

2-5 

IO 

I-I34 

66.0 

8S!o(C) 

0.863 

16.0 

0.8l4 

3-5 

20 

1.146 

79.0 

io8.2(C) 

0.869 

20.0 

0.809 

5-o 

3° 

I  .156 

93-o 

0.876 

24.0 

0.8o6 

6-5 

40 

I  .165 

106.0 

.  .  . 

0.890 

30.0 

0-804 

8-5 

5° 

I-I73 

I2O-O 

0.908 

37-o 

0.803 

10.5 

60 

I.lSo 

132.0 

0.928 

47.0 

13.0 

70 

I.lSy 

145.0 

17-5 

100  gins.  abs.  methyl  alcohol  dissolve  21.8  gms.  CO(NH2)2  at  19.5°. 
loogms.abs.  ethyl  alcohol  dissolve  5.06  gms.  CO(NH2)2at  19.5°.       (de  Bmyn,  1903.) 


SOLUBILITY  OF  UREA  IN  ALCOHOLS. 

(Timofeiew,  1894.) 

Gms. 

100  Gms. 
olvent. 

Isopropyl  Alcohol 


Alcohol. 

t°. 

per  zoo  Gn 
Solvent. 

Methyl  Alcohol 

—  12 

II 

tt 

O 

14.2 

" 

19 

20.9 

M 

40 

36.4 

" 

62 

66.6 

" 

71 

107.4 

Ethyl  Alcohol 

-  9 

2.69 

u 

o 

3-26 

" 

18 

5 

" 

41 

9-45 

" 

60 

16.3 

tt 

81 

30.8 

Propyl  Alcohol 

0 

1.65 

tt 

20 

2.56 

tt 

40 

5-12 

" 

60 

7.72 

tt 

80 

12.28 

" 

98 

18.06 

Alcohol. 


Isobutyl  Alcohol 


Isoamyl  Alcohol 
tt 

it 

(C 

It 

Capryl  Alcohol 

a 

Ally  Alcohol 
SOLUBILITY  OF  UREA  IN  ETHYL  ACETATE  CONTAINING  SMALL  AMOUNTS 


Gms.  CCXNHj) 

t°. 

per  100  Gms. 

Solvent. 

19 

4           5.76 

20 

6.17 

Si 

23.46 

0 

1.  01 

19 

1.65 

41 

3-12 

60 

4.40 

80 

6-34 

98 

10 

20 

1.18 

60 

3-41 

80 

4.88 

83 

5-24 

6.15 

10 

4           0.56 

OS 

2 

19 

4          9-37 

OF  WATER 

AT  25°. 

(Lewis  and  Burrows,  1912.) 

Gms.  H2O  per  100 

Gms.  Urea 

Gms.  H2O  per 

Gms.  Urea 

Gms.  Solvent. 
(Ethyl  Acetate  +H2O). 

per  TOO  Gms. 
Sat.  Sol. 

100  Gms.  Solvent. 
(Ethyl  Acetate  +HjO). 

per  too  Gms. 
Sat.  Sol. 

0 

O.oSo 

1.677 

0.308 

0.652 

0.148 

2.0O6 

0.328* 

I.  112 

0.198 

2.138 

0.342 

1.638 

0.296 

3-234 

o-343t 

A  second  liquid  phase  was  suspected  here. 


t  A  second  liquid  phase  could  be  distinguished. 


UREA 


738 


SOLUBILITY  OF  UREA  IN  ETHYL  ETHER. 

(Gortner,  1914.) 

When  0.3255  gm.  urea  was  extracted  in  a  Soxhlet  apparatus  with  anhydrous 
ether  for  48  hours,  the  extract  was  found  to  contain  0.072  gm.  urea.  An  approxi- 
mate estimate,  based  on  the  volume  of  liquid  and  the  number  of  siphonings  per 
hour  indicates  a  solubility  of  0.0004  gm.  urea  per  100  cc.  of  ether. 

100  gms.  glycerol  dissolve  about  50  gms.  urea  at  15°. 

100  gms.  pyridine  dissolve  0.96  gm.  urea  at  20-25°.  (Dehn,  1917.) 

100  gms.  aq.  50%  pyridine  dissolve  21.53  gms.  urea  at  20-25°. 


Diphenyl  UREA. 

100  gms.  H2O  dissolve  0.015  g"1'  diphenyl  urea  (sym  or  uns.?)  at  20-25°. 

"        pyridine  dissolve  6.85  gms.  diphenyl  urea  (sym  or  uns.?)  at  20-25°. 

"        aq.  50%  pyridine  dissolve  5.3  gms.  diphenyl  urea  (sym  or  uns.?)  at 
20-25°.  (Dehn,  1917.) 


ThioUREA  NH2.CS.NH2. 

loo  gms.  H2O  dissolve  9.1  gms.  thiourea  at  20-25°. 

"        pyridine  dissolve  12.5  gms.  thiourea  at  20-25°. 

"        aq.  50%  pyridine  dissolve  41.2  gms.  thiourea  at  20-25' 


(Dehn,  1917.) 


Allyl  ThioUREA   (Thiosinamine)  NH2.CS.NH.C3H6. 

100  cc.  H2O  dissolve  about  5.9  gms.  NH2.CS.NH.C3H6  at  15-20°. 

100  cc.  90%  alcohol  dissolve  about  50  gms.  NH2.CS.NH.C3H6  at  15-20°. 

(Squire  and  Caines,  1905.) 


Phenyl  ThioUREA  (Phenyl  thiocarbamide)  CS.NH2.NHC6H6. 
SOLUBILITY  IN  WATER. 

(Rothmund,  1900;  Biltz,  1903;  Hollman  and  Antusch,  1894;  Bogdan,  1902-03.) 

One  liter  aq.  solution  contains  2.12  gms.  CS(NH2).NHC6H6  at  20°  (B.),  (R.) 
and  2.4  gms.  at  25°.  (H.  and  A.).     Bogdan  gives  2.547  gms.  at  25°. 


SOLUBILITY  OF  PHENYL  THIOUREA  AT  25°  IN  AQUEOUS  SOLUTIONS  OF. 


Potassium  Nitrate. 

Sodium  Nitrate. 

(Bogdan,  1902-03.) 

(Bogdan,  1902-03.) 

Gms.  Mols. 
KNOa  per 
jooo  Gms. 
HzO. 

Gms.  per 
1000  Gms^.  H2O. 

Gms.  Mols. 
NaNO3  per 
jooo  Gms. 
H20. 

Gms.  per 
looo  Gms.  H2O. 

KNO,. 

CS(NH2) 
.NHCftHg. 

NaNO3. 

CS(NH2) 
NHQ»H5. 

1.045 
0.5123 
O.2O26 
0.1007 

105-7 
5I-84 
20.50 
IO.I9 

2-38 
2.48 

2-54 
2-56 

1.024 
0.5065 
0.2031 
0-0986 

87.14 

43.10 

17.28 

8-39 

2.26 
2  .46 

2.51 
2-53 

0.0503 
0-0333 

5-09 
3-36 

2-55 
2-55 

0-0540 
0-0335 

4-59 
2.84 

2-54 
2-54 

739 


Phenyl  ThioUREA 


SOLUBILITY  OF  PHENYL  THIOUREA  IN  AQUEOUS  SALT  SOLUTIONS  AT  20°. 

(Biltz,  1903;  Rothmund,  1900.) 

Millimols  and  the  Equivalent  Cms.  CSCNH^NHCjHs  Dissolved  per  Liter  of 
Aqueous  Salt  Solution  of  Concentration: 


0.125  Normal 

0.25  Normal 

0.5  Normal. 

i  Normal 

Millimols. 

Gms. 

Millimols. 

Gms. 

Millimols. 

Gms. 

Millimols. 

Gms. 

IAIO, 

12 

•95 

1.97 

12.82 

I  .96 

12.03 

I 

•83 

10 

.69 

1.61 

NH4N03 

14 

2.15 

14.4 

2.21 

14-53 

2 

.22 

14 

.91 

2.27 

i(NH4)2S04 

J3 

•51 

2  -05 

12.84 

1.96 

11.78 

I 

•79 

9 

.98 

1.52 

iBaC!2 

13 

.12 

1-99 

12  .92 

i-97 

12.22 

I 

.86 

10 

.44 

1  -59 

iBa(N03)2 

13 

.98 

2.13 

13.98 

2.13 

13.90 

2 

.12 

CsNO3 

14 

•53 

2  .21 

14.90 

2.27 

15.23 

2 

•33 

. 

.. 

LiNO3 

13 

.96 

2.13 

13.96 

2.13 

13-93 

2 

.12 

13 

•73 

2.10 

£MgSO4 

*3 

.40 

2.04 

12.78 

I  .95 

n-54 

I 

•75 

9 

•43 

i-43 

KC2H3O2 

.40 

2  .04 

12-95 

1-97 

12.14 

I 

•85 

10 

•74 

1.62 

KBr 

13 

•5° 

2  .05 

13-35 

2  .04 

12.80 

X 

•95 

ii 

.76 

1.79 

KC103 

I3 

.86 

2.  II 

13.60 

2  .06 

13.12 

I 

•99 

KC1 

*3 

.40 

2  .04 

12.73 

1.94 

12.19 

X 

•85 

10 

•54 

i.  60 

Kl 

14 

.12 

2.15 

14.48 

2  .21 

I4-31 

2 

.18 

14 

.60 

2.23 

KNO3 

13 

.89 

2.12 

I3-85 

2  .11 

I3-52 

2 

•05 

12 

.82 

i  .96 

KN02 

14 

•52 

2.21 

14.65 

2.23 

13.80 

2 

.11 

12 

.51 

1.92 

JK2SO4 

13 

•25 

2  -03 

12.49 

I.9I 

ii  .11 

I 

.69 

8 

•73 

i-33 

RbN03 

14 

.22 

2.l6 

14.44 

2.19 

14-39 

2 

.18 

14 

.22 

2.17 

iNa2C03 

13 

.29 

2  .04 

12.52 

I.9I 

ii  .05 

I 

.68 

8 

•58 

1.32 

NaClO3 

13 

•75 

2  .09 

I3-65 

2.08 

13.07 

I 

.98 

12 

.21 

1.86 

NaClO4 

14 

2.15 

14.05 

2.14 

I3-58 

2 

.06 

12 

•56 

1.92 

NaCl 

.28 

2  .02 

12.83 

i-95 

ii  .90 

X 

.81 

10 

.02 

1.52 

Nal 

13 

.98 

2.13 

14.07 

2.14 

14.29 

2 

.18 

13 

.96 

2.13 

NaNO3 

•94 

2.12 

13-77 

2.10 

13  .32 

2 

.04 

12 

•57 

1.92 

NaNO2 

14 

•34 

2.18 

13.82 

2  .11 

13.06 

I 

.98 

II 

•52 

i  .75 

JNa2S04 

13 

2  .00 

12.35 

1.87 

10.85 

I 

•63 

8 

•30 

1.27 

SOLUBILITY  OF  PHENYL  THIOUREA  IN  ETHYL  ALCOHOL  SOLUTIONS  OF 
SEVERAL  SALTS  AT  28°. 

(Thorin,  1915.) 


Normality 

Mols. 

Normality 

Mols. 

Salt. 

of  Salt 
in 

NHj.CS.NHQHg 
per  100  Gms. 

Salt. 

of  Salt 
in 

NHs.CS.NH.QHj 
per  too  Gms. 

QHBOH. 

Sat.  Sol. 

QHBOH. 

Sat.  Sol. 

None 

(pure  C2H5OH) 

o  .  2065 

Nal 

0.043 

O.2I02 

LiCl 

0.168 

0.2274 

n 

0.086 

0.2148 

tt 

o-337 

0.2360 

t( 

0.172 

0.2198 

(C 

0.673 

o  .  2440 

n 

0-343 

0.2271 

tc 

1.346 

0.2494 

it 

0.685 

0.2359 

CaCl- 

0.061 

0.2IOI 

NaBr 

0.022 

o  .  2098 

ft 

0.122 

0.2135 

tt 

0.043 

0.2194 

tt 

0.244 

0.2194 

tt 

0.086 

0.2165 

tt 

0.487 

0.2279 

tt 

O.I72 

0.2257 

u 

0.975 

0.2372 

» 

Phenyl  ThioUREA 


740 


SOLUBILITY  OF  PHENYL  THIOUREA  IN  MIXTURES  OF  ETHYL  ALCOHOL 
AND  WATER  AT  25°. 

(Holleman  and  Antusch,  1894.) 


Cms. 

Vol.         CS(NH2)          Sp.  Gr. 
per  cent      NHCsHs  of 

Alcohol,  per  100  Cms.    Solutions. 
Solvent. 


Cms. 

Vol.         CS(NH2)         Sp.Gr. 
per  cent       NHC«H5  of 

Alcohol,  per  100  Cms.     Solutions. 
Solvent. 


100 

3-59 

95 

4-44 

0.8200 

90 

4.69 

0.8389 

85 

4-99 

0.8544 

80 

4-70 

0.8679 

75 

4-45 

0.8810 

70 

3-92 

0.8915 

65 

3-40 

0.9018 

60 

2.80 

0.9128 

50 

1.87 

0.9317 

40 

i  -13 

o  .  9486 

25 

0.56 

0.9679 

IS 

0.38 

0.9788 

o 

0.24 

0.9979 

See  remarks  under  a.  acetnaphthalide,  p.  13. 

SOLUBILITY  OF  PHENYL  THIOUREA  IN  AQUEOUS  SOLUTIONS  OF  PROPYL 
AND  OF  ETHYL  ALCOHOL  AT  25°. 

(Bogdan,  1902-03.) 

In  Aq.  Propyl  Alcohol.  In  Aq.  Ethyl  Alcohol. 


G.  Mols. 

Gms.  per  loop  Gms.H2O 

G.  Mols. 

Gms.  per  1000  Gms.  H2O 

CjHrOH  per 
1000  GDIS. 
H2O. 

C3H7OH. 

CS(NH2)' 
NHC6H6. 

C2HfiOH  per 
1000  Gms. 
H20. 

C2H5OH. 

CS(NH2) 

1-035 

62  .IO 

3.587 

I  .IOIO 

49.60 

3-*93 

0.5448 

32.688 

3.124 

0-5355 

24.12 

2.931 

0.1059 

6-354 

2.643 

o  .  1094 

4-932 

2  .629 

0.05526 

3-3l6 

2-599 

0.05018 

2  .26 

2.589 

0-04854 

2  .912 

2.586 

0.03271 

1-473 

2-577 

In  Propyl  Alcohol 

at  o°. 

i  .000 

60.06 

I  .21 

o.ioo 

6.01 

1.047 

SOLUBILITY  OF  PHENYL  THIOUREA  IN  AQUEOUS  SOLUTIONS  OF  ACETONE, 
MANNITOL,  CANE  SUGAR,  DEXTROSE,  AND  UREA. 

(Bogdan,  1902-03.) 


Aqueous 
Non  Electro- 

Gms. per  1000 
to                       H?0 

Gms. 

Aqueous 
Non  Electro- 

to 

Gms.  per  1000  Gms. 
H20. 

lyte. 

Non  Elec- 
trolyte. 

SSH<NC§fl 

lyte. 

• 

Non  Elec- 
trolyte. 

CS(NH2) 
NHC6H6. 

(CH3)2CO 

25 

7 

.478 

2 

.667 

C6H1206 

25 

180 

.40 

3 

.042 

tt 

tt 

2 

.513 

2 

•579 

a 

tt 

90 

.46 

2 

•83 

a 

u 

I 

.908 

2 

•573 

11 

11 

29 

.29 

2 

.69 

C.H8(OH), 

It 

182 

.11 

3 

.04 

" 

11 

18 

.01 

2 

•654 

tt 

(I 

91 

•05 

2 

.78 

" 

" 

9 

•554 

a 

.603 

C^H^On 

25 

338 

.6 

3 

•457 

CO(NH2)2 

ft 

63 

.08 

3 

.306 

it 

M 

170.4 

3 

.015 

tt 

11 

29 

•93 

2 

.892 

tt 

tt 

34-36 

2 

•634 

(I 

It 

6.132 

2 

.6l8 

tt 

tt 

18 

.28 

2 

•596 

tt 

tl 

4 

.942 

2 

-605 

»t 

tt 

10 

.09 

'  2 

•572 

ft 

It 

2 

.009 

2 

•572 

* 

0 

342 

.18 

I 

.420 

tt 

0 

60 

.11 

1 

.310 

U 

tt 

34 

.22 

I 

.044 

tt 

tt 

6 

.01 

I 

.048 

741 


UREIDE 


UREIDE   OF   GLUCOSE   CH2OH.(CHOH)4.CH  :  N.CO.NH2. 

100  gms.  absolute  ethyl  alcohol  dissolve  0.04  gm.  ureide  of  glucose  at  25°. 
85,6%  .      "  "       0.73    " 


methyl  alcohol 


0.22 


(Schoorl,  1903.-) 


URETHAN  (Ethyl  Carbamate)  NH2.CO2.C2H6.     (See  also  p.  296.) 
SOLUBILITY  OF  URETHAN  IN  SEVERAL  SOLVENTS. 

(Speyers,  1902.) 

Interpolated  and  calculated  from  the  original  results  which  are  given  in  terms 
of  molecules  urethan  per  100  mols.  solvent. 


Solubility  in  Water. 


Solubility  in  Methyl  Alcohol. 


/  — 

Mols. 

Gms 

r~~ 
\i7*.      e 

Mols. 

Gms. 

t°. 

Wt.  of 

I  CC. 

Solu- 

.•     _ 

CO(NH2) 
OC2H6  per 
100  Mols. 

CO(NH2) 
OC2H6per 
100  Gms. 

Wt.  or 

I  CC. 

Solu- 

CO(NH2) 
OC2H5per 
100  Mols. 

8§» 

zoo  Gms. 

tion. 

H20. 

H20. 

tion. 

CH3OH. 

CH3OH. 

o 

1.023 

3-6i 

I7.8 

0.956 

31.18 

86.76 

IO 

1-033 

6.0 

29.7 

0-977 

41  -o 

II4-I 

15 

i  .042 

15.0 

74-2 

0.989 

47-5 

I32.I 

20 

i  .060  • 

31.0 

153-3 

I  -OOO 

54-5 

i$*  -7 

25 

1.073 

50.0 

247-3 

I.OI3 

62.5 

173-9 

3° 

1.078 

65.0 

321.4 

I  .024 

72.0 

200.3 

40 

i  .065 

77.0 

380.7 

1.045 

89.0 

247-7 

Solubility  in  Ethyl 

Alcohol. 

Solubility 

in  Propyl 

Alcohol. 

t°. 

Wt.  of 

I  CC. 

Solu- 

A"     _ 

Mols. 
CO(NH2) 
OC2H5per 
100  Mols. 

Gms. 
CO(NH2) 
OC2H5  per 
loo  Gms. 

Wt.of 

I  CC. 

Solu- 

4.*     _ 

Mols. 
CO(NH2) 
OC2HS  per 
100  Mols. 

Gms. 
CO(NH2) 
OC2H5  per 
100  Gms. 

lion. 

C2H5OH. 

C2H5OH. 

tion. 

CaHyOHo 

C-jHyOH. 

o 

0.8914 

23.91 

46.26 

0.880 

19.48 

28.9 

IO 

0.930 

36.0 

69.6 

0.906 

31.0 

46.0 

15 

0.950 

43-o 

89.2 

0.923 

4O.O 

59-3 

20 

0.968 

50.0 

96.7 

0.942 

51.0 

75-7 

25 

0.985 

59-o 

II4.I 

0.963 

6o-O 

89.0 

30 

i  .001 

70.0 

135-4 

0.983 

68.0 

100.9 

40 

I-°35 

88.0 

170.2 

1.025 

85.0 

126.1 

Solubility  in  Chloroform. 

Solubility  in  Toluene. 

t° 

Wt.  of 

I  CC. 

Solu- 

Mols. 
CO(NH2) 
OC2H6per 

100  Alois. 

Gms. 
CO(NH2) 
OCsHsper 
100  Gms. 

Wt.of 

I  CC. 

Solu- 

Mols. 
CO(NH2) 
OC2H6  per 
100  Mols. 

Gms. 
CO(NH2) 
OCsH  per 
loo  Gms. 

tion. 

CHC13. 

CHCU. 

tion. 

CeHsCHa. 

CcHsCHg. 

0 

.404 

27.56 

20.  6 

0.887 

1-77 

I.7I 

10 

•340 

41 

30.6 

0.874 

5-o 

4.84 

X5 

.310 

46 

34-4 

0.875 

10.  0 

9.68 

20 

.280 

53 

39  6 

0-883 

16.0 

15.48 

25 

.240 

60 

44-8 

0.902 

25.0 

24.18 

30 

.203 

67 

50.0 

0.927 

44.0 

42.58 

40 

I.I25 

80 

59-7 

o-995 

85.0 

82.24 

100  gms.  sat.  solution  in  liquid  CO2  contain  4  gms.  urethan  at  the  critical  tem- 
perature, 23.5°;  at  30.5°  the  mixture  separates  with  two  layers.    (Buchner,  1905-06.) 


100  gms.  pyridine  dissolve  21.32  gms.  urethan  at  20-25°. 

i oo  gms.  aq.  50%  pyridine  dissolve  101.1  gms.  urethan  at  20-25* 


(Dehn,  1917.) 


URETHAN  742 

SOLUBILITY  OF  URETHAN  DERIVATIVES  IN  WATER. 

(Odaira,  1915.) 

Gms.  Cmpd. 

Name.  Formula.  t°.    per  100  Gms. 

H20. 

Detonal  (Diethyl  Aceturethan)  (CjHs^CH.CO.NH.CO.OCjHs  ...  0.526 

Epronal  (Ethylpropyl  Aceturethan)  (QH6)(C3H7)CH.CO.NH.CO.OC2H5  cold  0.143 

Dipronal  (Dipropyl  Aceturethan)  (C3H7)CH.CO.NH.CO.OC2H6  20  0.040 

Probnal  (Propylbutyl  Aceturethan)  (C3H7)(C4H9)CH.CO.NH.CO.OC2H5  20  0.032 

Dibnal  (Dibutyl  Aceturethan)  (C4H9)2CH.CO.NH.CO.OC2HB  ...  0.008 

Oenanthyl  Urethan  CH3(CH2)6CO.NH.CO.OC2H5  ...  0.021 

n  Isoamyl  Urethan  (C2H5)2CH.NH.CO.OC2H6  20  0.410 

a  Bromethyl  Propyl  Aceturea  (CiHsXCsH^CBr.CO.NH.CO.NHj  20  0.041 


DISTRIBUTION  OF  URETHAN  DERIVATIVES  BETWEEN  WATER  AND  OLIVE  OIL. 

Gms.  Cmpd.  per    Dist.  Ratio 

Name.  Formula.  t°.        -       '°°^  -  :>    Conc-°ii 

H2O      Olive  Oil    7^—  -- 
Layer.      Layer.      Conc-H2o 

Ethyl  Urethan  NHiCOOQH,  ord.  4.52  0.615  0.136(1) 

Methyl  Urethan  NH2COOCH3  ord.  7.50  0.275  0.037(1) 

Aceturethan  CHsCONH.COOCjHs  17-20  2.94  0.389  0.132(2) 

Epronal  (QHsXCjHOCH.CO.NH.CO.OCjHj      ".  0.076  0.257  3.3(2) 

Detonat  (QHj.CH.co.NH.co.OCiH.         " 


Veronal  (diethylbar-  [  rrvxrwrm  r  <r  H  ^  "        o.  180    o.  020    o.  n  (2) 

bituricacid)  }  COCNHCOWXCqW,  \o.M    0.032    0.12(2) 

(i)  Baum,  1899;  H.  von  Meyer,  1909.  (2)  Odaira,  1915. 


URIC  ACID 

SOLUBILITY  IN  WATER. 

(Blarez  and  Deniges,  1887;  at  15°  Magnier,  1875.) 


Gms.  CsJL^Oa.  Gms.  C6H^tOa  Gms. 

t*.  per  100  Gins.  t°.  per  100  Gms.  t°.  per  100  Gms. 

H20.  H30.  H20. 

O       0.002  30       0.0088  70        0-0305 

10       0.0037          4°       0-0122  80        0-0390 

15       O.OO53          50       O.OI7O          9O        0-0408 

20  0.006  60  0-0230  loo  0-0625 

One  liter  of  very  carefully  purified  CO2  free  water  dissolves  0.0253  gm.  uric 
acid  at  18°.  Constant  agitation  and  temperature  were  employed.  With  finely 
divided  uric  acid,  saturation  was  reached  after  one  hour.  The  amount  dissolved 
was  determined  by  the  difference  in  weight  between  the  amount  of  sample  taken 
and  that  remaining  undissolved.  (His,  Jr.  and  Paul,  1900.) 

One  liter  of  pure  CO2  free  water  dissolves  0.0649  Sm-  uric  acid  at  37°.  The 
amount  dissolved  was  determined  by  difference  and  only  20-25  minutes  agitation 
allowed  for  saturation.  It  is  stated  that  on  long  contact  with  water,  the  uric 
acid  breaks  down  and  the  solubility  and  conductivity  increase  directly  with  time. 

(Gudzeit,  1909.) 

One  liter  of  water  dissolves  0.0645  grn-  uric  acid  at  37°.    (Bechhold  and  Ziegler,  1910.) 

One  liter  of  serum  dissolves  0.9  gm.  uric  acid  at  37°. 


743  URIC  ACID 

SOLUBILITY  OF  URIC  ACID  IN  AQUEOUS  SOLUTIONS  OF  ACID  AT  18°. 

(His,  Jr.  and  Paul,  1900.) 

Concentration  of  Aq.  Acid.  Gms.  Uric  Acid 

Acid.  t- • per  1000  cc. 

Normality.  Per  cent.  Sat  Sol. 

Hydrochloric  i  3.65  0.0236 

3-75  13-69  0.0263 

6.24  22.77  0-0375 

Sulfuric  i  4.9  0.0227 

3.2  15.67  0.0205 

6.4  31-34  0.0183 

Additional  data  for  the  solubility  of  uric  acid  in  aqueous  sulfuric  acid  are  given 
by  Tafel  (1901).  A  saturated  solution  of  crystallized  uric  acid  in  80  wt.  per  cent 
aqueous  H2SO4  was  prepared  by  warming  to  about  120°  and  allowing  to  stand. 
Portions  of  the  clear  solution  were  diluted  with  increasing  amounts  of  water  and 
the  mixtures  allowed  to  stand  many  days  in  closed  flasks  which  were  frequently 
shaken.  The  precipitated  uric  acid  was  then  filtered  off  and  weighed  and  the 
amount  remaining  in  solution  calculated  by  difference.  The  following  results 
were  obtained. 

Wt.  %  of  aq.  H2SO4  72.5     70.5    68        66.5    62.5     59.5 

Gms.  uric  acid  per  100  gms. 
aq.  H2S04  6.45    3.85     1.60    0.64    0.35    0.312 

An  approximate  determination  of  the  solubility  of  uric  acid  in  alcohol  by  ex- 
traction in  a  Soxhlet  apparatus,  gave  0.00008  gms.  per  100  cc.   A  similar  determi- 
nation with  ether  as  solvent,  gave  negative  results.  (Gortner,  1914.) 
IOO  gms.  95%  formic  acid  dissolve  0.04  gm.  uric  acid  at  20°.  (Aschan,  1913.) 
pyridine  dissolve  0.21  gm.  uric  acid  at  20-25°.  (Dehn,  1917.) 
"        aq.  50%  pyridine  dissolve  0.75  gms.  uric  acid  at  20-25°.  " 


VALERIC  ACID  n  CH3(CH2)3COOH  (n  Propyl  Acetic  Acid). 

When  valeric  acid  is  shaken  with  water  at  16°,  two  layers  are  formed. 
100  gms.  of  the  aqueous  layer  contain  3.4  gms.  CHsCCt^sCOOH. 
100  gms.  of  the  acid  layer  contain  90.4  gms.  CHsCCf^sCOOH. 

/Lieben  and  Rossi,  1871.) 


DISTRIBUTION  OF  VALERIC  ACID  BETWEEN  BENZENE  AND  95.8%  SULFURIC 

ACID. 

(Gurwitsch,  1914.) 

The  mixtures  were  made  at  o°  and  brought  to  equilibrium  by  shaking  for  5 
minutes  at  18°,  and  allowing  to  stand  over  night. 

",  Gms.  Valeric  Acid  per  too  Gms.  Gms.  Valeric  Acid  per  100  Gms. 

Benzene  Layer.  H2SO4  Layer.  •  Benzene  Layer.  H2SO4  Layer. 

7.60  46.4  I  36.7 
4.78  44.8  0.58  35.2 
3.64  43.5  0.29  32.7 

2.61  41.4  0.20  30.7 

1.62  39.5  0.04  26.1 

1.48  38.1  0.007  23-8 

The  coefficient  of  distribution  of  isovaleric  acid  between  benzene  and  water  at 
room  temperature  is,  cone,  in  CeH6  -r  cone,  in  HjO  =  2.744.  (King  and  Narracott,  1909.) 


VALERAMIDES 


744 


DISTRIBUTION  OF  VALERAMIDES  BETWEEN  WATER  AND  OLIVE  OIL  AT  15°. 

(Harrass,  1903.) 


Amide. 


Formula. 


Valeramide 

Valerethylamide 

Valerdiethylamide 

Valerdimethylamide 

Lactdiethylamide 


CH3(CH2)3CONH2 

CH3(CH2)3CONH(C2H5) 

CH3(CH2)3CON(C2H5)2 

CH3(CH2)3CON(CH3)2 

CH3CHOHCON(C2H5)2 


Gms.  Cmpd.  per 
per  100  cc. 

Ratio 

Conc.oU 

Water 
Layer. 

Olive  Oil 
Layer. 

Conc.H2o 

0.769 

O.24I 

0-3I3 

I  .029 

O.26l 

0.254 

0.231 

1-339 

5-797 

O.QII 

o-379 

0.416 

1.256 

0.194 

0.154 

VANILLIN  CeHs.CHO.OCHg.OH,  1.3.4. 

100  gms.  H2O  dissolve  I  gm.  vanillin  at  20-25°. 

100  gms.  pyridine  dissolve  316  gms.  vanillin  at  20-25°. 


(Dehn,  191?-) 


DISTRIBUTION  OF  VANILLIN  BETWEEN  WATER  AND  ETHER  AT  25°. 

(Marden,  1914.) 


Dist.  Coef. 

0.108 
O.IIO 


Gms.  Vanillin  per  100  cc. 
H2O  Layer.  Ether  Layer. 

0.0l64  0.1294 

O.O242  0.1854 

0.0403  0.3310  O.IO4 

Fusion-point  data  for  mixtures  of  vanillin  and  orthovanillin  are  given  by 
Noelting  (1910).  Qualitative  solubilities  of  orthovanillin  in  a  number  of  solvents 
are  also  reported.  Data  for  the  sintering,  melting  and  clear  liquid  points  for 
mixtures  of  vanillin  and  an  extensive  series  of  compounds  are  given  by  Lehmann 
(1914). 


VERATRINE 


SOLUBILITY  IN  SEVERAL  SOLVENTS. 


Solvent. 


Water 
Water 

3%  H3B03  in  Aq. 
50%  Glycerol 
Aniline 
Pyridine 
Piperidine 
Diethylamine 
Oil  of  Sesame 


t°. 

Gms.  Veratrine 
per  loo  Gms. 
Solvent. 

25 

0.057 

20 

O.II4 

ord. 

6 

20 

37 

20 
20 

'75 
83 

20 

271 

20 

i-39 

Authority. 

(U.  S.  P.  VIII.) 
(Zalai,  1910.) 

(Baroni  &  Barlinetto,  1911.) 
(Scholtz,  1912.) 


(Zalai,  1910.) 


VERATROLE  Ce 

F.-pt.  data  for  mixtures  of  veratrole  and  p  xylene  are  given  by  Paterno  and 
Ampola  (1897). 

VERONAL   (Diethylbarbituric  Acid)  CO<  (NHCO)2>  C(C2H6)2.  See  also  p.  742. 
100  cc.  H2O  dissolve  0.625  gm.  veronal  at  15-20°.  (Squire  &  Caines,  1905.) 

100  cc.  90%  alcohol  dissolve  11.7  gms.  veronal  at  15-20°. 
100  cc.  ether  dissolve  8.7  gms.  veronal  at  15-20°.  " 


VESUVIN. 

loo  gms.  water 

pyridine 


.  50%  pyridine 


dissolve    8.5  gms.  vesuvin  at  20-25°.       (Dehn,  1917.) 
i.       K.t»« 


31-4 


745  WATER 

WATER  H2O. 

SOLUBILITY  OF  WATER  IN  BENZENE,  PETROLEUM  AND  PARAFFINE  OIL. 

(Groschuff,  1 91 1.) 

The  synthetic,  sealed  tube  method  was  used  and  the  experiments  were  made 
with  very  great  care.  The  mixtures  were  first  superheated  sufficiently  to  bring 
all  the  water  into  solution  and  then  cooled  until  a  fine  mist  was  formed.  The 
temperature  of  appearance  and  disappearance  of  this  fine  mist  was  determined  re- 
peatedly. The  benzene  was  of  dm  =  0.8799.  The  petroleum  was  American 
water  white,  of  d  =  0.792.  It  was  freed  from  HzO  by  distilling  3  times  from 
melted  Na  and  boiled  at  190-250°  at  atmospheric  pressure.  The  paraffine  oil 
was  first  heated  to  120-130°  and  then  distilled  twice  under  vacuum  over  melted 
Na  and  once  without  Na.  Its  du  =  0.883  and  b.-pt.  was  2OO°-3OO°  at  10  mm. 
pressure. 


Results  for: 
H2O  +  Benzene. 

H20  +  Petroleum. 

H2O  +  Paraffine  Oil. 

t°. 

+  3 
23 
40 

55 
66 

77 

Cms.  H2O 
per  100  Gms.  Sol. 

0.030 

0.061 
0.114 
0.184 
o-255 
o-337 

t°. 

+  18 

23 
30 
36 
53 

Gms.  H2O 
per  100  Gms.  Sol. 

0.0012 
0.005 
O.OO7 
0.008 
O.OI2 
O.O26 

t°. 

59 
61 
66 
79 
85 
94 

Gms.  H2O 
per  100  Gms.  Sol. 

0.031 
0.035 
0.043 
0.063 
0.075 
O.OQ7 

''•per 

+  16 
5° 
65 
73 
77 
94 

Gms.  H2O 
100  Gms.  Sol. 

0.003 
O.OI3 
0.022 
O.O3O 
0.035 
0.055 

Observations  on  the  solubility  of  water  in  essential  oils  are  given  by  Umney  and 
Bunker  (1912). 

XENON  Xe.  SOLUBILITY  IN  WATER. 

(von  Antropoff,  1909-10.) 

The  results  are  in  terms  of  the  coef.  of  absorption  /3,  as  defined  by  Bunsen  (see 
p.  227)  and  modified  by  Kuenen  in  respect  to  the  substitution  of  mass  for  volume 
of  water. 

t°.  0°.  10°.  20°.  30°.  4°°.  50°. 

Abs.Coef.j9         0.2180    0.1500    0.1109    0.0900    0.0812    0.0878 

NitroXYLENES. 

loo  gms.  95%  formic  acid  dissolve  0.71  gm.  trinitro-w-xylene  (m.  pt.  173°)  at 

18.5°.  (Aschan,  1913.) 

F.-pt.  data  for  mixtures  of  2.3,  dinitro-£-xylene  and  2.6,  dinitro-£-xylene  are 
given  by  Blanksma  (1913). 

XYLENOL   1.3.4,  C6H3.(CH3)2.0H. 

MISCIBILITY  OF  AQUEOUS  ALKALINE  SOLUTIONS  OF  XYLENOL  WITH  SEVERAL 
ORGANIC  COMPOUNDS,  INSOLUBLE  IN  WATER. 

(Sheuble,  1907.) 

To  5  cc.  portions  of  aq.  KOH  solution  (250  gms.  per  liter)  were  added  the  given 
amounts  of  the  aq.  insoluble  compound  from  a  buret  and  the  xylenol,  dropwise, 
until  solution  occurred.  Temperature  not  stated. 

Composition  of  Homogeneous  Solution. 

cc.  Aq.  KOH.  cc.  Aq.  Insol.  Cmpd.  Gms.  Xylenol. 

5  2  (=  1.64  gms.)  Octyl  Alcohol  (i)  i 

S  5  (  =  4-io     «   )  1.7 

5  2  (=1.74     "   )  Toluene  4.1 

5  3  (=2.61     "   )  5 

(i)  The  normal  secondary  octyl  alcohol,  i.e.,  the  so-called  capryl  alcohol,  CH3(CH2)5.CH(OH)CH,. 


YTTERBIUM  746 

YTTERBIUM   CobaltiCYANIDE  Yb2(CoC6N6)2.9H2O. 

1000  gms.  aqueous  10%  HC1  (^15  =  1.05)  dissolve  0.38  gm.  of  the  salt  at  25°. 

(James  and  Willand,  1916.) 

YTTERBIUM  OXALATE  Yb2(C2O4),.ioH2O. 

SOLUBILITY  IN  WATER  AND  IN  SEVERAL  AQUEOUS  SOLUTIONS. 

Aqueous- Solution  of:  Per  cent  Cone.      +<>         Gms.  YbztQOOs  A   fl,    •«. 

ofAq.Sol.         *        per  100  cc.  Solvent.  Authonty. 

Water  ...  25          O.OOO334   (Rimbach  and  Schubert,  1909.) 

(NH4)2C2O4.H2O  3.26          Ord.        0.095  (Cleve,  1902.) 

Methylamine  Oxalate        20  5 . 24*  (Grant  and  James,  1917.) 

Ethylamine  Oxalate        20  5.86* 

Triethylamine  Oxalate    20  2.05* 

Sulfuric  Acid  (i  n)  4.9  °-372        (Cleve,  1902.) 

*  The  authors  do  not  state  whether  their  figures  are  for  anhydrous  or  hydrated  salt. 

YTTERBIUM   Dimethyl  PHOSPHATE  Yb2[(CH3)2PO4]6. 

loo  gms.  H2O  dissolve  1.2  gms.  Yb2[(CH3)2PO4]6  at  25°  and  0.25  gm.  at  95°. 

(Morgan  and  James,  1914-) 

YTTERBIUM  SULFATE  Yb2(S04)3.8H2O. 

SOLUBILITY  IN  WATER. 

(Cleve,  1902.) 

Gms.  Yb2(S04)3 
t°.  per  100  Gms. 

H20. 

80  6.92 

90  S-83 

100  4-67 

YTTERBIUM  Bromonitrobenzene  SULFONATE  Yb(C6H3Br.NO2.SO3f  1.4.3)3.- 
I2H2O. 
100  gms.  sat.  solution  in  water  contain  7.294  gms.  of  the  anhydrous  salt  at  25°. 

(Katz  and  James,  1913.) 

YTTRIUM   CHLORIDE  YC13. 

100  gms.  alcohol  dissolve    61.1  gms.  YC13  at  15°.  (Matignon,  1906.) 

60.5  gms.  YC13  at  2O°.  (Matignon,  1909.) 

pyridine  dissolve    6.5  gms.  YC13  at  15°.  (Matignon,  1906.) 

YTTRIUM   CobaltiCYANIDE  Y2(CoC6N6)2.9H2O. 

1000  gms.  aq.  10%  HC1  (d^  —  1.05)  dissolve  2.78  gms.  of  the  salt  at  25°. 

(James  and  Willand,  1916.) 

YTTRIUM   GLYCOLATE  Y(C2H3O3)3.2H2O. 

One  liter  of  water  dissolves  2.447  gms-  of  the  salt  at  20°. 

(Jantsch  and  GrUnkraut,  1912-1913.) 

YTTRIUM  IODATE  Y(IO3)3.3H2O. 

100  gms.  H2O  dissolve  0.53  gm.  yttrium  iodate.  (Berlin.) 

YTTRIUM  MALONATE  Y2(C3H2O4)3.8H2O. 

SOLUBILITY  IN  AQUEOUS  MALONIC  ACID  AND  AMMONIUM  MALONATE 

SOLUTIONS. 

(Holmberg,  1907.) 

Gms.  YjCCsH/jO^j 

Solvent.  t°.  per  100  Gms. 

Solvent. 

1  Gm.  Am.  Malonate  per  10  cc.  Solution  20  0.3 

2  Gms.  Malonic  Acid  per  10  cc.  Solution  20  2.3 


Gms.  Yb2(S04)3 
t°.               per  TOO  gms.                t. 
H20. 

Gms.  Yb2(S04)3 
per  100  Gms. 
H20. 

O 

15-5 

44.2 
34-6 

55 
60 

10-4 

35 

19.1 

70 

7  .22 

747 


YTTRIUM  NITRATE 


YTTRIUM   Basic  NITRATE  3Y2O3.4N2O5.2H2O. 

EQUILIBRIUM  IN  THE  SYSTEM  YTTRIUM  NITRATE,  YTTRIUM,  HYDROXIDE 

AND  WATER  AT  25°.      (James  and  Pratt,  1910.) 

The  determinations  were  made  with  very  great  care.     The  mixtures  were  ro- 
tated 4^  months. 


Sat.  Sol.  ' 

Gms.  per  100  Gms 
H2O. 

Solid  Phase.              g^5  gol 

Gms.  per  100  Gms. 
H?0. 

•s     Solid  Phase. 

Y(NO3)3. 

Y203  as 
Y(OH)3. 

Y(N03)3. 

Y203  as 
Y(OH),. 

1.0260 

3-13 

0 

014 

Y(OH)3                             1.4867 

73 

•03 

0.078 

3Y203 

4N206.2H20 

.1106 

13.87 

o 

034 

" 

.5587 

89 

.06 

0 

074 

" 

.1907 

24.94 

o 

063 

" 

.6259 

103 

.80 

0 

075 

" 

•2517 

33-02 

0 

160 

"+3Y203.4N205.2H20 

.6931 

122 

.40 

o 

080 

« 

-3268 

44-35 

0 

114 

3Y203.4N205.2H20 

.7440 

137 

.IO 

o 

083 

"  +y(N03)3 

.4104 

58.61 

0 

095 

" 

.7446 

141 

.6 

o 

1 

f(NQOs 

YTTRIUM  OXALATE  Y2(C2O4)3.9H2O. 

One  liter  H2O  dissolves  o.ooi  gm.  Y2(C2O4)s  at  25°,  determined  by  the  elec- 
trolytic method.  (Rimbach  and  Schubert,  1909.) 

100  gms.  aqueous  ammonium  oxalate  solution  (3.26%  (NH4)2C2O4.H2O) 
dissolve  0.01714  gm.  Y2(C2O4)3.9H2O  at  room  temp.  (Cleve,  1902.) 

loo  gms.  aq.  2.16  n  H2SO4  dissolve  0.6884  gm.  Y2(C2O4)3  at  25°.     (Wirth,  1912.) 

loo  gms.  aq.  4.32  n  H2SO4  dissolve  1.4  gms.  Y2(C2O4)3  at  25°. 

100  cc.  aq.  20%  methylamine  oxalate  dissolve  0.877  gm.  yttrium  oxalate  at 
ord.  temp. 

loo  cc.  aq.  20%  ethylamine  oxalate  dissolve  1.653  gms.  yttrium  oxalate  at  ord. 
temp. 

100  cc.  aq.  20%  triethylamine  oxalate  dissolve  1.006  gms.  yttrium  oxalate  at 
ord.  temp.  (Grant  and  James,  1917.) 

YTTRIUM  Potassium  OXALATE  Y2(C204)3.4K2C2O4.i2H2O. 

SOLUBILITY  IN  WATER  AT  25°.    (Pratt  and  James,  1911.) 

The  determinations  were  made  with  great  care.     The  mixtures  were  constantly 
rotated  for  8  weeks. 
^5  of   Gms.  per  100  Gms. 
H2O. 


Solid  Phase. 


Sol.    ^ 

^(CA), 

K2C204. 

.008 

Trace 

1.31           Solid  Solution 

•035 

O.O2 

5-30 

•059 

O.O6 

8.88 

.096 

0.27 

14.50 

.132 

0.72 

20.27 

.166 

i-37 

26  .  02  Y2(C2O4)3.4K2C2O4.i2H2O 

^5  Of   Gms.  per  100  Gms. 
Sat.  H2O. 


Solid  Phase. 


Sol.    Y2(CA)i.  K,CA- 

.174 

.50     27  .  44  YJ(C204)3.4K2C2O4.i2H2O 

.199 

.  222 

•49     32-83 
.48     37-68 

K 

.231 

.42     39.12 

K2Q04 

.228 

.09     38.77 

.218    o          37.87 

" 

YTTRIUM   DimethylPHOSPHATE  Y2[(CH3)2PO4]6. 

100  gms.  H2O  dissolve  2.8  gms.  Y2[(CH3)2PO4]6  at  25°  and  0.55  gm.  at  95°. 

(Morgan  and  James,  1914.) 

YTTRIUM   SULFATE  Y2(SO4)3. 

SOLUBILITY  OF  YTTRIUM  SULFATE  IN  AQUEOUS  SOLUTIONS  OF  SODIUM 

SULFATE  AT  25°.      (James  and  Holden,  1913.) 

Equilibrium  was  reached  very  slowly  and  it  was  necessary  to  rotate  the  mixtures 
for  14  months  before  final  equilibrium  was  reached. 


Gms.  per  100  Gms. 
H20. 

Y2(S04)3. 

Na2S04.    ' 

5-6i 

1.29 

6.38 

3-85 

7.40 

6.21 

8.43 

8.53 

5-86 

7-57 

4-75 

7.72 

3-42 

10.14 

2.36 

11.36 

2.02 

13.42 

Solid  Phase. 


Y2(S04), 


"  +Y2(S04)3.Na2S04.2H20 
Y2(SO4)3.NaiSO4.2H2O 


Gms.  per  100  Gms. 
H20. 

Y2(S04)3. 

Na2S04. 

1.90 

14.89 

1.79 

16.51 

1.86 

18.44 

2.99 

19.96 

3-°4 

21.05 

2.27 

27.14 

i-52 

28.22 

1.61 

28.13 

5.38 

o 

Solid  Phase. 
Y2(SO4)s.Na2SO4.2HsO 


YTTRIUM  SULFONATES  748 

SOLUBILITY  OF  YTTRIUM  SULFONATES  IN  WATER. 

Gms.  Anhy. 
Sulfonate.  Formula.  t°.    S^°Inc^te         Authority. 

Gms.  H2O. 
Yttrium  Benzene  Sulfonate    Y(C6HSSO3)3.9H2O  15      60.4  (Holmberg,  1907.) 

"      m  Nitro- 
benzene Sulfonate  Y(C6H4.NO3.SOs)3.7H2O  15     48.3 
Yttrium  Bromonitrobenzene 

Sulfonate  Y(C6H3Br.NO2.SO3.i.4.2)3.ioH2O   25       3.88  (Katz& James, '13.) 

YTTRIUM  TARTRATE  Y2(C4H4O6)3.5H2O. 

SOLUBILITY  IN  AQUEOUS  TARTARIC  ACID  AND  AMMONIUM  TARTRATE 

SOLUTIONS  AT  2O0.      (Holmberg,  1907.) 

Gms.  Gms. 

Aq.  Solvent.  pe^Gms.  Aq.  Solvent.  J£g£Ji 

Sat.  Sol.  Sat.  Sol. 

1  gm.  Am.  Tartrate  per  10  cc.  2  gms.  Tartaric  Acid  per  10  cc. 
solution                                             0.6          solution  0.02 

2  gms.  Am.  Tartrate  per  10  cc.          i .  i      4  gms.  Tartaric  Acid  per  10  cc. 
solution  solution  0.02 

ZEIN  (Protein  from  Corn). 

SOLUBILITY  IN  AQUEOUS  ALCOHOL  SOLUTIONS  AT  25°. 

(Galeotti  and  Giampalmo,  1908.) 

Dry  powdered  zein  was  added  to  the  alcohol  +  water  mixtures  and  the  solutions 
kept  at  25°  and  shaken  frequently  during  24  hrs.  The  removed  undissolved  resi- 
due was  dried  to  constant  weight  and  weighed. 

Vol.  %  CiHjOH"  Gms.  Zein  per  Vol.  %  Ci,H5OH  Gms.  Zein  per 

in  Solvent.  100  Gms.  Sat.  Sol.  in  Solvent.  100  Gms.  Sat.  Sol. 

10  0.05  60  18.57 

20  O.II  70  I9-87 

30  O.2I  80  7.8l 

40  0.51  90  4.51 

5O  1.43  IOO  0.02 

Similar  results  are  given  for  the  solubility  of  zein  in  mixtures  of  C2H6OH  +  H2O 
+  CHC13  at  20°  and  C2H5OH  +  H2O  +  acetone  at  25°. 

ZINC  ACETATE  Zn(C2H3O2)2.2H2O. 

SOLUBILITY  IN  AQUEOUS  ETHYL  ALCOHOL  AT  25°.    (Seideii,  1910.) 

TTT.    m  •  Gms.  Zn-                       W4.  m  Gms.  Zn- 

rHOTT  ^  of           (C2H302)2.2H2O              rn'oH  4»  of  (C2H3O2)22H2O 

£&S,  Sat.  Sol.             per  zoo  Gms.  Jt&SS  Sat.  Sol.          per  100  Gms. 

in  Solvent.  ^Sat  Sd  in  Solvent.  *  Sat  Sol 

o       .168     30.80         60      0.920     10. 60 
10       .127     27.20         70      0.880      7.80 

20          .090       23.70  80        0.850        5.50 

30          .055       20.40  90        0.830        4.20 

40       .015     17  95      0.825      4 

50      0.970     13.80        loo      0.796      1.18* 

*  =  gms.  anhydrous  salt.    The  solid  phase  was  Zn(C2H3O2)2.2H2O  in  all  cases  except  this  solution. 
ioo  gms.  H2O  dissolve  41.6  gms.  Zn(C2H3O2)2.H2O  at  15°,  d  of  sat.  sol.  =  1.165. 

(Greenish  and  Smith,  1902.) 

ioo  cc.  anhydrous  hydrazine  dissolve  4  gms.  zinc  acetate  with  separation  of  a 
white  suspension  at  ordinary  temperature.  (Welsh  and  Broderson,  1915.) 

ZINC  ARSENATE  Zn3(AsO4)2.8H2O. 

ioo  gms.  95%  formic  acid  dissolve  0.26  gm.  Zn3(As04)2  at  21°.       (Aschan,  1913.) 

ZINC  ARSENITE  Zn3(AsO3)2. 

ioo  gms.  95%  formic  acid  dissolve  0.36  gm.  Zn3(AsO3)2  at  21°.        (Aschan,  1913.) 


749  ZINC  BENZOATE 

ZINC   BENZOATE  Zn(C7H6Oa)a. 

SOLUBILITY  IN  WATER. 

(Pajetta,  1906.) 
t°.  15-9°.         17°.         27-8°.        31-3°.        37-5°.        49-8°.         59-° 

Cms.  Zn(C7H5O2)2  per 

100  gms.  aq.  solution    2.55     2.49     2.41     2.05     1.87     1.62     1.45 

ZINC   BROMIDE  ZnBr2.2H2O. 

SOLUBILITY  IN  WATER. 

(Dietz,  1900;  see  also  Etard,  1894.) 


t°. 

Gms.  ZnBrg 
per  too  Gms. 
Solution. 

Mols.  ZnBr2 
per  TOO 
Mols.H20. 

Solid 
Phase. 

t°. 

Gms.  ZnBr2 
per  100  Gms. 
Solution. 

Mols.  ZnBr3 
per  100 
Mols.H2O. 

Solid 
Phase. 

-T5 

77-^3 

27.0 

ZnBr2.3H2O 

25 

82.46 

37-6 

ZnBr2.2H2O 

—  10 

78-45 

29.1 

" 

30 

84.08 

42-3 

« 

-  5 

80.64 

33-3 

" 

37 

86.20 

50.0 

" 

-  8 

79.06 

30.2 

ZnBr2.2H2O 

35 

85-45 

46.9 

ZnBra 

o 

79-55 

31-1 

" 

40 

85-53 

47-4 

" 

+  13 

80.76 

33-5 

" 

60 

86.08 

49-5 

" 

18 

81.46 

35-i 

" 

80 

86.57 

5I-S 

M 

100 

87.05 

53-8 

M 

ZINC  BICARBONATE  Zn(HCO3)2. 

SOLUBILITY  OF  ZINC  BICARBONATE  IN  WATER  CONTAINING  CARBON  DIOXIDE. 

(Smith,  1918.) 

For  description  of  the  experimental  method  see  iron  bicarbonate,  p.  336. 
Results  at  25°.  Results  at  30°. 


Atmospheres 
Pressure  of 
C02,  Calc.  by 
Henry's  Law. 

Gm.  Mols. 
Free  H2CO3 
per  Liter. 

Gm.  Mols. 
Zn(HCO3)2 
per  Liter. 

Gm.  Mols. 
Free  H2CO3 
per  Liter. 

Gm.  Mols. 
Zn(HC03)2 
per  Liter. 

4.12 

0.1390 

0.00194 

0.1838 

O.OO2I5 

5-33 

0.1797 

O.OO2II 

0.3838 

0.00277 

7.64 

0.2579 

0.00242 

0.4038 

0.00286 

10.61 

0.3580 

O.OO27O 

0.4601 

o  .  00308 

12.  16 

0.4103 

0.00278 

o  .  6064 

0.00324 

13.29 

o  .  4480 

O.OO29I 

0.6257 

0.00337 

19-73 

0.6657 

0.00317 

0.7470 

0.00352 

20.65 

0.6969 

0.00319 

0.8351 

0.00376 

22.56 

0.7610 

0.00343 

I  .  0840 

0.00339 

40.61 

I.370I 

0.00445 

I.I275 

0.00429 

The  calculated  pressures  are  lower  than  the  actual  pressures  since  Henry's  Law 
does  not  hold  at  very  high  pressures. 

"  If  zinc  carbonate  were  not  hydrolytically  dissociated,  its  solubility  in  pure 
water  at  25°,  would  be  4.58  X  io~*  gms.  mols.  per  liter."  (Smith,  1918.) 

ZINC   CARBONATE  ZnC03. 

Ageno  and  Valla  (1911)  report  that  the  solubility  of  ZnCO3  in  water  at  25°  is 
1.64. io~4  mols.  =  0.206  gm.  per  liter. 

One  liter  of  aq.  5.85%  NaCl  solution  dissolves  0.0586  gm.  ZnCO3  at  14°. 
One  liter  of  aq.  745%  NaCl  solution  dissolves  0.0477  gm.  ZnCO3  at  14°. 

(Cantoni  and  Passamanik,  1905.) 


ZINC  CHLORATE 


750 


ZINC   CHLORATE  ZnClO3. 

SOLUBILITY  IN  WATER. 

(Meusser,  1902;  at  18°,  Mylius  and  Funk,  1897.) 


-18 
o 
8 

15 
18 


Cms. 


Zn(ClO3)2 
too  Cms.  per  100 


Mols. 
Zn(C 


per 

Solution. 
55-62 

59-19 
60.20 
67.32 
66.52 


Solid  Phase. 

H20. 

9 . 70    Zn(ClO3)2.6H2O 
II.08 
11.72 
15.96 


15.39     Zn(C103)2.4H20     —13 
Sp.  Gr.  of  solution  saturated  at  18°  =  1.916. 


Cms.  Mols. 

Zn(C103)2       Zn(C103)2       Solid  Phase 
per  100  Cms.  per  100  Mols.     "        ^nase. 


Ice 


Solution. 
30         67.66 
4O         69  .  06 

H20. 

16.20 
17.29 

55      75-44 
Ice  curve 

24 

13      30.27 
9       26.54 

3-36 
2.80 

ZINC   CHLORIDE  ZnCl2. 

SOLUBILITY  IN  WATER. 

(Mylius  and  Dietz,  1905;  see  also  Dietz,  1900;  Etard,  1894.) 


A0        Gms.ZnCl2per  looGms.            Solid 

Gms.ZnCkper  looGms.         Solid 

Water.       Solution.                  Phase. 

'     Water. 

Solution. 

Phase. 

-  5 

14 

12.3                    Ice 

9 

360 

78.3 

.aiH2O  +  .H2O 

—  10 

25 

20-  o 

6 

385 

79-4 

ZnCl2.2iH2O 

-40 

83 

45-3 

6 

298 

74-9 

ZnCljj.iJHjjO 

-62 

104 

51.0      Ice  +  Zn£I2.4H20 

10 

330 

76.8 

" 

-5o 

"3 

53.0      ZnCl2.4H2O 

20 

368 

78.6 

•« 

-40 

127 

55-9 

26 

423 

80.9 

.i}H20+ZnCl2.H2O 

-30 

1  60 

6l-5       ^H20  +  .3H20 

26.3 

433 

81.2 

.iJH2O  +  ZnCla 

-10 

189 

65.4      ZnCl2.3H2O 

0 

342 

77-4 

ZnCl2.H2O 

o 

208 

67.5 

10 

364 

78.4 

" 

+  5 

230 

69.7 

20 

396 

79.8 

" 

6-5 

252.4 

71.6 

28 

436 

81.3 

ZnCl2.H20  +  ZnCla 

5 

282 

73-8 

31 

477 

82.7 

ZnCl2JH2O 

0 

309 

25 

432 

81.2 

ZnCla 

o 

235 

70  •  I      ZnCl2.2iH2O 

.40 

452 

81.9 

•« 

6.5 

252 

71-6      .2}H2O  +  .3H2O 

60 

488 

83.0 

« 

10 

272 

73  •  *      ZnCla-aiHaO 

80 

543 

84.4 

« 

12.5 

303 

75.2 

100 

615 

86.0 

•• 

«•$ 

335 

262 

CO 

IOO.O 

« 

SOLUBILITY  OF  OXYCHLORIDES  OF  ZINC  IN  AQUEOUS  SOLUTIONS  OF  ZINC 
CHLORIDE  AT  ROOM  TEMPERATURE. 

(Driot,  1910.) 


ZnCl2. 

ZnO. 

ouiiu  jriiase. 

8.22 

0.0137 

ZnCl,.4ZnO.6H2O 

23.24 

0.138 

" 

45-95 

0.497 

" 

51.5 

0.604 

" 

56.9 

0.723 

«' 

'  ZnCl2. 

ZnO.    ' 

62.85 

0.884 

ZnCl2.4Zn0.6H20 

96 

1.792 

" 

124.7 

3-213 

" 

144.8 

2.64 

" 

203 

i-59 

ZnClj.Zn0.iiH2O 

Results  are  also  given  for  mixture  of  the  oxychloride  and  oxide  in  aqueous  zinc 
chloride  solutions  at  various  temperatures. 


751 


ZINC   CHLORIDE 


SOLUBILITY  OF  ZINC  CHLORIDE-AMMONIUM  CHLORIDE  MIXTURES   IN   WATER. 

(Meerburg,  1903.) 


Isotherm  for  o°. 

Cms.  per  ioo  Gms. 
Solution.                Solid 

ZnCl2. 
0 

NH4C1. 
22.8 

NH4C1 

3-5 

23.0 

" 

7  -1 

23-5 

H 

10.2 

23-9 

" 

15-1 

24.7 

" 

18.0 

25-3 

" 

22.4 

26.0 

" 

24.2 

26.1 

" 

25-7 

26.3 

NH4C1  + 

27-5 

26.4 

a 

30-7 

25-7 

" 

33-9 

25-3 

«« 

38.8 

24.4 

" 

42.6 

24.6 

a  +  b 

44-3 

21-3 

b 

49-2 

15  .3 

" 

52.6 

11.9 

" 

55-4 

IO.O 

" 

59-3 

7-5 

•• 

62.1 

6.8 

M 

Isotherm  for  20°. 


Isotherm  for  30°. 


Gms.  per  ioo  Gms. 
Solution. 


ZnCl2. 

NH4C1.     ' 

o.o 

26.9 

5-i 

27.1 

9-5 

27.4 

12.7 

27-5 

J5-7 

27.7 

18.0 

27.9 

23-5 

29.0 

26.0 

29-5 

29-5 

28.1 

32-3 

27.7 

35-8 

27.0 

38-7 

26.9 

40.2 

26.6 

41.9 

26-3 

43-2 

26.0 

46.9 

21  .O 

53-2 

14-5 

58-4 

II  .1 

62  .7 

8.7 

66.6 

7-9 

Solid 
Phase. 

NHiCl 


Gms.  per  ioo  Gms. 
Solution. 


NH4C1  +  . 
a 


a  +  b 
b 


ZnCI2. 

NH4C1. 

0-0 

29-5 

9.2 

29.4 

16.0 

29.7 

2O.  2 

30.1 

24.7 

30-4 

26.3 

30.8 

27.2 

30.2 

30.1 

29.6 

36.8 

28.2 

42.4 

27-3 

43-8 

27-3 

45-o 

24.4 

5r-2 

I7.6 

61  .9 

10-4 

66.9 

9-2 

75-6 

6.1 

7o-3 

7.6 

78.5 

3-2 

76.9 

3-5 

79-8 

1.6 

81.6 

o.o 

Solid 
Phase. 

NHiCl 


ZnClj 


a  =  ZnCl2.3NHCl3,.    b  = 
IOO  gms.  abs.  acetone  dissolve  43.5  gms.  ZnCl2  at  18°,  d&  of  sat.  sol.  =  1.14. 

(Naumann,  1904.) 

ioo  gms.  glycerol  dissolve  50  gms.  ZnCl2  at  15.5°.  (Ossendowski,  1907.) 

loo  cc.  anhydrous  hydrazine  dissolve  8  gms.  ZnCl2  at  room  temp. 

(Welsh  and  Broderson,  1915.) 

When  I  gm.  of  zinc  as  chloride  is  dissolved  in  ioo  cc.  of  aq.  10%  HC1  and 
shaken  with  ioo  cc.  of  ether,  0.03  per  cent  of  the  metal  enters  the  ethereal  layer. 

(Mylius,  1911.) 

ZINC   CHROMATES. 

EQUILIBRIUM  IN  THE  SYSTEM  ZINC  OXIDE,  CHROMIUM  TRIOXIDE  AND 
WATER  AT  25°. 

(Groger,  1911.) 

An  excess  of  ZnO  was,  in  each  case,  shaken  for  3  days  at  25°,  with  gradually  in- 
creasing concentrations  of  chromic  acid. 


Gms.  per  Liter  Sat.  Sol. 


Solid  Phase. 


Gms.  per  Liter  Sat.  Sol. 


ZnO. 

Cr03.  ' 

0.409 

0.604  4ZnO.CrO3.3H2O 

2.24 

4.19        " 

5-  .86 

II.5          "  +3ZnO.CrO3.2H2O 

10.7 

22.2        3ZnO.CrO3.2H2O 

26.7 

57-5          " 

30-4 

66.7           "  +4ZnO.CrO3.3H2O 

32.2 

70  .  6        4ZnO.CrO3.3H2O 

ZnO. 

66.1 

CrO3. 
151 

ouuu  jruase. 
4ZnO.CrO3.3H2O 

83.7 

123 

192 

285 

"  +3Zn0.2Cr03.H20 
3ZnO.2CrO3.H2O 

193 

196 

450 
46l 

"  +ZnO.CrO3.H2O 

202 

389 

475 
940 

ZnO.CrO3.H20 

ZINC  CINNAMATE  752 

ZINC   CINNAMATE  Zn(C6H6CH:CHCOO)2. 

100  cc.  sat.  solution  in  water  contain  0.144  §m«  zmc  cinnamate  at  26.5°. 


(De  Jong,  1909.) 

ZINC   CYANIDE  Zn(CN)2. 

100  cc.  concentrated  Zn(C2H3O2)2  +  Aq.  dissolve  0.4  gm.  Zn(CN)2. 

100  cc.  concentrated  ZnSO4  -j-  Aq.  dissolve  0.2  gm.  (Joannis,  1882.) 

loo  gms.  H2O  dissolve  0.24  gm.  zinc  mercuric  thiocyanate,  ZnHg(CNS)4at  15°. 

(Robertson,  P.  W.,  1907.) 


ZINC   FLUORIDE  ZnF2.4H2O. 

One  liter  of  water  dissolves  16  gms.  at  18°. 


(Dietz,  1900.) 


ZINC  HYDROXIDE  Zn(OH)2. 

One  liter  of  water  dissolves  0.0042  gm.  ZnO  at  18°,  conductivity  method. 

(Dupre  and  Bialas,  1903.) 

One  liter  of  water  dissolves  o.oi  gm.  at  25°.  (Bodlander,  1898.) 

SOLUBILITY  OF  ZINC  HYDROXIDE  IN  AQUEOUS  SOLUTIONS  OF: 


Ammonia  and  Ammonia  Bases  at  I7°-I9°. 
(Herz,  1902.) 


Sodium  Hydroxide  at  Ord.  Temp. 
(Rubenbauer,  1902.) 


Normality 
of 

Normality 
of  Dis- 

Gms. ZnO 

Gms.  per  20  cc.  Solution         _  MoL 

the  Base. 

solved  Zn. 

Solution. 

Na.                     Zn.            the  NaOH. 

0.0942NH3 

O-OOII 

0.00185 

0.1012         0-0040         4  .50 

0.236         " 

O.OIIO 

O.OlSo 

0.1978            O.OI5O            2.33 

0.707          " 

0.059 

0.0958 

0.4278            O.O442            I  .06 

O.O005 

O-OOoS 

0-6670           O.I77I            0.70 

0.472 

O-OoSl 

0.0132 

0.9660           0.9630           0.48 

0.944 

O.O3 

0.0484 

1.4951            0.2481            0.31 

0.068  NH2C2H5 

0.0003 

0.0005 

2.9901        0.3700        0.16 

0.51 

O.0045 

O.OO74 

Moist  Zn  (OH)  2  used.     So- 

0.68 

0-0098 

0-0161 

lutions  shaken  5  hours. 

SOLUBILITY  OF  ZINC  HYDROXIDE  IN  AQUEOUS  SOLUTIONS  OF  AMMONIUM 

HYDROXIDE. 


Results  of  Euler  (1903). 


Results  of  Bonsdorff  (1904)  at  25°. 


t°. 

Normality 
of  Aq. 
Ammonia. 

Mols.  Zn 
per  Liter. 

Normality 
of  Aq. 
Ammonia. 

Gms.  ZnO 
per  Liter. 

Normality 
of  Aq. 
Ammonia. 

Gms.  ZnO 
per  Liter. 

15-17 

0.485 

O.OI3-O.OIO* 

0.3II 

0.85 

0.321 

0-34 

15-17 

0.97 

0.034 

0.825 

3-84 

0.643 

0.845 

21 

0-253 

O.OO29 

1.287 

7.28 

I.2I5 

2.70 

21 

0.259 

0.0022* 

1.928 

5-07 

21 

0.500 

O.OO97 

2.570 

7.01 

21 

0.518 

O.OO7O 

3-213 

10.  16 

f  Euler  states  that  the  higher  results  of  Herz  are  due  to  incompletely  purified 
zinc  hydroxide  and  uses  material  precipitated  from  the  nitrate  for  his  experiments. 
Different  preparations  of  Zn(OH)2  containing  from  55  to  77  per  cent  H2O  were 
used  and  in  the  two  cases  marked  *  ZnO  was  used. 

Bonsdorff  used  for  his  second  series  of  determinations,  Zn(OH)2  precipitated 
from  the  nitrate  and  brought  in  moist  condition  into  the  ammonia  solutions. 


753  ZINC  HYDROXIDE 

SOLUBILITY  OF  ZINC  HYDROXIDE  IN  AQUEOUS  POTASSIUM  HYDROXIDE 

SOLUTIONS. 

(Klein,  1912.) 

The  determinations  were  made  by  adding  aq.  ZnSO4  solution  (containing  one 
gm.  mol.  per  liter)  to  aq.  KOH  solutions  until  a  permanent  precipitate  just 
appeared.  The  titrations  are  also  recalculated  to  mols.  per  liter  and  correction 
made  for  the  dilution  of  the  KOH  solution  by  the  aq.  ZnSO4. 


Normality  of 
Aq.  KOH. 

cc.  ZnSO4 
Sol.  per  50  cc. 
Aq.  KOH. 

t^aicu 

tacea  iviois.  per  i^uer  01 

oat.  aoi. 

Oric  Cone. 
KOH. 

Corrected  Cone, 
of  KOH. 

Cone,    of  Zn. 

I 

5-5 

t 

0.9 

O.IO 

1.78 

13-1 

I.78 

1.42 

0.209 

2 

14-3 

2 

I.S6 

0.223 

2.22 

17.9 

2.22 

1-63 

0.266 

2-5 

18.8 

2-5 

I.8l 

0.272 

3 

24.6 

3 

2.02 

0.330 

3-6 

29.1 

3-6 

2.28 

0.368 

4 

34 

4 

2.38 

0.405 

6 

56  (?) 

6 

2.78 

0.540 

SOLUBILITY  OF  ZINC  HYDROXIDE  IN  ONE  PER  CENT  AQUEOUS  SALT 
SOLUTIONS  AT  i6°-2o°. 

(Snyder,  1878.) 

The  CO2  free  Zn(OH)2  dissolved  is  calculated  as  milligrams  Zn  per  liter  of  the 
given  salt  solution.     Additional  determinations  are  also  given. 

Aq.  Salt       Mgs.  Zn  per  Aq.  Salt  Mgs.  Zn  per  Aq.  Salt          Mgs.  Zn  per 

Solution.     Liter  Solution.  Solution.        Liter  Solution.  Solution.        Liter  Solution. 

Nad  51  K2S04  37.5  K2C03  o 

KC1  43  MgS04  27  NH4C1  95 

CaCl2  57.5  KN03  17.5  NH4N03  77 

MgCl2  65  Ba(N03)2  25  (NH4)2S04  88 

BaCl3  38 

ZINC  IODATE  Zn(IOi)i. 

100  gins.  H2O  dissolve  0.87  gm.  Zn(IO3)2  cold  and  1.31  gms.  hot. 

(Rammelsberg,  1838.) 

ZINC   IODIDE  ZnI2. 

• 

SOLUBILITY  IN  WATER. 

(Dietz,  1900;  see  also  Etard,  1894.) 

Gms.  ZnI2    Mols.  ZnI2  Gms.  ZnI2         Mols.  ZnI2 

t°.          per  100  Gms.     per  100     Solid  Phase.     t°.        per  100  Gms.  per  100  Mols.  Solid  Phase. 
Solution.       Mols.H2O.  Solution.  H2O. 

—  IO  80.50  23.3      ZnI2.2H2O          O  8l.II  24.2  ZnI3 

—  5   80.77    23-7    "    *8   81.20    24.4     " 
o    81.16    24.3    "     40    81.66    25.1     " 

+  10   82.06    25.8    "    60   82.37    2^-4 

22     83.12     27.8      "      80     83.05     27.5 
27     89.52     50.3      "      TOO     83.62      28.7 

Sp.  Gr.  of  sat.  solution  of  the  anhydrous  salt  at  18°  =  2.725. 

loo  gms.  glycerol  dissolve  40  gms.  ZnI2  at  15.5°.  (Ossendowski,  1907.) 


ZINC 

NITRATE 

754 

ZINC 

NITRATE 

Zn(N03)2. 

SOLUBILITY  IN  WATER. 

(Funk,  1900.) 

Gms. 

Mols. 

Gms. 

Mols. 

* 

Zn(NO3)oper   ZnNO3  per       Solid 
*  •              TOO  Gms.             100             Phase. 

t  °. 

Zn(N03)2per 
100  Gms. 

Zn(N03)2 

100 

per       Solid 
Phase. 

Solution. 

Mols.  H2O. 

Solution. 

Mols.  H20. 

-25 

40.12 

6.36 

Zn(NO3)2.9H2O 

18 

53-50 

IO-9 

Zn(N03)3.6H20 

—  22 

•5     40-75 

6-54 

44 

25 

55-90 

12  -O 

44 

—  20 

42.03 

6.89 

M 

36-4 

63.63 

I6.7 

" 

-18 

43-59 

7-34 

" 

36 

64.63 

17.4 

41 

-18 

44-63 

7.67 

Zn(NO3)2.6H2O  33.5        65  .  83 

I8.3 

44 

~~I5 

45.26 

7.86 

it 

37 

66.38 

z8.« 

Zn(N03)2.3H20 

-13 

45-51 

7-94 

* 

40 

67.42 

19.7 

«« 

—  12 

45-75 

8.01 

(i 

4i 

68.21 

20.4 

M 

0 

48.66 

9.01 

41 

43 

69.26 

21.4 

44 

-1-12 

•5     52-0 

10,3 

•4 

45-5 

77-77 

33-3 

M 

ZINC   OXALATE  ZnC2O4.2H2O. 

One  liter  H2O  dissolves  0.0057  Sm-  ZnC2O4  at  9.76°,  0.0064  §m-  at  I7-92°  and 
O.OO7I5  gm.  at  26.15°.  (Kohlrausch,  1908.) 

SOLUBILITY  OF  ZINC  OXALATE  IN  AQUEOUS  AMMONIUM  OXALATE 
SOLUTIONS  AT  25°. 

(Kunschert,  1904.) 


Mol.  Normal  (NH4)2C204 
Mol.  Zn  per  Liter 


0.05      o.io      0.15        0.20        0.25 
0.0022  0.0055  °-OIO55  0.0174    0.0257 

Complex  ammonia  zinc  oxalates  are  formed.  When  more  than  0.15  free  oxalate 
is  present  the  complex  has  the  formula,  (NH4)4Zn(C2O4)3.  In  the  more  dilute 
solutions  it  has  the  composition,  (NH4)2Zn(C2O4)2. 


ZINC   Ammonium  PHOSPHATE   ZnNH4PO4. 

One  liter  sat.  solution  in  water  contains  0.0136  gm.  ZnNH4PO4  at  10.5°  and 
0.0145  gm.  at  17.5°.  (Artmann,  1915.) 


ZINC   SULFATE  ZnSO4. 

SOLUBILITY  IN  WATER. 

(Cohen,  1900;  at  50°;  Callender  and  Barnes,  1897;  Etard,  1894;  Poggiale,  1843;  Mulder.) 


t°. 

Gms.  ZnSO4 

per  100  Gms.         Solid             «.  o 

Solution. 

Water. 

Phase. 

-  5 

28.21 

39-30 

ZnSO4.7H2O       25 

O.I 

29-54 

41-93 

39 

9.1 

32.01 

47-09 

"           5° 

IS 

33-81 

50.88 

70 

25 

36.67 

57-90 

80 

35 

39-98 

66.61 

90 

39 

41  .21 

70.05 

100 

-   5 

32.00 

47-oS 

ZnSO4.6H2O    1  2O 

01 

33-09 

49.48 

140 

1  60 


ns.  ZnSO4 

per  100  Gms 

Solid 
Phase. 

Solution. 

Water. 

38-94 

63.74 

ZnSO4.6H2O 

41  .22 

70.06 

.6H2O  +  .?H2O 

43-45 

76.84 

ZnS04.6H20 

47-5 

88.7 

.6H20  +  .H2O 

46.4 

86.6 

ZnSOvHzO 

45-5 

83-7 

44 

44-7 

80.8 

44 

41  .7 

71  .5 

44 

38.0 

61-3 

44 

33-o 

49-3 

44 

TheSp.  Gr.  of  a  sat.  sol.  of  ZnSO4  in  water  at  15°  is  1.452.       (Greenish  and  Smith,  i 
Data  for  the  solubility  of  ZnSO4  in  water  at  high  pressures  are  given  by  Cc 
and  Sinnige  (1909,  1910.) 


902.) 
Cohen 


755 


ZINC   SULFATE 


SOLUBILITY  OF  ZINC  SULFATE  —  SODIUM  SULFATE  MIXTURES  IN  WATER. 

(Koppel,  Gumpery,  1905.) 


Gms.  per  100 
Gms.  Solution. 

Gms.  per  100 
Gms  H2O. 

Mols. 
Mols. 

3er  100 
H2O.                   Solid 

t  °. 

ZnSO4. 

Na2SO4 

ZnSO4.        Na2SO4.        ZnSO4. 

Na2S04:             Phase' 

o 

27 

.19 

5 

•33 

40.30 

7.90 

4 

•50 

I 

.  OI        (  ZnSO4.7H2O  + 

5 

27 

•85 

6 

.27 

42.28 

9-52 

4 

•71 

1 

2  j        j      Na2SO4.ioH2O 

25 

17 

•58 

15 

•63 

26.32 

23.40 

2 

•94 

2 

.96        ZnNa2(SO4)2.4H2O 

30 

17 

.66 

15 

•58 

26.47 

23-44 

2 

•95 

2 

•97 

35 

17 

•59 

15 

.70 

26.36 

23-52 

2 

•94 

2 

.98 

40 

17 

•75 

15 

•72 

26.68 

23-63 

2 

.98 

2 

•99 

10 

29 

.16 

7 

.16 

45-79 

ii  .24 

5 

.11 

I 

.42     • 

15 

30 

.70 

6 

.40 

48.81 

10.17 

5 

•45 

I 

.29 

20 
25 

32 

•Si 

5 
4 

•36 

.41 

52-34 
56-15 

8.62 
7.22 

6 

.84 

•27 

I 
O 

.09 
.91 

3o 

36 

^28 

3 

.80 

60-55 

6-34 

6 

.76 

0.8l 

35 

38 

.18 

3 

•30 

65-25 

5-64 

7 

.28 

O 

.71     J 

38 

40 

38 

38 

•83 
.26 

2 
2 

.90 

.78 

66.64 
64.89 

4.98 
4.71 

7 

7 

•44 
.24 

0 
0 

•63 
.60 

10 

27 

.91 

7 

.92 

43-50 

12.34 

4 

•85 

I 

•565 

20 

24 
19 

.28 
.14 

10.90 

14.58 

36.92 
28.77 

16.71 
21.95 

4 
3 

.12 
.21 

2 

2 

.12 

•79 

25 

13 

•31 

19 

•94 

J9-93 

29.87 

2 

.22 

3 

•785 

30 

6 

.96 

27 

•75 

10.67 

42-51 

I 

.19 

5 

•39     J 

35 

5 

.61 

30 

•03 

8.72 

46.61 

O 

.971 

5 

.91 

ZnNa2(SO4)24H2O 

40 

5 

.96 

28 

•65 

9.16 

43-83 

I 

.02 

5 

•555  . 

"7~N<l2SO4 

SOLUBILITY  OF  ZINC  SULFATE  IN  AQUEOUS  ETHYL  ALCOHOL. 

(Schiff,  1861.) 


Concentration  of  Alcohol  10  per  cent 

Gms.  ZnSO4.7H2O  per  100  Gms.  Solution        51.1 


20  per  cent     40  per  cent 
39  3-45 


100  gms.  abs.  methyl  alcohol  dissolve  0.65  gm.  ZnSO4  at  18°,   5.90  gms. 
ZnSO4.7H2O  at  18°. 

100  gms.  50  per  cent  methyl  alcohol  dissolve  15.7  gms.  ZnSO.7H2O  at  18°. 

(de  Bruyn,  1892.) 

100  gms.  glycerol  dissolve  35  gms.  zinc  sulfate  at  15.5°.  (Ossendowski,  1907.) 

ZINC   SULFIDE   ZnS. 

One  liter  H2O  dissolves  70.6. lO"6  mols.  ZnS  =  0.0069  Sm-  at  l8°.  determined 
by  the  conductivity  method,  assuming  complete  dissociation  and  hydrolysis. 

(Weigel,  1906,  1907.) 

ZINC   SULFITE  ZnSO3.2H2O. 

IOO  gms.  H2O  dissolve  0.16  gm.  ZnSO3.2H2O.  (Houston  and  Trichborne,  1890.) 


ZINC   SULFONATES 


SOLUBILITY  IN  WATER. 

Formula. 


Gms.  Anhy. 

Name.  Formula.  t°.     Salt  per  100     Authority. 

Gms.  H20. 

Zinc  |8 Naphthalene  Sulfonate  (CioH7.S03)2Zn.6H2O    25  0.45     (Witt,  1915.) 

Zinc    2-Phenanthrene    "         (Ci4H9.S03)2Zn.6H2O    20  0.083   (Sandquist, '12.) 

3-          "  "          (Ci4H9.S03)2Zn.4H2O     20  0.19 

20  0.15 


ZINC   SULFONATES 


756 


SOLUBILITY  OF  ZINC  PHENOLSULFONATE,  p  (C6H4.OH.SO3)2Zn.8H2O,  IN 
AQUEOUS  ALCOHOL  SOLUTIONS  AT  25°. 

(Seidell,  1910.) 


Wt.%C_   . 
in  Solvent. 

O 
20 
40 

47 
60 


<*25  Of 

Sat.  Sol. 
1.185 

1. 161 


1. 106 


GmS.  (CgH4.OH.-     »rr.      c/    /-•  TT  /~VTT 

cr»  \  v.,  str  f)  n~,    VVt.  %  C2H5Uil 
t  Sol       in  Solvent- 


39-8 

40.7 
42.1 
42.2 

41.6 


80 
90 
92.3 

95 

IOO 


4.5  Of 

Sat.  Sol. 

1-057 
1.047 
1.048 
1.052 

J-o75 


Gms.  (C6H4.OH.- 
S03)^Zn.8H20  per 


40.7 
41.4 
41.9 
42.9 


ioo  gms.  H2O  dissolve  37  gms.  (C6H4.OH.SO3)2Zn.8H2O  at  15°  and  di5  of  sat. 

sol.  =  I.I62.  (Greenish  and  Smith,  1902.) 

ZINC   TARTRATE  C4H4O6.Zn.2H2O. 

SOLUBILITY  IN  WATER. 

(Cantoni  and  Zachoder,  1905.) 


15 

20 

25 
30 
35 


Gms. 

C4H4O6.Zn.2H2pper 
ioo  cc.  Solution. 

0.019 

0.022 

0.036 
0.041 
°-°55 


40 

45 

50 
55 
60 


Gms. 

n^Hjp  per 
ioo  cc.  Solution. 

0.060 

0.073 

0.087 
0.116 
0.104 


65 

70 

75 
80 
85 


Gms. 

C4H4O6.Zn.2H2O  per 
ioo  cc.  Solution. 

o.ioo 

0.088 

0.078 
0.059 
0.041 


ZINC  VALERATE  Zn(C4H9COO)2.2H2O. 
SOLUBILITY  OF  ZINC  VALERATE  IN  AQUEOUS  ALCOHOL  SOLUTIONS  AT  25°. 

(Seidell,  1910.) 


Wt.  % 
C2H5OH 
in  Solvent. 

^5  Of 

Sat.  Sol. 

Gms.  Zn(C4H9- 
COO)2.2H2O 
per  ioo  Gms. 
Sat.  Sol. 

Wt.% 
C2H5OH 
in  Solvent. 

d25  of 
Sat.  Sol. 

Gms.  Zn(C4H9- 
COO)2.2H20 
per  ioo  Gms. 
Sat.  Sol. 

0 

1.004 

1.44 

85 

0.836 

2-15 

20 

0.972 

0-75 

90 

0.827 

3-20 

40 

0.936 

0.76 

92-3 

0.828 

5-50 

00 

0.894 

I-I5 

95 

0.832 

8.80 

80 

0.848 

1.70 

IOO 

0.844 

15.60 

ZIRCONIUM   SULFATE   Zr(SO4)2. 
SOLUBILITY  OF  ZIRCONIUM  SULFATE  IN  AQUEOUS  SULFURIC  ACID  AT  37.5°. 

(Hauser,  1907.) 


Gms.  per  ioo  Gms.  Sat.  Sol. 


ZrO2. 

S03. 

19-5 

25.46 

18.8 

27 

16.2 

29.1 

9-6 

32.3 

5-3 

34.7 

3-51 

36.01 

1.03 

38.2 

0.46 

39-8 

0-33 

42.1 

o.  14 

46.8 

Gms.  per  ioo  Gms.  Sat.  Sol. 
• 


Zr(S04)2.4H20 


ZrO2. 

SO3. 

0.15 

56.7 

0.50 

57-5 

2 

59-5 

4-4 

61.4 

4-55 

61-5 

3-33 

63.8 

i.  80 

64.2 

I.  12 

66.8 

0.96 

68.4 

0.10 

81.5 

+Zr(S04)2.H2S04.3H20 

Zr(so,)2.Haso4.3H,o 


Zr(S04)2.H2SO4.H2O 


Results  at  22°  show  only  slight  differences  from  the  above  figures,  hence,  the 
temperature  coefficient  for  this  salt  is  quite  small.  In  an  earlier  paper  Hauser 
(J905)  gives  data  for  the  basic  sulfate  4ZrO2.3SO3.i4H2O. 


METHODS   FOR  THE  DETERMINATION  OF 
SOLUBILITY 

A  quantitative  determination  of  a  solubility  consists  essentially 
of  two  operations;  the  preparation  of  the  saturated  solution  and  its 
subsequent  analysis.  In  those  cases  where  these  steps  are  per- 
formed separately  the  method  may,  in  general,  be  designated  as 
the  analytical  and  in  those  where  they  are  combined,  as  the  syn- 
thetic. In  both  cases,  however,  the  consideration  of  first  import- 
ance is  the  assurance  that  final  equilibrium  between  solvent  and 
solute  has  been  reached.  Since  this  point  is  that  at  which  no  further 
change  occurs  in  the  relation  between  the  amount  of  the  compound 
in  solution  and  that  remaining  undissolved,  the  only  criterion  of 
saturation  is  the  evidence  that  the  concentration  of  the  solution  has 
not  changed  during  a  longer  or  shorter  interval  of  time,  during 
which  those  conditions  which  would  tend  to  promote  such  a  change 
have  been  allowed  to  operate. 

Of  the  conditions  which  promote  most  effectively  the  attainment 
of  equilibrium  between  a  solute  and  a  solvent,  the  provision  for  the 
intimate  contact  of  the  two  is  most  important.  In  other  words, 
only  by  the  thorough  mixing  which  agitation  or  effective  stirring 
provides  can  the  point  of  saturation  be  reached  with  certainty.  In 
the  case  of  the  reciprocal  solubility  of  liquids,  the  point  of  equi- 
librium is  usually  attained  within  a  much  shorter  period  than  in  the 
case  of  solids  dissolved  in  liquids.  In  the  latter  case,  the  necessary 
disintegration  of  the  solid,  incident  to  its  solution  in  the  liquid,  is  a 
process  which  is  restricted  to  the  surface  layers  of  the  solid,  and, 
therefore,  unless  a  large  area,  such  as  a  finely  divided  state  provides, 
is  available,  and  unless  that  portion  of  the  solvent  which  has  acted 
upon  a  given  surface  area  is  repeatedly  replaced  by  fresh  solvent, 
the  process  of  solution  will  be  greatly  retarded.  It  is  quite  evident 
that,  although  a  solution  in  contact  with  even  very  finely  divided 
solid  may  promptly  become  saturated  in  the  immediate  vicinity  of 
the  solid  without  stirring,  the  distribution  of  the  dissolved  material 
to  the  remainder  of  the  solvent  would  depend  upon  diffusion,  and 
since  the  rate  at  which  this  proceeds  would  diminish  as  the  concen- 
tration differences  became  equalized,  the  process  would  take  place 

757 


METHODS   FOR  THE  DETERMINATION  OF   SOLUBILITY 

at  a  gradually  diminishing  rate.  If  the  point  of  equilibrium  is 
approached  from  supersaturation,  the  above  remarks  apply  with 
equal  effect,  since  only  at  the  surface  of  the  solid  can  the  excess  of 
salt  leave  the  solution  and,  without  other  provision  than  diffusion 
for  successively  bringing  the  entire  amount  of  the  solution  in  con- 
tact with  the  solid,  the  deposition  of  the  excess  of  dissolved  material 
can  occur  only  at  a  very  slow  rate.  The  importance  of  active  and 
continuous  agitation  of  the  solid  and  solution,  in  effecting  satura- 
tion, cannot,  therefore,  be  too  strongly  emphasized.  It  may  in  fact 
be  assumed  that  determinations  of  the  solubility  of  solids,  made 
without  continuous  agitation,  are  always  open  to  the  suspicion  that 
the  results  do  not  represent  the  final  equilibrium  which  soich  data 
are  required  to  show. 

Since  solubility  is  a  function  of  temperature,  the  accurate  control 
of  the  temperature  in  making  a  solubility  determination  is  another 
one  of  the  indispensible  requisites  of  accuracy.  In  general,  it  may 
be  stated  therefore,  that  every  procedure  designed  for  preparing  a 
saturated  solution  must  include  provision  for  the  accurate  control 
of  the  temperature  and  for  active  and  continuous  agitation  or  stir- 
ring of  the  solution.  In  the  case  of  the  solubility  of  gases,  which  will 
be  considered  in  a  separate  section,  provision  for  the  control  of  the 
pressure  must  also  be  made. 

It  is  obvious  that  since  the  solubilities  of  various  compounds 
differ,  and  that  of  one  compound  is  affected  by  the  presence  of  an- 
other, the  accurate  determination  of  this  constant  for  a  particular 
molecular  species  presupposes  that  only  this  one  substance  is  pres- 
ent in  the  pure  solvent.  That  is,  accuracy  of  results  demand  that 
only  pure  compounds  be  involved  in  a  given  determination,  con- 
sequently, no  effort  should  be  spared  to  make  it  certain  that  the 
highest  possible  purity  of  both  solute  and  solvent  has  been  attained. 

Apparatus  for  the  Determination  of  the  Solubility  of  Solids  by  the 
Analytical  Method.  —  The  types  of  apparatus  which  have  been 
developed  for  the  preparation  of  saturated  solutions  of  solids  in 
liquids  differ  principally  in  respect  to  whether  designed  for  multiple 
or  single  determinations  at  a  given  temperature.  Examples  of  the 
first  type  are  illustrated  by  Figs.  I  and  2. 

It  will  be  noted  that  in  the  one  case  (Fig.  i)  the  bottles  containing 
the  solutions  are  stationary  and  the  liquid  in  each  and  in  the  con- 
stant temperature  bath  is  kept  in  motion  by  means  of  revolving 
stirrers.  This  form  of  apparatus  was  used  by  Moody  and  Leyson 
(1908)  for  the  determination  of  the  solubility  of  lime  in  water  and  is 
particularly  adapted  for  relatively  slightly  soluble  compounds  for 

758 


METHODS  FOR  THE  DETERMINATION  OF  SOLUBILITY 


FIG,  i. 


METHODS   FOR  THE  DETERMINATION  OF  SOLUBILITY 

which  rather  large  quantities  of  the  saturated  solution  are  needed 
for  accurate  analysis.  There  is  also  shown  in  the  figure  the  pro- 
vision for  withdrawing  the  saturated  solution  through  a  filter 
within  the  inverted  thistle  tube.  The  stirrers  in  the  bottles  are 
fitted  with  mercury  seals  to  prevent  access  of  air  containing  carbon 
dioxide.  Other  features  of  the  apparatus  will  be  readily  understood 
from  the  drawing. 

A  more  common  type  of  apparatus,  designed  for  the  simultaneous 
saturation  of  several  solutions  at  the  same  temperature,  is  that 
illustrated  by  Fig.  2,  in  which  the  bottles  containing  the  solutions 
are  slowly  rotated  in  the  constant  temperature  bath.  The  form 
shown  is  that  described  by  Noyes  (1892).  This  type  of  apparatus 
has  the  advantage  that  the  solid  is,  to  a  large  extent,  kept  in  suspen- 
sion in  the  liquid  and,  therefore,  offers  the  most  favorable  oppor- 
tunity for  continuous  and  uniform  contact  with  the  solution.  Many 
examples  of  this  form  of  apparatus,  differing  principally  in  size  and 
in  the  direction  of  movement  of  the  containers,  are  described  in  the 
literature. 

Of  the  second  type  of  apparatus,  designed  for  a  single  determina- 
tion at  a  given  temperature,  many  varieties  have  been  developed 
for  particular  conditions.  Of  these,  the  following  examples  have 
been  selected  as  typical  of  this  class  and,  it  is  hoped,  will  illustrate 
most  of  their  desirable  features.  They  are,  in  general,  adaptations 
of  earlier  designs  and  it  is  not  intended  that  the  name  given  in  con- 
nection with  each  is  that  of  the  investigator  who  deserves  the  credit 
for  originating  the  type.  The  drawings  will,  for  the  most  part, 
be  readily  understood  without  detailed  explanations.  The  dimen- 
sions are  not  stated,  since  they  can  usually  be  varied  to  suit  the 
needs  of  almost  any  problem. 

In  Fig.  3  is  shown  the  apparatus  used  by  the  Earl  of  Berkeley 
(1904)  for  the  very  careful  determinations  of  the  solubility  of 
inorganic  salts  in  water.  The  features  of  particular  interest  in 
connection  with  it  are,  that  the  water  bath  itself  is  made  to  serve 
as  the  temperature  regulating  device,  and  the  apparatus  for  with- 
drawing and  simultaneously  filtering  the  saturated  solution  is  a 
combination  of  pipet  and  pycnometer.  This  was  provided  with 
ground  glass  caps  for  each  end  and  the  stem  was  accurately  grad- 
uated. It  was,  of  course,  carefully  standardized  before  use.  The 
flexible  iron  plate  shown  was  made  of  a  disc  from  the  receiver  of 
a  telephone.  The  apparatus  was  used  for  determinations  at  tem- 
peratures between  30°  and  90°  and  the  range  of  variations  from 
the  set  temperature  of  the  bath  was,  for  2-3  hour  periods,  within 

760 


METHODS   FOR  THE  DETERMINATION  OF   SOLUBILITY 

about  0.2°.  For  the  inner  vessel  containing  the  salt,  the  range 
was  about  0.05°.  At  each  temperature  two  determinations  of  den- 
sity and  solubility  were  mad  ;  one  on  the  solution  obtained  by 
stirring  a  supersaturated  solution  in  contact  with  solid  salt,  and 
the  other  on  the  solution  obtained  by  stirring  an  unsaturated  solu- 
tion in  contact  with  an  excess  of  salt. 


FIG.  3. 

In  the  case  of  determinations  at  the  boiling  point  a  special 
apparatus  was  required.  Two  forms,  described  by  the  Earl  of 
Berkeley  (1904),  are  shown  in  Figs.  4 -and  5.  The  first  was  used 
for  the  less  soluble  salts  and  consisted  of  an  outer  tube  A  con- 
taining water  and  an  inner  tube  B  containing  salt  and  solution. 
By  boiling  the  water  vigorously  and  closing  the  side  tube  C,  steam 
passing  through  the  tube  D  stirred  the  solution  thoroughly  and 
the  temperature  rose  to  the  boiling  point  of  the  saturated  solution 
and  remained  constant  when  saturation  was  attained.  The  second 
form  of  apparatus  (Fig.  5)  was  devised  for  use  with  extremely 

761 


METHODS   FOR   THE   DETERMINATION   OF   SOLUBILITY 


soluble  salts.  In  these  cases  it  was  found  that  the  larger  quan- 
tity of  steam  required  for  thorough  stirring  dissolved  so  much 
salt  that  it  was  necessary  to  have  a  very  large  excess  present.  In 
this  apparatus  the  steam  was  generated  in  a  boiler  A  and  conducted 
through  the  tube  B  to  the  bottom  of  the  large  test  tube  C  containing 
the  excess  of  salt  and  solution.  The  test  tube  was  immersed  in  the  oil 


THERMOMETER 


PLWINUM  HIRE. 
FOR  PULLING  OFF 
THE  FILTER  — 


THERMOMETERS 


PLATINUM 

WIRE  FOR 
PUL  UNG  OFF 
f/LTEK 


STIRRER 


FIG.  4. 


FIG.  5. 


bath  D  which  was  vigorously  stirred  and  maintained  at  a  tempera- 
ture close  to  that  of  the  boiling  point  of  the  saturated  solution. 
When  the  temperature  of  the  oil  bath  was  below  the  boiling  point, 
salt  dissolved;  when  above,  salt  was  thrown  out  of  solution. 
Considerable  difficulty  was  experienced  in  filling  the  pycnometer 
with  the  saturated  solution  without  introducing  errors  due  to 
steam  bubbles  caused  by  the  suction  which  was  applied. 

762 


METHODS   FOR  THE  DETERMINATION   OF   SOLUBILITY 


A  comparatively  simple  form  of  the  type  of  apparatus  used  by 
Victor  Meyer  in  1875  and  modified  by  Reicher  and  van  Deventer 
(1890)  and  by  Goldschmidt  (1895),  is  described  by  Hicks  (1915)  and 
shown  in  the  accompanying  Fig.  6.  A  glass  cylinder  A  is  closed  at 


FIG.  6. 


FIG.  7. 


each  end  with  large  one-hole  rubber  stoppers.  The  mixture  of  salt 
and  solution  is  contained  in  this  cylinder  and  is  stirred  by  the 
rotation  of  the  tube  E  which  is  provided  with  an  enlargement  at 
its  lower  end  in  which  there  are  two  small  holes  at  H  and  I.  The 

763 


METHODS   FOR  THE  DETERMINATION   OF   SOLUBILITY 

stirrer  rotates  in  the  bearing  formed  by  the  hollow  wooden  cylin- 
der J.  The  glass  rod  K  carries  a  rubber  stopper  L  which  closes 
the  filtering  tube  M,  in  which  a  platinum  cone  N  supports  an 
asbestos  filter  0.  The  siphon  P  connects  the  filtering  tube  with 
the  flask  R  which  is  provided  with  an  outlet  through  the  small 
tube  S.  The  apparatus  is  immersed  in  a  constant  temperature 
water  bath  W,  to  about  the  level  shown  After  stirring  the  mix- 
ture of  salt  and  solution  a  sufficient  length  of  time  for  attainment 
of  saturation,  the  undissolved  salt  is  allowed  to  settle  and  the 
rubber  stopper  is  withdrawn  from  the  filter  tube  by  means  of  the 
glass  rod  K.  Suction  is  applied  through  the  tube  5  to  hasten 
the  filtering  and  the  clear  solution  collected,  at  the  temperature  of 
the  bath,  in  the  previously  weighed  flask  R. 

A  similar  apparatus  was  used  by  Walton  and  Judd  (1911),  for 
determination  of  the  solubility  of  lead  nitrate  in  pyridine.  This 
is  shown  in  Fig.  7  and  consists  of  a  glass  test  tube  fitted  with  a 
stirrer  which  turns  in  a  mercury  seal,  thus  preventing  loss  of 
solvent  by  evaporation  or  the  admission  of  moisture  from  the  air. 
To  take  a  sample  of  the  saturated  solution,  the  weighing  tube  A 
was  introduced  into  the  larger  tube  through  a  hole  in  the  stopper. 
After  reaching  the  temperature  of  the  bath  the  stirrer  was  stopped, 
the  end  of  the  small  tube  B,  which  was  covered  with  a  piece  of 
closely- woven  muslin,  was  dipped  below  the  surface  of  the  solu- 
tion and  the  liquid  drawn  into  A  by  applying  suction  at  C.  The 
tube  A  was  then  removed,  weighed  and  the  contents  analyzed. 

An  apparatus  which  was  used  by  Donnan  and  White  (1911), 
for  the  determination  of  equilibrium  in  the  system  palmitic  acid 
and  sodium  palmitate  is  shown  in  Fig.  8.  The  stirring  in  this  case 
was  accomplished  by  means  of  a  current  of  dry  air,  free  of  carbon 
dioxide.  The  apparatus  consists  of  two  parts,  namely,  an  inner 
chamber  E,  where  equilibrium  was  attained,  and  an  outer  case  A, 
designed  for  isothermal  filtration.  The  whole  was  immersed  in  a 
thermostat  to  the  level  W.  A  side  tube  B  permitted  connection 
with  a  filter  pump.  C  is  a  weighing  bottle  to  receive  the  filtered 
saturated  solution  and  D  a  Gooch  crucible  provided  with  a  paper 
filter.  The  cork,  closing  A,  was  covered  with  a  plastic  layer  to 
render  it  air-tight.  The  tube  at  the  lower  end  of  E  was  closed 
with  a  ground  glass  plug  F,  the  stem  of  which  was  enlarged  to  a 
small  bulb  at  G  and  then  drawn  out  to  pass  easily  through  H, 
leaving  an  air  free  outlet  around  it.  The  small  cork  I  was  used 
to  support  the  stopper  when  lifted  to  allow  the  contents  of  E  to 
flow  down  for  filtration.  The  dry  air  by  which  the  mixture  was 

764 


METHODS   FOR  THE  DETERMINATION  OF   SOLUBILITY 

stirred  was  drawn  through  K  by  applying  suction  at  H.  The 
preheating  of  this  air  was  accomplished  by  drawing  it  through  a 
thin  spiral  immersed  in  the  thermostat.  The  connection  between 
the  equilibrium  apparatus  and  preheater  was  made  through  a 
mercury  seal,  which  permitted  lifting  the  apparatus  easily  without 
damage  to  the  fragile  preheater  permanently  mounted  in  the 
bath.  This  apparatus  provided  for  the  recovery,  separately,  of 


FIG.  8. 


the  saturated  solution  and  undissolved  solid.  These  authors  also 
describe  an  improved  electrically  heated  and  controlled  constant 
temperature  bath. 

Determinations  at  lower  temperatures  than  can  be  constantly 
maintained  with  the  aid  of  a  water  bath  require  special  forms  of 
apparatus  which  permit  of  temperature  control  under  more  or 
less  restricted  conditions.  An  apparatus  of  this  type,  which  was 
used  by  Cohen  and  Inouye  (1910),  for  determination  of  the  solu- 
bility of  phosphorus  in  carbon  disulfide,  is  shown  in  Fig.  9,  and 
is  intended  for  the  range  of  temperature  between  — 10°  and  +10°. 
The  saturating  vessel  D  consists  of  a  glass  cylinder  to  the  upper 

765 


METHODS   FOR  THE  DETERMINATION  OF   SOLUBILITY 

end  of  which  is  cemented  a  steel  collar  E,  containing  a  deep  channel. 
A  mixture  of  litharge  and  glycerol  was  used  as  the  cementing 
material  for  this  purpose.  The  inverted  steel  cover  F  fits  into  the 
channel  of  this  collar  and  the  seal  of  the  joint  is  effected,  in  the 
usual  way,  by  means  of  a  layer  of  mercury.  The  cover  F  is  pro- 
vided with  a  brass  tube  K,  to  which  the  pulley  M  is  attached,  and 


FIG.  9. 


is  also  pierced  by  the  tightly  cemented-in  glass  tube  /.  The  glass 
rod  Gt  containing  on  its  lower  end  the  three  stirring  wings  H  H  H, 
is  cemented  into  the  brass  tube  K.  The  saturating  vessel  is,  for 
stability,  tightly  fastened  in  a  hole  in  a  block  of  lead,  5,  contained 
in  the  Dewar  cylinder  A.  An  atmosphere  of  CO2  in  the  saturat- 
ing vessel  is  provided  by  introducing  CO2  under  pressure  through 
7  and  allowing  the  excess  to  escape  through  the  mercury  seal  in  E. 
After  charging  the  apparatus,  /  is  closed  with  a  rubber  tube  and 
plug  and  the  stirrers  H  H  H  set  in  motion.  A  Witt  stirrer,  O, 
keeps  the  contents  of  the  bath  in  rapid  circulation.  Water  is 

766 


METHODS   FOR   THE   DETERMINATION   OF   SOLUBILITY 

used  in  the  bath  for  temperatures  above  o°,  and  alcohol  for  those 
below  o°.  The  regulation  of  the  temperature  is  accomplished  by 
addition  of  ice  or  solid  CO2  as  found  necessary  and,  therefore,  re- 
quires very  close  attention  on  the  part  of  the  experimenter. 

A  novel  and  simple  form  of  apparatus,  which  was  used  by  Bahr 
(1911),  for  the  determination  of  the  solubility  of  thallium  hydroxide 
at  temperatures  up  to  40°  is  shown  in  Fig.  10.  As  will  be  seen,  this 


FIG.  ii. 

consists  of  a  gas  washing  flask  to  the  arms  of  which  a  Y  tube  pro- 
vided with  two  stop-cocks  is  sealed.  The  inside  walls  of  the 
apparatus  were  coated  with  hard  paraffin  and  the  required  amounts 
of  thallium  hydroxide  and  water  introduced.  It  was  then  im- 
mersed in  a  water  bath  and  the  contents  stirred  by  means  of  a 
current  of  hydrogen,  which  entered  as  shown  and  with  A  and  E 
closed,  passed  through  D  and  out  at  B.  When  it  was  desired  to 

767 


METHODS   FOR  THE  DETERMINATION   OF   SOLUBILITY 

remove  a  sample  of  the  solution  for  analysis,  B  and  D  were  closed 
and  the  liquid  forced  through  A  into  the  pycnometer  by  means  of 
gas  pressure  entering  through  E.  For  temperatures  above  40°, 
the  form  of  apparatus  shown  in  Fig.  n  was  used.  In  this  case  K 
represents  a  copper  cylinder  with  double  walls,  of  which  the  inner 
compartment  G,  contains  concentrated  salt  solution  which  is 
stirred  by  a  stream  of  air  (not  shown),  and  the  outer  compart- 
ment contains  a  layer  of  heating  liquid  H.  The  glass  tube  L  con- 
tains the  mixture  of  thallium  hydroxide  and  water  which  is  stirred 
by  means  of  a  current  of  hydrogen  (not  shown).  When  saturation 
is  attained  the  tube  A ,  of  small  bore  and  thick  walls  and  provided 
with  a  small  asbestos  filter,  is  introduced  and  the  saturated  solution 
forced  over  into  the  receptacle  B  by  pressure  of  hydrogen  which 
enters  at  C.  The  heating  liquid  in  B  is  the  same  as  used  in  H. 
The  following  heating  liquids  with  the  boiling  points  shown  were 
used:  Allyl  chloride,  46°;  Ethylene  chloride,  55°;  Chloroform,  61°; 
Methyl  alcohol,  66°;  Benzene,  80°;  Benzene-Toluene  mixture,  91°; 
Water,  100°. 

A  somewhat  more  elaborate  apparatus,  in  which  the  constant 
temperature  is  maintained  by  means  of  the  vapor  of  a  boiling 
liquid,  is  shown  in  Fig.  12.  This  apparatus  was  developed  by 
Tyrer  (1910)  for  the  very  accurate  determination  of  the  solubili- 
ties of  anthraquinone,  anthracene  and  phenanthraquinone  in  single 
and  mixed  organic  solvents.  The  solvent  with  excess  of  the  solute 
was  placed  in  A  and  kept  in  constant  agitation  by  means  of  the 
vertically  acting  stirrer  shown.  The  tube  A  is  surrounded  by  a 
bath  of  vapor  which  circulates  through  the  cylinder  B,  condenses 
in  C,  and  returns  to  the  boiling  flask  M.  When  the  solution  is 
saturated  it  is  allowed  to  settle,  and  the  clear  solution  run  out 
(by  raising  the  tube  D)  into  a  small  graduated  flask  E,  which  is 
maintained  at  the  same  temperature  as  the  solution  A.  The  tem- 
perature of  the  vapor  bath  is  varied  by  changing  the  pressure 
under  which  the  liquid  in  the- flask  M  is  boiling.  For  this  purpose, 
the  manostat  P  is  provided.  The  temperature  can,  with  care,  be 
maintained  constant  to  0.01°.  For  this  purpose  the  apparatus 
must  be  air-tight,  the  liquid  in  the  boiling  flask  must  not  bump 
(which  is  entirely  prevented  by  placing  a  layer  of  mercury  in  the 
flask)  and  a  pure  boiling  liquid  must  be  used. 

Although  illustrations  of  special  forms  of  apparatus  designed  for 
securing  equilibrium  in  solubility  determinations  could  be  extended 
far  beyond  the  number  given,  it  is  believed  that  the  principal 
features  have  been  made  clear  and  it  will  no  doubt  be  possible  to 

768 


METHODS   FOR  THE  DETERMINATION   OF   SOLUBILITY 

adapt  the  devices  here  shown  to  many  other  cases  for  which  accu- 
rate determinations  of  solubility  may  be  desired. 

Separation  of  Saturated  Solution  from  Undissohed  Solid.  —  The 
next  point,   after  the  establishment  of  equilibrium  between  the 


FIG.  12. 

solvent  and  solution,  is  the  matter  of  successfully  separating  the 
saturated  solution  from  the  undissolved  solid,  preparatory  to  its 
analysis.  There  are,  undoubtedly,  many  cases  where  this  is  a  very 
serious  problem.  This  is  especially  so  for  extremely  soluble  com- 
pounds, which  yield  viscous  solutions  as  well  as  for  those  which 
do  not  readily  settle  out  of  the  solution  or  cannot  be  removed  by 

769. 


METHODS   FOR  THE  DETERMINATION  OF  SOLUBILITY 

ordinary  filtration.  It  is,  of  course,  necessary  to  maintain  the 
mixture  at  the  temperature  at  which  saturation  was  obtained  until 
the  complete  separation  of  the  solution  and  solid  has  been  effected. 
The  operation  should,  therefore,  as  a  general  thing,  be  conducted 
in  the  same  bath  used  for  preparing  the  saturated  solution.  Sev- 
eral forms  of  apparatus  designed  for  this  purpose  are  shown  in 
the  diagrams  given  in  the  preceding  pages.  For  solutions  which 
can  be  readily  separated  from  the  undissolved  solid,  a  graduated 
pipet  to  which  a  stem  with  a  plug  of  filtering  material  can  be 
attached  and  which  is  adapted  to  being  easily  weighed,  is  the  most 
convenient. 

Analysis  of  the  Saturated  Solution.  —  The  weight  of  a  known 
volume  of  the  perfectly  clear  solution,  that  is,  its  specific  gravity, 
should  always  be  determined.  This  weighed  quantity  of  solution, 
or  a  known  dilution  of  it,  furnishes  a  very  convenient  sample  for 
the  determination  of  the  amount  of  dissolved  compound. 

In  regard  to  the  analysis,  the  procedure  must  be  selected  en- 
tirely on  the  basis  of  the  number  and  character  of  the  constituents 
present.  In  cases  of  the  solubility  of  single  non-volatile  compounds, 
in  solvents  which  can  be  more  or  less  easily  removed  by  volatiliza- 
tion, the  plan  in  most  general  use  is  the  evaporation  of  a  known 
amount  of  the  solution  to  dryness  and  weighing  the  residue.  Special 
forms  of  apparatus  to  be  used  for  this  purpose  have  been  proposed 
from  time  to  time.  These  are,  usually,  vessels  with  tubular  open- 
ings, arranged  so  that  a  current  of  dry  air  can  be  drawn  over  the 
surface  of  the  heated  sample. 

In  the  case  of  solubility  determinations  in  which  the  saturated 
solution  contains  more  than  one  dissolved  compound,  the  applica- 
tion of  the  usual  gravimetric  or  volumetric  procedures  will,  of 
course,  be  necessary.  Where  unique  methods  have  been  developed, 
a  brief  reference  to  them  will  usually  be  found  in  the  body  of  the 
book,  in  connection  with  the  results  for  the  compound  in  question. 

In  certain  cases,  where  the  direct  determination  of  the  amount 
of  the  dissolved  compound  present  in  the  solution  would  be  very 
difficult  or  impossible,  an  indirect  method  can  sometimes  be  used. 
For  this  purpose,  a  carefully  weighed  amount  of  the  compound 
must  be  used,  and,  after  the  period  of  saturation,  the  undissolved 
residue  is  filtered  off  under  conditions  which  reduce  losses  to  a 
minimum  and,  after  drying  to  its  original  condition,  it  is  weighed, 
and  the  amount  which  has  been  dissolved  found  by  subtracting 
the  weight  of  the  undissolved  residue  from  the  quantity  originally 
present. 

770 


METHODS  FOR  THE  DETERMINATION  OF   SOLUBILITY 

Identification  of  the  Solid  Phase.  —  As  already  mentioned  in  the 
chapter  on  General  Information,  the  solubility  of  a  compound, 
which  is  capable  of  existing  in  several  forms,  depends  upon  the 
particular  form  in  which  it  is  present  in  contact  with  the  satu- 
rated solution.  The  question  of  the  composition  of  the  solid  phase 
is,  therefore,  of  considerable  importance  for  the  accurate  deter- 
mination of  solubility.  Although  the  identification  of  the  solid 
phase  presents  little  difficulty  in  the  majority  of  cases,  it  some- 
times happens  that  it  can  be  made  only  by  a  more  or  less  indirect 
method.  The  principal  reason  for  this  is  that  adhering  solution  can 
usually  not  be  completely  removed  from  the  solid  phase  and  the 
analysis,  consequently,  does  not  give  direct  information  of  the 
required  accuracy. 

A  method  which  has  been  used  considerably  for  identifying  the 
solid  phase  is  that  known  as  the  residue  method  of  Schreinemakers 
(1893).  It  is  based  on  the  principal  that  if  an  analysis  is  made  of 
both  the  saturated  solution  and  of  a  mixture  of  the  saturated  solu- 
tion and  the  solid  phase  of  unknown  composition,  the  two  points  so 
obtained,  when  plotted  on  a  coordinate  system,  lie  on  a  line  con- 
necting the  point  representing  the  composition  of  the  solid  phase  and 
the  solubility  curve  of  the  system.  Similar  analyses  of  another  sat- 
urated solution  of  the  system  and  of  its  mixture  with  the  solid 
phase,  locate  another  such  line.  Since  all  lines  so  determined 
when  extended,  pass  through  the  point  representing  the  compo- 
sition of  the  solid  phase,  their  intersection  locates  this  point 
definitely. 

Although  the  original  description  of  this  method  by  Schreine- 
makers was  illustrated  by  an  example  drawn  on  the  rectangular 
system  of  coordinates,  it  has  been  used  much  more  extensively,  in  a 
practical  way,  in  connection  with  the  later  developed  equilateral 
triangular  diagram.  In  this  case,  each  apex  of  the  triangle  repre- 
sents one  of  the  three  components  of  the  system,  each  point  on  a  leg, 
a  mixture  of  two,  and  each  point  within  the  triangle  a  mixture  of  all 
three  components.  When  a  number  of  saturated  solutions  are 
analyzed,  the  results  correspond  to  points  on  the  solubility  curve  of 
the  system.  If  now  some  of  the  solid  phase  with  adhering  solution 
is  removed  from  each  mixture  and  analyzed,  it  is  evident  that  the 
results  thus  obtained,  being  for  samples  made  up  of  both  the  satu- 
rated solution  and  the  solid  phase,  give  points  which  lie  on  lines 
connecting  the  two.  The  points  on  the  curve  for  the  pure  saturated 
solutions  being  known,  it  is  necessary  only  to  connect  them  with  the 
points  for  the  corresponding  mixtures  of  solid  phase  and  saturated 

771 


METHODS   FOR   THE   DETERMINATION  X)F   SOLUBILITY 

solution,  and  to  prolong  the  lines  to  their  common  intersection. 
This  will  necessarily  be  at  the  point  representing  the  composition 
of  the  pure  solid  phase. 

In  applying  the  residue  method  of  Schreinemakers,  if  the  inter- 
secting lines  which  fix  the  point  corresponding  to  the  solid  phase 
meet  at  a  very  narrow  angle,  definite  information  as  to  its  composi- 
tion may  not  be  secured.  For  cases  such  as  these,  a  procedure  to 
which  the  name  "tell-tale"  method  was  given  by  Kenrick  (1908) 
and  which  is  described  in  detail  by  Cameron  and  Bell  (1910),  has 
been  developed.  This  method  consists  in  adding  to  the  mixture  a 
small  amount  of  an  entirely  different  compound  which  remains 
wholly  in  the  solution.  After  equilibrium  has  been  reached,  a  por- 
tion of  the  saturated  solution  and  of  the  solid  phase  with  adhering 
solution  are  analyzed,  and  the  quantity  of  the  added  "tell-tale" 
compound  in  each  determined.  From  the  result,  showing  the  con- 
centration of  the  added  compound  in  the  saturated  solution,  and  the 
amount  of  it  found  in  the  mixture  of  solid  and  solution,  the  quantity 
of  solution  in  contact  with  the  solid  can  be  calculated.  Since  the 
composition  of  the  solution  is  also  known,  the  difference  between 
the  composition  of  the  solid  plus  solution  and  of  the  amount  of 
solution  known  to  be  present,  is  the  composition  of  the  pure  solid. 

Transition  Temperatures  can  frequently  be  accurately  determined 
by  relatively  simple  means,  and  since  such  data  are  useful  in  estab- 
lishing fixed  points  on  solubility  curves  they  are  valuable  adjuncts 
to  directly  determined  solubility  data. 

Synthetic  Method.  —  The  procedures  which  have,  so  far,  been 
mentioned  are  all  classed  as  analytical  methods  of  solubility  deter- 
mination. In  contradistinction  to  these  is  the  equally  useful  reverse 
process,  by  which  the  solvent  and  solute  are  brought  together'  in 
previously  measured  quantities  and  the  temperature  ascertained  at 
which  the  solution  is  saturated.  To  this  procedure  the  designation 
synthetic  method  of  solubility  determination  has  been  applied. 
One  of  the  earliest  investigators  to  use  this  method  extensively  was 
Alexejeff  (1886)  and  it  is,  therefore,  frequently  referred  to  as  the 
Alexejeff  synthetic  method  of  solubility  determination. 

The  synthetic  method  can,  of  course,  be  used  both  for  the  solu- 
bility of  solids  in  liquids  and  for  liquids  in  liquids,  but  it  is  in  the 
latter  case  that  it  is  of  greatest  service.  Its  points  of  superiority, 
particularly  in  the  case  of  the  reciprocal  solubility  of  liquids,  are 
that  the  upper  limits  of  the  determinations  can  be  extended  far 
beyond  the  boiling  point  temperature  and  are,  in  fact,  limited  only 
by  the  resistance  of  the  glass  to  pressure  or  to  the  action  of  the 

772 


METHODS  FOR  THE  DETERMINATION  OF  SOLUBILITY 

liquid.  Only  small  quantities  of  the  solute  and  solvent  are  required 
for  a  determination.  It  is  applicable  to  compounds  for  which 
quantitative  methods  of  analysis  are  not  available  or  are  of  a  tedious 
character.  The  mixtures,  being  contained  in  sealed  tubes,  are  not 
subject  to  the  action  of  constituents  of  the  air,  nor  are  losses,  due  to 
volatilization,  to  be  feared.  Although,  in  the  case  of  solids,  diffi- 
culties incident  to  the  supersaturation,  resulting  from  failure  of  the 
crystals  to  separate  on  cooling,  are  encountered,  with  liquids 
the  point  of  saturation  is  made  instantly  and  strikingly  evident  by 
the  beginning  of  opalescence  or  clouding  which  occurs,  and  errors 
due  to  supersaturation  are  rarely  encountered.  A  sure  criterion 
that  supersaturation  does  not  occur  rests  on  the  observation  of  the 
temperature  at  which  the  cloudy  solution  again  clears.  If  this 
temperature  coincides  with  the  temperature  of  the  beginning  of 
opalescence,  it  is  certain  that  supersaturation  has  not  occurred. 
The  observation  of  the  temperature  of  saturation  can  be  repeated 
as  often  as  desired,  and  the  accuracy  of  the  determination  is  ordi- 
narily limited  only  by  the  care  taken  in  making  it. 

The  limitations  of  the  method,  aside  from  the  supersaturation 
which  may  occur  in  the  case  of  solids,  are  principally  those  resulting 
from  the  low  temperature  coefficients  of  solubility  possessed  by 
certain  compounds,  and  which  usually  occur  in  the  vicinity  of 
maxima  or  minima  of  solubility  curves.  Although  a  "critical  cloud- 
ing" occurs  in  the  vicinity  of  the  so-called  critical  solution  point, 
this  possesses  a  characteristic  appearance  which  is  easily  distinguish- 
able from  the  clouding  observed  at  the  saturation  point,  and  errors 
of  observation  due  to  it  are  not  to  be  apprehended.  In  fact,  it  has 
been  pointed  out  that  supersaturation  disappears  at  the  critical 
point,  and  the  synthetic  method  is  ordinarily  very  accurate  in  the 
vicinity  of  the  critical  solution  temperature. 

Since,  by  the  synthetic  method  the  results  are  necessarily  obtained 
under  different  pressures,  this  question  has  been  given  consideration 
from  the  theoretical  and  the  practical  side.  Although  it  is  possible 
that  extremely  high  pressures  would  exert  an  influence,  the  conclu- 
sion appears  justified,  that  under  ordinary  conditions,  in  which 
pressures  of  10  atmospheres  are  not  exceeded,  no  notable  effect 
would  be  produced.  The  solubility  curves  obtained  by  this  method 
do  not  show  any  abnormalities  due  to  this  cause. 

In  the  case  of  the  determination  of  the  solubility  of  solids  by  the 
synthetic  method,  the  operation  consists  in  preparing  a  mixture  of  a 
carefully  determined  amount  of  the  solvent  and  of  the  solid,  and 
subjecting  it  to  gradually  increasing  temperature  and  to  constant 

773 


METHODS   FOR  THE  DETERMINATION   OF   SOLUBILITY 

agitation,  while  a  continual  observation  of  the  changes  taking  place 
in  the  solid  is  made.  When  all  but  a  few  small  crystals  have  dis- 
solved, the  change  in  temperature  is  regulated  much  more  carefully 
and  note  is  taken  of  the  point  at  which  the  edges  of  these  final 
crystals  begin  to  change  from  sharp  to  rounded,  or  vice  versa,  or 
where  the  sizes  of  the  particles  visibly  increase  or  diminish.  Care 
must,  of  course,  be  taken  not  to  allow  the  last  portions  of  the  solid 
to  dissolve;  otherwise,  on  cooling,  considerable  supersaturation  may 
occur  before  the  solid  begins  to  separate  from  solution.  The  method 
is,  naturally,  most  serviceable  where  the  change  in  solubility  with 
temperature  is  considerable,  and  where  convenient  methods  for  the 
direct  analysis  of  the  solution  are  not  available. 

The  procedure  of  a  determination  in  the  case  of  the  reciprocal 
solubility  of  liquids  consists  in  introducing  by  means  of  capillary 
funnels  weighed  amounts  of  the  two  liquids  into  small  glass  tubes 
and  sealing  the  ends.  The  amount  of  air  space  in  the  tubes  should 
be  kept  low.  Many  convenient  devices  for  weighing  and  intro- 
ducing the  liquids  have  been  described.  In  the  case  of  very  volatile 
liquids  it  may  be  necessary  to  introduce  them  in  thin  walled  bulbs, 
which  can  be  broken  after  the  tube  containing  the  mixture  has  been 
sealed.  The  tube  is  then  placed  in  a  large  beaker  of  water,  or  higher 
boiling  liquid  if  necessary,  and  heat  applied  until  the  contents  of  the 
tube,  on  being  shaken,  become  homogeneous.  The^temperature  is 
then  allowed  to  fall  very  slowly  and  an  observation  made,  while  the 
tube  is  constantly  agitated,  of  the  temperature  of  first  appearance 
of  opalescence.  This  observation  can  be  repeated  as  many  times  as 
desired  and  the  temperatures  of  appearance  and  disappearance  of 
the  clouding,  which  usually  differ  by  only  a  few  tenths  of  a  degree, 
can  be  ascertained  with  certainty. 

Since,  by  the  synthetic  method  the  data  are  for  irregular  intervals 
of  temperature,  in  order  to  obtain  results  for  a  particular  tem- 
perature it  is  necessary  to  plot  the  several  determinations  on  coordi- 
nate paper  and  from  the  solubility  curve  so  obtained,  read  the  value 
for  the  temperature  in  question. 

Freezing-point  Method.  —  A  modification  of  the  synthetic  method, 
which  is  applicable  particularly  to  solutions  which  contain  relatively 
large  amounts  of  the  dissolved  compound,  is  that  which  consists  in  a 
determination  of  the  freezing-point  of  the  mixture.  This  point  is, 
in  fact,  the  temperature  at  which  the  separating  solid  compound  is 
in  equilibrium  with  the  solution. 

The  difference  between  the  freezing-point  determination  and  the 
observation  of  the  point  of  growth  or  diminution  of  a  crystal  in  a 

774 


METHODS   FOR  THE  DETERMINATION  OF   SOLUBILITY 

liquid  is  that,  in  the  former,  the  establishment  of  equilibrium  is 
recognized  exclusively  by  the  change  of  the  thermometer.  The 
solution  is  cooled  gradually,  during  which  the  thermometer  sinks 
slowly  to  a  point  below  the  freezing  temperature.  As  soon  as  the 
first  crystal  appears,  either  spontaneously  or  by  intentional  intro- 
duction (seeding),  the  thermometer  rises  suddenly  to  the  freezing- 
point  and  remains  stationary  for  some  time. 

This  method  can,  of  course,  be  used  in  a  large  number  of  cases  for 
the  determination  of  solubility.  Those  portions  of  the  solubility 
curves  of  salts  in  water  for  which  ice  is  the  solid  phase,  are  practi- 
cally always  determined  in  this  way  and  it  may  be  said,  in  general, 
that  for  determinations  made  at  low  temperatures,  the  freezing-point 
method  is  to  be  selected  whenever  possible. 

For  the  practical  execution  of  the  method  the  very  well  known 
apparatus  of  Beckmann  is  most  convenient  and  satisfactory.  The 
determinations  must,  of  course,  be  made  with  all  the  refinements 
which  have  been  developed  for  accurate  freezing-point  measure- 
ments. 

The  method  has  been  used  extensively  for  the  discovery  of 
addition  compounds.  Its  use  for  this  purpose  is  based  upon  the 
principle  that  if  to  a  pure  compound,  A,  a  second,  B,  is  added,  the 
freezing-point  of  A  is  lowered;  similarly  the  freezing-point  of  B  is 
lowered  by  A,  and  the  two  descending  curves  thus  obtained  inter- 
sect at  the  eutectic.  If,  however,  a  compound,  AxBy  is  formed, 
this  also  acts  as  a  pure  substance  and  its  freezing-point  is  lowered 
by  either  A  or  B.  Hence  the  freezing-point  lines  do  not  meet  at  a 
single  eutectic  but  exhibit  in  this  case  a  maximum,  the  position  of 
which  indicates  the  composition  of  the  compound. 

Volume  Change  Method.  —  Still  another  method,  which  is  a  modi- 
fication of  the  synthetic,  is  that  designed  to  indicate  the  reciprocal 
solubility  of  liquids  by  a  determination  of  the  volume  changes  which 
occur  when  two  relatively  sparingly  miscible  liquids  are  shaken 
together  in  a  closed  vessel.  The  apparatus  consists  usually  of  a 
cylindrical  receptacle  which  is  provided  with  a  constricted  grad- 
uated section  either  at  one  end  or  near  the  middle.  Such  volumes  of 
liquids  are  chosen  that  the  meniscus  separating  them  lies  in  the 
constricted  graduated  tube.  The  determination  consists  in  super- 
imposing measured  volumes  of  each  liquid  and  noting  the  position 
of  the  meniscus  before  and  after  a  period  of  shaking  at  constant 
temperature.  From  the  increase  or  decrease  of  volume  of  the  two 
layers,  as  estimated  from  the  change  in  position  of  the  meniscus, 
the  reciprocal  solubility  of  the  two  liquids  is  calculated.  It  is  to  be 

775 


METHODS   FOR  THE   DETERMINATION   OF   SOLUBILITY 

noted,  however,  that  the  solubility  of  liquids  is  in  practically  all 
cases  reciprocal,  and  without  an  analysis  of  the  two  layers  the  true 
solubility  can  not  usually  be  deduced. 

Titmtion  Method.  —  A  special  case  of  the  reciprocal  solubility  of 
liquids  is  that  representing  equilibrium  in  ternary  systems  yielding 
two  liquid  layers.  Such  equilibria  are  usually  determined  by  rel- 
atively simple  titration  procedures,  but  for  the  interpretation  and 
description  of  the  results,  special  terms  have  been  developed  and 
these  require  more  or  less  detailed  explanation. 

When  a  third  liquid  is  added  to  a  mixture  of  two  others  which  are 
miscible  to  only  a  slight  extent,,  the  added  liquid,  if  soluble  in  each 
of  the  others,  will  distribute  itself  between  the  two  and  an  equi- 
librium will  be  reached.  If  the  two  layers  are  then  analyzed  and 
the  results  plotted  on  coordinate  paper,  two  points,  corresponding 
to  the  two  layers,  will  be  obtained.  If  more  of  the  third  liquid  is 
added,  equilibrium  will  again  be  established  after  a  short  period  of 
shaking  and  the  analysis  of  the  two  layers,  to  which  the  designation 
conjugate  layers  has  been  given,  will  fix  two  more  points  when  plotted 
on  the  coordinate  paper.  The  process  may  be  repeated  until  a 
considerable  number  of  points  have  been  obtained.  When  this  has 
been  done,  it  will  always  be  found  that  these  points  are  the  locus  of  a 
smooth  curve,  to  which  the  designation  binodal  curve  has  been  given. 
If  the  pairs  of  points  corresponding  to  the  conjugate  layers  are 
connected,  the  lines  so  obtained  are  defined  as  tie  lines.  Since  it  is 
evident  that  with  the  continued  addition  of  the  third  or  consolute 
liquid,  a  point  must  finally  be  reached  at  which  the  resulting  mixture 
will  no  longer  separate  into  two  conjugate  layers,  the  tie  lines  suc- 
cessively determined  as  above  described,  will  become  shorter  and 
shorter  until  finally  the  last  one  is  reduced  to  the  point  correspond- 
ing to  the  homogeneous  mixture  of  the  three  components.  To  this 
is  given  the  name  plait  point. 

Although  for  the  above  example  a  ternary  system  made  up  of 
three  liquids  has  been  taken,  there  are  a  large  number  of  salts  and 
other  solid  compounds  which,  when  dissolved  in  mixtures  of  liquids 
of  certain  concentrations,  cause  the  latter  to  separate  into  conjugate 
liquid  layers.  These  systems  have  aroused  much  interest  from  time 
to  time  and  considerable  data  for  them  are  given  in  the  literature. 

Since  it  is  usually  difficult  and  frequently  impossible  to  analyze 
directly  a  homogeneous  mixture  of  liquids,  and  thus  determine  the 
points  on  a  binodal  curve,  a  simple  titration  method  for  this  purpose 
has  come  into  general  use.  By  means  of  this  a  homogeneous 
mixture  of  known  amounts  of  two  of  the  components  is  titrated  with 


METHODS   FOR  THE  DETERMINATION   OF  SOLUBILITY 

the  third  just  to  the  point  of  initial  separation  of  the  second 
layer,  which  is  usually  very  sharply  indicated  by  the  appearance  of 
clouding  or  opalescence.  The  procedure  may  also  be  reversed  and 
the  consolute  liquid  added  just  to  the  point  of  clearing  of  the  cloudy 
mixture  of  the  other  two.  By  this  plan  the  synthetically  derived 
composition  of  one  of  the  two  conjugate  layers  and  thus  of  one  point 
on  the  binodal  curve  is  known.  The  determination  of  the  tie  line 
and  therefore,  the  identification  of  the  corresponding  point  on  the 
curve  for  the  conjugate  liquid,  requires  an  additional  experiment 
for  its  location.  Several  procedures  for  this  purpose  have  been  de- 
veloped. They  usually  depend  upon  the  determination  of  one  or 
more  constants  of  specially  prepared  pairs  of  conjugated  liquids, 
such  as  their  specific  gravities  or  refractive  indices.  In  the  case 
of  mixtures  of  which  one  member  can  be  easily  determined  analyti- 
cally, tie  lines  can  be  located  by  the  quantitative  determination  of 
this  member  in  pairs  of  conjugated  liquids. 

In  general,  the  titration  method  for  the  determination  of  the 
solubility  of  liquids  is  applicable  to  many  cases.  The  facts,  that 
equilibrium  is  attained  so  promptly  in  liquids  and  that  the  evidence 
of  the  appearance  of  a  second  insoluble  layer  is  usually  so  striking, 
make  it  of  great  value.  Refinements  have  been  introduced  such 
as  the  addition  of  liquid  or  solid  dyes  to  the  mixture  in  order  to 
facilitate  the  detection  of  the  end  point,  and  the  development  of 
particular  forms  of  apparatus  for  measuring  and  weighing  the 
liquids.  The  constituents  of  the  mixtures  are  usually  weighed  but 
the  volume  relations  and,  therefore,  the  specific  gravities  can  also 
be  approximately  estimated,  by  using  graduated  vessels  for  making 
the  titrations,  and  measuring  in  them  the  volumes  of  the  final 
mixtures.  A  very  ingenious  method  for  ascertaining  indirectly  the 
composition  of  the  liquid  mixtures  in  the  case  of  the  system 
naphthalene,  acetone  and  water,  is  described  on  p.  444. 

As  a  usual  thing  the  temperature  coefficients  are  not  very  great 
in  the  case  of  liquid  mixtures  and  the  very  accurate  control  of  the 
temperature  is  not  imperative.  When  such  control  is  necessary, 
however,  the  use  of  a  thermostat  does  not  seriously  complicate  the 
determination. 

Distribution  Coefficients.  —  As  mentioned  above,  when  a  third 
compound  is  added  to  a  mixture  of  two  liquids  which  are  relatively 
immiscible,  it  will  dissolve  to  a  certain  extent  in  each  and  the  com- 
position of  the  two  layers  represent  conjugate  points  on  the  binodal 
curve  for  the  system.  The  results  are,  however,  of  interest  from 
another  point  of  view,  namely  that  of  the  distribution  of  the  com- 

777 


METHODS   FOR   THE   DETERMINATION   OF   SOLUBILITY 

pound  between  the  two  solvents.  This  distribution  coefficient  is, 
in  many  cases,  of  considerable  interest  in  connection  with  analytical 
methods  based  on  shaking  out  procedures  and  also  in  connection 
with  such  problems  as  the  molecular  state  of  compounds  in  solution, 
their  dissociation  and  other  points  of  theoretical  interest.  Distri- 
bution coefficients  have,  therefore,  been  studied  to  a  large  extent 
and  much  data  for  them  are  available.  In  general,  the  determina- 
tions are  made  by  relatively  simple  methods.  The  amount  of  the 
compound  present  in  a  definite  amount  of  each  layer,  after  equi- 
librium has  been  established  by  adequate  agitation,  is  determined 
in  any  manner  most  convenient.  If  the  total  amount  of  solute  is 
known,  and  that  found  in  one  layer,  the  amount  in  the  other  can,  of 
course,  be  calculated  by  difference.  The  results  are  usually  ex- 
pressed on  the  volume  basis,  since  it  is  the  ratio  of  the  amounts 
present  in  the  same  molecular  state  in  equal  volumes  of  the  two 
layers  which  is  a  constant,  independent  of  temperature  and  con- 
centration. 

It  is  evident  that  when  the  concentration  at  the  saturation  point 
is  considered,  the  amount  of  the  compound  which  enters  each  layer 
depends  upon  its  solubility  in  the  liquid,  consequently  the  dis- 
tribution coefficient  is  the  relation  of  the  solubilities  of  the  dissolved 
substance  in  the  two  solvents.  Variations  from  this,  aside  from 
changes  in  molecular  state,  etc.,  in  one  or  the  other  solvent  are  due 
to  such  causes  as  the  reciprocal  solubility  of  the  so-called  immiscible 
solvents,  which  will,  of  course,  be  influenced  by  the  presence  of  the 
dissolved  compound,  especially  at  the  higher  concentrations.  Vari- 
ations of  the  coefficient  with  temperature  would  result  in  cases 
where  the  solubilities  of  the  compound  in  the  two  solvents  do  not 
change  at  the  same  rate  with  temperature. 

Electrolytic  Conductivity  Method.  —  Of  the  physical  properties 
which  can  be  used  for  the  determination  of  the  concentration  of  a 
solution,  such  as  specific  gravity,  refractive  index,  etc.,  the  electro- 
lytic conductivity  is  of  particular  value  in  the  case  of  those  very 
sparingly  soluble  compounds  which  yield  solutions  too  dilute  to  be 
analyzed  by  gravimetric  or  volumetric  methods.  By  its  use  the 
progress  of  the  saturation  can  be  followed  without  separating  the 
undissolved  solid  from  the  solution,  or  even  removing  the  portion 
used  for  the  determination.  The  special  electrical  equipment 
which  is  required,  however,  and  the  need  for  water  of  exceptional 
purity  and  of  vessels  of  particular  qualities,  restrict  its  general  use. 

The  method  of  calculating  the  concentration  from  the  conduc- 
tivity is  based  on  the  assumption  that  at  the  very  great  dilutions 

778 


METHODS   FOR   THE  DETERMINATION   OF   SOLUBILITY 

involved,  complete  dissociation  occurs.  Therefore,  the  limiting 
value  to  which  the  equivalent  conductivity  approaches  at  infinite 
dilution  is,  for  practical  purposes,  attained,  and  A  =  A*>  =  la  +  /*, 
where  la  and  4  are  the  ionic  conductivities  of  the  anions  and  kations. 
These  values  are  known  for  all  the  principally  occurring  ions.  The 
observed  specific  conductivity  K  is,  however,  connected  with  the 
equivalent  conductivity  and  the  concentration  t\  by  the  equation 

A  =  -,  in  which  77  represents  the  concentration  in  gram-equivalents 

V 
per    cubic    centimeter.      Rearrangement    and    substitution    give 

TJ  =  j — r— T-  .     From  this  equation  the  solubility  of  the  substance 

I'a  T  i'k 

under  investigation  is  calculated  by  substituting  the  measured 
specific  conductivity  of  the  solution  and  the  known  values  of  the 
ionic  conductivities. 

The  Solubility  of  Gases  in  Liquids.  —  When  a  gas  and  a  liquid  are 
intimately  mixed  by  shaking,  a  definite  amount  of  the  gas  will  be 
dissolved  by  the  liquid  and,  simultaneously,  the  vapor  of  the  liquid 
will  mix  with  the  gas  in  the  space  above  the  liquid.  The  partial 
pressure  of  the  liquid  in  the  gas  space  is  almost  exactly  the  same  as 
that  of  the  pure  liquid  at  the  solution  temperature,  since  the  in- 
fluence of  the  relatively  slight  amount  of  dissolved  gas  is  insignifi- 
cant in  by  far  the  most  cases.  The  amount  of  gas  which  is  dissolved 
depends  both  on  the  nature  of  the  gas  and  of  the  liquid  and  is, 
furthermore,  a  function  of  the  temperature,  and  pressure. 

In  regard  to  the  influence  of  pressure,  the  absorption  law  of  Henry 
holds  for  the  most  part,  when  the  gas  solubility  is  not  too  great. 
According  to  it,  the  amount  of  pure  gas,  which  is  taken  up  at  con- 
stant temperature  by  a  given  amount  of  liquid  is  proportional  to 
the  pressure  of  the  gas. 

The  temperature  acts  almost  always  in  the  sense  that  the  solu- 
bility decreases  as  the  temperature  rises. 

The  solubilities  of  gases  are  usually  expressed  either  in  terms  of 
the  Bunsen  "Absorption  Coefficient"  /3,  or  the  Ostwald  "Solubility 
Expression"  /.  Definitions  of  these  are  given  on  p.  227. 

The  experimental  methods  for  the  determination  of  the  solubility 
of  gases  vary  according  to  the  nature  of  the  gas.  For  those  which 
dissolve  in  relatively  large  amounts  and  can  be  analytically  deter- 
mined with  accuracy,  the  saturated  solution  may  be  analyzed  by 
ordinary  quantitative  methods.  Thus,  in  the  case  of  the  solubility 
of  sulfur  dioxide  in  aqueous  solutions  of  salts  (see  p.  706,  results  by 
Fox,  1902),  the  solutions  were  saturated  by  passing  a  stream  of  the 

779 


METHODS   FOR   THE   DETERMINATION   OF   SOLUBILITY 

gas  through  them  at  atmospheric  pressure  and,  when  equilibrium 
was  attained,  a  measured  portion  of  the  solution  was  withdrawn, 
transferred  to  an  excess  of  standardized  iodine  solution  and  the 
excess  of  the  latter  titrated  with  thiosulfate.  A  gravimetric  pro- 
cedure was  used  by  Christoff  (1905)  for  the  determination  of  the 
solubility  of  carbon  dioxide  in  aqueous  salt  solutions.  In  this  case 
the  solutions  were  weighed  before  and  after  the  passage  of  the  gas 
through  them  and  the  increase  in  weight,  after  applying  necessary 
corrections,  taken  to  represent  the  solubility  at  the  temperature  of 
the  experiment  and  at  atmospheric  pressure.  The  absorption  flasks 
were  of  special  shape  and  the  gas  was  previously  passed  through  a 
series  of  U  tubes,  containing  the  same  aqueous  solution,  in  order 
to  prevent  loss  of  water  from  the  experimental  solution  which, 
otherwise,  would  have  occurred. 

In  the  great  majority  of  cases,  however,  gas  solubility  is  deter- 
mined by  a  method  based  upon  the  measurement  of  the  volume  of 
the  gas  absorbed.  The  apparatus  consists  essentially  of  an  absorp- 
tion flask  for  the  liquid,  connected  by  means  of  a  tube  of  small  bore 
to  a  graduated  buret  in  which  the  gas  is  measured  above  mercury, 
the  level  of  which  can  be  altered  by  raising  or  lowering  a  container 
connected  with  the  buret  by  means  of  a  rubber  tube.  Many  forms 
of  this  apparatus  have  been  described  and  the  disadvantages  of  the 
earlier  forms  have  gradually  been  remedied.  A  relatively  simple 
form  of  this  apparatus,  but  one  which  embodies  the  essential 
features  required  for  accuracy,  is  that  described  by  McDaniel  (1911) 
for  the  determination  of  the  solubility  of  methane,  ethane  and 
ethylene  in  a  large  number  of  organic  solvents  at  various  tem- 
peratures. 

This  apparatus  is  shown  in  Fig.  13.  A  is  an  ordinary  gas  buret 
and  B  an  absorption  pipet  of  the  form  first  used  by  Ostwald.  "The 
buret  and  pipet  are  connected  by  means  of  the  glass  capillary  M 
sealed  directly  onto  each,  so  that  the  whole  forms  one  solid  piece 
of  glass  apparatus  without  rubber  or  cement  connections  of  any  kind; 
thus  any  possibility  of  leaks  from  these  extremely  troublesome 
sources  is  entirely  avoided.  The  whole  apparatus  is  clamped 
solidly  to  a  rigid  support  so  that  it  can  be  taken  up  in  the  hands 
and  shaken  for  the  purpose  of  bringing  the  gas  into  intimate  contact 
with  the  liquid.  The  pipet  and  buret  are  each  provided  with  a 
three-way  stopcock,  C  and  D.  These  can  be  turned  in  such  a  way 
as  to  allow  the  gas  to  sweep  out  the  air  from  the  connecting  capillary. 
By  the  same  means  the  two  vessels  may  also  be  connected  directly 
with  each  other  as  well  as  separately  with  the  outside  air  or  source 


IETHODS   FOR   THE  DETERMINATION   OF   SOLUBILITY 


of  gas  supply.  The  pipet  and  buret  are  each  provided  with  a  water 
jacket,  P  and  Q.  The  temperature  of  each  is  regulated  by  means 
of  the  electrically  heated  coils  K  and  L."  These  coils  are  of 
manganin  wire  and  are  connected  in  series.  The  rate  of  evolution 
of  heat  in  the  jackets  was  adjusted  in  the  first  place  by  varying  the 
length  of  the  manganin  wire,  until  the  temperature  was  the  same  in 
each  jacket.  Stirring  was  accomplished  by  blowing  air  through 
the  tubes  I  and  /.  The  differences  in  temperature  between  the 
pipet  and  buret  were  never  greater  than  0.1°. 


T 


M 


B 


FIG.  13. 


FIG.  14. 


In  carrying  out  a  determination  by  this  method  it  is,  of  course, 
necessary  that  the  solvent  be  completely  free  of  dissolved  air  or 
other  gas.  This  is  perhaps  the  most  important  part  of  the  deter- 
mination and  a  special  form  of  apparatus  for  the  purpose  is  described 
by  McDaniel  (1911)  and  is  shown  in  Fig.  14.  "The  liquid  was 
boiled  under  diminished  pressure  in  the  flask  C  attached  directly 

781 


METHODS  FOR  THE  DETERMINATION   OF   SOLUBILITY 

to  the  lower  opening  of  the  pipet  by  means  of  the  rubber  stopper  as 
shown  in  the  figure.  Connection  with  the  air  pump  is  made  at  D. 
During  the  boiling  the  lower  opening  of  the  inlet  tube  E  is  above  the 
surface  of  the  liquid  in  C,  the  stopcock  B  being  closed.  When  the 
air  has  been  completely  expelled,  the  screw  pinchcock  F  is  closed 
while  the  air  pump  is  still  in  operation.  The  flask  C  is  now  raised 
until  the  lower  end  of  E  reaches  nearly  to  the  bottom  of  the  flask. 
The  air  pump  is  now  connected  at  G  and  the  cock  H  opened  so  as 
to  make  connection  with  the  pipet.  B  is  now  opened  and  the  inflow 
of  air  through  D  regulated  by  gradually  opening  F  in  such  a  manner 
that  the  liquid  is  very  slowly  forced  up  into  the  pipet.  In  this 
manner  the  liquid  never  comes  into  contact  with  the  air  under  full 
atmospheric  pressure  but  only  under  greatly  diminished  pressure. 
The  absorption  of  air  under  these  conditions  can  only  be  inappre- 
ciable, especially  since  the  liquid  in  the  flask  remains  perfectly  quiet, 
and  only  the  lower  portion  is  used." 

Having  filled  the  pipet  B,  Fig.  13,  with  the  air-free  solvent  as 
just  described,  "T  is  connected  with  the  source  of  gas  supply  and 
the  cocks  C  and  D  are  turned  in  such  a  way  as  to  allow  the  gas  to 
sweep  out  the  air  from  the  capillary,  M.  The  buret  is  then  filled 
in  the  usual  manner  by  lowering  the  leveling  tube  F,  the  cock  D 
having  been  turned  so  as  to  connect  T  with  E.  Care  is  taken  to 
keep  the  entering  gas  under  a  slight  pressure  by  keeping  the  mercury 
level  in  F  slightly  above  that  in  A .  This  prevents  air  from  entering 
through  any  leaks  in  the  train  connecting  the  gas  generator  with  the 
buret."  The  gas  must  be  completely  saturated  with  the  vapor  of 
the  solvent  and  this,  with  other  than  aqueous  solvents,  may  require, 
in  addition  to  drawing  it  through  some  of  the  solvent  in  H,  that  a 
thin  layer  be  placed  in  the  buret  and  time  allowed  for  it  to  saturate 
the  gas  sample. 

"After  again  allowing  the  current  of  gas  to  flow  through  the 
capillary  M  for  a  short  time  the  buret  and  pipet  are  connected  with 
each  other  by  turning  the  three-way  cocks  D  and  C  in  the  proper 
direction.  The  determination  of  the  amount  of  absorption  is  then 
made  as  follows:  A  portion  of  the  gas  is  passed  into  the  pipet  by 
raising  F  and  opening  G,  the  displaced  liquid  being  caught  in  a 
graduated  cylinder.  The  cock  C  is  closed  and  the  gas  and  liquid  in 
the  pipet  brought  into  intimate  contact  with  each  other  by  shaking 
the  whole  apparatus.  C  is  now  opened  to  allow  gas  to  enter  from 
the  buret  to  replace  that  absorbed.  This  process  is  repeated  until, 
on  opening  C,  there  is  no  further  decrease  in  the  volume  of  gas  in  A. 
The  volume  absorbed  is  found  by  subtracting  from  the  original 

782 


METHODS   FOR  THE  DETERMINATION   OF   SOLUBILITY 

volume  of  gas,  the  volume  remaining  in  the  buret  plus  the  volume 
in  the  pipet.  The  volume  of  gas  in  the  pipet  is  equal  to  the  volume 
of  liquid  drawn  off.  The  volume  of  liquid  remaining  is  easily 
calculated  from  the  known  volume  of  the  pipet.  The  absorption 
coefficient  or  '  solubility '  is  the  ratio  of  the  volume  of  gas  absorbed , 
measured  at  the  temperature  of  the  experiment,  to  the  volume  of 
the  saturated  liquid.  It  may  be  reduced  to  the  coefficient  used  by 
Bunsen  by  dividing  by  (i  +  a/)." 

In  the  case  of  the  majority  of  investigators  who  have  used  this 
method,  particularly  for  determinations  at  high  or  low  tempera- 
tures, the  absorption  pipet  has  been  kept  at  the  temperature  of  the 
experiment  and  the  gas  measuring  buret  at  room  temperature,  the 
two  being  connected  by  means  of  a  flexible  capillary  which  permits 
the  absorption  pipet  to  be  independently  shaken.  This  arrange- 
ment makes  it  necessary,  in  calculating  the  absorption  coefficients, 
to  apply  the  usual  corrections  for  temperature  and  vapor  pressure 
to  the  volume  of  gas  in  the  buret.  This  is  a  complication  which  in 
some  cases  causes  uncertainties  in  regard  to  the  accuracy  of  the 
results  as  finally  calculated. 

A  somewhat  more  elaborate  form  of  apparatus  than  that  just 
described  was  developed  by  Drucker  and  Moles  (1910)  for  determi- 
nations in  cases  where  the  solubility  is  very  small.  These  authors 
give  results  for  hydrogen  and  nitrogen  in  aqueous  solutions  of 
glycerol.  The  particular  feature  of  the  apparatus  is  that  only  about 
one-tenth  the  usual  amount  of  solvent  is  employed  and  solubilities 
as  low  as  only  one-tenth  that  of  nitrogen  in  water  at  25°  can  be 
measured. 

An  apparatus  designed  for  determinations  at  very  high  pressures, 
using  a  Caillet  compression  tube,  is  described  by  Sander  (1911-12). 
It  was  used  for  determination  of  the  solubility  of  carbon  dioxide  in 
water,  alcohols,  and  other  organic  solvents.  The  principle  involved 
TS  that  the  pure  gas  is  first  compressed  above  mercury  in  a  graduated 
tube  and  the  volumes  corresponding  to  given  pressures  noted.  Simi- 
lar readings  are  then  taken  for  the  same  gas  after  a  small  accurately 
measured  amount  of  solvent  has  been  introduced  into  the  graduated 
tube.  The  difference  between  the  two  volumes  at  the  same  tem- 
perature and  pressure,  reduced  to  I  kg.  per  sq.  cm.  and  I  cc.  of 
liquid,  represents  the  solubility  of  the  gas  in  the  given  solvent. 

Finally,  attention  should  be  called  to  the  method  of  determination 
of  gas  solubility  based  on  the  principle  that,  for  volatile  solutes 
which  obey  the  laws  of  Dalton  and  Henry,  the  amount  which  is 
carried  away  by  an  inert  gas  when  known  volumes  are  bubbled 

783 


METHODS   FOR   THE   DETERMINATION   OF   SOLUBILITY 

through  solutions  of  known  strength  of  volatile  solute,  can  be  used 
to  measure  the  comparative  solubilities  in  solvents  of  different  con- 
centrations. An  example  of  this  method  is  the  determination  of 
the  solubility  of  ammonia  in  aqueous  salt  solutions  by  Abegg  and 
Riesenfeld  (1902).  The  very  ingenious  apparatus  consists  of  a 
generator  for  developing  a  stream  of  H2  +  O2  from  aqueous  NaOH, 
by  means  of  an  electric  current  measured  with  the  aid  of  a  copper 
voltmeter,  and  the  volume  of  gas  thus  determined.  This  was  passed 
through  a  spiral  in  the  vessel  containing  the  ammonia  solution  of 
known  concentration.  The  mixed  gases  passing  out  of  this  were 
received  in  a  third  vessel  containing  5  cc.  of  o.oi  n  HC1.  Electrodes 
were  provided  in  this' vessel  and,  by  means  of  conductivity  measure- 
ments, the  point  determined  at  which  all  of  the  HC1  became  satu- 
rated with  NH3.  Since  the  volume  of  the  H2  +  O2  required  for  this 
purpose  was  known,  the  partial  pressure  of  the  NH.s  in  the  mixture 
could  be  directly  ascertained.  Comparative  determinations  of  the 
vapor  pressure  of  the  ammonia  in  water  and  a  series  of  salt  solutions 
made  in  this  way  were  calculated  to  ammonia  solubilities  on  the 
basis  of  the  relation  that,  for  two  solutions  of  equal  ammonia  con- 
tent, the  ammonia  pressure  is  reciprocally  proportional  to  the  solu- 
bility of  the  ammonia  in  them. 


784 


AUTHOR  INDEX 


Abbott,  G.  A.  and  Bray,  W.  C. 

(1909)  J.Am.Chem.Soc.,  31,  729-763- 
Abe,  Ryuji. 

(1911)  Mem.Coll.Sci.Eng.  (Kyoto), 
3,  212. 

(1911)  J.Tok.Chem.Soc.,  32,  980. 
(1911-12)    Mem.Coll.Sci.Eng. 

(Kyoto),  3,  13. 

(1912)  J.Tok.Chem.Soc.,  33,  1087. 
Abegg,  R. 

(1903)  Z.Elektrochem.,  9,  550. 
Abegg,  R.  and  Cox,  A.  J. 

(1903)  Z.physik.Chem.,  46,  n. 
Abegg,  R.  and  Pick,  H. 

(1905)  Ber.,  38,  2573. 

(1906)  Z.anorg.Chem.,  51,  I. 
Abegg,  R.  and  Riesenfeld,  H. 

(1902)  Z.physik.Chem.,  40,  84. 
Abegg,  R.  and  Sherrill,  M.  S. 

Z.Elektrochem.,  9,  550. 
Abegg,  R.  and  Spencer. 

(1905)  Z.anorg.Chem.,  46,  406. 
Acree,  S.  F.  and  Slagle,  E.  A. 

(1909)  Am.Chem.Jour.,  42,  135. 
Adrian!,  J.  H. 

(1900)  Z.physik.Chem.,  33,  453-476. 
Ageno,  F.  and  Valla,  E. 

(1911)  Atti  accad.Lincei,  20,  II,  706. 

(1912)  ist.Ven.[VIII],  14,  II,  331. 

(1913)  Gazz.chim.ital.,  43,  II,  168. 
d'Agostino,  E. 

(1910)  Rend. soc.chim.ital. (Roma),  2, 

II,  171. 
Aignan,  A.  and  Dugas,  E. 

(1899)  Compt.rend.,  129,  643. 


Alexejew,  Wladimir.     (Alexejeff.) 
(i886)Wied.Ann.Physik.,28,305,338. 

Allen,  E.  T.  and  White,  W.  P. 
(1909)  Am.Jour.Sci.[4],  27,  I. 

Altschul. 

(1896)  Monatsh.Chem.,  17,  575. 

Alluard. 

(1864)  Compt.rend.,  59,  500. 

(1865)  Liebig's  Ann.,  133,  292. 
Amadori,  M. 

(1912)  Atti  accad.Lincei,  21,  II,  67, 

184,  769,  690. 

(i9i2a)  Atti  accad.Lincei,  21,  I,  467, 
667-73. 

(1913)  Atti  accad.Lincei,  22,  I,  453, 

609;  22,  II,  333. 

(1915)  Atti  accad.Lincei,  24,  II,  204. 
Amadori,  M.  and  Becarelli,  R. 

(1912)  Atti  accad.Lincei,  21,  II,  698. 
Amadori,  M.  and  Pampanini,  G. 

(1911)  Atti  accad.Lincei,  20,  II,  475, 

572. 
Amat,  L. 

(1887)  Compt.rend.,  105,  809. 
Anderson. 

(1888-89)  Proc.Roy.Soc.(Edin.),  16, 

319. 
Andrae. 

(1884)  J.prakt.Chem.  [2],  29,  456. 
Andrews,  L.  W.  and  Ende,  C. 

(1895)  Z.physik.Chem.,  17,  136. 
Anon. 

(1903)  Bull.soc.pharm.    (Bordeaux), 

p.  7. 

(1904)  Pharm.Jour.(Lond.),  72,  77. 


1  The  abbreviations  of  the  names  of  the  journals  referred  to  in  this  index  agree, 
for  the  most  part,  with  those  adopted  for  Chemical  Abstracts.  They  will,  there- 
fore, be  readily  understood  in  all  but  a  few  cases.  One  abbreviation  which  differs 
from  that  used  in  Chemical  Abstracts  is  Proc.  k.  Akad.  Wet.  (Amst.)  instead  of 
Proc.  Acad.  Sci.  Amsterdam.  It  refers  to  the  English  edition  of  Verslag  koninkl 
ke  Akademie  van  Wetenschappen  te  Amsterdam. 

Another  abbreviation  which  has  been  adopted  for  the  present  index  is  the  use 
of  "Tables  arinuelles  "  for  the  French  title,  Tables  annuelles  de  Constantes  et 
Donnees  Numerique  de  Chemie,  de  Physique  et  de  Technologic,  of  the  Interna- 
tional Tables  of  Constants  and  Numerical  Data  published  in  Paris  under  the 
direction  of  the  general  secretary,  Professor  Marie.  Of  the  three  volumes  which 
have  been  published,  Vol.  I  contains  data  for  the  year  1910  and  was  issued  in 
1912;  Vol.  2  is  for  the  year  1911  and  appeared  in  1913;  and  Vol.  3  contains  data 
for  1912  and  was  issued  in  1914. 

785 


AUTHOR   INDEX 


Anthony,  C.  G. 

(1916)    Bonfort's   Wine   and    Spirit 

Circular,  Apr.  loth, 
von  Antropoff,  A. 

(1909-10)      Proc.Roy.Soc.  (London), 

A  83,  474-83. 

Armstrong,  H.  E.  and  Eyre,  J.  V. 
(1910-11)      Proc.  Roy.  Soc.  (London), 

(A),  84,  123-135. 
(1913)   Proc. Roy. Soc. (London),  (A), 

88,  234. 

Armstrong,  H.  E.,  Eyre,  J.  V.,  Hussey, 
A.  V.,  and  Paddison,  W.  P. 

(1907)  Proc. Roy. Soc. (London),  (A), 

79i  564-576. 
Ange,  see  Auge. 
d'Ans,  see  D'Ans. 
d'Anselme. 

(1903)  Bull.soc.chim.  [3],  29,  372. 
Archibald,  E.  H.,  Wilcox,  W.  G.  and 

Buckley,  B.  G. 

(1908)  J.Am.Chem.Soc.,  30,  747-60. 
Arctowski,  H. 

(1894)  Z.anorg.Chem.,  6,  267,  404. 

(1895)  Compt.rend.,  121,  123. 
(1895-6)  Z.anorg.Chem.,  n,  272-4. 

Armit,  H.  W. 

(1907)  Jour.Hygiene,  7,  525-51. 
Arndt,  K. 

(1907)  Ber.,  40,  427. 
Arndt,  K.  and  Loewenstein,  W. 

(1909)  Z.Elektrochem.,  15,  784-90. 
Arrhenius,  S. 

(1893)  Z.physik.Chem.,  n,  396. 
Arth,  G.  and  Cretien. 

(1906)  Bull.soc.chim.  [3],  35,  778. 
Artmann,  P. 

£1912-13)  Z.anorg.Chem.,  79,  333. 

(1915)  Z.anal.Chem.,  54,  90. 
Aschan,  Ossian. 

(1913)  Chem.Ztg.,  37,  1117. 
AssBlin,  E. 

(1873)  Compt.rend.,  76,  884. 

(1873)  Jahresber.Chem.,  1063. 
Aten,  A.  H.  W. 

(1905)  Z.anorg.Chem.,  47,  387. 

(1905-06)    Z.physik.Chem.,    54,    86, 
124. 

(1909)  Z.physik.Chem.,  68,  41. 

(1912)  Proc.k.Akad.Wet.  (Amst.),  15, 

(1912-13)  Z.physik.Chem.,  81,  268. 

(1913)  Z.physik.Chem.,  83,  443. 

(1914)  Z.physik.Chem.,  86,  1-35. 
(i9Ha)  Z.physik.Chem.,  88, 321-379. 

Atkins,  W.  R.  G.  and  Werner,  E.  A. 

(1912)  J.Chem.Soc.(Lond.),  101,1167. 
Aubert,  A.  B. 

(1902)  J.Am.Chem.Soc.,  24,  690. 
Auerbach,  F.  § 

(1903)  Z.anorg.Chem.,  37,  353-77. 

(1904)  Z.Elektrochem.,  10,  163. 


Auerbach,  F.  and  Barschall,  H. 

(1908)      Arb.Kais.Gesundheitsamt., 
27,  183-230. 

(1908)  Chem.Abs.,  2,  1125. 
Auge,  E. 

(1890)  Compt.rend.,  no,  1139. 
Bagster,  L.  S. 

(1911)  J.Chem.Soc.(Lond.),  99, 1218. 
Bahr,  F. 

(1911)  Z.anorg.Chem.,  71,  85. 
Bakunin,  M.  and  Angrisani,  T. 

(1915)  Gazz.chim.ital.,  45,  I,  204. 
Ballo,  Rezso. 

(1910)  Z.physik.Chem.,  72,  439. 
Baly. 

(1900)  Phil.Mag.  [5],  49,  517. 
Bancroft,  W.  D. 

(1895)  Phys.  Rev.,  3,  31,  122,  193, 

205. 
Banthisch. 

(1884)  J.prakt.Chem.,  [2],  29,  54. 
Barker,  T.  V. 

(1908)  J.Chem.Soc.(Lond.),  93,  15. 
Barnes,  H.  T. 

(1900)  J.Phys.Chem.,  4,  19. 
Barnes,  H.  T.  and  Scott. 

(1898)  J.Phys.Chem.,  2,  542. 
Baroni,  T.  and  Barlinetto,  V. 

(1911)  Giorn.farm.chim.,  60,  193. 

(1911)  "  Tables  annuelles,"  2,  474. 
Barre,  M. 

(1909)  Compt.rend.,    148,    1604-6; 

149,  292. 

(1910)  Compt.rend.,  150,  1321,  1599; 

151,  871-3. 

(1911)  Ann.chim.phys.,  [8],  24,  149- 

167,  202,  210-223. 

(1912)  Bull.soc.chim.  [4],  n,  646. 
Basch. 

(1901)  Dissertation  (Berlin),  p.  17. 
Baskov,  A. 

(1913)  Jour.Russ.Phys.Chem.Soc., 

45,  1608. 

(1914)  Ann.inst.Electrotechnique 

(Petrograd),  n,  143. 

(1915)  J.Russ.Phys.Chem.Soc.,    47, 

1533-5- 
Bassett,  H.  Jr. 

(1908)  Z.anorg.Chem.,  59,  1-55. 
(1917)      J.Chem.Soc.(Lond.),      in, 

620-42. 
Bassett,  H.  Jr.  and  Taylor,  H.  S. 

(1912)  J.Chem.Soc.(Lond.),  101,  576. 
(1914)      J.Chem.Soc.(Lond.),      105, 

1926-41. 
Bathrick. 

(1896)  J.Phys.Chem.,  I,  159. 
Battelli  and  Martinetti. 

(1885)  Atti     accad.sci.Torino,     20, 

844. 
Baubigny,  H. 

(1908)  Bull.soc.chim.  [4],  3,  772. 
(1908)  Compt.rend.,  146,  1263. 


786 


AUTHOR   INDEX 


Baud,  E. 

(1909)  Bull.soc.chim.  [4],  5,  1022. 

(1909)  Compt.rend.,  148,  96. 

(1912)  Ann.chim.phys.  [8],  27,  95-8. 
(i9i2a)  Bull.soc.chim.  [4],  n,  948. 
(i9i3a)  Compt.rend.,  156,  317. 
(i9i3b)  Ann.chim.phys.  [8],  29,  131- 

136. 
(19130)  Bull.soc.chim.  [4],  13,  436. 

(1913)  Ann.chim.phys.,  [8],  29,  131. 
Baud,  E.  and  Gay,  L. 

(1910)  Compt.rend.,  150,  1688. 

(1911)  Bull.soc.chim.  [4],  9,  119. 
Baum,  Fritz. 

(1899)      Archiv.  exp.Path.u  Pharm., 

42,  119-137- 
Baume,  G. 

(1911)  J.chim.phys.,  9,  245. 

(1914)  J.chim.phys.,  12,  216. 
Baume,  G.  and  Borowski,  W. 

(1914)  J.chim.phys.,  12,  276-81. 
Baume,  G.  and  Georgitses,  N. 

(1912)  Compt.rend.,  154,  650. 
(1914)  J.chim.phys.,  12,  250. 

Baume,  G.  and  Germann,  F.  O. 

(1911)  Compt.rend.,  153,  569. 

(1914)  J.chim.phys.,  12,  242. 
Baume,  G.  and  Pamfil,  G.  P. 

(1911)  Compt.rend.,  ?52>  IO95- 

(1914). J.chim.phys.,  12,  256. 
Baume,  G.  and  Perrot,  F.  L. 

(1911)  Compt.rend.,  152,  1763-5. 

(1914)  J.chim.phys.,  12,  225. 
Baume,  G.  and  Tykociner,  A. 

(1914)  J.chim.phys.,  12,  270-5. 
Baup. 

(1858)  Ann.chim.phys.  [3],  53,  468. 
Baxter,  G.  P.,  Boylston,  A.  C.  and  Hub- 
bard,  R.  A. 

(1906)  J.Am.Chem.Soc.,  28,  1343.     . 
Bechold  and  Ziegler. 

(1910)  Z.angew.Chem.,  23,  29. 
Beck,  K. 

(1904)  Z.physik.Chem.,  48,  657. 
Beck,  K.  and  Stegmiiller,  Ph. 

(1910)  Arb.Kais.Gesundheitsamt., 

34,  447- 

(1911)  Z.Elektrochem.,  17,  843-48. 
Beckmann,  E.  and  Stock,  A. 

(1895)  Z.physik.Chem.,  17,  130. 
Behrend,  R. 

(1892)  Z.physik.Chem.,  10,  265. 

(1893)  Z.physik.Chem.,  u,  466. 
Bell. 

(1867)  Chem.News.,  16,  69. 
Bell,  J.  M. 

(1905)  J.  Phys.  Chem.,  9,  544. 

(1911)  J.Am.Chem.Soc.,  33,  940. 
Bell,  J.  M.  and  Buckley,  M.  L. 

(1912)  J.Am.Chem.Soc.,  34,  10. 
Bell,  J.  M.  and  Taber,  W.  C. 

(1907)  J.Phys.Chem.,  n,  637-8. 

(1908)  J.Phys.Chem.,  12,  174. 


Bellucci,  I. 

(1912)  Atti  accad.Lincei,  [5],  21,  II, 

610. 

(1913)  Gazz.chim.ital.,  43,  I,  521. 
Bellucci,  I.  and  Grassi,  L. 

(1913)  Gazz.chim.ital.,  43,  II,  712. 

(1913)  Atti  accad.Lincei  [5],  22,  II, 

676. 

(1914)  Gazz.chim.ital.,  44,  I,  559. 
Benedicks. 

(1900)  Z.anorg.Chem.,  22,  409. 
Bennett,  R.  R. 

(1912)  Pharm. Jour. (Lond.),  89,  146. 
Bergius,  F. 

(1910)  Z.physik.Chem.,  72,  338-61. 
Berju  and  Kosminiko. 

(1904)  Landw.Vers.Sta.,  60,  422. 
Berkeley,  Earl  of. 

(1904)    Phil.Trans.Roy.Soc.(Lond.), 

203,  A.,  189-215. 
Berkeley,  Earl  of,  and  Appleby,  M.  P. 

(1911)  Proc.Roy.Soc.,  85,  503. 
Bernardis,  G.  B. 

(1912)  Atti  accad.Lincei  [5],  21,  II, 

442. 
Bernfeld. 

(1898)  Z.physik.Chem.,  25,  72. 
Bertheaume,  J. 

(1910)  Compt.rend.,  150,  1064. 
Berthelot,  M. 

(1904)  Ann.chim.phys.  [8],  3,  146. 

(1904)  Compt.rend.,  138,  1649. 
Berthelot,  M.  and  Jungfleisch. 

(1872)  Ann.chim.phys.  [4],  26,  400. 
Bertrand. 

(1868)  Monit.Scient.  [3],  10,  477. 
Beurath,  A. 

(1912-3)  J.prakt.Chem.  [2],  87,  423. 
Bevade,  J.  (Bewad). 

(1884)  Ber.,  17,  R.,  406. 

(1885)  Bull.soc.chim.  [2],  43,  123. 
Bianchini,  G. 

(1914)  Atti  accad.Lincei   [5],   23,   I, 

609. 
Biginelli,  P. 

(1908)  Gazz.chim.ital.,  38,  I,  559-82. 
Billitzer,  J. 

(1902)  Z.physik.Chem.,  40,  535. 
Biltz,  W. 

(1903)  Z.physik.Chem.,  43,  42. 
Biltz,  W.  and  Marcus,  E. 

(1911)  Z.anorg.Chem.,  71,  167. 
Biltz,  W.  and  Wilke. 

(1906)  Z.anorg.Chem.,  48,  299. 
Birger,  Carlson,  see  Carlson,  Birger. 
Biron. 

(1899)  J.Russ.Phys.Chem.Soc.,    31, 

5T7- 
Bissell,  D.  W.  and  James,  C. 

(1916)  J.Am.Chem.Soc.,  38,  873. 
Blanksma,  J.  J. 

(1910)  Chem.Weekblad.,  7,  418. 

(1912)  Chem.Weekblad.,  9, 


787 


AUTHOR  INDEX 


Blanksma,  J.  J. 

(1913)  Chem.Weekblad.,  10,  136. 

(1914)  Chem.Weekblad.,  n,  28. 
Blarez. 

(1891)  Compt.rend.,  112,  434,    939, 

1213. 
Blarez  and  Deniges. 

(1887)  Compt.rend.,  104,  1847. 
Bodlander,  G. 

(1891)  Z.physik.Chem.,  7,  317,  361. 

(1892)  Z.physik.Chem.,  9,  734. 
(1898)  Z.physik.Chem.,  27,  66. 

Bodlander,  G.  and  Eberlein,  W. 

(1903)  Ber.,  36,  3948. 
Bodlander,  G.  and  Fittig,  R. 

(1901-02)  Z.physik.Chem.,  39,  597- 

612. 
Bodlander,  G.  and  Storbeck. 

(1902)  Z.anorg.Chem.,  31,  22,  460. 
Bodtker,  E. 

(1897)  Z.physik.Chem.,  22,  510,  570. 
Boeke,  H.  E. 

(1907)  Z.anorg.Chem.,  50,  335. 

(1911)  NJahr.Min.,  i,  48,  61. 

(1911)  Sitzber.k.Akad.Wiss.  (Berlin), 

24,  632-8. 
Boeseken,  J. 

(1912)  Rec.trav.chim.,  31,  354-360. 
Boeseken,  J.  and  Carriere. 

(1915)  Rec.trav.chim.,  34,  181. 
Boeseken,  J.  and  Waterman,  H. 

(1911)  Verslag.k.Akad.Wet.(Am3t.), 

2<>»  SSS- 

(1912)  Proc.k.Akad.Wet.(Amst.),  14, 

620. 
Boericke,  F. 

(1905)  Z.Elektrochem.,  n,  57. 
Bogdan,  P. 

(1902-3)  Ann. Sci. Univ. Jassy,  2,  47. 

(1905)  Z.Elektrochem.,  n,  825. 

(1906)  Z.Elektrochem.,  12,  490. 
Bogitch,  B. 

(1915)  Compt.rend.,  161,  790-1. 
Bogojawlensky,  A.  and  Winogradow,N. 

(1907)  Z.physik.Chem.,  60,  433. 

(1916)  Sitzber.Natur.Ges. Univ.  Dor- 

pat.,  15,  230-37. 
Bogojawlensky,    A.,   Winogradow,   N. 

and  Bogolubow. 
(1906)  Sitzber.Natur.Ges.  (Dorpat.), 

(1916)  Sitzber.Natur.Ges.  (Dorpat.), 

15,  216-29. 
Bogorodsky. 

(1894)    J.Russ.Phys.Chem.Soc.,    26, 

209. 

(1894)  Chem.Centralbl.,  II,  514. 
Bogousky. 

(1905)     J.Russ.Phys.Chem.Soc.,   37, 

92. 
Bohling. 

(1884)  Z.anal.Chem.,  23,  518. 


Bohr,  C. 

(1899)  Wied.Ann.Physik.    [3],    68, 

50.3- 

(1910)  Z.physik.Chem.,  71,  47-50. 
Bohr,  C.  and  Bock. 

(1891)     Wied.Ann.Physik     [2],     44, 

318. 
Boks. 

(1902)  Dissertation,  Amsterdam. 
Bonner,  W.  D. 

(1910)  J.Phys.Chem.,  14,  738-789. 
Bonsdorff,  W. 

(1904)  Z.anorg.Chem.,  41,  180. 
Bornwater,  J.  T.  and  Holleman,  A.  F. 

(1912)  Rec.trav.chim.,  31,  230. 
Borodowski,  W.  and  Bogojawlenski. 

(1904)    J.Russ.Phys.Chem.Soc.,    36, 

559-6o. 
Botta. 

(1911)  Zentralbl.Min.Geol.,  p.  123. 
Bottger,  W. 

(1903)  Z.physik.Chem.,  46,  521-619. 
(1906)  Z.physik.Chem.,  56,  83-94. 

Boubnoff,  N.  and  Guye,  Ph.  A. 

(1911)  J.chim.phys.,  9,  304. 
Bougault. 

(1903)  J.pharm.chim.  [6],  18,  116. 
Boulouch,  R. 

(1902)  Compt.rend.,  135,  165. 

(1906)  Compt.rend.,  142,  1045. 
Bourgoin. 

(1874)  Bull.soc.chim.  [2],  21,  no. 

(1878)  Ann.chim.phys.  [5],   13,  406; 
I5>  165. 

(1884)  Bull.soc.chim.  [2],  42,  620. 
Boutaric,  A. 

(1911)  Compt.rend.,  153,  876-7. 
Bowen,  N.  L. 

(1914)  Am.Jour.Sci.  [4],  38,  207-264. 
Bowen,  N.  L.  and  Anderson,  Olaf . 

(1914)  Am.Jour.Sci.  [4],  37,  487. 
Boyle,  Mary. 

(1909)  J.Chem.Soc.(Lond.),  95,  1696. 
Boyle,  R.  W. 

(1911)  Phil. Mag.  [6],  22,  840-854. 
Bradley,  W.  P.  and  Alexander,  W.  B. 

(1912)  J.Am.Chem.Soc.,  34,  17. 
Bramley,  A. 

(1916)      J.Chem.Soc.(Lond.),      109, 

469-96. 
Brand,  H. 

(1911)  Neues  Jahrb.Min.Geol.(Beil. 

Bd.),  32,  627-700. 

(1912)  Zentralbl.Min.Geol.and  Pal., 

26-32. 

(1913)  Neues  Jahrb.Min.Geol.,     I, 

9-27. 
Brandan. 

(1869)  Liebig's  Ann.,  151,  340. 
Braun,  L. 

(1900)  Z.physik.Chem.,  33,  732. 
Brauner,  B. 

(1898)  J.Chem.Soc.(Lond.),  73,  955. 


788 


AUTHOR   INDEX 


Bray,  Wm.  C. 

(1905-06)  Z.physik.Chem.,  54,  569- 

608. 
Bray,  W.  C.  and  Connolly,  E.  L. 

1(1910)  J.Am.Chem.Soc.,  32,  937. 
(1911)  J.Am.Chem.Soc.,  33,  1485. 
Bray,  W.  C.  and  MacKay,  G.  M.  T. 

(1910)  J.Am.Chem.Soc.,    32,    914, 

1207. 
Bray,  Wm.  C.  and  Winninghoff. 

(1911)  J.Am.Chem.Soc.,  33,  1663. 
Breithaupt,  J. 

(        )  These,  Univ.  of  Geneve.,  38, 

No.  446. 
Briegleb. 

(1856)  Liebig's  Ann.,  97,  95. 
Brinton,  Paul  H.  M.  P. 

(1916)  J.Am.Chem.Soc.,  38,  2365. 
Brissemoret,  M. 

(1898)  J.pharm.chim.   [6],  7,   176-8. 
Bronsted,  J.  N. 

(1906)  Z.physik.Chem.,  55,  377. 
(1909)    7th    Int.    Congress    Applied 

Chem.,  10,  no. 

(1911)  Z.physik.Chem.,  77,  132. 

(1912)  Z.physik.Chem.,  80,  208,  214. 
Brown,  J.  C. 

(1907)  Proc.Chem.Soc.,  23,  233. 
(1907)      J.Chem.  Soc.(Lond-),       91, 

1826-31. 
Brown,  O.  W. 

(1898)  J.Phys.Chem.,  2,  51. 
Browning  and  Hutchins. 

(1900)  Z.anorg.Chem.,  22,  380. 
Bruner,  L. 

(1898)  Z.physik.Chem.,  26,  147. 
Bruner,  L.  and  Zawadski,  J.,  el  al. 

(1909)  Bull.Internat.acad.Sci.      Cra- 
covie,  [3],  9,  A,  267-312,  377. 

(1910)  Z.anorg.Chem.,  67,  454-5. 
(1910)  Chem.  Abs.,  4,  980,  2758. 

Bruni,  G. 

(1898)  Gazz.chim.ital.,  28,  II,  508- 

529- 

(1899)  Atti  accad.Lincei,   [5],  8,  II, 

141. 

(1900)  Gazz.chim.ital.,  30,  I,  25-35. 
Bruni,  G.  and  Berti,  P. 

(1900)  Gazz.chim.ital.,  30,  II,  324. 
Bruni,  G.  and  Finzi,  F. 

(1905)  Gazz.chim.ital.,  35,  II,  in- 

131- 
Bruni,  G.  and  Gorni,  F. 

(1899)  Atti  accad.Lincei,  [5],  8,  II,  188. 

(1900)  Atti  accad.Lincei,  [5],  9, 11,326. 
Bruni,  G.  and  Meneghini. 

(1909)  Z.anorg.Chem.,  64,  193. 

(1910)  Gazz.chim.ital.,  40,  I,  682. 
de  Bruyn,  C.  A.  Lobry. 

(1890)  Rec.trav.chim.,  9,  188. 
(1892)  Z.physik.Chem.,  10,  782-789. 
(1892)   Rec.trav.chim.,  n,  29,  112- 
156. 


de  Bruyn,  C.  A.  Lobry. 

(1894)  Rec.trav.chim.,  13,  116,  150. 

(1899)  Rec.trav.chim.,  18,  87. 

(1900)  Z.physik.Chem.,  32,  63,  85, 

92,  101. 

(1903)  Rec.trav.chim.,  22,  411. 
de  Bruyn,  C.  A.  Lobry,  and  van  Eken- 
stein,  W.  A. 

(1899)  Rec.trav.chim.,  18,  150. 

(1900)  Rec.trav.chim.,  19,  7. 
Bubanovic,  F. 

(1913)     Med.K.Vetenskapsakad.No- 
belinst,  2,  No.  33. 

'(1913)  Chem.Abs.,  7,  2886. 
Bube,  Kurt. 

(1910)  Z.anal.Chem.,  45,  525-96. 
Buchner,  E.  H. 

(1865)    Sitzber.k.Akad.Wiss.(Wein), 
52,  2,  644. 

(1905-06)  Z.physik.Chem.,  54,  665- 

88. 
Buchner,  E.  H.  and  Karsten,  B.  J. 

(1908-9)    Proc.k.Akad.Wet.(Amst.), 

n,  504. 
Buchner,  E.  H.  and  Prins,  Ada. 

(1912-13)  Z.phys.Chem.,  81,  113-120 
Bugarszky,  S. 

(1910)  Z.physik.Chem.,  71,  753. 
Bunsen,  Robert. 

(1877)  "  Gasometrische  Methoden," 

2nd  Ed. 
Bunsen-Heurich. 

(1892)  Z.physik.Chem.,  9,  438. 
Bylert,  V. 

(        )  These,  Amsterdam. 
Cabot,  G.  L. 

(1897)  J.Soc.Chem.Ind.,  16,  417. 
Cady,  H.  P. 

(1898)  J.Phys.Chem.,  2,  168,  206. 
Caille. 

(1909)  Compt.rend.,  148,  1461. 
Calcagni,  G. 

(1912)   Gazz.chim.ital.,  42,  II,  653, 

661. 
(i9i2a)  Atti  accad.Lincei,  [5],  21,  II, 

72. 
Calcagni,  G.  and  Mancini,  G. 

(1910)  Atti  accad.Lincei,  [5],  19,  II, 

424. 
Calcagni,  G.  and  Marotta,  D. 

(1912)  Gazz.chim.ital.,  42,  II,  669- 
680. 

(1912)  Atti  accad.Lincei,  [5],  21,  II, 

93,  243,  284. 

(1913)  Gazz.chim.ital.,  43,  II,  380. 

(1913)  Atti  accad.Lincei,  [5],  22,  II, 

373,  443- 

(1914)  Gazz.chim.ital.,  44,  I,  487. 
Callender  and  Barnes. 

(1897)  Proc.Roy.Soc.,  62,  149. 
Calvert,  H.  T. 

(1901)  Z.physik.Chem.,  38,  521-540. 


789 


AUTHOR  INDEX 


Calzolari,  F. 

(1912)  Gazz.chim.ital.,  42,  II,  85-92. 
(         )      Acc.sc.med.e.nat.di  Ferora, 

85,  150. 
Cambi,  L. 

(1912)  Atti  accad.Lincei,  [5],  21,  I, 
776,  791. 

(1912)  Atti  accad.Lincei,  [5],  21,  II, 

839- 
Cambi,  L.  and  Speroni,  G. 

(1915)  Atti  accad.Lincei,  [5],  24,  I, 

736. 
Cameron,  F.  K. 

(1898)  J.Phys.Chem.,  2,  413. 

(1901)  J.Phys.Chem.,  5,  556. 

Cameron,  F.  K.  and  Bell,  J.  M. 

(1905)  J.Am.Chem.Soc.,  27,  1512. 

(1906)  J.Am.Chem.Soc.,     28,     1220, 

1222. 
(i9o6a)  J.Phys.Chem.,  10,  210. 

(1907)  J.Phys.Chem.,  n,  363. 

(1910)  J.Am.Chem.Soc.,  32,  869. 
Cameron,  F.  K.,  Bell,  J.  M.,  and  Robin- 
son, W.  O. 

(1907)  J.Phys.Chem.,  n,  396-420. 
Cameron,  F.  K.  and  Breazeale,  J.  F. 

(1903)  J.Phys.Chem.,  7,  574. 

(1904)  J.Phys.Chem.,  8,  335. 
Cameron,  F.  K.  and  Patten,  H.  E. 

(1911)  J.Phys.Chem.,  15,  67. 
Cameron,  F.  K.  and  Robinson,  W.  O. 

(1907)  J.Phys.Chem.,  n,  577,    641, 

691. 

(i9O7a)  J.Phys.Chem.,  n,  273-8. 
(1909)  J.Phys.Chem.,  13,  157,  251. 
Cameron,  F.  K.  and  Seidell,  A. 

(1901)  Bull.  No.  18,  Division  of  Soils, 

U.  S.  Dept.  Agr. 
(igoia)  J.Phys.Chem.,  5,  643. 

(1902)  J.Phys.Chem.,  6,  50. 
Campetti,  A. 

(1901)  Atti  accad.Lincei.,  [5],  10,  II, 

99-102. 

(1902)  Z.physik.Chem.,     41,     109, 

(abstract). 
(1917)     Atti    accad.sci.Torino,     52, 

114-21. 
Campetti,  A.  and  Del  Grosso,  C. 

(1913)  Nuovo  cimento,  [6],  6,  379- 

417 
(1913)    Mem. R.accad.Sci. (Torino), 

[II],  61,  187. 

(1911)    "Tables  annuelles,"  2,  433. 
Cantoni,  H.  and  Basadonna. 

(1906)  Bull.soc.chim.,  [3],  35,  731. 
Cantoni,  H.  and  Diotalevi,  D. 

(1905)  Bull.soc.chim.,  [3],  33,  27-36. 
Cantoni,  H.  and  Goguelia,  G. 

(1905)  Bull.soc.chim.,  [3],  33,  13. 
Cantoni,  H.  and  Jolkowsky. 

(1907)  Bull.soc.chim.  [4],  i,  1181. 
Cantoni,  H.  and  Passamanik. 

(1905)  Ann.chim.anal.appl.,  10,  258. 


Cantoni,  H.  and  Zachoder. 

(1905)  Bull.soc.chim.,  [3],  33,  747. 
Cap  and  Garot. 

(1854)  J.pharm.chim.,  [3],  26,  81. 
Capin,  J. 

(1912)  Pharm.Jour.(Lond.),  88,  65, 

from      (1911)      Bull.soc. 
pharm. (Bordeaux),  414. 
Carlinfanti,  E.  and  Levi-Malvano,  M. 

(1909)  Gazz.chim.ital.,  39,  II,  353- 

75- 
Carlson,  Birger. 

(1910)  Klason-Festschrift,     247-66 

(Stockholm). 

(1910)  "  Tables   annuelles,"  i,   379. 
Carnelly. 

(1873)    Liebig's  Ann.,    166,    (116?), 

155- 

(1873)  J.Chem.Soc.(Lond.),   [2],   n, 

323- 
Carnelly  and  Thomson. 

(1888)  J.Chem.Soc.(Lond.),  53,  799. 
Caro. 

(1874)  Arch.Pharm.,  [3],  4,  145. 
Carpenter. 

(1886)  J.Soc.Chem.Ind.,  5,  286. 
Carr,  F.  H.  and  Pyman,  F.  L. 

(1914)  J.Chem.Soc.(Lond.),      105, 

1 602-1 1. 
Carrara  and  Minozzi. 

(1897)  Gazz.chim.ital.,  27,  II,  955. 
Carveth,  H.  R. 

(1898)  J.Phys.Chem.,  2,  213. 
Caspari,  W.  A. 

(1915)  J.Chem.Soc.(Lond.),    107, 

162-171. 
Cassuto,  L. 

(1913)  Nuovo  cimento,  6,  1903. 
Cavazzi,  A. 

(1916)  Gazz.chim.ital.,  46,  II,  122-35 

(1917)  Gazz.chim.ital.,  47,  II,  49-63. 
Centnerszwer,  M. 

(1899)  Z.physik.Chem.,  29,  715. 

(1910)  Z.physik.Chem.,  72,  437. 
Centnerszwer,  M.  and  Teletow,  I. 

(1903)  Z.Elektrochem.,  9,  799. 
de  Cesaris,  P. 

(1911)  Atti  accad.Lincei,   [5],  20,  I, 

597,  749" 
Chancel  and  Parmentier. 

(1885)  Compt.rend.,  100,  473,  773- 
Chandler,  E.  E. 

(1908)  J.Am.Chem.Soc.,  30,  696. 
Chattaway,  F.  D.  and  Lambert,  Wm.  J. 
(1915)      J.Chem.Soc.(Lond.),      107, 

1768,  1776. 
Chavanne,  G.  and  Vos,  J. 

(1914)  Compt.rend.,  158,  1582. 
Chikashigi,  M. 

(i9ii-i2)Mem.Coll.Sci.Eng.(Kyoto), 

3,  197-206. 
(1911)  Z.anorg.Chem.,  72,  109. 


790 


AUTHOR  INDEX 


Chikashigi,  M.  and  Yamanchi,  Y. 

(1916)  Mem.Coll.Sci. Kyoto,  1,341-7. 
Chilesotti,  A. 

(1908)  Atti  accad.Lincei,  [5],  17,  II, 

475- 
Christensen. 

(1885)  J.prakt.Chem.,  [2],  31,  166. 
Christoff,  A. 

(1905)  Z.physik.Chem.,  53,  321. 

(1906)  Z.physik.Chem.,  55,  627. 

(1912)  Z.physik.Chem.,  79,  459. 
Christy,  S.  B. 

(1901)  Elektrochem.Ztschr.,  7,  205. 
Chugaev,  L.  and  Khlopin,  W. 

(1914)  Z.anorg.Chem.,  86,  159. 
Cingolani,  M. 

(1908)  Gazz.chim.ital.,  38,  I,  305. 

(1908)  Atti  accad.Lincei.,  [5],  17,  I, 

265. 
Ciusa,  R.  and  Bernard!,  A. 

(1910)  Gazz.chim.ital.,  40,  II,  159. 
Claasen,  H. 

(1911)  Z.Ver.Zuckerind.,6i,  489-509. 
Cleve. 

(1866?)  K.  Svenska  Vetenskaps- 
Akad.Handl.(Stockholm), 
10,  9,  7. 

(1874)  Bull.soc.chim.,  [2],  21,  344. 
(1885)  Bull.soc.chim.,  [2],  43,  166. 
Cleve,  Astrid. 

(1902)  Z.anorg.Chem.,  32,  157. 
Cloez. 

(1903)  Bull.soc.chim.  [3],  29,  167. 
Clowes,  F.  and  Biggs,  J.  W.  H. 

(1904)  J.Soc.Chem.Ind.,  23,  358. 
Cocheret,  D.  H. 

(1911)  Dissertation,  Leiden. 

(1911)  "Tables  Annuelles"2,  439, 

444. 
Cohen,  Ernst. 

(1900)  Z.physik.Chem.,  34,  189,  622. 
(1903)  Z.Elektrochem.,  9,  433. 

(1909)  Z.Elektrochem.,  15,  600. 
Cohen,  E.  and  Inouye,  K. 

(1910)  Z.physik.Chem.,  72,  411-424. 
(1910)  Chem.Weekblad.,  7,  277. 

Cohen,  E.,  Inouye,  K.  and  Euwen,  C. 

(1910)  Z.physik.Chem.,  75,  257. 
Cohen,  E.  and  Sinnige,  L.  R. 

(1910)  Trans. FaradaySoc.,  5,  269. 
Conn,  E. 

(1895)  Z.physik.Chem.,  18,  61. 
Colani,  A. 

(1913)  Compt.rend.,  156,  1075,  1908. 

(1916)  Bull.soc.chim.,  [4],  19,  405. 
(19163)  Compt.rend.,  163,  123-5. 

(1917)  Compt.rend.,     165,     111-3, 

234-6. 
Colson,  A. 

(1907)  Compt.rend.,  145,  1167,. 
Comanducci,  E. 

(1912)  Rend.soc.chim.ital.,    [2],    4, 

313. 


de  Coninck,  Oechsner. 

(1893)  Compt.rend.,  116,  758. 

(1894)  Compt.rend.,  118,  471. 

(1900)  Compt.rend.,  130,  1304;  131, 

1219. 

(1901)  Bull.acad.roy.(Belgique),  350. 
(1903)  Ann.chim.phys.,  [7],  28,  7. 
(1905)  Chem.Centralbl.,  76,  II,  883. 

(1905)  Bull.acad.roy.(Belgique),   pp. 

257,  359- 

(1906)  Compt.rend.,  142,  571. 
Conroy. 

(1898)  J.Soc.Chem.Ind.,  17,  104. 
Cooper,  H.  C.,  Shaw,  R.  I.,  and  Loomis, 

N.  E. 

(1909)  Am.Chem.Jour.,  42,  461. 

(1909)  Ber.,  42,  3991. 
Copisarow,  M. 

(1915)  Chem.News.,  112,  247. 
Coppadoro,  A. 

(1909)  Gazz.chim.ital.,  39,  II,  625. 

(1911)  Rend.soc.chim.ital.,    [2],    30, 

207. 

(1912)  Gazz.chim.ital.,  42,  I,  240. 

(1912)  Atti  accad.Lincei,  [5],  21,  II, 

842. 

(1913)  Gazz.chim.ital.,  43,  I,  138. 
de  Coppet,  L.  C. 

(1872)  Ann.chim.phys.,  [4],  25,  528, 

532. 
(1883)  Ann.chim.phys.,  [5],  30,  417. 

(1899)  Ann.chim.phys.,  [7],  16,  275. 
Corliss,  Harry  P. 

(1914)  J.Phys.Chem.,  18,  681. 
Cossa,  A. 

(1868)  Ber.,  i,  138. 

(1869)  Z.anal.Chem.,  8,  145. 
Costachescu,  N. 

(1910)  Ann.Sci.Univ.(Jassy),  7,  I. 
Coste,  J.  H. 

(1917)  J.Soc.Chem.Ind.,  36,  846-53. 

(1918)  J.Soc.Chem.Ind.,  37,  170. 
Cottrell,  et  al 

(1901)  Sitzber.k.Akad.Wiss. (Berlin), 

P-  1035. 
Couch,  J.  F. 

(1917)  Am.Jour.Pharm.,  89,  243-51. 
Courtonne,  H. 

(1877)  Ann.chim.phys.,  [5],  12,  569. 

(1882)  Compt.rend.,  95,  922. 
Cowper,  R. 

(1882)  J.Chem.Soc.(Lond.),  41,  254. 
Creighton,  H.  J.  M.,  and  Ward,  W.  H. 

(1915)  J.Am.Chem.Soc.,  37,  2333. 
Croft. 

(1842)  Phil.Mag.,  [3],  21,  356. 
Crompton,  H.  and  Walker,  M. 

(1912)  J.Chem.Soc.(Lond.),  101,  958. 
Crompton,  H.  and  Whiteley,  M.  A. 

(1895)  J.Chem.Soc.(Lond.),  67,  327. 
Crookes,  Wm. 

(1864)  J.Chem.Soc.(Lond.),  2,  134. 


791 


AUTHOR   INDEX 


Crowell,  R.  D. 

(1918)  J.Am.Chem.Soc.,  40,  455. 
Cuno,  E. 

(1908)  Ann.physik.,  [4],  25,  346-76. 
(1908-09)  Ann.physik.,  [4],  28,  663-4. 

(1907)  Ber.physik.Ges.,  5,  735~8. 
Curtis,  H.  A.  and  Titus,  E.  Y. 

(1915)  J.Phys.Chem.,  19,  740. 
Curtius  and  Jay. 

(1889)  J.prakt.Chem.,  [2],  39,  39. 
Dahms,  A. 

(1895)  Wied.Ann.Physik.,  54,486-519. 

(1896)  Wied.Ann.der  Physik.,  60, 122. 

(1899)  Ann.chim.phys.,  [7],  18,  140. 
Dakin,   H.   D.,    Janney,    N.    W.   and 

Wakemann,  A.  J. 

(1913)  J.Biol.Chem.,  14,  241. 
van  Damm,  W.  and  Donk,  A.  D. 

(1911)  Chem.Weekblad,  8,  848. 
Dancer. 

(1862)  J.Chem.Soc.(Lond.),  15,  477. 
D'Ans,  J. 

(1908)  Ber.,  41,  1776-7. 

(1909)  Z.anorg.Chem.,  62,  129-167. 
oga)  Z.anorg.Chem.,  63,  225-9. 
ogb)  Z.anorg.Chem.,  65,  228. 

19090)  Z.anorg.Chem.,  61,  91-5. 
(1913)  Z.anorg.Chem.,  80,  235. 
D'Ans,  J.  and  Fritsche,  O. 

(1909)  Z.anorg.Chem.,  65,  231. 
D'Ans,  J.  and  Schreiner,  O. 

(1910)  Z.anorg.Chem.,  67,  437. 
(i9ioa)  Z.physik.Chem.,  75,  95-107. 

D'Ans,  J.,  Shepherd,  L.  D'Arey  and 
Gunther,  P. 

(1906)  Z.anorg.Chem.,  49,  356-61. 
D'Ans,  J.  and  Siegler,  R. 

(1913)  Z.physik.Chem.,  82,  35-44. 
Davidsohn,  J.  and  Wrage,  W. 

(1915)  Chem.Rev.Fett.Harz.Ind.,  22, 

9-14. 
Davis,  H.  S. 

(1916)  J.Am.Chem.Soc.,  38,  1169. 
Dawson,  H.  M. 

(1901)  J.Chem.Soc.(Lond.),  79,  242. 

(1902)  J.Chem.Soc.(Lond.)  81,  1086- 

1097. 

(1904)  J.Chem.Soc.(Lond.),  85,  467. 
(1906)  J.Chem.Soc.(Lond.),  89,  1668. 

(1908)  J.Chem.Soc.(Lond.),  93,  1310. 

(1909)  Z.physik.Chem.,  69,  110-122. 
(i909a)      J.Chem.Soc.(Lond.),      95, 

370-81. 

(19095)  J.Chem.Soc.(Lond.),  95,874. 
Dawson,  H.  M.  and  Gawler,  R. 

(1902)  J.Chem.Soc.(Lond.),  81,  524. 
Dawson,  H.  M.  and  Goodson,  E.  E. 

(1904)  J.Chem.Soc.(Lond.),  85,  796. 
Dawson,  H.  M.  and  Grant. 

(1901)  J.Chem.Soc.(Lond.),  81,  512. 
Dawson,  H.  M.  and  McCrae,  J. 

(1900)  J.Chem.Soc.(Lond.),       77, 

1239-62. 


Dawson,  H.  M.  and  McCrae,  J. 

(igoia)  J.Chem.Soc.(Lond.),  79,  493. 

(1901  b)      J.Chem.Soc.(Lond.),     79, 

1069. 
Dehn,  Wm.  M. 

(1917)  J.Am.Chem.Soc.,  39,  1400. 

(i9i7a)  J.Am.Chem.Soc.,  39,  1378. 
De  Jong  (see  de  Jong). 
Delange,  Leon. 

(1908)  Bull.soc.chim.,  [4],  3,  910-5. 
Delepine. 

(1892)  J.pharm.chim.,  [5],  25,  496. 
(1895)  Bull.soc.chim.,  [3],  13,  353. 
(1908)  Bull.soc.chim.,  [4],  3,  904. 

Demarcay. 

(1883)  Compt.rend.,  96,  1860. 
Demassieux,  N. 

(1913)  Compt.rend.,  156,  892. 

(1914)  Compt.rend.,  158,  183,  702. 
Denham,  H.  G. 

(1917)  J.Chem.Soc.(Lond.),  in,  39. 
Derick,  C.  G.  and  Kamm,  O. 

(1916)  J.Am.Chem.Soc.,  38,  415. 
Dernby,  K.  G. 

(i9i8)Medd.k.Vetenkapsakad.Nobel 

inst.,  3,  No.  1 8. 
Derrien. 

(1900)  Compt.rend.,  130,  722. 
Deszathy. 

(1893)  Monatsh.Chem.,  14,  249. 
De  Visser,  L.  E.  O. 

(1898)  Rec.trav.chim.,  17,  182,  346. 
Dewey,  F.  P. 

(1910)  J.Am.Chem.Soc.,  32,  318. 
Dhar,  N.  and  Datta,  K. 

(1913)  Z.Elektrochem.,  19,  584. 
Diacon. 

(1866)  Jahrsber.Chem.,  61. 
Dibbits. 

^1874)  Z.anal.Chem.,  13,  139. 

74)   J.prakt.Chem.,    [2],   10,  417, 

439- 
Dieterich. 

(1890)  Pharm.Centrh.,  31,  395. 
Dietz. 

(1898)  Pharm.Ztg.,  43,  290. 

(1899)  Z.anorg.Chem.,  20,  260. 

(1899)  Ber.,  32,  95. 

(1900)  Wiss.Abt.p.t.Reichanstalt,  ;, 

433- 
Dimroth,  O.  and  Mason,  F.  A. 

(1913)  Liebig'sAnn.,  399,  108. 
Ditte,  A. 


\io/$}   v^umpt.i  ciiu. 

(1877)  Compt.rend. 
(1881)  Compt.rend. 
(1881)  Ann.chim.ph 
(1896)  Compt.rend. 
(1897)  Compt.rend. 

OU,     1  l<Jif. 

85,  1069. 
92,  242,  718. 

ys.,  [5],  24,  226. 
123,  1282. 
124,  30. 

T-_1        _ 

(1898)  Ann.chim.phys.,  [7],  14,  294. 
Dittmar. 

(1888)  J.Soc.Chem.Ind.,  7,  730. 


792 


AUTHOR   INDEX 


Dittrich,  C. 

(1899)  Z.physik.Chem.,  29,  485. 
Ditz,  H.  and  Kanhauser,  F. 

(1916)  Z.anorg.Chem.,  98,  128-40. 
Divers. 

(1870)  J.Chem.Soc.(Lond.),  23,  171. 

(1899)  J.Chem.Soc.(Lond.),  75,  86. 
Doerinckel,  F. 

(1907)  Metallurgie,  8,  201-9,  408. 
Dolezalek,  F.  and  Finckli,  K. 

(1906)  Z.anorg.Chem.,  51,  320-7. 
Dolgolenko,  W. 

(1907)  Jour.Russ.Phys.Chem.Soc.  39, 

841. 
Dolinski,  J.  H. 

(1905)  Ber.,  38,  1835. 
Donath,  E. 

(1911)  Chem.Ztg.,  35,  773~4- 
Donk,  A.  D. 

(1908)  Chem.Weekblad,  5,  529,  629, 

767. 

(1916)  Chem.Weekblad,  13,  92-97. 
Donk,  M.  G. 

(1905)  Bull.  No.  90,  Bureau  Chem. 

U.  S.  Dept.  Agr. 
Donnan,  F.  G.  and  Burt,  B.  C. 

(1903)  J.Chem.Soc.(Lond.),  83,- 335. 
Donnan,  F.  G.  and  Thomas,  J.  S. 

(1911)  J.Chem.Soc.(Lond.),99, 1788. 
Donnan,  F.  G.  and  White,  A.  S. 

(1911)  J.Chem.Soc.(Lond.),  99,  1669. 
van  Dorp,  G.  C.  A. 

(1910)  Z.physik.Chem.,  73,  284-289. 

(1911)  Chem.Weekblad.,  8,  269. 

(1912)  8th       Internat.Cong.Appl. 

Chem.,  22,  239. 

(1913-14)  Z.physik.Chem.,  86,  109. 
Dott,  D.  B. 


(1906)  Pharm.. 

(1907)  Pharm.] 
(1910)  Pharm/ 
(1912)  Pharm.. 


our.(Lond.),  76,  345. 
our.(Lond-),  78,  79. 
our.(Lond.),  85,  795. 
our.(Lond.),  88,  424. 


Doumer  and  Deraux. 

(1895)  J-  pharm.chim.,  [6],  i,  50. 
Doyer,  J.  W. 

(1890)  Z.physik.Chem.,  6,  481. 
Draper. 

(1887)  Chem.News.,  55,  169. 
Dreyer,  F. 

(1913)     Ann.Inst.Polyt.(Petrograd), 

20,  326. 
Dreyer,  F.  and  Rotarski. 

(1905-06)  Z.physik.Chem.,  54,  356. 
Driot. 

(1910)  Compt.rend.,  150,  1426. 
Drucker,  K. 

(1901)  Z.anorg.Chem.,  28,  362. 

(1912)  Z.Elektrochem.,  18,  246. 
Drucker,  K.  and  Moles,  E. 

(1910)  Z.physik.Chem.,  75,  405. 
Duboin,  A. 

(1905)  Compt.rend.,  141,  385. 


Duboin,  A. 

(1906)  Compt.rend.,  142,   395,    573, 

887,  1338. 
Dubois  and  Fade. 

(1885)  Bull.soc.chim.,  [2],  44. 
Dubowitz,  H. 

(1911)    Seifensieder  Ztg.,    38,    1164, 

1208. 

(         )  Vegnesceti  lapok.,  6,  397. 
Dubrisay,  Rene. 

(1911)  Compt.rend.,  153,  1077. 

(1912)  Compt.rend.,  154,  431. 
Dubroca,  M. 

(1904)  J.chim.phys.,  2,  447. 

(1907)  J.chim.phys.,  5,  463-87. 
Dukelski,  M.  P. 

(1906)  Z.anorg.Chem.,  50,  42. 

(1907)  Z.anorg.Chem.,  53,  327~337J 

54,  45—9. 
(1907)    J.Russ.Phys.Chem.Soc.,    39, 

975-88. 

(1909)  Z.anorg.Chem.,  62,  114-8. 
Dunn. 

(1882)  Chem.News,  45,  272. 
Dunningham,  A.  C. 

(1912)      J.Chem.Soc.(Lond.),      101, 


J.Chem.Soc.(Lond.),    105, 

368-79,  73*3,  2630. 
Dunnington  and  Long. 

(1899)  Am.Chem.Jour.,  22,  217. 
Dunstan,  W.  R.  and  Umney,  J.  C. 

(1892)  J.Chem.Soc.(Lond.),  61,  391. 
Dupre  and  Bialas. 

(1903)  Z.angew.Chem.,  16,  55. 
Dutilh,  H. 

(i9i2)Verh.k.Akad.Wet.(Amst.),[n] 
4,60. 

(1912)  "  Tables  annuelles,"  3,  336. 
Ebelmen. 

(1852)  Liebig's.Ann.,  [3],  5,  189. 
Eder. 

(1876)  Dingier  polyt.J.,  221,  89,  189. 

(1878)  J.prakt.Chem.,  [2],  17,  45. 

(1880)    Sitzber.k.Akad.Wiss.(Wien), 

82,  Abt.  II,  1284. 
Efremov,  N.  N. 

(1912)  Ann. Inst. Polytechnic  (Petro- 

grad),  18,  391. 

(1913)  J.Russ.Phys.Chem.Soc.,    45, 

348-62. 

(1915)  Bull.acad.sci.Petrograd,  1309- 

36. 

(1916)  Bull.acad.sci.Petrograd,  21-46. 
Eggink,  B.  G. 

(1908)  Z.physik.Chem.,  64,  492. 
Ehlert,  H.  and  Hempel,  W. 

(1912)  Z.Elektrochem.,  18,  727. 
van  Ekenstein,  W.  A.  and  de  Bruyn, 
C.  A.  Lobry. 

(1896)  Rec.trav.chim.,  15,  225. 
Emerson,  W.  H. 

(1907)  J.Am.Chem.Soc.,  29,  1750-6. 


793 


AUTHOR   INDEX 


Emich. 

(1884)  Monatsh.Chem.,  3,  336. 
Emmerling. 

(1869)  Liebig's  Annaien,  150,  257. 
von  Ende,  C.  L. 

(1901)  Z.anorg.Chem.,  26,  148. 
Engel. 

(1886)  Compt.rend.,  102,  114. 

(1887)  Compt.rend.,  104,  507,  913. 

(1888)  Ann.chim.phys.,  [6],  13,  348- 

385- 

(1889)  Ann.chim.phys.,  [6],  17,  347. 
(1891)  Bull.soc.chim.,  [3],  6,  17. 

Enell. 

(1899)  Pharm.Centralh.,  38,  181. 

(1899)  Z.anal.Chem.,  38,  386. 
Engfeldt,  N.  O. 

(1913)  Farmaceutisk  Revy,  No.  8. 

(1913)  Apoth.Ztg.,  28,  182. 

(1913)  Pharm.Jour.(Lond.),  90,  769. 
aglish,  S.  and  Turner,  W.  E.  S. 

(1915)  J.Chem.Soc.(Lond.),      107, 

774-83. 
Enklaar,  J.  E. 

(1901)  Rec.trav.chim.,  20,  183. 
Ennis,  A.  J. 

(1914)  J.Chem.Soc.(Lond.),      105, 

,350-64. 
Eppel. 

(1899)  Dissertation,  Heidelberg. 
Erdmann. 

(1893)  Ber.,  26,  2439. 
Erdmann  and  Bedford. 

(1904)  Ber.,  37,  1184. 
Etard. 

(1877)  Compt.rend.,  84,  1090. 
(1884)  Compt.rend.,  98,  1434. 

(1894)  Ann.chim.phys.,   [7],  2,  526- 

570;  3,  275. 
von  Euler,  H. 

(1903)  Ber.,  36,  2879,  3400. 

(1904)  Z.physik.Chem.,  49,  315. 

(1916)  Z.physik.Chem.,  97,  291. 
von  Euler,  H.  and  Lb'wenhamn,  E. 

(1916)  Z.Elektrochem.,  22,  199-254. 

(1916)  Chem.Abs.,  10,  3021. 

(1917)  Chem.Abs.,  n,  915. 
Euwes,  P.  C.  J. 

(1909)  Rec.trav.chim.,  28,  298. 
Ewers,  Erich. 

(1910)  Milchwirschaft.Zentr.,  6  (3?), 

155- 

van  Eyk,  see  Van  Eyk. 
Fahrion,  W. 

(1916)  Chem.Umschau,  23,  34-5. 
Falciola,  P. 

(1910)  Gazz.chim.ital.,  40,  II,  218. 

(1910)  Seifens  Ztg.,  38,  506. 
Farmer,  R.  C. 

(1901)  J.Chem.Soc.(Lond.),  79,  865. 

(1903)  J.Chem.Soc.(Lond.),  83,  1446. 
Farmer,  R.  C.  and  Warth,  F.  J. 

(1904)  J.Chem,Soc,(Lond.),  85, 1713. 


Fastert,  C. 

(1912)  Kali,  [6],  454. 

(1912)  Neue.Jahrb.Min.Geol.  (Beil. 

Bd.),  33,  286. 
Faucon,  A. 

(1909)  Compt.rend.,  148,  1189. 

(1910)  Ann.chim.phys.,  [8],   19,  70- 

152. 
Fauzer. 

(1888)  Math.u.Natur.Wiss.Ber.(Un- 

garn),  6,  1.54. 
de  Fazi,  R. 

(1916)  Gazz.chim.ital.,  46,  I,  345. 
Fedotieff,  P.  P. 

(1904)  Z.physik.Chem.,  49,  168. 

(1910-11)  Z.anorg.Chem.,  69,  26. 

(1911-12)  Z.anorg.Chem.,  73,  178. 
Fedotieff,  P.  P.  and  Iljinsky. 

(1913)  Z.anorg.Chem.,  80,  119. 
Fedotieff,  P.  P.  and  Koltunoff,  J. 

(1914)  Z.anorg.Chem.,  85,  251. 
Feit,  W.  and  Przibylla,  K. 

(1909)  Z.Kali,  3,  393-8. 
Fenton,  H.  J.  H. 

(1898)  J.Chem.Soc.(Lond.),  73,  479. 
Ferchland. 

(1902)  Z.anorg.Chem.,  30,  133. 
Field. 

(1859)  J.Chem.Soc.(Lond.),  n,  6. 
Filehne,  Wm. 

(1907)  Beitrage    Chem.Physiol   u. 

Pathol.,  10,  304. 
Findlay,  Alex. 

(1901)  J.Chem.Soc.(Lond.),  85,  403. 
Findlay,  Alex. 

(1902)  J.Chem.Soc.(Lond.),  81,  1217. 
(1904)  J.Chem.Soc.(Lond.),  85,  403. 

(1908)  Chem.News,  96,  163. 

(1908)  Analyst,  33,  391. 

Findlay,  Alex,  and  Creighton,  H.  J.  M. 

(1910)  J.Chem.Soc.(Lond.),  97,  536- 

61. 

(1911)  Biochem.Jour.,  5,  294. 
Findlay,  A.  and  Hickmans,  E.  M. 

(1907)  J.Chem.Soc.(Lond.),  91,  905. 

(1909)  J.Chem.Soc.(Lond.),  95,  1389. 
Findlay,  A.  and  Howell,  O.  R. 

(i9i4)J.Chem.Soc.(Lond.),  105,  291- 
98. 

(1915)  J.Chem.Soc.(Lond.),      107, 

282-4. 
Findlay,  Alex,  and  King,  G. 

(1913)  J.Chem.Soc.(Lond.),i03,ii7o. 

(1914)  J.Chem.Soc.(Lond.),  105, 1297. 
Findlay,  Alex.,  Morgan,  I.  and  Morris, 

I.  P. 
(1914)      J.Chem.Soc.(Load.),      105, 

779-82. 
Findlay,  Alex,  and  Shen,  B. 

(1911)  J.Chem.Soc.(Lond.),  99,  1313. 

(1912)  J.Chem.Soc.(Lond.),      101, 

1459-68. 


794 


AUTHOR   INDEX 


Findlay,  Alex,  and  Williams,  T. 

(1913)  J.Chem.Soc.(Lond.),  103,  636. 
Fischer,  Emil. 

(1906)  Ber.,  39,  4144-5. 
Fisher,  V.  M. 

(1914)  J.Russ.Phys.Chem.Soc.,    46, 

1250-70. 

Fisher,  V.  M.  and  Miloszewski,  F. 
(1910)  Kosmos  (Lemberg),  35,  538- 

42. 

(1910)  Chem.Zentr.,  II,  1048. 
Flaschner,  O. 

(1908)  Z.physik.Chem.,  62,  493-8. 

(1909)  J.Chem.Soc.(Lond.),  95,  668- 

85- 
Flaschner,  O.  and  MacEwan,  B. 

(1908)  J.Chem.Soc.(Lond.),  93,  1000. 
Flaschner,  O.  and  Rankin,  I.  G. 

(1909)  Sitzber.k.Akad.Wiss.(Wien), 

118,  116,  695-722. 

(1910)  Monatsh.Chem.,  31,  23-50. 
Flawitzki,  F. 

(1909)  J.Russ.Phys.Chem.Soc.,    41, 

739- 
Fluckiger. 

(1887)  Arch.Pharm.,  [3],  25,  542. 
Fock. 

(1897)  Z.Kryst.Min.,  28,  365,  397. 
Fokin,  S.  J. 

(1912)    J.Russ.Phys.Chem.Soc.,    44, 

163. 
Fonda,  G. 

(1910)  Dissertation,  Karlsruhe. 
Fontein,  F. 

(1910)  Z.physik.Chem.,  73,  212-251. 
Fonzes-Diacon. 

(1895)  J.pharm.chim.,  [6],  I,  59. 
Foote,  H.  W. 

(1903)  Am.Chem.Jour.,  30,  341. 

(1903)  Z.physik.Chem.,  46,  81. 

(1904)  Am.Chem.Jour.,  32,  252. 

(1907)  Am.Chem.Jour.,  37,  124. 

(1910)  J.Am.Chem.Soc.,  32,  618-22. 
(1912)  J.Am.Chem.Soc.,  34,  880. 

(1915)  J.Am.Chem.Soc.,    37,    290, 

1 200. 
Foote,  H.  W.  and  Andrew,  I.  A. 

(1905)  Am.Chem.Jour.,  34,  153,  165. 
Foote,  H.  W.  and  Chalker,  W.  C. 

(1908)  Am.Chem.Jour.,  39,  564,  567. 
Foote,  H.  W.  and  Haigh,  F.  L. 

(1911)  J.Am.Chem.Soc.,  33,  459. 
Foote,  H.  W.  and  Levy. 

(1907)  Am.Chem.Jour.,  37,  119. 
Foote,  H.  W.  and  Saxon,  Blair. 

(1914)  J.Am.Chem.Soc.,  36,  1695. 
Foote,  H.  W.  and  Walden,  P.  T. 

(1911)  J.Am.Chem.Soc.,  33,  1032. 
Forbes,  G.  S. 

(1911)  J.Am.Chem.Soc.,  33,  1937. 
de  Forcrand,  R. 

(1909)  Compt.rend.,  149,  719. 
(i909a)  Compt.rend.,  149,  1344. 


de  Forcrand,  R. 

(1911)  Compt.rend.,  152,  1210, 

(1912)  Compt.rend.,  154,  133. 

(1912)  Compt.rend.,  155,  118,  1767. 
de  Forcrand,  and  Fonzes-Diacon. 

(1902)  Ann.chim.phys.,  [7],  26,  253. 
Formanek. 

(1887)  Chem.Centralbl.,  18,  270. 
Forster. 

(1892)  Ber.,  25. 
Foster,  B.  and  Neville,  H.  A.  D. 

(1910)  Proc.Chem.Soc.,  26,  236. 
Fox,  Chas.  J.  J. 

(1902)  Z.physik.Chem.,  41,  458. 

(1903)  Z.anorg.Chem.,  35,  130. 

(1909)  J.Chem.Soc.(Lond.),  95,  878- 

89. 

(i909a)  Trans.Faraday  Soc.,  5,  68. 
Fox,  Chas.  J.  J.  and  Gauge,  A.  J.  H. 

(1910)  J.Chem.Soc.(Lond.),  97,  377- 

85- 
Fraenckel,  F. 

(1907)  Z.anorg.Chem.,  55,  223-32. 
Francois,  M. 

(1900)  Compt.rend.,  130,  1024. 
Frankforter,  G.  B.  and  Cohen,  Lillian. 

(1914)  J.Am.Chem.Soc.,  36,  1103-34. 
(1916)  J.Am.Chem.Soc.,  38,  1139. 

Frankforter,  G.  B.  and  Frary,  F.  C. 

(1913)  J.Phys.Chem.,  17,  402-473- 
Frankforter,  G.  B.  and  Temple,  S. 

(1915)  J.Am.Chem.Soc.,    37,   2697- 

2716. 
Fraps,  G.  S. 

(1901)  Am.Chem.Jour.,  27,  290. 
Free,  E.  E. 

(1908)  J.Am.Chem.Soc.,  30,  1366-74. 
Fresenius. 

(1846)  Liebig's  Annalen,  59,  118. 

(1890)  Z.anal.Chem.,  29,  418. 

(1891)  Z.anal.Chem.,  30,  672. 
Freundlich,  H.  and  Posnjak,  E. 

(1912)  Z.physik.Chem.,  79,  174. 
Freundlich,  H.  and  Richards,  M.  B. 

(1912)  Z.physik.Chem.,  79,  692. 
Freundlich,  H.  and  Seal,  A.  N. 

(1912)  Z.Chem.Ind.Koll.,  u,  258. 
Friedel. 

(1869)  Liebig's  Ann.,  149,  96. 
Friedel  and  Gorgeu. 

(1908)  Compt.rend.,  127,  590. 
Friedel  and  Lachburg. 

(1869)  Bull. soc. chim.,  [2],  12,  92. 
Friedlander,  T. 

(1901)  Z.physik.Chem.,  38,  389. 
Friedrich,  K. 

(1907)  Metallurgie,  4,  480,  671. 

(1908)  Metallurgie,  5,  114. 

(1914)  Metallurgie  u.Erz.,   n,   196— 

200. 
Fronmuller. 

(1878)  Ber.,  n,  92. 


795 


AUTHOR  INDEX 


Fujimura,  T. 

(1914)  Mem.Col.Sci.Kyoto,  i,  63-68. 
Fulda,  W. 

(1909)  Arb.Kais.Gesundheitsamt,  30, 

81. 
Funk,  R. 

(1899)  Z.anorg.Chem.,  20,  412. 

(1900)  Wiss.Abh.p.t.Reichanstalt,  3, 

440. 

(igooa)  Ber.,  33,  3697. 
Furcht,  M.  and  Lieben,  A. 

(1909)     Sitzber.k.akad.Wiss  (Wien), 

118,  116,  383. 

(1909)  Monatsh.Chem.,  30,  555. 
Fiirth. 

(1888)  Monatsh.Chem.,  9,  311. 
Galeotti,  G. 

(1906)  Z.physiol.Chem.,  48,  473. 
Galeotti,  C.  and  Giampalmo,  G. 

(1908)  Z.Chem.Ind.Kolloide,  3,  118- 

GarelU,  F. 

(1894)  Gazz.chim.ital.,  24,  II,  263. 
Garelli,  F.  and  Calzolari,  F. 

(1899)  Gazz.chim.ital.,  29,  264. 
Garside. 

(1875)  Chem.News,  31,  245. 
Gaudechon,  H. 

(1910)  Compt.rend.,  150,  467. 
Gaus. 

(1900)  Z.anorg.Chem.,  25,  236. 
Gay-Lussac. 

(1819)  Ann.chim.phys.,  n,  314. 
Gazarolli  and  Thurnbalk. 

(1881)  Liebig's  Ann.,  209,  184. 
Geffcken,  G. 

(1904)  Z.physik.Chem.,  49,  271,  296. 
Geiger. 

(1904)  Dissertation  (Berlin). 
Gemsky,  N. 

(1914)  Neues  Jahrb.Min.Geol.(Beil. 

Bd.),  36,  513-58. 
von  Georgievics,  G. 

(1913)  Z.physik.Chem.,  84,  358. 

(1913)  Monatsh.Chem.,  34,  734. 

(1915)  Z.physik.Chem.,  90,  54. 
(1915)  Monatsh.Chem.,  36,  400. 

Gerard. 

(1901)  /\nn.chim.anal.,  6,  59. 
Gerardin. 

(1865)    Ann.chim.phys.,    [4],    5,  129, 

134,  147,  158. 
Gerlach. 

(1869)  Z.anal.Chem.,  8,  250,  281. 

(1889)  Z.anal.Chem.,  28,  473. 
Gibbs,  H.  D. 

(1908)  Philippine  J.Sci.,  3,  A  357. 
Gill,  H.  W. 

(1914)  J.Chem.Met.Soc.(S.  Africa), 

14,  290-2. 
van  Ginneken,  P.  J.  H. 

(1911)  Verslag.k.Akad.Wet.(Amst.), 

20,  337. 


van  Ginneken,  P.  J.  H. 

Z.Ver.Zuckerind,  62.  421-39. 
Ginsberg,  A.  S. 

(i9o6)Ann.Inst.Polyt.(Petrograd),6, 
493- 

(1908)  Z.anorg.Chem.,  59,  346. 

(1909)  Z.anorg.Chem.,  61,  122. 
Giolitti,  F.  and  Bucci,  G. 

(1905)  Gazz.chim.ital.,  35,  II,  162-9. 
Giolitti,  F.  and  Vecchiarelli,  V. 

(1905)  Gazz.chim.ital.,  35,  II,  170. 
Giran,  H. 

(1903)  Jour.physique,  [4],  2,  807. 
(i9O3a)  Ann.chim.phys.,  [7],  30,  249. 

(1906)  Compt.rend.,  142,  398. 

(1908)  Compt.rend.,  146,  270,  1270. 

(1913)  Bull.soc.chim.,  [4],  13,  1050. 
Giraud,  H. 

(1885)  Bull.soc.chim.,  [2],  43,  552. 
von  Girsewald,  C.  and  Wdokitin,  A. 

(1909)  Ber.,  42,  856-9. 
Giua,  M. 

(1914)  Ber.,  47,  1718-23. 

(1915)  Gazz.chim.ital.,   45,    I,    339, 

557;  II,  32,  348. 

(1916)  Gazz.chim.ital.,  46,  I,  289;  II, 

274. 
(1916)  Atti  accad.Lincei,  [5],  25,  I, 

99-105. 
Gladstone. 

(1854)  J.Chem.Soc.(Lond.),  6,  n. 
Glauser,  R.  Th. 

(1910)  Z.anorg.Chem.,  66,  437. 
Glowezynski,  Z. 

(1914)  Kolloidchem.Beihefte,  6,  147- 

176. 
Gniewosz,  St.  and  Walfisz,  Al. 

(1887)  Z.physik.Chem.,  i,  70. 
Gockel. 

(1897)  Chem.Zentralbl.,  II,  401. 
Godeffroy. 

(1876)  Ber.,  9,  1337,  1369. 

(1886)  Z.oster.Apoth.Ver.,  No.  9. 
Goldblum,  H.  and  Stoffella,  G. 

(1910)  J.chim.phys.,  8,  154. 
Goldblum,  H.  and  Terlikowski,  F. 

(1912)  Bull.soc.chim.,    [4],    n,  146- 

159- 
Goldschmidt,  H. 

(1895)  Z.physik.Chem.,  17,  154. 

(1898)  Z.physik.Chem.,  25,  95. 
Goldschmidt,  H.  and  Cooper,  H.  C. 

(1898)  Z.physik.Chem.,  26,  715. 
Goldschmidt,  H.  and  Eckardt,  M. 

(1906)  Z.physik.Chem.,  56,  389. 
Goldschmidt,  H.  and  Sunde,  E. 

(1906)  Z.physik.Chem.,  56,  15. 
Goodwin,  W.  L. 

(1882)  Ber.,  15,  3039. 
van  der  Goot,  Tetta  Polak. 

(1913)  Z.physik.Chem.,  84,  419-450. 
Gordon,  V. 

(1895)  Z.physiLChem.,  18,  1-16. 


796 


AUTHOR  INDEX 


Gore. 

(1870)  Proc.Roy.Soc.,  18,  158. 
Gori,  G. 

(1913)  Boll. chim. farm.,  52,  891-5. 
(1915)  Chem.Abs.,  9,  1827. 

Gortner,  R.  A. 

(1914)  Biochem.Bull.,  3,  468-9. 
Gothe,  E. 

(1915)  Chem.Ztg.,  39,  305-?- 
Gott,  B.  S.  and  Muir,  M.  P. 

(1888)  J.Chem.Soc.(Lond.),  53,  138. 
Grahmann,  W. 

(1913)  Z.anorg.Chem.,  81,  257-314. 
Grant,  A.  J.  and  James,  C. 

'(1917)  J.Am.Chem.Soc.,  39,  934. 
Green,  W.  F. 

(1908)  J.Phys.Chem.,  12,  655-60. 
Greenish,  H.  G. 

(1900)  Pharm.Jour.(Lond.)f  65,  190- 

95- 
Greenish,  H.  G.  and  Smith,  F.  A.  U. 

(1901)  Pharm.Jour.(Lond.),  66,  774- 

777,  806-811. 

(1902)  Pharm.Jour.(Lond.),  68,  510- 

532. 

(1903)  Pharm.Jour.(Lond.),  71,  881. 
Grehant,  N. 

(1894)  Compt.rend.,  118,  594. 
Grb'ger,  Max. 

(1911)  Z.anorg.Chem.,  70,  135. 
Groschuff,  E. 

(1901)  Ber.,  34,  3318. 

(1903)  Ber.,  36,  1791,  4351. 
(1908)  Z.anorg.Chem.,  58,  102,  113. 

(1910)  Chem.Weekblad.,  7,  687. 

(1911)  Z.Elektrochem.,  17,  348. 
Grube,  G. 

(1914)  Z.Elektrochem.,  20,  342. 
Gruttner,  G. 

(1914)  Ber.,  47,  3259. 
Gudzeit,  F. 

(1908)  Z.physiol.Chem.,  56,  150-179. 

(1909)  Z.physiol.Chem.,  60,  27,  38- 

68. 
Guerini,  B. 

(1912)  Thesis,  Lausanne. 
Guerin,  G. 

(1913)  J.pharm.chim.,  [7],  7,  438. 

(1913)  Pharm.Jour.(Lond.),  90,  769. 
Guertler. 

(1904)  Z.anorg.Chem.,  40,  337. 
Guild,  Ed.  J. 

(1907)  Pharm.Jour.(Lond.),  78,  357. 
Guntz,  A.  and  Guntz,  Jr.,  A.  A. 

(1914)  Ann.chim.,  2,  101. 
Gurwitsch,  L. 

(1914)  Z.physik.Chem.,  87,  329. 
Guthrie. 

(1875)  Phil.Mag., 

(1876)  Phil.Mag., 
(1878)  Phil.Mag., 
(1884)  Phil.Mag., 


4],  49,  210. 

i,  366. 
5,  6,  40. 


»  "»  ^ 
,  18, 


30,  504. 


Guthrie,  A. 

(1901)  J.Soc.Chem.Ind.,  20,  224. 
Haber,  F.  and  van  Ordt,  G. 

(1904)  Z.anorg.Chem.,  38,  387. 
Hager. 

(1875)  Chem.Zentralbl.,  135. 

(1903)  "  Handbuch  de  Pharmaceuti- 
schen  Praxis."     3rd.  Ed. 
Hahn. 

(1877)    Wyandotte   Silver   Smelting 

Works. 
Halban,  Hans  v. 

(1913)  Z.physik.Chem.,  84,  129,  145. 
Halberstadt. 

(1884)  Ber.,  17,  2965. 
Hamberg. 

(1885)  J.  prakt.Chem.,  [2],  33,  433. 
Hamberger,  Anna. 

(1906)  Z.anorg.Chem.,  50,  427. 
Hamburger,  E. 

(1911)     Arch.ges.Physiol.(Pfluger's), 

143,  187. 
von  Hammel,  A. 

(1915)  Z.physik.Chem.,  90,  121. 
Hampshire,  C.  H.  and  Pratt,  W.  R. 

(1913)  Pharm.Jour.(Lond.),  91,  140. 
Hanausek. 

(1887)  J.pharm.chim.,  [5],  15,  509. 
Hantzsch,  A. 

(1901)  Verh.d.Vers.Deutsch  Ntf.u. 

Artze,  150-2. 

(1902)  Chem.Zentrbl.,  II,  922. 
(1911)  Ber.,  44,  2006. 

Hantzsch,  A.  and  Sebalt,  F. 

(1899)  Z.physik.Chem.,  30,  258-99. 
Hantzsch,  A.  and  Vagt,  A. 

(1901)  Z.physik.Chem.,  38,  705-742. 
Harkins,  W.  D. 

(1911)    J.Am.Chem.Soc.,    33,    1807- 

1827. 
Harkins,  W.  D.  and  Clark,  Geo.  L. 

(1915)  J.Am.Chem.Soc.,  37,  1816. 
Harkins,  W.  D.  and  Paine,  H.  M. 

(1916)  J.Am.Chem.Soc.,  38,  2709. 
Harkins,  W.  D.  and  Pearce,  W.  T. 

(1916)    J.Am.Chem.Soc.,    38,    2694, 

2717. 
Harkins,  W.  D.  and  Winninghoff,  W.  J. 

(1911)  J.Am.Chem.Soc.,  33,  1827-36. 
Harrass,  Paul. 

( 1 903)  Arch  .internat  .Pharmacodyamie 

et  Therapie,  n,  431-463. 
Hartley,  H. 

(1908)  J.Chem.Soc.(Lond.),  93, 741-5. 
Hartley,  H.  and  Barrett,  W.  H. 

(1909)  J.Chem.Soc.(Lond.),       95, 

1178-85. 

Hartley,  H.,  Drugman,  J.,  Vlieland,  C. 

A.,  and  Bourdillon,  Robt. 

(I9I3)  J.Chem.Soc.(Lond.),  103, 1749. 

Hartley,  H.,  Jones,  B.  M.  and  Hutchin- 

son,  G.  A. 
(1908)  J,Chem.Soc.(Lond.),  93,  825. 


797 


AUTHOR  INDEX 


Hartley,  H.  and  Thomas. 

(1906)  J.Chem.Soc.(Lond.),  89,  1028. 
Haslam. 

(1886)  Chem.News.,  53,  87. 
Hasselblatt,  M. 

(1913)  Z.physik.Chem.,  83,  1-39. 
Hatcher,  R.  A. 

(1902)  Am.Jour.Pharm.,  74,  136. 
Hatcher,  W.  H.  and  Skirrow,  F.  W. 

(i9i7)J.Am.Chem.Soc.,39, 1939-1977. 
v.  Hauer. 

(1858)  J.prakt.Chem.,  74,  433. 
Hauser,  O. 

(1905)  Z.anorg.Chem.,  45,  194. 

(1907)  Z.anorg.Chem.,  54,  196-212. 
Hauser,  O.  and  Wirth,  F. 

(1908)  Z.anal.Chem.,  47,  389. 

(1909)  J.prakt.Chem.,  [2]  79,  358-68. 
(i9O9a)  Z.angew.Chem.,  22,  484. 
(1912)  Z.anorg.Chem.,  78,  75-94. 

Heath,  W.  P. 

(1915)  Privately   Printed,    Atlanta, 

Ga. 
Hehner,  O.  and  Mitchell,  C.  A. 

(1897)  J.Am.Chem.Soc.,  19,  40. 
van  der  Heide. 

(1893)  Z.  physik.Chem.,  12,  418. 
Heintz. 

(1854)  Pogg.Annalen,  92,  588. 
Heise,  G.  W. 

(1912)  J.Phys.Chem.,  16,  373. 
Helff,  A. 

(1893)  Z.physik.Chem.,  12,  217. 
Hellwig. 

(1900)  Z.anorg.Chem.,  25,  166-183. 
Hempel,  W. 

(1901)  Z.angew.Chem.,  14,  865. 
Hempel,  W.  and  Tedesco,  H. 

(1911)  Z.angew.Chem.,  24,  2469. 
Henderson,  W.  N.  and  Taylor,  H.  S. 

(1916)  J.Phys.Chem.,  20,  670. 
Hendrixon,  W.  S. 

(1897)  Z.anorg.Chem.,  13,  73. 
Henkel,  H. 

(1905)  Dissertation,  Berlin. 

(1912)  Landolt      &      Bernstein's, 

"  Tabellen,"  4th  Ed.,  602. 
Henry. 

(1884)  Compt.rend.,  99,  1157. 
Herold,  J. 

(1905)  Z.Elektrochem,  n,  417. 
Herrmann,  Gottfried. 

(1911)  Z.anorg.Chem.,  71,  257-302. 
Herz,  W. 

(1898)  Ber.,  31,  2671. 

(1900)  Z.anorg.Chem.,  25,  155. 

(1902)  Z.anorg.Chem.,  30,  281. 

(1903)  Z.anorg.Chem.,  33,  355. 
(1903)  Z.anorg.Chem.,  34,  205. 
(1905)  Dissertation  (Berlin). 
(1910)  Z.anorg.Chem.,  68,  69,  165. 
(i9ioa)  Z.anorg.Chem.,  66,  93,  358. 
(19100)  Z.anorg.Chem.,  65,  341-4. 


Herz,  W. 

(19100)  Z.anorg.Chem.,  67,  365. 

(1911)  Z.anorg.Chem.,  70,  70,  170. 

(191  la)  Z.anorg.Chem.,  71,  206. 

(191  ib)  Z.anorg.Chem.,  72,  106. 

(1911-12)  Z.anorg.Chem.,  73,  274. 

(1917)  Z.Elektrochem.,  23,  23-4. 
Herz,  W.  and  Anders,  G. 

(1907)  Z.anorg.Chem.,   52,    164-72, 

271-8. 
Herz,  W.  and  Bulla,  A. 

(1909)  Z.anorg.Chem.,  63,  282-4. 

(1911)  Z.anorg.Chem.,  71,  255. 
Herz,  W.  and  Fischer,  H. 

(1904)  Ber.,  37,  4747. 

(1905)  Ber.,  38,  1140. 
Herz,  W.  and  Knoch. 

(1904)  Z.anorg.Chem.,  41,  319. 

(1905)  Z.anorg.Chem.,  45,  263-8. 
Herz,  W.  and  Kuhn.  F. 

(1908)  Z.anorg.Chem.,  58,  159-67. 

(1908)  Z.anorg.Chem.,  60,  152-62. 
Herz,  W.  and  Kurzer,  A. 

(1910)  Z.Elektrochem..  16,  240,  869. 
Herz,  W.  and  Lewy. 

(1905)  Z.Elektrochem.,  n,  818. 
Herz,  W.  and  Muhs,  G. 

(1903)  Ber.,  36,  3717. 
Herz,  W.  and  Paul,  W. 

(1913)  Z.anorg.Chem.,  82,  431. 

(1914)  Z.anorg.Chem.,  85,  214. 
Herz,  W.  and  Rathmann,  W. 

(1913)  Z.Elektrochem.,  19,  553,  887. 
Herzfeld. 

(1892)  Z.Ver.Zuckerind.,  181. 

(1897)  Z.Ver.Zuckerind.,  34,  820. 
von  Hevesy,  Geo. 

(1900)  Z.physik.Chem.,  73,  537. 

(1909)  Z.Elektrochem.,  15,  529. 

(1911)  Phys.Ztschr.,  12,  1214. 

(1912)  J.Phys.Chem.,  16,  429. 
von  Hevesy,  G.  and  Rona,  E. 

(1915)  Z.physik.Chem.,  89,  303. 
Hicks,  W.  B. 

(1915)  J.Am.Chem.Soc.,  37,  844. 
Hildebrand,  J.  H.,  Ellefson,  E.  T.  and 

Beebe,  C.  W. 

(1917)  J.Am.Chem.Soc.,  39,  2302. 
Hill,  A.  E. 

(1908)  J.Am.Chem.Soc.,  30,  68-74. 
(1917)  J.Am.Chem.Soc.,  39,  218-31. 

Hill,  A.  E.  and  Simmons,  J.  D. 

(1909)  J.Am.Chem.Soc.,  31,  821-39. 
(1909)  Z.physik.Chem.,  67,  594-617. 

Hill,  A.  E.  and  Zink,  W.  A.  H. 

(1909)  J.Am.Chem.Soc.,  31,  44. 
Hill,  C.  A.  and  Cocking,  T.  T. 

(1912)  Pharm.Jour.(Lond.),  89,  155. 
Hill,  J.  Rutherford. 

(1900)  Pharm.Jour.(Lond.),  64,  185. 
Hilpert,  S. 

(1916)  Z.angew.Chem.,  29,  I,  57-9. 
(1916)  Chem.Abs.,  10,  1924. 

798 


AUTHOR  INDEX 


Hinrichsen,  F.  W.  and  Sachsel,  E. 

(1904-05)  Z.physik.Chem.,  50,81-99. 
His,  W.  Jr.  and  Paul,  T. 

(1900)    Z.physiol.Chem.,    31,    1-42, 

64-78. 
Hissink,  D.  J. 

(1900)  Z.physik.Chem.,  32,  557. 
Hitchcock,  F.  R.  M. 

(1895)  J.Am.Chem.Soc.,  17,  529. 
van't  Hoff,  J.  H. 

(1901)  Sitzber.k.Akad.Wiss. (Berlin), 

P-  1035. 

(1905)  Z.anorg.Chem.,  47,  247. 

(1912)  "  Untersuchungen  iiber  die 
Bildungsverhaltnisse  der 
Ozeanischen  Salzablager- 
ungen,  inbesondere  des 
Staasfurter  Salzlagers." 
von  J.  H.  van't  Hoff  et  al 
Herausgegeben  von  H. 
Precht  &  E.  Cohn. 
(Leipzig,  1912). 
van't  Hoff,  J.  H.  and  Goldschmidt,  H. 

(1895)  Z.physik.Chem.,  17,  508. 
van't  Hoff,  J.  H.  and  Meyerhofifer,  W. 

(1898)  Z.physik.Chem.,  27,  75. 

(1899)  Z.physik.Chem.,  30,  64-88. 
van't  Hoff,  J.  H.  and  Kenrick,  F.  B. 

(1912)  "  Ozeanischen  Salzablagerun- 

gen,"  pp.  37-40. 
Hoffmann,  Fr.  and  Langbeck,  K. 

(1905)  Z.physik.Chem.,  51,  303,  393, 

412. 

Hofmann,  K.  A.,  Hobold,  K.  and  Quoos. 
(1911-12)    Liebig's  Ann.,    386,304- 

3!7- 
Hofmann,  K.  A.  and  Hobold,  K. 

(1911)  Ber.,  44,  1776. 

Hofmann,  K.  A,,  Kirmireuther,  K.  and 

Thai,  A. 

(1910)  Ber.,  43,  188. 
Hofman,  K.  A.,  Roth,  R.,  Hobold,  K. 

and  Metzler,  A. 
(1910)  Ber.,  43,  2628. 
Hoglund,  A.  T. 

(1912)  Z.Ver.Zuckerind.,  1118-1127. 
Hoitsema,  C. 

(1895)  Z.physik.Chem.,  17,  651. 
(1898)  Rec.trav.chim.,  17,  310. 
(18983)  Z.physik.Chem.,  27,  315. 

Holde,  D. 

(1910)  Z.Elektrochem.,  16,  442. 
Holland,  A. 

(1897)  Ann. chim. anal.,  2,  243. 
Holleman,  A.  F. 

(1893)  Z.physik.Chem.,  12,  135. 

(1896)  Rec.trav.chim.    15,  159. 

(1898)  Rec.trav.chim.    17,  247,  324. 
(1910)  Rec.trav.chim.   29,  396. 


(1913)  Rec.trav.chim. 

(1914)  Rec.trav.chim. 


136. 
6-29. 


Holleman,  A.  F.  and  van  den  Arend,  J.  E. 
(1909)  Rec.trav.chim.,  28,  411. 


Holleman,  A.  F.  and  Antusch,  A.  C. 

(1894)  Rec.trav.chim.,  13,  293. 
Holleman,  A.  F.  and  de  Bruyn,  B.  R. 

(1900)   Rec.trav.chim.,   19,  83,   191, 

365. 
Holleman,  A.  F.  and  Caland,  P. 

(1911)  Ber.,  44,  2506. 
Holleman,  A.  F.,  Hartogs,  J.  C.,  and 

van  der  Linden,  T. 
(1911)  Ber.,  44,  705. 
Holleman,  A.  F.  and  Huisinga,  J. 
(1908)  Rec.trav.chim.,  27,  275. 
Holleman,  Kohlrausch  and  Rose. 

(1893)  Z.physik.Chem.,     12,     129, 

241. 
Holleman,  A.  F.  and  van  der  Linden,  T. 

(1911)  Rec.trav.chim.,  30,  318. 
Holleman,  A.  F.  and  Pollak,  J.  J. 

(1910)  Rec.trav.chim.,  29,  429. 
Holleman,  A.  F.  and  Rinkes,  I.  J. 

(1911)  Rec.trav.chim.,  30,  55. 
Holleman,  A.  F.  and  Sluiter,  C.  H. 

(1906)  Rec.trav.chim.,  25,  212. 
Holleman,  R. 

(1903)  Z.physik.Chem.,  43,  129-159. 
(1905-06)   Z.physik.Chem.,   54,  98- 

no. 
Holmberg,  O. 

(1907)  Z.anorg.Chem.,  53,  83-134. 
Holt,  A.  and  Bell,  N.  M. 

(1914)  J.Chem.Soc.(Lond.),  105,  633. 
Holty,  J.  G. 

(1905)  J.Phys.Chem.,  9,  764. 
Homfray,  I.  F. 

(1910)  J.Chem.Soc.(Lond.),97,  1669. 
Hooper. 

(1882)  Pharm.J.(Lond.),  [3],  13,  258. 
Horiba,  S. 

(191 1-12)  Mem.Coll.Sci.Eng.(Kyoto), 
3,  63-78. 

(1914-16)    Mem.Coll.Sci. (Kyoto),  I, 

Horn,  D.  W. 

(1907)  Am.Chem.Jour.,  37,  471. 
Horn,  D.  W.  and  Van  Wagener. 

(1903)  Am.Chem.Jour.,  30,  347. 
Houston  and  Trichborne. 

(1890)  Brit.Med.Jour.,  1063. 
Howe,  Jas.  L. 

(1894)  J.Am.Chem.Soc.,  16,  388. 
Hudson,  C.  S. 

[1904)  J.Am.Chem.Soc.,  26,  1072. 
'1908)  J.Am.Chem.Soc.,  30,  1767-83. 

Hudson,  C.  S.  and  Yanovsky,  E. 

(1917)  J.Am.Chem.Soc.,  39,  1037. 
Huecke. 

(1884)  J.prakt.Chem.,  [2],  29,  49. 
Hiifner,  G. 

(1895)  Archiv.anat.u.physiol.,    209- 

212. 

(1906-07)  Z.physik.Chem.,  57,  615- 

622. 
(1907)  Z.physik.Chem.,  59,  416. 


799 


AUTHOR  INDEX 


Hiifner,  G.  and  Kulz. 

(1895)  J.prakt.Chem.,  28,  256. 
Hulett,  G.  A. 

(1901)  Z.physik.Chem.,  37,  406. 
Hulett,  G.  A.  and  Allen,  L.  E. 

(1902)  J.Am.Chem.Soc.,  24,  674. 
Hunt. 

(1870)  Am.Jour.Sci.,  [2],  40,  154. 
Hiittig,  Gustav,  F. 

(1914)  Z.physik.Chem.,  87,  144.  * 
Ulingworth,  B.  and  Howard,  A. 

(1884)  Phil.Mag.,  [5],  18,  124. 
Imadsu,  A. 

(1911-12)       Mem.Coll.Sci.Eng.  (Ky- 
oto), 3,  257-63- 
Inglis,  J.  K.  H. 

(1903)  J.Chem.Soc.(Lond.),  83,  1010. 
Irving  and  Young. 

(1888)  J.Chem.Soc.(Lond.),  56,  344. 
Isaac,  Florence. 

(1908)  J.Chem.Soc.(Lond.),  93,  398, 

927. 
(1910)  Proc.Roy.Soc.(Lond.),  84,  A, 

348. 

(1913)  Proc.Roy.Soc.(Lond.),  88,205. 
van  Itallie,  E.  J. 

(1908)  Z.anorg.Chem.,  60,  358-65. 
van  Iterson-Rotgans,  J.  W. 

(1913)  Chem.Weekblad.,  10,  920-37. 

(1914)  Z.physik.Chem.,  87,  305. 
Iwaki,  J. 

(1914)  Mem.Coli.Sci.(Kyoto),  i,  81-8. 
Iwig  and  Hecht. 

(1886)  Liebig's  Ann.,  233,  167. 
Jackson,  R.  F. 

(1914)  J.Am.Chem.Soc.,  36,  2350. 

(1914)  Bull.BureauStandards,  2,  331- 

Jacobs,  W.     34' 

(1917)  Chem.Weekblad.,  14,  208-12. 
Jacobson,  C.  A.  and  Holmes,  A. 

(1916)  J.Biol.Chem.,  25,  29-53. 
Jaeger,  A. 

(1901)  Z.anorg.Chem.,  27,  25. 
Jaeger,  F.  M. 

(1904)  Z.Kryst.Min.,  38,  583. 

(1905)  Proc.k.Akad.Wet.(Amst.),  7, 

665. 

(1906)  Proc.k.Akad.Wet.(Amst.)f  8, 

618. 

(1907)  Z.Kryst.Min.,  42,  236-76. 

(1907)  Rec.trav.chim.,  26,  329. 

(1908)  Proc.k.Akad.Wet.(Amst.), 436. 
(1912)  8th  Int.Cong.Appl.Chem.,  2, 

139- 
Jaeger,  F.  M.  and  Doornbosch,  H.  J.  D. 

(1912)  Z.anorg.Chem.,  75,  261. 
Jaeger,  F.  M.  and  van  Klooster,  H.  S. 

(1912)  Z.anorg.Chem.,  78,  245. 
Jaeger,  F.  M.  and  van  Kregten,  J.  R.  N. 
(1912)  Proc.k.Akad.Wet.(Amst.),  14, 
733. 


Jaeger,  F.  M.  and  Menke,  J.  B. 

(1912)  Z.anorg.Chem.,  75,  241-260. 
(1912)  Proc.k.Akad.Wet.(Amst.),  14, 

724. 
Jaenecke,  E. 

(1908)  Z.physik.Chem.,  64,  343. 

(1912)  Z.physik.Chem.,  80,  I. 
Jakowkin,  A.  A. 

(1895)  Z.physik.Chem.,  18,  588. 

(1896)  Z.physik.Chem.,  20,  38. 
(1899)  Z.physik.Chem.,  29,  630. 

James,  C.  and  Holden,  H.  C. 

(1913)  J.Am.Ch,em.Soc.,  35,  559. 
James,  C.  and  Pratt,  L.  A. 

(1910)  J.Am.Chem.Soc.,  32,  873. 
James,  C.  and  Robinson,  J.  E. 

(1913)  J.Am.Chem.Soc.,  35,  754. 
James,  C.  and  Whittemore,  C.  F. 

(1912)  J.Am.Chem.Soc.,  34,  1168. 
James,    C.,    Whittemore,    C.    F.    and 
Holden,  H.  C. 

(1914)  J.Am.Chem.Soc.,  36,  1854. 
James,  C.  and  Willand,  P.  S. 

(1916)  J.Am.Chem.Soc.,  38,  1499. 
Jantsch,  G. 

(1912)  Z.anorg.Chem.,  76,  321. 
Jantsch,  G.  and  Griinkraut,  A. 

(1912-13)   Z.anorg.Chem.,   79,  309- 

321. 
Jaques,  A. 

(1910)  Trans.FaradaySoc.,  5,  235. 
Jarry,  R. 

(1897)  Compt.rend.,  124,  288-91. 
(1899)  Ann.chim.phys.,  [7],  17,  342. 

Jellinek,  K. 

(1911)  Z.anorg.Chem.,  70,  86-134. 
Jensen,  H.  R. 

(1913)  Pharm.Jour.(Lond.),  90,  658- 

60. 
Jo,  Inohiko. 

(1911)  Mem. coll. sci.Eng. (Kyoto),  3, 

41-9,  212. 

(1912)  Tokyo  Chem.Soc.,  33,  No.  7, 

July. 
Joannis,  A. 

(1882)  Ann.chim.phys.,  [5],  26,  489. 

(1906)  Ann.chim.phys.,  [8],  7,  41. 
Johnson. 

(1886)  Chem.News.,  54,  75. 
Johnston,  J. 

(1915)  J.Am.Chem.Soc.,    37,   2001- 

2020. 
Johnston,  J.  and  Williamson,  E.  D. 

(1916)  J.Am.Chem.Soc.,  38,  975-83. 
Jolin. 

(1889)  Arch.anat.u.physiol.,  262. 
Jones,  B.  M. 

(1908)  J.Chem.Soc.(Lond.),  93,  1744. 
Jones,  Grinnel,  and  Hartman,  M.  L. 

(1915)  J.Am.Chem.Soc.,  37,  241. 

(1916)  Trans.  Am. Electrochem.Soc., 

30,  295-326. 


800 


AUTHOR  INDEX 


Jones,  H.  C. 

(1907)  Carnegie  Publication  No.  60, 

Washington,  D.C. 
Jones,  H.  O. 

(1907-98)  Proc. Cambridge  Phil.Soc., 

14,  27-9. 
Jones,  W.  J. 

(1911)  J.Chem.Soc.(Lond.),  99,  392. 
de  Jong,  A.  W.  K. 

(1909)  Rec.trav.chim.,  28,  343. 

(1912)  Rec.trav.chim.,  31,  256. 
Jb'rgensen. 


20,  195. 
30,  i. 
2J,  42,  208. 


(1879)  J.prakt.Chem., 

(1884)  J.prakt.Chem., 
(1890)  J.prakt.Chem., 

Joulin. 

(1873)  Ann.chim.phys.,  [4],  30,  260. 
Journiaux,  M. 

(1912)  Bull. soc.chim. (Paris),  [4],  u, 

129,  516,  546-52. 
Joyner,  R.  A. 

(1912)  Z.anorg.Chem.,  77,  108. 
Jungfleisch,  E. 

(1912)  Compt.rend.,  155,  801. 
Jungfleisch,  E.  and  Landrieu,  Ph. 

(1914)  Ann.chim.,  2,  1-56,  333. 

(i9i4a)  Compt.rend.,  158,  1306-11. 
Jiirgens. 

(1885)  Jahresber.Chem.,  1722. 
Just,  G. 

(1901)  Z.physik.Chem.,  37,  342-367. 
Juttner,  F. 

(1901)  Z.physik.Chem.,  38,  56-75. 
Kachler,  M.  J. 

(1870)  Bull. soc.chim.,  13,  460. 
Kahlenberg,  L.  and  Brewer,  R.  K. . 

(1908)  J.Phys.Chem.,  12,  283-9. 
Kahlenberg,  L.  and  Krauskopf,  F.  C. 

(1908)  J.Am.Chem.Soc.,  30,  1104-15. 
Kahlenberg,  L.  and  Wittich,  W.  J. 

(1909)  J.Phys.Chem.,  13,  421-5. 
Kahlukow,  I.  and  Sachanow,  A. 

(I9°9)    J.Russ.Phys.Chem.Soc.,    41, 

1755- 
Karandeeff,  B. 

(1909)  Zentralbl.Min.Geol.,  p.  728. 

(1910)  Z.anorg.Chem.,  68,  188. 
Karl,  G. 

(1910)  Z.anorg.Chem.,  68,  57. 
Karplus. 

(1907)  Dissertation,  Berlin. 

Landolt  &  Bornstein's  "  Tab- 

ellen  "  4th  Ed.,  p.  563. 
Karsten. 

(1864-5)       Ann.der  Chem.u.Pharm. 

Suppl.Bd.,  3,  170. 
Karsten,  B.  J. 

(1907)  Z.anorg.Chem.,  53,  367. 
Katz,  S.  H.  and  James,  C. 

(1913)  J.Am.Chem.Soc.,  35,  872. 
Kendall,  J. 

(1911)  Proc.Roy.Soc.(Lond.),  A,  85, 

200-19. 


Kendall,  J. 

(1912)  PJiil.Mag.  [6],  23,  958. 

(1914)  J.Am.Chem.Soc.,  36,  1722. 

(i9i4a)  J.Am.Chem.Soc.,  36,  1222. 

(1916)     .Am.Chem.Soc.,  38,  1309. 
Kendall,  J.  and  Booge,  J.  E. 

(1916)  .Am.Chem.Soc.,  38,  1712. 
Kendall,    .  and  Carpenter,  C.  D. 

(1914)  .Am.Chem.Soc.,  36,  2502. 
Kendall,    .  and  Gibbons,  W.  A. 

(1915)  J.Am.Chem.Soc.,  37,  149. 
Keppish. 

•    (1888)  Monatsh.Chem.,  9,  589. 
Kernot,  G.,  d'Agostino,  E.  and  Pelle- 
grino,  M. 

(1908)  Gazz.chim.ital.,  38,  I,  532-54. 
Kernot,  G.  and  Pomilio,  M. 

(1912)     Rend.accad.sci.fis.nat.(Nap- 

oli),  [3],  17,  353-8. 
Ketner. 

(1901-02)  Z.physik.Chem.,  39,  645. 
Keyes,  D.  B.  and  Hildebrand,  J.  H. 

(1917)  J.Am.Chem.Soc.,  39,  2129. 
Keyes,  D.  B.  and  James,  C. 

(1914)  J.Am.Chem.Soc.,  36,  634. 
King,  Chas.  A.  and  Narracott,  P. 

(1909)  Analyst,  34,  436-8. 
King,  H.  and  Orton,  K.  P.  J. 

(1911)  J.Chem.Soc.(Lond.),99,  1381. 
King,  Harold  and  Pyman,  F.  L. 

(1914)      J.Chem.Soc.(Lond.),      105, 

1238-59. 
Kirschner,  A. 

(1912)  Z.physik.Chem.,  79,  247. 
Klaus. 

(1905)  Phys.Ztschr.,  6,  820. 
Klein,  O. 

(1912)  Z.anorg.Chem.,  74,  158. 
Kleven. 

(1872)  Chem.Centralbl.,  434. 
Klobbie,  E.  A. 

(1897)  Z.physik.Chem.,  24,  623. 
van  Klooster,  H.  S. 

(1910-11)    Z.anorg.Chem.,    69,    122, 

135-57. 

(1912-13)  Z.anorg.Chem.,  79,  223-9. 
(1917)  J.Phys.Chem.,  21,  513-18. 
Klose,  G. 

( 1 907 )  Archi v.  I nternat .  Pharmacody- 
namie    et    Therapie,    17, 

459-63. 
Knietsch,  R. 

(1901)  Ber.,  34,  4099. 
Knopp. 

(1904)  Z.physik.Chem.,  48,  97-108. 
Knox,  Joseph. 

(1909)  J.Chem.Soc.(Lond.),  95, 1760. 
Kobayashi,  M. 

(1911-12)       Mem. Coll. Sci.Eng.  (Ky- 
oto), 3,  218. 
de  Kock,  A.  C. 

(1904)  Z.physik.Chem.,  48,  131. 


801 


AUTHOR   INDEX 


Kofler,  M. 

(1913)  Monatsh.Chem.,  34,  389. 

(1913)     Sitzber.k.Akad.Wiss.(Wien) 
Abt.,  I  la,  122,  1473-80. 
Kohler. 

(1879)  Z.anal.Chem.,  18,  242. 
Kohler. 

(1897)  Z.Ver.Zuckerind.,  47,  447. 
Kohlrausch,  Fr. 

(1879)  Wied.Ann.,  i. 

(1891)  Ber.,  24,  3561. 

(1891)  Wied.Ann.,  44,  577. 

(1897)  Sitzber.k.Akad.Wiss. (Berlin), 

90. 

(1903)  Z.physik.Chem.,  44,  197. 
(1904-05)  Z.physik.Chem.,  50, 355-6. 

(1908)  Z.physik.Chem.,  64,  121-69. 
Kohlrausch,  F.  and  Rose,  F. 

(1893)  Z.physik.Chem.,  12,  129,  135, 

241. 
Kohn,  M. 

(1909)  Z.anorg.Chem.,  63,  337-9. 
Kohn,  M.  and  O'Brien. 

(1898)  J.Soc.Chem.Ind.,  17,  100. 
Kohn,  M.  and  Klein,  A. 

(1912)  Z.anorg.Chem.,  77,  254. 
Kohnstamm  and  Cohn. 

(1898)  Wied.Ann.,  65,  344. 
Kohnstamm,  Ph.  and  Timmermans,  J. 

(i9i3)Proc.k.Akad.Wet.(Amst.),i02i. 
Kolb. 

(1872)  Bull.soc.ind.Mulhouse,  222. 
de  Kolossovsky,  N. 

(1911)   Bull. soc.chim. (Paris),   [4],  9, 
632-7. 

(1911)  Bull.soc.chim.(Belg.),  25,  183, 

235- 
Kolthoff,  I.  M. 

(1917)  Chem.Weekblad.,  14,  1081. 
Konig. 

(1894)  Monatsh.Chem.,  15,  23. 
de  Koninck,  L.  L. 

(1907)  Bull.soc.chim.(Belg.),  21,  141. 
Konowalow,  D. 

(1898)      Jour.Russ.Phys.Chem.Soc., 

W,  30,  367- 

(1898)  Chem.Zentralbl.,  II,  659. 
(i899a)  Jour.  Russ.  Phys.Chem.Soc., 

3i»  910- 
(i899b)    Jour.Russ.Phys.Chem.Soc., 

3i»  985. 

(1900)  Chem.Zentralbl.,  I,  646. 
(igoob)  Chem.Zentralbl.,  I,  938. 

(1903)  Ann.Phys.(Wied.),  [41,10,375, 
Koopal,  S.  A. 

(1911)  Dissertation,  Leyden,  p.  128. 
(1911)   "Tables  annuelles,"  2,  463. 
Koppel,  J. 

(1901-02)  Z.physik.Chem.,  42,  8. 

(1904)  Z.anorg.Chem.,  41,  377. 

(1905)  Z.physik.Chem.,  52,  405. 

(1906)  Ber.,  39,  3738. 


Koppel,  J.  and  Blumenthal,  R. 

(1907)  Z.anorg.Chem.,  53,  228-67. 
Koppel,  J.  and  Cahn,  M. 

(1908)  Z.anorg.Chem.,  60,  53-112. 
Koppel- Gumpery. 

(1905)  Z.physik.Chem.,  52,  413. 
Koppel,  J.  and  Holtkamp,  H. 

(1910)  Z.anorg.Chem.,  67,  274. 
Koppel-Wetzel. 

(1905)  Z.physik.Chem.,  52,  395. 
Korreng,  E. 

(1914)  Neues   Jahrb.Min.Geol.(Beil 

Bd.),  37,  51-124. 

(1915)  Z.anorg.Chem.,  91,  194. 
Krasnicki. 

(1887)  Monatsh.Chem.,  8,  597. 
Kremann,  R. 

(1904)  Monatsh.Chem.,    25,    1242- 

1324. 

(1905)  Monatsh.Chem.,  26,  143. 

(1906)  Monatsh.Chem.,  27,  91-107, 

125-80,  627. 

(1907)  Monatsh.Chem.,  28,  8,  895, 

1125. 

(1908)  Jahrber.k.geol.Reichsanstalt 

(Wien),  58,  662. 

(1909)  "The  Use  of  Thermic  Analysis 

for  the  Detection  of  Chemical 
Compounds,"  Sammlung 
Chem.  u.  Chem.-Techn.  Vor- 
trage,XIV,6-7,  pp.  213-288 
(F.  Enke,  Stuttgart). 

(1910)  Monatsh.Chem.,  31,  843,  855. 
(i9ioa)  Monatsh.Chem.,  31,  275. 

(1911)  Monatsh.Chem.,  32,  609. 

(         )    Sitzber.k.Akad.Wiss.(Wien), 

120,  lib,  329. 
Kremann,  R.  et  al. 

(1908)  Monatsh.Chem.,  29,  863-91. 
Kremann,  R.  and  Borjanovics,  V. 

(1916)  Monatsh.Chem.,  37,  59-84. 
Kremann,  R.,  Daimer  and  Beunesch. 

(1911)  Monatsh.Chem.,  32,  620. 
Kremann,  R.  and  Ehrlich. 

(1908)     Jahrber.k.geol.Reichsanstalt 

(Wien),  58,  569. 
Kremann,  R.  and  Hofmeier,  F. 
(1908)  Monatsh.Chem.,  29,  mi. 
(1910)  Monatsh.Chem.,  31,  201. 
Kremann,  R.  and  Huttinger,  K. 

( 1 908)    Jahrber. k.Geol. Reichsanstalt 

(Wien),  58,  637. 
Kremann,  R.  and  Janetzky,  E. 

(1912)  Monatsh.Chem.,  33,  1055-62. 
Kremann,  R.  and  Kerschbaum,  F. 

(1907)  Z.anorg.Chem.,  56,  218-22. 
Kremann,  R.  and  Klein,  H. 

(1913)  Monatsh.Chem.,  34,  1291. 
Kremann,  R.  and  Kropsch,  R. 

(1914)  Monatsh.Chem.,  35,  561,  823, 

841. 
Kremann,  R.  and  Noss,  F. 

(1912)  Monatsh.Chem.,  33,  1205. 


802 


AUTHOR  INDEX 


Kremann,  R.  and  Rodemund,  H. 
(1914)    Monatsh.Chem.,    35,    1065- 
1086. 

(1914)  Z.anorg.Chem.,  86,  373. 
Kremann,  R.  and  Rodinis,  O. 

(1906)  Monatsh.Chem.,  27,  125-180. 
Kremann,  R.  and  Schoulz,  R. 

(1912)    Monatsh.Chem.,    33,    1063, 

1081. 
Kremann,  R.  Wischo,  F.  and  Paul,  R. 

(1915)  Monatsh.Chem.,  36,  915. 
Kremann,  R.  and  Zitek,  A. 

(1909)  Monatsh.Chem.,  30,  311-40. 
Kremers. 

(1852)  Pogg.Ann.,  85,  248. 

(1854)  Pogg.Ann.,  92,  497. 

(1855)  Pogg.Ann.,  94,  271;  95,  468. 
1856)  Pogg.Ann.,  99,  47. 

i856a)  Pogg.Ann.,  97,  5. 
1858)  Pogg.Ann.,  103,  57,  133,  165. 
(1858)  Pogg.Ann.,  104,  133. 
(1860)  Pogg.Ann.,  in,  60. 
Kreusler  and  Herzhold. 

(1884)  Ber.,  17,  34. 
Krug,  W.  H.  and  Cameron,  F.  K. 

(1900)  J.Phys.Chem.,  4,  188. 
Krug,  W.  H.  and  McElroy,  K.  P. 

(1892)  J.Anal.Ch.,  6,  184. 
Krusemann,  H.  D. 

(1876)  Ber.,  9,  1467. 
Kriiss,  G.  and  Nilson,  L.  F. 

(1887)  Ber.,  20,  1696. 
Kruyt,  H.  R. 

(1908)  Z.physik.Chem.,  64,  513. 
(1908-09)  Z.physik.Chem.,  65,  497. 
(1912)  Z.physik.Chem.,  79,  667. 

Krym,  V. 

(1909)  J.Russ.Phys.Chem.Soc.,    41, 

382-5;  Chem.Zentr.,  II,  68 1. 
Kulisch. 

(1893)  Monatsh.Chem.,  14,  567. 
Kultascheff. 

(1903)  Z.anorg.Chem.,  35,  187. 
Kumpf. 

(1882)  Wied.Ann.Beibl.,  6,  276. 
Kunheim  and  Zimmerman. 

(1884)  Dingler.polyt.J.,  252,  478. 
Kunschert,  F. 

(1904)  Z.anorg.Chem.,  41,  338. 
Kuriloff,  B. 

(1897)  Z.physik.Chem.,  24,  441-467. 
(i897a)  Z.physik.Chem.,  23,  93,  547, 

673. 

(1898)  Z.physik.Chem.,  25,  419-440. 
Kurnakov,  N.  S.  and  Efrenov,  N.  N. 

(1912)      Jour.Russ.Phys.Chem.Soc., 

44,  1992-2000. 
(1912)  Ann.Inst.Polyt.(Petrograd), 

18,  105. 
Kurnakov,  J.,  Krotkov,  D.  and  Oksman, 

M. 
(1915)      Jour.Russ.Phys.Chem.Soc., 

47,  558-88. 


Kurnakov,  H.  and  Kviot,  I. 

(1913)     Ann.Inst.Polyt.(Petrograd), 

20,  664. 
Kurnakov,  N.  S.  and  Solovev,  V. 

(1916)  J.Russ.Phys.Chem.Soc.,    48, 

1338. 
Kurnakov,  N.   S.  and  Wrzesnewsky, 

J.  B. 

(1912)  Z.anorg.Chem.,  74,  89. 
Kurnakov,  N.  S.  and  Zemcznzny. 
(1907)  Z.anorg.Chem.,  52,  186. 
Kiister,  F.  W. 

(1890)  Z.physik.Chem.,  5,  601. 

(1891)  Z.physik.Chem.,  8,  577. 
(1895)  Z.physik.Chem.,  17,  357. 

Kiister,  F.  W.  and  Dahmer,  Geo. 

(1905)  Z.physik.Chem.,  51,  240. 
Kiister,  F.  W.  and  Heberlein,  E. 

(1905)  Z.anorg.Chem.,  43,  56. 
Kiister,  F.  W.  and  Kremann,  R. 

(1904)  Z.anorg.Chem.,  41,  19, 
Kiister  and  Thiel. 

(1899)  Z.anorg.Chem.,  21,  116. 

(1903)  Z.anorg.Chem.,  33,  139. 
Kiister,  F.  W.  and  Wiirfel,  Walter. 

(1904-5)  Z.physik.Chem.,  50,  70. 

van  der  Laan,  F.  H. 

(1907)  Rec.trav.chim.,  26,  29. 
Lachaud,  M.  and  Lepierre,  C. 

(1891)  Bull.soc.chim.,  [3],  6,  230-5. 
Ladenburg,  A. 

(1902)  Ber.,  35,  1256. 
Ladenburg,  A.  and  Doctor,  G. 

(1899)  Ber.,  32,  50. 
Ladenburg,  A.  and  Herz,  W. 

(1898)  Ber.,  31,  937. 
Ladenburg,  A.  and  Sobecki. 

(1910)  Ber.,  43,  2375. 
Lai  De,  R. 

(1917)  J.Chem.Soc.(Lond.),  in,  55. 
Lami,  Pio. 

(1908)  Chem.Zentr.,  II,  755. 
(1908)  Boll. chim. farm.,  47,  435-441. 

Lamouroux,  F. 

(1899)  Compt.rend.,  128,  998. 
Lamy. 

(1863)  Ann.chim.phys.,  [3],  67,  408. 
(1878)  Ann.chim.phys.,  [5],  14,  145. 
Landau,  M. 

(1893)  Monatsh.Chem.,  14,  712. 
(1910)  Z.physik.Chem.,  73,  200-11. 

Landolt  and  Bprnstein. 

(1912)  Physikalisch-Chemische  Tab- 

ellen,  4th  Ed. 
Langheld,  K.  and  Oppmann,  F. 

(1912)  Ber.,  45,  3753. 
Lassaigne. 

(1876)  J.chim.med.,  12,  177. 
von  Laszczynski,  St. 

(1894)  Ber.,  27,  2285. 
Laurie,  A.  P. 

(1912)  Proc.Roy.Soc.(Edin.),  31,388. 


AUTHOR  INDEX 


Lautz,  H. 

(1913)  Z.physik.Chem.,  84,  633. 
Laws,  E.  G.  and  Sidgwick,  N.  V. 

(1911)  J.Chem.Soc.(Lond.),  99,  2088. 
Leather,  J.  W.  and  Mukerji,  J.  M. 

(1913)  Mem. Dept.Agr. (India),  Chem. 

Sen,  3,  177-204. 
Leather,  J.  W.  and  Sen,  J.  N. 

(1909)  Mem.  Dept.Agr.  (India),  Chem. 
Sen,  i,  117-131. 

(1914)  Mem.  Dept.Agr.  (India),  Chem. 

Sen,  3,  205-34. 
Lebeau,  P. 

(1906)  Ann.chim.phys.,  [8],  9,  482-4. 

(1911)  Compt.rend.,  152,  440. 
Lebedew,  P. 

(1911)  Z.anorg.Chem.,  70,  302,  316. 
LeBlanc,  M.  and  Novotny,  K. 

(1906)  Z.anorg.Chem.,  51,  181-201. 
LeBlanc,  M.  and  Noyes,  A.  A. 

(1890)  Z.physik.Chem.,  6,  386. 
LeBlanc,  M.  and  Schmandt,  W. 

(1911)  Z.physik.Chem.,  77,  621-30. 
Lecat. 

(1909)  These,  Brussels. 
LeChatelier. 

(1894)  Compt.rend.,   118,  350,  709, 
800. 

(1897)  Compt.rend.,  124,  1094. 
de  Leeuw,  H.  L. 

(1911)  Z.physik.Chem.,  77,  311. 
van  Leeuwen,  J.  Docters. 

(1897)  Z.physik.Chem.,  23,  44. 
Lefort. 

(1878)  Ann.chim.phys.,  [5],  15,  326. 
Lehmann,  M. 

(1914)  Chem.Ztg.,  38,  389,  402. 
Leidie. 

(1882)  Compt.rend.,  95,  87. 

(1890)  Compt.rend.,  in,  107. 
Lenher,  V.  and  Merrill,  H.  B. 

(1917)  J.Am.Chem.Soc.,  39,  2630. 
Leopold,  G.  H. 

(1909)  Z.physik.Chem.,  66,  361. 

(1910)  Z.physik.Chem.,  71,  51. 
Lepierre,  C.  and  Lachaud,  M. 

(1891)  Compt.rend.,  113,  196. 
Lespieau. 

(1894)  Bull.soc.chim.,  [3],  n,  72. 
Levi,  M.  G. 

(1901)  Gazz.chim.ital.,  31,  II,  523. 

(1902)  Z.physik.Chem.,  41,  no. 
Levi-Malvano,  M. 

(1906)  Z.anorg.Chem.,  48,  446. 
(1905)  Atti  accad.Lincei,  [5],  14,  II, 

502-10. 
Lewis,  G.  N.  and  Burrows,  G.  H, 

(1912)  J.Am.Chem.Soc.,  34,  1525. 
Lewis,  G.  N.  and  Storch,  H. 

(1917)  J.Am.Chem.Soc.,  39,  2551. 
Lewis,  W.  K. 

(1914)  J.Ind.Eng.Chem.,  6,  308. 


Ley,  H.  and  Heimbuchen. 

(1904)  Z.Elektrochem.,  10,  303. 
Ley,  H.  and  Schaefer,  K. 

(1906)  Ber.,  39,  1263. 
Lichty,  D.  M. 

(1903)  J.Am.Chem.Soc.,  25,  474. 
Lidoff. 

(1893)  Bull.soc.chim.,  [3],  10,  356. 
Lieben  and  Rossi. 

(1871)  Liebig's  Ann.,  159,  60. 
Liebermann,  C. 

(1902)  Ber.,  35,  1094. 

(1903)  Ber.,  36,  180. 
.      Limbosch,  H. 

(1909)  Bull.soc.chim.Belg.,  23,  179- 

200. 
Lincoln,  A.  T. 

(1900)  J.Phys.Chem.,  4,  176. 

(1904)  J.Phys.Chem.,  8,  251. 
van  der  Linden,  T. 

(1912)  Ber.,  45,  237. 

(1916)  Arch.Suikerind,  24,  1113-28. 

(1917)  Chem.Abs.,  n,  3122. 
Linebarger,  C.  E. 

(1892)  Am.Chem.Jour.,  14,  380. 

(1894)  Am.Chem.Jour.,  16,  214. 
,           (1895)  Am.Jour.Sci.,  49,  48-53- 

Lindner,  J. 

(1912)  Monatsh.Chem.,  33,  645. 
Linhart,  G.  A. 

(1915)  J.Am.Chem.Soc.,  37,  258-274. 
Little,  W.  G. 

(1909)  Biochem.Jour.,  4,  30. 
Lloyd,  S.  J. 

(1918)  J.Phys.Chem.,  22,  300-3. 
Locke. 

(1901)  Am. Chem. J.,  26,  174. 

(1902)  Am.Chem.J.,  27,  459. 
Loewel. 

(1851)  Ann.chim.phys.,  [3],  33,  382. 

(1855)  Ann.chim.phys.,  [3],  43,  413. 
Long. 

(1888)  J.Anal.Chem.,  2,  243. 
Longi. 

(1883)  Gazz.chim.ital.,  13,  87. 
Longuimine. 

(1862)  Liebig's  Ann.,  121,  123. 
Lord,  R.  C. 

(1907)  J.Phys.Chem.,  u,  182. 
Lorenz,  R.,  Jabs,  A.  and  Eitel,  W. 

(1913)  Z.anorg.Chem.,  83,  39. 
Lorenz  and  Ruckstuhl. 

(1906)  Z.anorg.Chem.,  51,  70. 
Lothian,  J. 

(1909)  Pharm.Jour.(Lond.),  82,  292. 
Louise,  E. 

(1909)  Compt.rend.,  149,  284-6. 

(1911)  J.pharm.chim.,  [7],  3,  377-385- 

(1911)  J.pharm.chim.,  [7],  4,  193-7  • 

(1911)  Ann.fals.,  4,  302-5. 
Lowel. 

(1851)  Ann.chim.phys.,  [3],  33,  3«2. 

804 


AUTHOR  INDEX 


Lb'wenherz,  R. 

(1894)  Z.physik.Chem.,  13,  479. 

(1895)  Z.physik.Chem.,  18,  82. 
(1898)  Z.physik.Chem.,  25,  395-410. 

Lubarsch. 

(1889)  Wied.Ann.Physik.,  [2],  37,  525. 
Lubavin. 

(1892)    J.Russ.Ph^    Chem.Soc.,    24, 

389. 
de  Lucchi,  G. 

(1910)  Russ.min.,  32,  21. 

(1910)  "Tables  annuelles, "1,381, 403. 
Lumiere,  A.  and  L.  and  Seyewetz,  A. 

(1902)  Bull.soc.chim.,  [3],  27,  1213. 
Lumsden,  J.  S. 

(1902)  J.Chem.Soc.(Lond.),  81,  355. 

(1905)  J. Chem.Soc.  (Lond.),  89,  90. 
Lunden,  Harold. 

(1905-6)  Z.physik.Chem.,  54,  564. 

(1913)         Medd.K.Vetenskapsakad. 
Nobelinst.,  2,  No.  15. 

(1913)  Chem.Abs.,  7,  2887. 
Luther,  R.  and  Leubner,  A. 

(1912)  J.prakt.Chem.,  [2],  85,  314. 

(i9i2a)  Z.anorg.Chem.,  74,  389. 
Lutz,  O. 

(1902)  Ber.,  35,  2462. 
(1910)  Ber.,  43,  2637. 

van  Maarseveen,  G.  (Goldschmidt,  H.) 

(1898)  Z.physik.Chem.,  25,  90-99. 
Maass,  O.  and  Mclntosh,  D. 

(1912)  J. Am. Chem.Soc.,  34,  1279. 

(1913)  J.Am.Chem.Soc.,  35,  538. 
Maben. 

(1883-84)    Pharm. Jour. (Lond.),    [3], 

14,  505- 
MacAdam,  D.  J.,  Jr.  and  Pierle,  C.  A. 

(1912)  J.Am.Chem.Soc.,  34,  604. 
MacArthur,  C.  G. 

(1916)  J.  Phys.Chem.,  20,  495. 
McBride,  R.  S. 

(1910)  J. Phys.Chem.,  14,  189-200. 
McCaughey,  W.  J. 

(1909)  J.Am.Chem.Soc.,  31,  1261. 
McCoy,  H.  N.  and  Smith,  H.  J. 

(1911)  J.Am.Chem.Soc.,  33,  468-473. 
McCoy,  H.  N.  and  Test,  Chas.  D. 

(1911)  J.Am.Chem.Soc.,  33,  473-6. 
McCrae,  J.  and  Wilson,  W.  E. 

(1903)  Z.anorg.Chem.,  35,  n. 
M'David,  J.  W. 

(1909-10)      Proc.Roy.Soc.       (Edin- 
burgh), 30,  440-7. 
McDaniel,  A.  S. 

(1911)  J. Phys.Chem.,  15,  587-610. 
McDermott,  F.  Alex. 

(1911)  J.Am.Chem.Soc.,  33,  1963. 
McDonnell,  C.  C.  and  Smith,  C.  M. 

(1916)  J.Am.Chem.Soc.,  38,  2366. 
Mclntosh,  D. 

(1903)  J. Phys.Chem.,  7,  350. 
Mackenzie. 

(1877)  Wied.Ann.Physik.,  [2],  I,  450. 


McLauchlan,  W.  H. 

(1903)  Z.physik.Chem.,  44,  600-633. 
Maclaurin. 

(1893)  J.Chem.Soc.(Lond.),  63,  729. 
Magnanini,  G. 

(1901)  Gazz.chim.ital.,  31,  II,  542. 
Magnier. 

(1875)  Bull.soc.chim.,  [2],  23,  483. 
von  Mailfert. 

(1894)  Compt.rend.,  119,  951. 
Maigret. 

(1905)  Bull.soc.chim.  [3],  33,  631. 
Mallet. 

(1897)  Am.Chem.Jour.,  19,  807. 
Malvano,  L. 

(1906)  Z.anorg.Chem.,  48,  446. 
Malvano,  L.  and  Mannino. 

(1908)  Atti  accad.Lincei,  [5],  17,  II, 

484. 
Mameli,  E.  and  Mannessier,  A. 

(1913)  Gazz.chim.ital.,  43,  II,  594. 
Manchot  and  Zechentmayer. 

(1906)  Liebig's  Ann.,  350,  368. 
Mandelbaum,  R. 

(1909)  Z.anorg.Chem.,  62,  370-82. 
Manuelli,  A. 

(1916)  Ann.chim.applicata,  5,  13-24. 
Mar. 

(1892)  Am.J.Sci.,  [3],  43,  521. 
Marc,  R. 

(1906)  Z.anorg.Chem.,  48,  425. 

(1907)  Z.anorg.Chem.,  53,  301. 
Marchionneschi,  M. 

(1907)  Apoth.Ztg.,  22,  544. 
(1907)  Boll.chim.farm.,  387. 
Marckwald,  W. 

(1902)  Ber.,  35,  1599. 
(1904)  Ber.,  37,  1041. 


Harden, 

(1914)  ! 
(1916)  ; 
Marden, 

(1916)  . 

(1917)  . 


W. 

.Ind.Eng.Chem.,  6,  315-20. 


.Am.Chem.Soc., 
W.  and  Dover, 


310. 
ary  V. 


.Am.Chem.Soc.,  38,  1239. 


.Am.Chem.Soc.,  39,  4. 
Marie,  C.  and  Marquis,  R. 

(1903)  Compt.rend.,  136,  684. 
Marignac. 

(1853)  Ann.chim.phys.,  [3],  39,  184. 

(1861)  J.prakt.Chem.,  83,  202. 

(1866)  Ann.chim.phys.,  [4],  8,  65. 
Marino. 

(1905)  Gazz.chim.ital.,  35,  II,  351. 
Markwald. 

(1899)  Ber.,  32,  1089. 
Marsh,  J.  E.  and  Struthers,  R.  de  J.  F. 

(1905)  J.Chem.Soc.(Lond.),  87,  1879. 
Marshal,  A. 

(1906)  J. Chem.Soc. (Lond.),  89,  1381. 
Marshall. 

(1891)  J. Chem.Soc. (Lond.),  59,  771. 
Marshall,  H.  and  Bain,  D. 

(1910)  J. Chem.Soc. (Lond.), 97, 1074- 
1085. 


805 


AUTHOR   INDEX 


Marshall,  H.  and  Cameron,  A.  T. 

(1907)  J.Chem.Soc.(Lond.),  91,  1522. 
Mascarelli,  L. 

(1906)  Atti  accad.Lincei,   [5],   15,   I, 

192;  II,  459. 
(I9o6a)  Atti  accad.(Lincei),   [5],   15, 

192. 
(I9o6a)  Gazz.chim.ital.,  36,  II,  880- 

893. 

(1908)  Atti  accad.Lincei,   [5],   17,   I, 

29. 

(1909)  Gazz.chim.ital.,  39,  I,  251-84. 
Mascarelli,  L.  and  Ascoli,  U. 

(1907)  Gazz.chim.ital.,  37,  I,  125. 
Mascarelli,  L.  and  Constantino,  A. 

(1909)  Atti  accad.Lincei,  [5],  18,  II, 

104. 

(1910)  Gazz.chim.ital.,  40,  I,  41. 
Mascarelli,  L.  and  Pestalozza,  U. 

(1907)  Atti  accad.  Lincei,  [5],i6,  II, 

574- 

(1908)  Gazz.chim.ital.,  38,  I,  51. 

(1908)  Atti  accad.Lincei,  [5],  17,  I, 

601-9. 

(1909)  Gazz.chim.ital.,   39,   I,  218- 

231. 
Mascarelli,  L.  and  Sanna,  G. 

(1915)  Atti  accad.Lincei,  [5],  24,  II, 

94- 
Massink,  A. 

(1916)  Z.physik.Chem.,  12,  351-80. 

(1917)  Chem.Weekblad.,  14,  756. 
Massol  and  Maldes. 

(1901)  Compt.rend.,  133,  287. 
Masson,  I. 

(1912-13)  Proc.Roy.Soc.(Edin.),  33, 

64-8. 
Masson,  J.  J.  Orme. 

(1911)  J.Chem.Soc.(Lond.),  99,  1132. 

(1912)  J.Chem.Soc.(Lond.)  101,  103. 
Mathers,  F.  C.  and  Schluederberg,  C.  G. 

(1908)  J.Am.Chem.Soc.,  30,  211. 
Mathews,  J.  H.  and  Benger,  E.  B. 

(1914)  J.Phys.Chem.,  18,  264. 
Mathews,  J.  H.  and  Ritter,  P.  A. 

(1917)  J.Phys.Chem.,  21,  269-74. 
Mathews,  J.  H.  and  Spero,  S. 

(1917)  J.Phys.Chem.,  21,  402-6. 
Matignon,  C. 

(1906)   Ann.chim.phys.,    [8],   8,  249, 
388,  407.  * 

(1909)  7th     Internat.Cong.Appl. 

Chem.,  2,  53-57- 
(igoga)  Compt.rend.,  148,  550. 
Matteoschat,  A. 

(1914)  Z.ges.Schiess.u.Sprengstoffw., 

9,  105-6. 
Matthes,  F. 

(1911)  Neues  Jahrb.Min.Geol.  (Beil. 

Bd.),  31,  342-85- 
Maumee. 

(1864)  Compt.Fend.,  58,  81. 


Mayer. 

(1856)  Liebig's  Ann.,  98,  193. 
Mayer,  O. 

(1903)  Ben,  36,  1741. 
Mazatto. 

(1891)  Nuovo.cimento,  [3],  29,  21. 
Meerburg,  P.  A. 

(1902)  Z.physik.Chem.  40,  647. 

(1903)  Z.anorg.Chem.,  37,  203. 

(1904)  Chem.Weekblad.,  i,  474. 

(1905)  Z.anorg.Chem.,  45,  i,  324. 

(1908)  Z.anorg.Chem.,  59,  136-42. 

(1909)  van  Bemmlen  Festschrift,  pp. 

356-60. 

(1911)  Chem.Zentralbl.,  I,  1036. 
Meerum-Terwogt. 

(1905)  Z.anorg.Chem.,  47,  203. 
Mees,  C.  E.  K.  and  Piper,  C.  W. 

(1912)  Photogr.Jour.,  33,  227. 
Phot ogr. Jour.,  36,  ?H- 
Photogr.Jour.,  52,  2^1-37. 

Meineke. 

(1891)  Liebig's  Ann.,  261,  360. 
Melcher,  A.  C. 

(1910)  J.Am.Chem.Soc.,  32,  50-66. 
Meldrum,  R. 

(1913)  Chem.News.,  108,  199. 
Mellor,  J.  W. 

(1901)  J.Chem.Soc.(Lond.),  79,  225. 
Meneghini,  D. 

(1912)  Gazz.chim.ital.,  42,  II,  474. 
Menge,  Otto. 

(1911)  Z.anorg.Chem.,  72,  169-218. 
Menke,  J.  B. 

(1912)  Z.anorg.Chem.,  77,  283. 
Menschutkin,  B.  N.  (see  pp.   379  and 

39i). 
(i905)Mem.St.PetersburgPolyt.Inst., 

4,  75-101. 

(1906)  Mem.St. Petersburg  Polyt.Inst., 

5,  355-388. 

(1907)  Z.anorg.Chem.  52,  9,  155;  53, 

26. 

(i907a)  Z.anorg.Chem.,  54,  89-96. 
(i9o8)Mem.St. Petersburg  Polyt.Inst., 

9,  200-222. 
(i909)Mem.St. Petersburg  Polyt.Inst., 

n,  261,  567;  12,  i. 

(1909)  Z.anorg.Chem.,  61,  106,  113. 

(19 1 o) Mem.St. Petersburg  Polyt.Inst., 

13,1,263,411,565;  14,251. 

(191  i)Mem.St. Petersburg  Polyt.Inst., 

15*  65,  397,  613,  647,  757. 
(i9i2)Mem.St. Petersburg  Polyt.Inst., 


16,  33,  397- 
L.  W.  C.  and  Dutt,  N.  N. 


Menzies,  A. 

(1911)  J.Am.Chem.Soc.,  33,  1266. 
Menzies,  A.  W.  C.  and  Humphrey,  E.G. 

(1912)  8th  Int. Congr.Appl. Chem.,  2, 

175-8. 

Menzies,  A.  W.  C.  and  Potter,  P.  D. 
(1912)  J.Am.Chem.Soc.,  34,  1452. 


806 


AUTHOR  INDEX 


Merriman,  R.  W. 

(1913)  J.Chem.Soc.(Lond.),  103,1774. 
Mescherzerski. 

(1882)  Z.anaLChem.,  21,  399. 
Metzner. 

(1894)  Compt.rend.,  119,  683. 
van  Meurs,  C.  J. 

(1916)  Z.physik.Chem.,  91,  313-46. 
Meusser,  A. 

(1902)  Ber.,  35,  1303,  1422. 
(1905)  Z.anorg.Chem.,  44,  80. 

Meyer,  J. 

(1909)  Z.Elektrochem.,  15,  266. 

(1911)  Ber.,  44,  2969. 
Meyer,  H,  von. 

(1901)  Archiv.exp.Pathol.u.Pharma- 

kol.,  46,  334. 
(1909)    7th    Int. Cong. Appl.     Chem. 

Sec.,  4,  A2,  44. 
Meyer,  Hans  von  and  Beer,  R. 

(1913)  Monatsh.Chem.,  34,  1202. 

Meyer,    Hans    von,     Brod,    L.    and 

Soyka,  W. 

(1913)  Monatsh.Chem.,  34,  1125. 
Meyer,  R.  J. 

(1914)  Z.anorg.Chem.,  86,  285. 
Meyer,  Victor. 

(1875)  Ber.,  8,  998. 
Meyerhoffer,  W. 

(1904)  Landolt  and  Bornstein  "Tab- 

ellen,"  4th  Ed.,  1912,  p.  486. 

(1905)  Z.physik.Chem.,  53,  513-603. 

(1912)  Landolt  and  Bornstein  "Tab- 

ellen,"  4th  Ed.,  p.  481. 
Meyerhoffer,  W.  und  Saunders. 

(1899)  Z.physik.Chem.,  28,  466;  31, 

382. 
Michael,  Arthur. 

(1901)  Ber.,  34,  3641,  3656. 
Michael,  Arthur  and  Garner,  W.  W. 

(1903)  Ber.,  36,  904. 
Michel  and  Kraft. 

(1854)  Ann.chim.phys.,  [3],  41,  471. 

(1858)  Ann.chim.phys.,  [3],  41,  478. 
Miczynski,  Z.  N. 

(1886)  Monatsh.Chem.,  7,  255-72. 
Middelberg,  W. 

(1903)  Z.physik.Chem.,  43,  305-353. 
Miers,  H.  A.  and  Isaac,  F. 

(1907)  Proc.Roy.Soc.(Lond.),  79,  A, 

332. 

(1908)  Trans.  Roy.Soc.(Lond.),   209, 

A,  364- 

(i9o8a)  J.Chem.Soc.(Lond.),  93,  931. 
Milbauer,  J. 

(1912-13)  J.prakt.Chem.,  [2],  87,  398. 
Milikau,  J. 

(1916)  Z.physik.Chem.,  92,  59-80. 
Miller,  W.  Lash  and  McPherson,  R.  H. 

(1908)  J.Phys.Chem.,  12,  709. 
Mills,    W.    H.,    Parker,    H.    V.    and 
Prowse,  R.  W. 

(1914)  J.Chem.Soc.(Lond.), 105,1541. 


Mills,  R.  V.  and  Wells,  R.  C. 

(1918)     Bull.U.S.Geol.Sur/ey,    No. 

693,  P-  72. 
Miolati,  A. 

(1892)  Z.physik.Chem.,  9,  651. 
Mjtscherlich. 

(1832)  Pogg.Ann.,  25,  301. 
Moissan,  H. 

(1882)  Bull.soc.chim.,  [2],  37,  296. 

(1885)  Ann.chim.phys.,  [6],  4,  136. 
Moissan,  H.  and  Siemens,  F. 

(1904)  Compt.rend.,  138,  657,  1300. 

(1904)  Bull.soc.chim.,  [3],  31,  1010. 

(1904)  Ber.,  37,  2088. 
Moles,  E.  and  Jimeno,  E. 

(1913)  Anales.soc.espan.fis.quim.,  II, 

393- 
Moles,  E.  and  Marquina,  M. 

(1914)  Anales.soc.espan.fis.quim.,  12, 

383-93. 
Monkemeyer. 

(1906)  NJahrb.Min.Geol.(Beil.Bd.), 

22,  I. 

Moody,  G.  T.  and  Leyson,  L.  F. 

(1908)  J.Chem.Soc.(Lond.),  93,  1767. 
Moore,  B.  and  Roaf,  H.  E. 

(1904)      Proc.Roy.Soc.(Lond.),     73, 

382-412. 

Moore,  B.,  Wilson,  F.  P.  and  Hutchin- 
son,  L. 

(1909)  Biochem.Jour.,  4,  347. 
Moore,  T.  S.  and  Winmill,  T.  F. 

(1912)  J. Chem. Soc.(LoncL),  101,1662. 
Morey,  Geo.  W. 

(1917)    J.Am.Chem.Soc.,    39,    1173- 

1229. 
Morgan,  J.  L.  R.  and  Benson,  H.  K. 

(1907)  J.Am.Chem.Soc.,  29,  1176. 
(1907)  Z.anorg.Chem.,  55,  356. 

Morgan,  J.  C.  and  James,  C. 

(1914)  J.Am.Chem.Soc.,  36,  10-16. 
Morell,  R.  S.  and  Hanson,  E.  K. 

(1904)  J.Chem.Soc.(Lond.),  85,  1520. 
Morse,  H. 

(1902)  Z.physik.Chem.,  41,  708-734. 
Moser,  L. 

(1909)  Z.anorg.Chem.,  61,  384. 
Moufgang,  E. 

(1911)  Wochschr.Brau.,  28,  434-6. 

(1911)  J.Soc.Chem.Ind.,  30,  1210. 
Much  in,  G. 

(1913)  "  Solubility  of  Calcium  Iodide 
in  Organic  Solvents,"  Pamphlet, 
45  pp.  and  12  charts,  Kharkoff, 
1913.    (Reprint  in  the  Russian 
language  received  from  author.) 
See     also      Trav.sco.sci. physic. 
Chem.Univ.  Kharkoff    39    fasc., 
24,  1-49,  I9I3- 

Muir. 

(1876)  J.Chem.Soc.(Lond.),29,  857. 


807 


AUTHOR  INDEX 


Mulder,  G.  J. 

(1864)  Scheikundige  Verhandelingen 
en  Onderzoekingen,  Vol.  3,  Pt.  2, 
Bijdragen   tot   de   Geschiedenis 
van  Het  Scherkungig  Gebonden 
Water,  Rotterdam,  1864. 
Mulder,  Gay-Lussac,  Etard. 
-    (1894)  Ann.chim.phys.,  [7],  2,  528. 
MueUer,  J.  H. 

(1917)  J.Biol.Chem.,  30,  39~4O. 
Mueller,  P.  and  Abegg,  R. 

(1906)  Z.physik.Chem.,  57,  514. 
Miiller,  C. 

(1910)  NJahrb.Min.Geol.(Beil.Bd.), 

30,  i. 
(1912-13)  Z.physik.Chem.,  81,  483- 

503. 
Miiller. 

(1887)  Compt.rend.,  104,  992. 

(1889)  Wied.Ann.Physik.,  [2],  37,  29. 

(1892)  Ann.chim.phys.,  [6],  27,  409. 
Miiller,  H. 

(1912)  J.Chem.Soc.(Lond.), 101,2400. 
Muller,  W. 

(1903)  Apoth.Ztg.,  18,  208,  249,  257. 
Muraro,  F. 

(1908)  Gazz.chim.ital.,  38,  I,  427;  II, 

507- 
Muthmann  and  Kuntze. 

(1894)  Z.Kryst.Min.,  23,  368. 
Muthmann  and  Rolig. 

(1898)  Z.anorg.Chem.,  16,  455. 

(1898)  Ber.,  31,  1728. 
Mylius,  F. 

(1901)  Ber.,  34, 2208. 

(1911)  Ber.  44,  1315. 

(1911)  Z.anorg.Chem.,  70,  209. 
Mylius,  F.  and  Dietz. 

(1901)  Ber.,  34,  2774. 

(1905)  Z.anorg.Chem.,  44,  217. 

(1905)  Ber.,  38,  921. 
Mylius,  F.  and  Forster. 

(1889)  Ber.,  22,  1 100. 

(1892)  Ber.,  25,  70. 
Mylius,  F.  and  Funk,  R. 

(1897)  Ber.,  30,  1718. 

(1900)  Wiss.Abh.p.t.Reichsanstalt,  3, 

(1900)  Ber.,  33,  3686. 
Mylius,  F.  and  von  Wrochem,  J. 
(1900)  Wiss.Abh.p.t.Reichsanstalt,  3, 

462. 

(1900)  Ber.,  33,  3689. 
Nacken,  R. 

(i907a)    Nachr.kgl.Ges.Wissenschaft 

(Gottingen),  602. 
(i907b)Jahrb.Min.Geol.(Beil.Bd.),24, 

i. 
(i907c)Zentralbl.Min.Geol.,262,30i. 

(1910)  Sitzber.kgl.preuss.Akad.Wis., 

1016-26. 
Nagornow,  N.  N. 

(1911)  Z.physik.Chem.,  75,  578. 


Nanty,  T. 

(1911)  Compt.rend.,  152,606. 
Narbutt,  J.  V. 

(1905)  Z.physik.Chem.,  53,  704-712. 
Nasini,  R.  and  Ageno,  I. 

(1910)  Z.physik.Chem.,  69,  482. 

(1911)  Gazz.chim.ital.,  41,  I,  131. 
Naumann,  Alex. 

(1904)  Ber.,  37,  3600,  4328. 

(1909)  Ber.,  42,  3789. 

(1910)  Ber.,  43,  313. 
(1914)  Ber.,  47,  1370. 

Naumann,  Alex,  and  Rucker,  A. 

(1905)  Ber.,  38,  2293. 
Naumann,  Alex,  and  Schier,  A. 

(1914)  Ber.,  47,  249. 
Neave,  G.  B. 

(1912)  Analyst.,  37,  399. 
Nernst,  W. 

(1889)  Z.physik.Chem.,  4,  379. 
(1891)  Z.physik.Chem.,  8,  no. 

Newth. 

(1900)  J.Chem.Soc.(Lond.),  77,  776. 
Nicol,  W.  W.  J. 

(1891)  Phil.Mag.(Lond.),  [5],  31,  369, 

386. 
Nicolardot. 

(1916)  Compt.rend.,  163,  355-7. 
Nichols,  J.  B. 

(1918)  J.Am.Chem.Soc.,  40,  402. 

von  Niementowski,  S.  and  von  Rosz- 

kowski,  T. 

(1897)  Z.physik.Chem.,  22,  146. 
Noelting,  F. 

(1910)  Ann.chim.phys.,  [8],  19,  486. 
Nordenskjold  and  Lindstrom. 

(1869)  Pogg.Ann.,  136,  314. 
Noss,  F. 

(1912)  Dissertation,  Graz. 

(1912)  Landolt  and  Bornstein  "  Tab- 

ellen,"  4th  Ed.,  p.  467. 
Noyes,  A.  A. 

(1890)  Z.physik.Chem.,  6,  248. 

(1892)  Z.physik.Chem.,  9,  606,  623. 
Noyes,  A.  A.  and  Abbott,  C.  G. 

(1895)  Z.physik.Chem.,  16,  130. 
Noyes,  A.  A.  and  Boggs,  C.  R. 

(1911)  J.Am.Chem.Soc.,  33,  1650. 
Noyes,  A.  A.  and  Chapin,  E.  S. 

(1898)  Z.physik.Chem.,  27,  443. 

(1899)  J.Am.Chem.Soc.,  21,  513. 
Noyes,  A.  A.  and  Clement. 

(1894)  Z.physik.Chem.,  13,  413. 
Noyes,  A.  A.  and  Farrel,  F.  S. 

(1911)  J.Am.Chem.Soc.,  33,  1654. 
Noyes,  A.  A.  and  Hall,  F.  W. 

(1917)  J.Am.Chem.Soc.,  39,  2529. 
Noyes,  A.  A.  and  Kohr,  D.  A. 

(1902)  J.Am.Chem.Soc.,  24,  1144. 
(1902-03)  Z.physik.Chem.,  42,  336- 

42. 
Noyes,  A.  A.  and  Sammet,  G.  V. 

(1903)  Z.physik.Chem.,  43,  526. 


808 


AUTHOR   INDEX 


Noyes,  A.  A.  and  Schwartz,  D. 

(1898)  Z.physik.Chem.,  27,  279-284. 

(1898)  J.Am.Chem.Soc.,  20,  744. 
Noyes,  A.  A.  and  Seidenslicker. 

(1898)  Z.physik.Chem.,  27,  359. 
Noyes,  A.  A.  and  Stewart,  M.  A. 

(1911)  J.Am.Chem.Soc.,  33,  1658. 
Noyes,  A.  A.  and  Whitcomb,  W.  H. 

(1905)  J.Am.Chem.Soc.,  27,  756. 
Odaira,  I. 

(1915)  M  em.  Coll.  Sci.(  Kyoto),  i,  324, 

330. 
Oddo,  B. 

(1913)  Gazz.chim.ital.,  43,  II,  275. 
Okada,  K. 

(i9i4)Mem.Coll.Sci.(Kyoto),    i,  95- 

103. 
Olie,  Jr.,  J. 

(1906)  Z.anorg.Chem.,  51,  29-70. 

(1907)  Z.anorg.Chem.,  53,  273-80. 
Olivari,  F. 

(1908)  Atti  accad.Lincei,  [5],  17,  II, 

512,  584,  717. 

(1909)  Atti  accad.Lincei,  [5],  18,  II, 

96. 

(1911)  Atti  accad.Lincei,   [5],  20,  I, 

470-4. 

(1912)  Atti  accad.Lincei,  [5],  21,  I, 

718. 
Ordway. 

(1865)  Am.Jour.Sci.,  [2],  40,  173. 
Orloff. 

(1902)  J.Russ.Phys.Chem.Soc.,    37, 

949- 
Orton,  K.  J.  P.  and  King,  H. 

(1911)  J.Chem.Soc.(Lond.),  99,  1192. 
Osaka,  Y. 

(1903-8)  Mem.Coll.Sci.Eng. (Kyoto), 
i.  93,  265,  290. 

(1909)  7th     Int.Cong.Appl.Chem., 

4  A,  308. 

(1910)  Mem.Coll.Sci.Eng.  (Kyoto), 

2,21-35. 

(1910)  Nature  (London),  84,  248. 
(1910-1  i)Mem. Coll. Sci.Eng.  (Kyoto), 

3,  58. 

(1911)  J.Tok.Chem.Soc.,  32,  870. 
Osaka,  Y.  and  Abe,  R. 

(1911)  Mem.Coll.Sci.Eng. (Kyoto),  3, 

51-4- 

(1911)  J.Tok.Chem.Soc.,  32,  446. 
Osborne,  T.  and  Harris,  I.  F. 

(1905)    Am.Jour.Physiol.,    14,    151- 

171. 
Osipoff  and  Popoff. 

(1903)  J.Russ.Phys.Chem.Soc.,    35, 

637. 
Ossendowski,  A.  M. 

(1907)  Pharm.J.(Lond.),  79,  575. 

U907)  J.pharm.chim.,  [6],  26,  162. 
Ost. 

(1878)  J.prakt.Chem.,  [2],  17,  232. 


Oswald,  M. 

(1914)  Ann.chim.,  i,  57-79. 
(1912)  Compt.rend.,  155,  1504. 
(1912)  8th  Int.Cong.Appl.Chem.,  2, 

205. 
Oudemans,  A.  C.  Jr. 

(1872)  Z.anal.Chem.,  n,  287. 
Padoa,  M. 

(1904)  Atti  accad.Lincei,  [5],  13,  I, 

723;  II,  31. 
Padoa,  M.  and  Rotondi,  G. 

(1912)  Atti  accad.Lincei,  [5],  21,  II, 

626. 
Padoa,  M.  and  Tibaldi. 

(1903)  Atti  accad.Lincei,  [5],  12,  II, 

1 60. 
de  Paepe,  Desire. 

(1911)  Bull.soc.chim.Belg.,  25,  174. 
Pajetta,  R. 

(1906)  Gazz.chim.ital.,  36,  II,  67, 155, 

300. 

(1907)  Pharm.Jour.(Lond.),  79,  315. 
Palazzo  and  Batelli. 

(1883)  Atti  accad.sci.Torino,  19,  514. 
Panfiloff. 

(1893)    J.Russ.Phys.Chem.Soc.,    25, 
162. 

(1893)  Chem.Centralbl.,  II,  910. 
(i893a)  J.Russ.Phys.Chem.Soc.,  25, 

262. 

(1894)  Z.anorg.Chem.,  5,  490. 
Parker,  E.  G. 

(1914)  J.Phys.Chem.,  18,  653. 
Parmentier. 
•   (1887)  Compt.rend.,  104,  686. 

(1892)  Compt.rend.,  114,  1002. 
Parravano,  N. 

(1909)  Gazz.chfm.ital.,  39,  II,  58. 
Parravano,  N.  and  Calcagni,  G. 

(1908)  Atti  accad.Lincei,  [5],   17,   I, 

731-8. 

(1910)  Z.anorg.Chem.,  65,  i. 
Parravano,  N.  and  de  Cesaris,  P. 

(1912)  Att  accad.Lincei,  [5],  21,  I, 

535- 
(i9i2a)  Atti  accad.Lincei,  [5],  21,  I, 

800. 
(i9i2b)   Gazz.chim.ital.,  42,   II,  i- 

191. 

Parravano,  N.  and  Fornaini,  M. 
(1907)  Gazz.chim.ital.,  37,  II,  521. 

(1907)  Atti  accad.Lincei,  [5],  16,  II, 

465- 
Parravano,  N.  and  Mieli,  A. 

(1908)  Atti  accad.Lincei,  [5],  17,  II, 

33-4- 

(1908)  Gazz.chim.ital.,  38,  II,  536. 
Parsons,  Chas.  L.  and  Corliss,  H.  P. 

(1910)  J.Am.Chem.Soc.,  32,  1367. 
Parsons,  C.  L.  and  Corson,  H.  P. 

(1910)  J.Am.Chem.Soc.,  32,  1383. 
Parsons,  C.  L.  and  Perkins,  C.  L. 

(1910)  J.Am.Chem.Soc.,  32,  1387. 


809 


AUTHOR  INDEX 


Parsons,  C.  L.  and  Whittemore,  C.  F. 

(1911)  J.Am.Chem.Soc.,  33,  1933. 
Partheil  and  Ferie. 

(1903)  Archiv.Pharm.,  241,  554. 
Partheil  and  Hubher. 

(1903)  Archiv.Pharm.,  241,  413. 
Partington,  J.  R. 

(1911)  J.Chem.Soc.(Lond.),  99,  315. 
Pascal,  P. 

(1909)  Ann.chim.phys.,  [8],  16,  374. 

(1912)  Bull.soc.chim.,    [4],    n,   323, 

596,  1033. 

(1913)  Bull.soc.chim.,  [4],  13,  746. 

(1914)  Bull.soc.chim.,  [4],  15,  454. 
Pascal,  P.  and  Normand,  L. 

(1913)    Bull.soc.chim.,    [4],    13,  154- 

202,  879. 
Paterno,  E.  and  Ampola,  G. 

(1897)  Gazz.chim.ital.,   27,   I,   481- 

536. 
Paterno,  E.  and  Mieli,  A. 

(1907)  Atti  accad.Lincei,  [5],  16,  II, 

153- 

(1907)  Gazz.chim.ital.,  37,  II,  330. 
Paterno,  E.  and  Salimei,  G. 

(1913)  Gazz.chim.ital.,  43,  II,  245. 
Patrick  and  Aubert. 

(1874)  Trans. Kansas  Acad.Sci.,  19. 
Patten,  H.  E.  and  Mott,  W.  R. 

(1904)  J.Phys.Chem.,  8,  153. 
Patterson,  A.  M. 

(1906)  J.Am.Chem.Soc.,  28,  1734. 
Paul,  T. 

(1894)  Z.physik.Chem.,  14,  in. 

(1896)  Z.physik.Chem.,  25,  95, 
(1901)  Arch.Pharm.,  239,  64. 

(1915)  Z.Elektrochem.,  21,  543. 
(1917)  Z.Elektrochem.,  23,  65-86. 

Paul,  Th.,  Ohlmiiller,  W.,  Heise,  R. 
and  Auerbach,  Fr. 

(1906)  Arb.Kaiserl.Gesundheitsamt., 

23,  333-388. 
Pawlewski,  Br. 

(1893)   Anzeiger  Akad.Wiss.Krakau, 
p.  379. 

(1898)  Ber.,  30,  2806. 

(1899)  Ber.,  32,  1040. 

(1900)  Ber.,  33,  1223. 
Pawlewski,  Br.  and  Filemonowicz. 

(1888)  Ber.,  21,  2973. 
Payen. 

(1852)  Compt.rend.,  34,  356. 
Pearce,  J.  N.  and  Fry,  E.  J. 

(1914)  J.Phys.Chem.,  18,  667. 
Pearce,  J.  N.  and  Moore,  T.  E. 

(1913)  Am.Chem.Jour.,  50,  218. 
Peddle,  C.  J.  and  Turner,  W.  E.  S. 

(1913)      J.Chem.Soc.(Lond.),      103, 

1205. 
Pelabon. 

(1897)  Compt.rend.,  124,  35. 
(1904)  J.chim.phys.,  2,  320. 

(1907)  Compt.rend.,  145,  118. 


Pelabon. 

(1908)  Compt.rend.,  146,  975. 

(1909)  Ann.chim.phys.  [8],  17,  526- 

66. 

(1913)  Compt.rend.,  156,  705-7. 
Pelet-Jolivet. 

(1909)  Revue  gen. mat. col.,  p.  249. 
Pellini,  G. 

(1906)  Gazz.chim.ital.,  36,  II,  461. 
(i9o6a)  Atti  accad.Lincei,  [5],  15,  I, 
629. 

(1909)  Atti  accad.Lincei,  [5],  18,  I, 

703;  II,  21,  280. 

(1910)  Atti  accad.Lincei,  [5],   19,  I, 

331- 
Pellini,  G.  and  Amadori,  M. 

(1912)  Atti  accad.Lincei,   [5],  21,  I, 

294. 
Pellini,  G.  and  Coppola,  A. 

(1913)  Atti  accad.Lincei,   [5],  23,  I, 

147. 
Pellini,  G.  and  Pedrina,  S. 

(1908)  Atti  accad.Lincei,  [5],  17,  II 

78. 
Pellini,  G.  and  Vio,  G. 

(1906)  Atti  accad.Lincei,  [5],  15,  II, 

46-53. 
Pelouze. 

(1869)  Compt.rend.,  68,  1179;  69,  56. 
Penny. 

(1855)  Phil.Mag.,  [4],  10,  401. 
Perman,  E.  P. 

(1901)  J.  Chem.Soc.(Lond.),  79,  718. 

(1902)  J.Chem.Soc.(Lond.),  81,  480. 

(1903)  J.Chem.Soc.(Lond.)(  83,  1168. 
Pettersson,  O.  and  Sonden,  K. 

(1889)  Ber.,  22,  1439. 
Pfannl,  M. 

(1911)  Monatsh.Chem.,  32,  250. 
Pfaundler  and  Schnegg. 

(1875)     Sitzber.k.Akad.Wis.(Wien)., 

?i,  II,  351- 
Pfeiffer,  H. 

(1892)  Z.physik.Chem.,  9,  469. 
Pfeiffer,  Geo.  J. 

(1897)  Z.anorg.Chem.,  15,  194-203. 
Pfeiffer,  P.  and  Modelski,  J.  v. 

(1912)  Z.physiol.Chem.,  81,  331-3. 
Pfeiffer,  P.  and  Wurgler. 

(1915)  Ber.,  48,  1939. 

(1916)  Z.physiol.Chem.,  97,  128-47. 
Phelps,  I.  K.  and  Palmer,  H.  E. 

(1917)  J.Am.Chem.Soc.,  39,  140. 
Philip,  James  C. 

(1903)  T.Chem.Soc.(Lond-),  83,  814. 
(1905)  j.Chem.Soc.(Lond.),  87,  992. 
-(1913)  J.Chem.Soc.(Lond.),  103,  284. 
Philip,  J.  C.  and  Bramley,  A. 

(1915)      J.Chem.Soc.(Lond.),      107, 

377-387,  1832- 
Philip,  J.  C.  and  Garner,  F.  B. 

(1909)  J.Chem.Soc.(Lond.),       95, 

1466-73. 


8lO 


AUTHOR   INDEX 


Philip,  J.  C.  and  Smith,  S.  H. 

(1905)       J.Chem.Soc.(Lond.),       87, 
I735-I75L 

Pickering,  S.  U. 

(1890)  J.Chem.Soc.(Lond.),  57,  331- 
(1890-91)  Proc.Roy.Soc.(Lond.),  49, 

25- 

(1893)  J.Chem.Soc.(Lond.),  63,  141, 

463,  909,  998. 
(i893a)  Ben,  26,  2307. 
(1895)  J.Chem.Soc.(Lond.),  67,  669. 

(1912)  Landolt       and        Bornstein, 
"  Tabellen,"  4th  Ed.,  p.  471. 

(1915)      J.Chem.Soc.(Lond.),      107, 

942-54. 
Pictet,  Raoul. 

(1894)  Compt.rend.,  119,  642. 
Pictet,  R.  and  Altschul,  M. 

(1895)  Z.physik.Chem.,  16,  78. 
(1894)  Compt.rend.,  119,  678-82. 

Pierre. 

(1847)  J.pharm.chim.,  [3],  12,  237. 
Pina  de  Rubies,  S. 

(1913)  Anales  soc.espan.fis.quin.,  n, 

422-35- 

(1914)  Anales  soc.espan.fis.quin.,  12, 

343-9; 

(1914)  Archiv.sci.physique,naturelle 

(Madrid),  [4],  38,  414-22. 

(1915)  Chem.Zentralbl.,  I,  521. 
Pinnow,  J. 

(1911)  Z.anal.Chem.,  50,  162. 

(1915)  Z.anal.Chem.,  54,  321-345- 
Plato, 

(1907)  Z.physik.Chem.,  58,  350. 
Pleissner,  M. 

(1907)  Arb.Kais.Gesundheitsamt,  26, 

384-443. 
Plotnikow,  W.  A. 

(1911)  Ann. inst.Polytech. Kiev.,    n, 

310. 
(1915)    J.Russ.Phys.Chem.Soc.,    47, 

1062-4. 
Poggiale. 

(1843)  Ann.chim.phys.,  [3],  8,  467. 
Pohl. 

(1852)  J.prakt.Chem.,  56,  216. 
(1860)    Sitzber.k.Akad.Wiss.(Wien), 

41,  627. 
Pollacci. 

(1896)  L'Orosi,  19,  217. 
Pollitzer,  F. 

(1909)  Z.anorg.Chem.,  64,  121-48. 
Poma,  G. 

(1909)  Atti  accad.Lincei,  [5],  18,  I, 

133-8. 

(1910)  Gazz.chim.ital.,  40,  I,  197. 

Poma,  G.  and  Gabbi,  G. 

(1912)  Gazz.chim.ital.,  42,  II,  8. 

(1911)  Atti  accad.Lincei,  [5],  20,  I, 

464-70. 


Porlezza,  C. 

(1914)  Atti  accad.Lincei,  [5],  23,  II, 

*  *    5°9'  597' 
Power,  F.  B. 

(1882)  Am.Jour.Pharm.,  54,  97-99. 
Power,  F.  B.  and  Tutin. 

(1905)  J.Chem.Soc.(Lond-),  87,  24. 
Pratolongo,  U. 

(1913)  Atti  accad.Lincei,  [5],  22,  I, 

388. 

(1914)  Atti  accad.Lincei,  [5],  23, 1, 46. 
Pratt,  L.  A.  and  James,  C. 

(1911)  J.Am.Chem.Soc.,  33,  488. 
Precht,  H.  and  Wittgen,  B. 

(1881)  Ber.,  14,  1667. 

(1882)  Ber.,  15,  1666. 
Presse,  C.  H. 

(1874)  Ber.,  7,  599. 
Prins,  Ada. 

(1909)  Z.physik.Chem.,  67,  689-722. 
Prunier. 

(1879)  J.pharm.chim.,  [4],  29,  136. 
Puckner,  W.  A.  and  Hilpert,  W.  S. 

(1909)  J.Am.Med.Assoc.,  52,  311. 
Puckner,  W.  A.  and  Warren,  L.  E. 

(1910)  Proc.Am.Pharm.Assoc.,    58, 

1007. 
(1910)  Lab. Reports  Am.Med.Assoc., 

3>  123. 
Puschin,  N.  A.  and  Baskow,  A. 

(1913)  Z.anorg.Chem.,  81,  347-63. 
Puschin,  N.  A.  and  Glagoleva,  A.  A. 

(1914)  Ann.Inst.Electrotechnique 

(Petrograd),  n,  284. 

(1915)  J.Russ.Phys.Chem.Soc.,    47, 

100-13. 

Pushin,  N.  A.  and  Grebenschikov,  I.  V. 
(1913)    J.Russ.Phys.Chem.Soc.,    45, 

741-5- 
Pushin,  N.  and  Kriger,  J. 

(1913)  Ann.Inst.Electrotechnique 

(Petrograd),  9,  235. 

(1914)  J.Russ.Phys.Chem.Soc.,    46, 

559- 

Pushin,  N.  A.  and  Mazarovich,  G.  M. 
(1914)    J.Russ.Phys.Chem.Soc.,    46, 

1366-72. 
(1914)  Ann.Inst.Electrotechnique 

(Petrograd),  10,  205. 
Quercigh,  E. 

(1912)  Atti  accad.(Lincei),  [5],  21,  I, 

417,  786. 

(1914)  Atti  accad.(Lincei),  [5],  23,  I, 
449,  825. 

Rabe,  W.  O. 

(1901)  Z.physik.Chem.,  38,  175-184. 

(1902)  Z.anorg.Chem.,  31,  156. 
Rack,  G. 

(1914)  Centr.Min.Geol.,  326-8. 
Radan. 

(1889)  Liebig's  Ann.,  251,  129. 


811 


AUTHOR  INDEX 


Raffo,  M.  and  Rossi,  G. 

(1915)  Gazz.chim.ital.,  45,  I,  45- 
Rammelsberg. 

(1838)  Pogg.Ann.,  43,  665;  44,  575- 
(1841)  Pogg.Ann.,  52,  81,  96. 
(1892)  J.prakt.Chem.,  [2],  45,  153. 
Ramstedt,  Eva. 

(1911)  Radium,  8,  253^6. 
Rankin,  G.  A.  and  Merwin,  H.  E. 

(1916)  J.Am.Chem.Soc.,  38,  568. 
Rankin,  G.  A.  and  Wright. 

(1915)  Am.Jour.Sci.,  [4],  39,  i~79. 
Raoult. 

(1874)  Ann.chim.,  [5],  i,  262. 
Raupenstrauch,  G.  A. 

(1885)  Monatsh.Chem.,  6,  585. 
Rebiere,  G. 

(1915)  Bull.soc.chim.,    [4],    17,   268, 

Regnault  and  Wiilejean. 

(1887)  Chem.Centralbl.,  18,  252. 
Reich. 

(1891)  Monatsh.Chem.,  12,  464. 
Reichel,  H. 

(1909)  Biochem.Ztschr.,  22,  156. 
Reicher,  L.  T.  and  van  Deventer,  C.  M. 

(1890)  Z.physik.Chem.,  5,  560. 
Reid. 

(1887-88)  Proc.Roy.Soc.(Edin.),  15, 

151- 
Reid,  H.  S.  and  Mclntosh,  D. 

(1916)  J.Am.Chem.Soc.,  38,  615-25. 
Reinders,  W. 

(1900)  Z.physik.Chem.,  32,  494,  514. 
(1906)  Z.physik.Chem.,  54,  609. 

(1914)  Proc.k.Akad.Wet.(Amst.),  16, 

1065. 

(1915)  Z.anorg.Chem.,  93,  202. 
Reinders,  W.  and  de  Lange,  S. 

(1912-13)  Z.anorg.Chem.,  79,  230. 

(1912)  Proc.k.Akad.Wet.(Amst.),  15, 

474- 
Reinders,  W.  and  Lely,  Jr.  D. 

(1912)  Proc.k.Akad.Wet.(Amst.),  15, 

486. 
Reinitzer,  D. 

(1913)  Z.angew.Chem.,  26,  456. 
Reissig. 

(1863)  Liebig's  Ann.,  127,  33. 
Retgers,  J.  W. 

(1893)  Z.anorg.Chem.,  3,  253,  344. 

(1893)  Rec.trav.chim.,  12,  229. 
Rex. 

(1906)  Z.physik.Chem.,  55,  355. 
Reychler,  A. 

(1910)  J.chim.phys.,  8,  618. 
Reynolds,  J.  E.  and  Werner,  E.  A. 

(1903)  J.Chem.Soc.(Lond.},  83,  5. 
Richards,  T.  W. 

(1897)  Z.anorg.Chem.,  3,  455. 
Richards,  T.  W.  and  Archibald,  E.  H. 

(1901-02)  Proc.Am.Acad.,  37,  345. 

(1902)  Z.physik.Chem.,  40,  385-98. 


Richards,  T.  W.  and  Churchill. 

(1899)  Z.physik.Chem.,  28,  314. 
Richards,  T.  W.  and  Faber,  H.  B. 

(1899)  Am.Chem.Jour.,  21,  167-172. 
Richards,  T.  W.  and  Kelley. 

(1911)  J.Am.Chem.Soc.,  33,  847. 
Richards,  T.  W.,  McCaffrey  and  Bisbee. 

(1901)  Z.anorg.Chem.,  28,  85. 
Richards,  T.  W.  and  Meldrum,  W.  B. 

(1917)  J.Am.Chem.Soc.,  39,  1821-2. 
Riedel. 

(1906)  Z.physik.Chem.,  56,  243. 
Riesenfeld,  E.  H. 

(1902)  Z.physik.Chem.,  41,  346. 

(1903)  Z.physik.Chem.,  45,  461. 
Riley,  W.  A. 

(1911)  Jour.Inst. Brewing,  17,  124. 
(1911)  "  Tables  annuelles,"  2,  428. 
Rimbach,  E. 

(1897)  Ber.,  30,  3079. 
(1902)  Ber.,  35,  1300. 

(1904)  Ber.,  37,  463. 

(1905)  Ber.,  38,  1553-7,  1570. 
Rimbach,  E.  and  Korten,  F. 

(1907)  Z.anorg.Chem.,  52,  407. 
Rimbach,  E.  and  Schubert,  A. 

(1909)  Z.physik.Chem.,  67,  183-200. 
Rindell,  A. 

(1910)  Z.physik.Chem.,  70,  452-8. 
Ringer,  W.  E. 

(1902)  Z.anorg.Chem.,  32,  212. 
(1902)  Rec.trav.chim.,  21,  374. 
Ritzel,  A. 

(1911)  Z.Kryst.Min.,  49,  152. 
Robertson,  B. 

(1908)  J.Biol.Chem.,  5,  147-54. 
Robertson,  P.  W. 

(1907)  Chem.News,  95,  253. 
Robinet. 

(1864)  Compt.rend.,  58,  608. 
Robinson,  F.  W. 

(1909)  J.Chem.Soc.(Lond.),      95, 

1353-9- 
Robinson,  W.  O.  and  Waggaman,  W.H. 

(1909)  J.Phys.Chem.,  13,  673-8. 
Rodt,  V. 

(1916)     Mitt.k.  Materials    prufungs- 
amt,  33,  426-33. 

(1916)  Chem.Zentr.,  I,  1270. 
Rodwell. 

(1862)  J.Chem.Soc.(Lond.),  15,  59. 
Roelofsen. 

(1894)  Am.Chem.Jour.,  16,  466. 
Rogier  and  Fiore. 

(1913)  Bull.sci.Pharmacologique,  20, 

7,  72. 
Rohland,  P. 

(1897)  Z.anorg.Chem.,  15,  412. 

(1898)  Z.anorg.Chem.,  18,  328. 
Roloff,  M. 

(1894)  Z.physik.Chem.,  13,  341. 

(1895)  Z.physik.Chem.,  17,  325-56. 
(1895)  Z.physik.Chem.,  18,  572-84. 


812 


AUTHOR  INDEX 


Roozeboom,  H.  W.  B. 

(1884)  Rec.trav.chim.,  3,  29-87. 

(1885)  Rec.trav.chim.,  4,  69. 

(1887)  Rec.trav.chim.,  6,  342. 

(1888)  Z.physik.Chem.,  2,  459,  518. 

(1889)  Rec.trav.chim.,  8,  1-146. 

(1890)  Z.physik.Chem.,  5,  201. 

(1891)  Z.physik.Chem.,  8,  532. 

(1891)  Rec.trav.chim.,  10,  271. 

(1892)  Z.physik.Chem.,  10,  477. 

(1893)  Rec.trav.chim.,  12,  205. 

(1899)  Proc.k.Akad.Wet.(Amst.),  I, 

466. 
Roscoe. 

(1866)  J.Chem.Soc.(Lond.),  19,  504. 
Roscoe  and  Dittmar. 

(1859)  Liebig's  Annalen,  112-234. 
Rosenbladt. 

(1886)  Ber.,  19,  2531. 
Rosenheim,  A.  and  Bertheim,  A. 

(1903)  Z.anorg.Chem.,  34,  430. 
Rosenheim,  A.  and  Davidsohn,  I. 

(1903)  Z.anorg.Chem.,  37,  315. 
Rosenheim,  A.  and  Griinbaum. 

(1909)  Z.anorg.Chem.,  61,  187. 
Rosenheim,  A.  and  Pritze,  M. 

(1908)  Ber.,  41,  2708. 

(1909)  Z.anorg.Chem.,  63,  275-81. 
Rosenheim,  A.,  Stadler  and  Jakobsohn. 

(1906)  Ber.,  39,  2841. 
Rosenheim,  A.  and  Weinheber,  M. 

(1910-11)  Z.anorg.Chem.,  69,  263. 
Roshdestwensky,  A.  and  Lewis  W.  C. 
McC. 

(1911)  J.Chem.Soc.(Lond.),  99,  2144. 

(1912)  J.Chem.Soc.(Lond.),      101, 

2098. 
van  Rossem,  C: 

(1908)  Z.physik.Chem.,  62,  681-712. 
Rossler. 

(1873)  J.prakt.Chem.,  [2],  7,  14. 
Roth. 

(1897)  Z.physik.Chem.,  24,  123. 
Rothmund,  V. 

(1898)  Z.physik.Chem.,  26,  459,  475. 

(1900)  Z.physik.Chem.,  33,  406. 
(1908)  Z.Elektrochem.,  14,  532. 

(1910)  Z.physik.Chem.,  69,  523-546. 
(1912)  Nernst. Festschrift,  391-4. 
(1912)  Chem.Zentr.,  II,  1261. 

Rothmund,  V.  and  Wilsmore,  N.  T.  M. 

(1898)  Z.physik.Chem.,  26,  475. 

(1902)  Z.physik.Chem.,  40,  623. 
Rotinjanz,  L.  and  Rotarski,  T. 

(1906)    J.Russ.Phys.Chem.Soc.,    38, 

782. 
Rozsa,  M. 

(1911)  Z.  Elektrochem,  17,  935. 
Rubenbauer. 

(1902)  Z.anorg.Chem.,  30,  334. 
Rudorff. 

(1862)  Pogg.Ann.,  116,  63. 
(1869)  Ber.,  2,  70. 


Rudorff. 

(1872)  Pogg.Ann.,  145,  608. 

(1873)  Ber.,  6,  482. 

(1885)  Ber.,  18,  1160. 
Ruer. 

(1906)  Z.anorg.Chem.,  49,  365. 
Ruff,  Otto. 

(1909)  Ber.,  42,  4029. 
Ruff,  Otto  and  Fischer,  G. 

(1903)  Ber.,  36,  418-428. 
Ruff,  O.  and  Hecht,  L. 

(1911)  Z.anorg.Chem.,  70,  61. 
Ruff,  Otto  and  Geisel,  E. 

(1906)  Ber.,  39,  838. 
Ruff,  Otto  and  Plato,  W. 

(1903)  Ber.,  36,  2358-2365. 
Ruff,  O.  and  Schiller,  E. 

(1911)  Z.anorg.Chem.,  72,  341. 
Ruff,  O.  and  Winterfeld. 

(1903)  Ber.,  36,  2437. 
Rupert,  F.  F. 

(1909)  J.Am.Chem.Soc.,  31,  866. 

(1910)  J.Am.Chem.Soc.,  32,  748. 
Rutten  and  van  Bemmelen. 

(1902)  Z.anorg.Chem.,  30,  386. 
Ryd,  S. 

(1917)  Z.Elektrochem.,  23,  19-23. 
S. 

(1905)  Apoth.Ztg.,  20,  1031. 
Sackur,  O. 

(1911-2)   Z.physik.Chem.,  78,  553- 
568. 

(1913)  Z.physik.Chem.,  83,  297-314. 
Sackur,  O.  and  Fritzmann,  E. 

(1909)  Z.Elektrochem.,  15,  842-6. 
Sackur,  O.  and  Taegener,  W. 

(1912)  Z.Elektrochem.,  18,  722. 
Sahmen,  R. 

(1905-06)  Z.physik.Chem.,  54,  m- 

120. 
Sakabe,  S. 

(1914)  Mem.Coll.Sci. (Kyoto),  i,  57- 

61. 
Salkowski,  H. 

(1883)  Ber.,  18,  321. 

(1901)  Ber.,  34,  1947. 
Salkower,  B. 

(1916)  Am.J.Pharm.,  88,  484. 
Salzer. 

(1886)  Liebig's  Ann.,  232,  114. 
Sammet,  V. 

(1905)  Z.physik.Chem.,  53,  644-48. 
Sander,  W. 

(1911-12)  Z.physik.Chem.,  78,  513- 

549- 
Sandonmm,  C. 

(1911)  Atti  accad.Lincei,  [5],  20,  I, 

•     173,  253. 

(1911)  Gazz.chim.ital.,  41,  II,  146. 
(1911)  Atti  accad.Lincei,  [5],  20,  II, 

62,  497,  572,  588,  646. 
(191  la)  Atti  accad.Lincei,  [5],  20,  I, 

457,  76o. 


813 


AUTHOR  INDEX 


Sandonnini,  C. 

(1912)  Atti  accad.Lincei,  [5],  21,  I, 

208-13,  479. 
(i9i2a)  Atti  accad.Lincei,  [5],  21,  II, 

197,  524»  635. 
(i9i2b)  Atti  Ist.Ven.,  71,  553. 

(1913)  Atti  accad.Lincei,  [5],  22,  I, 

630;  II,  21. 

(1914)  Atti  accad.Lincei,   [5],  23,  I, 

962. 

(1914)  Gazz.chim.ital.,  44, 1,  296,  382 
Sandonnini,  C.  and  Aureggi,  P.  C. 
(1912)  Atti  accad.Lincei,   [5],  21,  I, 

493- 
Sandonnini,  C.  and  Scarpa,  G. 

(191  la)  Atti  accad.Lincei,  [5],  20,  II, 

62. 
(191  ib)  Atti  accad.Lincei,  [5],  20,  II, 

497- 

(1912)  Atti  accad.Lincei,  [5],  21,  II, 

77-84. 

(1913)  Atti  accad.Lincei,  [5],  22,  II, 

21,  163,  518. 
Sandquist,  H. 

(1911)  Liebig's  Ann.,  379,  85. 

(1912)  Liebig's  Ann.,  392,  76. 
Ark.Kem.Min.Geol.,  4,  8-8 1. 

Saposchinikow,  Gelvich  et  al. 

(1903)  J.Russ.Phys.Chem.Soc.,    35, 

(1904)  Z.physik.Chem.,  49,  688-96. 
Savorro,  Eglie. 

(1914)  Atti  accad.sci.  (Torino),    48, 

948-59. 

(1914)  Chem.Abs.,  8,  340. 
Sborgi,  U. 

(1913)  Atti  accad.Lincei,  [5],  22,  I, 

91,  636,  716,  798. 

(1915)  Atti  accad.Lincei,  [5],  24,  I, 

1225. 
Sborgi,  U.  and  Mecacci,  F. 

(1915)  Atti  accad.Lincei,  [5],  24,  I, 

443—8. 

(1916)  Atti  accad.Lincei,  [5],  25,  II, 

327,  386,  455. 
Scaffidi,  V. 

(1907)  Z.physik.Chem.,  52,  42. 
Scarpa,  G. 

(1912)  Atti  accad.Lincei,  [5],  21,  II, 

720. 
(1915)  Atti  accad.Lincei,  [5],  24,  I, 

741,  955;  II,  476. 
Scarpa,  O. 

(1904)  J.chim.phys.,  2,  449. 
Schachner,  Paul. 

(1910)  Biochem.Centralbl.,  9,  610. 
Schaefer,  G.  L. 

1910)  Am.Jour.Pharm.,  82,  175. 
1910)  Pharm.Jour.(Lond.),  84,  757. 
1912)  Am.Jour.Pharm.,  84,  389. 

(1913)  Am.Jour.Pharm.,  85,  441. 
Schafer,  H. 

(1905)  Z.anorg.Chem.,  45,  310. 


Schaefer,  W. 

(1914)  Neues  Jahrb.Min.Geol.,  I,  15- 

24. 
von  Scheele,  C. 

(1899)  Ber.,  32,  415. 
Scheffer,  F.  E.  C. 

(1911)  Proc.k.Akad.Wet.(Amst.),  13, 

829;  14,  195. 

(1912)  Z.physik.Chem.,  76,  161. 
(i9i2a)  Proc.k.Akad.Wet.(Amst.), 

15,  38o. 
Scheibler,  C. 

(1872)  Ber.,  5,  343. 

(1883)  J.pharm.chim.,  [5],  8,  540. 

(1891)  Ber.,  24,  434. 
Schenck,  R.  and  Rassbach,  W. 

(1908)  Ber.,  41,  2917. 
Scheuble,  R. 

(1907)  Liebig's  Ann.,  351,  473-80. 
Scheuer,  Otto. 

(1910)  Z.physik.Chem.,  72,  525-35. 
Schiavor,  G. 

(1902)  Gazz.chim.ital.,  32,  II,  532. 
Schick,  K. 

(1903)  Z.physik.Chem.,  42,  163. 
Schierholz. 

(1890)  Sitzber.k.Akad.Wiss.(Wien.), 

101,  2&,  4. 

Schiff. 

(1859)  Liebig's  Ann.,  109,  326. 

(1860)  Liebig's  Ann.,  113,  350. 

(1861)  Liebig's  Ann.,  118,  365. 
Schiff  and  Monsacchi. 

(1896)  Z.physik.Chem.,  21,  277. 
Schindelmeiser. 

(1901)  Chem.Ztg.,  25,  129. 
Schlamp,  A. 

(1894)  Z.physik.Chem.,  14,  272. 
Schloesing. 

(1871)  Compt.rend.,  73,  1273. 

(1872)  Compt.rend.,  74,  1552;  75,  70. 
Schlossberg,  J. 

(1900)  Ber.,  33,  1082. 
Schmidlin,  J.  and  Lang,  R. 

(1910)  Ber.,  43,  2813. 

(1912)  Ber.,  45,  905. 
Scholl,  R.  and  Steinkopf. 

(1906)  Ber.,  39,  4393. 
Scholtz,  M. 

(1901)  Ber.,  34,  1623. 
(1912)  Arch.Pharm.,  250,  418. 

Scheme. 

(1873)  Ber.,  6,  1224. 
Schonfeld. 

(1885)  Liebig's  Ann.,  95,  5. 
Schoorl,  N. 

(1903)  Rec.trav.chim.,  22,  40. 
Schrefeld. 

(1894)  Z.Ver.Zuckerind,  44,  971. 
Schreinemakers,  F.  A.  H. 

(1892)  Z.physik.Chem.,  9,  65,  71. 

(1897)  Z.physik.Chem.,  23,  417-41. 

(1898)  Z.physik.Chem.,  25,  543-67. 


814 


AUTHOR  INDEX 


Schreinemakers,  F.  A.  H. 

(1898)  Z.physik.Chem.,  26,  237-54. 
(18980)  Z.physik.Chem.,  27,  95-122. 

(1899)  Z.physik.Chem.,  29,  577. 

(1900)  Proc.k.Akad.Wet.(Amst.),  2, 

i. 

(1900)  Z.physik.Chem.,  33,  79. 
(1903)  Z.anorg.Chem.,  37,  207. 

(1906)  Z.physik.Chem.,  55,  89. 

(1907)  Z.physik.Chem.,  59,  641. 
(1908-09)  Z.physik.Chem.,  65,  555, 

575- 

(1908)  Chem.Weekblad.,  5,  847. 

(1909)  Z.physik.Chem.,  66,  687-98. 

(1909)  Chem.Weekblad.,  6,  131,  140. 
(1909-10)   Z.physik.Chem.,  68,  83- 

103. 

(1910)  Arch.neer.sc.ex.nat.,   [2],   15, 

81,  117. 

1910)  Z.physik.Chem.,  69,  557~68. 
ioa)  Z.physik.Chem.,  71,  109-16. 

I9iob)  Chem.Weekblad.,  7,  333. 

1911)  Proc.k.Akad.Wet.(AmstJ,  13, 

1163. 

Schreinemakers,  F.  A.  H.  and  de  Baat, 
W.  C. 

(1908)  Chem.Weekbl.,  5,  465-72. 
(1908-9)  Z.physik.Chem.,  65,  586. 

(1909)  Z.physik.Chem.,  67,  551-60. 

(1910)  Chem.Weekblad.,  7,  259. 
(igioa)  Arch.neer.sc.ex.nat.,  [2],  15, 

4-15- 

(1914)  Proc.k.Akad.Wet.(Amst.),  17, 

533,  78i. 

(1915)  Proc.k.Akad.Wet.(Amst.),  17, 

mi. 
(1915)  Verslag.k.Akad.Wet.(Amst.), 

23,  1097;  May. 
(1917)    Chem.Weekblad.,    14,    141, 

203,  244. 
(1917)  Chem.  Weekblad.,  14,  262-7, 

288. 
Schreinemakers,  F.A.H.  and  Cocheret, 

D.  H. 

(1905)  Chem.Weekblad.,  2,  771-778. 
Schreinemakers,  F.  A.  H.  and  Cocheret, 

D.  H.,  Filippo,  H.  and  de 
Waal,  A.  J.  C. 

(1901)  Z.physik.Chem.,  59,  645. 
Schreinemakers,  F.  A.  H.  and  Deuss, 

J.  J.  B. 

(1912)  Z.physik.Chem.,  79,  554. 
Schreinemakers,   F.   A.   H.   and  Van 
Dorp,  W.  A.  Jr. 

(1906)  Chem.Weekblad.,  3,  557-561. 

(1907)  Z.physik.Chem.,  59,  641-69. 
Schreinemakers,  F.  A.  H.  and  Figee,  T. 

(1911)  Chem.Weekblad.,  8,  683-8. 
Schreinemakers,  F.  A.  H.  and  Filippo, 

A.  Jr. 

(1906)  Chem.Weekblad.,  3,  157-165. 
(1906)  Chem.Zentralbl.,  77,  I,  1321. 


Schreinemakers,  F.  A.  H.  and  Hoenen, 
P.  H.  J. 

(1909)  Chem.Weekblad.,  6,  51. 
Schreinemakers,  F.  A.  H.  and  Van  der 

Horn   van   den   Bos,    J. 
L.M. 

(1912)  Z.physik.Chem.,  79,  551. 
Schreinemakers,  F.  A.  H.  and  Jacobs, 

W. 

(1910)  Chem.Weekblad.,  7,  215. 
Schreinemakers,  F.  A.  H.  and  Massink, 

A. 

(1910)  Chem.Weekblad.,  7,  214. 
Schreinemakers,  F.  A.   H.   and  Mei- 

jeringh,  D.  J. 

(1908)  Chem.Weekblad.,  5,  811. 
Schreinemakers,  F.   A.  H.   and   Van 
Provije,  D.  J. 

(1913)  Proc.k.Akad.Wet.,  15,  1326. 
Schreinemakers,  F.  A.  H.  and  Thonus, 

J.  C. 
(1912)  Proc.k.Akad.Wet.(Amst.),  15, 

472. 
Schroder. 

(1893)  Z.physik.Chem.,  u,  449. 
Schroeder,  J. 

(1905)  Z.anorg.Chem.,  44,  6. 

(1908)  J.prakt.Chem.,  [2],  77,  267-8. 
Schiikarew,  A. 

(1901)  Z.physik.Chem.,  38,  543. 
Schukow. 

(1900)  Z.Ver.Zuckerind,  50,  313. 
Schuler. 

(1879)  Sitzb.k.Akad.Wis. (Berlin), 79, 

302. 
Schultz. 

(1860)  Zeit.Chem.,  [2],  5,  531. 

(1861)  Pogg.Ann.,  113,  137. 
Schulze. 

(1881)  J.prakt.Chem.,  [2],  24,  168. 
Schweissinger. 

(1884-85)  Pharm.Ztg. 
Schweitzer. 

(1890)  Z.anal.Chem.,  29,  414. 
Schwicker. 

(1889)  Ber.,  22,  1731. 
Sedlitzky. 

(1887)  Monatsh.Chem.,  8,  563. 
Seidell,  A. 

1902)  Am.Chem.Jour.,  27,  52. 

1907)  J.Am.Chem.Soc.,  29,  1088-95. 

1908)  Trans. Am. Electrochem.Soc., 

13,  319-329- 

(1909)  J.Am.Chem.Soc.,  31,  1164. 

(1910)  Bull.No.67  Hygienic  Labora- 

tory, U.  S.  Public  Health 

Service, 
(igioa)  Proc.Am.Pharm.Assoc.,    58, 

1031. 

(1912)  Am.Chem.Jour.,  48,  453-67. 
Seidell,  A.  and  Smith,  J.  G. 
(1904)  J.Phys.Chem.,  8,  493. 


815 


AUTHOR  INDEX 


Self,  P.  A.  W.  and  Greenish,  H.  G. 

(1907)  Pharm.Jour.(Lond.),  78,  327. 
Seliwanow,  Th. 

(1914)  Z.anorg.Chem.,  85,  337. 
Sehnal,  J. 

(1909)  Compt.rend.,  148,  1394. 
Serullas. 

(         )  Ann.chim.phys.,  22,  118. 
Sestini. 

(1890)  Gazz.chim.ital.,  20,  313. 
Setschenow. 

(1892)  Ann.chim.phys.,  [6],  25,  226. 
Setterburg. 

(1882)  Liebig's  Annalen,  211,  104. 
Seubert  and  Elten. 

(1892)  Z.anorg.Chem.,  2,  434. 
Seyler,  C.  A. 

(1908)  Analyst,  33,  454~7- 
Seyler,  C.  A.  and  Lloyd,  P.  V. 

(1909)  J.Chem.Soc.(Lond.),  95>I347~ 

Shad,  H.  and  Bornemann,  K. 

(1916)  Metall  u.Erz.,  13,  251-62. 
Sharwood,  W.  J. 

(1903)  J.Am.Chem.Soc.,  25,  576. 
Sherrill,  M.  S. 

(1903)  Z.physik.Chem.,  43,  705-740. 
Sherrill,  M.  S.  and  Eaton,  F.  M. 

(1907)  J.Am.Chem.Soc.,  29,  1643. 
Sherrill,  M.  S.  and  Russ,  D.  E. 

(1907)  J.Am.Chem.Soc.,  29,  1657-61. 
Shiomi,  T. 

(1908)  Mem.Coll.Sci.Eng.  (Kyoto),  i, 

406-13. 
Sidgwick,  N.  V. 

(1910)  Proc.Chem.Soc.(Lond.),    26, 

60-1. 

(1911)  J.Chem.Soc.(Lond.),99,  1123. 

(1915)  J.Chem.Soc.(Lond.),  107,  672. 
Sidgwick,  N.  V.,  Pickford,  P.  and  Wils- 

don,  B.  H. 

(1911)  J.Chem.Soc.(Lond.),9Q,ii22- 

1132. 
Sidgwick,  N.  V.,  Spurrell,  W.  J.  and 

Davies,  T.  E. 
(1915)      J.Chem.Soc.(Lond.),      107, 

1202-13. 
Siebeck. 

(1909)  Scand.Arch.f.Physiol.,  21,  368. 
Sieger,  W. 

(         )  Dissertation,  Delft,  156. 

(1912)  "Tables,  annuelles,"  3,  337. 
Sieverts,  A.  and  Co-workers. 

(1909)  Ber.,  42,  338. 

(1910)  Ber.,  43,  893. 
(1912)  Ber.,  45,  221. 

Sieverts,  A.  and  Bergner,  E. 

"-  4s> 


(1905)  Z.physik.Chem.,  51,  577-602. 
(1916)  J.Am.Chem.Soc.,  38,  2632. 
Sims. 


(1861)  Liebig's  Ann.,  118,  340. 


Sinnige,  L.  R. 

(1909)  Z.physik.Chem.,  67,  432-45. 
Sisley,  P. 

(1902)  Bull.soc.chim.,  [3],  27,  905. 
Skirrow,  F.  W. 

(1902)  Z.physik.Chem.,  41,  144. 
Skinner,  S. 

(1892)  J.Chem.Soc.(Lond.),  61,  342. 
Skossareswky,  M.  and  Tchitchinadze, 

(1916)  J.chim.phys.,  14,  153-175. 
Skrabal,  A. 

(1917)  Monatsh.Chem.,  38,  25-9. 
Slade,  R.  E. 

(1912)  Z.Elecktrochem.,  18,  i. 
Sloan  and  Mallet. 

(1882)  Chem.News.,  46,  194. 
Slothouwer,  J.  H. 

(1914)  Rec.trav.chim.,  33,  327. 
Smirnoff,  Wladimer. 

(1907)  Z.physik.Chem.,  58,  373,  667. 
Smith. 

(1912)  Landolt  and  Bornstein  "Tab- 

ellen,"  4th  Ed.,  p.  481. 
Smith  and  Bradbury. 

(1891)  Ber.,  24,  2930. 
Smith,  A.  and  Carson,  C.  M. 

(1908)  Z.physik.Chem.,  61,  200. 
Smith,  A.  and  Eastlack,  H.  E. 

(1916)  J.Am.Chem.Soc.,    38,    1500, 

1265. 
Smith,  A.,  Holmes,  W.  B.  and  Hall,  E.S. 

(1905)  J.Am.Chem.Soc.,  27,  805. 
Smith,  A.  and  Menzies,  A.  W.  C. 

(1909)  J.Am.Chem.Soc.,  31,  1183-91. 
Smith,  C.  and  Watts,  C.  H. 

(1910)  J.Chem.Soc.(Lond.),  97,  568. 
Smith,  F.  Hastings. 

(1917)  J.Am.Chem.Soc.,  39,  1309. 
Smith,  G.  McP.  and  Ball,  T.  R. 

(1917)  J.  Am.Chem.Soc.,  39,  217. 
Smith,  Herbert,  J. 

(1918)  J.Am.Chem.Soc.,  40,  879-885. 
Smith,  W.  R. 

(1909)  J.Am.Chem.Soc.,  31,  245. 
Smits,  A. 

(1903)  Z.Elecktrochem,  9,  663. 
Smits,  A.  and  Bokhorst,  S.  C. 

(1915)  Z.physik.Chem.,  89,  374. 
Smits,  A.  and  Kettner,  A. 

(1912)  Proc.k.Akad.Wet.(Amst.),  15, 

685. 
Smits,  A.  and  de  Leeuw,  H.  L. 

(1910)  Proc.k.Akad.Wet.(Amst.),  13, 

329- 
Smits,  A.  and  Maarse,  J. 

(1911)  Proc.k.Akad.Wet.(Amst.),  14, 

192. 
Smits,  A.  and  de  Mooy. 

(1910)  Verslag.Akad.Wet.(Amst.), 
19,  293. 


816 


AUTHOR   INDEX 


Smits,  A.  and  Postma,  S. 

(1914)  Proc.k.Akad.Wet.(Amst.),  17, 

183- 
Smolensky,  S. 

(1911-12)  Z.anorg.Chem.,  73,  293. 
Sneider. 

(1866)  Pogg.Ann.,  127,  624. 
Snell,  J.  F. 

(1898)  J.Phys.Chem.,  2,  474,  484. 
Snyder. 

(1878)  Ber.,  n,  936. 
Soch,  C.  A. 

(1898)  J.Phys.Chem.,  2,  43. 
Sommer,  F. 

(1914)  Z.anorg.Chem.,  86,  85. 
Sosman,  R.  B.  and  Merwin,  H.  E. 

(1916)  J.Wash.Acad.Sci.,  6,  532-537- 
Souchay  and  Leussen. 

(1856)  Liebig's  Ann.,  99,  33. 
Spencer,  J.  F. 

(1912)  Z.physik.Chem.,  80,  701. 

(1913)  Z.physik.Chem.,  33,  293. 
Spencer  and  LePla. 

(1909)  Z.anorg.Chem.,  65,  14. 
Speyers,  C.  L. 

(1902)  Am.J.Sci.,  [4],  14,  294. 
Spielrein,  C. 

(1913)  Compt.rend.,  157,  46. 
Spring  and  Romanoff. 

(1896)  Z.anorg.Chem.,  13,  34. 
Squire,  P.  W.  and  Caines,  C.  M. 

(1905)  Pharm.Jour.(Lond.),  74,  720, 

784. 
v.  Stackelberg,  E.  F. 

(1896)  Z.physik.Chem.,  20,  337-58. 
van  der  Stadt,  E. 

(1902)  Z.physik.Chem.,  41,  353. 
Stanley,  H. 

(1904)  Chem.News,  89,  193. 
Stark,  G. 

(1911)  Z.anorg.Chem.,  70,  174. 
Steger. 

(1903)  Z.physik.Chem.,  43,  595. 
Stern,  Otto. 

(1912-13)  Z.physik.Chem.,  81,  468. 
Staronka,  W. 

(1910)  Anzeiger  akad.Wis.Krakau. 

Ser.A.,  372-98. 

(1910)  Chem.Zentralbl.,  81,  1741. 
Stasevich,  N. 

(1913)    J.Russ.Phys.Chem.Soc.,    45, 

912-30. 
Steele  and  Johnson. 

(1904)  J.Chem.Soc.(Lond.),  85,  116. 
Steiner,  P. 

( 1 894)  Ann.der. Physik.  ( Wiederman) , 

52,  275. 
Stemwehr. 

(1902)  Ann.der  Physik. (Drude),  [4], 

9,  1050. 
Stepanow,  A. 

(1907)  Z.ges.Schiess.u.Sprengstoffw., 


Stepano,  A. 

(1910)  J.Russ.Phys.Chem.Soc.,  42, 
489. 

(1910)  Liebig's  Ann.,  373,  219. 
Stiassny. 

(1891)  Monatsh.Chem.,  12,  601. 
Stich,  C. 

(1903)  Pharm.Ztg.,  48,  343. 

(1903)  Pharm.Jour.(Lond.),  70,  700. 
Stock,  A. 

(1904)  Ber.,  37,  1432. 

(1910)  Ber.,  43,  156,  1227. 
Stock,  A.  and  Kuss,  E. 

(1917)  Ber.,  50,  159-164- 
Stoermer,  R.  and  Heymann,  P. 

(1913)  Ber.,  46,  1255. 
Stolba. 

(1865)  J.prakt.Chem.,  94,  406. 
(1867)  J.prakt.Chem.,  101,  I. 
(1872)  Z.anal.Chem.,  n,  199. 
(1877)  Chem.Centralbl.,  418,  578. 
(1883)  Chem.Centralbl.,  293. 
(1889)   Chem.Techn.Cent.,  Anz.,  7, 

Stolle.  459' 

(1900)  Z.Ver.Zuckerind.,  50,  331. 
Stoltzenberg,  H. 

(1912)  Ber.,  45,  2248. 

(1914)  Z.physik.Chem.,  92,  461-94. 
Stortenbecker,  W. 

(1888)  Rec.trav.chim.,  7,  152. 

(1889)  Z.physik.Chem.,  3,  n. 
(1897)  Z.physik.Chem.,  22,  62. 
(1900)  Z.physik.Chem.,  34,  109. 

(1902)  Rec.trav.chim.,  21,  407. 

(1907)  Rec.trav.chim.,  26,  245. 
Straub,  Jan. 

(1911)  Z.physik.Chem.,  77,  332. 
Stromholm,  D. 

(1900)  Ber.,  33,  835. 

(1903)  Z.physik.Chem.,  44,  721-32. 

(1908)  Z.anorg.Chem.,  57,  72-103. 
Struve. 

1870)  Z.anal.Chem.,  9,  34. 
1899)  J.prakt.Chem.,  [2],  61,  457. 
Sudborough,  J.  J.  and  Lakhumalani, 

J.V. 

(1917)  J.Chem.Soc.(Lond.),  in,  44. 
Sudhaus,  Kathe. 

(1914)  Neues  Jahrb.Min.Geol.(Beil. 

Bd.),  37,  1-50. 
Sulc. 

(1900)  Z.anorg.Chem.,  25,  401. 
Siiss,  J. 

(1913)  Z.Kryst.Min.,  51,  262. 
Suyver,  J.  F. 

(1905)  Rec.trav.chim.,  24,  381,  397. 
Swan,  Clifford,  M. 

(1899)  "  Chemistry  Thesis,"  Mass. 
Inst.Technology,  (un- 
published). 

(1911)  J.Am.Chem.Soc.,  33,  1814. 


817 


AUTHOR  INDEX 


Swinne,  R. 

(1913)  Z.physik.Chem.,  84,  348. 
Szathmary  de  Szachmar,  L.  v. 

(1910)  Z.Farb.Ind.,  7,  215. 

(1910)  Chem.Abs.,  4,  1381. 
de  Szyszkowski,  Bohdan. 

(1915)  Medd.K.Vetenskapsakad,No- 

belinst.,  3,  Nos.  3,  4,  5. 
Taber,  W.  C. 

(1906)  J.Phys.Chem.,  10,  593. 

(1906)  Bull.,  33,  Bureau  of  Soils,  U.  S. 

Dept.  Agr. 
Tafel,  J. 

(1901)  Ber.,  34,  263. 
Takenchi,  J. 

(1915)  Mem.Coll.Sci. (Kyoto),  1,249- 

55- 
Tamm,  O. 

(1910)  Z.physik.Chem.,  74,  499. 
Tarugi,  N. 

(1904)  Gazz.chim.ital.,  34,  I,  329. 

(1914)  Gazz.chim.ital.,  44,  I,  131. 
Tarugi,  N.  and  Checchi,  Q. 

(1901)  Gazz.chim.ital.,  31,  II,  430, 

445- 
Taverne,  H.  J. 

(1900)  Rec.trav.chim.,  19,  109. 
Taylor,  H.  S.  and  Henderson,  W.  N. 

(1915)  J.Am.Chem.Soc.,  37,  1692. 
Taylor,  S.  F. 

(1897)    J.Phys.Chem.,    i,   301,   468, 

720. 
Tcherniac,  J. 

(1916)  J.Chem.Soc.  (Lond.), 109,1239. 
Tetta  Polak'van  der  Goot. 

(1913)  Z.physik.Chem.,  84,  419-50. 
Than. 

(1862)  Liebig's  Ann.,  123,  187. 
Thiel. 

(1903)  Z.physik.Chem.,  43,  656. 
Thilo. 

(1892)  Chem.Ztg.,  16,  II,  1688. 
Thin,  R.  G.  and  Gumming,  Alex.  C. 

(1915)      J.Chem.Soc.(Lond.),      107, 

361-6. 
Thomas. 

(1896)  Compt.rend.,  123,  943. 
Thomas,  J.  S.  and  Rule,  A. 

(1917)  J.Chem.Soc.  (Lond.),    in, 

1063-85. 
Thompson,  M.  de  K. 

(1910)  Met.Chem.Eng.,  8,  279,  324. 

(1910)  Proc.Am.Acad.,  45,  431-52. 
Thonus,  J.  C. 

(1913)  Verslag.k.Akad.Wet.(Amst.), 

Thorin,  E.  G. 

(1915)  Z.physik.Chem.,  89,  687. 
Tichomirow,  W. 

(1907)  J.Russ.Phys.Chem.Soc.,    39, 

(1908)  Chem.Zentralbl.,  I,  n. 


Tilden,  W.  A. 

(1884)  J.Chem.Soc.(Lond.),  45,  269, 

409. 
Tilden  and  Shenstone. 

(1883)  Proc.Roy.Soc.(Lond.),  35,  345 

(1884)  Phil.Trans.,  23-31. 

(1885)  Proc.  Roy.  Soc.   (Lond.),  38, 

331- 
Timofeiew,  Wladimir. 

(1890)  Z.physik.Chem.,  6,  147. 

(1891)  Compt.rend.,  112,  1137,  1224. 
(1894)  Dissertation  (Kharkhov.) 

Timofeiew  and  Kravtzov. 

(1915)  Chem.Abs.,  9,  2896. 
(1917)  Chem.Abs.,  n,  788. 

Timmermans,  J. 

(1907)  Z.physik.Chem.,  58,  129-213. 

(1910)  Proc.k.Akad.Wet.(Amst.)  13, 

523- 

(1911)  "  Recherches  experimentales 

sur  les  phenomenes  de 
demixtion  des  melanges 
liquides  "  (These)  Brux- 
elles.  Avril,  1911. 

(1912)  Bull.soc.chim.(Belg.),  26,  382. 
Tinkler,  C.  K. 

(1913)  J.Chem. Soc.  (Lond.), 103, 2176. 
Titherby,  A.  W. 

(1912)  Pharm. Jour. (Lond.),  88,  94. 
Tobler. 

(1855)  Liebig's  Ann.,  95,  193. 
Tower. 

(1906)  Z.anorg.Chem.,  50,  382. 
Traube. 

(1884)  Ber.,  17,  2304. 
Traube,  I. 

(1909)  Ber.,  42,  2185,  4185-8. 
Trautz  and  Anschutz. 

(1906)  Z.physik.Chem.,  56,  238. 
Treadwell  and  Reuter. 

(1898)  Z.anorg.Chem.,  17,  185. 
Treis,  K. 

(i9i4)Neues.Jahr.Min.(Beil.Bd.),37, 

766-818. 
Trevor. 

(1891)  Z.physik.Chem.,  7,  470. 
Truthe,  W. 

(i9i2)Z.anorg.Chem.,  76,  129-173. 
Tsakalotos,  D.  E. 

(1909)  Bull.soc.chim.,  [4],  5,  397-4°9- 

(1910)  Jour.chim.phys.,  8,  343. 

(1912)  Bull.soc.chim.,  4],  11,287. 

(1913)  Bull.soc.chim.,   4],  13,  282. 

(1914)  J.chim.phys.,  12,  461-3. 
Tsakalotos,  D.  E.  and  Guye,  P.  A. 

(1910)  J.chim.phys.,  8,  340. 
Tschugaeff,  L.  A.  and  Chlopin  W. 
(Chugaev,  L.  and  Khlopin,  W.) 

(1914)  Z.anorg.Chem.,  86,  159. 
Tschugaeff,  L.  A.  and  Kiltinovic,  S.  S. 

(1916)  J.Chem. Soc. (Lond.)  109, 1286. 
Tuchschmidt,  C.  and  Follenius,  0. 

(1871)  Ber.,  4,  583. 


818 


AUTHOR  INDEX 


Turner,  W.  E.  S.  and  Bissett,  C.  C. 

(1913)  J.Chem.Soc.(Lond.),  103,1904. 
Tutton,  A.  E.  H. 

(1897)  J.Chem.Soc.(Lond.),  ?i>  850. 

(1907)     Proc.Roy.Soc.(LoncL),     79, 

(A)  351-82. 
Tyrer,  Dan. 

(1910)  Jour.Chem.Soc.(Lond.),    97» 

1778-1788. 

(igioa)  Jour.Chem.Soc.(Lond.),  97, 
621-632. 

(1911)  Proc.Chem.Soc.(Lond.),    27, 

142. 
Uhlig,  J. 

(1913)  Centr.Min.Geol.,  417-22. 
Ullik. 

(1867)  Liebig's  Ann.,  144,  244. 
Umney,  J.  C.  and  Bunker,  S.  W. 
>  (1912)  Perf.  Essent.  Oil  Record,  3, 

ioi;4,38. 
Unkovskaja,  V. 

(1913)    J.Russ.Phys.Chem.Soc.,    45, 
x  1099. 

u.  s.  P.,  vni. 

(1907)  U.    S.     Pharmacopoeia,   8th, 

decennial  revision. 
Usher,  F.  L. 

(1908)  Z.physik.Chem.,  62,  622-5. 
(1910)  J.Chem.Soc.(Lond.),  97,  66- 

78. 
Usso. 

(1904)  Z.anorg.Chem.,  38,  419. 
Uyeda,  K. 

(1909-10)  Mem. Coll. Sci.Eng.  (Ky- 
oto), 2,  245-261. 

(1912-13)  Mem.Coll.Sci.Eng.  (Ky- 
oto), 5,  147-50. 

(1912)  8th  Int.Cong.Appl.Chem.,  22, 

237. 
Valenta. 

(1894)  Monatsh.Chem.,  15,  250. 
Valeton,  J.  J.  P. 

(1910)  Verslag  k.Akad.Wet.(Amst.), 

18,  755-  • 
Valeur,  A. 

(1917)  Compt.rend.,  164,  818-20. 
Van  de  Moer,  J. 

(1891)  Rec.trav.chim.,  10,  47. 
Vandevelde,  A.  J.  J. 

(1911)  Bull.soc.chim.(Belg.),  25,210. 
Van  Eyk,  C. 

(1899)  Z.physik.Chem.,  30,  430. 

(1900)  Proc.k.Akad.Wet.(Amst.),  2, 

480. 

(1901)  Proc.k.Akad.Wet.(Amst.),  3, 

98. 

(1905)  Z.physik.Chem.,  51,  721. 
(1905)  Chem.News.,  91,  295. 

Van  Name,  R.  S.  and  Brown,  W.  G. 

(1917)  Am.Jour.Sci.,  [4],  44,  105-23. 
Van  Slyke,  L.  L.  and  Winter,  O.  B. 

(1913)  Science,  38,  639. 


Vanstone,  E. 

(1909)  J.Chem.Soc.(Lond.),  95,  597. 

(1913)  J,Chem.Soc.(Lond.),      103, 

1828. 

(1914)  J.Chem.Soc.(Lond.),      105, 

1491-1503. 

Van't  Hofif  see  van't  Hoff. 
Van  Wyk,  H.  J. 

(1902)  Z.anorg.Chem.,  32,  115. 

(1905)  Z.anorg.Chem.,  47,  1-52. 
Varenne  and  Pauleau. 

(1881)  Compt.rend.,  93,  1016. 
Vasiliev,  A.  M.  (Wasilieff). 

(1909)  J.Russ.Phys.Chem.Soc.,    41, 

748-53;  953-7- 

(1910)  J.Russ.Phys.Chem.Soc.,    42, 

423,  562-81. 
(1910)  Chem.Zentralbl.,11,  1527. 

(1910)  "  Tables  annuelles,"  I,  381. 

(1911)  J.Russ.Phys.Chem.Soc. 

(1912)  Chem.Abs.,  6,  577. 

(1912)    J.Russ.Phys.Chem.Soc.,    44, 

1076. 
Vaubel. 

(1895)  J.prakt.Chem.,  [2],  52,  72. 

(1896)  Z.physik.Chem.,  25,  95. 
(1899)  J.prakt.Chem.,  [2],  59,  30. 
.(1903)  J.prakt.Chem.,  [2],  67,  472. 

Vesterberg,  A. 

(1912)  8th  Inter.Congr.Appl.Chem., 

2,  238,  255. 

Vezes,  M.  and  Mouline,  M. 

(1904)  Bull.soc.chim.,  [3],  31,  1043. 

(1905-06)  Proc.  verb. soc.phys.nat. 

(Bordeaux),  123. 
Viala,  F. 

(1914)  Bull.soc.chim.,  [4],  15,  5. 
Vignon,  Leo. 

(1891)  Bull.soc.chim.,  [3],  6,  387,  656. 

(1891)  Compt.rend.,  113,  133. 
Virck. 

(1862)  Chem.Centralbl.,  402. 
Voerman,  G.  L. 

(1906)  Chem.Zentralbl.,  77,  I,  125. 

(1907)  Rec.trav.chim.,  26,  293. 
Vogel,  Fritz. 

(1903)  Z.anorg.Chem.,  35,  389. 
Vogel. 

(1867)  Neues  Repert.Pharm.,  16,  557. 

(1874)  Neues  Repert.Pharm.,  23, 335. 
Volkhouskii. 

(1910)    J.Russ.Phys.Chem.Soc.,    41, 

1763;  42,  1 1 80. 
Vortisch,  E. 

(1914)  Neues  Jahrb.Min.Geol.(Beilt 
Bd.),  38,  185-272. 

(19143)  Neues  Jahrb.Min.Geol.(Beil. 

Bd.),  38,  513-24- 
Vulpius. 

(1893)  Pharm.Centralh.,  34,  117. 
de  Waal,  A.  J.  C. 

(1910)  Dissertation,  Leyden. 

(1910)  "  Tables  annuelles." 


819 


AUTHOR  INDEX 


Waddell,  John. 

(1898)  J.Phys.Chem.,  2,  236. 

(1899)  J.Phys.Chem.,  3,  160. 

(1900)  J.Phys.Chem.,  4,  161. 
Waentig,  P.  and  Mclntosh,  D. 

(1916)    Trans. Roy.Soc. (Canada),   9, 

203^9. 
Wagner. 

(1867)  Z.anal.Chem.,  6,  167. 
Wagner,  C.  L. 

(1910)  Z.physik.Chem.,  71,  430. 
Wagner,  K.  L.  and  Zeraer,  E. 

(1911)  Monatsh.Chem.,  31,  833. 
Wagemmann,  K. 

(1912)  Metallurgie,  9,  518,  537. 
Walden,  P.  T. 

.     (1905)  Am.Chem.Jour.,  34,  149. 

(1906)  Z.physik.Chem.,  55,  712. 
Walden,  P.  T.  and  Centnerszwer,  M. 

(1902-03)  Z.physik.Chem.,  42,  454. 
Walker,  J. 

(1890)  Z.physik.Chem.,  5,  195. 
iWalker,  J.  and  Fyffe,  W.  A. 

(1903)  J.Chem.Soc.(Lond.),  83,  179. 
Walker,  J.  and  Wood,  J.  K. 

(1898)  J.Chem.Soc.(Lond.),  73,  620. 
Wallace. 

(1855)  J.Chem.Soc.(Lond.),  7,  80. 
Wallace. 

(1909)  Z.anorg.Chem.,  63,  I. 
Waller,  A.  D. 

(1904-05)  Proc.Roy.Soc.(Lond.),  74, 

55- 
Walton,  J.  H.  Jr.,  and  Judd,  R.  C. 

(1911)  J.Am.Chem.Soc.,  33,  1036. 
Walton,  J.  H.,  and  Lewis,  H.  A. 

(1916)  J.Am.Chem.Soc.,  38,  633. 
Wartha. 

(1885)  Z.anal.Chem.,  24,  220. 
Warynski,  T.  and  Kourapatwinska,  S. 

(1916)  J.chim.phys.,  14,  328-35. 
Washburn,  E.  W.  and  Maclnnes. 

(1911)  Z.Elektrochem.,  17,  503. 
Washburn,  E.  W.  and  Read,  J.  W. 

(1915)  Proc.Nat.Acad.Sci.(y.  S.  A.), 

i,  191-5- 

Wasilieff  (see  Vasiliev). 
Wedekind,  E.  and  Paschke,  F. 

(1910)  Z.physik.Chem.,  73,  127. 
Wegscheider,  R. 

(1907)  Liebig's  Ann.,  351,  87. 
Wegscheider,  R.  and  Walter,  H. 

(1905)  Monatsh.Chem.,  26,  685. 
(1907)  Monatsh.Chem.,  28,  633-72. 

Weigel,  O. 

(1906)  Nachr.kgl.Ges.Gottingen,    p. 

525-48. 

(1907)  Z.physik.Chem.,  58,  293-300. 
Weiller,  P. 

(1911)  Chem.Ztg.,  35,  1063-5. 
von  Weimarn,  P.  P. 

(1911)  Z.physik.Chem.,  76,  218. 


Weisberg. 

(1896)  Bull.soc.chim.,  [3],  15,  1097. 
Wells,  H.  L. 

(1892)  Am.Jour.Sci.,  [3],  44,  221. 
Wells,  H.  L.  and  Wheeler,  H.  L. 

™(!,892^  Am.Jour.Sci.,  [3l,  43,  475- 
Wells,  R.  C. 

(1915)  J.Wash.Acad.Sci.,  5,  617-22. 

(1915)  J.Am.Chem.Soc.,  37,  1704. 
Wells,  R.  C.  and  McAdam,  D.  J.,  jr. 

(1907)  J.Am.Chem.Soc.,  29,  721-7. 
Welsh,  T.  W.  B.  and  Broderson,  H.  J. 

(1915)  J.Am.Chem.Soc.,  37,  816. 
Wempe,  G. 

(1912)  Z.anorg.Chem.,  78,  298-327. 
Wenger. 

(1892)  Am.Chem.Jour.,  16,  466. 
Wenger,  Paul. 

(1911)  Dissertation,  Geneve. 

(1911)  "  Tables  annuelles,"  2,  411. 
Wentzel. 

(        )  Dammer's  "  Handbuch,"  II, 

2,  858. 
Wenze. 

(1891)  Z.angew.Chem.,  5,  691. 
Werner,  E.  A. 

(1912)  J.Chem.Soc.(Lond. ),  101,2169. 
Wester,  D.  H.  and  Bruins,  A. 

(1914)  Pharm.Weekblad,  51,  1443-6. 
Wheeler,  H.  L. 

1892)  Am.J.Sci.,  [3],  44,  123. 

1893)  Am.J.Sci.,  [3],  45,  267. 
i893a)  Z.anorg.Chem.,  3,  432. 

Wherry,  E.  T.  and  Yanovsky,  E. 

(1918)  J.Am.Chem.Soc.,  40,  1072. 
Whipple,  G.  C.  and  Whipple.  M.  C. 

(1911)  J.Am.Chem.Soc.,  33,  362. 
Whitby,  G.  S. 

•     (1910)  Z.anorg.Chem.,  67,  107-9. 
Whitney,  W.  R.  and  Melcher,  A.  C. 

(1903)  J.Am.Chem.Soc.,  25,  78. 
Wibaut,  J.  P. 

(1909)  Chemisch  Weekblad,  6,  401. 

(1913)  Rec.tr.av.chim.,  32,  269. 
Wigand,  A. 

(1910)  Z.physik.Chem.,  75,  235. 
Wildeman. 

(1893)  Z.physik.Chem.,  n,  421. 
Willstaetter. 

(1904)  Ber.,  37,  3753. 
Wilsmore. 

(1900)  Z.physik.Chem.,  35,  305. 
Wingard,  A. 

(1917)     Svensk.Farm.Tidskrift,     21, 

289-93. 

(1917)  Chem.Abs.,  u,  2748. 
Winkler,  L.  W. 

(1887)   J.prakt.Chem.,    [2],   34,  177; 

36,  177- 

(1891)  Ber.,  24,  3609. 
(1899)  Chem.Ztg.,  23,  687. 

(1901)  Ber.,  34,  1409,  1421. 


820 


AUTHOR  INDEX 


Winkler,  L.  W. 

(1905)  Landolt  and  Bernstein  "  Tab- 

ellen,"  3rd  Ed.,-  p.  604. 

(1906)  Z.physik.Chem.,  55,  350. 
(1912)  Landolt  and  Bornstein  "  Tab- 

ellen,"  4th  Ed.,  p.  597,  601. 
Winteler,  F. 

(1900)  Z.Elektrochem.,  7,  360. 
Winterstein,  E. 

(1909)  Arch. exp. Path. u.Pharm.,  62, 

Wirth,  F. 

(1908)  Z.anorg.Chem.,  58,  219. 

(1912)  Z.anorg.Chem.,  76,  174-200. 

(1912-13)  Z.anorg.Chem.,  79,  357. 

(1914)  Z.anorg.Chem.,  87,  1-12. 
Wirth,  F.  and  Bakke,  B. 

(1914)  Z.anorg.Chem.,  87,  29,  47. 
Witt,  O.  N. 

(1915)  Ber.,  48,  767. 
v.  Wittorff,  N. 

(1904)  Z.anorg.Chem.,  41,  83. 
Wolfmann. 

(1897)    Oster.Ung.Z.Zuckerind.,    25, 

997- 
Wolters. 

(1910)  N.Jahrb.Min.Geol.(Beil.Bd.), 

jo,  57- 


Wood,  J.  Kerfoot. 
8)  J.< 


(1908)  J.Chem.Soc.(Lond.),  93,  412. 
Wood,  J.  K.  and  Scott,  J.  D. 

(1910)  J.Chem.Soc.(Lond.),  97,  1573. 
Wood,  T.  B.  and  Jones,  H.  O. 

(1907-08)  Proc. Cambridge  Phil.Soc. 

14,  171-6. 
Worden,  E.  C. 

(1907)  J.Soc.Chem.Ind.,  26,  452. 
Worley,  F.  P. 

(1905)  J.Chem.Soc.(Lond.),  87,  1107. 
Woudstra,  H.  W. 

(1912)  8th  Int.Cong.Appl.Chem.,  12, 

251- 
Wright  and  Thomson. 

(1884-85)  Phil.Mag.  [5],  17,288;  19,  i. 
Wright,  Thomson  and  Leon. 

(i89i)Proc.Roy.Soc.(Lond.),49, 185. 
Wroczynski,  A.  and  Guye,  P.  A. 

(1910)  J.chim.phys.,  8,  197. 


Wroth,  B.  B.  and  Reid,  E.  E. 

(1916)  J.Am.Chem.Soc.,  38,  2322. 
Wrzesnewsky,  J.  B. 

(1912)  Z.anorg.Chem.,  74,  95. 
Wuite,  J.  P. 

(1913-14)  Z.physik.Chem.,  86,  349- 

82. 
Wiirfel. 

(1896)  Dissertation,  Marburg. 
Wiirgler,  J. 

(1914)  Dissertation,  Zurich. 
Wuth,  B. 

(1902)  Ber.,  35,  2415. 
van  Wyk,  see  Van  Wyk. 
Wyrouboff,  G. 

(1869)  Ann.chim.phys.,  [4],  16,  292. 

(1901)    Bull.soc.chim.,    [3],   25,    105, 

121. 
Yamamoto. 

(1908)  J.Coll.Sci.(Tokyo),  25,  XI. 
Young,  S.  W. 

(1897)  J.Am.Chem.Soc.,  19,  851. 
Young,  S.  W.  and  Burke,  W.  E. 

(1904)  J.Am.Chem.Soc.,  26,  1417. 

(1906)  J.Am.Chem.Soc.,  28,  321. 
Zaayer,  H.  G. 

(1886)  Rec.trav.chim.,  5,  316. 
Zaharia,  A. 

(1899)   Bul.soc.  de  sciinte  dia  Bu- 
curesci    (Roumania),    8, 

53-61- 
Zalai,  D. 

(1910)  Gy6gyszereszi  Ertesito  (Bu- 
dapest), 1 8,  366. 

(1910)  "  Tables  annuelles,"  i,  410. 
Zambonini,  F.  F. 

(1913)  Atti  accad.Lincei,    [5],  22,  I, 

523- 
Zawidzki,  V. 

(1904)  Z.physik.Chem.,  47,  721. 
Zemcznzny. 

(1908)  Z.anorg.Chem.,  57,  267. 
Zemcznzy  and  Rambach. 

(1910)  Z.anorg.Chem.,  65,  403. 
Zukow,  A.  and  Kasatkin,  F. 

J.Russ.Phys.Chenl.Soc.,    41, 
157-66. 


821 


SUBJECT  INDEX 


Acenaphthene,  I,  2,  16 

bromo,  2 

chloro,  2 

iodo,  2 
Acetaldehyde,  2 

phenyl  hydrazone,  2 

trithip,  732 
Acetamide,  2 

tribromo,  2 

trichloro,  2 
Acetanilide,  3,  4 

chloro  and  bromo,  4 

nitro,  4,  79 

oxymethyl,  13 
Acetanisidine,  13 
Acetic  acid,  5-8,  84,  89,  366,  500, 

chloro,  5,  9-11 

cyano,  n 

esters,  12 

Acetic  anhydride,  5 
Acetins,  mono,  di  and  tri,  13 
Acetnaphthalide,  13 
Acetone,  13-15,  50,  125,  197,  248, 
480,  511,525,534,648,695 

phenyl  hydrazone,  487 
Acetphenetidine,  477 
Acetophenol,  89 
Acetophenone,  9,  10,  16,  84 

amino,  730 
Acetotoluidine,  732 
Aceturethan,  742 
Acetyl  acetone,  16 
Acetyldiphenylamine,  283 
Acetylene,  16,  17,  438 

bi  iodide,  17 

Acetylsalicylic  acid,  101,  593 
Acetyl  tribromophenol,  486 
Aconitic  acid,  17 
Aconitine,  17 
Acrylic  acid,  trichloro,  1 8 
Actinium,  18 
Adipic  acid,  18 
Adipinic  acid,  18 
Adonitol,  dibenzal,  698 
Agaric  acid,  18 
Air,  19 
Alanine,  19,  20 

phenyl,  486 
Albumin,  20 

Alcohol  (Ethyl),  2,  12,  65,  66,  71 
125,  126,  160,  163,  235,  239, 
247,  248,  286-294,  296,  298- 
313,  404-5,  438-9, 466-7, 501, 
io,  530,  533,  571,  574,  628, 
671 


Alizarin,  20 
Allantoin,  20 
Allocinnamic  acids,  254 
Allyl  alcohol,  511,  534,  647 

isothiocyanic  ester,  443 

mustard  oil,  77 

thio  urea,  738 
Aloin,  20 
Alums,  30-32,  67,  180,  249,  582,  587, 

713 
Aluminium  bromide,  21-24 

chloride,  25-27 

fluoride,  27 

hydroxide,  28 

oxide,  28,  210 
626  rubidium  alum,  582 

sulfate,  29,  31 

sulfide,  29 

thallium  alum,  713 
Aminopropionic  acid,  19 
Aminosuccinic  acid,  692 
Ammonia,  33-38,  70,  436 
444,      Ammonium  acetate,  39 

acid  oxalate,  59 

acid  sulfate,  64 

antimony  sulfide,  69 

arsenates,  39 

alum,  30 

benzoate,  39 

bicarbonate,  41-43 

bismuth  citrate,  150 

borates,  40 

bromide,  40,  99,  504 

bromide,  propyl,  benzyl,  etc.,  41 

bromide,  tetraethyl,  41 

bromide,  tetramethyl,  41 

cadmium  bromide,  41,  167-8 

cadmium  chloride,  170-1 

cadmium  iodides,  177 

cadmium  sulfate,  67 

calcium  ferrocyanide,  51 

calcium  sulfate,  214 

carbonate,  13,  4^ 

cerium  sulfate,  241,  243 

cerium  nitrate,  241 

chloride,  43,  44-50,  60,  107,  109,  274, 


337-8,  353,  643,  7|i 
iloru 


chloride  carnellite,  48 
chloride,  ethyl  and  methyl,  50 

,  72,  chromates,  51 

245,  chromium  alum,  32 

300,  chromium  sulfate,  67 

509-          citrates,  51 

cobalt  chlorides,  256 
cobalt  malonate,  259 

822 


636, 


SUBJECT  INDEX 


Ammonium    acetate,    cobalt    sulfate, 

67 

copper  chloride,  265-6,  270 
copper  sulfate,  273,  557 
didymium  nitrate,  281 
fluoboride,  51 
fluosilicate,  62 
formate,  52 
glycyrrhizate,  307 
indium  sulfate,  67 
iodate,  52 
iodide,  52 

iodide  phenyl  trimethyl,  55 
iodide  tetra  amyl,  55 
iodide  tetra  ethyl,  53,  55 
iodide  tetra  methyl,  54,  55 
iodide  tetra  propyl,  54,  55 
iodomercurate,  55 
iridium  chlorides,  55,  335 
iron  alum,  67 
iron  chloride,  337 
iron  sulfate,  67 
lanthanum  nitrate,  347 
lanthanum  sulfate,  348 
lead  chloride,  353 
lead  cobalticyanide,  43 
lead  sulfate,  67 
lithium  sulfate,  68 
lithium  tartrate,  69 
magnesium  arsenate,  39 
magnesium  ferrocyanide,  389 
magnesium  nitrate,  59 
magnesium  phosphate,  61 
magnesium  sulfate,  68 
manganese  molybdate,  59 
manganese  phosphate,  62 
manganese  sulfate,  68,  404 
mercuric  bromide,  406 
molybdate,  tetra,  55 
nickel  sulfate,  68,  273 
nitrate,  45,  55-60 
oleate,  59 

oxalate,  59,  376,  735 
palmitate,  60 
perchlorate,  43,  44 
perchlorate  derivatives,  44 
periodate,  52 
permanganate,  62 
persulfate,  69 
phosphates,  60,  61,  62 
phosphites,  62 
phosphomolybdate,  55 
picrate,  62 

platinum  bromide,  41 
platinum  chloride,  498 
platinous  nitrite  compounds,  499 
ruthenium  nitrosochloride,  587 
salicylate,  62 
selenate,  62 
silico  fluoride,  62 
sodium  phosphates,  62 
sodium  sulfate,  68 
sodium  sulfite,  69 


Ammonium  acetate,  sulfate,  45,  56,  60, 
63-69,  274,  404,  556,  594 

sulfoantmionate,  69 

sulfonates,  69 

stearate,  63 

strontium  sulfate,  68 

tartrate,  69 

tetroxolate,  59 

thiocyanate,  35,  70 

thorium  oxalate,  60,  722 

thorium  sulfate,  724 

trinitrate,  57 

urate,  70 

uranyl  carbonate,  43,  733-4 

uranyl  nitrate,  735 

uranyl  oxalate,  735 

uranyl  propionate,  736 

vanadate,  meta,  70 

vanadium  sulfate,  69 

zinc  chloride,  751 

zinc  oxalate,  754 

zinc  phosphate,  754 

zinc  sulfate,  69,  273 
Amygdalin,  70 
Amyl  acetate,  12,  70,  71 

alcohol,  71,  72 

alcohol,  iso,  71,  72,  291 
Amylamine,  72 

hydrochloride  (iso),  72 
Amyl  ammonium  iodide,  tetra,  55 

ammonium  perchlorates,  44 

benzene,  84 

benzene  (iso),  90 

bromide  (iso),  292 

butyrate,  70 
Amylene,  72,  73 

hydrate,  73 
Amyl  ether,  (iso),  292 

formate,  70,  71 

malonic  acid,  399 

propionate,  70 
Andromedotoxine,  73 
Anethol,  13,  73 
Aniline,  21,  72-80,  88,  89,  443 

bromo,  21,  79 

dimethyl,  21,  123,  132 

ethyl,  79 

hydrochloride,  74,  78 

methyl,  21,  79,  292 

nitro,  4,  78,  79,  80 

nitro  methyl,  tetra,  79 

nitroso,  79 

nitroso  dimethyl,  77,  79 

propyl,  79 

sulfate,  80 
Anisaldehyde,  10 
Anisic  acid,  80 
Anisidine,  80 
Anisole,  80,  84,  89 

nitro,  80,  421 
Anthracene,  81,  82 
Anthraflavine,  83 


823 


SUBJECT   INDEX 


Anthraquinone,  82,  83 

hydroxy,  83 
Anthrarufine,  83 
Antimony,  83,  705,  712 

ammonium  sulfide,  69 

lithium  sulfide,  366,  373 

penta  chloride,  94 

penta  fluoride,  94 

potassium  sulfide,  500-1 

potassium  tartrate,  96 

selenides,  95 

sodium  sulfide,  627-8 

sulfide,  277,  365 

tri  bromide,  83-88 

tri  chloride,  88-94 

tri  fluoride,  95 

tri  iodide,  95 

tri  oxide,  95 

tri  phenyl,  95 

tri  sulfide,  95 
Antipyrine,  4,  96 

Apomorphine,  hydrochloride,  97,  442 
Arabinose,  696 
Arachidic  acid,  97 
Arbutin,  97 
Argon,  97 

Aribitol,  monobenzal,  698 
Arsenic,  98,  705,  712 

pentoxide,  100 

sulfide  (ous),  101 

tri  bromide,  98 

tri  chloride,  98 

tri  iodide,  95,  98 

tri  oxide,  39,  98-100,  629,  642 
Asparagine,  101 
Asparaginic  acid,  101 
Aspirin,  101,  593 
Astrakanit,  641,  668 
Atropine,  101,  102 

methyl  bromide,  102 
Auric,  Aurous,  (see  Gold) 
Azelaic  acid,  102 
Azoanisol,  103 

phenetol,  103 

Azobenzene,  16,  88,  102,  103,  123,  133, 
1 66 

amino,  103 

hydroxy,  103 

Azobenzoic  acid  ethyl  ester,  103 
Azolitmine,  104 
Azonaphthalene,  103 
Azophenetol,  103,  104 
Azotoluene,  103 
Azoxyanisol,  103 
Azoxybenzene,  103 
Azoxybenzoic  acid  ethyl  ester,  103 
Azoxy  phenetol,  103 

Barbituric  acid,  diethyl,  744 
Barium  acetate,  104 

amyl  sulfate,  121,  122 

arsenate,  104 

benzene  sulfonates,  122 


114 


Barium  acetate,  benzoate,  104 

borates,  105 

bromate,  105 

bromide,  99,  105,  106 

butyrate,  106 

cadmium  chloride,  171 

camphorates,  106 

cinnamates,  112 

citrates,  112 

caproate,  107 

carbonate,  107,  108,  in,  509,  557 

chlorate,  108 

chloride,  45,  99,  108-111,  643 

chromate,  in,  112 

cyanide,  112 

ferrocyanide,  112 

fluoride,  in,  112 

formate,  113 

glycerolphosphates,  119 

hydroxide,  105,  109,  113, 

iodate,  114 

iodide,  106,  in,  112,  114 

iodide  mercuric  cyanide,  423 

iodomercurate,  115 

iso  caproate,  107 

iso  succinate,  120 

laurate,  120 

malate,  115 

malonate,  115 

molybdate,  115 

myristate,  120 

nitrate,  45,  55,  109,  113,  115-7,  166, 
542 

nitrite,  117,  118 

oxalate,  118,  119 

oxide,  106,  in,  119 

phenanthrene  sulfonates,  122 

palmitate,  120 

perbromide,  106 

perchlorate,  108 

periodide,  115 

persulfate,  122 

picrate,  119 

potassium  ferrocyanide,  112 

propionate,  119 

salicylate,  119 

salicylate,  dinitro,  119 

silicate,  119 

stearate,  120 

succinate,  120 

sulfate,  in,  120,  121,  509,  557 

sulfite,  122 

sulfonates,  122 

tartrate,  122,  123 

truxilate,  123 
Behenic  acid,  123 

methyl  ester,  123 
Benzalaniline,  123 
Benzalazine,  123 
Benzaldehyde,  10,  84,  89,  123,  287 

trithio,  732 

hydroxy,  10 

nitro,  10,  123,  124 

824 


SUBJECT  INDEX 


Benzaldoxime,  124 

nitro,  124 

Benzalic  compounds  of  alcohols,  698 
Benzamide,  124 
Benzanilide,  124 

chloro,  124 
Benzaniline,  103 
Benzazonaphthalene,  103 
Benzene,  2,  5,  9,  10,  21,  77*  79,  83,  90, 
103,  124,  125-132,  135,  287,  482, 
576,  581,  702 

bromo,  14,  21,  90,  129,  288,  436,  572 

bromochloro,  etc.,  129 

bromo,  chloro,  iodo,  85 

bromo  nitro,  23,  24,  26 

chloro,  5,  90,  129,  130 

chloro,  bromo,  iodo  and  fluoro,  128 

chloronitro,  22,  23,  25,  77,  128 

disulfone  chlorides,  130 

dibromo,  21,  91 

dichloro,  91 

ethyl,  85,  90 

fluoro,  90 

fluoronitro,  85 

hexahydro,  280 

iodo,  90 

isoamyl,  90 

mixed  halogen  substituted,  129,  130 

nitro,  i,  4,  5,  21,  22,  25,  77,  79,  90,  91, 
103, 128, 131, 132,288,303,408,421 

nitro  chloro,  etc.,  129,  130 

nitroso,  77,  131 

propyl,  85,  91 

sulfonic  acid,  84,  89 

tri  nitro,  478 
Benzhydrol,  128,  132 
Benzil,  2,  9,  10,  88,  103,  124,  132,  136 
Benzine,  133 
Benzoic  acid,  5,  9,  10,  77,  84,  89,  128, 

I33-H5 

amino,  137,  138 

amino  nitro,  138 

bromo,  chloro  and  iodo,  139,  140 

chloro,  136,  139 

dinitro  oxy,  145 

fluoro,  136,  140 

halogen  substituted,  139 

iodo,  140 

isopropyl,  279 

methoxy,  80 

methyl,  141 

methyl  esters,  140 

nitro,  136,  141-5,  590 

nitro  chloro,  and  bromo,  145 
Benzoic  aldehyde,  nitro,  2 

anhydride,  145 
Benzoin,  103,  124,  133,  145 
Benzonitrile,  21,  84,  90 
Benzophenone,  10,  13,  22,  27,  84,  88, 
89,  103,  146,  166 

tetra  methyl  diamido,  440 
Benzoquinone,  10 
Benzosulfonazole,  587-8 


Benzosulfonic  acids,  amino,  136 
Benzoyl  chloride,  21,  27,  84,  89,  146 
Benzoyl  phenyl  carbinol,  145 

phenyl  hydrazine,  487 

tetra  hydroquinaldine,  146 
Benzyl  acetate,  288 

acetone,  di,  9 

alcohol,  288 

Benzylamine,  hydrochloride,  147 
Benzyl  amino  succinic  acid,  692 
Benzylaniline,  123,  145,  147 
Benzyl  carbamide,  226 

chloride,  80 

chloride,  nitro,  128,  147 

ethyl  ether,  288 
Benzylidene  aniline,  124,  145 

naphthylamines,  147 
Benzylidenes,  chloro  nitro,  147 
Benzyl  phenol,  147 
Beryllium  acetate,  147 

fluorides,  148 

hydroxide,  148 

laurate,  148 

meta  vanadate,  149 

myristate,  148 

oxalate,  148 

palmitate,  148 

phosphate,  148 

stearate,  148 

sulfate,  148,  149 
Betaine,  149 

salts,  149 
Betol,  149 
Bismuth,  150 

ammonium  citrate,  150 

chloride,  150 

citrate,  150 

double  nitrates,  151 

hydroxide,  151 

iodide,  151 

nitrate,  151 

oxide,  152 

oxychloride,  150 

salicylate,  152 

selenide,  152 

sulfide,  152 

telluride,  152 

triphenyl,  152 
Borax,    629-631    (see    Sodium    tetra.- 

borate) 
Boric  acid,  40,  153-57,  189,  367,  630 

tetra,  157 

Boric  anhydride,  157 
Borneol,  224 
Boron  trifluoride,  157 
Brassidic  acid,  158 
Brassidinic  acid,  123 
Bromal  hydrate,  158 
Bromethyl  propyl  aceturea,  742 
Bromine,  15,  150,  158-62 
Bromoform,  128,  162 
Brucine,  162 

perchlorate,  162 


825 


SUBJECT   INDEX 


Brucine,  sulfate,  163 

tartrate,  163 
Butter  fat,  302 

Butadiene,  diphenyl,  163,  254 
Butane,  163 
Butyl  acetate,  12,  163 

alcohol,  iso,  291 

alcohols,  164,  165 

ammonium  perchlorate,  44 

bromide,  iso,  292 

chloral,  165 

chloral  hydrate,  165 

formate,  163 

malonic  acid,  399 

sulfine  perchlorate,  698 
Butyric  acid,  102,  146,  165-6,  224 

trichloro,  166 
Butyric  aldehyde,  163 

Cacodylic  acid,  167 
Cadmium    ammonium     bromide, 
167-168 

ammonium  chloride,  170-1 

ammonium  iodides,  177 

barium  chloride,  171 

bromide,  167 

caesium  sulfate,  186 

chlorate,  169 

chloride,  in,  167,  169-174 

cinnamates,  174 

cyanide,  175 

fluoride,  170,  175 

hydroxide,  175 

iodide,  167,  170,  175,  176,  177 

magnesium  chloride,  171 

nitrate,  178 

oxalate,  60,  178  ^ 

potassium  bromide,  168 

potassium  chlorides,  173-4 

potassium  iodides,  178 

potassium  sulfate,  179 

rubidium  bromide,  168 

rubidium  chloride,  172 

rubidium  sulfate,  587 

silicate,  178 

sodium  bromide,  169 

sodium  chloride,  174 

sodium  iodide,  178 

sodium  sulfate,  180 

sulfate,  170,  178,  179 

sulfide,  1 80 
Caesium  alum,  32,  180 

bicarbonate,  181 

bromide,  181 

carbonate,  181 

chlorate,  181 

chloraurate,  181 

chloride,  182,  183 

chromates,  181,  183 

cobalt  malonate,  259 

dihydroxy  tartrate,  186 

double  sulfates,  186 

fluoboride,  181 


Caesium  alum,  fluoride,  27,  183 

gold  chloride,  181,  308 

hydroxide,  183 

iodate,  183 

iodides,  183-4 

iridium  chlorides,  182 

iron  chloride,  340 

lead  bromides,  181 

mercuric  bromide,  181 

mercuric  chlorides,  182 

nitrate,  184 

oxalate,  185 

perchlorate,  181 

periodate,  183 

permanganate,  185 

platinum  chloride,  182,  498 

selenate,  185 

sulfate,  185 

tartrate,  dihydroxy,  186 

telluracid  oxalate,  185 
41,  tellurium  bromide,  712 

tellurium  chloride,  182,  712 

thallium  chloride,  182 

uranyl  chloride,  734 

uranyl  nitrate,  735 
Caffeine,  186-187 
Calcite,  192,  193 
Calcium  acetate,  187-8  ^ 

ammomium  ferrocyanide,  51 

ammonium  sulfate,  67,  214 

benzoate,  188 

bitartrate,  222 

borates,  188-9 

bromide,  99,  189 

bromide  mercuric  cyanide,  423 

butylacetate,  1 88 

butyrates,  190 

camphorates,  190 

caproate,  190 

caprylate,  190 

carbonate,  191-5,  218 

chlorate,  196 

chloride,  99,  ill,  119,  121,  170,  189, 
195-202,  641 

chloride  acetamidate,  198 

chloride  acetic  acidate,  198 

chloride  alcoholates,  199 

chromates,  199 

cinnamates,  200 

citrate,  200 

ethyl  acetate,  188 

fluoride,  167,  189,  198,  2OI 

formate,  201 

glycerophosphate,  2OI 

heptoate,  201 

hydroxide,  200-5,  215 

iodate,  206 

iodide,  198,  201,  206 

iodo  mercurate,  206 

lactate,  206 

magnesium  chloride,  196 

malates,  206-207 

malonate,  207 

826 


SUBJECT   INDEX 


Calcium  acetate,  methyl  acetate,  188 

methyl  pentanate,  190 

nitrate,  203,  207-9,  222 

nitrite,  209 

oenanthate,  201 

oleate,  209 

oxalate,  209-10 

oxide,  157,  189,  198,  210 

pelargonate,  212 

perbromide,  189 

periodide,  206 

phenanthrene  sulfonates,  220 

phosphates,  210,  211,  212 

potassium  ferrocyanide,  200 

potassium  sulfate,  218 

propionate,  212 

propyl  acetate,  188 

rubidium  sulfate,  218 

salicylate,  213 

selenate,  213 

silicate,  119,  198,  201,  213 

sodium  thiosulfate,  222 

succinates,  213 

sulfate,  195,  198,  203,  212,  214-20 

sulfate  anhydrite,  214 

sulfide,  213,  220 

sulfite,  220 

tartrate,.22i-2 

thiosulfate,  208,  222 

titanate,  213 

valerates,  223 
Calomel,     413     (see    also     Mercurous 

chloride) 

Camphene,  10,  128,  223 
Camphor,  8,  9,  136,  166,  223-5,  593 

benzoyl,  224 

bromo,  225,  593 

chloro,  225 

Camphoric  acid,  190,  225,  368,  383,  508, 
633,  678 

anhydride,  225 
Camphoroxime,  225 
Cane  sugar  (see  Sugar) 
Cantharidine,  226 
Caoutchouc,  226 

Capryl  alcohol,  239,  278,  481,  745 
Carbamides,  226 
Carbazol,  128,  227 
Carbinol  (see  Methyl  alcohol) 
Carbon  dioxide,  227-234,  438 

disulfide,  5,  128,  235 

monoxide,  235-238 

oxysulfide,  238 

tetrachloride,  125,  239,  288,  435,  572 
Carmine,  239 
Carnallite,  388,  641 
Carnellite,  ammonium  chloride,  48 

potassium  chloride,  48 
Carvacrol,  239 
Carvoxime,  240 
Cascarilla  oil,  468 
Casein,  2JO 
Catechol,  240  « 


Cellose,  696 
Cephaeline  salts,  240 
Cerium  acetate,  241 

ammonium  nitrate,  241 

ammonium  sulfate,  241 

butyrates,  241 

chloride  (ous),  242 

citrate,  242 

cobalticyanide,  242 

dimethyl  phosphate,  242 

double  nitrates,  242 

double  sulfates,  243 

fluoride,  242 

formate,  241 

glycolate,  242 

iodate,  242 

malonate,  242 

oxalate,  242 

propionate,  241 

selenate,  243 

sulfate,  243-4 

sulfonates,  244 

tartrate,  244 

tungstate,  244 
Cesium,  (see  Caesium) 
Cetyl  alcohol,  9,  244,  574 
Chloral  formamide,  245 

hydrate,  96,  244-5  , 
Chlorine,  15,  150,  160,  239,  245-7 

dioxide,  247 

monoxide,  247 

trioxide,  247 

Chloro  acetic  acid  esters,  12 
Chloroform,  14,  15,  77,  126,  131,  247 

248,  289,  435,  571 
Cholesterol,  248-9 

acetate,  248 

digitonide,  248 

stearic  acid  ester,  249 
Cholesteryl  benzoate,  103 

isobutyrate,  103 

propionate,  103 
Choline  perchlorate,  249 
Chromic  acid,  51,  250,  372,  584,  651 
Chromium  alums,  249 

ammonium  alum,  32 

ammonium  sulfate,  67 

caesium  alum,  180 

chlorides,  249,  250 

double  salts,  250 

nitrates,  250 

sulfates,  250 

thiocyanate,  250 

potassium  cyanide,  531 

potassium  thiocyanate,  531 

rubidium  alum,  582 

thallium  alum,  713 

trioxide,  183,  250 
Chrysarobin,  250 
Chrysene,  250 
Cineole,  251 
Cinchona  alkaloids,  251 


827 


SUBJECT   INDEX 


Cinchonidine,  251 

salts,  252 
Cinchonine,  251 

salts,  252 

Cinchotine  salts,  252 
Cinnamic  acid,  9,  10,  136,  252-254 
bromo,  253,  254 
chloro,  254 
methoxy,  254 
Cinnamic  aldehydes,  chloro  and  bromo, 

254 
Cinnamylidene,  123,  147,  163,  254 

acetophenone,  16 
Citric  acid,  51,  254-55 
Cobalt  acetate,  256 
amines,  255 

ammonium  chlorides,  256 
ammonium  sulfate,  67  - 
bismuth  nitrate,  151 
bromide,  256 
caesium  sulfate,  iS6 
cerium  nitrate,  242 
chlorate,  256 
chloride,  45,  256-8 
citrates,  258 
double  salts,  255 
fluoride,  258 
gadolinium  nitrate,  304 
iodate,  258 
iodide,  258 

lanthanum  cyanide,  346 
lanthanum  nitrate,  347 
lead  cyanide,  357 
malate,  259 
malonates,  259 
neodymium  cyanide,  449 
neodymium  nitrate,  449 
nitrate,  259 
oxalate,  259 
perchlorate,  256 
potassium  citrate,  258 
potassium  sulfate,  557 
praseodymium  nitrate,  568 
rubidium  nitrite,  259 
rubidium  sulfate,  587 
samarium  nitrate,  594 
sulfate,  259-60 
sulfide,  260 
thallium  cyanide,  717 
ytterbium  cyanide,  746 
.  yttrium  cyanide,  746 
Cocaine,  261 
•     hydrochloride,  261 

perchlorate,  261 
Cocaline,  302 
Codeine,  261 
phosphate,  261 
sulfate,  261 
Colchicine,  262 

salts,  262 
Collidine,  262 
Congo  red,  262 
Coniine,  262 


Copiapite,  344 
Copper  acetate,  262-3 

ammonium  chloride,  265-6,  270 

ammonium  sulfate,  273,  557 

bromide,  167,  263 

caesium  sulfate,  186 

carbonate,  263-4 

chlorate,  264 

chloride,     109,    in,     150,    264-270, 
274 

chloride  (ous),  170,  183,  198 

cyanide,  270,  531 

hydroxide,  270 

iodate,  271 

iodide,  177,  271 

manganese  sulfate,  403 

nitrate,  271,  360 

oxalate,  272 

oxide,  270,  272 

potassium  carbonate,  264 

potassium  chloride,  267-8,  270 

potassium  sulfate,  274,  557 

rubidium  sulfate,  587 

sodium  sulfate,  276 
-    sulfate,  63,  272-7,  403,  454 

sulfide,  95,  277 

sulfonates,  277 

thallium  sulfate,  720 

tartrate,  277 

thiocyanate,  278 
Cotton  seed  oil,  294,  436,  468 
Coumarin,  132,  278 
Cream  of  tartar,  564-566 
Cresol,  9,  10,  77,  128,  251,  278,  279 

trinitro,  279 
Crotonic  acid,  9,  10,  279 

chloro,  279 
Cryolite,  28 
Cumidine,  pseudo,  279 
Cuminic  acid,  279 
Cyanimide,  279 
Cyanogen,  280 

Cyclohexane,  5,  86,  91,  128,  280 
Cyclohexanol,  280 
Cyclohexanone,  280 
Cymene,  85,  91 

pseudo,  86 

Cryptopines,  methyl,  279 
Cytisine,  280 

Detonal,  742 

Dextrin,  281 

Diacetyl  morphine,  442 

Diacetyl  racemic  ether,  281 

tartaric  ether,  281 
Diamine  mercuric  chloride,  419 
Dibenzyl,  103,  123,  133,  145,  147,  281 

acetone,  9 

hydrazine,  147 
Dibnal,  742 
Dicyandiamidine,  279 
Didymium  ammonium  nitrate,  281 

potassium  sulfate,  281 


828 


SUBJECT  INDEX 


Didymium  sulfate,  281 

sulfonates,  281 

Diethylamine  (see  Ethyl  amine),  281 
Diethylbarbituric  acid,  742,  744 
Diethyldiacetyl  tartrate,  131 
Diethylene  ether,  302 
Diethylketone,  289 
Diethyl  oxalate,  10 
Dihydro  naphthoic  acids,  447 
Dimethoxystilbene,  103 
Dimethyl  amine  (see  Methyl  amine) ,  437 

malonate,  10 

oxalate,  9,  10 

pyrone,  5,  9,  10,  21,  132,  136,  143, 
1 66,  253,  279,  304,  346,  400,  448, 
484,  486,  495,  575 

succinate,  5,  9,  10 

terephthalate,  10 

urea,  484 

xanthine,  721 
Dionin,  281,  442 
Diphenyl,  86,  91,  128,  282 

acetylene,  123,  254 

amine,  130,  132,  282-3 

amine  blue,  283 

amine,  hexanitro,  283 

butadiene,  123 

imide,  227 

hydrazine,  123 

methylamine,  283 

oxide,  282 

selenide,  283 

sulfide,  283 

telluride,  283 

urea,  738 
Dipyridyl  77,  132 
Dipronal,  742 
Dipropylazophenetol,  103 
Double  mercuric  chlorides,  420 
Dulcitol,  dibenzal,  698 
Dyes,  283 
Dysprosium  oxalate,  283 

Edestin,  283 

Egg  albumin,  20 

Elaterin,  284 

Emetine  and  salts,  284 

Epronal,  742 

Erbium  dimethyl  phosphate,  284 

oxalate,  284 

sulfate,  284 

sulfonate,  284 
Erusic  acid,  123,  158,  284 
Erythritol,  284,  698 

dibenzyl,  698 
Eserine,  492 
Ethane,  285 
Ethane,  diphenyl,  88 
Ether,  ethyl,  5,  10,  15,  16,  83,  128,  131, 
247,  248,  282,  289-290,  295,  297-9, 
313,  323,  425,  541 

petroleum,  477 


Ethyl  acetate,    10,    12,   77,    160,   247, 

285-6,  290,  313 
Ethyl  alcohol  (see  Alcohol) 

amine,  di,  128 

amine  hydrochloride,  296 

amine,  tri,  102,  in,  133,  224,  405 

amines,  294-6 

ammonium  bromide,  tetra,  41 

ammonium  chloride,  tetra,  50 

ammonium  iodide,  tetra,  53,  55 

ammonium  perchlorates,  44 

benzene,  90 

benzoate,  10 

bromide,  160,  290,  296,  436,  572 

butyrate,  290,  296 

carbamate,  296,  741-2 

chloracetate,  12 

diacetyl  tartrate,  di,  300 

dichlor  acetate,  12 
Ethylene,  301 

bromides,  5,  22,  79,  103,  128,  131, 
280,  281,  283,  300,  301,  431 

chlorides,  128,  291,  296 

cyanide,  302,  693 

tetraphenyl,  302 
Ethyl  ether  (see  ether) 

formate,  299 

Ethylidene  chloride,  291,  296 
Ethyl  iodide,  296 

ketone,  di,  300 

malonic  acid,  399 

methyl  ketone,  299,  534,  649 

morphine,  281,  442 

morphine  hydrochloride,  443 

piperidine,  496 

propionate,  290,  300 

succinimide,  693 

sulfine  perchlorate,  698 

sulfonium  iodide,  tri,  699 

sulfon  methanes,  435 

trichlor  acetate,  12 
Ethyl  urethan,  742 

valerates,  300 
Eucaine  and  salts,  302 
Eucalyptole,  251 
Europium  sulfonate,  302    ' 

Fats,  302 
Fatty  acids,  468 
Ferric  (see  Iron) 
Ferrous  (see  Iron) 
Fluorene,  132,  145,  303 
Fluorenone,  132 
Fluorescein,  303 
Formaldehyde,  303 
Formamide,  5,  166,  303 
Formanilides,  chloro,  303 
Formic  acid,  5,  126,  130,  303,  304 
Fruit  sugar,  695-7 
Fumaric  acid,  304 
Furfuralazine,  123 
Furfurol,  304 


829 


SUBJECT  INDEX 


Gadolinium  cobalticyanide,  304 

dimethyl  phosphate,  305 

double  nitrates,  304 

glycolate,  304 

oxalate,  304-5 

sodium  sulfate,  305 

sulfate,  305 

sulfonates,  305 
Galactose,  305,  695-7 
Gallic  acid,  305-6 
Germanium  dioxide,  306 

potassium  fluoride,  535 

sulfide,  306 
Glass,  306 
Glaserite,  559,  641 
Globulin,  306 
Glucoheptose,  696 
Glucose,  306,  695-97 
Glutaminic  acid,  306 

hydrochloride,  307 
Glutaric  acid,  307 
Glycerol,  75,  125 
Glycine,  in,  307 
Glycocoll,  307 

trimethyl,  149 
Gly colic  acid,  307 

phenyl,  307 
Glycyrrhizic  acid,  307 
Gold,  308,  705,  712 

caesium  chloride,  181 

chloride,  308 

double  chlorides,  308 

lithium  chloride,  369 

phosphorus  trichloride,  308 
Grape  sugar,  695-97 
Guaiacol,  251,  309 

carbonate,  309 
Guanidine,  triphenyl,  2,  309 
Gulose,  697 
Gun  cotton,  465 

Helianthin,  309 

Helium,  309-310 

Hemoglobin,  309 

Heptane,  239,  278,  291,  310,  436,  481 

Heptpic  acid,  ^3 10 

Heroine,  442 

Hexahydrobenzene,  280 

Hexamethylene,  280 

tetramine,  310 

Hexane,  78,  131,  291,  310,  436 
Hexanitrodiphenylamine,  283 
Hippuric  acid,  310-11 
Holocaine  hydrochloride,  311 
Homatropine  hydrobromide,  311 
Hydrastine,  311 

Hydrastinine  hydrochloride,  311 
Hydrazides,  312 
Hydrazine,  312 

dibenzyl,  147 

nitrate,  312 

perchlorate,  312 

sulfate,  312 


Hydrazobenzene,  103,  123,  145,  147 
Hydriodic  acid,  312 
Hydrobenzene,  103,  147 

tetra,  87 

Hydrobenzoic  acids,  hexa,  140 
Hydrobenzoin,  133 
Hydrobromic  acid,  15,  160,  248,  313 
Hydrochloric  acid,  247,  248,  298,  313-5, 

517,  649 

Hydrocinnamic  acid,  253,  570 
Hydrocyanic  acid,  315 
Hydrofluoric  acid,  315 
Hydrogen,  316-21 

peroxide,  321-2 

selenide,  322 

sulfide,  37,  313,  315,  322-3 
Hydroquinol,  15,  77,  103,  224,  251,  254, 

323-4 

chloro  and  bromo,  324 

diacetyl  chloro  and  bromo,  324 
Hydroquinone  (see  Hydroquinol) 
Hydroxy  benzaldehyde,  123 

benzoic  acids,  140,  141 

benzoic  acid,  dinitro,  145 
Hydroxylamine,  324 

hydrochloride,  324 
Hyoscine  hydrobromide,  325 
Hyoscyamine,  324 
Hypophosphoric  acid,  490 

Iditol,  tribenzal,  698 

Indan  carboxylic  acid,  nitro,  325 

Indigo,  325 

Indium  ammonium  sulfate,  67 

caesium  alum,  180 

iodate,  325 
Inositol,  iso,  325 
lodic  acid,  325,  536,  654 
Iodine,  55,  95,  98,  150,  160,  184,  206, 

247,  271,  325-34,  429,  537,  713 
lodoeosine,  335 
lodoform,  335 
lodol,  335 
Iridium  ammonium  chlorides,  55,  335 

caesium  chlorides,  182 

chloride,  335 

double  salts,  335 

potassium  chloride,  526 

rubidium  chlorides,  585 
Iron  ammonium  sulfate  (alum),  67 

bicarbonate,  336 

bromide  (ous),  335 

caesium  alum,  180 

caesium  chloride,  340 

caesium  sulfate,  186 

carbonate  (ous),  336 

chloride,  150,  267,  270,  336-40 

fluoride,  652 

formate  340 

hydroxide,  341,  342 

nitrate,  341 

oleate,  342 

oxalate,  342 


830 


SUBJECT   INDEX 


Iron  ammonium  sulfate  (alum),  oxide, 
210,  342 

phosphates,  342 

potassium  chloride,  339-40 

potassium  sulfate,  345,  558 

rubidium  alum,  582 

rubidium  sulfate,  587 

sodium  sulfate,  344 

sulfate,  29,  64,  179,  343-45 

sulfide,  277,  342,  345 

sulfonates,  345 

thallium  alum,  713 

thallium  cyanide,  717 

thiocyanate,  345 
Isoamyl  alcohol,  574 

urethan,  742 
Isobehenic  acid,  123 
Isobutyl  acetate,  formate,  etc.,  163 

alcohols,  164-5,  574 
Isobutylamine  hydrochloride,  165 
Isobutyric  acid,  165-6 
Isoerusic  acid,  123 
Isopentane,  77,  476 
Isophthalic  acid,  490 
Isopropyl  aicohol,  511,  533,  571 

amine,  573 

bromide,  573 

chloride,  573 

iodide,  573 
Itaconic  acid,  345 

Kainite,  641 
Keratin,  345 
Kieserite,  641 
Krypton,  345 

Lactdiethylamide,  744 
Lactic  acid,  125,  346 

trichloro,  346 
Lactose,  695-97 
Lanthanum  ammonium  nitrate,  347 

bromate,  346 

citrate,  346 

cobalticyanide,  346 

dimethyl  phosphate,  348 

double  nitrates,  347 

double  sulfates,  348 

glycolate,  346 

iodate,  346 

malonate,  346 

molybdate,  347 

oxalate,  347 

sulfate,  348 

sulfonates,  348 

tartrate,  349 

tungstate,  349 
Laurie  acid,  349 
Lead,  349,  705,  712 

acetate,  349-350  ^ 

ammonium  chloride,  353 

ammonium  cobalticyanide,  43 

ammonium  sulfate,  67 

arsenate,  350 


Lead,  benzoate,  351 

borate,  351 

bromate,  351 

bromide,  150,  351-2 

caesium  bromides,  181 

caprate,  352 

caproate,  352 

caprylate,  352 

carbonate,  352-3 

chlorate,  353 

chloride,  46,  III,  150,  170,  198,  270, 
339,  351,  353-56 

chromate,  353,  357 

citrate,  357 

diphenyl  dicyclohexyl,  352 

double  cyanides,  357 

ferricyanide,  357 

fluoride,  351,  356,  357 

fluoro  chloride,  356 

formate,  358 

heptylate,  352 

hexyl  bromide,  352 

hexyl  chloride,  352 

hydroxide,  358 

hyposulfate,  365 

iodate,  358 

iodide,  351,  356,  357,  358,  359 

laurate,  352,  360 

malate,  359 

myristate,  352 

nitrate,  116,  360-2 
Lead  nonylate,  352 

oxalate,  362 

oxides,  351,  356,  357,  362 

palmitate,  352,  360,  362 

peroxide,  362 

persulfate,  365 

phosphate,  357,  362 

potassium  chloride,  355 

potassium  ferricyanide,  357 

potassium  iodide,  359 

potassium  sulfate,  364,  558 

stearate,  352,  360,  362 

succinate,  363 

sulfate,  357,  362-65 

sulfide,  95,  277,  345,  356,  365 

sulfonates,  365 

tartrate,  366 

tetraphenyl,  352,  362 

tetracyclohexyl,  352 
Lecithin,  366 
Leonite,  641 
Leucine,  366 
Lignoceric  acid,  97,  366 
Ligroin,  366 

Lime  (see  Calcium  hydroxide) 
Linseed  oil,  468 
Lithium,  37,  366 

acetate,  366 

ammonium  sulfate,  68 

ammonium  tartrate,  69 

antimony  sulfide,  366,  373 

benzoate,  367 

831 


SUBJECT  INDEX 


Lithium,  bicarbonate,  369 

bichromate,  372 

borate,  367 

bromate,  367 

bromide,  100,  367 

camphorate,  368 

carbonate,  368-9 

chlorate,  369 

chloraurate,  369 

chloride,  100,  in,  183,  198,  270,  356, 
370-1 

chromate,  372 

citrate,  372 

fluoride,  27,  373 

formate,  373 

gold  chloride,  308,  369 

hippurate,  373 

hydroxide,  367,  371-3 

hypophosphate,  377 

iodate,  374 

iodide,  373,  374 

lodo  mercurate,  374 

laurate,  374,  375 

mercuric  iodide,  374 

molybdate,  375 

myristate,  374,  375 

nitrate,  117,  376 

nitrite,  376 

oleate,  374 

oxalate,  60,  376 

oxide,  378 

palmitate,  374,  375 

permanganate,  377 

phosphate,  377 

potassium  sulfate,  377 

salicylate,  377 

silicate,  119,  213,  367,  378 

sodium  sulfate,  377 

stearate,  374,  375 

sulfate,  29,  64,  121,  179,  220,  259, 
274,  343,  365,  369,  376,  377,  378 

sulfoantimonate,  366,  373 

tartrates,  378 
Lutidine,  574 
Lyxose,  696 

Magnesium,  378 
acetate,  378 

ammonium  arsenate,  39 
ammonium  ferrocyanide,  389 
ammonium  nitrate,  59 
ammonium  phosphate,  61 
ammonium  sulfate,  68 
benzoate,  379 
bicarbonate,  385-86 
bismuth  nitrate,  151 
bromate,  379 
bromide,  379 

bromide  alcoholates,  379,  381 
bromide  anilinates,  379,  381 
bromide  compounds,  379,  382-3 
bromide  etherate,  379-80 


Magnesium,    bromide    phenylhydrazi- 
nates,  379,  382 

cadmium  chloride,  171 

caesium  sulfate,  186 

calcium  chloride,  196 

camphorate,  383 

carbonate,  13,  384-86 

cerium  nitrate,  242 

chlorate,  387 

chloride,  46,  in,  170,  196,  198,  339, 
356,  371,  387-8,  641 

cinnamate,  389 

chromate,  389 

ferrocyanides,  389 

fluoride,  389 

fluosilicate,  396 

gadolinium  nitrate,  304 

hydroxide,  385,  389,  390 

hypophosphate,  395 

iodate,  390 

iodide,  390 

iodide  alcoholates,  391,  392 

iodide  anilinates,  391,  392 

iodide  compounds,  391,  393,  394 
Magnesium  iodide  etherates,  391,  392 

iodo  mercurate,  394 

lanthanum  nitrate,  347 

laurate,  394 

mercuric  iodide,  394 

myristate,  394 

neodymium  nitrate,  449 

nitrate,  395 

oleate,  395 

oxalate,  60,  395 

oxide,  28,  210,  378,  395 

palmitate,  394 

phosphate,  395 

platinic  cyanide,  389 

potassium  ferrocyanide,  389 

potassium  chloride,  388 

potassium  chromate,  389 

potassium  sulfate,  396,  397 

praseodymium  nitrate,  568 

rubidium  sulfate,  587 

salicylate,  395 

samarium  nitrate,  594 

silicate,  213,  378,  396 

sodium  sulfate,  668 

stearate,  394 

succinate,  396 

sulfate,  273,  388,  396-7,  480,  641,  668 

sulfite,  397 

sulfonates,  397 
Maleic  acid,  304,  398 
Malaminic  acid,  398 
Malonic  acid,  299,  398-9 
Malonic  acids,  substituted,  399 
Maltose,  695-7 
Mandelic  acid,  398-400 
butyl  esters,  400 
methyl  esters,  400 

Manganese  ammonium  molybdate,  59 
ammonium  phosphate,  62 


832 


SUBJECT   INDEX 


Manganese  ammonium  molybdate,  am- 
monium sulfate,  68,  404 

bismuth  nitrate,  151 

borate,  400 

bromide,  400 

caesium  sulfate,  1 86 

carbonate,  401 

cerium  nitrate,  242 

chloride,  47,  in,  170,  198,  356,  371, 
388,  401 

cinnamate,  401 

copper  sulfate,  403 

fluosilicate,  401 

hydroxide,  401-2 

hypophosphite,  402 

iodomercurate,  402 

lanthanum  nitrate,  347 

mercuric  iodide,  402 

neodymium  nitrate,  449 

nitrate,  402 

oxalate,  402 

oxide,  402 

potassium  chloride,  401 

potassium  vanadate,  405 

praseodymium  nitrate,  568  . 

rubidium  sulfate,  587 

samarium  nitrate,  594 

silicate,  119,  213,  396,  402 

sodium  sulfate,  404 

sulfate,  274-5,  378,  403-5 

sulfide,  405 

titanate,  402 
Mannitol,  166,  405,  698 

tribenzal,  698 
Mannose,  695-7 
Matico  oil,  468 
Mellibose,  696 

Mellitic  acid,  hexamethyl,  431 
Menthane,  431 

Menthol,  128,  131,  224,  245,  431 
Menthyl  mandelates,  400 
Mercury,  378,  598 

acetate,  406 

ammonium  iodide,  55 

barium  iodide,  115 

benzoate,  406 

bromide,  131,  158,  351,  406-8 

caesium  bromide,  181 

caesium  chlorides,  182 

calcium  iodide,  206 

chloride,    47,    80,     no,     182,    268, 
409-21,  526 

cinnamate,  422 

cyanide,  422-4 

diphenyl,  95,  152,  430 

double  cyanides,  423 

fulminate,  424 

iodide,  170,  177,  408,  421,  424-9,  616 

iodide  diamine,  429 

lithium  iodide,  374 

magnesium  iodide,  394 

manganese  iodide,  402 

nitrate,  429 


Mercury,  oxide,  429-30 

potassium  chloride,  410,  420 

potassium  iodide,  425,  541 

rubidium  chloride,  412 

selenite,  430 

sodium  chloride,  411 

sodium  iodide,  656 

strontium  iodide,  682 

sulfate,  430-1 

sulfide,  431 

zinc  thiocyanate,  752 
Mesitylene,  86,  92,  292 
Meta  arsenic  acid,  98 
Methacetin,  13 
Methane,  432-3 

diphenyl,  86,  92,  433 

triphenyl,  88,  282,  309,  433-4 
Methoxybenzoic  acid,  80 
Methoxycinnamic  acid,  103 
Methoxystilbene,  di,  677 
Methyl  acetate,  12,  247,  435 

alcohol,  5,  37,  72,  128,  160,  235,  247, 
248,  280,  286,  299,  313,  315,  323, 
435,  436,  501 ,  5i°.  574 

amines,  437,  438 

amine  chloroplatinates,  438 

amine  hydrochloride,  438 

ammonium  bromide,  tetra,  41 

ammonium  chloride,  tetra,  50 

ammonium  iodide,  tetra,  54,  55 

ammonium  perchlorates,  44 

aniline,  21,  292 

aniline,  di,  132 

anisate,  10 

benzoate,  10,  21 

benzoic  acids,  730 
Methylene  blue,  439 

bromide,  21,  439 
Methyl  butyrate,  438 

carbinol,  tri,  227 

chloride,  315,  439 

cinnamate,  9,  10 

cryptopines,  279 

ether,  37,  248,  301,  315,  438 

ethyl  ketone,  299,  534,  649 

hexyl  carbinol,  574 

iodide,  436,  439 

iso  thiocyanate,  443 

malonic  acid,  399 

mellitic  acid,  hexa,  431 

mustard  oil,  223 

orange,  309,  459 

oxalate,  439 

phenyl  carbamide,  226 

phenyl  picramides,  492 

picric  acid,  495 

piperidines,  496 

propionate,  439 

propyl  azo  phenol,  103 

pyridines,  574 

pyridines,  tri,  262 

pyridine  zinc  chloride,  574 

salicylate,  251,  439 


833 


SUBJECT   INDEX 


Methyl  butyrate,  succinic  acid,  711-2 

sulfate,  440 

sulfine  perchlorate,  698 

sulfone  methanes,  435 

toluate,  10 

urea,  484 

urethan,  431,  742 

valerate,  438 
Michler's  ketone,  440 
Milk  sugar,  695^-97 
Molybdenum  trioxide,  440 
Molybdic  acid,  440 
Morphine,  441 

acetate,  442 

hydrochloride,  442 

perchlorate,  442 

salts,  442 

sulfate,  442 

tartrate,  442 
Mustard  oil,  443 
Myristic  acid,  443 

Naphthalene,  5,  9,  13,  21,  79,  86,  92, 
98,  123,  128,  130-2,  166,  223-4, 
251,  279,  282-3,  300-1,  324,  431, 
433-4,  443-7 

bromo,  87,  92 

chloro,  87,  92 

dihydro,  446 

nitro,  86,  92,  224,  283,  408,  421,  446 

picrate,  126 

sulfonic  acid,  446 
Naphthoic  acid,  447 
Naphthoic  acids,  dihydro,  447 
Naphthols,  10,  128,  224,  251,  283,  301, 
446,  447,  448,  593,  703, 

Pirate  447 
Naphthyl  acetate,  10 

amine,  79,  224,  240,  283,  309,  446, 
448 

amine  sulfonic  acids,  448 

benzoate,  448 

hydrazones  of  sugars,  697 

salicylate,  149 
Narceine,  448 
Narcotine,  449 
Neodymium  chloride,  449 

cobalticyanide,  449 

dimethyl  phosphate,  450 

double  nitrates,  449 

glycolate,  449 

molybdate,  449 

nitrate,  450 

oxalate,  449-50 

sulfonates,  450 

tungstate,  450 
Neon,  450 

Neurine  perchlorate,  450 
Nickel  ammonium  sulfate,  68,  273 

bismuth  nitrate,  151 
Nickel  bromate,  451 

bromide,  451 

caesium  sulfate,  186 


Nickel  bromate,  carbonate,  451 

car  boxy  1,  451 

cerium  nitrate,  242 

chlorate,  451 

chloride,  47,  452 

citrate,  452 

gadolinium  nitrate,  304 

hydroxide,  452 

iodate,  452 

iodide,  453 

lanthanum  nitrate,  347 

malate,  453 

neodymium  nitrate,  449 

nitrate,  453 

oxalate,  453 

perchlorate,  451 

potassium  citrate,  452 

potassium  sulfate,  455,  557 

praseodymium  nitrate,  568 

rubidium  sulfate,  587 

samarium  nitrate,  594 

sodium  sulfate,  454 

sulfate,  453-5 

sulfide,  455 

thallium  sulfate,  720 
Nicotine,  456 
Nigella  oil,  468 

Niobium  potassium  fluoride,  456 
Nitric  acid,  224,  395,  456-7,  542 

oxide,  438,  461,  465 
Nitrocellulose,  465 
Nitrogen,  457-461 

oxide  (ic),  461 

oxide  (ous),  462-5 

tetroxide,  465 

Nitrophenyl  chloroform,  248 
Nitrosobenzene,  131 
Nitrosopiperidine,  496 
Nitrosyl  chloride,  247 
Nitrous  oxide,  462-5 
Novocaine,  466 

hydrochloride,  466 

Octane,  466 

Octyl  alcohol,  239,  278,  481,  745 
Oenanthyl  urethane,  742 
Oils,  302,  468 

baldo  leaves,  468 

castor,  oleic,  olive,  etc.,  249 

cotton  seed,  294,  436 

helianthus  annus,  468 

olive,  468 

turpentine,  440,  733 
Oleic  acid,  248,  466-7 
Olein,  tri,  467 
Orthovanillin,  744 
Osmic  acid,  468 
Oxalic  acid,  59,  185,  348,  376,  468-9 

549-51,  66 1 

Oxybenzoic  acids,  140,  141,  251 
Oxybenzoic  acid,  dinitro,  145 
Oxygen,  470-3 


834 


SUBJECT  INDEX 


Ozokerite  paraffin,  475 
Ozone,  473-4 

Palladium  chloride,  474 

Palmitic  acid,  97,  248,  443,  467,  474~5, 

677 

acetic  ester,  446 

acid  cetyl  ester,  475 
Palmitin,  tri,  467,  475 
Papaverine,  475 
Paraffin,  283,  446,  475 
Paraformaldehyde,  303 
Paraldehyde,  2,  128,  301 
Para  morphine,  721 
Pentane,  476 

iso,  77,  131,  282 
Peptone,  476 
Perchloric  acid,  476 
Perseitol,  dibenzal,  698 
Petroleum,  294 

benzine,  133 

ether,  477 
Phenacetin,  477 
Phenanthraquinone,  477-8 
Phenanthrene,  128,  132,  145,  223,  282, 
283,  443,  478-79 

picrate,  479 
Phenetidine,  acet,  477 
Phenetol,  86,  93,  292 

dinitro,  80 

Phenol,  9,  10,  15,  76,  78,  79,  83,  86,  93, 
102,  123,  124,  127,  131-3.  135,  H6, 
156,  224,  227,  251,  280,  283,  295, 
300,  301,  310,  315,  373,  397,  423, 
433,  445,  446,  448,  466,  479-84, 
536,  682,  704 

dinitro,  4,  303 
Phenols,  amino,  136,  251 

acetyl  tribromo,  486 

bromo,  484,  486 

chloro,  15,  77,  79,  283,  486 

iodo,  486 

nitro,  15,  77,  128,  251,  446,  484-6 

nitroso,  486 

tribromo,  132 

Phenolate  of  phenyl  ammonium,  484 
Phenolphthalein,  486 
Phenyl  acetic  acid,  9,  12 

alanine,  486 

amine,  di,  21,  80,  128,  282-3 

amine,  tri,  282 

anisyl  ketone,  10 

benzoate,  ip 

carbinol,  tri,  227 

diacetylene,  di,  163 

dibromo  propionic  acid,  570 
Phenylene  diamines,  486 
Phenyl  ether,  132 

ethylene,  tetra,  302 

glycolic  acid,  307 

glyoxal  phenyl  hydrazone,  307 

guanidine,  tri,  2,  309 

hydracrylic  acid,  732 


Phenyl  hydrazines,  484,  486-7 

hydrazine,  di,  163 

hydrazones  of  sugars,  697 

methane,  di,  433 

methane,  tri,  282,  309,  433-4,  704 

methyl  amine  hydrochloride,  438 

methyl  carbamide,  226 

piperidines,  di,  497 

propiolic  acid,  570 

propionic  acid,  254,  570 

salicylate,  10,  251,  593 

selenide,  dibromo,  487 

selenium  bromide,  di,  596 

telluride,  dibromo,  487 

tellurium  bromide,  di,  596 

thiocarbamide,  738-9,  740 

thio  urea,  738-740 

trimethyl  ammonium  iodide,  55 
Phloroglucinol,  487 
Phosphomolybdic  acid,  488 
Phosphoric  acid,  224,  489-90 
Phosphorus,  488-9 

acid,  489 

sulfides,  489 

triiodide,  95,  98 
Phthalic  acids,  490 
Phthalic  acids,  nitro,  491 
Phthalic  anhydride,  491 
Phthalide,  2,  309 

carbpxylic  acid,  492 
Phthalimide,  492 
Phthalonic  acid,  492 
Phthalyl  hydroxylamine  324 

phenyl  hydrazides,  312,  487 
Physpstigmine,  492 

salicylate,  492 

sulfate,  492 
Phytosterol,  248 
Picramides,  methyl  phenyl,  492 
Picric  acid,  5,  81,  240,  279,  301,  303, 
309,  446-8,  484,  486,  492-5,  731 

methyl,  495 
Picrotoxine,  495 
Picoline,  574 
Pilocarpine,  496 

hydrochloride,  496 

nitrate,  496 
Pinacplin,  496 
Pimelic  acid,  495 
Pinene,  293 

hydrochloride,  496 
Pipecoline,  496 
Piperidine,  280,  496 

propyl,  262 

Piperidines,  di  phenyl.  497 
Piperidine  hydrochloride,  496 

methyl,  496 
Piperine,  496,  497 
Piperonal,  9,  10,  136 

nitro,  ID 

Piperonilic  aldehyde,  2 
Platinates,  chloro,  of  hydrocarbon  sul- 
fines,  499 


835 


SUBJECT   INDEX 


Platino  amines,  499 

Platinous     nitrite     ammonium     com- 
pounds, 499 
Platinum  alloys,  497 

ammonium  bromide,  41, 

bromide,  497 

caesium  chloride,  182 

chlorides,  499 

double  chlorides,  498 

magnesium  cyanide,  389 

potassium  bromide,  497 
Ponceau,  499 
Potasammonium,  500 
Potassium,  37,  500 

acetate,  500 

acid  sulfates,  560 

alum,  30,  31 

amyl  sulfate,  564 

antimony  sulfide,  500-1 

antimony  tartrate,  96 

arsenate,  501 

barium  ferrocyanide,  112 

benzoate,  502 

beryllium  fluoride,  148 

bicarbonate,  508-9 

bioxalate,  551 

bisulfate,  560,  563 

bitartrate,  564-6 

bitartrate,  dimethyl  ester,  566 

borates,  502 

bromate,  503 

bromide,  100,  167,  263,  480,  504-7 

bromide,  mercuric  cyanide,  423 

butyrate,  508 

cadmium  bromide,  168 

cadmium  chlorides,  173-4 

cadmium  iodides,  178 

cadmium  sulfate,  179 

calcium  ferrocyanide,  200 

calcium  sulfate,  218 

camphorates,  508 

carbonate,  13,  35,  264,  353,  369, 
508-12,  544,  557 

carbonyl  ferrocyanide,  531 

cerium  sulfate,  243 

chlorate,  512-15,  714 

chloride,  45,  48,  109,  in,  121,  170, 
174,  183,  196,  198,  267,  270,  274, 
307,  339,  340,  356,  371,  388,  410, 
480,  504,  505,  507,  509,  512,  516- 
26,  531,  543,  552,  637,  641,  643, 
668,  672 

chloride,  carnellite,  48 

chloride  mercuric  cyanide,  423 

chloro  iridate,  526 

chloro  platinate,  498 

chromate,  353,  526-30,  559 
Potassium  chromium  alum,  249 

chromium  molybdate,  250 

chromithiocyanate,  531 

chromocyanide,  531 

citrate,  530 

cobalt  citrate,  258 


Potassium  chromium  alum,  cobalt  mal- 

onate,  259 
cobalt  sulfate,  557 
copper  carbonate,  264 
copper  chloride,  267-8,  270 
copper  sulfate,  274,  557 
cyanate,  531 
cyanide,  270,  531 
dichromate,  527-30 
didymium  sulfate,  281 
dihydroxy  tartrates,  566 
dipropyl  malonate,  512 
ethyl  sulfate,  563-4 
ferricyanide,  531-2 
ferrocyanide,  531-2 
ferrosulfate,  558 
fluoboride,  502 

fluoride,  27,  112,  242,  507,  526,  532-4 
fluotitanate,  568 
formate,  535 
germanium  fluoride,  535 
gold  chloride,  308 
hippurate,  311 
hydroxide,  501,  502,  507,  509,  526, 

529,  534-6,  555,  558 
hypophosphate,  555 
hypophosphite,  555 
iodate,  536 
iodide,  100,  177,  326,  425,  504,  505, 

507,    518,    519,    526,    534,    536, 


iodide 


lide  mercuric  cyanide,  423 

iodomercurate,  541 

iridium  chloride,  526 

iron  chloride,  339-40 

iron  sulfate,  345 

lanthanum  sulfate,  348 

lead  chloride,  355 

lead  cobalticyanide,  357 

lead  ferricyanide,  357 

lead  iodide,  359 

lead  sulfate,  364,  558 

lithium  sulfate,  377 

lithium  tartrate,  378 

magnesium  chloride,  388 

magnesium  chromate,  389 

magnesium  ferrocyanide,  389 

magnesium  sulfate,  396,  397 

manganese  chloride,  401 

manganese  sulfate,  405 

mercuric  cyanide,  423 

mercuric  chloride,  410-11,  420 

mercuric  iodide,  425,  541 

meta  borate,  502 

meta  phosphate,  502,  526,  534,  555 

methyl  sulfate,  564 

molybdate,  529,  530,  541 

nickel  citrate,  452 

nickel  sulfate,  455,  557 

niobium  fluoride,  456 

nitrate,  45,  55,  116,  117,  208,  360, 
376,  480,  506,  509,  519,  520,  521, 
541,  542-8,  552,  643,  657,  659,  718 


836 


SUBJECT   INDEX 


Potassium    chromium    alum,    nitrite, 

548-9 

oxalate,  60,  549-52,  735 

perborates,  502 

perchlorate,  515,  554 

periodate,  536 

permanganate,  552-4 

persulfate,  563 

phosphates,  526,  534,  554-5 

phosphomolybdate,  555 

picrate,  554,  719 

platinum  bromide,  497 

platinum  chloride,  498 

pyrpphosphate,  526,  534,  555 

rubidium  perchlorate,  583 

rubidium  nitrosochloride,  587 

selenate,  556 

silicate,  378,  556 

sodium  carbonate,  512 

sodium  sulfate,  668,  559 

sodium  sulfite,  564 

sodium  tartrate,  566 

sodium  thiosulfate,  568 

stannate,  556 

stannous  chloride,  522 

strontium  sulfate,  558 

succinate,  691 

sulfate,  31,  45,  64,  121,  149,  1 66,  179, 
220,  259,  274,  365,  378,  388,  397, 
405,  480,  509,  512,  522,  526,  529, 
530,  534,  541,  544,  552,  556-62, 
643,  668,  719 

sulfide,  564 

sulfoantimonate,  500-1 

sulfonates,  564 

tantalum  fluoride,  710 

tartrate,  564-566 

tellurate,  566 

telluric  acid  oxalate,  552 

tellurium  bromide,  712 

tetroxalate,  552 

thiocyanate,  70,  566-7 

thiosulfate,  568 

titanium  fluoride,  568 

thorium  sulfate,  724 

tungstate,  530,  541,  562 

uranyl  butyrate,  733 

uranyl  carbonate,  512 

uranyl  chloride,  734 

uranyl  nitrate,  735 

uranyl  oxalate,  735 

uranyl  propionate,  736 

uranyl  sulfate,  736 

vanadate,  568 

yttrium  oxalate,  747 

zinc  cyanide,  532 

zinc  sulfate,  557 

zinc  vanadate,  568 
Praseodymium  chloride,  568 

dimethyl  phosphate,  569 

double  nitrates,  568 

glycolate,  568 

molybdate,  568 


Praseodymium  chloride,  oxalate,  568 

sulfate,  569 

sulfonates,  569 

tungstate,  569 
Probnal,  742 
Propione,  300 
Propiolic  acid,  phenyl,  570 
Propionic  acid,  303,  315,  436,  569-70 

acid,  amino,  19 

acid,  iodo,  570 

acid,  phenyl,  570 

aldehyde,  570 
Propionitrile,  571 
Propyl  acetate,  12,  571 

alcohol,  5,  128,  511,  571-2,  574,  636, 
647 

alcohol,  iso,  533 

ammonium  iodine,  tetra,  54,  55 
.  ammonium  perchlorates,  44 

amine  hydrochloride,  573 

amines,  572-3 

anisole,  73 

benzene,  91 

bromide,  293,  573 

butyrate,  571 

chloride,  573 
Propylene,  573 
Propyl  formate,  571 

iodide,  573 

malonic  acid,  399 

piperidine,  262,  496 

propionate,  571 

sulfine  perchlorate,  698 
Pseudo  cumidine,  279 
Pyrene,  573 

Pyridinamino  succinic  acids,  575 
Pyridine,  21,  127,  136,  258,  279,  439, 

446,  484,  486,  574 
Pyridines,  methyl,  ethyl,  etc.,  574 

trimethyl,  262 
Pyrocatechol,    15,    77,    146,   224,   251, 

324,  446,  575 
Pyrogallol,  15,  224,  575 
Pyrone,    dimethyl    (see    Dimethylpy- 

rone 

Pyrophosphoric  acid,  490 
Pyrotartaric  acid,  307,  711-2 
Pyroxylin,  465 

Buinaldine,  benzoyl  tetrahydro,  146 
uinidine,  251,  575 
salts,  575 
sulfate,  576 

Quinine,  128,  251,  576,  577 
glycerophosphate,  578 
hydrochloride,  578 
pyrotartrates,  579 
salicylate,  578 
salts,  577-8 
sulfate,  578 
tannates,  579 

Buinhydrone,  575 
uinol,  132,  448 


837 


SUBJECT  INDEX 


Quinoline,  484,  486 
ethiodide,  579 

Radium  emanations,  579^80 
Rape  oil,  468 
Raffinose,  695-97 
Resorcinol,  15,  77,  131,  146,  224, 
283,    324,    446,    484,    495, 
580-1,  654 
Retene,  145 

Rhamnitol,  dibenzal,  698 
Rhamnose,  696 
Rhodium  salts,  581 

sodium  nitrite,  660 
Rosolic  acid,  582 
Rosaniline,  581 

hydrochloride,  582 
Rubidium  alum,  32,  582 

bicarbonate,  582 

bromide,  582 

bromiodide,  585 

cadmium  bromide,  168 

cadmium  chloride,  172 

caesium  nitrosochloride,  587 

calcium  sulfate,  218 

carbonate,  582 

chlorate,  583 

chloride,  183,  270,  356,  371,  412 

chromate,  584 

cobalt  nitrite,  259 

dichromate,  584 

dihydroxy  tartrate,  587 

double  sulfates,  587 

fluoboride,  582 

fluoride,  27,  584 

fluosilicate,  586 

hydroxide,  536,  584-5 

gold  chloride,  308 

iodate,  585 

iodide,  585 

iridate,  585 

mercuric  chloride,  412 

molybdate,  585 

nitrate,  586 

perchlorate,  583 

periodate,  585 

periodides,  585 

permanganate,  554,  586 

platinum  chloride,  498 

potassium  perchlorate,  583 

ruthenium  nitrosochloride,  587 

selenate,  586 

silicotungstate,  586 

sulfate,  220,  587 

tellurate,  586 

telluric  acid  oxalate,  586 

tellurium  bromide,  712 

tellurium  chloride,  584,  712 

thallium  chloride,  583. 

thiocyanate,  567 

uranyl  chloride,  734 

uranyl  nitrate,  735 
Ruthenium  salts,  587 


251, 

575, 


Saccharin,  587-8 

Salicin,  588 

Salicylamide,  588 

Salicylates,  methyl  and  phenyl,  251 

Salicylic  acid,  15,,  136,  251,  480,  575, 

588-93 
aldehyde,  10 

Salol,  9,  96,  149,  224,  225,  245,  309,  431, 
448,  593 
chl 


Samarium  chloride,  594 

dimethyl  phosphate,  594 

double  nitrates,  594 

glycolate,  594 

oxalate,  594 

sodium  sulfate,  594 

sulfate,  594 

sulfonates,  595 
Santonin,  593 
Scandium  oxalate,  595 

sulfate,  595 
Schonite,  641 

Scopolamine  hydrobromide,  325 
Sebacic  acid,  595 
Selenic  acid,  596 
Selenious  acid,  597 

anhydride,  597 

Selenium,  334,  408,  421,  596,  720 
583          bromide,  diphenyl,  596 

dioxide,  597 

Silica,  210,  362,  378,  395,  402,  556,  597 
Silicon,  598 

iodides,  598 

tetraphenyl,  302,  362,  598,  729 
Silicotungstic  acid,  598 
Silver,  598,  705,  712 

acetate,  598-9,  622 

acetyl  propionate,  617 

arsenate,  600 

arsenite,  600 

benzoate,  600 

borate,  600 

bromate,  60 1 

bromide,  351,  367,  507,  582,  601-4 

butyrate,  604 

caproates,  605 

carbonate,  605 

chloroacetate,  599-600 

chlorate,  605 

chloride,  183,  198,  270,  356,  371,  388, 
583,  604-12 

chromate,  612 

citrate,  613 

eyanide,  531,  613 

dichromate,  613 

ethyl  methyl  acetate,  600 

ferricyanide,  613 

fluoride,  613-4 

fulminate,  614 

heptoate,  614 

iodate,  614-5 

iodide,  271,  359,  374,  537,  604,  605, 
611,  615-6 

isobutyrate,  604 

838 


SUBJECT   INDEX 


Silver,  isovalerate,  624 

laurate,  617 

levulinate,  617 

malate,  617 

methyl  ethyl  acetate,  600 

myristate,  617 

nitrate,  57,  546,  548,  599,  617-9 

nitrite,  1 18, 209, 376,  549, 619-20,  660 

onanthylate,  614 

oxalate,  620 

oxide,  620-1 

palmitate,  617 

permanganate,  621 

phosphate,  621 

propionate,  621 

propyl  (di)  acetate,  600 

salicylate,  621 

selenides,  95,  152 

sodium  cyanide,  613 

stearate,  617 

succinate,  621 

sulfate,  219,  378,  562,  621-3 

sulfide,  29,  95,  101,  277,  365,  611,  624 

sulfonates,  624 

tartrate,  624 

thallium  cyanide,  613 

thiocyanate,  567,  605,  624 

valerates,  624-5 

vanadate,  625 
Sodammonium,  625 
Sodium,  37,  625 

acetate,  500,  626-7 

acid  phosphate,  663 

alum,  32 

ammonium  phosphates,  62 

ammonium  sulfate,  68 

ammonium  sulfite,  69 

antimony  sulfide,  627-8 

arsenates,  628-9 

benzoate,  187,  629 

beryllium  fluoride,  148 

biborate,  630-1 

bicarbonate,  43,  634,  637-8 

bisulfate,  670,  672 

borate,  367 

borate  (tetra),  629-31 

bromate,  631 

bromide,  99, 167,  604-5,  631-2,  634-5 

cacodylate,  633 

cadmium  bromide,  169 

cadmium  chloride,  174 

cadmium  iodide,  178 

cadmium  sulfate,  180 

caesium  sulfate,  186 

calcium  thiosulfate,  222 

camphorates,  633 

carbonate,  13,  218,  509,  512,  633-7, 
647,  655 

cerium  sulfate,  243 

chlorate,  639 

chloride,  45,  49,  109-11,  121,  166, 
170,  174,  183,  196-8,  267-8,  270, 
274,  339,  356,  371,  388,  411,  48o, 


507,    512,    517,    519,    521-2,    526, 

544-5,  548,  562,  583,  611,  632,  635, 

637,  639-49,  66 1,  669-71,  690 
chromates,  649-52 
cinnamate,  652 
citrate,  652 
copper  sulfate,  276 
cyanide,  270,  531,  613,  649 
dichromate,  650-2 
diethyl  barbiturate,  629 
dihydrogen  phosphate,  663 
ferrocyanide,  532,  652 
fluoride,  27,  175,  357,  534,  632,  649, 

652 

fluosilicate,  652   • 
fluozirconate,  676 
formate,  653 
gadolinium  sulfate,  305 
glycerophosphate,  653 
gold  chloride,  308 
hydrogen  arsenate,  629 
hydrogen  phosphate,  662 
hydrosulfite,  673 
hydroxide,  109,  113,  536,  585,  627, 

629,    630,    632,    643,    649,    651-4, 

663,  670 
iodate,  654 
iodide,  177,  616,  632,  634,  649,  652, 

654-6 

iodide  mercuric  cyanide,  423 
iodomercurate,  656 
iron  sulfate,  344 
lanthanum  sulfate,  348 
lithium  sulfate,  377 
lithium  tartrate,  378 
magnesium  sulfate,  668 
manganese  sulfate,  404 
mercuric  chloride,  41 1 
mercury  iodide,  656 
meta  borate,  502,  631 
meta  phosphate,  631 
meta  vanadate,  676 
molybdate,  440,  656 
nickel  sulfate,  454 
nitrate,  55,  58,  109,  116-7,  208,  222, 

360,  376,  509,  519,  545-6,  548,  618, 

632,  635,  644-5,  656-61 
nitrite,  649,  659-60 
nitrophenol,  662 
oleate,  480,  660 
oxalate,  552,  660-1 
palmitate,  661 
perchlorate,  639 
phenolate,  662 
phenol  sulfonate,  674 
phosphate,  662 
phosphate  fluoride,  664 
phosphites,  664 
picrate,  664 

potassium  carbonate,  512 
potassium  sulfate,  559,  668 
potassium  tartrate,  566 
potassium  thiosulfate,  568 


839 


SUBJECT  INDEX 


Sodium,  pyrophosphate,  631,  649,  664 

rhodonitrite,  660 

salicylate,  187,  590,  665 

samarium  sulfate,  594 

selenate,  665 

silicate,  119,  213,  378,  396,  631,  665 

silver  cyanide,  613 

stannate,  665 

succinates,  665-6 

sulfate,  121,  179,  218,  220,  259-60, 
274,  365,  378,  397,  405,  522,  526, 
559,  562,  623,  632,  637,  641,  649, 
651-2,  656,  658,  660-1,  667-72, 

747 

sulfide,  455,  672 

sulfite,  673 

sulfoantimonate,  627-8 

sulfonates,  673-4 

tartrate,  566,  674 

tellurates,  674 

tetraborate,  367,  629-31 

tetrachromate,  650 

tetraiodofluorescein,  335 

thiocyanate,  567 

thiosulfate,  208,  222,  628,  674-5 

thorium  sulfate,  725 

trichromate,  650 

tungstate,  656,  665,  672,  675 

uranyl  chromate,  734 

uranyl  oxalates,  66 1 

urate,  676 

yttrium  sulfate,  747 

zinc  sulfate,  755 

zirconium  fluoride,  676 
Sorbitols,  benzal,  698 
Sorbose,  697 
Sparteine,  676 

sulfate,  676 

Stannous,  stannic  (see  Tin) 
Stearic  acid,  97,  248,  446,  467-8,   475, 

676-7 

Stearin,  tri,  225,  467,  475,  677 
Stilbene,  88,  103,   123,   133,  147,   280, 

677 
Strontium  acetate,  677 

ammonium  sulfate,  68 

benzoate,  678 

bromate,  678 

bromide,  100,  678 

camphorate,  678 

carbonate,  649,  678-9 

chlorate,  679 

chloride,  100,  in,  119,  170,  198, 
356,  371,  388,  526,  649,  679,  680 

chromate,  680 

cinnamate,  68 1 

fluoride,  680,  68 1 

formate,  68 1 

glycerophosphate,  68 1 

hydroxide,  678,  680-2 

hyposulfate,  365 

iodate,  682 

iodide,  682 


Strontium  acetate,  iodide  mercuric  cy- 
anide, 423 

iodomercurate,  682 

malate,  683 

malonate,  683 

mercuric,  iodide,  682 

molybdate,  683 

nitrate,  361,  546,  548,  659,  68 1,  683 

nitrite,  620,  683-4 

oxalate,  684 

oxide,  157,  198,  680,  684 

periodide,  682 

permanganate,  684 

potassium  sulfate,  558 

salicylate,  684 

silicate,  378,  665 

succinate,  685 

sulfate,  378,  562,  672,  680,  685-6 

tartrate,  686 

tungstate  (di),  686 
Strychnine,  687 

salts,  688-9 
Suberic  acid,  689 
Succinic  acid,  136,  480,  666,  690-2 

acid,  amino,  692 

acid,  bromo,  692 

acid,  chloro,  692 

acids,  pyridinamino,  575 

acid  nitrile,  102,  133,  135,  224,  299, 

405,445,  618,  649,693 
Succinimide,  693 
Sucrose  (see  Sugar) 
Sugar,    166,    187,    198,  205,  397,   512, 

548,  627,  636,  648,  672,  693-8 
Sulfanilic  acid,  698 
Sulfine  chloroplatinates,  499 
Sulfonal,  435,  448,  593 
Sulfonium  perchlorates,  698 

iodide,  triethyl,  699 
Sulfur,    76,    127,    130,    150,    160,   247, 
334,  421,  446,  489,  564,  596,  672, 
699-705,  720,  729 

dioxide,  160,  224,  247,  315,  436,  438, 

705-8 

Sulfuric  acid,  5,  9,  10,  16,  124,  136, 
145,  146,  278,  279,  484,  486,  575, 
708-9,  726,  731 

Sulfon  methanes,  ethyl,  and  methyl,  435 
Sulfur  trioxide,  708-9 
Sulfuryl  chloride,  247,  708 
"Superphosphates,"  212 
Syngenite,  218 

Tachhydrite,  196,  641 

Talitol,  tribenzal,  698 

Tannic  acid,  710 

Tantalum  potassium  fluoride,  710 

Tartaric  acid,  480,  481,  710-11 

Telluric  acid,  712 

Telluric  acid  caesium  oxalate,  185 

acid  potassium  oxalate,  552 

acid  rubidium  oxalate,  586 
Tellurium,  334,  596,  705,  712,  720 


840 


SUBJECT   INDEX 


Tellurium,  bromide,  diphenyl,  596 

caesium  chloride,  182 

chromium  alum,  249 

double  salts,  712 

rubidium  chloride,  584 

tetra  iodide,  713 
Terephthalic  acid,  490 
Terpin  hydrate,  712 
Tetra  hydrobenzene,  89 

iodo  pyrrol,  335 
Tetronal,  435 
Thallium  alum,  32,  713 

bisulfate,  720 

bromate,  713,  716 

bromide,  713 

caesium  chloride,  182 

carbonate,  713 

chloride,  in,  150,  170,  183,  198,  270, 
339,  356,  371,  388,  526,  583,  611, 
649,  680,  713,  715-8 

chlorate,  714 

chromate,  717 

cyanide,  717 

double  cyanides,  717 

double  sulfates,  720 

fluoride,  717 

hydroxide,  717 

iodate,  718 

iodide,  713,  718 

mercuric  cyanide,  423 

nitrate,  547,  548,  619,  659,  718 

oxalate,  718 

perchlorate,  714 

phosphate,  718 

picrate,  719 

platinum  chloride,  498 

rubidium  chloride,  584 

selenate,  719 

silver  cyanide,  613 

sulfate,  31,  719-20 

sulfide,  720 

sulfite,  720 

thiocyanate,  716,  720 

vanadates,  721 
Thallo  thallic  chloride,  717 
Thebaine,  721 
Theobromine,  187,  721 
Theocin,  721 
Theophylline,  721 
Thiocarbamide  (thiourea),  70 

diodo  di,  226 
Thiophene,  128 

carbonic  acids,  721 
Thiophenylazine,  123 
Thiosinamine,  738 
Thiourea  (thiocarbamide),  70,  738 
Thorium  ammonium  oxalate,  60,  722 

ammonium  sulfate,  724 

borate,  722 

chloro  acetates,  721 

chloro  oxalate,  723 

emanations,  721 

hippurate,  722 


Thorium  ammonium  oxalate,  nitroben- 
zene sulfonate,  725 

oxalate,  722-3 

picrate,  723 

potassium  sulfate,  724 

selenate,  723 

sodium  sulfate,  725 

sulfate,  723-5 
Thoulet  solution,  541 
Thulium    bromo    nitrobenzene    sulfo- 
nate, 725 

oxalate,  725 
Thymol,  5,  10,  146,  227,  251,  446,  484, 

495,  593,  725-6 
Tin,  334,  705,  712,  726 

chloride,  170,  198,  247,  270,  356,  371, 

388,  401,  522,  713,  726-7 
diphenyl,  430 
hydroxide,  728 
iodide,  728-9 
oxalate,  729 

potassium  chloride  (ous),  522 
sulfate,  729 
sulfide  (ous),  95 
tetraphenyl,  598,  729 
triphenyl,  95 
Titanium  potassium  fluoride,  568 

silicate,  119 
Tolane,  103,  123,  147 
Toluene,  21,  87,  88,  93,  239,  247,  278, 

293,  301,  313,  481,  704,  729-30, 

745 
bromo,  128,  227,  293,  301,  484,  572, 

693,  726,  730 
chloro,  87,  93 
chloro  nitro,  730 
dinitro,  I 
nitro,  24,  26,  27,  77,  79,  87,  93,  128, 

132,  283,  293,  300,  303,  408,  421, 

446,  465,  478,  729-30 
sulfonamines,  729 
sulfochloride,  730 
trinitro,  I,  16,  224,  495,  575 
Toluic  acids,  9,  10,  12,  136,  575,  730, 

731 

Toluidines,  79,  136,  224,  240,  283,  293, 
324,  431,  446,  448,  484,  486,  581, 
731-2 

Tolyl  carbamide,  226 

Trehalose,  696 

Tribenzylamine,  730 

Triethylamine,  102,  in  (see  Ethyl- 
amine) 

Trimethylamine,  437  (see  Methyl- 
amines) 

Trimethylethylene,  72 

Triolein,  467 

Trional,  435 

Trioxymethylene,  303 

Tripalmitin,  467,  475 

Triphenylamine,  282,  732 

Triphenyl  arsine,  732 

Triphenylbismuthine,  732 


841 


SUBJECT  INDEX 


Triphenyl  phosphine,  732 

guanidine,  2 

stibene,  732 

Tristearin,  467,  475,  677 
Trithioacetaldehyde,  732 
Trithiobenzaldehyde,  732 
Tropaeolin,  309 
Tropic  acid,  732 
Tungsten  trioxide,  675 
Turpentine,  294,  440,  733 

Ulexine,  280 

Uranyl  ammonium  carbonate,  43,  733-4 

ammonium  oxalate,  735 

ammonium  propionate,  736 

caesium  chloride,  734 

chloride,  733-4 

double  nitrates,  735 

iodate,  734 

nitrate,  734-5 

oxalate,  66 1,  735-6 

potassium  butyrate,  733 

potassium  carbonate,  512 

potassium  chloride,  734 

potassium  oxalate,  735 

potassium  propionate,  736 

potassium  sulfate,  736 

rubidium  chloride,  734 

sodium  chromate,  734 

sodium  oxalates,  66 1 

sulfate,  736 

tetra  methyl  ammonium  chloride,  734 
Uranium  sulfate,  736 
Urea,  279,  484,  486,  737-8 

diphenyl,  738 

Urethan,  80,  128,  283,  296,  421,  446, 
484.  593,  730,  741-2 

derivatives,  742 

methyl,  431 
Uric  acid,  742-3 
Ureide  of  glucose,  741 

Valeramides,  744 
Valeric  acid,  743 
Vanadium  ammonium  sulfate,  69 

caesium  alum,  180 

rubidium  alum,  582 

thallium  alum,  713 
Vanillic  aldehyde,  2 
Vanillin,  9,  10,  744 
Vaselin,  5 
Veratrine,  744 
Veratrol,  730,  744 
Veronal,  742,  744 
Vesuvin,  744 
Vinyl  sulfine  perchlorate,  698 

Water,  5,  125,  131,  133,  138-42,  144, 
164-6,  227,  235,  245,  248,  280, 
282,  285,  287,  294-5,  297,  299, 
302,  468,  487,  589,  593,  729,  730, 

Weldmint  oil,  468 


Xanthine,  dimethyl,  721 

Xanthone,  132 

Xenon,  745 

Xylenes,  2,  5,  21,  88,  94,  128,  281,  294, 

301,  484,  581,  693,  705,  730,  744 
nitro,  745 
Xylenol,  745 
Xylidene,  79,  484 
Xylitol,  dibenzal,  698 
Xylose,  696 

Ytterbium  benzene  sulfonate,  746 

cobalticyanide,  746 

dimethyl  phosphate,  746 

oxalate,  746 

sulfate,  746 
Yttrium  chloride,  746 

cobalticyanide,  746 

dimethyl  phosphate,  747 

glycolate,  746 

hydroxide,  747 

iodate,  746 

malonate,  746 

nitrate,  747 

oxalate,  747 

potassium  oxalate,  747 

sodium  sulfate,  747 

sulfate,  747 

sulfonates,  748 

tartrate,  748 

Zein,  748 
Zinc,  150,  712 

acetate,  748 

ammonium  chloride,  751 

ammonium  oxalate,  754 

ammonium  phosphate,  754 

ammonium  sulfate,  69,  273 

arsenite,  748 

benzoate,  749 

bicarbonate,  749 

bismuth  nitrate,  151 

bromide,  749 

caesium  sulfate,  186 

carbonate,  749 

cerium  nitrate,  242 

chlorate,  750 

chloride,  in,  150,  170,  198,  270, 
339,  356,  388,  401,  680,  713,  727, 
750-1 

chromates,  751 

cinnamate,  752 

cyanide,  531,  752 

fluoride,  652,  752 

gadolinium  nitrate,  304 

hydroxide,  752-3 

iodate,  753 

iodide,  753 

lanthanium  nitrate,  347 

mercuric  thiocyanate,  752 

neodymium  nitrate,  449 

nitrate,  395,  754 

oxalate,  60,  754 


842 


SUBJECT   INDEX 

Sine,  oxychlorides,  750  Zinc,  sulfate,  274-5,  404.  754~5 
phenol  sulfonate,  756  sulfide,  277,  345,  365,  624,  755 

potassium  cyanide,  532  sulfite,  755 

potassium  sulfate,  557  sulfonates,  755-6 

potassium  vanadate,  568  tartrate,  756 

praseodymium  nitrate,  568  thallium  cyanide,  717 

rubidium  sulfate,  587  thallium  sulfate,  720 

samarium  nitrate,  594  valerate,  756 

silicate,  178,  378  Zirconium  sodium  fluoride,  676 
sodium  sulfate,  755  sulfate,  756 


843 


Table  Showing  the  Volume  Number  and  Corresponding  Year 

(Those  journals  marked  (*)  were  examined  page  by  page  for  solubility  data.     In 

last  number  recorded  for  each  journal  is  that 


1900 

1901 

1902 

1903 

1904 

IQ05 

1906 

Am  Chem  Jour.  (*)       

23-4 
72 
W9-io 

25 
310-14 

l7llQ-2I 

W?-3 

238 

1% 

33 

25-6 

73 

1  1-2 

26 

314-19 
22-24 

6 
4-6 
239 

10 

34 

27-8 
74 
13-4 
27 
320-26 
25-27 
7 
7-9 
240 
n 
35 

29-30 

75 
15-6 
28 
326-30 
28-30 
8 

IO-I2 

241 
12 
36 

3J~2 
76 
17-8 
29 

«rf 

9 
13-15 

242 

13 

37 

33-4 
77 
19-20 
30 
338-43 
4-6 
10 
16-18 
243 
14 
38 

35-6 

78 

21-2 
31 
344-51 

7-9 
ii 
19-21 
244 

15 
39 

i 

35 
20 

Am  Jour  Pharm.  (*)  

Am.  Jour.  Sci.  (t)  

Analyst  (t)  
Ann  Chem   (Liebig's)  (t)  

Ann  chim  phys.*  (*)  

Ann  chim  anal,  (t)  ".  •  • 

Ann.  Physik  (Wied.)  (t)  
Arch.  Pharm.  (f)  -  
Atti  accad  Lincei  (*) 

Ber  (*) 

Biochem,  J.  (t)  

Bull  soc  chim   (*) 

l3]23 

14 

25 
IS 

27 
16 

29 
17 

i 

33 
19 

Bull.  soc.  chim.  belg.  (*)  
Chem.  Abs.  (*) 

Chem.  News  (t)  .  .  . 

81-2 

83-4 

85-6 

87-8 

89-90 

I 

28 
138-9 

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1  Changed  to  Ann.  chim.  in  1914. 


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of  Publication  of  Fifty  Chemical  and  Related  Periodicals. 

the  case  of  those  marked  (f),  the  tables  of  contents  only  were  searched.    The 
of  the  last  complete  volume  examined.) 


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1908 

1909 

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15-16 

17-18 

19-20 

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24-25 

26-27 

28-29 

30-31 

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11-12 

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16-17 

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93-95 

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Briggs,  R.,  and  Wolff,  A.  R.     Steam-Heating i6mo,  o  75 

Bright,  C.     The  Life  Story  of  Sir  Charles  Tilsoji  Bright 8vo,  *4  50 

—  Telegraphy,  Aeronautics  and  War 8vo,  6  oo 

Brislee,  T.  J.     Introduction  to  the  Study  of  Fuel.  .8vo   (Reprinting.) 

Broadfoot,  S.  K.     Motors:    Secondary  Batteries i2mo,  o  75 

Broughton,  H.  H.     Electric  Cranes  and  Hoists 

Brown,  G-.     Healthy  Foundations i6mo,  o  75 

Brown,  H.     Irrigation 8vo    (Reprinting.) 

Brown,    H.      Rubber 8vo,  2}  50 

W.  A.     Portland  Cement  Industry 8vo,  3  oo 

Brown,    Wm.    N.      Dipping,    Burnishing,     Lacquering    and    Bronzing 

Brass  Ware   i2mo,  *i  50 

—  Handbook    on    Japanning i2mo,  *2  oo 

Brown,  Wm.  N.     The  Art  of  Enamelling  on  Metal i2mo,  *2  oo 

—  House    Decorating    and    Painting i2ino,  *2  oo 

—  History  of  Decorative  Art i2mo  *o  50 

—  Workshop    Wrinkles    8vo,  *i  oo 

Browne,  C.  L.    Fitting  and  Erecting  of  Engines 8vo,  *i  50 

Browne,  R.  E.     Water  Meters i6mo,  o  75 

Bruce,  E.  M.     Detection  of  Common  Food  Adulterants i2mo,  i  40 

Brunner,  R.     Manufacture  of  Lubricants,  Shoe  Polishes  and  Leather 

Dressings    8vo,  3  50 

Buel,  R.  H.     Safety  Valves iGmo,  o  75 

Bunkley,  J.  W.     Military  and  Naval  Recognition  Book i6mo,  i  oc 

Burley,  G.  W.     Lathes.    Their  Construction  and  Operation 12010,  2  oo 

—  Machine  and  Fitting  Shop  Practice.     2  vols izmo,  each,  2  oo 

—  Testing  of  Machine  Tools i2mo,  2  oo 

Burnside,   W.     Bridge    Foundations i2mo,  *2  oo 


,6         D.  VAN  NOSTRAND  CO.'S  SHORT  TITLE  CATALOG 

Burstall,  F.  W.    Energy  Diagram  for  Gas.    With  Text 8vo,  i  50 

Diagram.     Sold  separately *i  oo 

Burt,  W.  A.    Key  to  the  Solar  Compass i6mo,  leather,  2  50 

Buskett,   E.   W.     Fire   Assaying i2mo,  *i  25 

Butler,  H.  J,     Motor  Bodies   and   Chassis . 8vo,  *3  oa 

Byers,  H.  G.,  and  Knight,  H.  G.    Notes  on  Qualitative  Analysis. . .  ,8vo, 

(New  Edition  in  Preparation.) 

Cain,  W.    Brief  Course  io  the  Calculus i2mo,  *i  75 

Elastic    Arches    i6mo,  o  75 

. Maximum    Stresses    i6mo,  o  75 

Practical    Designing    Retaining    of   Walls i6mo,  o  75 

Theory   of   Steel-concrete   Arches   and   of   Vaulted    Structures. 

iGmo,  o  75 

Theory   of    Voussoir   Arches i6mo,  o  75 

Symbolic    Algebra    i6mo,  o  75 

Calvert,   G.    T.     The   Manufacture    of    Sulphate    of    Ammonia    and 

Crude  Ammonia   i2mo,  4  oo 

Camm,    S.^    Aeroplane    Construction xarno,  3  oo 

Carhart,   H.   S.     Thermo   Electromotive   Force   in   Electric   Cells, 

(In  Press.} 

Carey,  A.  E.,  and  Oliver,  F.  W.     Tidal  Lands 8vo,  5  oo 

Carpenter,   F.   D.     Geographical   Surveying i6mo, 

Carpenter,  R.  C.,  and  Diederichs, H.   Internal  Combustion  Engines. 8vo,  5  50 

Carter,  H.  A.    Ramie  (Rhea),  China  Grass i2mo,  *3  oo 

Carter,  H.  R.     Modern  Flax,  Hemp,  and  Jute  Spinning 8vo,  *3  50 

Bleaching,  Dyeing  and  Finishing  of  Fabrics 8vo,  *i  25 

Cary,  E.  R.     Solution  of  Railroad  Problems  with  the  Slide  Rule. .  i6mo,  *i  oo 

Casler,  M.  D.    Simplified  Reinforced  Concrete  Mathematics i2mo,  *i  oo 

Cathcart,  W.  L.     Machine  Design.     Part  I.  Fastenings 8vo,  *3  oo 

Cathcart,  W.  L.,  and  Chaff e e,  J.  I.     Elements  of  Graphic  Statics.  .  .8vo,  *3  oo 

• Short  Course  in  Graphics i2mo,  i  50 

Caven,  R;  M.,  and  Lander,  G.  D.   Systematic  Inorganic  Chemistry.  i2mo,  2  25 

Chalkley,  A.  P.    Diesel  Engines 8vo,  *4  oo 

Chalmers,  T.  W.     The  Production  and  Treatment  of  Vegetable  Oils, 

4to,  7  50 

Chambers'    Mathematical    Tables 8vo,  2  50 

Chambers,  G.  F.     Astronomy i6mo,  *i  50 

Chappel,    E.      Five    Figure    Mathematical    Tables 8vo,  250 

Charnock,    Mechanical    Technology 8vo,  3  50 

Charpentier,    P.      Timber 8vo,  *6  oo 

Chatley,  H.     Principles  and  Designs  of  Aeroplanes i6mo,  o  75 

How  to  Use  Water  Power i2mo,  *i  50 

—  Gyrostatic   Balancing    8vo,  *i  25 

Child,  C.  D.    Electric  Arc 8vo,  *2  oo 

Christian,  M.    Disinfection  and  Disinfectants i2mo,  2  50 

Christie,  W.  W.     Beiler-waters,  Scale,  Corrosion,  Foaming 8vo,  *3  oo 

• Chimney  Design  and  Theory 8vo,  *3  oo 

Furnace    Draft    i6mo,  o  75 

• Water:  Its  Purification  and  Use  in  the  Industries 8vo,  *2  oo 

Church's   Laboratory   Guide 8vo,  2  50 

Clapham,  J.  H.     Woolen  and  Worsted  Industries 8vo,  200 


D.  VAN  NOSTRAND  CO.'S  SHORT  TITLE  CATALOG         7 

Clapperton,   G.     Practical  Papermaking 8vo    (Reprinting.} 

Clark,  A.  G.     Motor  Car  Engineering. 

Vol.   I.     Construction *4  oo 

Vol.  II.     Design    8vo,  *3  50 

Clark,  C.  H.    Marine  Gas  Engines.    New  Edition 2  oo 

Clarke,  J.  W.,  and  Scott,  W.    Plumbing  Practice. 

Vol.      I.     Lead  Working  and  Plumbers'  Materials 8vo,  *4  oo 

Vol.    II.    Sanitary  Plumbing  and  Fittings (In  Press.") 

Vol.  III.     Practical  Lead  Working  on  Roofs (In  Press.} 

Clarkson,  R.  P.    Elementary  Electrical  Engineering  (In  Press.} 

Clerk,  D.,  and  Idell,  F.  E.    Theory  of  the  Gas  Engine .i6mo,  o  75 

Clevenger,  S.  R.     Treatise  on  the  Method  of  Government  Surveying. 

i6mo,   morocco,  2  50 

Clouth,  F.     Rubber,  Gutta-Percha,  and  Balata 8vo,  *6  oo 

Cochran,  J.    Concrete  and  Reinforced  Concrete  Specifications 8vo,  *2  50 

• Treatise  on  Cement  Specifications 8vo,  *i  oo 

Cocking,  W.  C.     Calculations  for  Steel-Frame  Structures i2mo,  *2  50 

Coffin,  J.  H.  C.    Navigation  and  Nautical  Astronomy i2mo,  3  oo 

Colburn,  Z.,  and  Thurston,  R.  H.     Steam  Boiler  Explosions. ..  .i6mo,  o  75 

Cole,   R.   S.     Treatise   on   Photographic   Optics i2mo,  2  oo 

Coles-Finch,  W.     Water,  Its  Origin  and  Use .' 8vo,  *5  oo 

Collins,  C.  D.    Drafting  Room  Methods,  Standards  and  Forms Svo,  2  oo 

Collins^  S.  Hoare.     Plant  Products  and  Chemical  Fertilizers Svo,  3  oo 

Collis,  A.  G.     High  and  Low  Tension  Switch-Gear  Design Svo,  *3  50 

Switchgear    i2mo,  o  50 

Colver,    E.   D.    S.      High    Explosives Svo,  12  50 

Comstock,  D.  F.,  and  Troland,  L.  T.     The  Nature  of  Electricity  and 

Matter    Svo,  2  50 

Coombs,  H.  A.     Gear  Teeth i6mo,  o  75 

Cooper,  W.  R.    Primary  Batteries 8vo,  *6  oo 

Copperthwaite,  W.  C.     Tunnel  Shields 4to,  *g  oo 

Corfield,  W.   H.     Dwelling  Houses i6mo,  075 

Water   and   Water-Supply i6mo,  o  75 

Cornwall,  H.  B.     Manual  of  Blow-pipe  Analysis Svo.  *2  50 

Cowee,  G.  A.    Practical  Safety  Methods  and  Devices Svo,  4  oa 

Cowell,  W.  B.     Pure  Air,  Ozone,  and  Water i2mo,  *a  50 

Craig,  J.  W.,  and  Woodward,  W.  P.     Questions  and  Answers  Abo*t 

Electrical  Apparatus i2mo,  leather,  i  50 

Craig,  T.     Motion  of  a  Solid  in  a  Fuel i6mo,  o  75 

—  Wave    and    Vortex    Motion i6mo,  o  75 

Crehore,  A.  C.     Mystery  of  Matter  and  Energy Svo,  i  oo 

— .  New  Theory  of  the  Atom (In  Press.} 

Crocker,  F.  B.,  and  Arendt,  M.    Electric  Motors 8vo,  *2  50 

Crocker,  F.  B.,  and  Wheeler,  S.  S.  The  Management  of  Electrical  Ma- 
chinery   I2H10,  *I  OO 

Crosby,  E.  TJ.,  Fiske,  H.  A.,  and  Forster,  H.  W.  Handbook  of  Fire 

Protection i2mo,  4  oo 

Cross,  C.  F.,  Bevan,  E.  J.,  and  Sindall,  R.  W.  Wood  Pulp  and  Its 
Uses  Svo  (Reprinting.} 

Crosskey,   L.   R.     Elementary   Perspective Svo,  i  50 


8          D.  VAN  NOSTRAXD  CO.'S  SHORT  TITLE  CATALOG 

Crosskey,  L.  R.,  and  Thaw,  J.    Advanced  Perspective 8vo,  2  oo 

Culley,  J.  L.     Theory  of  Arches i6mo,  o  75 

Gushing,  H.  C.,  Jr.,  and  Harrison,  N.    Central  Station  Management. ,,  *2  oo 


Dadourian,  H.  M.    Analytical  Mechanics i2mo,  *3  oo 

— Graphic  Statics    8vo,  o  75 

Danby,  A.    Natural  Rock  Asphalts  and  Bitumens 8vo,  *2  50 

Darling,  E.  R.     Inorganic  Chemical  Synonyms ii.mo,  i  oo 

Davenport,  C.     The   Book 8vo,  2  oo 

Davey,  N.    The  Gas  Turbine 8vq,  *4  oo 

Davies,  F.  H.    Electric  Power  and  Traction 8vo,  *2  oo 

— — Foundations   and   Machinery   Fixing i6mo,  i  oo 

Deerr,   N.     Sugar   Cane 8vo,  10  oo 

De  la  Coux,  H.    The  Industrial  Uses  of  Water 8vo,  5  oo 

Del  Mar,  W.  A.    Electric  Power  Conductors 8vo,  *2  oo 

Denny,  G.  A.    Deep-level  Mines  of  the  Rand 4to,  *io  oo 

De  Roos,  J.  D.  C.     Linkages ifcmo,  o  75 

Derr,  W.  L.    Block  Signal  Operation Oblong  i2mo,  *i  50 

Desaint,  A.    Three  Hundred  Shades  and  How  to  Mix  Them 8vo,  *g  oo 

De  Varona,  A.     Sewer  Qases i6mo,  o  75 

Devey,  R.  G.    Mill  and  Factory  Wiring i2mo,  i  oo 

Dichmann,  Carl.     Basic   Open  Hearth   Steel   Process i2mo,  4  oo 

Dieterich,  K.     Analysis  of  Resins,  Balsams,  and  Gum  Resins. ..  .8vo,  *3  50 

Dilworth,  E.  C.    Steel  Railway  Bridges 4to.  *4  oo 

Dinger,  Lieut.  H.  C.    Care  and  Operation  of  Naval  Machinery. ..  lamo,  *3  oo 
Dixon,  D.  B.     Machinist's  and  Steam  Engineer's  Practical  Calculator. 

i6mo,  morocco,  i  25 

Dommett,  W.  E.     Motor  Car  Mechanism 12010,  *2  oo 

Dorr,  B.  F.    The  Surveyor's  Guide  and  Pocket  Table-book. 

i6mo,  morocco,  2  oo 

Draper,  C.  H.     Heat  and  the  Principles  of  Thermo-Dynamics.  .  i2mo,  2  25 

Draper,  E.  G.     Navigating  the  Ship 12010,  2  oo 

Dubbel,  H.    High  Power  Gas  Engines 8vo,  *5  oo 

Dumesny,  P.,  and  Noyer,  J.    Wood  Products,  Distillates,  and  Extracts. 

8vo,  *5  oo 
Duncan,  W.  G.,  and  Penman,  D.  The  Electrical  Equipment  of  Collieries. 

8vo,  *5  oo 

Dunkley,  W.  G.  Design  of  Machine  Elements.  Two  volumes.  .8 vo,each,  2  oo 

Dunstan,  A.  E.,  and  Thole,  F.  B.  T.     Textbook  of  Practical  Chemistry. 

i2mo,  *i  40 

Durham,  H.  W.     Saws. 8vo,  2  50 

Duthie,  A.  L.     Decorative  Glass  Processes 8vo,  2  50 

Dwight,  H.  B.     Transmission  Line  Formulas 8vo,  *2  oo 

Dyke,  A.  L.     Dyke's  Automobile  and  Gasoline  Engine  Encyclopedia, 

8vo,  5  oo 

Dyson,  S.  S.    A  Manual  of  Chemical  Plant.     12  parts.  .. -4to,  paper,  7  50 

Dyson,  S.  S.,  and  Clarkson,  S.  S.     Chemical  Woiks 8vo,  *g  oo 

Eccles,  W.  H.     Wireless  Telegraphy  and  Telephony i2mo,  *8  80 


D.  VAN  NOSTRAND  CO.'S  SHORT  TITLE  CATALOG  9 

Eck,  J.     Light,   Radiation   and  Illumination 8vo,  250 

Eddy,  L.  C.     Laboratory  Manual  of  Alternating  Currents i2mo,  o  50 

Edelman,  P.  Inventions  and  Patents i2mo,  *i  50 

Edgctmbe,  K.    Industrial  Electrical  Measuring  Instruments 8vo,  5  oo 

Edler,    R.      Switches    and    Switchgear 8vo,  4  oo 

Eissler,  M.     The  Metallurgy  of  Gold 8vo,  9  oo 

The  Metallurgy  of  Silver 8vo,  4  oo 

The  Metallurgy  of  Argentiferous   Lead 8vo,  6  25 

A  Handbook  on  Modern  Explosives 8vo,  5  oo 

Ekin,  T.  C.    Water  Pipe  and  Sewage  Discharge  Diagrams folio,  *3  oo 

Electric  Light  Carbons,  Manufacture  of 8vo,  i  oo 

Eliot,  C.  W.,  and  Storer,  F.  H.     Compendious  Manual  of  Qualitative 

Chemical  Analysis i2mo,  *i  25 

Ellis,  C.     Hydrogenation  of  Oils 8vo,  7  50 

Ultraviolet   Light,  Its   Applications   in   Chemical   Arts i2mo, 

(In  Press} 

and  Meigs,  J.  V.     Gasolene  and  Other  Motor  Fuels..  (In  Press.} 

Ellis,  G.     Modern  Technical  Drawing 8vo,  *2  oo 

Ennis,  Wm.  D.     Linseed  Oil  and  Other  Seed  Oils 8vo,  5  oo 

Applied    Thermodynamics 8vo,  5  oo 

Flying  Machines  To-day i2mo,  *i  50 

Vapors  for  Heat  Engines i2mo,  *i  oo 

Ermen,  W.  F.  A.     Materials  Used  in  Sizing 8vo,  *2  oo 

'Erwin,  M.    The  Universe  and  the  Atom i2mo   (Reprinting.} 

Ewing,  A.  J.     Magnetic  Induction  in  Iron 8vo,  5  oo 

Fairchild,  J.  F.     Graphical  Compass  Conversion  Chart  and  Tables...  o  50 

Fairie,  J.     Notes  on  Lead  Ores i2mo,  *o  50 

—  Notes  on  Pottery  Clays i2mo,  *2  oo 

Fairley,  W.,  and  Andre,  Geo.  J.     Ventilation  of  Coal  Mines. ..  .i6mo,  o  75 

Fairweather,  W.  C.    Foreign  and  Colonial  Patent  Laws 8vo,  *3  oo 

Falk,   K.   G.     Chemical   Reactions:    Their   Theory   and  Mechanism. 

(In  Press.} 

Fanning,  J.  T.     Hydraulic  and  Water-supply  Engineering 8vo,  *5  oc 

Farnsworth,  P.  V.     Shop  Mathematics i2mo  (In  Press.} 

Fay,  I.  W.     The  Coal-tar  Dyes 8vo,  5  oa 

Fernbach,  R.  L.     Glue  and  Gelatine > 8vo,  *3  oo 

Findlay,  A.    The  Treasures  of  Coal  Tar i2mo,  2  oo 

Firth,  J.  B.    Practical  Physical  Chemistry i2mo]  i  25 

Fischer,  E.     The  Preparation  of  Organic  Compounds i2mo,  i  50 

Fisher,  H.  K.  C.,  and  Darby,  W.  C.     Submarine  Cable  Testing.  .  .8vo,  4  oo 

^leischmann,  W.     The  Book  of  the  Dairy 8vo,  4  50 

Fleming,  J.  A.    The  Alternate-current  Transformer.     Two  Volumes.  8vo. 

Vol.    I.     The  Induction  of  Electric  Currents *6  50 

Vol,  II.     The  Utilization  of  Induced  Currents 6  50 

Propagation   of   Electric   Currents 8vo,  3  50 

A  Handbook  for  the  Electrical  Laboratory  and  Testing  Room.    Two 

Volumes 8vo,  each,  *6  5° 

Fleury,  P.     Preparation  and  Uses  of  White  Zinc  Paints 8vo,  3  oo 

Flynn,  P.  J.     Flow  of  Water : 12mo>  0  75 

Hydraulic    Tables    i6tno,  o  75 


10        D.  V*.N  NOSTRAND  CO.'S  SHORT  TITLE  CATALOG 

Foster,  H.  A.     Electrical  Engineers'  Pocket-book.      (Seventh  Edition.) 

i2mo,  leather,  5  oo 

—  Engineering  Valuation  of  Public  Utilities  and  Factories 8vo,  *3  oo 

Fowle,  F.  F.     Overhead  Transmission  Line  Crossings 12  mo,  *i  50 

The  Solution  of  Alternating  Current  Problems ....  .8vo  (In  Press.) 

Fox,   W.    G.     Transition   Curves i6mo,  o  75 

Fox,  W.,  and  Thomas,  C.  W.     Practical  Course  in  Mechanical  Draw- 
ing   1 2010,  i  25 

Foye,  J.  C.     Chemical  Problems i6mo,  o  75 

—  Handbook    of    Mineralogy i6mo,  075 

Francis,  J.  B.     Lowell  Hydraulic  Experiments 4to,  15  oo 

Franzen,  H.     Exercises  in  Gas  Analysis i2mo,  *i  oo 

Fraser,   E.   S.,  and  Jones,  R.  B.     Motor  Vehicles   and  Their  Motors, 

Svo,   fabrikoid,  2  oo 

Freudemacher,  P.  W.     Electric  Mining  Installations iamo,  i  oo 

Friend,  J.  N.     The  Chemistry  of  Linseed  Oil i2mo,  i  oo 

Fritsch,  J.    Manufacture  of  Chemical  Manures .8vo,  5  oo 

Frye,  A.  I.     Civil  Engineers'  Pocket-book i2mo,  leather,  *5  oo 

Fuller,  G.  W.     Investigations  into  the  Purification  of  the  Ohio  River. 

4to,  *io  oo 
Furaell,  J.     Paints,  Colors,  Oils,  and  Varnishes Svo. 


Gant,  L.  W.     Elements  of  Electric  Traction Svo,  *2  50 

Garcia,  A.  J.  R.  V.     Spanish-English  Railway  Terms Svo,  3  co 

Gardner,  H.  A.     Paint  Researches,  and  Their  Practical  Applications, 

Svo,  *s  oo- 
Garforth,  W.  E.     Rules  for  Recovering  Coal  Mines  after  Explosions  and 

Fires i2mo,  leather,  i  50 

Garrard,  C.  C.    Electric  Switch  and  Controlling  Gear Svo,  *6  oo 

Gaudard,    J.     Foundations i6mo,  o  75 

Gear,  H.  B.,  and  Williams,  P.  F.     Electric  Central  Station  Distribution 

Systems Svo,  *s  50 

Geerligs,  H.  C./  P.     Cane  Sugar  and  Its  Manufacture Svo,  *6  oo 

Chemical  Control  in  Cane  Sugar  Factories 4to,  5  oo 

Geikie,  J.     Structural  and  Field  Geology Svo,  4  50 

—  Mountains.     Their  Growth,  Origin  and  Decay Svo,  4  50 

—  The  Antiquity  of  Man  in  Europe Svo,  *s  oo 

Georgi,  F.,  and  Schubert,  A.     Sheet  Metal  Working Svo,  3  50 

Gerhard,  W.  P.     Sanitation,  Watersupply  and  Sewage  Disposal  of  Country 

Houses i2mo,  *2  oo 

Gas  Lighting    i6mo,  o  75 

—  Household   Wastes    i6mo,  o  75 

—  House    Drainage    i6mo,  o  75 

—  Sanitary  Drainage  of  Buildings i6mo,  o  75 

Gerhardi,    C.    W.    H.      Electricity    Meters Svo,  *y  20 

Geschwind,  L.     Manufacture  of  Alum  and  Sulphates Svo,  5  oo 

Gibbings,  A.  H.     Oil  Fuel  Equipment  for  Locomotives.     Svo. 

(Reprinting.} 

Gibbs,  W.  E.     Lighting  by  Acetylene .  . 12010,  *i  50 


D.  VAN  NOSTRAND  CO.'S  SHORT  TITLE  CATALOG  n 

Gibson,  A.  H.     Hydraulics  and  Its  Application 8vo,  6  oo 

• Water  Hammer  in  Hydraulic  Pipe  Lines i2mo,  2  50 

Gibson,  A.  H.,  and  Ritchie,  E.  G.    Circular  Arc  Bow  Girder 4to,  *s  50 

Gilbreth,  F.  B.     Motion  Study i2mo,  *2  oo 

—  Primer  of  Scientific  Management i2mo,  *i  oo 

Gillmore,  Gen.  Q.  A.    Roads,  Streets,  and  Pavements iamo,  i  25 

Godfrey,  E.     Tables  for  Structural  Engineers i6mo,  leather,  *2  50 

Golding,  H.  A.     The  Theta-Phi  Diagram i2mo,  *2  oo 

Goldschmidt,  R.     Alternating  Current  Commutator  Motor 8vo,  *3  oo 

Goodchild,   W.     Precious   Stones 8vo,  2  50 

Goodell,    J.    M.      The    Location,    Construction    and    Maintenance    of 

Roads    8vo,  2  oo 

Goodeve,  T.  M.     Textbook  on  the  Steam-engine i2mo,  2  50 

Gore,  G.     Electrolytic  Separation  of  Metals 8vo,  4  50 

Gould,  E.  S.     Arithmetic  of  the  Steam-engine i2mo,  i  oo 

—  Calculus    i6mo,  o  75 

—  High  Masonry  Dams i6mo,  o  75 

Gould,  E.  S.    Practical  Hydrostatics  and  Hydrostatic  Formulas.  .16 mo,  o  75 

Gratacap,  L.  P.    A  Popular  Guide  to  Minerals 8vo,  *2  oo 

Gray,  H.  H.    Gas-Works  Products 8vo    (/;/  Prrss.) 

Gray,  J.     Electrical  Influence  Machines i2mo,  2  oo 

Marine    Boiler   Design i2mo    (Reprinting.) 

Greenhill,  G.     Dynamics  of  Mechanical  Flight 8vo,  *2  50 

Greenwood,  H.   C.     The  Industrial   Gases 8vo    (///   Press.} 

Gregorius,    R.      Mineral    Waxes i2mo,  3  oo 

Grierson,  R.     Some  Modern  Methods  of  Ventilation 8vo,  *s  oo 

Griffiths,  A.  B.     A  Treatise  on  Manures i2mo   (Reprinting.} 

Gross,  E.     Hops 8vo,  *5  oo 

Grossman,  J.     Ammonia  and  Its  Compounds i2mo,  i  50 

Groth,  L.  A.     Welding  and  Cutting  Metals  by  Gases   or  Electricity. 

8vo,  2  50 

Grover,  F.     Modern  Gas  and  Oil   Engines .8vo,  *3  oo 

Grunerf  A.     Power-loom   Weaving 8vo,  *s  50 

Grunsky,  C.  E.     Topographic  Stadia  Surveying i6mo,  2  oo 

Guldner,  H.     Internal  Combustion  Engines (In  Press.) 

Gunther,  C.   0.     Integration 8vo,  i  50 

Gurden,  R.  L.     Traverse  Tables folio,  half  morocco,  *y  50 

Guy,  A.  E.     Experiments  on  the  Flexure  of  Beams 8vo,  *i  25. 

Haenig,  A.     Emery   and   Emery  Industry 8vo,  *2  50 

Hainbach,   R.     Pottery   Decoration i2mo,  3  50 

Hale,    A.   J.     The   Manufacture    of   Chemicals   by   Electrolysis.     8vo, 

(In  Press.) 

Hale,  W.  J.     Calculations  of  General   Chemistry i2mo,  i  50 

Hall,  C.  H.     Chemistry  of  Paints  and  Paint  Vehicles i2mo,  *2  oo 

Hall,  R.  H.     Governors  and  Governing  Mechanism i2mo,  *2  50 

Hall,  W.  S.    Elements  of  the  Differential  and  Integral  Calculus 8vo,  2  75 

—  Descriptive  Geometry 8vo  volume  and  a  4to  atlas,  4  oo 

Haller,  G.  F.,  and  Cunningham,  E.  T.     The  Tesla  Coil i2mo,  *i  25 

Halsey,  F.  A.     Slide  Valve  Gears i2mo,  i  50 

— The   Use    of    the   Slide    Rules i6mo,  075 

Worm  and   Spiral   Gearing i6mo,  o  75 


12       D.  VAN  NOSTRAND  CO.'S  SHORT  TITLE  CATALOG 

Hancock,  H.     Textbook  of  Mechanics  and  Hydrostatics 8vo,  i  50 

Hardy,  E.     Elementary  Principles  of  Graphic  Statics i2mo,  *i  50 

flaring,  H.     Engineering  Law. 

Vol.  I.     Law  of  Contract 8vo,  *4  oo 

Harper,  J.  H.    Hydraulic  Tables  on  the  Flow  of  Water i6mo,  *2  oo 

Harris,  S.  M.    Practical  Topographical  Surveying (In  Press.) 

Harrow,  B.    Eminent  Chemists  of  Our  Times:  Their  Lives  and  Work. 

(In  Press.) 

Haskins,  C.  H.     The  Galvanometer  and  Its  Uses i6mo,  i  50 

Hatt,  J.  A.  H.     The  Colorist square  i2mo,  *i  50 

Hausbrand,  E.    Drying  by  Means  of  Air  and  Steam 12010,  2  50 

—  Evaporating,  Condensing  and  Cooling  Apparatus 8vo,  6  oo 

Hausmann,  E.     Telegraph  Engineering 8vo,  *3  oo 

Hausner,  A.    Manufacture  of  Preserved  Foods  and  Sweetmeats. ..  .8vo,  3  50 
Hawkesworth,  J.     Graphical  Handbook  for  Reinforced  Concrete  Design. 

4to,  2  oo 

Hay,  A.     Continuous  Current  Engineering 8vo,  ;:  2  50 

Hayes,  H.  V.    Public  Utilities,  Their  Cost  New  and  Depreciation. .  .8vo,  *2  oo 

—  Public  Utilities,  Their  Fair  Present  Value  and  Return 8vo,  *2  oo 

Heath,  F.  H.    Chemistry  of  Photography 8vo..  (In  Press.) 

Heather,  H.  J.   S.     Electrical  Engineering 8vo,  4  50 

Heaviside,  0.     Electromagnetic  Theory.     Vols.  I  and  II....8vo,  each, 

(Reprinting.) 

Vol.    Ill 8vo     (Reprinting.)- 

Heck,  R.  C.  H.     The  Steam  Engine  and  the  Turbine 8vo,  4  50 

Steam-Engine  and  Other  Steam  Motors.    Two  Volumes. 

Vol.  I.     Thermodynamics  and  the  Mechanics 8vo,  4  50 

Vol.   II.     Form,   Construction,   and   Working 8vo,  550 

Notes  on  Elementary  Kinematics 8vo,  boards,  *i  oo 

Graphics  of  Machine  Forces 8vo,  boards,  *i  oo 

Heermann,  P.     Dyers'  Materials i2mo,  3  oo 

Hellot,  Macquer  and  D'Apligny.   Art  of  Dyeing  Wool,  Silk  and  Cotton.  8vo,  *2  oo 
Bering,  C.,  and  Getman,  F.  H.     Standard  Tables  of  Electro-Chemical 

Equivalents    i2mo,  *2  oo 

Bering,  D.  W.     Essentials  of  Physics  for  College  Students 8vo,  2  25 

Herington,  C.  F.     Powdered  Coal  as  Fuel 8vo,  3  oo 

Herrmann,  G.    The  Graphical  Statics  of  Mechanism i2mo,  2  oo 

Herzfeld,  J.     Testing   of  Yarns   and   Textile   Fabrics 8vo. 

(New  Edition  in  Preparation.) 

Hildenbrand,    B.    W.      Cable-Making i6mo,  o  75 

Hilditch,  T.  P.     A  Concise  History  of  Chemistry i2mo,  *i  50 

Hill,  M.  J.  M.    The  Theory  of  Proportion 8vo,  *2  50 

Hillhouse,  P.  A.     Ship  Stability  and,  Trim .8vo,  4  50 

Hiroi,  I.     Plate  Girder  Construction i6mo,  o  75 

— ^Statically-Indeterminate  Stresses i2mo,  2  50 

Hirshf eld,  C.  F.    Engineering  Thermodynamics i6mo,  o  75 

Hoar,  A.     The  Submarine  Torpedo  Boat i2mo,  *2  oo 

Hobart,  H.  M.    Heavy  Electrical  Engineering 8vo,  *4  50 

—  Design   of    Static    Transformers i2mo,  250 

—  Electricity 8vo,  *2  oo 

—  Electric  Trains 8vo,  *2  50 

Electric  Propulsion  of  Ships 8vo,  *2  50 


D.  VAN  NQSTRAND  CO.'S  SHORT  TITLE  CATALOG  13 

Hobart,  J.  F.    Hard  Soldering,  Soft  Soldering  and  Brazing I2mo,  i  25 

Hobbs,  W.  R.  P.    The  Arithmetic  of  Electrical  Measurements. ..  .i2mo,  o  75 

Hoff,  J.  N.     Paint  and  Varnish  Facts  and  Formulas i2mo,  i  50 

Hole,  W.     The  Distribution  of  Gas 8vo,  *8  50 

Hopkins,  N.  M.     Model  Engines  and  Small  Boats i2mo,  i  25 

—  The    Outlook    for    Research    and    Invention i2mo.  2  oo 

Hopkinson,  J.,  Shoolbred,  J.  N.,  and  Day,  R.  E.     Dynamic  Electricity. 

i6mo.  o  ?!> 

Homer,  J.     Practical  Ironf ounding 8vo,  *2  oo 

—  Gear  Cutting,  in  Theory  and   Practice 8vo    (Reprinting.) 

Houghton,  C.  E.     The  Elements  of  Mechanics  of  Materials i2mo,  2  50 

Houstoun,  R.  A.    Studies  in  Light  Production 12010,  2  oo 

Hovenden,  F.     Practical  Mathematics  for  Young  Engineers 12010,  *i  50 

Howe,  G.     Mathematics  for  the  Practical  Man i2mo,  i  50 

Koworth,  J.     Repairing  and  Riveting  Glass,  China  and  Earthenware. 

8vo,  paper,  *o  50 

Hoyt,  W.  E.     Chemistry  by  Experimentation 8vo,  *»  70 

Hubbard,   E.     The   Utilization   of   Wood-waste 8vo,  *2  50 

Hiibner,  J.    Bleaching  and  Dyeing  of  Vegetable  and  Fibrous  Materials. 

8vo   (Reprinting.). 

Hudson,  0.  Ff    Iron  and  Steel 8vo,  •<.  ^ 

Humphreys,  A.  C.  The  Business  Features  of  Engineering  Practice .  8vo,  2  50- 

Hunter,  A.    Bridge  Work 8vo.  (In  Press.) 

Hurst,  G.  H.     Handbook  of  the  Theory  of  Color 8vot  *3  50 

Dictionary  of  Chemicals  and  Raw  Products 8vo,  *5  oo 

Lubricating  Oils,  Fats  and  Greases 8vo,  *$  oo 

Soaps    , 8vo,  *6  oo 

Hurst,  G.  H.,  and  Simmons,  W.  H.     Textile  Soaps  and  Oils 8vo,  3  50 

Hurst,  H.  E.t  and  Lattey,  R.  T.     Text-book  of  Physics 8vo,  *3  oo 

Also  published  in  three  parts. 

Part      I.    Dynamics  and  Heat i  50 

Part    II.     Sound   and   Light ,  150 

Part  in.    Magnetism  and  Electricity *i  50 

Hutchinson,  R.  W.,  Jr.    Long  Distance  Electric  Power  Transmission. 

i2mo,  *3  oo 

Hutchinson,  R.  W.,  Jr.,  and  Thomas,  W.  A.    Electricity  in  Mining.  i2mo. 

(In  Press.) 

Hyde,  E.  W.     Skew  Arches i6mo.  o  75 

Hyde,  F.  S.    Solvents,  Oils,  Gums,  Waxes 8vo,  *2  oo 

Induction  Coils i6mo.  o  75 

Ingharn,  A.  E.    Gearing.    A  practical  treatise 8vo,  *2  50 

Ingle,  H.     Manual  of  Agricultural  Chemistry 8vo    (In  Press.} 

Inness,  C.  H.    Problems  in  Machine  Design i2mo,  *3  oo 

—  Centrifugal  Pumps i2mo,  *3  oo 

The  Fan  ...,,, i2mo,  *4  oo 

Jacob,  A.,  and  Gould,  E.  S.    On  the  Designing  and  Construction  of 

Storage   Reservoirs    i6mo.  o  75 

Jacobs,  F.  B.    Cam  Design  and  Manufacture (  In  Press.) 


I4       D.  VAN  NOSTRAND  CO.'S  SHORT  TITLE  CATALOG 

James,  F.  D.     Controllers  for  Electric  Motors 8vo.  *  oo 

Jehl,  F.     Manufacture  of  Carbons 8vo.  5  oo 

Jennings,  A.  S.     Commercial  Paints  and  Painting 8vo.  2  so 

Jennison,  F.  H.    The  Manufacture  of  Lake  Pigments.  .8vo  (In  Press.) 

Jepson,  G.    Cams  and  the  Principles  of  their  Construction 8vo,  *i  50 

Mechanical  Drawing 8vo  (In  Preparation.) 

Jervis-Smith,   F.  J.     Dynamometers 8vo.  4  oo 

Jockin,  W.    Arithmetic  of  the  Gold  and  Silversmith 12010,  *i  oo 

Johnson,  C.  H.,  and  Earle,  R.  P.     Practical  Tests  for  the  Electrical 

Laboratory  (  /;/  Press.) 

Johnson,  J.  H.    Arc  Lamps  and  Accessory  Apparatus i2mo,  o  75 

Johnson,  T.  M.     Ship  Wiring  and  Fitting i2mo   (Reprinting.)' 

Johnston,  J.  F.  W.,  and  Cameron,  C.    Elements  of  Agricultural  Chemistry 

and  Geology iimo,  2  60 

Joly,  J.    Radioactivity  and  Geology i2mo   (Reprinting.) 

Jones,  H.  C.    Electrical  Nature  of  Matter  and  Radioactivity i2mo,  *2  oo 

Nature  of  Solution 8vo,  *3  50 

New  Era  in  Chemistry i2mo,  *2  oo 

Jones,  J.  H.    Tinplate  Industry 8vo,  *s  oo 

Jones,  M.  W.    Testing  Raw  Materials  Used  in  Paint i2mo,  *2  50 

Jordan,  L.  C.    Practical  Railway  Spiral i2mo,  leather,  *i  50 

Juptner,  H.  F.  V.    Siderclogy:  The  Science  of  Iron 8vo,  *s  oo 

Kapp,   G.     Alternate    Current    Machinery i6mo,  o  75 

Kapper,  F.     Overhead  Transmission  Lines. 4to,  ^400 

Keim,  A.  W.    Prevention  of  Dampness  in  Buildings 8vo,  *2  50 

Keller,  S.  S.,  and  Knox,  W.  E.    Analytical  Geometry  and  Calculus. ..  2  oo 
Kemble,  W.  T.,  and  Underbill,  C.  R.    The  Periodic  Law  and  the  Hydrogen 

Spectrum 8vo,  paper,  *o  50 

Kemp,  J.  F.     Handbook  of  Rocks 8vo,  *i  50 

Kennedy,  A.  B.  W.,  and  Thurston,  R.  H.    Kinematics  of  Machinery. 

i6mo,  o  75 
Kennedy,  A.  B.  W.,  Unwin,  W.  C.,  and  Idell,  F.  E.     Compressed  Air. 

i6mo,  o  75 

Kennedy,  R.     Flying  Machines ;  Practice  and  Design i2mo,  2  50 

—  Principles  of  Aeroplane  Construction 8vo,  *2  oo 

Kent.  W.     Strength  of  Materials i6mo,  o  75 

Kershaw,  J.  B.  C.     Fuel,  Water  and  Gas  Analysis.  .8vo   (In  Press.) 

Electrometallurgy    8vo,  2  50 

Electro-Thermal  Methods   of  Iron  and  Steel  Production 8vo,  *3  oo 

Kinzbrunner,  C.    Continuous  Current  Armatures 8vo,  i  50 

-  Testing  of  Alternating  Current  Machines 8vo,  *2  oo 

Kinzer,  H.,  and  Walter,  K.    Theory  and  Practice  of  Damask  Weaving, 

8vo,  4  oo 
Kirkaldy,   A..   W.,    and   Evans,   A.    D.     History    and    Economics    of 

Transport 8vo,  *s  oo 

Kirkbride,  J.     Engraving  for  Illustration 8vo,  *i  oo 

Kirschke,  A.     Gas  and  Oil  Engines i2mo,  *i  50 


D   VAN  NOSTRAND  CO.'S  SHORT  TITLE  CATALOG  15 

Klein,  J.  F.     Design  of  a  High-speed  Steam-engine 8vo,  *5  oo 

Physical  Significance  of  Entropy 8vo,  *i  50 

Klingenberg,  G.     Large  Electric   Power  Stations 4to,  *5  oo 

Knight,  R.-Adm.  A.  M.     Modern  Seamanship 8vo,  *6  50 

Pocket   Edition i2mo,   f abrikoid,  3  oo 

Knott,  C.  G.,  and  Mackay,  J.  S.     Practical  Mathematics 8vo,  2  50 

Knox,  J.     Physico-Chemical  Calculations. i2mo,  i  50 

Fixation  of  Atmospheric  Nitrogen.  .  .7 i2mo,  i  oo 

Koester,  F.     Steam-Electric  Power  Plants 4to,  *5  oo 

Hydroelectric  Developments  and  Engineering 4to,  *5  oo 

Koller,   T.     The   Utilization   of   Waste   Products 8vo,  *5  oo 

—  Cosmetics    8vo,  *2  50 

Koppe,  S.  W.     Glycerine xarno,  *s  50 

Kozmin,    P.    A.     Flour    Milling 8vo,  750 

Krauch,   C.     Chemical   Reagents 8vo,  ^  oo 

Kremann,  R.     Application  of  the  Physico-Chemical  Theory  to  Tech- 
nical Process  and  Manufacturing  Methods 8vo,  3  oo 

Kretchmar,  K.     Yarn  and  Warp  Sizing 8vo,  *$  oo 

Laff argue,  A.     Attack  in  Trench  Warfare i6mo,  o  50 

Lallier,  E.  V.    Elementary  Manual  of  the  Steam  Engine i2mo,  *2  oo 

Lambert,  T.     Lead  and  Its  Compounds 8vo,  *3  50 

—  Bone    Products    and    Manures 8vo,  *3  50 

Lamborn,  L.  L.     Cottonseed  Products 8vo,  4  oo 

Modern  Soaps,  Candles,  and  Glycerin 8vo,  **j  50 

Lamprecht,  R.    Recovery  Work  After  Pit  Fires .8vo,  5  oo 

Lanchester,  F.  W.     Aerial  Flight.     Two  Volumes.     8vo. 

Vol.  I.     Aerodynamics *6  oo 

Vol.   II.     Aerodonetics *6  oo 

Lanchester,  F.  W.    The  Flying  Machine 8vo,  *3  oo 

Industrial   Engineering:    Present  and   Post- War  Outlook. . .  i2mo,  i  oo 

Lange,  K.  R,    By-Products  of  Coal-Gas  Manufacture xamo,  2  50 

La  Rue,  B.  F.     Swing  Bridges i6mo,  o  75 

Lassar-Cohn,  Dr.     Modern  Scientific   Chemistry i2mo,  2  25 

Latimer,  L.  H.,  Field,  C.  J.,  ,and  Howell,  J.  W.    Incandescent  Electric 

Lighting    i6mo,  o  75 

Latta,  M.  N.     Handbook  of  American  Gas-Engineering  Practice.  .8vo,  5  oo 

American  Producer  Gas  Practice 4to,  *6  oo 

Laws,  B.  C.     Stability  and  Equilibrium  of  Floating  Bodies 8vo,  4  50 

Law&on,    W.    R.      British    Railways.      A    Financial    and    Commercial 

Survey 8vo,  200 

Leask,  A.  R.     Refrigerating  Machinery i2mo    (Reprinting.) 

Lecky,  S.  T.  S.    "Wrinkles"  in  Practical  Navigation 8vo,  10  oo 

—  Pocket   Edition    i2mo,  5  oo 

—  Danger   Angle i6mo,  2  50 

Le  Doux,  M.     Ice-Making  Machines i6mo,  o  7$ 

Leeds,  C.  C.    Mechanical  Drawing  for  Trade  Schools oblong  4to,  2  25 

Mechanical   Drawing  for  High   and  Vocational   Schools 4to,  i  50 

Principles    of    Engineering   Drawing 8vo    (In  'Press.) 

Lefevre,    L,     Architectural   Pottery 4to,  7  oc 

Lehner,  S,    Ink  Manufacture 8vo,  2  50 

Lemstrom,  S.    Electricity  in  Agriculture  and  Horticulture 8vo,  *i  50 

Letts,  E.  A.     Fundamental  Problems  in  Chemistry 8vo,  *2  oo 

Le   Van,  W.  B.     Steam-Engine  Indicator i6mo,  o  7$ 


!6        D.  VAX   XOSTRAXD  CO.'S  SHORT   ^ITLE  CATALOG 

Lewes,  V.  B.    Liquid  and  Gaseous  Fuels Svo,      3  oo 

—  Carbonization   of    Coal 8vo,     :  5  oo 

Lewis  Automatic  Machine  Rifle  ;   Operation  of i6mo,     *o  Go 

Licks,  H.  E.     Recreations  in  Mathematics i2mo,      i  50 

Lieber,  B.  F.     Lieber's  Five  Letter  American  Telegraphic  Code  .8vo,  ^15  oo 
. Spanish    Edition    3vo,  ^15  oo 

—  French   Edition 8vo,  "15  oo 

—  Terminal  Index 8vo,     *2  50 

—  Lieber's  Appendix folio,  *i5  oo 

—  Handy  Tables 4to,  *2  50 

Bankers  and  Stockbrokers'  Code  and  Merchants  and  Shippers' 

Blank  Tables 8vo,  *i$  oo 

—  100,000,000  Combination  Code .8vo,  *io  oo 

Livermore,  V.  P.,  and  Williams,  J.    How  to  Become  a  Competent  Motor- 
man  i2mo,  *i  oo 

Livingstone,  R.     Design  and   Construction   of   Commutators 8vo,  450 

—  Mechanical  Design  and  Construction  of  Generators 8vo,  4  50 

Lloyd,  S.   L.     Fertilizer  Materials i-zmo,  2  oo 

Lockwood,  T.  D.    Electricity;  Magnetism,  and  Electro-telegraph.   ....  STO,  2  50 

—  Electrical  Measurement  and  the  Galvanometer i2mo,  o  75 

Lodge,  O.  J.  Elementary  Mechanics i2mo,  i  50 

Loewenstein,  L.  C.,  and  Crissey,  C.  P.     Centrifugal  Pumps.. 5  oo 

Lomax,  J.  W.     Cotton  Spinning 12010,  i  50 

Lord,  R.  T.     Decorative  and  Fancy  Fabrics Svo,  *3  50 

Loring,  A.  E.    A  Handbook  of  the  Electromagnetic  Telegraph.  . .  i6mo,  o  75 

Lowy,  A.     Organic  Type  Formulas o  10 

Lubschez,  B.  J-    Perspective 12010,  *i  50 

Lucke,  C.  E.    Gas  Engine  Design Svo,  *?.  oo 

-  —  Power  Plants:   Design,  Efficiency,  and  Power  Costs.     2  vols. 

(In  Preparation.) 
Luckiesh,   M.     Color   and   Its    Application Svo,      3  50 

—  Light  and  Shade  and  Their  Applications 8vo,      3  oo 

—  Visual   Illusions (In    Preparation. ) 

Lunge,  G.    Coal-tar  and  Ammonia.     Three  Volumes .8vo,  *25  oo 

—  Technical  Gas  Analysis Svo,    *4  $& 

Manufacture  of  Sulphuric  Acid  and  Alkali.     Four  Volumes 8vo, 

Vol.    I.     Sulphuric  Acid.     In  three  parts (Reprinting.) 

Vol.  I.     Supplement   Svo   (Reprinting.) 

Vol.  II.    Salt  Cake,  Hydrochloric  Acid  and  Leblanc  Soda.    In  two 

parts (In    Press. ) 

Vol.  III.    Ammonia  Soda (In  Press.) 

Vol.  IV.     Electrolytic  Methods (In  Press.) 

—  Technical  Chemists'  Handbook tamo,  leather,    *4  oo 

—  Technical  Methods  of  Chemical  Analysis. 

Vol.   I.      In  two  parts Svo,  *i$  oo 

Vol.  II.     In  two  parts , 8vo,  *i8  oo 

Vol.  III.     In  two  parts Svo,  *i8  oo 

The  set   (3  vols.)   complete *5o  oo 

Luquer,  L.  M.     Minerals  in  Rock  Sections  ..  .  .8vo,     *i  5» 


D.  VAN  NOSTRAND  CO.'S  SHORT  TITLE  CATALOG  17 

MacBride,  J.  D.     A  Handbook  of  Practical  Shipbuilding, 

i2mo,  fabrikoid,  2  oo 

Macewen,  H.  A.    Food  Inspection 8vo,  *2  50 

Mackenzie,  N.  F.     Notes  on  Irrigation  Works 8vo,  *2  50 

Mackie,  J.     How  to  Make  a  Woolen  Mill  Pay 8vo,  *2  oo 

Maguire,  Wm.  R.    Domestic  Sanitary  Drainage  and  Plumbing  ....  8vo,  4  oo 

Malcolm,  H.  W.     Submarine  Telegraph  Cable 9  oo 

Malinovzsky,    A.      Analysis    of    Ceramic    Materials    and    Methods    of 

Calculation (In  Press.} 

Mallet,  A.    Compound  Engines i6mo, 

Mansfield,   A.    N.     Electro-magnets i6mo,  o  75 

Marks,  E.  C.  R.    Construction  of  Cranes  and  Lifting  Machinery. i2mo,  *2  75 
Manufacture  of  Iron  and  Steel  Tubes i2mo,  2  50 

—  Mechanic*!  Engineering  Materials 12010,  *i  50 

Marks,  G.  C.     Hydraulic  Power  Engineering 8vo,  4  50 

Marlow,  T.  G.    Drying  Machinery  and  Practice. ..  .8vo   (Reprinting.) 

Marsh,  C.  F.     Concise  Treatise  on  Reinforced  Concrete  8vo,  *2  50 

Reinforced  Concrete  Compression  Member  Diagram.     Mounted  on 

Cloth  Boards *i  .50 

Marsh,  C.  F.,  and  Dunn,  W.     Manual  of  Reinforced  Concrete  and  Con- 
crete  Block   Construction i6mo,  cloth,  2  oo 

Marshall,  W.  J.,  and  Sankey,  H.  R.     Gas  Engines 8vo,  2  oo 

Martin,  G.     Triumphs  and  Wonders  of  Modern  Chemistry 8vo,  *3  oo 

—  Modern   Chemistry    and    Its    Wonders 8vo,  *s  oo 

Martin,  N.    Properties  and  Design  of  Reinforced  Concrete 8vo,  i  50 

Martin,  W.  D,     Hints  to   Engineers i2mo,  2  oo 

Massie,  W.  W.,  and  Underbill,  C.  R.    Wireless  Telegraphy  and  Telephony. 

i2mo,  *i  oo 

Mathot,  R.  E.     Internal  Combustion  Engines 8vo,  5  oo 

Maurice,  W.    Electric  Blasting  Apparatus  and  Explosives 8vo,  *3  50 

Shot  Firer*s  Guide 8vo,  *i  50 

Maxwell,  F.     Sulphitation  in  White  Sugar  Manufacture i2mo,  4  oo 

Maxwell,  J.  C.     Matter  and  Motion i6mo,  o  75 

Maxwell,  W.  H.,  and  Brown,  J.  T.    Encyclopedia  of  Muni.ipal  and  Sani- 
tary Engineering 4to,  *io  oo 

Mayer,  A.  M.    Lecture  Notes  on  Physics 8vo,  2  oo 

McCracken,  E.  M.,  and  Sampson,  C.  H.     Course  in  Pattern  Making. 

(In  Press.) 

McCullough,  E.     Practical  Surveying i2mo,  2  50 

McCullough,  R.  S.     Mechanical  Theory  of  Heat 8vo,  3  50 

McGibbon,  W.  C.    Indicator  Diagrams  for  Marine  Engineers 8vo,  "3  50 

—  Marine  Engineers'  Drawing  Book oblong  4to,  *2  50 

McGibbon,  W.  C.     Marine  Engineers  Pocketbook i2mo,  *4  50 

Mclntosh,   J.    G.      Technology    of    Sugar 8vo,  *6  oo 

—  Industrial    Alcohol     ; 8vo,  *3  50 

Manufacture  of  Varnishes  and  Kindred  Industries.     Three  Volumes. 

8vo. 

Vol.     I.     Oil  Crushing,  Refining  and  Boiling 7  oo 

Vol.  II.    Varnish  Materials  and  Oil  Varnish  Making.  (Reprinting.) 

Vol.  III.     Spirit  Varnishes  and  Materials (Reprinting.) 

McKay,  C.  W.     Fundamental   Principles   of  the  Telephone  Business. 

8vo.   (In  Press.) 


i8       D.  VAN  NOSTRAND  CO.'S  SHORT  TITLE  CATALOG 

McKillop,  M.,  and  McKillop,  A.  D.     Efficiency  Methods i2mo,  i  50 

UcKnight,  J.  D.,  and  Brown,  A.  W.     Marine  Multitubular  Boilers....  *2  50 

McMaster,  J.  B.     Bridge  and  Tunnel  Centres i6mo,  o  75 

McMechen,  F.  L.     Tests  for  Ores,  Minerals  and  Metals i2mo,  *i  co 

McNair,  Jas.  B.     Citrus  By-Products : (hi    press.) 

Meade,  A.     Modern   Gas   Works   Practice 8vo,  *8  50 

Melick,  C.  W.     Dairy  Laboratory  Guide 12010,  *i  25 

"Mentor."     Self-Instruction  for  Students  in  Gas  Supply.     i2mo. 

Elementary    2  50 

Advanced    2  50 

- — Self-Instruction   for   Students   in   Gas    Engineering.      i2mo. 

Elementary    2  oo 

Advanced   2  oo 

Merivale,  J.  H.     Notes  and  Formulae  for  Mining  Students i2mo,  i  oo 

Merritt,  Wm.  H.    Field  Testing  for  Gold  and  Silver i6mo,  leather,  2  oo 

Mertens.     Tactics  and  Technique  of  River  Crossings 8vo,  2  50 

Mierzinski,  S.     Waterproofing  of  Fabrics 8vo,  2  50 

Miessner,  B.  F.    Radio  Dynamics i2mo,  *2  oo 

Miller,  G.  A.     Determinants . .  i6mo, 

Miller,  W.  J.     Introduction  to  Historical  Geology i2mo,  2  25 

Milrpy,  M.  E.  W.     Home  Lace-making i2mo,  *i  oo 

Mills,  C.  N.    Elementary  Mechanics  for  Engineers 8vo,  *i  oo 

Mitchell,  C.  A.     Mineral  and  Aerated  Waters 8vo,  *3  oo 

Mitchell,  C.  A.,  and  Prideaux,  R.  M.    Fibres  Used  in  Textile  and  Allied 

Industries .'../ ...8vo,  3  50 

Mitchell,  C.  F.,  and  G.  A.    Building  Construction  and  Drawing.     i2mo. 

Elementary  Course    2  oo 

Advanced   Course 3  oo 

Monckton,   C.    C.   F.     Radiotelegraphy 8vo,  200 

Monteverde,  R.  D.     Vest  Pocket  Glossary  of  English-Spanish,  Spanish- 
English  Technical  Terms 64mo,  leather,  *i  oo 

Montgomery,  J.  H.     Electric  Wiring  Specifications i6mo,  *i  oo 

Moore,  E.  C.  S.    New  Tables  for  the  Complete  Solution  of  Ganguillet  and 

Kutter's   Formula    8vo,  *6  oo 

Moore,  Harold.     Liquid  Fuel  for  Internal  Combustion  Engines.  .  .8vo,  5  oo 
Morecroft,  J.  H.,  and  Hehre,  F.  W.     Short  Course  in  Electrical  Testing. 

8vo,  i  75 

Morgan,  A.  P.    Wireless  Telegraph  Apparatus  for  Amateurs I2mo,  *i  50 

Morrell,  R.  S.,  and  Waele,  A.  E.     Rubber,  Resins,  Paints  and  Var- 
nishes     8vo    (In    Press.) 

Moses,  A.  J.    The  Characters  of  Crystals 8vo,  *2  oo 

—  and  Parsons,  C.  L.     Elements  of  Mineralogy 8vo,  *3  50 

Moss,  S.  A.     Elements  of  Gas  Engine  Design i6mo,  o  75 

— -The    Lay-out   of    Corliss   Valve    Gears i6mo,  o  75 

Mulford,  A.  C.    Boundaries  and  Landmarks i2mo,  *i  oo 

Mulford,  A.  C.     Boundaries  and   Landmarks 12010,  i  oo 

Munby,  A.  E.     Chemistry  and  Physics  of  Building  Materials.  ..  .8vo,  2  50 

Murphy,  J.  G.    Practical  Mining i6mo,  i  oo 

Murray,  B.  M.    Chemical  Reagents 8vo  (  In  Press.) 

Murray,  J.   A.     Soils   and   Manures 8vo,  200 

Nasmith,  J.     The  Student's  Cotton  Spinning 8vo,  4  50 

Recent  Cotton   Mill  Construction i2mo,  3  oo 


D.  VAN  NOSTRAND  CO.'S  SHORT  TITLE  CATALOG  19 

tieave,  G.  B.,  and  Heilbron,  I.  M.     Identification  of  Organic  Compounds. 

i2mo,  i  50 

Neilson,  R.  M.    Aeroplane  Patents 8vo,  *2  oo 

Kerz,    F.     Searchlights 8vo    (Reprinting.) 

Newbigin,  M.  I.,  and  Flett,  J.  S.     James  Geikie,  the  Man  and  the 

Geologist 8vo,  3  50 

Newbiging,  T.     Handbook  for  Gas  Engineers  and  Managers 8vo,  7  50 

Newell,  F.  H.,  and  Drayer,  C.  E.    Engineering  as  a  Career.  .i2mo,  cloth,  *i  oo 

Nicol,  G.     Ship  Construction  and  Calculations 8vo,  *io  oo 

Nipher,  F.  E.     Theory  of  Magnetic  Measurements i2mo,  i  oo 

Nisbet,  H.    Grammar  of  Textile  Design 8vo,  7  50 

Nolan,    H.      The    Telescope i6mo,  o  75 

Norie,  J.  W.    Epitome  of  Navigation  (2  Vols.) octavo,  15  oo 

—  A  Complete  Set  of  Nautical  Tables  with  Explanations  of  Their 

Use    octavo,  6  50 

North,  H.  B.   Laboratory  Experiments  in  General  Chemistry 12010,  *i  oo 

<^ 

O'Connor,  H.     The   Gas  Engineer's   Pocketbook i2mo,   leather,  400 

Ohm,  G.  S.,  and  Lockwood,  T.  D.     Galvanic  Circuit i6mo,  o  75 

Olsen,  J.  C.     Text-book  of  Quantitative  Chemical  Analysis 8vo,  400 

Ormsby,  M.  T.  M.     Surveying i2mo,  2  oo 

Oudin,  M.  A.    Standard  Polyphase  Apparatus  and  Systems 8vo,  *3  oo 

Pakes,  W.  C.  C.,  and  Nankivell,  A.  T.    The  Science  of  Hygiene  .  .8vo,  *i  75 

Palaz,  A.     Industrial   Photometry -. 8vo,  4  oo 

Palmer,  A.  R.     Electrical  Experiments i2mo,  o  75 

—  Magnetic  Measurements  and  Experiments i2mo,  o  75 

Pamely,  C.     Colliery  Manager's  Handbook 8vo,  *io  oo 

Parker,  P.  A.  M.     The   Control   of   Water 8vo,  600 

Parr,  G.  D.  A.     Electrical  Engineering  Measuring  Instruments. ..  .8vo,  *3  50 
Parry,  E.  J,    Chemistry  of  Essential  Oils  and  Artificial  Perfumes. 

Vol.  I.     Monographs    on    Essential    Oils 9  oo 

Vol.  II.     Constituents  of  Essential  Oils,  Analysis 7  oo 

Foods  and  Drugs.     Two  Volumes. 

Vol.    I.    The   Analysis   of    Food   and    Drugs 8vo,  950 

Vol.  II.     The  Sale   of  Food  and   Drugs  Acts 8vo,  3  50 

—  and  Coste,  J.  H.    Chemistry  of  Pigments .8vo,  *5  oo 

Parry,  L.     Notes  on  Alloys 8vo,  *s  50 

—  Metalliferous  Wastes   8vo,  *2  50 

—  Analysis  of  Ashes  and  Alloys 8vo,  *2  50 

Parry,  L.  A.     Risk  and  Dangers  of  Various  Occupations 8vo,  *3  50 

Parshall,  H.  F.,  and  Hobart,  H.  M.    Electric  Railway  Engineering .  4to,  7  50 

Parsons,  J.  L.     Land  Drainage 8vo,  *i  50 

Parsons,  S.  J.  Malleable  Cast  Iron 8vo   (Reprinting.) 

Partington,  J.  R.     Higher  Mathematics  for  Chemical  Students.  .i2mo,  2  50 
Textbook  of  Thermodynamics 8vo,  *4  oo 

—  The    Alkali    Industry 8vo,  3  oo 

Patchell,  W.  H.     Electric  Power  in  Mines 8vo,  *4  oo 

Paterson,  G.  W.  L.    Wiring  Calculations i2mo,  *2  50 

—  Electric  Mine  Signalling  Installations i2mo,  *i  50 

Patterson,  D.     The  Color  Printing  of  Carpet  Yarns 8vo,  *3  50 

Color   Matching    on   Textiles 8vo,  *3  50 

Textile   Color   Mixing 8vo,  *3  50 


20       D.  VAN  NOSTRANt)  CO.'S  SHORT  TITLE  CATALOG 

Paulding,  C.  P.     Condensation  of  Steam  in  Covered  and  Bare  Pipes.   8vo,  *2  oo 

-  Transmission  of  Heat  through  Cold-storage  Insulation i2mo,  *i  oo 

Payne,    D.    W.      Iron    Founders'    Manual 8vo,  4  oo 

Peddle,  R.  A.    Engineering  and  Metallurgical  Books 12010,  *i  50 

Peirce,  B.     System  of  Analytic  Mechanics 4to,  10  oo 

—  Linear   Associative   Algebra 4to,  2  50 

Perkin,  F.  M.,  and  Jaggers,  E.  M.     Elementary  Chemistry.    ...i2mo,  i  co 

Perrin,  J.    Atoms 8vo,  *2  50 

Perrine,  F.  A.  C.     Conductors  for  Electrical  Distribution 8vo,  *3  50 

Petit,  G.     White  Lead  and  Zinc  White  Paints. 8vo,  *2  oo 

Petit,  R.     How  to  Build   an  Aeroplane 8vo,  i  50 

Pettit,    Lieut.   J.    S.     Graphic  Processes i6mo,  075 

Philbrick,   P.   H.     Beams   and   Girders '. i6mo, 

Phin,  J.     Seven  Follies  of  Science : 12010,  *r  50 

Pickworth,  C.  N.    Logarithms  for  Beginners .i2mo,  boards,  i  oo 

—  The  Slide  Rule izmo,  i  50 

Pilcher,  R.  B.     The  Profession  of  Chemistry lamo    (In   Press.) 

Pilcher,  R.  B.,  and  Butler-Jones,  F.    What  Industry  Owes  to  Chemical 

Science tamo,  i  50 

Plattner's  Manual  of  Blow-pipe  Analysis.    Eighth  Edition,  revised.  8vo,  4  oo 

Plympton,  G.  W.    The  Aneroid  Barometer i6me,  o  75 

How   to   Become   an    Engineer x6oi«,  o  75 

Van  Nostrand's   Table   Book i6ano,  o  75 

Pochet,  M.  L.     Steam  Injectors i6mo,  o  75 

Pocket  Logarithms  to  Four  Places i6mo,  o  75 

i6mo,  leather,  i  oo 

Polleyn,  F.     Dressings  and  Finishings  for  Textile  Fabrics 8vo,  *3  50 

Pope,  F.  G.    Organic  Chemistry izmo,  2  50 

Pope,  F.  L.     Modern  Practice  of  the  Electric  Telegraph 8vo,  i  50 

Popplewell,  W.  C.     Prevention  of   Smoke 8v«,  *3  50 

Strength  of  Materials 8v«,  *2  50 

Porritt,  B.  D.     The  Chemistry   of  Rubber 12019,  i  oo 

Porter,  J.  R.    Helicopter  Flying  Machine . .   izrno,  i  50 

Potts,  H.  E.     Chemistry  of  the  Rubber  Industry 8vo,  2  50 

Practical  Compounding  of  Oils,  Tallows  and  Grease 8v»,  *3  50 

Pratt,  A.  E.    The  Iron  Industry 8vo  (hi  Press.) 

•  The  Steel  Industry 8vo    (In   Press.) 

Pratt,  Jas.  A.    Elementary  Machine  Shop  Practice (In  Press.) 

Pratt,  K.    Boiler  Draught 12010,  *i  25 

Prelini,  C.    Earth  and  Rock  Excavation 8vo,  *3  oo 

Graphical  Determination  of  Earth  Slopes 8vo,  *2  oo 

Tunneling.    New  Edition 8vo,  *3  oo 

Dredging.    A  Practical  Treatise 8vo,  *3  oo 

Prescott,  A.  B.,  and  Johnson,  0.  C.  Qualitative  Chemical  Analysis .  .  8vo,  4  oo 
Prescott,  A.  B.,  and  Sullivan,  E.  C.     First  Book  in  Qualitative  Chemistry. 

Prideaux,  E.  B.  R.     Problems  in  Physical  Chemistry 8vo,  *2  oo 

— —  The  Theory  and  Use  of  Indicators 8vo,  5  oo 

Prince,  G.  T.    Flow  of  Water iamo,  *2  oo 

Pull,  E.     Modern  Steam  Boilers 8vo,  5  oo 

Pullen,  W.  W.  F.     Application  of  Graphic  Methods  to  the  Design  of 

i2mo,  *i  50 

Structures    I2mo,  3  Oo 

-  Injectors:    Theory,   Construction   and  Working izmo,  *2  oo 

—  Indicator  Diagrams    8vo,  3  o-> 

—  Engine  Testing !ttf,  *5  50 


D.  VAN  NOSTRAND  CO.'S  SHORT  TITLE  CATALOG  21 

Purday,  H.  F.  P.     The  Diesel  Engine  Design 8vo   (In  Press.) 

Putsch,  A.     Gas  and  Coal-dust  Firing 8vo,  *2  50 

Rafter,  G.  W.    Mechanics  of  Ventilation i6mo,  o  75 

Potable  Water  i6mo,  o  75 

—  Treatment    of    Septic    Sewage i6mo,  .v  o  75 

—  and  Baker,  M.  N.    Sewage  Disposal  in  the  United  States.  ..  .4to,  6  oo 

Raikes,  H.  P.     Sewage  Disposal  Works 8vo,  *4  oo 

Randau,   P.     Enamels  and   Enamelling 8vo,  *s  oo 

Rankine,  W.  J.  M.,  and  Bamber,  E.  F.    A  Mechanical  Text-book.  .8vo,  4  oo 

—  Civil  Engineering  8vo.  7  50 

—  Machinery   and    Millwork 8vo,  6  oo 

-  The  Steam-engine  and  Other  Prime  Movers 8vo,  6  oo 

Rankine,  W.  J.  M.,  and  Bamber,  E.  F.     A  Mechanical  Text-book 8vo,  3  50 

Raphael,  F.  C.     Localization  of  Faults  in  Electric  Light  and  Power  Mains. 

8vo,  3  50 

Rasch,    E.     Electric   Arc    Phenomena 8vo,  2  oo 

Rathbone,  R.  L.  B.     Simple  Jewellery 8vo,  2  50 

Rausenberger,  F.     The  Theory  of  the  Recoil  Guns 8vo,  *5  oo 

Rautenstrauch,  W*  Notes  on  the  Elements  of  Machine  Design.  8 vo,  boards,  *i  50 
Rautenstrauch,  W.,  and  Williams,  J.  T.     Machine  Drafting  and  Empirical 
Design. 

Part  I.  Machine    Drafting 8vo,  i  50 

Part  II.  Empirical  Design (In  Preparation.) 

Raymond,  E.  B.     Alternating  Current  Engineering 12010,  *2  50 

Rayner,  H.     Silk  Throwing  and  Waste  Silk  Spinning 8vo, 

Recipes  for  the  Color,  Paint,  Varnish,  Oil,  Soap  and  Drysaltery  Trades, 

Svo,  *5  oo 

Recipes  for  Flint  Glass  Making i2mo,  *s  oo 

Redfern,  J.  B.,  and  Savin,  J.    Bells,  Telephones i6mo,  o  75 

Redgrove,  H.  S.     Experimental  Mensuration i2mo,  i  50 

Reed,  S.    Turbines  Applied  to  Marine  Propulsion *5  oo 

Reed's  Engineers'  Handbook Svo,  *g  oo 

— —  Key  to  the  Nineteenth  Edition  of  Reed's  Engineers'  Handbook.  .8vo,  4  oo 

Useful  Hints  to  Sea-going  Engineers i2mo,  3  oo 

Reid,  E.  E.    Introduction  to  Research  in  Organic  Chemistry.  (In  Press.} 
Reinhardt,  C.  W.     Lettering  for  Draftsmen,  Engineers,  and  Students. 

oblong  410,  boards,  i  oo 
Reinhardt,  C.  W.   The  Technic  of  Mechanical  Drafting, 

oblong,  4to,  boards,  *i  oo 

"Reiser,  F.     Hardening  and  Tempering  of  Steel i2mo,  2  50 

Reiser,  !N.     Faults  in  the  Manufacture  of  Woolen  Goods Svo,  2  50 

—  Spinning   and  Weaving  Calculations Svo,  *$  oo 

Renwick,  W.  G.     Marble  and  Marble  Working Svo    (Reprinting.) 

tteuleaux,    F.     The    Constructor 4to,  400 

Rey,  Jean.     The  Range  of  Electric  Searchlight  Projectors Svo, 

(Reprinting.} 

Reynolds,  ©.,  and  Idell,  F.  E.    Triple  Expansion  Engines i6mo,  o  75 

Rhead,  G.  F.     Simple  Structural  Woodwork i2mo,  *i  25 

Rhead,  G.  W.     British  Pottery  Marks Svo,  3  50 

Rhodes,  H.  J.     Art  of  Lithography Svo,  5  oo 

Rice,  J.  M.,  and  Johnson,  W.  W.     A  New  Method  of  Obtaining  the  Differ- 
ential of  Functions i2mo,  o  50 


22       D.  VAN  NOSTRAND  CO.'S  SHORT  TITLE  CATALOG 

Richards,  W.  A.    Forging  of  Iron  and  Steel i2mo,  2  oo 

Richards,  W.  A.,  and  North,  H.  B.    Manual  of  Cement  Testing. . . .  i2mo,  *i  50 

Richardson,  J.     The  Modern  Steam  Engine 8vo,  *3  50 

Richardson,  S.  S.     Magnetism  and  Electricity i2mo,  *2  oo 

Rideal,   E.    K.     Industrial    Electrometallurgy 8vo,  3  oo 

—  The  Rare  Earths  and  Metals 8vo    (In  Press.) 

Rideal,  S.     Glue  and  Glue  Testing 8vo,  *s  oo 

—  The    Carbohydrates 8vo    (In    Press.) 

Riesenberg,  F.    The  Men  on  Deck i2mo,  3  oo 

—  Standard  Seamanship  for  the  Merchant  Marine.  i2mo  (In  Press.) 

Rimmer,  E.  J.    Boiler  Explosions,  Collapses  and  Mishaps 8vo,  *i  75 

Rings,  F.     Reinforced  Concrete  in  Theory  and  Practice i2mo,  *4  50 

Reinforced  Concrete  Bridges 4to,  *$  oo 

Ripper,  W.     Course  of  Instruction  in  Machine  Drawing folio,  *6  oo 

Roberts,  F.  C.    Figure  of  the  Earth i6mo,  o  75 

Roberts,  J.,  Jr.     Laboratory  Work  in  Electrical  Engineering 8vo,  *2  oo 

Robertson,  L.  S.    Water-tube  Boilers 8vo,  2  oo 

Robinson,  J.  B.     Architectural  Composition 8vo,  *2  50 

Robinson,  S.  W.     Practical  Treatise  on  the  Teeth  of  Wheels.  .i6mo,  o  75 

—  Railroad   Economics    i6mo,  o  75 

—  Wrought  Iron  Bridge  Members i6mo,  o  75 

Robson,  J.  H.     Machine  Drawing  and  Sketching 8vo,  *2  oo 

Roebling,  J.  A.    Long  and  Short  Span  Railway  Bridges folio,  25  oo 

Rogers,  A.     A  Laboratory  Guide  of  Industrial  Chemistry 8vo,  2  oo 

• Elements    of   Industrial    Chemistry i2mo,  *3  oo 

Manual  of  Industrial  Chemistry 8vo,  *s  oo 

Rogers,  F.     Magnetism  of  Iron  Vessels i6mo,  o  75 

Rohland,  P.     Colloidal  and  Crystalloidal  State  of  Matter i2mo, 

(Reprinting.) 

Rollinson,  C.     Alphabets Oblong,  i2mo,  *i  oo 

Rose,  J.    The  Pattern-makers'  Assistant 8vo,  2  50 

• Key  to  Engines  and  Engine-running i2mo,  2  50 

Rose,  T.  K.     The  Precious  Metals 8vo,  2  50 

Rosenhain,    W.      Glass    Manufacture 8vo»,  5  oo 

—  Physical.  Metallurgy,  An  Introduction  to 8vo,  4  oo 

Roth,   W.   A.     Physical   Chemistry 8vo,  *2  oo 

Rowan,  F.  J.    Practical  Physics  of  the  Modern  Steam-boiler 8vo,  *3  oo 

—  and  Idell,  F.  E.     Boiler  Incrustation  and  Corrosion i6mo,  o  75 

Roxburgh,   W.     General   Foundry   Practice 8vo,  2  50 

Ruhmer,    E.      Wireless    Telephony 8vo,  4  50 

Russell,  A.     Theory  of  Electric  Cables  and  Networks 8vo,  *3  oo 

Rust,  A.     Practical  Tables  for  Navigators  and  Aviators 8vo,  3  50 

Rutley,   F.     Elements   of  Mineralogy i2mo,  i  50 

Sandeman,  E.  A.    Notes  on  the  Manufacture  of  Earthenware.  ..i2mo,  3  50 

Sanford,  P.  G.    Nitro-explosives 8vo,  *4  oo 

Saunders,  C.   H.     Handbook   of   Practical    Mechanics i6mo,  i  50 

leather,  2  oo 

Sayers,  H.  M.    Brakes  for  Tram  Cars 8vo,  *i  25 

Schaefer,   C.   T.     Motor   Truck   Design 8vo,  250 

Scheele,  C.  W.     Chemical  Essays 8vo,  *2  50 

Scheithauer,  W.     Shale  Oils  and  Tars 8vo,  *4  oo 


D.  VAN  NOSTRAND  CO.'S  SHORT  TITLE  CATALOG       23 

Scherer,  jR.     Casein , M '. 8vo,  3  50 

Schidrowitz,  P.    Rubber,  Its  Production  and  Industrial  Uses Svo,  *6  oo 

Schindler,  K.     Iron  and  Steel  Construction  Works izmo,  *2  oo 

Schmall,  C.  N.    First  Course  in  Analytic  Geometry,  Plane  and  Solid. 

i2mo,  half  leather,  *i  75 

and  Shack,  S.  M,     Elements  of  Plane  Geometry xamo,  i  25 

Schwarz,  E.  H.  L.     Causal  Geology Svo,  *3  oo 

Schmeer,  L.     Flow   of   Water 8vo,  150 

Schweizer,  V.    Distillations  of  Resins Svo,  5  oo 

Scott,  A.  H.     Reinforced  Concrete  in  Practice !2mo,  2  oo 

Scott,   W.   W.     Qualitative   Analysis.     A  Laboratory  Manual.     New 

Edition    3  oo 

Standard   Methods   of   Chemical   Analysis Svo,  *6  oo 

Scribner,  J.  M.    Engineers'  and  Mechanics'  Companion.  .i6mo,  leather,  i  50 
Scudder,   H.     Electrical    Conductivity   and   lonization   Constants   of 

Organic  Compounds Svo,  *3  oo 

Seamanship,  Lectures  on i2mo,  2  oo 

Searle,  A.  B.    Modern  Brickmaking Svo  (In  Press,) 

Cement,    Concrete    and    Bricks , .Svo,  3  oo 

Searle,    G.    M.      "Sumners'    Method."      Condensed    and    Improved. 

iGmo,  o  75 

Seaton,  A.  E.    Manual  of  Marine  Engineering Svo,  10  oo 

Seaton,  A.  E.,  and  Rounthwaite,  H.  M.    Pocket-book  of  Marine  Engi- 
neering  i6mo,  leather,  5  oo 

SeeJigmann,  T.,  Torrilhon,  G.  L.,  and  Falconnet,  H.    India  Rubber  and 

Gutta  Percha    Svo,  6  oo 

Seidell,  A.     Solubilities  of  Inorganic  and  Organic  Substances ....  Svo,  7  50 

Sellew,  W.  H.     Steel   Rails 4to,  *io  oo 

Railway  Maintenance  Engineering i2mo,  3  oo 

Senter,  G.     Outlines  of  Physical  Chemistry i2mo,  *2  50 

Text-book  of  Inorganic  Chemistry i2mo,  *3  oo 

Sever,  G.  F.    Electric  Engineering  Experiments Svo,  beards,  *i  oo 

Sever,  G.  F.,  and  Townsend,  F.    Laboratory  and  Factory  Tests  in  Elec- 
trical Engineering Svo,  *2  50 

Sewall,  C.  H.    Wireless  Telegraphy Svo,  *2  oo 

Lessons  in  Telegraphy i2mo,  *i  oo 

Sexton,  A.  H.    Fuel  and  Refractory  Materials i2mo  (Reprinting.) 

-Chemistry  of  the  Materials  of  Engineering ismo,  *3  oo 

Alloys  (Nan-Ferrous) Svo,  3  50 

Sexton,  A.  H.,  and  Primrose,  J.  S.  G.  The  Metallurgy  of  Iron  and  Steel. 

Svo,  *6  50 

Seymour,  A.     Modern   Printing  Inks Svo,  3  oo 

Shaw,  Henry  S.  H.     Mechanical  Integrators i6mo,  o  75 

Shaw,  S.     History  of  the  Staffordshire  Potteries Svo,  2  50 

Chemistry  of  Compounds  Used  in  Porcelain  Manufacture. ..  .Svo,  *6  oo 

Shaw,   T.   R.     Driving    of    Machine   Tools i2mo,  *2  oo 

Precision    Grinding    Machines i2mo,  5  oo 

Shaw,   W.   N.     Forecasting   Weather Svo    (Reprinting.) 

Sheldon,   S.,  and  Hausmann,   E.     Dynamo   Electric   Machinery,  A.C. 

and  D.C Svo   (In  Press.) 

1  Electric  Traction  and  Transmission  Engineering .i2mo,  2  50 

—  Physical  Laboratory  Experiments,  for  Engineering  Students.  .Svo,  *i  25 


24       D.  VAN  NOSTRAND  CO.'S  SHORT  TITLE  CATALOG 

Sherriff,  F.  F.    Oil  Merchants'  Manual  and  Oil  Trade  Ready  Reckoner, 

Svo,      3  50 

Shields,  J.  E.     Notes  on  Engineering  Construction i2mo,      i  50 

Shreve,  S.  H.    Strength  of  Bridges  and  Roofs 8vo,      3  50 

Shunk,  W.  F.    The  Field  Engineer i2mo,  fabrikoid,      2  50 

Silverman,  A.,  and  Harvey,  A.  W.     Laboratory  Directions  and  Study 

Questions  in  Inorganic   Chemistry 4to,  loose   leaf,      2  oo 

Simmons,  W.  H.     Fats,  Waxes  and  Essential  Oils.  .8vo   (In  Press.) 
Simmons,  W.  H.,  and  Appleton,  H.  A.    Handbook  of  Soap  Manufacture, 

3/0,    *4  oo 

Simmons,  W.  H.,  and  Mitchell,  C.  A.     Edible  Fats  and  Oils 8vo,    *3  50 

Simpson,  G.    The  Naval  Constructor i2mo,  fabrikoid,    *$  oo 

Simpson,  W.    Foundations , 8vo.   (In  Press.} 

Sinclair,  A.    Development  of  the  Locomotive  Engine. .  .8vo,  half  leather,      5  oo 

Sindall,  R.  W.    Manufacture  of  Paper 8vo  (Reprinting.) 

Sindall,  R.  W.,  and  Bacon,  W.  N.    The  Testing  of  Wood  Pulp 8vo, 

( Reprin  ting. ) 

Wood  and  Cellulose 8vo   (In  Press.) 

Sloane,  T.  O'C.    Elementary  Electrical  Calculations i2mo,     *2  oo 

Smallwood,  J.  C.    Mechanical  Laboratory  Methods.  ..  .  i2mo,  fabrikoid,      3  oo 

Smith,  C.  A.  M.    Handbook  of  Testing,  MATERIALS 8vo,  *2  50 

Smith,  C.  A.  M.,  and  Warren,  A.  G.     New  Steam  Tables 8vo,  *i  25 

Smith,  C.  F.     Practical  Alternating  Currents  ard  Testing 8vo,  *3  50 

Practical   Testing   of   Dynamos   and   Motors 8vo,  *3  oo 

Smith,  F.  E.     Handbook  of  General  Instruction  for  Mechanics .  .  .  izmo,       i  50 

Smith,  G.  C.     Trinitrotoluenes  and  Mono-  and  Dinitrotoluenes,  Their 

Manufacture  and   Properties i2mo,      2  oo 

Smith,  H.  G.    Minerals  and  the  Microscope i2mo,      2  oo 

Smith,  J.  C.     Manufacture  of  Paint 8vo,    *5  oo 

Smith,  R.  H.     Principles  of  Machine  Work i2mo, 

Advanced  Machine  Work i2mo,    *3  oo 

Smith,   W.     Chemistry   of   Hat   Manufacturing i2mo,    *3  50 

Snell,  F.  D.     Calorimetric  Analysis i2mo   (In   Press.} 

Snow,  W.  G.,  and  Nolan,  T.     Ventilation  of  Buildings i6mo,      o  75 

Soddy,  F.     Radioactivity 8vo    (Reprinting.) 

Solomon,  M.     Electric  Lamps 8vo,      2  oo 

Somerscales,  A.  N.     Mechanics  for  Marine  Engineers i2mo,      2  50 

Mechanical  and  Marine  Engineering  Science 8vo,    *$  oo 

Sothern,  J.  W.     The  Marine  Steam  Turbine Svo,  *i2  50 

Verbal  Notes  and  Sketches  for  Marine  Engineers Svo,  *i2  50 

—  Marine  Engine  Indicator  Cards Svo,      4  50 

Sothern,   J.    W.,    and    Sothern,    R.    M.     Simple   Problems   in   Marine 

Engineering  Design  i2mo, 

Souster,  E.  G.  W.    Design  of  Factory  and  Industrial  Buildings..  .8vo, 

Southcombe,  J.  E.     Chemistry  of  the  Oil  Industries Svo, 

Soxhlet,  D.  H.     Dyeing  and  Staining  Marble Svo, 

Spangenburg,  L.     Fatigue  of  Metals iGmo, 

Specht,  G.  J.,  Hardy,  A.  S.,  McMaster,  J.  B.,  and  Walling.   Topographical 

Surveying   i5mo, 

Spencer,  A.  S.     Design  of  Steel-Framed  Sheds Svo, 

Spiegel,  L.     Chemical  Constitution  and  Physiological  Action.  ..  .i2mo, 


D.  VAN  NOSTRAND  CO'.'S  SHORT  TITLE  CATALOG  25 

Sprague, .  E.  H.     Hydraulics i  amo,  2  co 

—  Elements   of   Graphic   Statics ; 8vo,  3  co 

— -—  Stability  of  Masonry i^rao,  2  oo 

—  Elementary  Mathematics  for  Engineers i2mo,  2  co 

—  Stability    of    Arches i?.mo,  2  oo 

—  Strength  of  Structural  Elements i2mo,  2  oo 

Moving  Loads  by  Influence  Lines  and  Other  Methods i2mo,  2  oo 

Stahl,  A.  W.     Transmission  of  Power i6mo, 

Stahl,  A.  W.,  aad  Woods,  A.  T.     Elementary  Mechanism i2mo,  *2  oo 

Standage,    H.    C.      LeatherworkersP    Manual 8vo,  *3  50 

—  Sealing  Waxes,  Wafers,  and   Other  Adhesives 8vo,  *2  50 

—  AgglHtiaants  of  All  Kinds  for  All  Purposes i2mo,  3  50 

Stanley,  H.    Practical  Applied  Physics (In  Press.) 

Stansbie,  J.  H.     Iron  and  Steel 8vo,  2  50 

Steadman,  F.  M.     Unit  Photography i2mo,  *2  oo 

Stecher,  G.  E.     Cork.    Its  Origin  and  Industrial  Uses i2mo,  i  oo 

Steinheil,  A.,  and  Voit,  E.     Applied  Optics*     Vols.  I.  and  II.     8vo, 

Each,  5  oo 

— .  Two    Volumes Set,  9  oo 

Steinman,  D.  B.     Suspension  Bridges  and  Cantilevers.     (Science  Series 

No.  127.)    o  75 


Stevens,  A.  B.     Arithmetric  of  Pharmacy i2mo,  i  50 

Stevens,  E.  J.     Field  Telephones  and  Telegraphs i  20 

Stevens,  H.  P.     Paper  Mill  Chemist i6mo,  4  oo 

Stevens,  J.  S.     Theory  of  Measurements i2mo,  *i  25 

Stevenson,  J.  L.    Blast-Furnace  Calculations i2mo,  leather,  2  50 

Stewart,  G.    Modern  Steam  Traps i2mo,  *i  75 

Stiles,  A.     Tables  for  Field  Engineers i2mo,  i  oo 

Stodola,  A.     Steam  Turbines 8vo,  5  oo 

Stone,  E.  W.    Elements  of  Radiotelegraphy i2mo,  fabrikoid,  2  50 

Stone,  H.     The  Timbers   of   Commerce Svo,  4  oo 

Stopes,  M.    The  Study  of  Plant  Life Svo,  2  oo 

Sudborough,  J.  J.,  and  James,  T.  C.   Practical  Organic  Chemistry ,.  lamo,  2  50 

Suf fling,  E.  R.     Treatise  on  the  Art  of  Glass   Painting Svo,  *3  50 

Sullivan,  T.  V.,  and  Underwood,  N.    Testing  and  Valuation  of  Build- 
ing and  Engineering  Materials (In  Press.) 

Sutherland,  D.  A.    The  Petroleum  Industry Svo   (In  Press.) 

Svenson,  C.  L.     Handbook  on  Piping Svo,  4  oo 

—  Essentials  «f  Drafting Svo,  i  75 

—  Mechanical  and  Machine  Drawing  and  Design (In  Press.) 

Swan,  K.    Patents,  Designs  and  Trade  Marks Svo,  2  oo 

Swinburne,  J.,  Wordingham,  C.  H.,  and  Martin,  T.  C.    Electric  Currents. 

i6mo,  o  75 

Swoope,  C.  W.    Lessons  in  Practical  Electricity i2mo,  *2  oo 

Tailfer,  L.     Bleaching  Linen  and  Cotton  Yarn  and  Fabrics 3vo,  7  co 

Tate,  J.  S.    Surcharged  and  Different  Forms  of  Retaining- walls.  .i6mo,  o  75 

Taylor,  F.  N.     Small  Water  Supplies i2mo,  *2  50 

—  Masonry  in  Civil  Engineering Svo,  *2  50 

Taylor,  W.  T.    Electric  Cable  Transmission  and  Calculation. (In  Press.) 

Calculation  of  Electric  Conductors 4to   (In  P,css.) 

Templeton,  W.    Practical  Mechanic's  Workshop  Companion. 

i2mo,  morocco,  a  oo 

Tenney,  E.  H.     Test  Methods  for  Steam  Power  Plants i2mo,  3  oo 

Terry,  H.  L.     India  Rubber  and  its  Manrfacture.  .8vo    (Reprinting.) 


26       D.  VAN  NOSTRAND  CO.'S  SHORT  TITLE  CATALOG 

Thayer,  H.  R.    Structural  Design.    8vo. 

Vol.     I.     Elements  of  Structural  Design 350 

Vol.   II.     Design  of  Simple  Structures 4  50 

Vol.  III.    Design  of  Advanced  Structures (In  Preparation.) 

Foundations  and  Masonry (In   Preparation.) 

Thiess,  J.  B.,  and  Joy,  G.  A.     Toll  Telephone  Practice 8vo,  *3  50 

Thorn,  C.,  and  Jones,  W.  H.    Telegraphic  Connections.. .  .oblong,  i2mo,  150 

Thomas,  C.  W.     Paper-makers'  Handbook . (In  Press.) 

Thomas,  J.  B.     Strength  of  Ships 8vo,  2  50 

Thomas,  Robt.   G.     Applied   Calculus ..izmo,  300 

Thompson,  A.  B.     Oil  Fields  of  Russia 4to,  10  oo 

—  Oil  Field   Development 10  oo 

Thompson,   S.   P.     Dynamo   Electric   Machines i6mo,  o  75 

Thompson,  W.  P.    Handbook  of  Patent  Law  of  All  Countries i6mo,  i  50 

Thomson,  G.    Modern  Sanitary  Engineering i2mo,  *s  oo 

Thomson,  G.  S.     Milk  and  Cream  Testing i2mo,  *2  25 

Modern  Sanitary  Engineering,  House  Drainage,  etc 8vo,  *3  oo 

Thornley,  T.     Cotton   Combing  Machines. 8vo,  *s  50 

—  Cotton    Waste    8vo,  ^3  50 

—  Cotton  Spinning.     8vo. 

First   Year    *i  50 

Second  Year *3  50 

Third   Year    *2  50 

Thurso,  J.  W.     Modern  Turbine  Practice 8vo,  *4  oo 

Tidy,  C.  Meymott.     Treatment  of  Sewage i6mo,  o  75 

rilmans,  J.     Water  Purification  and  Sewage  Disposal 8vo,  2  50 

Tinney,  W.  H.     Gold-mining  Machinery 8vo,  *3  oo 

Titherley,  A.  W.    Laboratory  Course  of  Organic  Chemistry 8vo,  *2  oo 

Tizard,  H.  T.     Indicators (In  Press.~) 

Toch,  M.    Chemistry  and  Technology  of  Paints 8vo,  4  50 

Materials  for  Permanent  Painting i2mo,  *2  oo 

Tod,  J.,   and  McGibbon,  W.  C.     Marine  Engineers'   Board   of  Trade 

Examinations    8vo,  *2  oo 

Todd,  J.,  and  Whall,  W.  B.     Practical  Seamanship 8vo,  12  oo 

Townsend,  F.    Alternating  Current  Engineering 8vo,  boards,  *o  75 

Townsend,  J.  S.    lonization  of  Gases  by  Collision 8vo,  *i  25 

Transactions  of  the  American  Institute  of  Chemical  Engineers,    8vo. 

Vol.  I.  to  XL,  1908-1918 8vo,  each,  6  oo 

Traverse  Tables  i6mo,  o  75 

Treiber,  E.  Foundry  Machinery i2mo,  2  oo 

Trinks,  W.  Governors  and  Governing  of  Prime  Movers 8vo,  3  50 

Trinks,  W.,  and  Housum,  C.  Shaft  Governors i6mo,  o  75 

Trowbridge,  W.  P.  Turbine  Wheels i6mo,  o  75 

Tucker,  J.  H.  A  Manual  of  Sugar  Analysis 8vo,  3  50 

Turnbull,  Jr.,  J.,  and  Robinson,  S.  W.  A  Treatise  on  the  Compound 

Steam-engine  i6mo,  o  75 

Turner,  H.  Worsted  Spinners'  Handbook i2mo,  *3  oo 

Turrill,  S.  M.    Elementary  Course  in  Perspective I2mo,  *i  25 

Twyford,  H.  B.     Purchasing 8vo,  *3  oo 

Storing,  Its  Economic  Aspects  and  Proper  Methods 8vo,  3  50 


D.  VAN  NOSTRAND  CO.'S  SHORT  TITLE  CATALOG  27 

Underbill,  C.  R.    Solenoids,  Electromagnets  and  Electromagnetic  Wind- 
ings     i2mo,  3  oo 

Underwood,  N.,  and  Sullivan,  T.  V.     Chemistry  and  Technology  of 

Printing   Inks    8vo,  *3  oo 

Urquhart,  J.  W.    Electro-plating i2mo,  2  oo 

Electrotyping , I2mo,  2  oo 

Usborne,  P.  O.  G.     Design  of  Simple  Steel  Bridges 8vo,  *4  oo 

Vacher,  F.    Food  Inspector's  Handbook i2mo, 

Van  Nostrand's  Chemical  Annual.     Fourth  issue  igiS.fabrikoid,  i2mo,  *3  oo 

—  Year  Book  of  Mechanical  Engineering  Data (In  Press.) 

Van  Wagenen,  T.  F.     Manual  of  Hydraulic  Mining i6mo,  i  oo 

Vega,  Baron  Von.     Logarithmic  Tables 8vo,  2  50 

Vincent,  C.    Ammonia  and  its  Compounds.  Trans,  by  M.  J.  Salter.Svo,  *2  50 

Vincent,  C.     Ammonia  and  its  Compounds 8vo,  2  50 

Virgin,  R.  Z.     Coal  Mine  Management (In  Press.) 

Volk,  C.     Haulage  and  Winding  Appliances 8vo,  *4  oo 

Von  Georgievics,  G.     Chemical  Technology  of  Textile   Fibres 8vo, 

—Chemistry  of  Dyestuffs 8vo,    (New  Edition  in  Preparation.) 

Vose,  G.  L.     Graphic  Method  for  Solving  Certain  Questions  in  Arithmetic 

and  Algebra    i6mo,  o  75 

Vosmaer,  A.    Ozone 8vo,  *2  50 

Wabner,  R.    Ventilation  in  Mines 8vo,  5  oo 

Wadmore,  T.  M.    Elementary  Chemical  Theory i2mo,  *i  50 

Wagner,   E.     Preserving   Fruits,   Vegetables,   and   Meat i2mo,  *2  50 

Wanner,  H.  E.,  and  Edwards,  H.  W.     Railway  Engineering  Estimates. 

(In  Press.) 

Wagner,  "J.  B.     Seasoning  of  Wood 8vo,  3  oo 

Waldram,  P.  J.     Principles  of  Structural  Mechanics i2mo,  4  oo 

Walker,  F.     Dynamo  Building i6mo,  o  75 

Walker,  J.     Organic  Chemistry  for  Students  of  Medicine 8vo,  4  oc 

Walker,  S.  F.     Steam  Boilers,  Engines  and  Turbines 8vo,  3  oo 

—  Refrigeration,  Heating  and  Ventilation  on  Shipboard i2mo,  *2  50 

— —  Electricity  in  Mining 8vo,  *4  50 

—  Electric   Wiring   and    Fitting 8vo,  2  50 

Wallis-Tayler,  A.  J.     Bearings  and  Lubrication 8vo,  *i  50 

Aerial  or  Wire  Ropeways 8vo    (Reprinting.) 

—  Preservation  of  Wood 8vo,  4  oo 

—  Refrigeration,  Cold  Storage  and  Ice  Making 8vo,  5  50 

—  Sugar    Machinery i2mo,  3  oo 

Walsh,  J.  J.    Chemistry  and  Physics  of  Mining  and  Mine  Ventilation, 

i2mo,  2  50 

Wanklyn,  J.  A.    Water  Analysis i2mo,  2  oo 

Wansbrough,  W.  D.    The  A  B  C  of  the  Differential  Calculus. ..  .  i2mo,  *2  50 

—  Slide  Valves i2mo,  *2  oo 

Waring,  Jr.,  G.  E.    Sanitary  Conditions i6mo,  o  75 

Sewerage  and  Land  Drainage *6  oo 

Modern  Methods  of  Sewage  Disposal i2mo,  2  oo 

How  to  Drain  a  House i2mo,  i  25 


28       D.  VAN  NOSTRAND  CO.'S  SHORT  TITLE  CATALOG 

Warnes,  A.  R.    Coal  Tar  Distillation 8vo,  *5  oo 

Warren,  F.  D.    Handbook  on  Reinforced  Concrete i2mo,  *2  50 

Watkins,  A.     Photography 8vo,  3  50 

Watson,  E.  P.    Small  Engines  and  Boilers lamo,  i  25 

Watt,  A.     Electro-plating  and  Electro-refining  of  Metals 8vo,  5  oo 

—  Electro-metallurgy izmo,  i  oo 

—  Paper-Making    8vo,  3  75 

Leather   Manufacture    8vo,  6  oo 

—  The  Art  of  Soap  Making 8vo,  4  oo 

Webb,  H.  L.  Guide  to  the  Testing  of  Insulated  Wires  and  Cables.  i2mo,  i  oo 

Wegmann,    Edward.      Conveyance    and    Distribution    of    Water    for 

Water  Supply 8vo,  5  oo 

Weisbach,  J.     A  Manual  of  Theoretical  Mechanics 8vo,  *6  oo 

Weisbach,  J.,  and  Herrmann,  G.     Mechanics  of  Air  Machinery.  ..  .8vo,  *3  75 

Wells,  M.   B.     Steel  Bridge  Designing 8vo,  *2  50 

Wells,   Robt.     Ornamental   Confectionery 12  mo,  3  oo 

Weston,  E.  B.    Loss  of  Head  Due  to  Friction  of  Water  in  Pipes.  .i2mo,  2  oo 

Wheatley,  0.     Ornamental  Cement  Work 8vo,  *2  25 

Whipple,  S.    An  Elementary  and  Practical  Treatise  on  Bridge  Building. 

8vo,  3  oo 

White,  C.  H.     Methods  of  Metallurgical  Analysis i2mo,  2  50 

White,  G.  F.     Qualitative  Chemical  Analysis i2mo,  140 

White,  G.  T.     Toothed  Gearing 12120,  *2  oo 

White,  H.  J.     Oil  Tank  Steamers 121*10,  i  50 

Whitelaw,   John.     Surveying 8vo,  450 

Whittaker,  C.  M.     The  Application  of  the  Coal  Tar  Dyestuff  s .  . .  8vo,  3  oo 

Widmer,  E.  J.     Military  Balloons 8vo,  3  oo 

Wilcox,  R.  M.     Cantilever  Bridges i6mo,  o  75 

Wilda,  H.     Steam  Turbines lamo,  2  oo 

—  Cranes   and   Hoists i2mo,  2  oo. 

Wilkinson,  H.   D.     Submarine   Cable   Laying  and   Repairing 8vo, 

{Reprinting.) 

Williamson,   J.     Surveying 8vo,  *3  oo 

Williamson,  R.  S.     Practical  Tables  in  Meteorology  and  Hypsometry, 

4to,  2  50 
Wilson,  F.  J.,  and  Heilbron,  I.  M.     Chemical  Theory  and  Calculations. 

i2mo,  *i  25 

Wilson,  J.  F.     Essentials  of  Electrical  Engineering 8vo,  2  50 

Wimperis,  H.  E.     Internal  Combustion  Engine 8vo,  "^3  oo 

Application  of  Power  to  Road  Transport i2mo,  ::;i  50 

—  Primer   of   Internal   Combustion    Engine i2mo,  i  50 

Winchell,  N.  H.,  and  A.  N.     Elements  of  Optical  Mineralogy 8vo,  *3  50 

Winslow,  A.     Stadia   Surveying i6mo,  o  75 

Wisser,  Lieut.  J.  P.     Explosive  Materials iGmo, 

— Modern  Gun  Cotton . . . . .  i6mo,  o  75 

Wolff,  C.  E.     Modern  Locomotive  Practice 8vo,  *4  20 

Wood,  De  V.     Luminiferous  Aether i6mo,  o  75 

Wood,  J.  K.     Chemistry  of  Dyeing i2mo,  i  oo 

Worden,  E.  C.     The  Nitrocellulose  Industry.     Two  Volumes 8vo,  *io  oo 

—  Technology  of  Cellulose  Esters.     In  10  volumes.     8vo. 

Vol.  VIII.     Cellulose  Acetate.  .                             *5  oo 


D.  VAN  NOSTRAND  CO.'S  SHORT  TITLE  CATALOG  29 

Wren,  H.     Organometallic  Compounds  of  Zinc  and  Magnesium,  .  i2mo,  i  oo 

Wiight,  A.  C.     Analysis  of  Oils  and  Allied  Substances • 8vo,  *3  50 

Wright,  A.  C.     Simple  Method  for  Testing  Painters'  Materials.  .  .8vo,  2  50 
Wright,  F.   W.     Design   of   a   Condensing   Plant.. i2mo    (Reprinting.') 

Wright,  H.  E.     Handy  Book  for  Brewers 8vo,  *6  oo 

Wright,  J.     Testing,  Fault  Finding,  etc.,  for  Wiremen i6mo,  o  50 

Wright,  T.  W.     Elements  of  Mechanics 8vo,  *z  50 

Wright,  T.  W.,  and  Hayford,  J.  F.    Adjustment  of  Observations.  ..8vo,  *3  oo 
Wynne,  W.  E.,  and  Sparagen,  W.     Handbook  of  Engineering  Mathe- 
matics  i2ino,  2  oo 

Yoder,  J.  H.,  and  Wharen,  G.  B.    Locomotive  Valves  and  Valve  Gears, 

8vo,  *3  oo 

Young,  J.  E.     Electrical  Testing  for  Telegraph  Engineers 8vo,  *4  oo 

Young,  R.   B.     The   Banket 8vo,  3  50 

Youngson.     Slide  Valve  and  Valve  Gears ' 8vo,  3  oo 

Zahner,  R.     Transmission  of  Power i6mo, 

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